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Thallium: A Comprehensive Guide To The Chemical Element

by chemdude71

Thallium is a chemical element with the symbol Tl and atomic number 81. It is a soft, bluish-white metal and is one of the least abundant elements on Earth. It was discovered in 1861 by British chemist William Crookes and named after the Greek word for “green twig”.

Thallium is one of the oldest known elements and has been used in a variety of applications throughout history.

 

Introduction

Thallium has some unique characteristics that make it stand out among other elements. It is highly reactive and can corrode many materials, including metals, plastics, and glass. As a result, it has found some niche uses, such as in thermometers, switches, and television tubes. Additionally, it is also used as a poison, and in the past was deliberately used to harm and even kill people.

The majority of thallium on the earth is found in the earth’s crust, in minerals such as iron pyrites, litharge, and thallite. It can also be found in the waters of oceans and other bodies of water. The majority of thallium produced today is from the processing of copper, lead, and zinc ores. Thallium can also be produced synthetically, though this is not widely practiced today.

Thallium has several physical properties that make it unique among elements. It is a soft and malleable metal, with a melting point of 303.5°C and boiling point of 1473°C. Thallium is also highly reactive and can form a variety of compounds with other elements, such as oxygen, sulfur, and chlorine. It is also a poor conductor of electricity.

Because of its reactivity, thallium has a variety of chemical properties. It can form several different compounds, including thallium(I) oxide, thallium(III) chloride, and thallium sulfate.

It can also form polymeric compounds, which are compounds that contain atoms of both thallium and other elements. Additionally, thallium has a nuclear property, which is the ability to be subjected to nuclear reactions, such as fission and fusion.

Thallium can be found in various forms, such as the metal itself, a sulfate salt, and an oxide. Its industrial uses are wide ranging, from the production of semiconductor materials to the manufacture of photographic chemicals. It also has some medical uses, such as in the treatment of cancer and as a tracer in medical imaging.

Thallium can be harmful, especially when it is ingested or inhaled. Its primary toxic effects are neurological, causing numbness, confusion, and even death in extreme cases. Therefore, it is important to take precautions when handling thallium and its compounds.

Overall, thallium is an element with some unique and valuable characteristics. Despite its potential risks, it has been used in a variety of applications throughout history and continues to be a key element in modern industry and science. This guide will provide an overview of thallium, its properties, sources, biological role, detection methods, and applications.

 

Properties of Thallium

Thallium is a chemical element with the symbol Tl and atomic number 81. It is a soft, bluish-white metal with a metallic luster that tarnishes in the air and is found in nature in trace amounts, usually in ores. Thallium is a member of the post-transition metal group and its properties make it a valuable component in a wide variety of applications.

Understanding the physical and chemical properties of thallium is important to know how it interacts with other elements and materials. Some of these properties include atomic weight, melting point, and boiling point.

Atomic Weight: Thallium has an atomic weight of 204.38 g/mol and is the third-lightest element in the periodic table. Its atomic weight is the sum of the number of protons and neutrons in an atom of thallium.

Melting Point: Thallium has a melting point of 303.5°C (577.9°F), which is higher than that of most metals. It is the only metal that is liquid at room temperature, though at higher temperatures it becomes a solid.

Boiling Point: Thallium also has a boiling point of 1473°C (2703°F). It is one of the few elements that have a higher boiling point than its melting point.

Chemical Properties: Thallium has two common oxidation states, +3 and +1. It has an affinity for sulfur, making it reactive with many elements, especially sulfur-containing compounds. It also has a tendency to form compounds with a variety of elements, including carbon, nitrogen, and oxygen.

Nuclear Properties: Thallium has a half-life of 3.78 days and is used in nuclear medical imaging. It is also used in nuclear power plants as a neutron absorber.

When exposed to air, thallium tarnishes quickly, forming a thin layer of corrosion on the surface of the metal. This layer of tarnish can be removed with a mild acid solution. Thallium is also highly toxic, so special precautions must be taken when handling it.

Thallium is a valuable component in a wide variety of applications, from electrical cables and semiconductors to medical imaging and nuclear power. Understanding the physical and chemical properties of thallium is essential to using it safely and effectively. By understanding its properties, we can ensure the safe handling, use, and disposal of this element.

 

Location and Sources

Thallium is a chemical element that has a wide variety of sources and forms and is found naturally in the environment. It is a soft, malleable, and bluish-white metal that is found in trace amounts in some rocks and soils. It can also be found in small amounts in some foods, as well as in industrial products such as pesticides, dyes, and photographic emulsions.

When it comes to the sources of thallium, it is primarily found in trace amounts in minerals such as crooksite, lorandite, and hutchinsonite. It is also found in sulfide ores, including copper, lead, zinc, and iron sulfide ores. In addition, it can be found as a by-product in the production of zinc, lead, and other metals.

Thallium exists in a variety of forms, such as thallium sulfide, thallium chloride, and thallium oxide. It is also present in some industrial products, including photochemical etching solutions, flame retardants, and some glass-making processes. It can also be found in some medical imaging equipment and other medical items.

Thallium has a number of industrial uses. It is used in the manufacture of semiconductor devices, as well as in the production of smoke detectors, anti-collision devices, and glass. It is also used in the production of lead-free solders, as well as in the preparation of semiconductor chips and optoelectronic devices. It is also a component of some photographic emulsions, as well as a catalyst in some chemical reactions.

Thallium can also be found in some foods, including grains, shellfish, and mushrooms. It is also found in some fertilizers, as well as in some coal ash. It can also be released into the environment through some industrial processes, such as the burning of coal and oil. The amount of thallium in food depends on the type of food and the amount of thallium that has been used in its production.

Thallium is a versatile chemical element that has a wide range of sources and forms. It can be found in trace amounts in some rocks and soils, as well as in some foods, industrial products, and medical items. It is also used in a variety of industrial processes, including the manufacture of semiconductor devices, smoke detectors, anti-collision devices, and glass.

Finally, it can be released into the environment through some industrial processes, such as the burning of coal and oil.

Biological Role

Thallium is a chemical element found in the periodic table, and it has a wide variety of effects on the human body, both beneficial and risky. When considering thallium, it’s important to understand how it interacts with the human body and what risks it might present.

Thallium is highly toxic, even at low levels of exposure, and can cause adverse reactions in humans. Inhalation and ingestion are the two primary ways that thallium enters the body.

It can be absorbed through the pores of the skin, as well as through the eyes and digestive system. Once inside the body, thallium accumulates in tissues and organs, including the kidneys, liver, heart, and brain.

Short-term exposure to thallium can lead to a variety of symptoms, such as nausea, vomiting, abdominal pain, and diarrhea. Long-term exposure can cause more serious health effects, such as kidney damage, liver damage, and even cancer. Thallium can also interfere with the nervous system, causing nerve damage and even paralysis.

The benefits of thallium are often overshadowed by its potential risks. However, thallium can have positive effects when used in the right way. Thallium can be used to diagnose certain diseases, such as acidosis, and it is also used in medical imaging procedures, such as X-rays and CT scans. Additionally, thallium can be used to treat certain types of cancer, as well as to reduce the risk of developing certain heart diseases.

However, thallium can also be dangerous when used incorrectly. Over-exposure can lead to health risks, and it can also be harmful to the environment if it isn’t carefully managed. Therefore, it’s important to understand the risks associated with thallium before using it.

Ultimately, thallium is a chemical element with both beneficial and risky effects. When used correctly, it can help diagnose and treat certain diseases, but it can also be harmful if not managed properly. It’s important to understand the effects of thallium before using it, especially when it comes to potential long-term health risks.

 

Detection and Applications

Thallium detection is an important factor in many industries, as it is used in many products and materials. In order to accurately detect and measure thallium, there are a variety of methods available. These methods include optical and atomic emission spectroscopy, X-ray fluorescence, neutron activation analysis, and inductively coupled plasma spectroscopy. Each of these methods has its own advantages and disadvantages, depending on the application.

One of the most common applications of thallium is in the manufacturing of semiconductors. It is especially useful in the production of low-voltage devices, such as diodes and transistors. Thallium is also commonly used in the production of radiation detectors, as it is highly sensitive to gamma rays and other ionizing radiation.

Thallium is also used in the production of infrared detectors, which are used in medical imaging, surveillance and remote sensing. Thallium sulfide is a common material used in infrared detectors due to its high absorption of infrared light and its low dark current.

In addition, thallium is used in the production of certain plastics, as it has a low melting point and is resistant to oxidation. Thallium is also used in the production of pigments, glass, and certain alloys.

Thallium is used in research and medicine in a variety of ways. For instance, it is used as a contrast agent in certain medical imaging procedures, such as CT scans and MRI scans. In addition, thallium can be used in experiments to measure radioactivity and to detect the presence of certain elements in a sample.

Finally, thallium is used in the production of certain drugs, such as thallium acetate, which is used to treat certain heart conditions. It is also used in industrial catalysts, such as thallium sulfate, which is used in the hydrotreating of crude oil.

In conclusion, thallium is a versatile and highly useful chemical element. It is used in a variety of applications, from semiconductors to medical imaging. In order to accurately detect and measure thallium, a variety of methods are available, including optical and atomic emission spectroscopy, X-ray fluorescence, neutron activation analysis, and inductively coupled plasma spectroscopy. Thallium is also used in the production of certain drugs, plastics, alloys, and pigments, as well as in research and medicine.

Therefore, thallium is an important chemical element that has a multitude of uses in many different industries.

Facts

Thallium is a chemical element with the symbol Tl
Its atomic number is 81.
Thallium, from Greek thallós, meaning “green shoot” or “twig”
Chemists William Crookes and Claude-Auguste Lamy discovered thallium independently in 1861
Thallium is a very soft, malleable, lustrous low-melting, silvery metal that tarnishes in air to the bluish-gray oxide.

It was found as a byproduct of sulfuric acid manufacturing.
A thallium atom has 81 electrons
Thallium is stored in mineral oils to prevent the oxidation and discoloration.
Thallium is found in the main minerals, crookesite, hutchinsonite, and lorandite.
Thallium has 41 isotopes which have atomic masses that range from 176 to 216.

203Tl and 205Tl are the only stable isotopes and make up nearly all of natural thallium
The presence of thallium in the earth’s crust is around 0.7 mg per kilogram
In the presence of water, the poisonous thallium hydroxide (TlOH) is formed.
Thallium is soft and malleable enough to be cut with an ordinary knife at room temperature.
The most stable radioactive isotope of thallium has a half-life of only 3.78 years.

Soluble thallium salts (many of which are nearly tasteless) are highly toxic
Thallium poisoning usually results in hair loss
Soluble thallium salts were historically used in rat poisons and insecticides.
The global production of thallium reaches 10 metric tonnes.
Approximately 65% of thallium production is used in the electronics industry
It is used in the pharmaceutical industry and in glass manufacturing.

Data

Thallium
Pronunciation THAL-ee-əm
Appearance silvery white
Standard atomic weight Ar°(Tl)
  • [204.382, 204.385]
  • 204.38±0.01 (abridged)
Thallium in the periodic table
Atomic number (Z) 81
Group group 13 (boron group)
Period period 6
Block   p-block
Electron configuration [Xe] 4f14 5d10 6s2 6p1
Electrons per shell 2, 8, 18, 32, 18, 3
Physical properties
Phase at STP solid
Melting point 577 K ​(304 °C, ​579 °F)
Boiling point 1746 K ​(1473 °C, ​2683 °F)
Density (near r.t.) 11.85 g/cm3
when liquid (at m.p.) 11.22 g/cm3
Heat of fusion 4.14 kJ/mol
Heat of vaporization 165 kJ/mol
Molar heat capacity 26.32 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 882 977 1097 1252 1461 1758
Atomic properties
Oxidation states −5,[2] −2, −1, +1, +2, +3 (a mildly basic oxide)
Electronegativity Pauling scale: 1.62
Ionization energies
  • 1st: 589.4 kJ/mol
  • 2nd: 1971 kJ/mol
  • 3rd: 2878 kJ/mol
Atomic radius empirical: 170 pm
Covalent radius 145±7 pm
Van der Waals radius 196 pm
Other properties
Natural occurrence primordial
Crystal structure ​hexagonal close-packed (hcp)
Speed of sound thin rod 818 m/s (at 20 °C)
Thermal expansion 29.9 µm/(m⋅K) (at 25 °C)
Thermal conductivity 46.1 W/(m⋅K)
Electrical resistivity 0.18 µΩ⋅m (at 20 °C)
Magnetic ordering diamagnetic
Molar magnetic susceptibility −50.9×10−6 cm3/mol (298 K)
Young's modulus 8 GPa
Shear modulus 2.8 GPa
Bulk modulus 43 GPa
Poisson ratio 0.45
Mohs hardness 1.2
Brinell hardness 26.5–44.7 MPa
CAS Number 7440-28-0
History
Naming after Greek thallos, green shoot or twig
Discovery William Crookes (1861)
First isolation Claude-Auguste Lamy (1862)
Main isotopes Decay
abun­dance half-life (t1/2) mode pro­duct
201Tl synth 3.0421 d ε 201Hg
203Tl 29.5% stable
204Tl synth 3.78 y β− 204Pb
ε + β+ 204Hg
205Tl 70.5% stable
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Facts

The Fascinating World Of Neodymium: A Comprehensive Overview

by chemdude71

Neodymium is a chemical element with the atomic symbol Nd, atomic number 60 and atomic weight 144.3. It belongs to the lanthanides group and has the electronic configuration [Xe]4f4 5d1 6s2. Neodymium has a melting point of 1021°C and a boiling point of 3074°C. It is a relatively abundant element on earth and is mainly found in igneous and metamorphic rocks.

 

Introduction

Neodymium was first discovered by Carl Auer von Welsbach in Vienna, Austria in 1885. He named it neodymium after the Greek words “neos” meaning new and “didymos” meaning twin. It was first isolated from a mineral called “didymia” which is now known to contain both praseodymium and neodymium.

The two elements could not be separated until 1925 when a method for isolating them was developed by Austrian chemist Baron Carl Auer von Welsbach.

Neodymium is a silvery-white metal that is relatively soft and ductile. It is highly reactive and tarnishes readily in air and reacts with water and steam to form hydrated neodymium compounds. It also reacts with acids and forms neodymium salts. Neodymium has six known oxidation states ranging from +3 to +5.

Neodymium is a relatively abundant element and can be found in igneous, metamorphic and sedimentary rocks. It is also found in phosphate and carbonate minerals as well as in some rare earth ores. Neodymium is also found in various sources of seawater and in some sedimentary rocks.

Neodymium has many uses and applications in industry and technology. It is primarily used in the production of permanent magnets, glass, welding, cutting and optical equipment. It is also used in lasers and optical equipment.

Neodymium is considered to be a non-toxic element, however, overexposure to it can cause adverse health effects such as skin and eye irritation. In addition, neodymium can have an environmental impact if it is not properly managed.

Neodymium is most commonly mined from monazite and bastnasite, which are rare earth ores. The process of production and extraction of neodymium is costly and requires a complex series of steps. The cost of production and extraction of neodymium varies depending on the source and quality of the ore.

Neodymium is a fascinating and useful element. It has a wide range of applications and uses in industry and technology. It is also an abundant element on earth and is relatively non-toxic. The future of neodymium production and use looks promising as technology advances and new uses for it are discovered.

 

Physical Characteristics

Neodymium is a chemical element with the symbol Nd and atomic number 60, and its atomic weight is 144.2 g/mol. It is part of the lanthanide series and is commonly found in the Earth’s crust in combination with other elements. Neodymium belongs to the group of transition metals, and it is located in period 6 in the periodic table.

Neodymium is a soft, malleable silver-colored metal at room temperature, and it has a melting point of 1021 °C and a boiling point of 3147 °C. It is a paramagnetic metal, and it is slightly more stable in air than other lanthanides due to a protective oxide layer that forms on its surface.

Neodymium is also a relatively abundant element, with an estimated abundance in the Earth's crust of about 39 parts per million.

Neodymium has five naturally occurring oxidation states; -3, 0, +1, +2, and +3. It is usually found in oxidation state +3, and its cationic form is a bright yellow color in solution. It is highly reactive and can form a variety of compounds with other elements, such as oxides, halides, nitrides, phosphides, and sulfides.

Neodymium is a vital element for many industries, and it is used in a wide range of applications, from electronics and lasers to glass manufacturing and welding and cutting. It is a key component in many permanent magnets, and its electrical and magnetic properties make it essential for the production of lasers and optical equipment.

Neodymium is an important element with a variety of uses and applications. Its fascinating properties make it a valuable asset and its production and mining are necessary to sustain its use in many industries.

 

Chemical Properties

Neodymium is one of the rare earth elements and is famously known for its strong magnetic properties. It is a relatively soft metal and has a silvery-white color. This element is highly reactive and its chemical properties make it a desirable material for many applications.

Neodymium has an atomic symbol of Nd, an atomic number of 60, and an atomic weight of 144. It is classified as a lanthanide with a group number of 3. The metal has a melting point of 1021°C and a boiling point of 3127°C.

The most common oxidation states of neodymium are +2 and +3. The +3 state is the most common, and it is similar to that of scandium, yttrium, and lanthanum. This element is highly reactive when exposed to air and can easily form a protective oxide layer in the form of Nd 2 O 3 . When heated to a point where the oxide layer is destroyed, the metal will further react with the oxygen in the air.

Neodymium also forms compounds with other elements such as halides, oxyhalides, oxides, hydroxides, and nitrates. The metal also reacts readily with water, forming a hydroxide solution and releasing hydrogen gas.

When neodymium is exposed to a high temperature, it forms a volatile neodymium oxide, which can be difficult to remove. This oxide can form in the presence of oxygen, sulfur, and chlorine.

Neodymium is also unique in its ability to form a variety of coordination complexes with various ligands. These coordination complexes can be used in many applications, including catalysts and fuel cells.

Neodymium compounds are also used as catalysts in the production of high-value compounds such as polymers, pharmaceuticals, and fine chemicals. The catalytic properties of neodymium are also used in the production of methanol and the production of hydrogen.

In addition, neodymium is used as a catalyst for the production of a wide variety of fuels including gasoline, diesel, and propane. Neodymium compounds are also used in the production of pigments, fluorescent powder, and paints.

 

Environmental Impact

Neodymium has a range of potential impacts on the environment. When exposed to the air, neodymium reacts with oxygen to form a neodymium oxide which can then be dispersed in the environment. Ingestion of neodymium oxide can cause health problems, and, depending on the level of exposure, can be dangerous and even fatal.

Neodymium is relatively non-toxic, but when large quantities are present in the environment, it can lead to long-term health issues.

Neodymium can also be toxic to aquatic organisms if it is released into bodies of water, and its environmental impact can vary depending on the levels of exposure. Neodymium can accumulate in the body tissues of organisms, accumulating over time. In addition, neodymium can bind to organic material in the water, and can therefore be taken up by aquatic organisms, which can lead to further accumulation in the body.

Neodymium can also be toxic to plants, animals, and other organisms. Neodymium can be found in the soil, and can cause damage to plants and animals. It can also be toxic to microorganisms in the soil, and can lead to the leaching of heavy metals and other materials into the water supply.

Neodymium can also be released into the atmosphere and can be dispersed into clouds, where it can be inhaled by humans and animals. Inhalation of neodymium oxide can lead to the formation of neodymium-related compounds in the body, which can be toxic and cause health problems.

Neodymium is also a potential radiological hazard and can be hazardous if it is mishandled. Neodymium can be radioactive when it is in its free form, and can cause health issues if it is not handled properly. Neodymium can also be released into the atmosphere if it is mishandled, and can be dispersed into the air, which can cause health problems if breathed in.

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Mining and Production

Neodymium is not found in its pure elemental form in nature but is mined from other sources. It is found in several minerals, such as monazite sand, bastnasite, and eudialyte. Monazite sand is the most common source of neodymium and is mined in large quantities in Brazil, India, Australia, and other areas of South Asia. On an industrial level, neodymium is mainly mined from two types of mineral deposits: carbonate-hosted deposits and placer deposits.

Carbonate-hosted deposits are found in areas where carbonate rocks have a high neodymium concentration. These deposits are the most common type of neodymium deposit, and they are found in China, Russia, Vietnam, and South Africa. Placer deposits are created when weathering and erosion cause neodymium to be released from its ore and collected in riverbeds. These deposits are found in Canada, India, Australia, and Brazil.

The process of extracting neodymium from the ore is a complicated and expensive one. The ore must first be crushed and ground down into smaller particles. The ore is then placed in special tanks and treated with sulfuric acid, which dissolves the neodymium and other metals. The solution is then filtered, and the neodymium is separated out and precipitated.

The purified neodymium is then heated to over 1000 degrees Celsius, which forms a solid neodymium oxide. The neodymium oxide is then reduced in a vacuum furnace to create neodymium metal.

The cost of producing neodymium depends on the type of deposit it is sourced from. Carbonate-hosted deposits can be more expensive to mine and process because of the complicated extraction process. Placer deposits can be less expensive to mine and process because they require less processing.

Neodymium is also available in recycled form. Recycled neodymium is typically cheaper than newly mined neodymium, but it is not as pure as newly mined neodymium. Recycled neodymium is mainly sourced from used electronics, such as old computers and cell phones.

The increasing demand for neodymium has caused some concerns about its availability. While neodymium deposits are found in many areas of the world, some countries, such as China, have begun limiting their production of neodymium in order to protect their own resources.

This has caused a rise in the prices of neodymium, as the supply of neodymium is becoming increasingly limited.

 

Uses and Applications

Neodymium is a rare earth element with many different uses and applications. It is used in many industries and plays an important role in the production of goods, from electronics to lasers and glass.

One of the most common uses for neodymium is in the production of permanent magnets. This is due to its high magnetic strength and resistance to demagnetization. It is used in the production of motors, hard disk drives, and microphones. Neodymium magnets are also used in magnetic resonance imaging (MRI) machines and wind turbines.

The glass industry often uses neodymium in the production of lenses and fiber optics. The element is used as an optical glass due to its ability to produce a wide range of colors. Neodymium is used to reduce the amount of light dispersion and to improve light transmission. This has made it a popular choice for telescopes, microscopes, and other devices that require high-precision optical components.

Neodymium is also used in arc welding and cutting. It is used in the form of a coating on electrodes in order to improve arc starts and decrease the amount of spatter. Neodymium produces a brighter arc, which is helpful in welding thin materials and materials with low melting points.

Neodymium is also a key component in the production of lasers and optical equipment. It is used in both solid-state and gas lasers due to its ability to produce intense laser light. It is also used in optical equipment, such as eyeglasses and sunglasses, due to its ability to create different colors of light.

Finally, neodymium is used in the production of nuclear reactors and nuclear weapons due to its ability to absorb neutrons. It is also used in the production of fuel rods for nuclear power plants.

Neodymium is an important element with many different uses and applications. Its ability to create different colors of light, produce intense laser light, and absorb neutrons make it a valuable asset in many industries. Its use in the production of permanent magnets, lasers, and optical equipment has made it an indispensable element in the modern world.

Facts

The name of the element is derived from the Greek word “neos didymos” meaning new twin
Neodymium is a chemical element with the symbol Nd
Its atomic number is 60
neodymium is as prevalent in the Earth's crust as nickel, copper, and cobalt.
It is a hard, slightly malleable, silvery metal that quickly tarnishes in air and moisture.

Neodymium's concentration is about thirty-eight milligrams per kilogram in the crust
Neodymium was discovered in 1885 by the Austrian chemist Carl Auer von Welsbach
The current reserves of neodymium are believed to be around eight million tons
Two of neodymium's radioactive isotopes, Nd-144 and Nd-150, are also found in nature.
Neodymium is the fourth member of the lanthanide series

It is most often found as a component in monazite and bastnasite minerals.
The world's production of neodymium was about 7,000 tons in 2004
Most of the world's commercial neodymium is mined in China
Naturally occurring neodymium (60Nd) is composed of five stable isotopes—142Nd, 143Nd, 145Nd, 146Nd and 148Nd
142Nd is the most abundant (27.2% of the natural abundance)

In all, 33 radioisotopes of neodymium have been detected as of 2022
To make neodymium magnets it is alloyed with iron, which is a ferromagnet.
Neodymium magnets (an alloy, Nd2Fe14B) are the strongest permanent magnets known
Neodymium is the fourth member of the lanthanide series

Data

Neodymium
Pronunciation (NEE-oh-DIM-ee-əm)
Appearance silvery white
Standard atomic weight Ar°(Nd)
 
  • 144.242±0.003
  • 144.24±0.01 (abridged)
Neodymium in the periodic table
Atomic number (Z) 60
Group f-block groups (no number)
Period period 6
Block   f-block
Electron configuration [Xe] 4f4 6s2
Electrons per shell 2, 8, 18, 22, 8, 2
Physical properties
Phase at STP solid
Melting point 1297 K ​(1024 °C, ​1875 °F)
Boiling point 3347 K ​(3074 °C, ​5565 °F)
Density (near r.t.) 7.01 g/cm3
when liquid (at m.p.) 6.89 g/cm3
Heat of fusion 7.14 kJ/mol
Heat of vaporization 289 kJ/mol
Molar heat capacity 27.45 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1595 1774 1998 (2296) (2715) (3336)
Atomic properties
Oxidation states 0, +2, +3, +4 (a mildly basic oxide)
Electronegativity Pauling scale: 1.14
Ionization energies
  • 1st: 533.1 kJ/mol
  • 2nd: 1040 kJ/mol
  • 3rd: 2130 kJ/mol
Atomic radius empirical: 181 pm
Covalent radius 201±6 pm
Other properties
Natural occurrence primordial
Crystal structure ​double hexagonal close-packed (dhcp)
Speed of sound thin rod 2330 m/s (at 20 °C)
Thermal expansion α, poly: 9.6 µm/(m⋅K) (at r.t.)
Thermal conductivity 16.5 W/(m⋅K)
Electrical resistivity α, poly: 643 nΩ⋅m
Magnetic ordering paramagnetic, antiferromagnetic below 20 K
Molar magnetic susceptibility +5628.0×10−6 cm3/mol (287.7 K)
Young's modulus α form: 41.4 GPa
Shear modulus α form: 16.3 GPa
Bulk modulus α form: 31.8 GPa
Poisson ratio α form: 0.281
Vickers hardness 345–745 MPa
Brinell hardness 265–700 MPa
CAS Number 7440-00-8
History
Discovery Carl Gustaf Mosander (1841)
First isolation Carl Auer von Welsbach (1885)
Named by Carl Auer von Welsbach (1885)
Main isotopes[5] Decay
  abun­dance half-life (t1/2) mode pro­duct
142Nd 27.2% stable
143Nd 12.2% stable
144Nd 23.8% 2.29×1015 y α 140Ce
145Nd 8.3% stable
146Nd 17.2% stable
148Nd 5.80% stable
150Nd 5.60% 6.7×1018 y β−β− 150Sm
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Facts

Lutetium: A Comprehensive Overview Of The Chemical Element

by chemdude71

Lutetium is a chemical element of the periodic table with the symbol Lu and atomic number 71. It belongs to the lanthanide group and is the last element in the lanthanide series.

Lutetium is a silvery-white metal with a density of 9.84 g/cm3 and a melting point of 1925°C. It is the fifth densest element and has the highest melting point of all lanthanides.

Introduction

Lutetium is a relatively rare element and has many unique properties. It has a high neutron capture cross-section, which makes it an ideal candidate for nuclear reactor fuel. It also has a strong ability to absorb gamma rays, making it useful in radiation therapy.

It is also highly resistant to corrosion and has a strong affinity for oxygen. This makes it useful for the production of oxygen compounds and it is also used as a stabilizing agent in alloys.

The history of Lutetium dates back to the early 1900s. It was first identified by Georges Urbain in 1907 when he separated ytterbium from a sample of yttrium oxide. However, he could not separate lutetium from his ytterbium sample and it was not until 1923 that it was re-discovered by Charles James.

Lutetium’s atomic structure is composed of 71 protons, 71 electrons and 108 neutrons. It has seven naturally occurring isotopes, ranging from Lu-143 to Lu-175, with the most common isotope being Lu-177. Its electron configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d1 6p6 7s2.

Compounds and alloys of Lutetium are also used in a variety of industrial applications. It is a component of the catalysts used in the production of synthetic rubber and is also used in the manufacture of high-temperature alloys and as a stabilizing agent in alloys. Common compounds of lutetium include lutetium oxychloride, lutetium fluoride, lutetium-177 oxide, and lutetium-178 chloride.

Lutetium (Lu) sublimed, dendritic

The oxidation states of lutetium range from +3 to +5. It is most stable in its +3 oxidation state, which is why it is used in compounds such as lutetium oxychloride and lutetium-178 chloride. The +4 oxidation state is also relatively stable and is used in compounds such as lutetium fluoride.

Lutetium is found naturally only in trace amounts in minerals such as monazite and xenotime. It is also found in the earth’s crust in small amounts but is not found in large enough quantities to be commercially viable.

The safety and hazards of lutetium must be taken into consideration when working with the element. Inhalation of lutetium dust can cause serious health problems, such as respiratory tract irritation. It is also highly toxic if swallowed, so protective equipment must be worn when handling the element.

Finally, some interesting facts about lutetium are that it has a strong ability to absorb gamma rays, it is highly resistant to corrosion, and it has the highest melting point of all the lanthanides. It is also used in the production of oxygen compounds and has a number of uses outside of chemistry.

In addition, Lutetium’s unique properties can give it some “superpowers” when used in combination with other elements.

 

Atomic Structure

Lutetium is a chemical element belonging to the Rare Earths group of elements and is represented by the symbol ‘Lu’. It is one of the heaviest elements in the periodic table with an atomic number of 71 and is located at the bottom of the lanthanide series. It is a soft, silvery-white metal that is malleable and ductile.

Atomic structure of lutetium is composed of protons and neutrons, which are present in the nucleus, and electrons, which orbit the nucleus. It has 71 protons in its nucleus, which are responsible for its atomic number. The number of neutrons in its nucleus varies, depending on the isotope present. Lutetium has seven naturally occurring isotopes, ranging from Lu-177 to Lu-183.

Its electron configuration is represented by [Xe] 4f14 5d1 6s2. This indicates that the outermost shell contains two electrons in the 6s orbital, one electron in the 5d orbital, and fourteen electrons in the 4f orbital. This electron configuration is similar to that of other rare-earth elements and gives lutetium its chemical properties.

Lutetium is a member of the lanthanide series of elements, and as such, shares many properties with other lanthanide elements. It has a very low boiling point and a low melting point. Its boiling point is 3675 K (3402 °C, 6156 °F) and its melting point is 1663 K (1390 °C, 2514 °F).

It has a crystal structure similar to that of other lanthanide elements and is cubic in shape. Its density is 9.841 g/cm3 and its atomic radius is 2.26 angstroms.

Overall, lutetium is a chemical element with unique properties and a complex atomic structure. Its protons, neutrons, and electrons come together to form a stable element that is an important part of science and industry. Its abundance in the Earth’s crust is relatively low, making it a rare element.

 

Compounds and Alloys

Lutetium is a chemical element with a number of interesting properties and a variety of compounds and alloys. It is important to understand the compounds and alloys that can be created with lutetium in order to benefit from its unique characteristics.

Common Compounds:

Lutetium oxide (Lu2O3) is the most commonly used compound of lutetium, and is a white powder that is stable at room temperature and pressure.

Lu2O3 is used in a variety of industries, including ferroelectrics, optics, and lasers. Other lutetium compounds include lutetium chloride (LuCl3), lutetium fluoride (LuF3), and lutetium sulfate (Lu2(SO4)3).

Industrial Applications:

Lutetium compounds have a variety of industrial applications. Lu2O3 is used in the electronics industry due to its ability to absorb infrared radiation. It is also used in the production of flat-panel displays and as an abrasive material. Lutetium chloride is used in photography, as it is sensitive to infrared light and can be used to detect invisible infrared light.

Lutetium sulfate is used in the production of synthetic diamonds, as it acts as a catalyst in the high-pressure, high-temperature process of diamond growth.

Common Alloys:

Lutetium is often combined with other elements to create alloys. One common alloy is lutetium-hafnium (LuHf), which is used in jet engines and nuclear reactors. This alloy has a low coefficient of thermal expansion, making it ideal for use in applications that require high temperatures and pressures.

Another common alloy is lutetium-titanium (LuTi), which is used in optics and aerospace applications due to its high thermal stability and low reactivity.

Lutetium has a variety of compounds and alloys that can be used in a number of industries. Its unique properties make it a valuable element in a number of applications, and its alloys allow for further customization to meet specific needs.

By combining lutetium with other elements, a wide range of compounds and alloys can be created with a variety of uses.

Oxidation States

The oxidation states of lutetium are very important in understanding its chemistry. Lutetium is an element in the lanthanide series, and its oxidation states are +3, +4, and +7. In its most common oxidation state, +3, lutetium has a filled outer f orbital.

The common oxidation states of lutetium are +3 and +4. In its +3 oxidation state, lutetium has a filled outer f orbital and a stable 6s2 electron configuration. In its +4 oxidation state, it has a filled outer f orbital and a stable 5d1 6s2 electron configuration.

The +7 oxidation state of lutetium is a bit less common than its +3 and +4 states, but is still important. In this state, lutetium has a filled outer f orbital and a stable 5d1 6s2 6p1 electron configuration. This state is also sometimes represented as Lu(VIII).

The +3 oxidation state of lutetium often forms compounds with oxygen, and is often used in oxidation reactions. For example, the oxide compound of lutetium and oxygen (Lu2O3) is used in a variety of industrial processes, including catalysis.

The +4 oxidation state of lutetium is also important, and is often used in reduction reactions. For example, lutetium tetraiodide (LuI4) is often used in the production of pharmaceuticals.

The +7 oxidation state of lutetium is also important, and is often used in complex reactions. For example, lutetium(VII) oxide (Lu2O7) is used in the production of specialty glass, and lutetium(VII) fluoride (LuF7) is used in the production of optical lenses.

While lutetium's oxidation states are important in understanding its chemistry, it is important to note that all of its oxidation states are not chemically stable. The +2 oxidation state is not stable, and will quickly decompose to the +3 or +4 state. This means that it is not possible to use lutetium in the +2 oxidation state in reactions.

 

Natural Occurrence

Lutetium is a rare and precious chemical element found in the periodic table, and it is not found in nature in its elemental form. Instead, it is found as a compound in the form of lutetium oxide, which is sometimes referred to as lutecia.

Lutecia is found in small amounts in rocks and minerals, such as monazite, xenotime, and euxenite. It is also found in trace amounts in zircon and in other rare and precious gems.

The most abundant source of lutetium is monazite, which is a silicate mineral that contains lutetium-176, lutetium-175, and other rare earth elements. The element is present in monazite in concentrations of up to 0.7 percent. Xenotime, which is a phosphate mineral, is also a common source of lutetium. It is found in concentrations of up to 0.1 percent in some samples.

Euxenite is another source of lutetium. It is a rare and complex mineral composed of several rare earth elements, including lutetium. It is found in concentrations of up to 0.2 percent. Zircon is yet another source of the element. It is found in concentrations of up to 0.05 percent.

Lutetium can also be found in trace amounts in other rare and precious gems, such as rubies and sapphires. It is found in concentrations of up to 0.1 percent in some samples.

In addition to these sources, lutetium can be recovered from nuclear waste streams in nuclear power plants. It is also produced as a by-product of the industrial recovery of uranium and thorium.

In terms of natural abundance, lutetium is the rarest of all the lanthanides, with an estimated abundance of 0.0021 parts per million in the Earth's crust. This makes it one of the rarest elements on the planet, with a concentration of just 0.00004 percent.

Lutetium can also be found in trace amounts in meteorites. It is believed to be a primordial element that was formed during the Big Bang, but its abundance is unknown due to its rarity.

 

Safety and Hazards

Lutetium is a highly toxic chemical element and any exposure to it must be avoided. It has been established that the element is a human health hazard and can cause severe poisoning if ingested, breathed in, or absorbed through the skin.

The health hazards associated with lutetium include irritation of the eyes, skin, and respiratory system; damage to the liver, kidney, and heart; and central nervous system depression. In severe cases, lutetium can cause death.

Exposure to lutetium can also cause significant environmental damage. Studies have shown that lutetium can have a detrimental impact on the soil and water, as well as on plant and animal life.

It is also essential to keep lutetium sealed away from the environment in an appropriate container, such as a glass jar or sealed metal drum. The container must also be properly labeled with information about the hazard.

In the event of a fire, lutetium must be kept away from water, as this can release hazardous gases into the air. It is also important to keep a fire extinguisher handy in case of an emergency.

In conclusion, lutetium is a highly toxic chemical element and must be handled with extreme caution. Proper safety protocols, such as wearing protective clothing and keeping lutetium sealed away from the environment, must be observed at all times.

 

Interesting Facts

Lutetium is an interesting and unusual chemical element that has many interesting properties and uses. Knowing a few interesting facts about this element can help you appreciate its various uses and understand why it is so important.

One of the most amazing things about lutetium is its ability to absorb energy and release it later. This is known as light emission and is used in various scientific studies. It can also be used in medical imaging to help doctors detect tumors and other diseases.

Another interesting property of lutetium is its ability to concentrate in certain areas. This is called lutetium concentration and can be used to identify mineral deposits, which can help scientists understand the geology of a particular area.

Another interesting fact about lutetium is its use as an additive in nuclear power plants. Lutetium is used to help control the reaction of the nuclear fuel, which helps keep the plant safe. It is also used in nuclear reactors to help regulate the amount of radiation that the reactor emits.

Lutetium is also used as a catalyst in chemical reactions. It helps speed up chemical processes and can be used in the production of plastics and other industrial materials. It is also used in the medical field to help break down certain proteins and to help speed up the body’s healing process.

In addition, lutetium is also used in certain medical imaging techniques, including PET scans. The element absorbs gamma radiation and then releases it, which helps to create images of the inside of the human body. This allows doctors to diagnose and treat certain diseases.

Finally, lutetium is also used in certain types of lasers. It is used to help control the beam of light, which helps make laser treatments more precise. This is especially effective in laser eye surgery and other medical laser treatments.

By understanding a few interesting facts about lutetium, it is easy to see that this element is an incredibly important part of our modern world. It is used in a variety of industries and applications and can help us better understand the world around us.

Facts

The element originally was named lutecium
Lutetium is a chemical element with the symbol Lu
Its atomic number is 71
It is a silvery white metal, which resists corrosion in dry air, but not in moist air.
Lutetium is the last element in the lanthanide series

It is traditionally counted among the rare earth elements
Lutetium atoms are the smallest of any of the lanthanides.
Three separate scientists discovered lutetium in 1907, independent of each other.
The mineral ytterbia was the source of lutetium discovered by the three researchers
Lutetium occurs on the Earth in form of two isotopes: lutetium-175 and lutetium-176.

Only one of those isotopes, lutetium-175, is stable, making it a monoisotopic element.
The unstable isotope, lutetium-176, has a half-life of almost 38 trillion years.
Only 2.5% of the lutetium found on Earth is in the unstable form.
Lutetium is the hardest lanthanide element.
It’s also the most expensive lanthanide.

The world production of lutetium (in the form of oxide) is about 10 tonnes per year.
Lutetium is only available in the Earth's crust at about 0.5 milligrams per kilogram.
It is one of the rarest and most expensive of the rare earth metals with the price about US$10,000 per kilogram
The element also has 43 known nuclear isomers

Data

Lutetium
Pronunciation lew-TEE-shee-əm
Appearance silvery white
Standard atomic weight Ar°(Lu)
  • 174.9668±0.0001
  • 174.97±0.01 (abridged)
Lutetium in the periodic table
Atomic number (Z) 71
Group group 3
Period period 6
Block   d-block
Electron configuration [Xe] 4f14 5d1 6s2
Electrons per shell 2, 8, 18, 32, 9, 2
Physical properties
Phase at STP solid
Melting point 1925 K ​(1652 °C, ​3006 °F)
Boiling point 3675 K ​(3402 °C, ​6156 °F)
Density (near r.t.) 9.841 g/cm3
when liquid (at m.p.) 9.3 g/cm3
Heat of fusion ca. 22 kJ/mol
Heat of vaporization 414 kJ/mol
Molar heat capacity 26.86 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1906 2103 2346 (2653) (3072) (3663)
Atomic properties
Oxidation states 0,[2] +1, +2, +3 (a weakly basic oxide)
Electronegativity Pauling scale: 1.27
Ionization energies
  • 1st: 523.5 kJ/mol
  • 2nd: 1340 kJ/mol
  • 3rd: 2022.3 kJ/mol
Atomic radius empirical: 174 pm
Covalent radius 187±8 pm
Other properties
Natural occurrence primordial
Crystal structure ​hexagonal close-packed (hcp)
Thermal expansion poly: 9.9 µm/(m⋅K) (at r.t.)
Thermal conductivity 16.4 W/(m⋅K)
Electrical resistivity poly: 582 nΩ⋅m (at r.t.)
Magnetic ordering paramagnetic[3]
Young's modulus 68.6 GPa
Shear modulus 27.2 GPa
Bulk modulus 47.6 GPa
Poisson ratio 0.261
Vickers hardness 755–1160 MPa
Brinell hardness 890–1300 MPa
CAS Number 7439-94-3
History
Naming after Lutetia, Latin for: Paris, in the Roman era
Discovery Carl Auer von Welsbach and Georges Urbain (1906)
First isolation Carl Auer von Welsbach (1906)
Named by Georges Urbain (1906)
Main isotopes[4] Decay
abun­dance half-life (t1/2) mode pro­duct
173Lu synth 1.37 y ε 173Yb
174Lu synth 3.31 y ε 174Yb
175Lu 97.4% stable
176Lu 2.60% 3.78×1010 y β− 176Hf
177Lu synth 6.65 d β− 177Hf
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Facts

Introducing Yttrium: History, Discovery, And Properties

by chemdude71

Yttrium is a chemical element that is classified as a transition metal in the periodic table. It is one of the rare earth elements, and its atomic number is 39. Yttrium was discovered in 1787 by Swedish chemist Carl Axel Arrhenius, while examining the minerals known as ytterbite or gadolinite.

The element was named after the village of Ytterby in Sweden, where it was first extracted from the minerals.

Introduction

Yttrium has some very unique properties that make it a highly sought-after material in many industries. Its physical properties, such as its atomic number and weight, melting and boiling points, and density, are all important characteristics.

It is also known for its chemical properties, such as its reactivity, oxidation states, and compounds. Yttrium plays an important role in the production of electronics, metals, and alloys, and in the manufacture of glass.

Yttrium has some interesting facts associated with it that make it an interesting element to learn about. Its name originates from the Swedish village of Ytterby, where it was first discovered. It is naturally occurring in some minerals, and its special properties have made it an important material in many industries.

Safety concerns regarding Yttrium include its potential environmental impacts, toxicity, and handling precautions. It is important to be aware of these safety concerns and to take the necessary precautions when handling Yttrium.

This article will provide an overview of Yttrium and will explore its history, discovery, properties, uses, and interesting facts. It will also discuss safety concerns and will provide information on how to properly handle Yttrium.

Physical Properties

Yttrium is an element in the periodic table with an atomic number of 39 and an atomic mass of 88.9. It is a silvery-white, rare Earth metal with a bright, lustrous appearance and low density. As a member of the lanthanide group, Yttrium is a transition metal, and is considered to be a moderately hard metal.

It has a melting point of 1522°C and a boiling point of 3345°C, with a density of 4.472 g/cm3. Yttrium is relatively unreactive, but can form compounds with oxygen or halogens to form yttrium oxide or halides. These compounds are typically yellow or white in color, and are highly insoluble in water.

At room temperature, Yttrium is a brittle and ductile metal. It has a low electrical conductivity and a higher thermal conductivity than most other metals, making it ideal for use in high-temperature applications. It also has a low Mohs hardness, meaning it is susceptible to wear and tear.

Yttrium's chemical properties are more complex than its physical properties. At high temperatures, its reactivity increases and it can form compounds with other metals and non-metals. It is able to form four oxidation states, from +3 to +7, making it a good redox catalyst. It is also able to form compounds with sulfur and phosphorus, and can form organometallic compounds with ligands such as acetylacetonate.

Yttrium has several unique properties that make it useful in a wide variety of applications. It is relatively non-toxic, odourless, and non-flammable, and it can form very strong alloys with other metals. It also has excellent magnetic properties, making it an ideal material for use in electronics and electrical equipment.

Finally, Yttrium is also able to absorb and retain neutrons, making it invaluable for use in nuclear reactors and in certain medical procedures. This property makes it an important component in the development of nuclear energy and nuclear medicine.

 

Chemical Properties

Yttrium is a transition metal, belonging to group 3 of the periodic table and its atomic number is 39. This makes it one of the most abundant elements in the Earth’s crust. Yttrium is also unique in that it has a very diverse range of chemical properties, which makes it useful in many applications.

Reactivity:

Yttrium is known to be relatively reactive, though not as reactive as other transition metals. Yttrium reacts with oxygen and nitrogen in the air to form a layer of oxide and nitride on the surface of the metal. This layer is stable and inert, protecting the metal beneath it. Yttrium also reacts with halogens to form yttrium halides, such as yttrium fluoride and yttrium chloride.

Oxidation States:

Yttrium is known to form several oxidation states, ranging from +1 to +7. Of these, +3 is the most common, owing to the element’s position in group 3 of the periodic table. The +3 oxidation state is also the most stable and is the one most often seen in nature.

Compounds:

Yttrium is known to form a wide variety of compounds, the most common of which are yttrium oxides and yttrium-containing salts. Yttrium oxides, such as yttrium oxide (Y2O3) and yttrium hydroxide (Y(OH)3), are widely used in many different industrial processes. They are also used as pigments and glazes in ceramic and glassmaking. Yttrium-containing salts, such as yttrium bromide (YBr3) and yttrium iodide (YI3), are used as catalysts in certain chemical reactions.

Yttrium is also known to form various yttrium-based alloys, such as yttrium-aluminum garnet (Y3Al5O12) and yttrium-iron garnet (Y3Fe5O12). These alloys are often used in the electronics industry, as they have excellent electrical properties. Yttrium is also used to strengthen steel, making it tougher and more resistant to corrosion.

In conclusion, the chemical properties of yttrium make it a very useful element. Yttrium can form a wide variety of compounds, alloys, and salts, which can be used in many different industrial processes. Its oxides and halides are also used in many applications, such as pigments, catalysts, and glazes. Yttrium is also used to strengthen steel, making it tougher and more resistant to corrosion.

 

Uses of Yttrium

Yttrium has many uses in various industries, from electronics to metals and alloys. It is a key component in a range of products from medical equipment to high-tech gadgets.

In electronics, yttrium is used in a variety of ways. It forms a component of the luminescent layer of liquid crystal displays, as well as being used to make magnets and other materials for semiconductor fabrication. For magnets, yttrium has the advantage of offering high coercivity, which is important for high-frequency applications. Yttrium is also used in a range of other electronic applications from microwave communication systems to imaging systems.

Yttrium is also used in the production of metals and alloys. Yttrium-based alloys are popular for their strength and light weight. These alloys are used in aircraft engines, automotive components, and fuel cells. Yttrium is also an important element for the production of superconductors, which have applications in the power grid and computer components.

Glassmaking is another major application for yttrium. Yttrium oxide can be used to produce a range of glass products, from optical lenses to fiber optics. It is also used in the production of special types of glass such as laser glasses, which are used in laser scanners and other imaging equipment. Yttrium-based glass is also used in medical equipment such as X-ray tubes and specialized lenses.

Yttrium has even been used in the production of fireworks and pyrotechnics. It can be used to create brilliant and colorful displays, and is often used in military applications for flares and other special effects.

Yttrium is a versatile and important element for many industries. Its various uses are constantly being explored and developed, and it is likely to remain an important element for years to come.

Interesting Facts

Yttrium is an element that has captured the interest of scientists and researchers for centuries due to its unique properties. As one of the transition elements, it is associated with a range of other elements in the periodic table, and this makes it a fascinating subject to study. Here are some interesting facts about yttrium:

Name Origin: Yttrium is named after the Swedish village of Ytterby, where it was first discovered. The element was discovered in 1787 by Carl Axel Arrhenius, a Swedish chemist and mineralogist.

Natural Occurrence: It is a naturally occurring element found in many minerals and ores, including monazite and bastnäsite. It is also found in trace amounts in some meteorites and lunar rocks.

Special Characteristics: Yttrium is a soft, silver-metallic element with a shiny surface. It has a relatively low melting point of 1522°C and a boiling point of 3345°C. It is also very malleable and ductile, and can be easily worked into different shapes for use in a range of applications.

Atomic Number and Weight: Yttrium has an atomic number of 39 and an atomic weight of 88.905. It is classified as a transition element and is part of the group of elements known as the rare-earth elements.

Melting and Boiling Points: Yttrium has a melting point of 1522°C and a boiling point of 3345°C. It is a relatively stable element, with a boiling point of one of the highest of all the rare-earth elements.

Density: Yttrium has a density of 4.47 g/cm3, which is higher than other rare-earth elements such as lanthanum and cerium.

Reactivity: Yttrium is a relatively nonreactive element. It is not reactive with air, water, or most acids and alkalis. It does, however, react with strong oxidizing agents and halogens.

Oxidation States: Yttrium has several oxidation states, from -1 to +4. It is most commonly found in the +3 state.

Compounds: Yttrium forms several compounds with other elements, including yttrium oxide, yttrium chloride, and yttrium nitrate. Yttrium-90 is a radioactive isotope commonly used in medical imaging and cancer treatments.

Uses of Yttrium: Yttrium is used in a variety of applications, from electronics to glassmaking. It is used as an alloying agent in stainless steel and other metals, and is also added to glass to give it additional strength and durability. It is also used in the manufacture of phosphors, which are used in fluorescent lighting, and other applications.

Applications in Electronics: Yttrium is used in many electronic applications, from semiconductors to fuel cells, and is an essential component of many modern electronics. It is often used in the manufacture of computer memory chips, and is also used in optical fibers.

Metals and Alloys: Yttrium is often added to other metals and alloys to enhance their properties. It is commonly used as an alloying agent in stainless steel, aluminium, and other alloys, and is also used in the manufacture of superalloys.

Glassmaking: Yttrium is used in the manufacture of speciality glasses, such as those used in optical fibers. It is also used in the manufacture of heat-resistant glassware, as well as glass with a high refractive index.

Safety Concerns: Yttrium is a toxic element, and handling it requires special precautions. It should be handled with gloves and protective eyewear, and its dust should not be inhaled.

Environmental Impact: Yttrium does not occur naturally in large concentrations in the environment, but is released into the environment through industrial activities. It can be toxic to aquatic life, and should be handled with care.

Toxicity: Yttrium is toxic when ingested, and can have serious effects on the human body. It can be absorbed through the skin, and can cause irritation and other symptoms, such as headaches, dizziness, nausea, and vomiting.

Handling Precautions: Proper precautions should be taken when handling yttrium. It should be kept in a dry, well-ventilated area, and should not be ingested. Protective clothing and eyewear should always be worn when handling the element.

These interesting facts about yttrium demonstrate why it is such an important element, with many diverse applications. It is an important element for a variety of industries, from electronics to glassmaking, and its special properties make it an essential component in many materials.

 

Safety Concerns

Yttrium is generally a non-toxic element, but it can be hazardous to health in its dust and compound forms. If inhaled, yttrium dust particles can irritate the respiratory system and cause inflammation, although the dust is not considered to be carcinogenic.

Long-term exposure to yttrium compounds, such as yttrium oxide, can also lead to breathing problems and skin irritation. To this end, it is important to take precautionary measures when handling yttrium compounds.

When it comes to the environment, yttrium is not considered to be a significant source of environmental pollution. It is not considered to be a hazardous waste and does not bioaccumulate in animals or plants. However, it is important to take measures to prevent yttrium from entering the environment, as it can have a detrimental effect on aquatic ecosystems.

Given its use in industrial processes, it is important to be aware of the potential risks and hazards associated with yttrium. It is important to take all necessary precautions to ensure safety when working with yttrium or yttrium-based compounds. Protective measures should include the use of protective clothing, gloves, goggles, and a face mask.

It is also important to ensure there are sufficient ventilation and exhaust systems, as well as adequate containment and disposal procedures for yttrium compounds.

It is also important to be aware of the storage requirements for yttrium and yttrium compounds. The compounds should be stored in a cool, dry place, away from direct sunlight and away from other toxic materials. Proper labeling and segregation should be used to ensure that yttrium is stored and handled correctly.

Finally, it is important to bear in mind that yttrium and its compounds are flammable. This means that all necessary safety measures should be taken to prevent fires and other accidents. It is important to use approved and suitable fire-fighting equipment in the event of a fire.

Overall, it is important to take necessary safety precautions when handling yttrium and its compounds. This includes the use of protective clothing and equipment, proper storage and containment, and suitable fire-fighting equipment. Taking these safety measures will help to ensure the safe handling and disposal of yttrium and its compounds.

 

Data

Yttrium
Pronunciation (IT-ree-əm)
Appearance silvery white
Standard atomic weight Ar°(Y)
  • 88.905838±0.000002
  • 88.906±0.001 (abridged)
Yttrium in the periodic table
Atomic number (Z) 39
Group group 3
Period period 5
Block   d-block
Electron configuration [Kr] 4d 5s
Electrons per shell 2, 8, 18, 9, 2
Physical properties
Phase at STP solid
Melting point 1799 K ​(1526 °C, ​2779 °F)
Boiling point 3203 K ​(2930 °C, ​5306 °F)
Density (near r.t.) 4.472 g/cm3
when liquid (at m.p.) 4.24 g/cm3
Heat of fusion 11.42 kJ/mol
Heat of vaporization 363 kJ/mol
Molar heat capacity 26.53 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1883 2075 (2320) (2627) (3036) (3607)
Atomic properties
Oxidation states 0, +1, +2, +3 (a weakly basic oxide)
Electronegativity Pauling scale: 1.22
Ionization energies
  • 1st: 600 kJ/mol
  • 2nd: 1180 kJ/mol
  • 3rd: 1980 kJ/mol
Atomic radius empirical: 180 pm
Covalent radius 190±7 pm
Other properties
Natural occurrence primordial
Crystal structure ​hexagonal close-packed
Speed of sound thin rod 3300 m/s (at 20 °C)
Thermal expansion α, poly: 10.6 µm/(m⋅K) (at r.t.)
Thermal conductivity 17.2 W/(m⋅K)
Electrical resistivity α, poly: 596 nΩ⋅m (at r.t.)
Magnetic ordering paramagnetic
Molar magnetic susceptibility +2.15×10−6 cm3/mol (2928 K)
Young's modulus 63.5 GPa
Shear modulus 25.6 GPa
Bulk modulus 41.2 GPa
Poisson ratio 0.243
Brinell hardness 200–589 MPa
CAS Number 7440-65-5
History
Naming after Ytterby (Sweden) and its mineral ytterbite (gadolinite)
Discovery Johan Gadolin (1794)
First isolation Friedrich Wöhler (1838)
Main isotopes Decay
abun­dance half-life (t1/2) mode pro­duct
87Y synth 3.4 d ε 87Sr
γ –
88Y synth 106.6 d ε 88Sr
γ –
89Y 100% stable
90Y synth 2.7 d β− 90Zr
γ –
91Y synth 58.5 d β− 91Zr
γ –
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Facts

Tellurium: A Rare Element With Unique Properties

by chemdude71

Tellurium is a rare chemical element with unique properties that make it a valuable resource in modern society. Discovered in 1782 by the chemist Franz Joseph Muller von Reichenstein, Tellurium remains one of the least abundant elements in the periodic table today.

This article will cover the unique properties of Tellurium and its various applications, as well as its sources and potential environmental impacts.

 

Introduction

Within the realm of chemical elements, Tellurium is classified as a non-metal. Its atomic weight is 127.6 g/mol, and it has a position in the periodic table at atomic number 52. This rare element is often compared to sulfur, selenium, and polonium due to its similarities in physical and chemical properties.

Tellurium is a silvery, brittle solid at room temperature. Its melting point is 722.66 degrees Celsius and its boiling point is 1,261 degrees Celsius. Its density is 6.24 g/cm3, and its electrical properties consist of a low electrical conductivity and high thermal conductivity.

Since its discovery, Tellurium has been used in a variety of industries. One of the most prominent applications of Tellurium is in electronics, particularly in cadmium telluride solar cells. Tellurium is also useful in metallurgy, as it strengthens and improves the properties of copper and stainless steel. Additionally, it is used in chemical production as a catalyst for manufacturing various compounds.

Despite its various uses, Tellurium remains a rare element and is mined from only a few select locations in the world. It is primarily extracted from copper and lead ore deposits and is synthesized in very limited quantities. The cost of Tellurium in the market depends on the amount of demand for the element and is usually quite expensive.

Tellurium is known to be toxic and is therefore subject to various regulations when used in industry. Potential health hazards associated with Tellurium include various respiratory and dermatological complaints. It is recommended that individuals who work with Tellurium wear protective clothing and use adequate ventilation, as exposure to the elements can cause adverse effects.

In conclusion, Tellurium is a rare element with unique properties that make it invaluable in many industries. Its physical and chemical properties make it a valuable resource in electronics, metallurgy, and chemical production. Despite its scarcity, its various applications necessitate its mining and synthesization.

It is important to be aware of the toxicity of Tellurium and to take the necessary precautions when working with the element.

Understanding the unique properties of Tellurium is essential to utilize this element to its fullest potential.

 

Chemical Properties

 

Atomic weight is an important parameter used to determine the chemical properties of any element. Tellurium has an atomic weight of 127.6, which places it in the category of non-metals. It is found in Group 16 (VIA) of the periodic table, and has the atomic number 52.

Tellurium is a brittle, silver-white solid at room temperature. Its melting point is 449°C, and its boiling point is 988°C, making it a relatively low-temperature element. It is also relatively dense, with a density of 6.24 g/cm3. Its electrical properties include a low resistivity and a high electron work function, which make it an excellent conductor of electricity.

Tellurium is an unusually stable element. It is resistant to oxidation and corrosion, and is not affected by acids, bases, or salt solutions. It is also highly stable at high temperatures, making it ideal for use in many industrial applications.

Tellurium is also unique in that it is the only element in its group that can form stable compounds with other elements. It can form compounds with the halogens, as well as sulfur, nitrogen, and carbon. These compounds are often used as catalysts or oxidizing agents in various industrial processes.

In addition, Tellurium is also an important catalyst in the production of drugs and other pharmaceuticals. It is used to catalyze chemical reactions, such as the synthesis of polymers, and is also essential in the production of certain antibiotics. It is also used as a catalyst in the production of organic chemicals, including plastics, rubber, and dyes.

 

Physical Properties

Tellurium belongs to the chemical element group, and it is a rare element. It has a wealth of unique physical properties that makes it desirable for certain applications.

The atomic weight of Tellurium is 127.6 amu, and it is classified as a non-metal. It is located in group 16 and period 5 of the periodic table.

Tellurium has a silver-white metallic luster, and its appearance can range from yellow to red. Its melting point is 449.51 °C, and its boiling point is 990 °C. It has a density of 6.24 g/cm3 at room temperature, and its electrical resistivity is 8.7×10-6 Ωm.

The physical properties of Tellurium make it highly desirable in certain applications due to its unique characteristics. For example, it is a very good conductor of electricity and heat, which makes it ideal for the electronics and metallurgy industries. Additionally, Tellurium can withstand extremely high temperatures, which makes it an ideal component in the chemical production industry.

Furthermore, Tellurium has a low vapor pressure, making it an ideal material for manufacturing corrosion-resistant alloys, as well as for use in catalysts and pigments. Finally, Tellurium is very stable in air, which makes it a useful material in the production of filaments and light bulbs.

In conclusion, Tellurium has a wealth of unique physical properties, which makes it a desirable material in a variety of industries. Its atomic weight, classification as a non-metal, and position in the periodic table are all important characteristics.

Additionally, its electrical properties, low vapor pressure, and stability in air make it an ideal material for the electronics, metallurgy, and chemical production industries.

 

Applications of Tellurium

Tellurium is widely used in many sectors due to its unique properties and composition. It is a relatively rare element, but offers many industrial and commercial advantages over other elements.

Its ability to form a number of alloys and its low toxicity makes it an attractive choice for many industries.

Uses of Tellurium in Electronics:

Tellurium is an important component in the electronics industry. It is used to produce semiconductors, which are essential components of electronic devices such as computers, cell phones, and other consumer products.

Tellurium is also used in the manufacture of transistors, which are commonly used in electronic circuits.

 

Uses of Tellurium in Metallurgy:

Tellurium is an important element in the production of steel and other metals. Tellurium-containing alloys are particularly durable and resistant to corrosion, making them ideal for use in machinery and other industrial applications.

Its ability to form alloys with other metals also makes it useful for producing specialized steel components.

 

Uses of Tellurium in Chemical Production:

Tellurium is commonly used in the production of various chemicals. It is used as a catalyst in the production of sulfuric acid, as well as in the production of rubber and plastics. It is also used as an additive in fuel production, as well as in the production of certain pharmaceutical drugs.

The attractiveness of Tellurium for various industrial applications is due in part to its low toxicity. It is considered a relatively safe element to use in comparison to other elements, making it a popular choice for many industries. Its ability to form a variety of alloys also makes it useful in the production of specialized components.

Its relatively low cost in comparison to other elements also makes it a cost-effective choice for the production of a variety of products.

 

Sources of Tellurium

Tellurium is a rare element, not found in its free state in nature. Thus, its presence is dependent on the availability of other elements and minerals.

Tellurium is found in the form of tellurides and can be found in minerals such as calaverite, sylvanite, and petzite. It is also a byproduct of copper, lead, and gold processing.

The main source of Tellurium is mining. It is obtained by the roasting of copper ore and then extracted from the crude ore. Mining is the most common method for extracting Tellurium and its compounds, it is used to remove the Tellurium from its ore. The Tellurium is then purified into one of its compounds.

Syntheses of Tellurium is also available, but the process of synthesizing Tellurium is expensive. Syntheses of Tellurium involves the use of high-temperature and high-pressure reactors to convert a range of elements into Tellurium. This process is often used in the production of semiconductors and other electronics.

Cost of Tellurium in the market can vary depending on the scarcity or abundance of the element. Prices have generally been rising due to the scarcity of Tellurium, but they have reached a certain level and have stabilized.

Prices will increase if demand for the element rises.

The availability of Tellurium is affected by a number of factors, such as the availability and cost of the source material, the location of the processing facilities, the cost of labor, and the cost of transport.

In addition, the availability of Tellurium is also affected by the environmental regulations set by governments.

The demand for Tellurium is increasing significantly due to its use in electronics, metallurgy, and chemical production. Thus, the cost of Tellurium is likely to remain high in the near future.

As the demand for Tellurium increases, so will the need for its sources and the cost of Tellurium.

 

Conclusion

Tellurium is a unique and rare element that has many unique properties and applications. Its atomic weight, classification as a non-metal, and position in the periodic table make it a fascinating element to study. Its appearance, melting and boiling points, density, and electrical properties also set it apart from other elements.

The uses of Tellurium in electronics, metallurgy, and chemical production are numerous, and its mining and syntheses help to ensure a steady supply of the element in the market. However, it is important to note that Tellurium is a toxic element and its usage must be regulated to protect the environment and public health.

In summary, Tellurium is an important element to study due to its unique properties and numerous applications. A comprehensive understanding of its properties can help to maximize its potential and minimize its risks. The benefits of understanding its properties are far-reaching and can help to usher in a new era of modern society.

 

Facts

Tellurium symbol is Te
Its atomic number is 52.
It is a brittle, mildly toxic, rare, silver-white metalloid
The element is named after the Latin tellus ‘earth'
Tellurium belongs to the chalcogen family of elements

Tellurium-bearing compounds were first discovered in 1782
Tellurium was first discovered by Franz-Joseph Müller von Reichenstein
Naturally occurring tellurium has eight isotopes.
Six of those isotopes, 120Te, 122Te, 123Te, 124Te, 125Te, and 126Te, are stable.
The other two isotopes, 128Te and 130Te, are slightly radioactive

It is found on Earth with nearly the same abundance as platinum.
Tellurium is usually found as calaverite, the telluride of gold
31 artificial radioisotopes of tellurium are known, with atomic masses ranging from 104 to 142
Tellurium has no biological function
Tellurium is far more common in the Universe than on Earth

In 2022, the major applications of tellurium were thin-film solar cells
In the 2020s, China produced about 50% of the world's tellurium
Tellurium and tellurium compounds are considered to be mildly toxic
In metallurgy, tellurium is added to iron, stainless steel, copper, and lead alloys
In 2022, the largest Te providers by volume were China, Russia, Japan, Canada, and Uzbekistan

The average annual price for 99.99%-pure tellurium was $74 per kilogram in 2018
The US Department of Energy has estimated that the demand for tellurium will cause a deficiency by 2025.
Amorphous tellurium is made by precipitating it from a solution of telluric acid.

 

Information

Tellurium
Pronunciation te-LURE-ee-əm
Appearance silvery lustrous gray (crystalline),
brown-black powder (amorphous)
Standard atomic weight Ar°(Te)
  • 127.60±0.03
Tellurium in the periodic table
Atomic number (Z) 52
Group group 16 (chalcogens)
Period period 5
Block   p-block
Electron configuration [Kr] 4d10 5s2 5p4
Electrons per shell 2, 8, 18, 18, 6
Physical properties
Phase at STP solid
Melting point 722.66 K ​(449.51 °C, ​841.12 °F)
Boiling point 1261 K ​(988 °C, ​1810 °F)
Density (near r.t.) 6.24 g/cm3
when liquid (at m.p.) 5.70 g/cm3
Heat of fusion 17.49 kJ/mol
Heat of vaporization 114.1 kJ/mol
Molar heat capacity 25.73 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) (775) (888) 1042 1266
Atomic properties
Oxidation states −2, −1, 0, +1, +2, +3, +4, +5, +6 (a mildly acidic oxide)
Electronegativity Pauling scale: 2.1
Ionization energies
  • 1st: 869.3 kJ/mol
  • 2nd: 1790 kJ/mol
  • 3rd: 2698 kJ/mol
Atomic radius empirical: 140 pm
Covalent radius 138±4 pm
Van der Waals radius 206 pm
Other properties
Natural occurrence primordial
Crystal structure ​trigonal
Speed of sound thin rod 2610 m/s (at 20 °C)
Thermal expansion 18 µm/(m⋅K) (at r.t.)
Thermal conductivity 1.97–3.38 W/(m⋅K)
Magnetic ordering diamagnetic
Molar magnetic susceptibility −39.5×10−6 cm3/mol (298 K)
Young's modulus 43 GPa
Shear modulus 16 GPa
Bulk modulus 65 GPa
Mohs hardness 2.25
Brinell hardness 180–270 MPa
CAS Number 13494-80-9
History
Naming after Roman Tellus, deity of the Earth
Discovery Franz-Joseph Müller von Reichenstein (1782)
First isolation Martin Heinrich Klaproth
Main isotopes
abun­dance half-life (t1/2)
120Te 0.09% stable
121Te synth 16.78 d
122Te 2.55% stable
123Te 0.89% stable[7]
124Te 4.74% stable
125Te 7.07% stable
126Te 18.8% stable
127Te synth 9.35 h
128Te 31.7% 2.2×1024 y
129Te synth 69.6 min
130Te 34.1% 8.2×1020 y
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Facts

Strontium: A Comprehensive Guide

by chemdude71

Strontium is an essential and abundant element found throughout the world. It is a chemical element in the periodic table with the atomic symbol Sr and atomic number 38.

Though it is not essential for human health, strontium is important for the development of living organisms. Strontium is used in a variety of industries and can be found in nature, synthetically produced, and even in isotopes.

In this comprehensive guide, we will explain the different types of strontium, the properties of strontium, the processing, production, and health effects of strontium, and the various applications of strontium.

 

Introduction

Strontium is a silvery-white metal that is very soft and malleable. It has an atomic mass of 88 and a density of 2.64 grams per cubic centimeter. Strontium is often found in nature as a component of different minerals and can be extracted from these.

It is also synthetically produced in a laboratory. Furthermore, there are a variety of strontium isotopes that can be produced, such as strontium-90, which is used in nuclear reactors.

The most common use of strontium is in the production of glass, electronics, and ceramics. It can also be used to make alloys and to strengthen metals. In addition to these industrial applications, strontium is used in medicine for its therapeutic benefits. It is commonly used to treat cancer and bone conditions such as osteoporosis. Strontium is also used in commercial products such as toothpaste, antacids, and fertilizers.

Though strontium has a variety of uses, it is important to understand the properties, processing, and production of strontium, as well as the potential health effects. In this comprehensive guide, we will discuss the different types of strontium, their physical and chemical properties, its processing and production, and the various applications of strontium.

We will also discuss the potential safety concerns and health effects associated with strontium. By the end of this guide, readers will have a better understanding of strontium and be able to make informed decisions about its use.

 

Types of Strontium

Strontium is an alkaline earth metal that can be found in nature in various forms. It's most commonly found in its mineral form, called strontianite, but it can also exist in an organic form or in compounds like strontium carbonate.

Some of the most common types of strontium include natural strontium, synthetic strontium, and its isotopes.

Natural Strontium

Natural strontium is the most commonly found form of the element and can be found in many minerals, such as strontianite, celestite, and strontium sulfate. It is also the form of strontium that is most often used in industrial applications.

It can be mined from the Earth or extracted from seawater or brines. Strontium can also be found in some plant and animal tissues in the form of strontium carbonate.

Synthetic Strontium

Synthetic strontium is a form of strontium that is artificially created in a laboratory. It is often used as a component of high-performance alloys, as well as in some medical devices and treatments. Synthetic strontium can also be used in nuclear reactors as a moderator or in nuclear weapons as a shield.

Isotopes of Strontium

Strontium has four naturally occurring isotopes—strontium-84, strontium-86, strontium-87, and strontium-88. These isotopes are all stable and non-radioactive, and they vary in their abundance in nature. Strontium-84 is the most abundant, accounting for about 82 percent of all naturally occurring strontium, followed by strontium-86 and strontium-88, which make up the remaining 18 percent. Strontium-87 is the least abundant and accounts for only 0.56 percent.

All of these isotopes have different properties, and they can be used for different purposes. For example, strontium-90 is used in medical treatments, and strontium-89 is used to treat bone metastases caused by prostate cancer. Strontium-90 is also used in nuclear reactors and nuclear weapons, and some isotopes are used in dating techniques to determine the age of rocks.

The different isotopes of strontium can also be used in a variety of industrial applications, such as in the production of glass, ceramics, and metals. Strontium also has many applications in the electronics industry, where it can be used to control the electrical properties of materials.

In conclusion, strontium is an alkaline earth metal that can exist in many forms, including natural, synthetic, and its isotopes. Natural strontium is the most common form and can be mined from the Earth or extracted from seawater or brines.

Synthetic strontium is artificially created in a laboratory and is used in high-performance alloys and medical treatments. There are also four naturally occurring isotopes of strontium, which all have different properties and applications.

 

Properties of Strontium

Strontium is an element with a wide range of unique properties that make it useful in a variety of applications. It has been used in industry for centuries, and scientists have learned a great deal about the properties of this element over the course of time.

This section will provide an overview of the physical, chemical, and reactivity properties of strontium, so that readers can get a better idea of what makes it such an important element.

Physical Properties of Strontium:

Strontium is a soft, silvery-white metal that has a relatively low melting point. It also has a relatively low density compared to other metals. Its atomic weight is 87.62 and it has an atomic number of 38.

Strontium is found in group 2 of the periodic table and it has an oxidation state of +2. Its symbol is Sr.

Chemical Properties of Strontium:

Strontium has a number of interesting chemical properties. It is a highly reactive element and can form a variety of compounds with other elements. Strontium is also a good conductor of electricity and heat.

It has low solubility in water, although it is slightly soluble in acids and alkalies.

Reactivity of Strontium:

Strontium is a very reactive metal and can react with both acids and bases. It is also able to form a variety of compounds with other elements. Strontium is also highly reactive when heated and can react explosively with chlorine and nitrogen.

The reactivity of strontium makes it useful in a number of industrial processes. It is used in pyrotechnics, fuel cells, and the production of special alloys. Strontium compounds are also used in the production of paints and ceramics.

Overall, strontium has a number of unique properties that make it a valuable element in a variety of industries. Its reactivity, low melting point, and low density make it a useful element in a wide range of applications.

 

Processing and Production

Strontium is a naturally occurring element that is found in the Earth’s crust. In order to extract, process, and produce products utilizing strontium, several steps must be taken.

This section will look at the detail of each step in the processing and production of strontium.

The process of extracting strontium begins with obtaining the necessary ore. The ore typically contains small amounts of strontium, so it needs to be concentrated. The common method for concentrating strontium is through froth flotation, which uses bubbles to separate the ore from the rock.

Once the ore has been extracted, it needs to be further processed. One of the main methods used to process strontium is through electrolysis. This involves passing an electric current through a solution of strontium salts, which separates the strontium from other elements. The resulting product is a strontium metal.

After the strontium has been processed, it needs to be produced into products. Depending on the purpose of the product, strontium can be further processed through a variety of methods. Strontium can be melted and cast into a variety of shapes and sizes. Strontium can also be combined with other metals to create alloys.

Strontium can also be used to create a variety of compounds. Strontium carbonate, strontium nitrate, and strontium sulfate are all common compounds of strontium. These compounds can be used in a variety of applications, such as in the production of ceramics, glass, and even pharmaceuticals.

Finally, strontium can be combined with other elements to create specialty products. Strontium can be combined with other metals to create magnets, or it can be combined with oxygen to create strontium oxide, which is used in a variety of colored glass products.

All of these methods are used to process and produce products using strontium. It is important to note that the safety of the products created from strontium depends on the application and how the element is used.

 

Health Effects of Strontium

The potential health effects of strontium have been studied for many years by scientists and medical professionals. This element is a relatively common constituent of the human body, and it has been found to be necessary for good health in certain circumstances.

Strontium is found in the bones and teeth of humans, where it is responsible for a number of metabolic processes that keep them strong and healthy. Strontium is also found in the soil, where it can be absorbed by plants and then enter the human body through food.

Strontium is an essential element for maintaining bone health. Research has shown that it can help increase bone density, which is important for avoiding osteoporosis. Strontium has also been found to help reduce pain and stiffness associated with osteoarthritis. Additionally, strontium can help reduce the risk of developing fractures, which is especially important for elderly individuals.

The safe levels of strontium exposure have been established by the Environmental Protection Agency (EPA). The EPA states that the average adult should not consume more than 0.7 milligrams of strontium per day. This level is considered to be safe for most adults, but it is still important to limit exposure to any other potential sources of the element.

Despite the generally accepted safe level of strontium exposure, there are still some potential health risks that can occur with higher levels of exposure. Studies have shown that long-term exposure to strontium can increase the risk of developing certain types of cancer, such as leukemia or lymphoma.

Additionally, high levels of strontium can interfere with the absorption of calcium, which can lead to weakened bones and an increased risk of fractures.

When it comes to strontium-related safety concerns, it is important to avoid consuming large amounts of strontium from dietary sources. Strontium can be found in some foods, such as green leafy vegetables, fish, and dairy products. It is also important to avoid drinking water that has been contaminated with strontium, as this can also cause health issues.

Finally, it is important to consider any potential interactions that strontium may have with other medications and supplements. Strontium can interact with certain medications, such as non-steroidal anti-inflammatory drugs (NSAIDs), and can also reduce the effectiveness of some vitamins and minerals.

As such, it is important to speak to a doctor or pharmacist before taking any new supplements.

 

Applications of Strontium

Strontium is a versatile chemical element with a variety of uses in industry, medicine, and commerce. Industrial applications of strontium include its use in nuclear reactors, as a component of glass, and in some fluorescent lights. In medicine, strontium can be used in the treatment of some types of cancer and to reduce pain associated with certain bone diseases. Commercially, strontium is used in a number of consumer products, including toothpaste and fireworks.

Industrial Uses of Strontium:

Strontium is an important element in the nuclear industry, where it is used as a component of nuclear reactor fuel. Strontium also helps to absorb neutrons released during the fission process, making it an important component in nuclear reactor design and operation.

Strontium is also used in the glass industry, where it helps to strengthen and improve the clarity of glass. Strontium is also used in some types of fluorescent lighting, where it helps to produce a more intense and even light.

Medical Uses of Strontium:

Strontium is also used in the medical field. It is used to treat certain types of cancer, such as leukemia, prostate cancer, and breast cancer. Strontium is also used to reduce pain associated with certain bone diseases.

Strontium has also been used in the treatment of osteoporosis, where it helps to increase bone mineral density.

Commercial Uses of Strontium:

Strontium is also used in a variety of consumer products. It is used in toothpaste, where it helps to reduce tooth sensitivity and improve the whitening effect of toothpaste. Strontium is also used in fireworks, where it helps to create intense and long-lasting colors in the night sky. Strontium has also been used in the manufacture of some types of paint pigments, providing vibrant colors.

Strontium is a versatile and versatile element that has a variety of uses in industry, medicine, and commerce. It is a key component in nuclear reactors, glass, and fluorescent lights and is also used to treat certain types of cancer and bone diseases.

It is also used in a variety of consumer products, including toothpaste and fireworks, as well as in the manufacture of some types of paint pigments. With its wide range of uses and applications, strontium is an important element in many industries.

Conclusion

In conclusion, strontium is a natural element that has a wide range of uses, both industrial and commercial. It has a number of different physical and chemical properties, as well as interesting reactivity in certain circumstances. Strontium can be extracted, processed, and produced into a variety of products with varying levels of concentration and safety.

Strontium has both positive and negative health effects, and its exposure should be limited to safe levels as recommended by experts in the field.

The industrial uses of strontium include its use in the production of color television or computer monitors, providing a reliable source of red phosphors. It can also be used in nuclear reactors to control the rate of fission, making it an essential component of the safety and efficiency of nuclear power plants.

Medical uses of strontium include its use in bone density scans and as an additive to medical bone implants to improve their strength and durability. Its commercial uses include its use in fireworks and paints, as well as its use as a dietary supplement.

Strontium is an important element and is used in a variety of applications, from industrial to medical and commercial. It is important to be mindful of its potential health risks and to limit its exposure as much as possible.

By understanding the various properties, uses, and potential health effects of strontium, individuals can make informed decisions about its usage and take the necessary precautions to remain safe.

This comprehensive guide has outlined the overview, benefits, and common uses of strontium, as well as the different types of strontium, their properties, and how they are processed and produced. It has also highlighted the potential health effects of strontium, as well as the various industrial, medical, and commercial uses of strontium.

Overall, strontium is a useful and important element with both positive and negative uses. It is important to use it responsibly and be mindful of its potential health risks. Further research into the effects of strontium on the environment, its long-term health effects, and possible alternative uses of the element can help inform decisions about its use and its proper management.

 

Facts

Strontium symbol is Sr
Its atomic number is 38
Strontium is a soft silver-white yellowish metallic element
It occurs naturally mainly in the minerals celestine and strontianite
Both strontium and strontianite are named after Strontian, a village in Scotland

The mineral was discovered in 1790 by Adair Crawford and William Cruickshank
Strontium was first isolated as a metal in 1808 by Humphry Davy
Natural strontium is a mixture of four stable isotopes: 84Sr, 86Sr, 87Sr, and 88Sr
88Sr makes up about 82.6% of all natural strontium
strontium-90 is radioactive and is one of the most dangerous components of nuclear fallout

Strontium is the 15th most abundant element on Earth
The three major producers of strontium as celestine as of 2015 are China, Spain, and Mexico
Strontianite is now known as strontium carbonite.
Strontium aluminate is frequently used in glow in the dark toys
Strontium carbonate and other strontium salts are added to fireworks to give a deep red colour

Strontium chloride is sometimes used in toothpastes for sensitive teeth.
There are sixteen known unstable isotopes of strontium.
It was used then to produce sugar from the sugar beet plant.
Around 300,000 tons of strontium are produced globally each year.
The drug strontium ranelate aids bone growth and increases bone density

The human body absorbs strontium as if it was calcium

Information

Strontium
Pronunciation

(STRON-tee-əm
Appearance silvery white metallic; with a pale yellow tint
Standard atomic weight Ar°(Sr)
  • 87.62±0.01
  • 87.62±0.01 (abridged)
Strontium in the periodic table
Atomic number (Z) 38
Group group 2 (alkaline earth metals)
Period period 5
Block   s-block
Electron configuration [Kr] 5s2
Electrons per shell 2, 8, 18, 8, 2
Physical properties
Phase at STP solid
Melting point 1050 K ​(777 °C, ​1431 °F)
Boiling point 1650 K ​(1377 °C, ​2511 °F)
Density (near r.t.) 2.64 g/cm3
when liquid (at m.p.) 2.375 g/cm3
Heat of fusion 7.43 kJ/mol
Heat of vaporization 141 kJ/mol
Molar heat capacity 26.4 J/(mol·K)
Atomic properties
Oxidation states +1, +2 (a strongly basic oxide)
Electronegativity Pauling scale: 0.95
Ionization energies
  • 1st: 549.5 kJ/mol
  • 2nd: 1064.2 kJ/mol
  • 3rd: 4138 kJ/mol
Atomic radius empirical: 215 pm
Covalent radius 195±10 pm
Van der Waals radius 249 pm
Other properties
Natural occurrence primordial
Crystal structure ​face-centered cubic (fcc)
Thermal expansion 22.5 µm/(m⋅K) (at 25 °C)
Thermal conductivity 35.4 W/(m⋅K)
Electrical resistivity 132 nΩ⋅m (at 20 °C)
Magnetic ordering paramagnetic
Molar magnetic susceptibility −92.0×10−6 cm3/mol (298 K)
Young's modulus 15.7 GPa
Shear modulus 6.03 GPa
Poisson ratio 0.28
Mohs hardness 1.5
CAS Number 7440-24-6
History
Naming after the mineral strontianite
Discovery William Cruickshank (1787)
First isolation Humphry Davy (1808)
Main isotopes
abun­dance half-life (t1/2)
82Sr synth 25.36 d
83Sr synth 1.35 d
84Sr 0.56% stable
85Sr synth 64.84 d
86Sr 9.86% stable
87Sr 7% stable
88Sr 82.6% stable
89Sr synth 50.52 d
90Sr trace 28.90 y

 

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Facts

Exploring The Properties And Uses Of Molybdenum

by chemdude71

Molybdenum is a chemical element with the symbol Mo and atomic number 42. It is a silvery-white transition metal that has been used in various industries since ancient times.

Molybdenum is one of the few elements that have both industrial and essential uses in human health and nutrition.

Molybdenum is classified as a member of the group 6 transition metals, which also includes chromium, tungsten, and manganese. It ranks as one of the moderately abundant elements in the Earth's crust.

The element is found in many minerals but is most commonly obtained from molybdenite, a mineral of molybdenum sulfide.

Introduction

Molybdenum has a relatively low melting point of 2617°C and a boiling point of 5560°C. It is a dense metal with a density of 10.2 g/cm3. It is also a relatively good conductor of electricity and heat, and it can form alloys with many other metals.

The chemical properties of molybdenum are quite unique. The element has the ability to absorb and form complexes with other elements and molecules, and it can act as a catalyst in certain chemical reactions. It can also form oxides and alloys with other metals, as well as form compounds with oxygen and nitrogen.

Molybdenum

The element has been used for thousands of years by various civilizations. Ancient Greeks used molybdenum to temper their steel, and the Romans used it to strengthen their armor and weapons.

In more modern times, molybdenum has found a variety of industrial uses, from its use in machinery to its use in aerospace engineering.

Molybdenum's importance to human health and nutrition has been known for centuries. It is an essential trace element that plays a vital role in human health, and deficiencies in molybdenum have been linked to a variety of health problems.

The element can be found in a variety of dietary sources, including leafy green vegetables, legumes, nuts and seeds.

This article will explore the properties and uses of molybdenum in detail. We will look at the element's chemical properties, its occurrence in nature, its role in human health and nutrition, its industrial uses, and its environmental effects.

We will also provide a summary of key points and our final thoughts on molybdenum.

 

Chemical Properties of Molybdenum

Molybdenum is a rare transition metal that is often found alongside other rare metals such as tungsten and chromium. It is an element with the atomic number 42, and is represented in the periodic table as Mo. Its atomic mass is 95.95 amu, and it is classified as a transition metal.

Molybdenum is known for its high melting point of 2,623°C and boiling point of 4,630°C, making it a valuable metal for industrial and commercial purposes. It has a density of 10.2 g/cm3 which makes it heavier than other metals, but still light enough to be manipulated easily.

Molybdenum has a crystal lattice structure that is hexagonal and close-packed in which its atoms are arranged in a 6-sided honeycomb pattern. This structure gives it strong binding capabilities and makes it difficult to corrode or degrade.

It is also malleable, ductile, and has a high tensile strength, making it ideal for use in machinery and industrial alloys.

The metallic element occurs primarily in sulfide ores, although it can also be found in ores containing molybdenum compounds. It is naturally found in many areas around the world, including the United States, Chile, Russia, Canada, and Australia.

Molybdenum is often used as an alloying agent in steels and other metals because it increases the hardness and lifetime of the metal while reducing its melting point. It is also used in the production of electronics, batteries, and nuclear reactors due to its high electrical conductivity and thermal conductivity.

Molybdenum is essential for human life, playing an important role in many body processes and enzyme reactions. It is found in trace amounts in certain foods such as nuts, legumes, and grains. It is also found in certain meats and is naturally produced in the gut of humans and animals.

In conclusion, Molybdenum is a valuable rare metal with many practical and industrial applications. It has a high melting point, a density of 10.2 g/cm3, and a crystal lattice structure that provides strong binding capabilities.

It is an essential element for human life, playing an important role in many body processes and enzyme reactions. It is found in trace amounts in certain foods and is naturally produced in the gut of humans and animals.

It is also an important alloying agent in steels and other metals, and is used in the production of electronics, batteries, and nuclear reactors due to its high electrical conductivity and thermal conductivity.

 

The Element in Nature

Molybdenum is a naturally occurring element and it is found widely distributed in the Earth's crust. While it is not abundant, it is more common than other elements like gold or platinum. It is a metal, and it is usually found in combination with other elements. Molybdenum is found as an oxide, sulfide, or silicate in various minerals.

When looking for Molybdenum in nature, one of the most common sources is molybdenite, which is a mineral composed mostly of molybdenum disulfide. This mineral is found in sedimentary and metamorphic rocks, particularly in areas where there has been magmatic-hydrothermal activity.

Molybdenum can also be found in other minerals such as wulfenite, powellite, and molybdite.

Molybdenum also has a geologic distribution that is distinct from other elements. It is most highly concentrated in the continental crust, with the highest concentrations typically found at mid-ocean ridges.

It is also abundant in some oceanic basalt and sediments, as well as in some continental basalt and sedimentary rocks.

In addition to its geologic distribution, Molybdenum is also found in different forms in different parts of the world. For example, it is found as an oxide in some areas, while in others it may be found as a sulfide. It is also found in a variety of different combinations with other elements, depending on the geologic environment in which it is found.

The abundance of Molybdenum in the environment also varies depending on the chemical and physical conditions in which it is found. Generally, it is more common in areas with a high pH level and a low temperature, such as in the oceans and in the Arctic. It is also more abundant in areas with higher levels of precipitation.

Overall, Molybdenum is a common element and is widely distributed in the environment. It is found in a variety of different minerals and in a variety of different geologic environments.

Its abundance in the environment is dependent on the chemical and physical conditions of its environment.

 

Molybdenum in Human Health and Nutrition

Molybdenum is an essential trace element for humans, playing an important role in human health and nutrition. It is an essential component of several important enzymes which are involved in cell functions and energy metabolism. Without enough molybdenum in the body, these processes cannot take place, leading to a range of health problems.

What role does it play in human health? Molybdenum plays a vital role in the functioning of a wide variety of enzymes, including xanthine oxidase, which is involved in breaking down purines, and sulfite oxidase, which is involved in breaking down the breakdown products of sulfur-containing amino acids. It also plays a role in transferring electrons in the mitochondria, assisting in the production of energy in the form of ATP.

Molybdenum is also important in the detoxification of sulfites, which are produced during the metabolism of sulfur-containing amino acids. It has been suggested that molybdenum helps in the breakdown of mercury and other heavy metals, and that it may be related to the prevention of some forms of cancer, although the evidence is inconclusive.

Sources of dietary molybdenum include many common foods, such as legumes, nuts, and grains. It is also found in tea, coffee, and chocolate. The daily recommended intake of molybdenum is 45 mcg per day for adults, and it is generally considered safe when consumed in amounts within this range.

Molybdenum deficiencies are rare, but they can occur in people with malabsorption disorders or with certain chronic medical conditions. Symptoms of molybdenum deficiency include anemia, growth retardation, and neurological problems. People who are at risk of deficiency should talk to their healthcare provider about supplementing with molybdenum, which is available in many forms, including tablets, capsules, and liquid solutions.

Overall, molybdenum plays a key role in human health and nutrition. It serves as an essential component of several important enzymes and helps to break down purines and sulfites. It also helps in the detoxification of metals and may be related to the prevention of certain types of cancer.

Molybdenum is found in a variety of foods, and deficiencies are rare, but people who are at risk should talk to their healthcare provider about supplementing with molybdenum.

 

Industrial Uses of Molybdenum

Molybdenum is an incredibly versatile element with many industrial uses, particularly in machinery, alloys, and aerospace. Due to its high melting point and low thermal expansion rate, it is an ideal material for high-temperature applications.

In its purest form, molybdenum is a silvery-white metal that is malleable and easily machined.

Uses in Machinery

Molybdenum is used in many different types of machinery. It is especially popular in automotive and aviation applications due to its strength and durability. It is often used to create valve seats and valve guides, as well as to form components of high-pressure pumps.

Molybdenum is also a key component in making precision tools, such as drill bits, lathe tools, and milling cutters.

Uses in Industrial Alloys

Molybdenum is also used in industrial alloys. It is a key component in stainless steel and other corrosion-resistant alloys. It is used in alloys to increase strength and reduce the risk of corrosion in a variety of applications.

Molybdenum is often added to copper alloys to increase their strength and resistance to corrosion. It is also used in iron alloys to reduce the risk of brittleness.

Uses in Aerospace

In the aerospace industry, molybdenum is used to create components that can withstand high temperatures and extreme pressures. Molybdenum is often added to titanium alloys to create a stronger and more heat-resistant material. It is also used in the manufacturing of aircraft turbine blades and jet engines, as well as spacecraft components.

Molybdenum is a key component in the production of many industrial products. It is used in a variety of applications to improve performance and durability. Its high melting point and low thermal expansion rate make it ideal for use in high-temperature applications.

Its strength and corrosion resistance also makes it well-suited for use in many types of alloys. Its versatility and durability make molybdenum an important element in the modern world.

 

Environmental Effects of Molybdenum

Molybdenum is the chemical element with atomic number 42 on the periodic table, and it has been known to have a number of industrial and environmental effects. The effects of molybdenum on the environment are both positive and negative, depending on the level of presence in the environment, as well as the use of the element.

Molybdenum, with its unique properties, can be used in a number of industrial processes, especially in the production and refining of metals. The element is also used in the production of sulfuric acid, which is a key component in the manufacturing of many products.

As a result, molybdenum can contribute to air pollution, water pollution, and soil contamination.

The presence of molybdenum in the environment can also affect the health of those who come into contact with it. In humans, molybdenum exposure can cause various health problems, such as nausea, headaches, dizziness, and a general feeling of malaise.

Long-term exposure to molybdenum can lead to an increased risk of cancer, reproductive issues, and other serious illnesses.

Molybdenum can also have a negative effect on plants and animals. The element has been found to be toxic to some species of aquatic life, and it can also reduce the growth of certain plants.

In addition, molybdenum can also cause the accumulation of other toxins in the environment, such as lead and cadmium.

The use of molybdenum in industrial processes is regulated in many countries, and the levels of molybdenum allowed in the environment are limited.

In addition, some countries have implemented rules and regulations on the use of molybdenum in order to protect the environment from the potential negative effects of the element.

Molybdenum is also used in some medical applications, and it can be used to prevent certain types of cancers and help treat other diseases. It has also been found to have antioxidant properties, which can help protect against certain types of diseases.

Although there is still much to learn about the effects of molybdenum on the environment, it is clear that it can have both positive and negative impacts.

In conclusion, molybdenum plays an important role in the environment, both in terms of industrial uses and its potential for environmental contamination. It is important for individuals and industries to understand the potential impacts of molybdenum on the environment, and to take necessary steps to minimize its impacts.

With careful management and research, we can ensure that molybdenum is used safely and effectively for the benefit of all.

Facts

Molybdenum is a chemical element with the symbol Mo
It has the atomic number 42
It is located in period 5 and group 6
The name is from Neo-Latin molybdaenum, which is based on Ancient Greek molybdos
The metal was first isolated in 1781 by Peter Jacob Hjelm

Molybdenum does not occur naturally as a free metal on Earth
There are 35 known isotopes of molybdenum, ranging in atomic mass from 83 to 117
Seven isotopes occur naturally, with atomic masses of 92, 94, 95, 96, 97, 98, and 100
Molybdenum-98 is the most abundant isotope, comprising 24.14% of all molybdenum
The free element, a silvery metal with a grey cast, has the sixth-highest melting point of any element.

During World War I, it was used both in armor plating and as a substitute for tungsten in high-speed steels.
Molybdenum is the 58th most abundant element in the Earth's crust with an average of 1.5 parts per million
Molybdenum is the 25th most abundant element in the ocean
It is the 42nd most abundant element in the Universe
The world's production of molybdenum was 250,000 tonnes in 2011

the largest producers being China, the United States, Chile, Peru and Mexico
The total reserves are estimated at 10 million tonnes
86% of molybdenum produced is used in metallurgy, with the rest used in chemical application
Molybdenum can withstand extreme temperatures without significantly expanding or softening
Molybdenum is also valued in steel alloys for its high corrosion resistance and weldability

Molybdenum had a value of approximately $30,000 per tonne as of August 2009
Molybdenum powder is used as a fertilizer for some plants, such as cauliflower
Molybdenum is an essential element in most organisms
At least 50 molybdenum-containing enzymes have been identified, mostly in bacteria
Molybdenum is an essential trace dietary element

The human body contains about 0.07 mg of molybdenum per kilogram of body weight
Molybdenum is also present within human tooth enamel and may help prevent its decay
Pork, lamb, and beef liver each have approximately 1.5 parts per million of molybdenum.
Other significant dietary sources include green beans, eggs, sunflower seeds, wheat flour, lentils, cucumbers, and cereal grain
Chronic exposure to 60 to 600 mg/m3 can cause symptoms including fatigue, headaches and joint pains.

At levels of 5000 mg/m3, molybdenum is immediately dangerous to life and health.
The Russian Luna 24 mission also discovered samples of molybdenum on the moon.

Information

Molybdenum
Pronunciation mə-LIB-də-nəm
Appearance gray metallic
Standard atomic weight Ar°(Mo)
  • 95.95±0.01
  • 95.95±0.01 (abridged)
Molybdenum in the periodic table
Atomic number (Z) 42
Group group 6
Period period 5
Block   d-block
Electron configuration [Kr] 4d5 5s1
Electrons per shell 2, 8, 18, 13, 1
Physical properties
Phase at STP solid
Melting point 2896 K ​(2623 °C, ​4753 °F)
Boiling point 4912 K ​(4639 °C, ​8382 °F)
Density (near r.t.) 10.28 g/cm3
when liquid (at m.p.) 9.33 g/cm3
Heat of fusion 37.48 kJ/mol
Heat of vaporization 598 kJ/mol
Molar heat capacity 24.06 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 2742 2994 3312 3707 4212 4879
Atomic properties
Oxidation states −4, −2, −1, 0, +1,[2] +2, +3, +4, +5, +6 (a strongly acidic oxide)
Electronegativity Pauling scale: 2.16
Ionization energies
  • 1st: 684.3 kJ/mol
  • 2nd: 1560 kJ/mol
  • 3rd: 2618 kJ/mol
Atomic radius empirical: 139 pm
Covalent radius 154±5 pm
Other properties
Natural occurrence primordial
Crystal structure ​body-centered cubic (bcc)
Speed of sound thin rod 5400 m/s (at r.t.)
Thermal expansion 4.8 µm/(m⋅K) (at 25 °C)
Thermal conductivity 138 W/(m⋅K)
Thermal diffusivity 54.3 mm2/s (at 300 K)
Electrical resistivity 53.4 nΩ⋅m (at 20 °C)
Magnetic ordering paramagnetic
Molar magnetic susceptibility +89.0×10−6 cm3/mol (298 K)
Young's modulus 329 GPa
Shear modulus 126 GPa
Bulk modulus 230 GPa
Poisson ratio 0.31
Mohs hardness 5.5
Vickers hardness 1400–2740 MPa
Brinell hardness 1370–2500 MPa
CAS Number 7439-98-7
History
Discovery Carl Wilhelm Scheele (1778)
First isolation Peter Jacob Hjelm (1781)
Main isotopes Decay
abun­dance half-life (t1/2) mode pro­duct
92Mo 14.7% stable
93Mo synth 4×103 y ε 93Nb
94Mo 9.19% stable
95Mo 15.9% stable
96Mo 16.7% stable
97Mo 9.58% stable
98Mo 24.3% stable
99Mo synth 65.94 h β− 99mTc
γ –
100Mo 9.74% 7.1×1018 y β−β− 100Ru
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Facts

A Comprehensive Guide To Niobium: Characteristics, Uses, And Benefits

by chemdude71

Niobium, an underrated element, has been used for decades in various industries, ranging from aerospace to medical and automotive applications. It is a chemical element and a transition metal with the symbol Nb and atomic number 41.

Niobium is a versatile element that is well-known for its corrosion resistance, magnetic properties, strength, and cost-efficiency.

Introduction

The first notable use of niobium was in 1801 when Charles Hatchett discovered it. He named the element columbium, but it was later renamed niobium in 1949 as the name columbium had already been used for another element.

Niobium is a silvery-grey metal that is soft, ductile, and malleable. It can be found in nature combined with other elements such as tantalum, zirconium, and thorium. It is also found in many ores, including niobite or columbite.

Niobium has an atomic number of 41 and atomic weight of 92.906. It has an oxidation state of +3 or +5 and a melting point of 2477°C.

The physical properties of niobium make it very attractive for a variety of applications. Its lightweight and high strength make it ideal for aerospace and automotive applications. It is also highly resistant to corrosion, making it well-suited for chemical and medical industries. Furthermore, it has low thermal neutron capture cross-sections, making it a suitable material for nuclear reactors and power plants.

Niobium has a variety of applications, making it an extremely useful element. It is used in the aerospace industry for rocket and airplane parts, as it is lightweight yet strong. It is also used in medical fields for surgical implants and prosthetics, due to its corrosion-resistant properties. Other applications for niobium include automotive parts, electronics, and steel production.

Niobium is also used in the form of superconductors, which are materials that can conduct electricity without any resistance. This makes them extremely energy-efficient and is the primary reason why niobium is used in this form.

It is also used in combination with other metals to produce alloys that are highly resistant to corrosion and have magnetic properties.

In conclusion, niobium is an underrated chemical element that has a wide range of uses and benefits. It has many physical properties that make it attractive for a variety of applications, such as aerospace, medical, and automotive uses. It is also used in forming alloys and superconductors that have corrosion-resistant and magnetic properties. Its strength and durability make it cost-effective and non-toxic, making it an optimal material for many industries.

 

Chemical Properties

Niobium is a chemical element with an atomic number of 41 and an atomic weight of 92.90638. It is located on the periodic table in the 5th group in the 5th period. It is a shiny, white-colored metal that is soft and ductile.

This element is best known for its corrosion resistance, magnetic properties, and its ability to be used as a superconductor.

The most common oxidation states of niobium are +2, +3 and +4. The melting point for niobium is 2477°C or 4491°F. The boiling point is 4744°C or 8571°F. At room temperature, niobium is brittle and fragile.

When heated, niobium is transformed into a ductile and malleable metal. It can also be alloyed with other metals such as iron, cobalt, nickel, and titanium. This allows niobium to be used in a variety of applications.

Niobium has an electronegativity that is comparable to iron, tin, and titanium. It also has a high thermal conductivity, electrical conductivity, and a low thermal expansion rate. Niobium also has a high tensile strength, making it an ideal material for use in aerospace applications.

Niobium is often used in alloys to increase strength and resistance to corrosion. It is also used in medical implants due to its non-toxic nature. It is commonly used in the automotive industry for lightweight components. Niobium is also used in electronics to increase the efficiency and performance of components such as transistors.

Niobium is a versatile chemical element that has a variety of uses and benefits. Its corrosion resistance, magnetic properties, and ability to be used as a superconductor make it an ideal material for a variety of applications. Its light weight and strength make it ideal for aerospace use, while its non-toxic nature makes it safe for medical applications.

Niobium is also cost-effective and can be easily alloyed with other metals to increase its strength and durability.

 

Applications

Niobium has a number of industrial uses that have been gaining in popularity over the last few decades. It is a highly versatile metal which makes it ideal for a wide range of applications in different industries. Here, we will take a look at the different ways that niobium is used across various industries.

Aerospace: Niobium is used in the aerospace industry as an alloying element. It is used to create lightweight, high-strength alloys which can be used in aircraft engines and other components. It also provides heat resistance and corrosion resistance which makes it ideal for these types of applications.

Medical: Niobium is used in medical applications such as implants and prosthetics. It is highly biocompatible, which makes it a great choice for medical applications. It is also non-toxic and lightweight, which makes it safe to use in the body.

Automotive: Niobium is used in automotive applications due to its ability to provide corrosion and heat resistance. It is used to create strong, lightweight alloys which can be used in car engines and other components. It is also used to create parts that are resistant to wear and tear.

Electronics: Niobium is used in the electronics industry due to its magnetic properties. It can be used to create coils and other components which can be used in a variety of different electronic applications. It is also highly conductive and provides a great deal of heat resistance, which makes it ideal for use in electronic components.

Niobium has a number of uses across various industries, which makes it a highly versatile and versatile metal. Its ability to provide corrosion and heat resistance, as well as its magnetic properties, make it a great choice for a wide range of applications.

 

Forming Niobium

Niobium is a chemical element with the atomic symbol Nb, atomic number 41, and an atomic weight of 92.906. It’s a soft, grey-white metal and, like many other metals, is found in nature in its elemental form.

There are two ways to isolate and form niobium: extraction and refining.

Extraction

Niobium is found in the form of ores, which are typically processed through pyrometallurgical extraction. This means heating and reducing the ore to its elemental form.

During this process, several other elements are also isolated and removed from the niobium ore. These elements can include iron, titanium, tantalum, and zirconium.

The second step of the extraction process is to separate the individual elements from the ore concentrate. This is accomplished through the use of a variety of solvent extraction and electrowinning techniques.

The final result of this process is a cold-pressed powder containing pure niobium.

 

Refining

The next step in forming niobium is to refine the ore concentrate. This is done using a variety of electrolysis and chemical processes such as the Hall-Heroult Process. This process creates a molten solution of niobium and impurities.

The impurities are then removed through a variety of filtration and purification techniques.

The final step of the refining process is to cast the niobium into ingots or bars in order to be used for a variety of purposes. This process is usually done in a vacuum furnace to ensure the highest quality product.

 

Alloying

Another way of forming niobium is by alloying it with other metals. This is done by adding other metals such as tantalum, titanium, or stainless steel to niobium ore. This creates a new material with different characteristics and properties.

Such alloys are used in the production of a variety of products such as aerospace parts, medical implants, and automotive parts.

Alloying niobium is also a great way to increase its strength and durability. This is because the addition of other metals creates a much stronger and more durable material than pure niobium.

There are a variety of ways to form niobium, but the most efficient and cost-effective methods are extraction and refining. These processes can be used to create a pure, cold-pressed niobium powder or a strong and durable alloy that can be used in a variety of applications.

 

Uses of Niobium

Niobium is a versatile element, offering a variety of uses across industries. Its unique physical and chemical properties make it a valuable component for a range of applications.

One of its most useful features is its ability to function as a superconductor. This means it can effectively carry and control electrical currents without any resistance. This property makes it ideal for use in advanced electrical motors, generators, and other electrical equipment.

Niobium also exhibits excellent corrosion resistance, which means it stands up well to harsh environments. This makes it a popular choice for medical implants, as well as for use in industrial and chemical processes.

Niobium also has some useful magnetic properties. This means that it can be used to create magnets that can be used in a range of devices, from refrigerators to electric motors.

In steel production, niobium can be used to strengthen the steel, making it more durable and resistant to corrosion. This makes it an invaluable resource for the automotive and construction industries.

Niobium can also be used to form alloys, which can be used to create a range of products. These alloys are often used to create items such as pipes and tubes due to their strength and durability.

Finally, niobium is also a very lightweight element, making it ideal for use in aircraft and other aerospace applications. The lightness of niobium makes it a popular choice for creating items such as propellers and turbines.

Overall, niobium offers a wide range of uses across a variety of industries. Its unique properties make it an invaluable element in the modern world. It is cost-effective, non-toxic, and durable, making it an ideal choice for many applications.

 

Benefits of Niobium

When it comes to benefits, there is no denying that niobium offers many advantages that make it an attractive option for many industries. Here are some of the main benefits of using niobium in various applications.

Strength and Durability: Niobium is a highly dense material which makes it incredibly strong and durable. It is an especially good choice for applications that require materials to be resistant to corrosion, wear, and tear, or any other environmental effects. Due to its impressive strength, niobium is also used for applications such as missile guidance systems and military vehicles.

Cost-Effective: Due to its abundance, niobium is an extremely cost-effective material. It is much cheaper than other materials such as titanium, which makes it an attractive option for many industries that require strong and durable materials at a lower cost.

Non-Toxic: Niobium is a non-toxic material which makes it safe for use in medical applications and other applications that require contact with the human body. It is also an environmentally friendly material that has no adverse effects on the environment.

Lightweight: Another advantage of niobium is its low weight. It is much lighter than other materials, such as steel, which makes it an ideal choice for applications such as aircraft and spacecraft parts where weight is a major factor.

These are just some of the main benefits of niobium that make it an attractive choice for many industries, such as aerospace, medical, automotive, and electronics. Its low cost, strength, and durability make it a great choice for many applications. It is also a non-toxic material which makes it safe to use in applications that need contact with the human body.

Finally, its lightweight nature makes it a great choice for applications where weight is a major factor. All of these benefits make Niobium an attractive option for many different industries.

Facts

Niobium is a chemical element with chemical symbol Nb
It has the atomic number 41
The name niobium was adopted internationally in 1950.
In 1801, Charles Hatchett discovered a new element in a sample of the ore columbite, and named it columbium.
The element was originally called columbium (symbol Cb).

The names ‘columbium’ and ‘niobium’ were both used to identify the element until 1949
There is only one known stable isotope of niobium, Nb-93.
The element name comes from ‘Niobe’ meaning daughter of Tantalus in Greek mythology.
Niobium is a lustrous, grey, ductile, paramagnetic metal in group 5 of the periodic table
Niobium becomes a superconductor at cryogenic temperatures

The metal takes on a bluish tinge when exposed to air at room temperature for extended periods
Niobium is estimated to be the 34th-most common element in Earth's crust, at 20 ppm
Minerals that contain niobium often also contain tantalum
By 2003, at least 32 radioisotopes had been synthesized, ranging in atomic mass from 81 to 113
The most stable is 92Nb with half-life 34.7 million years

The three largest currently mined deposits of pyrochlore, two in Brazil and one in Canada
Brazil produces about 88% of the world's supply.
The leading producer of niobium outside of Brazil is the Niobec Mine in Quebec, Canada.
Out of 44,500 tonnes of niobium mined in 2006, an estimated 90% was used in high-grade structural steel.
Niobium is considered a technology-critical element.

One of the most common niobium alloys is ferroniobium, where it is combined with iron.
Niobium is used in jewelry making because of its low level of toxicity.

Information

Niobium
Pronunciation ny-OH-bee-əm
Appearance gray metallic, bluish when oxidized
Standard atomic weight Ar°(Nb)
  • 92.90637±0.00001
  • 92.906±0.001 (abridged)
Niobium in the periodic table
Atomic number (Z) 41
Group group 5
Period period 5
Block   d-block
Electron configuration [Kr] 4d4 5s1
Electrons per shell 2, 8, 18, 12, 1
Physical properties
Phase at STP solid
Melting point 2750 K ​(2477 °C, ​4491 °F)
Boiling point 5017 K ​(4744 °C, ​8571 °F)
Density (near r.t.) 8.57 g/cm3
Heat of fusion 30 kJ/mol
Heat of vaporization 689.9 kJ/mol
Molar heat capacity 24.60 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 2942 3207 3524 3910 4393 5013
Atomic properties
Oxidation states −3, −1, 0, +1, +2, +3, +4, +5 (a mildly acidic oxide)
Electronegativity Pauling scale: 1.6
Ionization energies
  • 1st: 652.1 kJ/mol
  • 2nd: 1380 kJ/mol
  • 3rd: 2416 kJ/mol
Atomic radius empirical: 146 pm
Covalent radius 164±6 pm
Other properties
Natural occurrence primordial
Crystal structure ​body-centered cubic (bcc)
Speed of sound thin rod 3480 m/s (at 20 °C)
Thermal expansion 7.3 µm/(m⋅K)
Thermal conductivity 53.7 W/(m⋅K)
Electrical resistivity 152 nΩ⋅m (at 0 °C)
Magnetic ordering paramagnetic
Young's modulus 105 GPa
Shear modulus 38 GPa
Bulk modulus 170 GPa
Poisson ratio 0.40
Mohs hardness 6.0
Vickers hardness 870–1320 MPa
Brinell hardness 735–2450 MPa
CAS Number 7440-03-1
History
Naming after Niobe in Greek mythology, daughter of Tantalus
Discovery Charles Hatchett (1801)
First isolation Christian Wilhelm Blomstrand (1864)
Recognized as a distinct element by Heinrich Rose (1844)
Main isotopes Decay
abun­dance half-life (t1/2) mode pro­duct
91Nb synth 680 y ε 91Zr
92Nb trace 3.47×107 y β+ 92Zr
93Nb 100% stable
93mNb synth 16.12 y IT 93Nb
94Nb trace 20.4×103 y β− 94Mo
95Nb synth 34.991 d β− 95Mo
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Facts

All You Need To Know About Boron: A Comprehensive Guide

by chemdude71

Boron is a chemical element with the atomic number 5 and symbol B. First discovered in the early 19th century, it is a non-metal found in nature in different forms and compounds.

Boron is an essential element for plants, animals, and all living organisms on Earth. In addition, Boron has multiple industrial and medical applications.

Boron has several properties that give it many unique uses. It has a relatively low melting point, making it useful in metallurgy and construction. It also has low reactivity, making it a good electrical insulator.

Boron is also insoluble in water, making it valuable for a variety of chemical processes.

SONY DSC

Introduction to Boron

By weight, it is the 20th most abundant element in the universe. On Earth, it is found only in trace amounts in minerals, coal, and volcanic dust. Boron can be produced in the laboratory either by thermal decomposition of boron-containing compounds or through the electrolysis of boron halides.

Boron has several forms, including amorphous, crystalline, and metamorphic. Most crystalline forms of Boron have a metallic luster and are black or grayish in color. Amorphous Boron is a black, non-metallic powder with a high melting point. It is also insoluble in both water and oil.

Boron is found in many different minerals, such as borates, boron carbide, boron nitride, and boron hydride. It is also found in trace amounts in some types of seawater and fossil fuels.

Boron also has many medical uses. It is necessary for the proper formation and growth of bones, teeth, and other body tissues. It also plays an important role in cognitive function and is essential for healthy nerve cells.

In addition to its medical applications, Boron has a wide variety of industrial uses. It is used in metallurgy and ceramics, as well as in the production of plastics and carpentry.

Boron is also an environmental pollutant, with the potential for serious health risks to humans and other living organisms. It is released into the atmosphere through the burning of fossil fuels and can have toxic effects on humans and animals. It is important to be aware of the potential environmental impacts of Boron and to monitor and regulate its use.

In summary, Boron is an essential element for all life forms on Earth. It has unique properties that make it useful for a variety of applications, from medical to industrial.

It is important to be aware of the potential environmental impacts of Boron and to monitor and regulate its use.

 

Physical and Chemical Properties of Boron

Boron is an element found in nature that has a variety of physical and chemical properties. Boron is an atomic element with the symbol B and an atomic number of five.

It is located in Group 13 of the periodic table and is classified as a metalloid. Boron has a variety of unique properties that make it useful in a variety of industrial and medical applications.

Boron has a melting point of 2076 degrees Celsius and a boiling point of 3927 degrees Celsius. Its density is 2.37 grams per cubic centimeter and its electronegativity is 2.04 on Pauling’s scale. Boron is an extremely hard element and has high thermal and electrical conductivity. It is also resistant to corrosion and oxidation.

Boron is found in a variety of compounds and forms, including borates, boron carbide, boron nitride, and boron hydride. Borates are a group of compounds containing boron and oxygen. They are typically solid at room temperature and are used in a variety of industrial and medical applications.

Boron carbide and boron nitride are both extremely hard materials and are used in the production of abrasives and refractory materials. Boron hydride is a colorless gas with a pungent odor. It is used in the production of rocket fuels and explosives.

Boron is found in a variety of natural and synthetic sources. Natural sources include coal, oil, and seawater. Boron is also found in soil in the form of borate minerals. Synthetic sources of boron include boron-containing compounds such as boric acid and borates. Boron is also found in meteorites and other extraterrestrial rocks.

Boron is an important element in the human body and is essential for normal bone health and cognitive function. Boron deficiency has been linked to a number of health risks, including bone loss and cognitive decline. Boron supplements are available to help people get the recommended daily intake of boron.

Boron has a variety of industrial uses. It is used in metallurgy, ceramics, carpentry, plastics, and other manufacturing processes. Boron compounds are also used as catalysts in the production of polymers, fuel cells, and semiconductors.

Although boron is an important element in many industrial and medical applications, it can be toxic when released into the environment. It can be found in the atmosphere as a pollutant from industrial processes and can be toxic to humans.

It can also cause toxic effects in plants and animals, and is highly soluble in water, making it difficult to remove from water sources.

In conclusion, boron is an important element with a variety of physical and chemical properties. It has a variety of industrial and medical uses, and its compounds can be found in natural and synthetic sources. Boron is essential for normal bone health and cognitive function but can be toxic when released into the environment.

Understanding boron’s physical and chemical properties is important for making safe and effective use of this essential element.

 

Common Compounds of Boron

Boron is an element composed of several compounds, some of which are more commonly used than others. A few of the most common boron compounds include Borates, Boron Carbide, Boron Nitride, and Boron Hydride. Let's take a look at each of these common boron compounds.

Borates are a family of inorganic compounds that contain boron and oxygen. They are used in a wide variety of applications, including fertilizers, detergents, and flame retardants. Borates are also used in the production of ceramics and glass, as an ingredient in enamels, and as a preservative in insecticides.

Boron Carbide is a refractory ceramic material composed of boron and carbon. It is one of the hardest materials known, making it ideal for industrial applications such as abrasives, sandblasting, and polishing. It is also used in armor plating and in the production of nuclear reactors.

Boron Nitride is an inorganic compound composed of boron and nitrogen. It is used in cosmetics, as a lubricant, as a fire retardant, and as a non-stick coating in cookware. It is also used in the production of nanotubes, which are made of pure boron nitride.

Boron Hydride is a compound composed of boron and hydrogen. It is used as a fuel source, as a reducing agent, and in the production of lithium batteries. It is also used in the production of semiconductors, as a catalyst in organic chemistry, and as a lubricant for machined parts.

These are just a few of the common boron compounds used in modern industry. Each of these compounds has unique and useful properties that make them indispensable in various technological and industrial applications. It is clear that understanding the compounds of boron is essential to understanding its importance to modern society.

 

Sources of Boron

Boron is an abundant element on Earth and a wide variety of sources can be found in both natural and synthetic forms. Natural ores are found in rocks and minerals while synthetic ores are derived from chemical processes. In addition, boron is also present in the sun and other celestial bodies.

Natural Ores: Boron can be extracted from a variety of natural ores, including the borate minerals borax, colemanite, and ulexite. These minerals are often found in deposits formed from the evaporation of lake beds and hot springs and are then mined as a source of boron.

Synthetic Ores: Borates can also be manufactured by combining boric acid with an alkaline compound. This process is often used to create a more concentrated form of boron ore for use in industry.

Solar System Ores: Boron can also be found in many interplanetary bodies, such as asteroids and comets. In addition, boron is present in the sun and other stars and is believed to have been created during the formation of the solar system.

Boron is an essential element and is widely used in a variety of industries. Its availability from natural and synthetic sources makes it an ideal choice for a range of applications. In addition, boron's presence in celestial bodies provides a unique opportunity to study its role in the formation of the universe. As a result, boron is one of the most important elements in the periodic table.

 

Health Benefits of Boron

Boron has numerous health benefits that have been studied for decades. This mineral plays an important role in bone health, cognitive function, and metabolism. Here we are going to discuss all the health benefits of boron in detail.

Bone Health

Boron is essential for bone structure and strength. It helps in the absorption of calcium by the body, which is essential for the growth of healthy bones.

A deficiency of boron can lead to weak bones, osteoporosis, and an increased risk of fractures. Studies have found that when boron is added to a diet deficient in calcium, it helps in increasing bone density.

It also helps in preventing bone loss due to osteoporosis. Some studies have even found that boron supplementation can reduce the risk of hip fracture in elderly people.

Cognitive Function

Boron also plays an important role in cognitive function. It helps in the proper functioning of the brain and can improve concentration and focus.

Studies have found that boron can help improve memory and has a positive effect on cognitive performance. It has also been found to reduce aggression and anxiety.

Metabolism:

Boron is also crucial for the metabolism of other vitamins and minerals like calcium, magnesium, and vitamin D. It helps in the absorption of these essential vitamins and minerals into the body, which are crucial for many bodily functions.

Boron helps in regulating the levels of calcium and magnesium in the blood, which can help in preventing bone loss and improve overall health.

Deficiency:

Boron deficiency is rare but can lead to serious health problems if left untreated. Symptoms of boron deficiency include weak bones, impaired cognitive function, fatigue, and depression.

It is important to ensure that you get enough boron in your diet to prevent these health problems.

Supplementation:

Boron supplementation is recommended for those who are deficient in this mineral. Boron supplements are available in many forms, including capsules, tablets, and liquid extracts. These supplements can be taken daily to meet your daily boron needs. It is important to consult a doctor before taking any supplements as they can interact with other medications.

In conclusion, boron plays an important role in both keeping our bodies healthy and helping in many industrial processes. It is essential for bone health, cognitive function, and metabolism. It is important to ensure that you get enough boron from your diet or through supplementation. Boron deficiency can lead to serious health problems, so it is best to take the necessary precautions.

 

Industrial Uses of Boron

Boron is a versatile element that has a multitude of uses in industrial settings. Over the last century, boron has been used in a variety of industries, from metallurgy to carpentry. This element is essential for a large number of products, both in its elemental form and in its compounds. Here, we’ll explore the various industrial uses of boron.

Metallurgy: Boron is widely used in metallurgy, as it can be used to strengthen alloys and to improve their machinability. Boron-alloyed steels are often used in the aerospace and automotive industries, as they are both strong and light. Boron-alloyed steels are also used in the construction and agricultural industries.

Ceramics: Boron is used in the production of borosilicate glass, an extremely durable and heat-resistant material used for many applications, including cookware and laboratory equipment. In addition, boron is used to produce enamels and glazes, which are often used to decorate ceramics.

Carpentry: Boron is used in the production of plywood, as it adds strength and durability to the product. This type of plywood is resistant to water damage and is widely used in the construction of homes and furniture.

Plastics: Boron is often used in the production of polymers, as it can improve the strength and flexibility of the product. In addition, boron can be used to produce flame-retardant plastics, which are often used in the automotive and aerospace industries.

These are just a few examples of the industrial uses of boron. This versatile element is essential for a wide variety of products, and its uses are constantly expanding. From metallurgy to plastics, boron is an important part of the modern industrial world.

 

Environmental Impact of Boron

Boron is a naturally occurring element in the periodic table, found in many ores on Earth. It has a wide variety of uses and is found in many everyday products. While it is a necessary element, boron can also have a negative impact on the environment.

Boron pollution is a major environmental concern. It is often found in emissions from industrial processes, such as mining and smelting, as well as in waste from the burning of fossil fuels. Boron can also become an air pollutant through wind currents, or when it is released from factories.

Toxic effects of boron on humans can include eye and skin irritation, respiratory problems, and nausea. These effects can occur when air particles containing boron are breathed in. Long-term exposure can also cause damage to the liver and kidneys.

The presence of boron in the atmosphere can also lead to pollutants such as ozone, sulfur dioxide, and carbon dioxide. These pollutants can contribute to climate change and cause air pollution.

Boron pollution can also have a negative impact on water sources. When boron finds its way into rivers or lakes, it can become toxic to fish and other wildlife. It can also cause water contamination, making it unsafe for humans to drink.

In addition to the environmental hazards of boron pollution, it can also disrupt the balance of ecosystems. This can lead to a decrease in biodiversity and a decrease in productivity in certain areas.

Though boron can be a danger to the environment, it is also an essential element for many industrial processes and everyday products.

Proper management of boron is essential to ensure it is not damaging to the environment. By adhering to proper safety protocols and regulations, the environmental hazards associated with boron can be minimized.

 

Facts

Boron is a chemical element with the symbol B
Its atomic number 5.
The word boron was coined from borax
Borax in its mineral form first saw use as a glaze, beginning in China circa 300 AD
It constitutes about 0.001 percent by weight of Earth's crust.

Boron was not recognized as an element until it was isolated by Sir Humphry Davy and by Joseph Louis Gay-Lussac and Louis Jacques Thénard.
Boron is a solid at room temperature.
Boron is a period 2 chemical element, which is the second row on the periodic table.
Boron is a group 13 chemical element.
Boron has two stable isotopes.

The two stable isotopes are 11B and 10B.
Boron melts at 2075 °C (3767 °F), and boils at 4000 °C (7232 °F).
Boron is the lightest element having an electron in a p-orbital in its ground state.
Boron is mined from borate minerals found in the Earth’s crust.
Boron is used in fireworks and pyrotechnics to give a green color to the flares.

50% of the boron used annually is for insulation and structural materials.
Boron has the highest melting and boiling point of all the metalloids on the periodic table.
Boron oxide is used in glassmaking and ceramics.
Boron is available both in Amorphous form and Crystalline form.
Boron carbide is used in tank armor and bullet proof vests.

There are at least 100 minerals where you will find Boron.
Boric acid is an insecticide used against cockroaches, ants and fleas.
Plants need boron to help maintain the integrity of their cell walls.
Turkey produces about half of the global yearly demand
Turkey and the United States are the largest producers of boron products

23% of global boron production comes from the single Rio Tinto Borax Mine
boron is used as a dopant for semiconductors like silicon, silicon carbide and germanium.

Information

Boron
Pronunciation BOR-on
Allotropes α-, β-rhombohedral, β-tetragonal (and more)
Appearance black-brown
Standard atomic weight Ar°(B)
  • [10.806, 10.821]
  • 10.81±0.02 (abridged)
Atomic number (Z) 5
Group group 13 (boron group)
Period period 2
Block   p-block
Electron configuration [He] 2s2 2p1
Electrons per shell 2, 3
Physical properties
Phase at STP solid
Melting point 2349 K ​(2076 °C, ​3769 °F)
Boiling point 4200 K ​(3927 °C, ​7101 °F)
Density when liquid (at m.p.) 2.08 g/cm3
Heat of fusion 50.2 kJ/mol
Heat of vaporization 508 kJ/mol
Molar heat capacity 11.087 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 2348 2562 2822 3141 3545 4072
Atomic properties
Oxidation states −5, −1, 0,+1, +2, +3 (a mildly acidic oxide)
Electronegativity Pauling scale: 2.04
Ionization energies
  • 1st: 800.6 kJ/mol
  • 2nd: 2427.1 kJ/mol
  • 3rd: 3659.7 kJ/mol
  • (more)
Atomic radius empirical: 90 pm
Covalent radius 84±3 pm
Van der Waals radius 192 pm
Other properties
Natural occurrence primordial
Crystal structure ​rhombohedral
Speed of sound thin rod 16,200 m/s (at 20 °C)
Thermal expansion β form: 5–7 µm/(m⋅K) (at 25 °C)
Thermal conductivity 27.4 W/(m⋅K)
Electrical resistivity ~106 Ω⋅m (at 20 °C)
Magnetic ordering diamagnetic
Molar magnetic susceptibility −6.7×10−6 cm3/mol
Mohs hardness ~9.5
CAS Number 7440-42-8
History
Discovery Joseph Louis Gay-Lussac and Louis Jacques Thénard (30 June 1808)
First isolation Humphry Davy (9 July 1808)
Main isotopes Decay
abun­dance half-life (t1/2) mode pro­duct
10B 19.65% stable
11B 80.35% stable
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Facts

Bismuth: A Chemical Element With Surprising Characteristics

by chemdude71

Bismuth is a chemical element with the symbol Bi and atomic number 83. It is the heaviest element in the carbon family and is one of the few non-toxic elements.

It is frequently classified as a semi-metal or metalloid but has some unique characteristics that make it stand out from other elements in its group.

Bismuth has a variety of properties that make it both practical and interesting to study. Its atomic number is 83, placing it in the middle of the periodic table, and it's melting and boiling points are surprisingly low compared to other elements in its group.

It is also relatively dense for its size and has some interesting chemical properties. Bismuth has a low thermal conductivity, making it a desirable material in many applications.

Wismut (Bi) Kristalle oxidfrei

Introduction

When it comes to its uses, bismuth has been employed in a variety of industries. It is a key component in lead-free solder, which is often used in electrical wiring and plumbing. It is also used in metallurgy, nuclear reactors, cosmetics, and pharmaceuticals. Bismuth has a wide range of applications, making it a valuable element in many industries.

The history of bismuth is just as fascinating as its properties and applications. It was first discovered in the 15th century and was named after the German word for “white mass” due to its unique color. Since then, bismuth has been used in many early industrial applications and continues to play a role in the modern world.

There are also some interesting facts about bismuth. It is one of the few non-toxic elements, meaning it is generally safe to ingest. The color of bismuth compounds can vary depending on the compound, and it has the lowest thermal conductivity of any element.

When it comes to health effects, bismuth is generally accepted as safe to ingest. However, there are potential side effects and risks associated with high levels of bismuth intake. Therefore, it is important to take safety precautions when handling bismuth and use it in accordance with the recommended guidelines.

Bismuth is certainly an interesting chemical element with many surprising characteristics. From its properties and applications to its history and health effects, bismuth has much to offer and deserves further exploration.

 

Properties of Bismuth

Bismuth is a chemical element that has a series of unique and interesting characteristics. Its atomic number is 83, and it is positioned in group 15 in the periodic table. Bismuth has a unique allotrope, which is an arrangement of its atoms, and also has a relatively low melting and boiling point.

It has a very low density when compared to other metals, and its strength is lower than many of its counterparts.

When it comes to the physical properties of bismuth, it has a lustrous white color that tarnishes slowly and is soft enough to be cut with a knife.

Bismuth has an unusual crystal structure, which helps to contribute to its low thermal conductivity. Its malleability and ductility are also quite low when compared to other metals.

Bismuth has a wide range of chemical properties. It is a brittle, lustrous metal that is notable for its considerable reactivity with both oxygen and water. It is also highly resistant to acids, but can be attacked by concentrated nitric and sulfuric acids. Bismuth is also one of the few elements that is non-toxic.

Not only is bismuth unique in its chemical and physical properties, but it also has many uses and applications. In metallurgy, bismuth is used in various alloys to help reduce the melting points of other metals. It is also used in nuclear reactors to help control corrosion and the accumulation of neutron radiation. It is also commonly used in the production of lead-free solders, and it has been used in cosmetics and pharmaceuticals.

Bismuth is an element that has been known and used for centuries. It was first discovered and named in the 15th century by Georgius Agricola, although its existence in nature was known long before that.

In the 19th century, bismuth began to be used in industrial applications such as lead-free solders and alloys. Since then, its use has continued to expand as more applications and uses have been discovered.

Bismuth also has some surprising characteristics. It has a relatively low melting and boiling point compared to other metals, and it has one of the lowest thermal conductivities of any metal. It is also one of the few non-toxic elements, making it safer to handle and use than many of its counterparts.

Bismuth is generally accepted as safe to ingest, though there are potential risks and side effects associated with its use. It is also important to take caution when handling bismuth, as it is highly reactive and can be attacked by various acids.

In conclusion, bismuth is a chemical element with a series of unique and surprising characteristics. It has a low melting and boiling point, a low density, and one of the lowest thermal conductivities of any metal. It has many uses and applications, including in metallurgy and alloys, nuclear reactors, lead-free solders, cosmetics, and pharmaceuticals.

Though generally safe to ingest, it is important to take caution when handling bismuth, as it is highly reactive and can be attacked by various acids.

 

Uses and Applications of Bismuth

Bismuth is a chemical element found naturally throughout the world that has many interesting and important uses. A main characteristic of bismuth is its low melting point and low boiling point, which make it a versatile material for many applications.

Bismuth has a wide range of uses and applications that span from metallurgy and nuclear reactors to cosmetics and pharmaceuticals.

In metallurgy and alloys, bismuth is used primarily to create low-temperature alloys with other metals or elements. It is commonly added to tin, lead, and other metals to make them less brittle and easier to form.

Bismuth has a low melting point, and when added to other metals it is much easier to shape and form them. This makes bismuth an ideal choice for creating alloys for commercial use in the production of various products.

Bismuth is also widely used as a neutron absorber in nuclear reactors. This is due to its ability to absorb neutrons from the reactor core, thereby allowing for better control over the reactor’s temperature and power. Additionally, it can be used to help slow the rate of a nuclear chain reaction.

Lead-free solder is another important use for bismuth. It is often used as a substitute for lead in solders due to its non-toxic properties and low melting point. This makes bismuth a safer alternative for use in electrical and plumbing applications, where lead solder is not recommended.

Bismuth is also found in a variety of cosmetics, such as eye shadow, blush, lip gloss, and mascara. It provides a soft, shimmery look to these products. Its low melting point also helps keep the product from melting on the skin.

Finally, bismuth is used in a variety of pharmaceuticals. Bismuth subsalicylate, which is found in Pepto-Bismol and other medications, is a common form of bismuth used to treat stomach ailments such as diarrhea and nausea. Bismuth is also used in some antibiotics to help treat gastrointestinal tract infections and Helicobacter pylori.

These are just some of the many uses and applications of bismuth. Its unique chemical properties make it a versatile and useful element in many industries.

From its use in alloys to its role in pharmaceuticals, bismuth is an element that has a variety of surprising and beneficial applications.

 

History of Bismuth

The element bismuth, with the atomic number 83, was discovered and named in 1753 by the French chemist Claude François Geoffroy. Prior to this, bismuth was mistakenly thought to be either lead or tin. It was not until 1789, when Antoine Lavoisier formally classified bismuth as an element, that it was fully understood and accepted.

During the Industrial Revolution, bismuth was heavily used in metallurgical processes such as refining copper and the production of brass and bronze. Its use decreased in the early 20th century, however, when it was replaced by other elements such as lead.

In the modern era, bismuth is used primarily in nuclear reactors. It is also used in lead-free solders, in cosmetics, and in pharmaceuticals. Bismuth is known for its slow-acting and long-lasting effects, so it is an ideal choice for medical applications.

The compound bismuth oxide (Bi2O3) is produced from ore bismuthinite and is used in the production of certain glass and ceramic colors. Bismuth oxychloride, in turn, is used in cosmetics such as blushes and eyeshadows.

Bismuth is also a key component of many alloys, including bismuth-tin alloys for electrical contacts and bismuth-antimony alloys for typecasting and plastic molding. These alloys have much lower melting points than pure bismuth, making them easier to handle and shape.

Bismuth is also used in industrial catalysts, in which it helps to remove sulfur and nitrogen compounds from exhaust gases. Its low toxicity makes it an ideal choice for catalytic converters.

Finally, bismuth is also used in the production of radiation-shielding materials such as lead-bismuth eutectic alloys. These alloys are used in medical applications such as protecting patients from radiation exposure during medical imaging and in nuclear power plants.

In conclusion, bismuth has a long and varied history. It was discovered and named in 1753 and has since been used in metallurgy and alloys, nuclear reactors, lead-free solder, cosmetics, pharmaceuticals, industrial catalysts, and radiation-shielding materials. It's varied properties and low toxicity make it a versatile and valuable element.

 

Interesting Facts About Bismuth

Bismuth is an amazing and surprising chemical element, with a wide range of applications and interesting facts. One of the most interesting facts about this element is that it is one of the few non-toxic elements. This means that it can be ingested in small doses with no adverse health effects.

Another interesting fact about bismuth is the color of its compounds. While its pure form is a silvery-white metallic color, the compounds of bismuth are some of the most colorful in the world. This is due to the presence of bismuth oxychloride and other bismuth compounds, which can range from a pink hue to bright blues and greens.

Bismuth also has the unique distinction of having the lowest thermal conductivity of any metal. This means that it is an effective insulator, able to retain heat and keep it from traveling. This makes it ideal for use in the construction of insulating materials.

When it comes to its physical properties, bismuth has an atomic number of 83, and is a chemical element in the periodic table. In its solid form, its boiling point is 544.7°C and its melting point is 271.3°C. Bismuth also has a density of 9.78 grams per cubic centimeter. Additionally, it is one of the few metals that is not affected by air or water.

Bismuth also has some interesting chemical properties. It is an element that is highly reactive, and can easily form a variety of compounds. It has a high affinity for oxygen and sulfur, and it can form complexes with many other elements. This makes it a versatile and essential element for a wide range of applications.

In conclusion, bismuth is a unique and surprising element with a wide range of properties and applications. Its non-toxic nature makes it safe to ingest in small doses, and its low thermal conductivity makes it an effective insulator. Its impressive chemical properties give it a wide range of uses, and its compounds offer a multitude of colors.

While it can be dangerous to handle in large quantities, bismuth is an essential and versatile element that is essential to the modern world.

 

Health Effects of Bismuth

Bismuth is generally accepted as safe to ingest, making it a useful element in many pharmaceuticals. In fact, it has been approved as a food additive in the EU and other countries since the 1980s. As with any chemical element, however, there are potential side effects and risks associated with its use.

In humans, exposure to bismuth can result in minor skin and eye irritation, nausea, and dizziness. The element is rarely found in nature and, as such, direct exposure is unlikely. For this reason, there is little concern about acute toxicity from bismuth.

Long-term exposure to bismuth, however, can result in more severe health effects. This is because bismuth is a heavy metal with a tendency to accumulate in the body. In high doses, bismuth can cause serious health problems, such as kidney and liver damage, neurological disorders, and reproductive issues.

Bismuth is also toxic to the environment. It tends to accumulate in soil and water, leading to contamination and risk of poisoning to organisms living in these ecosystems. It is important to remember to dispose of bismuth-containing products properly to avoid potential contamination.

The use of bismuth in cosmetics and pharmaceuticals is highly regulated. In the EU, there is a strict limit on the amount of bismuth allowed in these products, and it is generally only used in very small doses.

To ensure safety when handling bismuth, it is important to wear protective clothing and a dust mask. Precaution should also be taken to avoid spills, as bismuth can be hazardous if ingested or exposed to skin and eyes.

Overall, bismuth is generally accepted as safe to ingest, and its use in small doses is well-regulated. However, there are still potential risks associated with long-term exposure or ingestion of large amounts of the element. For this reason, it is important to remember that caution should be taken when handling bismuth and to dispose of bismuth-containing products properly.

Facts

Bismuth is a chemical element with the symbol Bi
Its atomic number is 83.
Bismuth was discovered by Arabic alchemists prior to 1,000 AD.
Bismuth is a brittle metal with a dark, silver-pink hue
Bismuth is a solid at room temperature.

The word “bismuth” is a Latinized version of an Old German word, “weissmuth” or “white substance”
Bismuth is a period 6 chemical element, which is the sixth row on the periodic table.
Most common isotope is Bi-209
Bismuth ranks 65th in elemental abundance in the Earth’s crust
Bismuth is one of only a few elements whose liquid state has a higher density than its solid state.

Bismuth abundance in our solar system is 10 parts per billion by weight
bismuth has the highest electrical resistance, the lowest thermo-conductivity, and the highest Hall Effect.
Bismuth is a group 15 chemical element, which is the nitrogen group.
Bismuth is in the p-block on the periodic table of elements.
Bismuth metal has been known since ancient times

Bismuth is around twice as common as gold in the Earth's crust.
China, Peru, and Mexico are the major suppliers of bismuth.
In the Earth's crust, bismuth is about twice as abundant as gold.
The most important ores of bismuth are bismuthinite and bismite
The compound bismuth subsalicylate is used to prevent diarrhea.

Bismuth oxychloride is sometimes used in cosmetics, as a pigment in paint for eye shadows, hair sprays and nail polishes.
Almost 90% of the bismuth comes from China.
The U.S. imports about 80% of its bismuth from China.
Bismuth is typically obtained as a by-product in refining lead, copper, tin, silver, and gold ores.
Bismuth subsalicylate, sold under various brand names is a well-known remedy for stomach aches and diarrhea.

Information

Bismuth
Pronunciation BIZ-məth
Appearance lustrous brownish silver
Standard atomic weight Ar°(Bi)
  • 208.98040±0.00001
  • 208.98±0.01 (abridged)
Bismuth in the periodic table
Atomic number (Z) 83
Group group 15 (pnictogens)
Period period 6
Block   p-block
Electron configuration [Xe] 4f14 5d10 6s2 6p3
Electrons per shell 2, 8, 18, 32, 18, 5
Physical properties
Phase at STP solid
Melting point 544.7 K ​(271.5 °C, ​520.7 °F)
Boiling point 1837 K ​(1564 °C, ​2847 °F)
Density (near r.t.) 9.78 g/cm3
when liquid (at m.p.) 10.05 g/cm3
Heat of fusion 11.30 kJ/mol
Heat of vaporization 179 kJ/mol
Molar heat capacity 25.52 J/(mol·K)
Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 941 1041 1165 1325 1538 1835
Atomic properties
Oxidation states −3, −2, −1, 0,[2] +1, +2, +3, +4, +5 (a mildly acidic oxide)
Electronegativity Pauling scale: 2.02
Ionization energies
  • 1st: 703 kJ/mol
  • 2nd: 1610 kJ/mol
  • 3rd: 2466 kJ/mol
  • (more)
Atomic radius empirical: 156 pm
Covalent radius 148±4 pm
Van der Waals radius 207 pm
Other properties
Natural occurrence primordial
Crystal structure ​rhombohedral
Speed of sound thin rod 1790 m/s (at 20 °C)
Thermal expansion 13.4 µm/(m⋅K) (at 25 °C)
Thermal conductivity 7.97 W/(m⋅K)
Electrical resistivity 1.29 µΩ⋅m (at 20 °C)
Magnetic ordering diamagnetic
Molar magnetic susceptibility −280.1×10−6 cm3/mol
Young's modulus 32 GPa
Shear modulus 12 GPa
Bulk modulus 31 GPa
Poisson ratio 0.33
Mohs hardness 2.25
Brinell hardness 70–95 MPa
CAS Number 7440-69-9
History
Discovery Arabic alchemists (before AD 1000)
Main isotopes[5] Decay
abun­dance half-life (t1/2) mode pro­duct
207Bi synth 31.55 y β+ 207Pb
208Bi synth 3.68×105 y β+ 208Pb
209Bi 100% 2.01×1019 y α 205Tl
210Bi trace 5.012 d β− 210Po
α 206Tl
210mBi synth 3.04×106 y IT 210Bi
α 206Tl
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