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Completely analogous reactions occur for the niobium component, but the hexafluoride is typically predominant under the conditions of the extraction.
Completely analogous reactions occur for the niobium component, but the hexafluoride is typically predominant under the conditions of the extraction.
: Nb<sub>2</sub>O<sub>5</sub> + 12 HF → 2 H[NbF<sub>6</sub>] + 5 H<sub>2</sub>O
: Nb<sub>2</sub>O<sub>5</sub> + 12 HF → 2 H[NbF<sub>6</sub>] + 5 H<sub>2</sub>O
These equations are simplified: it is suspected that bisulfate (HSO<sub>4</sub><sup>−</sup>) and chloride compete as ligands for the Nb(V) and Ta(V) ions, when sulfuric and hydrochloric acids are used, respectively.<ref name=Chang/> The tantalum and niobium fluoride complexes are then removed from the [[aqueous]] solution by [[Liquid–liquid extraction|liquid-liquid extraction]] into [[organic solvents]], such as [[cyclohexanone]], [[octanol]], and [[methyl isobutyl ketone]]. This simple procedure allows the removal of most metal-containing impurities (e.g. iron, manganese, titanitum, zirconium), which remain in the aqueous phase in the form of their [[fluoride]]s and other complexes.
These equations are simplified: it is suspected that bisulfate (HSO<sub>4</sub><sup>−</sup>) and chloride compete as ligands for the Nb(V) and Ta(V) ions, when sulfuric and hydrochloric acids are used, respectively.<ref name=Chang/> The tantalum and niobium fluoride complexes are then removed from the [[aqueous]] solution by [[Liquid–liquid extraction|liquid-liquid extraction]] into [[organic solvents]], such as [[cyclohexanone]], [[octanol]], and [[methyl isobutyl ketone]]. This simple procedure allows the removal of most metal-containing impurities (e.g. iron, manganese, titanium, zirconium), which remain in the aqueous phase in the form of their [[fluoride]]s and other complexes.


Separation of the tantalum ''from'' niobium is then achieved by lowering the [[ionic strength]] of the acid mixture, which causes the niobium to dissolve in the aqueous phase. It is proposed that [[oxyfluoride]] H<sub>2</sub>[NbOF<sub>5</sub>] is formed under these conditions. Subsequent to removal of the niobium, the solution of purified H<sub>2</sub>TaF<sub>7</sub>] is neutralised with aqueous [[ammonia]] to precipitate hydrated tantalum oxide as a solid, which can be [[calcination|calcined]] to [[tantalum pentoxide]] (Ta<sub>2</sub>O<sub>5</sub>).<ref>{{cite book|last=Agulyanski|first=Anatoly|title=Chemistry of Tantalum and Niobium Fluoride Compounds|date=2004|publisher=Elsevier|location=Burlington|isbn=9780080529028|edition=1st}}</ref>
Separation of the tantalum ''from'' niobium is then achieved by lowering the [[ionic strength]] of the acid mixture, which causes the niobium to dissolve in the aqueous phase. It is proposed that [[oxyfluoride]] H<sub>2</sub>[NbOF<sub>5</sub>] is formed under these conditions. Subsequent to removal of the niobium, the solution of purified H<sub>2</sub>TaF<sub>7</sub>] is neutralised with aqueous [[ammonia]] to precipitate hydrated tantalum oxide as a solid, which can be [[calcination|calcined]] to [[tantalum pentoxide]] (Ta<sub>2</sub>O<sub>5</sub>).<ref>{{cite book|last=Agulyanski|first=Anatoly|title=Chemistry of Tantalum and Niobium Fluoride Compounds|date=2004|publisher=Elsevier|location=Burlington|isbn=9780080529028|edition=1st}}</ref>

Revision as of 01:50, 3 June 2017

Tantalum, 73Ta
Tantalum
Pronunciation/ˈtæntələm/ ​(TAN-təl-əm)
Appearancegray blue
Standard atomic weight Ar°(Ta)
Tantalum in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
Nb
↑
Ta
↓
Db
hafnium ← tantalum → tungsten
Atomic number (Z)73
Groupgroup 5
Periodperiod 6
Block  d-block
Electron configuration[Xe] 4f14 5d3 6s2
Electrons per shell2, 8, 18, 32, 11, 2
Physical properties
Phase at STPsolid
Melting point3290 K ​(3017 °C, ​5463 °F)
Boiling point5731 K ​(5458 °C, ​9856 °F)
Density (at 20° C)16.678 g/cm3 [3]
when liquid (at m.p.)15 g/cm3
Heat of fusion36.57 kJ/mol
Heat of vaporization753 kJ/mol
Molar heat capacity25.36 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 3297 3597 3957 4395 4939 5634
Atomic properties
Oxidation statescommon: +5
−3,? −1,[4] 0,? +1,? +2,[4] +3,[4] +4[4]
ElectronegativityPauling scale: 1.5
Ionization energies
  • 1st: 761 kJ/mol
  • 2nd: 1500 kJ/mol
Atomic radiusempirical: 146 pm
Covalent radius170±8 pm
Color lines in a spectral range
Spectral lines of tantalum
Other properties
Natural occurrenceprimordial
Crystal structure ​body-centered cubic (bcc)[3] (cI2)
Lattice constant
Body-centered cubic crystal structure for tantalum
a = 330.29 pm (at 20 °C)[3]
Thermal expansion6.3 µm/(m⋅K) (at 25 °C)
Thermal conductivity57.5 W/(m⋅K)
Electrical resistivity131 nΩ⋅m (at 20 °C)
Magnetic orderingparamagnetic[5]
Molar magnetic susceptibility+154.0×10−6 cm3/mol (293 K)[6]
Young's modulus186 GPa
Shear modulus69 GPa
Bulk modulus200 GPa
Speed of sound thin rod3400 m/s (at 20 °C)
Poisson ratio0.34
Mohs hardness6.5
Vickers hardness870–1200 MPa
Brinell hardness440–3430 MPa
CAS Number7440-25-7
History
DiscoveryAnders Gustaf Ekeberg (1802)
Recognized as a distinct element byHeinrich Rose (1844)
Isotopes of tantalum
Main isotopes[7] Decay
abun­dance half-life (t1/2) mode pro­duct
177Ta synth 56.56 h β+ 177Hf
178Ta synth 2.36 h β+ 178Hf
179Ta synth 1.82 y ε 179Hf
180Ta synth 8.125 h ε 180Hf
β− 180W
180mTa 0.0120% stable
181Ta 99.988% stable
182Ta synth 114.43 d β− 182W
183Ta synth 5.1 d β− 183W
 Category: Tantalum
| references

Tantalum is a chemical element with symbol Ta and atomic number 73. Previously known as tantalium, its name comes from Tantalus, a villain from Greek mythology.[8] Tantalum is a rare, hard, blue-gray, lustrous transition metal that is highly corrosion-resistant. It is part of the refractory metals group, which are widely used as minor components in alloys. The chemical inertness of tantalum makes it a valuable substance for laboratory equipment and a substitute for platinum. Its main use today is in tantalum capacitors in electronic equipment such as mobile phones, DVD players, video game systems and computers. Tantalum, always together with the chemically similar niobium, occurs in the minerals tantalite, columbite and coltan (a mix of columbite and tantalite).

History

Tantalum was discovered in Sweden in 1802 by Anders Ekeberg.[9][10] One year earlier, Charles Hatchett had discovered the element columbium (Now called Niobium).[11] In 1809, the English chemist William Hyde Wollaston compared the oxides derived from both columbium—columbite, with a density 5.918 g/cm3, and tantalum—tantalite, with a density 7.935 g/cm3, and concluded that the two oxides, despite their difference in measured density, were identical. He decided to keep the name tantalum.[12] After Friedrich Wöhler confirmed these results, it was thought that columbium and tantalum were the same element. This conclusion was disputed in 1846 by the German chemist Heinrich Rose, who argued that there were two additional elements in the tantalite sample, and he named them after the children of Tantalus: niobium (from Niobe, the goddess of tears), and pelopium (from Pelops).[13][14] The supposed element "pelopium" was later identified as a mixture of tantalum and niobium, and it was found that the niobium was identical to the columbium already discovered in 1801 by Hatchett.

The differences between tantalum and niobium were demonstrated unequivocally in 1864 by Christian Wilhelm Blomstrand,[15] and Henri Etienne Sainte-Claire Deville, as well as by Louis J. Troost, who determined the empirical formulas of some of their compounds in 1865.[15][16] Further confirmation came from the Swiss chemist Jean Charles Galissard de Marignac,[17] in 1866, who proved that there were only two elements. These discoveries did not stop scientists from publishing articles about the so-called ilmenium until 1871.[18] De Marignac was the first to produce the metallic form of tantalum in 1864, when he reduced tantalum chloride by heating it in an atmosphere of hydrogen.[19] Early investigators had only been able to produce impure tantalum, and the first relatively pure ductile metal was produced by Werner von Bolton in Charlottenburg in 1903. Wires made with metallic tantalum were used for light bulb filaments until tungsten replaced it in widespread use.[20]

The name tantalum was derived from the name of the mythological Tantalus, the father of Niobe in Greek mythology. In the story, he had been punished after death by being condemned to stand knee-deep in water with perfect fruit growing above his head, both of which eternally tantalized him. (If he bent to drink the water, it drained below the level he could reach, and if he reached for the fruit, the branches moved out of his grasp.)[21] Ekeberg wrote "This metal I call tantalum ... partly in allusion to its incapacity, when immersed in acid, to absorb any and be saturated."[22]

For decades, the commercial technology for separating tantalum from niobium involved the fractional crystallization of potassium heptafluorotantalate away from potassium oxypentafluoroniobate monohydrate, a process that was discovered by Jean Charles Galissard de Marignac in 1866. This method has been supplanted by solvent extraction from fluoride-containing solutions of tantalum.[16]

Characteristics

Physical properties

Tantalum is dark (blue-gray),[23] dense, ductile, very hard, easily fabricated, and highly conductive of heat and electricity. The metal is renowned for its resistance to corrosion by acids; in fact, at temperatures below 150 °C tantalum is almost completely immune to attack by the normally aggressive aqua regia. It can be dissolved with hydrofluoric acid or acidic solutions containing the fluoride ion and sulfur trioxide, as well as with a solution of potassium hydroxide. Tantalum's high melting point of 3017 °C (boiling point 5458 °C) is exceeded among the elements only by tungsten, rhenium and osmium for metals, and carbon.

Tantalum exists in two crystalline phases, alpha and beta. The alpha phase is relatively ductile and soft; it has body-centered cubic structure (space group Im3m, lattice constant a = 0.33058 nm), Knoop hardness 200–400 HN and electrical resistivity 15–60 µΩּcm. The beta phase is hard and brittle; its crystal symmetry is tetragonal (space group P42/mnm, a = 1.0194 nm, c = 0.5313 nm), Knoop hardness is 1000–1300 HN and electrical resistivity is relatively high at 170–210 µΩּcm. The beta phase is metastable and converts to the alpha phase upon heating to 750–775 °C. Bulk tantalum is almost entirely alpha phase, and the beta phase usually exists as thin films obtained by magnetron sputtering, chemical vapor deposition or electrochemical deposition from an eutectic molten salt solution.[24]

Chemical properties

Tantalum forms oxides with the oxidation states +5 (Ta2O5) and +4 (TaO2).[25] The most stable oxidation state is +5, as seen in tantalum pentoxide.[25] Tantalum pentoxide is the starting material for several tantalum compounds. The compounds are created by dissolving the pentoxide in basic hydroxide solutions or by melting it in another metal oxide. Such examples are lithium tantalate (LiTaO3) and lanthanum tantalate (LaTaO4). In the lithium tantalate, the tantalate ion TaO−
3 does not occur; instead, this part of the formula represents linkage of TaO7−
6 octahedra to form a three-dimensional perovskite framework; while the lanthanum tantalate contains lone TaO3−
4 tetrahedral groups.[25]

The fluorides of tantalum can be used for its separation from niobium.[26] Tantalum forms halogen compounds in the oxidation states of +5, +4, and +3 of the type TaX
5, TaX
4, and TaX
3, although multi-core complexes and substoichiometric compounds are also known.[25][27] Tantalum pentafluoride (TaF5) is a white solid with a melting point of 97.0 °C and tantalum pentachloride (TaCl5) is a white solid with a melting point of 247.4 °C. Tantalum pentachloride is hydrolyzed by water and reacts with additional tantalum at elevated temperatures by forming the black and highly hygroscopic tantalum tetrachloride (TaCl4). While the trihalides can be obtained by reduction of the pentahalides with hydrogen, the dihalides do not exist.[25] A tantalum-tellurium alloy forms quasicrystals.[25] Tantalum compounds with oxidation states as low as −1 have been reported in 2008.[28] As in the cases of most other refractory metals, the hardest known compounds of tantalum are its stable nitrides and carbides. Tantalum carbide, TaC, like the more commonly used tungsten carbide, is a very hard ceramic that is used in cutting tools. Tantalum(III) nitride is used as a thin film insulator in some microelectronic fabrication processes.[29] Chemists at the Los Alamos National Laboratory in the United States have developed a tantalum carbide-graphite composite material that is one of the hardest materials ever synthesized. Korean researchers have developed an amorphous tantalum-tungsten-copper alloy that is more flexible and two to three times stronger than commonly used steel alloys.[30] There are two tantalum aluminides, TaAl3 and Ta3Al. These are stable, refractory, and reflective, and they have been proposed[31] as coatings for use in infrared wave mirrors.

Isotopes

Main article: Isotopes of tantalum

Natural tantalum consists of two isotopes: 180mTa (0.012%) and 181Ta (99.988%). 181Ta is a stable isotope. 180mTa (m denotes a metastable state) is predicted to decay in three ways: isomeric transition to the ground state of 180Ta, beta decay to 180W, or electron capture to 180Hf. However, radioactivity of this nuclear isomer has never been observed, and only a lower limit on its half life of 2.0 × 1016 years has been set.[32] The ground state of 180Ta has a half life of only 8 hours. 180mTa is the only naturally occurring nuclear isomer (excluding radiogenic and cosmogenic short-living nuclides). It is also the rarest isotope in the Universe, taking into account the elemental abundance of tantalum and isotopic abundance of 180mTa in the natural mixture of isotopes (and again excluding radiogenic and cosmogenic short-living nuclides).[33]

Tantalum has been examined theoretically as a "salting" material for nuclear weapons (cobalt is the better-known hypothetical salting material). An external shell of 181Ta would be irradiated by the intensive high-energy neutron flux from a hypothetical exploding nuclear weapon. This would transmute the tantalum into the radioactive isotope 182Ta, which has a half-life of 114.4 days and produces gamma rays with approximately 1.12 million electron-volts (MeV) of energy apiece, which would significantly increase the radioactivity of the nuclear fallout from the explosion for several months. Such "salted" weapons have never been built or tested, as far as is publicly known, and certainly never used as weapons.[34]

Tantalum can be used as a target material for accelerated proton beams for the production of various short-lived isotopes including 8Li, 80Rb, and 160Yb.[35]

Occurrence

Tantalite, Pilbara district, Australia

Tantalum is estimated to make up about 1 ppm[36] or 2 ppm[27] of the Earth's crust by weight. There are many species of tantalum minerals, only some of which are so far being used by industry as raw materials: tantalite, microlite, wodginite, euxenite, polycrase. Tantalite (Fe, Mn)Ta2O6 is the most important mineral for tantalum extraction. Tantalite has the same mineral structure as columbite (Fe, Mn) (Ta, Nb)2O6; when there is more tantalum than niobium it is called tantalite and when there is more niobium than tantalum is it called columbite (or niobite). The high density of tantalite and other tantalum containing minerals makes the use of gravitational separation the best method. Other minerals include samarskite and fergusonite.

Grey and white world map with China, Australia, Brazil and Kongo colored blue representing less than 10% of the tantalum world production each and Rwanda colored in green representing 60% of tantalum world production
Tantalum producers in 2015 with Rwanda being the main producer

The primary mining of tantalum is in Australia, where the largest producer, Global Advanced Metals, formerly known as Talison Minerals, operates two mines in Western Australia, Greenbushes in the Southwest and Wodgina in the Pilbara region. The Wodgina mine was reopened in January 2011 after mining at the site was suspended in late-2008 due to the global financial crisis.[37] Less than a year after it reopened, Global Advanced Metals announced that due to again "... softening tantalum demand ...", and other factors, tantalum mining operations were to cease at the end of February 2012.[38] Wodgina produces a primary tantalum concentrate which is further upgraded at the Greenbushes operation before being sold to customers.[39] Whereas the large-scale producers of niobium are in Brazil and Canada, the ore there also yields a small percentage of tantalum. Some other countries such as China, Ethiopia, and Mozambique mine ores with a higher percentage of tantalum, and they produce a significant percentage of the world's output of it. Tantalum is also produced in Thailand and Malaysia as a by-product of the tin mining there. During gravitational separation of the ores from placer deposits, not only is cassiterite (SnO2) found, but a small percentage of tantalite also included. The slag from the tin smelters then contains economically useful amounts of tantalum, which is leached from the slag.[16][40]

Grey and white world map with Canada, Brazil and Mozambique colored blue representing less than 20% of the tantalum world production each and Australia colored in green representing 60% of tantalum world production
Tantalum producers in 2006 with Australia being the main producer

World tantalum mine production has undergone an important geographic shift since the start of the 21st century when production was predominantly from Australia and Brazil. Beginning in 2007 and through 2014, the major sources of tantalum production from mines dramatically shifted to the DRC, Rwanda, and some other African countries.[41] Future sources of supply of tantalum, in order of estimated size, are being explored in Saudi Arabia, Egypt, Greenland, China, Mozambique, Canada, Australia, the United States, Finland, and Brazil.[42][43]

It is estimated that there are less than 50 years left of tantalum resources, based on extraction at current rates, demonstrating the need for increased recycling.[44]

Status as a conflict resource

See also: Coltan mining and ethics and Coltan § Ethics of mining in the Democratic Republic of Congo

Tantalum is considered a conflict resource. Coltan, the industrial name for a columbite–tantalite mineral from which columbium (i.e. niobium) and tantalum are extracted,[45] can also be found in Central Africa, which is why tantalum is being linked to warfare in the Democratic Republic of the Congo (formerly Zaire). According to an October 23, 2003 United Nations report,[46] the smuggling and exportation of coltan has helped fuel the war in the Congo, a crisis that has resulted in approximately 5.4 million deaths since 1998[47] – making it the world’s deadliest documented conflict since World War II. Ethical questions have been raised about responsible corporate behavior, human rights, and endangering wildlife, due to the exploitation of resources such as coltan in the armed conflict regions of the Congo Basin.[48][49][50][51] However, although important for the local economy in Congo, the contribution of coltan mining in Congo to the world supply of tantalum is usually small. The United States Geological Survey reports in its yearbook that this region produced a little less than 1% of the world's tantalum output in 2002–2006, peaking at 10% in 2000 and 2008.[40]

The stated aim of the Solutions for Hope Tantalum Project is to "source conflict-free tantalum from the Democratic Republic of Congo"[52]

Production and fabrication

Time trend of tantalum production until 2012[53]

Several steps are involved in the extraction of tantalum from tantalite. First, the mineral is crushed and concentrated by gravity separation. This is generally carried out near the mine site.

Refining

The refining of tantalum from its ores is one of the more demanding separation processes in industrial metallurgy. The chief problem is that tantalum ores contain significant amounts of niobium, which has chemical properties almost identical to those of Ta. A large number of procedures have been developed to address this challenge.

In modern times, the separation is achieved by hydrometallurgy.[54] Extraction begins with a leaching the ore with hydrofluoric acid together with sulfuric acid or hydrochloric acid. This step allows the tantalum and niobium to be separated from the various non-metallic impurities in the rock. Although Ta occurs as various minerals, it is conveniently represented as the pentoxide, since most oxides of tantalum(V) behave similarly under these conditions. A simplified equation for its extraction is thus:

Ta2O5 + 14 HF → 2 H2[TaF7] + 5 H2O

Completely analogous reactions occur for the niobium component, but the hexafluoride is typically predominant under the conditions of the extraction.

Nb2O5 + 12 HF → 2 H[NbF6] + 5 H2O

These equations are simplified: it is suspected that bisulfate (HSO4−) and chloride compete as ligands for the Nb(V) and Ta(V) ions, when sulfuric and hydrochloric acids are used, respectively.[54] The tantalum and niobium fluoride complexes are then removed from the aqueous solution by liquid-liquid extraction into organic solvents, such as cyclohexanone, octanol, and methyl isobutyl ketone. This simple procedure allows the removal of most metal-containing impurities (e.g. iron, manganese, titanium, zirconium), which remain in the aqueous phase in the form of their fluorides and other complexes.

Separation of the tantalum from niobium is then achieved by lowering the ionic strength of the acid mixture, which causes the niobium to dissolve in the aqueous phase. It is proposed that oxyfluoride H2[NbOF5] is formed under these conditions. Subsequent to removal of the niobium, the solution of purified H2TaF7] is neutralised with aqueous ammonia to precipitate hydrated tantalum oxide as a solid, which can be calcined to tantalum pentoxide (Ta2O5).[55]

Instead of hydrolysis, the H2[TaF7] can be treated with potassium fluoride to produce potassium heptafluorotantalate:

H2[TaF7] + 2 KF → K2[TaF7] + 2 HF

Unlike H2[TaF7], the potassium salt is readily crystallized and handled as a solid.

K2[TaF7] can be converted to metallic tantalum by reduction with sodium, at approximately 800 °C in molten salt.[56]

K2[TaF7] + 5 Na → Ta + 5 NaF + 2 KF

In an older method, called the Marignac process, the mixture of H2[TaF7] and H2[NbOF5] was converted to a mixture of K2[TaF7] and K2[NbOF5], which was then be separated by fractional crystallization, exploiting their different water solubilities.

Electrolysis

See also: FFC_Cambridge_process

Electrolysis using a modified version of the Hall–Héroult process. Instead of requiring the input oxide and output metal to be in liquid form, tantalum electrolysis operates on non-liquid powdered oxides. The initial discovery came in 1997 when Cambridge University researchers immersed small samples of certain oxides in baths of molten salt and reduced the oxide with electric current. The cathode uses powdered metal oxide. The anode is made of carbon. The molten salt at 1,000 °C (1,830 °F) is the electrolyte. The first refinery has enough capacity to supply 3–4% of annual global demand.[57]

Fabrication and metalworking

All welding of tantalum must be done in an inert atmosphere of argon or helium in order to shield it from contamination with atmospheric gases. Tantalum is not solderable. Grinding tantalum is difficult, especially so for annealed tantalum. In the annealed condition, tantalum is extremely ductile and can be readily formed as metal sheets.[58]

Applications

Electronics

Tantalum electrolytic capacitor

The major use for tantalum, as the metal powder, is in the production of electronic components, mainly capacitors and some high-power resistors. Tantalum electrolytic capacitors exploit the tendency of tantalum to form a protective oxide surface layer, using tantalum powder, pressed into a pellet shape, as one "plate" of the capacitor, the oxide as the dielectric, and an electrolytic solution or conductive solid as the other "plate". Because the dielectric layer can be very thin (thinner than the similar layer in, for instance, an aluminium electrolytic capacitor), a high capacitance can be achieved in a small volume. Because of the size and weight advantages, tantalum capacitors are attractive for portable telephones, personal computers, and automotive electronics.[59]

Alloys

Tantalum is also used to produce a variety of alloys that have high melting points, strength, and ductility. Alloyed with other metals, it is also used in making carbide tools for metalworking equipment and in the production of superalloys for jet engine components, chemical process equipment, nuclear reactors, and missile parts.[59][60] Because of its ductility, tantalum can be drawn into fine wires or filaments, which are used for evaporating metals such as aluminium. Since it resists attack by body fluids and is nonirritating, tantalum is widely used in making surgical instruments and implants. For example, porous tantalum coatings are used in the construction of orthopedic implants due to tantalum's ability to form a direct bond to hard tissue.[61]

Tantalum is inert against most acids except hydrofluoric acid and hot sulfuric acid, and hot alkaline solutions also cause tantalum to corrode. This property makes it a useful metal for chemical reaction vessels and pipes for corrosive liquids. Heat exchanging coils for the steam heating of hydrochloric acid are made from tantalum.[62] Tantalum was extensively used in the production of ultra high frequency electron tubes for radio transmitters. The tantalum is capable of capturing oxygen and nitrogen by forming nitrides and oxides and therefore helps to sustain the high vacuum needed for the tubes.[26][62]

Other uses

Bimetallic coins minted by the Bank of Kazakhstan with silver ring and tantalum center.

The high melting point and oxidation resistance lead to the use of the metal in the production of vacuum furnace parts. Tantalum is extremely inert and is therefore formed into a variety of corrosion resistant parts, such as thermowells, valve bodies, and tantalum fasteners. Due to its high density, shaped charge and explosively formed penetrator liners have been constructed from tantalum.[63] Tantalum greatly increases the armor penetration capabilities of a shaped charge due to its high density and high melting point.[64][65] It is also occasionally used in precious watches e.g. from Audemars Piguet, F.P. Journe, Hublot, Montblanc, Omega, and Panerai. Tantalum is also highly bioinert and is used as an orthopedic implant material.[66] The high stiffness of tantalum makes it necessary to use it as highly porous foam or scaffold with lower stiffness for hip replacement implants to avoid stress shielding.[67] Because tantalum is a non-ferrous, non-magnetic metal, these implants are considered to be acceptable for patients undergoing MRI procedures.[68] The oxide is used to make special high refractive index glass for camera lenses.[69]

Precautions

Compounds containing tantalum are rarely encountered in the laboratory. The metal is highly biocompatible[66] and is used for body implants and coatings, therefore attention may be focused on other elements or the physical nature of the chemical compound.[70]

People can be exposed to tantalum in the workplace by breathing it in, skin contact, or eye contact. The Occupational Safety and Health Administration (OSHA) has set the legal limit (permissible exposure limit) for tantalum exposure in the workplace as 5 mg/m3 over an 8-hour workday. The National Institute for Occupational Safety and Health (NIOSH) has set a recommended exposure limit (REL) of 5 mg/m3 over an 8-hour workday and a short-term limit of 10 mg/m3. At levels of 2500 mg/m3, tantalum is immediately dangerous to life and health.[71]

References

  1. ^ "Standard Atomic Weights: Tantalum". CIAAW. 2005.
  2. ^ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
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