Osmium

This article is about the chemical element. For other uses, see Osmium (disambiguation).

Osmium (from Ancient Greek ὀσμή (osmḗ) 'smell') is a chemical element; it has symbol Os and atomic number 76. It is a hard, brittle, bluish-white transition metal in the platinum group that is found as a trace element in alloys, mostly in platinum ores. Osmium is the densest naturally occurring element. When experimentally measured using X-ray crystallography, it has a density of 22.59 g/cm³.^[9] Manufacturers use its alloys with platinum, iridium, and other platinum-group metals to make fountain pen nib tipping, electrical contacts, and in other applications that require extreme durability and hardness.^[10]

Osmium, ₇₆Os

Osmium
Pronunciation	/ˈɒzmiəm/ ​(OZ-mee-əm)
Appearance	silvery, blue cast
Standard atomic weight Ar°(Os)
	190.23±0.03^[1] 190.23±0.03 (abridged)^[2]
Osmium 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 Ru ↑ Os ↓ Hs rhenium ← osmium → iridium
Atomic number (Z)	76
Group	group 8
Period	period 6
Block	d-block
Electron configuration	[Xe] 4f^14 5d^6 6s^2
Electrons per shell	2, 8, 18, 32, 14, 2
Physical properties
Phase at STP	solid
Melting point	3306 K ​(3033 °C, ​5491 °F)^[3]
Boiling point	5281 K ​(5008 °C, ​9046 °F)^[4]
Density (at 20° C)	22.589 g/cm^3 ^[5]
when liquid (at m.p.)	20 g/cm^3
Heat of fusion	31 kJ/mol
Heat of vaporization	378 kJ/mol
Molar heat capacity	24.7 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 3160 3423 3751 4148 4638 5256
Atomic properties
Oxidation states	−4, −2, −1, 0, +1, +2, +3, +4, +5, +6, +7, +8 (a mildly acidic oxide)
Electronegativity	Pauling scale: 2.2
Ionization energies	1st: 840 kJ/mol 2nd: 1600 kJ/mol
Atomic radius	empirical: 135 pm
Covalent radius	144±4 pm
Spectral lines of osmium
Other properties
Natural occurrence	primordial
Crystal structure	​hexagonal close-packed (hcp) (hP2)
Lattice constants	a = 273.42 pm c = 431.99 pm (at 20 °C)^[5]
Thermal expansion	4.99×10^−6/K (at 20 °C)^[a]
Thermal conductivity	87.6 W/(m⋅K)
Electrical resistivity	81.2 nΩ⋅m (at 0 °C)
Magnetic ordering	paramagnetic^[6]
Molar magnetic susceptibility	11×10^−6 cm^3/mol^[6]
Shear modulus	222 GPa
Bulk modulus	462 GPa
Speed of sound thin rod	4940 m/s (at 20 °C)
Poisson ratio	0.25
Mohs hardness	7.0
Vickers hardness	4137 MPa
Brinell hardness	3920 MPa
CAS Number	7440-04-2
History
Discovery and first isolation	Smithson Tennant (1803)
Isotopes of osmium v e
Main isotopes^[7] Decay abun­dance half-life (t1/2) mode pro­duct ^184Os 0.02% 1.12×10^13 y^[8] α ^180W ^185Os synth 92.95 d ε ^185Re ^186Os 1.59% 2.0×10^15 y α ^182W ^187Os 1.96% stable ^188Os 13.2% stable ^189Os 16.1% stable ^190Os 26.3% stable ^191Os synth 14.99 d β^− ^191Ir ^192Os 40.8% stable ^193Os synth 29.83 h β^− ^193Ir ^194Os synth 6 y β^− ^194Ir
Category: Osmium view talk edit | references

Osmium is among the rarest elements in the Earth's crust, making up only 50 parts per trillion (ppt).^[11][12]

Characteristics

Physical properties

 

Osmium, remelted pellet

Osmium is the densest stable element. Reports conflicted on which of osmium or iridium is denser;^[10] as of 1995^[update], calculations of density from the X-ray crystallography data gives a value of 22.587±0.009 g/cm³ for osmium, slightly denser than the 22.562±0.009 g/cm³ of iridium.^[9] Both metals are nearly 23 times as dense as water, twice as lead, and 1+1⁄6 times as dense as gold.

Osmium has a blue-gray tint.^[10] The reflectivity of single crystals of osmium is complex and strongly direction-dependent, with light in the red and near-infrared wavelengths being more strongly absorbed when polarized parallel to the c crystal axis than when polarized perpendicular to the c axis; the c-parallel polarization is also slightly more reflected in the mid-ultraviolet range. Reflectivity reaches a sharp minimum at around 1.5 eV (near-infrared) for the c-parallel polarization and at 2.0 eV (orange) for the c-perpendicular polarization, and peaks for both in the visible spectrum at around 3.0 eV (blue-violet).^[13]

Osmium is a hard but brittle metal that remains lustrous even at high temperatures. It has a very low compressibility. Correspondingly, its bulk modulus is extremely high, reported between 395 and 462 GPa, which rivals that of diamond (443 GPa). The hardness of osmium is moderately high at 4 GPa.^[14][15][16] Because of its hardness, brittleness, low vapor pressure (the lowest of the platinum-group metals), and very high melting point (the fourth highest of all elements, after carbon, tungsten, and rhenium), solid osmium is difficult to machine, form, or work.

Chemical properties

Main article: Osmium compounds

Oxidation states of osmium
−4	[OsIn6−xSnx]^[17]
−2	Na 2[Os(CO) 4]
−1	Na 2[Os 4(CO) 13]
0	Os 3(CO) 12
+1	OsI
+2	OsI 2
+3	OsBr 3
+4	OsO 2, OsCl 4
+5	OsF 5
+6	OsF 6
+7	OsOF 5
+8	OsO 4, Os(NCH 3) 4

Osmium forms compounds with oxidation states ranging from −4 to +8. The most common oxidation states are +2, +3, +4, and +8. The +8 oxidation state is notable for being the highest attained by any chemical element aside from iridium's +9^[18] and is encountered only in xenon,^[19][20] ruthenium,^[21] hassium,^[22] iridium,^[23] and plutonium.^[24][25] The oxidation states −1 and −2 represented by the two reactive compounds Na
₂[Os
₄(CO)
₁₃] and Na
₂[Os(CO)
₄] are used in the synthesis of osmium cluster compounds.^[26][27]

 

Osmium tetroxide (OsO₄)

The most common compound exhibiting the +8 oxidation state is osmium tetroxide (OsO₄). This toxic compound is formed when powdered osmium is exposed to air. It is a very volatile, water-soluble, pale yellow, crystalline solid with a strong smell. Osmium powder has the characteristic smell of osmium tetroxide.^[28] Osmium tetroxide forms red osmates OsO
₄(OH)²⁻
₂ upon reaction with a base. With ammonia, it forms the nitrido-osmates OsO
₃N⁻
.^[29][30][31] Osmium tetroxide boils at 130 °C and is a powerful oxidizing agent. By contrast, osmium dioxide (OsO
₂) is black, non-volatile, and much less reactive and toxic.

Only two osmium compounds have major applications: osmium tetroxide for staining tissue in electron microscopy and for the oxidation of alkenes in organic synthesis, and the non-volatile osmates for organic oxidation reactions.^[32]

Osmium pentafluoride (OsF
₅) is known, but osmium trifluoride (OsF
₃) has not yet been synthesized. The lower oxidation states are stabilized by the larger halogens, so that the trichloride, tribromide, triiodide, and even diiodide are known. The oxidation state +1 is known only for osmium monoiodide (OsI), whereas several carbonyl complexes of osmium, such as triosmium dodecacarbonyl (Os
₃(CO)
₁₂), represent oxidation state 0.^{[29][30][33][34]}

In general, the lower oxidation states of osmium are stabilized by ligands that are good σ-donors (such as amines) and π-acceptors (heterocycles containing nitrogen). The higher oxidation states are stabilized by strong σ- and π-donors, such as O²⁻
and N³⁻
.^[35]

Despite its broad range of compounds in numerous oxidation states, osmium in bulk form at ordinary temperatures and pressures is stable in air. It resists attack by most acids and bases including aqua regia, but is attacked by F₂ and Cl₂ at high temperatures, and by hot concentrated nitric acid to produce OsO₄. It can be dissolved by molten alkalis fused with an oxidizer such as sodium peroxide (Na₂O₂) or potassium chlorate (KClO₃) to give osmates such as K₂[OsO₂(OH)₄].^[33]

Isotopes

Main article: Isotopes of osmium

Osmium has seven naturally occurring isotopes, five of which are stable: ¹⁸⁷
Os, ¹⁸⁸
Os, ¹⁸⁹
Os, ¹⁹⁰
Os, and (most abundant) ¹⁹²
Os. At least 37 artificial radioisotopes and 20 nuclear isomers exist, with mass numbers ranging from 160 to 203; the most stable of these is ¹⁹⁴
Os with a half-life of 6 years.^[36]

¹⁸⁶
Os undergoes alpha decay with such a long half-life (2.0±1.1)×10¹⁵ years, approximately 140000 times the age of the universe, that for practical purposes it can be considered stable. ¹⁸⁴
Os is also known to undergo alpha decay with a half-life of (1.12±0.23)×10¹³ years.^[8] Alpha decay is predicted for all the other naturally occurring isotopes, but this has never been observed, presumably due to very long half-lives. It is predicted that ¹⁸⁴
Os and ¹⁹²
Os can undergo double beta decay, but this radioactivity has not been observed yet.^[36]

¹⁸⁹Os has a spin of 5/2 but ¹⁸⁷Os has a nuclear spin 1/2. Its low natural abundance (1.64%) and low nuclear magnetic moment means that it is one of the most difficult natural abundance isotopes for NMR spectroscopy.^[37]

¹⁸⁷
Os is the descendant of ¹⁸⁷
Re (half-life 4.56×10¹⁰ years) and is used extensively in dating terrestrial as well as meteoric rocks (see rhenium-osmium dating). It has also been used to measure the intensity of continental weathering over geologic time and to fix minimum ages for stabilization of the mantle roots of continental cratons. This decay is a reason why rhenium-rich minerals are abnormally rich in ¹⁸⁷
Os.^[38] However, the most notable application of osmium isotopes in geology has been in conjunction with the abundance of iridium, to characterise the layer of shocked quartz along the Cretaceous–Paleogene boundary that marks the extinction of the non-avian dinosaurs 65 million years ago.^[39]

History

Osmium was discovered in 1803 by Smithson Tennant and William Hyde Wollaston in London, England.^[40] The discovery of osmium is intertwined with that of platinum and the other metals of the platinum group. Platinum reached Europe as platina ("small silver"), first encountered in the late 17th century in silver mines around the Chocó Department, in Colombia.^[41] The discovery that this metal was not an alloy, but a distinct new element, was published in 1748.^[42] Chemists who studied platinum dissolved it in aqua regia (a mixture of hydrochloric and nitric acids) to create soluble salts. They always observed a small amount of a dark, insoluble residue.^[43] Joseph Louis Proust thought that the residue was graphite.^[43] Victor Collet-Descotils, Antoine François, comte de Fourcroy, and Louis Nicolas Vauquelin also observed iridium in the black platinum residue in 1803, but did not obtain enough material for further experiments.^[43] Later the two French chemists Fourcroy and Vauquelin identified a metal in a platinum residue they called ptène.^[44]

In 1803, Smithson Tennant analyzed the insoluble residue and concluded that it must contain a new metal. Vauquelin treated the powder alternately with alkali and acids^[45] and obtained a volatile new oxide, which he believed was of this new metal—which he named ptene, from the Greek word πτηνος (ptènos) for winged.^[46][47] However, Tennant, who had the advantage of a much larger amount of residue, continued his research and identified two previously undiscovered elements in the black residue, iridium and osmium.^[43][45] He obtained a yellow solution (probably of cis–[Os(OH)₂O₄]²⁻) by reactions with sodium hydroxide at red heat. After acidification he was able to distill the formed OsO₄.^[46] He named it osmium after Greek osme meaning "a smell", because of the chlorine-like and slightly garlic-like smell of the volatile osmium tetroxide.^[48] Discovery of the new elements was documented in a letter to the Royal Society on June 21, 1804.^[43][49]

Uranium and osmium were early successful catalysts in the Haber process, the nitrogen fixation reaction of nitrogen and hydrogen to produce ammonia, giving enough yield to make the process economically successful. At the time, a group at BASF led by Carl Bosch bought most of the world's supply of osmium to use as a catalyst. Shortly thereafter, in 1908, cheaper catalysts based on iron and iron oxides were introduced by the same group for the first pilot plants, removing the need for the expensive and rare osmium.^[50]

Osmium is now obtained primarily from the processing of platinum and nickel ores.^[51]

Occurrence

 

Native platinum containing traces of the other platinum group metals

Osmium is one of the least abundant stable elements in Earth's crust, with an average mass fraction of 50 parts per trillion in the continental crust.^[52]

Osmium is found in nature as an uncombined element or in natural alloys; especially the iridium–osmium alloys, osmiridium (iridium rich), and iridosmium (osmium rich).^[45] In nickel and copper deposits, the platinum-group metals occur as sulfides (i.e., (Pt,Pd)S), tellurides (e.g., PtBiTe), antimonides (e.g., PdSb), and arsenides (e.g., PtAs₂); in all these compounds platinum is exchanged by a small amount of iridium and osmium. As with all of the platinum-group metals, osmium can be found naturally in alloys with nickel or copper.^[53]

Within Earth's crust, osmium, like iridium, is found at highest concentrations in three types of geologic structure: igneous deposits (crustal intrusions from below), impact craters, and deposits reworked from one of the former structures. The largest known primary reserves are in the Bushveld Igneous Complex in South Africa,^[54] though the large copper–nickel deposits near Norilsk in Russia, and the Sudbury Basin in Canada are also significant sources of osmium. Smaller reserves can be found in the United States.^[54] The alluvial deposits used by pre-Columbian people in the Chocó Department, Colombia, are still a source for platinum-group metals. The second large alluvial deposit was found in the Ural Mountains, Russia, which is still mined.^[51][55]

Production

 

Osmium crystals, grown by chemical vapor transport

Osmium is obtained commercially as a by-product from nickel and copper mining and processing. During electrorefining of copper and nickel, noble metals such as silver, gold and the platinum-group metals, together with non-metallic elements such as selenium and tellurium, settle to the bottom of the cell as anode mud, which forms the starting material for their extraction.^[56][57] Separating the metals requires that they first be brought into solution. Several methods can achieve this, depending on the separation process and the composition of the mixture. Two representative methods are fusion with sodium peroxide followed by dissolution in aqua regia, and dissolution in a mixture of chlorine with hydrochloric acid.^[54][58] Osmium, ruthenium, rhodium, and iridium can be separated from platinum, gold, and base metals by their insolubility in aqua regia, leaving a solid residue. Rhodium can be separated from the residue by treatment with molten sodium bisulfate. The insoluble residue, containing ruthenium, osmium, and iridium, is treated with sodium oxide, in which Ir is insoluble, producing water-soluble ruthenium and osmium salts. After oxidation to the volatile oxides, RuO
₄ is separated from OsO
₄ by precipitation of (NH₄)₃RuCl₆ with ammonium chloride.

After it is dissolved, osmium is separated from the other platinum-group metals by distillation or extraction with organic solvents of the volatile osmium tetroxide.^[59] The first method is similar to the procedure used by Tennant and Wollaston. Both methods are suitable for industrial-scale production. In either case, the product is reduced using hydrogen, yielding the metal as a powder or sponge that can be treated using powder metallurgy techniques.^[60]

Estimates of annual worldwide osmium production are on the order of several hundred to a few thousand kilograms.^[61][33] Production and consumption figures for osmium are not well reported because demand for the metal is limited and can be fulfilled with the byproducts of other refining processes.^[33] To reflect this, statistics often report osmium with other minor platinum group metals such as iridium and ruthenium. US imports of osmium from 2014 to 2021 averaged 155 kg annually.^[62][63]

Applications

Because osmium is virtually unforgeable when fully dense and very fragile when sintered, it is rarely used in its pure state, but is instead often alloyed with other metals for high-wear applications. Osmium alloys such as osmiridium are very hard and, along with other platinum-group metals, are used in the tips of fountain pens, instrument pivots, and electrical contacts, as they can resist wear from frequent operation. They were also used for the tips of phonograph styli during the late 78 rpm and early "LP" and "45" record era, circa 1945 to 1955. Osmium-alloy tips were significantly more durable than steel and chromium needle points, but wore out far more rapidly than competing, and costlier, sapphire and diamond tips, so they were discontinued.^[64]

Osmium tetroxide has been used in fingerprint detection^[65] and in staining fatty tissue for optical and electron microscopy. As a strong oxidant, it cross-links lipids mainly by reacting with unsaturated carbon–carbon bonds and thereby both fixes biological membranes in place in tissue samples and simultaneously stains them. Because osmium atoms are extremely electron-dense, osmium staining greatly enhances image contrast in transmission electron microscopy (TEM) studies of biological materials. Those carbon materials otherwise have very weak TEM contrast.^[32] Another osmium compound, osmium ferricyanide (OsFeCN), exhibits similar fixing and staining action.^[66]

The tetroxide and its derivative potassium osmate are important oxidants in organic synthesis. For the Sharpless asymmetric dihydroxylation, which uses osmate for the conversion of a double bond into a vicinal diol, Karl Barry Sharpless was awarded the Nobel Prize in Chemistry in 2001.^[67][68] OsO₄ is very expensive for this use, so KMnO₄ is often used instead, even though the yields are less for this cheaper chemical reagent.

In 1898, the Austrian chemist Auer von Welsbach developed the Oslamp with a filament made of osmium, which he introduced commercially in 1902. After only a few years, osmium was replaced by tungsten, which is more abundant (and thus cheaper) and more stable. Tungsten has the highest melting point among all metals, and its use in light bulbs increases the luminous efficacy and life of incandescent lamps.^[46]

The light bulb manufacturer Osram (founded in 1906, when three German companies, Auer-Gesellschaft, AEG and Siemens & Halske, combined their lamp production facilities) derived its name from the elements of osmium and Wolfram (the latter is German for tungsten).^[69]

Like palladium, powdered osmium effectively absorbs hydrogen atoms. This could make osmium a potential candidate for a metal-hydride battery electrode. However, osmium is expensive and would react with potassium hydroxide, the most common battery electrolyte.^[70]

Osmium has high reflectivity in the ultraviolet range of the electromagnetic spectrum; for example, at 600 Å osmium has a reflectivity twice that of gold.^[71] This high reflectivity is desirable in space-based UV spectrometers, which have reduced mirror sizes due to space limitations. Osmium-coated mirrors were flown in several space missions aboard the Space Shuttle, but it soon became clear that the oxygen radicals in low Earth orbit are abundant enough to significantly deteriorate the osmium layer.^[72]

•  
  The Sharpless dihydroxylation:
  R_L = largest substituent; R_M = medium-sized substituent; R_S = smallest substituent
•  
  Post-flight appearance of Os, Ag, and Au mirrors from the front (left images) and rear panels of the Space Shuttle. Blackening reveals oxidation due to irradiation by oxygen atoms.^[73][74]

Precautions

The primary hazard of metallic osmium is the potential formation of osmium tetroxide (OsO₄), which is volatile and very poisonous.^[75] This reaction is thermodynamically favorable at room temperature,^[76] but the rate depends on temperature and the surface area of the metal.^[77][78] As a result, bulk material is not considered hazardous^{[77][79][80][81]} while powders react quickly enough that samples can sometimes smell like OsO₄ if they are handled in air.^[33][82]

Price

Between 1990 and 2010, the nominal price of osmium metal was almost constant, while inflation reduced the real value from ~US$950/ounce to ~US$600/ounce.^[83] Because osmium has few commercial applications, it is not heavily traded and prices are seldom reported.^[83]

Notes

1. The thermal expansion of Os is anisotropic: the coefficients for each crystal axis (at 20 °C) are: α_a = 4.57×10⁻⁶/K, α_c = 5.85×10⁻⁶/K, and α_average = α_V/3 = 4.99×10⁻⁶/K.

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Cited sources

• Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. ISBN 978-1439855119.

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Look up osmium in Wiktionary, the free dictionary.

• Osmium at The Periodic Table of Videos (University of Nottingham)
• Flegenheimer, J. (2014). The mystery of the disappearing isotope. Revista Virtual de Química. V. XX. Available at
• Chisholm, Hugh, ed. (1911). "Osmium" . Encyclopædia Britannica. Vol. 20 (11th ed.). Cambridge University Press. p. 352.