Rhodium

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Rhodium, 45Rh
Rhodium powder pressed melted.jpg
Rhodium
Pronunciation /ˈroʊdiəm/ ​(ROH-dee-əm)
Appearancesilvery white metallic
Standard atomic weight Ar°(Rh)
Rhodium 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
Co
↑
Rh
↓
Ir
ruthenium ← rhodium → palladium
Atomic number (Z)45
Group group 9
Period period 5
Block   d-block
Electron configuration [ Kr ] 4d8 5s1
Electrons per shell2, 8, 18, 16, 1
Physical properties
Phase at  STP solid
Melting point 2237  K ​(1964 °C,​3567 °F)
Boiling point 3968 K​(3695 °C,​6683 °F)
Density (at 20° C)12.423 g/cm3 [3]
when liquid (at  m.p.)10.7 g/cm3
Heat of fusion 26.59  kJ/mol
Heat of vaporization 493 kJ/mol
Molar heat capacity 24.98 J/(mol·K)
Vapor pressure
P (Pa)1101001 k10 k100 k
at T (K)228824962749306334053997
Atomic properties
Oxidation states −3 [4] , −1, 0, +1, +2, +3, +4, +5, +6, +7 [5] (an  amphoteric oxide)
Electronegativity Pauling scale: 2.28
Ionization energies
  • 1st: 719.7 kJ/mol
  • 2nd: 1740 kJ/mol
  • 3rd: 2997 kJ/mol
Atomic radius empirical:134  pm
Covalent radius 142±7 pm
Rhodium spectrum visible.png
Spectral lines of rhodium
Other properties
Natural occurrence primordial
Crystal structure ​ face-centered cubic (fcc)(cF4)
Lattice constant
Cubic-face-centered.svg
a = 380.34 pm (at 20 °C) [3]
Thermal expansion 8.46×10−6/K (at 20 °C) [3]
Thermal conductivity 150 W/(m⋅K)
Electrical resistivity 43.3 nΩ⋅m(at 0 °C)
Magnetic ordering paramagnetic [6]
Molar magnetic susceptibility +111.0×10−6 cm3/mol(298 K) [7]
Young's modulus 380 GPa
Shear modulus 150 GPa
Bulk modulus 275 GPa
Speed of sound thin rod4700 m/s(at 20 °C)
Poisson ratio 0.26
Mohs hardness 6.0
Vickers hardness 1100–8000 MPa
Brinell hardness 980–1350 MPa
CAS Number 7440-16-6
History
Discovery and first isolation William Hyde Wollaston (1804)
Isotopes of rhodium
Main isotopes [8] Decay
abun­dance half-life (t1/2) mode pro­duct
99Rh synth 16.1 d β+ 99Ru
101Rhsynth4.07 y ε 101Ru
101mRhsynth4.343 dε 101Ru
IT 101Rh
102Rhsynth207 dβ+ 102Ru
β− 102Pd
102mRhsynth3.742 yβ+102Ru
IT102Rh
103Rh100% stable
105Rhsynth35.341 hβ− 105Pd
Symbol category class.svg  Category: Rhodium
| references

Rhodium is a chemical element; it has symbol Rh and atomic number 45. It is a very rare, silvery-white, hard, corrosion-resistant transition metal. It is a noble metal and a member of the platinum group. It has only one naturally occurring isotope, which is 103Rh. Naturally occurring rhodium is usually found as a free metal or as an alloy with similar metals and rarely as a chemical compound in minerals such as bowieite and rhodplumsite. It is one of the rarest and most valuable precious metals.

Contents

Rhodium is found in platinum or nickel ores with the other members of the platinum group metals. It was discovered in 1803 by William Hyde Wollaston in one such ore, and named for the rose color of one of its chlorine compounds.

The element's major use (consuming about 80% of world rhodium production) is as one of the catalysts in the three-way catalytic converters in automobiles. Because rhodium metal is inert against corrosion and most aggressive chemicals, and because of its rarity, rhodium is usually alloyed with platinum or palladium and applied in high-temperature and corrosion-resistive coatings. White gold is often plated with a thin rhodium layer to improve its appearance, while sterling silver is often rhodium-plated to resist tarnishing. Rhodium is sometimes used to cure silicones: a two-part silicone in which one part containing a silicon hydride and the other containing a vinyl-terminated silicone are mixed; one of these liquids contains a rhodium complex. [9]

Rhodium detectors are used in nuclear reactors to measure the neutron flux level. Other uses of rhodium include asymmetric hydrogenation used to form drug precursors and the processes for the production of acetic acid.

History

William Hyde Wollaston Wollaston William Hyde Jackson color.jpg
William Hyde Wollaston

Rhodium (Greek rhodon (ῥόδον) meaning "rose") was discovered in 1803 by William Hyde Wollaston, [10] soon after he discovered palladium. [11] [12] [13] He used crude platinum ore presumably obtained from South America. [14] His procedure dissolved the ore in aqua regia and neutralized the acid with sodium hydroxide (NaOH). He then precipitated the platinum as ammonium chloroplatinate by adding ammonium chloride (NH
4Cl). Most other metals like copper, lead, palladium, and rhodium were precipitated with zinc. Diluted nitric acid dissolved all but palladium and rhodium. Of these, palladium dissolved in aqua regia but rhodium did not, [15] and the rhodium was precipitated by the addition of sodium chloride as Na
3[RhCl
6]·nH
2O. After being washed with ethanol, the rose-red precipitate was reacted with zinc, which displaced the rhodium in the ionic compound and thereby released the rhodium as free metal. [16]

For decades, the rare element had only minor applications; for example, by the turn of the century, rhodium-containing thermocouples were used to measure temperatures up to 1800 °C. [17] [18] They have exceptionally good stability in the temperature range of 1300 to 1800 °C. [19]

The first major application was electroplating for decorative uses and as corrosion-resistant coating. [20] The introduction of the three-way catalytic converter by Volvo in 1976 increased the demand for rhodium. The previous catalytic converters used platinum or palladium, while the three-way catalytic converter used rhodium to reduce the amount of NOx in the exhaust. [21] [22] [23]

Characteristics

Z Element No. of electrons/shell
27cobalt2, 8, 15, 2
45rhodium2, 8, 18, 16, 1
77iridium2, 8, 18, 32, 15, 2
109meitnerium2, 8, 18, 32, 32, 15, 2 (predicted)

Rhodium is a hard, silvery, durable metal that has a high reflectance. Rhodium metal does not normally form an oxide, even when heated. [24] Oxygen is absorbed from the atmosphere only at the melting point of rhodium, but is released on solidification. [25] Rhodium has both a higher melting point and lower density than platinum. It is not attacked by most acids: it is completely insoluble in nitric acid and dissolves slightly in aqua regia.

Chemical properties

Wilkinson's catalyst Wilkinson's-catalyst-2D.png
Wilkinson's catalyst

Rhodium belongs to group 9 of the periodic table, but exhibits an atypical ground state valence electron configuration for that group. Like neighboring elements niobium (41), ruthenium (44), and palladium (46), it only has one electron in its outermost s orbital.

Oxidation states
of rhodium
+0Rh
4(CO)
12
+1RhCl(PH
3)
2
+2Rh
2(O
2CCH
3)
4
+3RhCl
3, Rh
2O
3
+4RhO
2
+5RhF
5, Sr
3LiRhO
6
+6RhF
6

The common oxidation state of rhodium is +3, but oxidation states from 0 to +7 are also observed. [26] [27]

Unlike ruthenium and osmium, rhodium forms no volatile oxygen compounds. The known stable oxides include Rh
2O
3 , RhO
2 , RhO
2·xH
2O, Na
2RhO
3, Sr
3LiRhO
6 and Sr
3NaRhO
6. [28] Halogen compounds are known in nearly the full range of possible oxidation states. Rhodium(III) chloride, rhodium trifluoride, rhodium pentafluoride and rhodium hexafluoride are examples. The lower oxidation states are stable only in the presence of ligands. [29]

The best-known rhodium-halogen compound is the Wilkinson's catalyst chlorotris(triphenylphosphine)rhodium(I). This catalyst is used in the hydroformylation or hydrogenation of alkenes. [30]

Isotopes

Naturally occurring rhodium is composed of only one isotope, 103Rh. The most stable radioisotopes are 101Rh with a half-life of 3.3 years, 102Rh with a half-life of 207 days, 102mRh with a half-life of 2.9 years, and 99Rh with a half-life of 16.1 days. Twenty other radioisotopes have been characterized with atomic weights ranging from 92.926 u (93Rh) to 116.925 u (117Rh). Most of these have half-lives shorter than an hour, except 100Rh (20.8 hours) and 105Rh (35.36 hours). Rhodium has numerous meta states, the most stable being 102mRh (0.141 MeV) with a half-life of about 2.9 years and 101mRh (0.157 MeV) with a half-life of 4.34 days (see isotopes of rhodium). [31]

In isotopes weighing less than 103 (the stable isotope), the primary decay mode is electron capture and the primary decay product is ruthenium. In isotopes greater than 103, the primary decay mode is beta emission and the primary product is palladium. [32]

Occurrence

Rhodium is one of the rarest elements in the Earth's crust, comprising an estimated 0.0002 parts per million (2 × 10−10). [33] Its rarity affects its price and its use in commercial applications. The concentration of rhodium in nickel meteorites is typically 1 part per billion. [34] Rhodium has been measured in some potatoes with concentrations between 0.8 and 30 ppt. [35]

Mining and price

Rh price evolution Rh price.png
Rh price evolution
Rhodium daily price 1992-2022 Rhodium daily Price 1992-2022.webp
Rhodium daily price 1992–2022

The industrial extraction of rhodium is complex because the ores are mixed with other metals such as palladium, silver, platinum, and gold and there are very few rhodium-bearing minerals. It is found in platinum ores and extracted as a white inert metal that is difficult to fuse. Principal sources are located in South Africa; in river sands of the Ural Mountains in Russia; and in North America, including the copper-nickel sulfide mining area of the Sudbury, Ontario, region. Although the rhodium abundance at Sudbury is very small, the large amount of processed nickel ore makes rhodium recovery cost-effective.

The main exporter of rhodium is South Africa (approximately 80% in 2010) followed by Russia. [36] The annual world production is 30 tonnes. The price of rhodium is highly variable.

Used nuclear fuels

Rhodium is a fission product of uranium-235: each kilogram of fission product contains a significant amount of the lighter platinum group metals. Used nuclear fuel is therefore a potential source of rhodium, but the extraction is complex and expensive, and the presence of rhodium radioisotopes requires a period of cooling storage for multiple half-lives of the longest-lived isotope (101Rh with a half-life of 3.3 years, and 102mRh with a half-life of 2.9 years), or about 10 years. These factors make the source unattractive and no large-scale extraction has been attempted. [37] [38] [39]

Applications

The primary use of this element is in automobiles as a catalytic converter, changing harmful unburned hydrocarbons, carbon monoxide, and nitrogen oxide exhaust emissions into less noxious gases. Of 30,000 kg of rhodium consumed worldwide in 2012, 81% (24,300 kg) went into this application, and 8,060 kg was recovered from old converters. About 964 kg of rhodium was used in the glass industry, mostly for production of fiberglass and flat-panel glass, and 2,520 kg was used in the chemical industry. [36]

Catalyst

Rhodium is preferable to the other platinum metals in the reduction of nitrogen oxides to nitrogen and oxygen: [40]

2 NO
x → xO
2 + N
2

In 2008, net demand (with the recycling accounted for) of rhodium for automotive converters made up 84% of the world usage, [41] with the number fluctuating around 80% in 2015−2021. [42]

Rhodium catalysts are used in a number of industrial processes, notably in catalytic carbonylation of methanol to produce acetic acid by the Monsanto process. [43] It is also used to catalyze addition of hydrosilanes to molecular double bonds, a process important in manufacture of certain silicone rubbers. [44] Rhodium catalysts are also used to reduce benzene to cyclohexane. [45]

The complex of a rhodium ion with BINAP is a widely used chiral catalyst for chiral synthesis, as in the synthesis of menthol. [46]

Ornamental uses

Rhodium finds use in jewelry and for decorations. It is electroplated on white gold and platinum to give it a reflective white surface at time of sale, after which the thin layer wears away with use. This is known as rhodium flashing in the jewelry business. It may also be used in coating sterling silver to protect against tarnish (silver sulfide, Ag2S, produced from atmospheric hydrogen sulfide, H2S). Solid (pure) rhodium jewelry is very rare, more because of the difficulty of fabrication (high melting point and poor malleability) than because of the high price. [47] The high cost ensures that rhodium is applied only as an electroplate. Rhodium has also been used for honors or to signify elite status, when more commonly used metals such as silver, gold or platinum were deemed insufficient. In 1979 the Guinness Book of World Records gave Paul McCartney a rhodium-plated disc for being history's all-time best-selling songwriter and recording artist. [48]

Other uses

Rhodium is used as an alloying agent for hardening and improving the corrosion resistance [24] of platinum and palladium. These alloys are used in furnace windings, bushings for glass fiber production, thermocouple elements, electrodes for aircraft spark plugs, and laboratory crucibles. [49] Other uses include:

In automobile manufacturing, rhodium is also used in the construction of headlight reflectors. [54]

Precautions

Rhodium
Hazards
GHS labelling:
H413
P273, P501 [55]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
0
0

Being a noble metal, pure rhodium is inert and harmless in elemental form. [56] However, chemical complexes of rhodium can be reactive. For rhodium chloride, the median lethal dose (LD50) for rats is 198 mg (RhCl
3) per kilogram of body weight. [57] Like the other noble metals, rhodium has not been found to serve any biological function.

People can be exposed to rhodium in the workplace by inhalation. The Occupational Safety and Health Administration (OSHA) has specified the legal limit (Permissible exposure limit) for rhodium exposure in the workplace at 0.1 mg/m3 over an 8-hour workday, and the National Institute for Occupational Safety and Health (NIOSH) has set the recommended exposure limit (REL), at the same level. At levels of 100 mg/m3, rhodium is immediately dangerous to life or health. [58] For soluble compounds, the PEL and REL are both 0.001 mg/m3. [59]

See also

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References

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  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. (4 May 2022). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN   1365-3075.
  3. 1 2 3 Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN   978-1-62708-155-9.
  4. ↑ Ellis J E. Highly Reduced Metal Carbonyl Anions: Synthesis, Characterization, and Chemical Properties. Adv. Organomet. Chem, 1990, 31: 1-51.
  5. ↑ Rh(VII) is known in the RhO3+ cation, see Da Silva Santos, Mayara; Stüker, Tony; Flach, Max; Ablyasova, Olesya S.; Timm, Martin; von Issendorff, Bernd; Hirsch, Konstantin; Zamudio‐Bayer, Vicente; Riedel, Sebastian; Lau, J. Tobias (2022). "The Highest Oxidation State of Rhodium: Rhodium(VII) in [RhO3]+". Angew. Chem. Int. Ed. 61 (38): e202207688. doi:10.1002/anie.202207688. PMC   9544489 . PMID   35818987.
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  11. ↑ Griffith, W. P. (2003). "Rhodium and Palladium – Events Surrounding Its Discovery". Platinum Metals Review. 47 (4): 175–183. doi: 10.1595/003214003X474175183 .
  12. ↑ Wollaston, W. H. (1805). "On the Discovery of Palladium; With Observations on Other Substances Found with Platina". Philosophical Transactions of the Royal Society of London . 95: 316–330. doi: 10.1098/rstl.1805.0024 .
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  14. ↑ Lide, David R. (2004). CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data . Boca Raton: CRC Press. pp.  4–26. ISBN   978-0-8493-0485-9.
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