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Rhodium is a chemical element with symbol Rh and atomic number 45. It is a rare, silvery-white, hard, and chemically inert transition metal. It is a member of the platinum group. It has only one naturally occurring isotope, 103Rh. Naturally occurring rhodium is usually found as the free metal, alloyed 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.

Rhodium is a noble metal, resistant to corrosion, found in platinum- or nickel ores together 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, produced after it reacted with the powerful acid mixture aqua regia.

The element's major use (approximately 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 for tarnish resistance.

Rhodium detectors are used in nuclear reactors to measure the neutron flux level.

HistoryEdit

File:Wollaston William Hyde Jackson color.jpg

Rhodium (Greek rhodon (ῥόδον) meaning "rose") was discovered in 1803 by William Hyde Wollaston,[1] soon after his discovery of palladium.[2][3][4] He used crude platinum ore presumably obtained from South America.[5] His procedure involved dissolving the ore in aqua regia and neutralizing the acid with sodium hydroxide (NaOH). He then precipitated the platinum as ammonium chloroplatinate by adding ammonium chloride (NH
4
Cl
). Most other metals like Cu, Pb, Pd and Rh were precipitated with Zn. Diluted nitric acid dissolved all but palladium and rhodium, which were dissolved in aqua regia, and the rhodium was precipitated by the addition of sodium chloride as Na
3
[RhCl
6
nH
2
O
. 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.[6]

After the discovery, 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.[7][8] The first major application was electroplating for decorative uses and as corrosion-resistant coating.[9] 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.[10][11][12]

CharacteristicsEdit

Z Element No. of electrons/shell
27 cobalt 2, 8, 15, 2
45 rhodium 2, 8, 18, 16, 1
77 iridium 2, 8, 18, 32, 15, 2
109 meitnerium 2, 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.[13] Oxygen is absorbed from the atmosphere only at the melting point of rhodium, but is released on solidification.[14] 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 propertiesEdit

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

Rhodium belongs to group 9 of the periodic table but has an atypical configuration in its outermost electron shells compared to the rest of the members. This can also be observed in the neighborhood of Template:Niobium (41), Template:Ruthenium (44), and Pd (46).

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

The common oxidation state of rhodium is +3, but oxidation states from +0 to +6 are also observed.[15]

Unlike ruthenium and osmium, rhodium forms no volatile oxygen compounds. The known stable oxides include Rh
2
O
3
, Template:RhO2, RhO
2
·xH
2
O
, Na
2
RhO
3
, Sr
3
LiRhO
6
and Sr
3
NaRhO
6
.[16] Halogen compounds are known in nearly the full range of possible oxidation states. Rhodium(III) chloride, rhodium(IV) fluoride, rhodium(V) fluoride and rhodium(VI) fluoride are some examples. The lower oxidation states are only stable if ligands are present.[17]

The best-known rhodium-halogen compound is the Wilkinson's catalyst chlorotris(triphenylphosphine)rhodium(I). This catalyst is used, for example, in the hydroformylation or hydrogenation of alkenes.[18]

IsotopesEdit

Main article: Isotopes of rhodium

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 (half-life: 20.8 hours) and 105Rh (half-life: 35.36 hours). There are also 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).[19]

The primary decay mode before the only stable isotope, 103Rh, is electron capture and the primary mode after is beta emission. The primary decay product before 103Rh is ruthenium and the primary product after is palladium.[20]

OccurrenceEdit

Rhodium is one of the rarest elements in the Earth's crust, of which it comprises an estimated 0.0002 parts per million (2 × 10−10).[21] Its rarity affects its price, and thus its usage in commercial applications.

Mining and priceEdit

File:Rh price.png

The industrial extraction of rhodium is complex, as the metal occurs in ores mixed with other metals such as Pd, Ag, Pt, and Au. It is found in platinum ores and extracted as a white inert metal which is very difficult to fuse. Principal sources are located in South Africa; in river sands of the Ural Mountains; and in North America, including the copper-nickel sulfide mining area of the Sudbury, Ontario, region. Although the quantity 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.[22] The annual world production of this element is 30 tonnes and there are very few rhodium-bearing minerals. The price of rhodium is historically highly variable. In 2007, rhodium cost approximately eight times more than gold, 450 times more than silver, and 27,250 times more than copper by weight. In 2008, the price briefly rose above $10,000 per ounce ($350,000 per kilogram). The economic slowdown of the 3rd quarter of 2008 pushed rhodium prices sharply back below $1,000 per ounce ($35,000 per kilogram); they rebounded to $2,750 by early 2010 ($97,000 per kilogram) (over twice the gold price), but in late 2013, the prices were a bit lower than $1000.[23]

Used nuclear fuelsEdit

Main article: Synthesis of precious metals

Rhodium is a fission product of uranium-235; therefore, each kilogram of fission products contains significant amounts of the lighter platinum group metals including rhodium. Used nuclear fuel might be a possible source for rhodium. However, the extraction is complex and expensive, and the also present radioactive isotopes of rhodium would require a storage for several half-lives of the longest-lived decaying isotope (i.e. about 10 years) to reduce the radioactivity. This makes this source of rhodium unattractive and no large-scale extraction has been attempted.[24][25][26]

ApplicationsEdit

The primary use of this element is in automobiles as a catalytic converter, which changes harmful unburned hydrocarbons, carbon monoxide, and nitrogen oxide emissions from the engine into less noxious gases. Of 30,000 kg of rhodium consumed worldwide in 2012, some 24,300 kg (81%) went into and 8,060 kg recovered from this application. About 964 kg of rhodium was used in the glass industry, mostly for production of fiberglass and flat-panel glass, and 2,520 kg in the chemical industry.[22]

CatalystEdit

In 2012, 81% of the world production of rhodium was consumed to produce three-way catalytic converters.[22] Rhodium shows some advantages over the other platinum metals in the reduction of nitrogen oxides to nitrogen and oxygen:[27]

2 NO
x
x O
2
+ N
2

Rhodium-based catalysts are used in a number of industrial processes; notably, in the automobile catalytic converters and for catalytic carbonylation of methanol to produce acetic acid by the Monsanto process.[28] It is also used to catalyze addition of hydrosilanes to molecular double bonds, a process important in manufacture of certain silicone rubbers.[29] Rhodium catalysts are also used to reduce benzene to cyclohexane.[30]

The complex of a rhodium ion with BINAP gives a widely used chiral catalyst for chiral synthesis, as in the synthesis of menthol.[31]

Ornamental usesEdit

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, which is silver sulfide (Ag2S) produced from the atmospheric hydrogen sulfide (H2S). Solid (pure) rhodium jewelry is very rare because the metal has both a high melting point and poor malleability, making such jewelry very hard to fabricate — rather than due to its high price.[32] Additionally, its typically higher cost assures that most of its jewelry usage is in the form of tiny amounts of powder, commonly called rhodium sponge, dissolved into electroplating solutions.

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.[33]

Other usesEdit

Rhodium is used as an alloying agent for hardening and improving the corrosion resistance[13] 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.[34] Other uses include:

  • An electrical contact material due to its low electrical resistance, low and stable contact resistance, and high corrosion resistance.[35]
  • Plated rhodium, made by electroplating or evaporation, is extremely hard and is used for optical instruments.[36]
  • It is also used as a filter in mammography systems because of the characteristic X-rays it produces.[37]
  • Rhodium neutron detectors are used in combustion engineering nuclear reactors to measure neutron flux levels – a method that requires a digital filter to determine the current neutron flux level, as there are three signals generated: immediate, a few seconds later, and a minute later, each with its own signal level, and all three are combined in the rhodium detector signals. The three Palo Verde nuclear reactors each have 305 rhodium neutron detectors, 61 detectors on each of five vertical levels, providing an accurate 3D "picture" of reactivity and allowing fine tuning to most economically burn the nuclear fuel.[38]

PrecautionsEdit

Being a noble metal, pure rhodium is inert. However, chemical complexes of rhodium can be reactive. Median lethal dose (LD50) for rats is 198 mg of rhodium chloride (RhCl
3
) per kilogram of body weight.[39] Like the other noble metals, all of which are too inert to occur as chemical compounds in nature, rhodium has not been found to play any biological role. If used in elemental form rather than as compounds, the metal is harmless.[40]

See alsoEdit

ReferencesEdit

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  17. Griffith, W. P. The Rarer Platinum Metals, John Wiley and Sons: New York, 1976, p. 313.
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  20. David R. Lide (ed.), Norman E. Holden in CRC Handbook of Chemistry and Physics, 85th Edition CRC Press. Boca Raton, Florida (2005). Section 11, Table of the Isotopes.
  21. Barbalace, Kenneth, "Table of Elements". Environmental Chemistry.com; retrieved 2007-04-14.
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