|
|
| Appearance |
silvery white metallic
 |
| General properties |
| Name, symbol, number |
ruthenium, Ru, 44 |
| Pronunciation |
/ruːˈθiːniəm/
roo-THEE-nee-əm |
| Element category |
transition metal |
| Group, period, block |
8, 5, d |
| Standard atomic weight |
101.07 |
| Electron configuration |
[Kr] 4d7 5s1 |
| Electrons per shell |
2, 8, 18, 15, 1 (Image) |
| Physical properties |
| Density (near r.t.) |
12.45 g·cm−3 |
| Liquid density at m.p. |
10.65 g·cm−3 |
| Melting point |
2607 K, 2334 °C, 4233 °F |
| Boiling point |
4423 K, 4150 °C, 7502 °F |
| Heat of fusion |
38.59 kJ·mol−1 |
| Heat of vaporization |
591.6 kJ·mol−1 |
| Molar heat capacity |
24.06 J·mol−1·K−1 |
| Vapor pressure |
| P (Pa) |
1 |
10 |
100 |
1 k |
10 k |
100 k |
| at T (K) |
2588 |
2811 |
3087 |
3424 |
3845 |
4388 |
|
| Atomic properties |
| Oxidation states |
8, 7, 6, 4, 3, 2, 1,[1], -2
(mildly acidic oxide) |
| Electronegativity |
2.2 (Pauling scale) |
| Ionization energies |
1st: 710.2 kJ·mol−1 |
| 2nd: 1620 kJ·mol−1 |
| 3rd: 2747 kJ·mol−1 |
| Atomic radius |
134 pm |
| Covalent radius |
146±7 pm |
| Miscellanea |
| Crystal structure |
hexagonal |
| Magnetic ordering |
paramagnetic[2] |
| Electrical resistivity |
(0 °C) 71 nΩ·m |
| Thermal conductivity |
117 W·m−1·K−1 |
| Thermal expansion |
(25 °C) 6.4 µm·m−1·K−1 |
| Speed of sound (thin rod) |
(20 °C) 5970 m·s−1 |
| Young's modulus |
447 GPa |
| Shear modulus |
173 GPa |
| Bulk modulus |
220 GPa |
| Poisson ratio |
0.30 |
| Mohs hardness |
6.5 |
| Brinell hardness |
2160 MPa |
| CAS registry number |
7440-18-8 |
| Most stable isotopes |
| Main article: Isotopes of ruthenium |
|
|
|
· r |
Ruthenium (
/ruːˈθiːniəm/ roo-THEE-nee-əm) is a chemical element with symbol Ru and atomic number 44. It is a rare transition metal belonging to the platinum group of the periodic table. Like the other metals of the platinum group, ruthenium is inert to most chemicals. The Russian scientist Karl Ernst Claus discovered the element in 1844 and named it after Ruthenia, the Latin word for Rus' (ancient Russia). Ruthenium usually occurs as a minor component of platinum ores and its annual production is only about 20 tonnes [3]. Most ruthenium is used for wear-resistant electrical contacts and the production of thick-film resistors. A minor application of ruthenium is its use in some platinum alloys.
A polyvalent hard white metal, ruthenium is a member of the platinum group and is in group 8 of the periodic table:
| Z |
Element |
No. of electrons/shell |
| 26 |
iron |
2, 8, 14, 2 |
| 44 |
ruthenium |
2, 8, 18, 15, 1 |
| 76 |
osmium |
2, 8, 18, 32, 14, 2 |
| 108 |
hassium |
2, 8, 18, 32, 32, 14, 2 |
However, it has an atypical configuration in its outermost electron shells: whereas all other group 8 elements have 2 electrons in the outermost shell, in ruthenium, one of those is transferred to a lower shell. This effect can be observed in the neighboring metals niobium (41), rhodium (45), and palladium (46).
Ruthenium has four crystal modifications and does not tarnish at normal temperatures. Ruthenium dissolves in fused alkalis, is not attacked by acids but is attacked by halogens at high temperatures. Small amounts of ruthenium can increase the hardness of platinum and palladium. The corrosion resistance of titanium is increased markedly by the addition of a small amount of ruthenium.[4]
This metal can be plated either by electroplating or by thermal decomposition methods. A ruthenium-molybdenum alloy is known to be superconductive at temperatures below 10.6 K.[4]
Naturally occurring ruthenium is composed of seven stable isotopes. Additionally, 34 radioactive isotopes have been discovered. Of these radioisotopes, the most stable are 106Ru with a half-life of 373.59 days, 103Ru with a half-life of 39.26 days and 97Ru with a half-life of 2.9 days.[5][6]
Fifteen other radioisotopes have been characterized with atomic weights ranging from 89.93 u (90Ru) to 114.928 u (115Ru). Most of these have half-lives that are less than five minutes except 95Ru (half-life: 1.643 hours) and 105Ru (half-life: 4.44 hours).[5][6]
The primary decay mode before the most abundant isotope, 102Ru, is electron capture and the primary mode after is beta emission. The primary decay product before 102Ru is technetium and the primary mode after is rhodium.[5][6]
Ruthenium is exceedingly rare, only the 74th most abundant metal on Earth.[7] This element is generally found in ores with the other platinum group metals in the Ural Mountains and in North and South America. Small but commercially important quantities are also found in pentlandite extracted from Sudbury, Ontario, Canada, and in pyroxenite deposits in South Africa. The native form of ruthenium is a very rare mineral (Ir replaces part of Ru in its structure).[8][9]
Roughly 12 tonnes of Ru is mined each year with world reserves estimated as 5,000 tonnes.[7] The composition of the mined platinum group metal (PGM) mixtures varies in a wide range depending on the geochemical formation. For example, the PGMs mined in South Africa contain on average 11% ruthenium while the PGMs mined in the former USSR contain only 2% based on research dating from 1992.[10][11]
Ruthenium, like the other platinum group metals, is obtained commercially as a by-product from nickel and copper mining and processing as well as by the processing of platinum group metal ores. During electrorefining of copper and nickel, noble metals such as silver, gold and the platinum group metals settle to the bottom of the cell as anode mud, which forms the starting point for their extraction.[8][9] In order to separate the metals, they must first be brought into solution. Several methods are available 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.[12][13] Osmium, ruthenium, rhodium and iridium can be separated from platinum and 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 Ru, Os and Ir is treated with sodium oxide, in which Ir is insoluble, producing water-soluble Ru and Os salts. After oxidation to the volatile oxides, RuO4 is separated from OsO4 by precipitation of (NH4)3RuCl6 with ammonium chloride or by distillation or extraction with organic solvents of the volatile osmium tetroxide.[14] Hydrogen is used to reduce ammonium ruthenium chloride yielding a powder.[15] The first method to precipitate the ruthenium with ammonium chloride is similar to the procedure that Smithson Tennant and William Hyde Wollaston used for their separation. Several 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 or by argon-arc welding.[16]
Fission products of uranium-235 contain significant amounts of ruthenium and the lighter platinum group metals{clarify|date = April 2012} and therefore used nuclear fuel might be a possible source of ruthenium. The complicated extraction is expensive and the radioactive isotopes of ruthenium that are present would make storage for several half-lives of the decaying isotopes necessary. This makes this source of ruthenium unattractive and no large-scale extraction has been started.[17][18][19]
The oxidation states of ruthenium range from 0 to +8, and −2. The properties of ruthenium and osmium compounds are often similar. The +2, +3, and +4 states are the most common. The most prevalent precursor is ruthenium trichloride, a red solid that is poorly defined chemically but versatile synthetically.[15]
Ru can oxidized to ruthenium(IV) oxide (RuO2, oxidation state +4) which can in turn be oxidised by sodium metaperiodate to ruthenium tetroxide, RuO4, a strong oxidizing agent with structure and properties analogous to osmium tetroxide. Like osmium tetroxide, ruthenium tetroxide is a potent fixative and stain for electron microscopy of organic materials, and is mostly used to reveal the structure of polymer samples.[20] Dipotassium ruthenate (K2RuO4, +6), and potassium perruthenate (KRuO4, +7) are also known.[21]
Tris(bipyridine)ruthenium(II) chloride.
Ruthenium forms a variety of coordination complexes. Examples are the many pentammine derivatives [Ru(NH3)5L]n+ which often exist in both Ru(II) and Ru(III). Derivatives of bipyridine and terpyridine are numerous, best known being the luminiscent tris(bipyridine)ruthenium(II) chloride.
Ruthenium form a wide range compounds with carbon-ruthenium bonds. Ruthenocene is analogous to ferrocene structurally, but exhibits distinctive redox properties. A large number of complexes of carbon monoxide are known, the parent being triruthenium dodecacarbonyl. The analogue of iron pentacarbonyl, ruthenium pentacarbonyl is unstable at ambient conditions. Ruthenium trichloride carbonylates (reacts with carbon monoxide) to give mono- and diruthenium(II) carbonyls from which many derivatives have been prepared such as RuHCl(CO)(PPh3)3 and Ru(CO)2(PPh3)3 (Roper's complex). Heating solutions of ruthenium trichloride in alcohols with triphenylphosphine gives tris(triphenylphosphine)ruthenium dichloride (RuCl2(PPh3)3), which converts to the hydride complex chlorohydridotris(triphenylphosphine)ruthenium(II) (RuHCl(PPh3)3).[15]
In the area of fine chemical synthesis, Grubbs' catalyst is used for alkene metathesis.[22]
Metal Ruthenides (Ru2-) are very rare, but are commonly found in superconductor applications, especially with regard to lanthanide metals e.g. cerium ruthenide (CeRu2).[23]
Though naturally occurring platinum alloys containing all six platinum group metals were used for a long time by pre-Columbian Americans and known as a material to European chemists from the mid-16th century, it took until the mid-18th century for platinum to be identified as a pure element. The discovery that natural platinum contained palladium, rhodium, osmium and iridium occurred in the first decade of the 19th century.[24] Platinum in alluvial sands of Russian rivers gave access to raw material for use in plates and medals and for the minting of ruble coins, starting in 1828.[25] Residues of platinum production for minting were available in the Russian Empire, and therefore most of the research on them was done in Eastern Europe.
It is possible that the Polish chemist Jędrzej Śniadecki isolated element 44 (which he called "vestium") from platinum ores in 1807. He published his discovery in Polish language in article "Rosprawa o nowym metallu w surowey platynie odkrytym" in 1808. His work was never confirmed, however, and he later withdrew his claim of discovery.[7] Jöns Berzelius and Gottfried Osann nearly discovered ruthenium in 1827.[26] They examined residues that were left after dissolving crude platinum from the Ural Mountains in aqua regia. Berzelius did not find any unusual metals, but Osann thought he found three new metals, pluranium, ruthenium and polinium. This discrepancy led to a long-standing controversy between Berzelius and Osann about the composition of the residues.[27]
In 1844, the Russian scientist Karl Klaus showed that the compounds prepared by Gottfried Osann contained small amounts of ruthenium, which Klaus had discovered the same year.[24] Klaus isolated ruthenium from the platinum residues of the rouble production while he was working in Kazan University, Kazan.[27] Klaus showed that ruthenium oxide contained a new metal and obtained 6 grams of ruthenium from the part of crude platinum that is insoluble in aqua regia.[27]
The name derives from Ruthenia, the Latin word for Rus', a historical area which includes present-day western Russia, Ukraine, Belarus, and parts of Slovakia and Poland. Karl Klaus used the name proposed by Gottfried Osann in 1828. He chose the element's name in honor of his birthland, as he was born in Tartu, Estonia, which was at the time a part of the Russian Empire.[24][28]
Because of its ability to harden platinum and palladium, ruthenium is used in platinum and palladium alloys to make wear-resistant electrical contacts. In this application, only thin plated films are used to achieve the necessary wear-resistance. Because of its lower cost and similar properties compared to rhodium,[16] the use as plating material for electric contacts is one of the major applications.[8][29] The thin coatings are either applied by electroplating[30] or sputtering.[31]
Ruthenium dioxide and lead and bismuth ruthenates are used in thick film chip resistors.[32][33][34] These two electronic applications account for 50% of the ruthenium consumption.[7]
Only a few ruthenium alloys are used other than those with other platinum group metals. Ruthenium is often used in small quantities in those alloys to improve certain of their properties.[clarification needed] The beneficial effect on the corrosion resistance of titanium alloys led to the development of a special alloy containing 0.1% ruthenium .[35] Ruthenium is also used in some advanced high-temperature single-crystal superalloys, with applications including the turbine blades in jet engines. Several nickel based superalloy compositions are described in the literature. Among them are EPM-102 (with 3 % Ru) and TMS-162 (with 6 % Ru), as well as TMS-138[36] and TMS-174.[37][38] both containing 6 % rhenium,[39]. Fountain pen nibs are frequently tipped with alloys containing ruthenium. From 1944 onward, the famous Parker 51 fountain pen was fitted with the "RU" nib, a 14K gold nib tipped with 96.2% ruthenium and 3.8% iridium.[40]
Ruthenium is a component of mixed-metal oxide (MMO) anodes used for cathodic protection of underground and submerged structures, and for electrolytic cells for chemical processes such as generating chlorine from salt water.[41] The fluorescence of some ruthenium complexes is quenched by oxygen, which has led to their use as optode sensors for oxygen.[42] Ruthenium red, [(NH3)5Ru-O-Ru(NH3)4-O-Ru(NH3)5]6+, is a biological stain used to stain polyanionic molecules such as pectin and nucleic acids for light microscopy and electron microscopy.[43] The beta-decaying isotope 106 of ruthenium is used in radiotherapy of eye tumors, mainly malignant melanomas of the uvea.[44] Ruthenium-centered complexes are being researched for possible anticancer properties.[45] Compared with platinum complexes, those of ruthenium show greater resistance to hydrolysis and more selective action on tumors.[citation needed] NAMI-A and KP1019 are two drugs undergoing clinical evaluation against metastatic tumors and colon cancers.
Ruthenium is a versatile catalyst. Hydrogen sulfide can be split by light by using an aqueous suspension of CdS particles loaded with ruthenium dioxide. This may be useful in the removal of H2S in oil refineries and other industrial processing facilities.[46] Organometallic ruthenium carbene and alkylidene complexes have been found to be highly efficient catalysts for olefin metathesis, a process with important applications in organic and pharmaceutical chemistry.[47]
Some ruthenium complexes absorb light throughout the visible spectrum and are being actively researched in various, potential, solar energy technologies. For example, Ruthenium-based compounds have been used for light absorption in dye-sensitized solar cells, a promising new low-cost solar cell system.[48]
Chemical vapor deposition of ruthenium (CVD) is used as a method to produce thin films of pure ruthenium on substrates. These films show promising properties for the use in microchips and for the giant magnetoresistive read element for hard disk drives.[49] Ruthenium was also suggested as a possible material for microelectronics because its use is compatible with semiconductor processing techniques.[50]
Many ruthenium based oxides show very unusual properties, such as a quantum critical point behavior,[51] exotic superconductivity,[52] and high temperature ferromagnetism.[53]
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- ^ Shlyk, Larysa; Kryukov, Sergiy; Schüpp-Niewa, Barbara; Niewa, Rainer; De Long, Lance E. (2008). "High-Temperature Ferromagnetism and Tunable Semiconductivity of (Ba, Sr)M2±xRu4∓xO11 (M = Fe, Co): A New Paradigm for Spintronics". Advanced Materials 20 (7): 1315. DOI:10.1002/adma.200701951.
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Chemical elements named after places
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| Named after terrestrial places |
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| Named after astronomical objects |
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vep:Rutenii
ruthenium(II)-chloride-powder.jpg)
