|Boiling Point: 4173°K, 3900°C, 7052°F
Melting Point: 2523°K, 2250°C, 4082°F
Electrons Energy Level: 2, 8, 18, 15, 1
Isotopes: 27 + 7 Stable
Heat of Vaporization: 595 kJ/mol
Heat of Fusion: 24 kJ/mol
Density: 12.37 g/cm3 @ 300°K
Specific Heat: 0.238 J/g°K
Atomic Radius: 1.89Å
Ionic Radius: 0.68Å
Electronegativity: 2.2 (Pauling); 1.42 (Allrod Rochow)
Vapor Pressure: 1.4 Pa @ 2250°C
1s2 2s2p6 3s2p6d10 4s2p6d7 5s1
Ruthenium was discovered and isolated by Russian scientist Karl Karlovich Klaus in 1844. 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.
Jons Jakob Berzelius and Gottfried Osann nearly discovered ruthenium in 1827. The men 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 and named one of them ruthenium.
The name derives from Ruthenia the Latin word for Russia, a historical area which includes present day Ukraine, Belarus, and parts of the Russia, Baltics, Slovakia and Poland. Karl Klaus called the element in honour of his birthland. He was born in Tartu, Estonia.
It is also possible that Polish chemist Jedrzej Sniadecki isolated element 44 (which he called vestium) from platinum ores in 1807. However his work was never confirmed and he later withdrew his discovery claim.
A polyvalent hard white metal, ruthenium is a member of the platinum group, has four crystal modifications and does not tarnish at normal temperatures, but does oxidize explosively. 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.
This metal can be plated either through electrodeposition or by thermal decomposition methods. One ruthenium-molybdenum alloy has been found to be superconductive at 10.6oK. The oxidation states of ruthenium range from +1 to +8, and -2 is known, though oxidation states of +2, +3, and +4 are most common.
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.
This metal is commercially isolated through a complex chemical process in which hydrogen is used to reduce ammonium ruthenium chloride yielding a powder. The powder is then consolidated by powder metallurgy techniques or by argon-arc welding.
It is also possible to extract ruthenium from spent nuclear fuel, which contains an average of 2 kg of ruthenium per metric ton. Ruthenium produced in such a way contains radioactive isotopes, some with a half-life of up to 373.59 days. Therefore this ruthenium has to be stored at least for 10 years in a secured area to allow it to become stable. Fission-derived ruthenium has a specific activity of 8.1 curies of radioactivity per gram. Under health physics safety rules any isotope that emits more than 1 ci of activity is a hazard; however, after 6 years the activity falls to 4.1 ci, after 7 years it is 2.2, after 8 years 1.1, after 9 years .55 ci and after 10 years only .27 ci. After 20 years the activity falls to 2.702E-4 ci, which is under the threshold for low level risk by even the most stringent health physics rules.
Due to its highly effective ability to harden platinum and palladium, ruthenium is used in Pt and Pd alloys to make severe wear-resistant electrical contacts. It is sometimes alloyed with gold in jewelry.
Ruthenium is also 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 from oil refineries and from other industrial processes.
Organometallic ruthenium carbene and allenylidene complexes have recently been found as highly efficient catalysts forolefin metathesis with important applications in organic and pharmaceutical chemistry.
Recently, large metallo-organic complexes of ruthenium have been found to exhibit anti-tumor activity and the first of a new group of anti-cancer medicine are now in the stage of clinical trials.
Some ruthenium complexes absorb light throughout the visible spectrum and are being actively researched in various, potential, solar energy technologies.
Ruthenium will also be used in some advanced high-temperature single-crystal superalloys, with applications including the turbine blades in jet engines.
Ruthenium red, [(NH3)5Ru-O-Ru(NH3)4-O-Ru(NH3)5]6+, is a biological stain used to visualize polyanionic areas of membranes.
Ruthenium-centered complexes are being researched for possible anticancer properties. Ruthenium, unlike traditional platinum complexes, show greater resistance to hydrolysis and more selective action on tumors. NAMI-A and KP1019 are two drugs undergoing clinical evaluation against metastatic tumors and colon cancers.
Fountain pen nibs are frequently tipped with alloys containing ruthenium. From 1944 onward, the famous Parker 51 fountain pen was outfitted with the "RU" nib, a 14K gold nib tipped with 96.2% ruthenium, 3.8% iridium.
Ruthenium compounds are often similar in properties to those of osmium and exhibit at least eight oxidation states, but the +2, +3, and +4 states are the most common. Examples are ruthenium (IV) oxide (Ru(IV)O2, oxidation state +4), dipotassium ruthenate (K2Ru(VI)O4, +6), potassium perruthenate (KRu(VII)O4, +7) and ruthenium tetroxide (Ru(VIII)O4, +8). Compounds of ruthenium with chlorine are ruthenium (II) chloride (RuCl2) and ruthenium (III) chloride (RuCl3).
|Ruthenium (II) Chloride, RuCl2||Ruthenium (III) Chloride, RuCl3|
|Ruthenium (IV) Oxide, RuO2||Dipotassium (VI) Ruthenate, K2RuO4|
|Potassium (VII) Perruthenate, KRuO4||Ruthenium (VIII) Tetroxide, RuO4|
It is quite easy to form compounds with carbon ruthenium bonds, these compounds tend to be darker and react more quickly than the osmium compounds. Recently Prof Tony Hill and his co-workers have been making compounds of ruthenium in which a boron atom binds to the metal atom.
The organometallic ruthenium compound that is easiest to make is RuHCl(CO)(PPh3)3. This compound has two forms (yellow and pink) that are identical once they are dissolved but different in the solid state.
An organometallic compound similar to ruthenocene, bis(2,4-dimethylpentadienyl)ruthenium, is readily synthesized in near quantitative yields and has applications in vapor-phase deposition of metallic ruthenium, as well as in catalysis, including Fischer-Tropsch synthesis of transportation fuels.
Important catalysts based on ruthenium are Grubbs' catalyst and Roper's complex.
Naturally occurring ruthenium is composed of seven isotopes. The most stable radioisotopes 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.
Twenty-seven other radioisotopes have been characterized with atomic weights ranging from 86.9 amu (87Ru) to 119.9 (120Ru). 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).
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.
|The compound ruthenium tetroxide, RuO4, similar to osmium tetroxide, is highly toxic and may explode. Ruthenium plays no biological role but does strongly stain human skin, may be carcinogenic and bio-accumulates in bone.|
|Ionization Energy (eV): 7.361 eV
Estimated Crustal Abundance: 1×10-3 milligrams per kilogram
Estimated Oceanic Abundance: 7×10-7 milligrams per liter