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Ruthenium red, [ (NH 3) 5 Ru-O-Ru (NH 3) 4 -O-Ru (NH 3) 5] 6+, is a biological stain used to stain polyanionic molecules such as pectin and nucleic acids for light microscopy and electron microscopy. [64] The beta-decaying isotope 106 of ruthenium is used in radiotherapy of eye tumors, mainly malignant melanomas of the uvea. [65]
primordial element. synthetic element. Group 8 is a group (column) of chemical elements in the periodic table. It consists of iron (Fe), ruthenium (Ru), osmium (Os) and hassium (Hs). [1] ". Group 8" is the modern standard designation for this group, adopted by the IUPAC in 1990. [1] It should not be confused with "group VIIIA" in the CAS system ...
Osmium (II) chloride, iridium (II) chloride, platinum (II) chloride. Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references. Ruthenium (II) chloride is an inorganic compound, a metal salt of ruthenium and hydrochloric acid with the formula RuCl. 2. [1][2]
The six platinum-group metals are ruthenium, rhodium, palladium, osmium, iridium, and platinum. They have similar physical and chemical properties, and tend to occur together in the same mineral deposits. [ 2 ]
Ruthenium compounds are compounds containing the element ruthenium (Ru). Ruthenium compounds can have oxidation states ranging 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 ...
Naturally occurring ruthenium (44 Ru) is composed of seven stable isotopes (of which two may in the future be found radioactive). Additionally, 27 radioactive isotopes have been discovered. Of these radioisotopes, the most stable are 106 Ru, with a half-life of 373.59 days; 103 Ru, with a half-life of 39.26 days and 97 Ru, with a half-life of 2 ...
Ruthenium (IV) oxide is the inorganic compound with the formula Ru O 2. This black solid is the most common oxide of ruthenium. It is widely used as an electrocatalyst for producing chlorine, chlorine oxides, and O 2. [1] Like many dioxides, RuO 2 adopts the rutile structure. [2][3]
The physical properties of the refractory elements vary significantly because they are members of different groups of the periodic table. [ 6 ] [ 7 ] The hardness, high melting and boiling points, and high enthalpies of atomization of these metals arise from the partial occupation of the outer d subshell , allowing the d electrons to ...