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Gallium does not occur as a free element in nature, but rather as gallium(III) compounds in trace amounts in zinc ores (such as sphalerite) and in bauxite. Elemental gallium is a liquid at temperatures greater than 29.76 °C (85.57 °F), and will melt in a person's hands at normal human body temperature of 37.0 °C (98.6 °F).
Compounds containing Ga–Ga bonds are true gallium(II) compounds, such as GaS (which can be formulated as Ga 2 4+ (S 2−) 2) and the dioxan complex Ga 2 Cl 4 (C 4 H 8 O 2) 2. [1] There are also compounds of gallium with negative oxidation states, ranging from -5 to -1, most of these compounds being magnesium gallides (Mg x Ga y).
Bauxite is the main source of the rare metal gallium. [17] During the processing of bauxite to alumina in the Bayer process, gallium accumulates in the sodium hydroxide liquor. From this it can be extracted by a variety of methods. The most recent is the use of ion-exchange resin. [18]
Organogallium compounds can be synthesized by transmetallation, for example the reaction of gallium metal with dimethylmercury: 2Ga + 3Me 2 Hg → 2Me 3 Ga + 3 Hg. or via organolithium compounds or Grignards: GaCl 3 + 3MeMgBr → Me 3 Ga + 3MgBrCl. The electron-deficient nature of gallium can be removed by complex formation, for example
Pages in category "Gallium compounds" The following 67 pages are in this category, out of 67 total. This list may not reflect recent changes. A. Aerogalnite;
Although most compounds are referred to by their IUPAC systematic names ... Gallium(III) oxide – Ga 2 O 3; Germanium dioxide – GeO 2; Gold(III) oxide – Au 2 O 3;
The composition of the Earth changed after its formation due to loss of volatile compounds, melting and recrystalization, selective loss of some elements to the deep interior, and erosion by water. [3]: 55 The lanthanides are especially difficult to measure accurately. [4]
Gallium compounds (67 P) G. Gallium alloys (7 P) I. Isotopes of gallium (45 P) Pages in category "Gallium" The following 8 pages are in this category, out of 8 total.