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Germanium tetrafluoride is a noncombustible, strongly fuming gas with a garlic-like odor. It reacts with water to form hydrofluoric acid and germanium dioxide. Decomposition occurs above 1000 °C. [5] Reaction of GeF 4 with fluoride sources produces GeF 5 − anions with octahedral coordination around Ge atom due to polymerization. [6]
Germanium difluoride forms orthorhombic crystals with a space group P2 1 2 1 2 1 (No. 19), Pearson symbol oP12, and lattice constants a = 0.4682 nm, b = 0.5178 nm, c = 0.8312 nm, Z = 4 (four structure units per unit cell). Its crystal structure is characterized by strong polymeric chains composed by GeF 3 pyramids.
Four tetrahalides are known. Under normal conditions GeI 4 is a solid, GeF 4 a gas and the others volatile liquids. For example, germanium tetrachloride, GeCl 4, is obtained as a colorless fuming liquid boiling at 83.1 °C by heating the metal with chlorine. [4] All the tetrahalides are readily hydrolyzed to hydrated germanium dioxide. [4]
Germanium tetrabromide is the inorganic compound with the formula GeBr 4. It is a colorless solid that melts near room temperature. It can be formed by treating solid germanium with bromine, or by treating a germanium-copper mixture with bromine: [2] Ge + Br 2 → GeBr 4. From this reaction, GeBr 4 has a heat of formation of 83.3 kcal/mol. [3]
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
Cobalt tetrafluoride, CoF 4; Curium tetrafluoride, CmF 4; Diboron tetrafluoride, B 2 F 4, a colorless gas; Dinitrogen tetrafluoride, N 2 F 4 (Tetrafluorohydrazine) Einsteinium tetrafluoride, EsF 4; Germanium tetrafluoride, GeF 4; Hafnium tetrafluoride, HfF 4; Iridium tetrafluoride, IrF 4; Iron tetrafluoride, FeF 4; Krypton tetrafluoride, KrF 4 ...
The melting point of SnF 4 is much higher (700 °C) than the other tin(IV) halides which are relatively low melting, (SnCl 4, −33.3 °C; SnBr 4, 31 °C; SnI 4, 144 °C). [1] The structure can also be contrasted with the tetrafluorides of the lighter members of group 14, ( CF 4 , SiF 4 and GeF 4 ) which in the solid state form molecular crystals.
Boron carbide – B 4 C [143] Boron nitride – BN [144] Boron suboxide – B 6 O [145] Boron tribromide – BBr 3 [146] Boron trichloride – BCl 3 [147] Boron trifluoride – BF 3 [148] Boron triiodide –BI 3 [149] Boron oxide – B 2 O 3 [150] Boroxine – B 3 H 3 O 3 [151] Decaborane – B 10 H 14 [152] Diborane – B 2 H 6 [153] Diboron ...