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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]
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.
Structure of xenon oxytetrafluoride, an example of a molecule with the square pyramidal coordination geometry. Square pyramidal geometry describes the shape of certain chemical compounds with the formula ML 5 where L is a ligand. If the ligand atoms were connected, the resulting shape would be that of a pyramid with a square base.
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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.
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