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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 tetrafluoride, GeF 4, a colorless molecular gas Index of chemical compounds with the same name This set index article lists chemical compounds articles associated with the same name.
It was the first discovered binary compound of a noble gas. [3] It is produced by the chemical reaction of xenon with fluorine: [4] [5] Xe + 2 F 2 → XeF 4. This reaction is exothermic, releasing an energy of 251 kJ/mol. [3] Xenon tetrafluoride is a colorless crystalline solid that sublimes at 117 °C.
Lewis structure of a water molecule. Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.
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 (predicted) Lead tetrafluoride, PbF 4; Manganese ...
To prevent decomposition, the xenon tetroxide thus formed is quickly cooled into a pale-yellow solid. It explodes above −35.9 °C into xenon and oxygen gas, but is otherwise stable. A number of xenon oxyfluorides are known, including XeOF 2, XeOF 4, XeO 2 F 2, and XeO 3 F 2. XeOF 2 is formed by reacting OF 2 with xenon gas at
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.
[7] [8] While Lewis supported the viewpoint of expanded octet, invoking s-p-d hybridized orbitals and maintaining 2c–2e bonds between neighboring atoms, Langmuir instead opted for maintaining the octet rule, invoking an ionic basis for bonding in hypervalent compounds (see Hypervalent molecule, valence bond theory diagrams for PF 5 and SF 6). [9]