Octafluoride
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An octafluoride is a compound or ion with the formula [MmRnF8]q− or [MmRnF8]q+, where n, m and q are independent variables and R any substituent and M is a central element (often a metal). All of the examples listed below are [MF8]q− with q between 1 and 4 inclusive.
No electrically neutral octafluorides are currently known to exist, although osmium octafluoride, OsF8, is theoretically possible. Osmium octafluoride was first reported in 1913, but in 1958 that compound was shown to be actually osmium hexafluoride.[1] A 1993 theoretical study predicted very weak bonds in osmium octafluoride and said that it would be difficult to ever detect experimentally. The study predicted that, if made, OsF8 would have Os–F bonds of two different lengths.[2]
Xenon octafluoride could probably never be synthesized.[3][4] This appears to be due to the steric hindrance of the fluorine atoms around the xenon atom. However, scientists continue to try to synthesize it.[5]
Anionic octafluorides
In contrast, many anionic octafluorides are known, such as the octafluorozirconate(IV) ([ZrF8]4−), octafluorotantalate(V) ([TaF8]3−), octafluoroniobate(V) ([NbF8]3−),[6] octafluoromolybdate(VI) ([MoF8]2−),[6] octafluorotungstate(VI) ([WF8]2−),[6] octafluororhenate(VII) ([ReF8]−),[6] octafluoroiodate(VII) ([IF8]−), octafluoroiridate(VII) ([IrF8]−),[7] and octafluoroxenate(VI) ([XeF8]2−) anions.
References
- ↑ Weinstock, Bernard; Malm, John G. (September 1958). "Osmium Hexafluoride and its Identity with the Previously Reported Octafluoride". Journal of the American Chemical Society. 80 (17): 4466–4468. Bibcode:1958JAChS..80.4466W. doi:10.1021/ja01550a007.
- ↑ Weldkamp, Achim; Frenking, Gernot (1993). "Quantum-mechanical ab initio investigation of the transition-metal compounds OsO4, OsO3F2, OsO2F4, OsOF6, and OsF8". Chemische Berichte. 126 (6): 1325–1330. doi:10.1002/cber.19931260609.
- ↑ Weinstock, Bernard; Weaver, E. Eugene; Knop, Charles P. (December 1, 1966). "The Xenon-Fluorine System". Inorg. Chem. 66 (5): 2189. doi:10.1021/ic50046a026. Retrieved 31 March 2023.
- ↑ Pauling, Linus (May 1933). "The Formulas of Antimonic Acid and the Antimonates". Journal of the American Chemical Society. 55 (5): 1895–1900. Bibcode:1933JAChS..55.1895P. doi:10.1021/ja01332a016. ISSN 0002-7863. Retrieved 31 March 2023.
- ↑ Cotton, F. Albert (17 September 2009). Progress in Inorganic Chemistry, Volume 6. John Wiley & Sons. p. 249. ISBN 978-0-470-16657-4. Retrieved 31 March 2023.
- 1 2 3 4 Riedel, S.; Kaupp, M. (30 Jul 2009). "The highest oxidation states of the transition metal elements". Coordination Chemistry Reviews. 253 (5–6): 606–624. doi:10.1016/j.ccr.2008.07.014.
- ↑ Jianyan Lin, Ziyuan Zhao, Chunyu Liu, Jing Zhang, Xin Du, Guochun Yang, and Yanming Ma (March 13, 2019). "IrF8 Molecular Crystal under High Pressure". J. Am. Chem. Soc. 141 (13): 5409–5414. doi:10.1021/jacs.9b00069. PMID 30864432. S2CID 76664353.
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