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==Neutral octafluorides== |
==Neutral octafluorides== |
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No electrically neutral octafluorides are currently known to exist, although [[osmium octafluoride]], {{chem2|OsF8}}, is theoretically possible. An early report of the synthesis of {{chem2|OsF8}} was much later shown to be a mistaken identification of [[Osmium hexafluoride|{{chem2|OsF6}}]].<ref name=”fluorides”>{{ cite journal | last1 = Riedel | first1 = S. | last2 = Kaupp | first2 = M. | title = The highest oxidation states of the transition metal elements | journal = Coordination Chemistry Reviews | date = 30 Jul 2009 | volume = 253 | issue = 5–6 | doi = 10.1016/j.ccr.2008.07.014 | pages = 606–624 | url = https://www.sciencedirect.com/science/article/abs/pii/S0010854508001355| url-access = subscription }}</ref> |
No electrically neutral octafluorides are currently known to exist, although [[osmium octafluoride]], {{chem2|OsF8}}, is theoretically possible. An early report of the synthesis of {{chem2|OsF8}} was much later shown to be a mistaken identification of [[Osmium hexafluoride|{{chem2|OsF6}}]].<ref name=”fluorides”>{{ cite journal | last1 = Riedel | first1 = S. | last2 = Kaupp | first2 = M. | title = The highest oxidation states of the transition metal elements | journal = Coordination Chemistry Reviews | date = 30 Jul 2009 | volume = 253 | issue = 5–6 | doi = 10.1016/j.ccr.2008.07.014 | pages = 606–624 | url = https://www.sciencedirect.com/science/article/abs/pii/S0010854508001355| url-access = subscription }}</ref> |
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[[Xenon octafluoride]] could probably never be synthesized.<ref>{{cite journal |last1=Weinstock |first1=Bernard |last2=Weaver |first2=E. Eugene |last3=Knop |first3=Charles P. |title=The Xenon-Fluorine System |journal=[[Inorg. Chem.]] |date=December 1, 1966 |volume=66 |issue=5 |page=2189 |doi=10.1021/ic50046a026 |url=https://pubs.acs.org/doi/10.1021/ic50046a026# |access-date=31 March 2023|url-access=subscription }}</ref><ref>{{cite journal |last1=Pauling |first1=Linus |title=The Formulas of Antimonic Acid and the Antimonates |journal=[[Journal of the American Chemical Society]] |date=May 1933 |volume=55 |issue=5 |pages=1895–1900 |doi=10.1021/ja01332a016 |bibcode=1933JAChS..55.1895P |url=https://pubs.acs.org/doi/abs/10.1021/ja01332a016 |access-date=31 March 2023 |language=en |issn=0002-7863|url-access=subscription }}</ref> 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.<ref>{{cite book |last1=Cotton |first1=F. Albert |title=Progress in Inorganic Chemistry, Volume 6 |date=17 September 2009 |publisher=[[John Wiley & Sons]] |isbn=978-0-470-16657-4 |page=249 |url=https://books.google.com/books?id=IhkQIoEGL24C&dq=xenon+octafluoride&pg=PA249 |access-date=31 March 2023 |language=en}}</ref> |
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==Anionic octafluorides== |
==Anionic octafluorides== |
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Latest revision as of 10:40, 7 February 2026
Compound with 8 fluorine atoms
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.
Neutral octafluorides
[edit]
No electrically neutral octafluorides are currently known to exist, although osmium octafluoride, OsF8, is theoretically possible. An early report of the synthesis of OsF8 was much later shown to be a mistaken identification of OsF6.[1]
Xenon octafluoride could probably never be synthesized.[2][3] 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.[4]
Anionic octafluorides
[edit]
In contrast, many anionic octafluorides are known, such as the octafluorozirconate(IV) ([ZrF8]4−), octafluorotantalate(V) ([TaF8]3−), octafluoroniobate(V) ([NbF8]3−),[1] octafluoromolybdate(VI) ([MoF8]2−),[1] octafluorotungstate(VI) ([WF8]2−),[1] octafluororhenate(VII) ([ReF8]−),[1] octafluoroiodate(VII) ([IF8]−), octafluoroiridate(VII) ([IrF8]−),[5] and octafluoroxenate(VI) ([XeF8]2−) anions.
- ^ a b c d e 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.
- ^ 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.
- ^ 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.
{{cite journal}}: CS1 maint: multiple names: authors list (link)
