View source for Chemistry:Krypton hexafluoride

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| OtherNames = Krypton(VI) fluoride
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| Kr=1|F=6
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| OtherCompounds = [[Chemistry:Xenon hexafluoride|Xenon hexafluoride]]
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'''Krypton hexafluoride''' is an inorganic chemical compound of [[Chemistry:Krypton|krypton]] and [[Chemistry:Fluorine|fluorine]] with the chemical formula {{chem2|KrF6}}. It is still a hypothetical compound.<ref>{{cite journal |last1=Dixon |first1=David A. |last2=Wang |first2=Tsang-Hsiu |last3=Grant |first3=Daniel J. |last4=Peterson |first4=Kirk A. |last5=Christe |first5=Karl O. |last6=Schrobilgen |first6=Gary J. |title=Heats of Formation of Krypton Fluorides and Stability Predictions for KrF<sub>4</sub> and KrF<sub>6</sub> from High Level Electronic Structure Calculations |journal=Inorganic Chemistry |date=1 November 2007 |volume=46 |issue=23 |pages=10016–10021 |doi=10.1021/ic701313h |pmid=17941630 |url=https://pubs.acs.org/doi/10.1021/ic701313h |access-date=28 March 2023 |language=en |issn=0020-1669}}</ref>

==History==
In 1933, [[Biography:Linus Pauling|Linus Pauling]] predicted<ref>{{cite book |last1=Williams |first1=Jeffrey H. |title=Crystal Engineering: How Molecules Build Solids |date=28 September 2017 |publisher=Morgan & Claypool Publishers |isbn=978-1-68174-625-8 |page=4–1 |url=https://books.google.com/books?id=3D9iDwAAQBAJ&dq=Krypton+hexafluoride&pg=SA3-PA14 |access-date=28 March 2023 |language=en}}</ref> that the heavier noble gases would be able to form compounds with fluorine and oxygen. He also predicted the existence of krypton hexafluoride.<ref>{{cite journal |last1=Pauling |first1=Linus |title=The Formulas of Antimonic Acid and the Antimonates |journal=[[Organization:Journal of the American Chemical Society|Journal of the American Chemical Society]] |date=May 1933 |volume=55 |issue=5 |pages=1895–1900 |doi=10.1021/ja01332a016 |url=https://pubs.acs.org/doi/abs/10.1021/ja01332a016 |access-date=28 March 2023 |language=en |issn=0002-7863}}</ref> So far, out of all possible krypton fluorides, only [[Chemistry:Krypton difluoride|krypton difluoride]] ({{chem2|KrF2}}) has been actually formed. It is a white crystalline solid that decomposes spontaneously at normal temperatures.<ref>{{cite journal |last1=Burbank |first1=R. D. |last2=Falconer |first2=W. E. |last3=Sunder |first3=W. A. |title=Crystal Structure of Krypton Difluoride at −80°C |journal=Science |date=22 December 1972 |volume=178 |issue=4067 |pages=1285–1286 |doi=10.1126/science.178.4067.1285 |pmid=17792123 |s2cid=96692996 |url=https://www.science.org/doi/10.1126/science.178.4067.1285 |access-date=28 March 2023 |language=en |issn=0036-8075}}</ref> This fact leads to suggest that krypton hexafluoride is also an unstable compound.

==References==
{{Reflist}}

{{Hexafluorides}}
{{fluorides}}

[[Category:Krypton compounds]]
[[Category:Fluorides]]
[[Category:Nonmetal halides]]
[[Category:Hexafluorides]]
[[Category:Fluorinating agents]]
[[Category:Hypothetical chemical compounds]]


{{Sourceattribution|Krypton hexafluoride}}