Editing Xenon (section)

=== Oxides and oxohalides ===
Three oxides of xenon are known: [[xenon trioxide]] ({{chem|XeO|3}}) and [[xenon tetroxide]] ({{chem|XeO|4}}), both of which are dangerously explosive and powerful oxidizing agents, and [[xenon dioxide]] (XeO<sub>2</sub>), which was reported in 2011 with a [[coordination number]] of four.<ref>{{cite journal
| author  = Brock, D.S.
| author2 = Schrobilgen, G.J.
| title   = Synthesis of the missing oxide of xenon, XeO<sub>2</sub>, and its implications for Earth's missing xenon
| journal = [[Journal of the American Chemical Society]]
| year    = 2011
| doi     = 10.1021/ja110618g
| volume  = 133
| issue   = 16
| pmid    = 21341650
| pages   = 6265–9
| bibcode = 2011JAChS.133.6265B
}}</ref> XeO<sub>2</sub> forms when xenon tetrafluoride is poured over ice. Its crystal structure may allow it to replace silicon in silicate minerals.<ref name="ChemistryWhere2011">{{Cite journal
| title      = Chemistry: Where did the xenon go?
| journal    = Nature
| volume     = 471
| issue      = 7337
| pages      = 138
| year       = 2011
| doi        = 10.1038/471138d
| bibcode    = 2011Natur.471T.138.
| doi-access = free
}}</ref> The XeOO<sup>+</sup> cation has been identified by [[infrared spectroscopy]] in solid [[argon]].<ref>{{cite journal
| author  = Zhou, M.
| author2 = Zhao, Y.
| author3 = Gong, Y.
| author4 = Li, J.
| title   = Formation and Characterization of the XeOO<sup>+</sup> Cation in Solid Argon
| journal = [[Journal of the American Chemical Society]]
| year    = 2006
| volume  = 128
| issue   = 8
| pmid    = 16492012
| pages   = 2504–5
| doi     = 10.1021/ja055650n
| bibcode = 2006JAChS.128.2504Z
}}</ref>

Xenon does not react with oxygen directly; the trioxide is formed by the hydrolysis of {{chem|XeF|6}}:<ref>{{cite book
| first     = John H.
| last      = Holloway
| author2   = Hope, Eric G.
| editor    = A. G. Sykes
| date      = 1998
| publisher = Academic
| title     = Advances in Inorganic Chemistry Press
| isbn      = 0-12-023646-X
| page      = 65
| url       = https://books.google.com/books?id=6iqXRtz6p3QC&pg=PA65
}}</ref>
: {{chem|XeF|6}} + 3 {{chem|H|2|O}} → {{chem|XeO|3}} + 6 HF

{{chem|XeO|3}} is weakly acidic, dissolving in alkali to form unstable ''xenate'' salts containing the {{chem|HXeO|4|−}} anion. These unstable salts easily [[disproportionation|disproportionate]] into xenon gas and [[perxenate]] salts, containing the {{chem|XeO|6|4−}} anion.<ref name="henderson">{{cite book
| first     = W.
| last      = Henderson
| title     = Main group chemistry
| date      = 2000
| publisher = [[Royal Society of Chemistry]]
| pages     = 152–53
| location  = Great Britain
| isbn      = 0-85404-617-8
| url       = https://books.google.com/books?id=twdXz1jfVOsC&pg=PA152
}}</ref>

Barium perxenate, when treated with concentrated [[sulfuric acid]], yields gaseous xenon tetroxide:<ref name="scott1" />
: {{chem|Ba|2|XeO|6}} + 2 {{chem|H|2|SO|4}} → 2 {{chem|BaSO|4}} + 2 {{chem|H|2|O}} + {{chem|XeO|4}}

To prevent decomposition, the xenon tetroxide thus formed is quickly cooled into a pale-yellow solid. It explodes above −35.9&nbsp;°C into xenon and oxygen gas, but is otherwise stable.

A number of xenon oxyfluorides are known, including {{chem|XeOF|2}}, [[xenon oxytetrafluoride|{{chem|XeOF|4}}]], {{chem|XeO|2|F|2}}, and {{chem|XeO|3|F|2}}. {{chem |XeOF|2}} is formed by reacting [[oxygen difluoride|{{chem|OF|2}}]] with xenon gas at low temperatures. It may also be obtained by partial hydrolysis of {{chem|XeF|4}}. It disproportionates at −20&nbsp;°C into {{chem|XeF|2}} and {{chem|XeO|2|F|2}}.<ref name="mackay1">{{cite book
| author    = Mackay, Kenneth Malcolm
| author2   = Mackay, Rosemary Ann
| author3   = Henderson, W.
| title     = Introduction to modern inorganic chemistry
| date      = 2002
| edition   = 6th
| publisher = CRC Press
| isbn      = 0-7487-6420-8
| url       = https://books.google.com/books?id=LpJPWKT3PNcC&pg=PA497
| pages     = 497–501
}}</ref> {{chem |XeOF|4}} is formed by the partial hydrolysis of {{chem |XeF|6}}...<ref>{{cite journal
| last    = Smith
| first   = D. F.
| s2cid   = 42752536
| year    = 1963
| title   = Xenon Oxyfluoride
| pmid    = 17810680
| journal = Science
| volume  = 140
| doi     = 10.1126/science.140.3569.899
| issue   = 3569
| bibcode = 1963Sci...140..899S
| pages   = 899–900
}}</ref>
:{{chem |XeF|6}} + {{chem |H|2|O}} → {{chem |XeOF|4}} + 2 {{chem |H|F}}
...or the reaction of {{chem|XeF|6}} with sodium perxenate, {{chem |Na|4|XeO|6}}. The latter reaction also produces a small amount of {{chem|XeO|3|F|2}}.

{{chem |Xe|O|2|F|2}} is also formed by partial hydrolysis of {{chem |Xe|F|6}}.<ref>{{cite book
| title     = Chemistry Textbook Part – 1 for Class XII
| publisher = NCERT
| isbn      = 978-81-7450-648-1
| page      = 204
| edition   = October 2022
| url       = https://ncert.nic.in/ncerts/l/lech107.pdf
| language  = English
| chapter   = P Block Elements
| date      = 2007
}}</ref>
:{{chem |Xe|F|6}} + 2 {{chem |H|2|O}} → {{chem |Xe|O|2|F|2}} + 4 {{chem |HF}}
{{chem|XeOF|4}} reacts with [[caesium fluoride|CsF]] to form the {{chem |XeOF|5|−}} anion,<ref name="mackay1" /><ref>{{cite journal
| title   = On the Structure of the [XeOF<sub>5</sub>]<sup>−</sup> Anion and of Heptacoordinated Complex Fluorides Containing One or Two Highly Repulsive Ligands or Sterically Active Free Valence Electron Pairs
| author  = Christe, K. O.
| author2 = Dixon, D. A.
| author3 = Sanders, J. C. P.
| author4 = Schrobilgen, G. J.
| author5 = Tsai, S. S.
| author6 = Wilson, W. W.
| journal = [[Inorganic Chemistry (journal)|Inorg. Chem.]]
| year    = 1995
| volume  = 34
| issue   = 7
| pages   = 1868–1874
| doi     = 10.1021/ic00111a039
}}</ref> while XeOF<sub>3</sub> reacts with the alkali metal fluorides [[potassium fluoride|KF]], [[rubidium fluoride|RbF]] and CsF to form the {{chem|XeOF|4|−}} anion.<ref>{{cite journal
| title   = Chlorine trifluoride oxide. V. Complex formation with Lewis acids and bases
| author  = Christe, K. O.
| author2 = Schack, C. J.
| author3 = Pilipovich, D.
| journal = [[Inorganic Chemistry (journal)|Inorg. Chem.]]
| year    = 1972
| volume  = 11
| issue   = 9
| pages   = 2205–2208
| doi     = 10.1021/ic50115a044
}}</ref>