linguistic:paraphrasing, stylistic:tone
Oxides and oxohalides

Three oxides of xenon are known: xenon trioxide (XeO) and xenon tetroxide (XeO), both of which are dangerously explosive and powerful oxidizing agents, and xenon dioxide (XeO), which was reported in 2011 with a coordination number of four. XeO forms when xenon tetrafluoride is poured over ice. Its crystal structure may allow it to replace silicon in silicate minerals. The XeOO cation has been identified by infrared spectroscopy in solid argon.

Xenon does not react with oxygen directly; the trioxide is formed by the hydrolysis of XeF:

XeO is weakly acidic, dissolving in alkali to form unstable xenate salts containing the HXeO anion. These unstable salts easily disproportionate into xenon gas and perxenate salts, containing the XeO anion.

Barium perxenate, when treated with concentrated sulfuric acid, yields gaseous xenon tetroxide:

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, XeOF, XeO F, and XeO F. XeOF is formed by reacting OF with xenon gas at low temperatures. It may also be obtained by partial hydrolysis of XeF. It disproportionates at −20 °C into XeF and XeO F. XeOF is formed by the partial hydrolysis of XeF...

...or the reaction of XeF with sodium perxenate, Na XeO. The latter reaction also produces a small amount of XeO F.

XeO F is also formed by partial hydrolysis of XeF.

XeOF reacts with CsF to form the XeOF anion, while XeOF reacts with the alkali metal fluorides KF, RbF and CsF to form the XeOF anion.