Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Chemical compound
Xenon oxytetrafluoride (XeOF 4) is an inorganic chemical compound. It is an unstable colorless liquid[2][3] with a melting point of −46.2 °C (−51.2 °F; 227.0 K)[4] that can be synthesized by partial hydrolysis of XeF 6, or the reaction of XeF 6 with silica[3] or NaNO 3:[5]
NaNO 3 + XeF 6 → NaF + XeOF 4 + FNO 2
A high-yield synthesis proceeds by the reaction of XeF 6 with POF 3 at −196 °C (−320.8 °F; 77.1 K).[6]
Like most xenon oxides, it is extremely reactive, and it hydrolyses in water to give hazardous and corrosive products, including hydrogen fluoride:
2XeOF 4 + 4H 2O → 2Xe + 8HF + 3O 2
In addition, some ozone and fluorine is formed.
^Martins, Joseph; Wilson, E. Bright Jr. (1964). "Microwave Spectrum of Xenon Oxytetrafluoride". The Journal of Chemical Physics. 41 (570): 570–571. Bibcode:1964JChPh..41..570M. doi:10.1063/1.1725910. ISSN 0021-9606.
^ abIbers, James A. (October 1965). "Molecular Structure". Annual Review of Physical Chemistry. 16: 375–396. Bibcode:1965ARPC...16..375I. doi:10.1146/annurev.pc.16.100165.002111. ISSN 0066-426X. LCCN a51001658. OCLC 1373069.
^Selig, Henry (1966-02-01). "Complexes of Xenon Oxide Tetrafluoride". Inorganic Chemistry. 5 (2): 183–186. doi:10.1021/ic50036a004. ISSN 0020-1669.
^Christe, Karl O.; Wilson, William W. (April 1988). "Convenient synthesis of xenon oxide tetrafluoride". Inorganic Chemistry. 27 (7): 1296–1297. doi:10.1021/ic00280a043. ISSN 0020-1669.
^Nielsen, Jon B.; Kinkead, Scott A.; Eller, P. Gary (1990-09-01). "A New Synthesis of Xenon Oxytetrafluoride, XeOF4". Inorganic Chemistry. 29 (18): 3621–3622. doi:10.1021/ic00343a063. ISSN 0020-1669.
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