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]
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
CompTox Dashboard (EPA)
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| Properties | |
| XeOF4 | |
| Molar mass | 223.23 g/mol |
| Appearance | colorless liquid |
| Density | 3.17 g/cm3, liquid |
| Melting point | −46.2 °C (−51.2 °F; 227.0 K) |
| Reacts with water | |
| Structure | |
| square pyramidal[1][2] | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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:
In addition, some ozone and fluorine is formed.
Reactions
editXeOF
4 reacts with H
2O in the following steps:
The XeO
3 formed is a dangerous explosive, decomposing explosively to Xe and O
2:
- 2 XeO
3 → 2 Xe + 3 O
2
In its liquid form, XeOF
4 exhibits amphoteric behaviour, forming complexes with both strong Lewis bases like CsF and strong Lewis acids like SbF
5.[7] It forms a 1:1 adduct with XeF
2, isostructural with XeF
2·IF
5,[8] as well as various heavy alkali metal fluorides.[4]
The reaction of XeOF
4 with XeO
3 provides a convenient synthesis route for XeO
2F
2.[9]
See also
editExternal links
edit- Xenon tetrafluoride oxide in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2022-04-13)
References
edit- ^ 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.
- ^ a b Smith, D. F. (1963-05-24). "Xenon Oxyfluoride". Science. 140 (3569): 899–900. Bibcode:1963Sci...140..899S. doi:10.1126/science.140.3569.899. ISSN 0036-8075. JSTOR 00368075. LCCN 17024346. OCLC 1644869. PMID 17810680. S2CID 42752536.
- ^ a b Ibers, 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.
- ^ a b 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.
- ^ Martin-Rovet, D.; Angelié, C.; Cauchetier, M.; Schrobilgen, G. J. (September 1982). "Various aspects of the reactivity of the xenon(VI) oxyfluoride: XeOF4". Journal of Fluorine Chemistry. 21 (1): 10. doi:10.1016/S0022-1139(00)85330-0. ISSN 0022-1139.
- ^ Bartlett, N.; Wechsberg, M. (October 1971). "The Xenon Difluoride Complexes XeF2 · XeOF4; XeF2 · XeF6 · AsF5 and XeF2 · 2 XeF6 · 2 AsF5 and Their Relevance to Bond Polarity and Fluoride Ion Donor Ability of XeF2 and XeF6". Zeitschrift für anorganische und allgemeine Chemie. 385 (1): 5–17. doi:10.1002/zaac.19713850103. ISSN 0044-2313. OCLC 1770423.
- ^ Huston, John L. (September 1967). "Xenon dioxide difluoride: isolation and some properties". The Journal of Physical Chemistry A. 71 (10): 3339–3341. doi:10.1021/j100869a035. ISSN 1089-5639.