Hexaoxygen difluoride
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| Identifiers | |
|---|---|
3D model (JSmol)
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| Properties | |
| F2O6 | |
| Molar mass | 133.991 g·mol−1 |
| Appearance | dark-brown solid at 60 K |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hexaoxygen difluoride is a binary inorganic compound of fluorine and oxygen with the chemical formula O6F2.[1][2] The compound is one of many known oxygen fluorides.[3]
Synthesis[edit]
The compound can be prepared by electric discharges through the F2—O2 mixture of the certain molar ratio at 60 to 77 K. The ratio is predicted to be 6:2.[4]
Physical properties[edit]
Hexaoxygen difluoride is an oxidizing agent. At 60 K, the compound looks like a dark-brown crystalline solid. If slowly warmed, it decomposes to lower oxygen fluorides and ozone. If quickly warmed to 90 K, it explodes, creating O2 and F2.[4]
References[edit]
- ^ Streng, A. G.; Grosse, A. V. (January 1966). "Two New Fluorides of Oxygen, O5F2 and O6F2 1,2". Journal of the American Chemical Society. 88 (1): 169–170. doi:10.1021/ja00953a035. Retrieved 19 May 2023.
- ^ Bailar, John Christian; Trotman-Dickenson, A. F. (1973). Comprehensive Inorganic Chemistry: Ge, Sn, Pb, Group VB, Group VIB, Group VIIB. Pergamon Press. p. 764. ISBN 978-0-08-017275-0. Retrieved 19 May 2023.
- ^ Bretherick, L. (27 October 2016). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier. p. 1622. ISBN 978-1-4831-6250-8. Retrieved 19 May 2023.
- ^ a b F Fluorine: Compounds with Oxygen and Nitrogen. Springer Science & Business Media. 29 June 2013. p. 134. ISBN 978-3-662-06339-2. Retrieved 19 May 2023.