Oxygen monofluoride is an unstable binary inorganic compound radical of fluorine and oxygen with the chemical formula OF.[1][2][3] This is the simplest of many oxygen fluorides.
Synthesis
- OF2 → OF + F
- F + O3 → OF + O2
Atmosphere
Oxygen- and fluorine-containing radicals like O2F and OF occur in the atmosphere. These, along with other halogen radicals, have been implicated in the destruction of ozone in the atmosphere. However, the oxygen monofluoride radicals are assumed to not play as big a role in the ozone depletion because free fluorine atoms in the atmosphere are believed to react with methane to produce hydrofluoric acid which precipitates in rain.[6]
- O3 + F → O2 + OF
- O + OF → O2 + F
References
- ^ Colussi, A. J.; Grela, M. A. (21 October 1994). "Rate of the reaction between oxygen monofluoride and ozone: Implications for the atmospheric role of fluorine". Chemical Physics Letters. 229 (1): 134–138. Bibcode:1994CPL...229..134C. doi:10.1016/0009-2614(94)01021-8. ISSN 0009-2614. Retrieved 27 March 2023.
- ^ Langhoff, Stephen R.; Bauschlicher, Charles W.; Partridge, Harry (November 1983). "Theoretical study of the dipole moment of oxygen monofluoride (OF)". Chemical Physics Letters. 102 (4): 292–298. Bibcode:1983CPL...102..292L. doi:10.1016/0009-2614(83)87044-4. Retrieved 27 March 2023.
- ^ "Oxygen monofluoride". National Institute of Standards and Technology. Retrieved 27 March 2023.
- ^ Haupt, Axel (22 March 2021). Organic and Inorganic Fluorine Chemistry: Methods and Applications. Walter de Gruyter GmbH & Co KG. p. 99. ISBN 978-3-11-065933-7. Retrieved 27 March 2023.
- ^ Nikitin, I. V. (13 March 2008). "HALOGEN MONOXIDES" (in Russian). Institute of Problems of Chemical Physics, Russian Academy of Sciences. Retrieved 27 March 2023.
- ^ Francisco J. S. (1993). "An ab initio investigation of the significance of the HOOF intermediate in coupling reactions involving FOO x and HO x species". The Journal of Chemical Physics. 98 (3): 2198–2207. Bibcode:1993JChPh..98.2198F. doi:10.1063/1.464199.