Oxygen monofluoride

Last updated
Oxygen monofluoride
Names
Other names
Fluorine oxide, fluorooxy radical, fluorooxidanyl
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
535
PubChem CID
  • InChI=1S/FO/c1-2
    Key: FXOFAYKVTOLJTJ-UHFFFAOYSA-N
  • [O]F
Properties
OF
Molar mass 35.00 g/mol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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.

Contents

Synthesis

OF is a radical that can be formed by thermal or photolytic decomposition of OF
2 [4]

OF2 → OF + F

or a reaction of fluorine and ozone: [5]

F + O3 → OF + O2

Atmosphere

Oxygen- and fluorine-containing radicals like OF and O2F occur in the atmosphere. These and other halogen radicals have been implicated in the destruction of ozone in the atmosphere.

O3 + F → O2 + OF
O + OF → O2 + F

However, 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 hydrogen fluoride, which precipitates in rain as hydrofluoric acid. [6]

References

  1. ↑ 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.
  2. ↑ 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.
  3. ↑ "Oxygen monofluoride". National Institute of Standards and Technology . Retrieved 27 March 2023.
  4. ↑ 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.
  5. ↑ Nikitin, I. V. (13 March 2008). "HALOGEN MONOXIDES" (in Russian). Institute of Problems of Chemical Physics, Russian Academy of Sciences . Retrieved 27 March 2023.
  6. ↑ 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.
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