Oxygen monofluoride

Oxygen monofluoride
Names
	Other names Fluorine oxide, fluorooxy radical, fluorooxidanyl
Identifiers
CAS Number	12061-70-0 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:30242;
ChemSpider	4937269;
Gmelin Reference	535
PubChem CID	6432002;
CompTox Dashboard (EPA)	DTXSID301315297;
	InChI InChI=1S/FO/c1-2 Key: FXOFAYKVTOLJTJ-UHFFFAOYSA-N;
	SMILES [O]F;
Properties
Chemical formula	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). Infobox references

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

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

OF₂ → OF + F

A reaction of fluorine and ozone:^[5]

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.

[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.

[1]

[2]

[3]

[4]

[5]

[6]