oxygen monofluoride
{{Chembox
| ImageAlt =
| ImageFile =
| ImageSize = 200px
| PIN =
| OtherNames = Fluorine oxide, fluorooxy radical, fluorooxidanyl
|Section1={{Chembox Identifiers
| CASNo = 12061-70-0
| CASNo_Ref = {{cascite|correct|CAS}}
| ChemSpiderID = 4937269
| ChEBI = 30242
| DTXSID = DTXSID301315297
| EINECS =
| Gmelin = 535
| PubChem = 6432002
| SMILES = [O]F
| StdInChI = 1S/FO/c1-2
| StdInChIKey = FXOFAYKVTOLJTJ-UHFFFAOYSA-N
}}
|Section2={{Chembox Properties
| Formula = OF
| MolarMass = 35.00 g/mol
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|Section3={{Chembox Hazards
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|Section6={{Chembox Related
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Oxygen monofluoride is an unstable binary inorganic compound radical of fluorine and oxygen with the chemical formula OF.{{cite journal |last1=Colussi |first1=A. J. |last2=Grela |first2=M. A. |title=Rate of the reaction between oxygen monofluoride and ozone: Implications for the atmospheric role of fluorine |journal=Chemical Physics Letters |date=21 October 1994 |volume=229 |issue=1 |pages=134–138 |doi=10.1016/0009-2614(94)01021-8 |bibcode=1994CPL...229..134C |url=https://www.sciencedirect.com/science/article/abs/pii/0009261494010218 |access-date=27 March 2023 |language=en |issn=0009-2614}}{{cite journal |last1=Langhoff |first1=Stephen R. |last2=Bauschlicher |first2=Charles W. |last3=Partridge |first3=Harry |title=Theoretical study of the dipole moment of oxygen monofluoride (OF) |journal=Chemical Physics Letters |date=November 1983 |volume=102 |issue=4 |pages=292–298 |doi=10.1016/0009-2614(83)87044-4 |bibcode=1983CPL...102..292L |url=https://ntrs.nasa.gov/citations/19840041941 |access-date=27 March 2023}}{{cite web |title=Oxygen monofluoride |url=https://webbook.nist.gov/cgi/inchi/InChI%3D1S/FO/c1-2 |access-date=27 March 2023 |language=en|publisher=National Institute of Standards and Technology}} This is the simplest of many oxygen fluorides.
Synthesis
- OF is a radical that can be formed by thermal of photolytic decomposition of Oxygen difluoride.{{cite book |last1=Haupt |first1=Axel |title=Organic and Inorganic Fluorine Chemistry: Methods and Applications |date=22 March 2021 |publisher=Walter de Gruyter GmbH & Co KG |isbn=978-3-11-065933-7 |page=99 |url=https://books.google.com/books?id=5fwkEAAAQBAJ&dq=Oxygen+monofluoride&pg=PA99 |access-date=27 March 2023 |language=en}}
:{{chem2|OF2 -> OF + F}}
- A reaction of fluorine and ozone:{{cite web |last1=Nikitin |first1=I. V. |title=HALOGEN MONOXIDES |url=https://www.uspkhim.ru/RCR3788pdf |publisher=Institute of Problems of Chemical Physics, Russian Academy of Sciences |access-date=27 March 2023 |language=ru |date=13 March 2008}}
:{{chem2|F + O3 -> OF + O2}}
Atmosphere
Oxygen- and fluorine-containing radicals like {{chem2|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.{{cite journal | author = Francisco J. S. | year = 1993 | title = An ab initio investigation of the significance of the HOOF intermediate in coupling reactions involving FOO x and HO x species | journal = The Journal of Chemical Physics | volume = 98 | issue = 3| pages = 2198–2207 | doi = 10.1063/1.464199 | bibcode = 1993JChPh..98.2198F }}
:{{chem2|O3 + F -> O2 + OF}}
:{{chem2|O + OF -> O2 + F}}
References
{{Reflist}}
{{Oxygen compounds}}
{{Fluorine compounds}}