This article relies largely or entirely on a single source. (October 2023) |
Nitrosyl fluoride (NOF) is a covalently bonded nitrosyl compound.
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| Names | |
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| IUPAC name
Nitrosyl fluoride[citation needed]
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| Other names
Nitrogen oxyfluoride[citation needed]
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| Identifiers | |
3D model (JSmol)
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| Abbreviations | NOF[citation needed] |
| ChemSpider | |
| ECHA InfoCard | 100.029.230 |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| NOF | |
| Molar mass | 49.0045 g mol−1 |
| Appearance | Colourless gas |
| Density | 2.657 mg mL−1(gas) 1.326 g/cm3(liquid) |
| Melting point | −166 °C (−267 °F; 107 K) |
| Boiling point | −72.4 °C (−98.3 °F; 200.8 K) |
| Reacts | |
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Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Physical properties
editThe compound is a colorless gas, with bent molecular shape.[1] The VSEPR model explains this geometry via a lone-pair of electrons on the nitrogen atom.
Chemistry
editNitrosyl fluoride is typically produced by direct reaction of nitric oxide and fluorine, although halogenation with a perfluorinated metal salt is also possible. The compound is a highly reactive fluorinating agent that converts many metals to their fluorides, releasing nitric oxide in the process:
- n NOF + M → MFn + n NO
For this reason, aqueous NOF solutions are, like aqua regia, powerful solvents for metals.[1]
Absent an oxidizable metal, NOF reacts with water to form nitrous acid, which then disproportionates to nitric acid:
- NOF + H2O → HNO2 + HF
- 3 HNO2 → HNO3 + 2 NO + H2O
These reactions occur in both acidic and basic solutions.[1]
Nitrosyl fluoride also forms salt-like adducts with Lewis-acidic fluorides; for example, BF3 reacts to give NOBF4. Similarly, the compound nitrosylates compounds with a free proton; thus alcohols convert to nitrites:[1]
- ROH + NOF → RONO + HF
Uses
editNitrosyl fluoride is used as a solvent and as a fluorinating and nitrating agent in organic synthesis.
References
edit- ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4.