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Nitrosyl fluoride (NOF) is a covalently bonded nitrosyl compound.
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| Names | |
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| IUPAC name
Nitrosyl fluoride[citation needed] | |
| Other names
Nitrogen oxyfluoride[citation needed] | |
| Identifiers | |
3D model (JSmol) |
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| Abbreviations | NOF[citation needed] |
| ChemSpider |
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| ECHA InfoCard | 100.029.230 
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| EC Number |
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PubChem CID |
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| UNII | |
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 | |
| Related compounds | |
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). | |
The 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.
Nitrosyl 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:
For this reason, aqueous NOF solutions, like aqua regia, are powerful solvents for metals.[1]
Absent an oxidizable metal, NOF reacts with water to form nitrous acid, which then disproportionates to nitric acid:
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]
Nitrosyl fluoride is used as a solvent and as a fluorinating and nitrating agent in organic synthesis. It has also been proposed as an oxidizer in rocket propellants.[citation needed]
