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| Names | |
|---|---|
| IUPAC name Nitrosyl fluoride[citation needed] | |
| Other names Nitrogen oxyfluoride[citation needed] | |
| Identifiers | |
3D model (JSmol) | |
| Abbreviations | NOF[citation needed] |
| ChemSpider |
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| ECHA InfoCard | 100.029.230 |
| EC Number |
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| UNII | |
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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 | |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Nitrosyl fluoride (NOF) is acovalently bondednitrosyl compound.
The compound is acolorless gas, withbent molecular shape.[1] TheVSEPR model explains this geometry via alone-pair of electrons on the nitrogen atom.
Nitrosyl fluoride is typically produced by direct reaction ofnitric oxide andfluorine, although halogenation with a perfluorinated metal salt is also possible. The compound is a highly reactivefluorinating agent that converts manymetals to theirfluorides, releasingnitric oxide in the process:
For this reason, aqueous NOF solutions are, likeaqua regia, powerful solvents for metals.[1]
Absent an oxidizable metal, NOF reacts withwater to formnitrous acid, which then disproportionates tonitric acid:
These reactions occur in both acidic and basic solutions.[1]
Nitrosyl fluoride also formssalt-likeadducts withLewis-acidicfluorides; for example,BF3 reacts to giveNOBF4. Similarly, the compound nitrosylates compounds with a free proton; thusalcohols convert tonitrites:[1]
Nitrosyl fluoride is used as asolvent and as afluorinating andnitrating[dubious –discuss] agent inorganic synthesis.[citation needed]
