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| Names | |
|---|---|
| IUPAC name Nitrosyl fluoride | |
| Other names Nitrogen oxyfluoride | |
| Identifiers | |
| CAS Number | |
| 3D model (JSmol) | |
| Abbreviations | NOF |
| ChemSpider | |
| ECHA InfoCard | 100.029.230 
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| PubChem CID | |
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| CompTox Dashboard (EPA) | |
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| Properties | |
| Chemical formula | NOF |
| Molar mass | 49.0045 g mol |
| Appearance | Colourless gas |
| Density | 2.657 mg mL(gas) 1.326 g/cm(liquid) |
| Melting point | −166 °C (−267 °F; 107 K) |
| Boiling point | −72.4 °C (−98.3 °F; 200.8 K) |
| Solubility in water | Reacts |
| Related compounds | |
| Related compounds | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
 Y verify (what is ?)
Infobox references
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Nitrosyl fluoride (NOF) is a covalently bonded nitrosyl compound.
Physical properties
The compound is a colorless gas, with bent molecular shape. The VSEPR model explains this geometry via a lone-pair of electrons on the nitrogen atom.
Chemistry
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:
- n NOF + M → MFn + n NO
For this reason, aqueous NOF solutions are, like aqua regia, powerful solvents for metals.
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.
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:
- ROH + NOF → RONO + HF
Uses
Nitrosyl fluoride is used as a solvent and as a fluorinating and nitrating agent in organic synthesis.
References
- ^ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4.