Nitrosyl fluoride
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| Names | |
|---|---|
| IUPAC name
Nitrosyl fluoride | |
| Other names
Nitrogen oxyfluoride | |
| Identifiers | |
| Abbreviations | NOF |
7789-25-5  | |
| ChemSpider | 109874 |
| EC number | 232-153-6 |
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| Jmol-3D images | Image |
| PubChem | 123261 |
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| Properties | |
| NOF | |
| Molar mass | 49.0045 g mol−1 |
| Appearance | Colourless gas |
| Density | 2.657 mg mL−1 |
| 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 noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
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| Infobox references | |
Nitrosyl fluoride, NOF, is a covalently bonded nitrosyl compound.
Reactions
NOF 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
NOF also fluorinates fluorides to form adducts that have a salt-like character, such as NOBF4.
Aqueous solutions of NOF are powerful solvents for metals, by a mechanism similar to that seen in aqua regia. Nitrosyl fluoride reacts with water to form nitrous acid, which then forms nitric acid:
- NOF + H2O → HNO2 + HF
- 3 HNO2 → HNO3 + 2 NO + H2O
Nitrosyl fluoride can also convert alcohols to nitrites:
- ROH + NOF → RONO + HF
It has a bent molecular shape.
Uses
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.
References
Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.