Nitrosyl fluoride
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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 |
| 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).
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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: this can be rationalized in the VSEPR model in terms of the lone-pair of electrons located on the N atom.
Uses
Nitrosyl fluoride is used as a solvent[citation needed] and as a fluorinating and nitrating agent in organic synthesis.[citation needed] 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 978-0-08-037941-8.