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Physical properties

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.

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:

For this reason, aqueous NOF solutions are, like aqua regia, powerful solvents for metals.²

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.³

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:⁴

Uses

Nitrosyl fluoride is used as a solvent and as a fluorinating and nitrating[dubious – discuss] agent in organic synthesis.

External links

• WebBook page for NOF
• National Pollutant Inventory - Fluoride and compounds fact sheet

References

1. Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4. 978-0-08-022057-4 ↩

2. Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4. 978-0-08-022057-4 ↩

3. Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4. 978-0-08-022057-4 ↩

4. Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4. 978-0-08-022057-4 ↩