Nitrosyl fluoride (NOF) is a covalently bonded nitrosyl compound.
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:
- n NOF + M → MFn + n NO
For this reason, aqueous NOF solutions, like aqua regia, are powerful solvents for metals.[1]
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.[1]
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:[1]
- ROH + NOF → RONO + HF
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.[citation needed]
References
- ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4.