Nitrosyl fluoride

Nitrosyl fluoride
Names
	IUPAC name Nitrosyl fluoride[citation needed]
	Other names Nitrogen oxyfluoride[citation needed]
Identifiers
CAS Number	7789-25-5 ;
3D model (JSmol)	Interactive image;
Abbreviations	NOF[citation needed]
ChemSpider	109874 ;
EC Number	232-153-6;
PubChem CID	123261;
UNII	9FXL2Q69DQ ;
	InChI InChI=1S/FNO/c1-2-3 Key: ZEIYBPGWHWECHV-UHFFFAOYSA-N ;
	SMILES FN=O;
Properties
Chemical formula	NOF
Molar mass	49.0045 g mol−1
Appearance	Colourless gas
Density	2.657 mg mL−1(gas) 1.326 g/cm3(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	Nitroxyl; Nitrosyl chloride; Nitrosyl bromide;
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Nitrosyl fluoride (N O F) 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 → MF_n + n NO

For this reason, aqueous NOF solutions are, like aqua regia, 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.

References

^ ^1.0 ^1.1 ^1.2 ^1.3 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4.

External links

[:0-1] 1.0 ^1.1 ^1.2 ^1.3 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 507. ISBN 978-0-08-022057-4.

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