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Nitrosyl fluoride

Nitrosyl fluoride
Skeletal formula of nitrosyl fluoride with measurements
Ball and stick model of nitrosyl fluoride
Names
IUPAC name
Nitrosyl fluoride[citation needed]
Other names
Nitrogen oxyfluoride[citation needed]
Identifiers
3D model (JSmol)
Abbreviations NOF[citation needed]
ChemSpider
ECHA InfoCard 100.029.230
EC Number
  • 232-153-6
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
Except where otherwise noted, data are 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: 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.

External links