Chemical elements
  Nitrogen
    Isotopes
    Energy
    Nitrogen Cycle
    Production
    Application
    Physical Properties
    Chemical Properties
      Nitrogen Chloride
      Nitrogen Iodide
      Monochloramine
      Nitrosyl Fluoride
      Nitrosyl Chloride
      Nitrosyl Bromide
      Nitryl Fluoride
      Nitryl Chloride
      Di-imide
      Nitramide
      Nitrohydroxylamine
      Hyponitrous acid
      Nitrous Oxide
      Nitric Oxide
      Nitrogen Trioxide
      Nitrogen Tetroxide
      Nitrogen Pentoxide
      Nitroso-nitrogen Trioxide
      Nitrous Acid
      Pernitric Acid
      Sulphur Nitride
      Pentasulphur Dinitride
    Ammonia
    Hydroxylamine
    Hydrazine
    Azoimide
    Nitric Acid

Nitryl Fluoride, NO2F






This compound is obtained by the action of nitric oxide on fluorine at the temperature of liquid air:

4NO + F2 = 2NO2F + N2.

At ordinary temperatures nitryl fluoride is a colourless, pungent- smelling gas, which attacks the mucous membrane. The liquid boils at - 63-5° C., and solidifies at -139° C. to a colourless solid. The vapour density is 2.24 (compared with air=1), which is almost identical with that required by the formula NO2F (2.26).

The gas is very reactive, and attacks many metals and non-metals, such as arsenic, antimony, aluminium, iron, mercury, alkali and alkaline earth metals, phosphorus, boron, and silicon. It has no action on hydrogen, sulphur, or carbon. Water decomposes nitryl fluoride with the quantitative formation of nitric and hydrofluoric acids:

NO2F + H2O = HNO3 + HF.


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