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

Nitrogen Iodide, N2H3I3






A very explosive compound of nitrogen and iodine, discovered by Courtois in 1812, was investigated later by Serullas, who prepared it by the action of an alcoholic solution of iodine on aqueous ammonia.

The action of strong ammonia solution on solid iodine also produces the substance as a black powder, which can be filtered off.

Alcoholic solutions of iodine and ammonia produce the same compound.

A convenient method is to add gradually a solution of iodine in potassium iodide to aqueous ammonia, when a black precipitate separates.

The reaction between iodine and ammonia appears to proceed in three stages. Firstly, hypoiodous acid and ammonium iodide are produced:

NH4OH + I2 = HOI + NH4I;

and the hypoiodous acid further combines with ammonia to form ammonium hypoiodite:

NH4OH + HOI = NH4IO + H2O.

Finally, the ammonium hypoiodite decomposes into nitrogen iodide:

3NH4ION2H3I3 + NH4OH + 2H2O.

The last reaction is apparently reversible, as the nitrogen iodide redissolves in strong ammonia.

Ammonium iodide and bleaching-powder solutions also give the explosive nitrogen iodide.


Properties of Nitrogen Iodide

Nitrogen iodide exists in the form of flattened needles which are copper-coloured by reflected light and red by transmitted light, with a density of 3.5. It is one of the most explosive of substances; when dry it will explode spontaneously or by the lightest contact, even that of a feather. Warming or exposure to strong light also causes its explosive decomposition, and in all its reactions it tends to break down into nitrogen and hydrogen iodide.

The composition of nitrogen iodide has been the subject of much investigation, but it seems that the usual product of ammonia and iodine is NI3.NH3. Sodium sulphite is oxidised to the sulphate according to the following equation: -

3Na2SO3 + N2H3I3 + 3H2O = 3Na2SO4 + 2NH4I + HI.

The reaction between nitrogen iodide and zinc ethyl confirms the composition N2H3I3:

N2H3I3 + 3Zn(C2H5)2 = 3ZnC2H5I + NH3 + N(C2H5)3.

A black explosive compound is obtained when silver nitrate is added to nitrogen iodide suspended in water, which has the composition NI3.AgNH2.

The hydrolysis of nitrogen iodide by water proceeds according to the equation

N2H3I3 + 3H2O ⇔ 2NH4IO + HIO.

Many substances are readily oxidised by nitrogen iodide: hydrogen iodide liberates iodine, hydrogen chloride forms iodine chloride, hydrogen cyanide gives iodine cyanide, ICN, and alkalies form a mixture of iodide and iodate.

At low temperatures a number of addition compounds of nitrogen iodide can be produced, such as NI3.2NH3, NI3.3NH3, and NI3.12NH3.
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