Chemical elements
  Lithium
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
      Lithium hydride
      Lithium chloride
      Lithium bromide
      Lithium iodide
      Lithium iodide tetrachloride
      Lithium hypochlorite
      Lithium chlorate
      Lithium perchlorate
      Lithium bromate
      Lithium iodate
      Lithium periodates
      Lithium monoxide
      Lithium peroxide
      Lithium hydroxide
      Lithium monosulphide
      Lithium polysulphides
      Lithium sulphite
      Lithium sulphate
      Lithium persulphate
      Lithium thiosulphate
      Lithium dithionate
      Lithium selenide
      Lithium selenite
      Lithium selenate
      Lithium chromate
      Lithium permanganate
      Lithium molybdates
      Lithium nitride
      Lithium hydrazoate
      Lithamide
      Lithium nitrite
      Lithium nitrate
      Lithium phosphide
      Lithium orthophosphate
      Lithium pyrophosphate
      Lithium metaphosphate
      Lithium arsenide
      Lithium meta-arsenite
      Lithium arsenate
      Lithium antimonide
      Lithium antimonate
      Lithium carbide
      Lithium carbonate
      Lithium percarbonate
      Lithium cyanide
      Lithium thiocyanate
      Lithium silicide
      Lithium silicates
      Lithium borates

Lithium nitride, Li3N






The nitride is best prepared by the action of nitrogen on the metal at ordinary temperatures, the product being a grey, amorphous, hygroscopic substance, unaffected by dry hydrogen or air, but rapidly decomposed by moisture. It absorbs both nitrogen and oxygen from the air. A ruby-red, crystalline modification is formed by the action of lithium on nitrogen at 450° to 460° C. It is less hygroscopic than the amorphous form, and does not absorb gases in the cold. At 840° to 845° C. in a current of nitrogen the amorphous nitride becomes crystalline. Water decomposes the nitride according to the equation

Li3N+3H2O = 3LiOH+NH3.

Guntz recommends the formation of the nitride as a convenient means of isolating argon, and its interaction with metallic chlorides as a method for preparing other nitrides. For the heat of formation he found 49.5 Cal. It is formed by the action of light on lithium imide, Li2NH:

2Li2NHLi3N+LiNH2.


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