Chemical elements
    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
      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 monoxide, Li2O

The Lithium monoxide, Li2O prepared by heating the metal in oxygen at 200° C. always contains the peroxide, but it can be obtained pure by heating the carbonate at 780° to 800° C. in a current of hydrogen, or by heating the hydroxide at 780° C. or the nitrate to fusion under similar conditions. The volatility of the monoxide necessitates careful regulation of the temperature.

Lithium monoxide forms a white, amorphous, more or less porous mass. Its melting-point is unknown, owing to its volatility at high temperatures. For the density of an impure specimen, Brauner and Watts found at 15° C. the value 2.102. At a high temperature it attacks platinum, but its great stability is exemplified by its indifference towards hydrogen, carbon, and carbon monoxide.

Lithium monoxide is slowly attacked by water, with formation of the intensely alkaline solution of the hydroxide. The heat evolved is given by the equation

[Li2O]+Aq.=2LiOH,Aq.+31.20 Cal.

Since the heat evolved by solution of 2 gram-atoms of lithium in water is 106.4 Cal., and the heat of formation of water is 68.3 Cal., the heat of formation of the oxide from its elements is given by the equation

2[Li]+(O)=[Li2O] +143.5 Cal.

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