Chemical elements
    Physical Properties
    Chemical Properties
      Beryllium Hydride
      Beryllium Fluoride
      Beryllium Chloride
      Beryllium Bromide
      Beryllium Iodide
      Beryllium Double Halides
      Beryllium Oxyhalides
      Beryllium Oxide
      Beryllium Hydroxide
      Beryllium Beryllate
      Beryllium Peroxide
      Beryllium Sulphide
      Beryllium Sulphide
      Beryllium Double Sulphates
      Beryllium Sulphite
      Beryllium Thiosulphate
      Beryllium Selenate
      Beryllium Chromate
      Beryllium Hydride
      Beryllium Chromite
      Beryllium Molybdate
      Beryllium Nitride
      Beryllium Azide
      Beryllium Nitrate
      Beryllium Phosphates, Phosphite, and Hypophosphite
      Beryllium Hypophosphate
      Beryllium Arsenates
      Beryllium Arsenite
      Beryllium Antimonate
      Beryllium Hydride
      Beryllium Vanadates
      Beryllium Niobate
      Beryllium Carbide
      Beryllium Borocarbide
      Beryllium Carbonate
      Beryllium Acetate
      Beryllium Oxalates
      Beryllium Cyanide
      Beryllium Platinocyanide
      Beryllium Silicates
      Beryllium Silicotungstate
      Beryllium Borate
      Beryllium Aluminate

Beryllium Oxide, BeO

Beryllium Oxide, BeO, obtained by heating the hydroxide, is a white powder which is very refractory and, like alumina, becomes difficultly soluble in acids by heating to redness. It can also be obtained by heating any beryllium salt containing a volatile acid. Concentrated nitric or hydrochloric acid only dissolves it slowly, but concentrated sulphuric acid readily converts it into the anhydrous sulphate. It is reducible by carbon in the electric furnace, and at a lower temperature if copper is present. Fluorine vigorously converts it into the fluoride. It melts at 2450° ± 56° C., and is very volatile near its melting-point.

When beryllia fuses and volatilises in the electric furnace it cools to hexagonal crystals that are slightly harder than corundum and are isomorphous with zinc oxide. It can also be crystallised from fused alkali silicates. At 4° C. its density is about 3; between 0° C. and 100° C., its specific heat is 0.247, and it is diamagnetic.

Parsons refers to a " light and feathery " oxide of beryllium which he obtained by heating a dry mixture of beryllium and ammonium chlorides. Beryllia obtained by strongly igniting the hydroxide is distinctly hygroscopic. In high vacuo beryllia gives a blue fluorescence.

Parsons was unable to obtain the blue oxide from the ignition of the hexahydrated sulphate reported by Levi-Malvano.

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