Chemical elements
    Physical Properties
    Chemical Properties
      Cerous hydride
      Cerous fluoride
      Cerous chloride
      Cerous oxychloride
      Cerous bromide
      Cerous iodide
      Cerous perchlorate
      Cerous bromate
      Cerous iodate
      Cerous oxide
      Cerous sesquioxide
      Cerous hydroxide
      Cerous sulphide
      Cerous persulphide
      Cerous oxysulphide
      Cerous sulphite
      Cerous sulphate
      Cerous dithionate
      Cerous selenite
      Cerous selenate
      Cerous chromate
      Cerous molybdate
      Cerous tungstate
      Cerous nitride
      Cerous nitrite
      Cerous nitrate
      Cerous hypophosphite
      Cerous orthophosphate
      Cerous vanadate
      Cerous carbide
      Cerous silicide
      Cerous carbonate
      Cerous thiocyanate
      Cerous platinocyanide
      Cerous oxalate
      Cerous silicate
      Ceric fluoride
      Ceric chloride
      Ceric iodate
      Ceroceric oxide
      Ceroceric hydroxide
      Ceric oxide
      Cerium dioxide
      Ceric hydroxide
      Perceric hydroxide
      Ceric hydrosulphate
      Ceric sulphate
      Ceric selenite
      Ceric chromate
      Ceric molybdate
      Ceric nitrate
      Ceric ammonium nitrate
      Ceric orthophosphate
      Ceric dihydrogen arsenate
      Ceric carbonate
      Perceric carbonate
      Ceric acetate
      Ceric oxalate
      Ceric acetylacetonate
      Ceric borate
    PDB 1ak8-1n65

Cerous oxide, Ce2O3

Cerium sesquioxide or cerous oxide, Ce2O3, so readily oxidises to form cerium dioxide that cerous salts of volatile oxyacids yield ceria when ignited in the air. The sesquioxide can be prepared by the reduction of the dioxide with hydrogen at 150 atmos. pressure and at a temperature of about 2000° C. In small quantities and mixed with much ceria and a little carbon, it is produced by the ignition of cerous oxalate in vacuo or in hydrogen. It is also produced in poor yield by heating ceria with zinc at the boiling-point of the metal, but it cannot be separated from the other products of the reaction.1 The simplest method yet known for its preparation consists in heating ceria with metallic calcium and dissolving out the lime and excess of calcium in aqueous ammonium chloride at -10° C. The sesquioxide is thus obtained as a yellowish-green powder which readily absorbs oxygen even at ordinary temperatures and burns easily when gently heated.

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