Chemical elements
  Copper
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
    Cuprous Compounds
    Complex Copper Compounds
    Cupric Compounds
      Cupric hydride
      Cupric fluoride
      Cupric chloride
      Copper hydroxide
      Cupric bromide
      Cupric iodide
      Cupric chlorate
      Cupric bromate
      Cupric iodate
      Cupric periodates
      Cupric oxide
      Copper peroxide
      Cupric hydroxide
      Cupric sulphide
      Cupric polysulphides
      Cupric sulphite
      Cupric sulphate
      Copper Sulphate
      Cupric selenide
      Cupric selenite
      Double Copper Selenates
      Cupric telluride
      Cupric dithionate
      Cupric tetrathionate
      Cupric hydrazoate
      Cupric nitrite
      Cupric nitrate
      Cupric phosphide
      Cupric hypophosphite
      Cupric phosphite
      Cupric orthophosphate
      Cupric pyrophosphate
      Cupric metaphosphate
      Cupric arsenate
      Cupric metantimonite
      Cupric pyroantimonate
      Cupric metantimonate
      Cupric acetylide
      Cupric carbide
      Cupric carbonates
      Cupric cyanide
      Cupric thiocyanate
      Cupric silicates
      Cupric metaborate
      Cupric acetate
    PDB 1a2v-1bxu
    PDB 1bxv-1fwx
    PDB 1g3d-1j9t
    PDB 1jcv-1mfm
    PDB 1mg2-1paz
    PDB 1pcs-1sii
    PDB 1sjm-1w6w
    PDB 1w77-2afn
    PDB 2ahk-2dv6
    PDB 2dws-2ggp
    PDB 2ghz-2mta
    PDB 2nrd-2vm3
    PDB 2vm4-2yah
    PDB 2yam-3bkt
    PDB 3bqv-3fyi
    PDB 3g5w-3mie
    PDB 3mif-3t6v
    PDB 3t6w-9pcy

Cupric carbonates






The normal salt has not been prepared. Malachite, CuCO3,Cu(OH)2, occurs in monoclinic crystals, density 3.7 to 4. It has been produced artificially. Azurite, 2CuCO3,Cu(OH)2, forms monoclinic crystals, density 3.5 to 3.88. It has been obtained by a laboratory method.

The formation of basic carbonates of copper by the interaction of solutions of cupric sulphate and of the carbonates of sodium has been investigated by Pickering. Sodium carbonate precipitates a blue, basic carbonate, 5CuO,2CO2,nH2O, which is converted by drying over sulphuric acid at 100° C. into another hydrate of green colour, 5CuO,2CO2,3H2O. In moist air the green hydrate becomes reconverted into the blue form:

5CuSO4 + 8Na2CO3 + 3H2O = 5CuO,2CO2 + 5Na2SO4 + 6NaHCO3.

The blue carbonate is transformed by concentrated aqueous sodium carbonate into cupric hydroxide, and by aqueous sodium hydrogen carbonate into malachite, 2CuO,CO2,H2O. Pickering considered ordinary commercial copper carbonate to be similar in constitution to malachite, a view questioned by Dunnicliff and Lai.

Sodium hydrogen carbonate and cupric sulphate react to precipitate a blue, basic carbonate, 5CuO,3CO2,nH2O, converted by drying at 100° C. into another blue hydrate, 5CuO,3CO2,7H2O. Another basic carbonate is also produced in the same reaction. It has the formula 8CuO,3CO2,6H2O, is dark blue in colour, and becomes green at 100° C. No other basic carbonate was isolated by Pickering. All the products are insoluble in water and sodium-carbonate solution, but dissolve slightly in solutions of carbon dioxide and of sodium hydrogen carbonate, with production of the normal carbonate or a double carbonate.

Feist has prepared a basic carbonate, 7CuO,4CO2,H2O, by powdering together crystallized cupric sulphate and sodium carbonate, and then adding water. It is difficult to separate the substance from a basic cupric sulphate simultaneously formed. Auger has described an amorphous basic carbonate of the formula 8CuO,5CO2,7H2O. Another basic carbonate, 7CuO,2CO2,5H2O, has been prepared by the interaction of a mixture of sodium carbonate and sodium hydrogen carbonate with cupric sulphate in aqueous solution. Complex carbonates of copper with sodium and potassium have also been obtained. An example of this type of double salt of the formula Na2Cu(CO3)2,3H2O crystallizes on addition of a solution of cupric acetate to one of sodium carbonate and sodium hydrogen carbonate at 50° C. It forms needles or rosettelike agglomerations, and above 100° C. it is converted into cupric oxide and sodium carbonate with elimination of water and carbon dioxide. It is decomposed by water, but can be recrystallized from a concentrated solution of sodium carbonate containing sodium hydrogen carbonate.


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