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

Copper peroxide, CuO2,H2O






At 0° C. neutral hydrogen peroxide converts an aqueous suspension of cupric hydroxide into the brown, crystalline peroxide. It is also produced by the interaction of solutions of cupric chloride and hydrogen peroxide with alcoholic potash at -40° or -50° C., and by the action of an ether-solution of hydrogen peroxide. on very finely powdered cupric hydroxide at 0° C. The product is always more or less impure. When moist, it decomposes rapidly with evolution of oxygen and formation of cupric oxide, but the decomposition of the dry substance is slow. In its reactions it behaves as a peroxide. Moser assigns to it the formula . The name peroxites has been suggested for the true salts of hydrogen peroxide.

The compounds obtained by the action of hydrogen peroxide on cupric hydroxide are regarded by Aldridge and Applebey as probably consisting of a mixture in varying proportions of cupric oxide and hydroxide with a yellow, gelatinous peroxide of the formula CuO2. A solution of sodium copper carbonate, Na2Cu(CO3)2, reacts with hydrogen peroxide to precipitate a very unstable, yellowish-brown peroxide, containing more oxygen than would correspond with the formula Cu2O3, but less than that required by CuO2.

In 1844 Kruger obtained pink solutions by the chlorination of alkaline suspensions of cupric hydroxide, and attributed the colour to the presence of salts (" cuprates ") of an acidic peroxide of copper. Aldridge and Applebey regard these so-called cuprates as having no real existence, the pink colour observed by Kruger being considered to be due to the formation of permanganate from traces of manganese dioxide.

This copper peroxide, Cu2O3, is stated to be formed as an orange-yellow substance by electrolytic oxidation with a high current-density at a copper anode immersed in concentrated caustic alkali, and also by the action of alkaline hypochlorite and hypobromite on cupric hydroxide and copper. Various investigators have described a compound with the same formula. An example is the interaction of potassium persulphate with a mixture of cupric hydroxide and barium hydroxide cooled with ice and salt, colour changes taking place in the solution, and a tenuous, amaranth-red precipitate being deposited. The substance formed yields oxygen with sulphuric acid, liberates chlorine from hydrochloric acid, oxidizes ammonia in the cold to nitrogen and nitrous acid and traces of nitric acid, decolorizes permanganate, and liberates iodine from potassium iodide. It is not a peroxide, since with dilute acids it does not yield hydrogen peroxide, and therefore differs from the orange-yellow peroxide obtained by means of hydrogen peroxide. The ratio between the percentages of copper and active oxygen present corresponds with the formula Cu2O3.


© Copyright 2008-2012 by atomistry.com