Copper(II) peroxide
3D model (JSmol)
  • InChI=1S/Cu.O2/c;1-2/q+2;-2
  • [Cu+2].[O-]-[O-]
Molar mass 95.945 g/mol
Appearance dark olive-green
Related compounds
Related compounds
Copper(IV) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Copper peroxide is an inorganic compound with the formula CuO2. It is an oxide of copper(II), with the two oxygen atoms as a peroxide unit. It appears as a dark olive green solid or similarly colored suspension and is unstable, decomposing to oxygen and other copper oxides.


Copper peroxide is prepared by the reaction of cold solutions of hydrogen peroxide and Schweizer's reagent, the latter prepared from copper hydroxide and dilute ammonia solution.[1] The Schweizer's reagent used must not contain excess ammonia.[1] Copper peroxide may also be produced by the reaction of an ice-cold solution of hydrogen peroxide with a suspension of copper hydroxide.[2] It may also form from the very slow reaction of finely divided cupric oxide with cold hydrogen peroxide.[3]


When wet, copper peroxide decomposes[4] at temperatures above 6°C; it "is far more stable when dry".[3]


  1. ^ a b The collected works of Sir Humphry Davy: Discourses delivered before the Royal society. Elements of agricultural chemistry, pt. I. The Chemical Society (Great Britain). 1894. p. 32.
  2. ^ Friend, John Newton (1924). A Text-book of Inorganic Chemistry. C. Griffin, Ltd. p. 276.
  3. ^ a b Journal of the Chemical Society of London, Volume 48, Part 1. London. 1885. p. 124.
  4. ^ Electrical World, Volume 39. 1902. p. 997.