Copper(II) oxide

Copper(II) oxide belongs to the monoclinic crystal system. The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration. ==Production==

It is produced on a large scale by pyrometallurgy, as one stage in extracting copper from its ores. The ores are treated with an aqueous mixture of ammonium carbonate, ammonia, and oxygen to ultimately give copper(II) ammine complex carbonates, such as . After extraction from the residues and after separation from iron, lead, etc. impurities, the carbonate salt is decomposed with steam to give CuO. : (180°C) : Dehydration of cupric hydroxide has also been demonstrated: : Copper(II) oxide can also be produced, at industrial scales, by chemical precipitation of copper(II) sulfate (CuSO4) with sodium hydroxide (NaOH) to form copper(II) hydroxide, which is then heated at around 250°C to produce CuO. ==Uses==

As a significant product of copper mining, copper(II) oxide is the starting point for the production of many other copper salts. For example, many wood preservatives are produced from copper oxide. Due to low bioactivity, negligible copper is absorbed. It is used when welding with copper alloys. A copper oxide electrode formed part of the early battery type known as the Edison–Lalande cell. Copper oxide was also used in a lithium battery type (IEC 60086 code "G"). Pyrotechnics and fireworks Used as moderate blue coloring agent in blue flame compositions with additional chlorine donors and oxidizers such as chlorates and perchlorates. Providing oxygen it can be used as flash powder oxidizer with metal fuels such as magnesium, aluminium, or magnalium powder. Sometimes it is used in strobe effects and thermite compositions as crackling stars effect. ==Reactions==

Copper(II) oxide reacts with mineral acids such as hydrochloric acid, sulfuric acid, and nitric acid to give the corresponding hydrated copper(II) salts: : CuO + 2 HNO3 → Cu(NO3)2 + H2O : CuO + 2 HCl → CuCl2 + H2O : CuO + H2SO4 → CuSO4 + H2O In presence of water it reacts with concentrated alkali to form the corresponding cuprate salts: : 2 NaOH + CuO + H2O → Na2[Cu(OH)4] It can also be reduced to copper metal using hydrogen, carbon monoxide, and carbon: : CuO + H2 → Cu + H2O : CuO + CO → Cu + CO2 : 2 CuO + C → 2Cu + CO2 When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary. ==Similar compounds==

An example of natural copper(I,II) oxide is the mineral paramelaconite, Cu+2Cu2+2O3. ==See also==