we have copper (II)oxide written as cuo by dividing its valency by 2(HCF) BUT why hydrogen peroxide is written as HO
Answers
Answer:
It is produced on a large scale by pyrometallurgy used to extract copper from ores. The ores are treated with an aqueous mixture of ammonium carbonate, ammonia, and oxygen to give copper(I) and copper(II) ammine complexes, which are extracted from the solids. These complexes are decomposed with steam to give CuO.
It can be formed by heating copper in air at around 300 – 800°C:
2 Cu + O2 → 2 CuO
For laboratory uses, pure copper(II) oxide is better prepared by heating copper(II) nitrate, copper(II) hydroxide or basic copper(II) carbonate:
2 Cu(NO3)2 (s) → 2 CuO (s) + 4 NO2 (g) + O2 (g) (180°C)
Cu(OH)2 (s) → CuO (s) + H2O (l) (80-100°C)
Cu2CO3(OH)2 (s) → 2CuO (s) + CO2 (g) + H2O (g) (290°C)
Explanation:
Copper(II) oxide dissolves in mineral acids such as hydrochloric acid, sulfuric acid or nitric acid to give the corresponding copper(II) salts:
CuO + 2 HNO3 → Cu(NO3)2 + H2O
CuO + 2 HCl → CuCl2 + H2O
CuO + H2SO4 → CuSO4 + H2O
It reacts with concentrated alkali to form the corresponding cuprate salts:
2 MOH + CuO + H2O → M2[Cu(OH)4]
It can also be reduced to copper metal using hydrogen, carbon monoxide, or carbon:
CuO + H2 → Cu + H2O
CuO + CO → Cu + CO2
2CuO + C → 2Cu + CO2
When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary.
Copper(II) oxide belongs to the monoclinic crystal system. The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration.[1]
The work function of bulk CuO is 5.3eV[4]
Copper(II) oxide is a p-type semiconductor, with a narrow band gap of 1.2 eV. Cupric oxide can be used to produce dry cell batteries.
s a significant product of copper mining, copper(II) oxide is the starting point for the production of other copper salts. For example, many wood preservatives are produced from copper oxide.[3]
Cupric oxide is used as a pigment in ceramics to produce blue, red, and green, and sometimes gray, pink, or black glazes.
It is also incorrectly used as a dietary supplement in animal feed.[5] Due to low bioactivity, negligible copper is absorbed.[6]
It is also used when welding with copper alloys.[7]
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").