Copper(II) oxide
| Copper(II) oxide | |
|---|---|
| |
| Systematic name | Copper(II) oxide |
| Other names | cupric oxide |
| Molecular formula | CuO |
| Molar mass | 79.545 g/mol |
| CAS number | [1317-38-0] |
| Density | 6.31 g/cm3 |
| Solubility (water) | ~0 g/l |
| Melting point | 1201 °C + |
| Boiling point | xx.x °C |
| Lattice constants | a=4.6837Å, b=3.4226Å, c=5.1288, β=99.54°[1] |
| Disclaimer and references | |
Copper(II) oxide or cupric oxide (CuO) is the higher oxide of copper. It is a black solid with an ionic structure which melts above 1200 °C with some loss of oxygen. It can be formed by heating copper in air, but in this case it is formed along with copper(I) oxide; thus, it is better prepared by heating copper(II) nitrate, copper(II) hydroxide or copper(II) carbonate:
CuCO3 → CuO + CO2
Copper(II) oxide is a basic oxide, so it 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
It can also be reduced to copper metal using hydrogen or carbon monoxide:
H2 + CuO → Cu + H2O
Copper (II) oxide has uses as a p-type semiconductor, with a narrow band gap of 1.2 eV.
See also
References
- ^ PRB, Vol 42, No 12, Page 10060 (2006)
External links
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