|Jmol-3D images||Image 1
|Molar mass||79.545 g/mol|
|Appearance||black to brown powder|
|Melting point||1,326 °C; 2,419 °F; 1,599 K|
|Boiling point||2,000 °C; 3,630 °F; 2,270 K|
|Solubility in water||insoluble|
|Solubility||soluble in ammonium chloride, potassium cyanide
insoluble in alcohol, ammonium hydroxide, ammonium carbonate
|Band gap||1.2 eV|
|Refractive index (nD)||2.63|
|Crystal structure||monoclinic, mS8|
|Space group||C2/c, #15|
|Lattice constant||a = 4.6837, b = 3.4226, c = 5.1288|
|Lattice constant||α = 90°, β = 99.54°, γ = 90°|
|Std enthalpy of
|EU Index||Not listed|
|EU classification||Harmful (Xn)
Dangerous for the environment (N)
|Other anions||Copper(II) sulfide|
|Other cations||Nickel(II) oxide
|Related compounds||Copper(I) oxide|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C or 77 °F, 100 kPa)
- 2 Cu + O2 → 2 CuO
- 2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
- Cu(OH)2 (s) → CuO (s) + H2O (l)
- CuCO3 → CuO + CO2
- 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 XOH + CuO + H2O → X2[Cu(OH)4]
- CuO + H2 → Cu + H2O
- CuO + CO → Cu + CO2
A laboratory method for preparing copper(II) oxide is to electrolyze water containing sodium bicarbonate at a moderate voltage with a copper anode, collect the mixture of insoluble copper hydroxide, basic copper carbonate, and copper carbonate precipitates, and heat it to release the hydrogen, carbon and excess oxygen.
Copper(II) oxide belongs to the monoclinic crystal system, with a crystallographic point group of 2/m or C2h. The space group of its unit cell is C2/c, and its lattice parameters are a = 4.6837(5), b = 3.4226(5), c = 5.1288(6), α = 90°, β = 99.54(1)°, γ = 90°. The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration.
Copper(II) oxide is an irritant. It also can cause damage to the endocrine and central nervous system. Contact to the eyes or skin can cause irritation. Ingesting cupric oxide powder can result in a metallic taste, nausea, vomiting and stomach pain. In more severe cases, there may be blood in vomit or black or tarry stools, jaundice and enlarged liver. Blood cells rupture resulting in circulatory collapse and shock. Inhalation can lead to damage to the lungs and septum. Inhalation of fumes during smelting of cupric oxide powder can lead to a disease called metal fume fever, which can result in flu like symptoms. Copper (II) oxide can cause a toxic build-up of copper in a small subset of the population with Wilson's disease. Handling copper (II) oxide powder should be done in well ventilated area, and care should be taken to avoid contact with the skin or eyes. However copper is an essential trace element for the normal function of many tissues, including the nervous system, immune system, heart, skin and for the formation of capillaries  as well as copper being extremely well metabolized by humans. Copper (II) oxide (Cupric oxide, not Cuprous oxide) has extremely low bioavailability (practically zero) and should not be taken in conditions of copper deficiency, especially as part of a multivitamin which also includes zinc or molybdenum. Excessive zinc or molybdenum intake eliminates copper from the body. Copper oxide is used in vitamins supplements as a safe source of copper and over-the-counter treatments. Copper oxide is also used in consumer products such as pillowcases and socks, due to its cosmetic and anti-microbial properties. The risk of dermal sensitivity to copper is considered extremely minimal.
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 used to produce cuprammonium hydroxide solutions, used to make rayon. It is also occasionally used as a dietary supplement in animals, against copper deficiency. Copper(II) oxide has application as a p-type semiconductor, because it has a narrow band gap of 1.2 eV. It is an abrasive used to polish optical equipment. Cupric oxide can be used to produce dry cell batteries. It has also been used in wet cell batteries as the cathode, with lithium as an anode, and dioxalane mixed with lithium perchlorate as the electrolyte. Copper(II) oxide can be used to produce other copper salts. It is also used when welding with copper alloys.
Another use for cupric oxide is as a substitute for iron oxide in thermite. This can turn the thermite from an incendiary to a low explosive.
Use in disposal
Here are equations depicting the decomposition of phenol and pentachlorophenol, respectively, with copper oxide:
- C6H5OH + 14CuO → 6CO2 + 3H2O + 14Cu
- C6Cl5OH + 2H2O + 9CuO → 6CO2 + 5HCl + 9Cu
- The effect of hydrostatic pressure on the ambient temperature structure of CuO, Forsyth J.B., Hull S., J. Phys.: Condens. Matter 3 (1991) 5257-5261 , doi:10.1088/0953-8984/3/28/001
- "Material safety data sheet: Copper (II) oxide". Iowa State University. 2003. Retrieved 2007-01-26.
- Uauy et al. (1998). "Essentiality of copper in humans". Am J Clin Nutr 67 (3): 952S–9S. PMID 9587135.
- Sen et al. (2002). "Copper-induced vascular endothelial growth factor expression and wound healing". Am J Physiol Heart Circ Physiol 282 (5): H1821–27. doi:10.1152/ajpheart.01015.2001. PMID 11959648.
- Baker, DH (1999 Dec). "Cupric oxide should not be used as a copper supplement for either animals or humans.". The Journal of nutrition 129 (12): 2278–9. PMID 10573563.
- "Vitamin Supplements:".
- Borkow G et al. (2009). "Improvement of facial skin characteristics using copper oxide containing pillowcases: a double-blind, placebo-controlled, parallel, randomized study". Int J Cosmet Sci 31 (6): 437–43. doi:10.1111/j.1468-2494.2009.00515.x. PMID 19467028.
- Borkow G et al. (2009). "Reducing the risk of skin pathologies in diabetics by using copper impregnated socks". Med Hypotheses 73 (6): 883–6. doi:10.1016/j.mehy.2009.02.050. PMID 19559540.
- Borkow G et al. (2005). "Copper as a biocidal tool". Curr Med Chem 12 (18): 2163–75. doi:10.2174/0929867054637617. PMID 16101497.
- Borkow G et al. (2004). "Copper-impregnated products with potent biocidal activities". FASEB J. 18 (14): 1728–30. doi:10.1096/fj.04-2029fje. PMID 15345689.
- Hostynek JJ, and Maibach HI (2003). "hypersensitivity: dermatologic aspects-an overview". Rev Environ Health 153 (3): 153–83. PMID 14672513.
- "Uses of Copper Compounds: Other Copper Compounds". Copper Development Association. 2007. Retrieved 2007-01-27.
- "Cupric Oxide Data Sheet". Hummel Croton Inc. 2006-04-21. Retrieved 2007-02-01.
- Kenney, Charlie W.; Uchida, Laura A. (April). "Use of copper (II) oxide as source of oxygen for oxidation reactions". Retrieved 2007-06-29
- F. P. Koffyberg and F. A. Benko (1982). "A photoelectrochemical determination of the position of the conduction and valence band edges of p-type CuO". J. Appl. Phys. 53 (2): 1173. doi:10.1063/1.330567.
|Wikimedia Commons has media related to Copper(II) oxide.|
- National Pollutant Inventory - Copper and compounds fact sheet
- Copper oxides project page
- CDC - NIOSH Pocket Guide to Chemical Hazards