Copper(II) oxide: Wikis

  

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Copper(II) oxide
Identifiers
CAS number 1317-38-0 Yes check.svgY
PubChem 14829
RTECS number GL7900000
Properties
Molecular formula CuO
Molar mass 79.545 g/mol
Appearance black powder
Density 6.31 g/cm3
Melting point

1201 °C (1474 K)

Boiling point

2000 °C

Solubility in water insoluble
Solubility in Ammonium hydroxide soluble
Band gap 1.2 eV
Structure
Crystal structure monoclinic, mS8[1]
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°
Hazards
MSDS Fischer Scientific
EU Index Not listed
NFPA 704
NFPA 704.svg
0
2
1
Flash point Non-flammable
Related compounds
Other anions Copper(II) sulfide
Other cations Nickel(II) oxide
Zinc oxide
Related compounds Copper(I) oxide
 Yes check.svgY (what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Copper(II) oxide or cupric oxide (CuO) is the higher oxide of copper. As a mineral, it is known as tenorite.

Contents

Chemistry

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:

2 Cu + O2 → 2 CuO

Here, it is formed along with copper(I) oxide as a side product; thus, it is better prepared by heating copper(II) nitrate, copper(II) hydroxide or copper(II) carbonate:

2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
Cu(OH)2 (s) → CuO (s) + H2O (l)
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
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]

It can also be reduced to copper metal using hydrogen or carbon monoxide:

CuO + H2 → Cu + H2O
CuO + CO → Cu + CO2

A laboratory method for preparing copper II oxide would be to electrolyze water containing sodium bicarbonate at a moderate voltage with a copper anode, collect the mixture of copper hydroxide, basic copper carbonate, and copper carbonate produced, and heat it.

Crystal structure

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°.[1] The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration.[1]

Unit cell of CuO part of CuO's crystal structure
the unit cell of copper(II) oxide
part of the crystal structure of CuO

Health effects

Copper(II) oxide is an irritant. It also can cause damage to the endocrine and central nervous system. Contact to the eyes can cause irritation and contact to the 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. [2]. 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 [3][4] as well as copper being extremely well metabolized by humans. Copper oxide is used in vitamins supplements as a safe source of copper[5] 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.[6][7][8][9]. The risk of dermal sensitivity to copper is considered extremely minimal.[10]

Uses

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.[11] 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.[12]

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

Cupric oxide can be used to safely dispose of hazardous materials such as cyanide, hydrocarbons, halogenated hydrocarbons and dioxins, through oxidation[13].

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

Properties

See also

References

  1. ^ a b c 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
  2. ^ "Material safety data sheet: Copper (II) oxide". Iowa State University. 2003. http://avogadro.chem.iastate.edu/MSDS/CuO.html. Retrieved 2007-01-26. 
  3. ^ Uauy et al (1998). "Essentiality of copper in humans". Am J Clin Nutr 67 (3): 952S-9S. http://www.ajcn.org/cgi/content/abstract/67/5/952S. 
  4. ^ Sen et al (2002). "Copper-induced vascular endothelial growth factor expression and wound healing.". Am J Physiol Heart Circ Physiol 282: H1821-27. http://ajpheart.physiology.org/cgi/content/abstract/282/5/H1821. 
  5. ^ "Vitamin Supplements:". http://www.empr.com/vitaminsmineralssupplements/centrum/drug/5901. 
  6. ^ 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. PMID 19467028. 
  7. ^ Borkow G, et al. (2009). "Reducing the risk of skin pathologies in diabetics by using copper impregnated socks.". Med Hypotheses 73(6): 883-6. PMID 19559540. 
  8. ^ Borkow G, et al. (2005). "Copper as a biocidal tool.". Curr Med Chem 12(18): 2163-75. PMID 16101497. 
  9. ^ Borkow G, et al. (2004). "Copper-impregnated products with potent biocidal activities.". FASEB J. 18(14): 1728-30. PMID 15345689. 
  10. ^ Hostynek JJ, and Maibach HI (2003). "hypersensitivity: dermatologic aspects-an overview". Rev Environ Health 153: 153–83. PMID 14672513. 
  11. ^ "Uses of Copper Compounds: Other Copper Compounds". Copper Development Association. 2007. http://www.copper.org/applications/compounds/other_compounds.html. Retrieved 2007-01-27. 
  12. ^ "Cupric Oxide Data Sheet". Hummel Croton Inc.. 2006-04-21. http://www.axxousa.com/data/cuox_d.html. Retrieved 2007-02-01. 
  13. ^ Kenney, Charlie W.; Uchida, Laura A. (April), Use of copper (II) oxide as source of oxygen for oxidation reactions, http://www.freepatentsonline.com/4582613.html, retrieved 2007-06-29 
  14. ^ 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: 1173. doi:10.1063/1.330567. 

External links


Simple English

[[File:|thumb|Copper(II) oxide]] Copper(II) oxide, also known as cupric oxide, is a chemical compound. Its chemical formula is CuO. It has copper in its +2 oxidation state. It also has oxide ions.

Contents

Properties

Copper(II) oxide is a black solid. It dissolves in acids to make copper(II) salts. It can react with carbon monoxide or hydrogen to make copper metal. It dissolves in very concentrated alkalis. It dissolves in ammonia to make a dark blue solution, similar to copper(II) hydroxide.

Preparation

It can be made by heating copper(II) hydroxide. It can also be made by heating copper in air. It can also be made by heating copper(II) carbonate or copper(II) nitrate.

Uses

Copper(II) oxide is used to color ceramics. It is also used to make thermite. It can react with many toxic chemicals to oxidize them, so they are not toxic any more. It can be added to vitamins to get copper into the body. It can also be added to clothing to kill germs.

Safety

Copper(II) oxide is toxic when eaten. It can be eaten in very small amounts, such as in vitamins. This adds copper to the body, which is needed.

See also








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