Copper(II) oxide 1177019 218512913 2008-06-10T23:46:59Z Freestyle-69 6502796 /* Uses */ Unneccesary capitals {{chembox new | ImageFile = copperIIoxide.jpg | ImageSize = | IUPACName = Copper(II) oxide | OtherNames = cupric oxide | Formula = CuO | Section1 = {{Chembox Identifiers | Abbreviations = | CASNo = 1317-38-0 | EINECS = | PubChem = | SMILES = | InChI = | RTECS = | MeSHName = | ChEBI = | KEGG = | ATCCode_prefix = | ATCCode_suffix = | ATC_Supplemental =}} | Section2 = {{Chembox Properties | MolarMass = 79.545 g/mol | Appearance = | Density = 6.31 g/cm<sup>3</sup> | MeltingPt = 1201 °C + (1474 K) | Melting_notes = | BoilingPt = | Boiling_notes = | Solubility = insoluble | SolubleOther = | Solvent = | BandGap = 1.2[[eV]] | pKa = | pKb = }} | Section3 = {{Chembox Structure | CrystalStruct = [[monoclinic]] | SpaceGroup = C2/c | LattConst_a = 4.6837 | LattConst_b = 3.4226 | LattConst_c = 5.1288 | LattConst_beta = 99.54 | Coordination = | MolShape = }} | Section4 = {{Chembox Thermochemistry | DeltaHf = | DeltaHc = | Entropy = | HeatCapacity = }} | Section5 = {{Chembox Pharmacology | AdminRoutes = | Bioavail = | Metabolism = | HalfLife = | ProteinBound = | Excretion = | Legal_status = | Legal_US = | Legal_UK = | Legal_AU = | Legal_CA = | PregCat = | PregCat_AU = | PregCat_US = }} | Section6 = {{Chembox Explosive | ShockSens = | FrictionSens = | ExplosiveV = | REFactor = }} | Section7 = {{Chembox Hazards | ExternalMSDS = [http://www.sciencelab.com/xMSDS-Cupric_oxide-9923595 ScienceLab.com] | EUClass = | EUIndex = | MainHazards = | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | NFPA-O = | RPhrases = | SPhrases = | RSPhrases = | FlashPt = | Autoignition = | ExploLimits = | PEL = }} | Section8 = {{Chembox Related | OtherAnions = | OtherCations = | OtherFunctn = | Function = | OtherCpds = }} }} '''Copper(II) oxide''' or '''cupric oxide''' (CuO) is the higher [[oxide]] of [[copper]]. As a mineral, it is known as [[tenorite]]. == Chemistry == It is a black solid with an [[Ionic bonding|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]]: : 2Cu(NO<sub>3</sub>)<sub>2</sub> → 2CuO + 4NO<sub>2</sub> + O<sub>2</sub> : Cu(OH)<sub>2</sub>(s) → CuO(s) + H<sub>2</sub>O(l) : CuCO<sub>3</sub> → CuO + CO<sub>2</sub> Copper(II) oxide is a [[basic oxide]], so it dissolves in [[mineral acid]]s such as [[hydrochloric acid]], [[sulfuric acid]] or [[nitric acid]] to give the corresponding copper(II) salts: : CuO + 2HNO<sub>3</sub> → Cu(NO<sub>3</sub>)<sub>2</sub> + H<sub>2</sub>O : CuO + 2HCl → CuCl<sub>2</sub> + H<sub>2</sub>O : CuO + H<sub>2</sub>SO<sub>4</sub> → CuSO<sub>4</sub> + H<sub>2</sub>O It can also be reduced to [[copper]] metal using [[hydrogen]] or [[carbon monoxide]]: : CuO + H<sub>2</sub> → Cu + H<sub>2</sub>O : CuO + CO → Cu + CO<sub>2</sub> It is also made by reacting solid [[copper]] with [[oxygen]] gas. : 2Cu + O<sub>2</sub> → 2CuO == Crystal structure == Copper(II) oxide belongs to the [[monoclinic crystal system]], with a [[crystallographic point group]] of 2/m or ''C<sub>2h</sub>''. 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°. {|align="center" class="wikitable" |[[Image:Copper(II)-oxide-unit-cell-3D-balls.png|200px|Unit cell of CuO]]||[[Image:Copper(II)-oxide-3D-balls.png|200px|part of CuO's crystal structure]] |- |<center>the unit cell of copper(II) oxide</center>||<center>part of the [[crystal structure]] of CuO</center> |} == Health effects == Copper(II) oxide is an irritant. It also can cause damage to the [[endocrine system|endocrine]] and [[central nervous system]]. Contact to the eyes can cause irritation and damage to the corneas, and potentially can cause conjunctivitis. Contact to the skin can cause irritation and discoloration. Ingesting cupric oxide can lead to central nervous system depression, liver and kidney damage, gastro-intestinal damage, [[Heart failure|circulatory system failure]] or damage to the vascular system. Inhalation can lead to damage to the lungs and septum. Inhalation of fumes of cupric oxide can lead to a disease called [[metal fume fever|Metal fume fever]], which has symptoms similar to influenza. Prolonged exposure to cupric oxide can lead to [[dermatitis]], and can cause a toxic build-up of copper in people with [[Wilson's disease]]. Handling copper(II) oxide should be done in well ventilated area, and care should be taken to avoid contact with the skin or eyes. After handling, one should wash thoroughly.<ref>{{cite web | title = MATERIAL SAFETY DATA SHEET: Copper (II) oxide | publisher = Iowa State University | date = 2003 | url = http://avogadro.chem.iastate.edu/MSDS/CuO.html | accessdate = 2007-01-26}}</ref> == 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.<ref>{{cite web | title = Uses of Copper Compounds: Other Copper Compounds | publisher = Copper Development Association | date = 2007 | url = http://www.copper.org/applications/compounds/other_compounds.html | accessdate = 2007-01-27}}</ref> 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 battery|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 oxide can be used to produce other copper salts. It is also used when welding with [[copper alloys]].<ref>{{cite web | title = Cupric Oxide Data Sheet | publisher = Hummel Croton Inc. | date = 2006-04-21 | url = http://www.axxousa.com/data/cuox_d.html | accessdate = 2007-02-01}}</ref> 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]]<ref>{{Citation | last = Kenney | first = Charlie W. | last2 = Uchida | first2 = Laura A. | title = Use of copper (II) oxide as source of oxygen for oxidation reactions | date = April | year = 1986 | url = http://www.freepatentsonline.com/4582613.html | accessdate = 2007-06-29}}</ref>. ==Properties== * [[Work function]]:5.3[[eV]]<ref>Solar Energy Materials and Solar Cells <b>91</b>, 843 (2007)</ref> ==See also== * [[Copper]] * [[Copper(I) oxide]] * [[Patina]] ==References== <references/> ==External links== *[http://www.npi.gov.au/database/substance-info/profiles/27.html National Pollutant Inventory - Copper and compounds fact sheet] [[Category:Oxides]] [[Category:Copper compounds]] [[Category:Semiconductor materials]] [[Category:Pyrotechnic colorants]] [[ar:أكسيد نحاس ثنائي]] [[cs:Oxid měďnatý]] [[da:Kobber(II)oxid]] [[de:Kupfer(II)-oxid]] [[es:Óxido cúprico]] [[it:Ossido rameico]] [[lv:Vara (II) oksīds]] [[hu:Réz(II)-oxid]] [[ms:Kuprum(II) oksida]] [[ja:酸化銅(II)]] [[pl:Tlenek miedzi(II)]] [[pt:Óxido de cobre (II)]] [[ru:Оксид меди(II)]] [[sk:Oxid meďnatý]] [[vi:Ôxít đồng (II)]] [[zh:氧化铜]]