Copper(II) Oxide - Wikipedia

Chemical compound – an oxide of copper with formula CuO Copper(II) oxide

Names
IUPAC name Copper(II) oxide
Other names Cupric oxide
Identifiers
CAS Number	1317-38-0 Y
3D model (JSmol)	Interactive image Interactive image
ChEBI	CHEBI:75955 N
ChEMBL	ChEMBL1909057 N
ChemSpider	144499 Y
ECHA InfoCard	100.013.882
EC Number	215-269-1
PubChem CID	14829
RTECS number	GL7900000
UNII	V1XJQ704R4 Y
CompTox Dashboard (EPA)	DTXSID5034488
InChI InChI=1S/Cu.O/q+2;-2 YKey: KKCXRELNMOYFLS-UHFFFAOYSA-N Y InChI=1/Cu.O/rCuO/c1-2Key: QPLDLSVMHZLSFG-PHEGLCPBAN InChI=1/Cu.O/q+2;-2Key: KKCXRELNMOYFLS-UHFFFAOYAT
SMILES [Cu]=O [Cu+2].[O-2]
Properties
Chemical formula	CuO
Molar mass	79.545 g/mol
Appearance	black to brown powder
Density	6.315 g/cm3
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 carbonate
Band gap	1.2 eV
Magnetic susceptibility (χ)	+238.9·10−6 cm3/mol
Refractive index (nD)	2.63
Structure
Crystal structure	monoclinic, mS8[1]
Space group	C2/c, #15
Lattice constant	a = 4.6837, b = 3.4226, c = 5.1288α = 90°, β = 99.54°, γ = 90°
Thermochemistry
Std molarentropy (S⦵298)	43 J·mol−1·K−1
Std enthalpy offormation (ΔfH⦵298)	−156 kJ·mol−1
Hazards
GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H302, H410, H412
Precautionary statements	P264, P270, P273, P301+P317, P330, P391, P501
NFPA 704 (fire diamond)	2 0 1
Flash point	Non-flammable
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m3 (as Cu)[2]
REL (Recommended)	TWA 1 mg/m3 (as Cu)[2]
IDLH (Immediate danger)	TWA 100 mg/m3 (as Cu)[2]
Safety data sheet (SDS)	Fisher Scientific
Related compounds
Other anions	Copper(II) sulfide
Other cations	Nickel(II) oxideZinc oxide
Related compounds	Copper(I) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Chemical compound

Copper(II) oxide or cupric oxide is an inorganic compound with the formula CuO. A black solid, it is one of the two stable oxides of copper, the other being Cu2O or copper(I) oxide (cuprous oxide). As a mineral, it is known as tenorite, or sometimes black copper. It is a product of copper mining and the precursor to many other copper-containing products and chemical compounds.[3]

Production

[edit]

It is produced on a large scale by pyrometallurgy, as one stage in extracting copper from its ores. The ores are treated with an aqueous mixture of ammonium carbonate, ammonia, and oxygen to ultimately give copper(II) ammine complex carbonates, such as [Cu(NH3)4]CO3. After extraction from the residues and after separation from iron, lead, etc. impurities, the carbonate salt is decomposed with steam to give CuO.[3]

It can be formed by heating copper in air at around 300–800 °C:

2 Cu + O2 → 2 CuO

For laboratory uses, copper(II) oxide is conveniently prepared by pyrolysis of copper(II) nitrate or basic copper(II) carbonate:[4]

2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2 (180°C) Cu2(OH)2CO3 → 2 CuO + CO2 + H2O

Dehydration of cupric hydroxide has also been demonstrated:

Cu(OH)2 → CuO + H2O

Reactions

[edit]

Copper(II) oxide reacts with mineral acids such as hydrochloric acid, sulfuric acid, and nitric acid to give the corresponding hydrated copper(II) salts:[4]

CuO + 2 HNO3 → Cu(NO3)2 + H2O CuO + 2 HCl → CuCl2 + H2O CuO + H2SO4 → CuSO4 + H2O

In presence of water it reacts with concentrated alkali to form the corresponding cuprate salts:

2 NaOH + CuO + H2O → Na2[Cu(OH)4]

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

CuO + H2 → Cu + H2O CuO + CO → Cu + CO2 2 CuO + C → 2Cu + CO2

When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary.

Structure and physical properties

[edit]

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 5.3 eV.[5]

Uses

[edit]

As a significant product of copper mining, copper(II) oxide is the starting point for the production of many 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.[3]

It is incorrectly used as a dietary supplement in animal feed.[6] Due to low bioactivity, negligible copper is absorbed.[7]

It is used when welding with copper alloys.[8]

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").

Pyrotechnics and fireworks

[edit]

Used as moderate blue coloring agent in blue flame compositions with additional chlorine donors and oxidizers such as chlorates and perchlorates. Providing oxygen it can be used as flash powder oxidizer with metal fuels such as magnesium, aluminium, or magnalium powder. Sometimes it is used in strobe effects and thermite compositions as crackling stars effect.

Similar compounds

[edit]

An example of natural copper(I,II) oxide is the mineral paramelaconite, Cu+2Cu2+2O3.[9][10]

See also

[edit]

• Patina
• Tenorite

References

[edit]

1. ^ a b 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. Crystallographic point group: 2/m or C2h. Space group: C2/c. Lattice parameters: a = 4.6837(5), b = 3.4226(5), c = 5.1288(6), α = 90°, β = 99.54(1)°, γ = 90°.
2. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
3. ^ a b c d Richardson, H. Wayne (2002). "Copper Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a07_567. ISBN 978-3-527-30673-2.
4. ^ a b O. Glemser and H. Sauer (1963). "Copper, Silver, Gold". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1. NY, NY: Academic Press.
5. ^ 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. Bibcode:1982JAP....53.1173K. doi:10.1063/1.330567.
6. ^ "Uses of Copper Compounds: Other Copper Compounds". Copper Development Association. 2007. Archived from the original on 2013-08-15. Retrieved 2007-01-27.
7. ^ Baker, David H. (1999). "Cupric Oxide Should Not be Used as a Copper Supplement for Either Animals or Humans". The Journal of Nutrition. 129 (12): 2278–2279. doi:10.1093/jn/129.12.2278. PMID 10573563.
8. ^ "Cupric Oxide Data Sheet". Hummel Croton Inc. 2006-04-21. Archived from the original on 2011-07-07. Retrieved 2007-02-01.
9. ^ "Paramelaconite".
10. ^ "List of Minerals". 21 March 2011.

External links

[edit] Wikimedia Commons has media related to Copper(II) oxide.

• National Pollutant Inventory - Copper and compounds fact sheet
• Copper oxides project page Archived 2011-07-25 at the Wayback Machine
• CDC - NIOSH Pocket Guide to Chemical Hazards

v t e Copper compounds
Cu(0,I)	Cu5Si
Cu(I)	CuBr CuCN CuCl CuF CuH CuI Cu2C2 Cu2Cr2O5 Cu2O CuOH CuNO3 Cu3P Cu2S CuS CuSCN C6H5Cu
Cu(I,II)	Cu4O3 Cu3H4O8S2
Cu(II)	Cu(BF4)2 CuBr2 CuC2 Cu(CH3COO)2 Cu(CF3COO)2 Cu(C3H5O3)2 CuCO3 Cu2CO3(OH)2 Cu(CN)2 CuCl2 / KCuCl3 / K2CuCl4 Cu(ClO3)2 Cu(ClO4)2 CuF2 Cu(NO3)2 Cu3(PO4)2 Cu3(BO3)2 Cu(N3)2 CuC2O4 CuO CuO2 Cu(OH)2 Cu(SCN)2 CuSO4 Cu3(AsO4)2 Cu(C11H23COO)2 Cu(C17H35COO)2 Cu(O2CC6H5)2 CuTe CuTe2 [Cu(NH3)4(H2O)]SO4
Cu(III)	K3CuF6 CuO−2
Cu(IV)	CuO2 Cs2CuF6

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb2O4) Boron suboxide (B12O2) Carbon suboxide (C3O2) Chlorine perchlorate (Cl2O4) Chloryl perchlorate (Cl2O6) Cobalt(II,III) oxide (Co3O4) Dichlorine pentoxide (Cl2O5) Iron(II,III) oxide (Fe3O4) Lead(II,IV) oxide (Pb3O4) Manganese(II,III) oxide (Mn3O4) Mellitic anhydride (C12O9) Praseodymium(III,IV) oxide (Pr6O11) Silver(I,III) oxide (Ag2O2) Terbium(III,IV) oxide (Tb4O7) Tribromine octoxide (Br3O8) Triuranium octoxide (U3O8)
+1 oxidation state	Aluminium(I) oxide (Al2O) Copper(I) oxide (Cu2O) Caesium monoxide (Cs2O) Dibromine monoxide (Br2O) Dicarbon monoxide (C2O) Dichlorine monoxide (Cl2O) Gallium(I) oxide (Ga2O) Iodine(I) oxide (I2O) Lithium oxide (Li2O) Mercury(I) oxide (Hg2O) Nitrous oxide (N2O) Potassium oxide (K2O) Rubidium oxide (Rb2O) Silver oxide (Ag2O) Thallium(I) oxide (Tl2O) Sodium oxide (Na2O) Water (hydrogen oxide) (H2O)
+2 oxidation state	Aluminium(II) oxide (AlO) Barium oxide (BaO) Berkelium monoxide (BkO) Beryllium oxide (BeO) Boron monoxide (BO) Bromine monoxide (BrO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chlorine monoxide (ClO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N2O2) Disulfur dioxide (S2O2) Europium(II) oxide (EuO) Germanium monoxide (GeO) Iron(II) oxide (FeO) Iodine monoxide (IO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Niobium monoxide (NbO) Palladium(II) oxide (PdO) Phosphorus monoxide (PO) Polonium monoxide (PoO) Protactinium monoxide (PaO) Radium oxide (RaO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Yttrium(II) oxide (YO) Zirconium monoxide (ZrO) Zinc oxide (ZnO)
+3 oxidation state	Actinium(III) oxide (Ac2O3) Aluminium oxide (Al2O3) Americium(III) oxide (Am2O3) Antimony trioxide (Sb2O3) Arsenic trioxide (As2O3) Berkelium(III) oxide (Bk2O3) Bismuth(III) oxide (Bi2O3) Boron trioxide (B2O3) Californium(III) oxide (Cf2O3) Cerium(III) oxide (Ce2O3) Chromium(III) oxide (Cr2O3) Cobalt(III) oxide (Co2O3) Curium(III) oxide (Cm2O3) Dinitrogen trioxide (N2O3) Dysprosium(III) oxide (Dy2O3) Einsteinium(III) oxide (Es2O3) Erbium(III) oxide (Er2O3) Europium(III) oxide (Eu2O3) Gadolinium(III) oxide (Gd2O3) Gallium(III) oxide (Ga2O3) Gold(III) oxide (Au2O3) Holmium(III) oxide (Ho2O3) Indium(III) oxide (In2O3) Iron(III) oxide (Fe2O3) Lanthanum oxide (La2O3) Lutetium(III) oxide (Lu2O3) Manganese(III) oxide (Mn2O3) Neodymium(III) oxide (Nd2O3) Nickel(III) oxide (Ni2O3) Phosphorus trioxide (P4O6) Praseodymium(III) oxide (Pr2O3) Promethium(III) oxide (Pm2O3) Rhodium(III) oxide (Rh2O3) Samarium(III) oxide (Sm2O3) Scandium oxide (Sc2O3) Terbium(III) oxide (Tb2O3) Thallium(III) oxide (Tl2O3) Thulium(III) oxide (Tm2O3) Titanium(III) oxide (Ti2O3) Tungsten(III) oxide (W2O3) Vanadium(III) oxide (V2O3) Ytterbium(III) oxide (Yb2O3) Yttrium(III) oxide (Y2O3)
+4 oxidation state	Americium dioxide (AmO2) Berkelium(IV) oxide (BkO2) Bromine dioxide (BrO2) Californium dioxide (CfO2) Carbon dioxide (CO2) Carbon trioxide (CO3) Cerium(IV) oxide (CeO2) Chlorine dioxide (ClO2) Chromium(IV) oxide (CrO2) Curium(IV) oxide (CmO2) Dinitrogen tetroxide (N2O4) Germanium dioxide (GeO2) Iodine dioxide (IO2) Iridium dioxide (IrO2) Hafnium(IV) oxide (HfO2) Lead dioxide (PbO2) Manganese dioxide (MnO2) Molybdenum dioxide (MoO2) Neptunium(IV) oxide (NpO2) Nitrogen dioxide (NO2) Niobium dioxide (NbO2) Osmium dioxide (OsO2) Platinum dioxide (PtO2) Plutonium(IV) oxide (PuO2) Polonium dioxide (PoO2) Praseodymium(IV) oxide (PrO2) Protactinium(IV) oxide (PaO2) Rhenium(IV) oxide (ReO2) Rhodium(IV) oxide (RhO2) Ruthenium(IV) oxide (RuO2) Selenium dioxide (SeO2) Silicon dioxide (SiO2) Sulfur dioxide (SO2) Technetium(IV) oxide (TcO2) Tellurium dioxide (TeO2) Terbium(IV) oxide (TbO2) Thorium dioxide (ThO2) Tin dioxide (SnO2) Titanium dioxide (TiO2) Tungsten(IV) oxide (WO2) Uranium dioxide (UO2) Vanadium(IV) oxide (VO2) Xenon dioxide (XeO2) Zirconium dioxide (ZrO2)
+5 oxidation state	Antimony pentoxide (Sb2O5) Arsenic pentoxide (As2O5) Bismuth pentoxide (Bi2O5) Dinitrogen pentoxide (N2O5) Diuranium pentoxide (U2O5) Neptunium(V) oxide (Np2O5) Niobium pentoxide (Nb2O5) Phosphorus pentoxide (P2O5) Protactinium(V) oxide (Pa2O5) Tantalum pentoxide (Ta2O5) Tungsten pentoxide (W2O5) Vanadium(V) oxide (V2O5)
+6 oxidation state	Chromium trioxide (CrO3) Molybdenum trioxide (MoO3) Neptunium trioxide (NpO3) Polonium trioxide (PoO3) Rhenium trioxide (ReO3) Selenium trioxide (SeO3) Sulfur trioxide (SO3) Tellurium trioxide (TeO3) Tungsten trioxide (WO3) Uranium trioxide (UO3) Xenon trioxide (XeO3)
+7 oxidation state	Dichlorine heptoxide (Cl2O7) Manganese heptoxide (Mn2O7) Rhenium(VII) oxide (Re2O7) Technetium(VII) oxide (Tc2O7)
+8 oxidation state	Iridium tetroxide (IrO4) Osmium tetroxide (OsO4) Ruthenium tetroxide (RuO4) Xenon tetroxide (XeO4) Hassium tetroxide (HsO4)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxypnictide
Oxides are sorted by oxidation state. Category:Oxides

v t e Oxygen compounds

Ag4O4 Al2O3 AmO2 Am2O3 As2O3 As2O5 Au2O3 B2O3 BaO BeO Bi2O3 BiO2 Bi2O5 BrO2 Br2O3 Br2O5 Br3O8 CO CO2 C3O2 CaO CaO2 CdO CeO2 Ce3O4 Ce2O3 ClO2 Cl2O Cl2O2 Cl2O3 Cl2O4 Cl2O6 Cl2O7 CoO Co2O3 Co3O4 CrO3 Cr2O3 Cr2O5 Cr5O12 CsO2 Cs2O3 CuO Dy2O3 Er2O3 Eu2O3 FeO Fe2O3 Fe3O4 Ga2O Ga2O3 GeO GeO2 H2O 2H2O 3H2O H218O H2O2 HfO2 HgO Hg2O Ho2O3 IO I2O4 I2O5 I2O6 I4O9 In2O3 IrO2 KO2 K2O2 La2O3 Li2O Li2O2 Lu2O3 MgO Mg2O3 MnO MnO2 Mn2O3 Mn2O7 MoO2 MoO3 Mo2O3 NO NO2 N2O N2O3 N2O4 N2O5 NaO2 Na2O Na2O2 NbO NbO2 Nd2O3 O2F OF OF2 O2F2 O3F2 O4F2 O5F2 O6F2 O2PtF6 more...