Cobalt(II,III) oxide

Cobalt(II,III) oxide[1]
Cobalt(II,III) oxide
Ball-and-stick model of the unit cell of Co3O4
Names
IUPAC name
cobalt(II) dicobalt(III) oxide
Other names
cobalt oxide, cobalt(II,III) oxide, cobaltosic oxide, tricobalt tetroxide
Identifiers
CAS Number
  • 1308-06-1 checkY
3D model (JSmol)
  • Interactive image
ChemSpider
  • 9826389 checkY
ECHA InfoCard 100.013.780 Edit this at Wikidata
EC Number
  • 215-157-2
PubChem CID
  • 11651651
RTECS number
  • GG2500000
UNII
  • USK772NS56 checkY
CompTox Dashboard (EPA)
  • DTXSID80892420 Edit this at Wikidata
InChI
  • InChI=1S/3Co.4O checkY
    Key: LBFUKZWYPLNNJC-UHFFFAOYSA-N checkY
  • InChI=1/3Co.4O/rCo2O3.CoO/c3-1-5-2-4;1-2
    Key: LBFUKZWYPLNNJC-PMPQCLQHAA
  • [Co]=O.O=[Co]O[Co]=O
Properties
Chemical formula
Co3O4

CoO.Co2O3

Molar mass 240.80 g/mol
Appearance black solid
Density 6.07 g/cm3[2]
Melting point 895 °C (1,643 °F; 1,168 K)
Boiling point 900 °C (1,650 °F; 1,170 K) (decomposes)
Solubility in water
Insoluble
Solubility soluble (with degradation) in acids and alkalis
Magnetic susceptibility (χ)
+7380·10−6 cm3/mol
Structure
cubic
Fd3m, No. 227[3]
Hazards
GHS labelling:
GHS09: Environmental hazardGHS08: Health hazard
Danger
H317, H334, H350, H411
P261, P273, P284, P304+P340, P342+P311
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Infobox references
Chemical compound

Cobalt(II,III) oxide is an inorganic compound with the formula Co3O4. It is one of two well characterized cobalt oxides. It is a black antiferromagnetic solid. As a mixed valence compound, its formula is sometimes written as CoIICoIII2O4 and sometimes as CoO•Co2O3.[4]

Structure

Co3O4 adopts the normal spinel structure, with Co2+ ions in tetrahedral interstices and Co3+ ions in the octahedral interstices of the cubic close-packed lattice of oxide anions.[4]

tetrahedral coordination geometry of Co(II) distorted octahedral coordination geometry of Co(III) distorted tetrahedral coordination geometry of O

Synthesis

Cobalt(II) oxide, CoO, converts to Co3O4 upon heating at around 600–700 °C in air.[4] Above 900 °C, CoO is stable.[4][5] These reactions are described by the following equilibrium:

2 Co3O4 ⇌ 6 CoO + O2

Applications

Cobalt(II,III) oxide is used as a blue coloring agent for pottery enamel and glass, as an alternative to cobalt(II) oxide.[6]

Cobalt(II,III) oxide is used as an electrode in some lithium-ion batteries, possibly in the form of cobalt oxide nanoparticles.

Safety

Cobalt compounds are potentially poisonous in large amounts.[7]

See also

  • Cobalt(II) oxide
  • Cobalt(III) oxide

References

  1. ^ "Cobalt(II,III) oxide 203114". Sigma-Aldrich.
  2. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  3. ^ "mp-18748: Co3O4 (cubic, Fd-3m, 227)". materialsproject.org. Retrieved 2019-12-20.
  4. ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1118. ISBN 978-0-08-037941-8.
  5. ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1520.
  6. ^ Frank Hamer, Janet Hamer (2004): The Potter's Dictionary of Materials and Techniques. University of Pennsylvania Press; 437 pp. ISBN 0812238109
  7. ^ MSDS[permanent dead link]
  • v
  • t
  • e
Cobalt(I)
  • HCo(CO)4
Cobalt(II)
  • CoBr2
  • Co(CN)2
  • CoCO3
  • CoC2O4
  • CoCl2
  • Co(ClO3)2
  • Co(ClO4)2
  • CoF2
  • Co(HCO2)2
  • CoI2
  • Co(NO3)2
  • Co3(PO4)2
  • Co(OAc)2
  • CoGeO3
  • CoO
  • Co(OH)2
  • CoS
  • Co(OCN)2
  • Co(SCN)2
  • CoSO4
  • CoSe
  • Co3P2
  • CoH2
  • Co(C3H6O3)2
  • C
    24
    H
    48
    CoO
    4
  • C
    36
    H
    70
    CoO
    4
Cobalt(0, III)Cobalt(II, III)
  • Co3O4
Cobalt(III)
  • CoAs
  • CoCl3
  • Co(NO3)3
  • Co2O3
  • CoF3
  • Co(OH)3
  • LiCoO2
Cobalt(III,IV)
  • NaxCoO2
Cobalt(IV)
  • CoF4
  • Cs2CoF6
  • CoC28H44
Cobalt(V)
  • Na3CoO4
  • v
  • t
  • e
Mixed oxidation states
+1 oxidation state
+2 oxidation state
+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)
  • Caesium sesquioxide (Cs2O3)
  • Californium(III) oxide (Cf2O3)
  • Cerium(III) oxide (Ce2O3)
  • Chromium(III) oxide (Cr2O3)
  • Cobalt(III) oxide (Co2O3)
  • 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
+5 oxidation state
+6 oxidation state
+7 oxidation state
+8 oxidation state
Related
Oxides are sorted by oxidation state. Category:Oxides
  • v
  • t
  • e
  • Ag4O4
  • Al2O3
  • AmO2
  • Am2O3
  • As2O3
  • As2O5
  • Au2O3
  • B2O3
  • BaO
  • BeO
  • Bi2O3
  • BiO2
  • Bi2O5
  • BrO2
  • Br2O3
  • Br2O5
  • Br
    3
    O
    8
  • 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...