Cobalt(II,III) oxide

Chemical compound From Wikipedia, the free encyclopedia

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] It occurs naturally as the rare mineral guite which is named in honor of Prof. Xiangping Gu (1964-). [5]

Quick facts Names, Identifiers ...
Cobalt(II,III) oxide[1]
Cobalt(II,III) oxide
Cobalt(II,III) oxide
Ball-and-stick model of the unit cell of Co3O4
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
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.780 Edit this at Wikidata
EC Number
  • 215-157-2
RTECS number
  • GG2500000
UNII
  • 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
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)
Insoluble
Solubility soluble (with degradation) in acids and alkalis
+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 ?)
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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][6] 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.[7]

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

See also

References

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