Cobalt(II,III) oxide

Cobalt(II,III) oxide[1]
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
RTECS number GG2500000
Properties
Co3O4

CoO.Co2O3

Molar mass 240.80 g/mol
Appearance black solid
Density 6.11 g/cm3
Melting point 895 °C (1,643 °F; 1,168 K)
Boiling point 900 °C (1,650 °F; 1,170 K) (decomposes)
Insoluble
Solubility soluble in acids and alkalis
+7380·10−6 cm3/mol
Structure
cubic
Hazards
R-phrases (outdated) R40 R41 R42 R43
S-phrases (outdated) S36/37
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
2
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

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.[2]

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.[2]

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.[3] Above 900 °C, CoO is stable.[3][4] These reaction are described by the following equilibrium:

2 Co3O4 ⇌ 6 CoO + O2

Applicatons

Cobalt(II,III) oxide is used as a blue coloring agent for pottery enamel and glass, as an alternative to cobalt(II) oxide.[5]

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.[6]

See also

References

  1. ↑ Sigma-Aldrich product page
  2. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1118. ISBN 0-08-037941-9.
  3. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1118. ISBN 0-08-037941-9.
  4. ↑ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1520.
  5. ↑ Frank Hamer, Janet Hamer (2004): The Potter's Dictionary of Materials and Techniques. University of Pennsylvania Press; 437 pages. ISBN 0812238109
  6. ↑ MSDS
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