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
CAS Number	1308-06-1 ;
3D model (JSmol)	Interactive image;
ChemSpider	9826389 ;
ECHA InfoCard	100.013.780
EC Number	215-157-2;
PubChem CID	11651651;
RTECS number	GG2500000;
UNII	USK772NS56 ;
CompTox Dashboard (EPA)	DTXSID80892420 ;
	InChI InChI=1S/3Co.4O Key: LBFUKZWYPLNNJC-UHFFFAOYSA-N ; InChI=1/3Co.4O/rCo2O3.CoO/c3-1-5-2-4;1-2 Key: LBFUKZWYPLNNJC-PMPQCLQHAA;
	SMILES [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
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
Crystal structure	cubic
Space group	Fd3m, No. 227
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H317, H334, H350, H411
Precautionary statements	P261, P273, P284, P304+P340, P342+P311
NFPA 704 (fire diamond)	2 0 0
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) 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 Co^IICo^III₂O₄ 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]

References

^ "Cobalt(II,III) oxide 203114". Sigma-Aldrich.
^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
^ "mp-18748: Co3O4 (cubic, Fd-3m, 227)". materialsproject.org. Retrieved 2019-12-20.
^ ^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.
^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1520.
^ Frank Hamer, Janet Hamer (2004): The Potter's Dictionary of Materials and Techniques. University of Pennsylvania Press; 437 pp. ISBN 0812238109
^ MSDS^{[permanent dead link]}

[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.

[G&E-4] 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.

[hamer-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]}

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