cobalt(II) dicobalt(III) oxide
cobalt oxide, cobalt(II,III) oxide, cobaltosic oxide, tricobalt tetroxide
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||240.80 g/mol|
|Melting point||895 °C (1,643 °F; 1,168 K)|
|Boiling point||900 °C (1,650 °F; 1,170 K) (decomposes)|
|Solubility||soluble (with degradation) in acids and alkalis|
|Fd3m, No. 227|
|H317, H334, H350, H411|
|P261, P273, P284, P304+P340, P342+P311|
|NFPA 704 (fire diamond)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
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.
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.
|tetrahedral coordination geometry of Co(II)||distorted octahedral coordination geometry of Co(III)||distorted tetrahedral coordination geometry of O|
Cobalt(II) oxide, CoO, converts to Co3O4 upon heating at around 600–700 °C in air. Above 900 °C, CoO is stable. These reaction are described by the following equilibrium:
Cobalt(II,III) oxide is used as a blue coloring agent for pottery enamel and glass, as an alternative to cobalt(II) oxide.
Cobalt(II,III) oxide is used as an electrode in some lithium-ion batteries, possibly in the form of cobalt oxide nanoparticles.
Cobalt compounds are potentially poisonous in large amounts.