Lithium cobalt oxide
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| Names | |
|---|---|
| IUPAC name
lithium cobalt(III) oxide
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| Other names
lithium cobaltite
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| Identifiers | |
12190-79-3  |
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| PubChem | 23670860 |
| Properties | |
| LiCoO 2 |
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| Molar mass | 97.87 g mol−1 |
| Vapor pressure | {{{value}}} |
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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 | |
Lithium cobalt oxide (LiCoO
2) is a chemical compound commonly used in the positive electrodes of lithium-ion batteries. The structure of LiCoO
2 is known theoretically and has been confirmed with techniques like x-ray diffraction, electron microscopy, neutron powder diffraction, and EXAFS:[2] it consists of layers of lithium that lie between slabs of octahedra formed by cobalt and oxygen atoms.[3] The space group is 
[4] in Hermann-Mauguin notation, signifying a rhombus-like unit cell with threefold improper rotational symmetry and a mirror plane. More simply, however, both lithium and cobalt are octahedrally coordinated by oxygen. These octahedrons are edge-sharing, and tilted relative to the layered structure. The threefold rotational axis (which is normal to the layers) is termed improper because the triangles of oxygen (being on opposite sides of each octahedron) are anti-aligned.
Batteries produced with LiCoO
2 cathodes, while providing higher capacity, are more reactive and have poorer thermal stability than chemistries such as the newer lithium-nickel-cobalt-aluminum-oxide types. This makes LiCoO
2 batteries susceptible to thermal runaway in cases of abuse such as high temperature operation (>130 °C) or overcharging. At elevated temperatures, LiCoO
2 decomposition generates oxygen, which then reacts with the organic electrolyte of the cell. This is a safety concern due to the magnitude of this highly exothermic reaction, which can spread to adjacent cells or ignite nearby combustible material.[5]
The compound's usefulness as an intercalation electrode was discovered in 1980[6] by John B. Goodenough's research group at Oxford.
References
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