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| Lithium oxide | |
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| IUPAC name | Dilithium oxide |
| Other names | Lithium monoxide Lithia |
| Identifiers | |
| CAS number | [12057-24-8] |
| PubChem | |
| SMILES |
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| Properties | |
| Molecular formula | Li2O |
| Molar mass | 29.8814 g·mol-1 |
| Appearance | white solid |
| Density | 2.013 g·cm-3 |
| Melting point |
1840 K |
| log P | 9.23 |
| Structure | |
| Crystal structure | cubic crystal system, cF12[1] |
| Space group | Fm3m, #225 |
| Coordination geometry |
Li, 4, tetrahedral O, 8, cubic |
| Hazards | |
| NFPA 704 |
 0
4
2
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| Related compounds | |
| Other anions | Lithium sulfide |
| Other cations | Sodium oxide Potassium oxide Rubidium oxide |
| Related oxides | Lithium peroxide Lithium superoxide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
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Lithium oxide (Li2O) or lithia is an inorganic chemical compound. Lithium oxide is formed along with small amounts of lithium peroxide when lithium metal is burned in the air and combines with oxygen[2]:
- 4Li+O2 → 2Li2O.
Pure Li2O can be produced by the thermal decomposition of lithium peroxide, Li2O2 at 450°C[2]
- 2Li2O2 → 2Li2O + O2
Contents |
Structure
In the solid state lithium oxide adopts an antifluorite structure which is related to the CaF2, fluorite structure with Li cations substituted for fluoride anions and oxide anions substituted for calcium cations.
The ground state gas phase Li2O molecule is linear with a bond length consistent with strong ionic bonding.[3][4] VSEPR theory would predict a bent shape similar to H2O.
Uses
Lithium oxide is used as a flux in ceramic glazes; and creates blues with copper and pinks with cobalt. Lithium oxide reacts with water and steam, and should be isolated from them.
Its usage is also being investigated for non-destructive emission spectroscopy evaluation and degradation monitoring within thermal barrier coating systems. It can be added as a co-dopant with yttria in the zirconia ceramic top coat, without a large decrease in expected service life of the coating. At high heat, lithium oxide emits a very detectable spectral pattern, which increases in intensity along with degradation of the coating. Implementation would allow in situ monitoring of such systems, enabling an efficient means to predict lifetime until failure or necessary maintenance.
See also
References
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This article needs additional citations for verification. Please help improve this article by adding reliable references. Unsourced material may be challenged and removed. (May 2008) |
- ^ Gitterstruktur der oxyde, sulfide, selenide und telluride des lithiums, natriums und kaliums Zintl E., Harder A., Dauth B., Zeitschrift für Elektrochemie und Angewandte Physikalische Chemie ( 1934) 40, 588-593
- ^ a b Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements, 2nd Edition, Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
- ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
- ^ A spectroscopic determination of the bond length of the LiOLi molecule: Strong ionic bonding, D. Bellert, W. H. Breckenridge, J. Chem. Phys. 114, 2871 (2001); doi:10.1063/1.1349424
External links
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