Lithium oxide: Difference between revisions
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==Overview== | ==Overview== | ||
'''Lithium oxide''' ([ | '''Lithium oxide''' ([[Lithium|Li<sub>2</sub>]][[Oxygen|O]]) 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<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref>: | ||
:4Li+O<sub>2</sub> → 2Li<sub>2</sub>O. | :4Li+O<sub>2</sub> → 2Li<sub>2</sub>O. | ||
Pure Li<sub>2</sub>O can be produced by the [ | Pure Li<sub>2</sub>O can be produced by the [[thermal decomposition]] of [[lithium peroxide]], Li<sub>2</sub>O<sub>2</sub> at 450°C | ||
:2Li<sub>2</sub>O<sub>2</sub> → 2Li<sub>2</sub>O + O<sub>2</sub> | :2Li<sub>2</sub>O<sub>2</sub> → 2Li<sub>2</sub>O + O<sub>2</sub> | ||
==Structure== | ==Structure== | ||
In the solid state lithium oxide adopts an antifluorite structure which is related to the [ | In the solid state lithium oxide adopts an antifluorite structure which is related to the [[calcium fluoride|CaF<sub>2</sub>]], fluorite structure with Li cations substituted for fluoride anions and oxide anions substituted for calcium cations.<br /> | ||
The ground state gas phase Li<sub>2</sub>O molecule is linear with a bond length consistent with strong ionic bonding.<ref name = "Wells">Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications ISBN 0-19-855370-6 </ref><ref> 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}}</ref> [ | The ground state gas phase Li<sub>2</sub>O molecule is linear with a bond length consistent with strong ionic bonding.<ref name = "Wells">Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications ISBN 0-19-855370-6 </ref><ref> 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}}</ref> [[VSEPR theory]] would predict a bent shape similar to H<sub>2</sub>O. | ||
==Uses== | ==Uses== | ||
Lithium oxide is used as a [ | 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 [ | 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== | ==See also== | ||
* [ | * [[Lithium]] | ||
* [[Lithium peroxide]] | |||
==References== | ==References== | ||
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==External links== | ==External links== | ||
* [http:// | * [http://www.ceramic-materials.com/cermat/oxide/li2o.html CeramicMaterials.Info entry] | ||
[ | [[Category:Oxides]] | ||
[ | [[Category:Lithium compounds]] | ||
[[Category:Inorganic compound stubs]] | |||
[ | [[ar:أكسيد ليثيوم]] | ||
[ | [[bs:Litijum oksid]] | ||
[ | [[cs:Oxid lithný]] | ||
[ | [[de:Lithiumoxid]] | ||
[[pt:Óxido de lítio]] | |||
{{WH}} | {{WH}} | ||
{{WS}} | {{WS}} | ||
Revision as of 16:56, 21 January 2011
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Overview
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[1]:
- 4Li+O2 → 2Li2O.
Pure Li2O can be produced by the thermal decomposition of lithium peroxide, Li2O2 at 450°C
- 2Li2O2 → 2Li2O + O2
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.[2][3] 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
This article needs additional citations for verification. (May 2008) (Learn how and when to remove this template message) |
- ↑ Template:Greenwood&Earnshaw
- ↑ 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
ar:أكسيد ليثيوم bs:Litijum oksid cs:Oxid lithný de:Lithiumoxid Template:WH Template:WS