Lithium oxide

Crystal structure
__ Li +      __ O 2−
General
Surname	Lithium oxide
other names	Dilithium oxide, lithia
Ratio formula	Li 2 O
Brief description	white, odorless solid
External identifiers / databases
CAS number 12057-24-8 EC number 235-019-5 ECHA InfoCard 100,031,823 PubChem 166630 ChemSpider 145811 Wikidata Q385662
properties
Molar mass	29.88 g mol −1
Physical state	firmly
density	2.01 g cm −3
Melting point	1427 ° C
solubility	reacts with water
safety instructions
GHS labeling of hazardous substances danger H and P phrases H: 314 P: 280-305 + 351 + 338-310
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Lithium oxide is a chemical compound made up of lithium and oxygen . It is used for the production of lithium niobate and as an additive in ceramics and glasses.

Extraction and presentation

Lithium oxide can be produced by burning lithium or by thermal decomposition of lithium peroxide or lithium hydroxide .

${\displaystyle \mathrm {4\ Li+O_{2}\longrightarrow \ 2\ Li_{2}O} }$

${\displaystyle \mathrm {2\ Li_{2}O_{2}{\xrightarrow {195^{\circ }C}}\ 2\ Li_{2}O\ +O_{2}} }$

${\displaystyle \mathrm {2\ LiOH\longrightarrow Li_{2}O+H_{2}O} }$

properties

Lithium oxide is a white, odorless solid. It has an anti-fluorspar type crystal structure (a = 4.611 Å). The standard enthalpy of formation of lithium oxide is ΔH _f ⁰  = −599.1 kJ / mol.

use

Lithium oxide is used as a starting material for the production of lithium niobate . It can also be used as an additive in the manufacture of ceramics and glasses. It can also be used in fusion reactors .

Individual evidence

1. ↑ https://www.chemicalbook.com/ChemicalProductProperty_DE_CB7164125.htm
2. ↑ ^{a b c} data sheet lithium oxide from AlfaAesar, accessed on December 15, 2010 ( PDF )(JavaScript required) .
3. ↑ ^{a b c} data sheet lithium oxide from Sigma-Aldrich , accessed on April 8, 2011 ( PDF ).
4. ^ George K. Schweitzer, Lester L. Pesterfield: The Aqueous Chemistry of the Elements . Oxford University Press, 2010, ISBN 978-0-19-974219-6 , pp. 100 ( limited preview in Google Book search).
5. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 1152.
6. ↑ ^{a b} Georg Brauer (Ed.), With the collaboration of Marianne Baudler u a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 951.
7. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 1176.
8. ↑ Doctoral thesis Ulrich Grusemann .
9. ↑ Lecture notes (PDF; 35 kB).
10. ↑ Risely Technical Service Report: The use of lithium oxide as the breeder in fusion reactors . July 1989, p. 30.