Lithium oxide CAS 12057-24-8

Introduction：Basic information about Lithium oxide CAS 12057-24-8, including its chemical name, molecular formula, synonyms, physicochemical properties, and safety information, etc.

Lithium oxide Basic information

• Product Name: Lithium oxide
• Synonyms: dilithiumoxide;Li2O;Lithium oxide (Li2O);lithiummonoxide;Lithiumoxid;lithiumoxide(li2o);Lithium Oxide,98.5%;oxydedelithium
• CAS: 12057-24-8
• MF: Li2O
• MW: 29.88
• EINECS: 235-019-5
• Product Categories: metal oxide;Lithium;Metal and Ceramic Science;Oxides;Inorganics;KT00001
• Mol File: 12057-24-8.mol

Lithium oxide Chemical Properties

Melting point	1427°C
density	2.013 g/mL at 25 °C (lit.)
form	Powder
color	White
Specific Gravity	2.013
Water Solubility	Soluble in water.
Sensitive	Air & Moisture Sensitive
Crystal Structure	Reverse CaF2 type
crystal system	Cube
Merck	14,5538
Space group	Fm3m
Lattice constant	a/nm b/nm c/nm α/o β/o γ/o V/nm3 0.463 0.463 0.463 90 90 90 0.0993
Major Application	battery manufacturing
InChI	1S/2Li.O/q2*+1;-2
InChIKey	FUJCRWPEOMXPAD-UHFFFAOYSA-N
SMILES	[Li+].[Li+].[O--]
CAS DataBase Reference	12057-24-8(CAS DataBase Reference)
NIST Chemistry Reference	Dilithium monoxide(12057-24-8)
EPA Substance Registry System	Dilithium oxide (12057-24-8)

Safety Information

• Hazard Codes: C
• Risk Statements: 34
• Safety Statements: 26-36/37/39-45
• RIDADR: UN 3262 8/PG 2
• WGK Germany: 3
• RTECS: OJ6360000
• TSCA: TSCA listed
• HazardClass: 8
• PackingGroup: II
• Storage Class: 8A - Combustible corrosive hazardous materials
• Hazard Classifications: Skin Corr. 1B

Lithium oxide Usage And Synthesis

Chemical Properties

Lithium oxide (Li2O) is one of simplest ionic oxides and it is isoelectronic to H2O. Two lithium atoms will each give one electron to the oxygen atom. forms the ionic bond between lithium and oxygen. The formula for lithium oxide is Li2O.
Lithium oxide is very corrosive. It reacts with water to make lithium hydroxide. It is toxic because of its strong alkalinity (being a base).
It is a highly insoluble thermally stable Lithium source suitable for glass, optic and ceramic applications. Lithium oxide is a white solid also known as lithia, it is produced when lithium metal burns in the presence of oxygen. Oxide compounds are not conductive to electricity. However, certain perovskite structured oxides are electronically conductive finding application in the cathode of solid oxide fuel cells and oxygen generation systems. They are compounds containing at least one oxygen anion and one metallic cation.

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, forming lithium hydroxide 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.

Uses

There are no current industrial uses which consume large quantities of lithium oxide.
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, forming lithium hydroxide 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.

Reactions

Lithium oxide reacts with water as it dissolves to form a solution of lithium hydroxide.
Lithium oxide is a strong base and reacts typically with acidic gases and liquids to form lithium salts. At elevated temperatures, lithium oxide also reacts with many solid nonmetal oxides (SiO2, B2O3, etc.) and metal oxides (A12O3, Fe2O3, etc.). High-temperature reactions are the basis for the fluxing action of lithium oxide, lithium hydroxide and lithium carbonate. Care must be taken to avoid the reaction of lithium oxide with reaction vessels at high temperatures.

Preparation

Lithium oxide is prepared by heating lithium metal in dry oxygen above 100°C:
4Li + O2→2Li2O
Another method of preparation that yields pure lithium oxide involves thermal decomposition of lithium peroxide:
2Li2O2→2Li2O + O2
Also, the oxide can be produced by heating the pure lithium hydroxide at 800°C in a vacuum:
2LiOH→Li2O + H2O

Health Hazard

To the best of our knowledge the chemical, physical and toxicological properties of lithium oxide have not been thoroughly investigated and reported.
The toxicity of lithium compounds is a function of their solubility in water.  Lithium ion has central nervous system toxicity.  The initial effects of lithium exposure are tremors of the hands, nausea, micturition, slurred speech, sluggishness, sleepiness, vertigo, thirst, and increased urine volume.  Effects from continued exposure are apathy, anorexia, fatigue, lethargy, muscular weakness, and changes in ecg.  Long-term exposure leads to hypothyroidism, leukocytosis, edema, weight gain, polydipsia/polyuria (increased water intake leading to increased urinary output), memory impairment, seizures, kidney damage, shock, hypotension, cardiac arrhythmias, coma, death.

Chemical Properties

finely divided white powder(s) or crusty material; readily absorbs CO2 and H2O from the atmospheric; made by heating LiOH to ~800°C in a vacuum or by thermal decomposition of lithium peroxide; used in ceramics and special glass formulations and in lithium thermal batteries [HAW93] [MER06] [KIR81] [FMC93]

Uses

Lithium oxide is a strong alkali that absorbs carbon dioxide and waterfrom the atmosphere. It is used in manufacturing ceramics and special types of glass.

Uses

Ceramics and special glass formulations, carbon dioxide absorbent.Lithium oxide is used as a flux in ceramic glazes, co-dopant with yttria in the zirconia ceramic top coat and as the cathode in the lithium ion batteries, which is used in power electronic devices like mobile phones, laptop computers and battery-powered cars. It is also used to prepare lithium hydroxide and lithium metal by electrolysis.

Preparation

Industrial and laboratory preparations. Only small volumes of material are preparedindustrially. Both industrial and laboratory preparations require the thermal decompositionof lithium peroxide or of lithium hydroxide.
Lithium peroxide, Li202 , is converted to lithium oxide, Li20, and oxygen by heatingto 450° in a stream of helium gas.
Thermal dehydration of lithium hydroxide is carried out at 675°C±10° under vacuumin a nickel container lined with silver foil.
Lithium carbonate may be converted to lithium oxide and carbon dioxide by heatingthe material to 700°C under vacuum in a platinum boat.
Industrial uses. There are no current industrial uses which consume large quantities oflithium oxide.
Lithium oxide reacts with water as it dissolves to form a solution of lithium hydroxide.Lithium oxide is a strong base and reacts typically with acidic gases and liquids to formlithium salts. At elevated temperatures, lithium oxide also reacts with many solid nonmetaloxides (Si02, B2O3, etc.) and metal oxides (A1203 , Fe2C>3, etc.). High-temperaturereactions are the basis for the fluxing action of lithium oxide, lithium hydroxide andlithium carbonate. Care must be taken to avoid the reaction of lithium oxide with reactionvessels at high temperatures.

General Description

Lithium oxide is a white crystalline solid. Its a strong base. It reacts with water and forms lithium hydroxide.

Structure and conformation

Solid lithium oxide adopts an antifluorite structure with four-coordinated Li+ centers and eight-coordinated oxides.The ground state gas phase Li2O molecule is linear with a bond length consistent with strong ionic bonding.VSEPR theory would predict a bent shape similar to H2O.

Lithium oxide Preparation Products And Raw materials

• Preparation Products: Lithium carbonate-->Lithium hydroxide monohydrate