Lithium oxide Property

Melting point:

1427°C

Density 

2.013 g/mL at 25 °C (lit.)

form 

Powder

Specific Gravity

2.013

color 

White

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

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

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 

Yes

HazardClass 

8

PackingGroup 

II

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Danger

Hazard statements

H314Causes severe skin burns and eye damage

Precautionary statements

P260Do not breathe dust/fume/gas/mist/vapours/spray.

P280Wear protective gloves/protective clothing/eye protection/face protection.

P301+P330+P331IF SWALLOWED: Rinse mouth. Do NOT induce vomiting.

P303+P361+P353IF ON SKIN (or hair): Remove/Take off Immediately all contaminated clothing. Rinse SKIN with water/shower.

P305+P351+P338IF IN EYES: Rinse cautiously with water for several minutes. Remove contact lenses, if present and easy to do. Continuerinsing.

Lithium oxide Chemical Properties,Usage,Production

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 water from 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 prepared industrially. Both industrial and laboratory preparations require the thermal decomposition of lithium peroxide or of lithium hydroxide.
Lithium peroxide, Li202 , is converted to lithium oxide, Li20, and oxygen by heating to 450° in a stream of helium gas.
Thermal dehydration of lithium hydroxide is carried out at 675°C±10° under vacuum in a nickel container lined with silver foil.
Lithium carbonate may be converted to lithium oxide and carbon dioxide by heating the material to 700°C under vacuum in a platinum boat.
Industrial uses. There are no current industrial uses which consume large quantities of lithium 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 form lithium salts. At elevated temperatures, lithium oxide also reacts with many solid nonmetal oxides (Si02, B2O3, etc.) and metal oxides (A1203 , Fe2C>3, 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.

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.