Lithium oxide CAS:12057-24-8

  • Product Name:Lithium oxide
  • CAS:12057-24-8
  • Molecular formula:Li2O
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Lithium oxide CAS:12057-24-8

Lithium oxide CAS:12057-24-8 Basic information

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

Lithium oxide CAS:12057-24-8 Chemical Properties

density: 2.013 g/mL at 25 °C(lit.)
Melting point: 1427°C
form: Powder
Water Solubility: Soluble in water.
NIST Chemistry Reference: Dilithium monoxide(12057-24-8)
Merck: 14,5538
Sensitive: Air & Moisture Sensitive
Specific Gravity: 2.013
CAS DataBase Reference: 12057-24-8(CAS DataBase Reference)
EPA Substance Registry System: Dilithium oxide (12057-24-8)
检验项目      Chemical CompositionLi2OLi2CO3NaFeCaZnMgCuNiSiCr
标 准 值  (%)    Standard≥98.5≤2.5≤0.01≤0.002≤0.01≤0.002≤0.005≤0.002≤0.002≤0.004≤0.001
检验值  (%)                      Analysis99.060.920.00130.00090.0030.00050.00010.00010.00010.0010.0001












Lithium oxide Usage And Synthesis
Chemical PropertiesLithium 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
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.
UsesThere 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.

PreparationLithium 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 Propertiesfinely 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]
UsesLithium 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.
UsesCeramics and special glass formulations, carbon dioxide absorbent
PreparationIndustrial 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.


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