산화 리튬

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]

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.