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• 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.

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• 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.

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