LITHIUM OXIDE Li2O

White, hygroscopic, refractory, when heated, does not decompose. Behaves as a typical oxide, reacts vigorously with water (formed alkaline solution), acids, metals, acid oxides, absorbs CO2 from air.


Obtaining Lithium oxide Li2O:

4Li + O2 = 2Li2O (t > 200°C, impurity Li2O2)

2LiOH = Li2O + H2O (800-1000°C, in the atm. of H2).

Li2CO3 = Li2O + CO2 (730-1270°C).

Li2CO3 + C(coke) = Li2O + 2CO (800°C).

4LiNO3 = 2Li2O + 4NO2 + O2 (475-650°C).


Reactions with Lithium oxide Li2O:

Li2O + H2O = 2LiOH.

Li2O + 2HCl (deluted) = 2LiCl + H2O.

Li2O + H2S = Li2S + H2O (900-1000°C).

2Li2O + Si = 4Li + SiO2 (1000°C).

Li2O + Mg = 2Li + MgO (t >800°C).

3Li2O + 2Al = 6Li + Al2O3 (t >1000°C).

Li2O + CO2 = Li2CO3 (500-600°C).

2Li2O + SiO2 = Li4Si04 (1000°C),

Li2O + SiO2 = Li2SiO3 (1200-1300°C).
 

Did you know?

The rarest naturally-occurring element in the earth's crust may be astatine. The entire crust appears to contain about 28 g of the element.