LITHIUM PEROXIDE Li2O2

White, when heated decomposes without melting. Fully hydrolyzed by water, reacts with acids. Vigorously absorbs CO2 from the air.


Obtaining Lithium peroxide Li2O2:

2 LiOH + H2O + 2 H2O2 (hot) = Li2O2-H2O2-3H2O↓ (in ethanol),

Li2O2-H2O2-3H2O = Li2O2 + H2O2 + 3 H2O (over P4O10, vacuum).


Reactions with lithium peroxide Li2O2:

2 Li2O2 = 2Li2O + O2 (200—400° C).

Li2O2-H2O = Li2O2 + H2O (t> 0° C).

Li2O2 + 2 H2O (cold) = 2 LiOH + H2O2

2 Li2O2 + 2 H2O (hot) = 4 LiOH + O2↑.

Li2O2 + 2 HCl (dilute, cold) = 2 LiCl + H2O2,

2 Li2O2 + 2 H2SO4 (dilute,hot.) = 2Li2SO4 + 2H2O + O2↑.

2 Li2O2 + 2 CO2 = 2 Li2CO3 + O2 (t>200° C),

Li2O2 + CO = Li2CO3 (40—70° C).

 

Did you know?

Ionic radius of metal are smaller than their atomic radius (lose electrons.)