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Question -

Knowing the electron gainenthalpy values for O → O− and O → O2− as −141 and 702 kJ mol−1 respectively,how can you account for the formation of a large number of oxides having O2− speciesand not O−?



Answer -

Stability of an ionic compounddepends on its lattice energy. More the lattice energy of a compound, morestable it will be.

Latticeenergy is directly proportional to the charge carried by an ion. When a metalcombines with oxygen, the lattice energy of the oxide involving O2− ionis much more than the oxide involving O− ion. Hence, the oxidehaving O2− ions are more stable than oxides having O−.Hence, we can say that formation of O2− is energetically morefavourable than formation of O−

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