7.53 Knowing the electron gain enthalpy 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- species and not O- ? (Hint: Consider lattice energy factor in the formation of compounds).
7.53 Knowing the electron gain enthalpy 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- species and not O- ? (Hint: Consider lattice energy factor in the formation of compounds).
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1 Answer
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7.53
Stability of an ionic compound depends on its lattice energy. More the lattice energy of a compound, more stable it will be. Lattice energy is directly proportional to the charge carried by an ion.
When a metal combines with oxygen, the lattice energy of the oxide involving O2- ion is much more than the oxide involving O- ion. Hence, the oxide having O2-ions are more stable than oxides having O-. Hence, we can say that formation of O2- is energetically more favorable that formation of O-.
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