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Chemistry
The p-Block Elements
knowing the electron gain enthalpy values for o r...

Question:
Knowing the electron gain enthalpy values for O → O^-and O → O^2-as -141 and 702 kJ mol^-1respectively, how can you account for the formation of a large number of oxides having O^2-species and not O^-? (Hint: Consider lattice energy factor in the formation of compounds).

Answer:

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 O^2-ion is much more than the oxide involving O^-ion. Hence, the oxide having O^2-ions are more stable than oxides having O^-. Hence, we can say that formation of O^2-is energetically more favourable than formation of O^-.

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Question:
Knowing the electron gain enthalpy values for O → O^-and O → O^2-as -141 and 702 kJ mol^-1respectively, how can you account for the formation of a large number of oxides having O^2-species and not O^-? (Hint: Consider lattice energy factor in the formation of compounds).

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Question: 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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Question:
Knowing the electron gain enthalpy values for O → O^-and O → O^2-as -141 and 702 kJ mol^-1respectively, how can you account for the formation of a large number of oxides having O^2-species and not O^-? (Hint: Consider lattice energy factor in the formation of compounds).