The formation of the oxide ion O2−(g) requires first an exothermic and then an endothermic step as shown below, O(g)+e→O−(g);ΔH=−142kJ/mol O−(g)+e→O2−(g);ΔH=844kJ/mol
These is because:
A
Oxygen has high electron affinity
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B
O− ion has comparatively larger size than oxygen atom
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C
O− ion will lead to resist the addition of another electron
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D
Oxygen is more electronegative
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Solution
The correct option is CO− ion will lead to resist the addition of another electron When an electron is further added to O− ion, there is an interelectronic repulsion observed by the extra electron to the incoming electron and hence energy has to be supplied in order to over come this repulsion thus giving rise to an endothermic reaction.