The formation of the oxide ion `O_((g))^(2-)` requires first an exothermic and then an endothermic step as shown below.
`O_((g)) +e^(-) = O_((g))^(-) DeltaH^(@) =- 142 kJ mol^(-1)`
`O_((g))^(-) + e^(-) = O_((g))^(2-) DeltaH^(@) = 844 kJ mol^(-1)` This is because of :

Options

A. `O^(-)` ion will tend to resist tha addition of another electron
B. Oxygen has high electron affinity
C. Oxygen is more electronegative
D. `O^(-)` ion has comparatively larger size than oxygen atom

Answer

A

Explanation

[`(DeltaH_(eg))_(2)` is an endothermic process]