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The formation of the oxide ion $O^{2} - (g)$ requires first an exothermic and then an endothermic step shown below
$O (g) + e^{-} = O^{-} (g); Δ H_{e g} = - 142 {kJmol}^{- 1}$
$O^{-} (g) + e^{-} = O^{2} - (g); Δ H_{e f} = + 844 kJ {mol}^{- 1}$
This is because:

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O^{-}

ion will tend to resist the addition of another electron of account of same charge,

Oxygen has high electron affinity

Oxygen is more electronegative

O^{-}

ion baa comparatively larger size than oxygen atom.

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detailed solution

Correct option is A

Due to strong e e e repulsion in small sized $O^{-}$ ion, $O^{-}$ ion has a tendency to reject the addition of another electron. In order to overcome this repulsive force, energy is needed.

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The formation of the oxide ion O2-(g) requires first an exothermic and then an endothermic step shown belowO(g)+e−=O−(g); ΔHeg=−142kJmol−1O−(g)+e−=O2−(g); ΔHef=+844kJmol−1This is because: