The formation of oxide ion `O^(2-)(g)` from oxygen atom requires first an exothermic and then an endothermic step as shown below
`O(g)+e^(-) rarr O^(-)(g), DeltaH^(-) = - 141 kj mol^(-1)`
`O^(-)(g) +e^(-) rarr O^(2-) (g), DeltaH^(-) =+ 780 kj mol^(-1)`
Thus, process of formation of `O^(2-)` in gas phase is unfavourable even through `O^(2-)` is isoelectronic with neon. It is due to the fact that A) oxygen is more electronegative B) addition of electron in oxygen results in larget size of the ion C) electron repulsion outweights the stability gained by achieving noble gas configuration D) `O^(-)` ion has comparatively smaller size than oxygen atom

Options

A. oxygen is more electronegative.
B. addition of electron in oxygen results in larger size of the ion.
C. electron repulsion outweights the stability gained by achieving noble gas configuration
D. `O^(-)` ion has comparatively smaller size than oxygen atom.

Answer

C

Explanation

There is electrostatic repulsion between the two species having same type of charge. So energy has to be given for the addition of additional electron to `O^(-)`.