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The formation of the oxide ion O ((g)) ^...

The formation of the oxide ion `O _((g)) ^(2-)` from oxygen atom requires first an exothermic and then an endothermic step as shown below :
`O _((g)) + e ^(-) to O _((g )) ^(-) ,Delta _(f) H^(0) =-141 kJ mol ^(-1)`
`O _((g)) ^(-) +e ^(-) to O _((g)) ^(-2) ,Delta _(f) H^(0) =+ 780 kJ mol ^(-1)`
Thus, process of formation of `O^(2-)` in gas phase is unfavourable even thrugh `O ^(2-)` is isoelectronic with neon. It is due to the fact that (2015)

A

`O^(-)` ion has comparatively smaller size than oxygen atom

B

Oxygen is more electronegative

C

Addition of electron in oxygen result in larger size of the ion

D

Electron repulsion outweights the stability gained by achieving noble gas configuration.

Text Solution

Verified by Experts

The correct Answer is:
D
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