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The formation of the oxide ions,O^(2-)((...

The formation of the oxide ions,`O^(2-)_((g))` from oxygen atom requires first an exothermic and then an endothermic step as shown below: `O_(g)+e^(-)toO^(-)_((g)),DeltaH^(@)=-141 KJ mol^(-1)`
`O^(-)_((g))`to`O^(2-)_((g)),DeltaH^(@)=+780 KJ mol^(-1)` thus,process of formation of `O^(2-)` in gas phase is unfavourable even though `O^(2-)` is isoelectronic with neon.It it due to the fact that,

A

electron repulsion outweighs the stability gained by achieving noble gas configuration

B

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

C

Oxygen is more electronegative

D

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

Text Solution

Verified by Experts

The correct Answer is:
A
Since electron repulsion predominate over the stability gained by achieving noble gas configuration . Hence, formation of `O^(2-)` in gas phase is unfavourble .
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