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The formation of the oxide ion O((g))^(2...

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 " kJmol"^(-1)`
This is because

A

`O^(-)` ion will tend to resist the 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

Text Solution

Verified by Experts

The correct Answer is:
A
`O^(-)` ion exerts a force of repulsion on the incoming electron. The energy is required to overcome it.
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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 :

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

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