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Question

The formation of the oxide ion, O2(g) from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+eO(g);ΔfH=141 kJ mol1O(g)+eO2(g);ΔfH=+780 kJ mol1
Thus, process of formation of O2 in gas phase is unfavourable even though O2 is isoelectronic with neon. It is due to the fact that,


A

O ion has comparatively smaller size than oxygen atom.

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B

oxygen is more electronegative

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C

addition of electron in oxygen results in larger size of the ion.

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D

electron repulsion outweighs the stability gained by achieving noble gas configuration.

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Solution

The correct option is D

electron repulsion outweighs the stability gained by achieving noble gas configuration.


When the oxygen atom gains one electron, it makes it more stable, which is reflected by the first equation. Adding another electron is really difficult due to the repulsion faced by it. This is shown by the second equation.


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