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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=141kJmol1
O(g)+eO2(g);ΔfH=+780kJmol1
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
oxygen is more electronegative
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B
addition of electron in oxygen results in larger size of the ion
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C
electron repulsion outweighs the stability gained by achieving noble gas configuration
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D
O ion has comparatively smaller size than oxygen atom
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Solution

The correct option is B electron repulsion outweighs the stability gained by achieving noble gas configuration
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 kJmol1
O(g)+eO2(g);ΔfH=+780 kJmol1
Thus, the process of formation of O2 in the gas phase is unfavorable even though O2 is isoelectronic with neon. It is due to the fact that electron repulsion outweighs the stability gained by achieving noble gas configuration.

When an electron is added to O anion, there is strong electrostatic repulsion between the two negative charges. Due to this, the second electron gain enthalpy of oxygen is positive.

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