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The formation of oxide ion 0^{2-} (g) from oxygen atom requires first an exothermic and then an endothermic step as shown below
O(g)+eO(g);H=141kjmol1O(g)+eO2(g);H=+780kjmol1
Thus, process of formation of O2 in gas phase is unfavourable even through O2 is isoelectronic with neon. It is due to the fact that
(a) Oxygen si more electronegative
(b) addition of electron in oxygen results in larger size of the ion
(c) electron repulsiion outweighs the stability gained by achieving noble gas configuration
(d) O ion has comparativly smaller size than oxygen atom

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Solution

Answer: (c) electron repulsion outweighs the stability gained by achieving the noble gas configuration

Although O2 has noble gas configuration isoelectronic with neon its formation is unfavourable due to the strong electronic repulsion between the negatively charged O ion and the second electron being added.
Hence, the electron repulsion outweighs the stability gained by achieving a noble gas configuration.


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