Periodic TableEasy
Question
The formation of the oxide ion O2-(g) requires first an exothermic and then an endothermic step as shown below
O(g) + e- O-(g) ;áƒHo = - 142 kJmol-1
O-(g) + e- O2-(g) ;áƒHo = - 844 kJmol-1
Options
A.Oxygen is more electronegative
B.O- ion has comparatively larger size than oxygen atom
C.O- ion will tend to resist the addition of another electron
D.Oxygen has high electron affinity
Solution
O-1(g) + e → O-2(g)
Due to the electronic repulsion, amount of the energy is needed to add electron
Due to the electronic repulsion, amount of the energy is needed to add electron
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