A) \[{{\text{F}}^{-}}\]
B) \[{{\text{O}}^{-}}\]
C) \[\text{O}\]
D) Na
Correct Answer: C
Solution :
As the size of atom decreases, a larger amount of energy is released when an electron is added to an isolated gaseous atom. Among the given species, the size of O atom is smallest (\[\because \]size of parent atom is smaller as compared to its anion), thus its electron affinity is highest. [Remember! the value of second electron affinity is generally positive. This is because, the second electron experience a greater force of repulsion from the existing electrons. Hence, to overcome this repulsion, some heat is absorbed. This is also the reason for lower electron affinity of \[{{F}^{-}}\] as compared to O.]
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