A) \[1{{s}^{2}},\text{ }2{{s}^{2}},\text{ }2{{p}^{3}}\]
B) \[1{{s}^{2}},\text{ }2{{s}^{2}},\text{ }2{{p}^{5}}\]
C) \[1{{s}^{2}},\text{ }2{{s}^{2}},\text{ }2{{p}^{6}},\text{ }3{{s}^{2}},\text{ }3{{p}^{5}}\]
D) \[1{{s}^{2}},\text{ }2{{s}^{2}},\text{ }2{{p}^{6}},\text{ }3{{s}^{2}},\text{ }3{{p}^{3}}\]
E) \[1{{s}^{2}},\text{ }2{{s}^{2}},\text{ }2{{p}^{6}},\text{ }3{{s}^{1}}\]
Correct Answer: C
Solution :
Generally electron affinity increases in a period and decreases in a group but due to smaller size and high electron density on fluorine atom, it experience high intereltronic repulsions. Thus,\[{{F}^{-}}\]ion is less stable in comparison to\[C{{l}^{-}}\]ion. Hence, electron affinity is highest for chlorine. Its electronic configuration is \[_{17}Cl=1{{s}^{2}},2{{s}^{2}},2{{p}^{6}},3{{s}^{2}},3{{p}^{5}}\]
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