A) \[Na,\,\,Mg\]
B) \[{{O}^{2-}},\,\,{{N}^{3-}}\]
C) \[L{{i}^{+}},\,\,B{{e}^{2+}}\]
D) \[B{{a}^{2+}},\,\,S{{r}^{2+}}\]
Correct Answer: C
Solution :
\[{{O}^{2-}}\]and\[{{N}^{3-}}\]both are isoelectronic but differ in the charge possessed by them. As the negative charge increases, the electrons are held less and less tightly by the nucleus, therefore ionic radii increases. Hence, ionic radii of\[{{N}^{3-}}\]is greater than\[{{O}^{2-}}\]. In a period from left to right atomic radii decreases but in a group on moving downwards it increases.
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