A) \[{{C}^{4-}}\]
B) \[{{C}^{3-}}\]
C) \[{{O}^{2-}}\]
D) \[M{{g}^{2+}}\]
Correct Answer: A
Solution :
These all are isoelectronic species. Greater the nuclear charge stronger is the attraction for same number of electrons and smaller is the ion. Thus, nuclear charge on \[{{C}^{4+}}\] ,\[{{N}^{3-}}\] and \[{{O}^{2-}}\], is 6, 7 and 8 respectively but nuclear charge on \[M{{g}^{2+}}\] is 12. Hence, \[{{C}^{4-}}\] has larger ionic radius than\[{{N}^{3-}}\], \[{{O}^{2-}}\]and \[M{{g}^{2+}}\].
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