Identify the correct order of the ionic size | vedclass

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(A) All the given species ($Ca^{2+}$,$K^{+}$,$Ar$,$Cl^{-}$,$S^{2-}$) are isoelectronic,meaning they all contain $18$ electrons.For isoelectronic speci

Vedclass · Accepted Answer

$Ca^{2+} < K^{+} < Ar < Cl^{-} < S^{2-}$

Vedclass · Answer

(A) All the given species ($Ca^{2+}$,$K^{+}$,$Ar$,$Cl^{-}$,$S^{2-}$) are isoelectronic,meaning they all contain $18$ electrons.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number,$Z$) increases.The atomic numbers are: $Ca$ $(Z=20)$,$K$ $(Z=19)$,$Ar$ $(Z=18)$,$Cl$ $(Z=17)$,$S$ $(Z=16)$.Since the nuclear charge follows the order $Ca^{2+} > K^{+} > Ar > Cl^{-} > S^{2-}$,the ionic size follows the inverse order:$Ca^{2+} < K^{+} < Ar < Cl^{-} < S^{2-}$.

Identify the correct order of the ionic size for the following isoelectronic species:

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