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(A) The given species $Ca^{2+}$, $Cl^{-}$, and $S^{2-}$ are isoelectronic, meaning they all contain $18$ electrons.SpeciesAtomic number $(Z)$Number of

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Radius of $Ca^{2+} < Cl^{-} < S^{2-}$

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(A) The given species $Ca^{2+}$, $Cl^{-}$, and $S^{2-}$ are isoelectronic, meaning they all contain $18$ electrons.SpeciesAtomic number $(Z)$Number of electrons$Ca^{2+}$$20$$18$$Cl^{-}$$17$$18$$S^{2-}$$16$$18$For isoelectronic species, the ionic radius decreases as the nuclear charge (atomic number) increases. Since the atomic numbers are $Z(S^{2-}) = 16$, $Z(Cl^{-}) = 17$, and $Z(Ca^{2+}) = 20$, the order of increasing radius is $Ca^{2+} < Cl^{-} < S^{2-}$.

Which of the following is correct regarding the ionic radii of the given species?

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