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(C) All the given species are isoelectronic,having $18$ electrons. In an isoelectronic series,the ionic radius decreases as the nuclear charge (atomic

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$Ti^{4+}$

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(C) All the given species are isoelectronic,having $18$ electrons. In an isoelectronic series,the ionic radius decreases as the nuclear charge (atomic number) increases. The atomic numbers are: $K (19)$,$Ca (20)$,$Sc (21)$,and $Ti (22)$. Since $Ti^{4+}$ has the highest nuclear charge $(Z = 22)$,it exerts the strongest attraction on the electrons,resulting in the smallest ionic radius. Thus,the order of ionic radii is: $K^{+} > Ca^{2+} > Sc^{3+} > Ti^{4+}$.

The ion with the smallest radius among the following is:

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