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Question

Find the correct order of the ionic radius of following isoelectronic species.

A
Ca2+<K+<Cl<S2
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B
Ca2+<K+<S2<Cl
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C
K+<Ca2+<S2<Cl
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D
K+<Ca2+<Cl<S2
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Solution

The correct option is A Ca2+<K+<Cl<S2
Isoelectronic species have same number of electrons in their electronic shells but their nuclear charge differs because of their difference in number of protons in the nucleus. With increase in number of protons in the nucleus the electrons are more attracted towards nucleus thereby causing the decrease in ionic radius.
Ca2+,K+,Cl1 and S2 have 18 electrons. But Ca2+ have 20 protons in its nucleus exerts higher effective nuclear charge than, K+ having 19 protons than, Cl having 17 protons and than S2 having 16 protons. So, order of effective nuclear charge is Ca2+>K+>Cl>S2.
As size is inversely proportional to effective nuclear charge, therefore, order of size is: Ca2+<K+<Cl<S2

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