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Chemistry Question on Classification of elements & periodicity in properties

The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species, K+,Ca2+,Mg2+,Be2+K^+, Ca^{2+}, Mg^{2+}, Be^{2+}

A

K+>Ca2+>Mg2+<Be2+K^+ > Ca^{2+} > Mg^{2+} < Be^{2+}

B

Be2+<Ca2+<Mg2+<K+Be^{2+} < Ca^{2+} < Mg^{2+} < K^+

C

Mg2+<K+<Be2+<Ca2+Mg^{2+} < K^+ < Be^{2+} < Ca^{2+}

D

K+<Ca2+<Mg2+<Be2+K^+ < Ca^{2+} < Mg^{2+} < Be^{2+}

Answer

K+<Ca2+<Mg2+<Be2+K^+ < Ca^{2+} < Mg^{2+} < Be^{2+}

Explanation

Solution

Smaller the size and higher the charge, more will be polarizing power of the cation. Since the order of the size of cation is K+>Ca2+>Mg2+>Be2+K^+ > Ca^{2+} > Mg^{2+} > Be^{2+} the correct order of polarizing power is K+>Ca2+>Mg2+>Be2+K^+ > Ca^{2+} > Mg^{2+} > Be^{2+}