The charge/size ratio of a cation determines | vedclass

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(D) The polarizing power of a cation is directly proportional to its charge density,which is defined by the ratio of charge to size.As the charge on t

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$K^{+} < Ca^{2+} < Mg^{2+} < Be^{2+}$

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(D) The polarizing power of a cation is directly proportional to its charge density,which is defined by the ratio of charge to size.As the charge on the cation increases and its ionic radius decreases,the polarizing power increases.For the given ions,the ionic radii follow the order: $K^{+} > Ca^{2+} > Mg^{2+} > Be^{2+}$.Since $Be^{2+}$ has the highest charge-to-size ratio and $K^{+}$ has the lowest,the increasing order of polarizing power is $K^{+} < Ca^{2+} < Mg^{2+} < Be^{2+}$.

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,$K^{+}, Ca^{2+}, Mg^{2+}, Be^{2+}$?

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