A) \[C{{a}^{2+}}<M{{g}^{2+}}<B{{e}^{2+}}<{{K}^{+}}\]
B) \[M{{g}^{2+}}<\,\,B{{e}^{2+}}<{{K}^{+}}<C{{a}^{2+}}\]
C) \[B{{e}^{2+}}<{{K}^{+}}<C{{a}^{2+}}<M{{g}^{2+}}\]
D) \[{{K}^{+}}<C{{a}^{2+}}<M{{g}^{2+}}<B{{e}^{2+}}\]
Correct Answer: D
Solution :
[d] \[{{K}^{+}}<\text{ }C{{a}^{2+}}<M{{g}^{2+}}<B{{e}^{2+}}\] Alkaline earth metals have higher charge (+2) than alkali metals (+1) but have lower in size than corresponding alkali metals. Thus, 1C" has lowest polarizing power. Among alkaline earth metals, size increases down the group. Therefore, polarizing power decreases down the group that is The overall polarizing power of the four cations increase in the order: \[{{K}^{+}},C{{a}^{2+}},M{{g}^{2+}}<B{{e}^{2+}}\]
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