A) \[L{{i}^{+}}<M{{g}^{2+}}<{{K}^{+}}<A{{l}^{3+}}\]
B) \[A{{l}^{3+}}<L{{i}^{+}}<M{{g}^{2+}}<{{K}^{+}}\]
C) \[A{{l}^{3+}}<M{{g}^{2+}}<{{K}^{+}}<L{{i}^{+}}\]
D) \[{{K}^{+}}<A{{l}^{3+}}<M{{g}^{2+}}<L{{i}^{+}}\]
Correct Answer: B
Solution :
\[L{{i}^{+}}=60\,\,pm,\,\,\,{{K}^{+}}=133\,\,pm\,\,,\,\,M{{g}^{2+}}=65\,\,pm\],\[A{{l}^{3+}}=53.5\,pm\] The correct increasing order of ionic radii is \[A{{l}^{3+}}<L{{i}^{+}}<M{{g}^{2+}}<{{K}^{+}}\] In general, on moving from left to right, the ionic radii decreases due to increased effective nuclear charge. On moving down a group, the number of shells increases and thats why ionic radii increase.
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