Chapter EH, Problem 11R

Solution

Interpretation : Lithium’s atomic and ionic radii closer to sodium or closer to magnesium, which is in group 2 is to be analyzed and explained.

Concept Introduction : The periodic table's first occurrence of lithium is among the alkalis. It is the lightest metal which is a solid.

Lithium’s atomic and ionic radii are closer to magnesium, which is in group 2 due to its smaller size and high polarizing power.

Lithium's characteristics are comparable to those of group 2 element magnesium.

The diagonal relationship in the periodic table is the name given to this kind of diagonal resemblance. It is caused by the elements' comparable ionic sizes and charge/radius ratios.

Lithium and magnesium have atomic and ionic radii that are closer to one another.

The atomic radii of lithium and magnesium are 152 pm and 160 pm.

The ionic radii of ${\text{Li}}^{\text{+}}$ is 76 pm and ${\text{Mg}}^{2+}$ is 72 pm.

Lithium exhibits anomalous behavior as a result of its small atom size and strong polarizing power (charge/radius ratio).