Question

Compare and contrast the chemistry of Group 1 metals with that of group 2 with respect to the following :
Polarizing power of cations increases on going from group 1 to group 2.

Answer 1

Hint: The polarization or polarizability depend upon charge upon radius ratio. The charge upon radius ratio is directly proportional to the polarizability. The group 1 elements can easily lose one electron while the group 2 elements can easily lose 2 electrons. Further, on moving left to right in the periodic table, the radius decreases due to increase in atomic size.

Complete answer:
First, let us see what polarization is.
The polarisation is the distortion of an electron cloud of negatively charged ion by the positively charged ion. The polarizability enhances the formation of covalent bonds.
The polarization or polarizability depend upon charge upon radius ratio.
As we all know that group 1 elements also called as alkali metals can lose one electron to attain noble gas configuration while the group 2 elements called alkaline earth metals can lose two electrons to attain noble gas configuration. So, the group 2 elements will have high charge upon radius ratio than group 1 elements.
The charge upon radius ratio is directly proportional to the polarizability. So, the group 2 elements will have higher polarizability than group 1 elements.

Note:
It must be noted that the group 1 elements have one electron in ‘s’ orbital. All other orbitals present are filled. By losing this electron, it attains the noble gas configuration which is very stable. In case of Group 2 elements, the ‘s’ has two electrons that can be lost to achieve noble gas configuration.