Import Question JSON

$\textbf{HINT:} \text{ Alkali metals lie on the extreme left of the periodic table.}$ $\textbf{Explanation:}$ $\text{(i) The general electronic configuration of alkaline earth metals is [noble gas] } ns^2\text{.}$ $\text{(ii) These metals lose two electrons to acquire the nearest noble gas configuration. Therefore, their oxidation state is +2.}$ $\text{(iii) These metals have atomic and ionic radii smaller than that of alkali metals. Also, when moved down the group, the effective nuclear charge decreases and this causes an increase in their atomic radii and ionic radii.}$ $\text{(iv) Since the alkaline earth metals have a large size, their ionization enthalpies are found to be fairly low. However, their first ionization enthalpies are higher than the corresponding group 1 metals.}$ $\text{(v) These metals are lustrous and silvery-white in appearance. They are relatively less soft as compared to alkali metals.}$ $\text{(vi) Atoms of alkaline earth metals are smaller than that of alkali metals. Also, they have two valence electrons forming stronger metallic bonds. These two factors cause alkaline earth metals to have high melting and boiling points as compared to alkali metals.}$ $\text{(vii) They are highly electropositive in nature. This is due to their low ionization enthalpies. Also, the electropositive character increases on moving down the group from Be to Ba.}$