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(D) Alkali metals $(Group \ 1)$ have only one valence electron per atom, which leads to weaker metallic bonding compared to alkaline earth metals $(Gr

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Lower ionization enthalpy

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(D) Alkali metals $(Group \ 1)$ have only one valence electron per atom, which leads to weaker metallic bonding compared to alkaline earth metals $(Group \ 2)$, which have two valence electrons. As a result, alkali metals are softer, have lower boiling points, and larger atomic/ionic radii than their corresponding alkaline earth metal counterparts. Furthermore, due to their larger atomic size and lower effective nuclear charge, alkali metals have lower ionization enthalpy values compared to alkaline earth metals.

When compared with alkaline earth metals, the alkali metals have

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