Explain the following.
Alkaline earth metals have low values of electronegativity; which decreases down the group.
- Electronegativity represents an attractive force exerted by the nucleus on shared electrons.
- The general outer electronic configuration of alkaline earth metals is ns2. They readily lose their two valence shell electrons to achieve a stable noble gas configuration. They are electropositive and hence, they have low values of electronegativity.
- As we move down the group atomic size increases, shielding effect increases, and effective nuclear charge decreases. Thus, the tendency to attract shared electrons decreases down the group.
Hence, the values of electronegativity decrease down the group.
Is there an error in this question or solution?