How does the shielding effect influence the metallic character of elements as you move down a group in the periodic table?

As you go down a group, the shielding effect grows because each new shell adds more inner electrons that push out the outer electron. This extra shielding lowers the effective nuclear charge felt by the valence electron, making it easier for the atom to lose that electron and behave like a metal. Consequently, the metallic character strengthens down the group. For example, sodium (group 1) loses one electron more readily than potassium, and cesium at the bottom of the same group is even more metallic because its outer electron is further shielded and farther from the nucleus. Thus, increasing shielding directly boosts metallicity as you descend a group.