Metallic character refers to the tendency of an atom to lose electrons and form positive ions, so it is closely tied to ionization enthalpy. Moving down a group, the number of electron shells increases and the outermost electrons lie farther from the nucleus and are better shielded, so the ionization enthalpy decreases. With electrons more easily lost, the metallic character increases steadily down a group. The option that metallic character decreases due to higher ionization enthalpy reverses the actual trend, since ionization enthalpy falls down a group. The option that it stays the same ignores the change in size and shielding. The option citing smaller atomic size is factually wrong because atoms get larger down a group. This trend, opposite to that across a period, is a key NCERT periodicity concept. Plausibility check: the increasingly metallic behaviour from carbon to lead within Group 14 directly illustrates the rise in metallic character down a group.