Q.State the general valence-shell electronic configuration of the p-block elements, and write out the specific configurations for the outermost shell of Group 13 (boron family) and Group 14 (carbon family). Which sub-shell is being progressively filled across the p-block?

p-Block groups share one organising idea: the group oxidation state equals the number of $ns^2np^x$ valence electrons (Table 11.1), yet almost every group's heavier members increasingly prefer an oxidation state two units LOWER than this "textbook" value — the seed of what later becomes the formally-named inert-pair effect. Across a p-block group, atomic radius, ionisation enthalpy and electronegativity are all expected to follow simple periodic rules (radius up, ionisation enthalpy down, electronegativity down as you descend a group) — but from Group 13 onward these trends develop real discontinuities once you cross from a simple noble-gas-core element (like Al) to one with filled d or f subshells hidden in its core (like Ga, In, Tl). Those buried d/f electrons shield the nucleus poorly, so the effective nuclear charge felt by the valence shell jumps unexpectedly at exactly those points, disturbing radius, ionisation enthalpy and electronegativity all at once. The acid–base character of oxides is a second recurring theme: within a group, oxides shift from acidic (lighter, non-metallic members) through amphoteric (intermediate members) to basic (heaviest, most metallic members) — seen in both Group 13 ($B_2O_3$ acidic → $Tl_2O_3$ basic) and Group 14 ($CO_2$ acidic → $PbO$ amphoteric).