Which statement is true about Group 14 elements and their Lewis acidity?

Group 14 elements, encompassing carbon, silicon, germanium, tin, and lead, exhibit varying degrees of Lewis acidity due to their differing electronegativities, atomic sizes, and available d-orbitals. While carbon is known for its strong covalent bonding and generally does not participate in hypervalent bonding, the other members of the group are capable of accommodating additional bonds through their larger atomic radii and availability of empty p and d orbitals.

Thus, silicon, germanium, tin, and lead can engage in hypervalent interactions, allowing them to accept additional electron pairs. This capability is substantially influenced by the size of the atoms; as we move down the group, the ability to accommodate additional ligands or electron pairs increases, making these heavier elements more Lewis acidic compared to carbon.

Thus, the correct statement reflects that all elements except carbon can exhibit hypervalent behavior, leading to their classification as Lewis acids. This unique characteristic of the non-carbon members in Group 14 allows them to form complexes with electron donors more readily than carbon, validating the assertion.