Evaluate the following statements related to group 14 elements for their correctness. (A) Covalent radius decreases down the group from C to Pb in a regular manner. (B) Electronegativity decreases from C to Pb down the group gradually. (C) Maximum covalance of C is 4 whereas other elements can expand their covalance due to presence of d orbitals. (D) Heavier elements do not form $$p\pi - p\pi$$ bonds. (E) Carbon can exhibit negative oxidation states. Choose the correct answer from the options given below :

We evaluate statements about Group 14 elements (C, Si, Ge, Sn, Pb):

(A) Covalent radius decreases down the group from C to Pb in a regular manner.

This is incorrect. The covalent radius generally increases down the group, not decreases. Also, the increase from Si to Ge is less pronounced due to the d-orbital contraction (scandide contraction).

(B) Electronegativity decreases from C to Pb down the group gradually.

This is incorrect. While the general trend is a decrease in electronegativity going down the group, it does not decrease gradually/uniformly. There are irregularities due to d- and f-orbital effects.

(C) Maximum covalence of C is 4 whereas other elements can expand their covalence due to presence of d-orbitals.

This is correct. Carbon has no d-orbitals in its valence shell, so its maximum covalence is 4. Si, Ge, Sn, and Pb have vacant d-orbitals and can expand their covalence beyond 4 (e.g., $$SiF_6^{2-}$$).

(D) Heavier elements do not form $$p\pi - p\pi$$ bonds.

This is correct. Due to their large atomic sizes, Si, Ge, Sn, and Pb cannot form effective $$p\pi - p\pi$$ multiple bonds, unlike carbon which readily forms $$C=C$$ and $$C \equiv C$$ bonds.

(E) Carbon can exhibit negative oxidation states.

This is correct. Carbon can show negative oxidation states, such as $$-4$$ in $$CH_4$$, $$-1$$ in $$C_2H_6$$, etc.

The correct statements are (C), (D), and (E) only.

The answer is Option B: (C), (D) and (E) Only.