The element that shows greater ability to form p-p multiple bonds is:

🧠 $\text{p}\pi$–$\text{p}\pi$ bonding (side-by-side overlap of p orbitals to form π bonds) is strongest when the atoms are small and have compact 2p orbitals that can overlap effectively. As the atomic radius increases down a group, p orbital overlap decreases.

• C (Period 2): small size, compact 2p orbitals → strong $\text{p}\pi$–$\text{p}\pi$ bonds → forms C=C, C=O, C≡N routinely ✓
• Si (Period 3): larger atomic radius → 3p orbitals more diffuse → poor $\text{p}\pi$–$\text{p}\pi$ overlap → Si prefers single bonds
• Ge, Sn: even larger → essentially no stable $\text{p}\pi$–$\text{p}\pi$ bonds

⚠️ This is why $\ce{SiO2}$ is a covalent network solid (Si–O single bonds) while $\ce{CO2}$ is a gas with O=C=O double bonds.

$\boxed{\text{Answer: (b) C}}$