The element that does not show catenation is:

🧠 Catenation requires strong element-element bonds — and Pb-Pb bonds are the weakest in Group 14 Catenation means an element bonds with itself to form chains, rings, or networks. The strength of the E–E single bond determines whether an element can do this. Going down Group 14, the atoms get bigger and more diffuse, so the E–E bond gets longer and weaker. Pb at the bottom has essentially no catenation tendency.

🗺️ Group 14 catenation tendency C: ~80 kcal/mol (C–C bond). Catenation is the reason organic chemistry exists — millions of compounds, chains and rings everywhere. Si: about half of C. Forms silanes up to $\ce{Si6H14}$, then chemistry runs out. Limited catenation. Ge: weaker still. Some chains exist but they are unstable. Sn: very weak Sn–Sn. A few small clusters, but no extensive catenation. Pb: essentially no catenation. The Pb–Pb bond is too long and weak to hold a chain together at room temperature.

So among the four options, Pb is the one that does not show catenation.

⚠️ The trap Students sometimes pick Sn because Sn is one place above Pb and they assume "everything stops at Sn". Sn does form some Sn–Sn bonded compounds (like $\ce{Sn2Cl4}$), even if limited. Pb truly does not. The order of catenation: C >> Si > Ge > Sn > Pb (essentially zero).

$\boxed{\text{Answer: (d)}}$