JEE Main 2024 — p Block Elements (Group 13 & 14) Question with Solution

$\mathrm{Gr}-14 \mathrm{EN}$

$\mathrm{C} 2.5$

$\mathrm{Si} 1.8$

$\mathrm{Ge} 1.8$

$\mathrm{Sn} 1.8$

$\mathrm{Pb} 1.9$

The electronegativity values for elements from $\mathrm{Si}$ to $\mathrm{Pb}$ are almost same. So Statement I is false.

1. Among them, Carbon and silicon are non-metals.
2. Germanium is metalloid in nature
3. Tin and lead are metal.

Reason for different metallic characteristics

1. The metallic character increases down the group from carbon to lead as nonmetal to metal.
2. The metallic character increases because the atomic size increases from Carbon to Lead.
3. As size increases, the ionization potential decreases down the group.
4. A decrease in ionization potential lead to an increase in the electropositive character of the element.

Hence, the metallic character increases down the group in group$-14$ as the ionization potential decreases to make it easier to lose an electron and increase the metallic character.