p-Block Elements - Group 14 Elements (Carbon Family)

Group 14 elements, known as the Carbon Family, include Carbon ($C$), Silicon ($Si$), Germanium ($Ge$), Tin ($Sn$), and Lead ($Pb$).

The general valence shell electronic configuration is $ns^2 np^2$.

Atomic radii increase down the group due to the addition of new energy shells, though the increase from $Si$ to $Pb$ is small due to poor shielding by $d$ and $f$ electrons.

Ionization Enthalpy decreases down the group. However, a slight increase is observed from $Sn$ to $Pb$ due to the poor shielding effect of $4f$ electrons.

Carbon shows an anomalous behavior due to its small size, high electronegativity, and the absence of vacant $d$-orbitals.

Catenation is the self-linking property of atoms to form long chains or rings. Carbon exhibits the maximum catenation power in the group: $C \gg Si > Ge \approx Sn > Pb$.

Carbon has three main allotropes: Diamond ($sp^3$ hybridized, tetrahedral), Graphite ($sp^2$ hybridized, layered structure), and Fullerenes ($sp^2$ hybridized, cage-like molecules like $C_{60}$).

Oxidation states: These elements show $+4$ and $+2$ oxidation states. The stability of the $+2$ oxidation state increases down the group due to the 'Inert Pair Effect', making $Pb^{2+}$ more stable than $Pb^{4+}$.

Carbon Monoxide ($CO$) is a neutral oxide and a powerful reducing agent, while Carbon Dioxide ($CO_2$) is an acidic oxide.

$SiCl_4$ undergoes hydrolysis because Silicon has vacant $d$-orbitals to accept lone pairs from water, whereas $CCl_4$ does not.