Question

Are non metals in the carbon family?

Answer 1

The electrical configuration of the group $14$ elements is $n{s^2}n{p^2}$ . The outermost p orbitals of these elements have two electrons. Metallic character increases from top to bottom because the ionisation energy of elements decreases as they move down the group, causing them to lose one electron. As a result, metallic character increases as the group progresses.

Complete answer:
The carbon family consists of metals, nonmetals and metalloids.
The periodic table's group $14$ elements are the second group in the p-block. It is called the carbon group. The elements in the group are Carbon ( $C$ ) , Silicon ( $Si$ ) , Germanium ( $Ge$ ) , Tin ( $Sn$ ) , Lead ( $Pb$ ) .
In their outermost energy level, all of these elements have four electrons. Only carbon and silicon create non-metal bonding among the Group $14$ elements (sharing electrons covalently). Tin and lead are metals, while germanium is a metalloid. From carbon to lead, the metallic character increases.
The increase in atomic size from carbon to lead causes the change from non-metallic to metallic nature. As a result, the ionisation potential of carbon to lead diminishes. As a result, the electropositive feature becomes more prominent, favouring ionic bonding, particularly at oxidation state $+ 2$ . Carbon and silicon, on the other hand, have a $+ 4$ oxidation state, generating covalent bonds with electron sharing.

Note:
Carbon, silicon, and germanium have extremely high melting and boiling points due to their extremely stable solid structures. Because of the inert pair effect, only two bonds are formed instead of four, $Sn$ and $Pb$ have a lower melting temperature. Carbon has an unusually high melting point.