Question

Use the localized electron model to describe the bonding in $\mathit{C}\mathit{C}{\mathit{l}}_{\mathbf{4}}$.

Short answer

In $CC{l}_4$the central atom is carbon. The structure of the molecule is tetrahedral. The four hybrid orbitals combine with four chlorine atoms each. The hybridization is ${\text{sp}}^{\text{3}}$.

Step-by-step solution

Step 1

The Lewis structure is as follows:

The central carbon is attached to four chlorine atoms.

Step 2

The four electron pairs that form the four C-Cl bond need a tetrahedral arrangement. This is obtained by the formation of four ${\text{sp}}^{\text{3}}$hybrid orbital from one 2s and three 2p orbitals of carbon. The four hybrid orbitals will have tetrahedral orientation in space and will combine with four atomic orbitals of chlorine to form four sigma bonds.