Question

Explain why a carbon atom cannot form five bonds using \({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{d}}\) hybrid orbitals.

Short answer

A carbon atom cannot form five bonds using \({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{d}}\) hybrid orbitals due to absence of d- orbital in it.

Step-by-step solution

Definition of Concept

The wave functions of atomic orbitals are combined in the hybridization process to form new orbitals with the same energy and shape. The LCAO method, or linear combination of atomic orbitals, is used to combine these atomic orbitals. These new orbitals with the same energy and shape are known as hybrid orbitals.

Explain why a carbon atom cannot form five bonds

Considering the given information:

\({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{d}}\)hybrid orbitals

Carbon has an atomic number of 6, and the orbital diagram for the given atom's valence shell is as follows:

\({\rm{C - 6}}\):

\(\begin{array}{*{20}{l}}{1{s^2}}&{2{s^2}}&{2{p^2}}\\{ \uparrow \downarrow }&{ \uparrow \downarrow }& \uparrow \end{array}\)

Because there is no d orbital in the electronic configuration of carbon, the carbon atom cannot form five bonds using\({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{d}}\)hybrid orbitals .

Therefore, due to the lack of a d- orbital, a carbon atom cannot form five bonds using\({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{d}}\)hybrid orbitals.

[B1]It has a complete valence shell, so it is unable to from any more bonds.