Question

What is the hybridization state of carbon in carbon dioxide?

Answer 1

Step 1: Hybridization:

• “Hybridization is defined as the process of intermixing of the orbitals of slightly different energies so as to redistribute their energies, resulting in the formation of a new set of orbitals of equivalent energies and shape.”

Step 2: Formula used for calculation:

• $\mathrm{Steric}\mathrm{number}=\frac{1}{2}\left(\mathrm{V}+\mathrm{M}-\mathrm{C}+\mathrm{A}\right)$
• Where V is the number of valence electrons, M is the monovalent electron, C is the positive charge and A represents the negative charge.

Step 3: Calculation for Hybridisation and shape of ${\mathrm{CO}}_2$:

• The total number of valence electrons in ${\mathrm{CO}}_2$ is 4 and there is 0 monovalent atom.
• $\mathrm{Steric}\mathrm{number}=\frac{1}{2}\left(4\right)=2$
• The steric number is 2, thus the hybridization of ${\mathrm{CO}}_2$ is $\mathrm{sp}$.
• The hybridization state of carbon in ${\mathrm{CO}}_2$ is $\mathrm{sp}$ hybridized.
• The two $\mathrm{sp}$ hybridized orbitals of the carbon atom overlap with two $\mathrm{p}$ orbitals of the oxygen atom to form two sigma $\left(\mathrm{\sigma }\right)$ bonds while the other two electrons of carbon are involved in $\mathrm{\pi }-\mathrm{\pi }$ bonding with the oxygen atom.
• Carbon dioxide has a linear geometry.