Question

What is the hybridization of the carbon atom in \(CO_2\)?

• A. \(sp^3\)
• B. \(sp^2\)
• C. \(sp\)
• D. \(sp^3d\)

Hint:

If the central atom has:
• 2 regions of electron density → \(sp\)
• 3 regions → \(sp^2\)
• 4 regions → \(sp^3\) Carbon in \(CO_2\) has two regions, hence \(sp\) hybridization.

Answer 1

The Correct Option is C

Concept: Hybridization is the mixing of atomic orbitals of similar energy to form new equivalent hybrid orbitals. The type of hybridization depends on the number of regions of electron density (sigma bonds or lone pairs) around the central atom.

Step 1: Determine the bonding in \(CO_2\). The structure of carbon dioxide is: \[ O = C = O \] Carbon forms two double bonds with two oxygen atoms.

Step 2: Count regions of electron density. Each double bond contains one sigma bond. Therefore, carbon has:
• 2 sigma bonds
• 0 lone pairs Total regions of electron density \(=2\).

Step 3: Determine hybridization. Two regions of electron density correspond to \(sp\) hybridization and a linear molecular geometry with bond angle \(180^\circ\). Thus, the hybridization of carbon in \(CO_2\) is \(sp\).