Given a carbon atom forming three $\sigma$ bonds and one $\pi$ bond, what type of hybrid orbitals are used by the carbon atom?

• A. $s{p}^2$ hybrid orbitals
• B. $s{p}^3$ hybrid orbitals
• C. Unhybridized $p$ orbitals only
• D. $sp$ hybrid orbitals

Answer: (A)

Verified step by step guidance

1. Identify the total number of bonds and their types formed by the carbon atom: three sigma (\sigma) bonds and one pi (\pi) bond.
2. Recall that sigma bonds are formed by the overlap of hybridized orbitals, while pi bonds are formed by the side-to-side overlap of unhybridized p orbitals.
3. Determine the hybridization state of the carbon atom based on the number of sigma bonds: three sigma bonds correspond to sp\u00b2 hybridization, which involves one s orbital and two p orbitals hybridizing.
4. Understand that the remaining unhybridized p orbital is used to form the pi bond, which is consistent with the presence of one pi bond in the molecule.
5. Conclude that the carbon atom uses sp\u00b2 hybrid orbitals for the three sigma bonds and retains one unhybridized p orbital for the pi bond.