What is the hybridization of the carbon atoms in benzene?

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Q: What is the hybridization of the carbon atoms in benzene?

Solution: The carbon atoms in benzene are sp2 hybridized, forming a planar structure with 120-degree bond angles.

Steps: 8

Step 1: Understand that benzene is a chemical compound with the formula C6H6, consisting of six carbon atoms and six hydrogen atoms.
Step 2: Recognize that each carbon atom in benzene is bonded to two other carbon atoms and one hydrogen atom.
Step 3: Identify that carbon has four valence electrons and needs to form four bonds.
Step 4: Determine that in benzene, each carbon atom forms three sigma (σ) bonds: two with neighboring carbon atoms and one with a hydrogen atom.
Step 5: Realize that to form these three bonds, carbon undergoes hybridization.
Step 6: Conclude that the hybridization of carbon in benzene is sp2 because it uses one s orbital and two p orbitals to create three equivalent sp2 hybrid orbitals.
Step 7: Note that the remaining p orbital on each carbon atom is used to form a delocalized pi (π) bond, contributing to the stability of the benzene ring.
Step 8: Finally, understand that the sp2 hybridization results in a planar structure with bond angles of approximately 120 degrees.