What type of hybridization occurs in the carbon atoms of benzene?

In benzene, each carbon atom is bonded to two other carbon atoms and one hydrogen atom, forming a planar structure with a bond angle of approximately 120 degrees. This trigonal planar arrangement around each carbon atom indicates the involvement of sp2 hybridization.

In sp2 hybridization, one s orbital mixes with two p orbitals to form three equivalent sp2 hybrid orbitals that are oriented 120 degrees apart in a plane. The remaining unhybridized p orbital, which is perpendicular to the plane of the sp2 orbitals, allows for the formation of a delocalized π system. This delocalization is what gives benzene its characteristic stability and unique aromatic properties, resulting in the molecule being represented with resonance structures.

Thus, the identification of sp2 hybridization in the carbon atoms of benzene is pivotal in understanding its bonding and stability, demonstrating that the correct answer aligns with the molecular geometry and electronic structure of benzene.