Benzene is an organic chemical compound with the molecular formula C6H6

Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one a bond with another carbon atom and one and one bond with another carbon atom. Each carbon atom also forms one o bond with a hydrogen atom. H Identify which types of orbitals overlap to form the bonds between the atoms in a benzene molecule. Drag the appropriate labels to their respective targets. ► View Available Hint(s) sp²-8 sp³-sp³ sp-sp sp²-sp² р-р Bonds formed Carbon-carbon a bond Carbon-carbon bond H Carbon-hydrogen o bond C-H H Type of orbitals involved P Pearson

The Correct Answer and Explanation is :

Answer:

• Carbon-carbon σ bond: sp²-sp²
• Carbon-carbon π bond: p-p
• Carbon-hydrogen σ bond: sp²-s

Explanation:

Benzene (C₆H₆) is an aromatic hydrocarbon with a planar cyclic structure where six carbon atoms form a hexagonal ring. The bonding in benzene can be understood through valence bond theory and hybridization.

1. Hybridization of Carbon Atoms
   Each carbon atom in benzene undergoes sp² hybridization, meaning that one s orbital and two p orbitals mix to form three sp² hybrid orbitals. These sp² orbitals lie in the same plane, forming σ bonds with adjacent carbon atoms and one hydrogen atom.
2. Formation of σ Bonds

• Carbon-Carbon σ Bonds: Each carbon atom forms two σ bonds with neighboring carbon atoms using its sp² hybrid orbitals. Thus, the C-C σ bonds arise from sp²-sp² orbital overlap.
• Carbon-Hydrogen σ Bonds: Each carbon atom forms a σ bond with a hydrogen atom using its remaining sp² hybrid orbital, which overlaps with the 1s orbital of hydrogen. Thus, C-H σ bonds are formed from sp²-s orbital overlap.

1. Formation of π Bonds
   The unhybridized p orbitals on each carbon atom are perpendicular to the plane of the benzene ring. These p orbitals overlap laterally, forming a delocalized π system above and below the ring. This leads to the formation of C-C π bonds from p-p orbital overlap.
2. Delocalization of Electrons
   The p orbitals of all six carbon atoms interact simultaneously, creating a continuous π electron cloud. This delocalization is responsible for benzene’s aromatic stability and its resistance to typical alkene reactions.

Conclusion:

• C-C σ bonds: sp²-sp² orbital overlap
• C-C π bonds: p-p orbital overlap
• C-H σ bonds: sp²-s orbital overlap

This bonding model explains benzene’s planar geometry, equal bond lengths, and high stability, distinguishing it from alkenes with localized double bonds.