H H C H C C C What are the geometry and hybridization around each H C H H carbon atom in benzene, C6H6 a. sp2, trigonal planar b.sp,linear c.sp3,tetrahedral d. sp3, trigonal planar
The Correct Answer and Explanation is:
Correct Answer: a. sp², trigonal planar
Explanation:
Benzene (C₆H₆) is a unique organic compound known for its stable ring structure and aromaticity. Its molecular structure consists of six carbon atoms arranged in a regular hexagon, with one hydrogen atom attached to each carbon. To understand the geometry and hybridization of each carbon atom in benzene, we need to analyze how the atoms are bonded and how electrons are distributed in the molecule.
Each carbon atom in benzene forms three sigma (σ) bonds: two with adjacent carbon atoms and one with a hydrogen atom. In order to form these three sigma bonds, the carbon atoms use sp² hybrid orbitals.
Hybridization is the process by which atomic orbitals mix to form new, equivalent hybrid orbitals suitable for bonding. For a carbon atom to form three sigma bonds, it needs three hybrid orbitals, which results from mixing one s orbital and two p orbitals. This hybridization is called sp².
The geometry associated with sp² hybridization is trigonal planar, which means the three hybrid orbitals are arranged in a flat, 120° planar geometry. This allows for the overlap of unhybridized p orbitals on each carbon atom, which are perpendicular to the plane of the ring. These unhybridized p orbitals overlap side-by-side to form a delocalized π electron cloud above and below the ring, giving benzene its characteristic stability and aromatic nature.
In summary, each carbon in benzene is:
- sp² hybridized, meaning it uses three hybrid orbitals to form sigma bonds,
- trigonal planar in geometry, with 120° bond angles,
- Part of a delocalized π electron system, contributing to the aromaticity of the molecule.
Therefore, the correct answer is:
a. sp², trigonal planar.
