Final answer:
Benzene has a planar hexagonal structure with equal bond lengths and 120-degree bond angles, does not consist of alternating single and double bonds but exhibits resonance, represented by a circle inside the hexagon to indicate delocalized electron bonding.
Step-by-step explanation:
The bonding in benzene can be described by the following statements:
- Benzene does not consist of alternating single and double bonds; the actual bonding situation is a hybrid of two resonance structures, leading to all C-C bonds being equivalent, which is not accurately depicted by alternating single and double bonds.
- Benzene has a planar hexagonal structure, which contributes to its stability and unique properties.
- The bond lengths in benzene are equal, reflecting the delocalized electrons across the carbon atoms that make benzene's structure and bonding very stable.
- The bond angles in benzene are indeed 120 degrees, as expected for a planar hexagonal molecule composed of sp²-hybridized carbon atoms.
- Benzene exhibits resonance; this characteristic is a consequence of the delocalization of electrons, which can be represented by a hexagon with an inscribed circle to symbolize the equivalent nature of the C-C bonds.