In the planar hexagonal geometry of benzene, the bond angles are defined by the trigonal planar geom — Hydrocarbons Chemistry Question

💡 Solution & Explanation

Because every carbon atom in benzene utilizes strictly $sp^2$ hybridization and no lone pairs are present on the carbons, the molecular geometry at each center is perfectly trigonal planar, imposing a strict $120^{\circ}$ bond angle. This perfectly matches the internal angle of a regular hexagon, making the ring fully strain-free.