Question

The force used to explain that the carbon-to-carbon bonds in benzene, C6H6, are identical is:

(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)"

Answer 1

The force used to explain that the carbon-to-carbon bonds in benzene are identical is resonance. Benzene is a planar aromatic hydrocarbon with a hexagonal ring structure and the carbon atoms in benzene are sp² hybridized, allowing for the delocalization of electrons and equal carbon-carbon bonds.

Step-by-step explanation:

In the case of benzene, the force used to explain that the carbon-to-carbon bonds are identical is resonance. Benzene is a planar aromatic hydrocarbon with a hexagonal ring structure. The carbon atoms in benzene are sp² hybridized, meaning they have three sigma bonds in a trigonal planar geometry and one unhybridized p orbital perpendicular to the plane. The delocalization of electrons throughout the molecule due to resonance allows all six carbon-carbon bonds in benzene to be equal.