The bond length in benzene is approximately 1.39 Å (angstroms), which is the average of the single bond lengths between carbon atoms in the benzene ring.
The bond length in benzene is shorter than a single bond because of the phenomenon known as resonance. The delocalized electrons in the benzene ring contribute to the stability of the molecule, causing the bonds to be shorter and stronger than a typical single bond.
The shorter bond length in benzene contributes to its unique properties, such as its high stability and reactivity. It also affects the molecule's physical properties, such as its melting and boiling points.
The bond length in benzene can be influenced by factors such as the number of π bonds in the molecule, the presence of functional groups, and the presence of substituents on the ring. These factors can affect the delocalization of electrons and alter the bond length.
The bond length in benzene can be experimentally determined using techniques such as X-ray crystallography or spectroscopy. These methods allow scientists to measure the distance between atoms in a molecule and determine the bond length.