Problem: The table below shows the normal boiling points of benzene and benzene derivatives.Why is the boiling point of bromobenzene higher than that of chlorobenzene?

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•  Chlorobenzene and bromobenzene both exhibit two types of intermolecular forces of attraction (IMFA)

1. London Dispersion Forces (LDF): This is present in all molecules and is the main force exhibited by non- polar molecules. The benzene ring of chlorobenzene and bromobenzene exhibits this type of IMFA.

2. Dipole-dipole Forces (DDF): This is exhibited by molecules which have a net dipole caused by the presence of an electronegative atom. The halogens (Cl and Br) are responsible for this type of IMFA in the benzene derivatives.

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Problem Details
The table below shows the normal boiling points of benzene and benzene derivatives.

C6H6, benzene, is a six membered ring with alternating single and double bonds and a normal boiling point of 80 degrees celsius.  C6H5Cl, chlorobenzene, is a benzene ring with a chlorine atom attached to one of the carbons instead of a hydrogen and a normal boiling point of 132 degrees celsius.  C6H5Br, bromobenzene, is a benzene ring with a bromine atom attached to one of the carbons instead of a hydrogen atom and a normal boiling point of 156 degrees celsius.  C6H5OH, called phenol or hydroxybenzene, is a benzene ring with an OH attached to one of the carbons instead of a hydrogen and a normal boiling point of 182 degrees celsius.

Why is the boiling point of bromobenzene higher than that of chlorobenzene?

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