This species is a derivative of benzene, with a single fluorine atom attached. Its melting point is -44 °C, which is lower than that of benzene, indicative of the remarkable effect of fluorination on the intermolecular interactions as seen throughout organofluorine chemistry. In contrast, the boiling points of PhF and benzene differ by only 4 °C.
Why is this true? Wikipedia doesn't elaborate on why.
From what I understand the melting point is the point at which the solid and liquid forms are in equilibrium.
Boiling point is the point at which the liquid and gas phases are in equilibrium.
I know that intermolecular forces play an integral role in melting and boiling point. However, why does it seem that the strength of the intermolecular forces in the solid phase is stronger than that in the liquid phase for fluorobenzene?