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This shows that as buckminsterfullerene hasmuch weaker inter-molecular forces than diamond, it has a much lower melting/boiling point. (Less energy required to break the forces of attraction.) Fullerene has a low melting point because it has not so strong bonds.
Accordingly, does fullerene have a high or low melting point?
They are made up of large molecules but do not have a giant covalent structure. Weak intermolecular forces exist between individual buckyballs. Little energy is needed to overcome these forces, so substances consisting of buckyballs are slippery and have lower melting points than graphite or diamond .
Subsequently, one may also ask, why does c60 have a low melting point?
Its molecules are made up of 60 carbon atoms joined together by strong covalent bonds. There are weak intermolecular forces between molecules of buckminsterfullerene. These need little energy to overcome, so buckminsterfullerene is slippery and has a low melting point.
Their unique molecular structure results in extraordinary macroscopic properties, including high tensile strength, high electrical conductivity, high ductility, high heat conductivity, and relative chemical inactivity (as it is cylindrical and "planar" — that is, it has no "exposed" atoms that can be easily displaced).