Graphene and buckminsterfullerene (C60C_{60}C60) are two well-known allotropes of carbon.
Which statement correctly describes and compares their bonding, structure, and properties?
Both graphene and buckminsterfullerene are classified as giant covalent structures with extremely high melting points, and neither is soluble in non-polar organic solvents.
In graphene, each carbon atom is covalently bonded to three other carbon atoms, whereas in buckminsterfullerene, each carbon atom is covalently bonded to four other carbon atoms to form the spherical cage.
Graphene conducts electricity due to delocalised electrons that are free to move across its giant structure, whereas bulk buckminsterfullerene is a poor conductor because its delocalised electrons are restricted within individual molecules.
Buckminsterfullerene has a higher melting point than graphene because the covalent bonds between individual C60C_{60}C60 molecules are exceptionally strong.
74 exam-style questions on OCR GCSE Chemistry Bonding. Each one has a worked solution and a mark scheme showing where the marks go.