Describe and compare three features of the structure and bonding in the three allotropes of carbon: diamond, graphite and C60 fullerene.

I will explain to students that even though they only need to use three features, it is important to learn and understand all five features to excel in the exam. This way, during the exam, the students may pick three features from the five to use in their answer. Furthermore, it helps avoid situations where students forget certain features having only learnt and understood three. My teaching method ensures that students are fully prepared for questions - having learnt more, relevant knowledge to answer the question. I will always use diagrams as it is vital for students to understand the content through the use of diagrams, specifically with this question.
Diamond is a giant macromolecular structure, whereas graphite is a layered structure of hexagonal rings. C₆₀ fullerene consists of spheres made of atoms arranged in hexagons. Diamond has covalent bonding, whilst graphite and C₆₀ fullerene have covalent bonding and London dispersion forces. In the diamond structure, each carbon atom is attached to four other carbon atoms in a tetrahedral arrangement of carbon atoms. Graphite and C₆₀ fullerene structures involve each carbon atom attached to three other carbon atoms. Diamond has no delocalised electrons, whereas graphite and C₆₀ fullerene do have delocalised electrons. Diamond has bond angles of 109^o, whilst graphite has bond angles of 120^o. C₆₀ fullerene has bond angles between 109^o and 120^o.