Lesson Plan: C1.4.05

Hamble Lesson Observation Plan
Learning About
What are fullerenes?
Keywords:
  • Extended writing: explain why the melting point and boiling point increases as the size of the molecule does in terms of intermolecular forces. (1)
  • Extended writing: explain why covalent substances do not conduct electricity. (1)
  • GF: Explain why pure water does not conduct electricity but tap water does conduct electricity. (1)
  • Extended writing: describe melting points and boiling points of covalent substances. (1)
  • Covalent: Bonding between two non metals. (1)
  • Graphite: each carbon atom is only covalently bonded to three other carbon atoms, rather than to four as in diamond. Graphite contains layers of carbon atoms. The layers slide over each other easily because there are only weak forces between them, making graphite slippery. (1)
  • Fullerenes: The fullerenes are a large class of allotropes of carbon and are made of balls, 'cages' or tubes of carbon atoms. Buckminster fullerene is one type of fullerene. (1)
  • Diamond: Diamond has a giant molecular structure. Each carbon atom is covalently bonded to four other carbon atoms. (1)
Memory Anchor:
Method Precise Learning Objective Linked Question / Activity
(Designed for maximum working out)		 Stepping Stones Pitstop Check
(Thinking Map)
Substances that consist of giant covalent structures are solids with very high melting points. Diamond, graphite and fullerenes are all examples of what type of structure?

Jigsaw research the four different types of covalent structure. Compare ready made 3D examples of giant covalent structures. EW: Why is a split ring commutator made out of Graphite. GF: Why would Fullerenes be used in drug delivery rather than graphite?
In diamond, each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, so diamond is very hard, has a very high melting point and does not conduct electricity. How many bonds can an individual atom of carbon form? How many bonds does each carbon form in an atom of a) Diamond b) Graphite
All of the atoms in these structures are linked to other atoms by strong covalent bonds. Molecules of diamond, graphite and fullerenes are all held together by what type of bonds?
Diamond and graphite (forms of carbon) and silicon dioxide (silica) are examples of giant covalent structures. Which giant covalent structures are made only from carbon?
Students should be able to recognise giant covalent structures from diagrams showing their bonding and structure.

The first fullerene to be discovered was Buckminsterfullerene (C60) which has a spherical shape. What was the first fullerene to be discovered and what is its shape?
Links To the Big Ideas
ForcesParticlesEnergyCells