Lesson Plan: C1.4.04

Hamble Lesson Observation Plan
Learning About
Why are giant covalent structures useful?
Keywords:
  • Delocalised: Electrons are free to move. (1)
  • Graphite: each carbon atom is only covalently bonded to three other carbon atoms, rather than to four as in diamond. (1)
  • Melting point: The temperature at which a change of state occurs from a solid to a liquid. (1)
  • Metallic bonding is the strong attraction between closely packed positive metal ions and a 'sea' of delocalised electrons. (1)
  • This is why metals have high melting points and boiling points. (1)
  • Metallic bonding: The particles in a metal are held together by metallic bonds. (1)
Memory Anchor:
Method Precise Learning Objective Linked Question / Activity
(Designed for maximum working out)		 Stepping Stones Pitstop Check
(Thinking Map)
Students should be able to explain the properties of diamond in terms of its structure and bonding. Why is diamond so hard, in terms of its structure and bonding?
Metals have giant structures of atoms with strong metallic bonding. This means that most metals have high melting and boiling points. Why do metals tend to have high melting and boiling points?

Create models of metallic structures. Use copper wire and silver nitrate solution to grow silver crystals. Practical: Metals and insulators electrical conduction. Video clips: BBC Bitesize The atomic structure of metals YouTube: What are metallic bonds?
In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between the layers. How many bonds does each carbon atom form in graphite and how does this impact it's structure?
In graphite, one electron from each carbon atom is delocalised. What happens to the spare electron that remains unused in a covalent bond in graphite?
These bonds must be overcome to melt or boil these substances. Why do giant covalent structures have very high melting and boiling points?
Students should be able to explain the properties of graphite in terms of its structure and bonding. Why is graphite soft and slippery?
Students should know that graphite is similar to metals in that it has delocalised electrons. How is graphite similar to metals?
Graphene is a single layer of graphite and has properties that make it useful in electronics and composites. What makes graphene useful in electronics and composites?
Carbon nanotubes are cylindrical fullerenes with very high length to diameter ratios. Their properties make them useful for nanotechnology, electronics and materials. What are the properties of carbon nanotubes and what do their properties make them useful for?
Students should be able to explain the properties of graphene in terms of its structure and bonding. What are the properties of graphene in terms of its structure and bonding?
Students should be able to recognise graphene and fullerenes from diagrams and descriptions of their bonding and structure

Fullerenes are molecules of carbon atoms with hollow shapes. The structure of fullerenes is based on hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms. What are fullerenes and what is their structure?
Students should be able to give examples of the uses of fullerenes, including carbon nanotubes. Name three uses of fullerenes?
Links To the Big Ideas
ForcesParticlesEnergyCells