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Questions 6.1(b)

  1. In what way is the structure of graphite similar to that of metals?

  2. In what way does the structure of graphite differ from that of metals?

  3. From the structure of graphite, suggest a reason why it is slippery.

  4. From the structure, explain why graphite conducts electricity.

  5. Graphite is much softer than diamond. Explain this from the structures.

  6. Graphite combines the properties of giant atomic and giant molecular structures. True or false? Explain your answer.




Answers to Questions 6.1(b)

  1. Graphite structure has mobile electrons (marked – in the diagram).
  2. Graphite structure has Van der Waal’s forces of attraction.
  3. The atoms in graphite are arranged in loose layers that can easily slip over one another.
  4. Graphite structure has a mobile electrons which have not taken part in covalent bonding.
  5. Graphite structure has Van der Waal’s forces which are weak sites that allow breakage. But diamond has a giant atomic structure.
  6. True. The layers (hexagonal) of atoms consist of very large numbers of atoms bonded together, which is an aspect of giant atomic structures. But it also has Van der Waal’s forces, which is an aspect of molecular structures.