Carbon

• In diamond, how many other carbon atoms is each carbon joined to covalently?

  4
• What are the physical properties of diamond?

  It is very hard, has a very high melting point, and does not conduct electricity.
• In graphite, how many other carbon atoms is each carbon bonded to covalently?

  3
• What structure do the carbon atoms form in graphite?

  Layers of hexagonal rings.
• Why can the layers in graphite slide over each other?

  Because there are no covalent bonds between the layers, only weak intermolecular forces.
• What does the delocalisation of electrons in graphite allow it to do?

  It allows graphite to conduct electricity.
• What is graphene?

  A single layer of graphite.
• What are the properties of graphene that make it useful in electronics and composites?

  It is very strong and elastic.
• What is the first fullerene to be discovered?

  Buckminsterfullerene (C60).
• What is the shape of Buckminsterfullerene (C60)?

  It has a spherical shape.
• What are carbon nanotubes?

  Cylindrical fullerenes with very high length to diameter ratios.
• What makes carbon nanotubes useful?

  Their properties make them useful for nanotechnology, electronics, and materials.
• What are some examples of uses for carbon nanotubes?

  • Lubricants
  • Drug delivery in the body
  • Catalysts
  • Reinforcing materials (e.g., tennis rackets)
• What type of bonds exist between the layers of graphite?

  No covalent bonds, only weak intermolecular forces.
• How does the structure of graphite contribute to its softness?

  The lack of covalent bonds between layers allows them to slide easily.
• How does the delocalisation of electrons in graphite compare to metals?

  Graphite has delocalised electrons similar to metals, allowing it to conduct electricity.
• What is the significance of the hexagonal rings in fullerenes?

  They form the basis of the structure of fullerenes, which may also include rings with five or seven carbon atoms.