Structure and bonding of carbon

• How many other carbon atoms is each carbon in diamond covalently bonded to?

  4
• What are the physical properties of diamond?

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

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

  Layers of hexagonal rings with no covalent bonds between the layers.
• Why can the layers in graphite slide over each other?

  Because there are no covalent bonds between the layers, only weak intermolecular forces.
• What makes graphite soft and slippery?

  The ability of the layers to slide over each other due to weak intermolecular forces.
• What happens to one electron from each carbon atom in graphite?

  It is delocalised.
• How does the delocalisation of electrons in graphite affect its properties?

  It makes graphite similar to metals and allows it to conduct electricity.
• What is graphene?

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

  It is very strong and elastic due to tightly bonded atoms and flexible planes.
• What are fullerenes?

  Molecules of carbon atoms with hollow shapes.
• What is the structure of fullerenes based on?

  Hexagonal rings of carbon atoms, which may also contain rings with five or seven carbon atoms.
• What is the first fullerene to be discovered?

  Buckminsterfullerene (C60).
• What shape does Buckminsterfullerene (C60) have?

  A spherical shape.
• What are carbon nanotubes?

  Cylindrical fullerenes with very high length to diameter ratios.
• Why are 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)