Graphite, Graphene, Fullerene and Polymers

• Graphite properties:

  • High melting and boiling point
  • Soft and slippery
  • Excellent conductor of electricity and heat
• Graphite formation:

  • Formed from the element Carbon
  • Each Carbon atom forms Three covalent bonds
  • Carbon atoms in graphite form Hexagonal rings
• Reasons for high melting and boiling points of graphite:

  • Strong covalent bonds require a lot of energy to break
• Structure of graphite:

  • Hexagonal rings arranged in layers
  • No covalent bonds between layers, allowing them to slide and make graphite slippery
• Delocalised electrons in graphite:

  • Each Carbon atom has a single electron in its outer shell not in a covalent bond
  • These electrons are released and called delocalised electrons
  • Delocalised electrons can move, allowing graphite to conduct thermal energy and electricity
• Graphene:

  • Single layer of Graphite
  • One atom thick
  • Excellent conductor of electricity due to delocalised electrons
  • Extremely strong
• Fullerenes:

  • Molecules of Carbon atoms with hollow shapes
  • Have hexagonal rings of Carbon atoms
  • Uses include pharmaceutical delivery, lubricants, and catalysts
• Carbon nanotubes:

  • High tensile strength, can be stretched without breaking
  • Excellent conductors of heat and electricity
  • Used to reinforce materials
• Polymers:

  • Made by joining thousands of small, identical molecules (monomers)
  • Monomers are often alkene molecules
  • Most polymers are solids at room temperature
  • Have intermolecular forces of attraction between polymer molecules, which are relatively strong
  • High melting and boiling points due to strong intermolecular forces