Allotropes of Carbon

• What are allotropes of carbon?


  Different structural forms of the same element in the same physical state
• What are the key properties of diamond?

  • Giant covalent structure
  • Each carbon forms four covalent bonds
  • Very hard
  • High melting point due to strong covalent bonds
  • Does not conduct electricity (no free electrons or ions)
• Why does diamond have a very high melting point?


  Because the strong covalent bonds take a lot of energy to break
• Why does diamond not conduct electricity?


  It has no free electrons or ions
• What are the characteristics of graphite?


  • Each carbon atom forms three covalent bonds
  • Arranged in sheets of hexagons
  • Weak bonds between layers allow them to move over each other
  • Soft and slippery, ideal for lubrication
  • High melting point due to strong covalent bonds
  • Conducts electricity and thermal energy due to delocalised electrons
• What structure do carbon atoms form in graphite?


  Sheets of carbon atoms arranged in hexagons
• How does the structure of graphite contribute to its lubricating properties?

  The weak bonds between layers allow them to slide over each other easily
• What allows graphite to conduct electricity?

  The presence of delocalised electrons
• What is graphene and its properties?


  • A sheet of carbon atoms joined in hexagons
  • One atom thick (two-dimensional)
  • Very strong due to covalent bonds
  • Incredibly light, useful in composite materials
  • Contains delocalised electrons, conducts electricity
• What is the thickness of graphene?


  One atom thick
• What are the applications of fullerenes?


  • Molecules shaped like closed tubes or hollow balls
  • Can cage other molecules for drug delivery
  • Huge surface area for industrial catalysts
  • Great lubricants
• What shapes can fullerenes take?


  Closed tubes or hollow balls
• How do fullerenes assist in drug delivery?


  They can cage other molecules, trapping them inside
• What are the properties of nanotubes?


  • Tiny carbon cylinders
  • High length-to-diameter ratio
  • Conduct electricity and thermal energy
  • High tensile strength (do not break when stretched)
• What is nanotechnology?


  Technology that uses very small particles such as nanotubes
• How can nanotubes be used in materials?


  To strengthen materials without adding much weight
• What is the potential use of graphene in electronics?


  It can conduct electricity through the whole structure
• What are the two allotropes of carbon mentioned in the study material?


  Diamond and Graphite
• What is the bonding structure of carbon atoms in diamond?


  Each carbon atom is bonded to 4 other carbon atoms.
• Why is diamond considered strong?

  Because a large amount of energy is required to break its bonds.
• Why does diamond not conduct electricity?

  Because it has no free electrons or ions.
• What are the properties of graphite mentioned in the study material?


  Graphite is soft, has a high melting point, and conducts electricity.
• How are carbon atoms arranged in graphite?


  Each carbon atom is bonded to 3 other carbon atoms in a hexagonal arrangement.
• What allows graphite to conduct electricity?


  Delocalized electrons that are free to move around.
• What is graphene?


  A single layer of graphite consisting of carbon atoms arranged in flat hexagons.
• What are fullerenes?


  Allotropes of carbon that have hollow shapes, such as tubes and spheres.
• How can fullerenes be used in medicine?


  They can deliver drugs to specific areas of the body.
• Why are fullerenes useful as industrial catalysts?


  They have a large surface area to volume ratio.
• What are carbon nanotubes used for?


  They are used in nanotechnology and electronics due to their ability to conduct electricity.
• How do fullerenes strengthen other materials?


  They add strength without adding significant weight.
• What is the Buckminster fullerene?


  It is the first sphere to be discovered made with 60 carbon atoms (C60).
• What is the arrangement of carbon atoms in graphene?


  Carbon atoms are arranged into flat hexagons.
• What are the key properties of diamond and graphite?

  Diamond:

  • Strong
  • High melting point
  • Does not conduct electricity

  
  

  Graphite:

  • Soft
  • High melting point
  • Conducts electricity
• What are the differences between graphene, graphite, and fullerenes?

  Graphene:

  • Single layer of carbon atoms in hexagons

  
  

  Graphite:

  • Multiple layers of carbon atoms
  • Soft and conducts electricity

  
  

  Fullerenes:

  • Hollow shapes (tubes and spheres)
  • Used in medicine and as catalysts