Allotropes diamond and graphite

• What are the two allotropes of carbon discussed in today's video?

  Diamond and graphite
• What are allotropes?


  Allotropes are different structural forms of the same element in the same physical state.
• In what physical state can carbon take different allotropes?

  Solid state
• What type of structure do both diamond and graphite have?

  Both diamond and graphite are giant covalent structures.
• How are the atoms arranged in diamond?

  In diamond, each carbon atom is covalently bonded to four other carbon atoms in a regular 3D pattern.
• Why is diamond very strong and has a high melting point?

  Because it has strong covalent bonds that require a lot of energy to break.
• Why doesn't diamond conduct electricity?

  Because it has no free electrons or ions that can move around.
• How does the bonding in graphite differ from that in diamond?

  In graphite, each carbon atom is bonded to only three other carbon atoms.
• What is the arrangement of atoms in graphite?

  The atoms in graphite are arranged into hexagons that form large flat sheets.
• Why is graphite relatively soft compared to diamond?

  Because the individual layers in graphite are held together weakly and can slide over one another.
• What allows graphite to conduct electricity and heat?

  The presence of delocalized electrons that are free to move around.
• What is a single layer of graphite called?

  Graphene
• What can scientists do with isolated layers of graphene?

  They can use them to make other structures such as spheres and tubes.
• What are the key differences between diamond and graphite?

  • Diamond:
  • Each carbon bonded to four others
  • Strong 3D structure
  • Very hard, high melting point
  • Does not conduct electricity

  
  

  • Graphite:
  • Each carbon bonded to three others
  • Arranged in hexagons forming layers
  • Relatively soft, high melting point
  • Conducts electricity due to delocalized electrons
• What are the allotropes of carbon mentioned in the video?

  • Diamond
  • Graphite
  • Graphene (single layer of graphite)
  • Fullerenes (to be discussed in the next video)