Diamond and Graphite

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

  Diamond and graphite
• What is an allotrope?

  Different structural forms of the same element
• In what physical state are carbon allotropes found?

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

  Giant covalent structures
• How are diamond and graphite similar in terms of atomic bonding?

  Both are made of covalently bonded atoms
• How many carbon atoms is each carbon atom in diamond bonded to?

  Four other carbon atoms
• What is the arrangement of carbon atoms in diamond?

  Regular 3D pattern
• Why is diamond very strong?

  It has strong covalent bonds
• Does diamond conduct electricity?

  No, it has no free electrons
• How many carbon atoms is each carbon atom in graphite bonded to?

  Three other carbon atoms
• What shape do the carbon atoms form in graphite?

  Hexagons
• How are the layers in graphite held together?

  Weakly, with no covalent bonds
• What property of graphite allows it to be relatively soft?

  Layers can slide over one another
• Does graphite have a high melting point?

  Yes, it has a very high melting point
• What happens to the spare electron in graphite?

  It becomes delocalized
• What does delocalized mean in the context of graphite?

  Free to move around
• What property do the delocalized electrons in graphite provide?

  Ability to conduct electricity and heat
• What is a single layer of graphite called?

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

  Make other structures like spheres and tubes
• What are the key differences between diamond and graphite?

  • Diamond:
  • Each carbon bonded to four others
  • Strong 3D structure
  • Does not conduct electricity
  • Very high melting point
  • Graphite:
  • Each carbon bonded to three others
  • Forms hexagonal layers
  • Conducts electricity due to delocalized electrons
  • High melting point but softer
• What are the properties of giant covalent structures like diamond and graphite?

  • Strong covalent bonds
  • High melting points
  • Hardness varies (diamond is hard, graphite is soft)
  • Conductivity varies (diamond does not conduct, graphite does)