Graphite

• What is the structure of graphite?

  Graphite is a giant covalent molecule formed from carbon atoms arranged in hexagonal rings.
• How does the structure of graphite relate to its properties?

  Graphite's layered structure allows it to be soft and slippery, while strong covalent bonds give it a high melting and boiling point.
• What is the process of melting graphite?

  • Break covalent bonds between carbon atoms
  • Requires a great deal of energy
• Why can't diamond conduct electricity?

  Diamond cannot conduct electricity because all outer electrons are involved in covalent bonds, leaving no free electrons to carry charge.
• What are the key properties of graphite?

  Graphite is soft and slippery, has a high melting and boiling point, and is a good conductor of electricity and heat.
• How does the structure of graphite contribute to its use as a lubricant?

  • Layers can slide over each other
  • Reduces friction between moving parts
• How does the bonding in graphite differ from that in diamond?

  Graphite has carbon atoms bonded to three others, while diamond has carbon atoms bonded to four others.
• What are delocalized electrons in graphite?

  Delocalized electrons are free-moving electrons that allow graphite to conduct electricity and heat.
• How does graphite's conductivity compare to that of metals?

  Graphite and metals both conduct electricity and heat due to delocalized electrons, but graphite is not a metal.
• What is the significance of graphite's high melting and boiling points?

  • Indicates strong covalent bonds
  • Requires a lot of energy to break bonds