Graphite

• What is the structure of graphite?

  Graphite is a giant covalent molecule.
• What should you be able to describe by the end of the video?

  You should be able to describe the structure and properties of graphite and link these properties to its structure.
• What is the main element that forms diamond?

  Carbon.
• How many covalent bonds does each carbon atom in diamond form?

  Each carbon atom forms covalent bonds to four other carbon atoms.
• Why is diamond considered a very hard substance?

  Because it has a large number of strong covalent bonds.
• What is required to melt diamond?

  You have to break all of the strong covalent bonds, which requires a great deal of energy.
• What is the melting and boiling point of diamond?

  Diamond has a very high melting and boiling point.
• Why can't diamond conduct electricity?

  Because all of the outer electrons are in covalent bonds, leaving no free electrons to carry electrical charge.
• What is the structure of graphite in terms of carbon atoms?

  Each carbon atom forms covalent bonds to three other carbon atoms.
• What shape do the carbon atoms form in graphite?

  The carbon atoms form hexagonal rings.
• How are the hexagonal rings of carbon atoms arranged in graphite?

  The hexagonal rings are arranged into layers with no covalent bonds between the layers.
• Why is graphite considered soft and slippery?

  Because the layers can slide over each other due to the absence of covalent bonds between them.
• How is graphite used in machines?

  Graphite is often used as a lubricant to reduce friction between moving parts.
• What is the melting point of graphite related to?

  It is related to the large number of strong covalent bonds that need to be broken.
• What allows graphite to conduct electricity and heat?

  The presence of delocalized electrons that can move freely.
• What are delocalized electrons?

  Electrons that are released from carbon atoms and can move freely.
• How does graphite compare to metals in terms of conductivity?

  Graphite is similar to metals because both have delocalized electrons that can move and conduct electricity and heat.
• What is the main element that graphite is formed from?

  Carbon.
• Why is graphite not considered a metal?

  Because graphite is formed from the element carbon, not from metallic elements.
• What are the key properties of graphite?

  • Soft and slippery
  • Very high melting and boiling point
  • Good conductor of electricity and heat
• How does the structure of graphite explain its properties?

  • Hexagonal rings of carbon atoms form layers
  • No covalent bonds between layers allow sliding (softness)
  • Delocalized electrons allow conductivity (electricity and heat)