Diamond and graphite

• What are the forms of carbon mentioned in the study material?

  Diamond, graphite, and graphene
• What are giant covalent substances?

  • Substances with many atoms joined by covalent bonds
  • Examples include diamond and graphite
• What is the structure of diamond?

  Diamond has a tetrahedral network structure.
• Why is diamond considered the hardest known natural substance?

  Because of its strong covalent bonds in a rigid network.
• Does diamond conduct electricity?

  No, diamond does not conduct electricity.
• What is the melting point of diamond?

  Diamond has a very high melting point.
• What is the bonding structure of graphite?

  Graphite has layers of hexagonal rings with covalent bonds between carbon atoms.
• Why can graphite conduct electricity?

  Because it has delocalised electrons that can move between layers.
• What is a property of graphite that makes it useful as a lubricant?

  Graphite is slippery due to weak forces between its layers.
• What is the difference in electrical conductivity between diamond and graphite?

  Diamond does not conduct electricity, while graphite does conduct electricity.
• How does the structure of diamond contribute to its hardness?

  The tetrahedral network structure with strong covalent bonds makes diamond very hard.
• What are delocalised electrons in graphite?

  Delocalised electrons are electrons that are not associated with a particular atom and can move freely.
• What is the role of electrodes in batteries?

  Electrodes establish electrical contact with a circuit.
• Why are diamond-tipped tools useful?

  Because diamond's hardness allows it to cut through tough materials.
• How do the properties of diamond and graphite differ due to their structures?

  Diamond is hard and does not conduct electricity, while graphite is slippery and conducts electricity.
• What is the significance of the weak forces between layers in graphite?

  They allow the layers to slide over each other, making graphite slippery.
• What is the main reason diamond does not conduct electricity?

  Diamond has no charged particles that are free to move.
• What is the relationship between the structure of diamond and its melting point?

  The strong covalent bonds in diamond contribute to its very high melting point.
• How do the properties of diamond and graphite reflect their different structures?

  Diamond's rigid structure makes it hard and non-conductive, while graphite's layered structure allows it to be slippery and conductive.