Gaint covalent structures

• What are the two forms of carbon discussed?

  Diamond and graphite
• What type of structure do diamond and graphite have?

  Giant structures of carbon atoms
• How are the structures of diamond and graphite different?

  Their structures lead to different properties
• What type of structure is diamond classified as?

  Giant covalent structure
• How many carbon atoms is each diamond carbon atom joined to?

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

  Regular tetrahedral network structure
• Does diamond have free electrons?

  No, there are no free electrons
• Why is diamond very hard?

  Due to its rigid network of carbon atoms
• What are some uses of diamond due to its hardness?

  Cutting tools like glass cutters
• What is the melting point characteristic of diamond?

  Very high melting point
• Does diamond conduct electricity?

  No, it does not conduct electricity
• What type of structure does graphite have?

  Giant covalent structure
• How many covalent bonds does each carbon atom in graphite form?

  Three covalent bonds
• What is the arrangement of carbon atoms in graphite?

  Layers of hexagonal rings
• Are there covalent bonds between the layers in graphite?

  No, there are no covalent bonds
• What type of electron is present in graphite?

  One non-bonded delocalised electron
• Why can graphite conduct electricity?

  Due to delocalised electrons moving freely
• What are some uses of graphite due to its electrical conductivity?

  Electrodes in batteries and electrolysis
• What makes graphite slippery?

  Weak forces between the layers
• What is a common use of graphite as a lubricant?

  In machinery and engines
• What is graphene?

  A single layer of graphite
• What are the properties of graphene due to its structure?

  Very high melting point and strength
• How does graphene conduct electricity?

  Due to delocalised electrons moving freely
• What are some uses of graphene in technology?

  Electronics and making composites
• What are giant covalent structures?

  • Large number of atoms joined by covalent bonds
  • Not molecules; number of atoms is variable
  • Form a giant lattice or network structure
  • Examples: diamond, graphite, silicon dioxide
• How do giant covalent structures differ from simple covalent molecules?

  • Giant covalent structures: large, variable number of atoms
  • Simple covalent molecules: small, fixed number of atoms
  • Both held by strong covalent bonds
• What are the properties of giant covalent structures?

  • High melting and boiling points
  • Insoluble in water and solvents
  • Very hard due to rigid network
  • Most do not conduct electricity, except graphite and graphene