Free Science Lessons: Graphite Structure and Properties

Introduction

• Focus of video: Understanding the structure of graphite, its properties, and how they relate to its structure.
• Comparison with diamond, another form of carbon.

Diamond (Recap)

• Diamond is a giant covalent molecule.
• Carbon atoms in diamond form covalent bonds with four other carbon atoms.
• Properties of Diamond:
  • Very hard due to strong covalent bonds.
  • High melting and boiling point because breaking covalent bonds requires a lot of energy.
  • Does not conduct electricity as all electrons are involved in covalent bonds.

Graphite

Structure

• Graphite is also a giant covalent structure.
• Each carbon atom forms covalent bonds with three other carbon atoms.
• Carbon atoms form hexagonal rings.
• Rings are arranged in layers.
• No covalent bonds between layers, allowing them to slide over each other.

Properties

• Soft and Slippery
  • Due to layers sliding over each other.
  • Used as a lubricant in machines.
• High Melting and Boiling Point
  • Requires breaking many strong covalent bonds.
• Conducts Electricity and Heat
  • Contains delocalized electrons from carbon's fourth outer electron.
  • Delocalized electrons allow for conductivity, similar to metals.

Comparison with Metals

• Graphite and metals both have delocalized electrons.
• Both conduct electricity and heat.
• Graphite is not a metal; it is composed of carbon atoms.

Conclusion

• Understanding graphite helps in explaining its practical applications and properties.
• Emphasis on the difference between graphite and metals.
• Availability of further resources and questions in the revision workbook linked.

Additional Resources

• Mention of a vision workbook for practice questions.