🧪 GCSE Biology Revision Newsletter - Graphite

Part 1 - Keywords:

• Graphite

• Giant Covalent Structure

• Carbon Atoms

• Covalent Bonds

• Delocalised Electrons

• Hexagonal Layers

• Weak Forces

• Conductivity

• Lubricant

• Electrodes

Part 2 - Key Facts:

• Graphite is a form of carbon with a giant covalent structure in which each carbon atom bonds with three others, creating layers of hexagonal rings.

• Each carbon atom has one delocalised electron that is free to move, allowing graphite to conduct electricity.

• The layers of graphite are held together by weak forces (Van der Waals forces), meaning they can slide over each other easily.

• This slippery nature makes graphite an effective lubricant in various applications.

• Graphite’s electrical conductivity also makes it useful for electrodes in batteries and for electrolysis processes.

• Despite being a non-metal, graphite’s structure gives it metallic properties, like conductivity.

Part 3 - Quick Quiz:

1. How many covalent bonds does each carbon atom form in graphite?

   • A) 2

   • B) 3

   • C) 4

2. Why can graphite conduct electricity?

   • A) It has delocalised electrons

   • B) It contains metal atoms

   • C) The layers are strongly bonded

3. What property of graphite makes it useful as a lubricant?

   • A) Its hardness

   • B) Its slippery layers

   • C) Its high melting point

Answers:

1. B

2. A

3. B

Part 4 - Going Further:

Question: Explain how the structure of graphite allows it to conduct electricity, and why this is unusual for a non-metal.

Answer: Graphite can conduct electricity due to the presence of delocalised electrons that are free to move between its layers. In each layer, each carbon atom is bonded to three others, leaving one electron per atom free. These free electrons can move across the structure, carrying electric current. This property is unusual for non-metals, as they typically lack free-moving electrons; however, graphite’s structure provides metallic-like conductivity.

Part 5 - Revision Tips:

To remember graphite’s unique properties, compare it with diamond—a different form of carbon. Consider how graphite’s layered structure gives it conductivity and slipperiness, unlike diamond.

Part 6 - More Help:

• BBC Bitesize - Graphite
  URL: BBC Bitesize Graphite Revision
  Description: This page covers the structure and properties of graphite, highlighting its unique layers and why it's both conductive and slippery. Interactive elements, summaries, and quizzes are available to help reinforce understanding​

• Save My Exams - Graphite Structure
  URL: Save My Exams Graphite Structure
  Description: A detailed revision guide explaining graphite’s covalent bonds, its electrical conductivity, and industrial uses, making it ideal for reviewing key concepts and properties related to GCSE Chemistry​

• YouTube Video - GCSE Chemistry Revision: Graphite
  URL: GCSE Chemistry Revision: Graphite - YouTube
  Description: This video provides a visual explanation of graphite’s molecular structure and properties, breaking down how its unique characteristics make it both soft and conductive—perfect for GCSE revision​

Part 7 - GCSE Science Flik Notes

If you are on mobile hold your finger over the image and click ‘save as’ or make it full screen and take a screen shot. You can then have these notes saved on your phone at all times.

See you next time for more GCSE Science revision support!