Uses of Graphite & Diamonds
Chemistry: Cambridge International GCSE Supplement, topic 2.6.3
Uses of Graphite and Diamond in Giant Covalent Structures
Graphite has a layered structure, having weak forces between layers, with free electrons. Diamond has a rigid 3D structure without free electrons, which makes it hard.
Structure and bonding of graphite
- Graphite has layers of carbon atoms bonded strongly by covalent bonds within each layer.
- Weak forces hold the layers together, allowing them to slide over each other.
- Electrons can move freely within the layers, making graphite conduct electricity.
- The structure relates directly to graphite's useful properties.
Uses of graphite – lubricant
- Graphite's slippery layers reduce friction between moving parts.
- This property makes graphite an excellent dry lubricant in machines.
- The layers slide easily, preventing metal wear and tear.
Uses of graphite – electrode
- Graphite conducts electricity because of mobile electrons between layers.
- Graphite is chemically inert and resists heat, ideal for electrodes in electrolysis.
- Electrodes made from graphite help carry current in cells and furnaces safely.
Structure and bonding of diamond
- Diamond has a giant covalent structure with each carbon atom bonded to four others.
- The bonds are strong and rigid, creating an extremely hard material.
- No free electrons exist, so diamond does not conduct electricity.
- The structure makes diamond ideal for cutting and abrasion uses.
Uses of diamond – cutting tools
- Diamond's hardness allows it to cut or grind hard substances effectively.
- Diamond-tipped tools can cut glass, metal, and stone with precision.
- Diamond's durability ensures tools last longer and perform better than other materials.
Test yourself on Uses of Graphite & Diamonds
What structural feature of graphite allows it to conduct electricity?