Carbon Structures - Diamond
Chemistry: AQA GCSE Higher, topic 2.3.11
Diamond
Diamond is an allotrope (form) of carbon. Diamond has the following properties:
Covalent bonds
- Every carbon atom in diamond is bonded to 4 other carbon atoms by strong covalent bonds.
- This creates a giant covalent structure.
Is diamond hard?
- There are lots of strong covalent bonds in diamond. This makes it very hard.
- Because diamond is hard, it is used as a cutting tool to cut other materials.
Does diamond conduct electricity?
- Diamond is NOT an electrical conductor because there are no delocalised electrons in the diamond structure.
What is diamond's melting point?
- A lot of energy is needed to break strong covalent bonds.
- Diamond has lots of strong covalent bonds. This means that diamond has a high melting point.
Test yourself on Carbon Structures - Diamond
Why is diamond used as a cutting tool?
Choose the correct statement about diamond in each pair
Why does diamond not conduct electricity?
Diamond contains many strong covalent bonds between its carbon atoms. How would diamond's hardness change if these bonds were much weaker?
Choose the correct statement about diamond in each pair