Giant Covalent Structures - Diamond
Chemistry: Cambridge International GCSE Supplement, topic 2.6.2
Diamond
Diamond is an allotrope (form) of carbon. Diamond has the following properties:
Covalent bonds
- Each carbon atom in diamond is bonded to 4 other carbon atoms by strong covalent bonds.
- This creates a giant covalent structure.
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 not conduct electricity
- Diamond does not conduct electricity because there are no delocalised electrons in the diamond structure.
High melting point
- A lot of energy is needed to break strong covalent bonds.
- Diamond has lots of strong covalent bonds. This means that it has a high melting point.
Test yourself on Giant Covalent Structures - Diamond
Why is diamond used as a cutting tool?
Properties of diamond
Why does diamond not conduct electricity?