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Diamond structure (AQA GCSE Chemistry)
Revision Note
Structure of a diamond
- Diamond and graphite are allotropes of carbon
- Both substances contain only carbon atoms but due to the differences in bonding arrangements they are physically completely different
- In diamond, each carbon atom bonds with four other carbons, forming a tetrahedron
- All the covalent bonds are identical, very strong and there are no intermolecular forces
Diagram showing the structure and bonding arrangement in diamond
Examiner Tip
You should be able to relate the physical properties of diamond to its bonding arrangement and structure.
Properties of Diamond
- Diamond does not conduct electricity
- All the outer shell electrons in carbon are held in the four covalent bonds around each carbon atom
- As a result, there are no freely moving particles to carry a charge
- Diamond has a very high melting point
- Diamond has a giant covalent structure
- There are strong covalent bonds between the carbon atoms
- These need lots of energy to break
- It is extremely hard and dense
- It has strong covalent bonds and each carbon atom is bonded to four other carbon atoms
- Diamond's hardness makes it very useful in cutting tools like drills
Examiner Tip
Diamond is the hardest naturally occuring mineral, but it is by no means the strongest. Students often confuse hard with strong, thinking it is the opposites of weak. Diamonds are hard, but brittle - that is, they can be smashed fairly easily with a hammer. The opposite of saying a material is hard is to describe it as soft.
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