Diamond Structure (AQA GCSE Chemistry)
Revision Note
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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 Tips and Tricks
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 Tips and Tricks
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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