Structures of Carbon
- Created by: Lucy Rennie
- Created on: 28-03-19 16:04
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- Structures of Carbon
- Fullerenes
- Fullerenes have a covalent molecular structure as they have a fixed number of atoms per molecule
- The number of carbons can range from 50 to 540 carbons per molecule
- As the molecules are large fullerenes and nanotubes are solid, the melting and boiling points are low
- Fullerenes have a carbon cage structure made up of rings of 5 and 6 carbons
- They also contain football shaped molecules and molecules known as nanotubes
- A Fullerene C60 is known as a Buckminster Fullerene
- Fullerenes contain double bonds and so can decolourise bromine solution in an addition reaction
- Fullerenes have delocalised electrons and so can not usually conduct electricity
- Fullerenes can however conduct electricity when exposed to certain wavelengths of light and so can be known as semi-conductors
- Fullerenes have a covalent molecular structure as they have a fixed number of atoms per molecule
- Diamond
- Diamond has a covalent network structure as they do not have a fixed number of atoms bonded together
- In diamond, strong covalent bonds are formed in all three dimensions, creating a tetrahedral structure
- During melting, the strong covalent bonds must be broken, therefore diamond has a very high melting and boiling point
- Diamond is very strong because of it's three dimensional network, and can only be broken by diamond
- Graphite
- Graphite consists of layers of covalent networks held together by weak intermolecular forces
- These weak intermolecular forces are easily broken
- This results in strong covalent bonds within the layers and London Dispersion Forces between the layers
- Each layer of covalent network contributes an electron to a pool between the layers
- These electrons are delocalised and so allow graphite to conduct electricity
- Graphite consists of layers of covalent networks held together by weak intermolecular forces
- Fullerenes
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