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7 GCSE Allotropes of Carbon
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Revision notes:
Section 1: Allotropes of Carbon (Diamond and Graphite)
Allotropes are structures of the same element but in different structural forms. For example, carbon has 4 allotropes that you need to recall.
Diamond:
In diamond, each carbon is bonded together with 4 other carbon atoms. It forms a rigid structures, and explains why diamond is hard. It has a high melting and boiling point because of the strong covalent bonds requiring lots of energy to break, and it does not conduct electricity because there are no free electrons or ions.
Graphite:
Graphite is different to carbon because in graphite, each carbon is only bonded to 3 other carbon atoms. This leaves 1 electron free, which has a charge and can move, and therefore explains why graphite can conduct electricity.
Graphene:
Graphene is a single layer of graphite. Therefore, each carbon is only bonded to 3 other carbon atoms. This leaves 1 electron free, which has a charge and can move, and therefore explains why graphite can conduct electricity.
Because it’s only one layer, it’s very light and strong.
Uses of graphene are: Electronics: very effective conductor of electricity due to free electrons. Very strong so useful in advanced materials (composites)
Graphite forms sheets that form layers. These layers are held together by weak intermolecular forces, so the layers can move over each other. This explains why graphite is soft and slippery. Finally, it is held together by strong covalent bonds, which require a lot of energy to break. This explains why graphite has a high melting and boiling point.
Fullerenes
Fullerenes are hollow cages of carbon atoms. An example is nanotubes, which are hollow tubes of carbon atoms. They have high melting and boiling points, due to the strong covalent bonds and do not conduct electricity, due to no free electrons or ions.
Uses: Drug delivery for medical applications Lubricants (weak forces between cages so easy for cages to slip over each other). Catalysts
Uses of nanotubes: High tensile strength so can be used in composite materials e.g. tennis rackets. High electrical conductivity
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Revision notes:
Section 1: Allotropes of Carbon (Diamond and Graphite)
Allotropes are structures of the same element but in different structural forms. For example, carbon has 4 allotropes that you need to recall.
Diamond:
In diamond, each carbon is bonded together with 4 other carbon atoms. It forms a rigid structures, and explains why diamond is hard. It has a high melting and boiling point because of the strong covalent bonds requiring lots of energy to break, and it does not conduct electricity because there are no free electrons or ions.
Graphite:
Graphite is different to carbon because in graphite, each carbon is only bonded to 3 other carbon atoms. This leaves 1 electron free, which has a charge and can move, and therefore explains why graphite can conduct electricity.
Graphene:
Graphene is a single layer of graphite. Therefore, each carbon is only bonded to 3 other carbon atoms. This leaves 1 electron free, which has a charge and can move, and therefore explains why graphite can conduct electricity.
Because it’s only one layer, it’s very light and strong.
Uses of graphene are: Electronics: very effective conductor of electricity due to free electrons. Very strong so useful in advanced materials (composites)
Graphite forms sheets that form layers. These layers are held together by weak intermolecular forces, so the layers can move over each other. This explains why graphite is soft and slippery. Finally, it is held together by strong covalent bonds, which require a lot of energy to break. This explains why graphite has a high melting and boiling point.
Fullerenes
Fullerenes are hollow cages of carbon atoms. An example is nanotubes, which are hollow tubes of carbon atoms. They have high melting and boiling points, due to the strong covalent bonds and do not conduct electricity, due to no free electrons or ions.
Uses: Drug delivery for medical applications Lubricants (weak forces between cages so easy for cages to slip over each other). Catalysts
Uses of nanotubes: High tensile strength so can be used in composite materials e.g. tennis rackets. High electrical conductivity
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