CBSE Class 10 Answered
Diamond |
Graphite |
Buckminster fullerene |
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In diamond the carbon atoms are covalently bonded to one another producing a three dimensional network solid.
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Graphite is also made of carbon atoms. Graphite consists of carbon atoms covalently bonded together in a layers made up of hexagons, like chicken wire. |
Buckminsterfullerene (Bucky ball) is an allotrope of carbon that is produced by firing high powered laser beams at graphite. |
Each carbon atom is bonded to four other atoms throughout the crystal lattice. |
Each carbon atom has three bonds and one free electron. |
Each molecule consists of a large number of carbon atoms covalently bonded to one another forming a sphere (similar to a soccer ball). |
Diamond has no free electrons because they are all involved in bonding and is therefore a poor conductor of electricity.
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The extra electrons are delocalised and can be moved along the layers by applying an external voltage. This is why graphite can conduct an electric current. |
They are extremely stable in nature.
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Diamond is the hardest substance known and is used to cut glass and in industrial drill bits. |
Graphite unlike diamond is extremely soft. |
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Diamond is widely sought after because of its rarity and unique cystalline structure and is used in jewellery. |
The parallel layers of graphite are weak intermolecular bonds, which allow the layers to easily slip over each other. This is what happens when writing or drawing with a graphite pencil on paper. |
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