daimond is the nonconductor of electricity but graphite is the conductor of electricity why?
Answers
Explanation:
Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. ... However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.
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Answer:
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Explanation:
Diamond has 3D carbon network so the structure is rigid with carbon bonded to four other carbon in space.
This is the reason that diamond is hardest substance known. Since all the four carbon atoms are involved in bonding and there is no free electron in the crystal structure of diamond. Therefore diamond is non-conductor of electricity.
Graphite has two dimensional sheet like structure. Each carbon atom is covalently bonded to three other carbon atom and fourth electron is forms a π bond. The various layers are held together by weak van der Waals forces of atoms. This is the reason graphite has soft and slippery structure. The electrons are de-localised over the whole sheet and they are mobile. Therefore graphite is a good conductor of electricity.