Why graphite is a good conductor of electricity where as diamond is not ?
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Answer:
Graphite has carbon atoms covalently bonded in planes. There are four possible bonding points but only three are occupied so the fourth electron is free to wander through the plane. However, it will not conduct perpendicular to that plane.
Diamond has a tetrahedral covalent bond structure in three dimensions. So all of the four bonding sites are occupied and there are no free electrons to conduct electricity.
Oddly, diamond does have a high thermal conductivity, which is not usually the case for insulators. Ordinarily, thermal and electrical conductivity go together. This can be attributed to the high strength of those covalent bonds, enhancing the ability to conduct heat by vibrations in the crystal lattice.
Explanation:
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Answer:
In a graphite molecule, one valence electron of each carbon atom remains free, Thus making graphite a good conductor of electricity. Whereas in diamond, they have no free mobile electron. Hence there won't be flow of electrons That is the reason behind diamond are bad conductor electricity..
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