Why does graphite conduct electricity and diamond does not?

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Eloy Gleichner asked a question: Why does graphite conduct electricity and diamond does not?
Asked By: Eloy Gleichner
Date created: Tue, Jun 15, 2021 4:24 AM
Date updated: Mon, Jul 25, 2022 12:23 AM

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Video answer: Why diamond is non conductor and graphite is conductor

Why diamond is non conductor and graphite is conductor

Top best answers to the question «Why does graphite conduct electricity and diamond does not»

Graphite can conduct electricity because of the delocalised (free) electrons in its structure… However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

  • As graphite is an allotrope of carbon it conducts electricity as it has delocalized electrons. Unlike diamonds they don't have delocalized electrons. So the electrons in their shell become a covalent bond making no electrons free to move so there is no flow of electricity in Diamond.

Video answer: The difference between diamond and graphite, giant covalent structures

The difference between diamond and graphite, giant covalent structures

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Why can graphite conduct electricity but diamond can not? In diamond the carbon atoms are bonded to four other atoms. Whereas, in graphite each carbon atom is only bonded to three other atoms. Therefore, there are delocalised (free) electrons in graphite, which can move and carry a charge so graphite conducts electricty.

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.

Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor. Graphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity.

Why can graphite conduct electricity but diamonds can’t? True, both diamonds and graphite are made from carbon. However, their structures are significantly different. Remember how graphite carbon atoms have a free electron? The same isn’t true for diamond: all four electrons have formed strong single bonds with other atoms.

(a) 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. Thats why diamond are bad conductor electricity. (b) A diamond is a giant molecule. The number of valence electrons in carbon atom is four.

As graphite is an allotrope of carbon it conducts electricity as it has delocalized electrons. Unlike diamonds they don't have delocalized electrons. So the electrons in their shell become a covalent bond making no electrons free to move so there is no flow of electricity in Diamond.

Diamond does not conduct electricity because it has no charged particles that are free to move. Graphite does conduct electricity because it has delocalised electrons which move between the layers.

Although diamond is also an allotrope of carbon, it does not conduct electricity because the four electrons of each carbon atom are localized in pure covalent bonds with the four nearest neighboring atoms.

Why does graphite conduct electricity but not a diamond? Graphite and Diamond both are allotropes of Carbon, yet diamond is a bad electrical conductor and graphite is a good conductor of electricity. The reason behind good electrical conductance of graphite is the delocalization of pi bond electrons above and below the sheets of carbon atoms.

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. Why do diamonds conduct heat?

graphite have a free electron and diamond desnt have free electron

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Video answer: 4.3 comparison of diamond & graphite (solid state)

4.3 comparison of diamond & graphite (solid state)