Why does graphite conduct electricity, but not diamond?

Question

Answer

Carbon atom has 4 electrons in it. Now,  in graphite crystal, each carbon atom is joined to only three other carbon atoms by covalent bonds. Thus, only three valence electrons of each carbon atom in graphite are used in bond formation. The fourth valence electrons of each carbon atom is free to move. Due to the presence of free electrons in a graphite crystal it conducts electricity.......nd in the case of diamond each carbon atom is linked to four other carbon atoms by covalent bonds and hence all the four valence electrons of each carbon atom are used up in forming the bonds. since there is no free electrons in the diamond crystal, so it does not conduct electricity.....

Answer

Graphite contains layers of carbon atoms. The layers slide over each other easily because there are only weak forces between them, making graphite slippery. These electrons can move through the graphite, carrying charge from place to place and allowing graphite to conduct electricity.and diamond can't conduct electricity Because they have a tetrahedron structure made by covalent bonds between carbon atoms. The crystal structure has no free electrons that can flow or travel between potential differences. Hence, no electricity (or little electricity) passes through diamond crystals which makes them poor conductors of electricity

Answer

Conductivity in Graphite vs. Diamond
Graphite and diamond are both forms of carbon but exhibit vastly different electrical properties. The difference in their conductivity can be attributed to their unique structural arrangements and bonding.
Structure of Graphite
- Graphite has a layered structure where carbon atoms are arranged in flat planes.
- Each carbon atom is bonded to three others, creating a hexagonal lattice.
- The fourth outer-shell electron of each carbon atom is free to move, forming delocalized pi bonds.
Electron Mobility
- The delocalized electrons in graphite can move freely between the layers.
- This mobility allows graphite to conduct electricity efficiently, as electrons can flow easily when an electric field is applied.
Structure of Diamond
- Diamond has a tetrahedral structure where each carbon atom is bonded to four others in a 3D arrangement.
- All four outer-shell electrons of each carbon atom are involved in strong covalent bonding, leaving no free electrons available.
Lack of Free Electrons
- The absence of free electrons in diamond means there are no charge carriers to facilitate electrical conduction.
- As a result, diamond is an excellent electrical insulator, despite being a good conductor of heat.
Conclusion
- The key difference lies in the availability of delocalized electrons in graphite versus the tightly bound electrons in diamond.
- This fundamental distinction in structure and bonding accounts for graphite's conductivity and diamond's insulating properties.

Answer

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