Why is diamond an insulator and graphite a conductor

Question

Answer

In diamond each electron is connected to to four other electrons and no free electron is present .In graphite three electrons are connected and the fourth electron is free which is responsible for vonducting electricity.

Answer

In graphite one carbon ayom is connected to three other carbon atoms so that one electron os free but in case of diamond one carbon atom is connected to four carbons atoms so there is no free electrons

Answer

Introduction:

Diamond and graphite are both forms of carbon, but they exhibit different electrical properties. While diamond is an insulator, graphite is a conductor. This difference arises due to the distinct atomic arrangements and bonding structures in the two materials.

Diamond as an insulator:

1. Atomic structure: Diamond consists of a three-dimensional lattice structure, where each carbon atom forms covalent bonds with four neighboring carbon atoms. This creates a tetrahedral arrangement, resulting in a strong and rigid network.

2. Band gap: In diamond, the valence and conduction bands are separated by a large energy gap, known as the band gap. This band gap is around 5.5 electron volts (eV) for diamond, which is a significant amount of energy required to promote electrons to the conduction band.

3. Forbidden energy levels: Due to the band gap, diamond does not have any available energy levels in the band structure for electrons to move freely. Therefore, it cannot conduct electricity as there are no free or mobile charge carriers.

Graphite as a conductor:

1. Atomic structure: Graphite consists of layers of carbon atoms arranged in a hexagonal lattice. Within each layer, carbon atoms are strongly bonded through covalent bonds, similar to diamond. However, between the layers, the carbon atoms are held together by weaker van der Waals forces, allowing them to slide over one another.

2. π-bonds and delocalized electrons: In graphite, each carbon atom forms three covalent bonds, leaving one unhybridized p-orbital empty. These p-orbitals overlap sideways, creating a network of π-bonds above and below the carbon layers. Electrons in these π-bonds are delocalized, meaning they are not confined to a specific atom but are spread over the entire layer.

3. Mobile charge carriers: The delocalized π-electrons in graphite can move freely within the layers. These mobile charge carriers are responsible for its electrical conductivity. Electrons can easily move from one layer to another, making graphite a good conductor of electricity.

Conclusion:

In summary, diamond is an insulator due to its three-dimensional lattice structure, large band gap, and absence of mobile charge carriers. On the other hand, graphite is a conductor because of its layered structure, presence of delocalized π-electrons, and the ability of these electrons to move freely between the layers.

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