Why does graphite conduct electricity and diamond does not?

Answer 1

: Diamond is made up of pure carbon. In the structure of diamond one carbon atom is attached to four other carbon atoms forming a covalent bond. All the electrons of each carbon atom is shared and the octet rule is satisfied. Hence no free electron is left for the conductance of electricity. : In case of graphite the carbon atoms naturally combine covalently with three other carbon atoms so every combined carbon has one unshared or free electron. Now this free electron is responsible for conductance in graphite. : Graphite and metals have free electrons to conduct electricity.

Answer 2

Graphite can conduct electricity because of the delocalised electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. Generally, in diamond, all the 4 outer electrons on each carbon atom are used in covalent bonding, so there are no other delocalised electrons.

Answer 3

Graphite conducts electricity because it has delocalized electrons that are free to move and carry an electric current. In contrast, diamond does not conduct electricity because it has a fully bonded and rigid three-dimensional lattice structure, which does not allow for the movement of electrons.

Answer 4

This is how I understand it: It has to do with the structure of graphite & diamond. Graphite has a layered structure of carbon atoms, one on top of another (kind of like sheets of paper stacked together). To form this structure the carbon atoms have three of its 4 outer electrons bonded with 3 other carbon atoms. The unbonded 4th electrons move freely between the graphite layers. This is why it is able to conduct electricity. The structure of the diamond has all four of its outer electrons bonded to 4 other carbon atoms, so there are no free electrons & thus it is a non-conductor of electricity. Hope this explanation helps.

Answer 5

In the bonding of graphite, the carbon atoms bond to form layers of hexagonal rings. and in each ring, there is one delocalised electron that allows electricity to be conducted. In diamond, the carbon atoms bond to form a tetrahedral, rigid arrangement. This does not allow electricity to be conducted as the electrons in the bonds are not free to move.

Answer 6

Like a metal, graphite is a very good conductor of electricity due to the mobility of the electrons in its outer valence shells. Other allotropes of carbon (like diamond) do not have the same electron mobility, and are not as conductive.

Answer 7

graphite have a free electron and diamond desnt have free electron

Answer 8

Graphite is a good conductor of electricity beacause graphite is sp-2 hybirdize orbit

Answer 9

Why is graphite is not good in diamonds?

Answer 10

Carbon contains free mobile ions.