Which allotrope of carbon conducts electricity?a)Graphiteb)Diamondc)Fullerened)Both Graphite and DiamondCorrect answer is option 'A'. Can you explain this answer?

Question

Answer

Graphite is an interesting material, an allotrope of carbon (as is diamond). It displays properties of both metals, and nonmetals. However, like a metal, graphite is a very good conductor of electricity due to the mobility of the electrons in its outer valence shells.

So option A is the correct answer.

Answer

In graphite, each carbon atom is covalently bonded to three other carbon atoms. since only three valence electrons of each carbon are involved in bond formation. The fourth electron of each carbon is 'free' to move and hence graphite conducts electricity. while in diamond all the valence carbon atoms are involved in bond formation.so, it does not conduct electricity.

Answer

Graphite conduct the electricity because it has a free electron in its outermost shell due to which it can move to conduct the electricity.

Answer

Graphite:
Graphite is an allotrope of carbon that conducts electricity. It is composed of layers of carbon atoms arranged in a hexagonal lattice structure. The layers are held together by weak Van der Waals forces, allowing them to slide over each other easily. This unique structure gives graphite its characteristic properties, including its ability to conduct electricity.

Conductivity of Graphite:
Graphite is a good conductor of electricity due to the presence of delocalized electrons. In the hexagonal lattice structure of graphite, each carbon atom is bonded to three other carbon atoms, forming strong covalent bonds within the layers. However, there is a weak interaction between the layers, which allows the electrons in the outermost orbitals of the carbon atoms to move freely between the layers. These delocalized electrons are not bound to any specific atom and can move along the layers, carrying an electric current.

Comparison with Diamond:
Diamond, another allotrope of carbon, does not conduct electricity. Unlike graphite, diamond has a different crystal structure. In diamond, each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement, forming a three-dimensional network of strong covalent bonds. This structure does not allow for the movement of electrons, as they are tightly held within the covalent bonds. Therefore, diamond is an insulator and does not conduct electricity.

Fullerene:
Fullerenes are another form of carbon allotropes, consisting of carbon atoms arranged in a hollow sphere, tube, or other shapes. While some fullerene structures, such as C60, can conduct electricity under certain conditions, the conductivity of most fullerene structures is relatively low compared to graphite.

Conclusion:
In conclusion, graphite is the allotrope of carbon that conducts electricity. Its unique hexagonal lattice structure allows for the movement of delocalized electrons, enabling the flow of electric current. Diamond, on the other hand, does not conduct electricity due to its tightly bound covalent structure. Fullerene structures can exhibit some conductivity but are generally less conductive compared to graphite.

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