Why is graphite a good conductor of electricity

Graphite is a good conductor of both electricity and heat. This is due to its molecular structure, which allows electrons to move freely through it.

Use app Login. Why is graphite a good conductor of electricity and a good lubricant? Explain with the help of diagram. Open in App. Verified by Toppr. Each carbon atom is bonded to three other carbon atoms in the same plane giving a hexagonal array. One of these bonds is a double-bond, and thus the valency of carbon is satisfied.

Why is graphite a good conductor of electricity

Graphite is a good conductor of heat and electricity because it contains. Therefore, graphite is a good conductor of heat and electricity because it contains free electrons which can conduct heat and electricity. Byju's Answer. Open in App. Conduction of heat and electricity: Graphite is the crystalline allotropes of carbon and it has a layered structure. Conduction of heat and electricity in a substance occurs due to the presence of free electrons in that material. Only three or four valence electrons of each carbon atom are involved in bonding, so, each carbon atom makes use of sp 2 hybrid orbitals, Thus the fourth valence electron of each carbon atom remains unpaired. This free electron is responsible for the conduction of heat and electricity. Graphite is a good conductor of heat and electricity because it contains :. Graphite is a good conductor of electricity because it has:. Graphite is a good conductor of electricity because:.

Hence it is used as a lubricant. Open in App.

Graphite is a great conductor, it is used in electrical cells. It is also found in motor oil and pencils. Because graphite is soft, it is combined with clay, and baked, and hardened before being inserted into wood for pencils. Graphite is made up of bonded carbon atoms. One carbon atom is strongly bonded to three other carbon atoms, resulting in carbon sheets. Each carbon atom is then bound weakly to two other carbon atoms, one to the sheet above it and another to the sheet below it. The strong bonds give graphite high boiling and melting points, while the weak bonds make graphite soft and flexible.

Graphite is a fascinating material that has garnered significant attention for its unique properties, particularly its ability to conduct electricity. In this article, we will delve into the reasons why graphite is such a good conductor of electricity, exploring its molecular structure, applications in various industries, and the implications for future technological advancements. Graphite is composed of carbon atoms arranged in a hexagonal lattice, forming layers of interconnected sheets. These sheets are held together by weak van der Waals forces, allowing them to easily slide past each other. This structure gives graphite its characteristic slippery feel and also enables the flow of electrons through the material. In graphite, each carbon atom is bonded to three other carbon atoms, leaving one electron free to move within the material. These delocalized electrons are not confined to a specific bond, allowing them to flow freely through the layers of graphite, carrying electrical current along the way.

Why is graphite a good conductor of electricity

Graphite is an allotropic form of carbon consisting of sacks of carbon layers. Let us know about conducting nature of graphite. Graphite is a good conductor of electricity even though bulk carbon does not contribute to the conduction. At the nanoscale, the orientation of carbon atoms in the graphite lattice faces different directions, so electrical conduction is possible in graphite.

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Substances like graphite which have these giant structures have very high melting points. Allotropes of Carbon. Graphite structure is formed by the hexagonal arrays being placed in layers one above the other. Also working in academia, Thomas has lectured on the topic of journalism to undergraduate and postgraduate students at The University of Sheffield. True, both diamonds and graphite are made from carbon. This is due to its molecular structure, which allows electrons to move freely through it. As you might have guessed, this is due to the strong covalent bonds between their atoms. Similar Questions. Therefore, graphite is a good conductor of heat and electricity because it contains free electrons which can conduct heat and electricity. Rather than loosen one sheet of molecules from another, you have to break the covalent bonding the particular way in which atoms are bonded together throughout the whole structure in order to melt the material. Hot Products. Dr Dong Liu is a physics lecturer at the University of Bristol.

Answer: the very reason why metals do.

As she points out, graphite is made from carbon atoms, which have four electrons in their outer shells. View Solution. Synthetic graphite can be produced with varying degrees of porosity—in other words, making the graphite porous so liquid, air or gas can pass through its layers. Byju's Answer. Graphite is a good conductor of heat and electricity because it contains. These free electrons make graphite a good conductor of electricity and also a good lubricant. Difficult is an understatement. Graphite is made up of layers of carbon atoms. Open in App. In short: graphite trumps diamond. GB Co Reg. Verified by Toppr. This doesn't only strengthen graphite's structure but allows electrons to move freely along the layers. We still don't recommend proposing with a graphite ring, though.