Your question: Why is graphite a good lubricant and electrical conductor?

Graphite is a good conductor of electricity. Its structure is the main reason for this property. Each carbon atom in graphite is directly linked to only three carbon atoms through covalent bonds. … These free electrons make graphite a good conductor of electricity and also a good lubricant.

Why is graphite good electrical conductor?

In a graphite molecule, one valence electron of each carbon atom remains free. Due to the free electrons in its framework, graphite can perform electricity. Therefore, graphite is said to be a good conductor of electricity.

Why is graphite a good lubricant?

The carbon atoms are strongly bonded together in sheets. Because the bonds between the sheets are weak, graphite shows lower shearing strength under friction force. Thus it can be used as a solid lubricant and has become one of traditional and primary solid lubrication materials.

Why is graphite a good conductor of electricity and diamond isn t?

In a graphite molecule, one valence electron of each carbon atom remains free, Thus making graphite a good conductor of electricity. Whereas in diamond, they have no free mobile electron. Hence there won’t be flow of electrons That is the reason behind diamond are bad conductor electricity.

Why is graphite a good conductor of electricity but diamond is a bad conductor of electricity?

In a graphite molecule, one valence electron of each carbon atom remains free, Therefore graphite gained a name of a good conductor of electricity. Whereas in diamond, they have no free mobile electron. so it has been said that diamonds are bad conductor electricity.

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Why graphite is used as lubricant explain by structure of graphite?

Graphite has a layered structure and different layers of graphite are bonded to each other by weak Vander Waal’s forces. These can slide over each other. Graphite is soft and slippery. Therefore, graphite can be used as a lubricant.

Why graphite conduct electricity even though it is a non metal?

In graphite, the carbon atoms are joined together and arranged in layers. The links between the carbon atoms in the layer are strong, but the links between the layers are weak. The layers easily slip over each other. … Graphite is a non-metal and it is the only non-metal that can conduct electricity.