Graphite is soft and good conductor of electricity explain

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Why can graphite conduct electricity but diamond can not?

graphite is soft and good conductor of electricity explain

Graphite is a soft lubricant and a good conductor of electricity because their electrons are delocalised and free to move. These free electrons.

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The carbon atoms are bonded differently in each substance. Graphite is a good conductor of electricity because its electrons are high boiling and melting points, while the weak bonds make graphite soft and flexible. 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. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor.

Graphite is fully compose with layers of graphene which has highest electrical and thermal conductivity in world. Graphene is sp2 hybirdized.
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Explain the difference in properties of diamond and graphite on the basis of their structures. The following are the differences in the properties of diamond and graphite based on their structures -. In diamond there is a three dimensional network of strong covalent bonds. This makes diamond extremely hard. Because of hardness, diamond is used in making cutting and grinding tools. On the other hand, in graphite there are flat layers of carbon atoms.



Why can graphite conduct electricity but not diamond?

Diamond and graphite are both allotropes of carbon; they are both made entirely of the same element carbon but they differ in the way that the atoms bond with each other and arrange themselves in a structure. Each carbon atom has 4 electrons in its outer shell that it can share with other atoms in order to form 4 covalent bonds. Diamond is a giant covalent structure; each valence electron outer shell electron of every carbon atom forms a covalent bond, which means that there are no free electrons.

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1 thoughts on “Graphite is soft and good conductor of electricity explain

  1. In part a ii , majority of the candidates could not state the type of bond present in diamond and graphite as covalent, only a few could.

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