Why is graphite a conductor of electricity but Diamond is not?

Why does graphite conducts electricity but not diamond Class 10?

Explanation: Graphite is a good conductor of electricity as each carbon atom is linked to three of its neighbouring carbon atoms. The fourth electon is free to move about. But diamond do not contain any free electon and all electrons are covalently bonded.

Why is graphite a good conductor of electricity but diamond is non conductor of electricity D state any two uses of graphite?

(c) Graphite is a good conductor of electricity because of free electrons presence in the graphite crystal. But there will be no free electrons in the diamond crystals, so there will not be any conductance of electricity. (d) Graphite is used for making leads for pencils and used as lubricants.

Why is diamond not electrically conductive?

Diamond is a form of carbon in which each carbon atom is joined to four other carbon atoms, forming a giant covalent structure. … It does not conduct electricity as there are no delocalised electrons in the structure.

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Why is graphite a conductor of electricity?

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.

How is graphite different from a diamond?

Graphite and diamond are two of the most interesting minerals. They are identical chemically – both are composed of carbon (C), but physically, they are very different. … Graphite is very soft and has a hardness of 1 to 2 on this scale. Diamonds are the hardest known natural substance and have a hardness of 10.

Why is diamond so hard?

The outermost shell of each carbon atom has four electrons. In diamond, these electrons are shared with four other carbon atoms to form very strong chemical bonds resulting in an extremely rigid tetrahedral crystal. It is this simple, tightly-bonded arrangement that makes diamond one of the hardest substances on Earth.

Why diamond is hard and graphite is soft?

The carbon atoms in graphite appear to bond with weaker intermolecular forces, allowing the layers to move over one another. The weak intermolecular forces are known as the weak Van der Waals forces. Therefore, diamond is hard but graphite is soft and slippery even though both have carbon present in them.

Is diamond conductor of electricity?

Most diamonds are electrical insulators and extremely efficient thermal conductors. Unlike many other minerals, the specific gravity of diamond crystals (3.52) has rather small variation from diamond to diamond.

Why is graphite not a good conductor of heat?

No, graphite is a conductor of electricity due to it’s structure where each atom is bonded with 3 other carbon atoms in sheets held together by weak van der waal’s force. The one electron of each carbon atom is free, which is responsible for conduction of electricity. But it is not a good conductor of heat.

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Why is diamond a good thermal conductor but not a good electrical conductor?

question_answer Answers(4) Diamond is a bad conductor of electricity but good conductor of heat. Electricity is conducted in a crystal by electrons that are relatively free. But in diamond, each carbon atom is covalently bonded with four other carbon atoms and there are no free electrons.

Is graphite a electrical conductor?

These delocalized electrons can all move along together on each layer, making graphite a good electrical conductor.

Is diamond a good conductor of heat?

Diamond is the most highly prized of gemstones. … Along with its carbon cousins graphite and graphene, diamond is the best thermal conductor around room temperature, having thermal conductivity of more than 2,000 watts per meter per Kelvin, which is five times higher than the best metals such as copper.

What is graphite and diamond structure?

Diamond and graphite are different forms of the element carbon. They both have giant structures of carbon atoms , joined together by covalent bonds .