Why is graphite a good conductor of electricity but diamond is a 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 does graphite conducts electricity but not diamond Class 10?

Graphite can conduct electricity because of the delocalised (free) electrons in its structure. However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

Why is diamond not a good conductor of electricity?

It does not conduct electricity. Every atom in a diamond is bonded to its neighbours by four strong covalent bonds, leaving no free electrons and no ions .

Which of the following is a good conductor of electricity diamond or graphite?

Graphite is the only non-metal which is a good conductor of electricity.

What are allotropes of carbon?

Diamond, graphite and fullerenes (substances that include nanotubes and ‘buckyballs’ , such as buckminsterfullerene) are three allotropes of pure carbon.

Why diamond is hard but not graphite?

However, diamond is harder than graphite because of the carbon atoms in a diamond form 4 covalent bonds in the form of tetrahedral structure. While the carbon atoms in the graphite form 4 covalent bonds in the form of hexagonal structure. This is the reason why diamond is harder than graphite.

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 graphite is a good 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.

Is graphite good conductor of electricity?

Is diamond an allotrope of carbon?

Why diamond and graphite are allotropic modifications of carbon?

Diamond & graphite are carbon elements, their chemical properties are same i.e. they form CO_2 on burning but differ in physical state. Hence they are allotropic modifications.

Why is graphite a good conductor?

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

answered Apr 25, 2019 by muskan15 (-3,443 points) (a) 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. Thats why diamond are bad conductor electricity.

What is the difference between carbon and graphite?

Both are pure carbon, however vary in crystalline framework because they are adhered differently. A carbon atom has 4 electrons that are unpaired as well as can develop bonds by pairing with electrons from various other atoms. When it comes to diamond and graphite we are speaking about just various other atoms of carbon.

What is the difference between Diamond and Graphite’s framework?

The diamond framework is hard to envision in 3 dimensional room, however very easy to see in a 3 dimensional version. In Graphite, 3 of the 4 electrons remain in covalent bonds With 3 bonds at 120 degrees from each different other one could make a level framework.

What is the difference between carbon and Diamond and allotropes?

The way the carbon atoms are arranged in space, however, is different for the three materials, making them allotropes of carbon. The differing properties of carbon and diamond arise from their distinct crystal structures. In a diamond, the carbon atoms are arranged tetrahedrally.