Why is graphite a better conductor of electricity than diamond?

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 good conductor of electricity but diamond not?

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.

Why is graphite good conductor of electricity?

Graphite is the one ‘allotropic form’ of carbon. 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 soft but diamond hard?

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.

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What are the difference between diamond and graphite?

For example, Graphite and diamond are two different allotropes of carbon.

Explain the difference in properties of diamond and graphite on the basis of their structures.

DIAMOND GRAPHITE
1) It has a crystalline structure. 1) It has a layered structure.
2) It is made up of tetrahedral units. 2) It has a planar geometry.

Why is diamond a good conductor of electricity?

Due to the tetrahedral arrangement of covalently bonded carbon atoms in diamonds, there are no free electrons that can move and carry currents in diamonds. Since the conduction of electricity requires the presence of free electrons.

What is graphite electrical conductivity?

Graphite is extensively used in electrodes for batteries and electrolysis reactions due to its high electrical conductivity of ~104 S cm1.

Why is graphite The softest?

Each layer is a planar sheet, composed of hexagonal rings of carbon atoms, with 3 electrons of each atom involved in single bonds with three adjacent atoms of hexagonal ring. The extra electron makes a very weak bond with the adjacent layer. The inter-layer distance can be easily changed. This makes graphite very soft.

Why diamond is harder than graphite?

We know that both diamond and graphite are made of carbon. 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.

Why do diamond and graphite differ in their properties?

Diamonds are formed due to covalent bonds which forms a strong three- dimensional network whereas graphite are formed due Van der Waal force which is weak. Thus, Graphite are formed of flat carbon atoms layers one upon other. These carbon atoms layers slip over each giving graphite a soft nature.

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How does diamond and graphite differ in terms of electrical conductivity and hardness?

Graphite, for example, has a melting point of more than 3,600°C. Variable electrical conductivity – diamond does not conduct electricity, whereas graphite contains free electrons so it does conduct electricity. Silicon is a semi-conductor – it is midway between non-conductive and conductive.

Why diamond and graphite have different properties because they have different?

Giant covalent structures contain many atoms joined together by covalent bonds to form a giant lattice. They have high melting and boiling points. Graphite and diamond have different properties because they have different structures. Graphite conducts heat and electricity well because it also has free electrons.