Why is graphite an unusual conductor?

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 so electrically conductive?

Graphite is an electrical conductor, hence useful in such applications as arc lamp electrodes. It can conduct electricity due to the vast electron delocalization within the carbon layers (a phenomenon called aromaticity). These valence electrons are free to move, so are able to conduct electricity.

What is unusual about graphite?

Graphite has no melting point at atmospheric pressure, is a good conductor of heat, and is resistant to many chemicals, which makes it an ideal material for crucibles. Crucibles are containers used in the production of metal, glass, and pigment and must be able to withstand extremely high temperatures.

Why graphite is good conductor of electricity but not diamond?

Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

Why does graphite only conduct electricity in one direction?

Each carbon atom possesses a sp² orbital hybridisation. The pi orbital electrons delocalized across the hexagonal atomic sheets of carbon contribute to graphite’s conductivity. In an oriented piece of graphite, conductivity parallel to these sheets is greater than that perpendicular to these sheets.

Why are electrodes made of graphite?

Graphite is insoluble in water. It has a high melting point and is a good conductor of electricity, which makes it a suitable material for the electrodes needed in electrolysis . These delocalised electrons can all move along together – making graphite a good electrical conductor.

What are the characteristics of graphite that makes it suitable to be used as pencil lead?

Its softness and streak make graphite useful in making “lead” for pencils. It is flexible, but not elastic. Crystals are uncommon, but when they occur, they are found as rough, six-sided (hexagonal) flakes. It breaks into minute, flexible flakes that easily slide over one another.

Why is graphite a good conductor of electricity although it is a covalent solid?

Graphite is a covalent solid that act as a good conductor of electricity and is soft. The fourth valence electron of each atom is present between different layers and is free to move which makes graphite a good conductor of electricity.

Why diamond is non conductor?

However, in diamond, each carbon atom is covalently bonded to four other carbon atoms. All four of the outer shell electrons in each carbon atom are engaged in bonding, leaving no delocalised electrons free to move around the structure and carry charge.

Why is graphite anisotropic in electrical conductivity?

Carbon atoms are arranged in different layers and each atom is covalently bonded to three of its neighboring atom in the same layer. Hence the transfer of electrons is possible. Hence graphite is anisotropic with respect to the conduction of electric current.

Why is graphite a good conductor of electricity?

Graphite is a good conductor of electricity because its electrons are delocalized or free to move around. Graphite is structured into planes with tightly bound atoms. There is a great deal of distance between planes, and they are bonded weakly together, allowing the electrons to move around.

Why is graphit good conductor of electricity?

Yes, graphite is a very good conductor of electricity because of delocalized electrons . Graphite forms layers of a hexagonal arrangement of atoms and each carbon atom form a covalent bond with three other carbon atoms, and therefore each carbon atom has one non-bonded electron which becomes delocalized and responsible for conducting electricity.

Why is graphite not the best conductor?

This means that while graphite might not be the best conductor (as there is only one delocalised electron per carbon atom), it is still a good conductor of electricity (unlike another allotrope of carbon, diamond, which contains no delocalised electrons as each carbon atom is covalently bonded to four other carbon atoms).

Why is graphite a good conductor of heat?

Graphite is a good conductor of heat for the same reason it is a good conductor of electricity . Electrical Conductivity of Graphite is due to loose electrons,which are results of De-localized bonding in the layers. (This is the cause for anisotropy in Graphite). Also this is the reason for conductivity of metals.