Why is graphite such a good conductor of electricity?

Why is diamond the hardest naturally occurring substance?

1) The structure of graphite is very unlike any other substances. It is composed of sheets of carbon atoms, and each of these is bonded to only three other atoms. This leaves the fourth valence electron of the carbon atom delocalized, which means it is free to move between the different sheets, therefore carrying the electrical charge through the network of carbon atoms which makes up the structure of graphite.

2) Because it has a giant covalent structure. To break the structure, numerous very strong covalent bonds between carbon atoms must be broken.

Two good answers to two difficult questions.

Graphite is a good conductor of electricity due to its unique structure and bonding. To understand this, we need to delve into the atomic structure of graphite.

Graphite is made up of carbon atoms arranged in layers that are tightly bonded within each layer but weakly bonded between the layers. The carbon atoms within each layer are arranged in a hexagonal lattice formation. These layers are referred to as graphene layers. Each carbon atom in a graphene layer is bonded to three neighboring carbon atoms, forming strong covalent bonds.

The reason graphite is a good conductor of electricity is because of the presence of delocalized electrons. In the structure of graphite, one electron from each carbon atom is not involved in the covalent bonding and becomes delocalized. These delocalized electrons are free to move within the layers and are responsible for conducting electricity.

When a potential difference is applied across a graphite material, these delocalized electrons are able to flow freely and carry an electric current. This ability to easily move the electrons makes graphite an excellent conductor of electricity.

Now, let's move on to the second question about diamond being the hardest naturally occurring substance.

Diamond is the hardest naturally occurring substance because of its strong and rigid molecular structure. The hardness of a material refers to its resistance to being scratched or deformed.

Diamond is made up of carbon atoms arranged in a three-dimensional lattice structure. Each carbon atom is bonded to four other carbon atoms through strong covalent bonds. This arrangement forms a tetrahedral network structure, where each carbon atom is surrounded by four neighboring carbon atoms.

The strength and hardness of diamonds are due to the strength of these covalent bonds, which require a significant amount of energy to break. The carbon-carbon bonds in a diamond are extremely strong, making it difficult for external forces to disrupt the structure.

Furthermore, the three-dimensional arrangement of carbon atoms in a diamond results in a tightly packed and highly symmetrical crystal lattice. This symmetric arrangement provides added stability to the structure, making it extremely resistant to deformation and giving diamond its high hardness.

In summary, the hardness of diamonds is a result of their strong covalent bonds and highly stable three-dimensional lattice structure.