Graphite is a unique form of carbon that conducts electricity due to its unique structure and bonding.

Graphite Structure:
- Graphite is composed of layers of carbon atoms arranged in a hexagonal lattice structure.
- Each carbon atom is covalently bonded to three other carbon atoms, forming a flat sheet or layer.
- The layers are held together by weak van der Waals forces, allowing them to slide over one another easily.

Delocalized Electrons:
- One of the key reasons why graphite conducts electricity is the presence of delocalized electrons.
- In the graphite structure, each carbon atom forms three covalent bonds, leaving one outer electron unbound.
- These unbound electrons are not localized to a specific carbon atom but are free to move along the layers of the graphite structure.
- These delocalized electrons are responsible for electrical conductivity as they can carry electric charge.

Mechanism of Electrical Conductivity:
- When a potential difference (voltage) is applied across a graphite sample, the delocalized electrons can move freely within the layers of the structure.
- As a result, an electric current is established as the electrons flow from the negatively charged electrode (cathode) to the positively charged electrode (anode).
- The layers of graphite act as a pathway for the movement of these delocalized electrons.

Properties Supporting Electrical Conductivity:
- Apart from its unique structure, graphite possesses several other properties that contribute to its conductivity.
- Graphite has a high electrical conductivity compared to other non-metals due to the presence of delocalized electrons.
- It also has a relatively low resistance to the flow of electric current.
- Additionally, graphite is a good conductor of heat, allowing for efficient dissipation of heat generated during the flow of electricity.

Applications:
- The electrical conductivity of graphite makes it suitable for various applications.
- It is commonly used in electrodes for batteries, fuel cells, and electrolysis processes.
- Graphite is also utilized as a lubricant in applications where low friction and electrical conductivity are required, such as in mechanical systems and electrical contacts.
- Moreover, it is used in the manufacturing of electrical wires, brushes, and heating elements.

In conclusion, the electrical conductivity of graphite is a result of its unique structure, which allows for the presence of delocalized electrons that can move freely within its layers. This property, along with other supporting factors, makes graphite an excellent conductor of electricity with various practical applications.

Graphite conducts electricity because graphite contain one free electron in every carbon - carbon bond.So due to the presence of the ions graphite conducts electricity.