as grphene is covalently bond, where is the free electrons from

Graphene is a unique material that consists of a single layer of carbon atoms arranged in a two-dimensional hexagonal lattice. Each carbon atom in graphene forms three strong covalent bonds with its neighboring atoms, resulting in a stable and planar structure. Although graphene is covalently bonded, it does have free electrons that contribute to its electrical conductivity. The delocalized π-electrons in the graphene lattice are responsible for this property. These electrons are not localized between any specific pair of carbon atoms but instead spread across the entire lattice. Due to the hexagonal arrangement and overlap of carbon orbitals, there are regions in the graphene structure where pi electrons can freely move, forming a conducting band. These delocalized electrons in graphene can move easily throughout the lattice, allowing for efficient electron transport and high electrical conductivity. This unique electronic structure is one of the factors that make graphene an excellent conductor, despite being a single layer of covalently bonded carbon atoms.