Covalent network bonding refers to a type of chemical bonding where atoms are connected in a continuous network entirely by covalent bonds. This results in the formation of covalent network solids, which are characterized by their extensive three-dimensional or two-dimensional structures. These solids, such as diamond, graphite, and silicon dioxide, exhibit remarkable properties due to the strength of the covalent bonds. They typically have high melting points because breaking the covalent bonds requires significant energy. Covalent network solids are also known for their hardness and brittleness, as seen in diamond, which is one of the hardest known materials. However, their electrical conductivity varies; for instance, diamond is an excellent insulator, while graphite conducts electricity due to the presence of delocalized electrons within its layers. These solids are generally insoluble in most solvents because the strong covalent bonds are not easily disrupted by solvent interactions