What type of bonding is primarily responsible for the properties of covalent networks?

Covalent networks are characterized by a specific arrangement of atoms connected through covalent bonds, forming a continuous network. This type of bonding involves the sharing of electron pairs between atoms, resulting in strong interactions that extend throughout the entire structure. This extensive network of covalent bonds gives materials like diamond and silicon carbide their high melting points and hardness, as breaking any part of the structure requires the disruption of many strong covalent bonds.

The strength and directionality of covalent bonding in these networks play a significant role in determining the physical properties of the materials, such as electrical conductivity, thermal stability, and rigidity. These properties contrast sharply with those of materials that rely on other types of bonding.

Ionic bonds, on the other hand, involve the electrostatic attraction between positively and negatively charged ions, which typically leads to different characteristics such as brittleness and solubility in water. Metallic bonding involves a "sea of electrons" that are free to move around, contributing to conductivity and malleability but is not relevant to the defining characteristics of covalent networks. Hydrogen bonding, while important in certain molecular compounds, is much weaker than covalent bonds and affects properties like boiling point but not the core properties of covalent network structures.