A crystalline solid held together by covalent bonds
Network solids have a three-dimensional structure with strong covalent bonds throughout, leading to a higher melting point compared to molecular solids which have weaker intermolecular forces. In network solids, a larger amount of energy is required to break the extensive network of covalent bonds, resulting in a higher melting point.
Network solids.
Network solids, or network atomic solids, are large crystals with covalent bonds holding the atoms together. Gemstones including diamonds and rubies are network solids. Crystalline solids have a constituent arranged in ordered patterns and include amethyst quartz.
Covalent-network solids are substances in which atoms are bonded together by strong covalent bonds in an extended network structure. This results in materials with high melting points, hardness, and electrical insulating properties. Examples include diamond and silicon carbide.
In network solids, attractive forces like covalent bonds, ionic bonds, and metallic bonds stabilize the structure. These strong bonds between atoms or ions help maintain the rigid and three-dimensional network structure of network solids.
Network solids are composed of an extended three-dimensional network of atoms bonded together by covalent bonds. Examples include diamond and quartz. The structural units in network solids are individual atoms or small groups of atoms connected to each other in a repeating pattern throughout the solid.
It can be categorised into -Ionic -Covalent molecular -Metallic -Covalent network
Nonmetal atom
Nonmetal atom
Pure sulfur (S) does not form network solids. You may be thinking of silicon (Si) which does.
Nonmetal atom
Nonmetal atom