Name at least four clements that, in at least one allotropic form, are network solids.

Allotropy refers to the phenomenon where an element can exist in two or more different forms, known as allotropic forms, in the same physical state. These allotropic forms have distinct structures and properties. For example, carbon, a versatile element, exhibits various allotropes including diamond and graphite. Diamond is a clear example of a network solid due to its tetrahedral structure where each carbon atom is covalently bonded to four others, creating a rigid three-dimensional lattice. In contrast, graphite consists of layered planes of hexagonally arranged carbon atoms with weaker forces between the planes, which is why graphite is not a network solid. Understanding allotropy is essential when classifying substances like network solids because it highlights how one element can form materials with vastly different characteristics.

Covalent networks, also known as covalent network solids, are a class of materials where atoms are connected by covalent bonds in a continuous network that extends throughout the entire solid. This structure results in exceptionally strong materials due to the robustness of the covalent bond. In a covalent network solid, each atom is usually bonded to multiple other atoms, forming a rigid, interconnected structure. This explains the high melting points, hardness, and low reactivity typical of such materials. Common examples of elements forming covalent networks are carbon (as diamond), silicon, boron, and germanium in specific allotropic forms. These networks create a highly ordered and stable structure, which greatly impacts the material's properties.

The crystalline structure relates to the highly ordered arrangement of atoms in a crystal. Atoms are positioned in a repeating pattern that spans three dimensions, creating a lattice structure. This structure is what gives a material its shape, strength, and other unique properties. Network solids like diamond or crystalline forms of silicon and germanium showcase crystalline structures where the order and repetition of the atoms through the lattice are evident. These characteristics significantly influence physical properties, such as refractive index and thermal conductivity. For instance, the ordered arrangement in diamond allows for remarkable light dispersion, contributing to its optical brilliance. Recognizing the significance of the crystalline structure is crucial in understanding the behavior and functionality of network solids.