![]() Ionic solids are held together by electrostatic forces between ions, molecular solids are formed by weak intermolecular forces, covalent network solids feature extensive covalent bonds, and metallic solids showcase a sea of delocalized electrons. Common examples include copper, aluminum, and iron.Ĭonclusion: The classification of crystalline solids provides insight into the diverse structures and properties exhibited by these materials. Metallic solids often possess high melting points and exhibit malleability and ductility. Metallic bonding allows for the free movement of valence electrons throughout the solid, giving rise to high electrical and thermal conductivity. Metallic Solids: Metallic solids are composed of a closely packed arrangement of metal atoms held together by metallic bonds.While diamond is extremely hard and transparent, graphite is soft and conducts electricity due to its layered structure. Diamond and graphite are prime examples of covalent network solids. Covalent network solids have exceptionally high melting points due to the strong covalent bonds present throughout the structure. This results in a three-dimensional network structure. Covalent Network Solids: Covalent network solids are characterized by a vast network of covalent bonds, where each atom is bonded to several neighboring atoms.Examples include solid water (ice) and organic compounds like sucrose (table sugar) and naphthalene (mothballs). Molecular solids generally have lower melting points compared to ionic solids. ![]() The molecules are arranged in a regular pattern, forming a solid structure. Molecular Solids: Molecular solids consist of individual molecules held together by intermolecular forces such as van der Waals forces or hydrogen bonding.Examples of ionic solids include common table salt (NaCl) and calcium carbonate (CaCO3). These solids tend to have high melting points and are brittle in nature. The ions are arranged in a three-dimensional lattice structure. Ionic Solids: Ionic solids are formed by the attraction between positively and negatively charged ions.In this article, we will delve into the classification of crystalline solids and explore the characteristics of each class. They exhibit a wide range of properties and find applications in various fields, including materials science, electronics, and pharmaceuticals. Classification of Crystalline SolidsĬrystalline solids are fascinating materials with a highly ordered and repetitive arrangement of atoms, ions, or molecules. This is because the electric charges on the constituent atoms are lined up in the same direction. Some crystals, such as quartz, can also generate an electric field when they are rubbed. This is because the atoms, molecules, or ions in a crystal are densely packed and orderly. The precise nature of the repeating pattern depends on the type of crystal.Ĭrystals are typically transparent or translucent, meaning that light can pass through them but they do not scatter it in all directions as a gas or liquid would. This regularity gives crystals their characteristic sparkle and hardness. The defining characteristic of a crystalline solid is that its constituent atoms, molecules, or ions are arranged in a repeating, three-dimensional pattern. The most common example of a hexagonal crystal is graphite. The most common example of a monoclinic crystal is gypsum.ĥ) Hexagonal crystals – These crystals have a six-sided lattice, with the atoms arranged in a hexagonal pattern. The most common example of an orthorhombic crystal is calcite.Ĥ) Monoclinic crystals – These crystals have a two-dimensional lattice, with the atoms arranged in a monoclinic pattern. The most common example of a tetragonal crystal is quartz.ģ) Orthorhombic crystals – These crystals have a three-dimensional lattice, with the atoms arranged in an orthorhombic pattern. The most common example of a cubic crystal is ice.Ģ) Tetragonal crystals – These crystals have a four-sided lattice, with the atoms arranged in a square pattern. 1) Cubic crystals – These crystals have a three-dimensional lattice, in which the atoms are arranged in a cubic pattern.
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