Inorganic solids can be classified into three main types based on the nature of the bonding between their constituent atoms or ions: ionic, covalent, and metallic. Here are the specific characteristics that can help identify each type of inorganic solid:1. Ionic solids:- These are composed of positively charged cations and negatively charged anions held together by strong electrostatic forces ionic bonds .- They generally have high melting and boiling points due to the strong ionic bonds.- They are usually hard and brittle.- In the solid state, they are poor conductors of electricity, but when dissolved in water or melted, they become good conductors due to the mobility of ions.- They usually dissolve in polar solvents like water but are insoluble in non-polar solvents like benzene.- Example: Sodium chloride NaCl is an ionic solid composed of Na+ and Cl- ions held together by ionic bonds.2. Covalent solids:- These are composed of atoms that are bonded together by covalent bonds, which involve the sharing of electrons between atoms.- They can be further divided into two subcategories: molecular solids and network covalent solids.- Molecular solids have discrete molecules held together by weak intermolecular forces e.g., van der Waals forces, hydrogen bonds , resulting in low melting and boiling points. They are generally poor conductors of electricity and heat. Example: Ice H2O is a molecular solid held together by hydrogen bonds.- Network covalent solids have a continuous network of covalently bonded atoms, resulting in high melting and boiling points due to the strong covalent bonds. They are generally hard and brittle, and poor conductors of electricity. Example: Diamond, which is composed of carbon atoms covalently bonded in a tetrahedral arrangement.3. Metallic solids:- These are composed of metal atoms held together by metallic bonds, which involve a "sea" of delocalized electrons surrounding positively charged metal ions.- They generally have high melting and boiling points due to the strong metallic bonds.- They are usually malleable and ductile, as the delocalized electrons allow the metal ions to slide past each other without breaking the metallic bonds.- They are good conductors of electricity and heat due to the mobility of the delocalized electrons.- Example: Copper Cu is a metallic solid with a characteristic metallic luster and high electrical conductivity.In summary, the specific characteristics that help identify inorganic solids as ionic, covalent, or metallic include their bonding type, melting and boiling points, hardness, electrical and thermal conductivity, and solubility in polar and non-polar solvents.