Ionic Solids – Class 12 | Chapter – 1 | Chemistry Short Notes Series PDF for NEET & JEE
Ionic Solids: Ionic solids are a type of crystalline solid composed of positively charged cations and negatively charged anions held together by ionic bonds. Ionic bonds are strong electrostatic attractions between oppositely charged ions, which result in the formation of a lattice structure in the solid. Ionic solids are typically hard and brittle, have high melting and boiling points, and are poor conductors of electricity in the solid state.
Types of Ionic Solids
Some of the common types of ionic solids:
- Simple Ionic Solids: These are ionic solids made up of only one type of cation and one type of anion. Examples include NaCl (sodium chloride) and MgO (magnesium oxide).
- Binary Ionic Solids: These are ionic solids made up of two types of ions, one cation and one anion. Examples include CaF2 (calcium fluoride) and LiBr (lithium bromide).
- Transition Metal Ionic Solids: These are ionic solids made up of transition metal cations and non-metal anions. Examples include Fe2O3 (iron oxide) and CuCl2 (copper chloride).
- Mixed Ionic Solids: These are ionic solids made up of two or more types of cations or anions. Examples include NaKSO4 (sodium potassium sulfate) and (NH4)2SO4 (ammonium sulfate).
- Coordination Ionic Solids: These are ionic solids where the cations are complex ions, which are coordination compounds with a metal ion at the center and ligands attached to it. Examples include K4[Fe(CN)6] (potassium hexacyanoferrate) and [Co(NH3)6]Cl3 (cobalt hexamine chloride).
- Polymeric Ionic Solids: These are ionic solids made up of repeating units of cations and anions that are covalently bonded to each other. Examples include NaSbF6 (sodium hexafluoroantimonate) and K3[Fe(CN)6] (potassium ferricyanide).
Properties of Ionic Solids
Some of the main properties of ionic solids:
- High melting and boiling points: Ionic solids have high melting and boiling points due to the strong ionic bonds that hold the constituent ions together. In order to melt or vaporize an ionic solid, a significant amount of energy is required to break these bonds.
- Hard and brittle: Ionic solids are usually hard and brittle, meaning that they tend to shatter or break apart when subjected to stress or impact. This is because the arrangement of the ions in the lattice structure is rigid and inflexible.
- Poor conductors of electricity in the solid state: Ionic solids are typically poor conductors of electricity in the solid state, as the ions are held in fixed positions within the lattice and cannot move freely. However, when an ionic solid is melted or dissolved in water, the ions become free to move and the material can conduct electricity.
- Solubility: The solubility of an ionic solid in a particular solvent depends on the polarity of the solvent and the strength of the ionic bonds. Polar solvents, such as water, are typically able to dissolve ionic solids, while nonpolar solvents are not.
- Crystal structure: Ionic solids often have a well-defined crystal structure, due to the regular arrangement of the constituent ions. This structure can be used to predict the properties of the solid, such as its melting point and solubility.
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