Maharashtra Board Class 12 Chemistry — Flashcards for Quick Revision

A: 1. Crystalline solids: Regular, periodic arrangement of particles; sharp melting points; anisotropic properties (except cubic); examples: NaCl, diamond, metals 2. Amorphous solids: Random arrangement

A: Isomorphism: Two or more substances having the same crystal structure and same atomic ratios. Examples: NaF and MgO (1:1 ratio), NaNO₃ and CaCO₃ (1:1:3 ratio) Polymorphism: A single substance existin

A: Ionic: Ions held by electrostatic forces; hard, brittle; high melting points; conduct when melted (NaCl) Covalent network: Atoms in 3D covalent network; very hard; high melting points; poor conductors

A: A solution is a homogeneous mixture of two or more pure substances. It consists of: • Solvent: Component present in larger quantity (usually liquid) • Solute: Component present in smaller quantity (ca

A: Types of Solutions: 1. Solid in Liquid: Sugar in water, NaCl in water 2. Solid in Solid: Metal alloys (brass, bronze) 3. Solid in Gas: Iodine in air 4. Liquid in Liquid: Ethanol in water, gasoline 5.

A: Solubility: Maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature (expressed in mol L⁻¹). Factors affecting solubility: 1. Nature of solute and solvent ('l

A: Ionic equilibrium is the equilibrium between ions and unionized molecules in solution. It is significant because it helps us: 1. Determine equilibrium constants and concentrations of ions 2. Understan

A: Strong Electrolytes: - Ionize completely or almost completely in solution - Examples: HCl, HNO₃, H₂SO₄, NaOH, KOH, NaCl - Single arrow (→) used in equations Weak Electrolytes: - Dissociate only parti

A: Degree of dissociation (α) is the fraction of total moles of electrolyte that dissociates into ions at equilibrium. Formula: α = (Number of moles dissociated)/(Total number of moles) Percent dissoci