![]() ![]() Hydrogen bonds, dipole-dipole forces and dispersion forces are present between water molecules. Separation of solvent molecules is endothermic as energy is absorbed to overcome intermolecular forces present between molecules.Dissolution of ionic compounds occurs in three steps:.For example, MgCl 2 has greater lattice energy than NaCl because magnesium ion has a +2 charge while sodium ion has a +1 charge. Greater the charge, higher the lattice energy. For example, KCl has lower lattice energy than NaCl because potassium ion is larger than sodium ion in terms of ionic radius. Larger the ions, lower the lattice energy. Lattice energy is dependent on two main factors:.$$$$įigure: Lattice energy of magnesium oxide is greater than that of sodium fluoride because magnesium and oxygen ions have greater charge. It is defined as the energy released through the formation of an ionic compound from its constituent ions.įor example, the formation of sodium chloride from sodium and chlorine ions releases 787 kilojoules of energy for every mole of sodium chloride. Lattice energy indicates bond strength of an ionic compound.Dissolution of ionic compounds requires energy equal to the lattice energy. Ionic compounds occupy a lattice structure, held together by electrostatic forces between cations and anions.This video will explore the different steps which are involved in the dissolution of an ionic compound - separation of water molecules, dissociation of compound into ions, hydration of ions. ![]() What are the processes involved in the dissolution of an ionic compound? This is part of the HSC Chemistry course under the topic equilibrium systems HSC Chemistry Syllabusĭescribe and analyse the processes involved in the dissolution of ionic compounds in water ![]()
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