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Transcript
School of Chemistry Course 1101 Introduction to Physical Chemistry Professor J.M. Kelly) (Lectures 1-6) LEARNING OBJECTIVES Intermolecular Forces, Solids, Liquids, and Solutions After these lectures you should: (a) Know about the main types of intermolecular forces. {London (dispersion), dipole-dipole, ion-dipole, hydrogen-bonding) (b) Know about the main features of the solid state structures (unit cells, coordination numbers, packing fractions etc.) For elements, cubic – and hexagonal- close packing; body-centred and facecentred cubic structures: For ionic compounds NaCl and CsCl structures. Octahedral and tetrahedral holes. Examples of network and molecular solids (c) Know about the Born-Haber cycle: calculation of lattice energy/enthalpy (ΔHL) (d) Understand the principal features of the phase diagrams of pure compounds including pressure dependence of melting and boiling points, triple point and critical point, variation of vapour pressure with temperature. (e) Be familiar with ΔH and ΔS of phase transitions. (f) Know about the factors affecting solubility of liquids; ideal solutions, entropy of mixing; real solutions, effect of intermolecular forces on ΔH of solution. (g) Know about the effect of pressure and temperature on the solubility of gases in liquids. Henry’s law. Application of Le Chatelier’s principle. (h) Understand thermodynamics cycles to explain qualitatively ΔH and ΔS of solution for ideal non-ionic and ionic solids. ΔH of hydration of ions. Effect of temperature on solubility and its relationship to ΔH of solution (ΔHsoln ) Some useful equations At melting point ΔHfus = TΔHfus + ΔHmix For dissolution of non-ionic compounds ΔHsoln = ΔHfus + ΔHmix For dissolution of ionic compounds ΔHsoln = - ΔHL + ΔHH {Note lattice energy (enthalpy) ΔHL is negative Hydration enthalpy ΔHH is negative}