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Learning Objectives General Chemistry II (CHEM 1474) Buckley – Fall 2010 Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009 Intermolecular Forces, Liquids, and Solids (Chapter 11) Very brief review of Lewis structures and molecular geometry Sample Exercises Got it? Needs work 3 Draw Lewis structures for and determine polarity of molecules through sp 8.45 – 8.64, 9.31 – hybridization (8.5-8.7, 9.1-9.6) 9.38 The kinetic-molecular description of gases, liquids and solids State assumptions of kinetic-molecular theory of gases (10.7) 10.71 – 10.74 Describe molecular level differences between gases, liquids, and solids (11.1) 11.1, 11.9 – 11.12 Intermolecular forces and their effect on properties Given a substance identify its intermolecular forces (11.2) 11.13 – 11.20 Properties of liquids and solids Define surface tension and viscosity and predict trends based on intermolecular 11.29-11.31 forces (11.3) Arrange a series of compounds in order of increasing or decreasing 11.5, 11.21-11.27, boiling/freezing point (11.3) 11.79 – 11.83, 11.100, 11.110 Interpret a phase diagram and locate the triple point and critical points (11.4, 11.6) 11.6, 11.41-11.42, 11.51 – 11.56 Define vapor pressure and relate it to boiling point (11.5) 11.43– 11.50, 11.91 Identify the three basic types of unit cell – cubic, body-centered cubic, and face- 11.59 – 11.68 centered cubic (11.7) Identify the bonding types – molecular, covalent network, ionic, and metallic - in 11.69 – 11.78 various solids (11.8) Properties of Solutions (Chapter 13) Chapter Exercises The solution process – a review of electrolytes Identify substances as acids, bases, or salts in aqueous solutions (4.3, handout) Identify substances as strong or weak/non electrolytes in aqueous solution (4.3, handout) Determine whether substances are soluble or insoluble in aqueous solution (4.2, handout) Write total ionic and net ionic equations for a variety of acid/base/salt reactions (4.2) Methods of expressing concentrations Work numerically with the expressions of mass percentage, ppm, ppb, molarity, molality, and mole fraction (4.5, 13.4) Factors affecting solubility Predict solubilities based on intermolecular forces (13.3) State and predict effects of temperature and pressure on solubility (13.3) Colligative properties Describe the four colligative properties of solutions and write the mathematical relationships that apply to each (13.5) Apply Raoult’s Law and the relationships between concentration and freezing point, boiling point, and osmosis (13.5) Colloids Qualitatively describe colloids (13.6) 4.29 – 4.36 4.1 - 4.18, 4.37 – 4.38, 4.19 – 4.22 4.23 – 4.28, 4.39 – 4.44, 4.59 – 4.76, 13.33 – 13.54, 13.85, 13.87 – 13.91, 13.114 – 13.116 13.11 – 13.14, 13.83 13.19 – 13.32 13.55 13.55 – 13.76, 13.92 – 13.98, 13.99 – 13.100, 13.104 – 13.105, 13.107, 13.112 – 13.113, 13.117 – 13.121 13.77 – 13.82 Chemical Kinetics (Chapter 14) Methods of expressing rates Given a chemical reaction, express the rate in terms of the stoichiometry (14.2) Factors that affect reaction rates Identify factors that affect a reaction rate and their effect (14.1) i. Dependence of rate on concentration Given experimental initial rate information, determine the rate law for a reaction (14.3) Given sufficient concentration/time information, find missing information for first- and second- order reactions (14.4) Use half-life relationships for first- and second-order reactions to find missing information (14.4) ii. Dependence on temperature Describe molecularly the effect of temperature on reaction rate (14.5) Apply the Arrhenius equation (14.5) iii. Catalysis Qualitatively describe the mechanisms of homogeneous, heterogeneous, and enzyme catalysis (14.7) Mechanisms and molecularity Given a mechanism, write the anticipated rate law (14.6) Simplify a rate law for a given mechanism given the rate determining step (14.6) Chemical Equilibrium (Chapter 15) The concept of equilibrium Describe the concept of a dynamic equilibrium (15.1) The equilibrium constant and its link to thermodynamics Given sufficient information, determine whether or not a system is at equilibrium (15.2) Relate Kc and Kp (15.2) Relate the equilibrium constant to the free energy (19.7) Interpreting and working with equilibrium constants Predict direction of equilibrium based on value of equilibrium constant (15.3) Given a chemical equilibrium write the expression for the equilibrium constant (15.3-15.4) Calculating equilibrium constants Use the equilibrium constant expression to find missing information (15.5) Use the equilibrium constant and given concentrations to predict the direction of reaction (15.6) Calculate equilibrium concentrations given starting concentrations and the equilibrium constant (15.6) LeChâtelier's Principle Predict shifts in equilibrium due to changes in concentration, volume, temperature, pressure, or the addition of catalyst (15.7) Acid-base equilibria (Chapter 16) Review of current acid-base concepts (4.3, 16.1) Bronsted-Lowry acids and bases Identify substances as Bronsted-Lowry acids or bases (16.2) Identify conjugate acid-base pairs (16.2) Determine relative acidity or basicity of substances (16.2) The autoionization of water Given hydronium or hydroxide concentration, determine the other (16.3) The pH scale Given hydronium, hydroxide, pH, and/or pOH determine the other values (16.4) Calculations involving strong acids and bases Determine hydronium, hydroxide, pH, and/or pOH values given a concentration of a strong acid or base (16.5) Calculations involving weak acids, weak bases, and salts Determine hydronium, hydroxide, pH, and/or pOH values given a concentration of a weak acid, weak base, or salt solution and the appropriate equilibrium constant (16.6-16.9) Acid-base behavior and chemical structure Identify factors that affect acid and base strengths (16.10) Lewis acids and bases Identify materials as Lewis acids or bases (16.11) Other Aspects of Aqueous Equilibria (Chapter 17) Common ion effect Identify “common ions” in a given solution Calculate the pH and associated quantities in systems made with compounds containing common ions (17.1) Buffered solutions Define and identify buffer systems (17.2) Calculate the pH and associated quantities in buffer systems (17.2) Calculate changes in pH when acids and bases are added to buffer solutions (17.2) Acid-base titrations Generate titration curves for strong acid-strong base, weak acid-strong base, polyprotic acid titrations (17.3) Solubility equilibria Given any chemical equation expressing the dissolution of a solid, write the mathematical expression for the Ksp (17.4) Given sufficient information, calculate missing information related to a solubility situation (17.4-17..5) Predict solubility based on the introduction of common ions (17.5) Qualitative analysis for metallic elements Given results of particular steps in Figure 17.22, state conclusions regarding the presence or absence of specific ions (17.7) Thermochemistry and Thermodynamics (Chapter 5 and 19) The nature of energy and its importance in chemistry Distinguish between kinetic and potential energy (5.1) Convert between energy units (5.1) Identify system and surroundings (5.1) Work with energy conversions, particularly heat and work (5.1) The First Law of Thermodynamics Relate internal energy to heat and work (5.2) Identify endothermic and exothermic changes (5.2) Identify properties as a state function or path function (5.2) Chemical applications of enthalpy Define enthalpy (5.3) Draw an enthalpy diagram for a reaction (5.4) Determine heat requirements for heating, cooling, and phase changes in physical changes (5.5) Given calorimetry data, determine enthalpies of change and reaction (5.5) Given sufficient information, apply Hess’ Law to determine enthalpies of reaction (5.6) Enthalpies of formation Use enthalpies of formation to determine enthalpies of reaction (5.7) Spontaneous processes Distinguish between the terms spontaneous and nonspontaneous process (19.1 Distinguish between reversible and irreversible processes (19.1) Entropy 5.1, 5.9-5.12, 5.16 5.13, 5.14 5.15, 5.17-5.18 5.3, 5.19-5.22 5.2, 5.5, 5.6 5.4 5.7 5.8 Describe the role of entropy in determining the spontaneity of a process (19.2) State and apply the Second Law of Thermodynamics (19.2) Free energy and its application to spontaneity Given sufficient information, calculate the Gibbs Free Energy for a reaction (19.5) Determine temperature ranges of spontaneity (19.5) Complete a nuclear transmutation equation given sufficient information (21.3) Describe the process of nuclear fission and the basic principles behind a nuclear fission reactor (21.7) Describe biological effects of radiation (21.9)