Course Schedule with ref to Silberberg Chemistry The Molecular Nature of Matter and Change 9th Edition CHEMISTRY 122 GENERAL COLLEGE CHEMISTRY I Spring 2022 Lecture Topics Monday January 17th Martin Luther King Day No classes Friday January 21st Last day to add drop without W grade Week 1 Jan 10 14 Chapter Reading Sections Pages 1 3 4 pp 12 31 2 2 5 pp 44 54 Independent Reading Chapter 1 1 2 pp 3 11 2 1 pp 42 44 2 Jan 17 21 2 5 8 pp 55 78 3 1 pp 93 99 3 Jan 24 28 3 1 4 pp 99 127 4 Jan 31 Feb 4 Finish 3 4 Limiting reactants and yields pp 118 127 4 1 2 pp 143 162 5 Feb 7 11 4 3 5 pp 162 186 6 Feb 14 18 4 6 pp 186 188 5 1 3 pp 203 219 7 Feb 21 25 5 4 6 pp 220 242 Definitions Units and Problem Solving Conversion factors in problem solving temperature scales significant figures calculations with significant figures precision and accuracy Three Mass Laws Dalton s Atomic Theory Atomic Theory Today protons neutrons electrons atomic number mass number atomic symbol Atomic Theory Today cont d atomic mass isotopes Introduction to the Periodic Table organization and classifying elements Ionic and Molecular Compounds introduction to valence electrons bonding in ionic versus covalent compounds Coulomb s Law periodic table trends for ion formation formulas for ionic and molecular compounds masses and naming of ionic and molecular compounds polyatomic ions compounds containing polyatomic ions hydrated ionic compounds acids Stoichiometry moles Avogadro s number molar mass Stoichiometry mass percent Chemical Formulas empirical molecular and structural formulas combustion analysis of organic compounds Writing and Balancing Chemical Equations Calculating Quantities of Reactants and Products reaction stoich limiting reactants theoretical actual and percent yields Solutions terms ionic and covalent compounds in water expressing concentration using Molarity preparing and diluting solutions Writing Equations for Aqueous Ionic Reactions molecular total ionic and net ionic equations Precipitation Reactions using Solubility Rules to predict precipitation stoichiometry Acid Base Reactions Neutralization strong vs weak acids and bases Arrhenius definition Proton Transfer concept Acid base stoichiometry Oxidation Reduction Reactions assigning oxidation numbers identifying oxidizing and reducing agents Redox Reactions Combination Decomposition Single Displacement Reactions and the Activity Series Combustion Reversibility of Reactions Gases overview pressure and measurement Boyle s Charles s and Avogadro s Laws Ideal Gas Law problem solving Algebraic Rearrangements of The Ideal Gas Law density molar mass mole fraction partial pressure and reaction stoichiometry Kinetic Molecular Theory kinetic energy root mean square speed effusion and diffusion Real Gases effect of interparticle attractions and particle volume Monday January 31st 6 00 7 15 PM EXAM 1 Chapters 1 1 4 2 1 8 3 1 4 Includes Independent Reading thru p 118 Monday February 28th 6 00 7 15 PM EXAM 2 Chapters 3 4 pp 118 127 4 1 6 5 1 6 1 Friday March 18th Last day to withdraw with college permission March 21 25 SPRING BREAK No Classes Wednesday March 30th 6 00 7 15 PM EXAM 3 Chapters 13 4 6 17 1 6 8 Feb 28 Mar 4 13 4 6 pp 552 554 561 565 568 570 571 9 Mar 7 11 17 1 4 pp 753 766 10 Mar 14 18 17 5 6 pp 767 788 18 1 2 pp 804 806 11 Mar 28 Apr 1 18 2 4 pp 807 815 Begin 18 5 pp 815 817 12 Apr 4 8 18 5 7 pp 817 832 13 Apr 11 15 18 8 pp 833 837 19 1 pp 853 863 Acid Base Review Solubility terms temp and solubility of solids in water Henry s Law Concentration Terms molarity molality parts by mass and volume mole fraction interconverting between terms Colligative Properties Raoult s Law electrolytes calculations with osmotic pressure van t Hoff factor uses of osmotic pressure Equilibrium state and Equilibrium Constant Reaction Quotient Q Understanding what Q means Writing Q in various forms effect of liquids and solids Ways of Expressing Q and Calculating K Expressing Equilibria with Pressure Terms Kc and Kp Determining Reaction Direction Solving Equilibrium Problems ICE tables quadratic formula Simplifying Assumption Le Chatelier s Principle Effect of concentration pressure volume temperature and catalyst Acid Base Equilibria Definitions Arrhenius definition Bronsted Lowry BL definition brief review of Lewis definition Applying the BL definition Writing acid base reactions with conjugate acid base pairs Relative Strength and Net Direction of an Acid Base Reaction pH and autoionization of water relationship between pH pOH and Kw characterizing strong acids and strong bases and calculating pH Weak acids Meaning of relationship between and acid Weak bases and their relation to weak acids Meaning of relationship between and base strength anions of weak acids act as weak bases relation between and of a conjugate strength Weak acids cont d Solving a variety of problems with Weak acid equilibria applying problem solving approach from Chapter 17 effect of concentration on the extend of acid dissociation behavior of polyprotic acids Molecular Properties and Acid Strength applying trends acid base pair Examples of weak bases ammonia and amines Acid Base Properties of Salt Solutions identifying when salts yield acid basic and neutral solutions Acid Base Buffers How a buffer works common ion effect challenging a buffer with strong acid or base Henderson Hasselbalch Equation buffer capacity and range buffer prep Acid base titrations strong acids strong bases weak acids strong bases weak bases strong acids polyprotic titration curves Indicators Choosing an acid base indicator Equilibria of Slightly Soluble Ionic Compounds determining solubility S from common ion and pH effects on solubility predicting precipitate formation 2 Monday April 18th 6 00 7 15 PM EXAM 4 Chapters 18 1 8 19 1 14 Apr 18 22 15 Apr 25 30 19 2 pp 863 875 19 3 pp 876 886 Review Final Exam Combined Section TBD Scheduled during finals week