CHEM 1062 - Principles of Chemistry II

• CHEM 1061  required.

AND

• Placement into MATH 0120 /MATH 1200 , or appropriate math placement score, or equivalent

1. At the conclusion of the lecture portion of this course, learners will demonstrate competency in the following areas:
   • Organic Chemistry
     • Draw structural formulas, condensed structural formulas, and skeletal (line-bond) structures of organic compounds.
     • Identify the structures of common functional groups such as alkene, alkyne, alcohol, ketone, etc.
     • Given the structure of an organic compound, write its IUPAC name (and vice-versa).
   • States of Matter: Intermolecular Forces, Liquids, and Solids
     • Identify the dominant intermolecular force for a molecular compound.
     • Make qualitative predictions (rankings) concerning the physical properties (such as melting point, boiling point, viscosity, surface tension, vapor pressure, etc.) of various liquids on the basis of their intermolecular forces.
     • Describe the molecular interactions that differentiate solids, liquids, and gases.
     • Describe and calculate the energies of phase changes.
     • Identify phase changes and interpret phase diagrams.
   • States of Matter: Solutions
     • Describe the energetics of solution formation.
     • Calculate and convert between the solution concentrations of percent, molarity, molality, and mole fraction.
     • Describe and perform mathematical calculations of solution colligative properties (such as vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure).
   • Kinetics
     • Determine the order of a reaction from the rate law.
     • Apply the integrated rate law and half-life equations for zero-order, first-order, and second-order reactions.
     • Describe how temperature, activation energy, and molecular orientation influence reaction rates, including the Arrhenius equation.
     • Determine the rate law from a reaction mechanism.
     • Describe how a catalyst influences the rate of a reaction.
   • Equilibrium: General
     • Write equilibrium constant expressions for chemical equations and find equilibrium concentrations from initial concentrations and the equilibrium constant.
     • Determine the effect of concentration change, volume change, temperature change, and addition of a catalyst on equilibrium using Le Chatelier’s Principle.
   • Equilibrium: Acid-Base
     • Define and identify acids and bases using the Arrhenius, Brønsted-Lowry, and Lewis definitions; relate strengths of acids and bases to their conjugate pairs.
     • Analyze equilibria of acids and bases using acid and base dissociation constants.
     • Calculate pH of acids, bases, and buffer solutions and construct acid/base titration curves.
   • Equilibrium: Solubility
     • Calculate Ksp using solubility data.
     • Use Ksp to determine solubility of pure compounds and in the presence of a common ion.
     • Describe the factors that affect solubility, including the common ion effect, pH, and complex ion formation.
   • Equilibrium: Electrochemistry
     • Determine oxidation numbers and balance aqueous redox reactions in acidic and basic solutions.
     • Calculate standard potentials for electrochemical cells and relate to standard free energy, potentials under nonstandard conditions, and the equilibrium constant.
   • Equilibrium: Thermodynamic Foundations
     • Calculate ΔH, ΔS, and ΔG for phase transitions and chemical reactions, using appropriate standard values from thermodynamic tables. This includes finding the temperature range (and the value of T), over which a reaction is spontaneous.
     • Apply the relationships between thermodynamic quantities such as enthalpy, entropy, and Gibbs energy, and the direction of change in natural processes.
     • Predict, on the basis of qualitative reasoning, the sign of ΔS for reactions and phase transitions.
     • Relate thermodynamic data (ΔH, ΔS, and ΔG) to the value of the equilibrium constant for a reaction (and vice versa).
   • Nuclear Chemistry
     • Write balanced nuclear equations.
     • Identify types of nuclear reactions including radioactive decay, fission, and fusion.
     • Analyze first-order decay of radionuclides.
2. At the conclusion of the laboratory portion of this course, learners will demonstrate competency in the following areas:
   • Conduct laboratory work in compliance with guidelines for personal lab safety and responsible management of chemical waste; this includes appropriate use of personal protective equipment and interpretation of Globally Harmonized System for Hazard Communication (GHS) labels.
   • Measure quantities such as mass, volume, temperature, and absorbance with proper technique, and record the results of measurements with the appropriate number of significant figures and units.
   • Record observations of chemical processes (such as precipitate formation, gas evolution, etc.) and write chemical reactions consistent with their observations.
   • Use proper techniques for laboratory procedures, such as titration, filtration, solution preparation, spectrophotometric measurements, etc.
   • Properly use glassware and equipment including beakers, Erlenmeyer flasks, volumetric pipets, burets, volumetric flasks, watch glasses, graduated cylinders, filtration apparatus, single-beam spectrophotometer, pH meter, and balances.
   • Effectively communicate lab procedures, observations, and results in the form of a laboratory notebook, written reports, and a verbal presentation.
   • Interpret and analyze qualitative observations and quantitative results, incorporating graphs and tables as appropriate.

1. Major Areas of Lecture Content
   • Organic chemistry including functional group identification and nomenclature
   • Liquids and solids including phase diagrams, intermolecular forces, and unit cells
   • Solutions including solubility theory, concentration units, and colligative properties
   • Kinetics including reaction orders, integrated rate laws, half-lives, reaction mechanisms, and activation energy
   • Equilibria including equilibrium calculations and Le Chatelier’s principle
   • Acids and bases including theories, strength, pH and concentration calculations, titration curves, and buffers
   • Solubility equilibria including basic solubility product calculations and common ion effect
   • Thermodynamics including laws, entropy, Gibb’s free energy, spontaneity, and relation to equilibria
   • Oxidation-reduction including balancing redox reactions, cell potentials, electrochemistry, and Nernst equation
   • Nuclear chemistry including types of radioactivity, radioactive decay, fission, fusion, transmutation, and mass defect
2. Major Areas of Laboratory Content
   • Use of a chemical structure drawing program
   • Organic functional group identification
   • Solution properties, e.g. solubility
   • Colligative properties
   • Kinetics
   • Equilibrium
   • pH and titration curves
   • Redox
   • Laboratory project and presentation