CHEM 1212 Lesson Objectives, Fall 2008 (Dr. Pennington)
Lesson
Reading
Assignment
1
 13.1
Lesson Objectives Description
Introduction to CHEM 1212 and Dr. Pennington
Describe the energetics of solute/solvent interaction during the dissolution process (Hsoln = H1 + H2 + H3).
Predict entropy changes in chemical reactions.
Discuss solution formation with respect to the enthalpy and entropy changes involved.
Differentiate between unsaturated, saturated and supersaturated solutions.

Be able to calculate when you have examples of each solution type.
Discuss crystallization with respect to saturated and supersaturated solutions.
2
 13.2 - 13.3

Predict relative solubilities of solutes in given solvents based on the following:
i. Solute / solvent interactions
ii. Pressure Effects (know the Henry's Law equation (and its terms) and be able to perform calculations using it)
iii. Temperature Effects
Express and calculate solution concentrations using the following units, and be able to convert between them:

3
 13.4
i. Mass Percent
ii. Parts per million (ppm)
iii. Mole Fraction
Quiz #1
iv. Molarity
v. Molality


4
 13.5 - 13.6
Describe Colligative properties with respect to each of the following (and be able to perform calculations with each):
i. Vapor-Pressure lowering
ii. Boiling Point Elevation
iii. Freezing Point Depression
Quiz #2
iv. Osmosis
Determine the Molecular Weight (molar mass) of a sample using colligative property data
Describe the four factors that affect reaction rates
 14.1 - 14.3
5
Calculate the average and / or instantaneous rate of a chemical reaction
Calculate relative reaction rates using reaction stoichiometry
Describe the concept of the rate law
Determine orders and the rate law for a chemical reaction.
1
Differentiate between first and second order reactions.
6
 14.4 
Use integrated rate laws in first and second order reactions.
Differentiate between graphical representations of first and second order reactions.
Quiz #3
Determine half-lives of first and second order reactions.
Describe activation energy and how it relates to temperature change in chemical reactions.
7
 14.5 - 14.6
Use the Arrhenius Equation to calculate the Activation energy for a chemical reaction.
Describe rate laws for elementary processes
Determine the rate law for a multi-step reaction.
Describe how catalysts speed up chemical reactions.
8
 14.7
 15.1 - 15.2
Quiz #4
Discuss how enzymes work.
Describe the concept of a dynamic equilibrium in terms of forward and reverse reactions.
Use the Haber process to describe the concept of the equilibrium concept
Write equilibrium expressions for chemical reactions.
9
 15.2 - 15.3
Differentiate and calculate between equilibrium constants and expressions in terms of concentration and pressure.
Describe the magnitude of the equilibrium constant and what it means in terms of the direction the reaction flows.
Perform calculations involving K
10
Exam #1 (Chapter 13, Chapter 14, Chapter 15.1-15.3)
Write equilibrium expressions for chemical reactions that exist in more than one phase (heterogeneous equilibria)
11
 15.4 - 15.6
12
 15.6 - 15.7

Quiz #5
Use ICE tables to calculate K values from initial and equilibrium concentrations.
Use ICE tables to calculate equilibrium concerntrations.
Predict the direction that an reaction will shift in order to reach equilibrium, using the reaction quotient (Q).
Use Le Chatelier's Principle to predict the direction that an equilibrium will shift when a change is made to it.
Describe basic differences between acids and bases.
Describe acid-base reactions in terms of Lowry-Bronsted acids and bases.
13
 16.1 - 16.4
Identify conjugate acids and bases.
Compare relative strengths of acids and bases.
Describe the autoionization of water, and calculate [H+] and [OH-] in a solution using it.
Define pH and describe the pH scale.

Describe how to measure pH (pH meter, indicators, pH paper)
Know the 7 strong acids and bases.
14
 16.5 - 16.6
Calculate pH's of strong acids and bases.
Compare ionization of strong vs. weak acids.
Quiz #6
Calculate the Ka of a weak acid.
2
15
 16.6, 16.7
16.19
Compare Ka (weak acids ) with Kb (weak bases).
Perform calculations involving Kb
Determine the acidity of a solution based on the salts it contains.
 16.11
16
 17.1 - 17.2
Define Lewis acids and bases.
Explain the common ion effect and how it affects acidity (Le Chatelier's Principle).
Calculate the pH of a weak acid when a common ion is involved.
Quiz #7

17
 17.1 - 17.2
Explain how buffers work, and what they are made up of.
Calculate the pH of a buffer.
Calculate pH changes in buffers when small amounts of H+ / OH- are added.
18
 17.3
Quiz #8
Describe acid-base titrations.
Perform acid-base titration calculations.
Describe graphical representations of acid-base titrations
19
 17.3 - 17.4
Describe the solubility product constant (Ksp)
Perform calculations involving solubility and Ksp.
20
Exam #2 (Chapter 15.4-15.7, Chapter 16, Chapter 17)

Define spontaneous and nonspontaneous processes.
Identify processes as spontaneous or nonspontaneous.
21
 19.1 - 19.2
Define the term 'entropy' (S).
Define the 2nd Law of Thermodynamics and how it relates to entropy.
Predict which samples will have the higher / lower entropy
Predict entropy changes in chemical reactions.

22
 19.3
Quiz #9
Compare entropy with probability, and the concept of 'microstates'.
Describe the 3rd Law of Thermodynamics
Define standard molar entropy of a substance.
Calculate entropy changes (S) in chemical reactions.
23
 19.4 - 19.5
Describe Gibbs Free Energy (G), its importance in spontaneity, and its dependence on H and S.

Define Standard Free Energy of Formation for a substance.

Calculate standard free energy changes for chemical reactions.
Describe the effect of temperature on free energy and spontaneity.
3
Determine oxidation states of species in redox reactions.
24
 20.1 - 20.2
Quiz #10
Determine oxidizing and reducing agents in redox reactions.
Balance redox reactions using the half-reaction method.
Draw a diagram of a galvanic cell and its essential components; describe the purpose of each component.
25
.3
Identify which way electrons will flow in a galvanic cell.
Describe, at the molecular level, what is happening at the electrodes in a galvanic cell.
Use standard reduction potentials to calculate the cell potential (E cell) of a particular galvanic cell.
26
 20.4 - 20.5  Compare relative strengths of oxidizing and reducing agents in galvanc cells.
Use standard reduction potentials to determine if a redox reaction is spontaneous or not.
Quiz #11
Describe the make-up of a concentation cell, and how it works.
27
Exam #3 (Chapters 19 and 20)
28
Final Exam Review
29
Final Exam Review
4