Chapter 10 Sections 1, 3 and 4: You must be able to draw and interpret Lewis structures; you must be able to predict molecular and electron-pair geometries of 'simple' molecules, determine bond angles and numbers of bonding and nonbonding electrons; and you must be able to predict the polarity of 'simple' molecules. (As review for the material we covered in Chapter 12.)
Chapter 12 Sections 1 - 6
kinetic-molecular (atomic level) view of matter;
phases and phase changes;
cooling/heating curves;
vapor pressure and the Clausius-Clapyron equation;
phase diagrams;
types of intermolecular attractive forces;
properties of liquid state and water;
types of crystalline solids;
simple cubic, body-centered cubic and face-centered cubic cells and density calculations.
Problem Sets 1, 2 and 3. (Review Problem Set problems 1a, 1b, 1f, 1g, 2, 8.) Blank copies of the problem sets and answers are at the Problem Set link.
Lecture notes for Wednesday, August 22 - Monday, September 10.
Help Sessions on Monday, August 27th, Monday August 29th, Wednesday, September 5th and Monday, September 10th.
Pre/post-Lectures Explorations #1 - 6, and In-Class Activity #1. Check the expert's responses to the explorations and In-Class Activity.
Chapter 10: Problems 10.61, 10.62, 10.64 - 10.67, and 10.84.
Chapter 12: Problems 12.1 - 12.4, 12.7, 12.8, 12.12, 12.13, 12.15, 12.16, 12.18, 12.19, 12.20, 12.21, 12.22, 12.23, 12.24, 12.25, 12.26, 12.28, 12.30 - 12.55, 12.69, 12.78, 12.83, 12.84, 12.86, 12.88, 12.93, 12.98, 12.99, 12.110b - d, 12.117, 12.121, 12.126, 12.140.
Section 1 - 5 (we did not discuss osmotic pressure in Sec 5, or colloids in Sec 6.)
types of solutions
predicting and explaining solubility
solution process and heats of solutions
temperature dependence of solubility
concentration expressions
colligative properties of nonelectrolytes, weak and strong electrolytes
Section 1 and 2 (only that material pertaining to alkanes and structural isomers)
Lewis structures of alkanes
nomenclature of alkanes (methane to decane)
structural isomers of alkanes and halo-substituted alkanes
Section 1 - 8
average, instantaneous and initial rates
initial rate method for determining the differential rate law (order and rate constant)
simple reactions
integrated rate law
graphic determination of the order of simple reaction
Collision Theory
Transition State Theory, activation energy, activated complex
Arrhenius equation
mechanisms, rate determining step, molecularity
catalysis
Sections 1 - 6
Meaning of the equilibrium constant (Kc and Kp), equilibrium constant expression, and the non-equilibrium reaction quotient (Q);
how K is effected when the chemical equation is reversed or multiplied by a coefficient;
determining new K from an overall reaction;
equilibrium reactions containing solids or liquids;
relationship between Kc and Kp;
predicting direction of chemical reactions/comparing Q and K;
solving for the equilibrium constant for a reaction;
solving for the equilibrium concentration of all species;
using the quadratic formula to solve for equilibrium concentrations of all species;
Le Chatelier's Principle;
using the van't Hoff equation.
Sections 1 - 5
Arrhenius definition of acids and bases;
memorize the strong acids and the strong bases discussed in class;
autoionization of water and Kw;
pH, pOH and pK;
Bronsted-Lowry definition of acids and bases;
conjugate acid-base pairs and relative strengths of BL acids and bases;
writing the equilibrim chemical equation and the equilibrium expression for any acid or base that dr. g. can imagine;
calculating Ka or Kb given initial concentrations and pH;
calculating pH given intial concentrations and K;
calculating pH for diprotic or triprotic acids;
writing the chemical equation that describes how the salt behaves as an acid or base;
Experiment #2:Qualitative Cation Analysis;
Survival Organic Chemistry: Hydrocarbons/alkenes, alkynes, aromatics, alcohols, carboxylic acids and amines;
Experiment #8: Photometric Determination of an Equilibrium Constant;
Experiment #3: Preparation of Aspirin.
Sections 1 - 7 (Note: even though Sections 1 - 5 were covered on Exam III, this material is still important to understand salts, common ions, neutralization reactions and buffers.)
Arrhenius definition of acids and bases;
memorize the strong acids and the strong bases discussed in class;
autoionization of water and Kw;
pH, pOH and pK;
Bronsted-Lowry definition of acids and bases;
conjugate acid-base pairs and relative strengths of BL acids and bases;
writing the equilibrim chemical equation and the equilibrium expression for any acid or base that dr. g. can imagine;
calculating Ka or Kb given initial concentrations and pH;
calculating pH given intial concentrations and K;
calculating pH for diprotic or triprotic acids;
writing the chemical equation that describes how the salt behaves as an acid or base;
trends in the strength of hydrohalic acids and oxy-acids;
acid-base properties of salt solutions;
calculating Ka or Kb for salts;
Sections 1 - 2 (Note: Our textbook takes a different approach to buffer solutions than we have. You are responsible for solving neutralization and buffer problems the way I described them in class and as shown in our problem sets. The Henderson-Hasselbalch equation has not been discussed in class, so do not use it when solving buffer problems.)
pH calculations of weak acid and its conjugate base (common ion);
pH calculations of weak base and its conjugate acid (common ion);
predicting the products of neutralization reactions;
calculating the K for a neutralization reaction;
titration curves of strong acids and strong bases;
titration curves of weak acids and strong bases;
calculating the pH at any point on a titration curve;
determining the reagents and concentration to prepare a buffer of a particular pH;
pH calculations of buffer solution;
effect on the pH of a buffer solution upon addition of a strong acid or a strong base;
Sections 1 - 4(Note: How far we get in this chapter will be determined on Friday, December 7, 2001)
predicting spontaneous change based on your chemical experience;
calculating Horxn for a chemical reaction;
predicting the sign of S for a chemical reaction/change;understanding the concept of dissorder as it relates to physical state, temperature, solutions and molecular complexity;
the relationship between Suniverse and spontaneity;
calculating Sorxn for a chemical reaction;
relating GSorxn to spontaneity of a chemical reaction;
calculating Gorxn for a chemical reaction;
Experiment #9: Potentiometric determination of a weak Acid equilibrium Constant (Important);
Experiment #3: Preparation of aspirin, and titration of an aspirin tablet;
Experiment #6: Colorimetric Determination of Phosphate ion in water;
Experiment #2: Qualitative Anion Analysis;
Web Experiment: Metal/Metal Ion Reactions (Introduction to the Activity Series)
Review previous exams to be sure you understand and are able to do problems that were missed on the first three hour examinations. If you missed a question on Exam I - III you should review that material. Some of the problems on the comprehensive final could be different fromthe problems on the hour exam. Additionally, Exam V could cover questions since Exam III that are not covered on Exam IV.