## 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 (K

_{c}and K_{p}), 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 K

_{c}and K_{p};## 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 K

_{w};## 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 K

_{a}or K_{b}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 K

_{w};## 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 K

_{a}or K_{b}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 K

_{a}or K_{b}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 H

^{o}_{rxn}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 S

_{universe}and spontaneity;## calculating S

^{o}_{rxn}for a chemical reaction;## relating GS

^{o}_{rxn}to spontaneity of a chemical reaction;## calculating G

^{o}_{rxn}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.