First-Year Chemistry - Section 001 - 2011 Winter Term
Intermolecular Forces, Chemical Kinetics, Equilibrium, Electrochemistry


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Chem 123 Section 001 Bulletin
Website last updated at 2011-04-05 18:45

 

 

 

PLEASE NOTE:  There is now a clear correlation between those who did well in the course to those who show up and learn in class.  Set aside "Chemistry" time in your busy schedule to study just this course.  Be consistent, keep up with your weekly work, and you will do well.

PLEASE NOTE:  There will be increased security at the exam sites.  Unlike high schools, UW does not tolerate academic misconduct.  If you get caught cheating, you will be expelled.  Don't do it!

 

 

LECTURE MATERIALS

 

Supplementary materials for the lectures will normally be loaded 24 hours before the lecture as we proceed.
Please check the table below.

 

  Practice problems for Edition 9 textbook -  Download list here

 

 

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PLEASE GO TO UW ACE FOR DETAILS OF FINAL EXAM AND THE SITTING ARRANGEMENT FOR THE PAC.

 

 

Week CLASS LOG:  What have we learned today? Reading Assignment HANDOUT
1 <Jan 5>  Course outline & scope | MODULE 1 (6): Phases and phase diagram of one-component system |
<Jan 7>
  Critical point | Triple point & supercritical fluid | CO2 vs H2O phase diagrams || Vapour pressure vs temperature curves & Clausius-Clapeyron equation
Chapter 12 Phase diagram
Vapour pressure
Triple point cells: Part I;Part 2
Supercritical fluid
Clausius-Clapeyron equation - Part 1; Part 2
Course outline
Water phase diagram.pdf
 
2 <Jan 10>  || Intermolecular forces | Dipole-dipole forces | London dispersion forces | Hydrogen bonding forces
<Jan 12>    | Examples of using these concepts to predict B.P & V.P. trends || Heating curves || Crystalline and amorphous solids | Bonding classification | Classification by Symmetry
<Jan 14>
 | Cubic unit cells: sc, bcc, fcc - number of atoms/unit cell, edge length, packing efficiency || Closest packed structures: hcp vs ccp
Chapter 12
Chapter 14
Intermolecular forces - General
Intermolecular forces - Materials
Lattice structures - Part 1
Lattice structures - Part 2: Holes and Ionic Structures
Crystalline solid classification.pdf
Packing efficiency.pdf
Sizes of holes.pdf

Structures of ionic solids.pdf
3 <Jan 17>  | Density of crystalline solid || Ionic solids and interstitial sites | Example | Tetrahedral, octahedral and cubic holes | Summary of ionic solids
<Jan 19>  || Born-Haber cycle and lattice energy || MODULE 2 (6): Chemical kinetics | Factors affecting rates of chemical reactions
<Jan 21>  || Quantifying reaction rate: Average vs instantaneous rates | Example | IUPAC definition of rate of reaction || Rate laws for chemical reactions - focus on decomposition reaction | Method of initial rates
Chapter 14 Introduction to Kinetics Module 2 examples.pdf
4 <Jan 24>  | Example | Integrated rate laws | Zero-order reaction | First-order reaction | Second-order reaction | Two examples || Analysis of concentration vs time data: Algebraic vs graphical approach 
<Jan 26>  | Two examples || Half life | Example || Summary || Reaction mechanisms
<Jan 28>  | From mechanism to rate law | Example to illustrate Steady State Approximation
Chapter 14
Chapter 15
Reaction mechanism

Factors affecting reaction rate

Reaction rate laws.pdf
Reaction mechanism.pdf
5 <Jan 31>  | Four examples | Justifying SSA ||Temperature effect on reaction rate
<Feb 2>  | Example || Catalysts | Example || Comments on mutlistep reactions 
<Feb 4>  MODULE 3 (4): Chemical equilibrium | Balance of reaction rates || Law of chemical equilibrium: Reaction quotient & equilibrium constant | Example & concept of dynamic equilibrium
Chapter 15
Chapter 16
Glowstick Demo

Chemical Kinetics -Summary

Catalysis
Module 3 examples.pdf
6 <Feb 7>  | Rules & conventions for Qc & Kc || Equilibrium problems | General example | Two examples to illustrate approximations
<Feb 9>  | Method of successive approximations || Gas-phase equilibria | Example || Manipulating reactions & equilibrium constants | Example || Le Chatelier principle
<Feb 11>  || Temperature dependence of K  | Example || Van't Hoff equation | Example MODULE 4 (4+5): Acids, bases and conjugate acid-base pairs
Chapter 16 Chemical Equilibrium - Part I,  Part II
 Le Chatelier's Principle
Le Chatelier's Principle - Demo
Chemical Equilibrium - Demo
Temperature Dependence of Equilibrium
Rules on K & Qc.pdf
7 <Feb 14>   | Self ionization of water & ion product of water & Kw | Example | The pH Scale || Ionization of acids and bases in water | Acidic, basic and neutral solutions | Acid ionization contants Ka & base ionization constants Kb  
<Feb 16
>   | Common strong acids & common strong bases | 2 examples on strong acid and strong base
<Feb 18>
 Early study break - No lecture
Chapter 16
Chapter 17
 Acids and Bases and You
 Acids and Bases
Strong Acid
Weak Acid
Weak Base
Module 4 examples.pdf
8 <Feb 21>  Reading week - No lecture
<Feb 23>  Reading week - No lecture
<Feb 25>
 Reading week - No lecture
Chapter 17    
9 <Feb 28>   2 examples on weak acid and weak base || Molecular structure & acid strength | Binary acids |
<Mar 2>  Term test
<Mar 4>
 Oxo acids || Polyprotic acids (H2A, H3A, etc.) | 2 examples || Systematic treatment of equilibrium
Chapter 17    
10 <Mar 7>  | 2 examples || Conjugate acid-base pairs revisited || Salt solutions
<Mar 9>  | 2 examples | Salts derived from polyprotic acids | Example || Common ion effect
<Mar 11>
 | Example || Acid-base neutralization reactions | Example || Buffer solutions | Example
Chapter 20 Conjugate Acids and Bases
 pKa and pKb
Buffers
Buffers - II
Module 4 Supplemental.pdf
11 <Mar 14>  | Preparation of a buffer solution | 2 examples | Buffer action | Example || Acid-base titrations
<Mar 16>  | Example
<Mar 18>
 | Chemical indicators for acid-base titrations | Example || Summary | 2 examples |  MODULE 6 (4): || Electrochemical cells | Redox reactions | Electrochemical cells: galvanic vs electrolytic

Chapter 20
Strong Acid Titration
Weak Acid Titration
 Equivalence Point
Titraton Summary
Module 6 examples.pdf
12 <Mar 21>  | Cell diagram | Salt bridge || Cell Potential  || Standard hydrogen electroded (SHE) | standard electrode potentials
<Mar 23>  || Using standard reduction potentials to calculate cell potential | Example | Sign of Eo
<Mar 25>
  | Oxidizing & reducing agents | Example || Nernst Equation | 2 Examples || Electrochemical cells & equilibrium |
Chapter 20
Chapter 18
Galvanic Cell Module 5 examples.pdf
13 <Mar 28>   2 Examples || Electrolytic cells & eletrolysis | MODULE 5 (4): || Ionic equilibria | Introduction to sparingly soluble salts | Molar solubiility & Ksp | Example | Example on common ion effect
<Mar 30>
  || Precipitation | Example | Selective precipitation | Example
<Apr 1>
 | Factors affecting solubility | pH effects: example | Complexing agents: example || Review |
Chapter 18    
14 Lectures are DONE!  Good luck with the exam!      

<Apr 20>  9:00-11:30 am @ PAC Final examination 

 


 

Frequently Asked Questions


Does one need to buy the textbook?   Yes.

Problems in downloading pdf files?
<1> Make sure your PDF reader is up to date - If not, go to the Adobe site and get the latest reader.  
<2> Try right-click on the filename, select either <Save target as...> or <Save link as...> (depending on which browser you are using) and save this file in a directory that you can read back later.
<3> If everything fails, call/e-mail me and I shall give/e-mail you a copy.
<4> There is a hardcopy of the solution manual at the library.

Mark review policy  Please refer to UW-ACE for any official policy.

 

EXAM INSTRUCTIONS Despite after Chem 120 and both term tests of Chem 123, there are still some students who don't want to follow the instructions on the exam in filling out the computer card and the exam paper.  In the final exam, the Chem 123 policy is that if the computer card and exam paper are not filled out according to the instructions (e.g. missing section number, missing name written in pen, missing id, etc), these will be thrown out and the student will get zero automatically on this exam.  There will be zero tolerance on this.  By now, we must learn how to follow the instructions, as there will no one there to bail us out from now on.  Please read and follow the instructions carefully.

 

The THREE Golden Rules in Writing Exam
(1)  Upon receiving the exam, write down what you know - your name, student id, test version number, course number, session number - This will calm your nerves as these are info you know you will get right!  And, this will allow you time to do the last-minute things at the end of the exam.
(2) In the first 5 minutes of the exam, scan over the complete exam once and identify the easy questions - This will allow your unconscious mind to work on the questions.  Select and do the easy questions first.
(3)  In the last 5 minutes of the exam, where applicable, cross out any junk that you have written down - This will help to clear your thought and to minimize infuriating the marker.  A messy paper obscures the real solutions - even if you might have written the solution down somewhere, the marker usually gives up and marks the question wrong if  the answer cannot be found in the first 10 seconds.  On the other hand, a "neat" and logically presented paper always wins gravy points from the marker.