Chem 120 - SECTION 004 - General Chemistry (Fall 2003)
      

Chem 120 - Section 004 - Bulletin
Website last updated at 2010-02-11 11:45

 

Study hard now and keep up with the problem sets below.  You have one last chance to prove yourself.

 

Coming soon

 

   FINAL EXAM: Thursday Dec 11 2-5 pm at PAC Area 1-12

More details about the final exam will be avaiable at the main C120 website.  Always trust the main C120 website.

Contrary to what I told the class on the last lecture, there will be different versions of the final exam.  Please follow the instructions carefully and make sure that the correct  CARD number (= VERSION) is used.

 

 

 About the webpage background - Scanning Electron Micrograph of Cobalt Nanogarden  - Part of the WATLabs' Nanotechnology program
Download a WATLabs promo 

 

Week CLASS LOG:  What have we learned today? Reading Assignment Problem Set
(Do not hand in)
1 <Sept 8>  General C120 and C120L info booklet, web-based materials || Course content ||  What is Chemistry? || More detailed summary of topics - Course action plan
<Sept 10>
 Periodic table - general reference to Ch 1 and 2. || Introduction to Stoichiometry || Law of Conservation of Mass || Law of Definite Proportions || Atomic Molecular Theory || Law of Multiple Proportions 
<Sept 12>
 Empirical formula and molecular formula || Concept of Molar Mass. An example || The Mole concept and the Conservation of Moles  
Ch 1-4

Chapter 2: 3, 7, 13, 21, 32, 55, 66, 67, 69, 80, 82, 86
Chapter 3: 3, 6, 7, 12, 21, 22,-24, 37, 38, 45, 46, 51, 53, 58, 60-62, 67, 68, 71-78, 83, 95, 96, 98, 100, 102, 106, 109

2 <Sept 15>  Microanalyses - volumetric and gravimetric analyses || Some examples on Stoichiometry
<Sept 17> 
Introduction to Solution Stoichiometry ||  What is a solution? || Defining the composition of a solution
<Sept 19>  
Two examples on Solution Composition || Concept of Solubility || What does Solubility depend on? Solute, Solvent, Temperature - Some examples
Ch 5

Microanalyses

 
Solution Composition

Solubility rules

Solubility and Reaction

Examples

Chapter 4: 5, 6, 10, 16, 18, 19, 23, 24, 25, 26, 27, 29, 36, 37, 44, 46, 51, 52, 54, 57, 58, 67-71, 75, 77, 80, 83, 85, 87, 88, 93, 96, 100
Extra B1, B2

3 <Sept 22>  General classification of typical reactions || Gravimetric and volumetric analyses || Practical examples about solution stoichiometry || Redox Stoichiometry || Define Red-Ox
<Sept 24>
 Define oxidation no. || Examples about oxidation no. || Examples on how to determine Oxidation number || The recipe for balancing Redox reactions || One practical example
<Sept 26>
 One more practical example on balancing redox reaction || Overview of Thermodynamics
Ch 5, 6

Oxidation Number

Gases-1

Gases-2

Chapter 5: 7, 14, 18, 21, 24, 25, 26, 27, 36, 38, 43, 46, 51-54, 57, 62, 65, 71, 73, 75, 89, 91, 94, 96, 97
Extra B3, B4, B5, B6

4 <Sept 29>  Bulk phases || Thermodynamic variables: P,V,T,n || Equation of state: PV = nRT || Introduction to gases and their laws || Ideal gas law and its deviations (compression factor Z)
<Oct 1>
 Ideal gases and their "non-ideal" behaviour || Practical examples involving ideal gases
<Oct 3>
 One more example on Gas Stoichoimetry || Mixtures of gases: Dalton's law of partial pressure || An example on mole fraction and partial pressure || Vapour pressure 
Ch 7

 

Chapter 6: 7, 8, 10, 13, 16, 17, 19, 21-24, 39, 41, 45, 46, 48, 52, 55, 57-64, 71, 74
Extra B7, B8

Chapter 6:   75, 79, 82, 83, 86, 90, 94, 96, 99, 103, 107, 109

5 <Oct 6>    Speed of particles in a gas || Diffusion and effusion || Graham's law of effusion
<Oct 8>
  Term Test #1 - For sample term test, please see the main C120 website.
<Oct 10>
  Concepts of Internal Energy, Work and Heat || Some examples || First law of thermodynamics || Example of using the first law
Ch 7, 9

Thermo


Chapter 7: 3, 8, 10, 13, 14, 17, 19, 21, 22, 24-26, 29, 31, 33, 36, 37,
40, 44, 48, 55, 57, 60, 62, 64, 67, 69

6

<Oct 13>  Thanksgiving Holiday - No lecture
<Oct 15>  
Enthalpy of physical changes || Enthalpy of chemical changes
<Oct 17>
 Standard enthalpy of formation || Reference states || Some examples || Hess' Law || Some examples on Hess' Law

Ch 9 Chapter 7: 73, 74, 76, 78, 80, 82, 87, 91, 94, 97, 98, 103, 106, 113
Extra B9
7 <Oct 20>  Comments on heat capacity || Bomb calorimeter  || Two examples on heat capacity 
<Oct 22>  
What is "classical" Quantum Theory? || Black body radiation and quantization of energy
<Oct 24>  
Photoelectric effect, electron diffraction and wave-particle duality || Line spectrum of the hydrogen atom and the Bohr model of the atom
Ch 9, 10
Quantum Theory
Chapter 9: 13, 16, 17, 22, 23, 31, 36, 41, 45, 49, 53, 54, 57, 61, 66, 71, 72, 73, 83, 84, 85, 86, 88, 90, 92, 93, 104, 109
8 <Oct 27>  Introduction to Wave Mechanics || Schrodinger equation || Operator and Wavefunction || Heisenberg Uncertainty Relation 
<
Oct 29>
  Atomic orbitals and quantum numbers || More discussion on orbitals and their densities
<Oct 31>
 
More on general observations about atomic orbitals || Many-electron system
Ch 10, 11

Wavefunctions


Extra B10-B3

9 <Nov 3>  Pauli exclusion principle || Electronic configuration and general observations || 

Building-up principle - Aufbau Principle
<Nov 5> 
Hund's rule || Example on electronic configuration and orbital diagram || Exception to Aufbau Principle || Examples of electronic configurations and orbital diagrams of ions || Magnetism of many-electron atoms
<Nov 7> 
Trends associated with various properties listed in the periodic tables || Atomic radius || Ionic radius || Ionization energy || Electron Affinity

Ch 11

Chapter 10: 3-5, 9, 11, 12, 16, 27, 28, 30, 40, 51
Extra B14

10 <Nov 10>  Chemical bonding: Ionic, covalent and metallic bonds
<Nov 12>  Term Test #2  -
For sample term test, please see the main C120 website.
<Nov 14>
  
Concepts of bond length and bond energy || Example || Ionic bonds ||  Formation of ion pair || Lattice energy || Ionic vs convalent bonding || Electronegativity
Ch 11, 12

Atomic Properties

 

Chapter 11: 2, 3, 9, 10, 12, 14, 15, 22, 24, 25, 27, 28, 31, 33, 45, 46, 47, 51, 52, 53, 57, 58, 62, 67, 68, 71, 72, 79, 80, 82, 83, 88, 91, 95,  99, 104, 108
Extra B15

11 <Nov 17>  Electronegativity || Dipole moment || Lewis theory of covalent bonding - assumptions || Recipe for Lewis structure || Formal charge || Bond order
<Nov 19>
 
Some examples on Lewis structures, and formal charges || Some examples on Lewis structure, formal charge, bond order || Stabilities of Lewis structures || Resonance structures and resonance hybrids || Exceptions to Octet rules
<Nov 21> 
Valence Shell Electron Pair Repulsion Theory || Basic ideas as an enhancement to the Lewis structure theory || Recipe || VSEPR pairs to basic configuration to geometry || Refinement || Some examples
Ch 12


MO Theory

Chapter 12: 6, 9, 11, 13, 14, 17, 18, 25, 27, 29, 31, 36, 38, 40, 42, 45, 48, 51, 69, 70, 75, 76, 80, 82
Extra B16-B20

12 <Nov 24>  Valence bond theory || Diatomic molecules: concept of sigma and pi bonds
<Nov 26>  
Polyatomic molecules: concepts of promotion and hybridization || Different types of hybrid orbitals for sigma bonding || Molecular orbital theory || Why is it necessary?
<Nov 28>  
Basic features of MO theory of diatomic molecules || Concepts of bonding, antibonding and non-bonding orbitals || Linear Combination of Atomic Orbitals ||
Ch 1-7, 9-12  
13 <Dec 1>  MO diagrams of diatomic molecules (H2, N2, O2, CO) || Electronic configurations || Paramagnetism of O2 || Course wrap-up - Course review:  What's on the Final Exam?    

Final examination:  Dec 11 2-5 pm at PAC GYM & MC

 



Frequently Asked Questions


Does one need to buy the textbook?   Yes.  But any older version of the same book would be OK.

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.
 

Three golden rules in writing exams

<1> Write down your name and ID on all the relevant exam papers and booklet and computer card - these are materials that you know are correct!
<2> Spend the next few minutes to read through the entire exam paper calmly and make sure that there is no missing page.  Identify the easy questions and do these first.

<3> Near the end of the exam, cross out messy stuff and identify your answers clearly.  Try to be as neat as possible in your final presentation of your answers.