CHEM 102/105 Section H1 Course details

Standard scientific calculators may be used, but those with extensive alphanumeric capabilities may not be used. A data sheet will be provided.
Requests for a regrade must be made before the lecture following the return of the exams. The entire exam will be regraded, not just the challenged portion; therefore, your score may go up or down. Only exams that are written in ink may be regraded.
Excused absences from midterm exams will be given only if supported by a University of Alberta Medical Statement form, obtained from University Health Services. Notes from a private doctor or medical clinic should be taken to University Health Services. In case of an excused absence on the midterm exam, the grade weight will be transferred to the final exam.
Unexcused absence will result in a grade of ZERO on the midterm exam.
A deferred final exam for all sections of CHEM 10X will be held on Friday, May 2, 2003, 09:00-12:00. Application for a deferred final exam must be made through the Registrar's office; see the University Calendar for regulation details.

Grading

	CHEM 102	CHEM 105
Midterm exam	25 %	30 %
Final exam	45 %	50 %
Laboratory	30 %	20 %

Assignments

Suggested problems from the textbook will be given during each lecture. These will not be graded, but you are strongly advised to work through them. The solutions to these problems may be found in the textbook solutions manual and will also be posted on the notice board outside W3-60. Additional problems will be assigned periodically and the full solutions will be distributed in class and posted on the notice board and on the course web site.

You are also strongly encouraged to read the relevant sections of the text prior to each lecture.

Course outline

Numbers in parentheses refer to sections in the text.

States of Matter
Ideal gases (5.3, 5.4)
Partial pressures and Dalton's law (5.5)
Kinetic molecular theory of gases (5.6)
Intermolecular forces (10.1)
Polar covalent bonds and dipole moments (8.1, 8.3, 8.7)
Liquids (10.2)
Solids (10.3)
Changes of state (10.8)
Molecular solids (10.6)
Structures of some covalent network solids (10.5)
Ionic solids (10.7)
Solutions (4.1, 4.2, 11.2)
Solubility Equilibria
Solubility product (15.6)
Precipitation and qualitative analysis (15.7)
Equilibria involving complex ions (15.8)
Thermodynamics
The nature of energy (6.1)
Enthalpy and calorimetry (6.2)
Hess's law (6.3, 6.4)
Sources of energy (6.5)
Bond dissociation enthalpies (8.8)
Spontaneous processes (16.1)
Entropy (16.2)
Free energy (16.4)
Entropy changes in chemical reactions (16.5)
Free energy and chemical reactions (16.6)
The meaning of ΔG for a chemical reaction (16.7 p. 818)
Free energy and equilibrium (16.8)
Free energy and work (16.9)
Oxidation Reduction Reactions and Electrochemistry
Redox reactions and oxidation state assignment (4.9)
Balancing redox reactions (4.10)
Galvanic cells (17.1)
Standard reduction potentials (17.2)
Cell potential. Electrical work and free energy (17.3)
The Nernst equation (17.4)
Batteries (17.5)
Corrosion (17.6)
Electrolysis and applications (17.7)
Chemical Kinetics
Reaction rates (12.1)
Rate laws and reaction order (12.2, 12.3)
Integrated rate laws (12.4, 12.5)
Reaction mechanisms (12.6)
Arrhenius equation (12.7)
Catalysis (12.8)
Transition Metals and Coordination Chemistry
The transition metals: a survey (20.1, 20.2)
Coordination compounds (20.3)
Isomers (20.4)