Welcome to the INS 2006/07 Program!
Chemistry Syllabus - Spring 2007 Quarter
| Week | Chapters | Concepts |
|---|---|---|
| 1 | 6 | First law of thermodynamics, enthalpy, functions of state, calorimetry (constant volume and constant pressure), Hess's law, standard molar enthalpy of formation |
| 2 | 12 & 15 | properties of gases, gas laws, the ideal gas, ideal gas law, density of gases, gas laws and stoichiometry, gas mixture, partial pressure, kinetic molecular theory, diffusion, effusion, Van der Waals equation for real gases, rates of chemical reactions, order, rate constant, rate law |
| 3 | 15 & 16 | integrated rate laws for zero, first, and second order reactions with their graphical representations, half life, radioactive decay, activation energy, transition state, Arrhenius equation, reaction mechanisms, elementary reactions, molecularity, reaction quotient, equilibrium constant (Kp and Kc), determination of the equilibrium constant and its relationship to the rate constant, nuclear chemistry (Sections 23.1, 23.2 self study with problems assigned for homework) |
| 4 | 16 & 17 | Le-Chatelier's principle, acid/base equilibria, Bronsted-Lowry definition of an acid, conjugated acids/bases, Ka, Kb, Kw, pH, pOH, nuclear chemistry (Section 23.3 self study with problems assigned for homework) |
| 5 | 17 | acidity and basicity of ionic compounds, polyprotic acids and bases, Lewis acid/base concept, molecular structure, bonding and acid/base behavior, nuclear chemistry (Section 23.4 self study with problems assigned for homework) |
| 6 | 18 | the common ion effect, buffers, acid-base titrations, nuclear chemistry (Section 23.5, 23.6 self study with problems assigned for homework) |
| 7 | 18 & 19 | indicators, solubility of salts, Ksp, entropy and free energy, nuclear chemistry (finish reading the remainder of chapter - self study) |
| 8 | 19 & 20 | relationship between free energy and equilibrium constant, voltaic cells, cell notation, standard hydrogen electrode, primary batteries, alkaline batteries, secondary batteries,electromotive force, standard reduction potentials, Nernst equation, relationship between cell potential, Gibbs free energy, and equilibrium constant, electrolysis of molten salts |
| 9 | 20 | electrolysis of solutions, counting electrons and matter deposited during electrolysis |
| 10 | 23 | review and prepare for exam |
Chemistry Syllabus - Winter 2007 Quarter
| Week | Chapters | Concepts |
|---|---|---|
| 2 | 7 | properties of light, classification of electromagnetic radiation, birth of quantum mechanics, Planck's equation, photoelectric effect, atomic spectra, Bohr model, Rydberg formula |
| 3 | 7 & 8 | de Broglie's equation, Schrodinger wave mechanics approach to the structure of the atom, Heisenberg uncertainty principle, wave function, orbitals, quantum numbers, shapes of orbitals, magnetism of materials, spin quantum number |
| 4 | 8 | writing electron configurations in spectroscopic, rare gas, and orbital box diagram notations for all elements, electronic configurations of ions |
| 5 | 8 | periodic properties of the elements, periodic trends |
| 6 | 9 | ionic bonds, Born-Haber cycle, covalent bonds, Lewis dot structures, resonance |
| 7 | 9 | formal charges, shapes of molecules |
| 8 | 10 | valence bond theory, hybridization model |
| 9 | 10 | molecular orbital theory |
| 10 | 6 | introductory thermodynamics, specific and molar heat capacities, heats of phase changes |
Chemistry Syllabus - Fall 2006 Quarter
| Week | Chapters | Concepts |
|---|---|---|
| 1 | 1 | classification of matter, physical & chemical properties & changes, temperature, units of measurement, precision, accuracy, error |
| 2 | 2 | structure of the atom, sub-atomic particles, isotopes, mole concept, molar mass, molecular weight |
| 3 | 3 | introduction to the periodic table, ions, writing formulas & naming ionic compounds |
| 4 | 3 & 4 | writing formulas & naming molecular compounds, molar mass, determination of empirical and molecular formulas, % composition, balancing chemical equations, stoichiometry |
| 5 | 4 | stoichiometry, percentage yield, limiting reactants |
| 6 | 5 | solubility of ionic compounds,strong and weak electrolytes, precipitation reactions, net ionic equations |
| 7 | 5 | acids & bases, acid base reactions, oxidation numbers |
| 8 | 5 | redox reactions, identification of oxidizing & reducing agents, molarity, molality, ppm, ppb, preparing solutions of desired concentrations from solids and by dilution |
| 10 | 5 | pH, titrations, stoichiometry of reactions in solution, balancing redox reactions that occur in acidic and basic media |
