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CHGN122 – Principles of Chemistry II
Contacts: Dr. Renee Falconer/Dr. Mark Seger, Chemistry and Geochemistry,
[email protected], [email protected]
Bulletin description:
CHGN122 – Principles of Chemistry II (I,II)- Continuation of CHGN121 Study of matter
and energy concentrating on chemical kinetics, thermodynamics, electrochemistry, organic
nomenclature, and chemical equilibrium (acid- base, solubility, complexa- tion, and redox).
Laboratory experiments emphasizing quan- titative chemical measurements. Prerequisite:
Grade of C or better in CHGN121. 3 hours lecture; 3 hours lab, 4 semester hours.
Purpose in the curriculum:
Chemistry is the field of science associated with atoms and molecules. It focuses on the
behavior and properties of matter, the relationship of energy with the bond-forming and
bond-breaking reactions that dictate chemical processes, and the creation of new
substances. It is often considered the central science, linking the physical sciences with
engineering, medicine, and life sciences. This course is part of the distributed science
requirement of the core curriculum.
Current Textbook:
McMurry and Fay, General Chemistry Atoms First The Foundation Science (1st edition),
Pearson Custom Publishing (ISBN 978-0-558-36635-3)
Learning outcomes/topics covered:
1. Liquids, solids and intermolecular forces: dispersion forces, dipole-dipole forces, hydrogen
bonding, ion-dipole forces, surface tension, vapor pressure, heating curves, viscosity, fusion,
freezing, condensation, sublimation, deposition, phase diagrams, crystalline solids.
2. Quantum mechanics: electromagnetic radiation, quantum mechanics, quantum numbers, shape
and energy of orbitals, Pauli Exclusion Principle, multi-electron atoms, Aufbau method,
valence bond theory, hybridization, simple molecular orbital theory.
3. Solutions: homogeneous/heterogeneous mixtures, colloids, “like dissolves like”, solute/solvent
forces, solubility vs. chemical structure, molarity, mass percent, concentration units, effect of
temperature and pressure on solubility, Henry’s Law, Raoult’s law, vapor pressure curves,
freezing-point depression/boiling-point elevation, osmotic pressure.
4. Chemical kinetics: rate of reactions, rates of consumption and formation, reaction orders, rate
law constants, first-, second- and zero-order rate laws and plots, half-life, reaction mechanisms
and molecularity of elementary reactions, potential energy profiles, activation energy, catalysts.
5. Chemical equilibrium: equilibrium vs reaction rates and concentrations, equilibrium constants
(Kc and Kp), relation to pressure, heterogeneous equilibrium, predicting direction of reaction to
reach equilibrium, reaction to stressors such as concentration, pressure or temperature changes,
effect of catalysts.
6. Acids and bases: Definitions of Arrhenius, Bronsted-Lowry and Lewis acid/bases, conjugate
acid/bases, strength of acid/base compared to water, equilibrium of water (Kw), pH, pOH,
indicators, relation of concentration and pH of solution, weak acid/weak base equilibrium, Ka,
Kb, pKa, pKb, pH of salt solutions, acidity of binary and oxyacids.
7. Aqueous ionic equilibrium: neutralization reactions, determining pH after addition of acid/base
at various times, buffers, Henderson-Hasselbalch equation, titration curves, polyprotic
acids/bases, solubility products for ionic compounds (Ksp), common ion effect, predicting
precipitation of ionic compounds,
8. Free energy and thermodynamics: spontaneity, entropy, effect of temperature on entropy,
Gibbs free energy to determine spontaneity, energy of reaction, energy of formation, energy of
reaction at nonstandard pressures/concentrations, energy of reaction and equilibrium.
9. Electrochemistry: galvanic cells, anode/cathode, direction of electron flow, cell potentials,
oxidizing/reducing strength, Nerst equation for non-standard conditions, cell potentials and
equilibrium, reactions of common batteries, fuel cells vs batteries, electrolytic processes.