Syllabus CHEM111B – General Chemistry II
Instructor: Thomas Cullen Class: MWF 8:00 am - 8:50 am in HSCI-100
Office: HSCI - 212
E-mail: tdcull[email protected]om
Office hours: Monday 9:05 am – 10:45 am, 1:00pm – 1:55pm
Wednesday 9:05 am – 10:45 am, 1:00pm – 1:55pm
Friday 9:05 am – 10:45 am, 1:00 pm – 2:00 pm ( ) or by arrangement
Textbook: Chemistry: A Molecular Approach. 3 Edition. Author: Tro. Publisher: Prentice-Hall.
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Supplemental handouts and extra practice questions may also be provided in class, if necessary.
Online Homework: Mastering Chemistry (www.masteringchemistry.com)
Course ID: MCCULLEN39794
iClicker: iclickers are required and will be used throughout lecture.
General Chemistry Experiments: The lab manual required for this class is:
Gen. Chem. II 2015, General Chemistry 2 Semester Lab Manual. Dr. Stephen Mezyk, Nancy Gardner &
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Dr. Ron Garber.
Course Objectives. For students in CHEM111B the important Student Learning Outcomes (SLO's) that
are assessed, are to:
understand how the solubility and energetics of solution formation relates to their various
intermolecular forces
use and interconvert standard solution concentration definitions
quantitatively calculate solution physical phenomena, including freezing point depression,
boiling point elevation and osmosis
define and quantitatively manipulate reaction rates, orders, rate laws, and reaction half-lives
understand how temperature and catalysts impact kinetics and mechanisms of reactions
quantitatively calculate equilibrium constant expressions, and determine involved species
concentrations for both gas and liquid reactions
understand and use Le Chatelier's Principle to predict equilibrium behavior
know the Arrhenius, Lowry-Bronsted and Lewis definitions of acids and bases
quantitatively calculate acid strength and pH of different acids, bases, and ions in water
relate acid strength to molecular structure
understand and quantitatively manipulate parameters such as species concentration and
solution pH in buffer, titration, salt solubility, and complex ion formation equilibria
understand differences between enthalpy, entropy and free energy in equilibrium systems
quantitatively relate thermodynamic systems to equilibria in standard and non-standard state
systems
balance oxidation-reduction equations, identify spontaneous chemical reactions
relate standard cell potential, free energy and equilibrium constants
understand batteries, electrolysis and corrosion concepts
understand the different types of radioactivity, radioactive decay of elements and its detection,
fusion and fission
understand the effects of radiation on life
Pre-requisite Courses: CHEM 111A (C or better). Students repeating this course must ALSO repeat the
laboratory portion. Past semester’s lab scores are NOT transferable. You will be dropped from this
course if you do not meet this pre-requisite.
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Exam Schedule:
Mid-term Exam I:Friday August 28 , 2015
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Chem 111A Review: Material covered in the first semester of General Chemisty.
Mid-term Exam II: Friday October 2 , 2015
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Chapter 12: Solutions: Solvents and solutes, temperature dependence, concentrations, colligative
properties, Raoult’s Law, Henry’s Law, osmotic pressure.
Chapter 13: Chemical Kinetics: Kinetic order, temperature dependence, rate laws, reaction
mechanisms and catalysis.
Chapter 14:Chemical Equilibria: Dynamic equilibria, K and K , Le Chatelier’s Principle, calculating
p c
equilibrium constants
Mid-term Exam III: Friday October 30 , 2015
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Chapter 15:Acids and Bases: Arrhenius, Bronsted and Lewis definitions, pH, strong and weak acids,
Ka and K , polyprotic acids.
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