Replaced Fall 2010
Fall 2004
Chabot College
Course Outline for Chemistry 1B
GENERAL COLLEGE CHEMISTRY II
Catalog Description
1B – General College Chemistry II
5 units
Continuation of Chemistry 1A. Chemical energetics and equilibria, solutions and ionic equilibria, acidbase chemistry, electrochemistry, coordination chemistry, kinetics, nuclear chemistry, organic chemistry,
and the chemistry of family groups of the periodic table. Laboratory emphasizes quantitative techniques,
including instrumentation, and qualitative analysis. Prerequisite: Chemistry 1A (completed with grade of
C or higher). 3 hours lecture, 6 hours laboratory.
[Typical contact hours: lecture 52.5, laboratory 105]
Prerequisite Skills:
Before entering the course, the student should be able to:
1.
solve problems involving the concepts listed under course content in Chemistry 1A;
2.
write short explanations describing various chemical phenomena studied in Chemistry 1A;
3.
write balanced chemical equations including net ionic equations;
4.
write balanced chemical equations for oxidation-reduction reactions;
5.
describe the different models of the atom;
6.
use standard nomenclature and notation;
7.
calculate enthalpies of reaction using calorimetry, Hess's law, heats of formation and bond energies;
8.
describe hybridization, geometry and polarity for simple molecules;
9.
draw Lewis dot structures for molecules and polyatomic ions;
10.
describe the bonding in compounds and ions;
11.
describe simple molecular orbitals of homonuclear systems;
12.
predict deviations from ideal behavior in real gases;
13.
explain chemical and physical changes in terms of thermodynamics;
14.
describe the nature of solids, liquids, gases and phase changes;
15.
describe metallic bonding and semiconductors;
16.
define all concentration units for solutions and solve solution stoichiometry problems;
17.
collect and analyze scientific data, using statistical and graphical methods;
18.
perform volumetric analyses;
19.
use a barometer;
20.
use a visible spectrophotometer;
21.
perform gravimetric analysis.
Expected Outcomes for Students:
Upon completion of the course, the student should be able to:
1.
solve problems involving gas phase equilibria;
2.
determine the extent of acid-base, precipitation and complex equilibria;
3.
interpret reactions in terms of Arrhenus, Bronsted-Lowry and Lewis acid-base theory;
4.
predict whether oxidation-reduction reactions will occur and set up voltaic and electrolytic cells;
5.
describe factors that affect the rate of chemical reactions and match mechanism with reaction
rates;
6.
describe current models for the bonding of coordination compounds;
7.
perform problems involving complex ion equilibria;
8.
describe changes that occur in the nucleus of atoms;
9.
identify organic compounds and simple isomers;
10.
analyze properties of family groups of the periodic table in terms of chemical principles;
Chabot College
Course Outline for Chemistry 1B, page 2
Fall 2004
11.
12.
13.
14.
15.
16.
17.
perform titrimetric experiments
measure pH with the use of pH meter or indicators;
perform quantitative laboratory experiments in an accurate and precise manner;
perform qualitative analysis of anions and cations in the laboratory;
collect and analyze scientific data, using statistical and graphical methods;
use a visible spectrophotometer;
perform laboratory experiments in an efficient, safe, and purposeful manner.
Course Content:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
Solutions and colligative properties
Principles of equilibrium; molecular equilibria
Acid-base theory
Acid-base, precipitation and complex equilibria
Electrochemistry
Coordination chemistry
Kinetics
Nuclear chemistry
Organic chemistry
Descriptive chemistry of the elements
Qualitative analysis
Titrations
Spectrophotometer
Laboratory safety
Methods of Presentation:
1.
2.
3.
4.
Lecture/discussion
Models, periodic tables, films, overlays
Demonstrations
Laboratory
Typical Assignments and Methods of Evaluating Student Progress:
1.
2.
Typical Assignments
a.
Read the chapter on Chemical Kinetics
1)
Work the sample problems in the chapter
2)
Work 20 problems selected by the instructor from the problems at the end of the
chapter
b.
After completing the experiment on the Iodine Clock Reaction, use the data to determine
the rate law and rate constant for the reaction. Then use spreadsheet software to plot
the natural logarithm of the rate constants at different temperatures vs. the inverse
temperatures. From the slope of the line, determine the energy of activation for the
reaction
Methods of Evaluating Student Progress
a.
Quizzes
b.
Written laboratory reports
c.
Accuracy and precision of experimental laboratory results
d.
Midterm examinations
e.
Final examination
Textbooks(s)(typical):
Chemistry: The Molecular Nature of Matter and Change, 3rd edition, Martin S. Silberberg, McGraw Hill,
2002
Chabot College
Course Outline for Chemistry 1B, page 3
Fall 2004
Special Student Materials:
1.
2.
3.
Safety goggles approved for Chemistry Laboratory
Scientific calculator
Laboratory coat/apron
LO:al
Revised: 10/24/03