Las Positas College
3033 Collier Canyon Road
Livermore, CA 94551-7650
(925) 373-5800
(925) 443-0742 (Fax)
Course Outline for Chemistry 1B
GENERAL COLLEGE CHEMISTRY
I.
CATALOG DESCRIPTION:
CHEM 1B — GENERAL COLLEGE CHEMISTRY — 5 units
Continuation of Chemistry 1A. Includes chemical energetics and equilibria, solutions and
ionic equilibria, acid-base 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.
II.
NUMBER OF TIMES COURSE MAY BE TAKEN FOR CREDIT: One
III.
PREREQUISITE AND/OR ADVISORY SKILLS:
Before entering the course, the student should be able to:
A.
B.
C.
D.
E.
F.
G.
H.
I.
J.
K.
L.
M.
N.
O.
P.
Q.
R.
S.
T.
U.
V.
W.
X.
Y.
Z.
AA.
solve complex problems involving the concepts listed under the course content for
Chemistry 1A;
write short explanations describing various chemical phenomena studied in
Chemistry 1A;
write balanced chemical equations including net ionic equations;
write balanced chemical equations for oxidation-reduction reactions;
describe the different models of the atom;
use standard nomenclature and notation;
Calculate enthalpies of reaction using calorimetry, Hess’s Law, heats of formation,
and bond energies;
describe hybridization, geometry and polarity for molecules and polyatomic ions;
draw Lewis dot structures for molecules and polyatomic ions;
describe bonding in compounds and ions;
describe simple molecular orbitals of homonuclear systems;
predict deviations from ideal behavior in real gases;
describe the nature of solids, liquids, gases and phase changes;
describe metallic bonding and semiconductors;
describe network covalent bonding;
define concentrations of solutions in terms of molarity, molality, normality, percent
composition, and ppm;
describe colligative properties of solutions;
solve solution stoichiometry problems;
determine the extent of molecular reactions through the study of equilibrium;
solve simple problems involving gas phase equilibria;
apply Le Châtelier’s principle to equilibria;
collect and analyze scientific data, using statistical and graphical methods;
perform volumetric analyses;
use a barometer;
use a visible spectrophotometer;
perform gravimetric analysis
acquire and analyze data with a computer and appropriate software.
Course Outline for Chemistry 1B
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GENERAL COLLEGE CHEMISTRY
IV.
EXPECTED OUTCOMES FOR STUDENTS:
Upon successful completion of the course, the student should be able to:
A.
B.
C.
D.
E.
F.
G.
H.
I.
J.
K.
L.
M.
N.
O.
P.
Q.
R.
S.
T.
U.
V.
solve problems involving gas-phase, acid-base, solubility, and complex ion equilibria;
calculate free energy of a reaction from standard free energies of formation and from
enthalpies and entropies of reaction;
predict the conditions under which a reaction will be spontaneous or
nonspontaneous;
determine the extent of acid-base, precipitation and complex equilibria;
interpret reactions in terms of Arrhenius, Bronsted-Lowry and Lewis acid-base
theory;
use acid dissociation constants to predict acid-base strength;
predict whether oxidation-reduction reactions will occur and set up voltaic and
electrolytic cells;
describe factors that affect the rate of chemical reactions;
write rate constant and related kinetic expressions based on reaction data;
interpret and evaluate reaction mechanisms;
describe current models for the bonding of coordination compounds;
name complex ions;
describe changes that occur in the nuclei of atoms;
name and describe the major functional groups in organic chemistry;
recognize properties of family groups of the periodic table in terms of chemical
principles;
perform titrimetric experiments;
measure pH with the use of pH meters or indicators;
merform 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;
acquire and analyze data with a computer and appropriate software and design
spreadsheets for data acquisition and analysis;
perform laboratory experiments in an efficient, safe, and purposeful manner.
V.
CONTENT:
A.
Laboratory Safety
B.
Solutions
C.
Thermodynamics
D.
Principles of equilibrium
E.
Acid-base theory
F.
Acid-base, precipitation, and complex equilibria
G.
Electrochemistry
H.
Coordination chemistry
I.
Kinetics
J.
Nuclear chemistry
K.
Organic chemistry
L.
Descriptive chemistry of the elements
M.
Qualitative analysis of anions and cations
N.
Titrations, including a potentiometic titration
O.
Spectrophotometric analysis
P.
Construction and analysis of batteries and electrolytic cells
VI.
METHODS OF INSTRUCTION:
A.
Lecture, informal with student questions encouraged
B.
Models, periodic tables, videos, overhead transparencies
C.
Computer simulations
D.
Demonstrations
Course Outline for Chemistry 1B
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GENERAL COLLEGE CHEMISTRY
E.
F.
G.
H.
Laboratory experimentation, including computer acquisition of data
Oral presentations on chemical topics (at the option of the instructor)
Field trips (at the option of the instructor)
Safety and proper respect for chemicals and scientific apparatus are constantly
stressed.
VII.
TYPICAL ASSIGNMENTS:
A.
Read the chapter on Chemical Kinetics
1.
Work all of the in-chapter problems.
2.
Work 10 problems selected from the end of the chapter problems for which
solutions are not provided in the text.
B.
Complete worksheets on Predicting Chemical Reactions.
C.
After completing the experiment on Electrochemical Cells and Electrolysis, Corrosion
and Passivation, use spreadsheet software to plot current vs. time and to integrate
current-time to get total charge. Use this and other experimental information to
calculate the thickness of the film on the anodized area.
VIII.
EVALUATION:
A.
Methods of evaluation
1.
Homework will be assigned, collected, and graded.
2.
Quizzes may be used at the option of the instructor.
3.
Written lab reports requiring appropriate use of ink and corrections
4.
Accuracy and precision of experimental work
5.
Midterm examinations or tests
6.
Final examination
B.
Frequency of evaluation
1.
Homework: 10 to 20 assignments; 1 or 2 per chapter
2.
Quizzes: options include daily, weekly, or biweekly
3.
Written lab reports: 1 to 2 per week
4.
Midterm examinations: 1 – 5 tests
C.
Typical exam questions:
1.
Calculate the approximate value for the standard free energy change, ∆G°, at
1000°C for the combustion of methane. (Table of Standard Enthalpies of
Formation at 25°C and Table of Standard Entropies at 25°C are provided.)
2.
What is the pH of a solution formed by the addition of 0.0088 mol NH4Cl(s) to
0.250 L of 0.0150 M NH3(aq)? Assume no volume change on the addition of
the solid ammonium chloride. (Tables with values of Ka and Kb are provided.)
3.
For the first order reaction: 2N2O5(g)  4NO2(g) + O2(g), it is found that the
concentration of N2O5 is 0.0750 mol/L after 15.0 min of reaction time and that
it is 0.0300 mol/L after 25.0 min of reaction time. Calculate the concentration
of N2O after 80.0 min of reaction time (include units).
4.
All the octahedral complexes of nickel(II), (e.g., [NiCl6}4–, [Ni(CN)6]4–) have the
same number of unpaired electrons, no matter what is the nature or strength
of the ligand. Why is this so? Be sure to provide the answer as to why in terms
of the theories studied in the course.
IX.
TYPICAL TEXTS:
A.
Jean B. Umland and Jon M. Bellama, General Chemistry, Third Edition. Pacific
Grove, CA: Brooks/Cole Publishing Company, 1999.
B.
Martin S. Silberberg, Chemistry: The Molecular Nature of Matter and Change, 2nd
ed., Boston: McGraw-Hill, 2000.
C.
Steven S. Zumdahl, Chemical Principles, 4th ed., Boston: Houghton-Mifflin Company,
2002.
X.
OTHER MATERIALS REQUIRED OF STUDENTS:
A.
Safety goggles approved for chemistry laboratory
Course Outline for Chemistry 1B
GENERAL COLLEGE CHEMISTRY
B.
C.
Scientific calculator
Student laboratory notebook
Creation Date:
1994
Revision Date:
1997, 10/02
Date approved by Curriculum Committee: December 2, 2002
Effective Date:
Fall 2003
chem1b
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