The City College of New York
Department of Chemistry
Chemistry 10401: General Chemistry Lec-Lab II
Sections B, B2, B3, B4
Professor Issa Salame
Class time:
Mondays and Wednesdays: 9:30 AM – 10:45 AM
(212) 650 – 6924
Office Location: MR1224
Prof.salame@gmail.com
************************************************************************
Catalog Description:
An in-depth introduction to the fundamental laws and techniques of chemistry for majors
in science and engineering. Topics include: chemical kinetics; chemical equilibrium;
acids and bases; free energy, entropy, and the second law of thermodynamics; electrochemistry; advanced bonding concepts; metals and coordination chemistry; nuclear
chemistry.
Prerequisites:
Co-requisites:
Chem 10301
Hours/Credits:
7 hours per week, 4 cr., 3 LECT., 3 LAB, 1 PLTL WORKSHOP
Textbook:
General Chemistry 4th ed. Vol. II by Hill, John W., Petrucci, Ralph H.,
McCreary, Terry W., and Perry, Scott S. 2005
ISBN 0-536-99994-5
Course objectives:
This course is the first of a two semester sequence and consists of three components (lecture,
laboratory, and workshop), which are integrated to provide a comprehensive but thorough
introduction to the principles of chemistry. The laboratory component introduces students to
common laboratory methods including visible spectroscopy and titrations. The workshop is a
peer-led, small group discussion of concepts and problem solving in general chemistry.
After completing this course students should be able to:
1. Discuss properties of solutions and the factors that affect
solubility, and understand and interpret colligative properties,
molality, and colloids and their applications to solutions.
2. Understand chemical kinetics, reaction rates, factors that
influence the reaction rates, reaction mechanisms, and catalysis.
3. Develop conceptual knowledge of equilibrium, equilibrium
constant, and their applications to systems at equilibrium, and apply
Le Chatelier’s principles and its applications to systems at
equilibrium.
4. Develop knowledge about acid-base equilibria, the pH scale,
perform calculations into the pH of solutions of acids and bases of
varying strengths, predict the strength of an acid or base by
Department
outcomes
a, d
a
a, d
a, b, e
1
examining its structural properties, and apply principles of buffered
solutions and the role they play in the environment and biological
system.
5. Explore solubility, factors the affect solubility, and the separation
of ions by precipitation.
6. Define entropy and the Second Law of Thermodynamics and
how to relate it to everyday life, define Gibbs free energy and its
relation to the enthalpy and entropy, and manipulate equations and
make sense out of relating the free energy, enthalpy, entropy, and
the equilibrium constants.
7. Develop the skills for balancing oxidation-reduction reactions,
explore electrochemical cells and the effect of concentration on the
cell potential, and Be aware of how batteries operate and building
different types of batteries.
8. Explore nuclear chemistry by exploring radioactivity, patterns of
nuclear stability, rates of decay, nuclear fission, nuclear fusion, and
the energy changes that accompanies a nuclear reaction.
9. Develop the capabilities to solve problems by combining several
concepts in chemistry.
10. Write a laboratory report including data and analysis.
11. Be able to conduct a variety of experiments (titrations,
spectroscopic) including accurate recording of results and
preparation of calibration curves.
12. Work as part of a problem solving team to solve chemistry
problems.
a, e
a, b, e
a, e
a
d, e
g
c, d, e
f, h
Topics covered:
1.
2.
3.
4.
5.
6.
7.
8.
9.
Physical Properties of Solutions
Chemical Kinetics: Rates and Mechanisms of Chemical Reactions
Chemical Equilibrium
Acids, Bases, and Acid–Base Equilibria
More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions
Thermodynamics: Spontaneity, Entropy, and Free Energy
Electrochemistry
Nuclear Chemistry
Chemistry and Life: More on Organic, Biological, and Medicinal Chemistry
Course schedule
Lecture:
Sections B, B2, B3, B4,
Section B
Section B2
Section B3
Section B4
Lab and workshop:
Lab and workshop:
Lab and workshop:
Lab and workshop:
Mondays: 9:30 am – 10:45 am
Wednesdays: 9:30 am – 10:45 am
Tuesday 2:00 – 5:50 pm
Thursday 2:00 – 5:50 pm
Friday 9:30 am – 1:20 pm
Friday 2:00 – 5:50 pm
Relationship of course to program outcomes:
The outcome of this course contribute to the following departmental
educational outcomes:
a.
demonstrate an understanding of the fundamental principles
of chemistry, including atomic and molecular structure,
Course
Objective
Numbers
1-8
2
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
quantum chemistry, chemical bonding, stoichiometry, kinetics
and mechanism, equilibrium, thermochemistry and
thermodynamics, molecular structure and function,
electrochemistry, and the periodic chemical properties of the
elements.
apply the fundamental principles of chemistry to life sciences,
the environment, materials, engineering, and emerging
technological fields of chemistry, as well as to everyday
situations.
conduct experiments and learn fundamental laboratory skills
analyze and interpret data
apply mathematical concepts to chemical problems
work as part of a problem-solving team
convey facts, theories and results about chemistry in written
form
use oral presentation to convey facts, theories and results
about chemistry
access and utilize chemical information technology
design and execute scientific research
apply ethical responsibilities and professional conduct
4, 6
11
1, 3, 9, 11
4-7, 9, 11
12
10
12
Assessment tools:
The final grade is calculated as follows:
Best two scores of the three in-class examinations
Quizzes – Grade to be added to exams
Final Exam
Laboratory and workshop
Homework and In-Class Quizzes
(30-35%)
(35%)
(20 - 25%)
(10%)
* The lowest grade exam will be dropped. Missing an exam will result in receiving a zero grade
for that particular exam and thus dropping that grade. There will not be any Make-up Exams.
Office Hours:
Monday:
11:00 am – 12:00 pm
Wednesdays: 11:00 am – 1:00 pm
Or by appointment
Office is located in the science building in room 1224
Absence Policy
Any student who misses more than four classes will be dropped from the course.
Statement on Academic Integrity
The CCNY policy on academic integrity will be followed in this course. The document can be
found through the CCNY website by clicking on Current Students  Academic Services 
Policy on Academic Integrity. All students must read the details regarding plagiarism and
cheating in order to be familiar with the rules of the college. Cases where academic integrity is
compromised will be prosecuted according to these rules. In addition, the Policy of Academic
Integrity can be found in the Undergraduate Bulletin 2007-2009 in Appendix B.3 on page 312.
3
Class Schedule
August 31st
Monday
Chapter 12: Physical Properties of Solutions

12.1 Some Types of Solutions

12.2 Solution Concentration

12.3 Energetics of Solution Formation

12.4 Equilibrium in Solution Formation
September 2nd
Wednesday Chapter 12: Physical Properties of Solutions

12.5 The Solubilities of Gases

12.6 Vapor Pressures of Solutions

12.7 Freezing Point Depression and Boiling Point Elevation
September 7th
Monday
*** NO CLASS *** College Closed ***
Labor Day
September 9th
Wednesday Chapter 12: Physical Properties of Solutions

12.8 Osmotic Pressure

12.9 Solutions of Electrolytes

12.10 Colloids
Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical
Reactions

13.1 Chemical Kinetics—A Preview

13.2 The Meaning of Reaction Rate
September 14th
Monday
Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical
Reactions

13.3 Measuring Reaction Rates

13.4 The Rate Law of a Chemical Reaction

13.5 First-Order Reactions
September 16th
Wednesday Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical
Reactions

13.5 First-Order Reactions

13.6 Reactions of Other Orders

13.7 Theories of Chemical Kinetics

13.8 Effect of Temperature on Reaction Rate
September 21st
Monday
Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical
Reactions

13.9 Reaction Mechanisms

13.10 Catalysis

13.11 Enzyme Catalysis
September 23rd
Wednesday Chapter 14: Chemical Equilibrium

14.1 The Dynamic Nature of Equilibrium

14.2 The Equilibrium Constant Expression
4

14.3 Modifying Equilibrium Constant Expressions
September 28th
Monday
*** NO CLASS *** College Open ***
September 29th
Tuesday
Monday Schedule
Chapter 14: Chemical Equilibrium

14.4 Qualitative Treatment of Equilibrium: Le Châtelier’s Principle

14.5 Some Illustrative Equilibrium Calculations
September 30th
Wednesday Chapter 14: Chemical Equilibrium

14.5 Some Illustrative Equilibrium Calculations

Catch-up and Review for first examination
October 5th
Monday
FIRST EXAMINATION (Chapters: 12, 13, and 14)
October 7th
Wednesday
October 12th
Monday
October 14th
Wednesday
October 19th
Monday
October 21st
Wednesday
October 26th
Monday
Chapter 15: Acids, Bases, and Acid–Base Equilibria

15.1 The Brønsted–Lowry Theory of Acids and Bases

15.2 Molecular Structure and Strengths of Acids and Bases

15.3 Self-Ionization of Water—the pH Scale
*** NO CLASS *** College Open ***
Columbus Day
Monday Schedule
Chapter 15: Acids, Bases, and Acid–Base Equilibria

15.4 Equilibrium in Solutions of Weak Acids and Weak Bases

15.5 Polyprotic Acids
Chapter 15: Acids, Bases, and Acid–Base Equilibria

15.6 Ions as Acids and Bases

15.7 The Common Ion Effect

15.8 Buffer Solutions
Chapter 15: Acids, Bases, and Acid–Base Equilibria

15.9 Acid–Base Indicators

15.10 Neutralization Reactions and Titration Curves

15.11 Lewis Acids and Bases
Chapter 16: More Equilibria in Aqueous Solutions: Slightly Soluble Salts
and Complex Ions

16.1 The Solubility Product Constant,

16.2 The Relationship Between
and Molar Solubility

16.3 The Common Ion Effect in Solubility Equilibria
5
October 28th
Wednesday
More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex
Ions

16.4 Will Precipitation Occur? Is It Complete?

16.5 Effect of pH on Solubility

16.6 Equilibria Involving Complex Ions

16.7 Qualitative Inorganic Analysis
November 2nd
Monday
SECON EXAMINATION (Chapters: 15, and 16)
November 4th
Wednesday Catch-up and Going Over Second Examination
November 9th
Monday
Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy

17.1 Why Study Thermodynamics?

17.2 Spontaneous Change

17.3 The Concept of Entropy
November 11th
Wednesday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy

17.4 Free Energy and Free Energy Change

17.5 Standard Free Energy Change, G
November 16th
Monday
Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy

17.6 Free Energy Change and Equilibrium

17.7 The Dependence of G and Keq on Temperature
November 18th
Wednesday Chapter 18: Electrochemistry

18.1 Half-Reactions

18.2 The Half-Reaction Method of Balancing Redox Equations
November 23rd
Monday
Chapter 18: Electrochemistry

18.3 A Qualitative Description of Voltaic Cells

18.4 Standard Electrode Potentials
November 25th
Wednesday Chapter 18: Electrochemistry

18.5 Electrode Potentials, Spontaneous Change, and Equilibrium

18.6 Effect of Concentrations on Cell Voltage

18.7 Batteries: Using Chemical Reactions to Make Electricity

18.8 Corrosion: Metal Loss Through Voltaic Cells
November 30th
Monday
Chapter 18: Electrochemistry

18.9 Predicting Electrolysis Reactions

18.10 Quantitative Electrolysis

18.11 Applications of Electrolysis
6
December 2nd
Wednesday Chapter 19: Nuclear Chemistry

19.1 Radioactivity and Nuclear Equations

19.2 Naturally Occurring Radioactivity

19.3 Radioactive Decay Rates

19.4 Synthetic Nuclides

19.5 Transuranium Elements

19.6 Nuclear Stability

19.7 Energetics of Nuclear Reactions

19.8 Nuclear Fission and Nuclear Fusion

19.9 Effect of Radiation on Matter

19.10 Applications of Radioactive Nuclides
December 7th
Monday
THIRD EXAMINATION (Chapters: 17, 18, and 19)
December 9th
Wednesday Catch-Up and Review
Final Examination will be scheduled during the final exam period between Tuesday the 15th
and Monday the 21st of December of 2009.
Recommended Exercises:
Chapter 12:
21, 23, 33, 34, 35, 37, 39, 51, 57, 58, 59, 62, 63, 67, 69, 71, 81
Chapter 13:
25, 31, 32, 37, 39, 41, 61, 63, 65, 67, 75, 85, 86
Chapter 14:
19, 21, 23, 25, 27, 29, 31, 33, 35, 37, 41, 43, 44, 47, 49, 51, 53, 55, 57, 59, 61, 63,
65, 67, 69, 71, 73
Chapter 15:
21, 23, 25, 31, 37, 39, 41, 43, 45, 47, 49, 51, 53, 59, 61, 63, 65, 69, 71, 73, 75, 81,
83, 85, 87, 103
Chapter 16:
19, 21, 25, 27, 29, 39, 41, 43, 47, 49, 53, 54, 65
Chapter 17:
19, 20, 35, 36, 37, 39, 41, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 69
Chapter 18:
25, 27, 28, 35, 37, 43, 45, 51, 53, 54, 57, 58, 59, 61, 79, 81, 92
Chapter 19:
21, 23, 25, 35, 37, 38, 43
Study Guides:
1. Plan at least three hours of study (reading the chapter and completing the problem sets “homework”) time for every hour you spend in class.
2. Do the problem sets individually (without help from friends or classmates) initially.
Please look at a related problem in the solution manual to help you solve the assigned
problem. If you are still unable to solve the problem, then ask a friend, classmate,
workshop leader, TA, or Professor for help.
3. Read the book and take notes as you read.
4. Attend workshop: finish the Self-Test, finish the workshop problems, and ask questions.
5. Seek help when you have difficulty (office hours, tutoring, study groups with workshop).
“I hear, I forget. I see, I remember. I do, I understand.”
Chinese proverb
7