The City College of New York s1
The City College of New York
Department of Chemistry
Chemistry 10401: General Chemistry Lec-Lab II
Sections H, H2, & H3
Professor Takoa J. Lawson
Class time: Mondays 6:30 PM – 8:10 PM & Wednesdays 6:15 PM – 7:05 PM
Workshop time: Mondays From 8:10 PM – 9:00 PM
Office Location: TBA
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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; electro-
chemistry; advanced bonding concepts; metals and coordination chemistry; nuclear
chemistry.
Prerequisites: Chem 10301
Co-requisites:
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 second 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.
How to succeed in General Chemistry… or A word to the wise…
Learning Chemistry is cumulative – if you miss a class you will miss a significant building block, which will affect your exam performance, scores, and final grade as well as your ability to understand material in future courses. So, attendance for all lectures, labs, and workshops while required is critical to your success. Further, your own practice by doing homework and becoming engaged with the material as well as engaged with your classmates in workshop and lab discussions of chemical concepts will help you build your knowledge to succeed. Learning these skills will prepare you for your chosen major and professional career.
After completing this course students should be able to: / Department outcomes1. 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 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, d
a
a, d
a, b, e
a, e
a, b, e
a, e
a
d, e
g
c, d, e
f, h
Topics covered:
1. Physical Properties of Solutions
2. Chemical Kinetics: Rates and Mechanisms of Chemical Reactions
3. Chemical Equilibrium
4. Acids, Bases, and Acid–Base Equilibria
5. More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions
6. Thermodynamics: Spontaneity, Entropy, and Free Energy
7. Electrochemistry
8. Nuclear Chemistry
9. Chemistry and Life: More on Organic, Biological, and Medicinal Chemistry
Relationship of course to program outcomes:
The outcome of this course contribute to the following departmental educational outcomes: / Course Objective Numbersa. demonstrate an understanding of the fundamental principles of chemistry, including atomic and molecular structure, 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.
b. 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.
c. conduct experiments and learn fundamental laboratory skills
d. analyze and interpret data
e. apply mathematical concepts to chemical problems
f. work as part of a problem-solving team
g. convey facts, theories and results about chemistry in written form
h. use oral presentation to convey facts, theories and results about chemistry
i. access and utilize chemical information technology
j. design and execute scientific research
k. apply ethical responsibilities and professional conduct / 1-8
4, 6
11
1, 3, 9, 11
4-7, 9, 11
12
10
12
Assessment tools:
The final grade is calculated as follows:
Three in-class examinations (35%)
Final Exam (35%)
Laboratory (15%)
Workshop (10%)
Quizzes (5%)
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 à Academic Services à 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.
Class Schedule
January 26th
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
· 12.5 The Solubilities of Gases
January 28th
Wednesday Chapter 12: Physical Properties of Solutions
· 12.6 Vapor Pressures of Solutions
· 12.7 Freezing Point Depression and Boiling Point Elevation
February 2nd
Monday 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
February 4th
Wednesday Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical Reactions
· 13.3 Measuring Reaction Rates
· 13.4 The Rate Law of a Chemical Reaction
February 9th
Monday 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
February 11th
Wednesday Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical
Reactions
· 13.9 Reaction Mechanisms
· 13.10 Catalysis
· 13.11 Enzyme Catalysis
February 16th
Monday *** NO CLASS *** College Closed ***
President’s Day
February 18th
Wednesday Chapter 14: Chemical Equilibrium
· 14.1 The Dynamic Nature of Equilibrium
· 14.2 The Equilibrium Constant Expression
· 14.3 Modifying Equilibrium Constant Expressions
February 23rd
Monday Chapter 14: Chemical Equilibrium
· 14.4 Qualitative Treatment of Equilibrium: Le Châtelier’s Principle
· 14.5 Some Illustrative Equilibrium Calculations
· 14.5 Some Illustrative Equilibrium Calculations
February 25th
Wednesday FIRST EXAMINATION (Chapters: 12, 13, and 14)
March 2nd
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
March 4th
Wednesday Chapter 15: Acids, Bases, and Acid–Base Equilibria
· 15.4 Equilibrium in Solutions of Weak Acids and Weak Bases
· 15.5 Polyprotic Acids
March 9th
Monday 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
March 11th
Wednesday 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
March 16th
Monday 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
March 18th
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
March 23rd
Monday SECON EXAMINATION (Chapters: 15, and 16)
March 25th
Wednesday Catch-up and Going Over Second Examination
March 30th
Monday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy
· 17.1 Why Study Thermodynamics?
· 17.2 Spontaneous Change
· 17.3 The Concept of Entropy
April 1st
Wednesday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy
· 17.4 Free Energy and Free Energy Change
· 17.5 Standard Free Energy Change,
·
April 6th
Monday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy
· 17.6 Free Energy Change and Equilibrium
· 17.7 The Dependence of and on Temperature
April 8
Wednesday *** NO CLASS***
Spring Recess
April 13th
Monday *** NO CLASS***
Spring Recess
April 15th
Wednesday *** NO CLASS***
Spring Recess
April 20th
Monday Chapter 18: Electrochemistry
· 18.1 Half-Reactions
· 18.2 The Half-Reaction Method of Balancing Redox Equations
April 22nd
Wednesday Chapter 18: Electrochemistry
· 18.3 A Qualitative Description of Voltaic Cells
· 18.4 Standard Electrode Potentials
April 27th
Monday 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
April 29th
Wednesday Chapter 18: Electrochemistry
· 18.9 Predicting Electrolysis Reactions
· 18.10 Quantitative Electrolysis
· 18.11 Applications of Electrolysis
May 4th
Monday 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
May 6th
Wednesday Chapter 19: Nuclear Chemistry
· 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
May 11th
Monday THIRD EXAMINATION (Chapters: 17, 18, and 19)
May 13th
Wednesday Catch-Up and Review
Final Examination will be scheduled during the final exam period between Saturday the 16th and Friday the 22nd of May 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
Chapter 23: 35, 41, 45
**complete additional practice as necessary to develop a complete understanding of each topic/concept covered
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
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