The City College of New York
Department of Chemistry
Chemistry 10401: General Chemistry Lec-Lab II
Sections B, B2, B3, B4, B5
Lecture time:
Mondays 9:00 AM – 10:50 AM and Wednesdays 9:00 AM – 9:50 AM
Professor Issa Salame
(212) 650 – 8386
Office Location: MR-1018
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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
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 and 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 ChatelierÕs 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.
Topics covered:
- 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, B5 Mondays: 9:00 am – 10:50 am
Wednesdays: 9:00 am – 9:50 am
Section B Workshop: Wednesdays 10:00 – 10:50 am
Lab: Tuesday 2:00 – 4:50 pm
Section B2 Workshop: Wednesdays 10:00 – 10:50 am
Lab: Thursday 2:00 – 4:50 pm
Section B3 Workshop: Wednesdays 10:00 – 10:50 am
Lab: Friday 10:00 am – 12:50 pm
Section B4 Workshop: Wednesdays 10:00 – 10:50 am
Lab: Monday 2:00 – 4:50 pm
Section B5 Workshop: Wednesdays 10:00 – 10:50 am
Lab: Friday 2:00 – 4:50 pm
Assessment tools
The final grade is calculated as follows:
Best two scores of the three in-class examinations (37.5%)
Quizzes – Grade to be added to exams
Final Exam (37.5%)
Laboratory (20%)
Workshop grade (5%)
* 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
Mondays: 4:00 pm – 5:00 pm
Wednesdays: 11:00 am – 12: 00 pm
Wednesdays: 4:00 pm – 5:00 pm
Or by appointment
Office is located in the science building in room 1018 (MR-1018)
Absence Policy
Any student who misses more than four classes will be dropped from the course.
Academic integrity
The CCNY policy on academic integrity will be followed. Document is posted on the CCNY website (CUNY policy on academic integrity—link is at the bottom of the home page). Make sure you have read the details regarding plagiarism and cheating, in case you are not clear about the rules of the college. Cases where academic integrity is compromised will be prosecuted according to these rules.
Class Schedule
January 28th
Monday Chapter 12: Physical Properties of Solutions
á 12.1 Some Types of Solutions
á 12.2 Solution Concentration
á 12.3 Energetics of Solution Formation
January 30th
Wednesday Chapter 12: Physical Properties of Solutions
á 12.4 Equilibrium in Solution Formation
á 12.5 The Solubilities of Gases
á 12.6 Vapor Pressures of Solutions
á 12.7 Freezing Point Depression and Boiling Point Elevation
February 4th
Monday Chapter 12: Physical Properties of Solutions
á 12.8 Osmotic Pressure
á 12.9 Solutions of Electrolytes
á 12.10 Colloids
February 6th
Wednesday Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical Reactions
á 13.1 Chemical Kinetics—A Preview
á 13.2 The Meaning of Reaction Rate
á 13.3 Measuring Reaction Rates
á 13.4 The Rate Law of a Chemical Reaction
February 11th
Monday Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical Reactions
á 13.5 First-Order Reactions
á 13.6 Reactions of Other Orders
á 13.7 Theories of Chemical Kinetics
February 13th
Wednesday Chapter 13: Chemical Kinetics: Rates and Mechanisms of Chemical
Reactions
á 13.8 Effect of Temperature on Reaction Rate
á 13.9 Reaction Mechanisms
á 13.10 Catalysis
á 13.11 Enzyme Catalysis
February 18th
Monday *** NO CLASS *** College Closed ***
PresidentÕs Day
February 20th
Wednesday Chapter 14: Chemical Equilibrium
á 14.1 The Dynamic Nature of Equilibrium
á 14.2 The Equilibrium Constant Expression
á 14.3 Modifying Equilibrium Constant Expressions
February 25th
Monday Chapter 14: Chemical Equilibrium
á 14.4 Qualitative Treatment of Equilibrium: Le Ch‰telierÕs Principle
á 14.5 Some Illustrative Equilibrium Calculations
February 27th
Wednesday Chapter 14: Chemical Equilibrium
á 14.5 Some Illustrative Equilibrium Calculations
March 3rd
Monday Chapter 15: Acids, Bases, and Acid–Base Equilibria
á 15.1 The Br¿nsted–Lowry Theory of Acids and Bases
á 15.2 Molecular Structure and Strengths of Acids and Bases
á 15.3 Self-Ionization of Water—the pH Scale
March 5th
March 10th
Monday Chapter 15: Acids, Bases, and Acid–Base Equilibria
á 15.4 Equilibrium in Solutions of Weak Acids and Weak Bases
á 15.5 Polyprotic Acids
March 12th
Wednesday Chapter 15: Acids, Bases, and Acid–Base Equilibria
á 15.6 Ions as Acids and Bases
á 15.7 The Common Ion Effect
March 17th
Monday Chapter 15: Acids, Bases, and Acid–Base Equilibria
á 15.8 Buffer Solutions
March 19th
Wednesday Chapter 15: Acids, Bases, and Acid–Base Equilibria
á 15.9 Acid–Base Indicators
á 15.10 Neutralization Reactions and Titration Curves
á 15.11 Lewis Acids and Bases
March 24th
Monday *** No Class ***
March 26th
Wednesday MondayÕs Schedule
Chapter 16: More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions
á
16.1 The Solubility Product
Constant, 
á
16.2 The Relationship Between 
and Molar Solubility
á 16.3 The Common Ion Effect in Solubility Equilibria
March 31st
Monday Chapter 16: More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions
á 16.4 Will Precipitation Occur? Is It Complete?
á 16.5 Effect of pH on Solubility
á 16.6 Equilibria Involving Complex Ions
á 16.7 Qualitative Inorganic Analysis
April 2nd
Wednesday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy
á 17.1 Why Study Thermodynamics?
á 17.2 Spontaneous Change
á 17.3 The Concept of Entropy
á 17.4 Free Energy and Free Energy Change
April 7th
Monday SECOND EXAMINATION (Chapters: 15, and 16)
April 9th
Wednesday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy
á
17.5 Standard Free Energy
Change, 
á 17.6 Free Energy Change and Equilibrium
á
17.7 The Dependence of 
and 
on
Temperature
Monday Chapter 17: Thermodynamics: Spontaneity, Entropy, and Free Energy
á
17.7 The Dependence of 
and 
on
Temperature
á 18.1 Half-Reactions
á 18.2 The Half-Reaction Method of Balancing Redox Equations
á 18.3 A Qualitative Description of Voltaic Cells
á 18.4 Standard Electrode Potentials
á 18.5 Electrode Potentials, Spontaneous Change, and Equilibrium
á 18.6 Effect of Concentrations on Cell Voltage
á 18.7 Batteries: Using Chemical Reactions to Make Electricity
á 18.8 Corrosion: Metal Loss Through Voltaic Cells
á 18.9 Predicting Electrolysis Reactions
á 18.10 Quantitative Electrolysis
á 18.11 Applications of Electrolysis
á 19.1 Radioactivity and Nuclear Equations
á 19.2 Naturally Occurring Radioactivity
á 19.3 Radioactive Decay Rates
á 19.4 Synthetic Nuclides
á 19.5 Transuranium Elements
á 19.6 Nuclear Stability
á 19.7 Energetics of Nuclear Reactions
á 19.8 Nuclear Fission and Nuclear Fusion
á 19.9 Effect of Radiation on Matter
á 19.10 Applications of Radioactive Nuclides
Monday THIRD EXAMINATION (Chapters: 17, 18, and 19)
á 23.1 Alkanes
á 23.2 Alkenes and Alkynes
á 23.3 Conjugated and Aromatic Compounds
á 23.4 Alcohols and Ethers
á 23.5 Aldehydes and Ketones
á 23.6 Carboxylic Acids, Esters, and Amides
á 23.7 Lipids
á 23.8 Carbohydrates
á 23.9 Proteins
á 23.10 Nucleic Acids: Molecules of Heredity
Final Examination will be scheduled during the final exam period between Monday the 19th and Saturday the 24th of May of 2008.
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
ÒI hear, I forget. I see, I remember. I do, I understand.Ó
Chinese proverb