Syllabus - CH 102 - General Chemistry 102
Manhattan College - Summer (II) 2019
Instructor: Dr. Carolyn Hyman
Chemistry 102 is the first part of a one year course in general chemistry. Students attend two 3 hour classes (Mon. and Wed.) a week starting July 1st, and ending on August 14th. Major topics to be covered include the gas laws, kinetics, equilibrium, acid-base chemistry, and electrochemistry.
Required Text: Chemistry: The Molecular Nature of Matter, 7thedition N. Jaspersen, A. Hyslop, and J.E. Brady.
Office: Chemistry Department Office, Hayden 4thfloor
Class Meeting Day and Time: Mon/Wed 1pm - 4 pm. Hayden 202
Academic Honesty Policy: Manhattan College places special emphasis on academic honesty. You may not lie, cheat, or steal in your academic endeavors, and you may not tolerate that behavior in others. If you have any direct knowledge of an apparent violation of the Honor Code you must provide your teacher with the name or identity of the person(s) alleged to have committed the violation(s). All violations of the Honor Code, including nonreporting of violations by others, will be reported to the dean of your school. All forms of clear academic dishonesty will result in an "F" for the course
Cell Phone and laptop policy: Cell phones will be turned off and stored in backpacks during class. Failure to comply with these policies will result in five points (for each offense) deducted from the upcoming exam grade.
Attendance: Attendance is required and will be taken in each class, but will not count towards grades. You are responsible for all the material covered in any class you miss; you are responsible for fulfilling all course requirements and for completing all course assignments; you are responsible for the entire content of the course; if you are absent from an exam, I am not required to provide a substitute exam. A scientific calculator is required for class. It must have basic functions capable of computations with numbers expressed in scientific notation. The Texas Instrument TI-84 models work well.
Recording Policy: You are encouraged to take copious notes during class. But you may not make audio, video, or photographic recordings of the lectures.
Exams There will be three 50-minute exams and a cumulative final exam. The ‘hour’ exams are held during class time. They test knowledge & understanding of the material that was studied during the previous three classes; but they can include a few questions on important topics from earlier exams. The tentative exam dates are There are no make-up exams!
Grades The exams make up 75% of your grade in the course. The cumulative final exam makes up 25% of your grade.
Homework: There will be reading and assigned problems at the end of each chapter covered in the text. This will reinforce the work covered in class, but will not be collected, nor will it count towards your grade. The intended sequence is for the assigned reading and problems to be done before each class that will be devoted to covering that material.
Make-up exams: These will be given only under extremeextenuating circumstances - such as a hospitalization or a death in the family. A legitimate verifiable note must be presented.
Final: The final exam is cumulative. The date is Wed. Aug 14th. Please plan accordingly. No exceptions will be made.
Tentative Exam Dates:
Tentative Schedule: Note that selected topics in each chapter will be covered.
July 1st Chapter 10.The properties of gases. The ideal gas law and its use in stoichiometry. The kinetic-molecular theory of gases. Deviations from ideal gas behavior.
July 3rd Chapter 13. Chemical Kinetics. Definition of the rate of a reaction. The dependence of rate on concentration. Using initial rates to determine rate laws. Activation energy and the transition state. The relationship between temperature, activation energy, and rate. Analysis of multistep reaction mechanisms. Catalysis, heterogeneous catalysts, and enzymes.
July 8th There will be a 1 hour exam at the start of class covering Chapters 10 and 13. Then the remainder of the class will begin coverage of Chapter 14. Chemical Equilibrium. Writing equilibrium constant expressions. Calculating equilibrium constants. Using equilibrium constants to predict the direction of chemical reactions and the equilibrium concentrations of reaction components. Using Le Châtelier’s Principle to predict the effect of volume, temperature, and pressure changes on the equilibrium concentrations of reactants and products.
July 10th The class will complete coverage of Chapter 14, Chemical Equilibrium.
July 15th Chapter 15. Acids and Bases, A Molecular Look. Qualitative aspects of acid-base chemistry in aqueous solution with emphasis on the Brønsted-Lowry definition. The idea of relative acid/base strength. The reciprocal relationship between conjugate acids and bases.
July 17th Chapter 16. Acid Base Equilibria in Aqueous Solution. The calculation of the equilibrium concentrations of the species in solutions of weak and strong monoprotic acids and bases; salts, and buffers.
July 22nd There will be a 1 hour exam at the start of class covering Chapters 14, 15, and 16. Then the remainder of the class will begin coverage of Chapter 11. Intermolecular Attractions and the Properties of Liquids and Solids. The nature of intermolecular interactions: dipole-dipole forces, London forces, and hydrogen bonding. Understanding the physical properties of pure substances – compressibility, diffusion, surface tension, viscosity, volatility, melting and boiling temperatures – in terms of intermolecular forces. Changes of state, heating diagrams, and the phase diagrams of pure substances. The bonding in and properties of metallic, ionic, covalent, and molecular solids. The crystal structures of copper, sodium chloride, diamond, graphite, buckminsterfullerene, ice, and carbon dioxide.
July 24th The class will complete coverage of Chapter 11. Intermolecular Attractions and the Properties of Liquids and Solids.
July 29th Chapter 12. The Properties of Solutions. Understanding the solubility of salts and molecular substances in terms of the intermolecular forces of the solute and solvent. Qualitative aspects of colligative properties, and of the effect of temperature and pressure on solubility.
July 31st Chapter 18. Thermodynamics. Understanding and calculating changes in enthalpy, entropy, and free energy. Using free energy changes to predict how ‘favorable’ a reaction is. How free energy changes depend on temperature. The relationship between free energy change and the equilibrium constant of a reaction.
August 5th There will be a 1 hour exam at the start of class covering Chapters 11, 12, and 18. Then the remainder of the class will begin coverage of Chapter 19. Electrochemistry. Constructing galvanic/voltaic cells. Utilizing standard reduction potentials to calculate the values of cell potentials, to predict the course of chemical reactions, to discuss relative chemical behavior, and to balance redox reactions. Commercial voltaic cells. The chemistry of electrolysis. The corrosion of iron.
August 7th The class will complete coverage of Chapter 19.
August 12th Final Exam Review.
August 14th Final Exam
- Teacher: Hyman Carolyn