• Credit: This course may not apply toward a degree until CHEM 1117 has been successfully completed. This course has been approved for Level 2 of the core curriculum and as a fulfillment of a science requirement for mechanical, electrical, industrial, and computer engineering majors only.
• Prerequisites: Math 1310 (Algebra) + one year of high school chemistry or CHEM 1301 at UH. * If you have not completed prerequisites for this class, you may be dropped with no refund.*
• Required Text: Silberberg, "Chemistry, The Molecular Nature of Matter and Change, 3e", Mosby, St. Louis, 2002.
• Required: Nonprogrammable scientific calculator, TI-30 or equivalent (buy one if you don’t have one).
• Optional but Recommended: UH Copy Center, Notes Packet
• Optional: E. Weberg "Study Guide to accompany Chemistry", Mosby, St. Louis, MO, 2002
• Optional: Silberberg, et al “Solutions Manual to accompany Chemistry”, Mosby, St. Louis, MO, 2002
• Help: Review sessions will be given the week of each exam. Additional review materials are available at the McGraw Hill Online Learning Center. (http://www.mhhe.com/silberberg/)
• Midterm tests will be given on Friday evenings on the dates listed on the back of this page.
• The following are prohibited in exam rooms: programmable calculators, pagers, beepers, cell phones and any other communication devices or electronic/alphanumeric storage devices.
• November 6 (Wednesday) is the last day to drop a course this semester.
• Thursday, December 5 will be the last lecture for this class. The final exam is at a special time, 11:00 AM, TUESDAY, December 10.
• Lecture attendance is required; students missing two or more lectures may be dropped without warning.
• The class grading system will be based upon weekly quizzes, three midterm exams, and a cumulative final exam. There will be a TOTAL of 100 points available for the entire semester.
• Online weekly quizzes will be administered through WebCT. The Chemistry Computer Lab (Fleming 36) is available for these quizzes. The highest 10 quiz grades throughout the semester will be averaged for a semester quiz grade. The quiz average will account for 10 points of the total 100.
• All examinations will be multiple-choice. The first three exams (20 questions each) will account for a total of 60 of the total 100 points.
• The final exam will be cumulative and will contain 30 questions and count for 30 of the total 100 points.
• Final grades will be equal to the total number of points scored. The grade scale will be (A³90%) (A-³85%) (B+³80%) (B³75%) (B-³70%) (C+³65%) (C³60%) (C-³56%) (D+³52%) (D³48%) (D-³44%) (F, below 44%)
• Students have two weeks after results are posted to resolve questions about scores. No changes after that.
• There are no makeup exams. Two-thirds of the final exam score can be used to substitute for any midterm exam (one) that is missed due to a documented family or medical emergency.
• No more than one exam can be made up using the final score during the semester.

Tables to Learn - Students are responsible for learning the material in each of the following items and tables.
1. The names and symbols of the first 36 elements in the periodic table (H - Kr).
2. Table 1.2 (p 17) SI Base Units
3. Table 1.3 (p 18) Common Decimal Prefixes Used with SI Units (Bold only)
4. Table 2.3 (p 67) Common Monatomic Ions
5. Table 2.4 (p 69) Some Metals That Form More Than One Monatomic Ion
6. Table 2.5 (p 69) Common Polyatomic Ions
7. Table 2.6 (p 70) Numerical Prefixes for Hydrates and Binary Covalent Compounds

Course Schedule
There will be no exam questions covering topics not specifically listed or included in class handouts.

Components of Matter	2.1 Elements, Compounds, and Mixtures 2.5 Atomic Theory Today
Quantum Theory and Electronic Structure	7.1 The Nature of Light 7.2 Atomic Spectra 7.4 The Quantum Mechanical Model of the Atom 8.2 Characteristics of Many-electron Atoms 8.3 The Quantum Mechanical Atom and the Periodic Table 8.4 Trends in Some Key Periodic Atomic Properties
Models of Chemical Bonding	2.7-2.8 Compounds: Introduction to Bonding and Formulas, Names, and Masses 3.1 The Mole (and Chemical Formulas) 9.1 Atomic Properties and Chemical Bonds 9.2 Ionic Bonding Model 9.5 An Introduction to Metallic Bonding 9.3 The Covalent Bonding Model 9.4 Between the Extremes: Electronegativity and Bond Polarity
EXAM 1, Friday, September 20, 5:30 pm, Melcher 160, 180
Properties of Molecules	10.1 Depicting Molecules and Ions with Lewis Structures 10.3 VSPER Theory and Molecular Shapes 10.4 Molecular Shape and Molecular Polarity
Chemical Reactions	3.3 Writing and Balancing Chemical Reactions 3.4 Calculating the Amounts of Reactant and Product 3.5 Fundamentals of Solution Stoichiometry
Chemical Kinetics	16.1 Factors That Influence Reaction Rate 16.2 Expressing the Reaction Rate 16.3 The Rate Law and Its Components 16.4 Integrated Rate Laws: Concentration Changes over Time 16.5 The Effect of Temperature on Reaction Rate 16.6 Explaining the Effect of Concentration and Temperature 16.8 Catalysis: Speeding Up a Chemical Reaction
EXAM 2, Friday, October 18, 5:30 pm, Melcher 160, 180
Chemical Equilibrium	17.1 The Dynamic Nature of the Equilibrium State 17.2 The Reaction Quotient and the Equilibrium Constant 17.4 Reaction Direction: Comparing Q and K 17.5 How to Solve Equilibrium Problems 17.6 Reaction Conditions and the Equilibrium State: LeChatelier's Principle
Thermodynamics	6.1 Forms of Energy and Their Conversion 6.2 Enthalpy: Heats of Reaction and Chemical Change 6.3 Calorimetry: Laboratory Measurements of Heats of Reaction 6.4 Stoichiometry of Thermochemical Equations 6.5 Hess's Law of Heat Summation 20.1 The Second Law of Thermodynamics: Predicting Spontaneous Change 20.2 Calculating the Change in Entropy of a Reaction 20.3 Entropy, Free Energy, and Work 20.4 Free Energy, Equilibrium, and Reaction Direction
Electrochemistry	21.1 Half-Reactions and Electrochemical Cells 21.2 Voltaic Cells: Using Spontaneous Reactions to Generate Electrical Energy 21.5 Electrochemical Processes in Batteries 21.6 Corrosion: A Case Study 21.7 Electrolytic Cells: Using Electrical Energy to Drive a Nonspontaneous Reaction
EXAM 3, Friday, November 15, 5:30 pm, Melcher 160, 180
Gases	5.1 Overview of the Physical States of Matter 5.2 Gas Pressure and its Measurement 5.3 The Gas Laws and Their Experimental Foundation 5.4 Further Applications of the Gas Laws
Liquids and Solids	12.3 Types of Intermolecular Forces 12.4 Properties of the Liquid State 12.6 The Solid State: Structure, Properties and Bonding
Materials Chemistry	12.7 Advanced Materials / 15.5 The Monomer-Polymer Theme I: Synthetic Macromolecules
FINAL EXAM, Tuesday, December 10, 11:00am, Melcher 160, 180 NOTE SPECIAL TIME FOR FINAL!!