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Colony High School Chemistry 2009-2010 Mr. Greg Giauque, Instructor Room 123 Description: This is an advanced Science course designed to prepare the student for either college Chemistry or AP Chemistry. The course covers the equivalent of one full year of general Chemistry, comparable to a first year course at a college or university. The course is a rigorous math-based course, with a strong laboratory component. It is intended for students who have demonstrated a willingness to commit considerable time to studying and completing assignments outside of class. The course will develop the student's ability to incorporate mathematical skills in the solution of chemistry problems, both through the use of textbook problems and laboratory activities. Since a significant emphasis will be placed on developing the student's ability to solve problems through dimensional analysis and estimation students are required to be enrolled in Algebra. Students will be required to do extensive writing, and to keep a thorough and accurate ongoing laboratory notebook. Grading Scale: 90-100% A, 80-89% B, 70-79% C, 60-69% D, 0-59% F Grade Weights: Exams 50%, Quizzes & Labs 30%, Homework 20% Grades: Grades will be determined by taking the number of points earned divided by the number of total possible points. Points can be earned by participating in the following activities: tests, quizzes, laboratory exercises, homework, and classroom participation (includes notetaking). There are no extra credit assignments unless all other assignments are completed. Your total points from the term will comprise 80% of your overall grade. The final exam will count 20%. REQUIRED materials: Scientific Calculator (must have LOG key, Ti 83 preferred), Text Book, Graph paper, Pencil, Straight edge, Lab Notebook, Colored Pencils & Black or Blue Pen. SUGGESTED materials: Periodic Table, 3 ring Binder TEXT: Zumdahl, Steven, Zumdahl, Susan L., DeCoste, Donald. Word of Chemistry. Evanston, Illinois: McDougal Littell. 2007. Laboratory Rules: See safety contract - YOU MUST WEAR GLASSES OR GOGGLES IN THE LAB AT ALL TIMES! Points may be deducted for not following this rule. The lab safety notes will discuss appropriate dress and procedures, which will be reviewed and discussed prior to the first lab session. Your safety contract MUST be on file before working in the lab. Students will keep a separate Lab Notebook that will be turned in for a grade upon lab completion. This notebook will be a 9.75” X 7.5” composition note book. The following is a listing of the labs scheduled for the course for the 2009 – 2010 school year. Labs may be added or removed at the instructor’s discretion. Labs will be student conducted (hands on) and are used to reinforce the materials taught in the lecture portion of the course. Laboratory Assignments: 1. Introduction to Lab Practices 2. MSDS Project 3. Measurement/ Conversion Lab 4. The Densities of Liquids and Solids 5. Naming Compounds Lab 6. Density Lab 7. Isotope Lab 8. Determination of Chemical Formula 9. Properties of Hydrates 10. Finding the Ratio of moles of reactants in a chemical reaction 11. Finding moles of CaCO3 12. Finding the Stoiciometric ratio of reactants in a chemical reaction 13. Analysis of an Unknown Chloride 14. Simple Titration 15. Determination of the Equilibrium constant of a Weak Acid. 16. Coffee Cup Calorimetry 17. Thermochemistry & Hess’s Law 18. Ink Chromatography 19. Gas Spectrum Analysis 20. Qualitative Analysis of Cations & Anions 21. Boyle’s Law 22. Charles Law 23. Lighter Lab 24. Triple point of Dry Ice 25. Kinetics of a reaction 26. Equilibrium & Le Chatelier’s Principle 27. Determining the Dissociation Constant of a weak acid 28. Determining the pKa of an unknown acid 29. pH Measurements of Buffers & their properties 30. Determination the Ksp of an Ionic compound 31. Spontaneity of a reaction, finding Gibbs free energy 32. Electrochemical Cells 33. Identification of an unknown substance 34. Determination of an ester Lab Text: Vonderbrink, Sally Ann, Laboratory Experiments for Advanced Placement Chemistry. Batavia, IL: Flinn Scientific, Inc. 2001. Slowinski, E.J., W.C., Wolsey, W.L. Masterson. Chemical Principles In The Laboratory, Eighth Edition, United States: Brooks/ Cole Thomson Learning Inc.2005 Topics Covered in Chemistry 2009-2010 1. Structure of matter (20)% a. Atomic Theory and atomic Structure i. Theory ii. Atomic Masses, Atomic Mass, Atomic Number, Isotopes iii. Electron Energy Levels, Atomic spectra, Quantum numbers, Orbitals iv. Periodic Relationships, radii, electronegativity, ionization energy, affinity, oxidation states. b. Chemical Bonding i. Binding forces 1. ionic, covalent, metallic, H bonding, van der Walls 2. Relationships to states, structure & properties of matter 3. Polarity of bonds, electronegativities c. Molecular models i. Lewis Structures ii. Valence Bonds, sigma, pi, resonance, hybridization iii. VSEPR Theory d. Geometry, isomerism, relationship to properties e. Nuclear Chemistry, half lives, radioactivity, applications, nuclear equations 2. States of matter (20%) a. Gases i. Boyles & Charles’s laws ii. Ideal gas law 1. Ideal gas law 2. Partial pressures iii. Kinetic Molecular Theory 1. Ideal gas law theory 2. Avogadro’s Theory & mole concept 3. Kinetic Energy & temperature 4. Deviations fro the gas law b. Liquids & Solids i. Liquids & Solids from the Kinetic Molecular viewpoint ii. Phase diagrams iii. Changes in state (triple points) iv. Structure of solids, Lattice energy c. Solutions i. Types of solutions & solubility ii. Concentrations, molarity, molality, normality iii. Colligative properties & Raoult’s law iv. Non-ideal behavior 3. Reactions (40%) a. Reaction types i. Acid Base 1. Arrhenius 2. Bronstead Lowry 3. Lewis ii. Precipitation iii. Oxidation-reduction (redox) 1. Oxidation numbers 2. The electrons role 3. Electrochemistry, electrolytic & galvanic cells, Faradays laws, standard half-cell potentials, Nernst equation b. Stoichiometry i. Net ionic equations ii. Balancing equations including redox iii. Mass & volume relationships, empirical formula, molecular formula, mole concept, limiting reactants. c. Equilibrium i. Dynamic equilibrium 1. physical & chemical: LeChatelier’s principle, equilibrium constants. ii. Quantitative 1. Equilibrium constants for gas reactions, Kp & Kc 2. Equilibrium constants for reactions in solution a. Asids & bases, pK & pH b. Solubility Ksp d. Kinetics i. Reaction rates ii. Reaction orders iii. Effect of temperature on rates iv. Energy of activation & Catalysts v. Rate determining step e. Thermodynamics i. State functions ii. First Law, Change in enthalpy, heat of formation, heat of reaction iii. Second Law, entropy, free energy of formation, free energy of reaction iv. Relationships of change in free energy to equilibrium constants and electrode potentials 4. Descriptive Chemistry (10%) a. Chemical reactivity & products of chemical reactions b. Periodic relationships i. Horizontal, vertical & diagonal ii. Group A & B elements iii. Element Families c. Organic chemistry i. Hydrocarbons & functional groups ii. Physical & chemical properties iii. Bonding, structure, empirical & chemical formula 5. Laboratory (10%) a. Notebook required b. Lab format c. Listing of labs