Download Week - Mat-Su School District

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