Honors Chemistry - Course Syllabus
Instructor: Rob Wilder
Room 211-A
Contact Information: e-mail – [email protected]
Phone: 582-4347 ext. 1211
Textbook:
Davis, Raymond E., Frey, Regina., Sarquis, Mickey., and Sarquis, Jerry L. Modern Chemistry. Austin, TX:
Holt, Rinehart, and Winston, 2009.
Online Resources:
1) http://www.chemeddl.org/
2) http://chemed.chem.wisc.edu/chempaths/GenChem-Textbook/Introduction-679.html
3) https://www.khanacademy.org/science/chemistry
Class overview:
Honors Chemistry is a look into the world of, mostly, inorganic chemistry. It will touch on the
foundations by which chemists operate. The basic concepts allow for a greater understanding into the
workings and characteristics of the materials we use every day and how life itself operates. Chemistry is
both descriptive and mathematical. We will explore both aspects in depth and you will need to be
proficient in both to be successful in the subject of chemistry.
Class expectations:
 Consistent attendance is important. Make every effort to be in class each day. If you are absent,
it is your responsibility to obtain any make-up work and notes. You may contact me using the email address above. Absences due to school business; field trips, athletic events, etc., do not
excuse you from the work for that day. Plan ahead.
 Come to class prepared each day with paper, pen or pencil, calculator, book, and completed
homework.
 Be on time. Class will begin promptly. Tardies to class will be handled in accordance with school
policy. (p. 19 of Student Planner)
 Portable electronic devices may not be used at any time unless permission is given. Phones and
tablets may not be used on a test as a calculator.
 There is no eating in class. You may drink water only in class, but never when we are in the lab.
 Treat everyone with the same level of respect.
 Raise your hand to be recognized before asking or answering a question.
 Ask for help sooner rather than later.
Assessment and grading: I use a point system to determine grades. Each assignment is given a point
value based on its importance to the unit. For example, unit tests will carry a 100 or more point value,
while a unit quiz may carry a 20 or 30 point value. At the end of each grading period the total points you
have earned will be compared to the total points possible and a percentage grade will be assigned.
Work that is turned in late will receive a 10% reduction for each day it is late up to 5 days, at which time
it will be given a zero. Daily homework grades are not accepted late.
The final course grade will be computed as follows:
(1st nine weeks grade x .45) + (2nd nine weeks grade x .45) + (final exam grade x .10)
Units of Instruction:
1. Introduction to Science and Chemistry: Basic Concepts (Test date: Thurs. 8/29)
 Scientific method
 Laboratory equipment: use and safety
 Mathematics in science: significant figures, scientific notation, formulas, dimensional
analysis, metric system and conversions, percent error
 Properties and classification of matter
 Density
Suggested Labs: Density (Modern p. 39), Behavior of Solids Upon Heating, Separating
the Components of a Mixture (Chromatography – micro), Percentage of Water in
Popcorn (Modern p. 64), Making Observations and Recording Data
2. Atomic Structure
Part I – (Test date: Wed. 9/11)
 Atomic history
 Properties of the atom and subatomic particles (protons, neutrons, electrons)
 Isotopes, atomic number, mass number, and atomic mass
 Nuclear chemistry: fission vs fusion, radioactive decay, half-life
 Atoms, ions, and molecules
Suggested Labs: Rutherford’s Experiment, Law of Conservation of Mass (Modern p. 94)
Half-Life Simulation,
Part II – (Test date: Fri. 9/20)
 Electromagnetic radiation: wavelength, frequency, and energy
 Models of the atom, including the quantum mechanical model
 Electron configurations, valence electrons, ground state, excited state, exceptional
configurations
Suggested labs: Flame Tests,
3. Periodic Table (Test date: Mon. 9/30)
 Periodic table and basic arrangement
 Names and symbols for selected elements
 Oxidation numbers
 Cations and anions
 Periodic trends: electron shielding, atomic size, ionic size, ionization energy,
electronegativity
Suggested labs: Period Trends and the Properties of Elements
4. Bonding (Test date: Fri. 10/11)
 Lewis dot symbols and Lewis structures
 Covalent and ionic bonds, bond polarity
 Single, double, and triple covalent bonds: length and strength
 Molecular geometry
 Molecular polarity
 Intramolecular and Intermolecular forces
Suggested Labs: Effects of Bonding on Properties (Modern p. 216), Building Models,
5. Nomenclature (Test Date: Fri. 10/18)
 Ionic compounds, molecular compounds, and acids
 Polyatomic ions
 Acids Defined: Arrhenius vs Bronsted-Lowry
Suggested Labs: Activity series of Metals
6. Reactions and Equations (Test date: Fri. 11/1)
 Chemical equations: write and balance
 Synthesis, decomposition, single replacement, double replacement, combustion
 Common solubility rules
 Net ionic equations
Suggested labs: Types of Reactions
7. Moles (Test date: Tues. 11/12)
 What is a chemistry mole?
 Mole conversion: mass and particles
 Molar mass and formula mass
 Percent composition
 Empirical and molecular formulas, hydrates
Suggested Labs: Determining the Empirical Formula for a Compound, Percent Water in a
Hydrate, Percent Oxygen in a Chlorate
8. Stoichiometry (Test date: Wed. 11/20)
 Moles-to-moles, moles-to-mass, mass-to-moles, mass-to-mass calculations
 Limiting and excess reagents
 Theoretical, actual, and percent yield
Suggested Labs: Stoichiometry and Gravimetric Analysis (Modern p. 326), How Much
Calcium Carbonate is in an Eggshell? (Modern p.528)
9. Gases (Test date: Fri. 12/6)
 Behavior of gases: Kinetic Molecular Theory related to P, V, and T
 Gas Laws: Boyles, Charles, Gay-Lussac, combined, ideal, and derivatives
 Gas stoichiometry
 Collecting a gas over water and partial pressure
 Rates of effusion and diffusion
Suggested Labs: Molar Mass of Butane, Hydrogen and Oxygen Collecting and Testing,
Triple Point of Dry Ice
10. Solutions
 Solute and solvent
 Solution equilibrium: saturated, unsaturated, and supersaturated
 Solubility and factors that affect it, solubility curves
 Expressing solution concentration: molarity, molality, and mass percent
 Solution acidity: [ H+] , [OH-], pH , pOH
 Solution stoichiometry
 Colligative properties
 Heating curves
Suggested Labs – Heat of Solution, Acid-Base Titration (Modern p.518)
Student Name ____________________________________ Grade: 10 11 12 (circle one)
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Phone Numbers : Home ________________________________
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Student Name ____________________________________ Grade: 10 11 12 (circle one)
Address ________________________________________________________ zip code _____________
Parent’s names _______________________________________________________________________
Phone Numbers : Home ________________________________
Parent’s cell: Father __________________________ Mother _______________________________
E-mail: yours ______________________________________
Parents: father ____________________________ mother _______________________________
Extracurricular activities: _______________________________________________________________