Download AP Chemistry - Chagrin Falls Schools

AP Chemistry Syllabus, 2012-13
Mrs. Christine Deighan
[email protected]
VM: 440-247-2072 ex 4422
AP Chemistry is the equivalent of freshman college inorganic chemistry.
Course Overview
Advanced Placement Chemistry meets one and one half periods per day for 75 minutes. AP Chemistry is a
second year chemistry course that prepares students to take the AP exam in May. Upon completion of the
course, students will have a solid background in introductory chemistry and the accompanying laboratory
component.
Fees
$25.00, AP Exam fee due 2nd semester
Materials
Students will need a three-ring notebook, book cover, dividers and a scientific calculator.
Text
Chemistry by Zumdahl and Zumdahl 7th Edition, Houghton Mifflin Company, 2007.
ISBN: 978-0-618-52844-8
Additional Reference Materials
Laboratory Experiments for Advanced Placement Chemistry by Sally Ann Vonderbrink, Ph.D., Flinn Scientific,
Inc., 1995. ISBN: 1-877991-34-1
Multiple Choice and Free Response Questions in Preparation for the AP Chemistry Examination by Demmin
and Hostage, 5th Edition, D & S Marketing Systems, 2005.
Flinn Labs, Flinn Scientific Company Catalog, 2008.
Chemistry: The Central Science Lab Book, by Nelson and Kemp, 10th Edition, Prentice Hall, 2006. ISBN: 013-146479-5
The Ultimate Equations Handbook by Hague and Smith, Flinn Scientific, 2001. ISBN: 1-877991-63-5
Assignments and Time Allotment
There are four types of assignments that students are expected to complete for each unit that is covered in class:
homework, lab(s), a chapter test, and free response questions. Typically, one chapter is covered every 8-10
days. Weekly assignment sheets are handed out to students and posted on line for reference.
Lab Reports
Students are required to complete a lab report for each student conducted lab experience. Reports include the
following components: Title, Purpose, Procedure, Original Data, Follow Up (Questions, Graphs, Calculations),
and Conclusion. Labs may be typed or handwritten, but the original data must be included in the lab report.
Grading
The instructor follows the school grading scale. Grades will be posted via the on-line gradebook.
Science Department Late Policies
7th Grade
8th Grade
9th Grade
10th Grade
11th Grade
12th Grade
Major Projects: 5% each day; after five days, no credit will be given
Everyday homework: 50% credit for a day late; after one day, no credit will be
given
Major Projects: 10% each day; after three days, no credit will be given
Everyday homework: 50% for one day late; after the first day late, no credit
will be given
Major Projects: 20% each day; after two days, no credit will be given
Everyday homework: NO credit will be given
Major Projects: 50% for one day late; after the first day late, no credit will be
given
Everyday homework: NO credit will be given
NO late work is accepted
NO late work is accepted
**If you are at school during any part of the day that an assignment is due, are on a school field trip, or on a
planned absence you are required to hand in the assignment to your teacher on the assigned date. Failure to do
so will result in an enforcement of the aforementioned late policies. Also, if a long term project was assigned
and you were either absent the day it was due or days leading up to the assignment, the expectation is that you
hand the assignment in on time.
Course Outline
Unit 1: Review of Classification of Matter, Atomic Theory and The Mole (3 weeks)
Topics
Classification of matter, properties of matter, units of measurement, uncertainty, significant figures,
dimensional analysis, atomic theory based on Dalton, Thomson, Millikan, Rutherford and the modern atomic
model, isotopes, atomic mass, mass number, regions of the periodic table, nomenclature, balancing chemical
equations, molar mass, percent composition calculations, the mole and calculations, empirical and molecular
formulas, limiting reactants, percent yield.
Student Conducted Lab Experiences
Determination of the Empirical Formula of Silver Oxide
Identification of Substances by Physical Properties
Separation of the Components of a Mixture
Gravimetric Analysis of a Metal Carbonate
Gravimetric Analysis of a Chloride Salt
Unit 2: Reactions and Stoichiometry of Aqueous Solutions
Topics
Strong vs. weak electrolytes, solubility rules, single and double replacement reactions, acid-base reactions,
Redox reactions, molarity calculations, dilution calculations, net ionic equations.
Student Conducted Lab Experiences
Chemical Reactions of Copper and Percent Yield
Determining the Stoichiometry of Chemical Reactions
Oxidation Reduction Titrations
An Activity Series
Unit 3: Thermochemistry
Topics
First Law of Thermodynamics, Enthalpy and calculations, Hess’s Law and Calculations, state functions,
spontaneous reactions, 2nd Law of Thermodynamics, Entropy, reversible processes, 3rd Law of
Thermodynamics, entropy change calculations, Gibbs Free Energy, standard free energy calculations, free
energy and equilibrium constants.
Student Conducted Lab Experiences
Thermodynamics – Enthalpy of Reaction and Hess’s Law
Unit 4: Electronic Structure of Atoms
Topics
The electromagnetic spectrum, Quanta and Photons, photoelectric effect, Bohr’s model and the Bright Line
Spectrum, DeBroglie, Heisenberg, Schrodinger, The Quantum Mechanical Model of the Atom, effective
nuclear charge, electron configurations, relationship between configurations and periodicity.
Student Conducted Lab Experiences
Flame tests of various metals (instructor created lab)
Unit 5: Periodic Properties
Topics
Electron shells vs. atomic radius, periodic properties including: ionization energy, electron affinities, common
reactions with metals and nonmetals, characteristics of groups, ionic and atomic radius.
Unit 6: Chemical Bonding
Topics
Lewis symbols and the octet rule, ionic bonding, lattice energy, ionic vs. atomic radius, covalent bonding, bond
polarity and electronegativity, Lewis structure, resonance structures, exceptions to the octet rule, strength of
covalent bonds.
Unit 7: Geometry and Bonding Theory
Topics
Molecular geometry, VSEPR theory, bond polarity, hybrid orbitals, multiple bonds, sigma and pi bonds
Student Conducted Lab Experiences
Molecular Geometries of Covalent Molecules: Lewis Structures and VSEPR Theory
Unit 8: Gases
Topics
Characteristics of gases, pressure, Boyle’s Law, Charles’ Law, Avogadro’s Law, Ideal Gas Law, Combined Gas
Law, Dalton’s Law of Partial Pressures, mole fraction, Kinetic Molecular Theory, Graham’s Law, real vs. ideal
gases
Student Conducted Lab Experiences
Determining the Molar Volume of a Gas
Calculation of the Molar Mass of a Gas
Unit 9: Intermolecular Forces, Liquids and Solids
Topics
Intermolecular forces: Van der Waals, ion-dipole, dipole-dipole, London dispersion, hydrogen bonding,
polarizability, periodic trends related to intermolecular forces, viscosity, surface tension, cohesive forces,
adhesive forces, capillary action, phase change vocabulary, vapor pressure and boiling point, phase diagrams,
normal melting point, triple points, critical point, structure of solids: crystalline, amorphous, molecular,
covalent network, ionic, metallic
Unit 10: Properties of Solutions
Topics
Solvation, hydration, enthalpy of solution formation, solution vocabulary, factors that affect solubility, periodic
trends related to solubility, Henry’s Law and calculations, concentration measures: mass percent, mole fraction,
molartiy, molality, colligative properties, Raoult’s Law, colloids.
Student Conducted Lab Experiences
Molar Mass by Freezing Point Depression
Unit 11: Kinetics
Topics
Reaction rates and factors that affect rate, concentration and rate, 1st Order Integrated Rate Law and
calculations, 2nd Order Integrated Law and calculations, half life, collision model, activation energy, reaction
mechanisms, catalysts.
Student Conducted Lab Experiences
Kinetics of a Reaction
Kinetics Lab – Reactions Between Crystal Violet and NaOH
Unit 12: Equilibrium and Acid-Base Equilibria (7 weeks)
Topics
Haber process, equilibrium expressions, Kc and Kp and calculations, heterogeneous equilibrium, Calculating
equilibrium constants, ICE charts, reaction quotients, LeChateliler’s Principle, Arrhenius, Bronsted-Lowry,
Lewis, pH scale and calculations, strong acids and bases, weak acids and Ka, percent ionization, weak bases and
Kb, pKa, pKb, common ion effect, buffered solutions, buffer capacity, acid-base titrations, solubility equilibria.
Student Conducted Lab Experiences
Equilibrium using Graduated cylinders
Determination of the Equilibrium Constant for the Formation of FeSCN+2
Titration of a Strong Acid with a Strong Base
Acid-Base Titrations
Exploring Equilibrium – It Works Both Ways
Determination of Ka of Weak Acids
PH Properties of Buffered Solutions
Determination of the Solubility-Product Constant for a Sparingly Soluble Salt (Nelson, Kemp)
Hydrolysis of Salts and pH of Buffer Solutions (Nelson, Kemp)
PH Properties of Buffer Solutions (Flinn)
Unit 13: Electrochemistry
Topics
Redox reactions and terminology, voltaic cells and reactions, cell EMF using standard reduction potentials,
spontaneity of redox reactions, Nerst Equation.
Student Conducted Lab Experiences
Electrochemistry – Galvanic Cells
Unit 14: Nuclear Energy
Topics
Nuclear equations, types of decay, nuclear stability, rates of decay, half-life.
Unit 15: Organic Chemistry
Topics
Alkanes, Alkenes and Alkynes – structure, isomers, nomenclature, common reactions, and periodic trends
Nomenclature and structure of common functional groups including: alcohols, ethers, aldehydes, ketones,
carboxylic acids, esters and amines