AP Chemistry Syllabus, 2012-13

Mrs. Christine Deighan

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: 0-13-146479-5

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 / 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
8th Grade / 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
9th Grade / Major Projects: 20% each day; after two days, no credit will be given
Everyday homework: NO credit will be given
10th Grade / Major Projects: 50% for one day late; after the first day late, no credit will be given
Everyday homework: NO credit will be given
11th Grade / NO late work is accepted
12th Grade / 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, periodictrends 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