Course:  4440 Advanced Placement Chemistry

Grade: 12

Instructor: Frank Karnish

Email:  karnishf@panthervalley.org

Phone: 570-645-2171

 

Course Information:

Class Meeting:  M-F

Room Number: 125

 

Course Description: 

The Advanced Placement chemistry course is designed to be the equivalent of the general chemistry course usually taken during the first college year.  Students in this course will attain a significant depth of understand of fundamentals and a competence in dealing with chemical problems and their calculations.  This course is designed to meet the Curricular Requirements as described by College Board.  The class meets for three 45-minute periods and three 90-minute periods  per week.

 

Prerequisite: 

• Successful completion of Chemistry and Algebra II

 

Course Objectives: [CR2]

After completing the course, the student will be able to explain how:

• Chemical elements are the building blocks of matter, which can be understood in terms of the arrangements of atoms.
• Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them.
• Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons.
• Rates of chemical reactions are determined by details of the molecular collisions.
• The laws of thermodynamics describe the essential role of energy, explain, and predict the direction of changes in matter.
• Bonds or attractions that can be formed can be broken.  These two processes are in constant competition, sensitive to initial conditions and external forces or changes.

 

Textbook(s): [CR1]

Chemistry: The Central Science by Brown, LeMay and Bursten, 13^th Edition, Pearson/Prentice Hall, 2015, ISBN 0-13-357412-8

 

Supplemental Sources:

• AP Chemistry Preparation Guide. Bobrow Test Preparation Services. 4^th Edition .Hoboken, 2000. CD-ROM.

• Chemistry, 10th Edition, Timberlake, Benjamin Cummings, N.Y., 2009. ISBN: 978-0-13-601970-1.
• Chemistry: Essential Laboratory Manual, 9^th Edition.  Timberlake. Pearson/Prentice Hall.  NJ.  2006. ISBN 0-8053-3023-2
• Chemistry, 8^th Edition. Zumdahl and Zumdahl, Brooks Cole, CA.  2010.  ISBN: 978-0-547-16817-3
• Science in Motion: Wilkes University.  Mobile educator with equipment such as GC, HPLC, IR., UV-VIS Spectrophotometers
• The Ultimate Chemical Equations Handbook by Hague and Smith, Flinn Scientific, Inc. 2001, ISBN 1-877992-63-5
• Laboratory Experiments for Chemistry the Central Science by Brown, LeMay and Bursten, 10^th Edition, Pearson/Prentice Hall, 2006
• Advanced Chemistry with Vernier by Randall, 1st Ed., Vernier Software and Technolgy, 2004, ISBN 1-929075-36-7

 

Other Required Materials:

• OSHA - approved goggles
• a scientific calculator
•  bound laboratory notebook

 

Suggested Materials:

• 3 ring binder for notes and organizing handouts

 

 

Preparation:

• Students will probably need to spend at least five hours a week studying outside of class.

• You will get the most out of the class if you:
• read the new material before coming to class,
• make adequate notes during lecture,
• Review text material discussed during class.
• Complete all assignments

 

 

Tentative Schedule:

• Unit 1:  Measurement, Matter, Molecules and Formula Units         (3 weeks)

• Chapter 1:  Matter and Measurement; classification of matter, properties of matter, units of measurement, dimensional analysis [C6]
• Chapter 2:  Atoms, Molecules and Ions; Atomic Theory, evidence of atomic structure, modern atomic structure, atomic weight, periodic table, molecular and ionic compounds (writing chemical formulas and nomenclature including acids and bases) [C1]
• Labs:  Basic Laboratory Techniques, (measurement, significant figures and dimensional analysis), Gas Chromatography:  separation of a mixture of alcohols (Science in Motion) HPLC:  caffeine analysis (Science in Motion) (6 class periods total) [C5], [C7]

 

 

• Unit 2:  Stoichiometry and Heat of Reaction            (5 and a half weeks)

• Chapter 3:  Stoichiometry, calculations with chemical formulas and equations, (formula and molecular weight, percent composition, molar mass, moles and number of particles, determining empirical and molecular formulas, balancing equations, reaction types, reaction Stoichiometry including calculation of amounts of substances, limiting reagents, theoretical and per cent yields.  [C3], [C4], [C6]
• Chapter 4:  Aqueous Reactions and Solution Stoichiometry; more reaction types (precipitation, acid-base neutralizations, oxidation-reduction), molarity, solution Stoichiometry calculations.  [C3], [C4[, [C6]
• Chapter 5:  Thermochemistry; energy, 1st Law of Thermodynamics, enthalpy and enthalpies of reaction, Hess’s Law, enthalpies of formation, calorimetry [C3], [C6]
• Labs:  Determination of a Chemical Formula, Determination of the Percent Water of Hydration, Determining Mole Ratios in a Chemical Reaction, Determining the Enthalpy of a Reaction, Synthesis of Alum (theoretical and Percent yields).  (12 class periods total) [C5], [C7]

 

 

• Unit 3:  Atomic Structure and Periodicity     (4 weeks)

• Chapter 6:  Electronic Structure of Atoms; wave nature of light, quantum theory, photons, line spectra, uncertainty principle, matter waves, atomic orbitals, electron configurations, quantum number sets, configurations and the periodic table [C1], [C4]
• Chapter 7:  Periodic Properties; history of the Periodic Table, effective nuclear charge and shielding, period and group trends in ionization energy, electron affinities, atom and ion sizes, electronegativity.  [C4]
• Labs:  Flame Tests ( 2 periods)

 

 

• Unit 4:  Bonding, Bonding Theories and Organic Chemistry           (4 weeks)

• Chapter 8:  Chemical Bonding; types of bonding, octet rule (and exceptions), ionic bonding and lattice energy, covalent bonding and drawing [C1]
• Chapter 9 Molecular Geometry and Bonding Theories; VSEPR model, molecular shapes and hybridization, multiple bonds ,valence bond theory, molecular orbital theory. [C1]
• Chapter 25 Organic Chemistry;  alkanes, alkenes, alkynes, functional groups and reactions that result in their formation, combustion, substitution and addition reactions, [C4]
• Labs:  HyperChem, a computer modeling program, IR:  Spectra of plastic films,  Synthesis and Analysis of Aspirin       ( 9 periods) [C5], [C7]

• Lewis structures, bond polarity, resonance structures, bond order, length and strength.

 

 

• Unit 5:  States of Matter        (6 weeks)

• Chapter 10 Gases;  characteristics of gases, pressure, Boyle’s Law, Charles’ Law, combined gas law, quantity-volume relationship and Avogadro’s Hypothesis, ideal gas law, Kinetic-Molecular Theory and gas behavior, gas density, Dalton’s Law of Partial Pressures; effusion, diffusion and Graham’s Law, deviations from ideality and the van der Waal’s equation. [C2], [C6]
• Chapter 11:  Intermolecular Forces, Liquid and Solids; K-M theory descriptions, intermolecular forces (dispersion, dipole-dipole, hydrogen bonding), liquid properties (viscosity, surface tension, b.p., vapor pressure, volatility, enthalpy of vaporization); structure, properties and bonding of solids( atomic, molecular, ionic, covalent network, metallic), phase changes and total energy, phase diagrams.[C2]
• Chapter 13 Solutions: the solution process, spontaneity and disorder, solution formation, solubility factors, concentration expressions, colligative properties and their calculations [S2], [C6]
• Labs:  Molar volume of a gas, Molar mass of a volatile Liquid , Evaporation and Intermolecular attractions., Boyle’s Law, Pressure-temperature relationship in Gases, Freezing Point Depression, Precipitations and Net Ionic Equations, the Activity Series. (18 periods) [C5], [C7]

 

 

• Units 6 Equilibrium    ( 6 weeks)

• Chapter 15 Equilibrium; equilibrium constant and K calculations, K_p and K_c, magnitude of K, K and Q, and predicting reaction direction; heterogeneous equilibria, Le Chatlier’s Principleand stress to equilibrium system       [C3], [C6]
• Chapter 16 Acid-Base Equilibria; characteristics of acids and vases, definitions, (Arrhenius, Bronsted-Lowry, Lewis); conjugate acid-base pairs, [H⁺] concentration and pH, [OH^-] and pOH, K_w, strong acids and bases, weak acids and bases, K_a and K_b calculations and relationship, acid-base properties of salt solutions, factors affecting acid  and base strengths. [C3], [C6]
• Chapter 17 Additional Aspects of Aqueous Equilibria; common ion effect, buffers (composition, capacity, pH range, addition of strong acid or base), buffer calculations, acid-base titrations (strong acid-strong base, weak acid-strong base, weak acid-strong base, polyprotic acids); solubility equilibria, solubility and K_sp, solubility and the common ion effect, solubility and pH, formation of complex ions, precipitations and separation of ions.,  Qualitative Analysis schemes.[C3], [C6]
• Labs:  standardization of NaOH, acid-base titrations, Ksp of Ca(OH)₂,  Buffers, Qualitative Analysis of an unknown   ( 20 periods) [C5], [C7]

 

 

• Unit 7 Thermodynamics and Electrochemistry        ( 3 weeks)

• Chapter 19, Thermodynamics; spontaneity, entropy and the 2^nd law of thermodynamics, qualitative predictions of DS, entropy changes in reactions, Gibbs free energy, free energy and temperature, free energy and K         [C3], [C6]
• Chapter 20:  Electrochemistry; oxidation states, balancing redox, voltaic cells, cell potential at standard conditions, reduction potential tables and the strength of oxidizing and reducing agents, EMF and DG, Nernst equation and finding concentrations, batteries, electrolysis and electrolytic cells, electrolytic calculations.
• Labs:  Electrochemistry:  Voltaic Cells      [[C5], [C7]      ( 3 periods)

 

 

• Unit 8 Kinetics and Nuclear Chemistry         ( 3 weeks)

• Chapter 15  Chemical Kinetics; factors affecting reaction rates, reaction rates and time, rates and stoichiometry, rate laws, isolation method of determining reaction orders and k, 1^st order kinetics, 2^nd order kinetics, rate and temperature dependence, Arrhenius equation, collision theory, activation energy, reaction mechanisms, elementary and multi-step mechanisms, rate law for the rate determining step, determining a possible rate law from the proposed mechanism.  [C3], [C6]
• Chapter 21:  Nuclear Chemistry; radioactivity, nuclear equations, alpha, beta and gamma decay, stability and radioisotopes, transmutations, nuclear decal calculations , decay constants and half life, binding energy, fission and reactors, fusion,  [C1], [C6]
• Labs:  Decomposition of Hydrogen Peroxide, complex decay of 2 isotopes of Ag (Brezeale reactor/Penn State/State College)            ( 6 periods)      [C5], [C7]

 

 

• Unit 9:  Review           (1 week)

• Review of equilibrium thermodynamics, electrochemistry, stoichiometry, bonding, phases, net ionic equations.  Practice tests

 

Grading and Assessment:

• A = 93 to 100 points
• B = 83 to 92 points
• C = 73 to 82 points

• D =65 to 72 points
• F = below 65 points