Successful completion of either Pre AP Chemistry or both Integrated Science I and II, and Algebra I.

Transcription

1 AP CHEMISTRY SYLLABUS PREREQUISITES: Successful completion of either Pre AP Chemistry or both Integrated Science I and II, and Algebra I. TEXT: Chemistry, Principles and Reactions, 5 th ed., Thomson/Brooks/Cole, ISBN: (Reference) Chemistry by Zumdahl and Zumdahl, 6 th ed., Houghton Mifflin Co., ISBN: GOALS: Students will improve their analytical reading and problem solving skills. Students will be able to safely and efficiently conduct laboratory experiments using appropriate lab apparatus/materials in order to make meaningful observations, collect and isolate meaningful data, analyze that data over a broad topic range to verify or reject hypotheses, as well as to be able to report findings formally and informally. Students will be aware of the interconnection of chemistry to all the other sciences. Students will earn an acceptable score on the AP Chemistry test in

2 May. LABORATORY NOTEBOOK: The laboratory notebook is mandatory and should be brought to class the day before and the day of the laboratory experiment. The laboratory notebook will be graded at the end of each quarter. COURSE NOTEBOOK: The course notebook is mandatory and must be brought to class daily. Students will be required to take notes for every chapter using the Dual Entry Journal format (as demonstrated by the instructor) before the lesson is discussed in class. The course notebook will serve as a review source for chapter, quarter and semester exams. The notebook will be graded each quarter HOMEWORK: Homework will be due on the day of each quiz and test day. Homework will be designed as practice for the quizzes and tests. Late homework will not be accepted under any circumstances.

3 COURSE CONTENT SEMESTER I Matter and Measurement 4 days significant figures, metric conversion, dimensional analysis set up, uncertainty in measurement Atoms, Molecules, and Ions 4 days Development of atomic theory, atomic structure, effective use of the periodic chart, electron configuration, writing formulas (molecular and ionic) Stoichiometry 7 days atomic mass determination from relative abundances of isotopes and molar

4 masses from formulas, mole relationships, mass relations in chemical formulas mass %, balancing equations, using balanced equations to predict yield, limiting reactants, % yield Reactions in Aqueous Solutions 6 days precipitation reactions based on rules of solubility, introduction of acid/base reactions, REDOX reactions, writing of balanced molecular and NET ionic equations, as well as equations for more sophisticated REDOX reactions, molarity, molality, normality, solution stoichiometry (heavy emphasis on limiting reactant problems) Gases 6 days Kelvin temperature, STP, units of pressure, gas laws (Charles, Boyles, Gay Lussac s, mixed, ideal, Grahams Law of Effusion, average speed, calculations involving all laws, stoichiometry of gaseous reactions, molar mass and density calculations as versions of ideal gas law, mole fractions, Dalton s law of partial pressures, calculations involving collection of gases by water displacement (water vapor pressure effect), kinetic theory of gases, calculations to determine average speed as function of molar mass, derivation of time and distance effusion laws from rate law, conditions for deviation from ideal gas law. Electron Configuration and Use of the Periodic Chart 7 days light, photons, and atomic spectra, dual nature of light, E=hv=hc/wavelength, Bohr s model using hydrogen, spectrum analyses, use of both Rydberg and Bohr constants in calculations of E, excited vs. ground state, electron configuration, Heisenberg Uncertainty Principle, Hund s Rule, Pauli Exclusion Principle (spin), Aufbau Principle, use of the periodic chart to predict expected electron configuration as opposed to diagonal rule, electron configurations of monatomic ions, quantum numbers, and periodic trends for the comparison of atomic radii, ionic radii, electronegativity, and ionization energy

5 Covalent Bonding and Molecular Geometry 7 days increased stability with electron pairing, valence electrons, Lewis structures, types of covalent bonds, octet rule, S=N A, resonance, octet rule and exceptions, expanded octets, VSEPR modeling, prediction of geometry of molecules and the reasons this is important, effect of unshared electron pairs and numbers of bonded atoms on a central atom on molecular geometry, bond polarity, atomic orbitals and hybridization, sigma and pi bonds, molecular orbital theory and calculation of bond order Thermochemistry 6 days principles of heat flow (system vs. surroundings), enthalpy defined, significance of the sign on answers to heat flow calculations, magnitude of heat flow, joule/kilojoules/calories as units of heat energy, q=ms(deltat), coffee cup and bomb calorimetry principles and calculations, writing appropriate thermochemical equations, stoichiometric calculations, application of First Law of Thermodynamics, applications of theories to gases. SEMESTER II Liquids and Solids 6 days molecular compounds and general characteristics, intermolecular forces (dispersion forces, dipole forces, hydrogen gbonding (N, O, F), network covalent, ionic, and metallic solids examples and characteristics of, calculations involving simple unit cells, liquid vapor equilibrium, vapor pressure defined and the influence of temperature on vapor pressure (Clausius Clapeyron), boiling, melting, and freezing points, critical temperature and pressure defined, interpretation of and construction of phase diagrams Solutions 5 days molarity, mole fraction, mass %, molality, mole fraction, ppm, molarity

6 molality conversions, solubility, temperature effects on solubility of gases, colligative properties defined, non electrolytes vs electrolytes, effect of solutes on f. pt. and b. pt., Van t Hoff factor, effect of solutes on vapor pressure, osmotic pressure, calculation of molar mass from colligative properties Reaction Rate 6 days definition, measuring rate, effect of concentrations of reactants on rate, rate expressions and rate constant, order of reaction defined, calculation of reaction order when two rates are known with only a single reactant, order of reaction with more than one reactant, reactant concentration and time, half life calculations, zero and second order reactions, models for reaction rate, reaction rate and temperature, Arrhenius equation, catalysis, reaction mechanisms and rate determining steps, deduction of rate expression from a proposed mechanism. Gaseous Equilibrium 9 days defining equilibrium, N 2 O 4 NO 2 equilibrium system, equilibrium constant expression, reciprocal rule, rule of multiple equilibria, k as a function of partial pressures or molarity, applications of the equilibrium constant to determine trends in the equilibrium sysytem, comparison of Q and K c, effect of changes on the equilibrium system, Le Chatelier Principle, relationship of K p and K c. Acid/Base Chemistry 5 days various definitions of acids/bases, conjugate acids/bases, amphoteric/amphiprotic defined, dissociation of water molecules into ions, K w, ph and poh, relationship of ph and poh to K w, strong/weak acids and bases, K a and K b used to determine molar concentrations in aquatic solutions, polyprotic acids and their subsequent K a s, acid/base properties of salt solution, neutralization reactions of acids and bases (again), calculations from titration data, indicators, choosing appropriate indicators, buffers and buffer systems, calculations of [H+] and [OH ] in buffer systems,

7 worrying a buffer system (calculations of ph and poh after addition of certain compounds, breaking a buffer system Precipitation Equilibria 6 days equilibria in precipitation reactions, K sp and solubility in water, common ion effect on solution equilibria, dissolving of precipitates using acids or bases (strong acid anion to react with basic anions or complexing agent such as NH 3 or OH to react with metal cations). Spontaneity of Reaction 5 days definition of spontaneous reactions, entropy, entropy changes and computations, free energy, Gibb s free energy, effects of temperature, pressure and concentration on reaction spontaneity, coupled reactions Electrochemistry 6 days voltaic cells, zinc/copper connection, anode/cathode reactions, function of salt bridge, identification of parts of the voltaic cell, identification of oxidation/reduction reactions, cell notation, cell voltage related to spontaneity, standard voltage, standard voltage for overall reactions, determination of spontaneity in a reaction, stand free energy changes Nuclear Chemistry 3 days half life, alpha and beta decay, gamma radiation Organic Chemistry 2 days general characteristics, alkanes, alkenes, alkynes, basic functional groups (halogens, alcohols, ketones, aldehydes, ethers, esters, carboxyl groups, amines, amides), benzene, basic naming of organic compounds

8 LABORATORY TOPICS (2hr 50 minute/lab) SEMESTER I #1 Introduction/Safety #2 Physicsl Properties #3 % Barium chloride dihydrate #4 Boyle s Law and Gases #5Determination of Emperical Formula #6 Chemical Reactions #7 Molar Volume of Oxygen and Weight of Mg

9 #8 Electrolytes #9 Evaporation #10 Formula Weight of a Volatile Liquid and Formula from Freezing Point Depression Data #11 Acid/Base Titration #12 Redox Titration #13 Calorimetric Determination of Iron SEMESTER II #14 Qualitative Analysis Chloride Group #15 Qualitative Analysis Basic Sulfide Group #16 Qualitative Analysis Soluble Group #17 Qualitative Analysis Unknown #18 Qualitative Analysis Unknown #19 Calorimetry #20 Kinetics of a Chromium EDTA Comples #21 Iodine Clock #22 Acid/Base Titration

10 #23 Electrolytic Cells #24 Organic Functional Groups