Unit 1 Matter and Measurement Time: covered during summer
Classification of matter, properties of matter, physical and chemical changes, separation of mixtures, units of measurement, temperature conversions, density, reasoning for significant figures, calculations involving significant figures, conversion of numbers using dimensional analysis.
Unit 2 Atoms, Molecules, and Ions Time: covered during summer
& first week of school
Discovery of atomic structure, cathode ray experiment, oil drop experiment, gold foil experiment, atomic numbers, mass numbers, atomic mass scale, average atomic mass, isotopes, charges of cations and anions, predicting formulas and names for binary ionic compounds using the periodic table, nomenclature and formulas involving polyatomic ions, nomenclature and formulas for molecular compounds, nomenclature and formulas for acids, simple organic compounds
Unit 3 Stoichiometry: Calculations w/ Chemical Formulas and Equations Time: 3 weeks
Balancing equations, synthesis and decomposition reactions, combustion reactions, calculating gram formula mass, percent composition by mass, molar mass, converting mass to moles, moles to mass, moles to number of particles, number of particles to moles, moles to volume at STP, volume at STP to moles, determining the formula of a compound from percent composition, determining the formula of an organic compound from combustion analysis, determining a molecular formula from an empirical formula, using a balanced chemical equation to determine amounts consumed or produced, identifying limiting reactants and calculating excess reactant remaining, determining theoretical and percent yield.
Unit 4 Chemical Reactions in Solution Time: 2 weeks
Dissociation of ionic compounds, ionization patterns of acids, strong and weak electrolytes, molarity of solutions, molarity of ions in solution, limiting reactant problems involving solutions, titration, dilution of a stock solution, calculation of molarity using density.
Unit 5 Writing Chemical Reactions Time: 3 weeks
Writing metathesis reactions that produce a precipitate, a gas, or a nonelectrolyte, writing chemical equations in balanced ionic form, writing single replacement reactions, writing synthesis and decomposition reactions based on pattern recognition, writing reactions that produce a soluble complex ion
Unit 6 Electronic Structure of Atoms Time: 2 weeks
The wave nature of light, quantized energy and photons, photoelectric effect, line spectra, calculating the energy of an electron in a hydrogen atom, calculating energy transitions in a hydrogen atom, the wave behavior of matter, Heisenberg’s uncertainty principle, orbitals and the four quantum numbers, representation of orbitals, orbital diagrams usingPauli’s exclusion principle, writing electron configurations using Hund’s rule, writing electron configurations for transition metals including anomalous configurations, writing electron configurations for cations and anions, identifying isoelectronic species.
Unit 7 Periodic Properties of the Elements Time 1 week
Effective nuclear charge, sizes of atoms and ions, ionization energy, electron affinity, explanation of trends based on atomic structure for radius, ionization energy, electron affinity including exceptions to the trends, properties of metals, nonmetals, metalloids
Unit 8 Chemical Bonding Time 2 weeks
Lewis diagrams for atoms and ions, Lewis diagrams for ionic and molecular compounds: including exceptions to the octet rule, lattice energy and ionic compounds, covalent bonds, polarity of molecules, electronegativity, explanation of electronegativity trends, measurement of dipole moments, calculation of formal charge, bond enthalpy, calculating enthalpy of reaction using bond energies, metallic bonds
Unit 9 Molecular Geometry Time 1.5 weeks
Valence shell electron pair repulsion theory, drawing Lewis structures, naming the electron pair geometry, naming the molecular geometry, bond angles, effect of lone pairs of electrons on bond angles, effect of molecular geometry on molecular polarity, hybridization of central atoms, sigma and pi bonds, delocalized pi bonding and resonance, bond order, molecular orbitals
Unit 10 Intermolecular Forces and Phases of Matter Time 1.5 weeks
Comparison of gases, liquids, solids on the molecular level including differences in movement and energy, molecule ion attraction, solubility of ionic compounds in water, dipole dipole attractions, hydrogen bonding, heating/cooling curves, phase diagrams, triple point, critical temperature and pressure, phase changes, energetics of phase changes, vapor pressure, boiling point, boiling point and intermolecular forces, properties of ionic, molecular, metallic, and network covalent substances, allotropes of carbon
Unit 11 Organic Chemistry Time 1 week
Series of hydrocarbons, structures and nomenclature of hydrocarbons, isomerism, reactions of saturated and unsaturated hydrocarbons, structure and properties of alcohols, ethers, aldehydes, ketones, carboxylic acids and esters, fermentation, saponification, esterification.
Unit 12 Thermochemistry Time 2 weeks
Forms of energy, units of energy, system and surroundings, comparing energy changes to enthalpy changes, endothermic and exothermic processes, enthalpies, calculating enthalpies of reactions using Hess’s law and enthalpies of formation, heat capacity, specific heat capacity, calorimetry, spontaneous processes, qualitative assessment of entropy, calculation of entropy for phase changes, predicting entropy changes in a chemical reaction, systems with perfect order, calculating free energy changes using both free energies of formation and enthalpy & entropy, predicting how free energy will be affected by temperature, calculating equilibrium constants from free energy values.
Unit 13 Gases Time 1.5 weeks
Description of pressure, measuring pressure of air and a confined gas, Boyle’s law, Charles’s law, Avogadro’s hypothesis, problem solving using the ideal gas equation, van der Waal’s equation, relating gas density to molar mass, partial pressures and mole fraction, experiments involving wet gas, kinetic molecular theory, Graham’s law of diffusion, calculating rates of effusion and diffusion.
Unit 14 Properties of Solutions Time 1.5 weeks
Energetics of solution formation, saturated solutions, solubility curves, effects of temperature and pressure on solubility, percent by mass, ppm, ppb, mole fraction, molarity, molality, converting between molality and molarity, concentration effects on: vapor pressure, boiling point, freezing point, and osmotic pressure, calculating molar mass from a colligative property.
Unit 15 Chemical Kinetics Time 2 weeks
Factors affecting the rate of a chemical reaction, change of rate with time, relating rates of appearance and disappearance based on stoichiometry, writing rate laws, determining the units of a rate constant, using initial rates to write rate laws, first order reactions, second order reactions, calculating reaction rates from experimental data, determining how concentration changes with time, activation energy, the Arrhenius equation, writing rate laws for multi step reaction mechanisms, identification of rate determining step, intermediates in a chemical reaction and catalysts, the effect of a catalyst on a reaction.
Unit 16 Equilibrium Time 3 weeks
Concept of chemical equilibrium, types of equilibria, writing equilibrium expressions for gaseous systems, writing equilibrium expressions for aqueous systems, relating Kp to Keq, qualitative analysis of K values, using the reaction quotient to predict how a reaction will shift, LeChatelier’s principle, predicting how concentrations will change in response to changes in concentration, pressure, or temperature, determining concentrations of reactants or products at equilibrium when given the equilibrium constant, determining concentrations of reactants or products when not given the equilibrium constant, solubility product constant calculations, qualitative comparison of solubility based on Ksp values, solving for concentration given a Ksp value, common ion effect, relating Ksp and the reaction quotient in order to determine the degree of solution saturation, calculating how much additional solute will dissolve in an unsaturated solution using Ksp, calculating which precipitate will form first when solutions are mixed based on Ksp values.
Unit 17 Acids and Bases Time 4 weeks
Concepts of acids and bases: Arrhenius, Bronsted - Lowry, and Lewis, predicting direction of a reaction based on strength of acid and bases, writing Lewis acid base chemical reactions, amphoterism, autoionization of water, Kw, mathematics of pH, pH scale, calculating pOH from pH, strength of acids based on percent ionization, determining pH for solutions of strong acids or bases, writing equilibrium expressions for weak acids, calculating percent ionization of a weak acid, calculating equilibrium constants for weak acids using molarity and pH, determining equilibrium constants for polyprotic acids, writing equilibrium expressions for weak bases, calculating molarity of a weak base given pH and the equilibrium constant, calculating hydroxide ion concentration given pH for weak and strong bases, hydrolysis of salts and pH, determining Kb given Ka, titration experiments, calculating pH at the equivalence point for titrations involving strong acids and strong bases, calculating pH at the equivalence point for titrations involving strong acids and weak bases, calculating the pH at the equivalence point for titrations involving weak acids and strong bases, titrations of polyprotic acids, the common ion effect and pH, composition and action of buffered solutions, calculating pH of a buffer, buffer capacity and pH range, calculating the pH of a buffered system after the addition of a strong acid or strong base, Henderson – Hasselbalch equation.
Unit 18 Electrochemistry Time 2 weeks
Identifying species oxidized or reduced in a chemical reaction, identifying oxidizing agents or reducing agents in a chemical reaction, writing half reactions for oxidation and reduction, balancing redox equations in acidic or basic solutions, components and function of voltaic cells, ion flow in a voltaic cell, comparison of reduction potentials in order to analyze oxidizing/reducing strength, calculating cell emf under standard conditions, calculating cell emf under nonstandard conditions using the Nernst equation, qualitative analysis of the effect of concentration changes on cell emf, calculating free energy changes based on cell emf, determining reaction spontaneity from cell emf, qualitative and quantitative aspects of electrolysis.
Unit 19 Nuclear Chemistry Time 1 week
Radioactivity, nuclear equations, types of radioactive decay, determining the type of decay from an equation, predicting the type of decay from the proton neutron ratio, the belt of stability, radioactive series, calculations based on half life, uses and dangers of radiation.
Assessment
Throughout each unit students, both in class and for homework, complete appropriate problems, requiring the same depth and understanding as the AP Exam. Problems and questions come from a variety of sources. Sources include: the primary text, the AP Test Prep book that accompanies the text, the test making question book that accompanies the text, questions from released AP Exams, and the textbook’s companion website. Tests are given in a multi unit format in congruence with the cumulative aspect of the AP Exam. Tests given contain multiple choice and essay/problem solving questions. Tests consistently feature a reaction writing portion to ensure preparation for the AP Exam.
Test 1 covers Units 1,2,3
Test 2 covers Units 4,5
Test 3 covers Units 6,7
Test 4 covers Units 8,9,10
Test 5 covers Units 11,12
Test 6 covers Units 13,14
Test 7 covers Units 15, 16
Test 8 covers Units 17,18,19
Laboratory Experiments:
Each lab experiment is a hands on experience involving physical skills, data collection/interpretation, collaborative effort, and problem solving techniques. Students spend a minimum of one double period per week involved in the hands on portion of the experiment, while calculations, organization and presentation of data will take additional time. Students will complete a lab write up for each experiment to include: title, purpose, materials, procedure, observations, data, calculations, graphs and charts, as well as any conclusion questions or problems. All lab write ups are to be done in a separate lab notebook that will be graded at the end of each quarter. Labs are done on small scale when appropriate to minimize the use of chemicals and materials.
Lab Schedule:
1. Significant Figures Unit 1 (2 hrs)
2. Densities of Liquids and Solids Unit 1 (2 hrs)
3. Separation of a Mixture Unit 1, 3 & 10 (2 hrs)
4. Determination of the Formula of an Ionic Unit 3 (2 hrs)
Compound
5. Volumetric Analysis of an Unknown Chloride Unit 3 & 4 (3 hrs)
6. Chemical Reactions – Synthesis, Decomposition, Unit 3, 4, 5, & 18 (3 hrs)
Double Replacement, Oxidation and Reduction
7. Activity Series of Metals Unit 5 & 18 (3 hrs)
8. Synthesis and Analysis of a Coordination Compound Unit 5 (2 hrs)
9. Atomic Spectra and Atomic Structure Unit 2 & 6 (3 hrs)
10. Valence Shell Electron Pair Repulsion Theory Unit 8 & 9 (3 hrs)
and Molecular Geometry
11. Molecular Models of Organic Compounds Unit 9 & 11(2 hrs)
12. Preparation of Aspirin and Oil of Wintergreen Unit 5 & 11 (3 hrs)
13. Enthalpy of Neutralization Unit 4, 12, & 17 (2 hrs)
14. Calorimetry of Snack Foods Unit 12 (2 hrs)
15. Molar Volume of a Gas and Determination of R Unit 3 & 13 (2 hrs)
16. Calculation of the Molar Mass of a Volatile Liquid Unit 3, 10, & 13 (2 hrs)
17. Colligative Properties: Freezing Point Depression Unit 14 (3 hrs)
and Molar Mass
18. Reaction Rates: Iodine Starch Clock Reaction Unit 4, 5, & 15 (2 hrs)
19. Properties of Systems in Chemical Equilibrium Unit 4, 16, & 17 (2hrs)
LeChatelier’s Principle
20. Determination of the Equilibrium Constant Unit 4, 5, & 16 (3 hrs)
for a Chemical Reaction using Spectrophotometry
21. Titration Curve of a Polyprotic Acid Unit 3, 4, & 17 (3 hrs)
including standardization of a basic solution
22. Voltaic Cells and The Electrolysis of Water Unit 18 (2hrs)