Summer Assignment



Course Objective

This course is intended to give the student the most thorough and comprehensive understanding of general chemistry beyond that expected upon completion of a first year college chemistry course. In addition, the student’s problem-solving and critical thinking skills will improve tremendously, allowing you to successfully complete the AP Examination in the spring.

Class Procedure

Because of the magnitude and specificity of AP Chemistry topics, some adjustments will need to be made in order to ensure that all required materials ore covered and to guarantee that the student can receive as much individual attention as possible.

1. Because of the amount of material, the pace of the course, and time constraints, students must be willing to put in a substantial amount of individual time into the class. In most cases, this means seeking other resources, working extra problems, and doing outside investigations.

2. Time is always a great concern. While 8 - 10 class periods per week is recommended for the AP Chemistry course, we have only five 70-minute periods per week. Furthermore, laboratory techniques and questions appear in one form or another on the exam. Labs typically require 1 - 3 hours each. Also, many problems must be worked in this course in order to increase the student’s rate of success. As a result, these adjustments must be made.

a. Class time will not be spent going over homework. If you are having troubles, arrangements should be made for other time periods.

b. Students may need to complete labs outside of regular class time. This may include before or after school and during lunch.

Grading

1. Tests account for approximately 50% of the total grade.

2. Lab assignments account for approximately 35% of the total grade.

3. Homework is assigned and accounts for 15% of your grade. If you receive an “A” average for the first 9-weeks, homework is optional for the 2nd 9-weeks. This resets at the semester.

Tests

Tests are a combination of multiple choice and free-response questions. Most of the multiple-choice questions come from the chapter under study. Some questions, however, are comprehensive, as students cannot forget anything in this class! The free-response questions are either problems that students work out or written explanations of why a given chemical phenomenon occurs. In addition, tests will be graded in the format that the College Board adopts. STUDENTS CANNOT KEEP THE TESTS. Completed tests will be kept on file for review purposes only.

Text/Resources

Zumdahl, Steven, and Susan Zumdahl. Chemistry, 8e. Brooks/Cole – Cengage Learning.

Summer Assignment

|Text Reference/Resource |Topics |Assignment/Evaluations |

|Chapter 1 |Units of measurement, both SI and derived. |Summer Assignment. |

|Chemical Foundations |Significant figures and calculations. | |

| |Temperature scales. | |

| |Density. | |

| |Classification of matter. | |

|Chapter 2 |Fundamental chemical laws – conservation of mass, definite proportions and multiple proportions. |Summer Assignment. |

|Atoms, Molecules and Ions |Dalton’s atomic theory. | |

| |Early experiments of Thomson, Millikan, and Rutherford to characterize the atom. | |

| |The modern view of atomic structure, including protons, electrons, neutrons, isotopes, atomic number and mass number. | |

| |Molecules and ions; molecular vs. ionic. | |

| |An introduction to the periodic table with emphasis on classifications and properties. | |

| |Naming/formulas of simple compounds – binary ionic, polyatomic ionic, binary covalent, and acids. | |

First Quarter

|Text Reference/Resource |Topics |Assignment/Evaluations |

|The Ultimate Chemical |Symbols and nomenclature. |End of topic exercises assigned upon |

|Equations Handbook |Simple inorganic formulas and nomenclature. |completion. |

| |Oxidation numbers: anions and cations. | |

| |Ternary nomenclature: Acids and salts. |AP Format Equation Writing Test. |

| |Complex ion formulas and nomenclature. | |

| |Organic nomenclature and simple reactions. | |

| |Balancing molecular equations. | |

| |Single replacement reactions. | |

| |Double replacement reactions. | |

| |Aqueous solutions and net ionic equations. | |

| |Redox equation balancing and reactions. | |

| |Electrolysis in aqueous solutions. | |

| |Complex ion reactions. | |

|Chapters 3 and 4 |Average atomic mass. |End of chapter problems (odd numbers). |

|Stoichiometry and Types of |Molar mass and calculations. | |

|Chemical Reactions and |Percent composition of compound and mass percent problems. |AP Format Multiple Choice and Free Response |

|Solution Stoichiometry |Empirical formula, molecular formula and combustion analysis problems. |Test. |

| |Stoichiometry of chemical equations, including limiting reactants and percent yield. | |

| |Composition of solutions – molarity, ion concentration, and dilution. | |

| |Precipitation reactions – determining the mass of precipitate formed. | |

| |Acid-base neutralization and an introduction to titrations. | |

|Chapter 6 |The nature of energy – potential, kinetic, and conservation. |End of chapter problems (odd numbers). |

|Thermochemistry |State functions. | |

| |System, surroundings, and the universe. |AP Format Multiple Choice and Free Response |

| |Exothermic v. endothermic. |Test. |

| |The First Law of Thermodynamics. | |

| |Enthalpy and Calorimetry – constant pressure and constant volume calculations. | |

| |Hess’s Law. | |

| |Standard enthalpies of formation, including standard state conditions and standard heats of reaction. | |

|Chapters 8 and 9 |Types of chemical bonds, including covalent, ionic and metallic bonding. |End of chapter problems (odd numbers). |

|Bonding: General Concepts and |Bonding properties. | |

|Covalent Bonding: Orbitals |Coulomb’s Law and lattice energy. |AP Format Multiple Choice and Free Response |

| |Electronegativity, bond polarity and dipole moments. |Test. |

| |Covalent bond energies and chemical reactions – single, double and triple bond energies and enthalpy calculations. | |

| |Localized electron bonding model. | |

| |Lewis structures – octet rule, diagramming, resonance, exceptions/violations of the octet rule, and formal charges. | |

| |VSEPR – geometry, diagramming, molecular polarity, single and multiple central atoms. | |

| |Hybridization – types of hybrid orbitals, sigma and pi bonding | |

Second Quarter

|Text Reference/Resource |Topics |Assignment/Evaluations |

|Chapter 12 |Introduction to reactions rates – initial rate, instantaneous rate, and rates of appearance and disappearance. |End of chapter problems (odd numbers). |

|Chemical Kinetics |Differential rate law – the meaning of reaction orders, the method of initial rates, solving for “k” and units of “k.” | |

| |Integrated rate law for zero, first and second order reactions, including half lives and graphical interpretation |AP Format Multiple Choice and Free Response |

| |Reaction mechanisms – molecularity, elementary steps, reaction intermediates, fast/slow/reversible reactions, and |Test. |

| |determination of a proper mechanism. | |

| |Collision Theory. | |

| |Transition State Theory. | |

| |Activation energy and the Arrhenius equation. | |

| |Potential energy diagrams. | |

| |Catalysis. | |

|Chapters 13, 14, 15, and 16 |The Law of Mass Action, equilibrium expressions, and the equilibrium constant and the manipulation of “K.” |End of chapter problems (odd numbers). |

|Chemical Equilibrium, Acids and|Kc vs. Kp and conversions. | |

|Base, Acid-Base Equilibria and |Q vs. K and calculations. |AP Format Multiple Choice and Free Response |

|Solubility and Complex Ion |Solving equilibrium problems using pressures, concentrations and the 5% rule. |Test. |

|Equilibria |Le Chatelier’s Principle and the effect of changes in concentration, pressure and temperature on “K.” | |

| |The nature of acids and bases, including definitions, conjugate acid-base pairs, hydronium and hydroxide, and Ka/Kb | |

| |expressions. | |

| |Trends in acid strength. | |

| |Monoprotic and polyprotic acids; Amphoterism. | |

| |The auto-ionization of water and the ion-product constant, Kw. | |

| |Calculations of pH and pOH from hydronium and hydroxide concentrations. | |

| |Calculating the pH of strong acids and bases. | |

| |Calculating the pH of weaks acids and bases – equilibrium problems and % dissociation. | |

| |Calculating the pH of polyprotic acids solutions. | |

| |Acid-base properties of salts – neutral, acid and basic solution formation and calculations. | |

| |The effect of structure on acid-base properties, including trends in binary acid and oxyacid strengths. | |

| |Lewis acids and bases. | |

| |Calculations with solutions of acids and bases containing a common ion. | |

| |Buffered solutions – preparation, pH determination, function, the Henderson-Hasselbach equation, buffer capacity and | |

| |indicators. | |

| |Calculations of titration/pH curves for systems of a strong acid – strong base, weak acid – strong base, and weak base – | |

| |strong acid. | |

| |Solubility equilibria and solubility product constant (Ksp) calculations, including the common ion effect and selective | |

| |precipitation. | |

| |Qsp vs. Ksp and the prediction of precipitate formation and Qualitative analysis. | |

Third Quarter

|Text Reference/Resource |Topics |Assignment/Evaluations |

|Chapter 17 |Spontaneous processes and entropy. |End of chapter problems (odd numbers). |

|Spontaneity, Entropy, and Free|Positional entropy. | |

|Energy |The 2nd Law of Thermodynamics. |AP Format Multiple Choice and Free |

| |The effects of temperature on spontaneity. |Response Test. |

| |The 3rd Law of Thermodynamics. | |

| |Entropy changes in chemical reactions and calculations. | |

| |Free energy and spontaneity, including the role in chemical reactions, dependence on temperature, relationship to | |

| |equilibrium and work, and calculations. | |

|Chapter 18 |Galvanic Cells – Oxidation and reduction, half reactions and the anode/cathode, diagramming, standard cell potentials and |End of chapter problems (odd numbers). |

|Electrochemistry |the standard reduction table, and line notations. | |

| |Cell potential, electrical work, free energy and calculations. |AP Format Multiple Choice and Free |

| |Dependence of cell potential on concentration, the Nernst equations and Q vs. K. |Response Test. |

| |Electrolysis, including diagramming, electroplating, and stoichiometric calculations. | |

|Chapter 5 |Pressure – units and conversions, barometer/manometer diagramming and calculations. |End of chapter problems (odd numbers). |

|Gases |The gas laws of Boyle, Charles and Avogadro including calculations. | |

| |The ideal gas law, the universal gas constant, and the derivation of other gas laws. |AP Format Multiple Choice and Free |

| |Gas stoichiometry – chemical reaction calculations, molar mass of a gas and gas density calculations. |Response Test. |

| |Dalton’s law of partial pressures, mole fraction and water displacement. | |

| |Kinetic Molecular Theory – postulates, gas properties and the ideal gas law, the meaning of temperature, and root mean | |

| |square speed. | |

| |Effusion, diffusion and Graham’s law. | |

| |Real vs. ideal gases and the van der Waal’s equation. | |

|Chapter 10 and Chapter 11 |Intermolecular forces and bonding forces for solids, liquids and solutions, including covalent network, ionic, metallic, |End of chapter problems (odd numbers). |

|Liquids and Solids |ion-dipole, dipole-dipole, H-bonding, ion-induced dipole, dipole-induced dipole, and London dispersion forces. | |

|and Properties of Solutions |Properties of a liquid – surface tension, capillary action, and viscosity. |AP Format Multiple Choice and Free |

| |Properties of a solid – lattice structures/unit cells, ionic/molecular/metallic solids, bonding in ionic/metallic solids, |Response Test. |

| |coordination numbers/packing efficiency, and substitutional/interstitial alloys. | |

| |Vapor pressure and changes of state, including enthalpies of vaporization and fusion, phase diagrams, and heating curves. | |

| |Solubility and saturation. | |

| |Concentration – molarity, molality, mole fraction, parts by mass, and parts by volume. | |

| |Colligative properties, including Raoult’s Law and the van’t hoff factor. | |

|Chapter 7 |Electromagnetic radiation and the properties of light, including wavelength, frequency, the speed of light, reflection, |End of chapter problems (odd numbers). |

|Atomic Structure and |refraction, and diffraction. | |

|Periodicity |The nature of matter, specifically the ideas of Planck, Einstein, and de Broglie, including quantized energy, the |AP Format Multiple Choice and Free |

| |photoelectric effect, duality and matter waves. |Response Test. |

| |The atomic spectrum of hydrogen – continuous spectrum and line spectrum. | |

| |The Bohr model for hydrogen – electron energy quantization and calculations. | |

| |The quantum mechanical model, specifically the ideas of Schrodinger and Heisenberg, including quantum numbers, orbital | |

| |shapes and energies, electron spin and the Pauli exclusion principle, polyelectronic atoms, the Aufbau principle, electron| |

| |configurations and orbital diagrams. | |

| |The modern periodic table and the works of Mendeleev and Moseley. | |

| |Periodic trends – atomic radius, ionization energies, electronegativity, electron affinity, shielding effect, effective | |

| |nuclear charge, ion size, and metallic character. | |

Fourth Quarter

|Text Reference/Resource |Topics |Assignment/Evaluations |

|Chapter 21 |Nuclear stability and radioactive decay, including the band of stability and trends. |End of chapter problems (odd numbers). |

|The Nucleus: A Chemist’s View |Types of decay – alpha, beta, gamma, positron and electron capture. | |

| |The kinetics of radioactive decay, half-life and radioactive dating. |AP Format Multiple Choice and Free |

| |Thermodynamic stability of the nucleus, binding energy and mass defect. |Response Test. |

| |Fusion vs. fission. | |

| |Effects of radiation – somatic vs. genetic damage. | |

|Chapter 22 |Alkanes, including isomerism and nomenclature. |End of chapter problems (odd numbers). |

|Organic and Biological |Alkenes, alkynes and nomenclature. | |

|Molecules |Aromatic hydrocarbons. |AP Format Multiple Choice and Free |

| |Functional groups. |Response Test. |

|AP Exam Review |AP Released Multiple Choice Tests. |Student will take 4 Mock AP Tests, w/ 75 |

| |AP Released Free Response Tests. |minutes devoted to Multiple Choice, 40 |

| | |minutes to Free Response “A” and 50 |

| | |minutes to Free Response “B.” |

Labs

Students will do 25 labs throughout year. Students will be notified of the lab schedule each quarter. Students will be randomly selected into groups of 2 or 3 students. Each lab has three components that each student must submit: 1) Pre-lab, which is due before the lab, 2) Data collection and observations, which is due at the end of each lab session, and 3) Post-lab/questions, due two days after the completion of the lab. Finally, students are required to keep a formal lab notebook for all assigned labs. Students will be provided guidelines for properly formatting lab reports. As previously stated, the lab assignments account for approximately 35% of the total grade.

Resources

Hague, Jr., George R., and Smith, Jane D. The Ultimate Chemical Equations Handbook. Flinn Scientific, Inc.

Holmquist, Dan D., and Volz, Don. Chemistry with Computers, 2e. Vernier Software & Technology.

Vonderbrink, Sally Ann. Laboratory Experiment for Advanced Placement Chemistry, 1e and 2e. Flinn Scientific, Inc.

|Title |Class |Time (minutes) | |Title |Class |Time (minutes) |

| |Periods | | | |Periods | |

|Determination of the Empirical Formula of |3 |150 | |The Determination of Keq for FeSCN2+ |2 |100 |

|Silver Oxide | | | | | | |

|Gravimetric Analysis of Metal Carbonate |1 |50 | |Determination of Ka for Weak Acids |1 |50 |

|Finding the Ratio of Moles of Reactants in a |1 |50 | |Acid – Base Titrations |2 |100 |

|Chemical Reaction | | | | | | |

|Thermodynamics – Enthalpy of Reaction and |1 |50 | |Selecting Indicators for Acid-Base |2 |100 |

|Hess’s Law | | | |Titrations | | |

|Heat of Combustion of Magnesium |1 |50 | |Preparation and Properties of Buffer |1 |50 |

| | | | |Solutions | | |

|Determining the Molar Volume of a Gas |1 |50 | |Determination of the Solubility Product of |1 |50 |

| | | | |an Ionic Compound | | |

|Determination of the Molar Mass of Volatile |1 |50 | |Separation and Qualitative Determination of |5 |250 |

|Liquids | | | |Cations and Anions | | |

|Liquid Chromatography |1 |50 | |Oxidation-Reduction Titrations |2 |100 |

|Determining the Concentration of a Solution: |1 |50 | |Analysis of Commercial Bleach |1 |50 |

|Beer’s Law | | | | | | |

|Molar Mass by Freezing Point Depression |2 |100 | |Electrochemical Cells |2 |100 |

|Kinetics of Reactions |3 |150 | |Synthesis, Isolation and Purification of an |2 |100 |

| | | | |Ester | | |

|Rate Law Determination of the Crystal Violet |1 |50 | |Predicting the Products of Chemical |2 |100 |

|Reaction | | | |Reactions and Writing Chemical Equations | | |

|Equilibrium and Le Chatelier’s Principle |1 |50 | | | | |

Spring 2011 Results:

|Score |Number |

|5 |11 |

|4 |4 |

|3 |2 |

|2 |1 |

|1 |2 |

Materials:

1. Large 3-ring binder

2. TI-89 Graphing Calculator

3. Goggles

4. Lab Notebook Carbon-less, duplicate copies, 100 pages. Student Lab Notebook: 100 Top Bound or Spiral Bound duplicate pages (Paperback) by Hayden-McNeil (Author) –

Contact Information

✓ matt.young@copley-

✓ Before school – 6:30 to 7:00

✓ During school – MODS 7-8-9

✓ After school – Appointment only.

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