Advanced Placement Chemistry Miss Rachel Benzoni Syllabus Mount Michael, 2011 – 2012 Text:
Brown; LeMay; Burston. (2009). Chemistry: The Central Science. 11th ed. [1] Scodellaro; Morrison. (2005). Essential Experiments for Chemistry. [2] Murov; Stedjee. (2000). Experiments and Exercises in Basic Chemistry.
Materials:
2” D-ring binder Homework notebook Laboratory notebook (with graph paper) Scientific calculator Safety goggles
Evaluation: Exams Homework Quizzes Labs
4 unit exams per semester Mastering Chemistry web application Chapter “Quests” (each chapter) 9 – 12 labs per semester + notebook
Approx % of grade 25% 25% 25% 25%
Grading Scale: Grade A+ A A-
% range 97.0 - 100 93.0 - 96.9 90.0 - 92.9
Grade B+ B B-
% range 87.0 - 89.9 83.0 - 86.9 80.0 - 82.9
Grade C+ C CD F
% range 77.0 - 79.9 73.0 - 76.9 70.0 - 72.9 60.0 - 69.9 Below 60.0
2011-2012 AP® CHEMISTRY SYLLABUS (may be subject to change)
All chapters refer to Brown, LeMay, & Bursten. Chemistry: The Central Science. 11th ed. Week Chapter & Topics Lab 1-2 Ch 1 Introduction: Matter and Measurement Lab 3B: • classification & properties of matter Elements, mixtures • units of measurement and compounds[1] • uncertainty in measurement (equipment, • dimensional analysis techniques) Ch 2 Atoms, Molecules, and Ions • evidence for the atomic theory Lab 4B: • atomic masses, determination by chemical & physical Empirical formula of means a compound[1] • atomic number and mass number, isotopes • molecular & ionic compounds • inorganic nomenclature
Week 3-4
5-6
7-8
9-10
Chapter & Topics Ch 3 Stoichiometry: Calculations with Chemical Formulas and Equations • law of conservation of mass • chemical equations, balancing • chemical reactivity and products of chemical reactions • formula weights • the mole • empirical formula • stoichiometry • limiting reactants Exam One - Ch 1, 2, & 3 Ch 4 Aqueous Reactions and Solution Stoichiometry • types of solutions • precipitation reactions • net & complete ionic equations • acid-base reactions • oxidation-reduction reactions • methods of expressing concentration • solution stoichiometry Ch 5 Thermochemistry • state functions • first law: change in enthalpy, heat of formation, heat of reaction • Hess’s law • heats of vaporization & fusion • calorimetry Ch 6 Electronic Structure of Atoms • nature of light, quantized energy • atomic spectra, Bohr model • electron energy levels • quantum numbers, atomic orbitals • electron configurations & periodic table Exam Two, Ch 4, 5, & 6 Ch 7 Periodic Properties of Elements • periodic relationships, such as atomic radii, ionization energies, electron affinities, oxidation states • horizontal, vertical, & diagonal relationships with examples from alkali metals, alkaline earth metals, halogens, & the first series of transition metals
Lab Lab 4C: Formula of a hydrate[1] Acid-Base and Redox (handout)
Making Solutions (handout) Acid-Base Titrations (handout)
Lab 6D: Limiting reactant and % yield in a precipitation reaction[1]
Lab 8B: Molar heats of reaction and Hess’s Law[1]
Week 11-12
13-14
15-16
17-18
Chapter & Topics Ch 8 Basic Concepts of Chemical Bonding • octet rule • types of bonding: ionic, covalent, etc. • polarity of bonds, electronegativity • Lewis structures • resonance • lattice energy Ch 9 Molecular Geometry and Bonding Theories • relationships to states, structure, &properties of matter • valence bond, hybridization, sigma & pi bonds • VSEPR • molecular orbitals • geometry of molecules & ions, relation to properties of structure Exam Three - Ch 7, 8, & 9 Ch 10 Gases • pressure • laws of ideal gases, equation of state of an ideal gas, partial pressures • kinetic molecular theory (KMT) • Avogadro’s hypothesis & the mole concept • kinetic energy & temperature • deviations from ideal laws Ch 11 Intermolecular Forces, Liquids, and Solids • KMT viewpoint on liquids & solids • properties of liquids • phase diagrams • change of state, including critical & triple points • structure & bonding of solids Ch 13 Properties of Solutions • the solution process • factors affecting solubility • Raoult’s law • expressing concentration • colligative properties, osmosis • colloids • nonideal behavior Exam Four - Ch 10, 11, & 13
Lab Molecular Models and Lewis Structures[2] Lewis Structures and Molecular Geometry[2]
Predicting Polarity from Molecular Shapes[2]
Molar mass of a gas OR Lab 7B: Measure the molar volume of hydrogen gas[1] Molar mass of air (handout)
Week 17-18 (cont’d)
Christmas Break
19-20
21-22 21-22 (cont’d)
23-24
25-26
Chapter & Topics Ch 14 Chemical Kinetics • concept of rate of reaction • use of experimental data & graphical analysis to determine reactant order, rate constants, & reaction rate laws • concentration & rate • effect of temperature change on rates • activation energy, catalysts • relationship between rate determining step & a mechanism Ch 25 Organic & Biochemistry • hydrocarbons & functional groups - structure, nomenclature, & chemical properties • polymers (from chapter 12) Ch 14 Kinetics, continued Ch15 Chemical Equilibrium • concept of dynamic equilibrium, chemical & physical • equilibrium constants • equilibrium constants in gaseous reactions • calculating equilibrium constants • LeChâtelier’s principle Ch15a Chemical Equilibrium, continued Exam Five - Ch 14, 15a, & 25 Ch15b Chemical Equilibrium, continued
Ch 16 Acid-Base Equilibria • Brønsted-Lowry, Arrhenius, & Lewis acids and bases • pH scale, Ka and pKa • strong acids & bases • weak acids & bases • acid-base properties of salt solutions Ch17 Additional Aspects of Aqueous Equilibria • common ion effect • buffers • acid-base titrations • solubility equilibria, Ksp • solubility product constants and precipitation • factors that affect solubility • amphoterism
Lab Purification of Vanillin using Recrystallization[2]
Melting Point Determination[2]
Lab 16B: Molar mass by freezing point depression[1] Lab 11B: The iodine clock reaction[1]
Lab 11D: Order of a reaction[1]
Week 27-28
27-28 (cont’d)
29-30
Spring Break
31-32
33-34 35-36
37-39
Chapter & Topics Ch17 Aspects of Aqueous Equilibria, continued Exam Six - Ch 15b, 16, & 17 Ch 19 Thermodynamics • spontaneous processes • second law and entropy • free energy of formation, free energy of reaction • free energy, enthalpy and entropy changes Ch 19 Thermodynamics, continued Ch 20 Electrochemistry • oxidation-reduction reactions • oxidation number • balancing redox reactions & electrons • voltaic cells, cell EMF, half cell potentials Ch 21 Nuclear Chemistry • nuclear equations • transmutation • half-lives & radioactivity • fission & fusion • chemical applications Ch 20 Electrochemistry, continued • relationship of change in free energy to electrode potentials • the Nernst equation • batteries • corrosion, & electrolysis Ch 21 Nuclear Chemistry, continued Ch 21 Nuclear Chemistry, Continued Exam Prep & Practice Exams AP Exam Exam Seven, Ch 19, 20 & 21 Ch 12 Modern Materials • liquid crystals • biomaterials • ceramics • superconductivity • thin films Final Exam - Comprehensive
Lab LeChatelier’s Principle (handout) Lab 12C: Determination of a solubility product constant[1] Lab 13D: Hydrolysis[1]
Titration Curves of Weak Acids and Bases (handout)
Lab 14C: Redox Titrations with Permanganate[1]
General Policies: I. Homework Class homework is assigned through the Mastering Chemistry web application. Reasonable progress on each chapter’s assignment is a daily requirement. You are expected to work together on the more challenging problems and keep examples in a homework journal. II. Exams There will be a “Quest” given at the end of each chapter. The Quest will consist of group and individual sections. Exams will be administered following the completion of each unit and will cover 2-3 chapters. You are expected to take the AP Chemistry exam in May. III. Labs Labs are performed during the double period every Thursday for the 36 weeks of the school year, from 10:25 AM to 11:30 AM, for a total of 51 hours of instructional time. You are required to maintain a lab notebook. The objectives, procedures, materials, and any safety information must be recorded prior to the lab period. If needed for quantitative exercises, a data table must also be ready before the lab period. Following the completion of the lab, calculations, error analysis, and conclusions will be added to the lab report. An electronic copy of your lab report for each lab must be posted on the class PBWorks site (http://rbenzoni.pbworks.com/) in a timely fashion for review and comments. You are expected to help your classmates edit their reports by providing constructive feedback on their lab reports. IV. Make-up work In the instance when a student must be absent from the regularly scheduled class meeting due to an excused absence, classroom activities must be made up in advance of the student’s absence. In the case of illness or other unplanned absences, the student will have the number of school days equal to the number of school days missed to complete and turn in all missed work. Makeup work is the responsibility of the student. V. Late papers Late work will be penalized 50% the first day it is late. Any work handed in later than one school day will receive no credit. VI. General behavior Strict adherence to the behavior policies as listed in the Mount Michael Student/Parent Handbook is required at all times in the class. Deviation from the behavior policies will be addressed in the strictest manner allowable by the administrative policies of Mount Michael. Any student expelled from the classroom or laboratory due to his behavior will receive a zero for the class activity. VII. Academic integrity/honesty Students are expected to follow the honesty policies as outlined in the Mount Michael Student/Parent Handbook. Any behavior contrary to the policy will result in the loss of credit for the activity. Further, a report to the Principal will be made detailing the academic dishonesty. Additional Credit: Participation in academic competitions and working as a tutor for Chemistry 1 students are examples of available extra credit options. Reasonable suggestions for additional credit may be considered at the instructor’s discretion.
Brown; LeMay; Burston. (2009). Chemistry: The Central Science. 11th ed. [1] Scodellaro; Morrison. (2005). Essential Experiments for Chemistry. [2] Murov; Stedjee. (2000). Experiments and Exercises in Basic Chemistry.
Materials:
2” D-ring binder Homework notebook Laboratory notebook (with graph paper) Scientific calculator Safety goggles
Evaluation: Exams Homework Quizzes Labs
4 unit exams per semester Mastering Chemistry web application Chapter “Quests” (each chapter) 9 – 12 labs per semester + notebook
Approx % of grade 25% 25% 25% 25%
Grading Scale: Grade A+ A A-
% range 97.0 - 100 93.0 - 96.9 90.0 - 92.9
Grade B+ B B-
% range 87.0 - 89.9 83.0 - 86.9 80.0 - 82.9
Grade C+ C CD F
% range 77.0 - 79.9 73.0 - 76.9 70.0 - 72.9 60.0 - 69.9 Below 60.0
2011-2012 AP® CHEMISTRY SYLLABUS (may be subject to change)
All chapters refer to Brown, LeMay, & Bursten. Chemistry: The Central Science. 11th ed. Week Chapter & Topics Lab 1-2 Ch 1 Introduction: Matter and Measurement Lab 3B: • classification & properties of matter Elements, mixtures • units of measurement and compounds[1] • uncertainty in measurement (equipment, • dimensional analysis techniques) Ch 2 Atoms, Molecules, and Ions • evidence for the atomic theory Lab 4B: • atomic masses, determination by chemical & physical Empirical formula of means a compound[1] • atomic number and mass number, isotopes • molecular & ionic compounds • inorganic nomenclature
Week 3-4
5-6
7-8
9-10
Chapter & Topics Ch 3 Stoichiometry: Calculations with Chemical Formulas and Equations • law of conservation of mass • chemical equations, balancing • chemical reactivity and products of chemical reactions • formula weights • the mole • empirical formula • stoichiometry • limiting reactants Exam One - Ch 1, 2, & 3 Ch 4 Aqueous Reactions and Solution Stoichiometry • types of solutions • precipitation reactions • net & complete ionic equations • acid-base reactions • oxidation-reduction reactions • methods of expressing concentration • solution stoichiometry Ch 5 Thermochemistry • state functions • first law: change in enthalpy, heat of formation, heat of reaction • Hess’s law • heats of vaporization & fusion • calorimetry Ch 6 Electronic Structure of Atoms • nature of light, quantized energy • atomic spectra, Bohr model • electron energy levels • quantum numbers, atomic orbitals • electron configurations & periodic table Exam Two, Ch 4, 5, & 6 Ch 7 Periodic Properties of Elements • periodic relationships, such as atomic radii, ionization energies, electron affinities, oxidation states • horizontal, vertical, & diagonal relationships with examples from alkali metals, alkaline earth metals, halogens, & the first series of transition metals
Lab Lab 4C: Formula of a hydrate[1] Acid-Base and Redox (handout)
Making Solutions (handout) Acid-Base Titrations (handout)
Lab 6D: Limiting reactant and % yield in a precipitation reaction[1]
Lab 8B: Molar heats of reaction and Hess’s Law[1]
Week 11-12
13-14
15-16
17-18
Chapter & Topics Ch 8 Basic Concepts of Chemical Bonding • octet rule • types of bonding: ionic, covalent, etc. • polarity of bonds, electronegativity • Lewis structures • resonance • lattice energy Ch 9 Molecular Geometry and Bonding Theories • relationships to states, structure, &properties of matter • valence bond, hybridization, sigma & pi bonds • VSEPR • molecular orbitals • geometry of molecules & ions, relation to properties of structure Exam Three - Ch 7, 8, & 9 Ch 10 Gases • pressure • laws of ideal gases, equation of state of an ideal gas, partial pressures • kinetic molecular theory (KMT) • Avogadro’s hypothesis & the mole concept • kinetic energy & temperature • deviations from ideal laws Ch 11 Intermolecular Forces, Liquids, and Solids • KMT viewpoint on liquids & solids • properties of liquids • phase diagrams • change of state, including critical & triple points • structure & bonding of solids Ch 13 Properties of Solutions • the solution process • factors affecting solubility • Raoult’s law • expressing concentration • colligative properties, osmosis • colloids • nonideal behavior Exam Four - Ch 10, 11, & 13
Lab Molecular Models and Lewis Structures[2] Lewis Structures and Molecular Geometry[2]
Predicting Polarity from Molecular Shapes[2]
Molar mass of a gas OR Lab 7B: Measure the molar volume of hydrogen gas[1] Molar mass of air (handout)
Week 17-18 (cont’d)
Christmas Break
19-20
21-22 21-22 (cont’d)
23-24
25-26
Chapter & Topics Ch 14 Chemical Kinetics • concept of rate of reaction • use of experimental data & graphical analysis to determine reactant order, rate constants, & reaction rate laws • concentration & rate • effect of temperature change on rates • activation energy, catalysts • relationship between rate determining step & a mechanism Ch 25 Organic & Biochemistry • hydrocarbons & functional groups - structure, nomenclature, & chemical properties • polymers (from chapter 12) Ch 14 Kinetics, continued Ch15 Chemical Equilibrium • concept of dynamic equilibrium, chemical & physical • equilibrium constants • equilibrium constants in gaseous reactions • calculating equilibrium constants • LeChâtelier’s principle Ch15a Chemical Equilibrium, continued Exam Five - Ch 14, 15a, & 25 Ch15b Chemical Equilibrium, continued
Ch 16 Acid-Base Equilibria • Brønsted-Lowry, Arrhenius, & Lewis acids and bases • pH scale, Ka and pKa • strong acids & bases • weak acids & bases • acid-base properties of salt solutions Ch17 Additional Aspects of Aqueous Equilibria • common ion effect • buffers • acid-base titrations • solubility equilibria, Ksp • solubility product constants and precipitation • factors that affect solubility • amphoterism
Lab Purification of Vanillin using Recrystallization[2]
Melting Point Determination[2]
Lab 16B: Molar mass by freezing point depression[1] Lab 11B: The iodine clock reaction[1]
Lab 11D: Order of a reaction[1]
Week 27-28
27-28 (cont’d)
29-30
Spring Break
31-32
33-34 35-36
37-39
Chapter & Topics Ch17 Aspects of Aqueous Equilibria, continued Exam Six - Ch 15b, 16, & 17 Ch 19 Thermodynamics • spontaneous processes • second law and entropy • free energy of formation, free energy of reaction • free energy, enthalpy and entropy changes Ch 19 Thermodynamics, continued Ch 20 Electrochemistry • oxidation-reduction reactions • oxidation number • balancing redox reactions & electrons • voltaic cells, cell EMF, half cell potentials Ch 21 Nuclear Chemistry • nuclear equations • transmutation • half-lives & radioactivity • fission & fusion • chemical applications Ch 20 Electrochemistry, continued • relationship of change in free energy to electrode potentials • the Nernst equation • batteries • corrosion, & electrolysis Ch 21 Nuclear Chemistry, continued Ch 21 Nuclear Chemistry, Continued Exam Prep & Practice Exams AP Exam Exam Seven, Ch 19, 20 & 21 Ch 12 Modern Materials • liquid crystals • biomaterials • ceramics • superconductivity • thin films Final Exam - Comprehensive
Lab LeChatelier’s Principle (handout) Lab 12C: Determination of a solubility product constant[1] Lab 13D: Hydrolysis[1]
Titration Curves of Weak Acids and Bases (handout)
Lab 14C: Redox Titrations with Permanganate[1]
General Policies: I. Homework Class homework is assigned through the Mastering Chemistry web application. Reasonable progress on each chapter’s assignment is a daily requirement. You are expected to work together on the more challenging problems and keep examples in a homework journal. II. Exams There will be a “Quest” given at the end of each chapter. The Quest will consist of group and individual sections. Exams will be administered following the completion of each unit and will cover 2-3 chapters. You are expected to take the AP Chemistry exam in May. III. Labs Labs are performed during the double period every Thursday for the 36 weeks of the school year, from 10:25 AM to 11:30 AM, for a total of 51 hours of instructional time. You are required to maintain a lab notebook. The objectives, procedures, materials, and any safety information must be recorded prior to the lab period. If needed for quantitative exercises, a data table must also be ready before the lab period. Following the completion of the lab, calculations, error analysis, and conclusions will be added to the lab report. An electronic copy of your lab report for each lab must be posted on the class PBWorks site (http://rbenzoni.pbworks.com/) in a timely fashion for review and comments. You are expected to help your classmates edit their reports by providing constructive feedback on their lab reports. IV. Make-up work In the instance when a student must be absent from the regularly scheduled class meeting due to an excused absence, classroom activities must be made up in advance of the student’s absence. In the case of illness or other unplanned absences, the student will have the number of school days equal to the number of school days missed to complete and turn in all missed work. Makeup work is the responsibility of the student. V. Late papers Late work will be penalized 50% the first day it is late. Any work handed in later than one school day will receive no credit. VI. General behavior Strict adherence to the behavior policies as listed in the Mount Michael Student/Parent Handbook is required at all times in the class. Deviation from the behavior policies will be addressed in the strictest manner allowable by the administrative policies of Mount Michael. Any student expelled from the classroom or laboratory due to his behavior will receive a zero for the class activity. VII. Academic integrity/honesty Students are expected to follow the honesty policies as outlined in the Mount Michael Student/Parent Handbook. Any behavior contrary to the policy will result in the loss of credit for the activity. Further, a report to the Principal will be made detailing the academic dishonesty. Additional Credit: Participation in academic competitions and working as a tutor for Chemistry 1 students are examples of available extra credit options. Reasonable suggestions for additional credit may be considered at the instructor’s discretion.
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