Course Syllabus

AP Chemistry

Marvin Ridge High School

 

Course Description

The AP Chemistry course is designed to be the equivalent of a two semester introductory college chemistry course.  Spanning both semesters, the course meets daily for a 90 minute period.  Instruction consists mostly of laboratory, lecture, discussions, demonstrations, and written assignments which may include research projects, in-class assignments, homework, and online activities. Laboratory will require students to observe proper safety precautions and turn in a written lab report.

 

Course Materials

Required Materials: 3-ring binder (one inch), paper, pen, pencil, scientific calculator

 (Because chemistry professors at some institutions ask to see a record of the laboratory work done by an AP student before making a decision about granting credit or placement in the chemistry program, students should keep a laboratory portfolio that includes reports of their laboratory work in such a fashion that the reports can be readily reviewed. Organize your notebook accordingly!) The textbook is Chemistry: AP Edition Chemistry  9^th edition by Zumdahl and Zumdahl, published by Brooks Cole, Cengage Learning.  Students are encouraged to purchase a Student Study Guide to prepare for course exams and an AP review book to help them study for the exam. The teacher prepares in-depth analyses of homework questions that students may use to review homework.

 

Instructional Philosophy

Students taking AP Chemistry can expect an engaging, hands-on learning experience.  Assessments will be designed to apply the rigors which students will experience during the taking of the AP Examination, so that students will be prepared with the content and test-taking skills required to reach their full potential during that examination. Students enrolled in the course are juniors and seniors who have successfully taken honors chemistry and are enrolled in upper level, honors math courses.  Students are expected to be self-motivated with the time and dedication to devote to a rigorous course.  Students should have good note-taking and study habits.  The course is a year-long class and students are required to take both semesters and sit for the AP exam in order to earn AP credit. 

 

Course Standards

Every AP Course is Required to Include These Topics

 

1. Structure of Matter (20%)
2. Atomic theory and atomic structure
3. Evidence for the atomic theory
4. Atomic masses; determination by chemical and physical means
5. Atomic number and mass number; isotopes
6. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
7. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
8. Chemical bonding
9. Binding forces
10. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
11. Relationships to states, structure, and properties of matter
12. Electronegativity differences, polarity of bonds, molecular symmetry, and polarity of molecules.
13. Molecular models
14. Lewis structures
15. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
16. VSEPR
17. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination

 complexes; dipole moments of molecules; relation of properties to structure

1. Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical applications

 

1. States of Matter (20%)
2. Gases
3. Laws of ideal gases
4. Equation of state for an ideal gas
5. Partial pressures
6. Kinetic molecular theory
7. Interpretation of ideal gas laws on the basis of this theory
8. Avogadro’s hypothesis and the mole concept
9. Dependence of kinetic energy of molecules on temperature
10. Deviations from ideal gas laws
11. Liquids and solids
12. Liquids and solids from the kinetic-molecular viewpoint
13. Phase diagrams of one-component systems
14. Changes of state, including critical points and triple points
15. Structure of solids; lattice energies
16. Solutions
17. Types of solutions and factors affecting solubility
18. Methods of expressing concentration (use of normalities is not tested)
19. Raoult’s law and colligative properties (nonvolatile solutes); osmosis
20. Nonideal behavior (qualitative aspects)

 

III. Reactions (35–40%)

1. Reaction types
2. Acid-base reactions; concepts of Arrhenius, Bronsted-Lowry and Lewis; coordination complexes; amphoterism
3. Precipitation reactions
4. Oxidation-reduction reactions
5. Oxidation number
6. The role of the electron in oxidation-reduction
7. Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst

equation; prediction of the direction of redox reactions

1. Stoichiometry
2. Ionic and molecular species present in chemical systems: net ionic equations
3. Balancing of equations, including those for redox reactions
4. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
5. Equilibrium
6. Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle; equilibrium constants
7. Quantitative treatment
8. Equilibrium constants for gaseous reactions: Kp, Kc
9. Equilibrium constants for reactions in solution

  (1) Constants for acids and bases; pK; pH

  (2) Solubility product constants; their application to precipitation; dissolution of slightly soluble compounds

  (3) Common ion effect; buffers; hydrolysis

1. Kinetics
2. Concept of rate of reaction
3. Use of experimental data and graphical analysis to determine reactant order, rate constants and reaction rate laws
4. Effect of temperature change on rates
5. Energy of activation; the role of catalysts
6. The relationship between the rate-determining step and a mechanism
7. Thermodynamics
8. State functions
9. First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law; heats of vaporization/fusion; calorimetry
10. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on

enthalpy and entropy changes

4. Relationship of change in free energy to equilibrium constants and electrode potentials

 

1. Descriptive Chemistry (10–15%)

Knowledge of specific facts of chemistry is essential for an understanding of principles and concepts. These descriptive facts, including the chemistry involved in environmental and societal issues, should not be isolated from the principles being studied but should be taught throughout the course to illustrate and illuminate the principles. The following areas should be covered:

1. Chemical reactivity and products of chemical reactions
2. Relationships in the periodic table: horizontal, vertical and diagonal with examples from alkali metals, alkaline earth

metals, halogens, and the first series of transition elements

3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)

 

1. Laboratory (5–10%)

The differences between college chemistry and the usual secondary school chemistry course are especially evident in the laboratory work. The AP Chemistry Exam includes some questions based on experiences and skills students acquire in the laboratory:

• making observations of chemical reactions and substances
• recording data
• calculating and interpreting results based on the quantitative data obtained
• communicating effectively the results of experimental work

 

The student will do the following laboratories during the year. (Proposed)

.               1. Density of Liquids and Solids (includes determination of %Deviation and % Error)            [inquiry]                    (2 days)

2. Analytic Separation of Inks Using Paper Chromatography
3. Analytic Separation of Solid Materials (Using Magnetism, Filtration, and Recrystallization) (2 days)
4. Spectrometry of Selected Gases and Metals
5. Identifying Types of Reactions (Excess Reactants, Activation Energies and Reaction Drives)
6. Determination of an Empirical Formula for Copper Sulfide
7. Determination of a Hydrate Formula for Copper Sulfate [inquiry]
8. Molecular Structure Simulation Using VSEPR and Balloons [inquiry] (2 days)
9. Determination of the Specific Heat of Copper
10. Determination of R Using Magnesium and Hydrochloric Acid [inquiry]
11. Thermochemistry [inquiry]
12. Beer Lambert Law
13. Reaction Kinetics
14. Equilibrium Constant
15. Le Chatelier’s Principle
16. Titration of Hydrochloric Acid with Sodium Hydroxide
17. Standardizing a Titrant
18. Titration of Vinegar with NaOH [inquiry]
19. Titration of a Diprotic Acid
20. Synthesis of Aspirin [inquiry]
21. Qualitative Analysis                                 (2 days)
22. Coordination Compounds and Color
23. Constructing a Galvanic Cell
24. Half-Life Simulation

                (These 24 labs require 28 days of lab. The class meets 90 minutes every day, so this constitutes 42 hours of lab.)

               

Major Course Projects and Assignments

The following is a summary of all units that will be taught during the year.

 

Fundamentals of Chemistry

Topics:  Lab Safety, How to read an MSDS, Scientific Method, Math Review, Units of Measurement, Uncertainty in Measurement, Significant Figures & Calculations, Dimensional Analysis, Temperature, Density, How to Write a Lab Report

 

The Atom

Topics:  Atomic History, Parts of the Atom, Ions and Isotopes, Molecules, and Ions, Nomenclature

 

Stoichiometry

Topics: Atomic Masses, The Mole, Molar Mass, Mole Calculations (Avogadro’s Number), Percent Composition, Empirical/Molecular Formulas, Equations, Stoichiometry

 

 

Types of Chemical Reactions and Solution Stoichiometry

Topics:  Solvation, Electrolytes, Reaction Types, Precipitation Reactions, Stoichiometry of PPT Rxns,Acids-Bases, ReDox Rxns

 

Gases

Topics:  Ideal/Combined Gas Laws, Gas Stoichiometry, Daltons Law, Kinetic Molecular Theory, Effusion/Diffusion, Real Gases

 

 

Thermochemistry

Topics:  Units of Energy, Endothermic/Exothermic, Enthalpy, Calorimetry, Hess’s Law, Enthalpy of Formation

 

Atomic Structure, Periodicity, and Bonding

Topics:  Bohr Model, QM Model, Orbitals, Periodic Table and Trends, Types of Bonds, Electronegativity, Lewis Structures, Polarity, Resonance, VSEPR shapes, Hybrid and Molecular Orbitals, Bond Order, Photoelectron Spectroscopy

 

Liquids and Solids

Topics:  IMFs, Liquids, Metals, Molecular and Ionic Solids, Vapor Pressure, Changes of State, Phase Diagrams

 

Properties of Solutions

Topics:  Energy and Solvation, Factors Affecting Solubility and Rate of Formation, Colligative Properties, Colloids

 

Unit 7:  Gases and Kinetic Molecular Theory (Chapter 5)

Topics:  Gas Laws, Dalton’s Law, Gas Density, Real/Ideal Gases, KMT, Ideal Gas Law, Effusion/Diffusion and Gas Stoichiometry

 

Reaction Spontaneity

Topics:  Units of Energy, Enthalpy, Calorimetry, Hess’s Law, Enthalpy of Formation, Reaction Spontaneity, Entropy, Gibbs Free Energy

 

Kinetics and Equilibrium

Topics:  Factors Affecting Reaction Rates, Rate Law Problems, Reaction Order, Reaction Mechanisms, Catalysts, Concept of Equilibrium, Equilibrium Constant; How to Solve Problems with Kc, Kp, Heterogeneous Equilibria, LeChatelier’s Principle

 

Acids and Bases and Their Equilibria

Topics:  Acid/Base Definitions, Strength,  pH Calculations for Stronf/Weak, Polyprotics, Solving Acid-Base Equilibria, Acidic-Basic Salts and Oxides, Effect of Molecular Structure on Acidity, Common Ion Effect, Buffers, Titrations,

 

Solubility and Complex Ion Equilibria

Topics:  Solubility Product Constant, Precipitation, Qualitative Analysis, Complex Ions

 

Spontaneity, Entropy, and Free Energy

Topics:  Entropy, Gibb’s Free Energy, Temperature Effects, Pressure Effects, Work

 

Electrochemistry

Topics:  Oxidation/Reduction, Galvanic Cells and SRPs, Work and Free Energy, Concentration Effects, Batteries, Corrosion, Electrolysis

 

Nuclear Chemistry

Topics:  Stability and Decay, Kinetics, Half-Life

 

Transition Metals and Coordination Chemistry

Topics: Transition Metals, The First Row, Coordination Compounds, Bonding in Complex Ions, Crustal Field Model

 

Organic and Biological Chemistry

Topics:  Alhanes, Alkenes-Alkynes, Aromatics, Derivatives, Polymers, Optical Rotation, Natural Polymers

 

 

Assessment and Grading Plan

 

Your AP Chemistry grade will be based on the following: tests; projects, quizzes and labs; and classwork and homework. 

Tests = 50%                            Quizzes/Labs/Projects = 30%                  Homework/Classwork = 20%

 

Make-up work and. Late work:          Make-up work is available to students as per county policy. 

Students have two days for each day absent to make up work.

Late work will earn less credit. (30% penalty - 1 day, 60% penalty - 2 days, After 2 days the penalty will be at the teacher’s discretion. Please talk to me about extenuating circumstances!)