Charlotte High School Advanced Placement Chemistry 2012-2013 Instructor: Mr. Mario D. Iorfida Room: G217 Email: Mario_Iorfida@ccps.k12.fl.us Phone: 575-5450, ext 1724 Web Site: www.apcscience.com Course Description: Advanced Placement (AP) Chemistry is designed to be the equivalent of a first year college general chemistry course. Students who enroll in AP Chemistry display a high level of competency in honors chemistry and a strong desire to pursue a major in the sciences as a college student. AP Chemistry is different from Chemistry Honors in that it goes more in depth with some topics as well as covers topics that were not addressed in the honors class. In order to be successful, the student should demonstrate a high level of commitment, motivation, and academic maturity. All students enrolled in AP Chemistry are expected to take the AP exam administered by the College Board in May. Textbook/Lab Manual: Brown, Theodore L., et al., Chemistry - The Central Science Tenth Edition. Upper Saddle River, NJ: Pearson Prentice Hall, 2006. Brown, Theodore L., et al., Chemistry - The Central Science Tenth Edition. Upper Saddle River, NJ: Pearson Prentice Hall, 2012. Vonderbrink, Sally Ann, Laboratory Experiments for Advanced Placement Chemistry Second Edition. Batavia, IL: Flinn Scientific, Inc., 2006. Student Supplies: - Three ring-binder - used for objective sheets, PowerPoint notes, lecture notes, completed exams/quizzes and other class materials. - Composition notebook this serves as a laboratory journal. - Graphing calculator TI-83 or later is recommended. - Review guide for AP Chemistry (Princeton Review, Barron s etc.) - is helpful if used along with the class. It is not very useful if it is not opened until a week before the exam. Goals of the Course: - Students are prepared to be critical and independent thinkers. - Students are able to analyze issues using scientific problem solving. - Students will be able to obtain a passing score on the AP Chemistry examination. - Students will be able to physically manipulate equipment and materials in order to make relevant observations and collect data; use the collected data to form conclusions and verify
hypotheses; and communicate and compare results both informally with others and as part of the written laboratory journal for the instructor. Expectations: It is expected that students will attend class faithfully, be punctual, courteous and display behavior that is expected of students in such a high level course. When a class is missed, it is the responsibility of the student to catch up on all material missed. Students will have a maximum of three days to resolve any missing assignments. Students are expected to print assignment sheets, PowerPoint notes, laboratory sheets, and any supporting material for the topics being covered during class. These materials are found on the apcscience website. Students will be asked to be in early for laboratory work. This is not optional but a specific requirement of this course. You will be allowed to be late to lab only once, any more than this and it may affect your lab grade for the course. Electronic devices may be used with instructor permission and for educational purposes only. Students using devices for non-educational purposes will have their privileges revoked. Assessments and Grades: Grade Scale: A: 90 100 B: 80 89 C: 70 79 D: 60 69 F: < 60 The student grade in this course will be based on total points earned in the following areas: Exams: Exams are administered by topic. Each exam will be comprehensive meaning that material will be seen over and over on a regular basis. Quizzes: Quizzes occur often to ensure understanding. Quizzes can be announced and unannounced. Laboratory work: Experimentation and lab reports written in the student lab journal. Homework Problems: Problems are assigned to enhance comprehension throughout the duration of the course. Midterm Exam: Midterm exam will cover all topics covered to that point, but is by no means an endpoint since all material will be seen as part of the AP examination. Other Considerations: - Students are expected to take an active role in their pursuit of knowledge. Students should read the material being discussed in class. This will help in the overall understanding of a topic, and it also helps build general chemical knowledge around the fundamentals taught in class. - If a student intends to use their AP Chemistry score for college credit it is up to the individual to research the college of their choice to see what their policy is. Policies differ widely form school to school so it is important to check. - This course is not designed to prepare students for any other examination (SAT subject test etc) other than the AP Chemistry exam.
- Students should be prepared to invest time outside of class to be successful. The College Board s recommendation is at least 5 hours a week outside of class instruction time. - Most students in AP Chemistry find that the course is challenging, even difficult at times. With a lot of hard work and persistence, most students find the benefits of the course to be very rewarding both now and in their future studies. Advanced Placement Chemistry Topic Outline Introductory, Review Concepts, and Organic Chemistry (Chapters 1-2, 6-9 and 25) I. Matter and Measurement A. The Study of Chemistry 1. Atomic and Molecular Perspective of Chemistry B. Classification of Matter 1. States of Matter 2. Pure Substances 3. Elements, Compounds, and Mixtures C. Properties of Matter 1. Physical and Chemical Changes 2. Separation of Mixtures D. Units of Measurement 1. SI Units 2. Length and Mass 3. Temperature 4. Derived SI Units 5. Volume and Density E. Uncertainty in Measurement 1. Precision and Accuracy 2. Significant Figures and Significant Figures in Calculations F. Dimensional Analysis 1. Using Two or More Conversion Factors 2. Conversions Involving Volume II. Atoms, Molecules, and Ions A. Atomic Theory B. Discovery of Atomic Structure 1. Cathode Rays and Electrons 2. Radioactivity 3. Nuclear Atom C. Modern View of Atomic Structure 1. Atomic Number, Mass Number, and Isotopes D. Atomic Weights 1. Atomic Mass Scale 2. Average Atomic Masses E. The Periodic Table F. Molecules and Molecular Compounds
III. IV. 1. Molecules and Chemical Formulas 2. Molecular and Empirical Formulas G. Ions and ionic Compounds 1. Predicting Ionic Charges 2. Ionic Compounds H. Naming Inorganic Compounds 1. Names and Formulas of Ionic Compounds 2. Names and Formulas of Acids 3. Names and Formulas of Molecular Compounds I. Simple Organic Compounds 1. Alkanes 2. Derivatives of Alkanes Electronic Structure of Atoms A. The Wave Nature of Light B. Energy and Photons 1. Photoelectric Effect C. Line Spectra and the Bohr Model 1. Limitations of Bohr s Model D. The Wave Behavior of Matter 1. The Uncertainty Principle E. Quantum Mechanics and Atomic Orbitals 1. Orbitals and Quantum Numbers F. Representations of Orbitals 1. s-orbitals 2. p-orbitals 3. d and f orbitals G. Electron Configurations 1. Hund s Rule 2. Pauli Exclusion Principle Periodic Properties of the Elements A. Effective Nuclear Charge B. Sizes of Atoms and Ions 1. Periodic Trends C. Ionization Energy 1. Periodic Trends 2. Electron Configurations of Ions D. Electron Affinities E. Group Trends 1. Alkali and Alkaline Earth Metals 2. Halogens and Noble Gases V. Chemical Bonding and Molecular Geometry A. Chemical Bonds 1. Lewis Symbols 2. Octet Rule B. Ionic Bonding 1. Energetics of Bond Formation
VI. 2. Polyatomic ions C. Covalent Bonding 1. Lewis Structures D. Bond Polarity and Electronegativity 1. Dipole Moments E. Resonance Structures F. Strength of Covalent Bonds 1. Bond Enthalpies, Enthalpy of Reaction and Bond Length G. VSEPR Model 1. Effect of Lone Pairs 2. Molecules with Expanded Valence Shells H. Molecular Shape and Polarity I. Covalent Bonding and Orbital Overlap J. Hybrid Orbitals 1. sp, sp 2, sp 3 Hybrid Orbitals 2. Hybridization involving d-orbitals K. Molecular Orbitals Organic Chemistry A. General Characteristics B. Naming and Structures of Alkanes, Alkenes, and Alkynes C. Functional Groups Laboratories: Analysis of Silver in an Alloy Analysis of Alum Stoichiometry, Aqueous Reactions and Solution Stoichiometry (Chapters 3 and 4) I. Stoichiometry: Calculations with Chemical Formulas and Equations A. Chemical Equations 1. Balancing 2. Indicating States B. Patterns of Chemical Reactivity Types of Reactions C. Avogadro s Number and the Mole D. Empirical Formulas 1. Molecular Formula from Empirical Formula 2. Combustion Analysis E. Limiting Reactants 1. Theoretical Yields II. Aqueous Reactions and Solution Stoichiometry A. General Properties of Aqueous Solutions 1. Electrolytic Properties 2. Ionic Compounds in Water 3. Molecular Compounds in Water 4. Strong and Weak Electrolytes B. Precipitation Reactions
1. Solubility Guidelines 2. Exchange Reactions 3. Ionic Equations C. Acid-Base Reactions 1. Acids and Bases Strong and Weak 2. Identifying Strong and Weak Electrolytes 3. Neutralization and Salts 4. Acid-Base Reactions with Gas Formation D. Oxidation-Reduction Reactions 1. Oxidation and Reduction 2. Oxidation Numbers 3. Oxidation of Metals by Acids and Salts 4. The Activity Series E. Concentrations of Solutions 1. Molarity 2. Expressing the Concentration of an Electrolyte 3. Interconverting Molarity, Moles, and Volume 4. Dilution F. Solutions Stoichiometry and Chemical Analysis 1. Titrations Laboratories: Determination of the Empirical Formula of Silver Oxide Finding the Ratio of Moles of Reactants in a Chemical Reaction Predicting Products of Chemical Reactions and Writing Chemical equations Redox Titrations (Handout Flinn Prepared AP Labs) Electrochemistry (Chapter 20) I. Oxidation and Balancing Redox Reactions A. Oxidation States B. Balancing Redox Equations 1. Half Reactions 2. Acidic/Basic solution II. Voltaic/Galvanic Cell A. Voltaic Cells B. Cell EMF 1. Standard Reduction Potentials 2. Strengths of Oxidizing and Reducing Agents C. Free Energy and Redox III. Batteries and Fuel Cells A. Lead acid Battery B. Alkaline Battery C. Nickel-Cadmium Battery D. Lithium-ion Battery E. Corrosion F. Electrolysis
Laboratories: An Activity Series Electrochemical cells Thermochemistry and Chemical Thermodynamics (Chapters 5 and 19) I. Thermochemistry A. Nature of Energy 1. Kinetic and Potential Energy 2. Units of Energy 3. System and Surroundings 4. Work and Heat B. First Law of Thermodynamics 1. Internal Energy 2. Relating ΔE to Heat and Work 3. Endothermic and Exothermic Processes 4. State Functions C. Enthalpy II. D. Enthalpies of Reactions E. Calorimetry 1. Heat Capacity and Specific Heat 2. Constant-Pressure Calorimetry 3. Constant-Volume (Bomb) Calorimetry F. Hess s Law G. Enthalpy of Formation 1. Using Enthalpies of Formation to Calculate Enthalpies of Reaction Chemical Thermodynamics A. Spontaneous Processes 1. Reversible and Irreversible Processes B. Entropy and the Second Law of Thermodynamics 1. Entropy Change 2. ΔS for Phase Changes C. Molecular Interpretation of Entropy 1. Molecular Motions and Energy 2. Boltzmann s Equation and Microstates 3. The Third Law of Thermodynamics D. Entropy Changes in Chemical Reactions E. Gibb s Free Energy 1. Free Energy and Temperature Laboratories: Enthalpy and Hess s Law Gases, Intermolecular Forces, Liquids, Solids (Chapters 10 and 11) I. Gases
II. III. IV. A. Characteristics of Gases B. Pressure 1. Atmospheric Pressure and the Barometer C. The Gas Laws 1. Boyle s Law 2. Charles s Law 3. Avogadro s Law D. The Ideal-Gas Equation 1. Relating Ideal-Gas Equation and the Gas Laws E. Further Applications of the Ideal-Gas Equation 1. Gas Densities and Molar Mass 2. Volume of Gases in Chemical Reactions F. Gas Mixtures and Partial Pressures 1. Partial Pressure and Mole Fractions 2. Collecting Gases over Water G. Kinetic-Molecular Theory 1. Application to the Gas Laws H. Molecular Effusion and Diffusion 1. Graham s Law of Effusion 2. Diffusion and Mean Free Path I. Real Gases: Deviations from Ideal Behavior 1. The van der Waals Equation Intermolecular Forces A. A Molecular Comparison of Gases, Liquids, and Solids B. Intermolecular Forces 1. Ion-Dipole Forces 2. Dipole-Dipole Forces 3. London Dispersion Forces 4. Hydrogen Bonding 5. Comparing Intermolecular Forces Liquids A. Properties of Liquids 1. Viscosity 2. Surface Tension B. Phase Changes 1. Energy Changes 2. Heating Curves 3. Critical Temperature and Pressure C. Vapor Pressure 1. Vapor Pressure on the Molecular Level 2. Volatility, Vapor Pressure, and Temperature 3. Vapor Pressure and Boiling Point D. Phase Diagrams 1. Phase Diagrams of H 2 O and CO 2 Solids A. Structures of Solids
1. Unit Cells 2. Crystal Structure 3. Close Packing of Spheres B. Bonding in Solids 1. Molecular Solids 2. Covalent-Network Solids 3. Ionic Solids 4. Metallic Solids Laboratories: Determining Molar Volume of a Gas Determination of the Molar Mass of Volatile Liquids Liquid Chromatography Properties of Solutions (Chapter 13) I. Solutions A. The Solution Process 1. Energy Changes and Solution Formation 2. Solution Formation, Spontaneity, and Disorder 3. Solution Formation and Chemical Reactions B. Saturated Solutions and Solubility II. Solubility of Solutions A. Factors Affecting Solubility 1. Solute-Solvent Interactions 2. Pressure Effects 3. Temperature Effects B. Ways of Expressing Concentration 1. Mass Percentage, ppm, and ppb 2. Mole Fraction, Molarity, and Molality 3. Conversion of Concentration Units III. Colligative Properties A. Colligative Properties 1. Lowering the Vapor Pressure 2. Boiling Point Elevation 3. Freezing Point Depression 4. Osmosis 5. Determination of Molar Mass IV. Colloids A. Hydrophilic and Hydrophobic Colloids B. Removal of Colloidal Particles Laboratories: Molar Mass by Freezing Point Depression Chemical Kinetics (Chapter 14) I. Reaction Rates and Method of Initial Rates
II. III. A. Factors that Affect Reaction Rates B. Reaction Rates 1. Change of Rate with Time 2. Reaction Rates and Stoichiometry C. Concentration and Rate 1. Exponents in the Rate Law 2. Units of Rate Constants 3. Using Initial Rates to Determine rate Laws Integrated Rate Law A. The Change of Concentration with Time 1. First Order Reactions 2. Second Order Reactions 3. Half life B. Temperature and Rate 1. The Collision Model 2. The Orientation Factor 3. Activation Energy 4. The Arrhenius Equation 5. Determining Activation Energy Reaction Mechanisms A. Types of Reaction Mechanisms 1. Elementary Reactions 2. Multistep Mechanisms 3. Rate Laws for Elementary Reactions 4. The Rate-Determining Step for a Multistep Mechanism 5. Mechanisms with a Slow Initial Step 6. Mechanisms with a Fast Initial Step B. Catalysis 1. Homogenous Catalysis 2. Heterogeneous Catalysis 3. Enzymes Laboratories: Kinetics of a Reaction Chemical Equilibrium (Chapter 15) I. The Concept of Equilibrium A. The Equilibrium Constant 1. Equilibrium Constants in Term of Pressure Kp 2. Equilibrium Constants and Units B. Interpreting and Working with Equilibrium Constants 1. The Magnitude of Equilibrium Constants 2. The Direction of Chemical equilibrium and K 3. Relating Chemical Equations and Equilibrium Constants C. Heterogeneous Equilibrium D. Calculating Equilibrium Constants
II. E. Applications of Equilibrium Constants 1. Predicting the Direction of Reaction 2. Calculating Equilibrium Concentrations LeChâtelier s Principle A. Change in Reactant or Product Concentration B. Effects of Volume and Pressure Changes C. The Effect of Catalysts Laboratories: Equilibrium and LeChatelier s Principle The Determination of K eq for FeSCN 2+ Acid-Base Equilibria and Additional Aspects of Aqueous Equilibria (Chapters 16 and 17) I. Acids and Bases A. Acids and Bases: A Brief Review B. Brønsted-Lowry Acids and Bases 1. H + Ion in Water 2. Proton-Transfer Reactions 3. Conjugate Acid-Base Pairs 4. Relative Strength of Acids and Bases C. The Autoionization of Water 1. The Ion Product of Water D. The ph Scale 1. Other p Scales 2. Measuring ph E. Strong Acids and Bases F. Weak Acids 1. Calculating K a from ph 2. Using K a to calculate ph 3. Polyprotic acids G. Weak Bases H. Relationship between K a and K b I. Acid-Base Properties of Salt Solutions 1. An Anion s Ability to React with Water 2. A Cation s Ability to React with Water 3. Combined Effect of Cation and Anion in Solution J. Acid-Base Behavior and Chemical Structure 1. Factors that Affect Acid Strength 2. Binary Acids 3. Oxyacids 4. Carboxylic Acids K. Lewis Acids and Bases 1. Hydrolysis of Metal Ions II. Aqueous Equilbria A. The Common-Ion Effect B. Buffered Solutions
1. Composition and Action of Buffered Solutions 2. Calculating ph of a Buffer 3. Buffer Capacity and ph Range 4. Addition of Strong Acids of Bases to Buffers C. Acid-Base Titrations 1. Strong Acid-Strong Base Titrations 2. Weak Acid-Strong Base Titrations 3. Titrations of Polyprotic Acids D. Solubility Equilibria 1. The Solubility Product Constant, Ksp 2. Solubility and Ksp E. Factors that Affect Solubility 1. Common-Ion Effect 2. Solubility and ph 3. Formation of Complex Ions 4. Amphoterism F. Precipitation and the Separation of Ions 1. Selective Precipitation of Ions G. Qualitative Analysis of Ions Laboratories: Determination of K a of Weak Acids Acid-Base Titrations Selecting Indicators for Acid-Base Titrations Analysis of Commercial Bleach Notes on Laboratory Work The differences between college chemistry and the usual secondary school chemistry course are especially evident in the laboratory work. The AP Chemistry Examination 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; and communicating effectively the results of experimental work. Colleges have reported that some AP candidates, while doing well on the examination, have been at a serious disadvantage because of inadequate laboratory experience. Meaningful laboratory work is important in fulfilling the requirements of a college-level course of a laboratory science and in preparing a student for sophomore-level chemistry courses in college. 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, placement, or both, in the chemistry program, students should keep reports of their laboratory work that can be readily reviewed. To address this point, students will be required to keep a laboratory notebook as a record of all experiments and their analysis done in class.