PREREQUISITE Completion of first year Chemistry or teacher recommendation.

Transcription

1 Advanced Placement Chemistry Lisa Graham Room 702 ext 4702 REQUIRED TEXT Chemistry the Central Science, Brown & Lemay, RECOMMENDED TEXT Cracking the AP Chemistry Exam, Princeton Review. REQUIRED MATERIALS Quadrille Bound Notebook Scientific Calculator PREREQUISITE Completion of first year Chemistry or teacher recommendation. COURSE OUTLINE The course is designed to pursue college-level studies in chemistry while still in secondary school. As such, the instruction level will assume that the student has a solid back ground in algebraic and arithmetic techniques. The course will be organized around 6 big ideas: 1. The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions. Structure of Matter 2. Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them. Properties of Matter Characteristics, States, and Forces of Attraction 3. Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons. Chemical Reactions 4. Rates of chemical reactions are determined by details of the molecular collisions. Reaction Rates 5. The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Thermodynamics 6. Any bond or intermolecular attraction that can be formed can be broken. These two processes are in a dynamic competition, sensitive to initial conditions and external perturbations. Equilibrium

2 EXPECTED STUDENT LEARNING RESULTS Students will have the opportunity to improve their skills in complex thinking and become effective communicators through reading, writing, solving mathematical problems, laboratory investigations, and oral presentations. Independent work and time management will help the student become a responsible, self-directed learner. Working with others during problem solving, laboratory investigations, peer tutoring, and global chemical issues that face society will contribute to the student becoming a more involved citizen. Understanding and following laboratory safety rules and understanding chemical toxicity encourages a healthy lifestyle. investigations will be an integral part of the course. 25% of instructional time will be devoted to hands-on laboratory work. Each student will be required to keep a bound notebook of these investigations. Each investigation will consist of a 25-minute lab preparation activity the day before each experiment and a 25-minute post laboratory analysis/conclusion activity the day after the experiment. The experimental portion of the lab is designed to utilize an entire 55-minute period. Therefore it is essential that you be prepared to begin experimental bench work the moment you walk into class. The laboratory report for each investigation will consist of purpose, chemical safety, procedure, data, data analysis, error analysis, and conclusion. Teaching Methods We will utilize the flipped classroom method for instruction. That is, each student will be responsible for accessing the lecture online before class. Note taking will be expected and evaluated for each lecture. Class time will be spent in small groups working on problems sets. Thus, concept discussions and problem solving will be emphasized. Each student will be expected to be prepared and take part in these activities. The pacing of the course will be near college atmosphere, the course coverage will be extensive and rapid. Thus, it will be necessary for each student to budget their study time accordingly in order to keep pace with the subject matter. Forming a study group and meeting once a week is highly recommended. ASSESSMENT AP Chemistry is a WEIGHTED grade subject. Thus, except for a D & F mark, all other grades are based on a 5-point scale. The course will be based on a point scale. Each test, quiz, lab, and assignment will have a point value. 99% of the overall grade will be determined by point accumulation. 1% of the final grade will be of a subjective nature. Students class participation and preparation, work quality, and academic growth will be considered in this portion of the mark. Scale: 90%=A, 80%=B, 68%=C, 58%=D. 55% of the grade is determined by tests and quizzes. 25% is laboratory. 10% is classwork. 10% is homework. There is no extra credit in this class, instead, complete all assigned work on time. No late homework (lecture notes) will be accepted. The only exception is absence, a student has one day to turn in the missed homework. In addition, any student that does not take the

3 AP Chemistry exam is required to take a 2 nd semester final exam which will count for 20% of their final grade. CITIZENSHIP In essence, any behavior that impedes the normal educational process of another student is considered unacceptable behavior. Tardiness, general disruptive behavior, lack of effort, all plays a part in this mark. Anyone who does not follow the lab safety rules, or who jeopardizes the safety of another will be recommended for expulsion from the class. ABSENCE Being absent on the day of a test, quiz, lab, or other assignments requires the student, on the first day of return, to make arrangements to complete these tasks. They are to be made up during lunch or after school. Upon making up the third test or quiz, students are no longer eligible to earn the highest mark possible on that assessment, that is, an A. COMMUNICATION I am available for tutoring most days during advisory and Wednesday after school, from 2:15-2:45. You can leave messages for me on the phone, but the most efficient way to communicate is by . Student grades are posted on the Power School website. If you do not have a username and password I highly encourage you to contact the PLHS site tech to obtain these.

4 COURSE OVERVIEW Introductory Concepts (3 weeks) Big Ideas 1 & 3 Chapters 1-3 I. Atomic Theory Symbols and Formulas I Periodic Table IV. Ionic and Covalent Bonds V. Nomenclature VI. Chemical vs. Physical Changes V Reactions and Balancing Equations VI Measurement Topics IX. Stoichiometry A. Percent Composition B. Empirical Formulas C. Mole Relationships 1. percent yield 2. limiting reagents 1. Work comfortably with the metric system. Work problems using dimensional analysis. 2. Understand and work with the correct number of significant digits. 3. Know the name and application of the common laboratory equipment. 4. Name the polyatomic ions, given the formula, and vice versa. 5. Name inorganic compounds, including acids, using the Stock system. 6. Write formulas for the names of inorganic compounds. 7. Work problems involving mole concepts, percent composition, empirical formulas, and molecular formulas. 8. Balance equations given both reactants and products. 9. Solve stoichiometric problems involving percent yield and limiting reactants. 10. Use the periodic table to identify atomic number and mass of an element. 11. Use the periodic table to identify metals, semimetals, and nonmetals. Work Density of Solids using the Synthesis of a Metal Alloy SP 2, 3, 6 Determine Mole Ratio of Reactants SP 2, 4, 5 Thin Layer Chromatograph SP 4,5

5 Chemical Reactions in Aqueous Solution (2 weeks) Big Ideas 1, 2, 3, & 6 Chapter 4 I. Molarity and dilutions I IV. Reaction types A. Acid base reactions B. Precipitation reactions C. Oxidation-reduction reactions Net ionic equations Balancing equations including redox. Activity 1. Work problems involving molarity and dilutions. 2. Distinguish between metals and nonmetals. 3. Write chemical equations, including net ionic, for synthesis,, single replacement, double replacement, redox, combustion, and acid/base reactions. 4. Apply the periodic law to chemical reactivity in predicting reaction products. 5. Discuss and use the activity series of the elements to predict single replacement reactions. 6. Apply the solubility rules to predict precipitation. 7. Use the Periodic Table to predict common oxidation states and utilize them in identifying what is being oxidized and what is being reduced. Students observe a demonstration of a series of chemical reactions and then write appropriately balanced chemical equations Guided Inquiry: What is the Relationship Between the Concentration of a Solution and the Amount of Transmitted Light Through the Solution? SP 2, 4, 5, 6 Activity Series of Elements SP 1, 4, 5 Titration of a Monoprotic Acid SP 1, 2, 5

6 The Kinetic-Molecular Theory and States of Matter (3 weeks) Big Ideas 2 & 3 Chapters 5, 10 I. Gas Laws A. Ideal Gases B. Boyle s law C. Charles law D. Gay-Lussac s law E. Dalton s law of partial pressure F. Graham s law G. Van der Waal s equation I Kinetic-Molecular Theory A. Kinetic energy of molecules B. Behavior of gases C. Deviation from ideality Liquids and Solids A. Liquids and solids from kinetic-molecular perspective B. Changes of state C. Structure of solids 1. State and discuss the major ideas of the kinetic-molecular theory. 2. Apply the kinetic-molecular theory to liquids and solids, as well as gases. 3. Discuss intermolecular forces and relate them to physical properties such as boiling point. 4. Discuss the methods and units for measuring pressure; convert between units. 5. Work problems using: Charles law, Boyle s law, Gay-Lussac s law, Avogadro s law, Dalton s law, the ideal gas law, Graham s law, and Van der Waal s equation. 6. Interpret heating curves as to melting point, boiling point and specific heat. 7. Discuss the phenomena of boiling, and are able to relate it to pressure. Molar Mass of Butane SP 2, 5 Determine Ratio of Molar Mass Using Effusion SP 2, 3, 4, 5 Determine Optimal Mole Ratio for Rocket Propulsion SP 2, 3, 4, 5, 6 Thermochemistry (3 weeks) Big Ideas 2, 3, & 5

7 Chapter 6 I. Thermal energy, heat, and temperature I IV. Calorimetry Enthalpy changes Hess law Activity 1. Learn the meaning of the following thermodynamic terms: enthalpy, delta H, exothermic, endothermic, system, surroundings, universe, heat of formation, heat of reaction, calorimetry, heat, calorie, joule, standard molar enthalpy of formation, molar heat of combustion. 2. Solve calorimetric problems involving q=(m)(c)(delta T). 3. Use Hess law to solve for heat of reaction. 4. Use stoichiometric principles to solve heat problems. Show In Pictures Students draw diagrams, no words, to describe endothermic vs. exothermic reactions including the breaking of reactant bonds and the forming of product bonds. Heat of Reaction Using Calorimetry SP 2, 4 Heating Curve of Water SP 1, 4, 5, 7 Analytical Gravimetric Determination SP 4, 5 Atomic and Nuclear Structure (3 weeks) Big Idea 1 Chapters 7, 21 I. Electronic structure A. Evidence for atomic theory B. Atomic number, mass, and mass number C. Electron energy levels: atomic spectra and atomic orbitals D. Periodic relationships Nuclear structure A. Nuclear equations B. Half-lives

8 C. Radioactivity 1. Name the major subatomic particles in an atom. 2. Discuss the Bohr model of the atom, and compare it to the quantum mechanical model of the atom. 3. Work problems involving quantum levels and energies of electron transitions. 4. Define and discuss the following terms or concepts: Heisenberg uncertainty principle, Pauli exclusion principle, wave-particle duality of matter, wave function of electrons, orbitals, aufbau principle, and Hund s rule. 5. Name the s and p orbitals. 6. Use the periodic table to identify families of elements and trends in ionization energy, electron affinity, electronegativity, and relative sizes of ions and atoms. 7. Relate the position of an element in the periodic table to its quantum electron configuration and to its reactivity with other elements in the table. 8. Balance nuclear equations. 9. List the types of radioactive emissions. 10. Compare and contrast 3 types of nuclear reactions fission, fusion, and decay. Activity Periodic Card Sort - Given a partial set of element information cards, students wil organize them into meaningful groupings and predict properties of missing cards based on location. Guided Inquiry: How Can Color Be Used to Determine the Mass Percent of Copper in Brass? SP 2, 4, 5, 6 Emission Spectra of Various Elements SP 1, 4, 5 Bonding and Molecular Structure (3 weeks) Big Idea 2 Chapters 8, 9 I. Binding forces A. ionic B. covalent C. metallic D. hydrogen bonding E. dispersion Relationships to states, structure, and properties of matter

9 I IV. Polarity of bonds and electronegativity Molecular models A. Lewis structures B. Valence bond: orbital hybridization, resonance, sigma and pi bonds V. VSEPR A. Geometry of molecules VI. V Polarity of molecules Relation of molecular structure to physical properties 1. Draw Lewis structures for the common atoms, ions, and molecules. 2. Use the periodic table to determine the number of electrons available for bonding. 3. Use periodic trends to predict bond type. 4. Distinguish between polar and nonpolar molecules. 5. Draw resonance structures. 6. Use the VSEPR model to predict molecular geometry. 7. Relate VSEPR to orbital hybridization. Activity Polar Tendencies - Students investigate the differences in behavior of various liquids with a charged lucite rod then account for those differences based on polarity of liquid molecules. Molecular Model Building / VSEPR SP 1, 7 Connecting Knowledge of Chemistry and Science With Societal and Technological Issues: Critical reading analysis of Graphene Water Filters (Reuters 3/13) which will include summary, identifying instances of fact vs. opinion, and a personal reflection. Solutions (1 1/2 weeks) Big Idea 2 Chapter 11 I. Types of solutions Factors affecting solubility

10 I Concentration measurements 1. Define solution vocabulary. 2. Discuss the effect that physical conditions have on solubility. 3. Use the concepts of intermolecular forces in discussing the dissolving process. 4. Separate compounds into electrolytes and nonelectrolytes. 5. Solve problems involving molarity and percent composition. Guided Inquiry: How Can We Determine the Actual Percentage of H2O2 in a Drugstore Bottle of Hydrogen Peroxide? SP 2, 4, 6 Separation by Distillation SP 4, 5, 7 Chemical Kinetics (2 weeks) Big Idea 4 Chapter 12 I. Rate of reaction I IV. Order of the reaction Factors that change the rate of the reaction A. Temperature B. Concentration C. Nature of substances D. Catalysts Relationship between the rate-determining step and the reaction mechanism 1. List the factors that influence the rate of a chemical reaction. 2. Use experimental data to determine the rate law, determine the order of each reactant and reaction, and to define proper units for the constant. 3. Compare and contrast zero, first, and second order reactions in terms of the plot needed to give a straight line, the relationship of the rate constant to the slope of the straight line, and the half-life of the reaction. 4. Use experimental data to postulate a reaction mechanism.

11 5. Interpret how changing the conditions of the reaction (i.e., temperature, pressure, concentration, and addition of a catalyst) affect both the rate and the rate constant of the reaction. 6. Discuss the role of a catalyst in the rate and mechanism of a reaction. Activity Given a set of manipulatives students will simulate the dissappearance of a reactant and based on the half life pattern, determine the order of that reactant. Guided Inquiry: What is the Rate Law of the Fading of Crystal Violet Using Beer s Law? SP 1, 2, 4, 5, 6 Equilibrium (2 weeks) Big Idea 6 Chapter 13 I. Concept of dynamic equilibrium Equilibrium constants and the law of mass action Activity 1. Describe the meaning of physical and chemical equilibrium, and give real life examples of each. 2. Write the law of mass action for any system at equilibrium. 3. Interpret the position of equilibrium from the size of the equilibrium constant. 4. Use Le Chatelier s principle to predict the direction a system in equilibrium will shift in order to reestablish equilibrium. 5. Know that temperature, pressure, and concentration will shift the position of equilibrium, 6. Understand that a catalyst will not have an effect on the equilibrium constant. 7. Solve problems involving the law of mass action, equilibrium concentrations and the value of the equilibrium constant. Students use data to calculate the concentration of either reactant or products or use these quantities to calculate the equilibrium constant.

12 Guided Inquiry: Can We Make the Colors of the Rainbow? An Application of Le Chatelier s Principle SP 4, 5, 6 Disturbing Equilibrium SP 4, 5, 6 Acid/Base Equilibrium (2 1/2 weeks) Big Ideas 3 & 6 Chapter 14 I. Arrhenius and Bronsted-Lowry I IV. Properties of acids and bases ph Equilibrium position and ph V. Acid base properties of salt solutions 1. Distinguish between the various modern theories of acids and bases. 2. Write balanced equations involving acids, bases, and salts. 3. Use the concept of conjugate acid-base pairs to predict reaction products. 4. Write a law of mass action for weak acid and weak base reactions at equilibrium. 5. Know and use the water constant, Kw. 6. Define ph, poh, Ka, Kb, and percent dissociation 7. Solve problems involving concentrations and ph of weak acid/base at equilibrium. 8. Recognize salts that undergo hydrolysis and write a reaction for the ion with water. Characterization of Indicators in Various ph Solutions SP 4, 5, 6 Weak Ionic Equilibrium (2 weeks) Big Idea 6 Chapter 15 I. Buffer systems Standardization of acid/base solutions

13 I Solubility product A. Factors affecting dissolution B. Molar solubility 1. Write a law of mass action for any reaction in equilibrium. 2. Solve problems involving buffering capacity. 3. Use a ph meter to determine a titration curve and ionization constant. 4. Pick a suitable indicator for a titration. 5. Determine the equivalence point(s) from a titration curve. 6. Write the solubility expression for slightly soluble compounds. 7. Solve problems involving: solubility product constants from solubility, molar solubility from Ksp, and concentrations of substances necessary to produce a precipitate. Guided Inquiry: To What Extent Do Common Household Products Have a Buffering Activity? SP 4, 5, 6 Solubility Product Constant (Ksp) for Calcium Sulfate SP 2, 4, 5 Chemical Thermodynamics (2 weeks) Big Ideas 5 & 6 Chapter 16 I. State functions I Laws of thermodynamics Relationship of change of free energy to equilibrium constants 1. List and define the meanings and common units for many thermodynamic symbols. 2. Define internal energy, PV, work, enthalpy, entropy, and free energy. 3. Determine the spontaneity of a reaction. 4. Discuss the laws of thermodynamics. 5. Understand the relationship between free energy change and equilibrium constants.

14 Qualitative Analysis to Identify 11 Unknown Solids SP 3, 4, 5, 6, 7 Electrochemistry (2 weeks) Big Idea 3 Chapter 17 I. Galvanic cells and cell potentials I Electrolytic cells Redox equations 1. Use the half-reaction method to balance redox equations. 2. Define electrochemical terms, redox, anode, cathode, anion, cation, and electrode. 3. Distinguish between an electrolytic and voltaic cell in terms of function and free energy. 4. Use a table of Standard Reduction Potentials to compute cell voltages. 5. Establish the relationship between free energy change, the cell potential, and the equilibrium constant. Electrochemical Cells SP 1, 4, 7 After AP Exam, Organic and Biochemical Issues Organic nomenclature, functional groups, structural formulas, important biochemical molecules and subunits of biochemical molecules are scattered around where I can stuff them before the AP and California State Standards exams. Synthesis of an Ester SP 4, 6, 7

15