Samples of Evidence to Satisfy the AP Chemistry Curricular Requirements

Transcription

1 Samples of Evidence to Satisfy the AP Chemistry Curricular What s here? This table presents samples of evidence that address the curricular requirements for AP Chemistry. For each curricular requirement, there are three separate samples of evidence provided. Each sample either fully or partially satisfies its requirement. The samples are taken from three distinct sample syllabi published in their entirety elsewhere on AP Central. The far-left column of the table presents each of the curricular requirements. In some cases, complex requirements have been broken down into their component parts. The columns to the right present the three evidence samples. How can I use this information? Use these samples to become familiar with both the nature of evidence and the variety of formats in which evidence can be presented. For any one curricular requirement, the ways in which evidence is both described and presented can vary considerably from course to course. No single format is preferred over any other. Narrative text, tables, bulleted lists, and other formats that clearly convey the content of your course are all acceptable. The most important consideration is that your syllabus (the evidence) clearly and explicitly satisfies the curricular requirements in their entirety. Curricular Description, the first of which is Structure of Matter (Atomic theory and atomic structure, Chemical bonding) Atomic and nuclear structure (Chapters 7 and 21) (3 weeks) I. Electronic Structure A. Evidence for the atomic theory B. Atomic masses C. Atomic number and mass number D. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals E. Periodic relationships II. Nuclear structure A. Nuclear equations B. Half-lives C. Radioactivity D. Chemical application Bonding and Molecular Structure (Chapters 8 and 9) (3 weeks) I. Binding forces A. ionic, B. covalent C. metallic D. hydrogen bonding E. van der Waals II. Relationships to states, structure, and properties of matter III. Polarity of bonds, Electronegativities IV. Molecular models A. Lewis structures B. Valence bond: Hybridization of orbitals, resonance, sigma and pi bonds. V. VSEPR A. Geometry of molecules and ions B. Structural, geometric, optical, and conformational isomerism of: 1. Organic molecules 2. Coordination complexes VI. Polarity of molecules VII. Relation of molecular structure to physical properties. Electronic structure and configuration History of atomic theory Types of bonding Intramolecular and intermolecular forces Molecular geometry Nuclear chemistry Unit 6: Atomic Structure Atomic spectra, Bohr atom, quantum numbers, atomic orbitals, electron configurations, s Flame test for metals using spectroscopes. Also, show discharge tubes and how they relate to wave length. Mention bright line spectra and have students use diffraction gratings to view spectra. Unit 7: Chemical Bonding Lewis structures, ionic bonding, character of bonds, covalent model, octet rule and exceptions, resonance, VSEPR model, and hybridization. VSEPR model building using styrofoam balls and pipe cleaners. Students must first make five geometries and be able to distinguish between electron and molecular geometry.

2 Description, the second of which is States of Matter (Gases, Liquids and solids, Solutions) The Kinetic-Molecular Theory and States of Matter (Chapters 5, 10) (2 weeks) I. Gas Laws A. Ideal gases B. Boyle s law C. Charles law D. Dalton s law of partial pressure E. Graham s law F. Henry s law G. Van der Wail s equation of state II. Kinetic-Molecular theory A. Avogadro s hypothesis and the mole concept B. Kinetic energy of molecules C. Deviations from ideality III. Liquids and solids A. Liquids and solids from the K-M viewpoint. B. Phase diagrams of one-component systems. C. Changes of state. D. Structure of solids including lattice energies Unit 4: Gases Ideal gas law, van der Waal's equation, Avogadro's Law, STP, Dalton's Law, Graham's Law, kinetic theory of gases, etc. Molecular mass of a volatile liquid (Masterton) Unit 8: Liquids and Solids Dipole-dipole interactions, hydrogen bonding, London forces, liquid state, types of solids, metallic bonding, network solids, vapor pressure, change of state, phase diagrams, and specific heat Unit 9: Properties of Solutions Electrolytes and nonelectrolytes, molarity, molality, mole fraction, colligative properties, Raoult's Law, Henry's law, freezing point depression, boiling point elevation, and osmotic pressure Date Chapter 10/2-10/ The Gaseous State 11/29-12/6 9 - Liquids & Solids 12/7-12/ Solutions Solutions and Colloids (Chapter 11) (2 ½ weeks) I. Types of solutions II. Factors affecting solubility III. Concentration issues IV. Raoult s Law and colligative properties V. Non-ideality Molecular mass determination by freezing point depression (Masterton) Description, the third of which is Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics) Types of Chemical Reactions and Solution Stoichiometry (Chapter 4) (2 weeks) I. Reaction types A. Acid base reactions 1. Arrhenius 2. Lowry-Brønsted 3. Lewis B. Precipitation reactions C. Oxidation reduction reactions 1. Oxidation number 2. Electron transport 3. Electrochemistry II. Stoichiometry III. Net ionic equations IV. Balancing equations (including redox) V. Mass-volume relationships with emphasis on the mole. Date Chapter 1/23-2/ Gaseous Chemical Equilibrium 2/5-2/ Acids and Bases 2/13-2/ Equilibria in Acid Base Solution 3/9-3/ Precipitation Equilibria Unit 10: Chemical Thermodynamics Gibbs free energy equation, laws of thermodynamics, enthalpy, entropy, free energy, energy and work, exothermic and endothermic reactions, and state functions Unit 11: Chemical Kinetics Reaction kinetics, rate law expressions, order of reactions, rate constant, half-life, activation energy, catalysts, and reaction mechanisms Kinetics of thiosulfate decomposition (Ehrenkranz) NOTE: Each of the evidence samples above provides an example of a different part of the Reactions portion of the curricular requirements as described in the AP Chemistry Course Description. Sample 1 is for reaction types and stoichiometry, Sample 2 is for equilibrium, and Sample 3 is for kinetics and thermodynamics. Therefore, each sample only partially satisfies the Requirement. Evidence for all five parts must appear in the syllabus to completely satisfy this Curricular Requirement.

3 Description, the fourth of which is Descriptive Chemistry (including relationships in the periodic table) The student will 1. Apply the periodic law to chemical reactivity in predicting reaction products. 2. Discuss the activity series of the elements. 3. Distinguish between metals and nonmetals. 7. Use the Periodic Table to predict common oxidation states. 8. Use the Activity series of elements to predict single replacement reactions. Organic chemistry is covered using a self-paced computer program. One unit is due in each of the first three quarters. Unit 6: Atomic Structure and Periodicity periodic table, trends in the periodic table in terms of physical and chemical properties. Organic chemistry nomenclature, functional groups, simple reactions. The Periodic Law and periodicity of properties Activity Series and redox potential tables Organic compounds nomenclature and properties Description, the fifth of which is Laboratory (Physical manipulations; Processes and procedures; Observations and data manipulation; Communication, Group collaboration, and the laboratory report) In each laboratory experiment, students will: physically manipulate equipment and materials in order to make relevant observations and collect data; use the collected data to form conclusions and verify hypotheses; communicate and compare their results and procedures (informally to other experimenters, and also in a formal, written report to the teacher). All of the experiments below, except where noted with *, will require hands-on work in the laboratory. In collaboration with other students, you will be called upon to collect, process, and manipulate data taken from physical observations, both measured and unmeasured, and then to develop and formally report your conclusions. Students are required to submit a complete report for each lab experiment, including an hypothesis, procedure, observations/data, calculations, and a conclusion. All reports are kept in a lab notebook. Very often students are called upon to make a presentation to the class about their hypotheses, calculations, and conclusions in a similar manner to the questions/problems-solving method described above. In this way, students are able to collaborate on the objectives and design of an experiment, to assist each other in reaching conclusions, and to gain insights into variance and sources of error.

4 The course emphasizes chemical calculations and the mathematical formulation of principles. The student will: Work comfortably with the metric system Work problems using dimensional analysis. Work problems involving calories and specific heat. Work problems involving mole concepts, molarity, percent composition, empirical formulas, and molecular formulas. Solve stoichiometric problems involving percent yield, and limiting reagents. Apply these concepts to the laboratory setting. Work problems using: Charles' law, Boyle's law, Gay- Lussac's Law, Avogadro's Law, Dalton's Law. Maxwell- Boltzmann Distribution Law, the Ideal Gas Law, and van der Waal's equation. Exposure to the kinds of questions and problems with the same depth and breadth as those on the AP Exam itself enhances and cements student learning. Students need plenty of opportunities to learn how to approach multiple-choice questions. Teach them that quantitative multiple-choice questions fall into one of these categories: 1. All answers are significantly different 2. All answers are given as different mathematical manipulations of the given 3. Some answers are close and actual calculation is necessary 4. Some answers are close but rounded values are easily manipulated to yield an answer -and reviewing all the answers before actual calculation is an effective way to select the best one. Completing multiple-choice questions without a calculator is an arduous task for students and must be practiced. Prepared materials, such as Demmin's review text or AP Released Exams, are helpful in the preparation of chapter tests, review sheets, and other assessment tools. AP Released Exams are an invaluable source for free-response questions. Use them freely in quizzes, as homework problems, on chapter exams, or for final reviews. Give timed practice AP Exams and review them as a class. Complete calculations of the mass % of CO2 Rf values for each of the FD & C dyes in both the standards and the candy Determine the Cp of an unknown substance and calculate its molar mass by using the Law of Dulong and Petit. Each student receives 6 to 10 old AP Exam questions/problems on the current chapter and is expected to complete them in two or three days. (The problems often do not contain all the parts of the original exam question; for example, I only assign those parts that pertain to the chapter we are covering.) In addition, each student is responsible for presenting two of the questions/problems on the over head projector for the entire class. Many students receive the same question, but they do not know who will be asked to do the presentation. Students receive points based on the quality of their presentation. I post the detailed solution to each problem in the classroom so they can examine beforehand the problems they do not understand. Unit I: Calculations and Uncertainty Dimensional analysis, uncertainty, significant figures empirical formulas, percent composition, percent yield, and solution stoichiometry molarity, molality, mole fraction, colligative properties, Raoult's Law, Henry's law, freezing point depression, boiling point elevation, and osmotic pressure Laws of mass action, equilibrium expressions, calculations of K and equilibrium concentrations. NOTE: The emphasis on calculations and mathematical formulation will require evidence throughout the syllabus.

5 The course includes a laboratory component comparable to collegelevel chemistry laboratories. A minimum of one double-period per week or its equivalent is spent engaged in laboratory work. A hands-on laboratory component is required. Each student should complete a lab notebook or portfolio of lab reports. Note: Online course providers utilizing virtual labs (simulations rather than hands-on) should submit their laboratory materials for the audit. If these lab materials are determined to develop the skills and learning objectives of hands-on labs, then courses which use these labs may receive authorization to use the "AP" designation. The AP Chemistry class meets for 45 minutes two days each week and for 95 minutes three days each week. A minimum of 45 minutes per day outside of class is expected. Each week, at least one of the 95-minute periods will be devoted to laboratory work. Students keep a formal laboratory notebook. This notebook is graded with each lab. Laboratory work counts 30% of the total class grade. Your laboratory notebook is design to organize your GRADED lab reports. It should not be brought to class daily, but will be graded at the end of each quarter. THIS NOTEBOOK IS MANDATORY! each experiment averages 2-3 laboratory periods per week. Our school offers two sections of AP Chemistry, which meet five days a week for 55 minutes, averaging about two periods per week for laboratories Students are required to submit a complete report for each lab experiment, including an hypothesis, procedure, observations/data, calculations, and a conclusion. All reports are kept in a lab notebook. NOTE: A listing of all lab activities should be included, with a short description of each, and also with evidence that the total lab time is a minimum of a double period or its equivalent per week.