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AP CHEMISTRY 2011/2012 COURSE EXPECTATIONS/OBJECTIVES Classroom Requirements: 2 inch three-ring binder for this class only 1 ½ inch three-ring Laboratory binder/portfolio Loose leaf paper Pencil and pen Graphing Calculator Box of lab gloves Provided by School/Required for Class: Zumdahl “Chemistry” Textbook Zumdahl Study Guide Zumdahl Experimental Chemistry Attendance/Tardies Attendance and tardies will be dealt with per the LNHS Student Handbook. Homework: Homework assignments must be clearly identified by page number, assigned questions, and date. Answers must be outlined with a box, excluding theory questions. Test Corrections/Re-Test: Re-tests are available on all chapter tests within 5 days of receiving a test grade. An average of the two grades will be recorded. Students will not be able to re-test unless all homework assignments, labs, and study guide questions have been completed. Students only receive 1 re-test per semester. Please choose wisely. Labs/Experiments Students are expected to abide by all laboratory safety regulations. Safety glasses, gloves, and aprons will be required for most lab experiments (provided by the school). For every day that an assigned lab report is late, the student will lose 10 percent. If a student is missing more than one lab each quarter, they will receive an “incomplete” until this deficiency is rectified. Once graded labs are returned, late labs will have a 50 percent reduction in points. Laboratory Notebook (Binder) A laboratory notebook is required to organize students’ graded lab reports. It should not be brought to class daily, but will be checked and graded at the end of each quarter. THIS NOTEBOOK IS MANDATORY PER COLLEGE BOARD!!!! Missed Notes, Homework, Assignments, Labs: Students are responsible for missed notes, homework, and assignments due to absence. This make-up work must be completed within (5) school days. Any exemptions will be dealt with by Administration. School Rules: Students are also required to abide by LNHS rules, including but not limited to: 1. No electronic devices (I-pods, cell-phones, pagers, etc….) 2. No profanity On-line Assignments: Students will be assigned on-line homework through the Quest program provided by the University of Texas. The student’s link to Quest is: https://quest.cns.utexas.edu/student. Information is also located on Ms. Carroll’s website: http://iss.schoolwires.com/1683204495640550/site/default.asp Course Evaluation: Semester One Reporting Period No. 1 Reporting Period No. 2 Mid-term AP Chemistry Exam Semester Two Reporting Period No. 3 Reporting Period No. 4 37.5 % 37.5 % 25 % 50 % Total 50 % 50 % 50 % Total Reporting Period Grade Evaluation: Labs/Lab Notebook Homework assignments Online Assignments Chapter Tests Quizzes Contact Information: E-mail Address: [email protected] Website: http://iss.schoolwires.com//Domain/2854 Phone Number: 704-799-9555, Extension 411 20 % 12 % 12 % 43 % 13 % AP Chemistry – Course Syllabus Class Profile: AP Chemistry is a year-long, 90 minute course. A typical week is organized to provide: 3-4 days of lecture focused on the key objectives listed in the syllabus, including teacher demonstrations 1-2 days of lab activity. Labs may exceed one 90 minute class, depending on the requirements of the specific lab activity. In addition, some sections/objectives are more conducive to lab activity than others and will have more lab activity. AP Chemistry Objectives: The AP Chemistry course is designed to be the equivalent of the general chemistry usually taken during the first college year. For some students, this course enables them to undertake, as freshmen, second-year work in chemistry sequence at their institution or to register in courses in other fields where general chemistry is a pre-requisite. For other students, the AP Chemistry course fulfills the laboratory science requirement and frees time for other courses. AP Chemistry should meet the objectives of a good general chemistry course. Students in such a course should attain a depth of understanding of fundamentals and a reasonable competence in dealing with chemical problems. The course should contribute to the development of the student’s abilities to think clearly and to express their ideas, orally and in writing, with clarity and logic. The college course in general chemistry differs qualitatively from the usual first secondly school course in chemistry with respect to the kind of laboratory work done by students. Quantitative differences appear in the number of topics treated, the time spent on the course by students, and the nature and the variety of experiments done in the laboratory. Prerequisites: The AP Chemistry course is designed to be taken only after the successful completion of a first course in high school chemistry (Chemistry 1). Surveys of students who take the AP Chemistry Exam indicate that the probability of achieving a grade of 3 or higher is significantly greater for students who successfully complete a first course in high school chemistry prior to undertaking the AP course. Thus, it is STRONGLY recommended that credit in a first-year chemistry course be a prerequisite for enrollment in an AP Chemistry class. In addition, the recommended mathematics prerequisites for an AP Chemistry class is the successful completion of a second-year algebra course. AP Chemistry Topics: 1. Structure of Matter (20 percent) a) Atomic theory and atomic structure b) Chemical bonding c) Nuclear chemistry 2. States of Matter (20 percent) a) Gases b) Liquids and solids c) Solutions 3. Reactions (35 – 40 percent) a) Reaction types b) Stoichiometry c) Equilibrium d) Kinetics e) Thermodynamics 4. Descriptive Chemistry (10 – 15 percent) a) Chemical reactivity and products of chemical reactions b) Relationships in the periodic table c) Introduction to organic chemistry 5. Laboratory (5 – 10 percent) a) Making observations of chemical reactions b) Recording data/Communicating effectively the results c) Calculating/interpreting results based on the quantitative data obtained. Unless otherwise noted, each laboratory will be “hands-on” and will involve: a) physical manipulation of equipment and materials in order to make relevant observations and collect data b) use the collected data to form conclusions and verify hypotheses c) communicate and compare their results and procedures (informally to classmates and in a formal, written report to the teacher) Resources: 1. Text – “Chemistry” by Zumdahl (6th Edition), ancillaries and supplements 2. The College Board Science Achievement Tests/Past AP Exams 3. Video/Internet Resources (APEX, Glencoe, Zumdahl Interactive 6.0) 4. Additional advanced chemistry texts (Brown et al, Hill et al, Holt Modern Chemistry, Glencoe Chemistry Matter and Change) 5. HM Class Prep with HM Testing v6.1 6. Princeton and Cole AP Chemistry Test Preparation AP CHEMISTRY COURSE OUTLINE This course is given in terms of the Zumdahl Chemistry textbook (6th Edition). The problems at the end of the chapters are very challenging and serve as an excellent tool for students to use to truly comprehend the material. The problems also indicate the depth of coverage required for each topic. Introduction: 1 day (Aug 25) Predictive Assessment: 1 day (Aug 26) Unit 1: Review of Chemistry I Honors Topics (Chapters 1-5, 11) August 29 – October 14 Chemical Foundations: Measuring and units Use of significant figures Dimensional analysis Classification of matter Lab: Identification of Unknown Substances (60 minutes) 1 day (Aug 29) Atoms, Molecules, and Ions: Early history of chemistry Law of Conservation of Mass Law of Definite Proportion Law of Multiple Proportions Dalton’s Atomic Theory Avogadro’s Hypothesis Early experiments to characterize atomic structure Modern view of the atom Introduction to the Periodic Table Naming compounds 1 day (Aug 30) Stoichiometry: 7 days Atomic mass, moles and molar mass (Aug 31, Sep 1,2, 6-8) Percent composition of compounds Empirical formula determination Chemical equations and stoichiometric calculations Limiting reagent, theoretical yield, percent yield Lab: Determination of the Empirical Formula of a Compound by the Decomposition of a Metallic Oxide and the Formation of a Metal Sulfide (120 minutes) Lab: Stoichiometric Determinations Lab (120 min) Lab: Iron Tango Lab (limiting reactant/percent yield) (75 minutes) Lab: Determination of the Percent of Water in a Hydrate (60 minutes) Gases: 5 days (Sep 12-16) Pressure Gas Laws of Boyle, Charles, and Gay-Lussac Ideal Gas Law Gas Stoichiometry Dalton’s Law of Partial Pressure Kinetic Molecular Theory Effusion and diffusion Real gases/atmosphere Lab: Determination of the Molar Volume of a Gas (120 minutes) Lab: Charles’ Law Experiment (30 minutes) Demo: Atmospheric pressure, Boyle’s Law REVIEW (CHAPTERS 1 – 3, 5) Sep 19, 20 (All Reviews include past AP questions, Zumdahl Study Guide questions) TEST 1 (CHAPTER 1 – 3) Sep 21(Wednesday) MID-QUARTER REPORT September 27 Types of Chemical Reactions and Solution Chemistry: 9 days Composition of solutions (Sep 22,23,26-30, Precipitation Oct 3,4) Acid/base reactions Oxidation/reduction reactions (time permitting) Stoichiometry problems involving solution chemistry Predicting Reactions, Net ionic equations**** (continual) Lab: Analysis of an Unknown Chloride (120 minutes) Lab: Reactions, Predictions, and Net Ionic Equations (240 minutes) Properties of Solution: 5 days Energies of solvation (Oct 5,6,7,10,11) Factors affecting solubility Vapor pressures and Raoult’s Law Boiling-point elevation and freezing-point depression Osmotic pressure Colligative properties Colloids Lab: Colligative Properties Lab(45 minutes) Lab: Determination of Molar Mass by Freezing Point (90 minutes) REVIEW (CHAPTERS 4, 11) TEST (CHAPTERS 4, 11) REPORT CARDS (QUARTER 1) Oct 12, 13 Oct 14 (Friday) November 3 Unit 2: Atomic Structure and Bonding: (Chapter 7, 8, part of 9) Oct 17 – Nov 4 Atomic Structure and Periodicity 7 Days Electromagnetic radiation (Oct 17-21, 24,25) Planck, photon, E=mc2 Dual nature of light DeBroglie equation Continuous vs. line spectra Bohr atom Modern view of the atom (wave function and probability) Heisenberg Uncertainty Principle Quantum numbers Orbital shapes and energies Electron spin, Aufbau Principle, Pauli Principle History of Periodic Table Periodic trends Alkali metal properties Lab: Flame Test for Metals (45 minutes) Lab: Spectral tubes/Diffraction grating to view spectra (45 minutes) Bonding: General Concepts: 5 Days Types of bonds (Oct 26-28,31, ) Electronegativity, electron affinity, & ionization energy (Nov 1) Bond polarity and dipole moment Electron configuration and sizes of atoms and ions Formations of ionic compounds Ionic character of covalent bonds Model of covalent bond energies Bond energies, enthalpy, and chemical reactions Localized electron bonding model Lewis structures Exceptions to octet rule Resonance VSEPR model Hybridization Lab: Molecular Model Lab No. 1(building structure using a molecular model kit, identifying bonding type, drawing Lewis Structure, identifying molecular shape and molecular force) (60 minutes) Lab: Molecular Model Lab No. 2 (Exceptions to the Octet Rule – uses toothpicks and Styrofoam balls to create structure)(60 minutes) REVIEW (CHAPTER 7-9) TEST (CHAPTER 7-9) MID-QUARTER REPORT Nov 2,3 Nov 4 (Friday) December 7 Unit 3: Chemical Equilibrium (Chapters 13-15) Nov 7 – Dec 21 Chemical Equilibrium: 5 days Equilibrium condition (Nov 7-10, 14) Equilibrium constant Kp (pressure) Heterogeneous equilibria Solving equilibrium problems Le Chatelier’s Principle Lab: Stresses Applied to Equilibrium Systems (Le Chatelier’s Principle) (90 min) Lab: Determination of Equilibrium Constant for a Chemical Reaction (120 min) Acids and Bases: 11 Days Nature of acids and bases (Nov 15-18, 21,22, Acid strength Nov 28-30, Dec 1,2) pH scale Calculating pH of strong and weak acid solutions Bases and base strength Polyprotic acids Acid/base properties of salts and oxides Lewis acid/base Solving acid/base problems Lab: Stresses Applied to Equilibrium Systems (Experiment 26) (150 minutes) Lab: Hydronium Ion Concentration and pH (90 minutes) Lab: Determination of an Acid Dissociation Constant, Ka (50 minutes) Lab: Determination of a Base Dissociation Constant, Kb (50 minutes) Lab: Determination of an Unknown Concentration by Acid/Base Titration (60 minutes) Lab: Titration of Weak Acid/Strong Base, Strong Acid/Strong Base, Weak Base/Strong Acid (4 days) – calculations, graphs, experimental procedure Lab: Soda Lab (50 minutes) Application of Aqueous Equilibria 10 Days Acid or base solutions with common ion (Dec 5-9, 12-16) Buffered solutions Buffer capacity Titrations and pH curves Choosing an appropriate indicator for titrations Solubility equilibria and solubility product Precipitation behavior as pH is varied Equilibria involving complex ions Lab: Oh, What a Buffer it is!!! (60 minutes) Lab: Determination of the Dissociation Constant of a Weak Acid (90 minutes) Lab: Determining the Ka of an Indicator (60 minutes) Lab: Ksp of Ca(OH)2 REVIEW (CH. 13-15) TEST (CH. 13-15) Unit 4: Thermodynamics and Electrochemistry Chapter 6, 16, and 17) Dec 19,20 Dec 21 (Wednesday) Jan 3 – Feb 16 Thermodynamics: 7 days Nature of Energy (Jan 3-6, 9-11) Three Law of Thermodynamics State functions Work, heat, and internal energy Enthalpy and calorimetry Hess’s Law Standard Enthalpies of Formation Present and future energy sources Lab: Observing Heat Changes (30 minutes) – mixing/observation of three thermochemical reactions, identification of endothermic or exothermic, identification as physical or chemical change. Lab: Determining the Specific Heat of an Unknown Metal – the specific heat capacity of a nail will be experimentally determined by measuring the temperature change of water and of the nail after it has been heated to approximately 850 degrees Celsius in a Bunsen burner (45 minutes) Lab: Thermochemistry and Hess’ Law – three different combinations of acids and bases are made. All of the reactions are exothermic. The temperature change of each reaction will be measured and the enthalpy will be calculated. The reactions are chosen so that subtracting the chemical equation for the second reaction from that of the first reaction will give the chemical equation for the third reaction. Consequently, according to Hess’ Law, subtracting enthalpy of the second equation for the first should lead to the enthalpy of the third; therefore, verifying Hess’ Law. (90 minutes) Lab: Measuring Energy Changes (Heat of fusion) – to determine the temperature and heat changes that occur when ice melts. A heating curve will be obtained in Part A and measurements will be taken in Part B to determine the experimental heat of fusion (60 minutes) Spontaneity, Entropy, and Free Energy: Spontaneous processes and entropy Free Energy Entropy changes and chemical reactionx Free energy and chemical reactions Dependence of free energy on pressure Free energy and equilibrium Free energy and work 6 days (Jan 12,13, 24-27) Electrochemistry: 11 days Galvanic cells (Jan 30,31, Feb 1-3, Standard reduction potentials Feb 6-10, 13) Cell potential, electrical work, and free energy Cell potential and concentrations Batteries Corrosion Electrolysis Commercial electrolytic processes Lab: Electrochemical Cells –several different half-cells are prepared and connected to find the voltages generated. The values are used to contract a table of “relative” electrode potentials. Also, the change in concentration of one of the solutions will be observed to see how this affects cell potential. Thirdly, we will determine the solubility product of silver chloride. Lab: Determination of Iron by Redox Titration (use potassium permanganate as a titrant in the analysis of an unknown sample containing iron). (120 minutes) REVIEW (CHAPTER 6, 16, 17) TEST (CHAPTER 17) MID-QUARTER REPORT Feb 14,15 Feb 16 (Thursday) March 1 Unit 5: Rate Kinetics (Chapter 12) 7 days Reaction rates (Feb 20-24, 28,29) Rate laws Determining rate laws Integrated rate laws Reaction mechanism Catalysis Lab: Temperature and Reaction Rates – inquiry lab – what effect does temperature have on the rate of a chemical reaction? (60 minutes) Lab: Introduction to Reaction Rates – investigate how changing the temperature of the reactants or how changing the concentration of potassium hydroxide will affect the rate of reaction of methylene blue (60 minutes) Demo: Iodine Clock reaction Unit 6: Nuclear Chemistry (Chapter 21) Nuclear stability and radioactive decay Kinetics of radioactive decay Nuclear transformation Detection and uses of radioactivity Thermodynamic stability of the nucleus Nuclear fission and fusion Effects of radiation 6 days (Mar 1,2, 5-8) REVIEW (CHAPTER 12/21) TEST (CHAPTER 12/21) REPORT CARDS (QUARTER 3) Unit 7: Review for AP Exam Mar 9/12 Mar 13 (Tuesday) April 7 27 days (Mar 14,15,16, 19-23, 26-29, Apr 2-5, 16-20, 23-27, 30 AP CHEMISTRY YEAR PLAN UNIT Introduction/Safety DATE Aug 25 Predictive Assessment Aug 26 Unit 1: Review of Chemistry 1 Honors Topics (Chapters 1-5, 11) Aug 29– Oct 14 Unit 2: Atomic Structure and Bonding (Chapters 7, 8, part of 9) Oct 17 – Nov 4 Unit 3: Chemical Equilibrium (Chapters 13-15) Nov 7 – Dec 21 Unit 4: Thermodynamics and Electrochemistry (Chapters 6, 16, and 17) Jan 3 – Feb 16 Unit 5: Rate Kinetics (Chapter 12) Feb 20 – Feb 29 Unit 6: Nuclear Chemistry Mar 1 – Mar 13 Unit 7: Review for AP Exam Mar 14– Apr 30 AP Chemistry Exam May 1, 2011 Organic Chemistry/Extra Labs May 2 – Jun 1 Unit 8: Confirmation: I have read and understand all of the information explained above! I will turn the portion in below the dotted line and keep the rest to serve as the first pages in my three-ring binder. Parent: Guardian Name ___________________ Name Signature ________________ Signature ________________ _______________ Parent e-mail Parent phone Date ______ Date