Curricular Requirements CR1 Students and teachers use a recently published (within the last 10 years) college- level chemistry textbook.

Transcription

1 AP Chemistry Syllabus Curricular Requirements Page(s) CR1 Students and teachers use a recently published (within the last 10 years) college- level chemistry textbook. 9 CR2 The course is structured around the enduring understandings within the big ideas as described in the AP Chemistry Curriculum Framework CR3a The course provides students with opportunities outside the laboratory environment to meet the learning objectives within Big Idea 1: Structure of matter. 3, 4, 6 CR3b The course provides students with opportunities outside the laboratory environment to meet the learning objectives within Big Idea 2: Properties of matter characteristics, states, and forces of attraction. 4, 5, 6 CR3c The course provides students with opportunities outside the laboratory environment to meet the learning objectives within Big Idea 3: Chemical reactions. 3, 4, 6 CR3d The course provides students with opportunities outside the laboratory environment to meet the learning objectives within Big Idea 4: Rates of chemical reactions. 5 CR3e The course provides students with opportunities outside the laboratory environment to meet the learning objectives within Big Idea 5: Thermodynamics. 4, 5, 6 CR3f The course provides students with opportunities outside the laboratory environment to meet the learning objectives within Big Idea 6: Equilibrium. 4, 5, 6 CR4 CR5a The course provides students with the opportunity to connect their knowledge of chemistry and science to major societal or technological components (e.g., concerns, technological advances, innovations) to help them become scientifically literate citizens. Students are provided the opportunity to engage in investigative laboratory work integrated throughout the course for a minimum of 25 percent of instructional time., 10, 11 2 CR5b CR6 CR Students are provided the opportunity to engage in a minimum of 16 hands- on laboratory experiments integrated throughout the course while using basic laboratory equipment to support the learning objectives listed within the AP Chemistry Curriculum Framework. The laboratory investigations used throughout the course allow students to apply the seven science practices defined in the AP Chemistry Curriculum Framework. At a minimum, six of the required 16 labs are conducted in a guided- inquiry format. The course provides opportunities for students to develop, record, and maintain evidence of their verbal, written, and graphic communication skills through laboratory reports, summaries of literature or scientific investigations, and oral, written, and graphic presentations. 2, 2,, 8 10, 11, 13, 14 1

2 AP Chemistry Syllabus Laboratory Investigation Sequence Lab Title Inquiry or Traditional Big Idea (BI) Learning Objectives (LO) Science Practice (SP) Analysis of Food Dyes in Beverages Inquiry , , 4, 5, 6 Percent Copper in Brass Inquiry ,1.16 4, 5, 6 Separating a Synthetic Pain Relief Mixture Inquiry , , 4, 5, 6 Acidity of Beverages Inquiry , 3.3 1, 2, 3, 4, 5, Green Chemistry Analysis of a Mixture Inquiry , 3.3, 3.5 1, 2, 4, 5, 6 Analysis of Hydrogen Peroxide Inquiry , 3.3, 3.9 2, 4, 5 Gravimetric Analysis of Calcium and Hard Water Inquiry , 2.10, 3.2, 3.3 1, 2, 4, 5, Designing a Hand Warmer Inquiry 5 3., 3.10, 4.1, 4.2 1, 4, 5, 6 Qualitative Analysis and Chemical Bonding Inquiry 2 Molecular Geometries of Covalent Molecules: Lewis Structures and the VSEPR Model 2.11, 2.13, 2.15, 2.16, 2.19, 2.20, , 4, Traditional , Models of Molecules Traditional , Separation of a Dye Mixture Using Chromatography Inquiry 2 2., 2.10, , 4, 5, 6 Rate of Decomposition of Calcium Carbonate Inquiry 4 3., 3.10, 4.1, 4.2 1, 4, 5, 6 Kinetics of Crystal Violet Fading Inquiry , 3.3, 4.1, 4.2 1, 2, 4, 5, 6 Application of LeChâtelier s Principle Inquiry , 6.3, 6.8, 6.9 1, 4, 5, Acid- Base Titrations Inquiry 6 Buffers in Household Products Inquiry 6 Properties of Buffer Solutions Inquiry , 1.20, 3.4, 3., 6.11, 6.12, 6.13, 6.15, 6.16, , 3., 6.12, 6.16, 6.19, , 3., , 6.18, 6.19, 6.20 Electrochemical Cells Traditional , , 2, 3, 4, 5, 2, 4, 5, 2, 4, 5, 1, 2, 4, 5, Molecular Geometry: Experience with Models Traditional , , 2

3 AP Chemistry Syllabus Activities that Support Learning Opportunities Outside of the Laboratory Setting Activity Title Mass Spectroscopy Combustion Analysis Empirical Formula Naming Ionic Compounds Polyatomic Ions Naming Molecular Compounds Naming Acids Coulombic Attraction Law of Conservation of Mass, Laws of Definite and Multiple Proportions Atomic Math Net Ionic Equations Solubility Acids and Bases Strong Versus Weak Acids Description of Activity & Outcomes Expected Describe 4 processes in mass spectrometer, explain how electromagnet separates particles by mass/charge ratio, read mass spectra to identify common ions, predict mass spectra for elements Write balanced chemical equation for combustion of hydrocarbons, find empirical formulas from mass of CO 2 and H 2 O from combustion analysis Write empirical formulas from molecular formulas, percent composition data and discuss limitations of empirical formulas Determine the proper names of ionic substances, determine the proper name and formula for atoms that form more than one type of ion Explore polyatomic ions their structures and names, draw models of ions, name and draw ternary ionic compounds Name molecular compounds, write formulas for molecular compounds, compare and contrast formulas and names for ionic and molecular compounds Name and write formulas for binary and ternary acids (oxyacids), learn when to use per, ic, ous, and hypo prefixes and suffixes. Using models to determine the relationship between distance and attractive force of subatomic particles, between Coulombic attraction and location on the periodic table, between number of protons and attractive force Use the law of conservation of mass, law of definite proportions, and the law of multiple proportions to determine percent by mass, compare compounds and formulas, determine the mass of an element in a compound Convert between mass, moles, and number of atoms; determine the number of subatomic particles in an isotope, calculate atomic mass based on isotope abundance; use the periodic table to find the mass and number of subatomic particles Write a net ionic equation when given molecular equation, identify spectator ions Quantify the amount of solute that is dissolved in a saturated solution, calculate the solubility of a solute, interpret solubility curves Explore the physical and chemical properties of acids and bases, compare and contrast the Arrhenius acids and bases to Bronsted- Lowry acids and bases, determine acid/conjugate base pairs Compare and contrast strong and weak acids on the basis of conductivity, electrolytes, concentration, and K a values Big Idea (LO) (SP) , 6, , , , , , , , , , 3

4 Activity Title Equilibrium Stoichiometry Activity Limiting Reactant Activity Calorimetry Bond Energy Heats of Formation Free Energy Work, Equilibrium, and Free Energy Electron Configurations Advanced Periodic Trends Photoelectron Spectroscopy Molecular Geometry Types of Bonds Description of Activity & Outcomes Expected Explain the importance of the following in reversible reactions: double arrow, concentrations of reactants and products; utilize the ICE method for calculating number of moles at equilibrium, predicting the direction of the equilibrium (favors the products or favors the reactants) Write and balance chemical equations, use the equations to perform stoichiometric calculations (determine number of moles/grams needed and produced), classify the type of chemical reaction observed Compare chemical limiting reactant to ingredients in a recipe, determine the limiting reactant then calculate moles and grams needed and produced based on the limiting reactant Explore the relationship between mass, temperature, heat energy, and the type of substance are related; define and calculate specific heat Predict the breaking or formation of bonds based on H values, predict endothermic or exothermic based on H, calculate H, determine the relationship between bond type and bond energy, calculate the net energy change of a reaction, analyze distance versus potential energy graphs for single and double bonds Identify a formation reaction as a synthesis reaction, explain why some formation reactions are endothermic, calculate standard enthalpy of new reaction Relate the entropy of a system to the degree of organization of molecules, relate the change in energy for a process to relative potential energy of reactants/products, describe entropy and enthalpy changes that will make a process spontaneous Predict the sign of G when given the initial conditions of a reaction and the K eq and K p compare amount of work done on a system given two sets of initial conditions of a reaction Based on a model of a house, determine how electrons fill up available spaces in an atom and how configurations are assigned, determine the electron configuration for an atom that is in an excited state Calculate the core charge to approximate effective nuclear charge, justify atomic radius, 1 st ionization energy, electronegativity trend data, use concepts of Coulombic attraction, electron shielding, effective nuclear charge Derive math relationship between kinetic energy, ionization energy, and photon energy, match proposed shell models with PES spectrums, compare PES spectra and explain shifts in peaks Predict 3- D molecular shape based on the Lewis structures, be able to examine a Lewis structure and determine the number of electron domains, apply VSEPR theory to 3- D molecular shapes, determine the bond angle based on the 3- D shape Describe the role of the electron in each type of bonding, identify the type of elements that would combine in different bonds, use electronegativity values to identify types of bonding Big Idea (LO) (SP) 1, 2, 6, 1, 5, 6, 1, 5, 6, 1, 5, 6, 4

5 Activity Title Polar and Nonpolar Molecules Properties of Covalent Bonds Lattice Energy Types of Solids Alloys Partial Pressures of Gases Deviations from the Ideal Gas Law Maxwell- Boltzmann Distributions Rate of Reaction Method of Initial Rates Reaction Quotient Common Ion Effect on Solubility Fractional Precipitation Common Ion Effect on Acid Ionization Description of Activity & Outcomes Expected Determine if molecule is polar or nonpolar by considering arrangement of polar bonds and lone pairs in 3- D space, apply symmetry to explain polarity Describe stable bond between atoms as an arrangement of the attractive and repulsive forces, predict which bond is strongest when comparing bonds of different order between similar atoms as well as different sizes Define lattice energy, use Born- Haber cycle to calculate lattice energy, determine which ionic compound has larger lattice energy based on size and charges of ions Describe 4 types of solids based on bonds, predict melting point and enthalpy of fusion based on type of solid, use chemical formula/melting point/heat of fusion to determine type of solid Identify an alloy as substitutional or interstitial when given a crystal lattice structure, predict changes in properties of a metal when an alloy is formed Use Dalton s law of partial pressures to find total pressure, calculate partial pressures given percent composition, use partial pressure in Ideal Gas Law calculations to find volumes or moles Explain why deviations in gas properties predicted by Ideal Gas Law are larger or smaller than expected, rank set of gases from largest to smallest deviation based on molecular volume and on differences in intermolecular forces Describe the effect of increased temperature and increased molar mass on distribution of particle speeds and kinetic energy, predict Maxwell- Boltzmann distribution for gas sample Determine the rate of change for a reactant or product from slope on reaction curve, predict rate of change for reactants and products when given rate of change for one component in a reaction Determine the order of a reaction using initial rate of reaction data, calculate the rate law constant for a reaction Write reaction quotient for chemical equilibrium, calculate Q using initial concentrations of all gaseous species in chemical equilibrium, predict direction reaction will proceed by comparing Q and K Describe effect of common ion in solution on solubility of insoluble salt, apply LeChatelier s Principle and common ion effect to either increase the formation of a precipitate or solubility of a salt Predict which precipitate will form first when a solution is added to a mixture of ions, calculate the concentration of added solution needed to form a precipitate, calculate the concentration of ions remaining in solution when a second precipitate starts to form Describe the effect on the percent ionization of a weak acid when a common ion is present in solution, calculate the percent ionization of a weak acid when a common ion is present Big Idea (LO) , (SP) 1, 5, 6, 1, 5, 6, 1, 5, 6, 5

6 Activity Title Buffers Strength of Acids Titration Curves Polyprotic Acids Oxidation and Reduction Electrochemical Cell Voltage Faraday s Law Batteries Introduction to Organic Reactions Alkane Nomenclature Polymer Chemistry Description of Activity & Outcomes Expected Identify a buffer solution as a mixture of a weak acid and a salt of a conjugate base in solution, explain why a buffer must contain both a weak acid and a conjugate base in order to neutralize both acids and bases Relate the strength of an acid to the ease of breaking the bond between H atom and conjugate base, rank binary acids in order of strength, rank oxy- acids in order of strength Describe the contents of a beaker containing a strong acid at any point during a titration and why it have the ph it does, calculate ph for strong acid sample being titrated at any point during titration given concentration and volume of acid and concentration of titrant, calculate concentration of an unknown strong acid from titration curve Read a graph of ph versus volume of titrant to determine if acid is monoprotic, diprotic, or triprotic; write the stepwise reactions for donation of H + from diprotic or triprotic acid; explain why ph at equivalence points of polyprotic Compare and contrast redox reactions with non- redox reactions. Write half reactions to show electron transfer in oxidation and reduction. Predict qualitatively the change in voltage of a cell as concentrations or partial pressures of gases are increased or decreased using LeChatelier s Principle, explain why voltage of an electrochemical cell is not constant over time Describe qualitatively how the time, current, and charge on the cation affect the productivity of an electrolytic cell, calculate the moles of product for an electrolytic cell given half reactions, time, and current of the cell Analyze a model of a voltaic cell for half reactions, electron flow, anodes, cathodes; draw a voltaic cell given certain ions and determine the anode and direction of flow of electrons, explain the role of a salt bridge Understand the curved- arrow notation and how it indicates flow of electrons from Lewis bases to Lewis acids in a reaction sequence, identify the bonding changes that occur in common organic reactions Name an alkane given its structure, draw the structure of an alkane given its name Identify reactions that are used to synthesize polymers, summarize information on polymer structure, properties, and uses Big Idea 6 (LO) , 3, (SP) 1, 5, 6, 1, 5, 6, 1, 5, 6, 1, 5, 6, 1, 5, 6, 1, 5, 6, 1, 5, 6, 6

7 AP Chemistry Course Syllabus Instructor: E- mail: Office Hours: Monday Friday :15 to 8:00 AM, after school, or by appointment Prerequisites: Chemistry with an A/B average Course Description: AP Chemistry is a freshman college level lab/problem- solving course. The course covers the topics recommended in the College Board s AP Chemistry Course Guide. We will use the textbook, Chemistry: The Central Science, as well as supplemental material on equation writing, organic chemistry, and exam review. This course is designed to prepare students for the Advanced Placement Chemistry Exam. The exam is required as part of this course and will be paid for by the school district (a $92 value). The date for this exam is set for May 1, 201. Most colleges grant credit for a passing score on this exam (please refer to specific colleges as to whether or not they allow credit and what score must be achieved). Much more detailed information on the course and exam is available on the internet at: chemistry?chem This course will involve substantial reading and homework. It is recommended, as with any college science course, that students dedicate a considerable number of hours outside the classroom working on chemistry. As a rule of thumb, college students are advised to spend 2 to 3 hours of study time per week for each credit a course is worth. AP Chemistry represents a 4- credit course per semester. Thus, students should plan to spend about 8 12 hours of weekly study time just for this AP course. The key for a student to have a successful year will depend upon his/her organizational skills. We will complete 16 guided- inquiry labs (and 4 traditional labs) for this course. We will be using Advanced Inquiry Labs for AP Chemistry from Flinn Scientific, Inc., 2016, which are based off of the 16 labs written by the College Board. All labs listed are guided- inquiry unless specifically noted as shorter, more traditional labs, and cover the science practices. At a minimum, 25% of instructional time will be spent in the laboratory. This amounts to an average of at least 100 minutes of in- class lab work each week (at least 2 class periods). There may be times when a student will be required to finish a lab before school, during lunch, or after school. If a student misses the lab, he/she will be required to do the lab outside of class time. Estimated lab times are included in this syllabus. Unless otherwise noted, all labs are wet labs and not simulations. Students will be required to maintain a lab notebook (provided by the school). If a student earns college credit for AP Chemistry, he/she must keep the lab notebook and take it to college with him. Any college professor has the right to see the notebook to ensure the laboratory requirements were satisfactorily met.

8 This Course Addresses the Six Big Ideas* for AP Chemistry Big Idea 1 Structure of Matter: The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangement of atoms. These atoms retain their identity in chemical reactions. Big Idea 2 Properties of Matter: Chemical and physical properties of materials can be explained by the structure and arrangement of atoms, ions, or molecules and the forces between them. Big Idea 3 Chemical Reactions: Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons. Big Idea 4 Rates of Chemical Reactions: Rates of chemical reactions are determined by details of the molecular collisions. Big Idea 5 Thermodynamics: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Big Idea 6 Equilibrium: Any bond or intermolecular attraction that can be formed can be broken. These two processes are in dynamic competition, sensitive to initial conditions and external perturbations. (* Taken from 2016 College Board s Concept Outline for AP Chemistry) This course also addresses the science practices for AP Chemistry set by the College Board. These practices are designed to get the students to think and act like scientists. The science practices are: Science Practice 1: The student can use representations and models to communicate scientific phenomena and solve scientific problems. Science Practice 2: The student can use mathematics appropriately. Science Practice 3: The student can engage in scientific questioning to extend thinking or to guide investigations within the context of the AP course. Science Practice 4: The student can plan and implement data collection strategies in relation to a particular scientific question. Science Practice 5: The student can perform data analysis and evaluation of evidence. Science Practice 6: The student can work with scientific explanations and theories. Science Practice : The student is able to connect and relate knowledge across various scales, concepts, and representations in and across domains. 8

9 Books: Textbook: Chemistry: The Central Science, AP Edition, Brown, LeMay, Bursten, Murphy, Woodward, and Stoltzfus. Pearson 2015 Exam Prep Book: Test Prep Series for AP Chemistry 2015 by Edward L. Waterman. Pearson Education : Activities for AP*Chemistry by Laura Trout. Flinn Scientific, Inc Teacher Lab Manual: AP Chemistry Guided- Inquiry Experiments: Applying the Science Practices. The College Board Labs: Advanced Inquiry Labs for AP Chemistry from Flinn Scientific, Inc Labs: Laboratory Experiments for Chemistry: The Central Science. Brown, LeMay, Bursten, Murphy, Woodward, and Stoltzfus. Pearson Education Materials: Laboratory Notebook quad- ruled, carbonless (this is provided for you) Safety Goggles (provided) 2 3- ring binder for notes, handouts, homework, etc. Pen, pencil, loose- leaf paper SCIENTIFIC CALCULATOR (TI- 30XA is fairly inexpensive at about $10 and super easy to use) Class Expectations: Arrive on time with necessary materials No food or drink allowed in class Complete assigned work on time Follow all laboratory and safety guidelines Ask for help when needed We will conduct class in a courteous and respectful manner. Appropriate penalties await those who choose to ignore this basic expectation. Attendance and participation in class discussions, labs, and group activities is expected and needed. For individual lab reports, activities, or homework, you may confer with your lab partner and share ideas. However, written answers must be on your own. If your answers are identical to your partner s answers, expect point deductions or no points at all. Posted Class Rules Be respectful Be safe; follow all safety precautions (written or oral) Be in your seat when the bell rings (we need to use every second of our class period) Bring all books and materials to class Follow directions the first time they are given 9

10 Attendance: Absences: You must see me prior to any anticipated absences to schedule homework and make- up work times. According to the school handbook, school related activities are pre- arranged absences. Technically, assignments and quizzes are due before you leave; however, I will probably allow you to turn work in when you return unless an assignment is due the day you are gone (turn them in early). You do NOT get days to make up these assignments because you were gone for a school related activity. If you miss class yet are in school later or earlier in the day, you are still responsible for stopping by and turning in assignments. If you are ill, the school handbook rules will apply. Keep in mind that we will move at a quick pace. Catching up as quickly as possible will be to your advantage. Please refer to the detailed daily outlines for each unit. Tardies: After 3 unexcused tardies (less than 10 minutes), you will serve an after school detention with the teacher. Furthermore, you will miss valuable instruction. We will start class immediately. Be on time. Safety: Think about safety at all times. You will be given separate safety instructions. Know and follow the rules. Violations of safety rules will result in exclusion from the lab and a grade of zero on the lab. Make- Up Work: Information will be posted on Google Classroom. Check for any vital information there. Also see the detailed outlines provided with each unit. Make sure to check the absent box on the wall for missing work. Also check with the teacher to see if there is more work or handouts you may require. Labs must be made up. The teacher must verify that you did indeed spend 25% of your class time in a laboratory setting. Time limits will follow the handbook rules. You have one day for every day you miss. It is to your advantage to get caught up as quickly as possible. Let the teacher know if you would like to work together before or after school. LATE WORK WILL NOT BE ACCEPTED. You will discover that in college late work is not accepted. If you miss a deadline (including taking a test or quiz), you will receive a zero in college. Because this is essentially a college course, it will be treated as such. If the test or quiz has been announced several days in advance and you are absent the day before, you will be expected to take the test or quiz with the rest of the class. If you are absent on the day of the test or quiz, you will take it the day you return. Extended illness or circumstances will be dealt with separately. Grades and Assessments: Your semester grade will consist of the following: 1. Tests: Tests will model the format of the AP exam, including multiple- choice questions and one or more multi- part free response problems. In class, tests will be given at the end of every unit. 2. Lab Papers and Notebook: For every lab, all students are expected to write and submit a formal lab paper following the format provided in this syllabus. The introduction and procedure sections must be written and teacher- approved PRIOR TO THE BEGINNING OF EACH LAB. The finished lab reports are due three days after the laboratory is completed. In addition, each 10

11 student must keep a laboratory notebook containing all observations and data collected in the experiments. The lab notebook may be checked and graded at the end of each quarter. There will be a log in the classroom. Students will sign- in for lab time as documentation of the 25% minimum requirement of class time devoted to laboratory. Students cannot pass the course without meeting the minimum lab time requirement. Remember that a student must keep the lab notebook and take it to college as proof that he/she did complete the 16 required, hands- on labs. 3. Reading Quizzes: In order to get the most out of this course, reading the textbook and understanding the content will be essential. At the introduction to each new chapter, you will take a short (5 10 minutes) quiz that will assess your reading comprehension. The quizzes will focus on the main idea and main topics of the chapter. You may take notes while you read; notes may be used on the quizzes. 4. : You will work in groups to solve problems through Process Oriented Guided Inquiry Learning () activities. s offer the student an opportunity to meet the learning objectives put forth by the College Board in a non- lab setting. s require students to interpret models, data tables, and graphs. Throughout the syllabus, you will see what AP Big Ideas, Learning Objectives, and Science Practices are covered by the s. The advantages to group work are many. Students become active learners. By discussing and explaining ideas back to others, students can develop a deeper understanding of the topics. Students are exposed to more ideas and can tackle more complex problems with each other s help. For group work to be successful, however, students are expected to follow these guidelines: Be considerate Listen without interrupting Ask questions when needed Help others in the group Make sure everyone in the group understands the ideas well enough to present them to the class Roles: Manager: actively participates, keeps the team on task, distributes work and assigns responsibilities, resolves disputes, and assures that all members participate and understand Spokesperson: actively participates, represents views and conclusions held by the majority, presents required oral reports and discussions to the class Recorder: actively participates, keeps a record of instructions and what the team has done, and prepares the final written report and other documentation in consultation with the others Strategy Analyst: actively participates, identifies and keeps a log of problem- solving strategies and methods, identifies and keeps a log of what the team is doing well, what needs improvement, and insights and discoveries regarding course content and individual and team performance 5. Homework/Textbook Problems: You will be assigned homework on worksheets or from the chapters. The problem numbers for each chapter will be posted on the board, Google Classroom, and on handouts. Generally, the problems assigned will have the answers in the back of the book. This is to help you see that you are on track and allow us to focus on the problems 11

12 that were most difficult for you during class time. You are not graded on whether or not you completed the problems correctly. Instead, you will receive a mark for showing your work and attempting all the problems. Each assignment will take a few hours to complete. Working through the assigned problems will increase your understanding of the topics and should increase your speed in problem- solving for the AP exam. Grading: All of your class work will be assigned a point value. The number of each of these graded assignments/assessments will vary from quarter to quarter. Grades will be determined by dividing points earned by points possible. This will be your quarterly percentage grade. Generally, the points will fit into these guidelines (depending on the size of the lab, labs may be worth more): activities 5 points Homework check marks (each check is worth 1 bonus point) Quizzes 10 points Labs 30 points Tests 100 points The following grade scale will be used: A: B: C: 0 9 D: F: 0 59 Semester grades will be composed as follows: 1 st quarter 40%, 2 nd quarter 40% and semester exam 20%. The same grading system will be used for both semesters. 12

13 The 10 Parts of a Laboratory Report A specific format will be given to the student for each lab (along with the point value for the lab). Students must follow that format and label all sections very clearly. AP Chemistry lab reports are much longer and more in depth than the ones completed in the first year chemistry course. Therefore, it is important that students don t procrastinate when doing pre- lab and post- lab work. Late labs will not be accepted. Labs not completed in class must be done at lunch or before/after school by appointment. Table of Contents Page Students will list their name, course, class period, and school year. As each experiment is recorded in the notebook, students will complete the table of contents page with the date of the experiment, the experiment title, and the lab notebook page number it begins on. Pre- Lab Work Pre- lab work is to be completed and turned in on the day the lab is performed. Make sure your NAME is on the lab as well! 1. Title The title should be descriptive. For example, ph Titration Lab is a descriptive title and Experiment 5 is not a descriptive title. 2. Date This is the date(s) the student performed the experiment. 3. Purpose A purpose is a statement summarizing the point of the lab. 4. Pre- Lab Questions Students will be given some questions to answer before the lab is done. They will need to either rewrite the question or incorporate the question in the answer. The idea here is that when someone (like a college professor) looks at a student s lab notebook, they should be able to tell what the question was by merely looking at their lab report. It is important to produce a good record of lab work. 5. Safety Outline any safety concerns or safety procedures that should be followed during the lab. 6. Procedure Outline Students need to write an outline of the procedure. They should use bulleted statements or outline format to make it easy to read. There should be adequate information listed that a student can perform the experiment from this outline. THERE WILL BE MORE THAN ONE PROCEDURE TO WRITE. Often, there is a introductory lab (or labs) and a guided- inquiry portion. The introductory lab is written for you and can easily be outlined or adapted. The guided- inquiry portion is a procedure that YOU write. The teacher will be looking for details, accuracy, and thoroughness in the guided inquiry procedure. 13

14 . Data Tables Students will need to create any data tables or charts necessary for data collection in the lab. 8. Data Students need to record all their data directly in their lab notebook. They are NOT to be recording data on their separate lab sheet. They need to label all data clearly and always include proper units of measurement. Students should underline, use capital letters, or use any device they choose to help organize this section well. They should space things out neatly and clearly. 9. Calculations and Graphs Students should show how calculations are carried out. Graphs need to be titled, axes need to be labeled, and units need to be shown on the axis. To receive credit for any graphs, they must be at least ½ page in size. 10. Conclusions This will vary from lab to lab. Students will be given direction as to what to write, but it is expected that all conclusions will be well thought out and well written. 11. Post Lab Error Analysis and Questions Follow the same procedure as for the Pre- Lab Questions. **A record of lab work is an important document, which will show the quality of the lab work that students have performed. If a student passes the AP Chemistry Exam, the student must keep the lab notebook as evidence of having completed the lab portion of the course. Any college professor may ask at any time to see proof of this notebook. 14

15 AP Chemistry Unit Overview Unit 1: Chemistry Fundamentals Matter, Measurement, Atoms, Molecules, Ions, Chemical Formulas Chapters: 1 (sections 2, 3), 2 (all sections), 3 (sections 3, 4, 5) Time Frame: 5 weeks Homework Sets Assigned: 2 s: 8 Number of Quizzes: 3 Number of Exams: 1 Big Ideas: 1, 3, 5 Enduring Understandings: 1A, 1B, 1D, 3C, 5D Learning Objectives: 1.1, 1.2, 1.3, 1.4, 1.5, 1.6, 1., 1.13, 1.14, 1.15, 1.16, 3.10, 5.10 Topics Covered: 1. Classification of Matter gas, liquid, solid, pure substance, elements, symbols, compounds, mixtures 2. Properties of Matter physical & chemical properties, physical & chemical change, separation of mixtures (filtration, distillation, chromatography) 3. Atomic Theory of Matter atoms, law of constant composition, law of conservation of mass, law of multiple proportions, Dalton s atomic theory 4. Modern View of Atomic Structure nucleus, electrons, atomic structure, atomic mass unit, electrical charges of subatomic particles, atomic number, mass number, isotopes, Coulomb s Law, mass spectroscopy 5. Molecules and Molecular Compounds molecules, chemical formulas, molecular formulas, empirical formulas, structural formulas 6. Ions and Ionic Compounds ion, cation, anion, polyatomic ions, ionic charges, ionic compounds. Formula Weights molar mass, percentage composition 8. Avogadro s Number and the Mole moles, Avogadro s number, molar mass, interconverting mass, moles and number of particles 9. Empirical Formulas from Analysis Calculation of empirical and molecular formulas, combustion analysis s: Mass Spectroscopy Combustion Analysis Empirical Formula Naming Ionic Compounds Polyatomic Ions Naming Molecular Compounds Naming Acids Coulombic Attraction Labs: Analysis of Food Dyes in Beverages (Big Idea 1, Investigation 1, guided inquiry), 100 minutes (LO 1.15, 1.16; SP 2, 4, 5, 6) Percent Copper in Brass (Big Idea 1, Investigation 2, guided inquiry), 150 minutes (LO 1.15, 1.16; SP 4, 5, 6) Separating a Synthetic Pain Relief Mixture (Big Idea 3, Investigation 9, guided inquiry), 100 minutes (LO 3.10, 5.10; SP 1, 4, 5, 6) 15

16 Unit 2: Stoichiometry, Balanced Reactions, Types of Reactions, and Reactions in Solution Chapters: 3 (section 1, 2, ) & 4 (all sections) Time Frame: 4 weeks Homework Sets Assigned: 4 s: 5 Number of Quizzes: 2 Number of Exams: 1 Big Ideas: 1, 2, 3 Enduring Understandings: 1E, 2A, 3A, 3B, 3C Learning Objectives: 1.4, 1.1, 1.18, 1.19, 1.20, 2.1, 2.2, 2.9, 2.10, 3.1, 3.2, 3.3, 3.4, 3.5, 3.6, 3., 3.8, 3.9, 3.10 Topics Covered: 1. Chemical Equations - chemical equations, reactants, products, balancing equations, coefficients 2. Simple Patterns of Chemical Reactivity synthesis, decomposition, combustion 3. Quantitative Information from Balanced Equations stoichiometry, using equations to interconvert mass, moles and number of particles 4. Limiting Reactants limiting reactant, theoretical yield, actual yield, percentage theoretical yield 5. General Properties of Aqueous Solutions molecules in water, non- electrolytes, ions in solution, strong electrolytes, weak electrolytes, chemical equilibrium 6. Precipitation Reactions precipitate, solubility, solubility guidelines, molecular (complete) equations, ionic equations, net ionic equations, spectator ions, writing net ionic equations, gravimetric analysis. Acids, Bases, and Neutralization Reactions Acids, proton donors, monoprotic acids, diprotic acids, bases, proton acceptors, hydroxides, strong and weak acids and bases, strong acids and bases as strong electrolytes, neutralization reactions, salts, ph 8. Oxidation Reduction Reactions Oxidation, reduction, redox reactions, oxidation numbers, determining oxidation numbers, displacement reactions, activity series 9. Concentrations of Solutions Molarity, calculating molarity, interconverting molarity, moles and solution volume, dilution, preparing solution concentrations 10. Solution Stoichiometry and Chemical Analysis titration, standard solution, equivalence point, titration calculations, mass relations in a neutralization reaction s: Net Ionic Equations Solubility Acids and Bases Strong Versus Weak Acids Equilibrium Labs: Acidity of Beverages (Big Idea 1, Investigation 4, guided inquiry), 100 minutes (LO 1.20, 3.3; SP 1, 2, 3, 4, 5, ) Green Chemistry Analysis of a Mixture (Big Idea 3, Investigation, guided inquiry), 100 minutes (LO 1.18, 3.3, 3.5; SP 1, 2, 4, 5, 6) Analysis of Hydrogen Peroxide (Big Idea 3, Investigation 8, guided inquiry), 100 minutes (LO 1.20, 3.3, 3.9; SP 2, 4, 5) Gravimetric Analysis of Calcium and Hard Water (Big Idea 3, Investigation 3, guided inquiry), 100 minutes (LO 1.19, 2.10, 3.2, 3.3; SP 1, 2, 4, 5, ) 16

17 Unit 3: Chemical Energy, Thermochemistry, and Thermodynamics Chapters: 5 and 19 Time Frame: 2.5 weeks Homework Sets Assigned: 5 s: 5 Number of Quizzes: 2 Number of Exams: 1 Big Ideas: 2, 3, 5, 6 Enduring Understandings: 2B, 2D, 3C, 5A, 5B, 5C, 5E, 6A, 6D Learning Objectives: 2.15, 2.23, 2.24, 3.11, 5.3, 5.4, 5.5, 5.6, 5., 5.8, 5.12, 5.13, 5.14, 5.15, 5.1, 5.18, 6.4, 6.25 Topics Covered: 1. The Nature of Energy- energy, work, kinetic energy, potential energy, Coulomb s Law, electrostatic potential energy, measurement of energy, joules, calories, system, surroundings, force, work, heat 2. The First Law of Thermodynamics energy diagrams, exothermic and endothermic reactions, temperature change, energy from foods and fuels, internal energy ( E), relating E to work and heat, exothermic, endothermic 3. Enthalpy & Enthalpies of Reaction enthalpy, pressure- volume work (P V), enthalpy of reaction ( H), thermochemical equation, enthalpy diagram, signs of H, relating heats to stoichiometry 4. Calorimetry and Hess s Law constant pressure calorimetry, calorimeter, heat capacity, molar heat capacity, specific heat capacity, calculating heats, heats added, subtracted like chemical equations 5. Enthalpies of Formation standard enthalpy of formation ( H f ), formation reaction, using H f to calculate enthalpies of reaction, enthalpy diagrams 6. Foods and Fuels combustion of natural gas, fossil fuels, petroleum, coal, sugars and fats, renewable energy sources. Spontaneous Processes spontaneous process, direction and extent of a reaction, reversible and irreversible processes 8. Entropy and the Second Law of Thermodynamics entropy (S), randomness, change in entropy ( S), S for phase changes, second law of thermodynamics 9. Molecular Interpretation of Entropy translational, vibrational and rotational energy, entropy and phase, third law of thermodynamics 10. Entropy Changes in Chemical Reactions standard molar entropies, entropy and temperature, molecular complexity 11. Gibbs Free Energy Free energy ( G), free energy and equilibrium, G = H - T S, standard free energy of formation 12. Free Energy, Temperature, and Equilibrium Constant temperature and spontaneous processes, phase changes, standard and nonstandard conditions, relationship between G and K s: Calorimetry Bond Energy Heats of Formation Free Energy Work, Equilibrium, and Free Energy Labs: Designing a Hand Warmer (Big Idea 5, Investigation 12, guided inquiry), 100 minutes (LO 3., 3.10, 4.1, 4.2; SP 1, 4, 5, 6) 1

18 Unit 4: Atomic Structure and Periodicity Chapters: 2 (sections 3, 4, 5), 6 (all), (all) Time Frame: 1.5 weeks Homework Sets Assigned: 3 s: 3 Number of Quizzes: 2 Number of Exams: 1 Big Ideas: 1 Enduring Understandings: 1B, 1C, 1D Learning Objectives: 1.5, 1.6, 1., 1.8, 1.9, 1.10, 1.12, 1.13 Topics Covered: 1. The Modern View of Atomic Structure atomic structure, atomic number, atomic mass, atomic weight, isotopes 2. The Periodic Table basic structure of the periodic table, periods, groups, metals/nonmetals/metalloids 3. Quantized Energy and Photons quantum, photoelectric effect 4. Quantum Mechanics, Atomic Orbitals, Representations of Orbitals quantum mechanical model, orbitals, electron shell, subshell, shell model, orbitals designated (s, p, d, f), relative energies, relative distance from the nucleus, probability distributions, electron density 5. Electron Configurations and the Periodic Table electron configuration, orbital diagram, core electrons, valence electrons, representative elements, transition elements, f- block elements 6. Effective Nuclear Charge effective nuclear charge, screening effect, valence electrons, inner core electrons, trends in effective nuclear charge. Size of Ions atomic radius, ionic radius, trends in atomic and ionic radii, isoelectronic series 8. Ionization Energy first ionization energy, successive ionization energies, trends in ionization energies, shells, subshells and trends, electron configurations of ions 9. Electron Affinities electron affinity as energy, trends, anomalies 10. Metals, Nonmetals, Metalloids metals, metallic character, metallic properties, nonmetals, nonmetal properties, metalloids, group trends s: Electron Configurations Advanced Periodic Trends Photoelectron Spectroscopy Labs: NONE 18

19 Unit 5: Bonding Chapters: 8 and 9 Time Frame: 3 weeks Homework Sets Assigned: 8 s: 5 Number of Quizzes: 2 Number of Exams: 1 Big Ideas: 1, 2, 5 Enduring Understandings: 1B, 2B, 2C, 2D, 5C, 5D Learning Objectives: 1.11, 2.1, 2.11, 2.13, 2.15, 2.16, 2.1, 2.18, 2.19, 2.20, 2.21, 2.22, 2.23, 5.1, 5.8 Topics Covered: 1. Lewis Symbols and the Octet Rule Lewis electron- dot symbols, octet rule 2. Ionic Bonding electron transfer, lattice energy, Coulomb s Law, s- and p- block electron configurations, transition metal ions 3. Covalent Bonding Lewis structures, multiple bonds 4. Bond Polarity and Electronegativity - bond polarity, polar and nonpolar bonds, electron density, polar molecules, dipoles, differentiating covalent and ionic bonding 5. Drawing Lewis Structures and Resonance determining Lewis structures, formal charge, resonance structures, delocalized electrons, depiction of resonance structures 6. Exceptions to the Octet Rule odd electrons, six electrons, expanded octets. Strengths of Covalent Bonds bond enthalpy, bond breaking, bond forming, calculations using bond enthalpies, bond lengths 8. Molecular Shape linear, bent, trigonal planar, tetrahedral, trigonal pyramidal, bond angles 9. The VSEPR Model valence shell electron pair repulsion, bonding pair, electron domain, nonbonding pair, molecular geometry, trigonal bipyramidal, see- saw, octahedral 10. Molecular Shape and Polarity bond dipole, polar molecules, electron densities in molecules 11. Hybrid Orbitals sp, sp 2, sp 3 hybridization, orbital overlap, multiple bonds, π and s bonds, delocalized electrons s: Molecular Geometry Types of Bonds Polar and Nonpolar Molecules Properties of Covalent Bonds Lattice Energy Labs: Qualitative Analysis and Chemical Bonding (Big Idea 2, Investigation 6, guided inquiry), 100 minutes (LO 2.11, 2.13, 2.15, 2.16, 2.19, 2.20, 2.22; SP 1, 4, ) Molecular Geometries of Covalent Molecules: Lewis Structures and the VSEPR Model (Traditional Lab from Chemistry: The Central Science.), 100 minutes (LO 2.21; SP 1, ) Models of Molecules (Traditional Lab adapted from Laboratory Experiments for World of Chemistry, Zumdahl, Zumdahl, and DeCoste), 50 minutes (LO 2.21; SP 1, ) 19

20 Unit 6: States of Matter and Intermolecular Forces Chapters: 10, 11, 12, 13 (only sections 1 4) Time Frame: 3 weeks Homework Sets Assigned: 4 s: 5 Number of Quizzes: 4 Number of Exams: 1 Big Ideas: 2, 5 Enduring Understandings: 2A, 2B, 2D, 5A, 5D Learning Objectives: 2.3, 2.4, 2.5, 2.6, 2., 2.8, 2.9, 2.10, 2.11, 2.12, 2.13, 2.14, 2.15, 2.16, 2.19, 2.20, 2.22, 2.23, 2.24, 2.25, 2.26, 2.2, 2.28, 2.29, 2.30, 2.31, 2.32, 5.2, 5.9, 5.10 Topics Covered: 1. The Gas Laws standard atmospheric pressure, atmospheres, torr, Boyle s Law (pressure- volume), Charles Law (temperature- volume), Boyle s law and Charles law plots, absolute zero, Avogadro s law, ideal gas, ideal- gas constant, calculations using ideal gas law, calculations of gas density, molar mass and volumes in chemical reactions 2. Gas Mixtures and Partial Pressures partial pressure, Dalton s law, water vapor pressure 3. The Kinetic- Molecular Theory of Gases Summary of KMT, molecular collisions, molecular origin of gas properties, molecular speed distributions (Maxwell- Boltzmann), temperature as average kinetic energy 4. Real Gases: Deviations From Ideal Behavior real vs. ideal gases, effect of intermolecular forces, structure of particles 5. A Molecular Comparison of Gases, Liquids, and Solids properties of the states of matter, particle explanations 6. Intermolecular Forces dispersion forces, polarizability, dipole- dipole forces, hydrogen bonding, ion- dipole forces, relative strengths of forces, explanation of molecular properties, solution formation. Select Properties of Liquids viscosity, surface tension, capillary action 8. Phase Changes energetics of phase changes, heat of fusion, heat of vaporization, heat of sublimation, heating curves, critical temperature and pressure 9. Vapor Pressure dynamic equilibrium, vapor pressure, volatility, distributions of kinetic energy, boiling point, vapor pressure plots 10. Classification and Structures of Solids metallic, ionic, covalent- network and molecular solids, atomic and molecular explanations, polymers, crystals, crystalline solids, amorphous solids 11. Metallic Solids metallic solids, alloys, substitutional and interstitial alloys, electron sea model, delocalized electrons, thermal and electrical conductivity, malleability and ductility 12. Ionic Solids ionic crystals, ionic interactions, atomic explanation of properties, brittleness, melting points, boiling points 13. Molecular Solids molecules, intermolecular forces, structural explanation of properties 14. Covalent- Network Solids diamond, graphite, semiconductors, doping, p- type, n- type, atomic explanations of properties s: Types of Solids Alloys Partial Pressures of Gases Deviations from the Ideal Gas Law Maxwell- Boltzmann Distributions Labs: Separation of a Dye Mixture Using Chromatography (Big Idea 2, Investigation 5, guided inquiry), 100 minutes (LO 2., 2.10, 2.13; SP 1, 4, 5, 6) 20

21 Unit : Rates of Chemical Reactions Chapters: 14 Time Frame: 2 weeks Homework Sets Assigned: 2 s: 2 Number of Quizzes: 1 Number of Exams: 1 Big Ideas: 3, 4, Enduring Understandings: 1D, 3A, 3B, 3C, 4A, 4B, 4C, 4D Learning Objectives: 1.16, 3.3, 3., 3.10, 4.1, 4.2, 4.3, 4.4, 4.5, 4.6, 4., 4.8, 4.9 Topics Covered: 1. Factors That Affect Reaction Rates effects of temperature, physical state, concentration, and catalysts 2. Reaction Rates reaction rate as change in concentration per time, graphical representations of rate, rate and stoichiometry 3. Concentration and Rate Laws initial rate, spectroscopic measurement of rates, rate law, rate constant, reaction order, rate constant units, method of initial rate 4. The Change of Concentration with Time integrated rate law, zeroth, first, and second order reactions, graphical representations, half- life, radioactive decay 5. Temperature and Rate the collision model, orientation factor, activation energy, activated complex, transition state, energy profile and reaction rate, graphical representations, Arrhenius equation (qualitative) 6. Reaction Mechanisms mechanisms, elementary reaction, unimolecular, bimolecular, and termolecular reactions, overall equation from elementary steps, intermediate, rate- determining step, mechanism and rate- determining step. Catalysis catalyst, homogeneous and heterogeneous catalysis, effect of catalyst on energy profile, surface catalyst, acid- base catalysts, enzymes, active site, substrate, lock- and- key model s: Rates of Reaction Method of Initial Rates Labs: Rate of Decomposition of Calcium Carbonate (Big Idea 4, Investigation 10, guided inquiry), 100 minutes (LO 3., 3.10, 4.1, 4.2; SP 1, 4, 5, 6) Kinetics of Crystal Violet Fading (Big Idea 4, Investigation 11, guided inquiry), 100 minutes (LO 1.16, 3.3, 4.1, 4.2; SP 1, 2, 4, 5, 6) 21