AP Chemistry Syllabus

Transcription

1 AP Chemistry Syllabus This course is designed to be an equivalent to a general chemistry course you would take in your first year of college. It is an advanced chemistry course that covers topics from the previous year in a more in depth manner and covers new topics that had not previously been covered. This course would prepare you for a second semester of college level chemistry if you choose, or are required, to take it. This course lasts for 2 semesters and will cover all topics required by AP College Board. A few topics include kinetics, equilibrium, thermodynamics, organic chemistry, and coordination chemistry. Towards the end of the spring semester, students have the option to take the AP Chemistry Exam, which will test the student s knowledge attained over the course. If a student passes this exam, they will receive college level credit for it. As we move closer to the exam date, we will take a larger look upon the exam as opposed to just chemistry topics. Student Goals: I have created my own goals for students in this course. They are seen below: Use an organizer or calendar to keep track of assignments and important dates. Work to become critical thinkers with a use of math skills and rhetoric. Read your chemistry textbook and laboratory manual before coming to class. Have a binder for AP Chemistry material where you can keep notes, past assignments, and a lab manual. Study the chemistry topics outside of class to gain and reinforce knowledge. Take the AP Chemistry exam in May and meet the minimum passing score for the exam ( score of 3 5). Leave this course with a better understanding of the world around us. Share your learned knowledge with others. Use a composition book to record all lab data. AP Chemistry Big Ideas: Big Idea 1: Structure of matter 1. Students will understand that the chemical elements are fundamental building blocks of matter. 2. Students will be able to fully understand the arrangement of atoms. 3. By doing laboratory experiments, the students will understand that atoms retain their identity in chemical reactions. Big Idea 2: Properties of matter characteristics, states, and forces of attraction 1. Students will understand that chemical and physical properties of materials exist. 1

2 2. Through extensive testing of elements, students will fully understand how each elements atoms are arranged, the chemical and physical properties of each element, as well as the forces that exist between and within each element. Big Idea 3: Chemical reactions 1. Through discussion and high level thinking, students will understand that the changes of matter involve the rearrangement and/or the reorganization of atoms as well as the transfer of electrons. Big Idea 4: Rates of chemical reactions 1. By completing several chemical reaction labs, the students will be able to see how rates of chemical reactions are determined by molecular collisions. Big Idea 5: Thermodynamics 1. Through an in depth lab and discussion, students will understand that the law of thermodynamics describe the essential role of energy. 2. The students will understand that the energy is what will drive changes of matter. Big Idea 6: Equilibrium 1. By watching and discussing demonstrations, students will understand that any bond or intermolecular attraction can be formed can be broken. What each student will need: Composition book (to keep all lab reports and to record laboratory data) Binder to keep track of all notes, handouts, and graded work Notebook ( that includes all notes taken in class) Zumdahl Chemistry textbook Laboratory safety goggles Calculator Lab Experience: In this course students must abide by any and all safety regulations. This includes wearing jeans, close toed shoes, and safety goggles for every laboratory exercise. At least 25% of this course will be lab activities as well as six (6) labs are guided inquiry labs as specified by the College Board. A specific format for each lab will be handed out before each lab activity. The lab along with the lab report will consist of: Pre Lab Work : Pre lab work is to be completed and turned in on the day the lab is performed. 1. Title 2. Date 3. Purpose: A purpose is a statement summarizing the lab. 4. Procedure Outline: Students need to write an outline of the procedure. 2

3 Note: If a student is doing a guided inquiry lab, they might have to write a full procedure that they develop. 5. Pre Lab Questions: Students will be given some questions to answer before the lab is started. 6. Data Tables: Students will need to create any data tables or charts necessary for data collection in the lab. 7. Data: Students need to record all their data directly in the appropriate notebook. 8. Calculations and Graphs: Students should show how calculations are carried out. 9. Conclusions: This portion of the lab should be thought out and written clearly. 10. Post Lab and Error Analysis Questions: The students will be given questions to answer after the lab is completed. Course Requirements and Grading: I will cover each chapter within the Zumdahl textbook every five to thirteen days. Each chapter has a set of problems assigned that will be completed and graded. Exams will consist of multiple choice questions and essay questions. Exams will be given at the end of each quarter. Students can correct their exams for ½ points back. Throughout the school year, i will provide practice AP exams for the students to complete. They will be graded and placed in the homework category. Labs will be completed within each chapter and a report will be due after the lab. You will use information accumulated in your composition book for guidance in writing the lab report. I will provide a template for how to write a lab report. All late work will receive a 10% reduction penalty each day and no credit will be given after the third day late. The student s final grades will be weighted using the following proportions: Homework: 20% Quizzes: 20% Labs/Reports: 30% Exams: 30% Required Texts: Chemistry by Zumdahl and Zumdahl, 7th ed., Houghton Mifflin Company, 2008 ISBN: ISBN 13: Lab Manual: Rather than using a single lab manual, we will use labs from a collection of lab manuals: Drake, Sheryl and Merli, Chris. Chemistry 106: Lab Manual. Eastern Illinois University Department of Chemistry. Eastern Illinois University, Charleston, IL. 3

4 Chemistry 1040: World of Chemistry. Eastern Illinois University Department of Chemistry. Eastern Illinois University, Charleston, IL. Chemistry: The Laboratory Eastern Illinois University Department of Chemistry. Eastern Illinois University, Charleston, IL. Chemistry: The Laboratory Sonnichsen, Laura B. Parkland College Department of Natural Sciences. Organic Chemistry I Laboratory (Chemistry 204). Course Schedule: Chapter 1: Chemical Foundations (1 week) Scientific method Units of measurement and conversions Significant figures Temperature and density 1) Use and apply the steps to the scientific method. 2) Apply knowledge of significant figures to laboratory work. 3) Successfully convert between units of temperature, mass, and length. 4) Classify matter and observe physical and chemical changes to occur. Experiment: 1) Laboratory Tools Students will know and understand the types of glassware and equipment we will be using throughout the course. Science Practice: 7 Chapter 2: Atoms, Molecules, and Ions (1.5 weeks) Dalton s atomic theory Atomic structure Empirical and molecular formulas Chemical equations and balancing Stoichiometry Limiting reactants and percent yields 1) Calculate the number of grams, moles, and atoms present in a substance. 2) Find the percent by mass of an atom in a compound. 3) Determine the empirical and molecular formulas of a compound. 4) Balance a chemical equation using coefficients. 4

5 5) Find the mass of a substance created during a chemical reaction, using a mole ratio. 6) Determine which reactant in a chemical reaction limits the reaction and what percentage of product is produced/expected. 7) Students will complete Finding the Ratio of Moles of Reactants in a Chemical Reaction Experiment: 1) Guided inquiry: Percent Copper in Copper (II) Oxide Students will be able to read and understand MSDS sheets as well as calculate the percent yield of copper. 2, 3, 4, and 5 2) Guided I nquiry: Synthesis and Characterization of AcetyLsalicylic Acid (aspirin) Students will be able to explain Organic Synthesis as well as to describe and explain differences in the properties of acetylsalicylic acid and salicylic acid by a simple chemical test. 2, 3, 5, and 6 Chapter 3: Stoichiometry (1.5 weeks) Moles, Molar mass Percent composition Empirical and molecular formulas Balancing equations Stoichiometry. Experiment 1: Percent Copper (II) Oxide 1, 2, 4, 5, 6, and 7 Experiment 2: Synthesis and Characterization of Acetylsalicylic acid 2, 3, 5, and 7 Chapter 4: Types of Chemical Reactions and Solution in Stoichiometry (2 weeks) Water Solution terminology Types of chemical reactions (DD, SR, S, D, C, AB, R) Precipitation 1) Describe the uniqueness of water and its role as a solvent. 2) Define the terms associated with solutions. 3) Calculate the strength of an acid or base. 5

6 4) Calculate the final molarity and volume of a substance when they mixed. 5) Determine what type of reaction is occurring, when provided with a chemical equation. 6) Determine if compounds are soluble in water. 7) Assign oxidation states to atoms in a compound of ion. 8) Understand how the oxidation states of atoms change in a redox reaction. Experiment: 1) Synthesis of Zinc Iodide and Matter Conservation By completing this lab experience, students will be able to determine the chemical formula, reconfirm the Conservation of Mass, and determine the element composition of the compound. 1, 2, 4, 5, 6, and 7 2) Solution Stoichiometry: Acid Base Titration Students will be able to : a) To determine the concentration of the given hydrochloric acid solution using acid base titration method. b) To determine the moles of hydrochloric acid in 100 ml of the solution. 2, 3, 5, and 7 Chapter 7: Atomic Structure and Periodicity (2 weeks) The Bohr model Quantum numbers Orbital rules (Aufbau, Pauli Exclusion, etc) Electron configuration Periodic trends (AR, EA, IE, IR, EN) Students will be able to : 1) Name the 7 types of electromagnetic radiation and draw/label the parts of a wave. 2) Explain and sketch the structure of an atom as designed by Bohr. 3) Calculate the 3 types of quantum numbers. 4) Write the ground state and valence electron configuration of an element according to the Pauli Exclusion Principle, Aufbau Principle, Hund s RUles, and electron spin quantum number. 5) Name how periodic trends occur on the periodic table and why they occur. Experiment: 1) The Color of Cations The students will be able to: a) Perform flame tests of metal cations in order to observe their characteristic colors. b) Match the flame colors observed to an appropriate wavelength of visible light, and then perform calculations to determine the frequency and energy of the emitted photons. c) Relate these results to the types of electronic transitions occurring in these elements. 1, 3, 6, and 7 6

7 Chapter 8 Bonding: General Concepts (1.5 weeks) Types of chemical bonds Polarity and dipole moments Ionic and covalent bonds Lewis structures and resonance The octet rule VSEPR model 1) Determine which type of bond occurs within a molecule or compound. 2) Use electronegativity values to calculate polarity and dipole moments. 3) Draw the Lewis structure of a molecule/ compound and appropriate resonance structures. 4) Check validity of a Lewis/resonance structure according to the octet rule. 5) Use the VSEPR model to predict molecular geometry. Experiment: 1) VSEPR Structure and Shape of Molecules 1)Learn how to draw Lewis structures for atoms which violate the octet rule. 2) Learn how to use Lewis structures and VSEPR and to predict the shapes of molecules. 3) Learn how to use the shape of a molecule to predict whether or not it is polar. 1, 3, and 7 Chapter 9: Covalent Bonding: Orbitals (1.5 weeks) Hybridization The molecular orbital model Bonding in diatomic molecules 1) Determine the appropriate hybridization of a molecule. 2) Graph the molecular orbital model of a molecule with bonding and antibonding orbitals. 3) Label multiple bonds as sigma or pi bonds. Experiment: 1) Chemical Bonding Polar and Nonpolar Students will be able to identify the two types of covalent bonds as well as understand the interaction of various solvents and solutes related to the specific characteristics of their bonds. 1, 3, 4, 5, and 6 7

8 Chapter 10: Liquids and Solids (1.5 weeks) Intermolecular forces Structures and types of solids Vapor pressures and changes of state Phase diagrams 1) Describe the types of intermolecular forces and apply them to different molecules. 2) Describe the structure of a solid using crystal lattice and discuss the structure of metals. 3) Understand the networking of solids. 4) Recreate a phase diagram using changes of states of a molecule. Experiment: 1) Vapor Pressure and Heat of Vaporization 1) Measure the pressure inside a sealed vessel containing a volatile liquid over a range of temperatures. 2) Determine the relationship between pressure and temperature of the volatile liquid. 3) Calculate the heat of vaporization of the liquid. 2, 3, 4, 5, 6, and 7 Chapter 19: The Prepresentative Elements: Groups 1A Through 4A (1 week) Hydrogen Group 1A elements Group 2A elements Group 3A elements Group 4A elements 1) Recognize the types of compounds formed from group 1A elements. 2) Describe the unique properties of hydrogen as a group 1A elements. 3) Describe the properties of group 2A elements. 4) Describe the properties of group 3A elements. 5) Describe the properties of group 4A elements. Experiment: 1) Demonstrations Science Practice: 7 Chapter 20: The Representative Elements: Groups 5A Through 8A (1 week) Group 5A elements (with nitrogen and phosphorous) Group 6A elements (with oxygen and sulfur). Group 7A elements Group 8A elements 8

9 1) Describe the properties of group 5A elements (specifically nitrogen and phosphorous). 2) Describe the properties of group 6A elements (specifically oxygen and sulfur). 3) Describe the properties of group 7A elements. 4) Describe the properties of group 8A elements. Experiment: 1) Demonstrations Science Practice: 7 Chapter 5: Gases (2 weeks) Gas laws (Boyle's, Charles, Avogadro, and Ideal) Gas stoichiometry Dalton s law of partial pressures Real gases 1) Identify and distinguish between the major gas contributions of scientists (Boyle, Charles, Avogadro, and Ideal) 2) Calculate the specifics of a gas using the ideal gas law and gas stoichiometry. 3) Calculate the partial pressures of different gases using Dalton s law of partial pressures. 4) Use the kinetic molecular theory to explain the properties of an ideal gas. 5) Identify between a real gas and an ideal gas. 6) Recall how gases are responsible for geologic pollution. 7) Complete the experiment, Molecular Mass of a Volatile Liquid. Experiment: 1) Determination of the Gas Constant and Molar Volume of a Gas 1) To experimentally determine the value of the gas constant, R. 2) To experimentally determine the volume of one mole of a gas at standard temperature and pressure. 2,3, 4, 5, 6, and 7 Chapter 21: Transition Metals and Coordination Chemistry (1 week) The transition metals Coordination compounds ( and compounds) Isomers Crystal field model 1) Locate and explain the diverse properties of the transition metals. 9

10 2) Construct the appearance of a coordination compound and name it. 3) Draw coordination compounds as different isomers (specifically structural isomers and stereoisomers). 4) Label a coordination compound as being chiral or not. 5) Identify between strong/weak field ligands. 6) Recognize biological uses of transitional metals in the human body. Experiment: 1) The Chemistry of Transition Metal Students will understand the chemistry of transition metals chromium, manganese, iron, and cobalt by observing reactions involving oxidation states. 1, 2, 3, 4, 5, 6, and 7 Chapter 11: Properties of Solutions (2 weeks) Solubility Vapor pressures Boiling point elevation Freezing point depression Osmotic pressures Colligative properties 1) Calculate the molarity, mass percent, mole fraction and molality of atoms in solution. 2) Understand the mechanisms for creating a solution. 3) Apply the laws of vapor pressure to realistic uses. 4) Compare the mechanisms for boil point elevation and freezing point depression. Experiment: 1) Solution Reactions: Identifying the Contents of Seven Bottles Students will: 1) Become familiar with applying the solubility rules to predict whether a precipitate forms. 2) Become familiar with other common reactions that involve the evolution of gases as a product. 3) Obtain exposure to deductive reasoning as a scientific approach. 1, 3, 5, 6, and 7 Chapter 14: Acids and Bases (2.5 weeks) Arrhenius, Lewis, Bronsted Lowry acid/base theories The ph scale Bases Polyprotic acids 10

11 1) Identify between the Arrhenius, Bronsted Lowry and Lewis theories of labeling acids and bases. 2) Relate acid/base strength to the ph scale. 3) Describe the amphoteric nature of water. 4) Use a logarithmic scale to calculate the ph and Kₐ values of acid solutions. 5) Identify common acids/bases used or found in everyday life. 6) Use an ICE diagram to calculate the ph of solutions. Experiment: 1) The Neutralizers: An Investigation of Common Acids & Bases, Natural Indicators, and Antacids. 1)Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II. 2)Predict products of an acid base neutralization 3)Describe tests that can be used to distinguish an acid from a base. Classify various solutions as acidic or basic, given their ph 4) Identify the Bronsted Lowry conjugate acid base pairs in an equation. 1, 2, 3, 4, 5, 6, and 7 2) Acids, Bases, and Buffer Solutions 1. understand conjugate acid base pairs and equilibria of weak acids and bases 2. perform calculations involving ionic equilibria 3. understand the components of buffer solutions and how they work to resist changes in ph 2, 3, 5, 6, and 7 Chapter 15: Applications of Aqueous Equilibria (1.5 weeks) Acids/Bases ions Buffers Titrations ph curves Indicators Students should be able to: 1) Determine how common ions affect a system of equilibrium. 11

12 2) Create a buffer and use it to resist a change in the ph of a solution. 3) Design and graph a ph curve from an acid/ base titration. 4) Describe the use and purpose of using an acid/base indicator. Experiment: 1) Buffer Solutions Students will be able to relate different types of buffer components. 2, 3, 4, 5, 6, and 7 Chapter 12: Chemical Kinetics (2.5 weeks) Reaction rates Rate laws Reaction mechanisms Catalysis 1) Determine the rate of which a reaction will occur. 2) Determine the rate law for a reaction and label it as a first or second order rate law. 3) Follow the individual steps that a reaction occurs at. Experiment: 1) Chemical Kinetics Students will determine the rate law for the reaction between bleach and two dyes, as well as, determine the rate constant for the same reaction. 2, 3, 4, 5, 6, and 7 Chapter 13: Chemical Equilibrium (2 weeks) Equilibrium constants Equilibrium with pressure Le Chatelier s Principle 1) Use the equilibrium expression to find the equilibrium constant of a reaction. 2) Use an ICE diagram to calculate the equilibrium concentrations of species in a reaction. 3) Determine how Le Chatelier s Principle is used to predict changes on a system of equilibrium. Experiment: 1) Chemical Equilibrium Students will be able to see that chemical reactions reach a state of equilibrium and then determine factors that can disturb the equilibria. 2, 3, 4, 5, and 6 12

13 Chapter 6: Thermochemistry (2 weeks) Enthalpy Calorimetry Hess s Law Standard enthalpy of formation 1) Distinguish between properties of endothermic and exothermic reactions. 2) Use a homemade calorimeter to calculate the amount of heat given off by an ignited substance. 3) Use Hess s Law to calculate the expected heat change during a chemical reaction. 4) Calculate the required amount of energy in order for a substance to be formed. 5) Determine how the greenhouse effect is cause by the burning of carbon based molecules. Experiment: 1) Chemical Equations: Energy Relationships Students will explore energy changes during chemical reactions, heat of reaction, and the connection between energy changes and chemical changes. 1, 2, 3, 4, 5, 6, and 7 Chapter 16: Spontaneity, Entropy, and Free Energy (1.5 weeks) Entropy The laws of thermodynamics Free energy Entropy in chemical reactions 1) Determine whether a reaction is a spontaneous or nonspontaneous process. 2) Discuss how entropy plays a role in the law of thermodynamics. 3) Calculate the free energy present in a reaction. Experiment: 1) Guided inquiry: Simultaneous Determination of Several Thermodynamic Quantities Students will study a system of soluble salt in water. From the solubility information at various temperatures, a variety of other thermodynamic quantities can be determined for the system. 1, 2, 3, 5, 6, and 7 Chapter 17: Electrochemistry (1.5 weeks) Galvanic cells Standard reduction potential Batteries and corrosion Electrolysis 13

14 1) Break down a redox reaction into half reactions. 2) Sketch a galvanic cell and use one to determine the cell potential of two metals. 3) Locate the correct value of standard reduction potential for a half reaction and use it to predict the voltage provided by a galvanic cell. 4) Use line notation to write the reaction completed with a galvanic cell. 5) Recognize what changes may affect the cell potential of a galvanic cell. Experiment: 1) Electrolysis Students will be able to see how to split water molecules and be able to explore the variables that affect the rate of hydrogen gas formation. 2, 3, 4, 5, and 7 Chapter 22: Organic and BIological Molecules (1.5 weeks) Alkanes, alkenes, and alkynes Aromatic hydrocarbons Polymers 1) Name and sketch the structure of straight lined carbon based molecules. 2) Distinguish the properties between Straight lined carbon based molecules via single, double, and triple bonds. 3) Reproduce the mechanism for a reaction involving alkanes, alkenes, and alkynes. 4) Analyze the properties of aromatic carbon chains. 5) Distinguish between the different common carbon based functional groups. 6) Describe the biological function of carbon based molecules. Experiment: 1) Isolation of Caffeine from Tea Students will be able to extract the caffeine from the tea powder through polar and nonpolar solvent technique. 2, 3, 4, 5, and 6 Chapter 18: The Nucleus: A Chemist's View (0.5 weeks) Radioactive decay Kinetics of radioactive decay Nuclear fusion and fission Effects of radiation 1) Distinguish between fission and fusion. 2) Fill in the appropriate values and elements involved in the radioactive decay of an element. 14

15 3) Understand the kinetics associated with nuclear decay and the nuclear transformation of one element or another. 4) Understand the methods of radioactive and carbon dating. 5) Determine the effect of radiation on the environment consider events that occurred in Hiroshima, Three Mile Island and Chernobyl. Experiment: 1) Testing For the Existence of Radon Students will become aware that radon goes through groundwater and can escape through daily household activities. They will know how to use and understand the test kit. 3, 4, 6, and 7 Topic Assignments Other materials Lab(s) and Science Practices Important Topics Chapter 1: Chemical Foundations #2, 5, 10 11, 16, 18, 21, 24 26, 28, 30 39, 41, 43 47, 49 52, 57 61, 65 66, 70, 74, 76 77, 84, 87, 92 Draw a model of the steps of the scientific method Laboratory tools Science Practice : 7 The scientific method, conversions, significant figures, temperature, and density. Chapter 2: Atoms, Molecules and Ions #11 13, 16 17, 19, 22, 24, 33, 40, 43 46, 49 50, , 60, 62, 64, 66, 68, 70, 80, 83 In textbook, Atoms, Molecules, and Ions Section 2.8 Students practice balancing equations, identify mole ratios, and limiting reactants of ionic and covalent compounds. Measurement: Physical Properties Finding the Ratio of Moles of Reactants in a Chemical Reaction 2, 3, 4, 5, and 6 Dalton s laws, nomenclature, and atomic structure. Chapter 3: Stoichiometry #7, 13, 18, In small groups, students us a Job s plot to Percent Copper (II) Oxide Moles, molar mass, percent composition, 15

16 21, 28, 30, 34, 36, 39 40, 52, 56, 60, 62, 64, 67 68, 70, 74, 76, 80, 84, 86, 90, 92, 94, 96, 98, 100 determine the stoichiometric relationship between different reactions. Science Practices:1, 2, 4, 5, 6, and 7 Synthesis and Characterization of Acetylsalicylic acid empirical and molecular formulas, balancing equations, and stoichiometry. 2, 3, 5, and 7 Chapter 4: Types of Chemical Reactions and Solution Stoichiometry #5, 10, 13, 16, 18, 22, 24, 28, 30, 34, 36, 38, 44, 48, 56, 60, 70, 74, 76, 80, 88, 106, 112 Synthesis of Zinc Iodide and Matter Conservation 1, 2, 4, 5, 6, and 7 Solution Stoichiometry: Acid Base titration Water, solutions, reaction types, and solution stoichiometry. 2, 3, 5, and 7 Chapter 7: Atomic Structure and Periodicity #5, 14, 16, 20, 24, 32, 60, 66, 68, 70, 72, 82, 86, 90, 94, 104, 106, , 124 Complete a web based research paper based on Microwaves and Waves on a String. Students will read Atomic Structure and the Periodic Table The colors of Cations 1, 3, 6, and 7 Quantum numbers, electron configuration, and periodic trends Chapter 8: Bonding General Concepts #1, 6 8, 11, 24, 26, 30, Students will create visual representations of ionic substances VSEPR Structure and Shape of Molecules Bonding types, polarity, dipole 16

17 34, 36, 38, 40, 42, 46, 68, 70, 72, 76, 78, 81, 92, 94, 96, 98, 100, 102, 126, 131 that connect microscopic to macroscopic structures. 1, 3, and 7 moments, Lewis structures, and the octet rule Chapter 9: Covalent Bonding Orbitals #1, 5, 10, 16, 18, 22, 28, 34, 36, 44, 56, 60 Students will create a model of a covalent bond that shows the structures and explain the difference between covalent and ionic bonds. Chemical Bonding Polar and Nonpolar 1, 3, 4, 5, and 6 Hybridization Chapter 10: Liquids and Solids #1, 14, 17, 20, 24, 36 37, 68 69, 72, 74, 110 Students will use models to understand the differences between liquids and liquids. They will read in the textbook. Vapor Pressure and Heat of Vaporization 2, 3, 4, 5, 6, and 7 Intermolecular forces and phase diagrams Chapter 19: Groups 1A 4A #2, 4, 6 7, 11 12, 14 19, 21 24, 31 34, 36, 40, 42, 44, 46, 48, 52, 54, 60, 63, 68, 81 Demonstrations Science Practice: 7 Hydrogen and group trends Chapter 20: Groups 5A 8A #1 3, 8, 10 14, 22, 25 26, 31 33, 38 39, 44, 52, 61 62, 75 Demonstrations Science Practice: 7 Group trends Chapter 5: Students are Gas laws, gas 17

18 Gases #6, 9, 17, 28, 34, 36, 38, 42, 56, 66, 78, 82, 84, 89 90, 94 asked to propose a model of a gas from the lab and class discussion. As a class we discuss gas properties and the students must complete a report. Determination of the Gas Constant and Molar Volume of a Gas Molecular Mass of a Volatile Liquid 2, 3, 4, 5, 6, and 7 stoichiometry, and partial pressures. Chapter 21: Transition Metals and Coordination Chemistry #2 3, 5, 11 18, 24, 25, 29 36, 39, 43, 45, 56, 59, 65 The Chemistry of Transition Metals Science Practices: 1, 2, 3, 4, 5, 6, and 7 Transition metals and coordination compounds Chapter 11: Properties of Solutions #6, 9, 10, 12, 25, 30, 37, 38, 57, 58, 70 Solution Reactions: Identifying the Contents of Seven Bottles Science Solutions, colligative properties, boiling point, and freezing point Practices: 1, 3, 5, 6, and 7 Chapter 14: Acids and Bases #2, 5, 13 15, 35, 27 31, 36 38, 44, 46, 48, 52, 58, 62, 72, 74, 78, 90, 94, 98, 106, 113, 118, 120, 122 Students will develop definitions and representations of acids and bases by deriving the equations that relate ph, etc. Students will define weak acids and bases and draw their molecular structures and explain the The Neutralizers: An Investigation of Common Acids and Bases, Natural Indicators, and Antacids Science Practices: 1, 2, 3, 4, 5, 6, and 7 Acids, Bases, and Buffer Solutions ph scale, acids, bases, and types of acid/base theory 18

19 strengths. 2, 3, 5, 6, and 7 Chapter 15: Applications of Aqueous Equilibria #1, 7, 10, 16, 18, 20, 22, 24, 28, 30, 32, 42, 54, 56, 62, 70, 76, 78, 86, 96, 104, 104 Students will read in chapter 15 and then prepare an NaOH solution to determine the concentration through titration. Buffer Solutions 2, 3, 4, 5, 6, and 7 Buffers, titrations, indicators, and titration curves Chapter 12: Chemical Kinetics #4, 7, 8, 11, 19, 24 26, 35, 49 Students will be able to explain how a graph shows zero, first, and second order kinetics. Also, they must show a graph of kinetics in: Amount versus Time Log(Amount) versus Time 1/Amount versus TIme Chemical Kinetics 2, 3, 4, 5, 6, and 7 Reaction rates, rate laws, and catalysis Chapter 13: Chemical Equilibrium #13, 17, 18, 20, 22, 33, 34, 52, 58, 60, 68, 72 Webinar Dueling Aquariums: An Equilibrium Demonstration Also, Salts and Solubility Chemical Equilibrium 2, 3, 4, 5, and 6 Equilibria, Le Chatelier s Principle Chapter 6: Thermochemis try #4, 11, 12, 18, 21, 22, 34, 36, 38, 42, 44, 56, 60, 62, 67, 72 Students will read then we will discuss the different heat capacities of reactions. Students will determine the heat of reactions. Chemical Equations: Energy Relationships 1, 2, 3, 4, 5, 6, and 7 Enthalpy, calorimetry, and Hess s Law 19

20 Chapter 16: Spontaneity, Entropy, and Free Energy #2, 4, 14, 19, 20, 24, 27, 28, 33, 34, 37, 38, 43 Students will read and then the students discuss qualitatively the two tendencies in nature. 1. The loss of energy 2. Tendency to go toward more disorder Simultaneous Determination of Several Thermodynamic Quantities 1, 2, 3, 5, 6, and 7 Entropy, free energy, and thermodynami cs Chapter 17: Electrochemist ry #1, 2, 13 16, 21, 26, 28, 30 32, 34, 40, 48, 51, 66, 74, 79, 111 Students will complete several redox reactions and justify them in terms of electron transfer. Electrolysis 2, 3, 4, 5, and 7 Galvanic cells and cell potential Chapter 22: Organic and Biological Molecules #2 4, 8, 9, 13 29, 31, 35, 36, 43, 44, 47, 48, 52, 55, 56, 61, 66, 68, 71, 83, 85, 100, 105, 114, 131, Isolation of Caffeine from Tea 2, 3, 4, 5, and 6 Organic properties and nomenclature Chapter 18: The Nucleus A Chemist s View #2, 4, 11, 12, 14, 19 21, 23, 35, 38, 42, 46, Testing for the Existence of Radon 3, 4, 6, and 7 Radioactive decay, fusion, fission, and radiation. 20