The Table of Contents

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The Table of Contents

AP CHEMISTRY COURSE SYLLABUS

THE TABLE OF CONTENTS

Page CONTENT

1. Table of Contents 2. Course Guidelines 3. Lab Report Requirements 5. Sample Rubric for Lab Reports 6.27. Course Topic Outline AP Chemistry Course Guidelines

Primary Text:

General Chemistry by Ebbing and Gammon, 9th Ed. Houghton Mifflin Company, 2009

ISBN: 0-618-93038-8

Primary Lab Manual:

Experiments for Advanced Placement Chemistry by Sally Ann Vonderbrink, Flinn Scientific, Inc. 2001 and Experiments in General Chemistry, R.A.D. Wentworth, Houghton Mifflin Company, 2009

Total Allotment of Time for Lab:

This course has 33 labs. Each lab takes approximately sixty to ninety minutes. This is a minimum of 2000 minutes in lab up to a maximum of 3000 minutes in lab per student.

Lab Requirements and Grading:

Students are required to keep and maintain a lab composition book. Students must work together to gain data for the lab. They must work collaboratively to complete the analysis and conclusions. Often, each group will be asked to report their data to the rest of the class so that all data analysis can be completed. The book is graded by rubric every quarter and counts as 25% of the total grade. Tests are 40%, quizzes 20% and homework the remaining 15%. The requirements of the lab notebook are on the following pages. A sample rubric for one of the labs is also included.

Other Source Material:

The Ultimate Chemical Equations Handbook by George Hague Jr. and Jane D. Smith, Flinn Scientific, Inc. 2001

A Demo A Day Vol. I and II by George R. Gross, B. Bilash II and John Koob, Flinn Scientific, Inc. 1995

Chemical Demonstrations: A Sourcebook for Teachers Vol I and II by Lee Summerlin, Christie L. Borgford, and Julie B. Ealy, The American Chemical Society 1988 Hands-On Chemistry Activities with Real-Life Applications. By Norman Herr and James Cunningham. The Center For Applied Research in Education, 1999.

Course Objectives and Philosophy:

 Students will acquire problem solving skills that will be needed to succeed in an advanced level chemistry course as well as in a technological society. They will learn how to critically think about the pressing social issues from a chemical and scientific viewpoint.  Students will acquire the course content of a first year college chemistry program with a mathematical emphasis.  Students will work in the laboratory to attain skills such as lab report writing and analysis. They will learn to work together as a team to solve problems. They will become acquainted with general equipment, chemicals and procedures. Lab Notebook Requirements

Source - Laboratory Experiments for Advanced Placement Chemistry by Sally Ann Vonderbrink, Flinn Scientific, Inc. 2001

The Laboratory Notebook

A laboratory notebook will be used to explain laboratory procedures, record all laboratory data, show how calculations are made, discuss the results of an experiment, and to explain the theories involved. A record of laboratory work is an important document which will show the quality of the laboratory work that you have done. You may need to show your notebook to the Chemistry Department at a college or university in order to obtain credit for the laboratory part of your Advanced Placement Chemistry course. As you record information in your notebook, keep in mind that someone who is unfamiliar with your work may be using this notebook to evaluate your laboratory experience in chemistry. When you explain your work, list your data, calculate values and answer questions, be sure that the meaning will be obvious to anyone who reads your notebook.

Procedure 1. Use a book with pages fastened in place. 2. Write your name and class on the front cover and inside the front cover. 3. In ink, number all the right-hand pages on the lower right corner if they are not already numbered. If you are left-handed, you may use the left pages instead of the right if you wish. 4. Save the first two pages for a Table of Contents. This should be kept current as you proceed. Each time you write up a lab, place the title and page number where the lab report begins in the Table of Contents. 5. Write in ink. Use only the right hand pages. You may use the left- hand pages for preliminary notes, pictures or for a quick graph. The left- hand pages will not be graded. 6. If you make a mistake DO NOT ERASE. Just draw ONE LINE through your error, and continue. It is expected that some errors will occur. You cannot produce a perfect, error-free notebook. Errors should be corrected by drawing one line through the mistake, and then proceeding with the new data. 7. Do not use the first person or include personal comments. Laboratory Reports Include the following information in your laboratory reports: 1. Title The title should be descriptive. Experiment 5 is not a descriptive title. 2. Date This is the date (or dates) you performed the experiment. 3. Purpose A brief statement of what you are attempting to do. 4. Procedure A one or two sentence description of the method you are using. You may refer to the lab manual for specific instructions, but you should include a brief statement of the method. Do not include lengthy, detailed directions. A person who understands chemistry should be able to read this section and know what you are doing. For every lab, on the left hand side, draw a pictorial of the lab procedure. This will help you to visualize the lab process prior to lab. 5. Data Record all your data directly in your lab notebook on the right-hand pages. Organize your data in a neat, orderly form. Label all data very clearly. Use correct significant digits, and always include proper units (g, mL, etc.). Underline, use capital letters, or use any device you choose to help organize this section well. Space things out—don't try to cram everything on one page. Use tables where appropriate. Tables need a descriptive title. This is the end of the section that will be needed for prelab. Prelab will be checked prior to lab on lab day. 10% off of the report for no prelab and you will not begin with other students until it is done. 6. Calculations and Graphs You should show how calculations are carried out. Give the equation used and show how your values are substituted into it. Give the calculated values. If graphs are included, make the graphs an appropriate size. Label all axes and give each graph a title. See the section on graphing. If experiments are not quantitative, this section may be omitted. Graphs should be done on a computer and cut and paste into the lab notebook.

7. Conclusions Make a simple statement concerning what you can conclude from the experiment. 8. Discussion of Theory In this section you should include such information as: What theory was demonstrated in this experiment? What do the calculations show? How was the purpose of the experiment fulfilled? Why does (or doesn't) the experiment work? Refer back to the purpose of the lab to write this section. Report the values you obtained in this section. 9. Experimental Sources of Error What are some specific sources of error, and how do they influence the data? Do they make the values obtained larger or smaller than they should be? Which measurement was the least precise? Instrumental error and human error exist in all experiments, and should not be mentioned as a source of error unless they cause a significant fault. Significant digits and mistakes in calculations are NOT a valid source of error. In writing this section it is sometimes helpful to ask yourself what you would do differently if you were to repeat the experiment and wanted to obtain better precision. If you can calculate a percent error or percent deviation, do so and include it in this section. 10.Questions Answer any questions included in the lab directions. Answer in such a way that the meaning of the question is obvious from your answer. Sample Rubric for Lab Report Grading:

Taken from Unit Three – Stoichiometry

Percent Yield Lab Rubric

This lab report is due at the end of this class period. Remember to work as a group but to still make sure your work is authentic. This rubric must be attached to the final copy. Grading is as follows:

PRE LAB: Drawing, title, purpose, procedure and data tables are complete. _____ 5pts

DATA: Tables are complete with units, sig figs _____ 5pts

DATA ANALYSIS: Write a balanced equation for the lab _____ 2pts

What is the solid product formed in this reaction? Use observations to verify. _____ 2pts

Questions 1-5 Units, sig figs, set up _____ 5pts

RESULTS AND CONCLUSIONS: A paragraph summarizing the purpose of the lab, the theory of the lab, the values you obtained, the error you experienced and how it specifically effected your results. _____ 10pts

Questions 1-3 _____ 3pts Calculate a percent yield for this experiment _____ 2pts

TOTAL _____ 34pts Course Topic Outline For each unit the students are provided with a list of unit objectives and assignments. These have been highlighted in the pages that follow.

Chapter One – Matter and Measurement (1.5-2 weeks)

Objectives – Students will be asked to….

1. Explain the definition of chemistry 2. Demonstrate an understanding of the process and stages of scientific (logical) problem solving. i.e. scientific method 3. List and describe the three states of matter, their general properties, and the methods for their phase changes. 4. Apply and recall definitions for physical and chemical change as well as for physical properties and chemical properties 5. Know the difference between elements, mixtures and compounds including the difference between heterogeneous and homogeneous mixtures 6. Know and apply the term phase to mixtures 7. Explain the methods of separation for mixtures and compounds as well as some of the techniques used to separate them. 8. Explain and be able to use scientific notation (standard form) 9. Identify and use SI units and prefixes 10. Be able to perform calculations and demonstrate an understanding of how to convert between units using unit analysis/factor label method/conversions/dimensional analysis 11. Explain the concept of derived units and use relationships relating to density 12. Explain the meaning of uncertainty and demonstrate an understanding of how to use the rules for determining significant figures and rounding 13. Explain the differences between, and be able to apply the concepts of accuracy, precision, and percent error. 14. Explain and be able to use, the formulas for the conversions of the three different temperature units

Chapter One – Laboratory Requirements: All student based – hands on

1) Safety and Equipment Lab – a lab that familiarizes students with basic lab safety and equipment usage and identification. 2) Accuracy and Precision Measurement Lab – a lab that allows students to make multiple measurements with known values to measure the accuracy and precision of their measurements. 3) Density of Liquids Lab – a lab that has students measure the density of several liquids. They analyze the results for accuracy and then are asked to identify an unknown. Chapter One – Major Assignments:

1) Reading – Ch. 1 2) Homework Sets – Ch. 1/Two Sets 3) Significant figures, accuracy, and precision worksheet 4) Quizzes – Unit Analysis 5) Test – Over all unit objectives Chapter Two – Atoms, Molecules and Ions (1.5 Weeks)

Objectives – Students will be asked to….

1. Briefly comment on the history of atomic theory 2. Outline the four main aspects of Dalton's atomic theory 3. Recall some of the experiments that led to the identification of sub-atomic particles 4. Describe the three particles that make up the atom and their relative charges, masses and positions in the atom 5. Show how to use the atomic number and mass number of an isotope to calculate the numbers of protons, neutrons and electrons present 6. Identify and be able to write an element’s symbol, including charge, mass number and atomic number for the element. 7. Explain what the term isotope means and be able to perform simple calculations relating to isotope data such as percent abundance problems. 8. Label the approximate locations of metals, non-metals and metalloids on the periodic table 9. Explain what groups, periods and families are on the periodic table 10. Describe the meaning of the terms molecule and ion 11. Identify the common anions and cations (including polyatomic ions) 12. Apply your knowledge and explain how to combine those anions and cations in the correct proportions to form ionic compounds with no net charge 13. Determine the names of ionic compounds 14. Determine the names of molecular compounds of two non- metals 15. Determine the names of acids 16. Determine the names of hydrated salts

Chapter Two – Laboratory Requirements: All student based – hands on

1) Isotope Lab – a lab that uses three different coins to simulate a mass spectrometer. Student use the data collected to determine the atomic mass of an element. 2) Strong and Weak Electrolytes – a lab that uses CBL’s to test for the presence of ions in solutions. Students use this data to suggest which compounds are strong electrolytes and acids as well as weak electrolytes and acids.

Chapter Two – Major Assignments:

1) Reading – Ch. 2 2) Homework Sets – Ch. 2/Three Sets 3) Quizzes – Atomic Mass 4) Test – Over all unit objectives Chapter Three – Stoichiometry (2 Weeks)

Objectives – Students will be asked to….

1. Demonstrate how to write chemical equations from formulas into words and vice versa 2. Demonstrate how to write chemical equations using chemical formulas and chemical symbols (this requires knowledge, and correct use of, chemical nomenclature) 3. Demonstrate your ability to use state symbols as part of chemical equation writing 4. Demonstrate how to balance chemical equations 5. Explain why balancing chemical equations is important 6. Explain the concept of percentage by mass 7. Calculate empirical formula from percent by mass data 8. Calculate and convert empirical formula to molecular formula by using molar mass data 9. Apply the concept of the mole in chemical calculations (including the application of Avogadro's number) 10. Use combustion data to calculate empirical formula of compounds 11. Explain the importance of, and be able to apply the concept of stoichiometric coefficients relating to reacting ratios 12. Demonstrate how to calculate the number of moles of a solid substance present in a reaction from data 13. Explain and apply the concept of a limiting reactant and excess reactant 14. Explain and apply the concept of percentage yield

Chapter Three – Laboratory Requirements: All student based-hands on

1) Finding Mole Ratios – a lab that uses different ratios of reactants to see which ratio creates the greatest amount of heat. This ratio is the ideal mole to mole ratio for the lab. 2) Percent Yield – a lab that uses iron and copper sulfate in a single replacement lab to generate copper. The copper is filtered off and collected. Data collected is used to determine the actual yield.

Chapter Three – Major Assignments

1) Reading – Ch. 3 2) Homework Sets – Ch. 3/Three Sets 3) Quizzes – Empirical/Molecular Formula; Percent Yield 4) Test – Over all unit objectives Chapter Four – Basic Solution Chemistry (1.5 Weeks)

Objectives – Students will be asked to….

1. Draw water’s shape and explain the significance of its shape 2. Explain how water’s shape and chemistry allow solutes to dissolve into water 3. Explain how to determine what types of substances will dissolve in water 4. Explain the process of solvation/hydration 5. Explain the difference between strong, weak and nonelectrolytes. 6. Identify what substances could be electrolytes 7. Calculate molarity and use the equation to calculate moles of solute or volume of solution. 8. Explain how a standard solution is prepared including how to calculate the amount of solute that is needed and the equipment that would be used 9. Explain the process of dilution 10. Explain how to do the calculations associated with dilutions. This includes what equipment should be used as well as interpretation of the dilution calculation.

Chapter Four – Laboratory Requirements: All student based-hands on

1) Preparing Solution Lab – Students prepare a solution from a solid and test the concentration using a colorimeter and Beer’s Law. This solution is then used to prepare a dilution and the concentration is tested again with the colorimeter. 2) Analysis of a Hydrate – Students design a lab in which they are to obtain 0.40 grams of an anhydrous salt. The source is the hydrated salt.

Chapter Four – Major Assignments

1) Reading – Ch. 4 2) Homework Sets – Ch. 4/ 1 Set 3) Quizzes – No Quiz this Unit 4) Test – Over all unit objectives Chapter Four – Solution Stoichiometry (2.5 Weeks)

Objectives – Students will be asked to….

1. Predict the products of reactions 2. Apply the rules to write a balanced equation for a reaction 3. Identify reaction types 4. Apply stoichiometry concepts to solution reactions 5. Write complete and net ionic equations for a reaction 6. Identify a Bronsted/Lowry acid or base 7. Identify the precipitate in a precipitation reaction 8. Identify a neutralization reaction and predict the products of a neutralization reaction 9. Apply stoichiometric concepts to acid/base titrations 10.Predict the oxidation states of atoms 11.Identify the species reduced and oxidized in a reaction as well as the reducing and oxidizing agent 12.Apply the rules to write half reactions for redox reactions 13.Apply the rules to balance acidic and basic redox reactions 14.Apply stoichiometry concepts to redox reactions and titrations 15.Identify ions based on solution color, flame tests, and qualitative analysis results.

Chapter Four – Laboratory Requirements: All student based-hands on

1) Acid/Base Titration – KHP is used to standardize a solution of sodium hydroxide. The sodium hydroxide solution will then be used to determine the concentration of a vinegar solution. 2) Redox Titration – Potassium permanganate is used to determine the percent mass of commercial hydrogen peroxide. 3) Qualitative Analysis of Cations and Anions

Chapter Four – Major Assignments

1) Reading – Ch. 4 2) Homework Sets – Ch. 4/ 3 Sets 3) Quizzes – Titration Quiz 4) Test – Over all unit objectives

Chapter Five – Gas Laws (2 Weeks)

Objectives – Students will be asked to….

1. Calculate problems by being able to convert between different units of pressure 2. Calculate problems by converting between different units of temperature 3. Explain and be able to use Boyle's law in calculations 4. Explain and be able to use Charles's law in calculations 5. Explain and be able to use Avogadro's law in calculations 6. Explain and be able to use the Combined gas law in calculations 7. Explain and be able to use the Ideal gas law in calculations 8. Explain and be able to use the van der Waals equation (modified ideal gas law) in calculations 9. Explain and be able to use Dalton's law of partial pressures in calculations 10.Explain the conditions that are used as standards in calculations 11.Be able to use molar gas volume in calculations such as stoichiometry 12.Explain the Kinetic theory as applied to gases 13.Explain the concept of, and be able to perform calculations involving, the root-mean-square-speed of gases 14.Define the terms effusion and diffusion and be able to perform calculations relating to those concepts 15.Calculate the molar mass of a gas using the ideal gas law 16.Calculate the density of a gas from the ideal gas law 17.Explain how the ideal gas law was derived 18.Explain the difference between ideal and real as it relates to gases 19.List some characteristics of several real and atmospheric gases

Chapter Five – Laboratory Requirements: All student based-hands on

1) Molar Volume of a Gas – Hydrogen gas is collected in a eudiometer as a result of the reaction between magnesium and aqueous hydrochloric acid. The combined gas law is used to determine the molar volume of a gas. 2) Molecular Mass of a Volatile Liquid – The ideal gas law is used to calculate the molar mass of a gas collected in a test tube.

Chapter Five – Major Assignments

1) Reading – Ch. 5 2) Homework Sets – Ch. 5/Six Sets 3) Quizzes – Ideal Gas Law and Density Applications 4) Test – Over all unit objectives also a pre-test assessment

Chapter Six & Eighteen– Thermochemistry - (2Weeks)

Objectives – Students will be asked to….

1. Explain definitions that describe the systems and the heat flow studied in thermochemistry 2. Explain and be able to define a definition and write suitable equations for standard enthalpy of formation 3. Define and apply the concepts of heat capacity, specific heat capacity and molar heat capacity 4. Define and give examples of state properties, intrinsic and extrinsic properties 5. Define and apply the concepts associated with calorimetry 6. Apply the Law of Conservation of Energy to thermochemical processes and calorimetry. 7. Apply and define the terms associated wit the First Law of Thermodynamics 8. Explain and be able to define a definition and write suitable equations for standard enthalpy of combustion 9. Explain and be demonstrate an understanding of Hess's law cycle or algebraic methods to calculate a given enthalpy change 10. Calculate average bond energy terms 11. Define the terms exothermic and endothermic 12. Explain and be able to apply the energetics of the ionic bond as described by the Born-Haber cycle and associated calculations 13. Draw and explain a heating and cooling curve and calculate the energy requirements at any time along the curve. 14. Define the terms and explain the concepts of entropy, enthalpy and free energy 15. List some sources for energy

Chapter Six & Eighteen – Laboratory Requirements: All student based- hands on

1) Thermochemistry and Hess’s Law – Three reactions take place in a coffee cup calorimeter to verify Hess’s Law. 2) The Specific Heat of a Metal – Using a coffee cup calorimeter and water the specific heat of a known metal and an unknown metal are obtained. 3) The Molar Heat of Fusion of Ice – Using a coffee cup calorimeter and water a known amount of ice is melted and the heat of fusion is determined based on q system = - q surroundings

Chapter Six & Eighteen – Major Assignments

1) Reading – Ch. 6 and 18 2) Homework Sets – Ch.6 and 18/2 Sets 3) Quizzes – Calorimetry Quiz 4) Test – Over all unit objectives

Chapter Seven – Quantum Model (2 Weeks)

Objectives – Students will be asked to….

1. Explain the Bohr model of the atom 2. Explain how line emission spectra are formed 3. Explain how the electron can be considered to have wave like properties as well as particle type properties 4. Explain how to use equations that relate the energy, frequency, speed and wavelength of waves including the Rydberg equation 5. Explain what each of the 4 quantum numbers n,l,ml, and ms represents 6. Identify the quantum numbers for an electron in an atom. 7. Explain and use the terms s, p, d and f and their use in electron sublevel/sub shell notation 8. List and explain the rules for filling orbitals and determining electronic configuration, including the Pauli exclusion principle, Hund's rule of maximum multiplicity and notable exceptions 9. Construct the electron configuration of the elements using the s, p and d and f notation 10. Construct the electron configuration of the elements using the noble gas abbreviation. 11. Construct the electron configuration of simple ions (including d block ions) 12. Describe the shapes of the s, p and d orbitals 13. Explain that orbitals are electron probability maps 14. Describe electron configurations using the electron box notation 15. Define the terms paramagnetic, diamagnetic and isoelectronic 16. Explain that regular, repeatable patterns occur across periods and within groups on the periodic table and understand the notable exceptions. 17. Explain that the noble gases have full outer shells that represent stable electron configurations 18. Explain how and why group I, II, VI and VII elements achieve pseudo noble gas electronic configurations 19. List and define the trends of ionization energy, electron affinity, electronegativity, atomic size and ionic size 20. Predict the group an element is in from ionization energy data 21. Explain and apply the terms diamagnetic and paramagnetic 22. List and explain how physical properties such as boiling point and melting point, change gradually when moving about the periodic table

Chapter Seven – Laboratory Requirements: All student based-hands on

1) Flame Tests – Elements are tested in a flame for their characteristic color. An unknown is also identified. 2) Spectral Lines Lab – Students observe the “finger prints” or spectral lines characteristic of several gas tubes.

Chapter Seven – Major Assignments

1) Reading – Ch. 7 2) Homework Sets – Ch. 7/ 3 Sets 3) Quizzes – No Quiz this unit 4) Test – Over all unit objectives

Chapter Eight – Transition Metals - (1 Week – At Home Independent Study with two days of in class questions and work)

Objectives – Students will be asked to….

1. Understand and be able to write electronic configurations of transition metals and their ions 2. Recall some colors of transition metals and understand when color occurs 3. Be able to recognize and name complex ions 4. Understand and be able to write equations for complex ion reactions (ligand exchange & decomposition)

Chapter Eight – Laboratory Requirements: No lab with this unit.

Chapter Eight – Major Assignments 1) Reading – Ch. 8 and Supplemental Material from The Ultimate Chemical Equations Handbook. 2) Homework Sets – 2 Sets from the Supplemental Material above 3) Quizzes – No quiz this unit 4) Test – Over all unit objectives – Take-home test

Chapter Nine – Basic Bonding (1.5 Weeks)

Objectives – Students will be asked to….

1. Explain that when forming chemical bonds atoms are attempting to form more stable electronic configurations 2. Explain the concept of ionic bonding and the nature of the ionic bond 3. Explain the concept of covalent bonding and nature of the covalent bond 4. List the general characteristics of ionic bonds and covalent bonds 5. Draw Lewis structures 6. Explain the concept of resonance related to Lewis structures 7. Explain the concept of formal charge related to Lewis structures 8. Predict the shape of, and bond angles in, simple molecules and ions using VSEPR theory 9. Explain the concept of the coordinate covalent bond related to Lewis structures 10. Explain that ionic bonding and covalent bonding are at two ends of a sliding scale of bond type 11. Explain that polyatomic ions are held together with covalent bonds 12. Explain the concept of electronegativity 13. Explain that polarization caused by small highly charged cations leads to ionic compounds exhibiting some covalent character 14. Explain that differences in electronegativity in covalent molecules causes dipoles and some ionic character in covalent compounds 15. Explain why molecules exhibit polarity 16. Predict the shapes of simple molecules and ions using Lewis structures 17. Solve problems associated with bond energies and bond lengths

Chapter Nine – Laboratory Requirements: Excel/Computer Lab

1) Graphing Trends – Ionization energy and electronegativity trends are graphed. Students analyze, interpret and explain the trends based on the graphical representation.

Chapter Nine – Major Assignments 1) Reading – Ch. 9 2) Homework Sets – Ch. 9 /3 Sets 3) Quizzes – VSEPR quiz 4) Test – Over all unit objectives

Chapter Ten – Advanced Topics in Bonding (1 Week)

Objectives – Students will be asked to….

1. Explain the nature of sigma and pi bonds 2. Identify different types of orbital hybridization 3. Explain molecular orbital theory in the context of homonuclear atoms and heteronuclear atoms. Know how paramagnatism relates to this topic.

Chapter Ten – Laboratory Requirements: No lab with this unit

Chapter Ten – Major Assignments 1) Reading – Ch. 10 2) Homework Sets – Ch.10 / 2 Sets 3) Quizzes – No Quiz 4) Test – Over all unit objectives

Chapter Eleven – Solids and Liquids (1.5 Weeks)

Objectives – Students will be asked to….

1. Explain the difference between intra and inter bonding 2. Explain the occurrence, relative strength and nature of dipole-dipole interactions, London dispersion forces and hydrogen bonds 3. Explain how solid structure influences properties as in diamond and graphite. 4. Explain the basics of solid unit cell structure 5. Explain the difference between an interstitial alloy and a substitutional alloy 6. Describe the nature of liquids 7. Explain the concept of vapor pressure and equilibrium 8. Identity the proper terms associated with state changes 9. Explain and be able to interpret phase diagrams 10. Explain the factors that affect solubility

Chapter Eleven – Laboratory Requirements: All student based-hands on

1) Intermolecular Forces Lab – The metal probe for the CBL is used to determine which of three volatile liquids evaporates the quickest thereby exhibiting the weakest intermolecular forces. Chapter Eleven – Major Assignments

1) Reading – Ch. 11 2) Homework Sets – Ch.10 / 2 Sets 3) Quizzes – Intermolecular forces quiz 4) Test – Over all unit objectives

Chapter Twelve- Solution Composition – (1 Week)

Objectives – Students will be asked to….

1. Explain the concept of vapor pressure and equilibrium 2. Relate changes (both quantitative and qualitative) in vapor pressure to addition of non-volatile solutes to solvents (Raoult's Law) 3. Explain Raoult's Law in terms of ideal solutions of two volatile components AND deviations from ideal behavior 4. Describe and use equations relating to quantitative treatments of boiling point elevation, freezing point depression, osmotic pressure and the van't Hoff factor 5. Explain the factors that affect solubility such as structure, pressure and temperature 6. Calculate molarity, molality, mole fraction, mass percents, and Normality 7. Analyze data from a solubility curve 8. Explain the concept of like dissolves like. 9. Show Henry’s Law

Chapter Twelve – Laboratory Requirements: All student based-hands on

1) Molecular Mass by Freezing Point – The freezing point of pure lauric acid is determined using CBL’s. The freezing point of the lauric acid is determined for a second time using a mixture of lauric acid and benzoic acid. The change in the freezing point as well as the molality of the mixture is used to calculate the molar mass of the benzoic acid.

Chapter Twelve – Major Assignments

1) Reading – Ch. 12 2) Homework Sets – Ch.12/ 2 Sets 3) Quizzes – No quiz this unit 4) Test – Over all unit objectives

Chapter Thirteen– Kinetics - (2 Weeks)

Objectives – Students will be asked to…. 1. List AND explain Collision Theory 2. List AND explain how temperature, concentration, surface area and catalysts affect a rate of reaction 3. Explain AND interpret a Maxwell-Boltzman distribution plot 4. Explain AND interpret an energy profile plot 5. Be able to deduce orders, rate equations and rate constants (including units) from initial rate data 6. Explain the link between the rate determining (slow step) in a reaction mechanism and the rate equation 7. Explain AND be able to interpret graphical data relating to rates

Chapter Thirteen – Laboratory Requirements: All student based-hands on

1) Study of the Kinetics of a Reaction – The iodine clock reaction is used along with micro scale techniques to observe the effects of different factors on the rate of reaction. The activation energy for the reaction will also be determined. 2) The Rate and Order of a Chemical Reaction – Using a colorimeter to measure % Transmittance, the rate law and the order of a reaction will be determined. The reaction is between KI and FeCl3.

Chapter Thirteen – Major Assignments

1) Reading – Ch. 13 2) Homework Sets – Ch.13/3 Sets 3) Quizzes – One Quiz – Rate Laws 4) Test – Over all unit objectives

Chapter Fourteen & Sixteen– Equilibrium & Acid-Base Equilibrium – (2 Weeks)

Objectives – Students will be asked to….

1. Explain the concept of dynamic equilibrium

2. Calculate and explain an expression in terms of concentrations for the equilibrium constant Kc given a chemical equation 3. Explain that equilibria take a finite amount of time to be achieved 4. Calculate values for Kc and associated data from initial concentrations 5. Calculate and explain expressions in terms of partial pressures for the equilibrium constant Kp given a chemical equation 6. Calculate values for Kp and associated data from pressure data 7. List and explain Le Châtelier's Principle 8. Explain the application of Le Châtelier's Principle and be able to predict the shift in position of equilibria and optimum conditions in reactions 9. Explaing and be able to apply the relationship of Kc to Kp, the different formats of Kc (reciprocals and roots) and the relationships in simultaneous equilibria 10. Explain and be able to apply to calculations, the concept of solubility product 11. Explain and be able to apply to calculations, the concept of common ion effect

Chapter Fourteen & Sixteen – Laboratory Requirements: All student based-hands on

1) Determination of the Equilibrium Constant for the Formation of FeSCN2+ - A calibration curve is created using a series of FeSCN2+ solutions and a colorimeter. The calibration plot is used to determine the equilibrium concentrations of a reaction between Iron (III) ion and HSCN. 2) Le Châtelier’s Principle – A cobalt complex undergoes a series of system stresses to visually see how the equilibrium will shift to adapt to the stress.

Chapter Fourteen & Sixteen – Major Assignments

1) Reading – Ch. 14 2) Homework Sets – Ch.14 and 16/3 Sets 3) Quizzes – Quiz – Expressions and Le Châtelier’s Principle 4) Test – Over all unit objectives Chapter Fifteen– Acid/Base Chemistry - (2-2.5 Weeks)

Objectives – Students will be asked to….

1. Define and explain the Bronsted Lowry, Arrhenius and Lewis definitions of an acids and bases.

2. Identify acid base conjugate pairs 3. Explain the difference between strong and weak acids in terms of ionization 4. Calculate the pH of strong acids and strong bases 5. Calculate pH of weak acids and weak bases using Ka and Kb 6. Explain the definition of Kw, the ionic product of water 7. Explain the definition of a buffer 8. Explain how a buffer works 9. Identify and calculate the pH of a buffer solution 10. List and describe the techniques and procedures associated with titrations 11. Sketch titration curves and be able to suggest a suitable indicator for a particular titration 12. Explain the hydrolysis of salts and the effect this has on pH 13. Explain the meaning of the term 'equivalence point' 14. Explain how indicators work

Chapter Fifteen – Laboratory Requirements: All student based-hands on

1) Determination of the Equivalent Mass & pKa of an unknown acid – The value of the equilibrium constant for a weak acid will be determined from a titration plot. Also, a standard NaOH solution will be used to titrate an unknown acid. The equivalent mass for this acid will then be calculated. 2) pH and Indicators – A serial dilution is created to test the range of several indicators. 3) pH and Common household substances Common household substances will be tested with various indicators to determine the pH range. Using the data collected, trends will be analyzed.

Chapter Fifteen – Major Assignments

1) Reading – Ch. 15 2) Homework Sets – Ch.15/4 Sets 3) Quizzes – One Quiz - Buffers 4) Test – Over all unit objectives

Chapter Nineteen – Electrochemistry (2 Weeks) Objectives – Students will be asked to….

1. Explain the definition of oxidation and reduction in terms of electrons

2. Explain and recall the definition of standard electrode potential 3. Explain and recall how to construct a cell diagram (line notation) and draw a diagram (picture) of the apparatus needed 4. List the conditions under which the standard electrode potentials are measured 5. Explain the nature and purpose of a salt bridge 6. Predict the likelihood of chemical reactions using standard electrode potentials and explain how those predictions may not prove to be accurate 7. Explain and use the Nernst equation 8. Explain the relationship between Gibbs free energy, equilibrium constants and Ecell, and be able to perform related calculations 9. Explain electrolysis and be able to perform quantitative calculations relating to it

Chapter Nineteen – Laboratory Requirements: All student based-hands on

1) Electrochemical Cells – Using half-cell, a standard table of electrode potentials is created. The table and the half-cells will then be used to determine the affect of concentration on the cell potential, the solubility product constant and the formation constant. 2) Electroplating – An electrochemical cell will be used to plate out a known quantity of copper onto the surface of brass. The information collected will then be used to determine the amount of energy used to plate the copper.

Chapter Nineteen – Major Assignments

1) Reading – Ch. 19 2) Homework Sets – Ch. 19/3Sets 3) Quizzes – Electrochemical Cells 4) Test – Over all unit objectives

Chapter Twenty– Nuclear Chemistry - (1 Week – At Home Independent Study with two days of in class questions and work)

Objectives – Students will be asked to…

1. Explain the phenomenon of radioactivity and the properties of radioactive particles 2. Discuss nuclear equations 3. Explain the concept of half-life and be able to perform calculations related to it 4. List some uses of radioactivity 5. Explain the term mass deficit 6. Explain the neutron:proton ratio and use it to make predictions about the stability of an atom 7. List and define the terms nuclear fission and fusion 8. Explain in very general terms that radioactivity involves the rearrangement of the nucleus, and chemical reactions involve the rearrangement of electrons

Chapter Twenty – Laboratory Requirements: No Labs for this Unit

Chapter Twenty – Major Assignments

1) Reading – Ch. 20 2) Homework Sets – Ch.120/1 Set 3) Quizzes – No quiz for this Unit 4) Test – Over all unit objectives Chapter Twenty – Reactions – Each week of Second Semester, on Wednesday, Students will be given a new reaction type. On Friday of that week they will be tested on those reactions. Each week the quiz will be cumulative so that students are always looking back at the previous reactions taught.

Objectives – Students will be asked to….

1. Solve net ionic equations for double replacement reactions by writing out the equations and balancing them 2. Solve net ionic equations for simple REDOX reactions by writing out the equations and balancing them 3. Solve net ionic equations for non-simple REDOX reactions by writing out the equations and balancing them 4. Solve net ionic equations for hydrolysis reactions by writing out the equations and balancing them 5. Solve net ionic equations for complex ion (transition metal) reactions by writing out the equations and balancing them 6. Solve net ionic equations for organic reactions by writing out the equations and balancing them

Chapter Twenty – Laboratory Requirements: These concepts are addressed in many of the previously listed labs.

Chapter Twenty – Major Assignments 1) Reading – Reactions Note Sheets 2) Homework Sets – Content is reflected on most homework sets. 3) Quizzes – Every Friday of Second Semester unit the AP test

Chapter Seventeen & Twenty One – Descriptive Chemistry-OR- Periodicity and Qualitative Analysis (Some of these objectives repeat from other units but they are integral to descriptive chemistry and have thus been repeated.) Time – 2.5 Weeks

Most of this unit will be spent in lab.

Objectives – Students will be asked to….

1. Explain that regular, repeatable patterns occur across periods and within groups on the periodic table and understand the notable exceptions. 2. Explain that the noble gases have full outer shells and that this represents stable electronic configurations 3. List and describe why group I, II, VI and VII elements achieve pseudo noble gas electronic configurations 4. List and explain the trends of ionization energy, electron affinity, electronegativity, atomic size and ionic size as they apply to the elements and their reactivity from the periodic table. 5. Predict the group number an element can be found using ionization energy data 6. List, define, and be able to apply the terms diamagnetic and paramagnetic 7. Explain how many physical properties like boiling point change gradually when moving about the periodic table 8. Describe what distinguishes a metal from a nonmetal and from a metalloid. In your description, explain how they react based on their electron configurations and their location on the periodic table. 9. Describe the properties and reactions associated with the main group metals, group I, II and Al. Be familiar with their common compounds. 10. List and describe the chemistry of the transitions metals (see the transition metals unit) 11. Describe the chemistry of the halogens and other common nonmetals. 12. Describe the chemical reactivity of the halogens and nonmetals. Know how they are prepared. 13. Explain the chemistry of the hydrogen halides. Know how they react and how they are prepared. Know how ammonia is prepared. 14. Describe the chemistry of the oxyacids and oxyanions of the halogens and the other common nonmetals. Explain how their chemistry relates to acid strength and redox reactions. 15. Explain how hydrogen reacts with other nonmetals such as N, P, O, and S. 16. Explain how the oxides of these nonmetals behave as well as how they react with water. 17. Explain the relationship between the strength of an acid and its Ka value. 18. Describe how to test for gas production from some common reaction types. 19. Apply the activity series to single replacement activities and understand the arrangement of this series based on their placement on the table. 20. Explain how to work the schemes associated with identifying cations in a lab. 21. Explain how to work the schemes associated with identifying anions in the lab. 22. List and describe the products of the reactions of a qualitative analysis lab such as complex ion, precipitates and separation techniques for precipitates.

Chapter Seventeen & Twenty One – Laboratory Requirements:

1. Qualitative Analysis of Cations – Students run a series of tests to become familiar with the chemistry of the metals and their ions. They will be asked to determine unknown ions based on these laboratory findings. 1. Qualitative Analysis of Anions - Students run a series of tests to become familiar with the chemistry of the nonmetals and their ions. They will be asked to determine unknown ions based on these laboratory findings.

Chapter Seventeen & Twenty One – Major Assignments

1) Reading – Students will be ask to reference Ch. 17 and 21 as well as Chapter 17 from Chemistry Principles and Reactions, Masterton and Hurley. 2) Homework Sets – Various Worksheets 3) Quizzes – No quiz this unit 4) Test – Successful Completion of the Lab previously sited.

Chapter Twenty three– Organic Chemistry - (1 Week – At Home Independent Study with two to three days of in class questions and lab work.) Objectives – Students will be asked to….

1. List the names some simple aliphatic organic compounds

2. Describe, explain, and be able to write equations for some organic reactions (Combustion, Substitution, Acid Base, Addition & Esterification)

Chapter Twenty three – Laboratory Requirements: All student based- hands on

1) Preparations of Esters – Small quantities of esters are generated and identified by small. 2) Hydrocarbons – Using molecular model kits, students will visually create hydrocarbon structures and isomers. Nomenclature of the compounds will also be emphasized.

Chapter Twenty three – Major Assignments

1) Reading – Ch. 23 2) Homework Sets – Ch. 23/1 Set 3) Quizzes – No quizzes for this unit 4) Test – Over all unit objectives

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