Unit 1: Chemical Fundamentals s1

AP Chemistry Syllabi/Prospectus 2013-2014 Mr. Niedenzu

New information from CMS (again): -very important-! AP/IB Exam Policy: As you may be aware, effective with the 2013-2014 school year, CMS will be paying for students to take AP and IB exams as a result of the 2013-2014 budget adopted by the CMS Board of Education. Our new Superintendent Heath Morrison is a big proponent fo the AP and IB exams and wants as many students as possible take these courses - The requirement that students in AP and IB courses must take the corresponding exam has been reinstated by CMS policy and regulations.

- There will be a policy in place for students who choose not to take AP/IB exams. There are some issues currently that CMS needs to work out with regards to this situation and I will update you as soon as I hear how they are going to handle this

- If you take the AP exams the new policy will be once again that you do NOT have to take a teacher made final but see note above

Payment Information and Options: No longer applicable. Fee Waivers: AP No longer applicable. Sponsorship Opportunities: No longer applicable

Overview: The AP Chemistry course meets daily for one 90 minute period. Labs are conducted during the week on alternating days. This course is designed to provide a solid, first-year college chemistry experience, both conceptually and in the laboratory. The labs serve to supplement the learning in the lecture section of the course. Problem-solving skills, both on paper and in the lab, are emphasized. There are weekly labs and during the last quarter three full practice AP tests are taken and graded according to AP grading scale. Laboratory: Students are required to submit a complete report for each lab experiment, including a hypothesis, procedure, observations/data, calculations, sources of error, and a conclusion. All reports are kept in a lab notebook. The students are also called upon to make a presentation to the class about their hypotheses, calculations, and conclusions – in this way students can collaborate on the objectives and design of an experiment, and assist each other in reaching conclusions, and gain insights into variance and sources of error. Lab descriptions are listed at end of syllabus after the resources. Reaction sets: Nationwide scores on the reaction sets on the AP exam are generally lower than one might or should expect. Our scores are always higher than the national average by a large margin because we practice these every week. We use all of the old AP reactions along with other sources including all the study guides – students receive a set each Monday and are required to turn them in on Friday. This year I have also included the balancing component which will be added on the exam this year along with a separate question on each – i.e. on a redox reaction can they identify which is the reducing agent or on an electrolysis reaction which gas is formed and on which electrode. Class rules Students need to have access to the internet to access my website and other resources we will use during the year. Cell phone use is not allowed during the school day – if I see it or hear it, it will be confiscated and turned in to the front office. No food is allowed in class. Only clear, colorless water bottles containing water will be permitted. Cheating will not be tolerated. Late work will have a letter grade deduction for each day late (unless there is some extenuating circumstance). Behavior issues will be dealt with “in house” – the administration has many other things to deal with and I will handle these issues as they arise. Also, be forewarned, I DO call parents at home and at work, and I will call you at home if you have been absent or are absent to check on things. Required materials: materials for taking notes scientific or graphing calculator graph paper colored pencils Absences: I will follow the CMS guidelines on absences, please recheck your handbook on this. If you are absent and want to stay current – email me immediately at school [email protected] I will respond immediately!!! Lab safety: All students will undergo a review of lab safety rules and have to sign (along with the parents) that they have read the safety rules, watched the safety video, know where all the safety equipment in the room is located and the proper way to use it. Homework: I do not assign a lot of homework at once – the problems I do assign are carefully selected – some of the assignments are already on my web page, some will have answers with the questions. Assignments/quizzes: BEWARE: I will give short quizzes in class almost every day!!! I do give retakes on these if needed. Missed assignments: CMS allows you 5 days to schedule a time/due date to turn in missed assignments – remember it is your duty to take care of this! Grades: All grades and attendance will now be done on Powerschool – there are four categories under thae grades – formal, informal, midterm and final – there will be no grade for final if you take the AP test in May. All other grades other than the midterm will be put in the formal category where I operate on the point system and generally most classes will have over 1000 points accumulated for each quarter. I will follow CMS guidelines on grade distribution. Point distribution is as follows: Quizzes: anywhere from 5 – 20 points Homework: from 10 – 20 points Lab reports: from 20 – 50 points Tests: from 30 – 70 points We will go over lab report format in class – be aware that this area is usually where many student’s grades suffer because they do not turn in reports on time! In general you will have a week to turn in reports after the lab is done. If a student is absent when the material is assigned or gone over the student will have 5 days from they return to submit it. If a student was present when assigned and does not have the assignment when due they will lose a letter grade for each day it is late. Tutoring: The chemistry department will have weekly scheduled tutoring availability – the schedule will be given to you during the first week of school. In the fall I have limited availability for tutoring due to coaching responsibilities. In the winter and spring I will be available after school each day for help. I also have at my disposal a recently retired AP Chemistry teacher who is very good available for outside tutoring. NOTE: During the year a new syllabus will be generated due to wholesale changes the AP Chemistry program has made this past year. I will be uploading a sample syllabus – which is what the College Board told us to do and comparing it with the current syllabus – it will change constantly as we go along.

Unit 1: Chemical Fundamentals Approximate number of days: 5 A. General aim: To describe the properties of matter, scientific matter, and chemical calculations. Students should become familiar with the various pieces of lab equipment, working with sig figs, metric system, naming compounds, the mole concept B. Content: 1. Nomenclature a. Inorganic nomenclature b. Organic nomenclature i. give examples of alkanes, alkenes, alkynes, aromatics and aliphatics ii. review structural formulas and functional groups iii. review IUPAC nomenclature system c. Transition Metals and Coordination chemistry - Complex nomenclature C. Content: 1. English and metric systems 2. SI units and prefixes 3. Precision and accuracy 4. Fahrenheit, Celsius, and Kelvin temperature scales 5. Conversion factors 6. Density calculations 7. Classification of matter into subgroups 8. Properties of matter 9. Separation of mixtures 10. Significant figures – on AP test allowed +/- one figure (put 3 and you will be ok most of the time) D. Assignments: Organic HW sets 1 p1091 #24 thru 40 even,and 2 p1093 #52-60 even, complex nomenclature practice sheet, organic test, complex nomenclature qz, old reaction prediction sets involving organic compounds; E. Labs: synthesis and analysis of aspirin lab – also Lab Safety Rules and procedures

Unit 2: Atomic Structure and the Periodic Table Approximate number of days: 10 A. General aim: To gain an understanding of the development of atomic structure. B. Content: 1. Basic assumptions of Dalton’s atomic theory 2. J.J Thompson’s determination of charge-to-mass ratio 3. Millikan’s oil drop experiment 4. Rutherford’s nuclear atom C. General aim: To study nuclear particles, half life and radioactive decay. D. Content: 1. Characteristics of radiation a. alpha particles b. beta particles c. positron production d. electron capture e. gamma radiation 2. Nuclear stability a. zone of stability b. magic numbers 3. Rate of decay a. half-life b. first-order process 4. Transformations a. accelerators b. synthesis of some transuranium elements 5. Detection a. Geiger counter b. scintillation counter c. radiocarbon dating 6. Binding energy-mass defect 7. Nuclear fission a. chain reaction b. critical mass 8. Nuclear fusion 9. Nuclear reactors E. Assignments: Homework set p337 # 40 thru 50 even, other practice problems and quizzes, test

Unit 3:Chemical Stoichiometry Approximate number of days: 10 A. General aim: To calculate quantities of materials reacted or produced in chemical reactions. Students will also apply the periodic law to chemical reactivity in predicting products along with discussing the activity series of the elements, distinguish between metals and nonmetals, use the properties of metals and nonmetals to predict reaction products including using the activity series to predict single replacement reactions. Also use the periodic table to predict common oxidation states. B. Content: 1. Mole concept 2. Percent composition 3. Determination of the empirical and molecular formula for a compound 4. Write and balance equations for: a. combustion reactions b. synthesis reactions c. decomposition reactions d. single replacement reactions e. double replacement reactions f. begin practicing reaction predictions (note new format on AP test for this year!!) – 3 given, have to do all three, balance and answer other questions on them – used to pick 5 of 8 with no balancing or other questions 5. Mass-mass calculations 6. Calculations involving a limiting reagent 7. Calculation of percent yield C. Assignments: homework sets 1 page 124 # 34 – 58 even, set 2 page 125 # 60 – 96 even (a,b only), test, first sets of reaction prediction D. Labs: % of Sulfate lab (gravimetric analysis), formula of hydrate lab (copper sulfate), molar ratio lab (single replacement with copper sulfate solution and solid iron)

Unit 4:Electronic structure and Periodicity(see also stoichiometry general aim) Approximate number of days: 6 A. General aim: To describe the electronic arrangement within an element and to account for the periodicity of elements. Students should be able to name the major subatomic particles in an atom, types of radioactive emissions, discuss the Bohr model and the other models, work problems involving quantum numbers and energies of electron transitions, the various Rules and Principles, shapes of orbitals, basics of the periodic law, work problems involving nuclear binding energy and half-life, balance nuclear equations B. Content: 1. Electromagnetic radiation: wavelength, frequency, velocity 2. Planck’s constant: energy and frequency 3. Dual nature of light 4. Bohr model 5. Heisenberg’s uncertainty principle 6. Electron probability distribution 7. Quantum numbers and electron orbitals 8. Paramagnetic vs. diamagnetic 9. Shapes of probability charge clouds for s, p, d, f orbitals 10. Pauli’s exclusion principle 11. Wave mechanical model 12. Aufbau principle 13. Hund’s rule 14. Electron configurations and dot diagrams for atoms 15. IUPAC periodic table 16. Effective nuclear charge and shielding 17. Periodic trends in ionization energy, electron affinity, atomic and ionic radius 18. Properties of elements by their periodic table group 19. Lanthanide contraction 20. Colors- solutions/flame tests/precipitates/elements, especially transition metal salts C. Assignments: flame test demo, homework set 1 page 338 # 52,60,62 64,66, 68-80 even, set 2 page 340 #86-96 even; test

Unit 5:Chemical Bonding Approximate number of days: 15 A. General aim: To characterize chemical compounds according to the type of bonding and the structure of molecules. Students should be able to draw Lewis structures, use electronegativity to predict bond types, distinguish between polar and nonpolar, ude bonding principles to determine oxidation states, draw resonance structures, assign formal charge, compare VB theory to MO theory, use VSEPR, draw MO diagrams B. Content: 1. Types of chemical bonds a. why an ionic bond forms b. why a covalent bond forms c. electronegativity d. polar bonds, dipole moment 2. Ionic bonds a. electron configurations b. formulas c. lattice energy 3. Covalent bonds a. localized electron-pair model i. bond energy ii. Lewis structures iii. octet rule and exceptions iv. molecular geometry, VSEPR, sigma and pi bonds v. formal charge b. shortcomings of valence bond theory: resonance c. molecular orbital model i. bond order ii. delocalization of orbitals 4. Isomerism a. Geometric isomers b. Stereoisomers C. Assignments: Molecular model labs, synthesis and analysis of alum lab, homework sets # 22-90 even (due various days, a and b only on those that have more two questions) p. 403- 406, quizzes, test D. Labs: .Molecular model labs, synthesis and analysis of alum lab

Unit 6:Gases Approximate number of days: 8 A. General aim: To investigate the laws and models that describe the properties and behavior of gases. Students should know the kinetic-molecular theory, intermolecular forces, units used in gas law problems, interpret phase diagrams and solubility curves along with working out gas law problems B. Content: 1. Measuring pressure: units, manometers and barometers 2. Gas laws: Boyle, Charles, Guy Lussac, Avogadro, Ideal, Dalton, Graham 3. Gas stoichiometry a. STP b. molar volume c. mass-volume calculations 4. Kinetic-molecular theory a. explain properties of gases b. define temperature 5. Real gases a. deviation from ideal behavior b. van der Waals correction C. Assignments: homework sets 1,2,3 (set 1 p. 233 32-46 even, set 2 48-60 even, set 3 64-80 even) gas test; old AP essay questions D. Labs: Molar volume of gas lab, Dumas method lab (molar mass of gas), R constant lab using decomposition of potassium chlorate

Unit 7:Liquids and Solids Approximate number of days: 7 A. General aim: To describe the intermolecular forces responsible for properties of liquids and solids and the process of changing from one state to another. B. Content: 1. Intermolecular forces a. dipole-dipole forces b. hydrogen bonding c. London dispersion forces 2. Properties of the liquid state a. surface tension b. capillary action c. viscosity d. vapor pressure 3. Types of solids a. amorphous b. crystalline cubic forms, close-packed forms 4. Determination of crystal structure 5. Bonding in metals a. electron-sea model b. band model 6. Network atomic solids a. properties of carbon and silicon b. semiconductors 7. Comparison of types of solids and properties 8. Changes of state a. specific heat b. freezing point c. boiling point d. heat of fusion e. heat of vaporization 9. Heating curve 10. Phase diagrams a. water b. carbon dioxide C. Assignments: homework sets page p. 500 – 505, # 36 – 90 even over several days; test; magnet demo; old AP essay questions; sodium polyacrylate demo (“waterlok”) D. Lab: Spec 20 lab and chromatography labs using column chromatography (use Beer’s law)

Unit 8:Thermochemistry/Thermodynamics Approximate number of days: 10 A. General aim: To relate the fundamental aspects of the energy changes that accompany chemical reactions. Students should be able to solve problems involving Hess’s law, heat problems, calorimetry problems and interconvert with electro and equilibrium problems B. Content: 1. Concept of energy a. potential energy, kinetic energy b. first law of thermodynamics c. heat d. work e. state functions f. system and surroundings g. endothermic and exothermic reactions h. internal energy of a system 2. Calorimetry a. use of a calorimeter b. heat capacity c. energy released as heat 3. Enthalpy change for a chemical reaction a. Hess’s law b. standard enthalpies of formation c. heat of reaction, e.g., heat of combustion C. General aim: To predict whether or not a process is spontaneous, based on properties of the reactants and products. D. Content: 1. Second law of thermodynamics 2. Spontaneity of process determined by entropy calculations 3. ∆Gsurroundings = -∆Hsystem / T 4. Calculation of ∆G for a process from standard free energies of formation 5. ∆G = ∆H - T∆S 6. Predicting spontaneity from ∆G 7. Calculation of ∆G at conditions other than standard temperature 8. Predicting spontaneity from sign notation of enthalpy and entropy 9. Calculation of Keq from ∆G E. Assignments: Specific heat lab, heat of neutralization lab, old AP essays, homework set 1 p. 819 #20-50 even, set 2 p. 282 #34-62 even, quizzes, test F. Lab: Specific heat lab, heat of neutralization lab

Unit 9:Solutions Approximate number of days: 8 A. General aim: To investigate the properties of solutions. Students should also be able to work out problems involving different concentration units, interpret solubility curves, work out problems involving colligative properties B. Content: 1. Solution composition: mass percent, molarity, molality, normality, mole fraction 2. Nature of solutions a. water as a solvent b. strong and weak electrolytes c. concentration expressed as molarity d. solubility rules for salts in water 3. Calculations involving concentration of solutions a. standard solutions b. dilution of solutions 4. Calculations involving reactions in solutions 5. Heat of solution a. lattice energy b. hydration energy 6. Factors that affect solubility a. structure of solute and solvent b. pressure c. temperature 7. Factors that affect vapor pressure a. concentration b. solute-solvent interactions 8. Colligative properties a. freezing point depression, boiling point elevation, electrolytes b. osmosis c. applications d. van’t Hoff factor C. Assignments: Freezing pt. depression lab, qualitative analysis lab, Reaction sets given each week during the year on Mondays – due Friday (use old ones from AP tests and others); homework sets 1 p. 181 #20 – 66 even, set 2 p. 547 # 12-70 even; test D. Labs: Freezing pt. depression lab, qualitative analysis lab (identification of 6 unknown cations)

Unit 10: Chemical Kinetics Approximate number of days: 7 A. General aim: To measure, alter, and predict the rates of chemical reactions. B. Content: 1. Reaction rates a. definitions and units b. instantaneous rates from plot of concentrations versus tie c. factors that affect rate: concentration, temperature, catalyst d. potential energy diagram for a reaction 2. Integrated rate law a. equations relating concentration and time b. reaction order determined form the plot needed to give a straight line c. determination of overall order 3. Reaction mechanism a. molecularity b. rate-determining step c. distinguishing between catalyst and intermediates in mechanism 4. Collision model a. activation energy: Arrhenius equation b. molecular orientations 5. Catalysts: homogeneous and heterogeneous 6. Half-life (first order for common nuclear) C. Assignments: Iodine clock reaction lab; old AP essay test (focus on finding rate law and rate constant when given a table of experimental values); methylene blue demo, homework p. 598 #22-60 even, quizzes, test D. Lab: Iodine clock reaction lab, bromate clock reaction lab, thiosulfate lab

Unit 11: Chemical Equilibrium, Part I Approximate number of days: 7 A. General aim: To investigate the characteristics of chemical equilibrium. Students should be able to solve equilibrium problems involving gases and solutions, understand the meaning of Q and K, understand LeChatelier’s principle to predict shifts; how temperature, pressure, concentration, catalysts affect or do not affect equilibrium B. Content: 1. System at equilibrium a. rates of forward and reverse reactions b. composition of equilibrium mixture c. law of mass action d. equilibrium expression e. equilibrium constant 2. Calculation of concentrations that characterize a given equilibrium position a. homogeneous equilibria b. heterogeneous equilibria c. Kc and Kp 3. Applications of K a. to predict extent of reaction b. to calculate equilibrium concentrations given initial concentrations 4. Le Chatelier’s principle a. change in concentration b. change in pressure c. change in temperature C. Assignments: LeChatelier’s principle lab with copper chloride (can tell shift by color changing greener or bluer), daily mini test assignments using Zumdahl’s Equilibrium book (red) D. Lab: LeChatelier’s principle lab with copper chloride (can tell shift by color changing greener or bluer), Ksp of magnesium oxalate lab by titrating with standardized potassium permanganate

Unit 12: Equilibrium, Part 2 - Acids and Bases Approximate number of days: 10 A. General aim: To apply chemical equilibrium principles to the interactions of acids and bases. B. Content: 1. Acid-base models a. Arrhenius b. Bronsted-Lowry c. Lewis 2. Equilibrium constants and acid strengths 3. Calculation of H for weak and strong acids and bases 4. Dissociation of water a. Kw b. amphoterism 5. Hydrolysis of salt solutions a. Kh b. equilibrium expression 6. Acidic and basic oxides C. Assignments: daily mini quizzes using Zumdahl’s red Equilibrium book

Unit 13: Equilibrium, Part 3- Aqueous Equilibria Approximate number of days: 10 A. General aim: To make aqueous equilibria calculations involving buffers, solubility products, and complex ions. B. Content: 1. Common ion effect a. acid dissociation equilibrium b. buffered solutions c. solubility of ionic solids 2. Buffered solutions a. characteristics b. calculation of pH c. Henderson-Hasselbach equation (use whenever you can!) d. buffer capacity 3. Titration curves a. strong acid-strong base b. weak acid-strong base c. strong acid-weak base d. polyprotic acids e. indicators 4. Solubility product a. calculation of Ksp given salt solubility b. calculation of salt solubility given Ksp c. calculation of salt solubility in solution containing a common ion d. selective precipitation 5. Complex ions a. equilibrium principles b. effect on the solubility of a salt C. Assignments: we will be using the Zumdahl “redbook” to through four subunits on equilibrium and we will be answering all the mini test in each chapter along with unit tests at the end of each chapter; unit 1 test on general equilibrium, unit 2 test on acid-base equilibrium, unit 3 test on buffers and titrations, unit 4 test on Ksp; old AP essay questions, quizzes, test D. Lab: spec-20 Ksp lab, Ka lab with pH meters

GREEN CRYSTAL LAB – after equilibrium we will take about 6 days to do the crystal lab which covers at least 8 of the lab components on the AP requirement list (see description in lab section)

Unit 14: Electrochemistry Approximate number of days: 7 A. General aim: To consider the theoretical basis of oxidation-reduction reactions. B. Content: 1. Oxidation-reduction equations a. half reactions b. oxidizing agent and reducing agent c. balanced net equation 2. Electrochemical cell a. sketch and label b. anode-oxidation c. cathode-reduction d. cell potential e. examples of common galvanic cells 3. Electrolytic cell a. sketch and label b. predicting products of reactions at anode and cathode 4. Standard electrode potentials a. relative to potential of standard hydrogen electrode b. comparison of strength of oxidizing agents c. Nernst equation for nonstandard conditions d. predict direction of spontaneous change 5. Cell voltage used to determine ∆G 6. Cell voltage used to determine Keq 7. Faraday’s laws of electrolysis 8. Applications of electrolysis 9. Stoichiometric calculations a. equivalent weight b. normality of oxidizing and reducing agents C. Assignments: homework p. 868 # 16 – 80 even (over various days), voltaic cell demo, voltaic cell simulations, electrolysis demo, old AP essays, quizzes, test D. Lab: electrolytic synthesis of iodoform lab, Creating Danielle cells and concentration cells lab

Teaching Resources

Text: NEW TEXT THIS YEAR Raymond Chang and Kenneth A. Goldsby, Chemistry, 11th edition (2014) ISBN 978-0-07-665610-3 McGraw Hill Company 1221 Avenue of Americas, New York, NY 10020

AP Chemistry workbook – Peter Demmin and David Hostage – Multiple-Choice & Free Response Questions in Preparation For The AP Chemistry Examination, 5th Edition (2005) D&S Marketing Systems, Inc. 1205 38th Street Brooklyn, NY 11218

AP Chemistry workbook – John Moore and Richard Langley – 5 Steps to a 5 AP Chemistry, 1st edition (2004) ISBN 0-07-141275-1 McGraw-Hill Two Penn Plaza New York, NY 10121-2298

AP Chemistry lab book – David Hostage and Martin Fossett, Laboratory Investigations AP Chemistry, 1st edition (2006) ISBN 1-4138-0489-6 The People’s Publishing Group, Inc. 299 Market Street Saddle Brook, New Jersey 07663

Multimedia – AP Chemistry Teacher’s Tools, www.FraneMedia.com 2nd edition 2005 PO Box 254 Pennington, NJ 08534-0254

Multimedia – AP Chemistry Neo/Lab Virtual Lab Software, www.neosci.com PO Box 22729 Rochester, NY 14692-2729

Multimedia – www.apexvs.com Apex Learning, Inc. (2006)

Chemistry AP Labs:

NOTE: all labs are hands on unless otherwise noted

Determining the Heat Capacity of an unknown metal Using the concept of the conservation of energy, students will determine the heat capacity of an unknown metal by heating a weighed sample, then placing it into a weighed amount of water in a calorimeter and recoding the temperature change. (1 hour)

Finding the Formula of a Hydrate Students will heat a weighed sample of a hydrate. Using the mass of the anhydrous sample, students will determine the moles of water and moles of anhydrous compound. (if you do copper sulfate 1.5 hours, if part of green crystal lab – making crystal 1.5 hours, hydrate part will take parts of two periods for about 2 hours)

Finding the Ratio of Moles of Reactants in a Chemical Reaction Students will mix a series of solutions, producing an exothermic reaction. Based on the mixture that produces the most heat, students can determine the stoichiometric ratio. (1.5 hours)

Synthesis and Analysis of an Alum Students will synthesis potassium aluminum sulfate (or some other “alum”). Students will then run several tests to determine the purity of the sample. (3.0 hours)

Determining the Molar Volume of a Gas Students react a known mass of magnesium ribbon with an excess of concentrated hydrochloric acid solution. They collect the hydrogen gas over water and calculate the molar volume once they have accounted for the different factors that affect pressure. (1 hour)

Thermochemistry and Hess’s Law Through a series of acid-base reactions, students will determine the heat of neutralizations for each reaction. From these values, they can then verify Hess’s Law. (1.5 hours)

Working with Molecular Models - Understanding the VSEPR Theory Students will use kits to build models of various molecules in order to show the different shapes. Students should understand how lone pair electrons impact the shape of the molecule. (1.5 hours)

Determination of the Molecular Mass of a Volatile Liquid Using the “Dumas” method, students will determine the molar mass of a small sample of a volatile liquid. (1.5 hours – expect poor results on this one)

Solving for the gas constant R Using the vanderWaals equation and decomposing potassium chlorate to produce oxygen gas you can solve for the gas constant R (1.5 hours – should get good results if carefull)

Determination of the Molecular Mass by Freezing Point Depression Using a computer simulation, students will investigate the effect of adding solutes to solvents. The van’t Hoff factor for electrolytes will be investigated. (1.5 hours)

Study of the Kinetics of a Reaction Students will determine the order of an iodine clock reaction and observe what factors affect the rate of a reaction. (1.5 hours)

Working with Molecular Models - Understanding Intermolecular Forces Students will use kits to build models of various molecules in order to show the different shapes. Students should understand how the arrangement of the atoms in these molecules determines whether or not the molecule is polar. (1.5 hours) Determination of the Equilibrium Constant for the Formation of FeSCN2+ by Spectrophotometric Analysis Using Beer’s Law, students will prepare a series of standards. Then a second set of solutions are prepared in which concentrations of each reactant are varied. (1.5 hours – other things can be used – thymol blue with different acid concentrations can be used)

Determination of the Dissociation Constant of a Weak Acid Using a pH meter during an acid-base titration, students will determine the dissociation constant of a weak monoprotic acid by titrating it against a strong base. (1.5 hours)

LeChatelier’s Principle - Studying Factors that Affect Equilibrium Students will study the effect of temperature, concentration changes, and the effect of a catalyst on the position of a reaction. (1.5 hours – copper chloride is good for this one)

Acid-Base Titrations - Strong Acid with a Strong Base vs. Weak Acid with a Strong Base Students will run a series of acid-base titrations using a pH meter in order to observe the differences between a neutralization reaction between a strong acid with a strong base versus a weak acid with a strong base. The concept of buffers will be introduced. (3.0 hours)

Working with Molecular Models - Study of Organic Functional Groups Students will use kits to build models of simple organic functional groups such as alkanes, alkenes, alcohols, and esters. (1 hour)

Synthesis and Analysis of Aspirin and an Ester Students will synthesize aspirin and then analyze it for purity and will also produce an ester. (Parts of three days, 3 hour)

Qualitative Analysis Lab The students are given 6 cations to separate and run verification test on (Mn,Cu,Ag,Fe,Al,Zn) and then are given an unknown sample of a combination of these and are asked to identify using a qualitative analysis scheme. (Parts of four days, 5 – 6 hours total)

“Green Crystal Lab” - Synthesis and Analysis of a complex of an iron complex salt This lab incorporates several of the labs suggested by the AP program, including the following: 1. the determination of the formula of a compound 2. determination of the percentage of water in a hydrate 3. standardization of a solution using a primary standard (NaOH with KHP) 4. determination of concentration by acid-base titration, including a weak acid or weak base 5. determination of concentration by oxidation-reduction titration (oxalate with permanganate) 6. determination of mass and mole relationship in a chemical reaction 7. synthesis of a coordination compound and its chemical analysis 8. separation by chromatography (this lab can take up to 5 days to do, approximately 6 – 7 hours)