University of Manitoba Faculty of Science, Department of Chemistry

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1 CHEM-1310 Summer 2010 Syllabus Page 1 of 10 University of Manitoba Faculty of Science, Department of Chemistry CHEM-1310: INTRODUCTION TO PHYSICAL CHEMISTRY (Chemical Reactivity) Course Syllabus, Summer 2010 Lecture time: Monday thru Friday 10:45-12:45 Lecture place: 204 Armes Lecturer: Dr. S. Vakili Lecturer contact: vakili@cc.umanitoba.ca Laboratory time: Monday thru Friday 1:30-4:30 Laboratory place: Parker Building Laboratory coordinator: Dr. S. Vakili Office hours : 1:30-3:00 each day that the lab is running or by appointment Office location: 256A Parker Building Course description and purpose: In CHEM-1310, chemical and physical reactivity and their applications will be studied. Following a brief review of relevant material, the five major areas of physical chemistry/chemical reactivity will be examined. These include: thermochemistry; chemical kinetics; chemical equilibrium; chemical thermodynamics; and acids, bases and aqueous equilibria. The purpose of this course is to, along with CHEM-1300, provide a foundation in chemistry. This is required not only for chemistry and biochemistry but also the fields of microbiology, dentistry, medicine, pharmacy and physics. The focus of the course is on quantitative analysis and problem-solving. An ability to do basic mathematics is required. Prerequisites, Registration and Exemptions You need to have completed CHEM-1300 or have been granted Departmental permission to register in this course. It is your responsibility to ensure that you meet the requirements as outlined in the general calendar. Do not assume that because the registration system allowed you to register that you may actually take the course. There will be no fee adjustments for withdrawal due to incomplete requirements and no credit for the course. If you have previously taken this course and received a minimum of 60% (9 of 15 marks) in the laboratory portion, you may qualify for a lab exemption. See Sharon, room 141 Parker, for the required papers. Note that your exemption may only be given once, within two calendar years after lab completion and that your original mark will be carried forward towards your mark in this course. You will be tested on laboratory material on the final examination, even if you have an exemption.

2 CHEM-1310 Summer 2010 Syllabus Page 2 of 10 Important dates and tentative schedule: Date Lecture Lab Groups A, B, C Lab Groups D, E, F Tues. July 27 First Lecture Group placement Group placement Wed. July 28 Expt #1, flow chart due --- Thurs. July Expt #1, flow chart due Fri. July 29 Assignment 1 due Expt #2, prelab, flow --- chart and report #1 due Mon. Aug 2 HOLIDAY HOLIDAY HOLIDAY Tues. Aug Expt #2, prelab, flow chart and report #1 due Wed. Aug 4 Expt #3 virtual due Expt #3 virtual due Thur. Aug 5 Assignment 2 due Expt #4, prelab, flow --- chart and report #2 due Fri. Aug Expt #4, prelab, flow chart and report #2 due Mon. Aug 9 Assignment 3 due Tues. Aug 10 MIDTERM MIDTERM MIDTERM Wed. Aug 11 Expt #5, prelab, flow --- chart and report #4 due Thurs. Aug Expt #5, prelab, flow chart and report #4 due Fri. Aug 13 Drop date Expt #6 virtual due Expt #6 virtual due Mon. Aug 16 Assignment 4 due Expt #8, prelab, flow Expt #7 virtual due chart and report #5 due Tues. Aug 17 Report #8 due Expt #8, prelab, flow chart and report #5 due Wed. Aug 18 Expt #7 virtual due Report #8 due Thurs. Aug 19 Assignment due, Last class Fri. Aug 20 Day off Mon. Aug 23 FINAL EXAM Grading Mark break down will be as follows: Scheme A Scheme B Midterm 25% Online Assignments 10% 10% Laboratory 15% 15% In Class Participation 5% 5% Final Exam 45% 70% Total 100% 100% It should be noted that no other method (e.g. writing an essay or retaking a test) of obtaining marks is possible, even if you are failing the course. Please noted that you require a C minimum (>50%) to continue to CHEM-1310 and that the best mark of the two marking schemes will be used for your grade. Please refer to the appropriate section

3 CHEM-1310 Summer 2010 Syllabus Page 3 of 10 of your general calendar for a complete listing of letter grade meanings. Assignment of letter grades to the above totalled percentage will be as follows: 90% A % B % D % A % C+ <40% F % B % C Midterm exam: This will be a two hour test with two parts to complete. Part A will be multiple choice with a bubble sheet to fill in. Part B will be open answer with areas to fill in. There will be NO makeup exam should you miss this midterm; marking scheme B will automatically apply. Assignments: There will be five (5) assignments worth 2% each (5 x 2% = 10%) due at midnight according to the schedule. These assignments will take time to complete so start before the day it is due. There will be a 50% loss each day in your mark for late submissions. Laboratory: Your lab schedule is found in this syllabus and your starting instructions are found on the first few pages. Important information about safety, syllabus and laboratory policy are found on the pink and yellow pages of your manual. This information must be read before coming to the first experiment. The lab is worth 15% of the courses final grade and you MUST HAVE a minimum of 9 of 15 marks or 60% to pass the course. The mark breakdown is 2.5 marks for pre-labs, 12.0 marks for flow charts and reports and 0.5 marks for performance/safety. Participation: This is done in class with your iclicker. You receive one point for each time you answer a question. If the question has a right answer, you will get a second point for picking the correct answer. The number of questions per class and the time that they are offered will vary/change. Marks will be posted throughout the term so be sure to check that your iclicker is working/set to the right frequency as there is no consideration given for missed/unrecorded answers. The mark will be calculated the following way: full 5 marks for having 75% or more of the total available points; 3 marks for having 50-75% of the total iclicker points; and 0 marks for having less than 50% of the iclicker points. Final Exam: This will be a three (3) hour exam and is cumulative (i.e. everything on the syllabus, done in class or seen in the lab is potentially there). The format will be the same as the midterm exam with a Part A multiple choice and a Part B open questions. Required Course Materials - Nivaldo J. Tro, Chemistry: A Molecular Approach. 1 st Edition; Pearson Education, Inc., Upper Saddle River, NJ, USA (2008).

4 CHEM-1310 Summer 2010 Syllabus Page 4 of 10 This may be bought as part of the package (ca. $150, ISBN ) along with your laboratory safety information, the MasteringChemistry kit and the solutions manual or on its own if it is used - iclicker/classroom Response System: ISBN This iclicker is also used in CHEM-1310, some second year chemistry courses as well as in other departments. It may be purchased new from the shelf (ca. $40) or used from the Bookstore Customer Service Desk (ca. $30). - Laboratory Manual: ISBN (ca. $12), F. Gauvin, K. Koczanski, Laboratory Manual and WHMIS Handbook for University 1 Chemistry CHEM-1300:Structure and Modelling in Chemistry, University of Manitoba. - Laboratory coat and safety glasses - MasteringChemistry Student Access Kit for Tro s Chemistry: A Molecular Approach This may be bought as part of the textbook package or separately if you have a used textbook (ca. $42, ISBN ) - Chemistry Laboratory Safety Video Workbook and DVD This may be bought as part of the textbook package or separately if you have a used textbook (ca. $20, ISBN ) - Calculator, scientific but non-programmable Optional Course Materials - Selected Solutions Manual for Tro s Chemistry: A Molecular Approach - Calculations Guide: E. Smirnova, N.R. Hunter, A Survival Kit for Stoichiometry, Ratios, and Proportions From the Chemistry Departmental Office, 360 Parker Building ($4, exact change only) - Print copies of the partial lecture notes and laboratory information found on the ANGEL Learning Site. To register your iclicker (if you have not already done so) 1) go to click on register 2) give the required information i) student ID is your UM 7-digit student number ii) iclicker ID is the number on the back of your iclicker iii) type the verification word (changes each time) 3) click the enter button Note: iclickers are not transferable between students unless the iclicker registration is changed. If you can not read the iclicker ID number or change your iclicker part way through term, talk to your lecturer. To register for the online MasteringChemistry assignments (please see the student access kit that came with MasteringChemistry): 1) ensure that your computer meets the system requirements as found in the student access kit or at Note: internet explorer and netscape work but other internet browsers might work better. 2) go to

5 CHEM-1310 Summer 2010 Syllabus Page 5 of 10 3) if this is your first time using MasteringChemistry (i.e. new user), click on the new students and follow the instructions. If you have used MasteringChemistry before, login in using your previous information 4) to enrol in the course, enter the following information: i) student ID is your 7-digit UM student number ii) course ID is CHEM1310S2010 To register for the LateNiteLabs: see what is in the blue pages of the lab manual for directions. Your section number is Expectations and Other Miscellaneous Things Classes will be a combination of lecture, powerpoint presentation, iclicker questions, problem solving and possibly demonstrations. The ANGEL Learning website will be used to post upcoming lecture material, marks and other important information. This can be accessed via Be sure to BRING TO EACH CLASS your iclicker, working pens/pencils, paper and your calculator. Cell phones, pagers, and ipods/mp3 players are to be turned off during class. Laptop computers are allowed so long as the sound is off. Please respect your fellow classmates, instructors and staff. The time in class will be used to highlight the major concepts. It should be noted that all material listed/assigned in this syllabus may be tested upon even if it is not covered in the lecture. Any information seen in the assignments or in the lab portion of the course is also testable. Laboratory attendance is required and is NOT OPTIONAL. Lecture attendance is highly recommended. Chemistry can be difficult, do not give up and do not procrastinate. Expect to spend at least two hours outside of class and lab time to study, do assignments, do problems and prepare reports. If you are having difficulties with the course material for any reason, please come talk to your lecturer (S. Vakili) and/or your lab TA (if appropriate). Modification of grading may occur only under special circumstances given documentation. If you have a disability/illness that affects your studies or are experiencing difficulties you may also discuss these with the following: Disability Services 155 University Center, (voice), (TTY) Learning Assistance Center 201 Tier Building, Student Counselling and Career Centre 474 University Center, Please refer to your general calendar for polices regarding academic integrity, grading, attendance and conduct. This calendar may be picked up from UMSU or viewed online. If you have questions about the posted exam mark/answers talk with your lecturer immediately. If you have questions about your lab reports, first contact your TA then the lab supervisor only if required. Appeal of your lab report must be done within two (2) days of the return of the report. No appeals of laboratory grades, assignments or midterm marks will be accepted after writing the final exam. If you wish to see/review your final exam papers prior to the end of the Grade Appeal period please contact the Chemistry Departmental office.

6 CHEM-1310 Summer 2010 Syllabus Page 6 of 10 Course Objectives and Program: Section I: Thermochemistry General: 6 hours. You should be able to: 1) describe the meaning of work, energy, heat and enthalpy; and 2) calculate the heat of a reaction using standard heat of formation. Textbook sections: , 9.4, 9.10 and in chapter 11, pages , Suggested problems: pages : 31, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 71, 73, 75, 77, 79, 81, 83, 85, 89, 91, 93, 95, 99, 101, 103, 107, 111. pages : 47, 49, 73, 75, 77, 97, 103, 109, 111. page 513: 67, 69, 71, 77, 79, 81. Specific Objectives I-1 Explain the difference between kinetic energy and potential energy. I-2 Describe the typical energy units and convert from one unit to another. I-3 Explain the conservation of energy and energy transfers by heat and work. I-4 Recognize and use thermodynamic terms: system, surroundings, heat, work, temperature, thermal equilibrium, exothermic, endothermic, and state function. I-5 Use specific heat capacity and the sign conventions for energy transfers. I-6 Distinguish between change in internal energy and change in enthalpy. I-7 Use thermochemical equations with the stoichiometry of reactants and products. I-8 Consider stoichiometric parameters in calculation of enthalpy changes. I-9 Determine lattice energies using the Born-Haber cycle. I-10 Explain the origin of enthalpy change for a reaction in terms of bond enthalpies. I-11 Use bond enthalpies to estimate the enthalpy of a reaction. I-12 Determine the average bond energy of a bond using given enthalpies of reaction. I-13 Describe how calorimeters are used to measure the quantity of thermal energy transferred during a process. I-14 Calculate the heat evolved or absorbed when an object or substance undergoes a known temperature change and/or undergoes a phase change. I-15 Determine the enthalpy of reaction using data from both constant-pressure and constant-volume calorimeter experiments. I-16 Apply Hess s Law to find the enthalpy change for a reaction. I-17 Use standard molar enthalpies of formation to calculate the thermal energy transfer during a reaction. I-18 Define and give examples of some chemical fuels, and evaluate their abilities to provide heating. I-19 Describe the main components of food and evaluate their contributions to caloric intake. Section II: Chemical Kinetics General: 6 hours. You should be able to: 1) describe why/how rates depend on concentration and temperature; 2) explain activation energy; and 3) use both rate laws and integrated rate laws to solve for a variable.

7 CHEM-1310 Summer 2010 Syllabus Page 7 of 10 Textbook sections: , 19.6 Suggested problems: Pages : 25, 27, 29, 31, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 73, 75, 77, 79, 85, 87, 89, 93, 95, 97, 99, 101, 105. Page 899: 49, 53, 57. Specific Objectives II-1 Define reaction rate and calculate average rates. II-2 Describe the effect reactant concentrations have on reaction rate. II-3 Determine rate laws and rate constants by the initial rates method. II-4 Determine reaction orders from a rate law. II-5 Use integrated rate laws to obtain orders and rate constants. II-6 Calculate concentration from time, time to reach a certain concentration, and halflives of first-, second- and zeroth-order reactions. II-7 Calculate the amount of radioactivity from half-lives of radioisotopes and vice versa. II-8 Be able to do problems on radiocarbon and uranium/lead dating. II-9 Define and give examples of unimolecular and bimolecular elementary reactions. II-10 Describe the energy profile of a reaction with transition states and intermediates. II-11 Define activation energy and frequency factor (collision frequency and steric factor). II-12 Use activation energy and frequency factor to calculate rate constant and rates under different conditions of temperature and concentration. II-13 Derive rate laws for unimolecular and bimolecular elementary reactions. II-14 Define reaction mechanism and identify rate-determining steps and intermediates. II-15 Given several reaction mechanisms, decide which is (are) in agreement with experimentally determined stoichiometry and rate law. II-16 Explain how a catalyst can speed up a reaction II-17 Describe the energy profile of a catalyzed- and non-catalyzed reaction II-18 Define the terms enzyme, substrate and inhibitor II-19 Describe the steps of heterogeneous catalytic processes. Section III: Chemical Equilibrium General: 5 hours; You should know how to: 1) write an equilibrium constant expression for a given chemical reaction; 2) use a reaction quotient to predict if the reaction will occur forwards or backwards; 3) solve K expressions for more than one concentration or pressure. Textbook sections: Suggested problems: Pages : 21, 23, 25, 27, 29, 31, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 73, 75, 77, 79, 81, 83, 85, 87, 89, 91, 93. Specific Objectives: III-1 Recognize a system at equilibrium and describe the properties of equilibrium systems. III-2 Describe the dynamic nature of equilibrium and the changes in concentrations of reactants that occurs as a system approaches equilibrium III-3 Write equilibrium constant expressions, given balanced chemical equations

8 CHEM-1310 Summer 2010 Syllabus Page 8 of 10 III-4 Obtain equilibrium constant expressions for related reactions from the expression for one or more known reactions III-5 Calculate K p from K c, or K c from K p, for the same equilibrium III-6 Calculate a value of K c for an equilibrium system, given information about initial and equilibrium concentrations III-7 Predict whether a reaction is product-favoured or reactant-favoured based on K values III-8 Calculate concentrations of reactants and products in an equilibrium system if K c and initial concentrations are known. III-9 Use the reaction quotient Q to predict in which direction a reaction will go to reach equilibrium III-10 Using Le Chatelier s principle, show how changes in concentration, pressure, volume and temperature shift equilibria. III-11 Use the change in enthalpy and the change in entropy qualitatively to predict whether products are favoured over reactants in a given reaction. III-12 List the general factors affecting chemical reactivity, and apply them to predict optimal conditions for producing products Section IV: Free Energy and Thermodynamics General: 6 hours. You should be able to: 1) describe the meaning of free energy and entropy; 2) calculate free energies of reactions using standard values; and 3) predict spontaneity. Textbook sections: Suggested problems: Pages : 27, 29, 31, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 73, 75, 77, 79, 81, 83, 85, 87, 95, 99, 101, 103. Specific Objectives: IV-1 Explain what is meant by product-favoured and reactant-favoured reactions and spontaneity IV-2 Explain the dispersion of matter and energy in simple terms of probabilities. IV-3 Describe and calculate he entropy change for a process occurring at constant temperature IV-4 Use qualitative rules to predict the sign of the entropy change for a process IV-5 State the Second and Third Laws of thermodynamics IV-6 Calculate the entropy change for chemical reactions, given standard molar entropies for elements and compounds. IV-7 Use entropy and enthalpy changes to predict whether a reaction is productfavoured (or spontaneous) IV-8 Describe the relationship between enthalpy and entropy changes, and Gibbs free energy IV-9 Using Gibbs free energy relationship, predict how temperature can affect a reaction. IV-10 Calculate Gibbs free energy change for a reaction using values of standard molar free energies of formation of compounds and calculate free energy change under nonstandard conditions

9 CHEM-1310 Summer 2010 Syllabus Page 9 of 10 IV-11 Relate Gibbs free energy and standard equilibrium constant for the same reaction and use this relationship to calculate one from the other IV-12 Describe how a reactant-favoured system can be coupled to a product-favoured system so that a desired reaction can be carried out Section V: Acids, Bases and Aqueous Ionic Equilibrium General: 7 hours. You should be able to: 1) explain Bronsted and Lewis acids and bases; 2) define ph and pka; 3) use theory to predict the ph of solutions of acids, bases, salts and buffers; 4) write solubility constant expressions; and 5) calculate solubilities with or without added salts. Textbook sections: , (note 16.7 for lab) Suggested problems: Pages : 35, 39, 41, 43, 45, 51, 53, 55, 57, 63, 65, 71, 77, 79, 85, 87, 89, 93, 95, 97, 101, 103, 105, 111, 119, 121, 125, 127, 129, 131, 133, 137, 147. Pages : 27, 31, 33, 39, 43, 45, 47, 53, 59, 65, 67, 71, 71, 73, 77, 83, 87, 89, 91, 95, 103, 105, 115, 117, 119, 123, 137, 141, 143. Specific Objectives: V-1 Define acids and bases according to Arrhenius and Bronsted s definitions V-2 Define and compare the strengths of acids and bases (weak and strong acids and bases) V-3 Identify conjugate base pairs and explain their relative strengths V-4 Describe how amines act as bases and how carboxylic acids ionize in aqueous solution V-5 Describe water s role in aqueous chemistry and explain the autoionization of water and show how this equilibrium takes place in aqueous solutions of acids and bases V-6 Classify solutions as being acidic, basic, or neutral based on concentrations of H 3 O + and OH - V-7 Explain what is meant by the ph scale V-8 Calculate ph (or poh) given [H 3 O + ] or [OH - ] V-9 Calculate [H 3 O + ] or [OH - ] given ph or poh V-10 Write the acid ionization constant expression for any weak acid and the base ionization constant expression for any weak base V-11 Estimate relative acid and base strengths from K a and K b values V-12 Write the ionization steps of polyprotic acids V-13 Calculate ph from K a or K b values and solution concentrations V-14 Describe the relationship between acid strength and molecular structure V-15 Explain the nature of zwitterions V-16 Describe the hydrolysis of salts in aqueous solution and predict whether a slat solution will be acidic, basic or neutral V-17 Recognize Lewis acids and bases and how they react V-18 Calculate the percent ionization (or percent hydrolysis) of a weak acid (or a weak base) from ph value and the acid (or the base) initial concentration V-19 Calculate K a of a weak acid (or K b of a weak base) from ph value and percent ionization (or percent hydrolysis) of that acid (or that base) V-20 Explain the dilution effect on the percent ionization (or hydrolysis) of a weak acid (or a weak base)

10 CHEM-1310 Summer 2010 Syllabus Page 10 of 10 V-21 Describe the effect of common ions on the percent ionization of weak acids and bases V-22 Explain how buffers maintain ph, how they are prepared, and the importance of buffer capacity V-23 Calculate the ph of a buffer solution, given the concentrations of weak acid or base and their salts V-24 Use the Henderson-Hasselbalch equation to calculate the ph of a buffer V-25 Determine the ph of a buffer solution after the addition of small amounts of strong acids or bases V-26 Interpret acid-base curves, and calculate the ph of the titrate solution at various stages of the titration V-27 Choose the correct indicator for a particular acid-base titration V-28 Explain how acid rain is formed and its effects on the environment V-29 Relate a K sp expression to its chemical equation V-30 Calculate the solubility product constant of a salt, given its solubility, and vice versa V-31 Describe the factors affecting the aqueous solubility of ionic compounds V-32 Apply Le Chatelier s principle to the common ion effect V-33 Calculate the solubility of a salt in a solution containing an ion common to that salt V-34 Predict the effect of ph on the solubility of a salt V-35 Predict whether a precipitate will form when two solutions of a salt are mixed Laboratory program: General: Approx. every second day. By the end you should be able to: (1) collect and process your data from experiments; (2) use graphical means to test chemical behaviour models; (3) write reports; (4) estimate error Textbook sections: Expt #1: sections 4.2, 4.3, Wet-lab Expt #2: sections 4.4, 4.8, Wet-lab Expt #3: sections 6.3, , Virtual lab Expt #4: sections 6.3, , Wet-lab Expt #5: sections 4.4, 13.2, 13.3, 13.5, Wet-lab Expt #6: sections 16.2, 16.3, Virtual lab Expt #7: sections 15.4, 15.5, 15.8, 15.9, 16.4, Virtual lab Expt #8: sections , , Wet-lab