CHEM2011. Physical Chemistry: Molecules, Energy and Change

Transcription

1 FACULTY OF SCIENCE SCHOOL OF CHEMISTRY CHEM2011 Physical Chemistry: Molecules, Energy and Change SEMESTER 1, 2015

2 Table of Contents 1. Information about the Course... 1! 2. Staff Involved in the Course... 2! 3. Course Details... 3! 4. Rationale and Strategies Underpinning the Course... 6! 5. Course Schedule... 7! 6. Assessment Tasks and Feedback... 8! 7. Additional Resources and Support... 9! 8. Required Equipment, Training and Enabling Skills... 9! 9. Course Evaluation and Development... 10! 10.! Administration Matters... 11! 11.! UNSW Academic Honesty and Plagiarism... 12!

3 Faculty of Science - Course Outline 1. Information about the Course NB: Some of this information is available on the UNSW Virtual Handbook 1 Year of Delivery Course Code Course Name Academic Unit Level of Course Units of Credit Session(s) Offered Assumed Knowledge, Prerequisites or Corequisites 2015 CHEM2011 Physical Chemistry: Molecules, Energy, and Change School of Chemistry Second year 6UoC S1 only Hours per Week 6 Number of Weeks 13 weeks Commencement Date CHEM1011 or CHEM1031 or CHEM1051, AND CHEM1021 or CHEM1041 or CHEM1061, AND MATH1011 or MATH1031 or MATH1131 or MATH1141 or MATH1231 or MATH March 2015 Summary of Course Structure (for details see 'Course Schedule') Component HPW Time Day Location Lectures 2 or 3 per week, see schedule (weeks 1 12) Lecture pm Mon. Old Main Building 230 Lecture pm Wed. Old Main Building 230 Lecture pm Fri. Old Main Building 230 Laboratory 3 Lab Option am Mon. Chem. Sciences 165 Lab Option pm Mon. Chem. Sciences 162/165 Tutorials 1 per week in designated weeks (in a lecture timeslot) see schedule see schedule Online Other activities, e.g., field trips TOTAL 6 Laboratory activities are held in weeks 2 12 only. Lectures in weeks NOTE: Lecture venues Special Details may change close to the start of semester, please check myunsw to get the latest and authoritative details. 1 UNSW Online Handbook: 1

4 2. Staff Involved in the Course Staff Role Name Contact Details Consultation Times Course Convenor Dr R. Haines Dalton 128, ext , by prior arrangement via Additional Teaching Staff Lecturers & Facilitators Dr L. Aldous Dalton 132, ext , Dr J. B. Harper Dalton 223, ext Prof. T. Schmidt Dalton 217, Prof. M. Stenzel Dalton 226, Tutors & Demonstrators Assoc. Prof. J. Dalton 131, Stride by prior arrangement via by prior arrangement via by prior arrangement via by prior arrangement via Technical & Laboratory Staff Other Support Staff Assoc. Prof. C. Zhao + others TBA B. Litvak S. Videnovic Dalton 127, chuan.zhao@unsw.edu.au Chem. Sciences 239, ext Chem. Sciences 137, ext

5 3. Course Details Course Description 2 (Handbook Entry) Course Aims 3 Student Learning Outcomes 4 Physical Chemistry seeks to explain chemical processes in terms of energy changes and the molecular nature of matter. This course introduces quantum mechanics and its role in determining the energies of atoms and molecules, followed by the laws of thermodynamics and their applications in chemistry, then links the two approaches with an introduction to statistical thermodynamics. The applications of thermodynamics to electrochemical processes are described, along with examples of practical importance in the areas of corrosion and the electrochemical cells. To complete the physical basis for understanding chemical reactions the factors affecting reaction rates, the role of reaction mechanisms, and molecular theory of reaction rates are described. CHEM2011 focuses on the principles of chemical thermodynamics, equilibrium electrochemistry, quantum mechanics and statistical mechanics, and chemical kinetics. A working knowledge of these is essential for an understanding of the conditions and techniques used to bring about chemical changes in industry and in the laboratory and for understanding all chemical reactions, including those in the environment and living organisms. On completion of CHEM2011 you should be able to: correctly use the language of thermodynamics (including such terms as: system, surroundings, state; change, path, process, adiabatic, isothermal, reversible; state function, internal energy, enthalpy, entropy, Gibbs function) apply U(T,V) and H(T, p) to simple problems involving changes in p,v,t (including the expansion of a perfect gas under various conditions) describe the measurement of the standard enthalpy change of combustion and of reaction define and use of standard enthalpy changes including fusion, vaporisation, sublimation; reaction, combustion, atomisation; standard enthalpy of formation; average bond enthalpies define entropy S, describe its determination (including the 3rd law) calculate the dependence of S on T (all substances) and on p and V (perfect gas only) describe the role of the zeroth, 1st, 2nd and 3rd laws in the development of chemical thermodynamics define the Gibbs function G and the chemical potential µ use tabulated data to estimate of H, U, S, G for chemical and physical processes describe and use thermodynamic criteria for spontaneous physical and chemical changes, for equilibrium apply thermodynamics to phase equilibrium problems including stability of the phases of a pure substance (including the pressure and temperature dependence of the stability) phase diagrams of pure substances (application of the Clapeyron and Clausius- Clapeyron equations) write down and use the thermodynamic formulation of the mass action law for equilibria involving gases, liquids, solutions, solids (activities and standard states introduced on an ad hoc basis) describe the postulates of quantum mechanics and their implications for experimental measurements. apply quantum mechanical principles to the 'particle in a box' system and list applications of the results. Sketch wavefunctions and calculate energy levels for particle in a box. correctly use the language of spectroscopy, including terms such as: ground state, excited state, degeneracy, resonance, transition moment, gross selection rule, specific selection rule, allowed transition, forbidden transition, Raman scattering, Stokes and anti-stokes scattering, Born-Oppenheimer approximation, Boltzmann distribution. describe the application of quantum mechanics to vibrational motion. Be able to calculate the vibrational frequency of a diatomic molecule. correctly use the terms: harmonic oscillator, anharmonic oscillator, force constant, reduced mass, overtone, hot band, combination band, rigid rotor. Be able to calculate the rovibrational energies of diatomic molecules within the harmonic oscillator approximationand describe the effects of anharmonicity. Be able to interpret the vibrational spectra of polyatomic molecules in terms of normal modes. correctly use the language of electrochemistry including: kinds of electrodes, components of cells, cell diagrams and notation, electrode potentials and sign convention display an understanding of the relation between electrochemistry and thermodynamics including: equations that relate thermodynamic quantities to electrochemically-measurable 2 UNSW Handbook: 3 Learning and Teaching Unit: Course Outlines 4 Learning and Teaching Unit: Learning Outcomes 3

6 quantities; the Nernst equation show an understanding of the chemistry and thermodynamics of electrolyte solutions; define activity and activity coefficient; quote and use the Debye-Hückel limiting equation, state the limitations of the limiting law and give extensions; describe a battery and explain the electrochemistry of power generation; give examples of different kinds of batteries; describe a fuel cell and give examples of fuel cells; show an understanding of the characteristics of a battery that determine its uses and limitations; describe corrosion of metals, in particular corrosion of iron; explain why corrosion is an electrochemical phenomenon and discuss the kinetics and thermodynamics of corrosion; give examples of corrosion and approaches to limiting corrosion. correctly use the language of chemical kinetics including: rate, rate law, order, molecularity, elementary and overall reaction, half-life; isolation method, pseudo-order, rate determining step, reactive intermediate, steady state approximation; mechanism; activation energy, frequency factor; catalyst; potential energy surface, reaction coordinate, steric factor, transition state. define the (true) rate in terms of the rate of change in any reactant or product establish the connection between the observable used to monitor the progress of the reaction and the variable in the rate equation use experimental data to propose and/or verify a rate law and determine the rate constant using: the method of initial rates (the isolation method) integrated rate equations for 1st order and simple cases of 2nd order reactions integrated rate equations for such other cases for which the appropriate equations are supplied define the half-life of a reactant and, for first and 2nd order reactions, relate it to rate constant derive a rate law from a hypothetical reaction mechanism (simple case only) define the rate determining step, describe and use the steady state approximation relate the equilibrium constant for the overall reaction to rate constants for individual steps use the Arrhenius equation to describe the variation of rate constants with temperature describe: the role of catalysts in altering the reaction rate interpret data for enzyme catalysed reactions in terms of the Michaelis-Menten mechanism describe the derivation of expressions for the rate constant according to collision theory and be able to use such expressions to calculate rate constants. correctly use the terms: collision cross section, reduced mass, steric factor, reactive cross section, potential energy surface in the context of polymerization reactions: be able to describe the reaction steps that govern step-growth and chain-growth reactions be able to list various initiation modes and calculate their rate of degradation and initiation be able to summarize the parameters that affect rate of initiation, propagation, chain transfer and termination be able to calculate the rate of propagation from parameters given be able to derive the equation for the rate of polymerization from the rate of initiation, propagation, chain transfer and termination be able to discuss what drives polymerizations from a thermodynamic point of view be able to use the Mayo Equation and discuss the effects of different modes of chain transfer on the degree of polymerization be able to discuss how rate constants affect the composition of the polymer be able to use the copolymer composition equation and understand the meaning of reactivity ratios be able to describe the equations that govern the rate of reaction of step-growth polymerizations be able to compare step-growth and chain-growth polymerization 4

7 Graduate Attributes Developed in this Course 5 Science Graduate Attributes 5 Research, inquiry and analytical thinking abilities Select the level of FOCUS 0 = NO FOCUS 1 = MINIMAL 2 = MINOR 3 = MAJOR Activities / Assessment 3 Didactic lecture, laboratory experiment, take home problems, laboratory preparation, self-assessed short problem solving in class/problem solving assignments, short answer questions, written reports, short answer and essay responses Capability and motivation for intellectual development 2 Didactic lecture, laboratory experiment, self-assessed short problem solving in class/problem solving assignments, short answer questions, written reports, short answer and essay responses Ethical, social and professional understanding 2 Laboratory preparation/short answer responses Communication 3 Laboratory experiment/ short answer responses Teamwork, collaborative and management skills 2 Laboratory experiment/ short answer responses Information literacy 1 Laboratory preparation/ short answer responses 5 Contextualised Science Graduate Attributes: 5

8 Major Topics (Syllabus Outline) Relationship to Other Courses within the Program Thermodynamics: zero'th, 1st, 2nd and 3rd laws of thermodynamics. Internal energy, enthalpy, entropy, Gibbs function, chemical potential. Thermodynamic properties of the perfect gas. Useful approximations for gases, liquids and solids. The measurement of thermodynamic quantities. Hess' law, Kirchoff's law; spontaneous changes, physical and chemical equilibrium; Clapeyron, Clausius-Clapeyron and van't Hoff equations, le Chatelier principle. Postulates of quantum mechanics; the wavefunction and its interpretation, Schrödinger equation, observables and operators. Example: particle in a box, energy levels, wavefunctions Principles of spectroscopy: types of spectroscopic experiment: emission versus absorption. photon frequency, wavenumber and energy; energy levels and transitions; typical spectra;, rotational, vibrational and electronic spectroscopy. Transition frequency/wavelength; intensity of transitions, populations (Boltzmann distribution) and transition moments, selection rules. Raman scattering, Stokes and anti Stokes lines, intensities. Quantum mechanics of molecular vibrations and vibrational spectroscopy. Electrochemistry: solutions of electrolytes; the activity of an ion in solution, activity coefficient; Debye-Hückel theory of ion activities. Redox reactions and electrochemistry; electrodes, half cells and cells; kinds of electrodes; cell and electrode notation; electrode potential and sign convention; current and the Faraday constant; galvanic cells and electrolytic cells; electrode potential and free energy; electrode potentials and ion activities - the Nernst equation; temperature effects, relationship of electrode potentials to: entropy change, enthalpy change, equilibrium constant. determination of thermodynamic quantities; batteries and fuel cells - construction, electrochemistry, examples; corrosion - electrochemistry, chemistry, kinetics, galvanic series, control by anodic and cathodic protection, galvanizing. Reaction rate defined, the rate law, rate constant, order. Elementary reactions, mechanism, rate determining step; relation to the rate law. Experimental determination of the rate law: the method of initial rates, methods using integrated rate equations for 1st order and for simple cases of 2nd order reactions; rate constants, half-life. Effect of temperature on reaction rates: the Arrhenius equation, activation energy, frequency factor. Complex reactions: opposing, consecutive and parallel reactions; catalysis and catalysts; enzyme catalysis, Michaelis-Menten mechanisms. Reaction kinetics and thermodynamics; rate constants and equilibrium constants. Introduction to molecular reaction kinetics: collision theory. Principles of radical polymerization: Thermodynamics of polymerizations, rate constants of radical polymerization including rate of initiation, rate of propagation, rate of termination, rate of change transfer; reactivity ratios of copolymerizations. Principles of polycondensation: kinetics of condensation reactions. CHEM2011 builds on the thermodynamics, electrochemistry and chemical kinetics introduced in first year chemistry courses and provides the basis for understanding the chemical processes and experimental techniques taught in third year chemistry courses. 4. Rationale and Strategies Underpinning the Course Teaching Strategies Rationale for learning and teaching in this course 6, Lectures present the factual content of the course and illustrative examples which include applications of the theory to specific situations. Since the lecture group is usually small there is opportunity for students to request clarification of issues. Laboratories provide additional illustrative examples of the material presented in lectures and develop data handling and presentation skills. Take home assignments include exercises which allow students to expand their comprehension of the course content. CHEM2011 is a content-rich course which introduces many concepts, the relations between those concepts and applications in all disciplines of chemistry. Lectures with immediate studentlecturer feedback provide the most time-effective way of introducing these concepts to students. Practical classes provide student-student interaction to facilitate co-operative learning and timely assessment of student work. Assessable personalised take-home assignments support and provide feedback for individual learning. 7 6 Reflecting on your teaching 7 6

9 5. Course Schedule Some of this information is available on the Online Handbook 8 and the UNSW Timetable 9. Week Lectures (day), Topics & Lecturers Tutorials (day), Topics & Lecturers Week 1 Mon, Wed, Fri: Thermodynamics, Dr Haines Week 2 Mon, Wed: Thermodynamics, Dr Haines Fri: Thermodynamics Week 3 Week 4 Mon, Wed, Fri: Thermodynamics, Dr Haines Mon, Thermodynamics, Dr Haines; Wed, Fri: Electrochemistry, Dr Aldous Mon, in lab class: Thermodynamics problems Practical (day), Topics & Lecturers (no lab classes) Mon: Introduction to laboratory and using spreadsheets Mon: Calorimetry (CL1) Mon: Lab report writing Workshop and Thermodynamics problems Other Assignment and Submission dates (see also 'Assessment Tasks & Feedback') Take home assignment due 13 March Take home assignment due 20 March Take home assignment due 27 March Week 5 Mon, Wed: Electrochemistry, Dr Aldous Mon: Vapour pressure (T3) Take home assignment due 2 April Week 6 * Mon, Wed: Electrochemistry, Dr Aldous Fri: Electrochemistry Mon: Enthalpy of solution (T1) Take home assignment due 17 April Week 7 Week 8 Mon, Wed, Fri: Quantum and Spec., Prof. Schmidt Mon, Wed, Fri: Quantum and Spec., Prof. Schmidt Mon: mid-semester test Mon: Particle in a box (Q1) Take home assignment due 24 April Take home assignment due 1 May Week 9 Mon, Wed, Fri: Chemical kinetics, Dr Harper Mon: Electrochemical cells (E3) Take home assignment due 8 May Week 10 Mon, Wed, Fri: Chemical kinetics, Dr Harper Mon: Reaction kinetics (R1A) Take home assignment due 15 May Week 11 Mon: Chemical kinetics, Dr Harper; Wed, Fri: Polymers, Prof. Stenzel Mon, in lab class: quantum and kinetics problems Mon: (2 hour tutorial on quantum and kinetics) Take home assignment due 22 May Week 12 Mon, Wed, Fri: Polymers, Prof. Stenzel Mon: Reaction kinetics (R1B) Take home assignment due 29 May Week 13 Mon: Polymers, Prof. Stenzel; Wed Fri: no lectures Mon: polymer problems (no lab classes) Take home assignment due 5 June *NB: As stated in the UNSW Assessment Policy: one or more tasks should be set, submitted, marked and returned to students by the mid-point of a course, or no later than the end of Week 6 of a 12-week session'

10 6. Assessment Tasks and Feedback 10 Task Knowledge & abilities assessed Assessment Criteria % of total mark Date of Feedback Release Submission WHO WHEN HOW Personalised takehome assignments Pre-lab exercises Laboratory reports In-semester test Final examination Concepts in thermodynamics (weeks 2-5), electrochemistry (weeks 6, 7), quantum chemistry (weeks 8, 9), and kinetics (weeks 10 12), polymers (week 13) Theory and skills for carrying out practical work as set out in the aims and introduction for that week's experiment Theory and skills as set out in the aims and introduction for each experiment; practical skills in the manipulation of laboratory equipment; data processing and presentation skills as set out in the student manual. Skills and topics covered in Thermodynamics and electrochemistry lectures Skills and topics covered in quantum, kinetics and polymer sections. Correct calculation of answers to numerical assignment problems. Correct answers to short answer questions and calculations. Accuracy and precision of experimental results; correctness of calculations; correct responses to short questions on interpretation of results; professional presentation of data in graphs and tables. Correct answers to short answer questions and calculations. Correct answers to questions and calculations. 10% Monday 9 am, weeks % start of semester 20% start of semester 20% lab time in week 7 40% as per final examination timetable Friday 5 pm of week released start of lab class assigned to that experiment end of laboratory class assigned to that experiment 60 minutes after release as per final examination timetable software (web) immediate marks, correct answers Demonstrator Demonstrator Course coordinator UNSW Examinations first hour of lab class start of following lab class conclusion of test and then within one week of test as per final examination timetable mark, comments, corrected answers mark, comments, corrected answers marks, comments on answers incorporated into final overall mark for course To be awarded a pass or higher grade in CHEM2011 you must meet ALL of these requirements: * Attendance at at least 80% at laboratory classes. * A total mark of 50 or more. * Satisfactory overall performance ( 35%, that is 21 out of 60) in the examination component (final examination + in semester test). * A mark of 50% (that is, 20 out of 40) in the continuous assessment tasks (assignments and laboratory pre-lab answers and reports), Failure to satisfy either of the last two criteria will result in an UF (Unsatisfactory Fail) grade being awarded, or further assessment being offered at the discretion of the course coordinator. Supplementary exams will take place in the week before the commencement of semester 2. Inability or failure to attend a supplementary examination will result in the original grade being confirmed. 10 Approaches to assessment: 8

11 7. Additional Resources and Support Text Books P.W. Atkins and J. DePaula, Elements of Physical Chemistry 6th edition 2013 (Oxford University Press) Blackman and Gahan: Aylward and Findlay's SI Chemical Data 7th edition 2014 (5th or 6th editions are OK) Available UNSW Library and Bookshop Course Manual Course manual available in print from UNSW Bookshop and as PDF from Moodle. Required Readings Readings from text as prescribed by lecturers. Additional Readings None Recommended Internet Sites < Societies Students of Chemistry Society (SOCS) - see Computer Laboratories or Study Spaces Dalton building G07 study area. 8. Required Equipment, Training and Enabling Skills Equipment Required Safety eyewear, laboratory coat, enclosed footwear. Students who wear spectacles are required to wear overglasses or goggles. Enabling Skills Training Required to Complete this Course Laboratory Safety and Ethics from CHEM1011 or CHEM1031 or CHEM1051 9

12 9. Course Evaluation and Development Student feedback is gathered periodically by various means. Such feedback is considered carefully with a view to acting on it constructively wherever possible. This course outline conveys how feedback has helped to shape and develop this course. Mechanisms of Review Last Review Date Comments or Changes Resulting from Reviews Major Course Review Changes to the content of the course (quantum mechanics and spectroscopy added, surface chemistry removed) and timing (delivered in semester 1) to improve integration with other core chemistry courses at second and third year. Change to new, more student-friendly textbook better focused on the course content. CATEI 11 Course Teaching % of students expressed satisfaction with the overall quality of the course. Some students requested positive as well as negative feedback on lab reports, and more concise lab notes. Other New for 2013: Changes to laboratory report forms to improve visibility of feedback from demonstrators. Portions of laboratory manual rewritten to improve clarity. Streamlined use of Excel by re-using spreadsheet from the introductory excel exercise in later experiments to reduce time required to complete laboratory reports. New for 2014: More detailed feedback on laboratory reports, including grading of aspects of the report on a poor to perfect scale. Workshop on report writing early in the semester. Rewriting of experimental procedures to be more economic with words. New for 2015: Restructure of content to integrate better with other second year chemistry courses, and to include polymer chemistry. The Student manual includes this inside the front cover: "Please advise the author or any member of the teaching staff of any corrections or suggestions for improvements to this manual. If you find anything unclear or inaccurate please let us know." All responses to this request are considered each year in revising the Student manual for the following year. 11 CATEI process: 10

13 10. Administration Matters Expectations of Students Assignment Submissions Occupational Health and Safety 12 Assessment Procedures UNSW Assessment Policy 13 Equity and Diversity A minimum of 80% attendance at laboratory classes is required to be considered for a pass in CHEM2011. IMPORTANT - a full description of the requirements to pass this course is in the assessment section (6) above. All computer use is subject to the Acceptable Use of UNSW IT Resources policy < Assignments in CHEM2011 are submitted and graded electronically. Laboratory reports are submitted in the laboratory class in which they are completed. All students should be aware of the UNSW Occupational Health and Safety policies available at UNSW:< Risk assessments for laboratory experiments are provided in the Student Manual. Any student who feels their performance may be affected by illness or misadventure should submit the required documentation to UNSW Student Central and advise the CHEM2011 course coordinator that they have done so. Those students who have a disability that requires some adjustment in their teaching or learning environment are encouraged to discuss their study needs with the course Convenor prior to, or at the commencement of, their course, or with the Equity Officer (Disability) in the Equity and Diversity Unit ( or Issues to be discussed may include access to materials, signers or note-takers, the provision of services and additional exam and assessment arrangements. Early notification is essential to enable any necessary adjustments to be made. Grievance Policy 14 School Contact Faculty Contact University Contact Dr Jason Harper Dalton Building room 223 j.harper@unsw.edu.au Tel: A/Prof Chris Tisdell Associate Dean (Education) cct@unsw.edu.au Tel: or Dr Gavin Edwards Associate Dean (Undergraduate Programs) g.edwards@unsw.edu.au Tel: Student Conduct and Appeals Officer (SCAO) within the Office of the Pro-Vice- Chancellor (Students) and Registrar. Telephone , studentcomplaints@unsw.edu. au University Counselling and Psychological Services 15 Tel: UNSW OHS Home page 13 UNSW Assessment Policy 14 Student Complaint Procedure 15 University Counselling and Psychological Services 11

14 11. UNSW Academic Honesty and Plagiarism What is Plagiarism? Plagiarism is the presentation of the thoughts or work of another as one s own. *Examples include: direct duplication of the thoughts or work of another, including by copying material, ideas or concepts from a book, article, report or other written document (whether published or unpublished), composition, artwork, design, drawing, circuitry, computer program or software, web site, Internet, other electronic resource, or another person s assignment without appropriate acknowledgement; paraphrasing another person s work with very minor changes keeping the meaning, form and/or progression of ideas of the original; piecing together sections of the work of others into a new whole; presenting an assessment item as independent work when it has been produced in whole or part in collusion with other people, for example, another student or a tutor; and claiming credit for a proportion a work contributed to a group assessment item that is greater than that actually contributed. For the purposes of this policy, submitting an assessment item that has already been submitted for academic credit elsewhere may be considered plagiarism. Knowingly permitting your work to be copied by another student may also be considered to be plagiarism. Note that an assessment item produced in oral, not written, form, or involving live presentation, may similarly contain plagiarised material. The inclusion of the thoughts or work of another with attribution appropriate to the academic discipline does not amount to plagiarism. The Learning Centre website is main repository for resources for staff and students on plagiarism and academic honesty. These resources can be located via: The Learning Centre also provides substantial educational written materials, workshops, and tutorials to aid students, for example, in: correct referencing practices; paraphrasing, summarising, essay writing, and time management; appropriate use of, and attribution for, a range of materials including text, images, formulae and concepts. Individual assistance is available on request from The Learning Centre. Students are also reminded that careful time management is an important part of study and one of the identified causes of plagiarism is poor time management. Students should allow sufficient time for research, drafting, and the proper referencing of sources in preparing all assessment items. * Based on that proposed to the University of Newcastle by the St James Ethics Centre. Used with kind permission from the University of Newcastle Adapted with kind permission from the University of Melbourne 12