CHEM2011 Physical Chemistry: Molecules, Energy and Change · 2014. 1. 15. · Component HPW Time Day Location Lectures 2 or 3 per week, see schedule (weeks 1 – 12) Lecture 1 1 5

FACULTY OF SCIENCE

SCHOOL OF CHEMISTRY

CHEM2011

Physical Chemistry: Molecules, Energy and Change

SEMESTER 1, 2014

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!

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Faculty of Science - Course Outline

1. Information about the Course NB: Some of this information is available on the UNSW Virtual Handbook1

Year of Delivery 2014 Course Code CHEM2011

Course Name Physical Chemistry: Molecules, Energy, and Change

Academic Unit School of Chemistry

Level of Course Second year

Units of Credit 6UoC

Session(s) Offered S1 only Assumed Knowledge, Prerequisites or Co-requisites

CHEM1011 or CHEM1031 or CHEM1051, AND CHEM1021 or CHEM1041 or CHEM1061, AND MATH1011 or MATH1031 or MATH1131 or MATH1141 or MATH1231 or MATH1241

Hours per Week 6

Number of Weeks 13 weeks

Commencement Date 3 March 2014 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 1 1 5 – 6 pm Mon. Chem. Sci. M11 Lecture 2 1 1 – 2 pm Tue. Chem. Sci. M10 Lecture 3 1 3 – 4 pm Thu. Law G23 Laboratory 3 Lab – Option 1 2 – 5 pm Mon. Chem. Sciences 162/165 Lab – Option 2 9 am – 12 pm Tue. Chem. Sciences 162

Tutorials 1 per week in designated weeks – see schedule

(in a lecture timeslot) see schedule

Online Other activities, e.g., field trips TOTAL 6

Special Details Laboratory activities are held in weeks 2 – 12 only. Lectures in weeks 1 – 12. NOTE: Lecture venues may change close to the start of semester, please check myUNSW to get the latest and authoritative details.

1 UNSW Online Handbook: http://www.handbook.unsw.edu.au

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2. Staff Involved in the Course

Staff Role Name Contact Details Consultation Times Course Convenor Dr R. Haines Dalton 128, ext. 54718,

[email protected] by prior arrangement via email

Additional Teaching Staff

Lecturers & Facilitators Dr L. Aldous Dalton 132, ext. 54656, [email protected]

by prior arrangement via email

Dr J. B. Harper Dalton 223, ext. 54692 [email protected]

by prior arrangement via email

Tutors & Demonstrators Prof. S. Kable Assoc. Prof. T. Schmidt + others TBA

Dalton 134, [email protected] Dalton 217, [email protected]

Technical & Laboratory Staff

B. Litvak S. Videnovic L. Cuba–Chiem

Chem. Sciences 239, ext. 54722 Chem. Sciences 137, ext. 54665 Chem. Sciences 239, ext. 54722

Other Support Staff

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3. Course Details

Course Description2 (Handbook Entry)

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.

Course Aims3

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.

Student Learning Outcomes4

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)

apply thermodynamics to a variety of chemical problems including important industrial processes (e.g. ammonia synthesis, steam reforming, blast furnace,

HCN synthesis, methanol synthesis …) the decomposition temperature of oxides, carbonates, etc.; the stability of hydrates 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 the rotation of objects, the general form of the rotational wavefunctions and boundary conditions for 2D and 3D rotation. For diatomic molecules, be able to calculate the moment of inertia and rotational constant and qualitatively sketch a pure rotational spectrum including the intensity 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

2 UNSW Handbook: http://www.handbook.unsw.edu.au 3 Learning and Teaching Unit: Course Outlines 4 Learning and Teaching Unit: Learning Outcomes

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mass, overtone, hot band, combination band, rigid rotor. Be able to calculate the ro-vibrational energies of diatomic molecules within the harmonic oscillator approximation. Describe the appearance of a ro-vibrational spectrum including labelling the P–, Q–, R–, and S–branches. Use the ro-vibrational spectrum to calculate rotational constants, and force constants. Be able to interpret the vibrational spectra of polyatomic molecules in terms of normal modes.

describe the interpretation of the partition function; given the algebraic expressions, be able to calculate the translational, vibrational and rotational partition functions. Be able to express the molecular partition function in terms of the translational, rotational, vibrational and electronic partition functions. Starting from appropriate algebraic expressions calculate thermodynamic quantities (internal energy, entropy, Gibbs energy, equilibrium constant) from the partition function.

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

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; Display an understanding of the movement of ions in an electrolyte, including the concepts: conductivity, mobility, transport; explain how conductivity measurements are made; state the Kohlrausch law and the law of independent migration of ions; determine equilibrium constants for dissociation for weak electrolytes and sparingly soluble salts from conductivity measurements

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

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Graduate Attributes Developed in this Course5 Science Graduate Attributes5

Select the level of

FOCUS 0 = NO FOCUS 1 = MINIMAL 2 = MINOR 3 = MAJOR

Activities / Assessment

Research, inquiry and analytical thinking abilities

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: http://www.science.unsw.edu.au/our-faculty/science-graduate-attributes

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Major Topics (Syllabus Outline)

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. Application to selected industrial and biological processes. 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. Statistical Mechanics: the Boltzmann distribution and the partition function; interpretation of the partition function; the translational, vibrational and rotational partition functions. Calculation of thermodynamic quantities (internal energy, entropy, Gibbs energy, equilibrium constant) from the partition function. 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. Conductance and resistance; conductivity and molar conductivity; Kohlrausch Law, law of independent migration of ions, ionic conductivity, mobility, transport number; applications – acid dissociation constant, solubility, detection in ion chromatography. 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. rate constants and equilibrium constants. Introduction to molecular reaction kinetics: collision theory.

Relationship to Other Courses within the Program

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

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.

Rationale for learning and teaching in this course6,

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 student-lecturer 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 7http://teaching.unsw.edu.au/guidelines

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5. Course Schedule Some of this information is available on the Online Handbook8 and the UNSW Timetable9.

Week

Lectures (day), Topics & Lecturers

Tutorials (day), Topics & Lecturers

Practical (day), Topics & Lecturers

Other

Assignment and Submission dates (see also 'Assessment Tasks & Feedback')

Week 1

Mon, Tue, Thu: Thermodynamics, Dr Haines

(no lab classes)

Week 2

Mon, Tue: Thermodynamics, Dr Haines Thu: Thermodynamics, Dr Haines

Mon/Tue: Introduction to laboratory and using spreadsheets

Take home assignment due 14 March

Week 3


Mon/Tue: Calorimetry (CL1)


Week 4


In lab class: Thermodynamics problems

Mon/Tue: Lab report writing Workshop and Thermodynamics problems


Week 5

Mon, Tue, Thu: Quantum and Spectroscopy, Dr Haines

Mon/Tue: Vapour pressure (T3)

Take home assignment due 4 April

Week 6 *

Mon, Tue, Thu: Quantum and Spectroscopy, Dr Haines

Mon/Tue: Enthalpy of solution (T1)


Week 7

Mon: Quantum and Spec., Dr Haines Thu: Electrochemistry, Dr Aldous

Tue: Quantum. Dr Haines Mon/Tue: Particle in a box (Q1)


Week 8

Mon, Tue, Thu: Electrochemistry, Dr Aldous Mon/Tue mid-semester test

Take home assignment due 2 May

Week 9

Mon, Tue, Thu: Electrochemistry, Dr Aldous Mon/Tue: Electrochemical cells (E3)


Week 10

Tue, Thu: Chemical kinetics, Dr Harper Mon: Electrochemistry, Dr Haines

Mon/Tue: Solution conductivity (E1)


Week 11

Mon, Tue, Thu: Chemical kinetics, Dr Harper

Mon/Tue: Reaction kinetics (R1A)


Week 12

Mon, Tue: Chemical kinetics, Dr Harper Thu: Kinetics, Dr Haines Mon/Tue: Reaction kinetics (R1B)


Week 13

Mon, Tue, Thu: no lectures (no lab classes)

Take home assignment due 6 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'

8 UNSW Online Handbook: http://www.handbook.unsw.edu.au 9 UNSW Timetable: http://www.timetable.unsw.edu.au/

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6. Assessment Tasks and Feedback10

Task

Knowledge & abilities assessed

Assessment Criteria

% of total mark

Date of

Feedback

Release

Submission

WHO

WHEN

HOW

Personalised take-home assignments

Concepts in thermodynamics (weeks 2-5), quantum chemistry (weeks 6, 7), electrochemistry (weeks 8 – 10), and kinetics (weeks 11 – 13)

Correct calculation of answers to numerical assignment problems.

10% Monday 9 am, weeks 2 – 13

Friday 5 pm of week released

software (web) immediate marks, correct answers

Pre-lab exercises

Theory and skills for carrying out practical work as set out in the aims and introduction for that week's experiment

Correct answers to short–answer questions and calculations.

10% start of semester

start of lab class assigned to that experiment

Demonstrator first hour of lab class

mark, comments, corrected answers

Laboratory reports

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.

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.

20% start of semester

end of laboratory class assigned to that experiment

Demonstrator start of following lab class

mark, comments, corrected answers

In-semester test

Skills and topics covered in Thermodynamics lectures

Correct answers to short answer questions and calculations.

15% lab time in week 8

60 minutes after release

Course coordinator

conclusion of test and then within one week of test

marks, comments on answers

Final examination

Skills and topics covered in quantum, electrochemistry and kinetics sections.

Correct answers to questions and calculations.

45% as per final examination timetable

as per final examination timetable

UNSW Examinations

as per final examination timetable

incorporated into final overall mark for course

To pass CHEM2011 you must meet ALL of these requirements: * An attendance record of at least 80% at scheduled classes. * A total mark of 50 or more. * A mark of 21 or more (out of 60) in the examination + test component. * A mark of 15 or more (out of 30) in the Laboratory Program (laboratory reports + pre–lab exercises). Supplementary examinations may be offered for academic or other reasons. Students are expected to make themselves available for these should they require them. For semester 1 courses these are typically held in the week preceding semester 2.

10 Approaches to assessment: http://teaching.unsw.edu.au/assessment

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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 http://www.chemistry.unsw.edu.au/current-students/undergraduate/socs

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

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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

2007 (as result of change to 12 week semester) 2009 2010

Changes to the way students acknowledge their reading of OH & S information in student manual. Reduction in amount of practical work. Redesign of report sheets to make lab report writing easier and faster. 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.

CATEI11

Course - 2013 Teaching - 2013

97% 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. 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: http://www.science.unsw.edu.au/our-faculty/course-and-teaching-evaluation-and-improvement-catei

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10. Administration Matters

Expectations of Students

A minimum of 80% attendance at laboratory classes is required to be considered for a pass in CHEM2011. (See other requirements to pass in the assessment section above.) All computer use is subject to the Acceptable Use of UNSW IT Resources policy .

Assignment Submissions

Assignments in CHEM2011 are submitted and graded electronically. Laboratory reports are submitted in the laboratory class in which they are completed.

Occupational Health and Safety12

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.

Assessment Procedures UNSW Assessment Policy13

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.

Equity and Diversity

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 (9385 4734 or http://www.studentequity.unsw.edu.au/. 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 Policy14

School Contact

Faculty Contact

University Contact

Dr Jason Harper Dalton Building room 223 [email protected] Tel: 9385 4692

A/Prof Julian Cox Associate Dean (Education) [email protected] Tel: 9385 8574 or Dr Gavin Edwards Associate Dean (Undergraduate Programs) [email protected] Tel: 9385 8063

Student Conduct and Appeals Officer (SCAO) within the Office of the Pro-Vice-Chancellor (Students) and Registrar. Telephone 02 9385 8515, email [email protected] University Counselling and Psychological Services15 Tel: 9385 5418

12 UNSW OHS Home page 13 UNSW Assessment Policy 14 Student Complaint Procedure 15 University Counselling and Psychological Services

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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: www.lc.unsw.edu.au/plagiarism 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

Documents

CHEM2011 Physical Chemistry: Molecules, Energy and Change · 2014. 1. 15. · Component HPW Time Day Location Lectures 2 or 3 per week, see schedule (weeks 1 – 12) Lecture 1 1 5