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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
2
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
3
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. Use Dirac bracket notation. State and prove the variation principle and explain its importance in obtaining approximate solutions to the Schrodinger equation.
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 construction of a typical laser and the common energy level schemes used in practical lasers and describe the characteristics and applications of laser radiation.
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
2 UNSW Handbook: http://www.handbook.unsw.edu.au 3 Learning and Teaching Unit: Course Outlines 4 Learning and Teaching Unit: Learning Outcomes
4
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
mass, overtone, hot band, combination band, rigid rotor. Use a Birge–Sponer plot to obtain the dissociation energy. Be able to calculate the ro-vibrational energies of diatomic molecules within the harmonic oscillator approximation and describe the effects of anharmonicity. 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
5
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
6
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
7
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, Thu: Thermodynamics, Dr Haines
Mon/Tue: Calorimetry (CL1)
Take home assignment due 21 March
Week 4
Mon, Tue, Thu: Thermodynamics, Dr Haines
In lab class: Thermodynamics problems
Mon/Tue: Lab report writing Workshop and Thermodynamics problems
Take home assignment due 28 March
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)
Take home assignment due 11 April
Week 7
Mon: Quantum and Spec., Dr Haines Thu: Electrochemistry, Dr Aldous
Tue: Quantum. Dr Haines Mon/Tue mid-semester test
Take home assignment due 17 April
Week 8
Mon, Tue, Thu: Electrochemistry, Dr Aldous Mon/Tue: Particle in a box (Q1)
Take home assignment due 2 May
Week 9
Mon, Tue, Thu: Electrochemistry, Dr Aldous Mon/Tue: Electrochemical cells (E3)
Take home assignment due 9 May
Week 10
Tue, Thu: Chemical kinetics, Dr Harper Mon: Electrochemistry, Dr Haines
Mon/Tue: Solution conductivity (E1)
Take home assignment due 16 May
Week 11
Mon, Tue, Thu: Chemical kinetics, Dr Harper
Mon/Tue: Reaction kinetics (R1A)
Take home assignment due 23 May
Week 12
Mon, Tue: Chemical kinetics, Dr Harper Thu: Kinetics, Dr Haines Mon/Tue: Reaction kinetics (R1B)
Take home assignment due 30 May
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/
8
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 be awarded a pass or higher grade in CHEM2011 you must meet ALL of these requirements: * An attendance record of 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: http://teaching.unsw.edu.au/assessment
9
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
<http://www.oxfordtextbooks.co.uk/orc/echem6e/>
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
10
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
11
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 <https://www.it.unsw.edu.au/students/policies/>.
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:<http://www.ohs.unsw.edu.au/>. 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
12
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
