Chem 1 Handbook - School of Chemistry - University of Glasgow

Chemistry-1
Course Handbook
2008 – 2009
1

FOREWORD
Welcome to first year Chemistry. Whether your intention is to stay with us to
complete an Honours B.Sc. or an M.Sci. degree in one of the Chemistry options, or to study
for some other degree, we hope you will enjoy and benefit from your time spent studying
chemistry.
The Chemistry-1 course has been designed to be both useful and interesting to all
students by providing a firm basis for later courses in Chemistry and other subjects. The
Chemistry-1 course is not easy; no course at University should be easy. It is challenging
and will be a major change from school/college chemistry. The onus is on you to read,
discuss and practise during the year. In addition to lectures and laboratory courses, you will
be required to attend problem sessions, which are intended to help you to understand the
concepts, to discuss these and to practice them by answering appropriate questions.
At university, with the large classes, you will have to organise your study time,
check your progress and, if you have difficulties, ask for help. Nobody is penalised for
asking for help or further explanation. The staff are here to help you, but we can only help if
we know you have a problem. There are regular voluntary tutorials where you can ask
questions. You can also ask the lecturer or any member of staff in problem session or
laboratory if you require help. For any matters relating to administration or personal
problems please consult the class head, Prof Bob Hill.
It is essential that you read this Handbook carefully and thoroughly. I would draw
your attention, particularly, to the sections dealing with the Award of Credits and Absence. It
is important that we have full details of any absences through illness or other problems
during the year in order that these may be taken into account in the assessment of your
work at the end of the course.
I am sure that you will find the Chemistry-1 course interesting
and enjoyable and that you will be successful at the end of the course. I look forward to
welcoming many of you into the Chemistry-2 course in a year’s time.
Professor S D Jackson
Head of Department of Chemistry
2

CONTENTS
3 Course Aims
4 Enrolment and Cost of Manuals
4 Teaching and Learning
5 Assessment and Examinations
6 Class Tests
6 Absence from Classes
7 Laboratory Work
8 Problem Solving Sessions
9 Tutorials, Class Notices
9 Grade point averages - guidelines
10 Staff-Student Committee, Alchemists, Beyond Chemistry - 1
11 Chemistry Beyond Level -2
12 Office Numbers, Books
13 Timetable
14-24 Lecture Content and Objectives
25-31 January 2008 Class Examination Paper
COURSE AIMS
to
to
to
to
to
to
broaden students' knowledge of the facts, theories, concepts, applications,
development and importance of chemistry;
enhance skills in - handling numbers, units, equations, diagrams and abstract ideas;
analysing data; prioritising information; making deductions; taking decisions;
making and justifying proposals; and in communicating and reporting clearly;
provide a sound basis for those students who may decide to proceed to Honours in
chemistry or a related science.
encourage interest in the subject and its interaction with other sciences;
give experience in the safe and accurate handling of chemical substances and
apparatus;
encourage development of learning strategies;
3

ENROLMENT
All students in the class must register, complete a class enrolment form and pay a fee of
£10 (collected in the lab in week 3) for the lab manuals, safety glasses and other materials
provided.
TEACHING AND LEARNING
LECTURES
There are 75 lectures, given Monday to Thursday and some Fridays
over 22 weeks. The class meets in two sections, one at 10 a.m. and
one at 3 p.m., in the Joseph Black Building Main Lecture Theatre (B4-
19). It is important to only go to the lectures at the time allocated to
you (once labs have been assigned).
Enter the Department by the central entrances.
Come in at the back of the theatre (level 5) and go out at the front of
the theatre (level 4).
Lectures provide facts, theories, demonstrations, textbook references
and background. An outline timetable is given on page 13 of this
Handbook. Guidance is also given on what you should be able to do
(Objectives) by the end of each group of lectures from pages 14 to
24.
PROBLEM
SESSIONS
LABORATORY
LEARNING
On some days the lecture time is used for problem-solving
workshops. Supplementary problems will be provided for you to work
on at home. More details are given on page 8.
Each student will attend one three-hour laboratory class per week
starting in week 4. Lab times are M, Tu, W, Th 2 - 5 and Tu, W, Th, F
10 - 1. You will be assigned a day and told your bench and first
experiment number. More details are given on page 7.
Involves all of these plus text books (see page 12), private study and
practice, general reading and discussion.
In lectures try to note down what is on the board or screen and as much as you can of the
key points of what is said. As soon as possible fill out your notes from memory, by
collaborating with a friend and by looking up books to reconstruct the full story.
We know that you will not always understand topics fully during the lecture. Later reading,
digestion, discussion and practice are needed. Book references will be given in lectures.
Look them up and incorporate diagrams, examples etc. from them into your notes.
Keep the lecture notes safe, in a binder with your name and class. Lecturers cannot provide
copies of lecture notes and it is expensive to photocopy other students' notes if you lose
yours and they can never be as good as your own. Students who “skip” lectures often find it
very difficult to catch up with their work. The purpose of a lecture is to help you understand
the material - not just to give you a set of notes. So attendance at all lectures helps you
to understand the chemistry.
4

ASSESSMENT
The final mark for the course will be made up as follows:
Laboratory work 10%
Class exam (2h)
30% (covering Semester 1 work)
Short tests
10% (4 tests in lecture times)
End of course exam (2h) 50% (covering the whole year’s work but with the emphasis on
Semester 2)
Previous exam papers will be available (see page 10) so you will know roughly what to
expect. Exams include lecture, lab, tutorial, and problem session material, knowledge,
understanding and application. As 50% of the final mark is from continuous assessment it is
important to work steadily throughout the year.
MINIMUM REQUIREMENTS FOR THE AWARD OF CREDITS
Students may be awarded credits for the course only if they meet the following
requirements:
• attend lectures
• perform satisfactorily in the mid-year class examination
• sit the four class tests
• have a good attendance record in laboratories and problem sessions
• achieve a satisfactory standard in the laboratory work
• sit the end-of-course examination.
Normally no grade or credits shall be awarded to a candidate who has not met these
requirements.
EXAMINATIONS
The Class examination (2 hours) will take place in December (time still to be fixed). The end
of course examination (2 hours) will be in April or May. Advice will be available on the
format of the exam and papers from previous years can be purchased from the Alchemists
Club (see page 10) and are also available from the University Library.
It is important that you do well in the Class examination as this forms 30% of your
final assessment. A poor performance will put pressure on you to work significantly harder
for the end of course exam. You do not get a second chance with the class exam. It is
vitally important for you to plan your work from the start with this in mind. Extenuating
circumstances (e.g. illness) at exam times must be reported to Prof Hill at the time and
supported by a medical certificate or other appropriate documentation. A copy of last year’s
class examination is at the back of this handbook.
Please note that all examinations should be written on the right-hand pages of the exam
book in ink. Please do not use red pens as this can cause confusion when the papers are
marked. Periodic tables will be available in examinations. You should provide your own
calculator for examinations. Programmable calculators are not allowed.
5

CLASS TESTS
Four class tests will take place on Fridays (October 24th, November 21 st , February 13 th and
March 20 th ) at normal lecture times in the lecture theatre that you use for the problem
sessions. Each test lasts 30 minutes allowing time for settling down before the test and
collection of test papers afterwards. A sample Class Test will be handed out during the
week before each test.
The purpose of the tests is to encourage you to work steadily throughout the year and to
give you an indication of your progress. Students who perform poorly in a Class Test will be
expected to attend revision tutorials, normally given by Prof Hill, at times displayed on the
notice board.
It is important that if you are absent from any of the class tests or examinations that you
explain your absence to Prof Hill otherwise this will affect your continuous assessment.
ABSENCE FROM CLASSES
ABSENCE FROM CLASSES FOR MORE THAN FIVE TERM DAYS
should be explained by a doctor's medical certificate or similar document which MUST be
submitted to the
Registrar’s Enquiry Office, Main University Building
The medical certificate will be copied by the Registrar’s Office to all the Class Heads of the
subjects you take and your Adviser of Studies.
ABSENCE FROM CLASSES FOR LESS THAN FIVE TERM DAYS
may be explained by a 'Self Certificate of Absence' (available in the Science Faculties Office
and submitted to
Science Faculties Office, Boyd Orr Building
For the overall assessment of the course, attendance credits will only be given if
absence was adequately explained by one or other of these routes.
IN ADDITION to these certificates you must inform Prof Bob Hill by letter or email
(bobh@chem.gla.ac.uk).
6

LABORATORY PRACTICAL WORK
The laboratory work (3 hours per week) is designed to give you practice in safely and
accurately carrying out preparations, analyses or measurements, reporting and interpreting
results.
It also offers a chance to
undertake chemical reactions yourself
operate instruments and collect experimental data
think about experiment design
check your understanding of particular topics
talk to demonstrators
Concepts, procedures and knowledge met in the lab may appear in written exams. Your
reports and oral answers will be marked and these marks and your attendance record
contribute to the award of lab grades and count for 10% of the overall mark.
Attendance is compulsory. Absences should be explained as above. If you miss a lab (for
whatever reason) you should see Prof Hill to arrange for an alternative time to complete that
lab. Remember that some concepts introduced in the lab (but not lectures) will be included
in the examinations.
You require a white lab coat for the labs - you will be provided with a lab manual and safety
glasses which you must bring along and wear at every lab.
Labs start in week 4 with a workshop on laboratory calculations.
SUMMATIVE ASSESSMENT
All feedback on coursework used in assessment, including mid-year class exam/class test
marks and laboratory grades, is strictly provisional for your guidance only, and is subject to
ratification by the Board of Examiners and External Examiners at the end of the academic
year. The University code of assessment is given in the General Section (page Gen. 10) of
the University Calendar 2008/2009 (www.glasgow.ac.uk/senate/calendar/current.html).
PLAGIARISM
Students are reminded that regulations regarding plagiarism (copying) apply to all work
contributing to assessment, including lab. reports and class tests. Except where specifically
directed, as part of a group project for example, all assessed work must be your own.
Copying of lab reports, for example, is plagiarism - students may share data, where
appropriate - but the report must be your own. See page Gen.48 of the University Calendar
2008/2009 (www.glasgow.ac.uk/senate/calendar/current.html).
7

PROBLEM SOLVING SESSIONS
These will be held at the normal lecture times (PS on timetable) and their purpose is to
practise using the knowledge you have gained from lectures and to prepare you for the
laboratory work.
Equipment
You will need a calculator giving scientific notation and logs to base 10 (log x) and logs to
base e (ln x) and inverse functions. Please note that programmable calculators are not
allowed in University examinations.
You will be provided with a periodic table that will be needed at some of the problem
sessions (and can be used in class tests). A periodic table will be provided in the class exam
and the end-of-course exam. Keep this periodic table unmarked for test purposes.
Procedure
The topics of the sessions will be announced in advance. After a short introduction you will
be asked to work through the problems collaborating with friends if you wish. Several tutors
will be available. Raise your hand if you need help with the problems. Answers and
explanations will be given as the session progresses but it is no use sitting waiting till they
are displayed - you will not have learned anything unless you work at it yourself.
Sometimes supplementary problems will be provided for you to try at home.
Solutions
The complete solutions to the problem sessions will be displayed on the Chemistry-1 on the
web: http://www.chem.gla.ac.uk/teaching/student_notices/year1.htm.
Attendance at problem sessions is compulsory (See Award of Credits). Absence for
good reason should be explained (see above). If you were absent for good reason you can
get copies of the sheets from Prof Hill.
Mobile Phones
Please note: mobile phones must be switched off during lectures, labs, problem sessions,
tests, examinations and in the library.
8

REVISION TUTORIALS
If you are having problems with a particular course you should see the lecturer concerned.
Revision tutorial sessions have been timetabled on certain Thursdays at normal lecture
times in the Main Lecture Theatre. These are not compulsory, but they do give an
opportunity for students to ask questions. Tutorials are normally given by Prof Hill.
CLASS NOTICES
Class notices, are posted in the Chemistry-1 display case on the ground floor of the central
block of the Joseph Black Building. Problem Session answers, details of laboratories and
results of class tests, class exam and laboratory grades will also be displayed. It is
important to look at this Notice board regularly for details of any class information,
particularly if you have been absent for some reason. Weekly Class News will be e-mailed
to your student e-mail address. You must check this regularly.
GRADE POINT AVERAGES: GUIDELINES
The grade awarded at the end of the course contributes towards you Grade Point Average.
See University Calendar 2008/2009 page Gen.12 which can be found on the following web
page: http://senate.gla.ac.uk/calendar/
Grade Grade descriptor Grade
points
A Excellent 16
B Very good 14
C Good 12
D Satisfactory 10
E Weak 8
F Poor 6
G Very poor 2
H 0
Total grade points = sum of credits x grade points
Grade point average (GPA) = Total grade points/Total credits
The grade point average and credit level requirement for B.Sc. and M.Sci. are given in full in
the University of Glasgow Calendar and the Catalogue of Courses. Please consult your
adviser of studies for full details. Some of the key points are listed below.
1. Your grade point average should normally be at 10 or above in each year of study.
2. Entry into level-3 courses requires a grade point average over the first two years of
above 11 for B.Sc (Hons) and above 12 for M.Sci.
3. Entry to many level-3 courses is on a competitive basis with a preference given to
those students with a high grade point average.
4. In addition some level-3 courses have a minimum grade requirement for entry.
It is therefore important that you make sure you work steadily throughout the year in every
subject. Low grades may cause problems with progress.
9

STAFF-STUDENT COMMITTEE AND OPINION SURVEYS
At the start of the session we will invite students in the Chemistry-1 class to volunteer to join
the Chemistry Staff-Student Liaison Committee which discusses courses and other
departmental business once or twice a term. These students have a special responsibility to
alert staff of any problems that develop in the running of the Chemistry-1 course.
All students will have an opportunity at some time to comment on aspects of the course via
questionnaires. Any difficulties are most quickly resolved by informing Prof Hill.
ALCHEMISTS' CLUB
The chemistry students club organises lectures, sports etc. and sells reprints of past exam
papers. The papers will be sold during labs or at the end of lectures. If you have problems
getting them see the Alchemists web site at http://www.chem.gla.ac.uk/alchemist/.
BEYOND CHEMISTRY-1
The following 30-credit courses are available in second year. Both Chemistry-2X and
Chemistry-2Y are required to continue with “Chemistry” courses beyond level-2. Similarly
both Environmental Chemistry-2A and 2B are required to continue with “environmental”
subjects beyond level-2 It is possible to do all 4 courses (120 credits).
Chemistry-2X – Molecules matter – the fundamentals
Taught throughout the year in parallel with Chemistry-2Y. The course is designed to give a
deeper understanding of the behaviour of molecules and beyond into solid state chemistry.
The topics covered include molecular thermodynamics, organic stereochemistry, solid state
chemistry, quantum mechanics, chemical bonding and symmetry, main group chemistry,
organometallic chemistry and enols and enolates.
Chemistry-2Y – Chemistry of the natural world
Taught throughout the year in parallel with Chemistry-2X. The course is designed not only
to be useful for intending chemists but also for those students who are intending to pursue
degrees in biology at the molecular level such as biochemistry, pharmacology, genetics etc.
Topics covered include spectroscopy, kinetics, aromatic chemistry, co-ordination chemistry,
organic synthesis, biophysical chemistry and applied organic chemistry. Both Chemistry 2X
and 2Y are required for entry into level-3 courses in Chemistry, Chemistry with medicinal
chemistry, Chemistry with forensic studies, Chemistry and mathematics, Biology and
chemistry and Chemical Physics.
Environmental Chemistry-2A – The natural environment
Taught in the first semester. This course aims to describe the chemistry and functioning of
the components of the natural environment, the interactions between these components and
the processes which operate within and between them. This will provide an understanding
of the chemistry of rocks, soils, sediments, water, air and living organisms. Particular
attention will be paid to the processes which cause mobilisation or immobilisation of
chemical species, their mobility and cycling between the different environmental
components. The chemistry of environmental materials and processes and the chemical
analysis of environmental samples are strongly emphasised to provide a sound scientific
background for understanding environmental problems and for monitoring, controlling and
cleaning up pollution.
10

Environmental Chemistry-2B – Environmental systems and pollution
Taught in the second semester. This course aims to describe the chemistry and behaviour
of environmental systems and the effect of human activity on them. The course acts as an
introduction, along with Environmental Chemistry 2A, to the subjects covered in greater
detail in the honours courses in Environmental Chemistry; Environmental Biogeochemistry
and Environmental Chemistry and Geography. Environmental Chemistry 2A, The Natural
Environment, should be taken as a co-requisite to provide entry to the level-3 courses in
“environmental” subjects, but each is a complete course in its own right, suitable for
students intending to proceed to level-3 in other subjects. These two courses also provide
an appropriate chemical background for students intending level-3 in biological, geographic
or earth sciences.
CHEMISTRY BEYOND LEVEL 2
There is a wide range of “chemistry” options available beyond level-2. Some degrees are
also available with Work Placement or European Placement opportunities. The following list
gives all the possibilities. Final decisions about degree choice are made at the end of
second year. *Subject to approval by Senate
Master in Science (M.Sci.) degree programmes:
Chemistry with Work Placement
Chemistry with European Placement
Chemistry with Medicinal Chemistry with Work Placement
Chemistry with Medicinal Chemistry with European Placement
Chemistry with Forensic Studies with Work Placement
Chemical Physics
Chemical Physics with Work Placement
Chemistry and Mathematics
Honours B.Sc. degree programmes: (4 year courses)
Chemistry
Chemistry with Medicinal Chemistry
Chemistry with Forensic Studies
Chemical Physics
Chemistry and Mathematics
Environmental Chemistry
Environmental Biogeochemistry
Environmental Chemistry and Geography
B.Sc. designated degree programmes: (3 year courses)
Chemistry
Chemistry with Medicinal Chemistry
Environmental Chemistry
Environmental Biogeochemistry
Geography, Chemistry and the Environment
Biology and Chemistry
Chemistry and Mathematics
More details about these courses will be given in the careers talk on Wednesday of week 22
and course handbooks etc. can also be found at:
http://www.chem.gla.ac.uk/teaching/documents.htm
11

OFFICE NUMBERS FOR LECTURERS
A4-35 Prof Bob Hill Class Head
Direct line 0141-330 5951; email bobh@chem.gla.ac.uk
A5-21 Dr Andy Freer
A4-25 Dr Justin Hargreaves
A5-25 Prof Chris Gilmore
A5-24 Prof John McGrady
A5-20 Dr Beth Paschke Quantitative lab organiser
A4-40a Prof Chick Wilson
RECOMMENDED TEXTBOOKS
All students should have a copy of “General Chemistry” by Ebbing and Gammon (9th
Edition) and “Organic Chemistry” by Hart, Craine and Hart (12th Edition), Houghton Mifflin
(available as a combined package). Earlier editions can also be used.
Students with poor mathematical ability will find the following useful:
Beginning Mathematics for Chemistry by Scott.
WEB SITES
Several websites are available that are useful for helping you understand certain aspects of
Chemistry. The following site has some useful links: http://www.chemistry.about.com. The
publisher of Ebbing & Gammon also has a useful web site. Details are available from the
textbook.
12

2008-2009 Chemistry-1 Timetable Lectures: Main Lecture Theatre
Week 0 1 2 3 4 5 6 7 8 9 10 11 12 13 1 2 3 4 5 6 7 8 9 10 11
Begins 15
Sep
22
Sep
29
Sep
06
Oct
13
Oct
20
Oct
27
Oct
03
Nov
10
Nov
17
Nov
24
Nov
01
Dec
08
Dec
15
Dec
12
Jan
19
Jan
26
Jan
02
Feb
09
Feb
16
Feb
23
Feb
02
Mar
09
Mar
16
Mar
23
Mar
Mon 10 RH JMcG PS JMcG RH RH PS RH RH AF AF CG CG CW CW BP BP JH JH RH RH RT
3 RH JMcG PS JMcG RH RH PS RH RH AF AF
Revision
Exams
CG CG CW CW BP BP JH JH RH RH RT
20
Apr
Revision
27
Apr
Tue
10 JMcG JMcG JMcG JMcG RH RH RH RH RH AF AF CG CG CW CW BP BP JH JH RH RH RT
3 JMcG JMcG JMcG JMcG RH RH RH RH RH AF AF
Revision
Exams
CG CG CW CW BP BP JH JH RH RH RT
Revision
Wed
Thur
10 JMcG JMcG JMcG PS RH RH RH RH RH AF PS CG CW CW PS BP PS JH RH RH RH RT
3 JMcG JMcG JMcG PS RH RH RH RH RH AF PS
Revision
Exams
CG CW CW PS BP PS JH RH RH RH RT
10 Enrol JMcG JMcG JMcG RH RT RH RH RH RT AF CG CW CW BP RT RT JH RH RH RT
3 Enrol JMcG JMcG JMcG RH RT RH RH RH RT AF
Revision
Exams
CG CW CW BP RT RT JH RH RH RT
Revision Revision
Start of Exam Period
Fri
10 RH T RT PS T RT T T
3 RH T RT PS T RT
Revisio
n
Exams
T T
Revision
Labs S S S S S S S S S Q Q Q Q Q Q Q Q
RH Prof Bob Hill Enrol, admin, skills, Lab introduction (3) PS Problem sessions (7)
JMcG Prof John McGrady The Periodic table (12) T Class tests (4)
RH Prof Bob Hill Organic Chemistry (18) RT Revision tutorials (10)
AF Dr Andy Freer Chemical Kinetics (6) S Synthesis Laboratory
CG Prof Chris Gilmore Attractions and Repulsions (6) Q Quantitative Laboratory
CW Prof Chick Wilson Chemical Energy Changes (8)
BP Dr Beth Paschke Aqueous Equilibria and pH (6)
JH DR Justin Hargreaves Transition Metals (6)
RH Prof Bob Hill Macromolecules (8) Examinations – December and April/May
RH Prof Bob Hill Careers (1)
13

Title:
Duration:
Trends and Patterns - the Periodic Table.
12 lectures, 2 problem sessions.
Lecturers: Prof J E McGrady
Aims:
To establish an understanding of the Periodic Table in order to be able to use it
to rationalise chemical behaviour, to make predictions of the chemical
behaviour of compounds so far not encountered, to appreciate the idea of
molecular structure and scientific disciplines in the “real” world
Objectives:
1. Recognise patterns among the elements in blocks, vertical columns and horizontal
rows.
2. Understand the basis of atomic structure including the idea of energy level, quantum
numbers and orbitals.
3. Know what the s, p, d and f orbitals are and how they form a logical base for building
up the periodic table.
4. Recognise where in the periodic table metals and non-metals lie and identify
borderline elements.
5. Count electrons in valence shells.
6. Understand the terms ionisation energy and electron affinity of an isolated atom and
the electronegativity of an atom in a molecule.
7. Know how these terms vary through the periodic table.
8. Derive oxidation states of atoms within molecules by using relative electronegativities.
9. Use oxidation states to write balanced equations for redox reactions.
10. Derive the oxidation states that are possible for an element.
11. Derive Born-Haber enthalpy cycles for simple ionic compounds.
12. State the effect that ion size and charge have on the lattice energy of an ionic solid.
13. Draw the NaCl lattice structure.
14. Describe the macroscopic properties of p-block elements that are the result of
covalent bonds between the atoms.
15. Decide upon situations in which covalent bond formation is likely.
16. Recognise the transformation from non-metal to metal going down a group and from
right to left across a period.
17. Use the VSEPR approach to predict and draw the shapes of covalent p-block
molecules.
Course Outline: The development and significance of the Periodic Table; atomic
structure and atomic orbitals; the relationship of the Periodic Table to atomic structure;
blocks, columns and rows; trends in properties such as ion size, ionisation potential,
electron affinity, electronegativity; oxidation states; balance redox equations; Born-Haber
cycles; ionic lattice structure, p-block elements, covalent bonding, polarity, VSEPR rules and
molecular shape; radioactivity.
14

Title:
Duration:
Lecturers:
Aims:
Organic Chemistry
18 lectures + 2 problem sessions
Prof R A Hill
To introduce the principles of organic chemistry
Objectives:
1. Understand structural isomerism and the various conventions for drawing structures.
2. Recognise functional groups, be able to use organic nomenclature and identify
primary, secondary, tertiary alkyl groups.
3. Relate physical properties to polarity, molecular weight and hydrogen bonding and
understand the terms chirality, optical activity, enantiomers, racemes.
4. Know preparations and properties of alkanes, alkenes, alkynes, interpret the
properties of alkenes in terms of π bonding and understand geometric isomerism.
5. Use Markovnikov’s rule to predict orientation of HX additions and explain the rule on
the basis of carbonium ion (carbocation or carbenium ion) stability.
6. Count electrons in molecules, ions and radicals; relate formal charge to electron
arrangement, and understand the terms homolysis, heterolysis, nucleophile and
electrophile and understand curly arrow drawings of mechanisms.
7. Deduce structures from experimental evidence and predict products of reactions.
8. Know methods of preparing alkyl halides and the substitution reactions which alkyl
halides undergo with nucleophiles including the mechanism and stereochemistry of
S N 2 and S N 1 reactions.
9. Know that many alkyl halides can react with bases to give often more than one alkene
by elimination and that alkyl halides can react with magnesium to give
organomagnesium halides (Grignard reagents) which are useful in synthesis.
10. Know methods of making alcohols and some of their physical properties in terms of
hydrogen bonding and how primary, secondary and tertiary alcohols behave towards
oxidising agents, that alcohols can form alkoxide ions and that protonated alcohols
can undergo substitution and elimination (dehydration) reactions.
11. Know methods of making ethers and appreciate their chemically inert nature.
12. Know how to prepare and name aldehydes and ketones and understand the bonding
and polarity of the carbonyl group.
13. Know how nucleophilic reagents that add to the carbonyl group and the types of
compounds produced and appreciate that addition may be followed by substitution
leading to acetals, or by elimination leading to imines.
15

14. Know that formation of dinitrophenylhydrazones (DNP’s) is a good test for aldehydes
and ketones, and that semicarbazones are good crystalline derivatives.
15. Understand that aldehydes may be distinguished from ketones by oxidation of
aldehydes to carboxylic acids.
16. Know how to name and prepare carboxylic acids and understand the acidity of the
COOH group in terms of delocalisation of charge in the anion.
17. Know methods of preparing esters and how to name them and that esters can be
hydrolysed in aqueous acid or in aqueous alkali.
18. Know typical reactions of acid chlorides.
19. Understand the preparation and names of primary, secondary and tertiary amines and
the related ammonium ions and understand the basicity of amines, and the neutrality
of quaternary ammonium ions.
20. Predict the products of reaction of amines with acids, alkyl halides, acid chlorides,
esters and anhydrides.
21. Account for the shape, polarity and neutrality of amides in terms of delocalisation of
electrons.
22. Know the products and mechanisms of hydrolysis and reduction of esters and amides.
23. Account for the shape, stability and chemical reactions of benzene in terms of
delocalisation of electrons and name simple substituted benzenes using numbers, and
the ortho, meta and para relationships.
24. Know that the properties of some groups attached to benzene are modified by the
benzene ring and account for the acidity of phenols terms of delocalisation in the
anion.
25. Be aware that infra-red spectroscopy can be used in the identification of functional
group.
Course Outline: Natural and synthetic covalent structures; examples of simple compounds
of everyday, industrial and medicinal importance; combustion analysis and molecular
weights; structural isomers with tetrahedral, trigonal and digonal carbons; rotation about
single bonds and equivalent hydrogens; drawing organic structures; polar and non-polar
bonds; functional groups and nomenclature; lone pairs, VSEPR rule applications and σ and
bonds; chirality and geometrical isomerism; physical properties related to structure,
hydrogen bonding and polarity; electron counting; stabilisation by electron delocalisation
(resonance and aromaticity); reaction mechanisms understood in terms of electron pair
movement indicated by curly arrows; nucleophiles and electrophiles; Markovnikov’s rule for
addition; S N and S E and elimination reactions; nucleophilic addition followed by elimination;
the foregoing principles developed alongside the chemistry of alkanes, alkenes, alkynes,
polymers, alkyl halides, alcohols, ethers, aldehydes, ketones, carboxylic acids and their
derivatives, amines and amides and simple benzene derivatives; infra-red spectroscopy.
16

Title:
Duration:
Lecturer:
Aims:
Chemical Kinetics
6 lectures + 1 problem session
Dr A A Freer
To introduce basic terms of chemical kinetics: to understand that information
about reaction rates is gained experimentally by exploring the factors which
influence them, such as concentrations of reactants, temperature and presence
of catalysts: to recognise that we can deduce a substantial amount of
information about reaction pathways and reaction control in both a chemical
and biological (enzyme) environment by studying reaction kinetics.
Objectives:
1. Understand the meaning of the rate of reaction and the factors which can influence it.
2. Define the order of reaction, rate constant and understand the rate law for a
reaction.
3. Understand the use of the isolation method and initial rates method for determining
the order and rate constant of a multicomponent reaction.
4. Understand the use of the integrated rate equations for first and second order
reactions to determine the rate constant from concentration and time data.
5. Define the half-life of first-order and second-order reactions.
6. Understand the Arrhenius equation, the Arrhenius plot, activation energy, E a ,
collision theory and the activated complex.
7. Understand what is meant by complex and elementary reactions, molecularity of an
elementary reaction, reaction mechanism, reaction intermediate and the rate
determining step of a complex reaction.
Course Outline: Definition of reaction rate; variation with time; rate law; reaction order;
initial rate method for determination of rate law; integrated rate equations for first and
second order reactions; graphical methods; half-life; activation energy; Arrhenius equation;
determination of E a from temperature dependence of k; simple and complex reactions;
molecularity of simple reaction; reaction mechanism, reaction intermediate and rate
determining steps.
17

Title:
Duration:
Lecturer:
Aims:
Attractions and Repulsions
6 lectures
Prof C J Gilmore
To understand the principles of intermolecular forces and how they determine
the properties of bulk materials
Objectives:
1. Understand the concepts of ionic and covalent bonds and how they arise.
2. Understand the concepts of bond polarity, dipole, dipole moment and bond dipole.
3. Be able to predict the bond dipole in simple situations for elements in periods 1, 2
and 3 and groups 1 to 17.
4. Understand attractive forces and be able to quote examples of them and have an
idea of their relative strengths and be able to predict which of the intermolecular
forces are operating for simple compounds.
5. Be able to predict, in a general way, the properties of simple substances once the
intermolecular forces have been ascertained.
6. Know that non-ideal gas behaviour leads to the van der Waals equation and be able
to use it in simple situations
7. Understand the different forces operating in solids and how they control the
properties of materials.
8. Understand how the molecules are arranged in liquid crystals and how liquid crystal
displays (LCDs) work.
Course Outline: Ionic bonds, covalent bonds, bond polarity, dipole, dipole moment and
bond dipoles. Ion-ion interactions in ionic solids; Atom-atom interactions in metals; Dipoledipole
interactions; Hydrogen bonding; London (or dispersion) forces and how these forces
manifest themselves in the behaviour of melting points, boiling points, vapour pressures,
and deviations from the ideal gas laws. Ionic, metallic, covalent network and molecular
solids. Liquid crystals.
18

Title:
Duration:
Lecturers:
Aims:
Chemical Energy Changes
8 lectures + 1 problem session
Prof C Wilson
To develop an understanding of the energy changes occurring during
chemical reactions. To understand the role these changes have in
determining the state of equilibrium of a reaction and whether a reaction will
be exothermic or endothermic.
Objectives:
1. Appreciate that there are different forms of energy and understand the principle of the
conservation of energy applied to chemical systems.
2. Know the factors that determine the direction of chemical reaction, and understand
why spontaneous reactions can be either exothermic or endothermic.
3. Understand the connection between disorder and entropy and be able to define
entropy in terms of heat and temperature.
4. Define free energy change ∆G o in terms of (a) maximum work obtainable and (b)
balance between enthalpy and entropy changes.
5. Recognise that electrode potential measurements can be used for direct determination
of free energy change.
6. Use the relationship ∆G o = -RTlnK p and appreciate that chemical equilibrium is
dynamic, its position can be determined from a knowledge of ∆G o and at equilibrium
∆G = 0.
7. Understand the difference between thermodynamics and kinetics and appreciate that
the value of ∆G o or K, the equilibrium constant, tells you nothing about the rate of
reaction, and that a catalyst has no effect on K.
Course Outline: The different forms of energy, conservation of energy, spontaneous
reactions, exothermic and endothermic reactions. Entropy and disorder. Enthalpy and free
energy changes. Electrode potentials. Chemical equilibrium.
19

Title:
Duration:
Lecturer:
Aims:
Aqueous Equilibria and pH
6 lectures + 1 problem session
Dr Beth Paschke
To investigate what happens when different substances are dissolved in water
and see what evidence there is for dissociation into ions, to see how to
calculate the pH of solutions of acids, bases, and salts, and to learn how to
make up buffer solutions.
Objectives: By the end of the course, students should be able to:
1. explain why water has such high values for most of its physical properties, know the
relative strengths of a hydrogen bond and a covalent bond and account for the lower
density of ice compared with water.
2. explain why water is such a good solvent for many ionic solids and polar molecules
and know what is meant by dielectric constant.
3. know the dissociation state of strong and weak electrolytes in aqueous solution.
4. discuss what is meant by α, the degree of dissociation, for weak electrolytes and
calculate dissociation constants for weak acids and weak bases from α and c.
5. recall what is meant by the ion-product constant of water, K w , be able to calculate pH
from [H + ], and vice versa, for strong acids; and pH from [OH – ], and vice versa, for
strong bases.
6. know the Arrhenius, BrØnstead-Lowry and Lewis definitions of acids and bases.
7. calculate the pH, K a , and pK a of a weak acid solution and be able to calculate the pOH,
pH, K b , and pK b of a weak base solution from α, the degree of dissociation, and c.
8. calculate the pH and α for a weak base solution from K b , and for a weak acid solution
from K a , and the concentration and recall the relationship between K a for a weak acid
and K b for its conjugate base.
9. discuss what is meant by a buffer solution and how to calculate the pH of a buffer
solution using the Henderson-Hasselbalch equation.
10. predict the acidity or basicity (qualitatively) of the four classes of salt solutions.
11. recall how the pH changes in acid-base titrations and how the Henderson equation
explains the functioning of a pH indicator.
12. apply the theory and techniques introduced during this course to related exercises.
Course outline: Water a solvent; hydrogen bonding; dipoles; dielectric constant; ice
structure; concentrations; electrolytes; degree of dissociation; pH; common ion effect;
dissociation constant for weak acids and bases; various definitions of acids and bases; K a
and K b ; pH calculation for strong and weak acids and bases; K = α 2 c/(1-α); extent of
ionization of weak acids and bases at various pH’s; salt hydrolysis; buffers; Henderson-
Hasselbalch equation, importance in biology; titration curves; indicators.
20

Title:
Duration:
Transition metals
6 lectures
Lecturers: Prof J Hargreaves
Aims:
To develop the chemistry of the d-block elements, to explain their shapes,
colours and magnetic properties, to relate these as far as possible to the
presence of d-electrons, to give an appreciation of how some d-block
compounds are used in the real world.
Objectives:
1. Know the factors which determine the energies of the d-electrons relative to the s and
p electrons.
2. Write the electronic configurations of the d block elements and their ions in various
oxidation states, and ‘know’ the oxidation states that are possible or a given element.
Be able to determine the oxidation number of a transition metal ion in a compound.
3. Know what is meant by co-ordination compound, complex ion, co-ordination number,
ligand, Lewis acid, Lewis base.
4. Know and be able to draw the preferred shapes for molecules and co-ordination
complexes having co-ordination numbers 4 and 6.
5. State what is meant by the denticity of a ligand and be able to give examples of
monodentate, bidentate and polydentate ligands. Understand what is meant by the
term chelating ligand, and know the uses of chelating ligands.
6. Understand what is meant be the terms isomer and isomerism.
7. Recognise and be able to draw cis-trans, mer-fac and chiral isomers.
8. Appreciate the concept of Crystal Field Theory and how it can be used to explain the
colours and magnetic properties of octahedral d block element complexes.
Understand the term ligand field strength, spectrochemical series and ligand field
stabilisation energies.
9. Know the occurrence and use of selected complexes.
10. Be able to apply any of the above concepts to unseen situations.
Course Outlines: Electronic configurations of d block elements; oxidation states; coordination
compounds, shapes, ligands, geometries, isomers, colour and magnetic
properties; Crystal Field Theory used to explain colour and magnetic properties; selected
uses.
21

Title:
Duration:
Macromolecules
8 lectures
Lecturers: Prof R A Hill
Aims:
To review the structures, preparation, properties and uses of synthetic
macromolecules and to introduce the chemistry of the main food components
and to show how the structures are related to their physical and nutritional
characteristics
Objectives:
1. Define and use the terms monomer, polymer, macromolecule, repeat unit and list
distinct properties associated with macromolecules.
2. Describe mechanisms by which alkenes can be polymerised and explain why these
lead to a range of molecular weights and list structures, properties and application of
various poly(alkene)s.
3. Draw representative structures for polyamides, polyesters, polyethers and silicones
and describe ways of making these and understand how cross-linking can be
achieved in such cases.
4. Relate the physical properties, biodegradability and applications to the functional
groups in the back-bone and side-chains and understand how side-chain functional
groups can be utilised in applications (e.g. Polyacrylic acid, sulphonated polystyrene,
etc.).
5. Know the names of the principal carbohydrates found in food and have a general
understanding of their structures and their properties and be aware of the basis of the
nomenclature of carbohydrates and the common mono- and di- saccharides.
6. Draw the structure of glucose in its open and cyclised forms and relate the chemistry
of acetals and hemicetals to sugar chemistry.
7. Draw the structures of the common triglycerides and understand their hydrolysis
reactions and relate the structures of fats to their properties.
8. Relate the chemistry of amino acids and amides to the chemistry of proteins and be
able to draw the products of hydrolysis of simple peptides and understand the
structural features of proteins and how this relates to their function.
Course Outline: Polyalkenes, polyesters, polyamides, polyethers, polyurethanes;
mechanisms of alkene polymerisation, addition and condensation polymerisation, range of
MWt, conformation, flexibility, glass transition, stability to heat, fire, solvents; backbone and
side-chain functional groups; crosslinking, resins; application related to structure;
biodegradation; Natural molecules, fats, proteins, sugars, cellulose.
22

Title:
Duration:
Organisers:
Aims:
Laboratory Course
17 x 3 hour sessions
Prof R A Hill and Dr B Paschke
(a) To demonstrate, illustrate and extend understanding of some of the basic
principles, processes and phenomena covered in associated lecture
courses, (b) to give training in experimental methods and practical skills
which cannot be taught by formal lectures but which can only be acquired
from hands-on experience, (c) to develop appropriate skills and confidence
in the safe handling of potentially hazardous materials, (d) to give
experience in the design of safe and effective experimental procedures to
investigate unfamiliar problems.
Objectives:
1. Carry out safely simple laboratory procedures such as weighing (rough or analytical
balance), titrating (use of burette and pipette), dissolving, crystallising and filtering:
safe manipulation of apparatus.
2. Manipulate safely and dispose of chemicals (in solid, liquid and solution form),
including corrosive alkalis and acids and strong oxidising agents.
3. Control and safely contain exothermic reactions.
4. Make and record accurate observations and make appropriate deductions.
5. Synthesise, isolate and purify simple organic and inorganic compounds and coordination
complexes.
6. Understand the term “standardisation” when applied to acid/base or redox reactions.
7. Understand when it is appropriate to use an analytical balance and when to use a
preparative balance.
8. Record accurately the numerical data associated with volumetric analyses, and be
able to use such data to calculate molarities and the purity of compounds.
9. Understand the theory of pH and conductometric titrations, solubility products, heat of
reaction and activation energy.
10. Understand shape, symmetry and polarity of organic compounds and appreciate the
properties and reactions of organic functional groups.
11. Have an awareness and knowledge of safe laboratory practice.
Course Outline: The thermite reaction, acid base titrations, nickel complexes and
double salts, iodimetry, copper or chromium complexes, pH titrations, conductometric
titrations, solubility product, heat of reaction, activation energy, shapes, symmetry and
polarity, aldehydes and ketones, carboxylic acids and esters, amines and amides and
methods of purification.
23

Title:
Duration:
Lecturers:
Aims:
Problem Sessions
7 problem sessions
All Chemistry staff
Problem Sessions: Provide the opportunity to undertake problem solving
exercises, singly or in groups, under staff supervision and assistance. To get
the most out of these sessions students are encouraged to:
1. Attempt written problems and assess their own expertise and confidence in
tackling such material.
2. To seek assistance immediately from tutorial staff in attendance when
difficulties arise.
3. To reinforce problem solving skills by attempting any additional
supplementary (homework) material provided.
4. To seek further guidance if supplementary material proves troublesome.
Objectives:
1. Be able to perform calculations and make deductions concerning material
presented in lectures and laboratories
2. Communicate effectively with fellow students and members of staff about
problems and difficulties of the Chemistry-1 course
Course Outline: Stoichiometry, volumetric calculations, Redox equations, kinetics,
organic structures, recations and mechanisms, thermodynamics and electrochemistry,
solution chemistry and pH, Chemistry-1 course material found difficult by a student.
24

(e) IF 3
[20]
Thursday 10th January 2008 2.30 - 4.30 p. m.
Chemistry-1
Class Examination
Answer any FIVE questions.
Label the exam books as Section A and Section B.
WRITE THE QUESTION NUMBERS ON THE FRONT OF EACH BOOK IN THE
ORDER YOU HAVE ANSWERED THEM.
Make sure you put your name and student number on each book.
You may use a calculator. A periodic table is on the last page of this paper.
Section A
1. Use Valence Shell Electron Pair Repulsion (VSEPR) rules to predict the shapes of the
following molecules. In each case:
(i) show your working
(ii) state the arrangement of electron pairs
(iii) define the molecular geometry
(iv) draw the structure clearly showing the geometry.
(a) PCl 5
(b) NH 3
(c) BrF 5
(d) SO 2
(periodic table on last page)
continued over
25

2. Metallic copper Cu reacts with nitrate ion [NO 3 ] - in acid solution to
produce Cu 2+ and nitrogen dioxide NO 2 .
(a)
What is the oxidation state of:
(i)
Copper before and after the reaction?
(ii)
Nitrogen in nitrate and in nitrogen dioxide?
[4]
(b)
(c)
(d)
Write the balanced “half equation” for metallic copper being
converted to Cu 2+ ions. [2]
Write the balanced “half equation” for nitrate ion [NO 3 ] - being converted to
nitrogen dioxide NO 2 . [4]
Combine the half equations to produce a balanced equation that
represents the overall redox process. [4]
(e) Identify the oxidising agent in this reaction and explain your answer. [2]
(f)
Write out the electron configuration for the following chemical entities using the
previous noble (inert) gas notation, e.g. Mg = [Ne]3s 2 :
(i) Al
(ii) S 2-
(iii) Ti 2+
(iv) Sn 2+ [4]
Continued over
26

3.(a)
The reaction CH 3 CHO → CH 4 + CO is second order with respect to CH 3 CHO
and has a rate constant, k, = 3.5 x 10 -2 mol -1 L s -1 at 200 °C.
(i) What is the rate of the reaction when [CH 3 CHO] = 0.30 mol L -1
[3]
(ii)
If the initial concentration of CH 3 CHO was 0.34 mol L -1 , what would
its value be after 240 s?
[4]
(b)
A pollutant in the earth’s atmosphere catalyses the destruction of the ozone
layer via the reaction 2O 3 → 3O 2 . The proposed mechanism for this reaction is:
k 1
O 3 + Cl → ClO +O 2
k 2
O 3 → O + O 2
k 3
ClO + O → Cl + O 2
(i)
Write the rate law for the first step of this mechanism.
(ii)
Identify the catalyst.
27

(iii)
Identify the reaction intermediates.
[3]
(c)
Write down the Arrhenius equation and briefly describe the two components
which are derived from Collision Theory.
[3]
(d)
The rate constants for the decomposition of gaseous dinitrogen pentoxide are
3.7 x 10 -5 s -1 at 25 °C and 1.7 x 10 -3 s -1 at 55 °C.
2N 2 O 5 → 4NO 2 + O 2
(i) Determine the activation energy for this reaction in kJ mol -1 [5]
(ii) Calculate the half-life for this reaction at 55 °C. [2]
[R = 8.314 J K -1 mol -1 ]
Section B (use a different book for this section)
Continued over
4. (a) Draw all the lone pairs of electrons (if any) missing from the
following structures: [6]
28

(i)
H 3 C O
H
(ii)
C
N
(iii)
H
C
H
O
(iv)
H
Br
(v)
H
H
C
H
(vi)
H
H
N
H
H
(b) When alkyl bromide A is treated with hydroxide, compounds B and C are formed.
Br
HO
C 4 H 8
+
C 4 H 10 O
A
B
C
(i) Draw the structures of B and C. [4]
(ii) What type of reaction has occurred in the formation of B? [1]
(iii) What type of reaction has occurred in the formation of C? [1]
(iv)
Draw the mechanism for the formation of C. Use curly arrows and
include all the lone pairs. [3]
(c) Combustion analysis was used to determine the composition of compound
D with the following results:
C = 31.9%; H = 5.3%; Cl = 62.8%; the molecular mass is 113 g mol -1
(i) What is the molecular formula of D? [1]
(ii) Draw all the structural isomers of D. [4]
[Relative atomic masses: C = 12, H = 1, Cl = 35.5]
continued over
29

5.
E
(a) What is the systematic name of alkene E? [1]
(b) Draw a geometrical isomer of E. [1]
(c)
Draw the products of reaction of E with the following reagents.
Indicate with an asterisk (*) any chiral centres in each of the products.
(i) Bromine [3]
(ii) Hydrogen bromide [3]
(iii) Hydrogen with a Pd catalyst [3]
(d)
(e)
Draw the mechanism of addition of HBr to E. Use curly arrows
and include all lone pairs of electrons. [4]
Ozonolysis of E using O 3 followed by treatment with zinc and acid gives
two organic products F and G. Draw the structures of F and G. [2]
(f)
Draw and name the product formed when benzene is treated with nitric acid
using sulfuric acid as catalyst.
[3]
continued over
30

6.
OH
C
O N CH 2
CH 3
CH 2
CH 3
H
(a) Identify the functional groups in compound H. [2]
(b) Draw the products formed when compound H is hydrolysed. [4]
(c) Will compound H show basic properties? Explain why. [2]
(d)
Predict the structure of the organic products J and L in the following
reactions: [4]
O
H 3 C
C
Cl
+
H 3 C
OH
J
I
O
K
NaBH 4
H 2 O
L
(e) What functional groups are present in compounds I, J, K and L? [4]
(f) Draw the mechanism for the reaction of compound I with methanol to give J.
Use curly arrows and include all lone pairs of electrons. [4]
End
31