All students in the class must matriculate, complete a class enrolment form and pay a fee of £15 (collected in the lab in the first week) for the lab manuals, notebooks, safety glasses and other materials provided.

PROBLEM On some Thursdays the lecture time is used for problem-solving SESSIONS workshops. Supplementary problems will be provided for you to work on at home. More details are given on page 7.

LABORATORY Each student will attend one three-hour laboratory class per week starting in week 1. Lab times are M, Tu, W, Th 2 - 5 and Tu, Th, F 10 - 1. You will be assigned a day and told your bench. More details are given on page 6.

In lectures try to note down what is on the board 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.

The final mark for the course will be made up as follows:

Laboratory work 10%

Class exam (2h) 30% (covering term 1 work)

Short tests 10% (4 tests in lecture times)

End of course exam (3h) 50% (covering the whole year’s work but with the emphasis on terms 2 and 3)

Previous exam papers will be available (see page 9) so you will know roughly what to expect. Exams include lecture, lab, tutorial, and workshop material, knowledge, understanding and application. As 50% of the final mark is from continuous assessment it is important to work steadily throughout the year.

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.

The Class examination (2 hours) will take place in week 13 (times still to be fixed). The end of course examination (3 hours) will be at the end of May or beginning of June. Advice will be available on the format of the exam and papers from previous years will be purchased from the Alchemists Club (see page 9).

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 Dr Hill at the time and supported by a medical certificate or other appropriate documentation.

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. Only clean "GlaxoWellcome" periodic tables will be allowed in examinations and programmable calculators are not allowed.

Four class tests will take place on Fridays (November 12th, December 10th, March 3rd and May 5th) at normal lecture times in the lecture theatre that you use for the problem sessions. The tests last 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 extra tutorials normally given by Dr 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 Dr Hill otherwise this will affect your continuous assessment.

should be explained by a doctor's medical certificate or similar document which MUST be submitted to the

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.

may be explained by a 'Self Certificate of Absence' (available in the Science Faculty Office and submitted to

IN ADDITION to these certificates you must also complete a Chemistry Department Certificate of Absence obtained outside from Dr Hill's Office (Room A4-35) and returned there.

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

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.

You require a white lab coat for the labs - you will be provided with a lab notebook and safety glasses which you must bring along and wear at every lab.

Labs start in week 1 with a workshop on laboratory calculations.

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.

"The University's degrees and other academic awards are given in recognition of the candidate's personal achievement. Plagiarism is therefore considered as an act of academic fraudulence and as an offence against University discipline. Plagiarism is defined as the submission or presentation of work, in any form, which is not one’s own without acknowledgement of the sources. (With regard to essays, reports and dissertations, a simple rule dictates when it is necessary to acknowledge sources. If a student obtains information or ideas from an outside source, that source must be acknowledged. Another rule to follow is that any direct quotation must be placed in quotation marks, and the source immediately cited)."

(University of Glasgow Calendar, 1998-99, p. Gen. 17)

These will be held on Friday in week 4 and on Thursdays in weeks 8, 11, 14, 19 and 22 at the normal lecture times and their purpose is to practise using the knowledge you have gained from lectures and to prepare you for the laboratory work.

You will be allocated to one of two lecture theatres. On these days you must sit in seats leaving VACANT ROWS to allow staff to circulate and reach everyone. Leave one row vacant between every two rows i.e. sit in rows 1,2, 4,5, 7,8 etc.

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 "GlaxoWellcome" periodic table which will be needed at some of the problem sessions (and can be used in class tests, the class exam and the end-of-course exam) - keep this periodic table clean for examination purposes.

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 written up - you will not have learned anything unless you work at it yourself.

Sometimes supplementary problems will be provided for you to try at home.

The complete solutions to the problem sessions will be displayed on the Chemistry-1 Notice board on the ground floor of the central block. It is not intended that these solutions should be copied - use them to check or complete your own answers. They will remain on display for a few weeks until the space is needed for new ones. A copy of the solutions will be available for consultation in the Chemistry Library (B5-08) – ask the librarian.

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 Dr Hill.

All students will be assigned a tutor who is a member of staff and who will be available at a set time each week (normally in a vacant lecture time) to discuss any problems you may have with chemistry topics. We will require all students to see their tutors occasionally but regular visits and discussions will be the most helpful. Your tutor has other teaching duties so sometimes will not be available at the allocated time. Try to call back at another time to see your tutor or make an appointment.

Class notices, as well as the weekly Class News, are posted in the Chemistry-1 display case on the ground floor of the central block. 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, particlularly if you have been absent for some reason.

The grade awarded at the end of the course contributes towards you Grade Point Average. As a guide, the approximate mark/grade correlations used in the Chemistry Department are as follows.

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.

It is therefore important that you make sure you work steadily throughout the year in every subject. Low grades may cause problems with progress.

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 Dr Hill.

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 in room A4-30.

Direct line 0141-330 5951; email bobh@chem.gla.ac.uk

A4-32c Dr Andy Benniston

C5-20 Prof Joe Connolly

A4-32d Dr Ron Cross Inorganic lab organiser

A4-13 Dr Andy Freer

A5-27 Dr Chris Gilmore

C3-03b Dr Dave Lennon

A3-22 Dr David MacNicol Organic lab organiser

A4-34 Dr Bob Peacock

A4-38 Dr Diane Stirling

A5-26 Dr David White Physical lab organiser

Tutor ..................................... Room ..........

All students should have a copy of "General Chemistry" by Ebbing and Gammon (6th Edition) and "Organic Chemistry" by Hart, Craine and Hart (10th 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.

The publishers of the textbooks have an interactive WEB Site. Details of the address and passwords will be provided later.

1999-2000 Chemistry-1 Timetable Lectures: Main Lecture Theatre

RH Dr Bob Hill Enrol, Admin and Skills (2) W Problem Sessions

RC Dr Ron Cross Laboratory Introduction (1) T Class Tests

JDC Prof Joe Connolly The Central Science (1) I Inorganic Laboratory Weeks 1-7

AB Dr Andy Benniston The Periodic Table (12) P Physical Laboratory Weeks 8-12

DL Dr David Lennon

AF Dr Andy Freer Chemical Kinetics (6) O Organic Laboratory Weeks 16-20

CG Prof Chris Gilmore Attractions & Repulsions (6)

JDC Prof Joe Connolly Organic Chemistry (18)

DS Dr Diane Stirling Chemical Energy Changes (8)

RDP Dr Bob Peacock

DW Dr David White Aqueous Equilibria & pH (7) Examinations - week 13 and late May / early June 2000

RC Dr Ron Cross Transition Metals (6) Tutorials - Thursdays/Fridays 10/3

RH Dr Bob Hill Macromolecules (8)

1. Recognise patterns among the elements in blocks, vertical columns and horizontal rows.
1. Understand the basis of atomic structure including the idea of energy level, quantum numbers and orbitals.
1. Know what the s, p, d and f orbitals are and how they form a logical base for building up the periodic table.
1. Recognise where in the periodic table metals and non-metals lie and identify borderline elements.
1. Count electrons in valence shells.
1. Understand the terms ionisation energy and electron affinity of an isolated atom and the electronegativity of an atom in a molecule.
1. Know how these terms vary through the periodic table.
1. Derive oxidation states of atoms within molecules by using relative electronegativities.
1. Use oxidation states to write balanced equations for redox reactions.
1. Derive the oxidation states that are possible for an element.
1. Derive Born-Haber enthalpy cycles for simple ionic compounds.
1. State the effect that ion size and charge have on the lattice energy of an ionic solid.
1. Draw the NaCl lattice structure.
1. Describe the macroscopic properties of p-block elements that are the result of covalent bonds between the atoms.
1. Decide upon situations in which covalent bond formation is likely.
1. Recognise the transformation from non-metal to metal going down a group and from right to left across a period.
1. Use the VSEPR approach to predict and draw the shapes of covalent p-block molecules.
1. Appreciate the main features of nuclear structure and the common types of radioactive decay.

Title: Chemical Kinetics

Duration: 6 lectures + 1 workshop

Lecturer: Dr A A Freer

Objectives:

1. Understand the meaning of the rate of reaction and the factors which can influence it.
1. Define the order of reaction, rate constant and understand the rate law for a reaction.
1. Understand the use of the isolation method and initial rates method for determining the order and rate constant of a reaction.
1. Understand the use of the integrated rate equations for first and second order reactions to determine the rate constant from concentration and time data.
1. Define the half-life of first-order and second-order reactions.
1. Understand the Arrhenius equation, the Arrhenius plot, activation energy, E_a, collision theory and the activated complex.
1. 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.
1. Understand the use of catalysts and biological catalysts (enzymes) and distinguish between homogeneous and heterogeneous catalytic processes.

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 why the properties of the different sorts of materials are quite different, and what these properties are.
8. Understand how the molecules are arranged in liquid crystals and how liquid crystal displays (LCDs) work.
9. Understand the general principles of X-ray crystallography.

Title: Organic Chemistry

Duration: 18 lectures + 2 workshops

Lecturers: Prof J D Connolly

Aims: To introduce the principles of organic chemistry

1. Understand structural isomerism and the various conventions for drawing structures.
1. Recognise functional groups, be able to use organic nomenclature and identify primary, secondary, tertiary alkyl groups.
1. Relate physical properties to polarity, molecular weight and hydrogen bonding and understand the terms chirality, optical activity, enantiomers, racemates.
1. Know preparations and properties of alkanes, alkenes, alkynes, interpret the properties of alkenes in terms of p bonding and understand geometric isomerism.
1. 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.
1. 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.
1. Deduce structures from experimental evidence and predict products of reactions.
1. Know methods of preparing alkyl halides and the substitution reactions which alkyl halides undergo with nucleophiles including the mechanism and stereochemistry of S_N2 and S_N1 reactions.
1. 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.
1. 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.
1. Know methods of making ethers and appreciate their chemically inert nature.
1. Know how to prepare and name aldehydes and ketones and understand the bonding and polarity of the carbonyl group.
1. 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.
1. Know that formation of dinitrophenylhydrazones (DNP’s) is a good test for aldehydes and ketones, and that semicarbazones are good crystalline derivatives.
1. Understand that aldehydes may be distinguished from ketones by oxidation of aldehydes to carboxylic acids.
1. 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.
1. Know methods of preparing esters and how to name them and that esters can be hydrolysed in aqueous acid or in aqueous alkali.
1. Know typical reactions of acid chlorides.
1. 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.
1. Predict the products of reaction of amines with acids, alkyl halides, acid chlorides, esters and anhydrides.
1. Account for the shape, polarity and neutrality of amides in terms of delocalisation of electrons.
1. Know the products and mechanisms of hydrolysis and reduction of esters and amides.
1. 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.
1. 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.

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 s and p 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.

Title: Chemical Energy Changes

Duration: 8 lectures + 1 workshop

Lecturers: Dr R D Peacock and Dr D Stirling

1. Appreciate that there are different forms of energy and understand the principle of the conservation of energy applied to chemical systems.
1. Know the factors which determine the direction of chemical change, and appreciate why spontaneous reactions can be either exothermic or endothermic.
1. Understand the connection between disorder and entropy and define entropy in terms of heat and temperature.
1. Define free energy change DG^o in terms of (a) maximum work obtainable and (b) balance between enthalpy and entropy changes.
1. Recognise that electrode potential measurements can be used for direct determination of free energy change.
1. Use the relationship DG^o = -RTlnK_p and appreciate that chemical equilibrium is dynamic, its position can be determined from a knowledge of DG^o and at equilibrium DG = 0
1. Appreciate that the value of DG^o or K the equilibrium constant tells you nothing about the rate of reaction, and that a catalyst has no effect on K.

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.
1. Explain why water is such a good solvent for many ionic solids and polar molecules and know what is meant by dielectric constant.
1. Know the dissociation state of strong and weak electrolytes in aqueous solution.
1. Understand what is meant by a , the degree of dissociation, for weak electrolytes and calculate dissociation constants for weak acids and weak bases from a and c.
1. Know what is meant by the ionic product of water, by pH, and be able to calculate pH from [H⁺], and vice versa, for strong acids; and pH from [OH^–], and vice versa, for strong bases.
1. Know the Arrhenius and Brønstead-Lowry definitions of acids and bases.
1. Know how to calculate the pH, K_a, and pK_a of a weak acid solution and how to calculate the pOH, pH, K_b, and pK_b of a weak base solution from a , the degree of dissociation, and c.
1. Know how to calculate the pH and a for a weak base solution from K_b, and for a weak acid solution from K_a, and the concentration and the relationship between K_a for a weak acid and K_b for its conjugate base.
1. Know what is meant by a buffer solution and how to calculate to pH of a buffer solution using the Henderson equation.
1. Know the acidity or basicity (qualitatively) of the four classes of salt solutions.
1. Know the pH changes in acid-base titrations and understand how the Henderson equation explains the functioning of a pH indicator.

1. Know the factors which determine the energies of the d-electrons relative to the s and p electrons.
1. Write the valence shell electronic configurations of the d block elements in various oxidation states and derive the oxidation states that are possible or a given element.
1. Know what is meant by co-ordination compound, complex ion, co-ordination number, ligand, Lewis acid, Lewis base.
1. Know and be able to draw the preferred shapes for molecules and co-ordination complexes having co-ordination numbers 4 and 6.
1. State what is meant by the denticity of a ligand and be able to give examples of monodentate and bidentate ligands.
1. Understand what is meant be the terms isomer and isomerism.
1. Recognise and be able to draw cis-trans, mer-fac and chiral isomers.
1. 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.
1. Know the occurrence and use of selected complexes.

1. Define and use the terms monomer, polymer, macromolecule, repeat unit and list distinct properties associated with macromolecules.
1. 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.
1. 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.
1. 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.).
1. 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.
1. Draw the structure of glucose in its open and cyclised forms and relate the chemistry of acetals and hemicetals to sugar chemistry.
1. Draw the structures of the common triglycerides and understand their hydrolysis reactions and relate the structures of fats to their properties.
1. 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.

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.
1. Manipulate safely and dispose of chemicals (in solid, liquid and solution form), including corrosive alkalis and acids and strong oxidising agents.
1. Control and safely contain exothermic reactions.
1. Make and record accurate observations and make appropriate deductions.
1. Synthesise, isolate and purify simple organic and inorganic compounds and co-ordination complexes.
1. Understand the term "standardisation" when applied to acid/base or redox reactions.
1. Understand when it is appropriate to use an analytical balance and when to use a preparative balance.
1. Record accurately the numerical data associated with volumetric analyses, and be able to use such data to calculate molarities and the purity of compounds.
1. Understand the theory of pH and conductometric titrations, solubility products, heat of reaction and activation energy.
1. Understand shape, symmetry and polarity of organic compounds and appreciate the properties and reactions of organic functional groups.
1. Design an efficient and safe synthetic experiment.
1. Have an awareness and knowledge of safe laboratory practice.

1. Be able to perform calculations and make deductions concerning material presented in lectures and laboratories
1. Communicate effectively with fellow students and members of staff about problems and difficulties of the Chemistry-1 course