(Mr liver)
A course of three lectures per week during Terms I and II, with laboratory work throughout the year.
Pre-requisite Standard. While there is no pre-requisite, it is strongly recommended that the students beginning the course should have a background of descriptive chemistry and basic chemical theory equivalent to Matriculation Chemistry. A knowledge of the subject up to this standard will be assumed as a basis for the course.
SYLLABUS
The course will consist of a treatment of basic physical, inorganic and organic chemistry, emphasizing aspects of the subject of importance in engineering investigations and practice.
The following syllabus provides a general guide to the topics to be discussed.
r. PHYSICAL CHLMISTRY
Chemical Kinetics. Factors influencing the rates of chemical reactions; collision theory of reaction. Catalysis—homogeneous and heterogeneous, with applications.
Chemical Equilibrium. Acid-base equilibria, calculation of pH, buffer solutions, indicators, titration curves. Complex ion equilibria.
The Properties of Gases, Liquids and Solids. The Kinetic theory of matter. The ideal gas equation; real gases and deviations from ideality; van der Waals' equation; liquefaction of gases and critical phenomena. The liquid state. Crystalline solids—metals, ionic, valence and molecular crystals. Crystal. defects. The band theory of solids. Influence of bond type on physical and chemical properties of crystalline solids. Solid-liquid-gas equilibria for one-component systems: the Phase Rule.
Solutions. Two-component systems; solutions; the properties of gas-gas, gas-liquid, liquid- liquid and solid-liquid systems. Fractional distillation. Distribution law. Colligative properties of dilute solutions.
Thermochemistry. The first law of thermodynamics; heat and work; internal energy and enthalpy; calorimetry; heat of combustion; the laws of Hess and Kirchhoff. Combustion of fuels.
Electrochemistry: Conductance of electrolyte solutions and the ionic theory. Oxidation- reduction equilibria, redox indicators, titration curves; electrode potentials; electrolytic cells; measurement of hydrogen ion concentration. Electrolysis. Overvoltage. Electro- deposition of metals. Corrosion. Factors influencing corrosion and methods of control- ling it.
Surface Chemistry and the Colloidal State. Surface phenomena. The colloidal state:
lyophobic and lyophilic sols. Viscosity of proteins. Gels. Emulsions. Chromatography.
Theory of Chemical Analysis. The theory and procedure involved in volumetric analysis such as is given in the laboratory work. Conductometric titrations; potentiometric titra- tions. Spectrophotometry.
Radiochemistry. Measurement of radioactivity; properties of radioactive isotopes and their applications to some typical chemical problems. The Szilard-Chalmers 'recoil effect'.
z. ORGANIC CHEMISTRY
The properties of homologous series. Aliphatic and aromatic hydrocarbons and their simpler derivatives. The main functional groups. Fuels; Plastics—thermosetting and thermoplastic, polymerization; other organic engineering materials.
LABORATORY WORK
Three hours per week throughout the year, covering quantitative analytical chemistry and general inorganic, physical and organic chemistry, the experiments being chosen to illustrate, amplify and extend the theory course.
The practical classes for this subject are taken in the Chemistry Laboratory of the Redmond Barry Building. The department supplies all the apparatus for which a fee of Siо must be paid to the University Branch of the National Bank, using a specially stamped bank slip obtained from the Laboratory. Evidence of payment must be pro- duced to the Laboratory before practical classes begin. The full fee is retained as no charge will be made for reasonable wear and breakage.
BOOKS
(a) Recommended for preliminary reading:
Stranks, D. R., Heffernan, M. L., Lee Dow, K. C., McTigue, P. T. and Withers, G. R..
Chemistry: A Structural View. (M.U.P., 1966.)
Gray, H. B. and Haight, G. P., Basic Principles of Chemistry. (Benjamin, 1967.) (b) Prescribed text-books
:
*Glasstone, S. and Lewis, D., Elements of Physical Chemistry. (Macmillan.) or *Barrow, G. M., Physical Chemistry. (and ed., McGraw-Hill, 1966.)
or *Ander, P. and Sonnessa, A. J., Principles of Chemistry: An Iii n to Theoreti cаl Concepts. (Collier-Macmillan, 1965.)
Mahan, B. H., University Chemistry. (Addison-Wesley, 1965.)
*Olver, N. H. (ed.), Departmental Publications:
Experiments in Chemistry. (1969 ed.)
(These laboratory handbooks are available only from the Chemistry Laboratory, Red- mond Barry Building.)
(c) Recommended for reference:
Glasstone, S., Textbook of Physical Chemistry. (2nd ed., Macmillan.) Moore, W. J., Physical Chemistry. (4th ed. Longmans.)
Olver, N. H. (ed.), Fundamental Aspects of Chemistry 1963. (Dept. of Chem., U. of M.) Van Vlack, L. H., Elements of Materials Science. (and ed., Addison-Wesley.) Bezzant, R. J., Basic Organic Chemistry. (McGraw-Hill, 1 966.)
Vogel, A. I., A Text-book of Quantitative Inorganic Analysis including Elementary Instrumental Analyses. (3rd ed., Longmans.)
Findlay, A. and Kitchener, J. A., Practical Physical Chemistry. (8th ed., Longman.) Aylward, G. H. and Findlay, T. J. V., Chemical Data Book. (and ed., Wiley, 1966.) ,
70
EXAMINATION
One 3-hour written paper, for Pass and Honours combined. The practical work of each student is assessed continually throughout the year, and is taken into account in deter- mining the success of candidates at the Annual Examination.
361-2. CHEMISTRY PART I B
A course of three lectures, one tutorial per week and laboratory work throughout the year. A preliminary standard equivalent to Matriculation Chemistry will be assumed. The
syllabus is basically similar to that of the Chemistry IA course with the restriction that
certain subjects are not developed so fully.
SYLLABUS
1. PHYSICAL -CHEMISTRY - -
Therniodynaitics: First law: thermodynamic properties, heat and work, functions of state, U and I; heat absorbed at constant volume and at constant pressure, specific heats.
Thermochemistry, standard states, standard enthalpy changes and enthalpies of for- mation. Kirchhoff's Law.
Gas behaviour: ideal and real gases. Kinetic theory of gases; deviations from ideal gas behaviour and their interpretation in terms of modifications made to kinetic theory postulates; van der Waalš s equation, virial equation.
Phase equilibria: One component systems: liquefaction and critical phenomena; variation of vapour pressure with temperature; phase transitions for a one component system, P-V and P-T diagrams; polymorphism and metastable states. Two or more component systems: liquid/vapour systems, Raoult's Law, Henry's Law, vapour pressure and boil- ing-point composition diagrams, distillation, azeotropes, elevation of boiling points.
Liquid/liquid systems, partially miscible liquids; distribution law. Liquid/solid systems, solubility, depression of freezing points, eutectics, compound formation, adsorption of a component at a surface.
Chemical equilibria involving the gas phase: Measurement of gas pressures; homogeneous equilibria, heterogeneous equilibria, examples of competing equilibria.
Chemical equilibria in solution: Measurement of concentrations in solution. Complex ion equilibria; stability and instability constants and their determination.
Determination of solubility and solubility products; calculations involving simultaneous equilibria.
Acid-base equilibria; acids and bases in non-aqueous solvents; calculation of pH from fundamental principles; buffer solutions; polyprotics; titration curves, indicators.
Redox equilibria : Half cells; the Nernst equation, cell reactions, equilibrium constants;
potentiometric measurements and application to the measurement of pH, etc. Free energy changes during redox reactions, relation to equilibrium constants; standard free energies. Electrolysis: decomposition and discharge potentials, order of discharge.
The conductance of electrolytes: Conductivity: molar conductance; Kohlrausch's law of independent migration; conductometric determination of concentrations and application to the measurement of К. and K ; conductiometric titrations. Effects of ion interaction.
Chemical kinetics: Measurement of reaction rate; rate laws, factors affecting rate; concen- tration (order; rate expressions for zero, first and second order reactions), temperature, catalysts and radiation. Simple collision theory model for reaction mechanisms; collision frequency and activation energy.
z. INORGANIC CHEMISTRY
Atomic Structure and the Theory of Valency: electrovalent, covalent, dative, hydrogen, metallic and van der Waals' bonding.
Structure of Solids: influence of bond type on chemical and physical properties afd type of structure.
Periodic Classification : comparative chemistry of selected elements with special reference to periodicity and electronic configuration.
з. ORGANIC CHEMISTRY
The scope
of
organic chemistry—Bonding, structure, and elementary stereochemistry of carbon compounds. An outline of the chemistry of hydrocarbons and their monofanc- tional derivatives in terms of molecular structure and the electronic mechanisms of reactions.LABORATORY WORK
Three hours per week, throughout the year, illustrating the principles of inorganic, physical and organic chemistry together with exercises in quantitative and qualitative analysis.
The practical classes for this subject are taken in the Chemistry Building. The department supplies all the apparatus for which a fee of $10 must be paid to the University Branch of the National Bank, using a specially stamped bank slip obtained from the department.
Evidence of payment must be produced to the department before practical classes begin.
BOOKS
(a) Recommended for preliminary reading:
Pauling, L., General Chemistry. (Freeman.)
Stranks, D. R. et al., Chemistry-A Structural View. (M.U.P.)
The content of lectures in Chemistry I В will be based on the assumption that all students have read the text-book by Stranks et al.
(b) Prescribed text-books:
Moore, W. J., Physical Chemistry. (4th cd., Longmans.)t or Mahan, B. H., University Chemistry. (Addison-Wesley.)
Physical Chemistry Part 1 Problems. (Departmental Publication. Available only frons the Chemistry School.)
Bell, C. F., and Lott. K. A. K„ Modern Approach to inorganic Chemistry. (Butterworth.) Allinger, N. L. and Allinger, J., Structures of Organic Molecules. (Prentice-Hall.) Saunders, W. H., ionic Aliphatic Reactions. (Prentice-Hall.)
Tedder, J. M. and Nechvatal, A., Basic Organic Chemistry. (Wiley.)
*Departmental Publication—Experiments in Chemistry. (í96g ed.) (This laboratory hand- book is available only from the School of Chemistry.)
Aylward, G. H. and Findlay, T. J. V. (eds), Chemical Data Book. (and ed., Wiley, 1966.) (c) Recommended for reference:
Gould, E. S., Inorganic Reactions and Structure. (Holt.)t
Brown. R. D. and O'Donnell, T. A., Manual of Elementary Practical Chemistry. (3rd ed..
M.U.P.)
Companion, A. L.. Chemical Bonding. (McGraw-Iii.)
Cartmell, E. and Fowles, G. W. A., Valency and Molecular Structure. (3rd ed., Butterworth.)
Harvey, K. B. and Porter, G. B., introduction to Physical inorganic Chemistry.
(Addison-Wesley.)
Books marked t are used by students proceeding to Chemistry II and Chemistry III.
EXAMINATION
One 3-hour paper in Physical Chemistry, one 2-hour paper in Inorganic Chemistry and one 2-hour paper in Organic Chemistry.
The practical work of each student is assessed continually throughout the year, and is taken into account in determining the success of candidates at the Annual Examination.