(Mr liver)
A course of three lectures per week during Terms I and II, with laboratory work throughout the year.
Prerequisite 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.
i. PHYSICAL CHEMISTRY
Chemical Kinetics. Factors influencing the rates of chemical reactions; collision theory of reaction. Catalysis—homogeneous and heterogeneous, with applications.
Chemical Equilibrium. Add-base equilibria, calculation of pH, buffer solutions, indicators, titration curves. Complex con 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-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; electrode potentials; electrolytic cells; measurement of hydrogen ion concentration. Electrolysis. Overvoltage. Electrodeposition of metals. Corrosion.
Factors influencing corrosion and methods of controlling 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.
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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 $io 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- diced 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.)
Pauling, L., General Chemistry. (2nd ed., Freeman.)
Diamant, R. M. E., Applied Chemistry for Engineers. (Pitman.)
Sionko, M. J. and Plane, R. A., Chemistry: Principles and Properties. (McGraw-Hill.
1966.)
(b) Prescribed text-books:
*Glasstone, S. and Lewis, D., Elements of Physical Chemistry. (Macmillan.) or *Barrow, G. M., Physical Chemistry. (2nd ed., McGraw-Hill, 1966.)
Mahan, B. H., University Chemistry. (Addison-Wesley, 1965.)
or Andrews, D. H. and Kokes, R. J., Fundamental Chemistry. (and ed., Wiley, 1965.)
*Olver, N. H. (ed.), Departmental Publications.
Experiments in Inorganic and Physical Chemistry. (1867 edition.) Experiments in Organic Chemistry. (1967 edition.)
(These laboratory handbooks are available only from the Chemistry Laboratory, Red- mond Barry Building.)
(c) Recommended for reference:
Glasstone, S., Textbook of Physical Chemistry. (znd ed., Macmillan.) Moore, W. J., Physical Chemistry. (4th ed. Longmans.)
Addison, W. E., Structural Principles in Inorganic Compounds. (Longmans.)
liver, 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.) Mackenzie, C. A., Unified Organic Chemistry. (Harper International Student Reprints
—Harper & Row.)
Berzant, R. J., Basic Organic Chemistry. (McGraw-Hill, 1966.)
Brown, R. D. and O'Donnell, T. A., Manual of Elementary Practical Chemistry. (3rd ed., M.U.P.)
Kolthoff, I. M. and Sandell, E. B., Textbook of Quantitative Inorganic Analysis. (3rd ed., Macmillan.)
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., Longmans.) Daniels, F., Williams, J. W., Bender, P., Alberty, R. A. and Cornwell, C. D., Experi-
mental Physical Chemistry. (6th ed., McGraw-Hill.)
Aylward, G. H. and Findlay, T. J. V., Chemical Data Book. (and ed., Wiley, 1966.) EXAMINATION
One 3-hour written paper, for Pass and Honours combined. There will be no practical examination, but the standard of the student's laboratory work will be assessed con- tinually throughout the year, and is taken into account in determining the success of the candidates at the Annual Examination.
420, CHEMISTRY PART I В
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.
Energetics of Chemical Reactions: heat of reaction, enthalpy, Hess's law, bond dis- sociation energies.
Chemical Equilibrium: homogeneous and heterogeneous equilibria in gases and solution;
determination of equilibrium constan ts.
Properties of electrolytes as found from conductance measurements; molar conductance;
law of independent ionic migration; conductimetric titrations.
Oxidation—reduction equilibria; reduction potentials; Nernst equation; half cells, cell reactions; equilibrium constants; potentiometric measurements and application to the determination of pH, pК,, К ,
etc.
redox indicators; free energy changes during redox reactions, relation to equilibrium constants; standard free energies.Electrolysis; deposition potentials; overvoltage; order of deposition.
Solubility equilibria; determination of solubility and solubility products; calculation of solubilities involving simultaneous equilibria (complex ions); precipitation titrations.
Acid/base equilibria; acids and bases in non aqueous solvents, calculation of pH from fundamental principles; buffer solutions; polyprotics; titration curves, indicators.
Gases : ideal and real gases; kinetic theory of gases,* deviations from ideal gas behaviour and interpretation in terms of modification of kinetic theory postulates; van der Waal's equation; critical state; liquefaction.
Phase Equilibria : one component systems, P-V and P-T diagrams; polymorphism and metastabl a states. Two component systems; gas-liquid, solid-liquid and solid-solid systems; partial miscibility; distribution law; miscible and volatile liquids; ideal and non ideal solutions; azeotropes; distillation.
Chemical Kinetics : measurement of reaction rate; rate laws; factors affecting rate : con- centration (order; rate expressions for first and second order reactions); temperature;
catalysts; radiation. Simple collision theory model for reaction mechanisms; collision frequency; energy distributions; activation energy.
*Note: Detailed formulation of the ist Law of Thermodynamics and the Kinetic Theory of Gases will not be presented but will be assumed to be known from coverage in Physics I. Students not taking physics will be supplied with a reading list to cover these topics to a suitable level.
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 and type of structure.
Introduction to . Co-ordination Chemistry : Werner's theory of cobalt , and platinum ammines, inorganic stereochemistry, isomerism, chelating ligands,. aqua armino and halide complexes of selected cations, stability constants.
Periodic Table : comparative chemistry of selected groups and periods of elements with special reference to periodicity and electronic configuration.
;. Organic Chemistry. The scope of organic chemistry. Principles of purification, qualitative and quantitative analysis of organic compounds. Functional, structural, optical and geometric isomerism, Structure oi= benzene.
The preparation and reactions of the following classes of compounds: paraffins, olefins, acetylenes, benzene, alcohols, phenols, halides, ethers, aldehydes, ketones, carboxylic acids and amines.
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 $io 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.
The full fee is retained as no charge will be made for reasonable wear and breakage.
BOOKS
(a) Recommended for preliminary reading:
Pauling, L., Gепeтal Chemistry. (Freeman.) .
Stranks, D. R. et al., Chemistry-A Structural View. (М.U.Р.) . (b) Prescribed text-books
Glasstone, S. and Lewis, D., Elements of Physical Chemistry. (Macmillan.)..
oт Daniels, F. and Alberty, R. A., Physical Chemistry. (Wiley.)t or Mahan, B. H., University Chemistry. (Addison-Wesley.)
or Slabaugh, W. H.. and Parsons, T. P., General Chemistry. (Wiley.)
Bell, C. F., and Lott, K. A. K., Modern Approach to Inorganic Chemistry. (Butterworth.) Morrison, R. T. and Boyd, R. N., Organic Chemistry. (Allyn & Bacon.)+
or English, J. and Cassidy. H. G.. Principles of Organic Chemistry. (McGraw-Hill.)t
*Departmental Publication—Experiments in Chemistry. (This laboratory handbook is available only from the School of Chemistry.) .
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(c) Recommended for reference:
Gilreath, E. S., Fundamental Concepts of Inorganic Chemistry. (McGraw-Hill.) 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.)
Books marked t are used by students proceeding to Chemistry II and Chemistry III.
EXAMINATION
One 3-hour paper in Physical Chemistry, one a-hour paper. in Inorganic Chemistry and one a-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.