New Chemistry Curriculum
New Chemistry Curriculum
New Chemistry Curriculum
ETHIOPIA
August, 2009
Addis Ababa
Ethiopia
Harmonized Curriculum for B.Sc. degree in Chemistry
Table of Contents
1. Rationale for the curriculum ....................................................................................................5
2. Aims, Goals and Objectives of the Program ............................................................................6
2.1 Aims of the Program ..........................................................................................................6
2.2 Goals of the Program..........................................................................................................6
2.3 Objectives of the Program ..................................................................................................6
3. Graduate Profile .......................................................................................................................6
3.1 Knowledge of chemistry ................................................................................................6
3.2 General intellectual and life skills ..................................................................................7
3.3 Values .............................................................................................................................7
4. Program Profile ........................................................................................................................7
5. Admission Requirements .........................................................................................................8
6. List of Major, Supportive and Common Courses ....................................................................8
6.1 Core Compulsory Courses .............................................................................................8
6.1.1 University Chemistry ......................................................................................................8
6.1.2 Analytical Chemistry..................................................................................................8
6.1.3 Physical Chemistry.....................................................................................................8
6.1.4 Organic Chemistry .....................................................................................................9
6.1.5 Inorganic Chemistry ...................................................................................................9
6.1.6 Applied Chemistry .....................................................................................................9
6.2 Core Elective Courses ....................................................................................................9
6.3 Supportive Courses ......................................................................................................10
6.4 Common Courses .........................................................................................................10
7. Summary of courses ...............................................................................................................10
8. Course Coding Style (Course Numbering) ............................................................................10
9. Sequencing of courses: Semester wise course breakdown.....................................................11
10. General Delivery Methods .......................................................................................................12
11. General Evaluation Methods ....................................................................................................13
12. Grading System ........................................................................................................................13
13. Duration of the Study ...............................................................................................................13
14. Grade Point Average Requirements for Graduation ................................................................13
15. Degree Nomenclature...............................................................................................................13
15.1 In English: ......................................................................................................................13
15.2 In Amharic: ....................................................................................................................13
16. Mechanism of Quality Assurance ............................................................................................13
17. Course descriptions, Course Outlines, Modes of Course Delivery and Modes of Performance
Evaluation.......................................................................................................................................14
17.1 University Chemistry Section ..................................................................................14
3. Graduate Profile
Students who have completed an undergraduate degree in chemistry will have acquired an
education at an advanced level, including:
• Knowledge of chemistry
• General intellectual and life skills and,
• Values
that equip them for employment, citizenship and lay the foundations for a lifetime of continuous
learning and personal development.
The chemistry graduates are expected to have the following attributes:
3.3 Values
• Value intellectual integrity, respect for truth and for the ethics of research and scholarly
activity;
• Demonstrate environmentally conscious attitude;
• Conduct assigned and professional activities with integrity and professional ethics;
• Contribute to the development of chemical industries with other professionals;
• Disseminate chemical knowledge;
• Enthusiastic about scientific ideas, discovery and learning
• Self-discipline and an ability to plan and achieve personal and professional goals;
• Willingness to engage in constructive public discourse and to accept social and civic
responsibilities;
• Respect for the values of other individuals and groups, and an appreciation of human and
cultural diversity;
• An awareness of international and global dimensions of intellectual, political and
economic activities, and behaving as a responsible citizen.
4. Program Profile
Main Aims of the program:
• To provide students with a broad and balanced foundation of chemical knowledge
and practical skills
• To develop in students the ability to apply their chemical knowledge and skills to
the solution of theoretical and practical problems in chemistry
• To encourage originality of thought
• To instil in students an appreciation of the importance of chemistry in an
industrial, economic, environmental and social context
• To provide students with the fundamentals of chemistry so that they can proceed
to further studies in specialized areas of chemistry or multidisciplinary areas
involving chemistry
5. Admission Requirements
a) Successful completion of the preparatory program with a pass mark in university entrance
examination and interest to study chemistry;
b) Diploma in chemistry from higher learning institutions fulfilment of the general University’s
admission requirements and
c) Other department specific requirements.
7. Summary of courses
SN Description Cr. Hrs
1 Major Courses 72
2 Supportive Courses 21
3 Common Courses 12
4 Elective 2/3
Total Requirement 107/108
Year II
Code Course Title Cr. Hr Course
type
Chem 331 Chemical Thermodynamics 3 Core
Chem 311 Inorganic Chemistry II 3 Core
Semester I Chem 313 Practical Inorganic Chemistry I 1 Core
Chem 321 Instrumental Analysis I 3 Core
Chem 323 Practical Instrumental Analysis I 1 Core
Chem 341 Organic Chemistry II 3 Core
Chem 343 Practical Organic Chemistry II 1 Core
EnLa 301 University Writing Skills 3 Common
Total 18
Year III
Course Course Title Cr. Hr Course
Code type
Chem 455 Environmental Chemistry and Toxicology 3 Core
Chem 411 Inorganic Chemistry III 4 Core
Chem 441 Practical Organic Chemistry III 2 Core
Semester I
Chem 453 Research Methodology and Scientific Writing 2 Core
Chem 431 Quantum Chemistry 4 Core
Chem 433 Practical Physical Chemistry II 1 Core
Chem 451 Industrial chemistry II 2 Core
Total 18
Course Course Title Cr. Hr Type
Code
Chem 422 Analysis of real samples 2 Core
Chem 452 Biochemistry 3 Core
Chem 432 Statistical Thermodynamics and Surface 3 Core
Semester II Chemistry
Chem 414 Practical Inorganic Chemistry II 2 Core
CEEd ... Civics and Ethical Education 3 Common
Mgmt Entrepreneurship 3 Common
Chem ... Elective 2/3 Core
Total 17/18
• Problem solving.
Letter grade A A− B + B B− C + C C− D+ D D− F
Numerical value 4.00 3.67 3.33 3.00 2.67 2.33 2.00 1.67 1.33 1.00 0.67 0.00
15.2 In Amharic:
የ ሣ ይ ን ስ ባ ች ለ ር ዲ ግ ሪ በ ኬ ሚ ስ ት ሪ¶
• Evaluation of student performance through, reports, tests, mid semester examinations, and
comprehensive final examination;
• Preparation of relevant teaching materials and laboratory manuals;
• Monitoring of instructors performance through student evaluation;
• Monitoring of instructors performance through colleague and Department Chairman
evaluation;
• Standardization of exams by Department Examination Committee (DEC);
• Communication of the evaluations to instructors;
• Stakeholders feedback on the relevance of the training program and qualities of
graduates;
• Conducting regular course self-evaluation, program self-evaluation and program peer and
external evaluation; and
• Seeking program accreditation by external accrediting agencies.
Course description:
Properties, Units and Measurement; The composition of matter, chemical reactions, reactions
Stoichiometry, Atomic structure and the periodic table, The Chemical Bond, Structure of
Molecules, The properties of Solutions, Chemical equilibrium, Introduction To Functional
Groups And Their Typical Reactions
Course rationale:
The course university chemistry is designed to make students more prepared to the all chemistry
courses by refreshing and summarizing the previous preparatory chemistry concepts before
tackling the advanced chemistry courses. It ensures readiness of the students for the higher
chemistry courses at university level and hence the name University chemistry is given.
Course outline
1. Properties, measurements, and units
1.1. The Properties of Substances
1.1.1. Physical and Chemical Properties
1.1.2. Substances and Mixtures
1.2. Measurements and Units
1.2.1. The International System of Units
1.2.2. Extensive and Intensive Properties
1.2.3. Conversion Factors
1.2.4. The Reliability of Measurements and Calculations
1.2.5. Significant Figures in Calculations
4. Reactions stoichiometry
4.1. Interpreting Stoichiometric Coefficients
I. Mole Calculations
4.1.2. Limiting Reactants
4.1.3. Chemical Compositions from Measurements of Mass
4.2. The Stoichiometry of Reactions in Solution
4.2.2. Molar Concentration
4.2.3. The Volume of Solution Required for Reaction
4.2.4. Titrations
5. Atomic structure and the periodic table
5.1. Light and Spectroscopy
5.1.2. The Characteristics of Light
5.1.3. Quantization and Photons
5.2. The Structure of the Hydrogen Atom
5.2.2. The Spectrum of Atomic Hydrogen
5.2.3. Particles and Waves
5.3. The Structure of Many-Electron Atoms
5.3.2. Orbital Energies
5.3.3. The Building-up Principle
5.4. A survey of Periodic Table
5.4.2. Blocks, Periods, and Groups
9. Chemical equilibrium
9.1. The Description of Chemical Equilibrium
9.1.2. Reactions at Equilibrium
9.1.3. The Equilibrium Constant
9.1.4. Heterogeneous Equilibria
Mode of delivery:
- Gapped lecture
- Group discussion
- Questioning and answering
Mode of assessment:
Quizzes, assignments, tests, mid-term and final examination.
Reference materials:
1. P.W. Atkins and J.A. Beran, General Chemistry, 2nd Ed., 1992.
2. R. Chang, General Chemistry: The Essential Concepts, 5th Ed., 2008
3. J.W. Hill and R.H. Petrucci, General Chemistry: An Integrated Approach, 2nd Ed., 1999.
4. J. E. Brady, J. W. Russel and J.R. Holum, General Chemistry: Principles and Structure,
5th Ed., 2006.
5. S. S. Zumdahal and S.A. Zumdahal, Chemistry, 7th Ed., 2007/
Course description:
Measuring mass, and volumes by using cylinder and burette, experimental errors, systematic and
random errors, significant digits/figures, beam balance, mean, mean deviation, Bunsen burner,
luminous and non-luminous flame, physical and chemical changes, properties and reaction of
substances, diffusion rates, kinetic theory of gases, Graham’s law of diffusion, percentage of
water of hydration, calculating equivalent weight; basic laboratory operations such as
recrystallization, simple distillation, fractional distillations and steam distillations.
Course rationale:
The course university practical chemistry is designed to make students more prepared to the all
practical chemistry courses starting from developing the general rules of laboratory, handling of
chemicals and instruments and operating skills of this instruments. In addition it is also designed
to refresh the previous preparatory chemistry concepts before tackling the advanced chemistry
courses. It ensures readiness of the students for the higher chemistry courses at university level
and hence the name University practical chemistry is given.
Course objectives:
Up on the completion of this course the students will be able to:
• grasp the general guidelines of laboratory
• develop the skill of mass and volume measurement
• Know the difference between systematic and random errors
• discuss the difference between physical and chemical changes
• operate Bunsen burner and discuss on parts and description of each part
• discus on the property of the flame of Bunsen burner
• verify the Graham’s law of diffusion and observe the motion of the molecules
• determine the percentage of water of hydration
• discuss on the methods of calculating equivalent weight
• carry out recrystallization, simple, fractional and steam distillations
Course outline
Experiment -1. Mass and volume measurements
Experiment -2. Bunsen burner
Experiment -3. Physical and chemical changes
Experiment -4. Diffusion of gases
Experiment-5. Determination of water of hydration
Experiment -6. Equivalent weight of a metal
Experiment-7. The effect of temperature on reaction rate
Experiment -8. Determination of solubility of salts
Experiment -9: Recrystallization
Experiment -10: Simple and Fractional distillations
Experiment -11: Extraction
Experiment -12: Steam distillation
Mode of delivery:
-Lecture by demonstration
-Group discussion during experiment time
-Questioning and answering
Mode of assessment:
-Experiment report-------------------40%
-Assignment---------------------------10%
-Attendance ----------------------------5%
-Final exam-----------------------------45%
-Total------------------------------------100%
Reference materials:
1. Experimental chemistry, Michell J. Seinko, Robert A. Plane, Stanley T. Marcus, 6th ed.
2. Ermias Dagne. Experiments in organic Chemistry I: Addis Ababa University; 1978
3. Laboratory manual for general and inorganic chemistry, Z. Vasilyeva, A. Granovskaya,
A. Taperova
4. Practical skills in chemistry John R. Dean, Alan M Jones, David Holmes, Rob Read,
Jonathan Weyers and Alan Jones.
5. General chemistry, UNO, KASK. J. David Rawn
Course description:
Introduction to the subject matter; Ionic equilibria; statistical evaluation of analytical data;
Solutions; titrimetric methods of analysis; gravimetric analysis:
Course rationale:
The course is designed to make the students develop competencies of chemical analysis, by using
the various chemical techniques such as gravimetric and/or titrimetric techniques. The course
familiarizes the students with statistical evaluation of analytical data. As a result the students,
after completion of the course, will develop the competency to carry out chemical analysis in
various fields such as chemical industry, agriculture, environmental chemistry, clinical
chemistry, medicine, pharmaceutical industries and others.
Course objectives:
Upon completion of this course the students will be able to:
• Describe the role of analytical chemistry in the society and day to day life;
• Describe different methods of chemical analyses;
• Discuss each step of the analytical process;
• compare and contrast different schemes of systematic cation and anion analysis;
• prepare solutions of different concentrations;
• describe some of the properties of solutions and chemical equilibria;
• describe the effect of different factors on solubility of a substance in a given solvent;
• discuss the application of solubility product principle and complex ion formation
reactions in chemical analyses;
• Discuss principles of redox reactions and their applications.
• Know different ways of validating analytical methods;
• apply different statistical tests to analytical data and indicate the reliability of
experimental results;
• distinguish among neutralization, precipitation, complexation and redox reactions and use
them as bases for quantitative determinations;
• select appropriate indicator for detecting the end point of a given titration;
• Carry out different titrimetric and gravimetric analyses.
Course outline:
1. Introduction
1.1 Definition of analytical chemistry
1.2 Roles of analytical chemistry
Mode of delivery:
- Lecture
- group discussion
- assignment in group or individually
- home work
Mode of assessment:
- Quizzes,
- assignments,
- tests,
- Mid-term and final examinations.
Reference materials:
1. Skoog, D.A.; West, D.M.; Holler, F.J. Fundamentals of Analytical Chemistry, 7th ed.;
Saunders College Publishing, New York, 1996.
2. Christian, G.D. Analytical Chemistry, 5th ed., John Wiley and Sons, Inc., New York,
1994.
3. Harris, D.C. Quantitative Chemical Analysis, 4th ed., W.H. Freeman and Company,
New York, 1995.
4. Jeffery, G.H.; Bassett, J.; Mandham, J.; Denney, R.C. Vogel’s Text Book of
Quantitative Chemical Analysis, John Wiley and Sons, Inc., New York 1991.
5. Manahan, S.E. Quantitative chemical analysis, Brooks/Cole publishing company,
California, 1986.
6. Fifield, F.W., Keale, D. Principles and practice of analytical chemistry, 3rd ed., Blakie
academic and professional, Glasgow, 1990.
7. Marmet, J.M.; Otto, M.; Widmer, H.M. (editors). Analytical chemistry, Wiley-VCH,
Weinheim,1998
Course description:
Selected experiments on neutralization, precipitation, complex formation, redox titrations and
gravimetric analysis, i.e., experiments on qualitative and quantitative analytical chemistry.
Course Rationale:
The course is designed for making the students know the classical techniques in both qualitative
and quantitative analysis. Moreover, the course familiarizes the students with basic principles of
gravimetric and titrimetric techniques. As a result the students, after completion of the course,
will develop the practical competency to carry out chemical analysis in various fields such as
chemical industry, agriculture, environmental chemistry, clinical chemistry, medicine,
pharmaceutical industries and others.
Objectives:
Upon completion of this course the students will be able to:
• Describe different methods of chemical analyses;
• analyze the presence and/or absence of cations and anions in a given sample;
• discuss the qualitative properties of selected cations and anions;
• describe the effect of different factors on solubility of a substance in a given solvent;
• discuss principles of redox reactions and their applications;
• distinguish among neutralization, precipitation, complexation and redox reactions and use
them as bases for quantitative determinations;
• select appropriate indicator for detecting the end point of a given titration;
• carry out different titrimetric and gravimetric analyses;
• interpret quantitative analytical results using figures;
• discuss and conclude qualitative and quantitative analytical results;
• compare the theoretical and practical aspects of analytical chemistry;
• Apply the different qualitative and quantitative techniques in their future career.
Course outline:
Experiments pool to be selected from for quantitative analyses:
Experiment 1: Gravimetric determination of Calcium
Experiment 2: Gravimetric determination of Iron
Experiment 3: Standardization of sodium hydroxide solution
Experiment 4: Determination of NaOH and Na2CO3 in the same solution
Experiment 5: Determination of Na2CO3 and Na2HCO3 in the same solution
Experiment 6: Determination of halides argentometrically
Experiment 7: Determination of Potassium dichromate using Sodium thiosulphate
Experiment 8: Determination of oxalate permanganometrically
Experiment 9: Determination of hardness of water
Experiment 10: Preparation of solutions from concentrated solids
Experiment 11: Preparation of solutions from liquids
Mode of delivery:
Brief lecture, group discussion, individual works, experimentation, demonstration
Mode of assessment:
Laboratory reports, class activities and regular attendance, quizzes and final examination
Reference materials:
1. Georg Schwedt. The essential guide to Analytical Chemistry, 2nd ed., Stuttgart-New York,
1996.
2. G. Svehla. Vogel’s qualitative inorganic analysis, 7th ed., 1996.
3. Negussie Retta. Quantitative Chemical Analysis Experiments for University Students
(manual), 2nd ed., Addis Ababa University, Sept. 2000.
4. Dr. Ivan Linko and Dr. Sree Lkshmi. Practical Analytical Chemistry I, Qualitative
Analysis (manual), Addis Ababa University, 1992.
5. I.T. Sidhwani and Sushmita Choduhry. Green alternative to qualitative analysis for
cations without H2S and other Sulfur-containing compounds, Journal, August 2008.
6. Harris, D.C. Quantitative Chemical Analysis, 4th ed., W.H. Freeman and Company, New
York, 1995.
7. J. Mendham. Quantitative Chemical Analysis, 6th ed., August 1999.
Course description:
Introduction to the subject matter; principles of chromatography; chromatographic methods and
instrumentation: gas chromatography, high performance liquid chromatography, supercritical
fluid chromatography, size exclusion chromatography, ion exchange chromatography,
electrophoresis; electroanalytical methods: conductometry, potentiometry, coulometry,
electrogravimetry and voltammetry; thermometric methods.
Course Rationale:
The course is designed to make the students develop competency in basic instrumental methods
of analysis. The course will familiarize the students with the basic knowledge of instrumentations
like in gas chromatography, high performance liquid chromatography, supercritical fluid
chromatography, size exclusion chromatography, ion exchange chromatography, electrophoresis,
potentiometry, conductometry, coulometry, electrogravimetry, voltammetry which are applicable
in various fields like, toxicology, environmental science, pharmaceuticals, quality controlling,
chemical industry, clinical chemistry, medicine and the like.
Course objectives:
After completing the course students will be able to:
• describe underlying principle governing chromatographic separations;
• distinguish among different chromatographic methods and discuss their applications;
• select appropriate conditions (mobile phase, stationary phase, column, detector, etc) for a
given chromatographic analysis;
• discuss the application of supercritical fluid chromatography;
• define electrophoresis and describe its application in chemical analysis.
• choose appropriate analytical method for analysis of a given sample;
• extract a given component from a sample using appropriate extraction technique.
• classify analytical methods into classical and instrumental methods and distinguish
between them;
• compare and contrast classical and instrumental methods with respect to speed,
sensitivity, precision, ease of automation, etc;
• describe underlying principle governing different electroanalytical methods; and
• discuss the qualitative and quantitative applications of different electroanalytical
methods.
Course outline:
1. Analytical separation techniques and classical method of analysis
2. Introduction to chromatographic separation
2.1 Historical background
2.2 Types of chromatography
2.3 Paper chromatography
2.4 Thin layer chromatography
2.5 Column chromatography
2.6 Efficiency of separation
2.7 Application (Qualitative and quantitative information)
3. Gas Chromatography (GC)
3.1 Principle of GC
3.2 Instruments for GC
3.3 Applications
4. High-performance Liquid Chromatography (HPLC)
4.1 Principle of HPLC
4.2 Instruments for HPLC
4.3 Parts of liquid (liquid) Chromatograph
4.3.1. Liquid (partition) chromatography
4.3.2. Liquid – solid (Adsorption) chromatography
4.3.3. Ion-exchange chromatography
4.3.4. Molecular exclusion chromatography
5. Introduction to Electro-analytical Chemistry
5.1 Electrochemical cells and cell potential
5.2 Current in electrochemical cells
5.3 Types of electro-analytical methods
6. Potentiometry
6.1 Basic principles
6.2 Types of electrodes
6.3 Instrumentation
6.4 Potentiometric Titration
7. Voltammetry
7.1 Excitation signals in voltammetry
7.2 Types of voltammetry
7.3 Polarography and Amperometry
8. Coulometry and Electrogravimetric Analysis
8.1 Types of coulometry
8.2 Separation of cathode and anode reactions
8.3 Current effect on voltages
9. Conductometry
9.1 Basic principles and Instrumentation
9.2 Application
9.3 Conductometric titration
10. Electrophoresis
Mode of delivery:
Lecture, group discussion, seminar on selected topics, reading assignments,
Mode of assessment:
Attendance, assignment in groups or individually, home work, quizzes, oral questions, tests, final
examination.
Reference materials:
1. D.A. Skoog, D.M. West and F.J. Holler, Fundamentals of Analytical Chemistry, 7th Ed.,
Saunders College Publishing, New York, 1996.
2. G.D. Christian, Analytical Chemistry, 5th Ed., John Wiley and Sons, Inc., New York,
1994.
3. D.C. Harris, Quantitative Chemical Analysis, 4th Ed., W.H. Freeman and Company, New
York, 1995.
4. G.H. Jeffery, J. Bassett, J. Mandham and R.C. Denney, Vogel’s Text Book of
Quantitative Chemical Analysis, John Wiley and Sons, Inc., New York 1991.
5. S.E. Manahan, Quantitative chemical analysis, Brooks/Cole publishing company,
California, 1986.
6. F.W. Fifield and D. Keale, Principles and practice of analytical chemistry, 3rd Ed., Blakie
academic and professional, Glasgow, 1990.
7. J.M. Marmet, M. Otto and H.M. Widmer (editors), Analytical chemistry, Wiley-VCH,
Weinheim, 1998.
Course description:
Experiments in chromatography (TLC, CC, GC, HPLC) and electroanalytical methods
(Potentiometry, Voltametry, Conductometry, coulometry, electrogravimetry, electrophoresis and
refractive index)
Course rationale:
The course is designed in order to make the students develop the practical competency and skills
in carrying out chemical analysis by using modern chromatographic and electroanalytical
instruments.
Course objective:
At the end of the course the students would be able to:
• Describe different types of analysis for the estimation of the concentration of an unknown
solution.
• Understand the theory behind every technique.
• Know the correct choice of the instrument for a given analysis.
Course outline:
1. Chromatography
1.1. Paper chromatography: Determination of Rf of the given substance (amino acid)
using an organic solvent
1.2. Thin layer Chromatography: Determination of Rf of a given dye (thymol blue,
bromo cresol, phenol red etc) using a solvent mixture
1.3. Determination of the number of constituents in a given mixture
2. Electrophoresis
2.1. Determination of the charge and distance moved by an amino acid by the
application of 300 V for a period of 1 hour using an electrophoretic power supply
2.2. Determination of the number of amino acids in the given mixture by
electrophoresis method
3. Potentiometry
3.1. Redox system: Estimation of the given ferrous ammonium sulphate
potentiometrically; a standard solution of 0.1 Potassium dichromate solution may
be provided
3.2. Acid-Base Titration: Estimation of hydrochloric acid potentiometrically using a
calomel electrode
3.3. Determination of single electrode potential; silver, zinc and copper electrodes may
be used
4. Conductometry
4.1. Acid-base Titration: Estimation of Hydrochloric acid conductometrically using
0.5N sodium hydroxide.
4.2. Cell constant: determination of cell constant of a given conductivity cell using a
conductivity meter
4.3. Equivalent conductance: determination of equivalent conductance of a given
strong electrolyte
5. Refractive Index
5.1. Constructing a calibration chart for the determination of sodium chloride or
potassium chloride; determination of unknown concentration of potassium
chloride.
5.2. Determination of percentage composition of the given mixture. Water and ethanol
may be used.
5.3. Studies on structural aspects.
5.4. Determination of Specific and Molar refractivity of some solutions.
Mode of assessment:
Practical examination/written examination may be conducted on the theories of various analytical
techniques. Reports submitted will be evaluated; attendance, observation while the student was
doing lab, oral questions and correcting laboratory report.
Mode of delivery:
Lecture method with demonstration of experiments. Students have to do in batches all the
experiments. Practical laboratory experiments, questioning, report writing.
Reference materials:
1. G. Schwedt, The essential guide to Analytical Chemistry, 2nd Ed., Stuttgart-New York,
1996.
2. G. Svehla, Vogel’s qualitative inorganic analysis, 7th Ed., 1996.
3. N. Retta, Quantitative Chemical Analysis Experiments for University Students (manual),
2nd Ed., Addis Ababa University, 2000.
4. Harris, D.C. Quantitative Chemical Analysis, 4th Ed., W.H. Freeman and Company, New
York, 1995.
5. J. Mendham, Quantitative Chemical Analysis, 6th Ed., August 1999.
Course description:
Introduction to the subject matter; analytical methods based on the interaction of electromagnetic
radiation with matter; atomic absorption and emission spectroscopy; instrumentation for
spectroscopy; ultraviolet and visible spectroscopy; infrared; nuclear magnetic resonance;
fluorescence; phosphorescence.
Course rationale:
The course is designed to make the students develop the theoretical competency in using
spectroscopic techniques for analytical purposes. The course familiarizes the students with the
theoretical background of the principles of spectroscopic instruments like atomic absorption,
atomic emission, ultraviolet-visible and infrared spectrophotometers ; nuclear magnetic
spectrometer; fluorescence and phosphorescence instrumentations, which are used in various
fields like, toxicology, environmental science, pharmaceuticals, quality controlling, chemical
industry, clinical chemistry, medicine and the like.
Course objectives:
After completing this course students will be able to:
• describe electromagnetic radiation;
• define terms such as spectroscopy, absorption and emission of emr
• discuss the qualitative and quantitative applications of different spectroscopic methods;
• elucidate structure of compounds from spectra by using data from joint spectroscopic
techniques;
• describe the underlying principles of different spectroscopic methods; and
• draw block diagrams for instruments of different spectrometric method.
Course outline:
1. Introduction to Spectroscopy
1.1 Electromagnetic Radiation and its interaction with matter
Mode of delivery:
Lecture, group discussion, seminar on selected topics, reading assignments.
Mode of assessment:
Attendance, assignment in groups or individually, home work, quizzes, oral questions, tests, final
examination.
Reference materials:
1. D.A. Skoog and J.J. Leary, Principle of Instrumental Analysis, 4th Ed. Saynders College
publishing, 1992.
2. C.N. Banwell and E.M. McCash, Fundamentals of Molecular spectroscopy, McGraw
Hill, 1994.
3. R. Davis and M. Freason, Mass spectrometry (analytical spectrometry by open learning),
John Wiley and Sons, 1987.
4. H. Gunter, NMR Spectroscopy, 2nd Ed., John Willey and Sons, 1995.
5. J. Hollas, Modern Spectroscopy, 3rd Ed. John Willey and sons, 1996.
6. J.D. Ingle and S.R. Crouch, Spectrochemical analysis, Prentice Hall, 1988.
7. L.D. Field, S. Sternhell and S. Kalman, Organic structure from spectra, 2nd Ed., John
Willey and sons, 1995.
8. J.R. Chapman, Organic Mass Spectrometry, 2nd Ed.; John Willey and Sons, 1993.
9. D.H. Williams and I. Fleming, Spectroscopic method in organic chemistry, 5th Ed.
McGraw Hill, 1995.
10. G.W. Ewing, Instrumental Method of Chemical Analysis, 5th Ed., 1985.
11. R.M. Silverstein, G.C. Bassler and T.C. Morril, Spectrometric Identification of Organic
Compounds, 5th Ed., John Willey and Sons, 1991.
Course description:
Experiments on spectroscopic techniques (absorption and emission techniques, molecular
spectroscopic techniques)
Course rationale:
The course is designed to make the students develop the practical competency in using
spectroscopic techniques for analytical purposes. The course familiarizes the students with the
practical skills of operating spectroscopic instruments.
Course objective:
• Describe different types of analysis for the estimation of the concentration of an unknown
solution;
• Understand the theory behind every technique;
• Know the correct choice of the instrument for a given analysis;
• Know the extent of accuracy in each method;
• Understand the precautions required in every method;
• Identify different parts of selected spectroscopic instruments and describe their respective
functions;
• Operate and run different spectroscopic instruments and generate spectrum of a given
substance;
• Use appropriate spectroscopic method for quantitative determination of sample
components; and
• Elucidate structure of a compound using joint spectroscopic techniques.
Mode of assessment:
Practical examination or written examination may be conducted on the theories of various
analytical techniques. Reports submitted will also be evaluated. Attendance, observation while
the student was doing laboratory and oral questions will have their own value.
Mode of delivery:
Lecture method with demonstration of experiments. Students have to do in batches all the
experiments.
Reference materials:
1. G.H. Jeffery, J. Bassett, J. Mandham and R.C. Denney, Vogel’s Text Book of
Quantitative Chemical Analysis, 6th Ed., John Wiley and Sons, Inc., New York 2000.
2. D.C. Harris, Quantitative Chemical Analysis, 4th Ed., W.H. Freeman and Company, New
York, 1995.
Course description:
Systematic analysis of real samples: sampling, preservation and preparation of samples for the
determination of the major, trace elements, inorganic compounds (speciation) and organic
compounds; biological samples; food and beverages; water and waste water samples; soils and
related samples.
Course rationale:
The course is designed to make the students develop the competency to analyze real samples
based on what they have already learnt. The course will familiarize the students with the
techniques of sampling, storage, and analysis of real samples.
Course objective:
After completing this course students will be able to:
• Select appropriate sampling and preservation of a particular real sample
• Identify preparation methods for analysis of metals by different methods
• Perform experiments on water, soil and air
Course outline:
1. Systematic analysis of real samples
2. Sampling, preservation and preparation of samples for the determination of the major,
trace elements, inorganic compounds (speciation) and organic compounds
3. Biological samples
4. Food and beverages samples
5. Water and waste water samples
6. Soils and related samples
Mode of delivery:
Practical laboratory experiments, questioning, report writing.
Harmonized Curriculum for B.Sc. degree in Chemistry 30 | P a g e
Harmonized Curriculum for B.Sc. degree in Chemistry
Mode of assessment:
Attendance, observation while the student was doing lab, oral questions, correcting laboratory
report, practical examination and written examination.
Reference materials:
To be designated at commencement of the course.
Course description:
Atomic structure, periodic trends, chemical bonding, Acid-base theory and solvent system,
chemistry of main group elements; chemistry of hydrogen, s-block, p-block and noble gases;
compounds of main group elements: synthesis, reactions and applications.
Course objectives:
After completion of this course, students will be able to:
• Discuss the current view of atomic structure
• Write & explain the electronic configuration
• Relate electronic configuration to the classification of elements in the periodic
table and their properties
• Explain the basic concepts of chemical bonding and structure
• Have a general overview of the descriptive chemistry of hydrogen and s p, d
and f- block elements
Course outline
1. Overview of Atomic theory and Periodic Table
1.1. Some principles of quantum mechanics
1.2. Radial and Angular wave functions and the quantum numbers
1.3. The periodic table and chemical periodicity
2. Chemical Bonding and Structure
2.1. Types of chemical bonding
2.2. Shape of simple covalent molecules
2.3. Theories of bonding for covalent molecules
2.4. Ionic solids
2.5. Metallic bonding and bonding theories
3. Acid base theory and the solvent system
3.1. Basic definitions
3.1.1. Strength of binary acids
3.1.2. Strength of Oxyacids
3.1.3. Strength of Lewis acid and base
3.2 Solvent systems
3.3 Hard –soft acid and bases
Mode of delivery:
Gaped lecture, lecture–demonstration, group work and presentation, individual assignment and
presentation, and project work.
Mode of assessment:
Oral questions, tests at the end of each chapter, assignment, group work, summative exam at the
end of the semester
Reference materials:
1. Basic Inorganic Chemistry, F.A Cotton, G. Wilkinson, and P.L. Gaus.
2. An Introduction to Inorganic Chemistry, Purcell and Kotz.
3. Modern Aspect of Inorganic Chemistry, H.J.Emeleus and A.G.Sharpe.
4. Inorganic Chemistry, Principles of Structure and Reactivity, J.E. Huheey.
5. A Text Book of Inorganic Chemistry, K N Upadhyaya 3rd edition.
6. Introduction to Inorganic Chemistry, G.I Brown.
Course description:
Group properties of transition elements: general physical and chemical properties, variable
oxidation states, stoichiometric and non-stoichiometric compounds, catalytic properties etc,
coordination compounds (historical development, nomenclature, isomerism, VBT, CFT, MOT),
metals and metallurgical processes, descriptive chemistry of transition and inner transition
elements (electronic structure, oxidation states, occurrences, isolations, reactions and uses of
selected d-block and f-block elements, and chemistry of their compounds).
Course rationale:
This course, Inorganic Chemistry II, allow the student to reflect the ease of recovery of metals
from their ores and to the ways in which the various metals and their compounds are handled in
the laboratory. It also provides responsiveness of electronic structure. Furthermore, the metallic
elements are the most numerous of the elements and their chemical properties are central to both
industry and contemporary research.
Course objectives:
After completion of this course, students will be able to:
• Have a clear understanding of the group properties of the transition elements
• Explain coordination compounds with respect to their formation, nomenclature,
geometry, isomerism and bonding theories (VBT, CFT and MOT)
• Describe metallurgical process in metals
• Have a general overview of the descriptive chemistry of transition elements
Course outline:
1. Chemistry of d-block elements
1.1 General physical properties of the elements
1.1.1. Density, melting and boiling points
1.1.2. Trends in the periodic table: size, IE, EN, etc.
1.2 General chemical properties
1.2.1. The inherent variable oxidation states and reactivity
1.2.2. Non-stoichiomtric compounds
1.3 Catalytic properties of the metals in the synthesis of:
1.3.1. Organic compounds
1.3.2. Inorganic compounds
1.4 Studies with specific reference to first series of transition metals
1.4.1 Occurrence and importance of compounds of the metals
2. Chemistry of f-block elements
2.1. General physical and chemical properties
2.1.1 Density, melting and boiling points, spectra, etc.
2.1.2 Trends in the periodic table: size, IE, EN, etc.
2.1.3 Reactivity
2.1.4 Occurrence and separation of their compounds
Mode of delivery:
Gapped lecture, lecture demonstration, group work and presentation, and project work.
Method of assessment:
Oral questions, tests at the end of each chapter, assignment, group work assessment, summative
exam at the end of the semester.
Text: A new Concise Inorganic Chemistry, J.D. Lee., 3rd or 5th edition.
Reference materials:
1. Basic Inorganic Chemistry, F.A cotton, G.Wilkinson, and P.L. Gaus.
2. An Introduction to Inorganic Chemistry, Purcell and Kotz.
3. Modern Aspect of Inorganic Chemistry, H.J.Emeleus and A.G.Sharpe.
4. Inorganic Chemistry, Principles of Structure and Reactivity, J.E. Huheey.
5. A Text Book of Inorganic Chemistry, K N Upadhyaya 3rd edition.
6. Introduction to Inorganic Chemistry, G.I. Brown.
Course description:
The chemistry of selected transition elements: titanium, vanadium, chromium, manganese, iron,
cobalt, nickel, copper, zinc, silver, cadmium, and mercury.
Course rationale:
The course is designed to give students competency in chemistry of transition elements mainly
titanium, vanadium, chromium, manganese, cobalt, nickel, copper, zinc, silicon, cadmium, and
mercury. The course familiarizes the students with the different oxidation states and reactions of
transition elements and their compounds. The students will be able to prepare compounds of
transitional metals and study their behaviours in different media (acidic, basic, neutral). The
course equips the students with the required competency to work in areas that require the
competency such as the chemical industry, agriculture, environmental chemistry, Geology,
Biology and others.
Course objective:
After completing this course, students will be able to:
• have a clear understanding of the group properties of the selected transition elements
• Preparation, identification and properties of compounds formed from selected
transition elements.
Harmonized Curriculum for B.Sc. degree in Chemistry 34 | P a g e
Harmonized Curriculum for B.Sc. degree in Chemistry
• Reactions of various oxidation states of the selected transition elements and study the
properties of the known compounds under different kinds of media (acidic, alkaline,
and neutral).
• Conversion of complex compounds of the transition elements into simplified once
using different kinds of techniques.
Course outline:
1. The chemistry of Titanium
1.1. Reaction of titanyl sulphate with aqueous NaOH and ammonia; preparation of
Orthotitanic acid
1.2. Reaction of titanyl sulphate with ammonium sulphide
1.3. Behaviour of Orthotitanic acid with respect to dilute sulphuric acid and sodium
hydroxide
1.4. Conversion of Orthotitanic acid in to Met titanic acid
2. The Chemistry of Vanadium
2.1. Reaction of Vanadium (V) compounds
2.2. Preparation of vanadium penta oxide
2.3. Dissolution of vanadium pentoxide in sulphuric acid and aqueous alkali; amphotoric
behaviour
2.4. Reaction of vanadium pentoxide with water, ”Metavanadic acid”
2.5. Conversion of tetra vanadate in to Hexa vanadate
2.6. Preparation of sparingly soluble vanadates
2.7. Synthesis of ammonium Thiovanadate and vanadium penta sulphide
2.8. Identification of vanadium (V) by means of the peroxo vanadium (V) reaction
2.9. Reaction of vanadium (IV) compounds
2.9.1. Preparation of vanadium dioxide
2.9.2. Amphoteric properties of vanadium dioxide
2.9.3. Reaction of vanadium (IV) by sulphite in aqueous solution
2.9.4. Hydroxide of tetravalent vanadium
2.9.5. Reducing properties of tetravalent vanadium; reduction of permanganate in acidic
medium
2.9.6. Identification of vanadium (v) by reduction with hydrochloric acid and
reoxidation with iron (III)
3. The Chemistry of Manganese
3.1. Manganese (II) compounds
3.1.1. Preparation of manganese (II) hydroxide and its oxidation by atmospheric oxygen
3.1.2. Action of ammonia on divalent manganese salts in the absence and in the presence
of ammonium salts
3.1.3. Oxidation of manganese (II) to its tetravalent state by bromine in alkaline medium
3.1.4. Oxidation of manganese (II) to heptavalent manganese by bromine in alkaline
solution with Cu (II) as a catalyst
3.2. Manganese (IV) compounds
3.2.1. Preparation and properties of permanganic anhydride
3.2.2. Thermal decomposition of potassium permanganate
3.2.3. pH dependence of the Oxidizing properties of potassium permanganate, Reaction
with sodium sulphite in acidic, neutral and alkaline medium
3.2.4. Oxidation of hydrogen peroxide by potassium permanganate
3.2.5. Oxidation of alcohol by potassium permanganate in acidic and alkaline medium
3.2.6. Synproportionation of manganese (II) and manganese (VII)
4. The chemistry of Chromium
Mode of delivery:
Practical laboratory experiments, questioning, report writing
Mode of assessment:
Oral questions, flow chart, observation, lab report, Group work Assessment, tests at the end of
each session, practical examination, and summative exam at the end of the semester.
Reference materials
1. A new Concise inorganic chemistry, J.D.Lee., 3rd or 5th edition.
2. Basic inorganic Chemistry, F.A cotton, G. Wilkinson, and P.L. Gaus.
3. An introduction to Inorganic chemistry, Purcell and Kotz.
4. Modern aspect of Inorganic chemistry, H.J. Emeleus and A.G. Sarpe.
5. Introduction to inorganic chemistry, G.I Brown.
Course description:
Symmetry and Group Theory; magneto chemistry; reaction mechanisms: inert and labile
complexes; substitution in octahedral and square planar complexes; trans effect; electron transfer
reactions: outer sphere and inner sphere mechanisms; Bioinorganic chemistry: metal ions and
their biological importance; photosynthesis; nitrogen fixation; oxygen carriers; transition metals;
organo-transition metal chemistry: synthesis, structure and bonding, reactions, applications.
Course rationale:
This course, Inorganic Chemistry III, create a chance to deal with concept of symmetry which
helps to determine the physical properties of a molecule and provides hints about how reactions
might occur. The electronic spectra help to demonstrate how to interpret the origins of the
electronic spectra of coordination compounds and to correlate these spectra with bonding.
Another feature that emphasize is the important role of steric congestion (which is responsible for
the ability of some organometallic compounds to withstand hydrolysis, and has led to the
synthesis of compounds containing multiple bonds between heavy metals) around the central
atom. The d and f-block elements has grown into a thriving areas that spans interesting new types
of reactions, unusual structures, and practical applications in organic synthesis and industrial
catalysis. Furthermore, the bioinorganic chemistry motivates to study further on the role of metal
ions in biology and their functions, pharmaceutical applications of metal ions and use of
inorganic compounds for therapy purpose.
Course objective:
• Understand the basic principles of Group theory;
• Apply the main concepts of group theory ;
• Demonstrate clear understanding of the concepts of Coordination Chemistry;
Organometallic chemistry and Bioinorganic Chemistry;
• Determine the Magnetic property of Organometallic complexes;
• Understand the structure and properties of organometallic complexes; and
• Classify Organometallic compounds.
Course outline:
1. Symmetry and Group Theory
1.1. Symmetry elements and operations
1.2. Point groups and molecular symmetry
1.3. Uses of point group symmetry
2. Coordination Chemistry
2.1. Introduction (Bonding in coordination compounds: Historical perspective, VBT,
CFT, MOT, LFT)
2.1.1. Formation and Stabilities of coordination compounds
2.1.2. Preparation of coordination compounds
2.1.3. Reactivities of coordination compounds
2.1.4. Kinetics and reaction mechanisms
2.1.5. Addition reactions
2.1.6. Electron transfer reactions
2.1.7. Spectral properties of transition metal compounds
2.1.8. Energy levels in an atom
2.1.9. Spin –orbit coupling
2.1.10. Russel -Sounder’s coupling
2.1.11. Spectroscopic terms and their determination
2.1.12. Terms of non-equivalent electrons
Mode of delivery:
Gaped-lecture, lecture-demonstration, group work, presentation, and project work.
Method of assessment:
Oral questions, tests at the end of each chapter, assignment, group work assessment, summative
exam at the end of the semester.
Course description:
Synthesis, isolation and characterization of a variety of inorganic compounds and the study of their
chemical properties.
Course rationale:
This course is designed to give the students competency in analyzing inorganic
compounds/species both in laboratory and in real samples. They will synthesize, isolate and
characterize inorganic species by using classical and instrumental techniques.
Course outline:
1. Synthesis of inorganic complexes and their characterization by various physicochemical and
spectroscopic techniques; selection can be made from the following list or from current
literature.
1.1. Metal acetylacetonates
1.2. Cis and trans isomers of [Co(en)2Cl2]Cl
1.3. Ion-exchange separation of oxidation states of vanadium.
1.4. Preparation of Ferrocene.
1.5. Preparation of triphenyl phosphene Ph3P, and its transition metal complexes.
1.6. Determination of Cr(III) complexes.
1.7. Tin (IV) iodide, Tin(IV) chloride, Tin(II) iodide.
1.8. (N,N)-bis(salicyldehyde)ethylenediamine Salen H2; and its cobalt complex
[Co(Salen)].
1.9. Reaction of Cr(III) with multidentate ligands, a kinetics experiment.
1.10. Vanadyl acetylacetonate.
1.11. Mixed valence dinuclear complex of Mangenese(III,IV).
1.12. Other new novel synthesis reported in literature from time to time II (a) Analysis
of ores, alloys and inorganic substances by various chemical methods.
2. Analysis of the samples by instrumental methods such as flame photometer, atomic
absorption spectrophotometer, pH-meter, potentiometer, turbidimeter, and electrochemical
methods.
3. Separation of mixtures of metal ions by ion exchange chromatography
4. Synthesis and thermal analysis of group II metal oxalate hydrates
Mode of delivery:
Practical laboratory experiments, questioning, report writing.
Method of assessment:
Oral questions, tests at the end of each chapter, assignment, group work assessment, summative
exam at the end of the semester.
Course description:
Historical background of Organic Chemistry; Bonding, Structure and Reactivity; Functional
groups (Nomenclature, physical and chemical properties), Stereochemistry: Chirality and Optical
activity; Stereoisomerism; Configuration: Cahn-Ingold-Prelog sequence rules for assigning
configuration, Introduction to major classes of Organic Reactions: Substitution Reactions,
Elimination reactions, Addition reactions; Rearrangement reactions.
Course rationale:
This course is primarily designed to offer basic understanding of structures, reactivities and
synthesis of simple organic compounds and the relationships between structure and properties.
Although the course follows mechanistic approach to reactions of organic compounds
(substitution, elimination, addition, rearrangement reactions), a chapter is devoted to brief
discussion of functional groups, their typical reactions and synthesis. This will enable the
students to understand the twin strategies of studying chemistry of the millions of organic
compounds by either classifying them according to the reaction types they undergo (mechanistic
approach) or according to their functional groups (functional group approach). The course also
introduces the concept of stereochemistry and stereoisomerism (configurational and
conformational isomerism) and its importance in organic reactions. This enables the students to
appreciate the more subtle types of isomerism than the obvious structural (constitutional)
isomerism. This course will complement practical organic chemistry-I course as theoretical
background and will create basic knowledge for next organic chemistry courses.
Course objectives:
Individuals who successfully complete this course will be able to:
• Understand historical development of organic chemistry,
• Draw reasonable and acceptable structural representations of organic molecules,
• Understand the modern bonding concepts in organic compounds and their influence
on properties of compounds,
• recognize various common organic functional groups,
• devise the preparation and reactions of common organic functional groups,
• understand stereochemistry, recognize conformational and configurational isomerism
as additions to stereoisomerism besides geometrical isomerism,
• Employ stereochemical considerations when analyzing mechanisms and
transformations,
• recognize the major types of heterolytic organic reactions,
• Describe mechanisms of addition, substitution, elimination and rearrangement
reactions.
Course outline:
1. Bonding, Structure and Reactivity
Method of assessment:
Oral questions, Short tests at the end of each chapter, assignment, group work assessment,
summative exam at the end of the semester.
Reference materials:
1. F.M. Menger, D. J. Goldsmith, L. Mondev, "Organic Chemistry", A concise
approach, 2nd Ed., 1975.
2. F.A. Carey, "Organic Chemistry", 5th Ed., 2003.
3. T.W.G. Solomons, Organic Chemistry, 7th Ed., 2004.
Course description:
The course is designed to give basic understanding and concepts of practical organic chemistry.
In the organic chemistry laboratory students will learn to decode some of the nature’s secrets and
a new language that will enable them to describe what they see through the magnifying class of
experimental organic chemistry. In this course students will also learn to work with organic
chemistry by obtaining them, identifying them, and transforming them. Furthermore, they will
learn many separation and purification techniques such as recrystallization, distillation,
chromatography, sublimation and extraction. It is extremely important that the students carefully
learn the scientific principles up on which each experiment is based.
Course rationale:
This course designed to make the students aware of basic organic laboratory activities such as
simple recrystallization, melting point determination, simple, steam and fractional distillation,
and chromatography techniques. In addition to this student will prepare simple organic
compounds like soap, aspirn in laboratory scale. Student will learn the laboratory safely and
regulation rules of organic laboratory. The course will give basic knowledge and skill on
experimental organic chemistry because organic chemistry is everywhere, from the delicate smell
of violets to the paper these words are printed on. It is in the laboratory where the advances of
science are made. Without laboratory work, science would be just a poetic fabrication.
Course objectives:
Upon successful completion of the course students will be able to:
• Train in performing organic chemistry experiments that have relevance in industrial,
teaching medical and biological fields.
• discuss the techniques used to purify contaminated organic compounds
• Study characteristics of organic compounds
• Develop an ability to synthesize different organic compounds
• Design and interpret their own experiments
• Understand the desirable techniques used to separate organic compounds from a mixture
• Proficient in the most important aspect of laboratory work
• Suggest methods of improving the experiment by pointing out the drawbacks encountered
and sources of errors
Course outline:
Experiment 1: Survey of Some Functional Groups
Experiment 2: Molecules in Three Dimensions (Stereochemistry)
Experiment 3: Nucleophilic Substitution at a Saturated Carbon: Preparation of N-Butyl Bromide
Experiment 4: Cyclohexene from Cyclohexanol
Experiment 5: Preparation of Aspirin
Experiment 7: Fats, Oils and Soaps: Preparation and Properties of Soap
Experiment 8: Olefins from Alcohols
Experiment 9: Introduction to Chromatography
Experiment 10: Diels-Alder Reactions
Experiment 11: Qualitative Organic Analysis
Mode of delivery:
Brief lecture, laboratory method, demonstration, gapped lecture, group discussion, and individual
work.
Mode of assessment:
• Flow chart preparation
• Observation writing
• Laboratory report
• Before, While and post lab evaluation
• Individual and group assessment
• Oral questions
• Final examination
Reference materials
1. Ermias Dagne. Experiments in organic Chemistry I: Addis Ababa University; 1978
2. Wendimagegn Mammo. Practical Organic Chemistry II Laboratory manual: Addis Ababa
University; 1996.
3. Hassan Bakr Amin, Riyadh. Practical Organic Chemistry: King Saud University, 2007
4. Vogel, A. I.; Furniss, B. S.; Vogel, Arthur Israel. Vogel's Textbook of practical organic
Chemistry; Longman Scientific & Technical; Wiley: London; New York, 1989.
5. Richard C. Larock. Comprehensive Organic Transformations: A Guide to Functional Group
Preparations. 1989
6. Corey, E. J., Angew. Catalytic Enantioselective Diels-Alder reactions: Methods, mechanistic
fundamentals, pathways, and applications. Chem, Int. Ed. Engl., 2002, 41, 1650.
Course description:
Concept of aromaticity; electrophilic and nucleophilic aromatic substitution reactions; the
properties, reactions and preparations of amines, Reaction of Carbonyl Compounds ( aldehydes,
ketones and carboxylic acids and their derivatives); oxidation-reduction reactions, chemistry of
biomolecules (carbohydrates, lipids, amino acids and proteins); Nucleic acids.
Course rationale:
This course designed to make students aware of organic reactions in detail and depth. It will
elaborate chemistry of aromatic, amine, carbonyl compounds, carboxylic acid, and oxidation–
reduction reactions. In addition, biological molecules such as carbohydrates, amino acids,
peptides, lipid, and nucleic acids are introduced to address basic concepts about natural product
chemistry.
Course objectives:
At the end of the course the students will be able to:
• Understand the concept of the aromaticity
• Distinguish aromatic compounds from the non aromatic ones
• Describe the mechanism of electophilic and nucliophilic aromatic substitution
reactions
• Describe the various chemical properties and reactions of carbonyl compounds
• Describe the various chemical properties and reactions of amines
Course outline:
1. The Chemistry of Aromatic Compounds
1.1 Aromaticity
1.2 Properties of Benzene and its Derivatives
1.3 Heterocyclic Aromatic Compounds
1.4 Aromatic Substitution Reactions and their Mechanism
1.4.1 Halogenation
1.4.2 Nitration
1.4.3 Friedel-Crafts Alkylation
1.4.4 Acylation
1.4.5 Sulphonation
1.4.6 Directing Effects of Substituents
1.4.7 Examples of Electrophilic Aromatic Substitution Reactions
1.4.8 Representative Reactions of pyrrole, furane, thiophen and pyridine
1.5 Nucleophilic Aromatic Substitution Reactions
1.5.1 Reactions of Aryl halides
1.5.2 Mechanisms of Nucleophilic Aromatic Substitution Reactions
1.6 Reactions of Aromatic Side Chains
1.6.1 Oxidation and Substitution of Alkyl Side-Chains
1.6.2 Reduction of Nitro Groups and Aryl Ketones
1.6.3 Conversion of Halogens to Organometallic Reagents
1.6.4 Hydrolysis and Fusion of Sulphonic Acids
1.6.5 Modifying the Influence of Strong Activating Groups
1.6.6 Diazotization of Primary Aromatic Amines and their Usefulness in
Synthesis of Aromatic Derivatives
2. Amines
2.1 Nomenclature & Structure
2.2 Properties of Amines: Physical and chemical properties
2.3 Basicity of Nitrogen Compounds
2.4 Acidity of Nitrogen Compounds
2.5 Reactions of Amines
2.6 Electrophilic Substitution at Nitrogen
2.7 Preparation of 1º-, 2º & 3º-Amines
2.8 Reactions with Nitrous Acid
2.9 Reactions of Aryl Diazonium Intermediates (See Diazotization Reactions)
2.10 Elimination Reactions of Amines (See Hofmann Eliminations)
3. Reactions of Carbonyl Compounds
3.1 Addition Reactions
3.1.1 Hydrates
3.1.2 Hemiacetals
3.1.3 Cyanohydrins
3.1.4 Carbinolamines
3.1.5 Addition of Grignard Reagents
3.1.6 Addition of Hydrogen
3.1.7 Hydride Additions (lithium-aluminum hydride and sodium-borohydride)
3.2 Addition-Elimination Reactions
3.2.1 Imines and related compounds
Mode of delivery:
Gaped-lecture, lecture-demonstration, group work & presentation & project work.
Method of assessment:
Oral questions, Short tests at the end of each chapter, assignment, group work assessment,
summative exam at the end of the semester.
Reference materials:
1. F.M. Menger, D.J. Goldsmith; L. Mandle, Organic chemistry: A Concise Approach, 2nd
Ed., 1974
2. T.W G. Solomons, Organic Chemistry, 7th Ed., 2004.
3. J. McMurry, Organic Chemistry, 4th Ed., 1996.
4. F. A. Carey, Organic Chemistry, 3rd Ed., 1996.
Course description:
Esterification reactions; acetylation of aniline; p-nitroaniline from acetanilide; azo dyes and the
dying process, oxidation of alkyl arenes; synthesis using the aldol condensation, Friedel-Crafts
reaction; and extraction of limonene from citrus fruit; isolation of caffeine from tea.
Course rationale:
This course designed to integrate the theoretical organic reaction with small-scale laboratory
practice. The course enable students to understand organic reactions such as Esterification
reactions; dehydration, acetylation, oxidation, aldol condensation, Friedel-Crafts reaction; and
the Diels-Alder reaction. Extraction technique is very helpful in organic research. Thus, under
this course extraction of limonene from citrus fruit and isolation of caffeine from tea are included
to introduce basic extraction skills. In addition to this, students will understand dying process.
Course objectives:
At the end of the course the students will be able to:
• Carry out small-scale laboratory synthesis involving esterifications , dehydrations,
acetylations, oxidations, aldol condensation, Friedel-Crafts reactions; and the Diels-
Alder reactions;
• Synthesize various dyes; and
• Interconvert one class of organic compounds to others.
Course outline
Experiment 1: p-Nitroaniline
Experiment 2: Acetylation of Aromatic-Amines: Preparation of Acetanilide
Experiment 3: Oxidation of Alkylarenes
Experiment 4: Azo Dyes and Ingrain Dyeing
Experiment 5: Kobel-Schmitt reaction: Preparation of β-Resorcyclic Acid (2,4-Dihydroxybenzoic Acid)
Experiment 6: Esterification: Preparation of Amyl Acetate
Experiment 7: The Aldol Condensation and Cannizzaro Reaction
Experiment 8: Preparation of Aldehydes and Ketones by Oxidation of Alcohols
Experiment 9: Introduction to Proteins
Experiment 10: Introduction to Carbohydrates
Mode of delivery:
Brief lecture, laboratory method, demonstration, gapped lecture, group discussion, and individual
work
Mode of assessment:
• Flow chart preparation
• Observation writing
• Laboratory report
• Before, while and post lab evaluation
• Individual and group assessment
• Oral questions
• Final examination
Reference materials:
1. Ermias Dagne. Experiments in organic Chemistry I: Addis Ababa University; 1978
2. Wendimagegn Mammo. Practical Organic Chemistry II Laboratory manual: Addis Ababa
University; 1996.
3. Vogel, A. I.; Furniss, B. S.; Vogel, Arthur Israel. Vogel's Textbook of practical organic,
Chemistry; Longman Scientific & Technical; Wiley: London; New York, 1989.
4. Whitford, D. Proteins: structure and function; John Wiley & Sons: Hoboken, NJ, 2005.
5. Richard C. Larock. Comprehensive Organic Transformations: A Guide to Functional Group
Preparations. .1989
6. Kürti, L.; Czakó, B. Strategic applications of named reactions in organic synthesis:
background and detailed mechanisms; Elsevier Academic Press: Amsterdam; Boston, 2005.
7. E. J. Corey, Angew. Catalytic enantioselective Diels-Alder reactions: Methods, mechanistic
fundamentals, pathways, and applications. Chem, Int. Ed. Engl., 2002, 41, 1650.
Course objective:
At the end of this course, students will be able to:
• Explain the mechanism of different types of reaction
• Explain factors influencing electron availability
• Correlate reactivity with structure
• Investigate reaction mechanism using kinetics
• Discuss energetic of reactions
• Discuss methods of establishing reaction mechanism
• Propose reaction mechanism for different reaction
• Understand pericyclic reactions.
Course description:
Correlation of structure with reactivity; linear free energy relationships; energetics, kinetics and
methods of establishing reaction mechanisms; the chemistry of reactive intermediates
(carbocations, carbanions, free radicals, carbenes and nitrenes); pericyclic reactions; applications
of Frontier Orbital Theory in electrocyclic reactions, cycloaddition and sigmatropic
rearrangements, Structure Elucidation of Organic Molecules using molecular spectroscopy.
Course rationale:
This course is designed to introduce organic reaction mechanism. It will elaborate correlation of
structure with reactivity, methods of establishing reaction mechanisms, and the chemistry of
reactive intermediates. For advanced organic chemistry the students should understand
applications of Frontier Orbital Theory in electrocyclic reactions, cycloaddition and sigmatropic
rearrangements. The course will enable the students to explain organic reactions with reasonable
mechanism. A chapter on spectroscopic methods of structure elucidation is included to enable the
students to elucidate structures of organic molecules.
Course outline:
1. Structure, Reactivity and Mechanism
1.1 Atomic orbital
1.2 Hybridization
1.3 Bonding in Carbon compound (Single, Double, Triple bonds)
1.4 The breaking and forming of bond
1.5 Factors influencing electron availability
1.5.1 Inductive effects
1.5.2 Mesomeric effects
1.5.3 steric effects
1.5.4 Effects of the medium
1.6 Correlation of structures with reactivity.
1.6.1 Electron demand
1.6.2 The Hammett equation
1.6.3 Substituent constant (σ)
1.6.4 Reaction constant (ρ)
2. Energetic, Kinetics and investigation of reaction mechanisms
2.1 Energetics of a Reaction: Thermodynamic Requirement for a Reaction
2.2 Kinetics of reaction
2.2.1 Reaction rate and free energy of activation
2.2.2 The rate-determining step
2.2.3 Molecularity
2.2.4 Kinetic Requirement for a Reaction
2.2.5 Kinetic and Thermodynamic Control
2.2.6 The Hammond Postulate
2.3 Methods of establishing reaction mechanism
2.3.1 The nature of the products
2.3.2 kinetic data
2.3.3 the use of isotopes (kinetic use of isotopes and non-kinetic use of isotopes)
2.3.4 the study of the reactive intermediates (Isolation, detection and trapping of
intermediates)
3 The chemistry of reactive intermediates
3.1 Carbinions
3.1.2 Carbanion generation
Mode of delivery:
Lecture, Lecture- demonstration, Assignment, inquiry, Laboratory, Discussion methods and
questioning techniques.
Mode of assessment:
Assignments, presentation, mid exam, Final exam, and continuous assessment techniques of
various types will be used.
Reference materials:
1. P. Sykes; Guide Book to Mechanism in Organic Chemistry, 1982.
2. R. B. Grossmann, The Art of Writing Reasonable Organic Reaction Mechanism, 2nd Ed., 2003.
Course description:
Physical characterization of organic compounds: preliminary examination, melting point, boiling
point, specific gravity, index of refraction of liquids; separation of mixtures; classification of
organic compounds by solubility; preparation of derivatives; use of spectroscopic methods for
structure determination; use of the chemical literature.
Course rationale:
This course designed to make the students skilful in measuring physical characterization of
organic compounds: preliminary examination, melting point, boiling point, specific gravity,
index of refraction of liquids. The students will also able to perform qualitative analysis of
elements and use spectroscopic methods for structure determination.
Course outline:
Here the students will take unknown organic compound or unknown substance then they will
determine and characterize the unknown substance (organic) in the sample.
Course description
Functionalization and Interconversion of functional groups; Formation of Carbon -carbon bonds
and ring closure and ring opening reactions; Analysis of synthetic pathways; Principles of
asymmetric synthesis and the use of protective groups in synthesis; Illustrative examples of
multistep synthesis.
Course objectives:
At the end of the course the students will be able to or familiar with the following concepts:
• Detailed knowledge about the various functional groups and their inter conversions using
special reagents
• Familiar with the mechanisms and the reagents in the organic reaction involving the c-c
bond formation,
• Ring opening and the ring closure reactions
• Familiar with the asymmetric synthesis
• Conduct the multi step synthesis
Course outline:
1. Functionalization and interconversion of functional groups
1.1 Functionalization
Mode of delivery:
Lecture, Lecture- demonstration, Assignment, inquiry, Laboratory, Discussion methods and
questioning techniques.
Mode of assessment:
Assignments, presentation, mid exam, final exam and continuous assessment techniques of
various types will be used.
Course description:
Ideal and real gases, Zeroth’s Law of Thermodynamics; First Law of thermodynamics,
Thermochemistry, second Law of Thermodynamics, third law of thermodynamics, chemical
equilibrium, phase equilibrium, solutions.
Course rationale:
This course is very important for students of chemistry as it makes students have good
understanding of bulk properties of system (thermodynamics) and enable them describe chemical
and physical changes mathematically by computing the change in properties of the system during
the change and Predict criteria for any change to take place.
Course objective:
Upon completion of this course the students would be able to:
• describe the properties of gases
• Explain the laws of thermodynamics
• Apply the laws of thermodynamics
• understand the effect of solutes on solvent in solution system
Course outline:
1. Ideal and real gases
1.1. The equation of state
1.2. Ideal Gases and Ideal gas laws
1.3. Real Gase laws
2. Units and Mathematics
2.1 Basic SI units
2.2 Derived Units
2.3 Logarithms and Exponents
2.4 Differentials and Integrals
3. Thermodaynamics
3.1 Thermodynamic terms
3.1.1 System and surroundings
3.1.2 State of a system
3.1.3 Properties of a system
3.1.4 Thermodynamic equilibrium, Zeroth's law of thermodynamics
3.1.5 Thermodynamical process
3.1.6 State functions
3.1.7 Mathematical techniques interconnecting the state functions
3.1.8 Heat and work
3.2 First law of thermodynamics
Mode of delivery:
Lecture, Lecture- demonstration, Assignment, inquiry, Laboratory, Discussion methods and
questioning techniques.
Mode of assessment:
Assignments, presentation, mid exam, final exam and continuous assessment techniques of
various types will be used.
Reference materials:
1. P.W. Atkins, Physical Chemistry, Oxford University Press, Oxford-New York, 2002.
2. T.R. Forester, Introductory Physical Chemistry, Addis Ababa University, 1990.
3. G.M. Barrow, Physical chemistry, 5th Ed., TATA McGraw-Hill Edition, New Delhi,
1992.
4. K. K. Sharma, A textbook of Physical Chemistry, Vicas Publishing House, New Delhi,
1981.
5. R.A. Alberty and R.J. Silbey, Physical Chemistry, Wiley and Sons Inc., New York, 1997.
Course description:
Kinetic theory of gases, Chemical Kinetics, Electrolyte solutions, Electrochemical Cell,
interfacial electrochemistry, Transport phenomenon.
Course rationale:
This course is designed to enhance and extend students' ability to understand gaseous properties,
rate of chemical reactions and electrochemistry through leaning theoretical law and principles
and conducting laboratory experiments, making observations and analyzing results, designing
and analyzing products, and formulating and testing hypotheses based on evidence so that they
are ready for making environmental and chemical analysis.
Course objective:
Upon completion of this course the students would be able to:
• Explain electrochemistry
• Apply the concept of conductance for analysis
• Indicate the principle of electrolytic conduction
• Apply the concept of chemical kinetics to predict mechanism of reaction
Course outline:
1. Electrolytic Solutions
1.1. Introduction
1.2. Transport properties
1.3. Activity and activity Coefficients
1.4. Theory of electrolytic conductance
1.5. Ionic equilibria
1.6. Application of electrolytic cells
2. Electrochemical Cells
2.1. Introduction
2.2. Reversible electrodes
2.3. Thermodynamics of electrochemical cells
2.4. Determination of standard electrode potential
2.5. Classes of electrochemical cells
2.6. Liquid junction potential
2.7. Measurement of pH
2.8. Membrane potentials
2.9. Examples of electrochemical cells
3. Interfacial Electrochemistry
3.1. Potential differences across interfaces
3.2. The electrical double layer
3.3. Thermodynamics of electrified interface
3.4. Electrochemical kinetics
4. Kinetic Theory of Gases
4.1. Postulates of the kinetic theory of gases
4.2. Ideal gas laws
4.3. Barometric formula
4.4. Distribution of molecular velocities
4.5. Molecular collisions
4.6. Collisions with a surface or hole
4.7. Transport phenomena
5. Chemical kinetics
5.1. The rates of chemical reactions
5.2. Reaction rate laws
5.2.1. First order reaction
5.2.2. Second order reaction
5.2.3. Third order and zero order reactions
5.2.4. Reversible or opposing reactions
5.2.5. Consecutive or sequential reactions
5.2.6. Parallel or side reactions
5.2.7. Chain reactions
5.2.8. Acid-base catalysed reactions
5.2.9. Enzyme catalysed reactions
5.3. Analysis of kinetic results
5.4. Reaction rate theories
5.4.1. Collision theory
5.4.2. Transition state theory
Mode of delivery:
Lecture, Lecture-demonstration, assignment, inquiry, Laboratory, discussion methods and
questioning techniques.
Mode of assessment:
Assignments, presentation, mid exam, final exam and continuous assessment techniques of
various types will be used.
Reference materials:
1. P.W. Atkins, Physical Chemistry, Oxford University Press, Oxford-New York, 2002.
2. T.R. Forester, Introductory Physical Chemistry, Addis Ababa University, 1990.
3. G.M. Barrow, Physical chemistry, 5th Ed., TATA McGraw-Hill Edition, New Delhi,
1992.
4. K. K. Sharma, A textbook of Physical Chemistry, Vicas Publishing House, New Delhi,
1981.
5. R.A. Alberty and R.J. Silbey, Physical Chemistry, Wiley and Sons Inc., New York, 1997.
Course description:
Experimental foundation of Chemistry; The Schrödinger equation; Operators in quantum
mechanics; Solution of Schrodinger equation for some simple systems; Atomic structure;
Molecular structures; chemical bond; molecular spectroscopy.
Course rationale:
The academic standards for quantum Chemistry are designed to lead students to develop a
knowledge base of science at microscopic level and enable students understand the science of
modern spectroscopic method of analysis. It also enriches students with knowledge of
computing properties of compounds and compares it with the experimental results so that they
develop full confidence of their scientific results.
Course objective:
Upon completion of this course the students would be able to:
• Distinguish between classical and wave mechanics
• Apply quantum mechanics to simple systems
• Describe molecular and atomic structure
• Describe interaction of electromagnetic radiation and matter
Course outline:
1. Introduction
2. Experimental Foundation of Quantum Theory
2.1. Black Body Radiation
2.2. Photoelectric Effect
2.3. The Compton Effect
2.4. Line Spectra of Atoms
2.5. Rutherford Model of the Atom
2.6. Bohr Model of the Atom
2.7. The Wave Properties of Particles
Mode of delivery:
Lecture, Lecture-demonstration, assignment, inquiry, Laboratory, discussion methods and
questioning techniques.
Mode of assessment:
Assignments, presentation, mid exam, final exam and continuous assessment techniques of
various types will be used.
Reference materials:
1. D.A. McQuarrie and J.D. Simon, Physical Chemistry: A Molecular Approach, University
Science Books, Sausalito, California 1997.
2. P.W. Atkins, Molecular Quantum Mechanics, Oxford University Press, Oxford 1997.
3. A.K. Chandra Introductory Quantum Chemistry, Tata McGraw-Hill, 1979.
4. I.N. Levin, Quantum Chemistry, Ally Bacon Inc., 1974.
5. D.A. McQuarrie, Quantum Chemistry, University Science Books, 1983.
Course description:
Introduction to statistical thermodynamics, Terminology and basic concepts, Distribution
function, Surface chemistry: Interfacial structure, Surface tension and surface free energy,
Methods of surface tension measurement, Nature and thermodynamics of Liquid-Gas interface,
the surface tension of solution, the two dimensional ideal gas laws, adsorption at the solid
solution interface.
Course objective:
At the end of the course the students will be able to:
• Know the basic concepts in statistical thermodynamics;
• Understand the surface phenomena by applying their chemical knowledge;
• Explain about adsorption phenomena;
• Describe the solid solution interface
Course rationale:
This course is designed to enhance and extend students' ability to understand the properties of
individual components of a system to explain particulate property of a system, structure of solid
surface and its application and the interaction of similar and different phases and its real
application.
Course outline:
1. Statistical Thermodynamics
1.1 Introduction
1.2 Terminology and Basic Concepts
1.3 Basic Statistics
1.4 Statistics of Particles
1.5 Distribution Functions
1.6 Partition Function
1.7 Thermodynamic Functions
1.8 Statistical Mechanics of Ensembles
1.9 Thermodynamic Properties of Ideal Gas
1.10 Statistical Derivation of the Equation of State for Non-ideal Fluids
Mode of delivery:
Lecture, Lecture- demonstration, assignment, inquiry, Laboratory, discussion methods and
questioning techniques.
Mode of assessment:
Assignments, presentation, mid exam, final exam and continuous assessment techniques of
various types will be used.
Reference materials:
1. R.P. Rastogi and R.R. Misra, Introduction of Chemical Thermodynamics, Vikas
Publishing House, New Delhi, 1978.
2. D.A. McQuarrie, Statistical Thermodynamics, Harper & Row, 1976.
3. P.W. Atkins, Physical Chemistry, Oxford University Press, Oxford-New York, 2002.
4. G.M. Barrow, Physical chemistry, 5th Ed., TATA McGraw-Hill Edition, New Delhi,
1992.
5. K. K. Sharma, A textbook of Physical Chemistry, Vicas Publishing House, New Delhi,
1981.
6. R.A. Alberty and R.J. Silbey, Physical Chemistry, Wiley and Sons Inc., New York, 1997.
Course description:
Solubility, viscosity, phase rule, partition coefficient, adsorption, surface tension, transition
temperature and freezing point, kinetics of reaction Thermochemistry.
Course rationale:
This practical course is supposed to be given for students of chemistry to visualize the theoretical
physical courses students take. Most importantly this practical course enable students develop
skill of analysis and do independent work through prediction of various physical properties of
substances.
Course objective:
At the end of this course the student will able to:
• Determine physical properties of matter;
• Develop some techniques of determination of physical properties matter; and
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Harmonized Curriculum for B.Sc. degree in Chemistry
Course outline
Experiments pool to be selected include
1. Enthalpy of Solution: Determine the enthalpy of solution ∆sH of a salt (e.g. KNO3).
2. Differential Scanning Calorimetry: Determine the molar heat of vaporisation ∆vapHm of a
solute (e.g. Oxalic acid).
3. Boiling Point Diagram of Binary System: Draw a boiling point diagram of a binary
system at ambient pressure (e.g. Chloroform and Ethanol).
4. Partial Miscibility of a Binary System: Draw a phase diagram of a partially miscible
system; and to determine the critical temperature Tc (e.g. Phenol in Water).
5. Phase Equilibria: Determine the enthalpy of solution ∆sH of an organic acid (e.g. Benzoic
acid).
6. Elevation of Boiling Point: Determine the apparent molecular weight of a non volatile
solute M2 (e.g. NaCl).
7. Ionic Equilibrium: Draw the titration curve (pH vs. base) and to determine the buffer
capacity β of a polyprotonic acid (e.g. H3PO4).
8. Hydrolysis reaction of a Solute with concentrated and diluted base solution: Determine
the reaction orders v and rate constants k of the reactions (e.g. Crystal violet with NaOH).
9. Thermodynamics of an Electrochemical Cell: Determine the cell potential E; and the free
Gibbs energy ∆rG, enthalpy ∆rH and entropy ∆rS of reaction of an electrochemical cell
(e.g. Daniel Cell).
10. Conductance of Strong and Weak Electrolytes: Determine the molar conductance Λm of
strong and weak electrolytes, and dissociation constant of weak electrolytes (e.g. HCl and
CH3COOH)
Course description:
Kinetic of Reaction, Conductance, electrochemistry, Spectroscopy, Computational software.
Course rationale:
This practical course is designed to familiarize students with mechanisms of by which rate of
reaction is determined. It also enable students develop skill of analysis of compounds based on
the electrochemical and optical characteristics of substances. This practical course familiarizes
students with the research tool used by chemists.
Course objective:
At the end of this practical section, students will be able to:
• Determine rate of any chemical reaction
• Measure conductance of electrolyte in solution
• Analyze sample with different electrochemical methods
• Develop skill of using chemistry soft ware to predict some properties of compounds
theoretically.
Course outline:
Experiments pool to be selected include
1. Determination of equilibrium bond separation of HCl (gas) from vibrational-rotational
spectrum.
2. Comparison of absorption strength of allowed and forbidden transitions.
3. Derivation of Frank-Condon progression for benzene molecule (gas) from UV-Vis
measurement.
4. Effect of concentration and solvent polarity on UV-Vis absorption spectra of compounds.
5. Measurement of Fluorescence spectra of some selected compounds.
6. Determination of equilibrium separation and stabilisation energy of H2+ using variation
method.
7. Quantum mechanical prediction of dipole moment, heat content, Gibb`s free energy of
molecules.
8. Quantum mechanical prediction of NMR, IR-spectra of compounds.
Mode of delivery:
Purely practical
Mode of assessment:
Attendance, Laboratory Report, Practical exam, Final exam.
Reference materials:
1. P.W. Atkins, physical chemistry sixth edition, Oxford University press, New York, 2004.
2. R. J. Silbey and R. A. Alberty, Physical chemistry 3rd Ed., Massachusetts Institute of
Technology, 2001.
3. J.R. Lakowicz, Principle of fluorescence spectroscopy, 2nd Ed., University of Maryland
school of Medicine, 1999.
4. A. J. Bard and L. R. Faulkner, Department of Chemistry and Biochemistry, University of
Texas at Austin, 2000.
Course description:
Use of the chemical literature: handbooks, chemical encyclopaedia, spectral collections, journals,
abstracts and indexes, monographs; research methods; scientific writing.
Course rationale:
By taking this course the students will have the necessary knowledge in searching journals,
chemical encyclopaedia, abstracts, indexes, and monographs. Moreover they will develop the
necessary calibre in scientific writings and research paper writing.
Course objectives:
At the end of the course the students will be able to know about the
• The importance of research
• To conduct and present research
Course outline:
1. Use of chemical literature
2. Use of handbooks, chemical encyclopedia and spectral collection
3. Accessing journals, abstracts and indexes
4. Using monographs
5. Research methods
6. Scientific writing
7. Preparing scientific paper and presentation
8. Evaluating scientific papers
Mode of delivery:
Lecture, lecture-demonstration, assignment, inquiry, discussion and questioning techniques and
seminar by students.
Mode of assessment:
Assignments, presentation (seminar), mid exam, final exam and continuous assessment
techniques.
Reference materials:
To be designated at the commencement of the course.
Course description:
Processes and processes variables and Introduction to unit operations, material balance and
energy balance. Water in the chemical industry; basic inorganic industrial processing (acids,
alkalis, salts; gases, fertilizers, ceramics, glass, cement, metals, pigments).
Course outline:
1. General Introduction
1.1. Introduction to Industrial Processes and Process Variables
1.2. Introduction to Unit Operations
1.3. Introduction to Material Balance and Energy Balance
2. Water in the chemical industry
2.1. Sources of water
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Harmonized Curriculum for B.Sc. degree in Chemistry
Mode of delivery:
Lecture, group discussion, assignment in group or individually, home work,
Mode of assessment:
Quizzes, assignments, tests, mid-term and final examination
Reference materials:
1. P.C. Jain and M. Jain, Engineering Chemistry by; Dhanpatrai and sons, Eleventh Edition,
1996.
2. B.K. Sharma, Industrial Chemistry, Goel publishing house; 11th Ed., 2004.
3. K.H. Buchel, H.H Moretto and P. Woditsch, Industrial Inorganic Chemistry, 2nd Ed.,
WILEY-VCH, 2000.
Course description:
Basic organic industrial processes (coal petroleum, main petrochemicals, basic organic products,
plastics, rubber and fibers; sugar; oils and fats, detergents, paper; foodstuff, pharmaceuticals,
agrochemicals; dye stuff,; leather).
Course objectives:
To enrich the knowledge of the students in
• Processing of coal and petroleum into value added products.
• Industrial organic synthesis
• Manufacture and properties of plastics, rubber, fibers
• Chemistry of Oils, fats, Soaps, detergents, Pharmaceuticals, Dyestuffs and
Insecticides
• Sucrose, Paper, Leather and Food processing Industries.
Course outline:
1. Coal and Petroleum Processing
1.1. Origin of coal and its ranking
1.2. Carbonisation of coal
1.3. Gasification of coal
1.4. Hydrogenation of coal
1.5. Petroleum – origin, Classification and mining
1.6. Distillation of petroleum
1.7. Rating of Petrol and Diesel
Mode of delivery:
Lecture, group discussion, assignment in group or individually.
Mode of assessment:
Quizzes, assignments, tests, mid-term and final examination.
Reference materials:
1. P.C. Jain and M. Jain, Engineering Chemistry by; Dhanpatrai & sons, Eleventh Edition,
1996.
2. B.K. Sharma, Industrial Chemistry, Goel publishing house; Eleventh Edition, 2004.
3. J.N. Delgado and W.A. Remers, Text book of organic medicinal and pharmaceutical
chemistry
17.6.4 Biochemistry
COURSE TITLE: BIOCHEMISTRY
COURSE 6 UMBER: CHEM 452
C REDIT H OURS: 3
CO6TACT H OURS: 3 LEC. HR/WEEK
PREREQUISITE: CHEM 342
Course description:
Unique properties of Water as applied to Life, Structure and chemistry of biomolecules (proteins,
carbohydrates, lipids, nucleic acids, Minerals and Hormones); enzymology; intermediary
metabolism and generation and storage of metabolic energy; oxidative-reductive processes;
selected metabolic pathways of carbohydrates and fats; integration of metabolism, Structure and
chemistry of biomolecules (proteins, carbohydrates, lipids, nucleic acids); enzymology;
Hormones and their roles in metabolic regulations; intermediary metabolism and generation and
storage of metabolic energy; oxidative-reductive processes; selected metabolic pathways of
carbohydrates and fats; integration of metabolism.
Course rationale:
The course, Biochemistry is designed to make our students familiar with the different types of
biological molecules so that they will understand the applications of chemistry in life. Moreover,
the students will understand the different metabolic reactions and pathways in different kinds of
living things.
Course objective:
At the end of the course the students will be able to:
• Understand the structures and chemistry of biological molecules namely: proteins,
carbohydrates, lipids and nucleic acids;
• Know the different metabolic reactions that take place in our body;
• Describe enzymology and enzymatic reactions
Course outline
1. Introduction to biochemistry
1.1. Definition and scope of biochemistry
1.2. Chemical and biochemical reactions
1.3. Chemistry of organelles (hierarchical organization of organelles in living cells,
composition, properties, and function of organelles)
2. Water, pH, and buffer
2.1. Introduction
2.1.1. Unusual properties of water to be used as a biological solvent
2.1.2. Role of water in biological system
2.1.3. Intermolecular forces (forces responsible for interaction of
bimolecules with water and those responsible for the integration of
biomolecules)
2.1.4. Colligative properties
2.2. Hydronium ion and pH
2.3. Physiological Buffers and buffering agent
2.4. Buffers used by cells
2.5. Some common Buffers used in biochemical reactions
3. Protein Structure and Function
3.1 Structure and function of Amino Acids
3.1.1 Introduction to Amino acids (essential and non-essential amino acids)
3.1.2 Structure of Amino Acids
3.1.3 Amino Acids as Buffers
3.1.4 Peptide Bond Formation (Peptide linkage)
3.2 Structure and function of Proteins
3.2.1. Primary Structure of Proteins
3.2.2. Secondary Structure of Proteins
3.2.3. Tertiary Structure of Proteins
3.2.4. Quaternary Structure of Proteins
3.2.5. Denaturation of Proteins
3.2.6. Uses of proteins
4. Enzymes
4.1. Definition of Enzymes
4.2. Properties of Enzymes
4.3. Major Classes of Enzymes
4. 4. Enzyme Kinetics
4.5. Enzyme Mechanism (mechanism of catalysis)
Mode of delivery:
Lecture, group discussion, assignment in group or individually
Mode of assessment:
Quizzes, assignments, tests, mid-term and final examination.
Text: P.C. Champe; R.A. Harvey, Biochemistry, 4th Ed., Lippincott,s Illustrated Reviews, 2007.
Reference materials:
1. J.M. Berg, J.L. Tymoczko and L. Stryer, Biochemistry, 5th Ed., 2005: and Student’s
Companion to Stryer’s Book.
2. Voet and Voet, Biochemistry, 2nd Ed., 1990.
3. Zubay, Parson and Vance, Principles of Biochemistry, 1995.
Course description:
Major chemical cycles and effects of environmental pollution in these systems; basics of
atmospheric chemistry; aquatic chemistry; soil chemistry; pollution of air, water and soil;
chemical toxicology: toxicants and their metabolism; energy production and its impact on the
environment; analytical methods in environmental studies; Introduction to green chemistry.
Course rationale:
The course, Environmental Chemistry and toxicology, is designed to familiarize the students with
the known pollutants of the environment that will affect the aquatic environment, soil, air and the
like. So the students will have the necessary knowledge about the pollutants and will be
concerned about their effect and also teach the society about it. Moreover they will part of the
solution to minimize the problem and controlling it.
Course objective:
Upon completion of this course the students would be able to:
• Familiarize with the concept of Environmental Chemistry;
• Identify the common causes of environmental pollution;
• Describe about Aquatic Chemistry and water pollution;
• Explain about Atmospheric Chemistry and Air pollution;
• Familiarize with the concept of Green Chemistry;
• Study some toxic organic chemicals and their effects; and
• Device methods to decrease pollution.
Course outline:
1. Introduction to Environmental Chemistry
1.1. Basic concepts in Environmental chemistry
1.2. Properties of chemicals in the environment
1.3. Environnemental transformation and degradation
1.3.1. Abiotic transformation and degradation
1.3.2. Biotransformation and degradation
1.4. Matter and cycles of matter
2. Aquatic chemistry and Water pollution
2.1. Introduction to the Fundamentals of aquatic chemistry
2.2. The Properties of water, a unique substance
2.3. Water Quality
2.4. Water quality requirements
2.5. Nature and types of Water pollutants
3. Atmospheric chemistry and Air pollution
3.1. Importance and physical characteristics of the atmosphere
3.2. Atmospheric chemical reactions
3.3. Air quality
3.4. Nature and classification of air pollutants
3.4.1. Gaseous inorganic air pollutants
3.4.2. Organic air pollutants
3.4.3. Photochemical smog
3.4.4. Chlorofluro compounds and ozone layer depletion
3.4.5. Green House Gases and Global warming
4. Soil Chemistry
4.1. Soil and agriculture
4.2. Nature and composition of soil
4.3. Nutrients in soil
4.4. Reactions in soil
4.5. Wastes and pollutants in soil
5. Environmental Toxicity and toxicology
5.1. Introduction
5.2. Organic and inorganic pollutants
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Harmonized Curriculum for B.Sc. degree in Chemistry
Mode of delivery:
Lecture, field trip, individual study and group assignment.
Mode of assessment:
Field trip report; term paper mid and final exams.
Reference materials:
1. S. E. Manahan, Environmental Chemistry, 7th Ed., 1999.
2. M.-H. Yu, Environmental Toxicology, 2nd Ed., CRC Press, 2005.
3. R.N. Reeve, Environmental Analysis, 1994.
Course description:
Independent study of problems under the supervision of an advisor approved by the Department
Course rationale:
By taking this course the students will have the capability in doing research on their own
preference that will make them to be capable enough in their graduate study. They will have a
practical experience by their own in sample collection up to report submission.
Course outline:
Since it is an independent study or research there is no course outline for it.
Mode of delivery:
Presentation by individual student
Mode of assessment:
Seminar, project or presentation.
Reference materials:
Any nationally and internationally accredited journals or scientific findings.
Course description:
Review on the Electronic structure of the atom; an overview of the periodic table; structure and
bonding in molecules (Bonding Theories); ionic solids; metallic bonding; hydrogen and hydrides;
acid-base theories and the solvent system; Oxidation and reduction. Overview of descriptive
chemistry of the representative elements (Groups 1, 2 and 13-18) with reference to: electronic
structures, general properties, oxidation states, occurrences, extractions, reactivities, common
uses of the elements and their simple compounds; bonding and reactions of their hydrides,
oxides, hydroxides, oxyacids, halides; introduction to transition metal chemistry and coordination
compounds.
Course rationale:
This course will help learners to have a deep understanding of their area of specialization by
providing basic knowledge of structure of atoms and molecules, basic knowledge of all elements
and their compounds.
Course objective:
Upon completion of this course the students would be able to:
• discuss the current view of atomic structure;
• relate electronic configuration to the classification of elements in the periodic
table and their properties;
• explain the basic concepts of chemical bonding;
• have the general overview of the descriptive chemistry of hydrogen, main
group elements and organometallic compounds;
• describe acid-base concepts based on different theories; and
• have the general overview of the descriptive chemistry of transition metals,
inner transition elements and name coordination compounds.
Course outline:
1. Introduction
1.1. Atomic theory (DAT)
1.2. Law of chemical combination
1.2.1. Conservation of mass
1.2.2. Definite composition
1.2.3. Multiple proportion
2. Structure of ionic solids
2.1. Radius ratio rules
Mode of delivery:
Group Discussion, lecture, Lecture (Seminar) by students, Reading Assignment.
Mode of assessment:
Group discussions, monthly tests, Performance in Seminar and semester examination.
Reference materials:
1. J.D. Lee, A new concise inorganic chemistry, 3rd or 5th Ed.,
2. K.N. Upadhyaya, A text book of inorganic chemistry, 3rd Ed.,
3. A.G. Sharpe, Inorganic chemistry, 3rd Ed.,
4. J.E. Huheey, Inorganic chemistry principles of structure and reactivity,
5. G.I. Brown, Introduction to inorganic chemistry,
6. R. Kapoor, S.K. Vasisht and R.S. Chopra, Inorganic chemistry,
Course description:
Chemical bonding; inductive, steric and resonance effects; Functional groups in organic
chemistry; stereochemistry; classes of organic reactions: substitution, elimination, addition and
rearrangement reactions, Chemistry of Aromatic Compounds; Carbonyl Reactions; Introduction
to biological molecules.
Course rationale:
This course will make students who take the course about the basic things in organic chemistry
which are in touch with our day-to-day activities and us also. So the course makes the students to
be familiar with the various biological molecules, natural products, synthetic compounds,
polymers and their roles, functions, functional groups, chemical and physical properties so that
they will apply to their different fields like Pharmacy, Biology, Medicine, Clinical Chemistry,
Human Anatomy and the like.
Course objective:
Upon completion of this course the students would be able to:
discuss the chemical bonding theories and influence of bonding types on properties of
compounds
predict the existence of the kinds of stereoisomers, represent and designate their
structures
determine the stereochemistry of organic molecules
describe the factors affecting reaction rates and explain mechanisms in organic reactions
give systematic name to different organic compounds
review of the classes of organic compounds
explain the physical and chemical behaviors of organic compounds based on their
functional groups.
explain the properties, preparation and reactions of aromatic compounds
discuss different types of reactions of carbonyl compounds
describe different classes of Biological molecules
Course outline:
1. Structure
1.1. Energy levels and Atomic orbitals
1.2. Covalent bonds
1.3. Molecular orbital theory
1.4. Orbital hybridization
2. Nomenclature
2.1. Alkanes
2.2. Alkenes and Alkynes
2.3. Alcohols
2.4. Aldehydes
2.5. Ketones
2.6. Amines
2.7. Ethers
2.8. Esters
2.9. Amides
2.10. Aromatics
3. Stereochemistry
3.1. Symmetry and dissymmetry
3.2. The asymmetric carbon
3.3. Optical isomerism
3.4. Fischer projections
3.5. Multiple asymmetric centers
3.6. Configuration
4. Substitution reactions
4.1. SN1 and SN2 mechanisms
4.2. Applications of substitution Reactions
4.2.1. Alcohols
4.2.2. Ethers
4.2.3. Carboxylic acids
4.2.4. Alkanes, Alkenes, and Alkynes
4.2.5. Amines
4.2.6. Epoxide Ring opening
4.2.7. Reactions of malonic ester and acetoacetic ester
5. Elimination reactions
5.1. Mechanisms
5.2. Evisences for mechanisms of elimination reaction
5.3. E1 versus E2
5.4. Elimination versus substitution
5.5. Applications of elimination reactions
5.5.1. Dehydration of Alcohols
5.5.2. Dehydrohalogenation of alkylhalides
5.5.3. Vicinal Dihalides
5.5.4. Hofmann Elimination
5.5.5. Acetate pyrolysis
5.5.6. Cope reaction
6. Addition Reactions
6.1. Mechanism
6.2. Reactivity
6.3. Rules of addition reactions
Method of delivery:
Reading assignments taking their own notes; Group discussion; Lecture; Demonstration;
Seminar.
Mode of assessment:
Assignment, Term paper; Exams (mid, final, test); Class activities; Oral examinations.
Reference materials:
1. Menger, Goldsmith and Mandell, Organic Chemistry: A concise approach 2nd Ed.,
2. A.C. Knope and W.E. Watts, Organic reaction Mechanisms, University of Ulster,
Northern Ireland, 1993.
3. R.B. Low, Organic reaction Mechanisms, Columbia University, 2nd Ed.,
4. T.W.G. Solomons, Organic Chemistry, 6th Ed., University of South Florida.
5. K.S. Tewair, S.N. Mehrotra and N.K. Vishnoi, A textbook of Organic Chemistry.
Course description:
Kinetic molecular theory; Chemical Equilibrium; Phase equilibrium; Colligative properties; Non-
electrolytic Solutions; Electrolyte Solutions; First Law of Thermodynamics; Thermochemistry;
The Second Law of Thermodynamics; The third law of thermodynamics; Electrochemistry;
Chemical Kinetics; Basic Quantum Chemistry.
Course rationale:
It provides the basics of physical chemistry to non-chemistry major students. It helps the learners
to have a deep understanding on their area of specialization.
Course objective:
Upon completion of this course the students would be able to:
• describe the physical states of matter
• describe the principles of thermodynamics
• describe the colligative properties of solutions
• explain phase equilibrium on the basis thermodynamic equations
• Solve the mathematical problems of thermodynamics
• solve the mathematical problems of electrochemistry
• relate the ideal gas model and that of real gases
• explain the kinetic theory of gases
• distinguish between classical and wave mechanics
• apply quantum mechanics to simple systems
Course outline
1. Kinetic Theory of Gases
1.1. Kinetic molecular theory of gases
1.2. Derivation of kinetic gas equation
1.3. Distribution of molecular velocities
1.4. Different kinds of velocities
1.5. Calculation of molecular velocities
1.6. Molecular collisions
1.7. Collisions with a surface or hole
1.8. Collision properties
1.9. Specific heat ratios of gases
1.10. Ideal and real gases
1.10.1. Deviations from ideal behaviour
1.10.2. Explanation of deviations
1.11. Van der Waal's equation
1.11.1. Limitations of Van der Waal's equation
1.11.2. Law of corresponding states
2. Chemical Equilibrium
2.1. The law of mass action and its applications
Mode of delivery:
Lecture, Historical, Lecture demonstration, Assignment, Discussion, inquiry, project methods
and questioning technique
Mode of assessment:
Assignments; Class room tests; Quiz; Standardized final exam
Reference materials:
1. P.W. Atkins, Physical Chemistry, Oxford University Press, Oxford-New York,
2002.
2. T.R. Forester, Introductory Physical Chemistry, Addis Ababa University, 1990.
3. G.M. Barrow, Physical chemistry, 5th Ed., TATA McGraw-Hill Edition, New
Delhi, 1992.
Course description:
Introduction to the subject matter; Ionic equilibria; statistical evaluation of analytical data;
Solutions; titrimetric methods of analysis; gravimetric analysis: chromatography;
instrumentation: electrophoresis; electroanalytical methods: thermometric methods.
Spectroscopic techniques
Course rationale:
The course is designed to make the students develop competencies of chemical analysis,
instrumental methods of analysis.
Course outline
1. Introduction
1.1 What is analytical chemistry?
1.2 Roles of analytical chemistry
1.3 Classification of Analytical Chemistry
1.4 Methods of chemical analysis
1.5 Steps in quantitative chemical analysis
2. Ionic equilibria
2.1 Acid-base equilibria
2.1.1 Theories of acids and bases
2.1.2 Dissociation of strong monoprotic acids and bases
2.1.3 Dissociation of weak monoprotic acids and bases
2.1.4 Dissociation of water and pH of aqueous solutions
2.1.5 Common ion effect
2.1.6 Buffer solutions
2.1.7 Hydrolysis of salts
2.2 Solubility product principle
2.2.1 Solubility, solubility equilibria and solubility product
2.2.2 Common ion effect and salt effect on solubility
2.2.3 Effect of acidity on solubility
2.3 Complexation equilibria
2.3.1 Complex ion and ligands
2.3.2 Complex formation equilibria with unidentate and multidentate ligands
Mode of delivery:
Lecture, Lecture demonstration, Assignment, Discussion, inquiry, project methods and
questioning technique
Mode of assessment:
Assignments; Class room tests; Quiz; Standardized final exam
Reference materials:
1. Skoog, D.A.; West, D.M.; Holler, F.J. Fundamentals of Analytical Chemistry, 7th ed.;
Saunders College Publishing, New York, 1996.
2. Christian, G.D. Analytical Chemistry, 5th ed., John Wiley and Sons, Inc., New York,
1994.
3. Harris, D.C. Quantitative Chemical Analysis, 4th ed., W.H. Freeman and Company,
New York, 1995.
4. Jeffery, G.H.; Bassett, J.; Mandham, J.; Denney, R.C. Vogel’s Text Book of
Quantitative Chemical Analysis, John Wiley and Sons, Inc., New York 1991.
5. Manahan, S.E. Quantitative chemical analysis, Brooks/Cole publishing company,
California, 1986.
6. Fifield, F.W., Keale, D. Principles and practice of analytical chemistry, 3rd ed., Blakie
academic and professional, Glasgow, 1990.
7. Marmet, J.M.; Otto, M.; Widmer, H.M. (editors). Analytical chemistry, Wiley-VCH,
Weinheim,1998
Course description:
Electronic and optical aspects of chemical instrumentation: measurement and instrumentation,
basic and digital electronics, input transducers and data acquisition, signal noise optimization,
computers in instrumentation, process instruments and automatic analysis, basics of optical
Course objectives:
upon the completion of this course students would be able to
• Distinguish the components of spectroscopy instruments and types of instruments
• Identify the use of each component in the instruments
• State the conversion of digital to analogue and vice versa
• Explain how the transistors work as amplifiers
• State how operational amplifier amplifies the signal and optimization of the signal
Course outline
1. Signal and Noise
1.1. Signal
1.1.1 The general concept
1.1.2 Modulations
1.1.3 Amplification and Attenuation
1.2 Noise
1.2.1 Signal to noise
1.2.2 Noise power
1.2.3 Source of noise
1.2.4 Signal to noise enhancement
2. Measurements and Instrumentation
2.1 Two terminal circuit elements and circuit analysis- Fundamental Laws of electricity
2.2 Simple DC circuits
2.2.1.1 Series resistive circuits : Voltage division , Loading
2.2.1.2 Parallel resistive circuits
2.2.1.3 DC Current resistance and voltage measurement
2.3 AC circuit Analysis
2.3.1 Reactive Components
Series RC circuits with DC sources
Rate of Current and Voltage Change
Phase relations between voltage and current
Series RC circuits with AC Sources: Reactance, Impendence
RC filter circuits
2.4 Semi conductors
2.41. Diodes
The pn junction diode
Mode of delivery:
Lecture, Lecture demonstration, Assignment, Discussion, inquiry, project methods and
questioning technique
Mode of assessment:
Assignments; Class room tests; Quiz; Standardized final exam
Course description:
The course will focus on understanding of radiant energy and the type of analytical instruments
and equipments used in clinical chemistry laboratory, specimen collection, handling, processing
and analysis of specimens for analytes that help in the diagnosis of diseases, and basic quality
assurance in clinical chemistry. The laboratory practical sessions will include instrument set up
and calibration, specimen collection, handling processing and analysis as well as calculation and
interpretation of test results.
Course objectives:
Up on completion of the course, students will be able to:
• State properties of solutes, solvents and solutions,
• Describe standard solutions, buffer solutions and their mode of action,
• Discuss pH concept and convert one unit format to another
• Describe the electro magnetic spectrum and state radiant sources for absorption
measurement
• Explain the interaction of radiant energy with matter and discuss fundamental laws of
absorption.
• Describe the basic components of spectrophotometer, colorimeter, flame photometer,
atomic absorption spectrophotometer,
• Select proper wave length for a given analyte and calibrate instruments
Course outline
1. Introduction to Clinical Chemistry tests
1.1. Solutions
1.2. Standard Solutions
1.3. Concepts of pH
1.4. Buffer solutions and their mode of action
1.5. Conversion of units of measure
2. Introduction to Radiant Energy
2.1. The Electro magnetic Spectrum
2.2. Radiant sources for absorption measurement
2.3. Interaction of Radiant Energy with matter
2.4. Absorption measurement
2.5. Fundamental Laws of Absorption
3. Analytical Procedures and Instrumentation
3.1. Introduction
3.2. Principles, Concepts, Fundamentals of the spectrophotometer, Colorimeter and flame
Photometer
3.3. Selection of proper wave lengths
3.4. General guide lines on calibration and the use of calibration curves
3.5. Basic introduction to Electrophoresis, Refractometry, Fluorometry, Turbidimetry and
Nephelometry
4. Specimen Collection, Handling, and Processing for Biochemical Analysis
4.1. Specimen Collection and Processing
4.2. Use of Preservatives and Anticoagulants in Biological Fluids
4.3. Factors Affecting Test Results
4.4. Preparation of Protein Free Filtrate (PFF)
5. Carbohydrates
5.1. Carbohydrate Chemistry
5.2. Metabolism of Carbohydrates
5.3. Diabetes Mellitus
5.4. Hypoglycemia
5.5. Measurement of Glucose in Body Fluids
5.6. Glucose Tolerance Test (GTT)
5.7. Kenton Bodies
5.8. Lactate and Pyruvate
Harmonized Curriculum for B.Sc. degree in Chemistry 89 | P a g e
Harmonized Curriculum for B.Sc. degree in Chemistry
Mode of delivery:
Lecture, Lecture demonstration, Assignment, Discussion, inquiry, project methods and
questioning technique, laboratory practicals
Mode of assessment:
Assignments; Class room tests; Quiz; Standardized final exam
Course description:
Pharmacologically active plant constituents: Introduction, history and general properties to the
main classes of plant constituents (alkaloids, flavonoids, phenols, glycosides, saponins,
terpenoids, and essential oils); The chemical interaction of drug molecules with biological
systems (enzymes, receptors, membranes and DNA); Physiological Effects of major classes of
pharmaceutical agents including central nervous system depressant and stimulants, analgesics,
anesthetics, cardiovascular agents and oral contraceptives; Quantitative structure-activity
relationships; Mechanisms of drug metabolism.
Course description:
Introduction to polymers; polymer synthesis (Non vinyl based polymerization, vinyl based
polymerization, ring opening polymerization, inorganic polymers, biological polymers); polymer
structure and properties (polymer solution, polymer in the bulk state, mechanical properties,
polymer flammability); Polymer Characterization; experimental determination of the sizes and
shapes of macromolecules.
Course objectives:
To impart knowledge in
• Synthesis of polymers and their reactions
• Mechanistic aspects of polymerisation
• Characterization, fabrication and testing of polymers
• Relationship between structure of polymers with their properties
• Different ways of Polymer degradation in the environment
• Polymers found in living organisms and their reactions.
Course outline:
1. Synthesis of Polymers
1.1. Types of polymerization
1.2. Condensation Polymerization
1.3. Addition Polymerization
1.3.1. Free radical polymerization
1.3.2. Ionic Polymerization
1.3.3. Coordination Polymerization
1.3.4. Ring opening polymerization
2. Reactions of Polymers
2.1. Reactions involving the main chain
2.2. Reactions involving the side group-Graft polymerisation
2.3. Surface reactions of polymers
3. Thermodynamics and kinetics of Polymerisation
3.1. Thermodynamics of polymerisation
3.2. Kinetics of step-growth polymerisation
3.3. Kinetics of free radical polymerization
Reference materials:
1. R. Harry, R.A. Frederic and W. Lampe, Contemporary polymer chemistry
2. J.R. Fried, Polymer Science and Technology, Pearson Education, Inc., 2nd Ed., 2004.
Course description:
Introduction: Basic constituents common to food products (Proteins, carbohydrates, fats, water,
lipids and micro nutrients such as minerals, vitamins); Properties of food (Color, flavor, taste,
etc); Influence and role of constituents of food on the quality of food; Methods of improving
quality of foods (preservatives and additives, processing, cooking, browning, storage, packing
etc); Toxicity of Foods: Natural toxins in food, chemical additives, methods of detoxification;
possible changes in nutritional values; regulatory control of food composition, quality and safety.
Course description:
Soil Chemistry: Soil composition, formation and reaction, colloidal chemistry of soil constituents
and solutions. Agro Chemicals: Pesticides and their mode of action (insecticides, fungicides and
herbicides): some novel methods of insect control pesticides in the environment and fertilizers.
Food Chemistry: Alcoholic fermentation, stimulant, flavors, spices, additive food coloring and
contaminates, chemistry of vitamins, fruits and vegetables, quality control in food services.
Course objectives:
To impart knowledge in
• Chemistry of soil formation, reaction and composition that supports the plant growth.
• Agrochemicals like pesticides and fertilizers for better plant growth
Course outline
1. Soil formation
1.1. Introduction
1.2. Physical weathering
1.3. Chemical weathering
1.4. Biological weathering
1.5. Humus formation
2. Soil Composition
2.1. Soil horizon or layers
2.2. Composition of soil
2.3. Properties of soil
3. Reactions in soils
3.1. Redox reactions
3.2. Acid–Base reactions
3.3. Ion-Exchange reactions
Reference materials:
1. P. Meenakshi, Elements of Environmental science and engineering, 2005.
2. A.K. De, Environmental Chemistry, 5th Ed., 2005.
Course description:
Chemistry of Solids (Nature, Structure and properties of solids and surface chemistry); Nuclear
Chemistry; Introduction to Group Theory (Symmetry elements, operations, and point groups,
Mathematical representation of symmetry operations, Characters and character tables); Chemical
Application of Group Theory (Vibrational spectroscopy, Electronic spectroscopy, Molecular
orbital theory)
Course objectives:
The course provides knowledge of solid state chemistry, nuclear chemistry and spectroscopy. It
offers additional information and directs the students for future specialization, especially in
research.
Course outline
1. Chemistry of Solids
1.1 Crystalline and Amorphous solids
1.1.1 Size and shape of Crystals
1.1.2 Space lattice, unit cell, Bravice lattices, seven basic crystal systems
1.2 Symmetry in Crystals
1.3 Radius ratio rules and their calculations for 3, 4 and 6 coordination
1.4 Packing of Spheres in Hexagonal, cubic close packing etc
1.5 Structure of metallic crystals
Reference materials:
1. J.D. Lee, Concise Inorganic Chemistry
2. C.E. Housecroft and A.G. Sharpe, Inorganic Chemistry
3. Puri and Sharma, Inorganic Chemistry
4. J. E. Huheey, Inorganic Chemistry
5. F.A. Cotton , Chemical application of group theory
Course description:
Quality and safety; industrial quality control of processes and products, quality requirements;
laboratory management, statistical quality control; international product and process standards;
industrial safety and loss prevention; environmental management systems; case studies of
selected industries.
Course outline
1. Processes and Process variables
1.1. Introduction
1.2. Units and Dimensions
1.3. Systems of units and conversion of units
1.4. Process variables: Mass and volume, Flow rate, Concentration, Pressure and
Temperature.
2. Safety in Chemical Processing Industries
2.1. Concern for chemical safety
2.2. Chemical plant safety
2.3. Hazards in Storage, handling and use of chemicals
2.4. Hazards and their control in important industries
3. Sewage and Waste Treatment
3.1. Sewage characteristics
3.2. Sewage treatment
3.3. Primary treatment
3.4. Secondary treatment
3.5. Tertiary treatment
3.6. Sludge disposal
4. Waste Minimisation and Pollution Prevention
4.1. Hierarchy of environmental management
4.2. Pollution prevention methodology
4.3. Pollution prevention techniques
4.4. Waste minimisation
4.5. Life cycle assessment
4.6. Sustainable manufacturing
4.7. Cleaner processes
5. Legal Control of Pollution
5.1. Responsibilities of Government agencies
5.2. Environmental laws and regulations
5.3. Environmental impact assessment
5.4. Polluters pay principle
5.5. International conventions and protocols on environment
6. Control of Industrial Pollution
6.1. Air pollution control
6.2. Water pollution control
6.3. Solid waste disposal
6.4. Noise pollution control
7. Industrial Waste Water and Hazardous Material Treatment Technology
7.1. Waste water treatment in
7.1.1. Sugar Industry and distillery
7.1.2. Tanneries
7.1.3. Textile and dyeing industries
7.1.4. Pesticides and Fertiliser industries
7.2. Definition, sources, transportation, minimization, treatment and disposal of hazardous
waste
7.3. Radioactive waste disposal
Mode of delivery:
Lecture, group discussion, assignment in group or individually.
Mode of assessment:
Quizzes, assignments, tests, and final examination.
Reference materials:
1. D.H.F. Liu and B.G. Liptak, Environmental Engineer’s Handbook, 2nd Ed., Lewis
Publishers,
2. S.C. Bhatia, Environmental Pollution and Control in Chemical Process Industries;
Khanna Publishers,
3. G.N. Pandey and G.C. Carney, Environmental Engineering, Tata McGraw-Hill.
Course description:
Overview of Biochemistry (molecular basis of life, structure-function correlation of biomolecules
such as protein structure and function with emphasis on non-covalent bonds; significance of
Biochemistry to other "molecular-scale" biological sciences such as molecular biology,
molecular genetics and immunology; Cells and Viruses: Overview; Nucleic Acids: DNA
Replication, Mutation and Repair, Genomes and Proteomics, Gene Transcription,
Posttranscriptional Processes and translation; Techniques of molecular biology: Expression
cloning, Polymerase chain reaction (PCR), Gel electrophoresis, Macromolecule blotting and
probing (Southern blotting, Northern blotting, Western blotting); Introduction to Biotechnology
and Bioinformatics.
Course description:
Revision on functions, Limits and Continuity; Derivatives; Application of the derivative;
Function; Inverse of a function and its derivative, inverse trigonometric, hyperbolic functions and
their derivatives; L’Hopital’s rule; Integration; Techniques of integration (by parts, substitution,
partial fraction, trigonometric integrals, trigonometric substitution); application of integration
(Volume, arc length, surface area); improper integrals.
Course objective:
At the end the course the students will be able to: Investigate properties of Functions; Understand
the concept of both limits and continuity intuitively and formally; Define the derivative of
elementary functions; Differentiate and integrate different types of functions; Apply
differentiation to find extreme values and solve optimization problem; Find area of some regions
using integrals; Sketch graphs of functions
Course outline:
1. Revisions Functions and Their Graphs (4 Hrs)
1.1. Definition of Functions
1.2. Examples of Functions
1.3. Graphs of Functions
2. Limits and Continuity (16 Hrs)
2.1. Formal Definition of Limit
2.2. Basic Limit Theorems
2.3. One-Sided Limits
2.4. Infinite Limits
2.5. Limits at Infinity
2.6. Formal Definition of Continuity
2.7. One-Sided Continuity
2.8. The Intermediate Value Theorem for Continuous Function and Its Applications
3. Derivatives (14 Hrs)
3.1. Definition of Derivatives
3.2. Geometric Interpretation of Derivative as a Slope
3.3. Differentiable Functions
3.4. Derivative of Combination of Functions
3.5. The Chain Rule
3.6. Application of Chain Rule; Related Rates and Implicit Differentiation
3.7. Higher Order Derivatives
3.8. Implicit Differentiation
4. Application of Derivatives (16 Hrs)
4.1. Extreme Values Of Functions
4.2. The Mean Value Theorem And Its Application
4.3. Monotonic Functions
4.4. The First Derivative And Second Derivative Tests
4.5. Concavity and Inflection Points
4.6. Curve Sketching
4.7. Tangent Line Approximation
4.8. Indeterminant Form and L’Hopitals Rule
4.9. Tangent Line Approximations
5. Integrals (14 Hrs)
5.1. Anti-Derivatives
5.2. Partitions; Lower Sum, Upper Sum, Riemann Sum
5.3. Definition of Definite Integral
5.4. Basic Properties Of Definite Integral
5.5. Techniques of Integration; By Substitution, By Part, By Partial Fraction
5.6. The Fundamental Theorems Of Calculus
5.7. Indefinite Integrals And Their Properties
5.8. Application Of Integration To Find Area Of A Plane Region and Volume Of Solid
Figure
5.9. Application of Integration to the concept of work
Course description:
Real Sequences; Real Series; Power and Tailor Series; Differential calculus; of functions of
several variables; multiple integrals; ordinary differential equations and Laplace transforms.
Course objective
• At the end of the course the students will be able to Extend the integral calculus concepts
of one variable in to several variables
• Determine the limit of functions of several variables if exist
• Check whether a function of several variables is continuous at a point and then in tits
domain or not
• Find partial derivatives of a function of several variables
• Apply the concept of partial derivative to find relative extreme and to solve some verbal
problems
• Evaluate multiple integrals
• Find surface area and volume of solid figures by use of double integral and triple integral.
• Relate the concept of calculus to vector notion
Course outline:
1. Real Sequences
1.1 Definition and examples
1.2 Convergence properties
1.3 Bounded and Monotonic sequence
1.4 Subsequences
2. Real Series
2.1 Definition of infinite series
2.2 Convergence and divergence, properties of convergent series
2.3 Nonnegative terms series
2.4 Tests of convergence: Integral, comparison, ration and root tests
2.5 Alternating series and test
2.6 Absolute and conditional convergence
2.7 Generalized convergence tests
3. Power Series
3.1 Definition of power series as any x0 and x0 = 0
3.2 Convergence and divergence, radius and interval of convergence
3.3 Algebraic operations between convergent power series
3.4 Different-ion and integration
3.5 Taylor series; Applications
3.6 Fourier series; Applicatios
4. Differential Calculus of Functions of Several Variables
4.1 Notations, examples, level curves and graphs
4.2 Limits and continuity
4.3 Partial derivatives; tangent lines, higher order partial derivatives
Course description:
Basic concepts, methods of data collection and presentation, frequency distribution and graphical
presentation; measures of central tendency, dispersion and shape; Elementary probability,
probability distribution; Binomial, Poisson, normal t-distribution ,chi-square; sampling and
sampling distribution means ,proportions and variance; statistics inference ,concepts of parameter
and statistics ,estimation (point and interval) and hypothesis testing for one mean, one proportion
and variance ,chi-square tests of association.
Course objectives:
This course is intended to accomplish the following:
• Provide students with an understanding and appreciation of statistics as a problem-solving
tool.
• Presenting the methods of data gathering.
• Teaching students to present data using the tools of descriptive statistics.
• Teaching the basics of probability that underlie statistical theory.
• Analyze cases in which discrete and continuous probability distributions apply.
• Apply probability distributions to random variables in order to solve applications
involving statistics.
• Discussing methods of estimation and hypothesis testing
• Teaching the method to study the relationship between two variables
Course outline:
1. Introduction
1.1. Definitions of statistics
1.1.1. Statistics and data
1.1.2. Statistics as a method
1.2. Some basic terminologies in statistics: Data, population, sample, parameter, Sample
statistic, etc.
1.3. Types of Statistical method
1.3.1. Descriptive statistics
1.3.2. Inferential statistics
1.4. Uses of statistics
1.5. Types of statistical data
1.5.1. Depending on type of variable
1.5.1.1.Qualitative Data (categorical data)
1.5.1.2.Quantitative data
1.5.2. Depending on time reference
1.5.2.1.Time series data
1.5.2.2.Cross-sectional data
1.5.3. Depending on scales of measurement: Normal, Ordinal, Interval and Ratio data
1.5.4. Based on source of data: Primary and secondary data
1.6. Scope of coverage of data collection: Census and sample survey
2. Classification and presentation of data
2.1. Classification of data Classification
2.1.1. Definition of Classification
2.1.2. Types of classification
2.1.2.1.Geographical or spatial
2.1.2.2.Chronological
2.1.2.3.Qualitative
2.1.2.4.Quantitative
2.2. Presentation of data
2.2.1. Frequency Distribution
2.2.1.1.Definition
2.2.1.2.Types of frequency distribution
2.2.1.3.Ungrouped (discrete) frequency distribution
2.2.1.4.Grouped (Continues) frequency distribution
2.2.1.5.Rules of constructing grouped frequency distribution
2.2.1.6.Relative frequency distribution
Harmonized Curriculum for B.Sc. degree in Chemistry 101 | P a g e
Harmonized Curriculum for B.Sc. degree in Chemistry
Mode of assessment:
Tests, Group assignment, Mid-semester Exam., Final exam.
Reference materials:
1. Miller and Freund, Probability and statistics for Engineers.
2. S.P. Gupta, Business Statistics.
3. V.K. Kapoor, Statistics problems and solutions.
4. W. Mendenhall, Introduction to probability and statistics.
5. S.P. Gupta, Introduction to Statistical methods.
6. J.L. Devore, Probability and statistics for engineers and the science, 3rd Ed.
7. R.E. Walpole, Probability and statistics for engineers and the scientists.
Course description
Vector algebra, Particle Kinematics and Dynamics, Work and Energy, Conservative forces and
Potential Energy Dynamics of Systems of Particles, Collision, Rotational Kinematics, Dynamics
and Static of a Rigid Body, Oscillations, Gravitation and Planetary Motion, Fluid Mechanics,
Heat
Course rationale:
At the end of this course students are expected to be acquainted with basic concepts in
mechanics, identify the connection between them and explain the common phenomena. They will
also develop skills of solving problems.
.
Course objectives:
Upon completion of this course students should be able to:
• compute average and instantaneous values of velocity, speed and acceleration
• derive the kinematic equations for uniformly accelerated one-dimensional motion
• solve problems involving bodies moving in one-dimensional and two-dimensional
motion
• using the concepts in calculus and trigonometry
• explain some implications of Newton’s laws of motion
• derive the work-energy theorem
• solve mechanics problem using impulse, momentum and the conservation of linear
momentum
• apply the law of conservation of linear momentum to collisions
• repeat the procedures followed in rectilinear motion for rotational motion
• explain basic laws of heat and thermodynamics
Course outline:
1. Vectors (2 hr)
1.1. Vector algebra
1.2. Geometrical & algebraic representation of vectors
1.3. Vector calculus
1.4. National Physics BSc Curriculum (Draft) Mechanics and Heat (Phys 205)
2. One and Two Dimensional Motions (6 hrs)
2.1. Average and instantaneous Velocity
2.2. Average and instantaneous Acceleration
2.3. Motion with Constant Acceleration
2.4. Projectile Motion
2.5. Uniform Circular Motion
3. Particle Dynamics (6 hrs)
3.1. Newton’s Laws of Motion
Method of delivery:
Presentation of the course is through lecture, a related guided problems section with demonstrator
assistance and additional assessed coursework, Online learning resources.
Mode of assessment:
• Homework will consist of selected end of chapter problems: 15%
• In-class participation (asking questions, discussing homework, answering questions): 5%
Text: R. A. Serway, Physics for Scientists & Engineers, 6th Ed., 2004.
Reference materials:
1. D. C. Giancoli, Physics for Scientists and Engineers, 4th Ed., 2005.
2. H.D. Young and R.A. Friedman, University Physics with Modern Physics, 12th Ed., 2008.
Course description
The topics to be included are Coulomb’s Law, Electric Field, Gauss’ Law, Electric Potential,
Electric Potential Energy, Capacitors and Dielectric, Electric Circuits, Magnetic Field, Bio-
Savart’s Law, Ampere’s Law, Electromagnetic Induction, Inductance, Circuits with Time
Dependent Currents, Maxwell’s Equations, ElectromagneticWave.
Course rationale
This course is designed to introduce concepts of classical electrodynamics with the aid of
calculus. It also emphasizes on establishing a strong foundation of the relation between electric
and magnetic phenomena; a concept that turns out to be a fundamental basis for many
technological advances.
Course objectives:
Upon completion of this course students should be able to:
• explain the basic concepts of electric charge, electric field and electric potential
• apply vector algebra and calculus in solving different problems in electricity and
magnetism
• analyze direct and alternating current circuits containing different electric elements and
• solve circuit problems
• describe properties of capacitors and dielectrics
• describe the magnetic field and solve problems related to the magnetic field and magnetic
• forces
• discuss about electromagnetic induction
• state Maxwell’s equation in free space
• describe some applications of Maxwell’s equations
• describe electromagnetic radiation in medium and free space.
Course Outline
1. Electric Field (4 hr.)
1.1. Properties of electric charges
1.2. Coulomb’s law
1.3. Electric field due to point charge
Mode of delivery:
Discussions, problem-solving and lecture methods are dominantly used through out the course.
Students are expected and encouraged to set, solve and present problems relevant to the lessons.
Mode of Assessment:
• Homework will consist of selected end of chapter problems: 15%
• In-class participation (asking questions, discussing homework, answering questions): 5%
• Two Tests (40%)
• Mid-semester and Semester final tests (40%)
Text: R. A. Serway, Physics for Scientists & Engineers, 6th Ed., 2004.
Reference materials:
1. D. C. Giancoli, Physics for Scientists and Engineers, 4th Ed., 2005.
2. H.D. Young and R.A. Friedman, University Physics with Modern Physics, 12th Ed., 2008.
Course description:
This course covers vectors, lines and planes; vector spaces; matrices; system of linear equations;
determinant; eigenvalues and eigenvectors; linear transformations.
Course objective:
The main objective of this course is to lay down a foundation for advanced studies in linear
algebra and related courses. At the end of successful completion of the course the students will
be able to:
Course outline:
1. Vectors
1.1. Definition of points in n-space
1.2. Vectors in n-space; Geometric interpretation in 2-and3-spaces
1.3. Scalar product and the norm of a vector, orthogonal projection, direction cosines
1.4. The vector product
1.5. Applications to area and volume
1.6. Lines and planes
2. Vector Spaces
2.1. The axioms of a vector space
2.2. Examples of different models of a vector space
2.3. Subspaces, Linear combinations and generators
2.4. Linear dependence and independence of vectors
2.5. Bases and dimension of a vector space
2.6. Direct sum and direct product of subspaces
3. Matrices
3.1. Definition of matrices
3.2. Operations of matrices
3.3. Types of matrices: square, identity, Scalar, diagonal, triangular, symmetric and skew
symmetric matrices
3.4. Elementary row and column operations
3.5. Row reduced echelon form of a matrix
3.6. Rank of a matrix
3.7. System of linear equations
4. Determinants
4.1. Definition of determinants
4.2. Properties of determinates and uniqueness
4.3. Adjoint and Inverse of a matrix
4.4. Creamer’s rule for solving system of linear equations
4.5. Determinant of transpose and product of matrices
4.6. The rank of matrix and subdeterminants
4.7. Determinant and volume
4.8. Eigenvalues and eigenvectors of a matrix
4.9. Diagonalization of a symmetric matrix
5. Linear Transformations
5.1. Linear transformations and examples
5.2. The rank and nullity of linear transformations
Mode of delivery:
Three lecture hours and two hours of tutorial per week. Home do assignments will be given for
each chapter covered.
Mode of assessment:
• Assignment/quizzes/ 20%
• Mid term exam 30%
• Final Exam 50%
Course description:
An overview of computers; Development of Computers; Input Devices; Output Devices; Central
Processing Unit; System Software; Application Software; Introductory concepts of Computer
Networks and the Internet; Microsoft Windows; Microsoft office.
Course objective:
This course is intended to give chemistry students the basic introduction to computers and uses of
computers. Specifically the students should be able to:
• Prepare and edit texts
• Make presentations
• Use MS excel, access etc
• Use chemical structure drawing software such as Chemdraw, Chemwindow etc
17.10.1 Entrepreneurship
COURSE TITLE: E6TREPRE6EURSHIP
COURSE CODE: MGMT 201
C REDIT HOURS: 3
CO6TACT HOURS: 3 LEC. HR/ WEEK
Course description:
Introduction; Effective organization, development, creation, and management personal
businesses; communication and interpersonal skills; economics; professional development
foundations; marketing: distribution, financing, marketing/information management, pricing,
product/service management, promotion, and selling; assessment of personal skills, the
components of the free enterprise system and it’s place in our global economy, human relation
and interpersonal skills, the importance of business ethics, and the role of quality and service
play in business.
Course description:
Course description:
Course description: