New Chemistry Curriculum

August, 2009

Addis Ababa

Ethiopia

HARMONIZED CURRICULUM

FOR B.Sc. DEGREE PROGRAM

IN CHEMISTRY

ETHIOPIA

Harmonization Team members:

Hailemichael Tesso, PhD, Assistant Professor, Adama University;

Tetemke Mehari, PhD, Associate Professor, Addis Ababa University;

Mesfin Redi, PhD, Assistant Professor, Addis Ababa University;

Fikre Mammo, PhD, Assistant Professor, Hawassa University ;

Ayalew Temesgen, PhD, Assistant Professor, Gondar University.

Harmonized Curriculum for B.Sc. degree in Chemistry

Harmonized Curriculum for B.Sc. degree in Chemistry 2 | P a g e

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



17.1.1 University chemistry ...............................................................................................14

17.1.2 University Practical Chemistry ...............................................................................17

17.2 Analytical chemistry section ..........................................................................................19

17.2.1 Analytical Chemistry...............................................................................................19

17.2.2 Practical Analytical Chemistry................................................................................21

17.2.3 Instrumental Analysis I ...........................................................................................23

17.2.4 Practical Instrumental analysis I .............................................................................25

17.2.5 Instrumental Analysis II ..........................................................................................27

17.2.6. Practical Instrumental analysis II ...........................................................................29

17.2.7. Analysis of Real Samples .......................................................................................30

17.3 Inorganic chemistry section ...........................................................................................31

17.3.1. Inorganic Chemistry I.............................................................................................31

17.3.2. Inorganic Chemistry II ...........................................................................................33

17.3.3 Practical Inorganic Chemistry I...............................................................................34

17.3.4. Inorganic Chemistry III ..........................................................................................36

17.3.5 Practical Inorganic Chemistry II .............................................................................39

17.4 Organic chemistry section ..............................................................................................40

17.4.1 Organic Chemistry I ................................................................................................40

17.4.2 Practical Organic Chemistry I .................................................................................42

17.4.3 Organic Chemistry II ...............................................................................................44

17.4.4 Practical Organic Chemistry II ................................................................................47

17.4.5 Physical Organic Chemistry ....................................................................................48

17.4.6 Practical Organic Chemistry III ..............................................................................51

17.4.7 Synthetic Organic Chemistry ..................................................................................51

17.5 Physical chemistry section .............................................................................................53

8.5.1 Physical Chemistry I (Chemical Thermodynamics) .................................................53

17.5.2 Physical Chemistry II (Chemical Kinetics and Electrochemistry)..........................55

17.5.3 Physical Chemistry III (Quantum Chemistry) ........................................................57

17.5.4 Physical Chemistry IV (Statistical Thermodynamics and Surface Chemistry) ......60

17.5.5 Practical Physical Chemistry I ................................................................................61

17.5.6 Practical Physical Chemistry II ...............................................................................62

17.6 Applied chemistry section ..............................................................................................63

17.6.1 Research Methodology and Scientific Writing .......................................................63

17.6.2 Industrial Chemistry I .............................................................................................64

17.6.3 Industrial Chemistry II ............................................................................................66

17.6.4 Biochemistry ...........................................................................................................68

17.6.5 Environmental Chemistry and Toxicology .............................................................71

17.6.6 Senior Student Project .............................................................................................73

17.7 Courses for non-chemistry majors .................................................................................74

17.7.1 Fundamentals of Inorganic Chemistry ....................................................................74

17.7.2 Fundamentals of Organic Chemistry.......................................................................76

17.7.3 Fundamentals of Physical Chemistry ......................................................................80

17.7.4. Fundamentals of Analytical Chemistry ..................................................................83

17.8. Elective courses .............................................................................................................86

17.8.4 Chemical Instrumentation .......................................................................................86

17.8.5 Clinical Chemistry...................................................................................................88

17.8.6 Medicinal Chemistry ...............................................................................................90

17.8.7 Polymer Chemistry ..................................................................................................91



17.8.8 Food Chemistry .......................................................................................................93

17.8.9 Agricultural chemistry.............................................................................................93

17.8.10 Physical Inorganic Chemistry ...............................................................................94

17.8.11 Industrial Safety and Quality Control ...................................................................95

17.8.12 Biochemistry and molecular biology ....................................................................97

17.9 Supportive Courses ........................................................................................................97

17.9.1 Calculus I for Chemists ...........................................................................................97

17.9.2 Calculus II for Chemists ..........................................................................................99

17.9.3 Introduction to Statistics .......................................................................................100

17.9.4 Mechanics and Heat for chemists..........................................................................104

17.9.5 Electricity and Magnetism for chemists II ............................................................106

17.9.6 Linear Algebra I for Chemists ...............................................................................108

17.9.7 Introduction to Computer Applications for Chemists ...........................................110

17.10 Common courses ....................................................................................................110

17.10.1 Entrepreneurship .................................................................................................110

17.10.2 Communicative English skills .............................................................................111

17.10.3 University Writing Skills ....................................................................................111

17.10.4 Civics and ethical Education ...............................................................................111



1. Rationale for the curriculum Nationwide need assessment survey was conducted using questionnaire and interview with

employers, alumina, students, and staff members of higher learning institutions. The aim of the

survey was to make use of the collected feed back in designing relevant curricula for the B.Sc.

program in chemistry.

The need assessment revealed that the following were major problems that need to be addressed

to make the quality of the graduates to the level expected.

According to the result of the survey, graduates of the old curriculum of chemistry display:

• Insufficient knowledge of chemistry,

• Insufficient practical skills

• Poor communicative skills

• Poor desire for team work

Similarly, incoming students exhibit

• Insufficient basic subject matter knowledge

• Poor language proficiency

• Poor comprehensive skills (critical thinking and analytical skills) etc.

The mode of delivery was described as being characterized by

• Non interactive teaching methods

• Uneven coverage of content and allocated credit hours

• Lack of relevant teaching materials

• Lack of tailored supportive courses

• Lack of formative assessment etc

External factors that contributed to the perceived problems included:

• Less emphasis was given for science subjects in the university entrance examination

• Lack of interface between preparatory program and university

• Unavailability of institution to produce laboratory technicians

• Mismatch between laboratory groups and existing facilities

The need for proposing the new B.Sc. curriculum is therefore to address problems from the

following sides:

• Students

• Stakeholders need

• Delivery

• Assessment.

The result of the need assessment and the fact that chemistry is changing in its

• Interaction with other disciplines

• Increasingly complex problems

• More advanced techniques and instrumentation

• Working in a global context

and education is changing

• to reflect new research in how students learn (e.g., inquiry-based and active learning,

team experiences)

• because student population is becoming more diverse by age, gender, ethnicity and

educational background have dictated the urgent need to design a fitting curriculum

which ensures production of quality graduates capable of satisfying the stakeholders’

requirements.



2. Aims, Goals and Objectives of the Program

2.1 Aims of the Program

The aims of undergraduate program in chemistry are:

1. To provide higher level training to a number of students who wish to secure B.Sc. degree

in chemistry at University level through standard quality education;

2. To prepare students for pursuing further education;

3. To establish a research centred community where scientific research is undertaken; and

4. To benefit the society.

2.2 Goals of the Program

The major goals of undergraduate program in chemistry are:

1. To establish in students an appreciation of the importance of the chemical science in

industrial, economic, environmental and social context;

2. To provide a basic education appropriate to graduates in chemistry;

3. To develop basic and practical skills in chemistry;

4. To develop the ability to apply the learned skills for solving practical problems; and

5. To provide a wide range of transferable skills to the graduates.

2.3 Objectives of the Program

The objectives of undergraduate program in chemistry are:

1. Produce skilled manpower of well-trained chemists capable of taking up positions in the

growing demand of the various sectors of the economy such as various industries, and

learning institutions, research institutions, as well as various environmental conservation

endeavours of the country;

2. Disseminate knowledge in chemistry and related areas through active participation in related

professional activities, such as Chemical Society of Ethiopia, Regional Networking,

Workshops, Symposia and Publications;

3. Develop capabilities for the provision of consultancy and technical services as well as short

term specialized training to both public and private sectors; and

4. To produce chemists who create job opportunities by applying the acquired knowledge and

skills.

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:

3.1 Knowledge of chemistry

• Master the fundamentals of chemistry including an understanding of broad conceptual and

theoretical elements;

• Posses an understanding and appreciation of the theoretical bases, methodologies and

characteristics of learning of chemistry, research and creative work in chemistry;



• An understanding and appreciation of current issues and debates in chemistry;

• Continue further specialized educations;

• Work as an industrial chemist in chemical processing industries;

• Be a potential candidate of a chemistry teacher;

• Serve as a research/graduate assistant in research /higher education institutions;

• Create job opportunities by the acquired chemical knowledge.

3.2 General intellectual and life skills

• Posses critical, conceptual and reflective thinking, intellectual openness and curiosity,

creativity and originality,

• Recognize when information is needed and locate, evaluate and use this information

effectively.

• An ability to access, identify, organize and communicate chemical knowledge effectively ,

• An ability to work independently as well as part of a team or group;

• An ability to lead in the community, professional associations etc.

• An ability to undertake numerical calculations and understand quantitative information.

• Perform qualitative and quantitative chemical analysis in chemical laboratories;

• Work as quality controllers in industries;

• Knowledgeable in IT and data processing skills in relation to chemical information.

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.

6. List of Major, Supportive and Common Courses

6.1 Core Compulsory Courses

6.1.1 University Chemistry

Course Code Course Title Cr. Hr.

Chem 201 University Chemistry 3

Chem 203 Practical University Chemistry 1

Subtotal 4

6.1.2 Analytical Chemistry

Course Code Course Title Cr. Hr

Chem 222 Analytical Chemistry 3

Chem 224 Practical Analytical Chemistry 1

Chem 321 Instrumental Analysis I 3

Chem 323 Practical Instrumental Analysis I 1

Chem 322 Instrumental Analysis II 3

Chem 324 Practical Instrumental Analysis II 1

Chem 422 Real Sample Analysis 2

Subtotal 14

6.1.3 Physical Chemistry


Chem 331 Physical Chemistry I (Chemical Thermodynamics) 3

Chem 334 Practical Physical Chemistry I 1

Chem 332 Physical Chemistry II (Chemical Kinetics and

Electrochemistry)

3

Chem 433 Practical Physical Chemistry II 1

Chem 431 Physical Chemistry III (Quantum Chemistry) 4

Chem 432 Physical Chemistry IV (Statistical Thermodynamics

and Surface Chemistry)

3

Subtotal 15



6.1.4 Organic Chemistry


Chem 242 Organic Chemistry I 3

Chem 244 Practical Organic Chemistry I 1

Chem 341 Organic Chemistry II 3

Chem 343 Practical Organic Chemistry II 1

Chem 342 Physical Organic chemistry 3

Chem 441 Practical Organic Chemistry III 2

Subtotal 13

6.1.5 Inorganic Chemistry


Chem 212 Inorganic Chemistry I 3

Chem 313 Practical Inorganic Chemistry I 1

Chem 311 Inorganic Chemistry II 3

Chem 414 Practical Inorganic Chemistry II 2

Chem 411 Inorganic Chemistry III 4

Subtotal 13

6.1.6 Applied Chemistry


Chem 352 Industrial Chemistry I 3

Chem 451 Industrial Chemistry II 2

Chem 452 Biochemistry 3

Chem 455 Environmental Chemistry and Toxicology 3

Chem 453 Research Methodology and Scientific Writing 2

Sub-total 13

6.2 Core Elective Courses


Chem 426 Chemical Instrumentation 3

Chem 416 Physical Inorganic chemistry 3

Chem 446 Synthetic organic chemistry 3

Chem 448 Polymer Chemistry 2

Chem 456 Agricultural chemistry 3

Chem 458 Medicinal chemistry 3

Chem 450 Clinical chemistry 3

Chem 454 Food chemistry 3

Chem 351 Internship in Chemistry 3

Chem 457 Biochemistry and Molecular Biology 3

Chem 462 Industrial Safety and Quality Control 2

Chem 460 Current Topics in Chemistry 2

Chem 459 Student Project 3

Subtotal 36



6.3 Supportive Courses

Course Code Course Title Cr Hr

Math 233 Calculus I for Chemists 3

Math 224 Linear Algebra for Chemists 3

Math 234 Calculus II for Chemists 3

Phys 206 Electricity and Magnetism for Chemists 3

Phys 205 Mechanics and Heat for Chemists 3

Comp 201 Introduction to Computer Applications for Chemists 3

Stat 273 Introduction to Statistics 3

Subtotal 21

6.4 Common Courses

Course Code Course Title Cr.hrs

EnLa 201 Communicative English skills 3

EnLa 301 University Writing Skills 3

CEEd 201 Civics and Ethical Education 3

Mgmt 401 Entrepreneurship 3

Subtotal 12

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

8. Course Coding Style (Course Numbering) In coding or numbering courses, the first four letters of the word “chemistry” with only the first

letter in CAPITAL i.e. Chem followed by three digit numbers are used whereby:

a) The first digit starts from 2;

b) The middle digit indicates the course stream areas of chemistry; and

-0- University Chemistry

-1- Inorganic Chemistry

-2- Analytical Chemistry

-3- Physical Chemistry

-4- Organic Chemistry

-5- Applied chemistry

-6-Miscellaneous courses

c) The last digit indicates the semester in which the course is delivered: odd-for first semester

and even for second semester;

d) For practical courses offered in the same semester with its lecture course, the next odd or

even number is used with few exceptions;

e) Space is let between the letters, Chem and the numbers.



9. Sequencing of courses: Semester wise course breakdown

Year I

Semester I

Course

Code

Course Title Cr. Hr Course

type

Chem 201 University Chemistry 3 Core

Chem 203 Practical University Chemistry 1 Core

Phys 205 Mechanics and Heat for Chemists 3 Supportive

Math 233 Calculus I for Chemists 3 Supportive

EnLa 201 Communicative English skills 3 Common

Comp 201 Introduction to Computer Applications for

Chemists

3 Supportive

Stat 273 Introduction to Statistics 3 Supportive

Total 19

Semester II

Course

Code


type

Chem 222 Analytical Chemistry 3 Core

Phys 206 Electricity and Magnetism for Chemists 3 Supportive

Chem 242 Organic Chemistry I 3 Core

Chem 244 Practical Organic Chemistry I 1 Core

Chem 212 Inorganic Chemistry I 3 Core

Chem 224 Practical Analytical Chemistry 1 Core

Math 234 Calculus II for Chemists 3 Supportive

Total 17

Semester I

Year II

Code Course Title Cr. Hr Course

type

Chem 331 Chemical Thermodynamics 3 Core

Chem 311 Inorganic Chemistry II 3 Core

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

Semester I

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

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

Semester II

Course

Code

Course Title Cr. Hr Type

Chem 422 Analysis of real samples 2 Core

Chem 452 Biochemistry 3 Core

Chem 432 Statistical Thermodynamics and Surface

Chemistry

3 Core

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

10. General Delivery Methods For theoretical courses given in class, student centred (active learning) methodology will be applied.

To achieve this, the following methods will be used:

• Brain storming,

• Lecture,

• Tutorial and seminars,

• Practical classes, field work, industrial visits,

• Group or individual assignments,

• Independent, web-based and computer assisted learning,

• Presentations and group discussion,

• Project work,

• Demonstration and observation and

Semester II

Course code Course Title Cr.

Hr

Type

Chem 332 Chemical kinetics and Electrochemistry 3 Core

Chem 342 Physical Organic Chemistry 3 Core

Chem 322 Instrumental analysis II 3 Core

Chem 324 Practical instrumental analysis II 1 Core

Chem 334 Practical Physical Chemistry I 1 Core

Chem 352 Industrial Chemistry I 3 Core

Math 224 Linear Algebra for Chemists 3 Supportive

Total 17



• Problem solving.

11. General Evaluation Methods The evaluation methods of students include:

• Quizzes, tests, mid-term, and final term exams;

• Assignments and attendances;

• Presentations in group or individual;

• Laboratory reports and flow charts;

• Practical and oral exams.

12. Grading System The system of grading shall be:

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

13. Duration of the Study The program shall be on the basis of three academic years of study.

14. Grade Point Average Requirements for Graduation

SN Description Minimum requirement

1 Cumulative GPA 2.00

2 Major GPA 2.00

3 No ''F'' in any course

15. Degree Nomenclature

15.1 In English:

Bachelor of Science Degree (B. Sc) in Chemistry

15.2 In Amharic:

የየየየ ሣሣሣሣ ይይይይ ንንንን ስስስስ ባባባባ ችችችች ለለለለ ርርርር ዲዲዲዲ ግግግግ ሪሪሪሪ በበበበ ኬኬኬኬ ሚሚሚሚ ስስስስ ትትትት ሪሪሪሪ¶

16. Mechanism of Quality Assurance Quality assurance is considered as the most important component of the teaching-learning

process. The Department of Chemistry uses the following systems of evaluation and monitoring:

Preparation of standard course outlines as per the course description:

• Assignment of qualified instructors to teach courses, instruct laboratory works, and

supervise student projects;

• Identification of standard textbooks for each course;

• Maintain appropriate student/teacher ratio;

• Provision of tutorial and practical classes keeping the appropriate tutor/student ratio (40/1

for tutorial and 20/1 for practicals);

• Provide proper advice to students;



• 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.

17. Course descriptions, Course Outlines, Modes of Course Delivery and Modes of Performance Evaluation

17.1 University Chemistry Section

17.1.1 University chemistry

COURSE TITLE: U6IVERSITY CHEMISTRY

COURSE CODE CHEM 201

CREDIT HOURS 3

CO6TACT HOURS: 3 LEC. HR/WEEK

PRE-REQUISITE

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



1.2.6. Mass Percentage Composition

2. The composition of matter

2.1. Elements

2.1.1. The Names and Symbols of the Elements

2.1.2. The Periodic Table

2.2. Atoms

2.2.1. The Nuclear Atom

2.2.2. The Masses of Atoms

2.2.3. Moles and Molar Mass

2.3. Compounds

2.3.1. Molecules and Molecular Compounds

2.3.2. Ions and Ionic Compounds

2.3.3. Chemical Nomenclature

3. Chemical reactions

3.1. Chemical Equations

3.1.1. Symbolizing Reactions

3.1.2. Balancing Equations

3.2. Precipitation Reactions

3.2.1. Net Ionic Equations

3.2.2. Using Precipitation Reactions in Chemistry

3.3. Acid-Base Reactions

3.3.1. Arrhenius Acids and Bases

3.3.2. Neutralization

3.3.3. The Brönsted Definitions

3.4. Redox Reactions

3.4.1. Electron Transfer

3.4.2. The activity series

3.4.3. Balancing reactions by using half-reactions

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



5.4.3. Periodicity of Physical Properties

5.4.4. Trends in Chemical Properties

6. The chemical bond

6.1. Ionic Bonds

6.1.2. The Energetics of ionic Bond Formation

6.1.3. Ionic Bonds and the Periodic Table

6.2. Covalent Bonds

6.2.2. The electron-pair bond

6.2.3. Lewis Structures of Polyatomic Molecules

6.2.4. Lewis Acids and Bases

6.2.5. Resonance

6.2.6. Exceptions to the Lewis Octet Rule

6.3. The Shapes of Molecules

6.3.2. Electron-pair Repulsions

6.3.3. Molecules with Multiple Bonds

7. The structures of molecules

7.1. Bond Parameters

7.1.2. Bond Strength

7.1.3. Bond Lengths

7.2. Charge Distributions in Compounds

7.2.2. Ionic versus Covalent Bonding

7.2.3. Assessing the Charge Distribution

7.3. The Valence-Bond Model of Bonding

7.3.2. Bonding in Diatomic Molecules

7.3.3. Hybridization

7.4. Molecular Orbital Theory

7.4.2. Molecular Orbitals

7.4.3. Bonding in Period 2 Diatomic Molecules

8. The properties of solutions

8.1. Measures of Concentration

8.1.2. Emphasizing the Amounts of Solute in Solution

8.1.3. Emphasizing Relative Amounts of Solute and Solvent Molecules

8.2. Solubility

8.2.2. Saturation and Solubility

8.2.3. The Effect of Pressure on Gas Solubility

8.2.4. The Effect of Temperature on Solubility

8.3. Colligative Properties

8.3.2. Changes in Vapor Pressure, Boiling Points, and Freezing Points

8.3.3. Osmosis

8.4. Mixtures of Liquids

8.4.2. Raoult’s Law for Mixtures of Liquids

8.4.3. The Distillation of Mixtures of Liquids

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



9.2. Equilibrium Calculations

9.2.2. Specific Initial Concentrations

9.2.3. Arbitrary Initial Concentrations

9.3. The Response of Equilibria to the Reaction Conditions

9.3.2. The Effect of Added Reagent

9.3.3. The Effect of Pressure

9.3.4. The Effect of Temperature

10. Intrduction to functional groups and their typical reactions

10.1. Alkanes, Alkenes and Alkynes

10.2. Aromatic compounds

10.3. Alcohols

10.4. Aldehydes and ketones

10.5. Carboxylic acids and their derivatives

10.6. Ethers

10.7. Amines

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/

17.1.2 University Practical Chemistry

COURSE TITLE: U6IVERSITY PRACTICAL CHEMISTRY

COURSE CODE CHEM 203

CREDIT HOURS 1

CO6TACT HOURS: 3 LAB. HR/WEEK

PRE-REQUISITE -

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%


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

17.2 Analytical chemistry section

17.2.1 Analytical Chemistry

COURSE TITLE: A6ALYTICAL CHEMISTRY

COURSE CODE: CHEM 222

CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC.HR/WEEK

PREREQUISITE:

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



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

2.3.3 Factors affecting stability of complexes

2.3.4 Effect of complexation on solubility

2.4 Oxidation-reduction equilibria

2.4.1 Redox reactions, reducing and oxidizing agents

2.4.2 Redox reactions in electrochemical cells and electrode potential

2.4.3 Dependence of electrode potential on concentration

2.4.4 Calculating equilibrium constant from electrode potential

3. Statistical evaluation of analytical data

3.1 Mean, Standard deviation, Variance

3.2 Accuracy and precision of measurements

3.3 Errors in analytical results

3.4 Confidence limit

3.5 Testing for significance (t-test and F-test)

3.6 Rejection test (Q-test)

4. Solutions and their concentrations

4.1 Types of solutions

4.2 Different ways of expressing concentration

4.3 Preparation of solutions

4.4 Activity and activity coefficient

5. Titrimetric methods of analysis

5.1 Fundamentals of titrimetry

5.1.1 Definition of terms

5.1.2 Ideal requirements for standard solutions

5.1.3 Volumetric calculations

5.2 Acid-base titration

5.2.1 Acid-base titration curves

5.2.2 Acid-base indicators

5.3 Precipitation titration

5.3.1 Titration curves

5.3.2 End point detection methods

5.4 Complexometric titration



5.4.1 Titration with aminopolycarboxylic acids (EDTA and its species)

5.4.2 EDTA titration curve


5.5 Redox titration

5.5.1 Derivation of redox titration curves

5.5.2 Oxidation-reduction indicators

6. Gravimetric analysis

6.1 Principle and types of gravimetric analysis

6.2 Properties of precipitates and precipitating agents

6.3 Steps in gravimetric analysis

6.4 Gravimetric calculations

Mode of delivery:

- Lecture

- group discussion

- assignment in group or individually

- home work

Mode of assessment:

- Quizzes,

- assignments,

- tests,

- Mid-term and final examinations.


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

17.2.2 Practical Analytical Chemistry

COURSE TITLE: PRACTICAL A6ALYTICAL CHEMISTRY


CREDIT HOURS: 1


PREREQUISITE:



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, 2

nd 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.

17.2.3 Instrumental Analysis I

COURSE TITLE: I6STRUME6TAL A6ALYSIS I


CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC. HR /WEEK

PREREQUISITE: CHEM 222 A6D CHEM 224

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



10.1 Basic principles of electrophoresis

10.2 Types and application of 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.


1. D.A. Skoog, D.M. West and F.J. Holler, Fundamentals of Analytical Chemistry, 7th Ed.,


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


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


7. J.M. Marmet, M. Otto and H.M. Widmer (editors), Analytical chemistry, Wiley-VCH,

Weinheim, 1998.

17.2.4 Practical Instrumental analysis I

COURSE TITLE: PRACTICAL I6STRUME6TAL A6ALYSIS I


CREDIT HOURS: 1


CO-REQUISITE: CHEM 321

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.



• Know the extent of accuracy in each method.

• Understand the precautions required in every method.

• Identify different parts of selected instruments and describe their respective functions.

• Separate, identify and determine the quantity of a given species from a sample by using

different chromatographic techniques (PC, TLC etc).

• Determine the quantity of a given species from a sample by using different

electroanalytical techniques (conductometry, potentiometry etc).

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.


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.

17.2.5 Instrumental Analysis II

COURSE TITLE: I6STRUME6TAL A6ALYSIS II


CREDIT HOURS: 3


PREREQUISITE: CHEM 321

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



1.2 Electromagnetic radiation and its quantum mechanical property

1.3 Absorption and Emission of Radiation

1.4 The electromagnetic spectrum

2. Absorption Laws (Quantitative Analysis)

2.1 Lambert-Beer's Law

2.2 Deviation from Beer's Law

2.3 Errors associated with Beer's Law

3. Instruments for optical spectroscopy

3.1 Components of optical instruments

3.1.1 Source of Radiation

3.1.2 Wave-length selectors

3.1.3 Sample containers

3.1.4 Radiation Detectors

3.1.5 Read out detectors and signal amplification systems

3.2 Optical systems used in spectroscopy: Single beam versus double beam

4. Atomic Absorption and emission spectroscopy

4.1 Principles

4.2 Instrumentation

4.3 Analytical Applications

5. Ultraviolet and Visible (UV-Vis) Spectroscopy

5.1 Introduction

5.2 Basic Principles

5.3 Absorption characteristics of some chromopores

5.4 Instrumentation

5.5 Application

6. Infrared Spectroscopy

6.1 Introduction

6.2 Energy levels in vibrating and rotating molecules

6.3 Characteristic vibrational frequencies

6.4 Factors affecting group frequencies

6.5 Instrumentation

6.6 Interpretation of some spectra

7. Nuclear Magnetic Resonance Spectroscopy (NMR)

7.1 Basic principle of NMR

7.2 NMR spectrometers

7.3 Proton NMR

7.4 C–13 NMR

7.5 Interpretation of NMR spectra

8. Structure elucidations by joint application of different spectroscopic methods: UV, IR, NMR

and mass spectrometry.

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.




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.

17.2.6. Practical Instrumental analysis II

COURSE TITLE: PRACTICAL I6STRUME6TAL A6ALYSIS II


CREDIT HOURS: 1



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.


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.

17.2.7. Analysis of Real Samples

COURSE TITLE: A6ALYSIS OF REAL SAMPLES


CREDIT HOURS: 2


PREREQUISITE: CHEM 323, CHEM 324

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.



Mode of assessment: Attendance, observation while the student was doing lab, oral questions, correcting laboratory

report, practical examination and written examination.


To be designated at commencement of the course.

17.3 Inorganic chemistry section

17.3.1. Inorganic Chemistry I

COURSE TITLE: I6ORGA6IC CHEMISTRY I


CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC. HR/ WEEK


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



4. The chemistry of Hydrogen

4.1 Compounds of hydrogen

4.2 Synthesis

4.3 Reactivity of hydrogen

4.4 Application of hydrogen

5. The chemistry of s-block elements

5.1 The chemistry of alkaline metals

5.1.1 General trends

5.1.2 Some compounds of alkali metals

5.1.3 Occurrences, reactivity and extraction of the metals

5.2 The chemistry of alkaline earth metals

5.2.1 General trends


6. The chemistry of p-block elements

6.1 The chemistry of boron group elements

6.1.1 Trends and some compounds of the group elements

6.1.2 Occurrences, reactivity and extraction of the elements

6.2 The chemistry of carbon group elements



6.3 The chemistry of nitrogen group elements



6.4 The chemistry of oxygen group elements



6.5 The chemistry of halogen group elements



6.6 The chemistry of noble gases



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

Text: A new concise inorganic chemistry, J.D. Lee 5th Ed..

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.



17.3.2. Inorganic Chemistry II

COURSE TITLE: I6ORGA6IC CHEMISTRY II


CREDIT HOURS: 3



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



2.1.5 Catalytic properties of the metals in synthesis

3. Coordination chemistry of transition metals

3.1 Definition, nomenclature and isomerism

3.2 Valence bond theory

3.3 Crystal field theory

3.4 Molecular orbital theory

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 5

th 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.

17.3.3 Practical Inorganic Chemistry I

COURSE TITLE: PRACTICAL I6ORGA6IC CHEMISTRY I


CREDIT HOURS: 1



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.



• 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



4.1. Preparation and reactions of Chromium (III) compounds

4.1.1. Preparation of chromium (III) oxide

4.1.2. Preparation of Chromic hydroxide

4.1.3. Amphotoric character of Chromium (III) hydroxide

4.2. Oxidation of tetravalent chromium to dichromate (VI) by peroxodisulphate in acidic

medium

4.2.1. Introversion of chromium and dichromate

4.2.2. Oxidation of iodide by dichromate in acidic medium

5. The chemistry of Iron

5.1. Preparation and properties of pyrophoric iron

5.2. Reaction of iron with acids

5.3. Preparation of ferrous hydroxide and its oxidation by atmospheric oxygen

5.4. Basic character of ferrous hydroxide

5.5. Reaction of iron (II) with potassium hexacyanoferrate (III); Trundle’s rule

5.6. Preparation and properties of ferric hydroxide

6. The chemistry of Molybdenum

6.1. Preparation and reactions of molybdenum (VI) compounds

6.2. Preparation and properties of molybdic acid

6.3. Amphoteric properties of molybdic acid

6.4. Preparation of molybdenyl hexacyanoferate (II)

6.5. Preparation of sparingly soluble molybdates

6.6. Preparation of thiomolybdate and molybdenum (VI) sulphide

6.7. Peroxomolybdates

6.8. Identification of molybdenum by its red hexathiocyanate molybdate (III) complex

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.

Text: Manual of Practical Inorganic Chemistry I

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.

17.3.4. Inorganic Chemistry III

COURSE TITLE: I6ORGA6IC CHEMISTRY III


CREDIT HOURS: 4





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



2.1.13. Terms of equivalent electrons

2.1.14. Electronic spectra of transition metal complexes

2.1.15. Selection rules

2.1.16. Nature of electronic transitions in complexes with d1-d9

configuration in octahedral and tetrahedral complexes

2.1.17. Magnetochemistry

3. Organometallic chemistry

3.1. Introduction

3.1.14. Historical background

3.1.15. Properties

3.1.16. Classifications of organometallic compounds by bond type

3.1.17. The ‘stability’ of organometallics compounds

3.2. Structure and bonding in organometallic compounds

3.2.14. Ionic

3.2.15. Covalent

3.2.16. Electron deficient complexes

3.3. Methods of formation of metal-carbon bonds

3.3.14. The reaction between a metal and an organic halogen compound

3.3.15. Metal exchange

3.3.16. Reactions of organometallic compounds with metal halides

3.3.17. Addition of metal hydrides to alkenes and alkynes

3.3.18. Formation of metal-carbon bonds by other insertion reactions

3.3.19. Preparation of π-bonded complexes

3.4. Catalytic applications of organometallic compounds

3.4.14. Description of catalysis

3.4.15. Properties of catalysis

3.4.16. Homogeneous catalysis

3.4.17. Heterogeneous catalysis

4. Bio-inorganic chemistry

4.1. Introduction

4.2. Essential elements

4.3. Oxygen utilization

4.4. Supply and storage of iron

4.5. Oxidation reduction processes

4.6. Metalloenzymes

4.7. Vitamin B12

4.8. Nitrogenase

4.9. Photosynthesis

4.10. Roles of Na+, K

+, Mg

2+, Ca

2+ and iron pumps

Mode of delivery:

Gaped-lecture, lecture-demonstration, group work, presentation, and project work.




Text: To be designated at the commencement of the course.



17.3.5 Practical Inorganic Chemistry II

COURSE TITLE: PRACTICAL I6ORGA6IC CHEMISTRY II


CREDIT HOURS: 2



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.




Text: To be designated at the commencement of the course.



17.4 Organic chemistry section

17.4.1 Organic Chemistry I

COURSE TITLE: ORGA6IC CHEMISTRY I

COURSE 6UMBER: CHEM 242

CREDIT HOURS: 3


PREREQUISITE:

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



1.1. Historical background of organic chemistry

1.2. Energy Levels and Atomic Orbitals

1.3. Bonding in carbon compounds:

1.3.1. Valence Bond Concept

1.3.2. Orbital Hybridizations

1.3.3. Molecular Orbital Concept

1.4. Factors influencing electron availability and reactivity of organic compounds

1.4.1. Inductive effect

1.4.2. Resonance effect

1.4.3. Steric effect

2. Functional groups in organic chemistry

2.1. The importance of Classification of organic compounds according to their

Functionality

2.2. Introduction to the common functional groups in organic chemistry, their typical

preparations and reactions.

2.1.1 Alkanes, alkenes, alkynes,

2.1.2 aromatic hydrocarbons,

2.1.3 alcohols, ethers, and epoxides

2.1.4 amines, nitriles

2.1.5 Aldehydes and ketones,

2.1.6 Carboxylic acids and their derivatives.

3. Stereochemistry

3.1 Definitions: Symmetry, Dissymmetry and Chirality

3.2 Elements of Symmetry

3.3 Stereoisomerism: Definition and Classes (Geometric, Configurational,

Conformational Isomerism)

3.4 Configurational (Optical) Isomerism

3.4.1 Common Criterion for Chirality: The Asymmetric Carbon

3.4.2 Enantiomers and their Properties

3.4.3 Optical Activity and Plane Polarized Light

3.4.4 Optical Rotation

3.4.5 Measurement of Optical Rotation: The Polarimeter

3.4.6 Specific Rotation

3.4.7 Racemic mixtures and their Properties

3.4.8 Configuration of Chiral Compounds

3.4.8.1 The Cahn-Ingold-Prelog (CIP) sequence rules for assigning

configurations

3.4.9 Fischer Projections

3.4.10 Multiple Stereogenic Centres

3.4.11 Diastereomers

3.4.12 Meso compounds

3.4.13 Resolution of Racemic Mixtures

3.5 Conformational Isomerism

3.5.1 Conformational Analysis in alkanes: Ethane and n-Butane

3.5.2 Cycloalkanes: Cyclopropane, cyclobutane, cyclopentane and Cyclohexane

3.5.3 Substituted Cycloalkanes: Methyl and Dimethyl cyclohexanes

4. Major organic reactions

4.1 Substitution Reactions

4.1.1 Introduction

4.1.2 SN2 and SN1 mechanism



4.1.3 Factors affecting SN2 and SN1 reactions

4.1.4 Applications of Substitution Reactions

4.2 Elimination reactions

4.2.1 Introduction

4.2.2 E2 and E1 mechanism

4.2.3 Elimination versus substitution

4.2.4 Zaistev’s and Hoffman rules

4.2.5 Applications of Elimination Reactions

4.2.6 Other Elimination Reactions

4.3 Addition Reactions

4.3.1 Mechanism and Reactivity

4.3.2 Markovnikove’s Rule

4.3.3 Anti-Markovnikove (Radical) Addition

4.3.4 Michael addition

4.3.5 Examples of Addition Reactions

4.3.6 Other Reactions of Double Bonds

4.3.6.1 Ozonization

4.3.6.2 Diels-Alder reaction

4.3.6.3 Glycol formation

4.3.6.4 Addition polymerization

4.4 Rearrangement reactions

4.4.1 Migration to electron deficient carbon

Wagner-Meerwien Rearrangement

4.4.2 Migration to electron deficient oxygen.

The Bayaer-Villiger Oxidation

4.4.3 Migration to electron deficient nitrogen

Beckmann Rearrangement

Hofmann Rearrangement

Mode of delivery:

Gapped-lecture, lecture-demonstration, group work & presentation & project work.


Oral questions, Short tests at the end of each chapter, assignment, group work assessment,

summative exam at the end of the semester.


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.

17.4.2 Practical Organic Chemistry I

COURSE TITLE: PRACTICAL ORGA6IC CHEMISTRY I


CREDIT HOURS: 1

CO6TACT HOURS: 3 LAB. HR/ WEEK

PREREQUISITE:



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


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.

17.4.3 Organic Chemistry II

COURSE TITLE: ORGA6IC CHEMISTRY II


CREDIT HOURS: 3



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



• Classify various preparative methods of biological molecule such as carbohydrates,

lipids, amino acids and proteins, and their important chemical properties

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



3.2.2 Wittig reaction

3.2.3 Acetals

3.2.4 Ester hydrolysis and formation

3.2.5 Reactions of acid chlorides

3.2.6 Reactions of acid anhydrides

3.2.7 Reactions of amides

3.2.8 Reductions of acid derivatives

3.3 Enolization-Ketonization reactions

3.3.1 Haloform Reaction of Methyl Ketones

3.3.2 Alkylations at the α-Carbon

3.3.3 Aldol and Related Condensation reactions

4. Oxidation–Reduction reactions

4.1. Oxidation Reactions

3.3.4 Alcohols

3.3.5 Aldehydes

3.3.6 Multiple Bonds

4.2. Reduction Reaction

3.3.7 Catalytic Hydrogenation

3.3.8 Hydride Reduction

3.3.9 Dissolving metal reduction

5. Introduction to Chemistry of Biomolecules

1.1 Carbohydrates

1.1.1 Glucose

1.1.2 The Structure and Configuration of Glucose

1.1.3 Anomeric forms of Monosaccharides

1.1.4 Glycosides

1.1.5 Disaccharides

1.1.6 Polysaccharides

1.2 Lipids

1.2.1 Fatty Acids

1.2.2 Fats & Oils

1.2.3 Waxes

1.2.4 Phospholipids

1.2.5 Prostaglandins

1.2.6 Terpenes

1.2.7 Steroids

1.3 Proteins and Amino Acids

1.3.1 α-Amino Acids

1.3.2 Reactions of Amino Acids

1.3.3 Synthesis of Amino Acids

1.3.4 Peptides & Proteins

1.3.5 The Primary Structure of Peptides

1.3.6 Secondary & Tertiary Structure of Large Peptides and Proteins

1.3.7 Peptide Synthesis

1.4 Nucleic Acids

1.4.1 Introduction to the chemistry of Nucleic Acids (Structure and Chemistry)

Mode of delivery:

Gaped-lecture, lecture-demonstration, group work & presentation & project work.




Oral questions, Short tests at the end of each chapter, assignment, group work assessment,

summative exam at the end of the semester.


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.

17.4.4 Practical Organic Chemistry II

COURSE TITLE: PRACTICAL ORGA6IC CHEMISTRY II


CREDIT HOURS: 1

CO6TACT HOURS: 3 LAB.HR/ WEEK


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



Experiment 11: Polymers

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



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.

17.4.5 Physical Organic Chemistry

COURSE TITLE: PHYSICAL ORGA6IC CHEMISTRY


CREDIT HOURS: 3



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



3.1.3 Carbanion stability

3.1.4 Typical reation of carbanions (Addition, Elimination, Substitution and

Rearrangements)

3.2 Carbocations

3.2.1 Carbocations

3.2.2 generation,

3.2.3 Carbocations stability,

3.2.4 Typical reactions of carbocations, (Addition, Elimination, Substitution and

Rearrangement)

3.3 Carbenes and Nitrenes

3.3.1 Generation and reactions of Carbenes and Nitrenes

3.4 Free radical reactions

3.4.1 Free radicals (stability, Methods of generation, typical reactions)

4 Pericyclic reactions

4.1 Introduction

4.2 Classes of Pericyclic reactions

4.3 Electrocyclic reactions

4.3.1 Typical reactions

4.3.2 Stereospecificity

4.3.3 stereoselectivity

4.4 Cycloadditions.


4.4.2 Regioselectivity



4.5 Sigmatopic arrangements




4.6 Ene Reactions

5. Structure Elucidation of Organic Compounds

5.1 Combustion Analysis for Determination of Elemental Composition

5.2 Ozonolysis for Determination of Sites of Unsaturations

5.3 Molecular Spectroscopy

5.3.1 Ultraviolet-Visible Spectroscopy

5.3.2 Infrared Spectroscopy

5.3.3 Nuclear Magnetic Resonance Spectroscopy

5.4 Mass Spectrometry

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.


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.



17.4.6 Practical Organic Chemistry III

COURSE TITLE: PRACTICAL ORGA6IC CHEMISTRY III


CREDIT HOURS: 2



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.

17.4.7 Synthetic Organic Chemistry

COURSE TITLE: SY6THETIC ORGA6IC CHEMISTRY


CREDIT HOURS: 3



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



1.1.1. Functionalization of alkanes,

1.1.2. Functionalization of alkenes,

1.1.3. Functionalization of alkynes,

1.1.4. Functionalization of aromatic hydrocarbon,

1.1.5. Functionalization of simple hetrocyclic compounds

1.2 Interconversion of functional groups

1.1.1. Transformation of the hydroxyl group,

1.1.2. Transformation of the amino group,

1.1.3. Transformation of the alkyl halides,

1.1.4. Transformation of the nitro compounds,

1.1.5. Transformation of the aldehydes, ketones, acid and acid derivatives

2. Formation of carbon-carbon bonds; ring closure and ring opening reactions

2.1 Formation of carbon-carbon bonds

2.2 Electrophilic carbon bonds

2.3 Nucleophilic carbon bonds,

2.4 Reaction of organometallic species

2.5 Ring closure, Intramolecular cyclization electrophile-nucleophile interaction,

cycloaddition, electrocyclic ring closure, ring opening reaction

2.6 Hydrolysis, Solvolysis, and other electrophile-nucleophile interaction, oxidative

and reductive ring opening, electrocyclic ring opening

3. Analysis of synthetic pathways

3.1. Synthetic strategies

3.2. target selection,

3.3. retrosynthetic analysis

4. Principles of asymmetric synthesis

4.1. What is asymmetric synthesis?

4.2. Asymmetric induction

5. Protective groups in synthesis

5.1 Alcohol protective groups,

5.2 Protective groups of aldehyde and ketones,

5.3 Protective groups of amino groups

5.4 Carboxylic acids protective groups

5. Illustrative examples of multi-step synthesis

Mode of delivery:



Mode of assessment:

Assignments, presentation, mid exam, final exam and continuous assessment techniques of




17.5 Physical chemistry section

8.5.1 Physical Chemistry I (Chemical Thermodynamics)

COURSE TITLE: PHYSICAL CHEMISTRY I

(CHEMICAL THERMODY6AMICS)


CREDIT HOURS: 3


PREREQUISITE: MATH. 231

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



3.2.1 Pressure volume work

3.2.2 Enthalpy (Heat content)

3.2.3 Heat capacities

3.2.2.1 Heat capacities (CP and CV) relationships

3.2.2.2 Heat capacity and temperature relationship

3.2.4 Reversible isothermal process

3.2.5 Reversible adiabatic process

3.2.6 Thermochemistry

3.2.6.1 Internal energy and enthalpy

3.2.6.2 The law of thermochemistry

3.3 Second law of thermodynamics

3.3.1 The Carnot cycle

3.3.2 Entropy

2.3.2.1 Entropy change in a reversible process

2.3.2.2 Entropy changes in an irreversible process

2.3.2.3 Entropy changes for an ideal gas

2.3.2.4 Entropy change in a chemical reaction

3.3.3 Free Energy

2.3.3.1 Dependence of Helmholtz free energy on volume and

temperature

2.3.3.2 Dependence of Gibbs free energy on pressure and temperature

3.3.4 Maxwell relations

3.3.5 Chemical potential

2.3.5.1 Gibbs-Duhem equation

2.3.5.2 Chemical potential for an ideal gas and gas mixture

3.4 Third law of thermodynamics 4. Chemical Equilibrium and Phase Equilibrium

4.1 Chemical Equilibrium

4.1.1 Standard Gibbs free energy of reaction and equilibrium

4.1.2 Relationship between Kp and Kc

4.1.3 Variation of equilibrium constant with temperature and pressure

4.2 Phase Equilibrium

4.2.1 Clapeyron and Clausius Clapeyron equation

4.2.2 Phase, components, degrees of freedom and phase rule

4.2.3 Phase diagram

4.2.3.1 A single component systems

4.2.3.2 A two component systems

4.2.3.3 A three component systems 5. Non Electrolyte Solutions

5.1 Solutions of gases in liquids (Henry's law)

5.2 Solutions of gases in gases (Daltons law of partial pressure)

5.3 Solutions of liquids in liquids (Raoult's law)

5.3.1 Completely miscible liquids

5.3.1.1 An ideal solution and vapour pressure of ideal solutions

5.3.1.2 Vapour pressure of non-ideal solutions

5.3.1.3 Boiling point diagrams of an ideal and real solutions

5.3.1.4 Fractional distillation

5.3.2 Partially miscible liquids

5.4 Solutions of non-volatile solutes (Colligative Properties)

5.4.1 Vapour pressure lowering



5.4.2 Boiling point elevation

5.4.3 Freezing point depression

5.4.4 Osmotic pressure

Mode of delivery:



Mode of assessment:




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.

17.5.2 Physical Chemistry II (Chemical Kinetics and Electrochemistry)

COURSE TITLE: PHYSICAL CHEMISTRY II

(CHEMICAL KI6ETICS A6D ELECTROCHEMISTRY)


CREDIT HOURS: 3



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:


• 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




Mode of assessment:







1992.


1981.


17.5.3 Physical Chemistry III (Quantum Chemistry)

COURSE TITLE: PHYSICAL CHEMISTRY III (QUA6TUM CHEMISTRY)


CREDIT HOURS: 4


PREREQUISITE: MATH. 231, MATH. 232

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:


• 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



2.8. Heisenberg's Uncertainty Principle

3. The Schrödinger Equation

3.1. Derivation of Schrödinger's Equation

3.2. Schrödinger Equation: Steady-State Form

3.3. Interpretation of the Ψ

4. Operations in Quantum Mechanics

4.1. Introduction

4.2. Eigenvalue and Eigenfunctions

4.3. Angular Momentum

4.4. Important Theorems

5. Solutions of Schrödinger Equations for Simple Systems

5.1. Introduction

5.2. Free Particle in One Dimension

5.3. Particles in a One Dimensional Box: The Colour of Conjugated Organic Molecules

5.4. Rotational Motion

5.4.1. Particle on a Ring

5.4.2. Particle on a Sphere

5.5. Harmonic Oscillator

5.5.1. Classical Treatment of Harmonic Oscillator

5.5.2. Quantum Mechanical Treatment of the Harmonic Oscillator

5.5.3. Vibration of Diatomic Molecules

5.5.4. Selection Rules for Harmonic Oscillator

6. Atomic Structure

6.1. The Hydrogen Atom

6.2. Schrödinger Equation of the Hydrogen Atom

6.3. Hydrogen Wave Functions

6.3.1. The Radical Wave Functions

6.3.2. The Angular Wave Functions

6.4. Energy Eigenvalues of H-Spectrum

6.4.1. Derivation of the Rydberg Formula

6.4.2. The Spectral Selection Rule

6.5. Atomic Spectra in Magnetic Field

6.6. The Electron Spin

6.6.1. Stern-Gerlach Experiment

6.6.2. Energy of Electron in Magnetic Field

6.7. Pauli Exclusion Principle

6.8. The Periodic Table

6.8.1. Electronic Structure of the He Atom

6.8.2. Slater Determinant

6.8.3. Short Notation of Electron Configuration: nlx notation

6.8.4. Change of Energy Levels by Screening and Penetration

6.9. Angular Momentum of Many Electron Atom

6.9.1. Spin-Orbit Interaction (Vector Model of the Atom)

6.9.2. The Spin-Orbit Coupling Schemes

6.9.3. Energy States of Atoms and their Term Symbols

6.9.4. Polyelectronic Atoms

6.9.5. Relative Energies of the States and Hund's Rule

7. Approximation Methods

7.1. Introduction

7.2. The He Atom



7.3. The Method of Independent Approximation

7.4. The Variation Method

7.5. Perturbation Method

7.6. Self-Consistent Field Approximation (SCF)

7.6.1. Hatree's Self-Consistent Field Theory

7.6.2. Hatree-Fock Self-Consistent Field (HFSCF) Theory

7.7. Ab Initio Method

8. The Chemical Bond

8.1. Introduction

8.1.1. Development of Valence Theory

8.1.2. Ionic Bond

8.1.3. Covalent Bond

8.2. Quantum Chemical Bond Description

8.3. Molecular Orbital Theory

8.3.1. The LCAO-MO Approximation 8.3.2.

The Hydrogen Molecular Ion, H2+

8.3.3. The Hydrogen Molecule

8.4. Valence Bond Theory

8.4.1. Hydrogen Molecule: Heitler-London Theory

8.4.2. The Shape of Polyatomic Molecules

8.4.3. Electronegativity

8.5. The Electronic Structure of Diatomic Molecules - MO Theory

8.6. Valence Bond Theory of π-electron Systems

8.7. Molecular Orbital Theory of π-electron Systems

8.8. Comparison of MO and VB Theories

9. Molecular Spectroscopy

9.1. Introduction

9.2. The Electromagnetic Radiation

9.3. The Width and Intensity of Spectral Transitions

9.4. Electronic Spectroscopy

9.5. Vibrational Spectroscopy

9.6. Rotational Spectroscopy

9.7. Vibrational-Rotational Spectra of Diatomic Molecules

9.8. Raman Spectroscopy

9.9. Electron-Spin Resonance

9.10. Nuclear Magnetic Resonance

Mode of delivery:

Lecture, Lecture-demonstration, assignment, inquiry, Laboratory, discussion methods and


Mode of assessment:



Text: H. Zewdie, Introductory Quantum Chemistry, AAU, A.A., 1999.




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.

17.5.4 Physical Chemistry IV (Statistical Thermodynamics and Surface Chemistry)

COURSE TITLE: PHYSICAL CHEMISTRY IV

(STATISTICAL THERMODY6AMICS A6D SURFACE CHEMISTRY)

COURSE CODE: CHEM432

CREDIT HOURS: 3



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:


• 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



1.11 Equilibrium Constants for Gas Phase Reactions

2. Physical Chemistry of Surfaces

2.1 Interfacial Structure

2.2 Surface Tension and Surface Free Energy

2.3 Methods of Surface Tension Measurement

2.4 Nature and Thermodynamics of Liquid-Gas Interface

2.5 The Surface Tension of Solutions

2.6 Surfaces of Solids

2.7 Absorption at the Solid Solution Interface

Mode of delivery: Lecture, Lecture- demonstration, assignment, inquiry, Laboratory, discussion methods and


Mode of assessment:



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.



1992.


1981.


17.5.5 Practical Physical Chemistry I

COURSE TITLE: PRACTICAL PHYSICAL CHEMISTRY I


CREDIT HOURS: 1

CO6TACT HOURS: 3 LAB.HR/WEEK

PREREQUISITE:

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



• Work with different instruments of analysis.

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)

Textbook: Practical Physical Chemistry I, D. Ohms and T. Solomon, AAU

17.5.6 Practical Physical Chemistry II

COURSE TITLE: PRACTICAL PHYSICAL CHEMISTRY II


CREDIT HOURS: 1

CO6TACT HOURS: 3 LAB. HR/ WEEK

PREREQUISITE: CHEM 334,

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.


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.

17.6 Applied chemistry section

17.6.1 Research Methodology and Scientific Writing

COURSE TITLE: RESEARCH METHODOLOGY A6D SCIE6TIFIC WRITI6G


CREDIT HOURS: 2


PREREQUISITE:

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.


To be designated at the commencement of the course.

17.6.2 Industrial Chemistry I

COURSE TITLE: I6DUSTRIAL CHEMISTRY I


CREDIT HOURS: 3



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



2.2. Dissolved solids, suspended solids, Hardness and alkalinity in water

2.3. Requisites of water for industries

2.4. Treatment of water by sedimentation, Filtration and membrane filtration (reverse

osmosis)

2.5. Water treatment by Ion-exchange Process and electro-dialysis

3. Hydrochloric, Hydrofluoric and Sulphuric acids

3.1. Methods of manufacture of hydrochloric acid and its uses

3.2. Industrial manufacture of hydrofluoric acid and its uses

3.3. Chamber process and contact process of manufacture of sulphuric acid and its handling

4. Common salts and the Chlor-alkali industry

4.1. Common salt and its resources

4.2. Chlor-alkali Industry – Introduction

4.3. Leblanc Process

4.4. Deacon Process

4.5. Electrolytic Processes

4.6. The Solvay process

5. Industrial derivatives of nitrogen

5.1. Cyanamide Process and Haber Process of Ammonia synthesis

5.2. Manufacture of Nitric acid and its uses

5.3. Manufacture of TNT, Nitrocellulose and Nitroglycerine

6. Fertilizers and Phosphoric acids

6.1. Chemistry of manufacture of phosphoric acid

6.2. Phosphoric acid series

6.3. Essential and trace elements for plant growth

6.4. Manufacture of nitrogenous fertilizers – calcium cyanamide, ammonium Nitrate and

urea

6.5. Potash Fertilizers

6.6. Manufacture of super phosphate and triple super phosphate fertilizers

7. Silicate Industry

7.1. Types of ceramics

7.2. Manufacture of structural clay products, white wares and stone wares

7.3. Glass and its properties

7.4. Manufacture of glass

7.5. Types of glasses

7.6. Classification of cement

7.7. Manufacture of Portland cement

7.8. Setting and hardening of Portland cement

8. Metallurgical Processes

8.1. Minerals and Ores

8.2. Concentration of ores

8.3. Roasting, calcination and smelting of ores

8.4. Refining of impure metal

8.5. Extraction of Iron and copper

9. High temperature materials

9.1. Refractories and their characteristics

9.2. Classification of refractories

9.3. Properties of refractories

9.4. Manufacture of refractories

9.5. Fire-Clay, Magnesite and Graphite bricks

10. Miscellaneous Products



10.1. Abrasives and their classification

10.2. Grinding wheels and abrasive paper

10.3. Dielectric materials and their characteristics

10.4. Thermal Insulators and their characteristics

10.5. Classification of thermal insulators and examples

Mode of delivery:

Lecture, group discussion, assignment in group or individually, home work,

Mode of assessment:

Quizzes, assignments, tests, mid-term and final examination


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.

17.6.3 Industrial Chemistry II

COURSE TITLE: I6DUSTRIAL CHEMISTRY II


CREDIT HOURS: 2

CO6TACT HOURS: 2 LEC. HRS/WEEK


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



1.8. Cracking, Alkylation, Hydrotreating and Reforming

2. Main Petrochemicals

2.1. Introduction to petrochemicals

2.2. Chemical conversions for manufacture of petrochemicals

2.3. Petrochemicals from Methane, Ethylene, Propylene, Butylenes and BTX

2.4. Manufacture of Acetylene, Ethylene oxide, Acrylonitile, Dimethyl terephthalate

3. Basic Organic Products

3.1. Introduction to Industrial organic synthesis

3.2. Manufacture of Methanol and Isopropanol

3.3. Manufacture of Formaldehyde and Acetaldehyde

3.4. Manufacture of Acetic acid

3.5. Manufacture of Acetone

3.6. Manufacture of Phenol and Styrene

4. Plastics, Rubber and Fibers

4.1. Introduction to polymers

4.2. Nomenclature of polymers

4.3. Addition and condensation polymerization

4.4. Methods of Polymerisation

4.5. Effect of polymer structure on properties

4.6. Plastics-Properties and classification

4.7. Moulding constituents of plastics

4.8. Moulding of plastics into articles

4.9. Preparation, properties and uses of PE, PVC and Bakelite

4.10. Rubber – properties

4.11. Natural and synthetic rubber

4.12. Natural and synthetic fibers

5. Chapter V Sucrose Industry

5.1. Manufacture of cane sugar

5.2. Manufacture of sucrose from Beet Root

5.3. Testing of sugar

6. Oils, Fats and Detergents

6.1. Introduction to oils and fats

6.2. Properties of oils and fats

6.3. Classification of oils

6.4. Manufacture of vegetable oils

6.5. Animal fats and oils

6.6. Analysis of oils and fats

6.7. Hydrogenation of oils

6.8. Manufacture of soap

6.9. Introduction to detergents

7. Paper Industry

7.1. Manufacture of pulp by mechanical and chemical process

7.2. Refining of pulp

7.3. Manufacture of paper

8. Chemical foodstuff processing

8.1. Introduction to fermentation

8.2. Alcohol Beverages

8.3. Manufacture of Beer, Spirit and wines.

9. Pharmaceuticals

9.1. Sulfonamide drugs



9.2. Antimalarial, antibacterial and antiviral agents

9.3. Antibiotics

10. Chemicals for agriculture

10.1. Introduction to Insecticides

10.2. DDT, BHC and Parathion

10.3. Fungicides – Baygon and 2,4,6-Trichloro Phenol

10.4. Herbicides–2,4-D and 2,4,5–T

10.5. Pesticides pollution

11. Dyestuff

11.1. Introduction to dyes

11.2. Colour and constitution

11.3. Methods of dyeing

11.4. Classification of dyes

12. Leather Industry

12.1. Animals skin

12.2. Preparation of skin for tanning

12.3. Vegetable tanning

12.4. Chrome tanning

12.5. Leather finishing

Mode of delivery:

Lecture, group discussion, assignment in group or individually.

Mode of assessment:



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


CREDIT HOURS: 3



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:


• 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)



4.6. Regulation of Enzyme activity (Activation/Inhibition)

5. Lipids

5.1. Definition of lipids

5.2. Fatty acids (saturated and unsaturated)

5.3. Triacylglycerols

5.4. Steroids and other lipids

5.5. Biological membranes

5.6. Membrane transports

6. Carbohydrates

6.1 Definition and Classification,

6.2 Monosaccharides

6.3 Disaccharides

6.4 Polysaccharides

7. Introduction to Metabolism

7.1 Metabolic Pathways

7.2 Bioenergetics

7.3 Regulations

8. Carbohydrate Metabolism

8.1 Structure of Carbohydrate

8.1.1 Overview

8.1.2 Digestion of Carbohydrate

8.2 Glycogen Metabolism/Starch

8.2.1 Overview

8.2.2 Degradation of Glycogen

8.3 Metabolism of Monosaccharides and Disaccharides (Overview)

8.4 Glycolysis

8.4.1. Fates of Pyruvate

8.4.2. Energy yield of Glycolysis

8.5 Citric Acid Cycle

8.6 Electron Transport Chain and Oxidative Phosphorylation

8.7 Hexose Monophosphate Pathway (Pentose Phosphate pathway)

8.7.1 Overview

8.7.2 NADPH/Pentose

8.8 Gluconeogenesis

8.8.1. Overview

8.8.2. Reactions Unique to Gluconeogenesis

8.8.3. Substrates for Gluconeogenesis

8.8.4. Regulations of Gluconeogenesis

9. Lipid Metabolism

9.1 Introduction

9.2 Metabolism of Dietary Lipids

9.2.1 Overview

9.2.2 Digestion, Absorption, Secretion, and Use of Dietary Lipids

9.3 Fatty Acid and Triacylglycerol Metabolism

9.4 Mobilization of Stored Fats and Oxidation of Fatty Acids

9.5 Phospholipid Metabolism

10. Amino Acids/Nitrogen Metabolism

10.1 Nitrogen Fixation and Synthesis of Amino Acids

10.1.2 Digestion of Dietary Proteins

10.1.3 Removal of Nitrogen from Amino Acids



10.1.4 Urea Cycle: The Major Pathway of Disposal of Nitrogen

10.2 Amino Acids: Metabolism of Carbon Atoms

10.1.1 Catabolism of the Carbon Skeletons of Amino Acids

10.1.2 Biosynthesis of Nonessential Amino Acids

10.3 Conversion of Amino Acids to Specialized Products: An overview

11: Integration of Metabolism

11.1 Metabolic Effects of Insulin and Glucagon

11.1.1 Overview

11.1.2. Insulin

11.1.3 Glucagon

11.2 Starvation and fasting; similarity and differences

11.3 Nutrition

11.4 Vitamins

12: Nucleic Acid Structure and Function

12.1 Structure of DNA and RNA

12.2 DNA Synthesis (Overview) (Replication)

12.3 RNA Synthesis

12.3.1 Overview

12.3.2 Transcription

12.4 Protein Synthesis

12.4.1 The Genetic Code

12.4.2 Translation

Mode of delivery:

Lecture, group discussion, assignment in group or individually

Mode of assessment:


Text: P.C. Champe; R.A. Harvey, Biochemistry, 4th Ed., Lippincott

,s Illustrated Reviews, 2007.


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.

17.6.5 Environmental Chemistry and Toxicology

COURSE TITLE: E6VIRO6ME6TAL CHEMISTRY A6D TOXICOLOGY


CREDIT HOURS: 3



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



5.3. Agricultural and pharmaceutical contaminants

5.4. Pesticides

5.5. PCB’s(polychlorinated biphenyls)

5.6. Nitrogen and phosphorous compounds

5.7. Toxic heavy metals and organo-metallic compounds

5.7.1. mercury

5.7.2. lead

5.7.3. arsenic

5.7.4. Chromium

6. Green chemistry

6.1. Introduction

6.2. The concept of Atom Economy

6.3. Design and application of surfactants for carbon dioxide

6.4. Designing an environmentally safe marine synthetic antifoulant

Mode of delivery:

Lecture, field trip, individual study and group assignment.

Mode of assessment:

Field trip report; term paper mid and final exams.


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.

17.6.6 Senior Student Project

COURSE TITLE: SE6IOR STUDE6T PROJECT


CREDIT HOURS: 3

CO6TACT HOURS:

PREREQUISITE:

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.




Any nationally and internationally accredited journals or scientific findings.

17.7 Courses for non-chemistry majors

17.7.1 Fundamentals of Inorganic Chemistry

COURSE TITLE: FU6DAME6TALS OF I6ORGA6IC CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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:


• 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



2.2. Close packing

2.3. Classification of ionic structures (AX, AX2)

3. Acid-base theories and the solvent system

4. Atomic structure

4.1. Atomic spectra of hydrogen

4.2. Atomic model (Bohr model of the atom)

4.3. Bohr theory

4.4. Quantum numbers

5. Chemical bonding and structure

5.1. Introduction to bonding

5.1.1. Purpose of bond formation

5.1.2. Types of bonds

5.1.2.1. The ionic bond

5.1.2.2. The covalent bonds

5.1.2.2.1. Lewis theory

5.1.2.2.2. Sidwick-Powell theory

5.1.2.2.3. Valence shell electron pair repulsion (VSEPR) theory

5.1.2.2.4. Valence bond theory

5.1.2.2.5. Molecular orbital theory

5.1.2.2.5.1. LCAO method

5.1.2.2.5.2. Rules for LCAOs

5.1.2.2.5.3. MO treatment for homonuclear & heteronuclear diatomic

molecules

5.1.2.3. The metallic bond

5.1.2.3.1. General properties of metals

5.1.2.3.2. Metallic bonding

6. Chemistry of main group elements

6.1. Chemistry of hydrogen

6.2. General properties of the elements

6.2.1. Size, Ionization energies, Electronaffinity, Electronegativity, Polarizing power

6.2.2. Polarizability-Fajan’s rule, Metallic character, Variable valency

6.2.3. Diagonal relation ships in the periodic table

6.3. Descriptive chemistry of representative elements

6.3.1. S-block elements

6.3.2. P-block elements

7. The Chemistry of transition elements

7.1. Physical and chemical properties

7.2. Size, Melting & boiling point, Ionization energy, Oxidation state, Color, Magnetic

property, Catalytic property, Ability to form compounds

7.3. Bonding in transition metal complexes

7.3.1. Crystal field theory (CFT)

7.3.2. Octahedral complexes

7.3.3. Tetrahedral complexes

7.3.4. Color of transition metal compounds

7.3.5. Nomenclature of coordination compounds

7.3.6. Isomerism

7.4. Descriptive chemistry selected transition elements

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.


1. J.D. Lee, A new concise inorganic chemistry, 3rd or 5

th 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,

17.7.2 Fundamentals of Organic Chemistry

COURSE TITLE: FU6DAME6TALS OF ORGA6IC CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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:


� 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



6.3.1. Markovnikov Rule

6.3.2. Michael Addition

6.3.3. Radical addition

6.4. Applications of Addition Reactions

6.4.1. Addition of halogen

6.4.2. Addition of hydrogen halide

6.4.3. Addition of hypohalous acids

6.4.4. Hydration of alkenes

6.4.5. Hydroboration

6.4.6. Diels-Alder addition

6.4.6.1. Kinetic versus Thermodynamic control of the Diels-Alder reaction

6.4.6.2. Stereochemistry of the Diels-Alder reaction

6.5. Catalytic hydrogenation

6.5.1. Ozonization

6.5.2. Peracid oxidation

6.5.3. Glycol formation

7. Aromatic substitution reactions

7.1. Introduction

7.2. Aromaticity

7.3. Aromatic substitution

7.4. Directing effects

7.5. Application of electrohilic substitutions

7.5.1. Halogenation

7.5.2. Sulfonation

7.5.3. Nitration

7.5.4. Friedel-Crafts Alkylation

7.5.5. Friedel-Crafts Acylation

7.5.6. Diazotization of Amines

7.5.7. Reactions of aromatic side chains

8. Carbonyl reactions

8.1. Carbonyl addition

8.2. Addition Elimination

8.3. Enolization-Ketonization

8.4. Application of Addition reactions

8.4.1. Hydrate formation

8.4.2. Hemiacetals and Hemiketals

8.4.3. Cyanohydrins

8.4.4. Carbinolamines

8.4.5. Addition of Grignard reagents

8.4.6. Addition of hydrogen

8.4.7. Lithiumaluminiumhydride and sodiumborohydride

8.5. Applications of addition-elimination reactions

8.5.1. Imines and related compounds

8.5.2. Wittig reaction

8.5.3. Acetal formation in acid media

8.5.4. Acids and their derivatives

8.5.5. Ester hydrolysis and formation in acid media

8.5.6. Acid chlorides

8.5.7. Acid anhydrides

8.5.8. Reduction of acid derivatives



8.6. Application of enolization-Ketonization reactions

8.6.1. Halogenation

8.6.2. Alkylation

8.6.3. Aldol condensation

8.6.4. Claisen-Schmidt condensation

8.6.5. Mannich condensation

8.6.6. Perkin condensation

8.6.7. Claisen condensation

9. Rearrangement Reactions

9.1. Rearrangement to an electro-deficient carbon

9.2. Rearrangement to electron-deficient oxygen

9.3. Rearrangement to electron-deficient Nitrogen

10. Oxidation-reduction reaction

10.1. Introduction

10.2. Oxidation Reaction

10.3. Alcohols and Aldehydes

11. Reduction reactions

11.1. Catalytic Hydrogenation

11.2. Chemical Reduction

11.3. Dissolving metal reductions

11.4. Acyloin condensation

12. Biological molecules

12.1. Glucose: An introduction to carbohydrate chemistry

12.2. Disaccharides and polysaccharides

12.3. Amino-acids, peptides, and proteins

12.3.1. The structure and properties of alpha-amino acids

12.3.2. Analysis of alpha-amino acids

12.3.3. Synthesis of alpha-amino acids

12.4. Peptides and proteins

12.5. Peptide synthesis

12.6. Introduction to Chemistry of Lipids

12.7. Introduction to Chemistry of Nucleic Acids

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.


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.



17.7.3 Fundamentals of Physical Chemistry

COURSE TITLE: FU6DAME6TALS OF PHYSICAL CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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:


• 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



2.2. The equilibrium stage

2.3. Thermodynamics and chemical equilibrium

2.4. The relation ship between equilibrium constants

2.5. Heterogeneous Equilibria

2.6. LeChateler’s principle and its applications

2.7. Equilibrium calculations

3. The Phase Rule

3.1. Phase-components-degrees of freedom

3.2. Derivation of the phase rule

3.3. One component systems

3.4. Phase diagrams

3.5. Polymorphism

3.6. Experimental determination of transition point

3.7. The water system

3.8. Two component systems

3.9. Three component systems

3.10. Phase transitions

4. Theory of Dilute Solutions

4.1. Colligative properties

4.2. Lowering of vapor pressure( Raoult's Law)

4.3. Derivation of Raoult's law

4.4. Determination of molecular mass from vapor pressure lowering

4.5. Measurement of lowering of vapor pressure

4.6. Boiling point elevation

4.7. Determination of boiling point elevation

4.8. Freezing point depression

4.9. Experimental determination of freezing point depression

4.10. Osmotic pressure

4.11. Colligative properties of electrolytes

4.12. Concept of activity and activity coefficient

5. Thermodynamics

5.1. Basic concepts of thermodynamics

5.2. Thermodynamic process

5.3. Nature of heat, work and energy

5.4. Internal energy

5.5. First law of thermodynamics

5.6. Enthalpy of a reaction

5.7. Applications of first law of thermodynamics

5.8. Process in nature

5.9. Entropy

5.10. Second law of thermodynamics

5.11. Combined form of first and second laws

5.12. Third law of thermodynamics

6. Electrochemistry

6.1. Introductory terms

6.2. Migration of ions

6.3. Relative speed of ions

6.4. Transport number

6.5. Determination of transport number

6.6. Determination of pH from EMF method



6.7. Classification of electrolytic cells

6.8. Galvanic cells

6.9. Determination of standard electrode potential

6.10. Reversible electrodes

6.11. Measurement of EMF of the cell

6.12. Construction of normal hydrogen electrode

6.13. Electrochemical series

6.14. Some commercial cells or batteries

7. Chemical Kinetics

7.1. Introductory terms

7.2. Derivation of integrated rate reactions

7.3. Units of rate constant

7.4. Half life of a reaction

7.5. Factors that influence the rate of reaction

7.6. Determination of order of a reaction

7.7. Examples of first, second and third order reactions

7.8. Analysis of kinetic results

7.9. Kinetics of ionic reactions

7.10. Pseudo order reactions

7.11. Theories of chemical kinetics

7.12. Catalysis

8. Elementary Quantum Chemistry

8.1. Introduction

8.2. Failure of classical mechanics

8.3. De-Broglie's concept of the dual nature of electron

8.3.1. Derivation of De-Broglie’s equation

8.3.2. Proof of De-Broglie’s equation

8.3.3. De-Broglie’s concept and Bohr’s theory

8.3.4. Experimental proof of De-Broglie’s concept

8.4. Heisenberg's uncertainty principle

8.4.1. Experimental proof of uncertainty principle

8.4.2. Applications of uncertainty principle

8.4.3. Limitations of uncertainty principle

8.5. Schrödinger’s wave equations

8.6. Derivation of Schrodinger’s equation

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.


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.

6. P.W. Atkins, Molecular Quantum Mechanics, Oxford University Press, Oxford

1997.

7. A.K. Chandra Introductory Quantum Chemistry, Tata McGraw-Hill, 1979.

8. I.N. Levin, Quantum Chemistry, Ally Bacon Inc., 1974.

9. D.A. McQuarrie, Quantum Chemistry, University Science Books, 1983.

17.7.4. Fundamentals of Analytical Chemistry

COURSE TITLE: FU6DAME6TALS OF A6ALYTICAL CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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



2.3.3 Factors affecting stability of complexes

2.3.4 Effect of complexation on solubility

2.4 Oxidation-reduction equilibria

2.4.1 Redox reactions, reducing and oxidizing agents

2.4.2 Redox reactions in electrochemical cells and electrode potential

2.4.3 Dependence of electrode potential on concentration

2.4.4 Calculating equilibrium constant from electrode potential

3. Statistical evaluation of analytical data

3.1 Mean, Standard deviation, Variance

3.2 Accuracy and precision of measurements

3.3 Errors in analytical results

3.4 Confidence limit

3.5 Testing for significance (t-test and F-test)

3.6 Rejection test (Q-test)

4. Solutions and their concentrations

4.1 Types of solutions

4.2 Different ways of expressing concentration

4.3 Preparation of solutions

4.4 Activity and activity coefficient

5. Titrimetric methods of analysis

5.1 Fundamentals of titrimetry

5.1.1 Definition of terms

5.1.2 Ideal requirements for standard solutions

5.1.3 Volumetric calculations

5.2 Acid-base titration

5.2.1 Acid-base titration curves

5.2.2 Acid-base indicators

5.3 Precipitation titration

5.3.1 Titration curves


5.4 Complexometric titration

5.4.1 Titration with aminopolycarboxylic acids (EDTA and its species)

5.4.2 EDTA titration curve


5.5 Redox titration

5.5.1 Derivation of redox titration curves

5.5.2 Oxidation-reduction indicators

6. Gravimetric analysis

6.1 Principle and types of gravimetric analysis

6.2 Properties of precipitates and precipitating agents

6.3 Steps in gravimetric analysis

6.4 Gravimetric calculations

7. Introduction to chromatographic separation

7.1 Historical background

7.2 Types of chromatography

7.3 Paper chromatography

7.4 Thin layer chromatography

7.5 Column chromatography

7.6 Efficiency of separation

7.7 Application (Qualitative and quantitative information)



8. Gas Chromatography (GC)

8.1 Principle of GC

8.2 Instruments for GC

8.3 Applications

9. High-performance Liquid Chromatography (HPLC)

9.1 Principle of HPLC

9.2 Instruments for HPLC

9.3 Parts of liquid (liquid) Chromatograph

9.4 Liquid (partition) chromatography

9.5 Liquid – solid (Adsorption) chromatography

9.6 Ion-exchange chromatography

9.7 Molecular exclusion chromatography

10. Introduction to Electro-analytical Chemistry

10.1 Potentiometry

10.2 Voltammetry

10.3 Coulometry and Electrogravimetric Analysis

10.4 Conductometry

11. Introduction to Spectroscopy

11.1 Electromagnetic Radiation and its interaction with matter

11.2 Absorption Laws (Quantitative Analysis)

11.4 Instruments for optical spectroscopy

11.5 Atomic Absorption and emission spectroscopy

11.6 Ultraviolet and Visible (UV-Vis) Spectroscopy

11.7 Infrared Spectroscopy

11.8 Nuclear Magnetic Resonance Spectroscopy (NMR)

Mode of delivery:

Lecture, Lecture demonstration, Assignment, Discussion, inquiry, project methods and

questioning technique

Mode of assessment:



1. Skoog, D.A.; West, D.M.; Holler, F.J. Fundamentals of Analytical Chemistry, 7th ed.;


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


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


7. Marmet, J.M.; Otto, M.; Widmer, H.M. (editors). Analytical chemistry, Wiley-VCH,

Weinheim,1998



17.8. Elective courses

17.8.4 Chemical Instrumentation

COURSE TITLE: CHEMICAL I6STRUME6TATIO6


COURSE CREDITS: 3


PREREQUISITE:

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



The i-v characteristics of diode

2.4.2. Transistors

Field effect transistors

Bipolar junction transistors

NPN and PNP transistors

Transistors as amplifier

Bipolar junction and field effect transistor amplifier characteristics

2.5 Operational amplification in chemical instrumentation-Properities of operational

amplification

2.1.1 Circuits employing operational amplifiers

Feedback circuits

Voltage Followers circuits

2.6 Amplification and measurement of transuded signals

2.6.1. Current measurement

2.6.2 Potential measurement

2.6.3 Resistance measurement

2.6.4 Comparison of Transducer outputs

2.7. Operational amplifiers to voltage and current control

2.8 Application of operational amplifiers to mathematical operations

2.8.1 Multiplication or division by a constant

2.8.2 Summing and difference amplifiers

2.8.3 Integrators and differentiators

3. Analog and Digital electronics

3.1 basic analogue and digital electronics

3.1.1 Analog Vs digital electronics

3.1.2 Analog signal components and circuits

3.1.3 Digital signal components and circuits

3.1.4 Relative advantage of Analog and Digital systems

3.2 Digital basics

3.2.1 Counting with binary and decimal numbers

3.2.2 Binary to decimal and Decimal to binary conversion

3.2.3 Binary codes

3.3 Basic digital circuit components

3.3.1 Signal shapers

3.3.2 Binary counters

3.3.3 Binary coded Decimal systems

3.3.4 Scalar

3.3.5 Clocks

4. Input transducers and data acquisition

1.1 Transducers

1.1.1 Input Transducers

1.1.2 Output Transducers

1.2 Data acquisition

1.2.1 Data acquisition system

1.2.2 Signal conditioning

1.2.3 Analog and digital signal conversion

1.2.4 Analog to digital conversion

1.2.5 Digital to Analog converters

1.2.6 Analog to digital converters

5. Computers in Instrumentation



5.1 Introduction to Microprocessors and Microcomputers

5.1.1 Computer Terminology

5.1.2 Hardware and Software

5.2 Operational modes of computerized instruments

5.3 Components computer

5.4 Application of computers

5.4.1 Active application

5.4.2 Passive application

6. Process instruments, automatic and automated method of analysis

6.1 Automatic instruments and automation

6.2 Flow injection analysis

6.3 Discrete automated system

6.4 Optical instruments-basics and components

Mode of delivery:


questioning technique

Mode of assessment:


17.8.5 Clinical Chemistry

COURSE TITLE: CLI6ICAL CHEMISTRY


CREDIT HOURS: 3

CO6TACT HOURS: 2 LEC. HR + 1 LAB. HR/ WEEK

PRE REQUISITE:

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



• Describe the principles of electrophoresis, chromatography refractometry fluorometry

turbidimetery and nephelometry

• State the type of specimens that can be analyzed in a clinical chemistry laboratory, collect

process and preserve specimens and list the factors that affect test results

• Explain the biochemistry and metabolism of carbohydrates,

• Discuss diabetes mellitus and hypoglycemia describes and performs the laboratory tests

for the measurement of glucose

• Explain the biochemistry and metabolism of amino acids and proteins

• Describe the principles of the methods and perform the laboratory tests for the analysis of

amino acids and proteins

• Explain functions of electrolytes discuss electrolytes and water balance electrolytes and

acid base balance describe and perform the laboratory tests for the measurement of

electrolytes and blood gases.

• Discuss quality assurance in clinical chemistry

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



5.9. Glycated Proteins

5.10. In born errors of Carbohydrate Metabolism

5.11. Glycogen Storage Disease

6. Amino Acides and Proteins

6.1. Basic Biochemistry of Amino Acids

6.2. The Amino Acidurias

6.3. Disorders of Amino Acid Metabolism

6.4. Analysis of Amino Acids

6.5. Basic Biochemistry of Proteins

6.6. Plasma Proteins, Complement Proteins and Immunoglobulin

6.7. Methods of Assessing the Plasma Proteins

6.8. Total Protein Determination

6.9. Assay Techniques for Albumin

6.10. Determination of Total Globulin

6.11. The Albumin to Globulin Ratio

7. Electrolyte and Blood Gases

7.1. Function of Electrolytes

7.2. Electrolytes and Water Balance

7.3. Condition of Fluid imbalance

7.4. Edema

7.5. Electrolytes and Acid-Base Balance

8. Quality Assurance in Clinical Chemistry

8.1. Introduction

8.2. Pre analytical stage

8.3. Analytical stage

8.4. Post analytical stage

9. Laboratory Practical Sessions

9.1. Lab 1: Preparation of standard solutions

9.2. Lab 2: Preparation of buffer solutions

9.3. Lab 3: Preparation of stock/working reagents

9.4. Lab 4: Instrument set up, calibration and selection of proper ware length for a given

analyte

9.5. Lab 5: Specimen collection, handling and processing

9.6. Lab. 6: Measurement of glucose

9.7. Lab 7: Analysis of amino acids and proteins

9.8. Lab. 8: Measurement of electrolytes in synthesis

Mode of delivery:


questioning technique, laboratory practicals

Mode of assessment:


17.8.6 Medicinal Chemistry

COURSE TITLE: MEDICI6AL CHEMISTRY


CREDIT HOURS: 3





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.

17.8.7 Polymer Chemistry

COURSE TITLE: POLYMER CHEMISTRY


CREDIT HOURS: 2



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



3.4. Free radical copolymerisation–Reactivity ratios

3.5. Kinetics of Ionic Polymerisation

4. Characterisation of polymers

4.1. Number and weight average molecular weights

4.2. Absolute and secondary methods of determination of molecular weights

4.3. Morphology of polymers

4.4. Glass transition temperature

4.5. Degree of crystallinity

5. Fabrication of polymers

5.1. Preparation of polymer films

5.2. Production of fibres

5.3. Foaming

5.4. Reinforced polymers

5.5. Polymer surface coatings

6. Testing of polymers

6.1. Mechanical tests

6.2. Tests for thermal properties

6.3. Electrical tests

6.4. Miscellaneous tests

7. Molecular structure, properties and uses of polymers

7.1. Influence of macromolecule skeleton

7.2. Influence of side groups

7.3. Electro active polymers

7.4. Electro–optical polymers

7.5. Biomedical applications of polymers

8. Polymer degradation and environment

8.1. Polymer degradation and stability

8.1.1. Thermal degradation

8.1.2. Oxidative and UV stability

8.1.3. Chemical and hydrolytic stability

8.1.4. Effects of radiation

8.2. Management of plastics for better environment

8.2.1. Recycling

8.2.2. Incineration

8.2.3. Biodegradation

9. Biological polymers and their reactions

9.1. Polysaccharides

9.1.1. General composition

9.1.2. Biological synthesis of polysaccharides and their reactions

9.2. Proteins


9.2.2. Types of proteins and their functions

9.2.3. Biological synthesis of proteins and their reactions

9.3. Polynucleotides


9.3.2. Synthesis and reactions of polynucleotides


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.



17.8.8 Food Chemistry

COURSE TITLE: FOOD CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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.

17.8.9 Agricultural chemistry

COURSE TITLE: AGRICULTURAL CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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



3.4. Precipitation reactions

3.5. Colloidal chemistry of soil constituents

4. Pesticides

4.1. Insecticides

4.2. Fongicides

4.3. Herbicides

4.4. Novel methods of insect control

4.5. Pesticides in the environment

5. Fertilisers

5.1. Plant nutrients

5.2. Functions of nutrients

5.3. Need for fertilisers

5.4. Nitrogenous fertilizers

5.5. Phosphate fertilizers

5.6. Potassium fertilisers

5.7. Mixed fertilizers

5.8. Fertilisers and the environment


1. P. Meenakshi, Elements of Environmental science and engineering, 2005.

2. A.K. De, Environmental Chemistry, 5th Ed., 2005.

17.8.10 Physical Inorganic Chemistry

COURSE TITLE: PHYSICAL I6ORGA6IC CHEMISTRY


CREDIT HOURS: 3


PREREQUISITE:

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



1.6 Structure of Ionic Crystals

1.6.1 Ionic crystal of AX type (ZnS, NaCl, CsCl)

1.6.2 Ionic crystal of AX2 type (CaF2, TiO2, SiO2)

1.6.3 Layer structure (CdI2, CdCl2)

1.7 Defects in solids and its Applications

2 Nuclear Chemistry

2.1 Structure of Nucleus

2.1.1 Liquid Drop Model & Shell Model

2.2 Forces in the nucleus (Nuclear forces)

2.2.1 Binding energy of the nuclei and its stability

2.2.3 Mass defect

2.3 Modes of decay i.e. α, β, γ etc

2.4 Half life period

2.5 Radioactivity

2.5.1 Radioactivity displacement law and Radioactivity decay series

2.5.2 Rate of radioactivity disintegration, nature of radiation emitted, there

detection and measurements

2.6 Nuclear Reactions

3 Introduction to Group Theory

3.1 Symmetry elements

3.2 Symmetry operations

3.3 Point groups

3.4 Mathematical representation of symmetry operations

3.5 Character tables

4. Chemical Application of Group Theory

4.1 Vibrational spectroscopy

4.2 Electronic spectroscopy

4.3 Molecular orbital theory


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

17.8.11 Industrial Safety and Quality Control

COURSE TITLE: I6DUSTRIAL SAFETY A6D QUALITY CO6TROL


CREDIT HOURS: 2

CO6TACT HOURS: 2 HOURS PER WEEK


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.


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.

17.8.12 Biochemistry and molecular biology

COURSE TITLE: BIOCHEMISTRY A6D MOLECULAR BIOLOGY

COURSE CODE CHEM457

CREDIT HOURS 3


PRE-REQUISITE CHEM 452

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.

17.9 Supportive Courses

17.9.1 Calculus I for Chemists

COURSE TITLE: CALCULUS I FOR CHEMISTS

COURSE CODE: MATHS 233

CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC HR + 2 TUT HR/WEEK

PREREQUISITE:

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

Text: R. Ellis, Calculus with Analytic Geometry, 5th Ed., 1993.



17.9.2 Calculus II for Chemists

COURSE TITLE: CALCULUS II FOR CHEMISTS

COURSE CODE: MATH 234

CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC HR + 2 TUT HR/WEEK

PREREQUISITE: MATH 233

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



4.4 Directional derivatives and gradient

4.5 Total differential and tangent planes

4.6 Applications: error estimation, tangent plane approximation of values of a

function

4.7 The chain rule, implicit differentiation

4.8 Relative extrema of functions of two variables

4.9 Largest and smallest values of a function on a given set

4.10 Extreme values under constraint conditions: Language’s multiplier

5. Multiple Integrals

5.1 Double integrals and their evaluation by iterated integrals

5.2 Double integrals in polar coordinates

5.3 Application: Area, center of mass of plane region, surface area

5.4 Multiple integrals in cylindrical and spherical coordinate

5.5 Multiple integrals in cylindrical and spherical coordinate

5.6 Application: Volume, center of mass of solid region

6. Partial Differential Equations

6.1 Int. to Partial Differential Equations

6.2 Finding solutions of PDE containing only partials of one variable.

6.3 Classification of PDE in terms of order, degree, hom. and non hom. constant and

variable coefficient

6.4 Linear First Order Homogenous PDE with constant coeff.

6.5 Classification of second Order Linear Homogeneous PDE with constant coeff.

6.6 Finding Gen. solutions of Euler’s Equations with constant coeff. (Hyperbolic,

parabolic and Elliptic Equations)

7. Special Functions

7.1 Spherical Harmonics

7.2 Legendre Transformatiom

7.2 Laugre Functions

7.3 Laplace Functions

7.4 Fourier Transformations

Text: R. Ellis, Calculus with Analytic Geometry, 5th Ed., 1993.

17.9.3 Introduction to Statistics

COURSE TITLE: I6TRODUCTIO6 TO STATISTICS

COURSE CODE: STAT 273

CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC. HR + 2 TUT. HR/WEEK

PREREQUISITE:

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



2.2.1.7.Cumulative frequency distribution (less than and more than)

2.3. Graphic and Diagrammatic presentation of data

2.3.1. Graphical presentation: Histogram, Frequency polygon, Cumulative frequency

curves (ogives), vertical line graph and line graph

2.3.2. Diagrammatical presentation: Bar charts (simple, component, multiple and

percentage), pie chart and pictogram.

3. Measures of central Tendency

3.1. Summation notation and properties of summation notation.

3.2. Definition and purpose (objective) of average

3.3. Mathematical Measures of central tendency

3.3.1. Arithmetic Mean

3.3.1.1.Simple Arithmetic Mean (for ungrouped and grouped data

3.3.1.2.Mathematical properties of Arithmetic Mean

3.3.1.3.Merits and Demerits of Arithmetic Mean

3.3.1.4.Weighted Arithmetic Mean

3.3.1.5.Combined mean

3.3.1.6.Geometric mean (for ungrouped and grouped data)

3.3.1.7.Harmonic mean (for ungrouped and grouped data)

3.3.1.8.Relationship among Arithmetic Mean, G.M, and H.M.

3.4. Positional measure of Central Tendency

3.4.1. The Median: Merits and Demerits of Median

3.4.2. The Quartiles or fractiles: Quartiles, Deciles and Percentiles

3.5. The Mode: Merits and Demerits of Mode

3.6. Empirical relationship among mean, Median and Mode.

4. Measures of depression and (Variation)

4.1. Definition and purpose of variation

4.2. Types of measures of variation

4.2.1. Absolute and relative measures of dispersion

4.2.2. Range and coefficient of range

4.2.3. Inter quartile range, quartile deviation and coefficient of quartile

4.2.4. Mathematical Measures of Dispersion

4.2.4.1.Mean (average) Deviation (about the mean and the medium)

4.2.4.2.Variance and Standard deviation

4.2.4.2.1. Coefficient of variation

4.2.4.2.2. Standard score (Z-score)

5. Simple Linear regression and Correlation

5.1. Regression

5.1.1. Definition

5.1.2. Fitting linear regression by least squares method

5.1.2.1.Regression equation of Y on X and X on Y

5.1.2.2.Prediction

5.2. Correlation

5.2.1. Definition

5.2.2. Measuring simple linear correlation coefficient

5.2.3. Measuring rank correlation coefficient, covariance and variances

6. Elementary Probability

6.1. Definitions and concepts: Random experiment, sample space, sample points, exhaustive

cases, etc

6.2. Counting Techniques

6.2.1. Multiplication principle (Fundamental of principle of counting)



6.2.2. Permutation and combination

6.3. Definition of probability, Classical (Mathematical) approach

6.3.1. Addition rule of probability

6.3.2. Conditional of probability

6.3.3. Multiplication rule of probability

6.3.4. Independent Events

6.3.5. Baye’s Theorem

7. Probability Distribution

7.1. Random variables: Definition and types of random variable

7.2. Probability Distribution of random variables

7.3. Distribution Function or Cumulative Distribution functions of random variables.

7.4. Expectation and variance of random variables

7.5. Some common probability distributions: Binomial, Poisson and Normal distributions

8. Sampling and Sampling Distributions

8.1. The Concept of Sampling

8.2. Reasons for Sampling

8.3. Sampling Techniques

8.3.1. Random (probabilistic) Sampling techniques: Simple random sampling

(SRSWOR and SRSWR), stratified random sampling, systematic random sampling,

cluster random sampling, Multistage cluster sampling

8.3.2. Non-random (Non-probabilities) sampling techniques: Judgment, Quota and

convenience sampling

8.3.3. Sampling Distribution

8.3.3.1.Sampling distribution of the Mean

8.3.3.2.Mean and standard deviation of the sampling distribution of the mean

9. Statistical estimation and hypothesis testing

9.1. The concept of estimation

9.2. Estimator and Estimates

9.3. Properties of best estimator

9.4. Point estimation: Point estimation of the population mean

9.5. Interval estimation: Confidence interval for the population mean (consider the three

cases

9.6. Hypothesis testing

9.6.1. Basic concepts of hypothesis testing: Statistical decisions, hypothesis and types of

hypothesis, test statistic, types of errors, and types of testes

9.6.2. Tests about population mean

9.6.3. Tests about the equality of two population mean

9.6.4. Goodness of fit test

9.6.5. Test of homogeneity

Mode of assessment:

Tests, Group assignment, Mid-semester Exam., Final exam.


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.

17.9.4 Mechanics and Heat for chemists

COURSE TITLE: MECHA6ICS A6D HEAT FOR CHEMISTS

COURSE CODE: PHYS 205

CREDIT HOURS: 3


PREREQUISITE:

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



3.2. Friction Force

3.3. Application of Newton’s Laws

3.4. Velocity dependent forces

4. Work and Energy (10 hrs)

4.1. Work done by constant and variable forces

4.2. The work energy theorem

4.3. Conservative and non-conservative forces, conservative force and potential energy

4.4. Conservation of mechanical energy

4.5. Power

5. Dynamics of System of Particles (9 hrs.)

5.1. Linear Momentum and Impulse

5.2. Conservation of Momentum

5.3. System of particles

5.4. Center of mass

5.5. Center of mass of a rigid body

5.6. Motion of system of particles

5.7. Elastic and Inelastic Collision (1-D & 2-D)

5.8. Elastic collisions in one-dimension

5.9. Two-dimensional elastic collisions

5.10. Inelastic collisions

5.11. Systems of variable mass

6. Rotation of Rigid Bodies (6 hrs)

6.1. Rotational motion with constant and variable angular accelerations

6.2. Rotational kinetic energy

6.3. Moment of inertia

6.4. Rotational dynamics

6.5. Torque and angular momentum

6.6. Work and Power in Rotational Motion

6.7. Conservation of Angular Momentum

6.8. Relation between linear and angular motions

7. Simple Harmonic Motion (3 hrs)

7.1. Energy in Simple Harmonic Motion

7.2. Equations of Simple Harmonic Motion

7.3. Pendulum

7.4. Damped and forced oscillations

7.5. Resonance

8. Heat and Thermodynamics (10 hrs)

8.1. Temperature, Zeroth law of thermodynamics

8.2. Heat, work, and Internal energy of a thermodynamic system

8.3. The first law of thermodynamics, and its consequences

8.4. The second law of thermodynamics, Carnot’s engine

8.5. Entropy, the third law of thermodynamics, Kinetic theory of gases

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%



• Two Tests (40%)

• Mid-semester and Semester final tests (40%)

Text: R. A. Serway, Physics for Scientists & Engineers, 6th Ed., 2004.


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.

17.9.5 Electricity and Magnetism for chemists II

COURSE TITLE: ELECTRICITY A6D MAG6ETISM FOR CHEMISTS II

COURSE CODE: PHYS 206

CREDIT HOURS: 3


PREREQUISITE: PHYS 205

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



1.4. Electric dipole

1.5. Electric field due to continuous charge distribution

1.6. Motion of charged particles in electric field

1.7. Gauss’ Law

2. Electric Potential (3 hrs.)

2.1. Electric potential energy

2.2. Electric potential due to point charges

2.3. Electric potential due to continuous charge distribution

2.4. Relations between potential and electric field

2.5. Equi-potential surfaces

3. Capacitance and Dielectrics (3 hrs.)

3.1. Capacitance

3.2. Combination of capacitors

3.3. Capacitors with dielectrics

3.4. Electric dipole in an external field

3.5. Electric field energy

4. Direct Current Circuits (3 hrs.)

4.1. Electric current and current density

4.2. Resistance and Ohm’s law

4.3. Resistivity of conductors

4.4. Electrical energy, work and power

4.5. Electromotive force

4.6. Combinations of Resistors

4.7. Kirchhoff’s Rules

4.8. RC Circuits

5. Magnetic Force (2 hrs)

5.1. Properties of magnetic field

5.2. Magnetic force on a current carrying conductor

5.3. Torque on a current loop in uniform magnetic field

5.4. Motion of charged particles in magnetic field

5.5. Hall Effect

6. Calculation of Magnetic Field (4 hrs)

6.1. Source of electric field

6.2. Biot-Savart’s law

6.3. The force between two parallel conductors

6.4. Ampere’s Law and its application

7. Electromagnetic Induction (7 hrs)

7.1. Magnetic flux

7.2. Gauss’s Law in Magnetism

7.3. Faraday’s Law of Induction

7.4. Lenz’s law

7.5. Induced Emf (including motional Emf)

7.6. Induced electric field

7.7. Displacement current

8. Inductance (4 hrs)

8.1. Self inductance and mutual inductance

8.2. RL circuits

8.3. Energy in Magnetic field

8.4. Oscillations in an LC circuits

9. AC Circuits (6 hrs)



9.1. AC sources and phasors

9.2. Resistors in an AC circuits

9.3. Inductors in an AC circuits

9.4. Capacitors in an AC circuits

9.5. The RLC series circuits

9.6. Power in an AC circuits

10. Maxwell’s Equations (4 hrs)

10.1. Maxwell’s equations

10.2. Electromagnetic waves

11. Nature of Light (6 hrs.)

11.1. Electromagnetic spectrum

11.2. Propagation and speed of light

11.3. Reflection and refraction

11.4. Refractive index and optical path

11.5. Reversibility principle

11.6. Fermat’s principle

11.7. Propagation of light in material medium

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.


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.

17.9.6 Linear Algebra I for Chemists

COURSE TITLE: LI6EAR ALGEBRA I FOR CHEMISTS

COURSE CODE: MATH 224

CREDIT HOURS: 3

CO6TACT HOURS: 3 LEC. HR + 2 TUT. HR/WEEK

PREREQUISITE: -

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:



• understand the basic ideas of vector algebra.

• understand the concept of vector space over a field

• understand the basic theory of matrices and its various applications

• determine eigenvalues and eigenvectors of a square matrix

• grasp the Gram-Schmidt process

• find an orthogonal basis of a vector space

• invert orthogonal matrices.

• understand the notion of a linear transformation

• find the matrix representation of a linear transformation with respect to two bases.

• find the eigenvalues and eigenvectors of a linear transformation.

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



5.3. Algebra of linear transformations

5.4. Matrix representation of linear transformations

5.5. Eigenvalues and eigenvectors of a linear transformation

5.6. Eigenspace of a linear transformation

6. Group Theory

6.1. Definition

6.2. Types of Groups and Representations

6.3. Reversible Representations

6.4. Irreversible Representations

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%

Text: D. Gemeda, An Introduction to Linear Algebra, Department of Mathematics, AAU, 2000.

17.9.7 Introduction to Computer Applications for Chemists

COURSE TITLE: I6TRODUCTIO6 TO COMPUTER APPLICATIO6S FOR CHEMISTS

COURSE CODE: COMP 201

CREDIT HOURS: 3

CO6TACT HOURS: 2 LEC. HR + 3 LAB. HR/WEEK

PREREQUISITE:

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 Common courses

17.10.1 Entrepreneurship

COURSE TITLE: E6TREPRE6EURSHIP

COURSE CODE: MGMT 201

CREDIT HOURS: 3




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.

17.10.2 Communicative English skills

COURSE TITLE: COMMU6ICATIVE E6GLISH SKILLS

COURSE CODE: FLE6 201

CREDIT HOURS: 3

Course description:

17.10.3 University Writing Skills

COURSE TITLE: U6IVERSITY WRITI6G SKILLS

COURSE CODE: FLE6 301

CREDIT HOURS: 3

Course description:

17.10.4 Civics and ethical Education

COURSE TITLE: CIVICS A6D ETHICAL EDUCATIO6

COURSE CODE: CEED 201

CREDIT HOURS: 3

Course description:

Documents

New Chemistry Curriculum