Download Revised Syllabus - M. Sc. First Year - Chemistry

SCHOOL OF CHEMICAL SCIENCES
Swami Ramanand Teerth Marathwada University,
Nanded-431606
Syllabus of M. Sc. First Year Chemistry
(Credit System)
Revised in academic year 2013-14 and to be implemented from
academic year 2014-15
1
CONTENT
1. Credit System Ordinance for M. Sc. Courses in School of Chemical Sciences
2. M. Sc. First Year Chemistry Common Syllabus for following specializations
running in the school
i) Analytical Chemistry
ii) Industrial Chemistry
iii) Organic Chemistry
iv) Medicinal Chemistry
v) Physical Chemistry
vi) Polymer Chemistry
3. Pattern for Question Papers
4. Internal Marks
2
Credit System Ordinance
SCHOOL OF CHEMICAL SCIENCES
SWAMI RAMANAND TEERTH MARATHWADA UNIVERSITY,
NANDED
(Credit–grade based performance and assessment (CGPA) System)
Features of the credit system
With effect from academic year 2014-2015
3
FEATURES OF THE CREDIT SYSTEM
1. Master’s degree would be of 100 credits each.
2. One credit course of theory will be of one clock hour per week running for
12 weeks.
3. Two credit course of theory will be of two clock hours per week running for
12 weeks.
4. Four credit course of theory will be of four clock hours per week running for
12 weeks
5. One credit course of practicals will consist of 4 hour of laboratory exercise
for 6 weeks.
6. Two credit course of practicals will consist of 4 hour of laboratory exercise
for 12 weeks.
7. Four credit course of practicals will consist of 8 hour of laboratory exercise
for 12 weeks
4
Each Semester shall have 4 Theory courses, 2 Practical
courses and 1 Seminar.
4 Theory Courses x 4 credits =
16 credits
2 Practical courses x 4 credits =
08 credits
1 Seminar x 1 credit
01 credit
=
_______________________________________________
Total
=
25 credits
 Two Semesters X 25 Credits = 50 Credits
 Two Credits, One Each in Two Semesters have been allocated for
seminar per paper. There shall be at least one seminar per paper.
Marks out of 25 will be allotted per semester for this.
 One Credit = 25 Marks; Two Credits = 50 Marks.

FOUR CREDITS (THEORY) = 100 Marks
______________________________________
Internal Exam
External Exam
(50 Marks)
(50 Marks)
 Break up of Internal Theory Exam. (50 marks) is as follows:
Test -1
Test-2
Home Assignment
Total
15
15
20
50
5
 Two credits (theory) = 50 marks (External Exam)
 Four Credits (PRACTICAL) = 100 MARKS
________________________________________
Internal Exam
(50 Marks)
External Exam
(50 Marks)
 Break up of internal Practical exam.(50 marks) is as follows,
Question 1
20
Question 2
Viva-voce
20
Record book
5
Total
5
50
 Break up of External Practical exam.(50 marks) is as follows,
Question 1
20
Question 2
Viva-voce
20
Record book
Total
5
50
5
 Two credits (SEMINAR) = 50 marks.
 Break up of Seminars (50 marks) is as follows,
Semester 1
Semester 2
25
25
6
Total
50
 Academic calendar showing dates of commencement and end of teaching,
internal assessment test and term end examination shall be duly notified
before commencement of each semester every year by the school.
 Credits system offers more options to the student.
 Credits system offer more flexibility to the student.
 Student can get requisite credits from the concerned school where he is
mutually permitted on terms mutually agreed to complete the same and be
eligible to appear for term end examination.
 The term end examinations however, shall be conducted by & at the school.
 Paper setting and assessment for a particular course would be the
responsibility of the course in-charge.
 These activities, including preparation of the result–sheets for the students,
would be coordinated by the School Examination committee comprising
course In-charges and HOD under supervision of the (Director).
7
 Marks obtained for each course would be converted to grade points as
shown in table 1
Table 1: Conversion of marks to grades in credits system
Marks obtained
100-90
89-80
79-70
69-60
59-55
54-45
44-40
39 and less
39 and less internal
Grade
A+
A
B+
B
C+
C
D
FC
FR
Grade points
10
09
08
07
06
05
04
0-FAIL BUT CONTINUE
0- FAILED ( CLEAR COURSE)
 A student who passes the internal tests but failed in semester Examination
(External) of course shall be given FC grade.
 Student with FC grade in a course would be granted credits for that course
but not the grade for that course. He/she shall have to clear the concerned
course within 1.5 year from appearing for the first time in concerned paper,
provided the number of courses with FC and FR grades together is 25% or
less of the courses of that semester.
 Failing which he/she shall be disqualified for credits and will have to opt for
other credits.
 Student who has failed in the internal tests of a course shall be given FR
grade and shall have to (clear) the concerned course.
8
 Grade points earned in each paper shall be calculated as grade points
obtained (vide table 1 above) X credits for the paper.
 The Student Performance Index (SPI) gives weighted performance index of
a semester with reference to the credits of a course.
The SPI shall be calculated as follows:
SPI =
Total earned grade points for the semester
_____________________________
Total credits for the semester.
 Final results: For the final results of a student Cumulative Performance
Index (CPI) based on total earned credits vis a vis total earned grade points
shall be calculated.
The CPI shall be calculated as follows,
CPI =
Total earned grade points
total credits i.e.100
 Student will have to complete 75 compulsory credits for the concerned
course, 15 elective credits in the subject concerned and 10 optional credits
incorporated in the syllabus structure of respective master (PG) course.
9
 Some of the elective credits and optional credits shall be chosen from
elective and optional courses offered by the school of Chemical Sciences or
other campus schools of the University.
 The school in consultation with the Dean, Faculty of Science can make
changes in syallbi.
CPI
9.0 8.0 7.0 6.0 5.5 4.5 4.0 0.0 -
10
8.9
7.9
6.9
5.9
5.4
4.4
3.9
FINAL GRADE
A+
A
B+
B
C+
C
D
F
 Final mark list will only show the grade and grade points and not the marks.
10
M. Sc. First Year Chemistry Syllabus
Swami Ramanand Teerth Marathwada University Nanded-431606
SCHOOL OF CHEMICAL SCIENCES
M. Sc. First Year Chemistry (credit system with effect from 2014-15)
Semester –I
Credits
CH-101 Physical Chemistry
(60 lectures)
4
CH-102 Inorganic Chemistry
(60 lectures)
4
CH-103 Organic Chemistry
(60 lectures)
4
CH-104 Basic principles of spectroscopy
(60 lectures)
4
CH-105
Laboratory Course 1 (Physical Chemistry)
(60 Hrs)
4
CH-106
Laboratory Course 2 (Inorganic Chemistry)
(60 Hrs)
4
CH-107
Seminar
1
Total Credits
25
Semester-II
Credits
CH-201 Physical Chemistry
(60 lectures)
4
CH-202 Inorganic Chemistry
(60 lectures)
4
CH-203 Organic Chemistry
(60 lectures)
4
CH-204 Computer Applications in Chemistry
(60 lectures)
CH-205
Laboratory Course 3 (Organic Chemistry)
(60 Hrs)
4
CH-206
Laboratory Course 4 (Analytical Chemistry)
(60 Hrs)
4
CH-207
Seminar
1
Total Credits
25
11
4
SEMESTER–I
CH-101: Physical Chemistry
1.
(60 Lectures)
Credits 4
Quantum Chemistry:
(A) Introduction and applications of Schrödinger equation: Postulates of quantum
mechanics, uncertainty principle, solutions of Schrödinger equation to model systems
viz. particle in one dimensional box, harmonic oscillator and rigid rotor, numerical on
1D box.
Home assignment: Application of Schrödinger equation to hydrogen atom.
(B) Approximate Methods: The variation method, variation theorem, linear variation
principle. Perturbation theory (first order and non degenerate)
Home assignment: Applications of variation method and perturbation theory to the
Helium atom.
(C) Angular Momentum: Angular momentum, orbital and angular momentum
operators, commutation relations, Eigen values and Eigen functions for angular
momentum, spin antisymmetry and Pauli’s exclusion principle.
Home assignment for students: Operator using ladder operators, addition of angular
momentum.
(D) Electronic Structure of Atoms:
Electronic configuration, Russell-Saunders
terms and coupling schemes, atomic states and term symbols, term separation energies
of the pn configuration and dn configurations, spin-orbit coupling and Zeeman
Splitting.
Home assignment: Introduction to the methods of self consistent field, the virial
theorem.
2.
Thermodynamics
(A) Classical Thermodynamics: Laws of thermodynamics, partial molar properties,
partial molar free energy, chemical potential, partial molar volume, partial molar heat
content, their significances, determinations of partial molar quantities, concept of
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fugacity and determination of fugacity by graphical method, numericals. Non-ideal
systems: Activity, activity coefficient, Debye-Huckel theory for activity coefficient of
electrolytic solutions, determination of activity and activity coefficients, ionic
strength, numerical on ionic strength and Debye-Huckel limiting law.
Home assignment: Application of phase rule to three component systems, Phase
Transformations.
(B) Statistical Thermodynamics:
Concept
of distribution,
thermodynamic
probability and most probable distribution. Ensemble: canonical, grand canonical and
micro-canonical ensembles, Partition functions: Translational, rotational, vibrational
and electronic partition functions, Numerical on Partition functions.
Home assignment: (a) Corresponding distribution laws, (Maxwell-Boltzmann
distribution law) (b) Heat capacity behaviour of solids – chemical equilibria constant
in terms of partition functions.
(C)
Non-equilibrium Thermodynamics: Thermodynamic criteria for non-
equilibrium states, entropy production and entropy flow for different irreversible
processes such as heat flow, chemical reaction. Transformation properties of fluxes
and forces, principle of microscopic reversibility and Onsager’s reciprocity relations
Home assignment: Irreversible thermodynamics for biological systems,
coupled
reactions.
3.
Surface Chemistry-I
Adsorption: Surface tension, capillary action, Freundlich adsorption isotherm,
Langmuir adsorption isotherm, Gibbs adsorption isotherm, estimation of surface area
(BET equation), surface films on liquids (Electro-kinetic phenomenon) and catalytic
activity at surfaces.
Home assignment: Modern techniques for investigating surfaces, Kelvin equation
for vapour pressure of droplets.
Books:
1) Physical Chemistry-P.W. Atkins, ELBS.
13
2) Introduction to Quantum Chemistry-A. K. Chandra, Tata McGraw Hill.
3) Quantum Chemistry-Ira N. Levine, Prentice Hall.
4) Coulson’s Valence-R. Mc Weeny ELBS.
5) Principles of Physical Chemistry-Puri, Sharma, Pathania, Vishal Publishing Co.
6) Molecular quantum mechanics, Vol. I & II, P. W. Atkins, Oxford university presss.
7) Physical Chemistry by Alberty and Silby, Jolly Wiley.
8) Statistical thermodynamics by T. L. Hill, Addison Wesley.
9) Chemical thermodynamics by F. T. Wall, W. H. Freeman & Co.
CH-102: Inorganic Chemistry
1.
(60 Lectures)
Credits 4
Stereochemistry and Bonding in Main Group Compounds
i) VSEPR Theory, Postulates, examples with its stereochemistry
ii) Walsh diagrams (discussion related to BeH2, H2O, BeF2)
iii) dπ- pπ bond, examples
iv) Bent rule and energetics of hybridisation.
v) Simple reaction of covalently bonded molecules (Atomic inversion, Berry
pseudorotation, Nucleophilic displacement and free radical mechanism).
2.
Reaction Mechanism of Transition Metal Complexes
a) Introduction:
i) Labile and Inert Complexes,
ii) Kinetic aspects of valence bond and crystal field theories.
b) Kinetics of octahedral substitution:
i) Acid hydrolysis, factors affecting acid hydrolysis, base hydrolysis,
ii) Base hydrolysis by conjugate mechanism (SN1CB), evidences in favour of
conjugate base mechanism.
c) Substitution reaction in square planar complexes:
i) Trans effect, Theories of Trans effect (Grinberg’s polarization theory and Pi
bonding theory),
ii) Applications of Trans effect.
ii) Mechanism of substitution reaction in square planar complexes.
14
d) Redox reactions:
i)The classification of redox reactions,
ii) Inner sphere mechanism and outer sphere mechanism
3.
Metal – Ligand Bonding
i) Limitations of Crystal field theory, Nephelauxatic effect
ii) Linear Combination of atomic orbitals (LCAO),
iii) Molecular orbital diagrams for homonuclear (from hydrogen to neon molecule)
& heteronuclear diatomic molecules heteronuclear diatomic molecules
iv) Molecular orbital theory for coordination complexes
v) Ligand group orbital (LGO) with respect to octahedral (with diagrams),
tetrahedral & square planar complexes (without diagrams).
vi) Pi bonding in metal complexes, Explaination of pi-bonding in metal complexes
by MOT (octahedral, tetrahedral and square planar complexes),
vii) Evidences for Pi bond formation in metal complexes.
4.
Home assignment:
i)Role of metal ions in biological system (sodium, potassium, Magnesium, Calcium,
Iron, Cobalt, Copper and Zinc).
ii) Chemistry of hemoglobin, myglobin, vitamin B12, Chlorophyll, ferredoxins.
iii) Model synthetic complexes of metals in inorganic chemistry
Books:
1) Inorganic Chemistry (Principles of structure and Reactivity), 4th edition, James Huheey, Eller
A. Keiter, Richard L. Keiter. Harper Collins College Publishers.
2) Selected Topics in Inorganic Chemistry. W. U. Malik, G.D. Tuli, R. D. Madan. S. Chand
Publications.
3) Advanced Inorganic Chemistry Vol I. Gurdeep Raj. Goel Publishing House.
4) Principles of Inorganic Chemistry. B. R. Puri, L. R. Sharma and K. C. Kalia. Milestone
Publishers & Distributors.
5) Advanced Inorganic Chemistry. Satish Kumar Agarwal & Keemti Lal. Pragati Prakashan
15
6) Advanced Inorganic Chemistry, (A comprehensive text). F.A. Cotton and G. Wilkinson,
Interscience Publishers, John Wiley & Sons.
7) Inorganic Chemistry, 5th edition. Shriver and Atkins. W. H. Freeman and Company, New
York.
8) Comprehensive Coordination Chemistry. Eds. G. Wilkinson, R. D. Gillars and J. A.
McCleverty, Pergamon.
9) Essentials of Bio-inorganic Chemistry, Neerja Gupta and Monal Singh, Pragati Prakashan.
CH-103: Organic Chemistry
1.
(60 Lectures)
Credits
4
Nature of Bonding in Organic Molecules
a) Chemical bonding and reactivity- Chemical bond, delocalization, Conjugation,
resonance, hyperconjugation, tautomerism, inductive effects, sterric effect.
b) Bonding other than covalent bonding: Ionic, hydrogen bond, inclusion compounds,
rotaxanes, catenanes, cyclodextrins, cryptands, fullerenes, crown ethers.
c) The relation between structure and acidity and basicity
d) Aromaticity: Benzenoid and non-benzenoid compounds, Huckels rule, antiaromaticity,
homoaromaticity.
Application to carbocyclic and heterocyclic systems, annulenes,
azulenes.
2.
Reaction Mechanism: structure and activity
a) Elementry and simple reaction, Hamonds postulate, Molecularity, Energy profile
diagram.
b) Thermodynamics of the reaction, kinetic of the reaction, thermodynamic verses
kinetic control of reactions, Hammett and Taft effect.
c) Kinetic isotopic effects, method of determining reaction mechanism
d) Structure and stability of reactive intermediates, carbenes, nitrenes, carbocations,
carbanions, benzynes, ylides, enamines and free radicals.
3.
Stereochemistry:
a) Concept of chirality and molecular dissymmetry.
16
b) Symmetry elements and chiral centres, Prochiral relationship,
homotopic,
enantiotopic and disteriotopic groups and faces.
c) Recemic modifications and their resolution, R and S nomenclature. Geometrical
isomerism E and Z. nomenclature.
d) Steriospeciffic and sterioselective reactions.
e) Asymmetric synthesis, optical activity in absence of chiralcarbaon, biphenyl, allenes
and spiranes, Chirality due to helical shape.
f) Conformational analysis: Cyclohexane (mono and disubstituted i.e. halo, hydroxyl
and methyl) and decallins, stability and reactivity.
4.
Substitution Reactions:
A. Aliphatic Nucleophilic:
a) Types of Aliphatic nucleophilic substitution Reactions-SN1, SN2, SET mechanism,
b) NGP by pi and sigma bonds, classical and non-classical carbocations, phenonium
ions, norbornyl system, carbocation rearrangement in NGP, SNi mechanism,
c) effect of structure, nucleophile, leaving group, solvent on rate of SN1 and SN2
reactions, ambident nucleophile, Phase transfer catalysis and regioselectivity.
B. Aliphatic Electrophilic:
a) Types of Aliphatic electrophilic substitution reaction: SE1, SE2, SEi.
b) Electrophilic substitution accompanied by double bond shift.
c) Effect of substrate, leaving group and solvent polarity on the reactivity.
5.
Free Radical Reaction:
a) Generation, charectrization and stability of free radicals.
b) Free radical mechanism, NGP in free radical reactions.
c) Reactivity for aliphatic and aromatic substrate at bridge head.
d) Hundsdiecker reaction.
6.
Home assignment:
Anomeric effect, angle strain and its effect on reactivity, effect of conjugation on
reactivity, stereochemistry of compounds containing N, P and S, confirmation of acyclic
17
molecules, isotopes in labelling experiments, Reed reaction, Diazo transfer reaction,
esterification and ester hydrolysis. Hard and soft acid bases concept. Beckman
reaarengment, rearrengment fragmentation of free radical reaction.
Books:
1) Advanced organic chemistry-Reaction mechanism and structure, Jerry March, Jhon Wiley.
2) Structure and mechanism in organic chemistry, C. K. Ingold, Cornell University Press.
3) Advanced organic chemistry, F. A. Carey and R. J. Sundberg, Plenum.
4) A guide book to mechanism in organic chemistry, Peter Sykes, Longman.
5) Stereochemistry of organic compounds, D. Nasipuri, New Age International.
6) Reaction mechanism in organic chemistry, S. M. Mukherji and S. P. Singh, Macmilan.
7) Modern organic reactions , R. O. C. Norman and J. M. Coxon, Blackie Academic and
Professional.
8) Organic chemistry, R. T. Morison Boyd, Prentice-Hall.
9) Stereochemistry of organic compounds, P. S. Kalsi, New Age Intrenational.
10) Modern organic reactions, H. O. House, Benjamin.
CH-104: Basic Principals of Spectroscopy
1.
(60 Lectures)
Credits 4
Unifying Principles: Characterization of electromagnetic radiation, quantitation of
energy, regions of the spectrum, interaction of radiation with molecular systems,
typyes of molecular energies, factors affecting width and intensity of spectral lines,
selection rule, general discussion on various molecular excitation processes.
2.
Microwave spectroscopy: Classification of molecules according to their moment of
inertia, rigid rotor model, effect of isotopic substitution on the transition frequencies,
stark effect, non-rigid rotor, selection rules, mechanism of interaction, spectra of
symmetric and asymmetric top molecules, applications of microwave spectroscopy.
3.
Infrared spectroscopy: Review of linear harmonic ascillator, vibrational energies
of diatomic molecules, zero point energy, force constant and band strengths,
anharmonicity, morse potential energy diagram, vibration rotation spectroscopy,
PQR branches, Breakdown of oppenheimer approximation, vibrations of polyatomic
18
molecules, selection rules, normal modes of vibrations, overtones, hot bands, fingerprint region, functional group identification.
4.
Raman spectroscopy: Classical and quantum theory, Raman effect, Stokes and
antistokes liner, Pure rotational, vibrational and rotation-vibration Raman spectra,
selection rules, mutual exclusion principles.
5.
Electronic spectroscopy: Beer-Lambert law, molar extinction coefficient, oscillator
strength and intensity of electronic transition, Frank-Candan Principles, ground and
first excited electronic states of diatomic molecule, radiative and non-radiative
decay, internal conversion, intersystem crossing, fluorescence and phosphorescence,
chromophore and qunochrome, types of electronic transitions in organic molecules.
6.
Photoelectron spectroscopy: Basic principles, photoelectric effect, ionization
process, koopman’s theory, photoelectron spectra of simple molecules, ESCA,
chemical information from ESCA.
7.
Electron spin resonance spectroscopy: Basic
principles, zero field splitting,
Kramer’s degeneracy, factors affecting ‘g’ value, hyperfine coupling phenomenon,
representation of ESR spectra, Applications of ESR in chemical analysis.
8.
Mossbauer Spectroscopy: The mossbauer effect, Principle, Mossbauer nuclei,
spectral line width, chemical isomer shift, quadrupole splitting, magnetic hyperfine
interaction, measurement techniques, elucidation of electronic structure of
119
Sn and
151
57
Fe,
Eu complexes using mossbauer data, Doppler shift and recoilless
fraction.
9.
Home assignment:
Books:
1.
C. N. Banwell, Fundamentals of molecular spectroscopy.
CH-105: Laboratory Course–1 (Physical Chemistry);
(60 Hrs)
Credit 4
Section-A: Instrumentation (any eight)
1. To determine velocity constant and energy of activation for saponification of ethyl acetate
by NaOH conductometrically.
19
2. To determine the relative strength of chloroacetic acid and acetic acid by
conductometrically.
3. To determine equivalent conductivity of strong electrolyte at several concentrations and
to verify Onsager’s equation.
4. To determine the solubility and solubility product of sparingly soluble salt,
[BaSO4/PbSO4] at different temperatures by conductometry.
5. To determine potentiometrically pK1 and pK2 values of H3PO4.
6. To determine Hammette constant of given substituted benzoic acid using pH-meter.
7. To determine pH values of various mixtures of sodium acetate and acetic acid in aqueous
solution and hence find out dissociation constant of acid.
8. To determine concentration of Cu (II) ion in given solution titrating with EDTA solution
by calorimetry.
9. To determine the relative strength of two acids by polarometry.
10. To study the variation of refractive index with composition of mixtures of CCl4 and
ethyl acetate.
Section-B: Non Instrumental (any eight)
1. To determine partial molar volume of ethanol and water mixture at given composition.
2. To determine molecular weight of high polymer by viscosity measurements.
3. To study the effect of surfactant on surface tension of water by using stalagmometer.
4. To determine the viscosity of mixtures by Ostwald’s viscometer.
5. To determine the solubility of benzoic acid at different temperature and hence to
determine its heat of solution.
6. To construct the phase diagram of three component system. [CHCl3, CH3COOH and
H2O]
7. Investigate the autocatalytic reaction between KMnO4 and oxalic acid.
8. To determine the rate constant of hydrolysis of ester [catalyzed by NaOH/HCl]
9. To investigate the adsorption of (oxalic acid/acetic acid) by activated charcoal and to test
the validity of Freundlich and Langmuir isotherm.
10. To study the surface tension concentration relationship for the solution.
20
CH-106: Laboratory Course-2 (Inorganic Chemistry)
(60 Hrs)
Credits 4
Minimum 16 experiments should be completed
1-4.
Basic Principles underlying Inorganic Chemistry Practicals, Laboratory safety &
Chemical Hazards:
1) Basic concepts regarding preparation of normal, molar, and percentage solutions.
2) Theoretical principles underlying qualitative analysis of inorganic mixtures.
3) Preparations of reagents & solutions required for semimicro qualitative analysis.
4) Information about Laboratory safety and chemical hazards
5-10. Qualitative analysis of inorganic mixtures (Detection of three acidic radicals and three
basic radicals) (6 mixtures)
11-16. Preparation of complexes (any six) (Relevant information about spectral, magnetic
properties & applications should be collected & provided to the students at least wherever
possible)
(i) Vanadium acetylacetonate VO(acac)3
(ii) Manganese acetylacetonate Mn(acac)3
(iii) Potassium trioxalato ferrate(III) K3[Fe(C2O4)3]
(iv) Hexammine nickel(II) chloride [Ni(NH3)6Cl2]
(v) Hexammine Cobalt(III) Chloride [Co(NH3)6Cl3 ]
(vi) Tetrammine Copper(II) sulphate [Cu(NH3)4SO4]
(vii) Cis-Potassium dioxalatodiaquochromate Cis-K[Cr(C2O4)2(H2O)2]
(viii) Chloropentammine cobalt(III) chloride [Co((NH3)5Cl)Cl2]
(ix) Mercury(II) tetrathiocyanatocobaltate(II) [HgCo(SCN)4]
IMPORTANT NOTES:
1. Each theory course is of 60 lectures out of which 15 lectures should be given for internal
tests, seminars, home assignments / tutorials and discussion for answer books of internal
tests.
2. Practical should be carried out on micro scale.
3. Each practical course should be given eight hours of laboratory work per week.
21
SEMESTER – II
CH-201: Physical Chemistry
1.
(60 Lectures)
Credits 4
Surface Chemistry-II
Micelles: Surface active agents, classification of surface active agents, micellisation,
hydrophobic interaction, critical miceller concentration (CMC), factors affecting CMC of
surfactants.
Home assignment: Solubilisation, micro emulsion reverse micelles, thermodynamics of
micellisation-phase separation and mass action models.
Macromolecules: Polymers, classification of polymers, electrically conducting, fire
resistant polymers, kinetics of polymerization, mechanism of polymerization, molecular
mass, number and mass average molecular mass, molecular mass determination by
osmometry, viscometry and light scattering methods, numericals.
Home assignment: Sedimentation, chain configuration of macromolecules, calculation
of average dimensions of various chain structures, proteins and nucleic acids.
2.
Electrochemistry
Electrochemistry
of
solutions:
Debye-Huckel-Onsager
treatment,
ion
solvent
interactions, thermodynamics of electrified interface, Lippmann equation, over potential,
exchange current density, derivation of Butler-Volmer equation, Tafel plot, quantum
aspects of charge transfer at electrodes-solution interfaces, tunnelling.
Semiconductor/electrolyte
interface:
Theory
of
double
layer
at
semiconductor/electrolyte interface, structure of double layer interface, flatband potential,
effect of light at semiconductor solution interface.
Polarography: Principle and theory of polarography, Ilkovic equation, diffusion current
and half wave potential and their significance. Numericals on Ilkovic equation and half
wave potential.
Corrosion: Introduction to corrosion, corrosion monitoring and prevention methods.
Home assignment: a) Structure of electrolyte interfaces: Guoy-Chapman, Stern,
Graham-Devanathan-Mottwatts, Tobin, Bockris, Devanathan models.
b) Electrocatalysis–influences of various parameters, hydrogen electrode.
c) Bioelectrochemistry, threshold membrane phenomena, Nernst-Planck equation.
22
d) Intrinsic and extrinsic semiconductors, p-type, n-type semiconductors.
3.
Chemical Kinetics
Order and molecularity of reaction, theories of reaction rates: collision theory of reaction
rates, steric factor, activated complex theory, Arrhenius equation, reactions in solution:
diffusion controlled reactions, ionic reactions and kinetic salt effect, steady state
approximation, kinetics of complex reactions: dynamics of chain reactions (hydrogenbromine reaction, pyrolysis of acetaldehyde), photochemical (hydrogen-bromine and
hydrogen-chlorine reactions). Kinetic and thermodynamic control of reactions,
Homogeneous catalysis: acid base and enzyme kinetics, Michaelis-Menten equation, Fast
reactions: study of fast reaction by flow methods, flash photolysis and nuclear magnetic
resonance method. Dynamics of unimolecular reactions: Lindemann theory of
unimolecular reactions. Numericals on rate constant, order of reaction and Arrhenius
equation.
Home assignment: (a) Steady state kinetics, treatment of unimolecular reactions. (b)
Dynamics and molecular motions, probing the transition reactions, kinetic salt effects.
Potential energy surfaces, dynamic chain (hydrogen-bromine reaction, pyrolysis state,
and dynamics of barrierless chemical reactions in solution. (c) Dynamics of unimolecular
reactions (Lindemann-Hinshelwood theory, Rice-Ramsperger-Kassel-Marcus [RRKM]
theory of unimolecular reactions).
Books:
1) Physical Chemistry-P. W. Atkins, ELBS.
2) Introduction to Quantum Chemistry-A. K. Chandra, Tata McGraw Hill.
3) Quantum Chemistry-Ira N. Levine, Prentice Hall.
4) Coulson’s Valence-R. Mc Weeny ELBS.
5) Chemical Kinetics-K. J. Laidler, McGraw Hill.
6) Kinetics and Mechanism of Chemical Transformations-J. Rajaraman and J. Kuriacose,
Macmillan.
7) Principles of Physical Chemistry-Puri, Sharma, Pathania, Vishal Publishing Co.
8) Micelles, Theoretical and Applied Aspects-V. Moroi, Plenum.
23
9) Modern Electrochemistry Vol. I & II, J. O. M. Bockris & A. K. N. Reddy, Plenum.
10) Introduction to Polymer Science-V. R. Gowarikar, N, V. Vishwanathan & J. Sridhar, Wiley
Eastern.
11) Physical chemistry of macromolecules, S. F. Sun, John-Wiley and Sons, INC.
CH-202: Inorganic Chemistry
1.
(60 Lectures)
Credits 4
Electronic Spectra and Magnetic Properties of Transition Metal Complexes:
a)Introduction, Coupling of orbital angular momentum, coupling spin angular
momentum, Spin-orbit Coupling, Coupling Schemes (Russel Saunders and j-j Coupling).
b) Term Symbol, Hund’s Rules for determination of ground state term symbol,
Microstates, Prediction of ground state term symbol for different configurations of
transition metals, Hole formulation, Racah Parameters.
c) Effect of Weak Octahedral and tetrahedral crystal field potential on terms, Orgel
diagrams (d1-d9 configuration) and Tanabe-sugano diagrams (d2 & d6 configuration).
d) Selection rules, Charge Transfer Spectra, Applications of Orgel diagrams to electronic
spectra of transition metal aqua complexes.
e) Calculations of Dq , B and β parameters (Graphical method and Konig’s Numerical
method).
f) Prediction of Magnetic moment values of certain transition ions (d1- d9 with various
oxidation states and various ligands), Anomalous magnetic moments, spin crossover.
2.
Metal π – Complexes:
a) Carbonyl complexes:
i) Introduction, Classification of carbonyl complexes
ii) Preparation, properties & structures of mono, di, & trinuclear carbonyl complexes
[V(CO)6, Cr(CO)6, Ni(CO)4, Fe(CO)5, Mn2(CO)10, Co2(CO)8, Fe2(CO)9, Fe3(CO)12]
iii) EAN rule and 18 electron rule for metal carbonyls, Numericals.
iv) Bonding in metal carbonyls
24
b) Nitrosyl Complexes:
i) Introduction,
ii) Linear v/s Bent nitrosyl,
iii) Preparation, properties, structure & applications of Sodium nitroprusside,
iv) Brown ring compound
c) Dioxygen and Dinitrogen complexes
3.
Boranes, Carboranes and Metal Clusters:
(a) Boranes & Carboranes
i) Introduction, Classification & nomenclature of boranes.
ii) Preparation, Properties and Structure of B2H6, B4H10 and B5H11
iii) Introduction & Classification of Carboranes.
iv) Chemistry of C2B10H12 (Di-carbacloso-dodecacarborane)
v) Wade’s rules for prediction of structure type in boranes & carboranes
vi) styx code (determination of styx code for B2H6, B4H10, B5H11, B10H14, B6H10 by
drawing their structures)
(b) Metal clusters:
i) Introduction, Classification of metal clusters
ii) Structures of Carbonyl Clusters (LNCC and HNCC)
iii) Structural aspects of Halide type Clusters (Di, tri, tetra & hexanuclear clusters)
iv) Cheverel phases and Zintl ions
v) Total electron count in HNCC, Numericals.
4.
Home assignment:
i) Metal deficiency and diseases
ii) Gold complexes with anti-arthritic, antitumor and anti-HIV activity
iii) Vanadium compounds in diabetes
25
Books:
1) Selected Topics in Inorganic Chemistry. W. U. Malik, G.D. Tuli, R. D. Madan. S. Chand
Publications.
2) Inorganic Chemistry (Principles of structure and Reactivity). James Huheey, Eller A. Keiter,
Richard L. Keiter. Harper Collins College Publishers.
3) Chemistry of the elements, 2nd edition. N. N. Greenwood and A. Earnshaw. Pergamon.
4) Inorganic Electronic Spectroscopy, A.B.P. Lever, Elsevier.
5) Magnetochemistry, R.L. Carlin, Springer Verlag.
6) Principles of Inorganic Chemistry. B. R. Puri, L. R. Sharma and K. C. Kalia. Milestone
Publishers & Distributors.
7) Advanced Inorganic Chemistry. Satish Kumar Agarwal & Keemti Lal. Pragati Prakashan
8) Advanced Inorganic Chemistry, (A comprehensive text). F.A. Cotton and G. Wilkinson,
Interscience Publishers, John Wiley & Sons.
9) Inorganic Chemistry, 5th edition. Shriver and Atkins. W. H. Freeman and Company, New
York.
10) Advanced Inorganic Chemistry Vol II. Gurdeep Raj. Goel Publishing House.
11) Use of inorganic Chemistry in Medicine, Edited by Nicholas P. Farrell, Royal Society of
Chemistry Publications.
CH-203 : Organic Chemistry
1.
(60 Lectures)
Credits 4
Aromatic Substitution Reaction:
A. Aromatic Electrophilic Substitution: Introduction, the arenium ion mechanism,
orientation and reactivity. Energy Profile diagram, steric effect and the ortho/para rati,
ipso attack, introduction of a third group into benzene ring, Electropihilic substitution in
polycyclic and heterocyclic ring system.
Some important name reactions: Diazonium coupling, Vilsmeieier-Haack reaction,
Bischler Nepieralski reaction, Gatterman-koch reaction.
A.
Aromatic Nucleophilic Substitution: SN1, SN2 SNAr and SRN1 mechanism.
Aromatic nucleophilic substitution via benzyne intermediate. Factor affecting reactivity
in aromatic nucleophilic substitution reaction.
26
Some important name reactions: ChiChibabin reaction, Somlet Houser and Smiles
rearrangement.
2.
Addition to Carbon-Carbon Multiple Bonds.
1. Electrophilic addition to C-C double bond.
2. Mechanism and stereochemical aspects of addition reaction involving electrophile,
nucleophile and free radicals.
3. Regio and chemo selectivity, orientation and reactivity, conjugate addition.
4. Addition to cyclopropane, hydroboration, Micheal reaction, Sharpless asymmetric
epoxidation, hydroxylation of alkene-diol formation
3.
Addition to Carbon-Heteroatom Multiple Bonds:
1. Some general and steriochemical aspect of addition to carbonyl compounds
2. Mechanism and stereochemistry of metal hydride reduction.
3. Addition of organo metallic compounds to carbon-heteromultiple bond (organo zinc,
organo copper, organo lithium, reagents to carbonyl and unsaturated carbonyl
compounds).
4. Some important name reactions: Wittig reaction, Knoevenagel, Claisen, Mannich,
Perkin and stobbe condensation.
4.
Elimination Reactions:
1. The E1, E2 and E1cB mechanisms. Orientation in Elimination reactions.
2. Hofman versus Saytzeff elimination, Pyrolytic syn-elimination.
3. Competition between substitution and elimination reactions.
4. Reactivity: effects of substrate structures, attacking base, the leaving group, the nature
of medium on elimination reactions. Pyrolytic elimination reactions.
5.
Pericyclic Reactions:
1. Molecular orbital symmetry, Frontier orbitals of ethelene, 1,3-butadien, 1,3,5hexatiene and allyl system.
2.
Classification of pericyclic reactions
27
3.
Woodward-Hoffmann correlation diagram, FMO and PMO approaches.
4. Electrocyclic reaction: conrotatory and disrotatary motion, 4n, 4n+2 and allyl system.
5. Cycloadditions:
Superafacial and antrafacial addition, 4n and 4n+2 system, 2+2
addition of ketenes, 1,3 dipolar cycloaddition and chelotropic reaction.
6. Sigmatropic reaarengments: Superafacial and antrafacial shifts of H, sigmatropic shifts
involving carbon moieties, 3,3 and 5,5 sigmatroic rearrengments.
7. Some important pericyclic reactions: Claisen, Cope and aza-cope rearrengments.
6.
Home Assignment:
1. Electrophilic metallation, Hoesch reaction, Arenechromium carbonyl complexes, VonRichter rearrangement.
2. Birch reduction, hydrogenation of double and triple bond, addition of carbine
(methylene), catalytic hydrogenation.
3. Amine catalysed condensation reaction, silanes, Reformatsky reaction, Dieckmann
condensation.
4. Problems on pyrolytic syn elimination Ei elimination.
5. Problems on sigmatrophic reactions, chelotropic reactions, The Ene reactions, FMO
approach and PMO approach.
Books:
1. Advanced organic chemistry-Reaction mechanism and structure, Jerry March, Jhon Wiley.
2. Structure and mechanism in organic chemistry, C. K. Ingold, Cornell University Press.
3. Advanced organic chemistry, F. A. Carey and R. J. Sundberg, Plenum.
4. A guide book to mechanism in organic chemistry, Peter Sykes, Longman.
5. Stereochemistry of organic compounds, D. Nasipuri, New Age International.
6. Modern organic reactions, R. O. C. Norman and J. M. Coxon, Blackie Academic and
Professional.
7. Organic chemistry, R. T. Morison Boyd, Prentice-Hall.
8. Organic reactions and their mechanism, P. S. Kalsi, New Age Intrenational.
9. Modern organic reactions, H. O. House, Benjamin.
10. Pericyclic reactions, S. M. Mukherji, Macmilan, India.
28
CH-204: Computer Applications in Chemistry
A.
(60 Lectures)
Credits 4
MS-Office
Introduction to MS-word:
1.
Starting word, Title bar, Tool bars, The Ruler, Scroll bars, The menu bar, the status bar,
wizards and templates.
2.
Basic text editing, adding text, deleting text, undo and redo, selecting text and perform
options, moving and copying text.
3.
Formatting : Character formatting, adding bold, italic or underlining with the toolbar, font
dialog box, select case, paragraph formatting adding borders and shading setting page
margins, numbering pages.
4.
Searching and proofreading tools: Find and replace, searching for special character,
choosing custom dictionary, checking grammer, thesaurus.
5.
Word file management: What is file management, creating folders, deleting files and
folders printing .
6.
Working with tables and columns: Creating table, using table tools, changing column
widths with qutofit, merging cells, Formatting, changing the border and line styles,
sorting tables, copying tables, deleting tables.
7.
Introduction to MS-Excel: Spreadsheet overview, starting excel creating spreadsheet,
excel menus, working with text and numbers: spreadsheets and numbers, spreadsheets
and text, finding numbers and text, working with formulas and functions introduction,
using basic formulas; using basic and advance functions, Formatting: Types of
formatting, using borders, colors and patterns, conditional format using styles, printing
spreadsheets and workbooks, Creating and formatting charts: Introduction to charts,
creating charts, formatting charts, exploring charts, Introduction to MS-Power point:
Applications of powerpoint, study of various power-point presentations, applying various
designs to slides, creating presentations including image.
B.
Introduction to Programming in C
1.
Introduction:
History of C language
Variables and constants
Key words
I/O statements in C.
29
Data types and operator,
2.
Control structures:
while, for)
3.
string
goto statement.
Introduction to Array
one dimensional and multi-dimensional
string manipulation functions (strlen, strcpy, strcmp).
standard (Library) function
4.
Functions:
5.
Structure and union:
structure
switch, l Looping statements (while, do –
break and continue statements
Array and strings :
array
if, if –else, nested if
user defined functions
Introduction to structure
Array of structure
structure within
introduction to union.
Books
1.
Let Us C: Yeshwant Kanitkar
CH-205: Laboratory Course – 3 (Organic Chemistry) (60 Hrs)
Credits 4
Preparation
Estimations
A)
Qualitative analysis (Separation of binary mixture) (any 8)
1.
Separation, purification and identification of compounds from binary mixture solid-solid,
solid-liquid and liquid-liquid mixtures are to be given for separation. Chemical methods
(no ether), ether separation as well as physical methods are used for separation of
mixtures.
2.
Not more than one gram of each solid and 3 ml of each liquid should be used for
preparing mixtures.
Following list of mixtures is given for guidance or any other combination of mixture may
be given.
Separation by chemical methods (no ether)
1.
Benzoic acid + Acetanilide
2.
β-Naphthol + Aniline
3.
α-Naphthyl amine + Urea
4.
Salicyolic acid + p-Taluidine
Ether separation
5.
Salicyclic acid + Phthalic acid
6.
Sulphonilic acid + Cinnamic acid
30
7.
Oxalic acid + p-Nitroaniline
8.
Oxalic acid + m-Dithiobenzene
Low boiling liquids
9.
Acetone + Nitrobenzene
10.
Ethylacetate + p-Cresol
High boiling liquids
11.
O-Cresol + Nitrobenzene
12.
m-cresol + p-Dichlorobenzene
3.
Purity of recrystalized compounds should be checked by TLC.
4.
Quality and quantity of the compounds and purity should be shown to the teacher /
examiner.
B.
Organic synthesis (any 8 should be carried out on microscale using 10 mmol of starting
material)
1.
Synthesis of 4-chloro toluene from p-toluidine (Sandmayer reaction)
2.
Synthesis of triphenyl methanol from benzoic acid.
3.
Synthesis of Dibenzylacetone from benzaldehyde (Aldol-condensation)
4.
Preparation of p-nitro/p-bromo-aniline from acetanilide.
5.
Synthesis of 7-hydroxy coumarin from resorcinol.
6.
Synthesis of 2,4-dihydroxy benzaldehyde from salicyaldehyde.
7.
Synthesis of 2,4-dihydroxy acetophenone from recercinol.
8.
Preparation of 1,2,4-tri-acetoxy benzene from hydroquinone
9.
Synthesis of p-methoxy acetophenone from anisole.
10.
Fries rearrangement of phenyl acetate to o/p-hydroxy acetophenone.
11.
Synthesis of
C.
Quantitative analysis (any four)
1.
Determination of iodine and saponification values of an oil sample.
2.
Estimation of nitro group by reduction.
3.
Estimation of glucose by iodination.
4.
Estimation of –COOH group.
-benzoil propionic acid from succinic anhydride.
31
5.
Estimation of CONH2 group
6.
Estimation of –COOR group
CH-206: Laboratory Course-4 (Analytical Chemistry) (60 Hrs)
Credits 4
Minimum 16 experiments should be completed
Error analysis and statistical analysis: (1) (a) Determination of relative error and percentage
relative error for the experimental data (b) Calculation of mean derivation and standard
derivation for the experimental data (c) Application of‘t’ test for experimental data. (2) (a)
Application of rejection criteria (‘Q’ test) for experimental data. (b) Treatment of analytical data
with least square method applied to Beer’s law for KMnO4 solutions.
Chromatography: (3) Separation of cations and anions by paper chromatography and
determination of their Rf values (4) Determination of ion-exchange capacity of an cation
exchanger and anion exchanger.
Conductometry: (5) Determination of the strength of strong acid and weak acid from mixture
solution conductometrically. (6) Analysis of aspirin by conductometric method.
pH metry: (7) Acid-base titration in non-aqueous media by pH-metry (benzoic acid in
ethanol/NaOH). (8) Determination pKa of weak acid by pH metry. (9) Determination of degree
of dissociation of weak electrolyte and to study the deviation from ideal behaviour that occurs
with a strong electrolyte.
Colorimetry: (10) Verification of Beer’s law of (a) KMnO4 and Cu+2 ammonia complex
solution. (11) Determination of empirical formula for the formation of ferric salicylate complex
by Job’s method. (12) Determination of stability constant for the formation of complex between
Fe+3 ions and 5-sulphosalicylic acid.
Polarimetry: (13) Determination of rate constant for inversion of cane sugar by Polarimetry.
(14) Study of inversion of cane sugar by enzyme kinetics.
32
Potentiometry: (15) Determination of the strength of halides in the given mixture using
potentiometry.
Kinetics: (16) To study the kinetics of iodination of acetone.
Flame photometry: (17) Estimation of Na+/K+ by flame photometry
(18) Determination of hardness of water by complexometric titration.
IMPORTANT NOTES:
1. Each theory course is of 60 lectures out of which 15 lectures should be given for internal
tests, seminars, home assignments / tutorials and discussion for answer books of internal
tests.
2. Practical should be carried out on micro scale.
3. Each practical course should be given eight hours of laboratory work per week.
33
Pattern for Question Papers
QUESTION PAPER PATTERN FOR 50 MARKS THEORY
PAPER
IMPORTANT NOTES:
1) Attempt any five questions out of seven.
2) All questions carry equal marks i.e. ten marks each.
Q.1: Explain the following (3 + 3 + 4 = 10 marks).
Q.2: Attempt the following questions (3 + 3 + 4 = 10 marks).
Q.3: Attempt the following questions (3 + 3 + 4 = 10 marks).
Q.4: Attempt the following questions (3 + 3 + 4 = 10 marks).
Q.5: Answer the following questions (5 + 5 = 10 marks).
Q.6: Answer the following questions (5 + 5 = 10 marks).
Q.7: Write short notes on the following:
34
(10 marks).
QUESTION PAPER PATTERN FOR 50 MARKS PRACTICAL
PAPER
Swami Ramanand Teerth Marathwada University, Nanded
SCHOOL OF CHEMICAL SCIENCES
M. Sc. Practical Examination (April-May/October-November 2014)
M. Sc. First Year (Semester-I / II)
Subject: Chemistry
Lab. Course:
Total Marks: 50
Time: 08 Hr
Date:
Q 1.
20 marks
Q 2.
20 marks
Q 3. Viva-Voce
05 marks
Q 4. Record Book
05 marks
35
Internal Marks
 Home assignment should be completed for each theory course before 15th of
the last month in the teaching semester.
 Mark list of internal tests, Seminars & Home Assignments should be
submitted to the Director within eight days after completion of concern
examination.
 Answer books of all Internal Examinations should be shown to the students.
 Maximum marks for each Internal Theory paper will be 50. Two test each of
15 marks (total 30 marks) + 20 mark for Home Assignment = 50 marks for
internal assessment of each Theory course paper.
 Maximum marks for each Internal Practical paper will be 50. Two questions
of 20 marks each + 5 marks for Viva- voce + 5 marks for Record Book = 50
marks for each internal Practical paper.
 Maximum marks for each External Theory Paper will be 50.

Maximum marks for each External Practical paper will be 50. Two questions
of 20 marks each + 5 marks for Viva- voce + 5 marks for Record Book = 50
marks for each External Practical paper.
36