MSC Chemistry MDU Rohtak

Will you please give here syllabus of MSC Chemistry course of Maharshi Dayanand University, Rohtak (MDU Rohtak) ?

[Arun Vats]

As you want I am here providing you syllabus of MSC Chemistry course of Maharshi Dayanand University, Rohtak (MDU Rohtak).

Syllabus :

First Semester :
Nomenclature
Inorganic Chemistry
Physical Chemistry
Organic Chemistry
General Spectroscopy
Computer for Chemists

2nd Semester :
Theory :
Nomenclature
Inorganic Chemistry
Physical Chemistry
Organic Chemistry
Computer for Chemists

Practical :
Inorganic Chemistry Practical
Physical Chemistry Practical
Organic Chemistry Practical

3rd semester :
Nomenclature
Inorganic Special-I/Physical Spl-
I/Organic Spl.-I
Inorganic Special-II/Physical Spl-
II/Organic Spl.-II
Inorganic Special-III/Physical Spl-
III/Organic Spl-III

M.Sc. Chemistry Ist Semester
Paper I CH-401 Inorganic Chemistry 4 hrs. / Week
Max. Marks: 80
Time: 3 Hrs.

Section-A
Stereochemistry and Bonding in Main Group compounds: VSEPR theory, d -p
bonds, Bent rule and energetic of hybridization.

(7 Hrs.)
Metal-Ligand Equilibria in solution
Stepwise and overall formation constants and their interactions, trends in stepwise
constants, factors affecting stability of metal complexes with reference to the nature of
metal ion and ligand, chelate effect and its thermodynamic origin, determination of
binary formation constants by pH-metry and spectrophotometry.
(8 Hrs.)

Section-B
Reaction Mechanism of Transition Metal Complexes-I
Inert and labile complexes, Mechanisms for ligand replacement reactions, Formation
of complexes from aquo ions, Ligand displacement reactions in octahedral complexesacid
hydrolysis, Base hydrolysis, racemization of tris chelate complexes, electrophilic
attack on ligands.
(15 Hrs.)

Section-C
Reaction Mechanism of Transition Metal Complexes-II
Mechanism of ligand, displacement reactions in square planar complexes, the trans effect,
theories of trans effect, mechanism of electron transfer reactions – types; outer sphere
electron transfer mechanism and inner sphere electron transfer mechanism, electron
exchange. (15 Hrs.)

Section-D
Isopoly and Heteropoly Acids and Salts
Isopoly and Heteropoly acids and salts of Mo and W: Structures of isopoly
and heteropoly anions.

(7 Hrs.)
Crystal Structures
Structures of some binary and ternary compounds such as fluorite, antifluorite, rutile,
antirutile, crystobalite, layer lattices- Cd I2, Bi I3; Re O3, Mn2O3, corundum, pervoskite,
Ilmenite and Calcite.
( 8 Hrs.)

M.Sc. Chemistry Ist Semester
Paper II CH-402 Physical Chemistry 4 hrs. / Week
Max. Marks: 80
Time: 3 Hrs.
Section-A
Quantum Mechanics: Postulates of Quantum Mechanics; derivation of Schrodinger
wave equation; Max-Born interpretation of and the Heisenberg’s uncertainty principle;
Quantum mechanical operators and their commutations relation, Hermition operators,
(elementary ideas, quantum mechanical operator for linear momentum and angular
momentum as Hermition operator). The average value of the square of Hermition
operators; commuting operators and uncertainty principle(x & p; E &t); Schrodinger
wave equation for a particle in one dimensional box; evaluation of average position,
average momentum and determination of uncertainty in position and momentum and
hence Heisenberg’s uncertainty principle, picorial representation of the wave equation of
a particle in one dimensional box and its influence on the kinetic energy of the particle in
each successive quantum level, lowest energy of the particle.

Section-B
Thermodynamics: Brief resume of first and second Law of thermodynamics.
Entropy changes in reversible and irreversible processes; variation of entropy with
temperature , pressure and volume, entropy concept as a measure of unavailable energy
and criteria for the spontaneity of reaction; free energy functions and their significance,
criteria for spontaneity of a process; partial molar quantities (free energy, volume ,heat
concept), Gibb’s-Duhem equation;
Section-C
Chemical Dynamics: Effect of temperature on reaction rates, Rate law for opposing
reactions of Ist order and IInd order, Rate law for consecutive Ist order reactions,
Collision theory of reaction rates and its limitations, steric factor, Activated complex
theory, Ionic reactions: single and double sphere models, influence of solvent and ionic
strength, the comparison of collision and activated complex theory.

Section-D
Electrochemistry:
Ion - Ion Interactions: The Debye -Huckel theory of ion- ion interactions: potential and
excess charge density as a function of distance from the central ion, Debye Huckel
reciprocal length, ionic cloud and its contribution to the total potential, Debye - Huckel
limiting law of activity coefficients and its limitations, ion - size effect on potential, ion -
size parameter and the theoretical mean - activity coefficient in the case of ionic clouds
with finite - sized ions.

Debye - Huckel -Onsager treatment for aqueous solutions and its limitations Debye-
Huckel-Onsager theory for non-aqueous solutions, the solvent effect on the mobality at
infinite dilution, equivalent conducftivity ( ) vs. concentration c 1/2 as a function of the
solvent, effect of ion association upon conductivity (Debye- Huckel - Bjerrum equation).

M.Sc. Chemistry Ist Semester
Paper III CH-403 Organic Chemistry 4 hrs. / Week
Max. Marks: 80

Section-A
Nature of Bonding in Organic molecules: Delocalized chemical bonding –conjugation,
cross conjugation, resonance, hyperconjugation , tautomerism. Aromaticity in benzenoid
and non-benzenoid compounds, alternant and non-alternant hydrocarbons, Huckel’s rule,
energy level of -molecular orbitals, annulenes, antiaromaticity, homo-aromaticity,
PMO approach. Bonds weaker than covalent, addition compounds, crown ether
complexes and cryptands, inclusion compounds, cyclodextrins, catenanes and rotaxanes

Section-B
Stereochemistry : Chirality, elements of symmetry, molecules with more than one chiral
centre, diastereomerism. Determination of relative and absolute configuration (octant rule
excluded) with special reference to lactic acid, aniline & mandelic acid. Methods of
resolution, optical purity, prochirality, enantiotopic and diastereotopic atoms, groups and
faces, asymmetric synthesis, cram’s rule and its modifications, prelog’s rule,
conformational analysis of cycloalkanes (upto six membered rings), decalins,
conformations of sugars, optical activity in absence of chiral carbon (biphenyls, allenes
and spiranes), chirality due to helical shape, geometrical isomerism in alkenes and
oximes, methods of determining the configuration.

Section-C
Reaction Mechanism: Structure and Reactivity: Types of mechanisms, types of
reactions, thermodynamic and kinetic requirements, kinetic and thermodynamic control,
Hammond’s postulate, Curtin-Hammett principle. Potential energy diagrams, transition
states and intermediates, methods of determing mechanisms, isotope effects. Hard and
soft acids and bases. Generation, structure, stability and reactivity of carbocations,
carbanions, free radicals, carbenes and nitrenes. Effect of structure on reactivity. The
Hammett equation and linear free energy relationship, substituent and reaction constants.
Taft equation.

Section-D
Purification Techniques: Chromatography: various types of chromatography, principles
and applications, counter current distribution, HPLC, electrophoresis

Natural and Synthetic Dyes: Indigo and Alizarin including their structure elucidation,
interaction between dyes and fibers, various classes of synthetic dyes including
heterocyclic dyes.

Dissachrides: Detailed study of maltose and lactose.

Paper IV CH -404 General Spectroscopy 90 Hrs. (3 Hrs. /week)
Max. Marks: 60
Time: 3 Hrs.

Section-A
1. Electromagnetic radiation, interaction of electromagnetic radiation with matter,
regions of the Spectrum the width and intensity of spectral transitions. Resolving power.

2. Rotational spectra- The rotation molecules, rotational spectra of diatomic
molecules, the spectrum of non-rigid rotator, the effect of isotopic substitutions,
rotational spectra of linear and symmetric top polyatomic molecules

3. Vibrational and Vibrational – Rotational Spectra: The vibrating diatomic
molecule; simple harmonic vibrations, anharmonicity of vibrations, the diatomic
vibrating rotator, the interaction of rotations and vibrations, the vibrations of
polyatonic molecules, analysis by infrared technique.

4. Electronics Spectra: Electronic spectra of idiatonic molecules, vibrational course
structure, and rotational fine structure of electronic band, the Frank-Condon
principle, intensity of vibrational-electronic band, dissociation energy, the Fortrat
diagram.

Section-B
5. NMR Spectra Dynamic and magnetic properties of atomic nuclei, nuclear
resonance, relaxation processeds, chemical effects in NMR e.g. chemical shift.
Absorption intensities, Spin-spin coupling, Elementary idea of time dependents
effects in NMR. Instrumentation line diagram.

6. Applications of UV, IR and NMR spectra in the structural elucidation of organic
compounds.

Section-C
Electronic Absorption Spectroscopy: Energy levels in diatomic molecules,
introduction to electronic transition, Assignment of transitions, Spectra of transition
metal complexes, Orgel diagrams, Calculation of Dq and for NiII complexes,
structural evidence from electronic spectra.
Nuclear Magnetic Resonance: Applications of spin-spin coupling to structure
alignment of inorganic compounds, evaluation of reaction rates of fast exchange
reactions, the double resonance technique.
Application of infra-red spectroscopy to the determination of inorganic compounds

M.Sc. Chemistry IInd Semester
Paper V CH-405 Inorganic Chemistry 4 hrs. / Week
Max. Marks: 80
Time: 3 Hrs.

Section-A
Metal-Ligand Bonding
Limitation of crystal field theory, molecular orbital theory, octahedral, tetrahedral or
square planar complexes, -bonding and molecular orbital theory.
(15 Hrs.)

Section-B
Electronic Spectra of Transition Metal Complexes
Spectroscopic ground states, correlation and spin-orbit coupling in free ions for Ist
series of transition metals, Orgel and Tanabe-Sugano diagrams for transition metal
complexes (d1 – d9 states) calculation of Dq, B and parameters, effect of distortion
on the d-orbital energy levels. Structural evidence from electronic spectrum, John-
Tellar effect, Spectrochemical and nephalauxetic series, charge transfer spectra,
electronic spectra of molecular addition compounds.

. (16 Hrs.)
Section-C
Magantic Properties of transition metal complexes
Elementary theory of magneto - chemistry, Guoy’s method for determination of
magnetic susceptibility, calculation of magnetic moments, magnetic properties of free
ions, orbital contribution, effect of ligand-field, application of magneto-chemistry in
structure determination, magnetic exchange coupling and spin state cross over.
( 8 Hrs. )

Metal Clusters
Structure and bonding in higher boranes, Wade’s rules, Carboranes, Metal
Carbonyl clusters- Low Nuclearity Carbonyl clusters, total electron count (TEC)
(8 Hrs.)

Section-D
Metal - Complexes
Metal carbonyls, structure and bonding, vibrational spectra of metal carbonyls for
bonding and structure elucidation, important reactions of metal carbonyls;
preparation, bonding, structure and important reactions of transition metal nitrosyl,
dinitrogen and dioxygen complexes; tertiary phosphine as ligand.
(15 Hrs.)

M.Sc. Chemistry IInd Semester
Paper VI CH-406 Physical Chemistry 4 hrs. / Week
Max. Marks: 80
Section-A
Schrodinger wave equation for a particle in a three dimensional box and the concept of
degeneracy of energy levels. Schrodinger wave equation for linear harmonic oscillator,
solution by polynomial method, zero point energy and its consequence. Schrodinger
wave equation for three dimensional Rigid rotator, energy of rigid rotator, space
quantization; Schrodinger wave equaqtion for hydrogen atom, separation of variable in
polar spherical coordinates and its solution, principle, azimuthal and magnetic quantum
numbers and the magnitude of their values, probability distribution function, radial
distribution function and shape of atomic orbitals (s,p & d).

Section-B
Thermodynamics: Brief resume of first and second Law of thermodynamics.
Entropy changes in reversible and irreversible processes; variation of entropy with
temperature , pressure and volume, entropy concept as a measure of unavailable energy
and criteria for the spontaneity of reaction; free energy functions and their significance,
criteria for spontaneity of a process; partial molar quantities (free energy, volume ,heat
concept), Gibb’s-Duhem equation; Classius – Clayperon equation; law of mass action
and its thermodynamic derivation. Third law of thermodynamics (Nernest heat theorem,
determination of absolute entropy, unattainability of absolute zero) and its limitation.
Phase diagram for two completely miscible components systems.

Section-C
Chain reactions: hydrogen - bromine reaction, pyrolysis of acetaldehyde, decomposition
of ethane. Photochemical reactions (hydrogen - bromine & hydrogen -chlorine
reactions). General treatment of chain reactions (ortho -para hydrogen conversion and
hydrogen - bromine reactions), apparent activation energy of chain reactions, chain
length, Rice- Herzfeld mechanism of organic molecules decomposition(acetaldehyde)
Branching chain reactions and explosions ( H2 - O2 reaction). Kinetics of (one
intermediate) enzymatic reaction : Michaelis - Menton treatment, evaluation of Michaelis
's constant for enzyme - substrate binding by Lineweaver - Burk plot, by Dixon and by
Eadie- Hofstae methods. Competitive and non-competitive inhibition.

Section-D
Ion Transport in solutions: Ionic movement under the influence of an electric field ,
mobility of ions, ionic drift velocity and its relation with current density, Einstein relation
between the absolute mobility and diffusion coefficient, the Stokes- Einstein relation , the
Nernst -Einstein equation, Waldens rule, the Rate- Process approach to ionic migration ,
the Rate process equation for equivalent conductivity, total driving force for ionic
transport, Nernst - Planck Flux equation, ionic drift and diffusion potential , the Onsager
phenomenological equations. The basic equation for the diffusion, Planck- Henderson
equation for the diffusion potential.

Here is the attachment.