Semester I Course Code Course Name Credits CHE-C 111 ... - CHE... · ... limitation of radius ratio rule, lattice defects ... chemical reactions, Baeyer’s strain theory and its

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Department of Chemistry Dr. Hari Singh Gour Vishwavidyalaya, Sagar (M.P.)

B.Sc.

Chemistry Semester - I

Semester I

Course Code Course Name Credits

CHE-C 111 Inorganic Chemistry 2

CHE-C 112 Organic Chemistry 1

CHE-C 113 Physical Chemistry 1

CHE-C 114 Laboratory Course 2

2

CHE-C 111

B.Sc. Semester I

Paper I : Inorganic Chemistry Credits : 02

30 Hrs

1. Atomic Structure : Idea of de Broglie matter wave, Heisenberg

uncertainty principle, atomic orbitals, Schrödinger wave equation,

significance of Ψ and Ψ2, Quantum numbers, radial and angular wave functions and probability distribution curves, shapes of s, p, d orbitals, effective nuclear charge.

8

2. Periodic Properties : Trends in periodic table and applications in

predicting and explaining the physical and chemical behaviors. Atomic radii, ionic radii, ionization energy, electron affinity and electro negativity.

3

3. Chemical Bonding : Valence bond theory and its limitations, directional characteristics of covalent bond, various types of hybridization and shapes of simple inorganic molecules and ions, Valence shell electron pair repulsion (VSEPR) theory to NH3 , H3O+, SF4, ClF3 , ICl2 and H2O . MO theory, homonuclear and heteronuclear (CO and NO) diatomic molecules, multicenter bonding in electron deficient molecules, bond strength and bond energy, percentage ionic character, from dipole moment and electro negativity difference. Weak interactions, Hydrogen bonding, van der Waal forces.

7

4. Ionic Solids : Concept and properties of ionic bond and structure of

ionc compounds, radius ratio effect and coordinationnumber, limitation of radius ratio rule, lattice defects, semiconductors, lattice energy and Born – Haber cycle, Solvation energy and solubility of ionic solids, polarizing power and Polarizability of ions, Fajan’s rule. Metallic bond – free electron, valence bond theory

7

5. Chemistry of Nobel gases : Chemical properties of the Nobel gases, chemistry of Xenon, structure and bonding in xenon compounds.

5

Course Coordinator: Dr. Yadvendra Rohan

3

CHE-C-112

B.Sc. Semester I

Paper – II : Organic Chemistry

Credits : 1

15 Hrs

1. Structure and Bonding :

Hybridization, bond length and bond angles, bond energy, localized and delocalized chemical bond, inclusion compounds, clatherates, charge transfer complexes, resonance, hyperconjugation, aromaticity, inductive and field effects, hydrogen bonding.

5

2. Mechanism of Organic reactions : Curved arrow notations, drawing electron movement with arrows, half-headed and double-headed arrows, homolytic and heterolytic bond breaking. Types of reagents – electrophilic and nucleophilic. Types of organic reactions, reactive intermediates – carbocations, carbanians, free radicals, carbenes, arynes and nitrenes (with examples)

5

3. Stereochemistry : Concept of isomerism, types of isomerism, optical isomerism. Elements of symmetry, chirality, enantiomers, chiral and achiral molecules with two stereogenic centers, distereomers, threo- and erythro distereomers, meso compounds, resolution, inversion, retention and recemization. Relative and absolute configuration and sequence rules. R.S. system of nomenclature.

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Course Coordinator : Prof. S.P.Shrivastava

4

CHE-C 113

B.Sc. Semester I

Paper –III : Physical Chemistry

Credits: 1 15 Hrs 1. Mathematical Concept :

Logarithmic relations, curves sketching, linear graphs and calculation of shapes, differentiation of functions like Xn , ex , sin x, log x; maxima and minima, partial differentiation and reciprocacity relations. Integration of some useful/relevant functions; permutations and combinations; factorials; Probability.

3

2. Computers: introduction to computers, different components of a computer, hardware and software, Input – Output devices, binary numbers and arithmetic. Introduction to computer languages, Programming operating system.

3

3. Gaseous states :

vander Waals equation of state, the isotherms of vander Waal equation, relationship between critical constant and vander Waal constants. The law of corresponding states, reduced equation of state.

3

4. Molecular velocities: Root mean square velocity, average and most probable velocities. Qualitative discussion of the Maxwell’s distribution of molecular velocities, collision number, mean free path and collision diameter, liquifictions of gases based on Joule – Thomson effect.

3

5. Liquid State : Intermolecular forces, structure of liquids ( a qualitative description). Structural differences between - solids, liquids and gases. Liquid crystals, difference between liquid crystals, solid and liquid. Classification, structure of nematic and cholestric phases. Thermo-graphy and seven segment cell.

3

Course oordinator ; Prof. Farid Khan

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DEPARTMENT OF CHEMISTRY

CHE-C-114

B.Sc. Semester I - Laboratory Course Credits: 2 Inorganic Chemistry : General Instructions

Demonstration and Calibration of fractional weights, balance and knowing volumetric measurement apparatus and measurement units. Simple Mixture analysis excluding anion and cation combinations Organic Chemistry : Detection of elements – Nitrogen, Sulphur and halogens. Qualitative analysis – detection of functional groups ( phenolic, carboxylic, carbonyl, esters, carbohydrates, amines, amides, nitro and anilides etc. ) in simple organic compounds Physical Chemistry

• Chemical kinetics – hydrolysis of methyl acetate/ ethyl acetate catalyzed by H+ ions

• Effect of strength of acid on rate of hydrolysis of ester

• Effect of acid types (HCl, H2SO4) on hydrolysis of ester (Relative strength of acids )

• Preparation of arsenius sulphides sol. A comparative account of coagulating power of mono-, di- and tri-valent salts

• Surface tension determination • Percentage composition of binary mixtures of organic

solvents/water, by surface tension.

Course Coordinator Prof. S.P.Shrivastava

Books :

1. Organic Chemistry, I.L.Finar, ELBS Publication

2. Organic Chemistry, Morrison and Boyed, Prentice-Hall.

3. Organic Chemistry, Jagdamba Singh, Pragati Prakashan,

4. Fundamentals of Organic Chemistry, Soloman, John Wiley & Sons.

5. Organic Chemistry , F.A. Carry, Mc Graw Hill Pub.

6. Advanced experimental Physical chemistry, J.B.Yadav, Goel Publishing House.

7. Vogel’s text Book of practical organic Chemistry, B.S.Furniss, A.J. Hannaford, V.

Rogers, P.W.G. SSmith and A.R. Tatchell, ELBS.

8. Experimental Organic Chemistry, Vol I and II, P.R.Singh, D.S. Gupta and K.S.

Bajpai, Tata McGraw Hill.

9. A laboratory hand book of Organic qualitative analysis and separations, V.S.

Kulkarni, S.P.pathak, D. ramchandra & Co., Pune.

10. Text book of organic practical chemistry, V.S. Kulkarni, S.P.pathak, D. ramchandra

& Co., Pune.

11. Organic Chemistry, Vol I,II and III, S.M. Mukherjee, S.P.Singh and R.P.Kapoor,

Wiley Eastern Ltd. New Age International.

6

Department of Chemistry Dr. Hari Singh Gour Vishwavidyalaya, Sagar (M.P.)

B.Sc.

Chemistry Semester II

Semester II






7

CHE-C 211

B.Sc. Semester II Paper – I : Inorganic Chemistry

Credits : 2 30 Hrs 1. Chemistry of S-block and p-block elements

s - Block elements : Comparative study, diagonal relationships, salient features of hydrides, Solvation and complexation tendencies including their functions in biosystems. p- Block elements : Comparative study (including diagonal relationship) of groups 13–17 elements, compounds like hydrides, oxides,halides of group 13-16, preparations, properties and structures of borazines, borohydrides, fullerenes, carbides,fluorocarbons, silicates, basic properties of halogens, interhalogens and polyhalides.

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2. Chemistry of d- block elements : First transition series -Properties of the elements of the first transition series, their binary compounds and the complexes illustrating relative stability of their oxidation states, coordination number and geometry. Second and Third transition series – General characteristics, comparative treatments with their 3d- analogues in respect of ionic radii, oxidation state and magnetic property.

10

3. Chemistry of f- block elements : Lanthanides elements- electronic structures, oxidation states and ionic radii, lanthanide contraction, complex formation, occurrence and isolation, lanthanide compounds. Actinides elements : general features and chemistry of actinides, Similarities between the later actinides and later lanthanides.

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Course Coordinator Dr. Yadvendra Rohan

8

CHE-C 212

B.Sc. Semester II Paper-II - Organic Chemistry

Credits : 1

15 Hrs

1. Stereochemistry : Nomenclature E and Z systems, geometric isomerism in alicyclic compounds, conformation analysis of ethane and n-butane, conformation of cyclohexane, axial and equatorial bonds, Newman projection and Sawhorse formulae, Fischer and Flying Wedge foumulae.

3

2. Alkanes and Cyclo alkanes : Nomenclature, isomerism and classification of carbon atoms in alkanes. Method of formation (with special reference to Wurtz reaction, Kolbe reaction, Corey House reaction, physical properties and chemical reactions of alkanes. Mechanism of Halogenation : Cycloalkanes : methods of preparations, chemical reactions, Baeyer’s strain theory and its limitations. Ring strain in cyclopropane and cyclobutane

5

3. Alkenes and Cycloalkenes :

General method of preparation and properties of alkenes. Dehydro-halogenation, dehydration, addition reaction with mechanism. Methods of preparation and chemical reactions of cycloalkenes.

4. Arenes and Aromaticity : Resonance structures, molecular orbital structure of benzene, Huckel rule – benzenoid and non benzenoid molecules. Aromatic electrophilic substitution : General pattern of the mechanism, side chain reactions of benzene derivative with mechanism

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5. Methods of formation and chemical reactions of alkyl and aryl halides. 2 Course Coordinator Prof. S.P.Shrivastava

9

CHE-C 213

B.Sc. Semester II Paper –III - Physical Chemistry

Credits : 1 15 Hrs 1. Solid state:

Definition of space lattice, unit cell. Laws of crystallography – law of constancy of interfacial angles , law of rationality of indices, law of symmetry. Symmetry elements in crystals.

4

2. X ray diffraction in crystals: Bragg’s equation. Determination of crystal structure of NaCl, KCl and CsCl, (Laue’s method and powder method.)

2

3. Chemical Kinetics : Theories of Chemical kinetics, effect of temperature on rate of reaction, Arrhenius equation, concept of activated energy. Simple collision theory based on hard sphere model, Transition state theory (equilibrium hypothesis ), Expression for the rate constants based on equilibrium constant and thermodynamic aspects.

5

4. Photochemistry Interaction of radiation with matter, difference between thermal and photochemical processes, Laws of photochemistry, Grothus – Drapper law, stark – Einstein law. Jabolonski diagram, description of fluorescence, phosphorosence, nonradiative processes, quantum yield, photosensitized reactions, energy transfer processes.

4

Course Coordinator : Prof. Farid Khan

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CHE-C-214

B.Sc. Semester II : Laboratory Course Credits – 2 30 Hrs

Inorganic Chemistry - Tests for combination of acid radicals - General idea for interfering radicals. - Simple Acid Base Titration

Organic Chemistry - Standardisation of Thermometer and determination of melting points

of Individual and mixed components - Determination of boiling points - Purification of organic compounds by sublimation, crystallisation, - Demonstration of various distillation.

Physical Chemistry : Determination of - - Reaction rate of decomposition of iodide by H2O2 - Distribution coefficients of iodine between water and CCl4 (Kerosene) - Coefficient of viscosity of liquids - Percentage composition of binary composition of organic solvents/water

by viscosity measurements. - Viscosity of amyl alcohol/water (V/V) compositions

Course Coordinator Dr. Ritu Yadav

Books : 1. Organic Chemistry, I.L.Finar, ELBS Publication 2. Organic Chemistry, Morrison and Boyed, Prentice-Hall. 3. Organic Chemistry, Jagdamba Singh, Pragati Prakashan, 4. Fundamentals of Organic Chemistry, Soloman, John Wiley & Sons. 5. Organic Chemistry , F.A. Carry, Mc Graw Hill Pub. 6. Advanced experimental Physical chemistry, J.B.Yadav, Goel Publishing

House. 7. Vogel’s text Book of practical organic Chemistry, B.S.Furniss, A.J.

Hannaford, V. Rogers, P.W.G. SSmith and A.R. Tatchell, ELBS. 8. Experimental Organic Chemistry, Vol I and II, P.R.Singh, D.S. Gupta and

K.S. Bajpai, Tata McGraw Hill. 9. A laboratory hand book of Organic qualitative analysis and separations,

V.S. Kulkarni, S.P.pathak, D. ramchandra & Co., Pune. 10. Text book of organic practical chemistry, V.S. Kulkarni, S.P.pathak, D.

ramchandra & Co., Pune. 11. Organic Chemistry, Vol I,II and III, S.M. Mukherjee, S.P.Singh and

R.P.Kapoor, Wiley Eastern Ltd. New Age International.

11

12. Department of Chemistry 13. Dr. Hari Singh Gour University, Sagar (M.P.)

14. 15. B.Sc.

16. Chemistry 17. Semester - III

Semester III






12

CHE C – 311

B.Sc. Semester III

Paper I - Inorganic Chemistry

Credits : 1 15 Hrs 1. Coordination Compounds :

Werner’s coordination theory and its experimental verification, Effective atomic number concept, chelates, nomenclature of coordination compounds, isomerism in coordination compounds, valance bond theory of transition metal complexes

8

2. Organometallic Chemistry :

Definition, Nomenclature and classification of organo-metallic compounds, preparation, properties bonding and applications of alkyls and aryls of Li, Al and Sn metals, nature of bonding in metal carbonyls and metal ethylonic complexes

7

Course Coordinator Dr. K.K.Raj

18. 19.

13

20. CHE-C-312

B.Sc. Semester III

Paper II - Organic Chemistry

Credits : 2 30 Hrs

1. Alcohols

Classification and nomenclature: Monohydric alcohols-nomenclature, methods of formation by reduction of aldehydes ketones, carboxylic acids and esters. Hydrogoen bonding. Acidic nature, Reactions of alcohols. Dihydric alcohols - nomenclature, methods of formation, chemical reactions of vicinal glycols, oxidative cleavage [Pb(OAc)4 and HIO4] and pinacol-pinacolone rearrangement. Trihydric alcohols - nomenclature and methods of formation, chemical reactions of glycerol.

6

2. Phenols

Nomenclature, structure and bonding. Preparation of phenols, physical properties and acidic character. Comparative acidic strengths of alcohols and phenols, resonance stabilization of phenoxide ion. Reactions of phenols - electrophilic aromatic substitution, acylation and carboxylation. Mechanisms of Fries rearrangement, Claisen rearrangement, Gatterman synthesis, Hauben-Hoesch reaction, Lederer-Manasse reaction and Reimer-Tiemann reaction.

6

3. Ethers and Epoxides

Nomenclature of ethers and methods of their formation, physical properties. Chemical reactions - cleavage and autoxidation, Ziesel’s method.Synthesis of epoxides. Acid and base-catalyzed ring opening of epoxides, orientation of epoxide ring opening, reactions of Grignard and organolithium reagents with epoxides.

3

4. Aldehydes and ketones Nomenclature and structure of the carbonyl group. Synthesis of aldenydes and ketones with particular reference to the synthesis of aldehydes from acid chlorides, synthesis of aldehydes and ketones using 1,3-dithianes, synthesis of ketones from nitriles and from carboxylic acids. Physical properties

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5. Mechanism of nucleophilic additions to carbonyl group with particular emphasis on benzoin, aldol, Perkin, Knoevenagel condensations. Condensation with ammonia and its derivatives.Wittig,Mannich reaction. Use of acetals as protecting group. Oxidation of aldehydes, Bayer-Villiger oxidation of ketones, Cannizzaro reaction. MPV, Clemmensen, Wolff-Kishner, LiAlH4 and NaBH4 reductions. Halogenation of enolizable

ketones. An introduction to α-, β-unsaturated aldehydes and ketones.

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Course Coordinator Prof. Mrs. S.D.Shrivastava

21.

14

22. 23.

CHE C – 313

B.Sc. Semester III

Paper III - Physical Chemistry

Credits : 1 15 Hrs

1 Thermodynamics I :-

Heat capacity, heat capacities at constant volume and pressure and their

relationship.Joule’s law – Joule – thomson coefficient and inversion temperature .

Calculation of w, q, dU & dH for the expansion of ideal gases under isothermal and

adiabatic conditions for reversbile process. Temperature dependence of enthalpy .

Kirchhoff’s equation.

Second law of thermodynamics: need for the law , different statements of the law.

Carnot cycle and it’s efficiency, Carnot theorem. Themodynamic scale of temperature

4

2 Themodynamics II :-

Concept of entropy as a sate function ,entropy as a function of V & T ,entropy as a

function of P & T ,entropy change in physical changes , Clausius inequality ,entropy as a

criteria of spontaneity and equilibrium .Entropy change in ideal hases and mixing of

gases.

Third law of thermodynamics : Nernst heat theorem ,statement and concept of residual

entropy ,evaluation of absolute entropy from heat capacity data .Gibbs and Helmoltz

functions ; Gibbs function (G) and Helmoltz function (A) as thermodynamics quantities,

A & G as criteria for thermodynamics equilibrium and spontaneity , their advantage over

entropy change .Variation of G & P , V & T

4

3 Chemical Equilibrium :-

Equilibrium constant and free energy .Thermodynamics derivation of law of mass action

.Le Chatlier’s principle .Reaction isotherm – reaction isochore – Clapeyron equation and

Clausius – Clapeyron equation , applications.

4

4 Phase Equilibrium :-

Statement and meaning of the terms – phase ,component and degree of freedom ,

derivation of Gibbs phase rule ,phase equilibria of one component system – water ,

Carbon dioxide and S systems .

Phase equilibria of two component system - solid liquid equlibria .simple eutectic – Pb-

Ag system ,desilverisation of lead .

Solid solutions – compound formation with congruent melting point (Mg-Zn) and in

congruent melting point (Ferric Chloride – Water) .

3

Course coordinator Shri R. C. Pawar

24. 25.

26.

15

27.

CHE-C-314

B.Sc. Semester III - Laboratory course Credits 2

Inorganic Chemistry :

Calibration of Fractional Weights, pipettes and Burettes.

Quantitative Analysis : (A) Volumetric analysis

Determination of Oxalic acid strength by titrating with NaOH

Estimation of Oxalic Acid by Redox KMnO4 titration

Determination of Acetic acid in commercial vinegar using NaOH

Determination of Alkali content in antacid tablet using HCl

Estimation of Fe2+

and Fe3+

by Redox K2Cr2O7 titration

Estimation of Cu2+

by Na2S2O3

Quantitative Analysis : (B) Gravimetric analysis

a.Analysis of Copper as CuCNS ; b. Zn as ZnNH4PO4.; c. Estimation of Barium as Barium sulphate.

Organic Chemistry:

Element detection by (Green Chemical Analysis) and conventional methods

Identification of Organic Compounds ( Carboxylic acids, carbohydrates, amides, phenols, ketones,

hydrocarbon, amines,nitro, halogen and sulphur containing compounds)

Physical Chemistry:

Transition Temperature :

Determination of Transition temperature of the given substance by thermometric / Dialometric

method. [eg MnCl2.4H2O / CuSO4.5H2O/SnCl2.2H2O/ Na2 SO4H2O].

Phase equilibrium :

To construct the phase diagram of two component ( Diphenyl amine – Benzophenone) system by

cooling curve method.

Thermochemistrty :

To determine the solubility of organic acids (benzoic acid, salicyclic acid etc). at different

temperatures and to determine ∆H of the dissolution process.

Basicity of an acid by thermochemical methods. To determine the heat of solution of KNO3 by

solubility method.

Kinetics

Study of Kinetics of enzymatic reaction (starch – amylase system)


16

Department of Chemistry Dr. Hari Singh Gour University, Sagar (M.P.)

B.Sc.

Chemistry Semester IV

Semester IV


CHE-C-411 Inorganic Chemistry 1

CHE-C-412 Organic Chemistry 2

CHE-C-413 Physical Chemistry 1

CHE-C-414 Laboratory Course 2

17

CHE C – 411 B.Sc. IV Semester

Paper I - Inorganic Chemistry Credits - 1 15 Hrs 1. Hard and Soft Acids and Bases (HSAB)

Bronsted-Lowery theory of Acids and Bases and Lewis Concepts of acid and base. Classification of acids and bases as hard and soft. Pearson’s HSAB concept, acid base strength and hardness. Softness, symbiosis theoretical basis of hardness and softness, electro-negativity and hardness and softness

8

2. Bio-inorganic Chemistry

Essential and trace elements in biological processes, metallo porphyrins with special reference to haemoglobin. Biological role of alkali and alkaline earth metal ions with special reference to Ca2+.

7

Course Coordinator Dr K.K. Raj

18

CHE-C-412

B.Sc. Semester IV

Paper-II - Organic Chemistry Credits : 2 30 Hrs

1. Carboxylic Acids

Nomenclature, structure and bonding, physical properties, acidity of Carboxylic acids, effects of substituents on acid strength, Preparation of carboxylic acids. Reactions of carboxylic acids. Hell-Volhard-Zelinsky reaction. Synthesis of acid chlorides, esters and amides. Reduction of carboxylic acids, Mechanism of decarboxylation. Methods of formation and chemical reactions of unsaturated monocarboxylic acids Dicarboxylic acids: methods of formation and effect of heat and dehydrating agents.

6

2. Carboxylic Acid Derivatives

Structure and nomenclature of acid chlorides, esters, amides (urea) and acid anhydrides. Relative stability of acyl derivatives physical properties, interconversion of acid derivatives by nucleophilic acyl substitution. Preparation of carboxylic acid derivatives, chemical reactions. Mechanisms of esterification and hydrolysis (acidic and basic)

3

3. Organic Compounds of Nitrogen

Preparation of nitroalkanes and nitroarenes. Chemical reactions of nitroalkanes. Mechanism of nucleophilic substitution in nitroarenes and their reductions in acidic, neutral and alkaline media. Picric acid. Halonitroarenes: reactivity. Structure and nomenclature of amines, physical properties. Stereochemistry of amines. Separation of mixture of primary, secondary and tertiary amines. Structural features effecting basicity of amines. Amine salts as phase-transfer catalysts. Preparation of alkyl and aryl amines (reduction of nitro compounds, nitriles), reductive amination of aldehydic and ketonic compounds. Gabriel-phthalimide reaction, Hoffmann bromide reaction.

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4. Electromagnetic Spectrum: Absorption Spectra Ultraviolet (UV) absorption spectroscopy - absorption laws (Beer- Lambert law), molar absorptivity, presentation and analysis of UV spectra, types of electronic transitions, effect of conjugation. Concept of chromophore and auxochrome. Bathochromic, hypsochromic, hyperchromic and hypochromic shifts. UV spectra of conjugated enes and enones. Infrared (IR) absorption spectroscopy - molecular vibrations, Hooke’s law, selection rules, intensity and position of IR bands, measurement of IR spectrum, fingerprint region, characteristic of various functional groups and interpretation of IR spectra of simple organic compounds.

9


19

CHE-C–413

B.Sc. Semester IV

Paper III - Physical Chemistry Credits : 1 15 Hrs

1. Partially miscible liquids Phenol - Water, trimethylamine – water, nicotine – water system. Lower and

upper absolute temperature, Effect of impurity on absolute temperature,

Immiscible liquids, steam distillation, Nernst distribution law –

thermodynamic derivation, applications.

3

2. Electro chemistry I Migration of ions and Kohlrausch law, Debye–Huckel–Onsager equation for

strong electrolytes (elementary treatment only),Transport number, definition

and determination by Hittorf method and moving boundary method,

Applications of conductivity measurement : determination of degree of

dissociation , determination of dissociation constant of acid , solubility of a

sparingly soluble salt , conductometric titrations

4

3. Electro-chemistry II Types of reversible electrodes - gas – metal ion , metal – metal ion, metal –

insoluble salt – anion and redox electrode . Electrode reactions, Nernst

equation , derivation of cell E.M.F and single electrode potential.

Electrolytic and Galvanic cells – reversible and irreversible cells ,

Representation of electro chemical cells .Calculation of thermodynamic

quantities of cell reaction (∆G, ∆H & K) , polarization , over potential and

hydrogen overvoltage .

4

4. Electro chemistry and corrosion Concentration cell with and without transport , liquid junction potential,

application of concentration cells – valency of ions , solubility product and

activity coefficient .

Defination of pH and pKa, determination of pH using hydrogen, quinhydrone

and glass electrodes by potentiometric method. Corrosion – types , theories

and methods of combating it .

4

Course Coordinator Shri R. C. Pawar

.

20

CHE-C-414

B.Sc. Semester IV Laboratory Course

Credits : 2

Inorganic Chemistry :

Quantitative Analysis : Volumetric analysis

Estimation of calcium concentration in chalk as Calcium oxalate by KMnO4

Estimation of hardness of Water by EDTA titration

Complexometric titration of Zn(II), Mg(II), Fe(II) with EDTA

Estimation of percentage of available chlorine in bleaching powder

Estimation of K2Cr2O7 (by titration with Na2S2O3)

Gravimetric analysis

Preparation and Analysis of Nickel as Ni(DMG)2 and Al(III) and Mg(II) using suitable

reagents.

Organic Chemistry:

Synthesis of following by (Green Chemical synthesis) and conventional methods

Acetylation of primary amines, Base catalysed aldol condensation, halogen addition to C=C

(carbon - carbon), [4+2] cycloaddition reaction.

Thin layer chromatography ; Determination of Rf values and identification of organic compounds

and separation of green leaves pigments.

Preparation and separation of 2,4- dinitro phenyl hydrazones of acetone,2-butanone, hexane – 2-

one and hexane – 3- one using toluene and light petroleum ether (40:60)

Separation of a mixture of dyes using cyclohexane and ethyl acetate (8.5:1.5).

Paper Chromatography : Ascending

Determination of Rf values and identification of organic compounds: amino acids and

monosacchrides

Physical Chemistry:

Phase equilibrium :

Determination of critical solution temperature of Phenol Water system.

Effect of Impurity on Critical Solution temperature.

Thermochemistrty :

To determine the heat of neutralization (strong acid – strong base)/Weak acid-weak base)

Determine the enthalpy of ionization.

To determine heat of solution of NH4NO3 / CaCl2.

Molar Mass

Determination of molar mass of a given polymer sample by viscosity measurement.

Course Coordinator Prof. S.K.Shrivastava

21


B.Sc.

Chemistry Semester V

Semester V






22

CHE C – 511

B.Sc. Semester V

Paper I – Inorganic Chemistry

Credits : 1 15 Hrs

1. Metal ligand Bonding in Transition metal complexes :

Limitations of valance bond theory, an elementary idea of crystal field theory,

crystal field splitting in octahedral, tetrahedral and square planer complexes, factors

affecting the crystal field parameters

8

2. Magnetic Properties of Transition Metal complexes :

Types of magnetic behaviours, method of determining magnetic susceptibility, spin

only formula, L-S coupling, correlation of and effective values, orbital

contribution to magnetic moments, applications of magnetic moment data for 3d-

metal complexes.

7

Course Coordinator Dr. K. K. Raj

CHE - C – 512

B.Sc. Semester V

Paper II – Organic Chemistry

Credits : 1 15 Hrs 1. Carbohydrates

Introduction and classification, osazone formation, mutual transformation, epimerisation, cyclic structure of glucose and fructose , mutarotation, General idea about disaccharides and polysaccharides, structure of sucrose, maltose, lactose and starch.

3

2. Fats , Oils and detergents Introduction, glycerides, hydrogenation of unsaturated oils, acid value, saponification value, iodine value, synthetic detergents,

3

3. Amino Acids, Peptides, Proteins

Introduction, classification of amino acids, acid base behaviours, iso-

electric point of amino acids, α-amino acid-preparation properties and physiological importance, peptide synthesis – classical and solid phase . End group analysis of amino acids, detection, classification and importance of proteins.

4

4. Synthetic Dyes Introduction, colours and constitution, chromophore, auxochrome and valency bond theory, synthesis of methyl orange, congo red, malachite green, crystal violet, phenolphthalein, fluorescein, indigo

5

Course Coordinator Prof. A. K. Banerjee

23

CHE- C – 513 B.Sc. Semester V

Paper III – Physical Chemistry Credits : 2 30 Hrs

1. Quantum Mechanism-I

Black body radiation, Plank’s radiation law, photoelectric effect, heat capacity of solids, Bohr’s model of Hydrogen atom (no derivation) and its defects, Compton Effect De-Broglie hypothesis, Heisenberg’s uncertainty principle, sinusoidal wave equation and its importance, physical interpretation of the wave function, postulates of quantum mechanism, particle in one dimensional box.

12

2. Quantum Mechanics-II Schrodinger wave equation for H- atom, separation into three equations (without derivation), quantum numbers and their importance, Hydrogen like wave functions, radial wave function, angular wave function Molecular orbital theory, basic idea- criteria for forming MO from AO, construction of MO’s by LCAO-H2

+ ion, calculation of energy levels from wave function, physical picture of bonding – anti

bonding, wave function, concept of σ ,σ∗ , π, π∗, orbitals and their characteristics. Hybrid orbitals – sp, sp2, sp3, calculation of coefficient of AO’s used in these hybrid orbitals. Introduction to valance bond models of H2, comparison of MO and VB models.

12

3. Spectroscopy

Introduction; electromagnetic radiation of the spectrum, basic features of different spectrometers, statement of Born-Oppenheimer Approximation, degree of freedom

2

4. Rotational Spectra Di atomic molecules, energy levels of a rigid rotors (semi classical principles), Selection rules, spectral intensity, distribution using population distribution (Maxwell-Boltzmann distribution) determination of bond length, qualitative description of non-rigid rotor, isotope effect.

4

Course Coordinator Dr. Vijay Verma

24

CHE-C-514

B.Sc. Semester V

Laboratory Course

Credits : 2 1. Inorganic :

Synthesis and Analysis

Preparation of sodium trisoxalato ferrate (III) Na3[Fe(C2O4)3] and determination of its

composition by permangnetometry

Estimation of copper and nickel (should be given in solution form).

Preparation of Copper tetraamine complex, [Cu(NH)3]SO4

Preparation of cis and trans bisoxalato diaqua chromate (III) ion.

2. Organic

Separation of fluorescene and methyl blue ; leaf pigments from spinach leaves.

Qualitative Analysis ;

Analysis of an organic mixture containing two solid components using water,NaOH and

NaHCO3 for separation and preparation of derivatives

3. Physical

Electrochemistry :

Conductometrically determine the strength of the given acid using standard alkali solution

Conductometrically determine the solubility of a sparingly soluble electrolyte

Conductometrically determine the rate of saponification of ethyl acetate

Conductometrically determine the ionisation constant of a weak acid

To titrate potentiometrically the given FAS ferrous ammonium sulphate solution using

KMnO4 / K2Cr2O7 as titrant and calculate the redox potential of Fe++/ Fe+++ system on

the hydrogen scale.

Course Coordinator Prof. O. P. Chourasia

25


B.Sc.

Chemistry Semester VI

Semester VI






26

CHE - C – 611

B.Sc. Semester VI

Paper – I : Inorganic Chemistry Credits : 1 15 Hrs

1. Electronic Spectra of transition metal complexes

Types of electronic transitions, selection rules for d-d transitions, spectroscopic

ground states, spectro-chemical series, Orgel energy level diagram for d1+

and d9

states, discussion of the electronic spectrum of [Ti(H2O)]3+

complex ion.

7

2. Thermodynamic and Kinetic aspects of Metal complexes

A brief outline of thermodynamic stability of metal complexes and factors

affecting the stability, substitution reactions of square-planer complexes

5

3. Silicones and Phosphazines

Silicones and Phosphazenes as complexes of inorganic polymers, nature of

bonding in triphosphazenes

3

Course Coordinator Dr. K.K.Raj

CHE - C – 612

B.Sc. Semester VI

Paper II - Organic Chemistry Credits : 1 15 Hrs 1. Organo-metallic Compounds

Organo magnesium, organo zinc and organo lithium compounds – preparation properties

and structure

4

2. Synthetic Polymers

Introduction, addition and condensation polymerization, Zeigler Natta reaction, Some

important polymers – polyesters, polyamides, phenol formaldehyde resin, urea

formaldehyde resin, polyureathane, epoxy resin, rubber (natural and synthetic)

4

3. Heterocyclic compounds

Introduction, pyrroles, furan, thiophene, pyridine – preparation, properties and structure,

condensation ring system, Fischer – Skraup and Bischler – Napieralski reaction, Properties

and structure of indole, quinoline and isoquinoline.

4

4. Organic synthesis via enolates :

Introduction, dimethyl malonate, ethylacetoacetate – preparation and properties, keto

enol tautomerism of ethylacetoacetate, enamines.

3

Course Coordinator Prof. A.K.Banerjee

27

CHE - C – 613

B.Sc. Semester VI

Paper – III : Physical Chemistry Credits : 2 30 Hours 1. Electronic Spectrum

Concept of potential energy curves for bonding and anti bonding molecular orbitals, quantitative description of selection rules and Frank Condon principle

4

2. Vibrational Spectrum

Infra red spectrum, energy levels of simple harmonic oscillators, selection rules, pure vibrational spectrum, intensity, determination of force constant and qualitative relation of force constant and bond energies, effect of anharmonic motion and isotope on spectrum, idea of vibrational frequencies of different functionl groups.

8

Raman Spectrum Concept of polarizability, pure Rotational and pure vibrational Raman spectra of diatomic molecules, selection rules

3. Physical properties and Molecular structures : Optical activity, polarization, - (Clausius – Mossotti equation) orientation of dipoles in an electric field, dipole moment, induced dipole moment, measurement of dipole moment – temperature method and refractivity method, dipole moment and structure of molecules, magnetic properties, paramagnetism, dimagnetism and ferromagnetism .

9

4. Solutions, Dilute Solutions and Colligative Properties Ideal and non ideal solutions, method s of expressing concentration of solutions, activity and activity coefficients Dilute solutions, colligative properties, Roult’s law, relative lowering of vapour pressure, molecular weight determination, Osmosis, law of osmotic pressure and its measurement, determination of molecular weight from osmotic pressure, Elevation of boiling point and depression of freezing point, Experimental methods for determining various colligative properties. Abnormal molar mass, degree of dissociation and association of solutes.

9

Course Coordinator Dr. Vijay Verma

28

CHE - C – 614

B.Sc. Semester VI

Laboratory Course Credits 2 Inorganic : Instrumentation

• Colorimetry : Job’s Method, Mole ratio method

• Explain the electronic spectra for KMnO4 / K2Cr2O7

• Adulteration in food stuffs, Effluent analysis,

• Solvent Extraction: Separation of acids/ Mg(II) and Fe(II)

• Ion Exchange methods : Separation Mg(II) and Fe(II)

Organic : Synthesis

• Acetylation of salicylic acid , aniline, glucose and hydroquinone,

benzoylation of aniline and phenol.

• Aliphatic electrophilic substitution : Preparation of Iodoform from ethanol

and acetone.

• Aromatic electrophilic substitution: Nitration, preparation m-dinitrobenzene,

preparation of para-nitroacetanilide.

• Halogenation : Preparation para-bromo acetanilide; preparation of 2,4,6 tri

bromo phenol,

• Diazotization / Coupling : Preparation of methyl orange and methyl red.

• Oxidation : Preparation of bnzoic acid from toluene,

• Reduction : Preparation of aniline from nitrobenzene, preparation of meta

nitro aniline from meta dinitro benzene.

Physical

• Refractometry :Polarimetry

o To verify law of refraction of mixtures (glycerol and water) using

Abbe’s refractometer.

o To determine the specific rotation of given optically active

compound.

• Molecular Weight determine :

o Determination of molecular weight of a non volatile solute by rast

method / Beckman freezing point method.

o Determination of the apparent degree of dissociation of an electrolyte

(NaCl) in aqueous solution at different concentration by

ebullioscopy.

• Colorimetry :

o To verify Beer-Lambert law for KMnO4 / K2Cr2O7 and determine the

concentration of the given solution of the substance.

• Potentiometry

• To determine the strength of given strong and weak acid by potentiometric

titration using (i). Platinum – quinhydron, glass electrode.

Course Coordinator Shri R. C. Pawar

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All Syllabi : Department of Chemistry

UG Chemistry

• UG Chemistry Semester I 2013-14

• UG Chemistry Semester II 2013-14

• UG Chemistry Semester III 2013-14

• UG Chemistry Semester IV 2013-14

• UG Chemistry Semester V 2013-14

• UG Chemistry Semester VI 2013-14

PG Chemistry

• PG Chemistry Semester I 2013-14

• PG Chemistry Semester II 2013-14

• PG Chemistry Semester III 2013-14

• PG Chemistry Semester IV 2013-14

UG Industrial Chemistry

• UG Industrial Chemistry Semester I 2013-14

• UG Industrial Chemistry Semester II 2013-14

• UG Industrial Chemistry Semester III 2013-14

• UG Industrial Chemistry Semester IV 2013-14

• UG Industrial Chemistry Semester V 2013-14

• UG Industrial Chemistry Semester VI 2013-14

PG Industria Chemistry • PG Industrial Chemistry Semester I 2013-14

• PG Industrial Chemistry Semester II 2013-14

• PG Industrial Chemistry Semester III 2013-14

• PG Industrial Chemistry Semester IV 2013-14

UG Pharmaceutical Chemistry

• UG Pharmaceutical Chemistry Semester I 2013-14

• UG Pharmaceutical Chemistry Semester II 2013-14

• UG Pharmaceutical Chemistry Semester III 2013-14

• UG Pharmaceutical Chemistry Semester IV 2013-14

• UG Pharmaceutical Chemistry Semester V 2013-14

• UG Pharmaceutical Chemistry Semester VI 2013-14 and

• UG Pharmaceutical Chemistry Semester V 2014-15

• UG Pharmaceutical Chemistry Semester VI 2014-15

Ph.D. (By course work) Chemistry

• Ph.D. Chemistry Semester I 2013-14

• Ph.D. Chemistry Semester II 2013-14

Documents

Semester I Course Code Course Name Credits CHE-C 111 ... - CHE... · ... limitation of radius ratio rule, lattice defects ... chemical reactions, Baeyer’s strain theory and its