CHEMISTRY HONOURS_Bsc part 3 syllabus

 

CHEMISTRY (HONOURS)
PAPER-V (THEORY)
PHYSICAL CHEMISTRY

Time-3 Hours. Full Marks-100

In all nine questions are to be set. The question 1 is objective (I x 20

marks) and will screen the entire paper. Student will be required to answer five questions of which question 1 is compulsory.

1. Elementary Quantum Mechanics 

-Black body radiation. Planck

radiation law, Photo-electric effect, heat capacity of solids Bohr's model of hydrogen atom (no derivation) and its defects. Compton effect. De-Broglie hypothesis, the Hsisenberg's uncertainty principle. Sinusoidal wave equation Hamiltoian operator. Schrodinger wave equation and its importance, Physical

interpretation of the wave function Postulates of quantum mechanics, Particle in a one dimensional box.

Sclrodinger wave equation for H-atom, Separation in three equations (without derivation). Quantum numbers & their importance hydrogen like

wave functions, radial wave functions, angular wave functions.

2. Spectroscopy  -Introduction, electromagnetic, radiation, regions of the spectrum, basic features of different spectrometers, statement of the Born Oppenheimer approximation.

Rotational Spectrum :-

 Diatomic molecules, Energy levels of a rigid rotator (semi-classical principles), selection rules, spectral intensity, distribution using population distribution (Maxwell Boltzmann distribution) determination of bond length, qualitative description of non-rigid rotator, isotope effect.

Vibrational Spectrum -Infrared spectrum, Energy levels of simple

harmonic oscillator 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 the spectrum

idea of vibrational frequencies of different functional group .

Raman spectrum, concept of polarizability, pure rotational and pure vibrational Raman spectra of diatomic molecules, selection rules.

Electronic Spectrum-

Concept of potential energy curves for bonding

and antibonding molecular orbital qualitative description of selection rules and Franck-Condon Principles.

Qualitative, description of . and n M. O .their energy levels and the

respective transitions.

3. Photochemistry -

Interaction of radiation with matter, differences

between thermal and photochemical processes, laws of photochemistry,

Grothus - Drapper law. Stark - Einstein law. Jablonski diagram depicting various processes occuring in the excited State, qualitative description of flurenscence, phosphorescence, non-radiative processes (internal conversion, intersystem crossing) quantum yield, photosensitized reactions energy transfer processes (simple examples).

4. Physical properties And Molecular Structure -

Optical activity, polarization- (clausius Mossotle eqn). 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, paramagnetism and

feeromgnetics.

5. Electrochemistry II :-

Type of reversible electrodes -gas metal ion, metal-metal ion, metal soluble salt anion and redox electrodes. Electrodes reactions, Nernest equation, derivation of cell E.M.F. and single electrodes potential, standard hydrogen electrode-reference electrodes -standard electrode, potential ,sign conventions, electrochemical series and its significance.

Electrolytic and Galvanic cells-reversible and inreversible cells, conventional representation of electro-chemical cells.

B.M.F. of a cell and its measurements, Computation of cell E.M.F. Calculation of thermodynamic quantities of cell reactions (AG, AH and K). Polarization over potential and hydrogen overvoltage concentration cell with,

and without transport, liquid junction potential, application of Concentration cells, valency of ions, solubility product and activity co-efficient potentiometric titrations.

Definition of pH and pka, determination of pH using hydrogen,

quinhydrone and glass. electrodes. Buffers; mechanism of buffer action,

enderson equation Hydrolysis of salts.

Corrosion-types, theories and methods of combating it.

6. Statistical Thermodynamics- 

Partition function: Interpretation of

the partition function; Translational, rotational vibrational and electronic

partition function. Expressions of internal energy enthalpy, entropy and Gibbs free energy in terms of Partition function.)

INORGANIC CHEMISTRY (THEORY)
PAPER-VI

Full Marks-100

Time-3 Hours

In all nine questions are to be set. The question I is objective (1 × 20

marks) Students will be required to answer five questions of which question 1 is Compulsory.

1. Metal-ligand Bonding in Transition Metal Complexes

Limitations of valence bond theory, an elementary idea of Crystal-field theory

Crystal field splitting in octahedral, tetrahedral and square planar

Complexes, factors affecting the Crystal-field parameters.

II. Magnetic Properties of Transition Metal Complexes -

Types of magnetic behavior, methods of determining magnet Susceptibility. spin-only formula. L-S coupling, correlation of and eff values. orbital contribution to magnetic moments, application of magnetic moment data for 3d -metal complexes.

III. Electron Spectra of Transition Metal Complexes-

Types of electronic transitions. selection rules for d-d transitions, spectroscopic ground states, spectrochemical series. Orgel energy level diagram for d'1and d'9 states

discussion of the electronic spectrum of [Ti(H2O) ]2+complex ion.

IV. Thermodynamic and Kinetic Aspects of Metal Complexes-

A brief outline of thermodynamic stability of metal complexes and factors affecting the stability. substitution reaction of square planar complexes.

V.Qrganometallic Chemistry 

Definition, nemenclature and

classification of organometalic componads, Preparation, properties, bonding and application of alkyls and aryls of Li, Al, Hg, Sn and Ti, a brief account of metal-ethylenic complexes and homogeaneous hydrogenation, mononuclear

carbonyls and the nature of bonding in metal carbonyls.

VI. Bio Inorganic Chemistry :-

Essential and trace elements in

biological processes, metalloperphyrins with special reference to hemoglobin and myoglobin Biological role of alkali and alkaline earth earth metal ions with special reference to Ca2+ Nitrogen fixation.

VII. Silicones and Phosphazenes

Silicones and phosphazenes as

examples of inorganic polymers. nature of bonding in triphosphazenes.

VIlI. Chemistry of Actinides

 General features and chemistry

actinides chemistry of separation of Np,Pu and Am, from U, similarly between the latter actinides and latter lanthenids.

ORGANIC CHEMISTRY (THEORY)
PAPER- VII

Time-3 Hours Full Marks-100

In all nine questions are to be set. The question 1 is Objective (1 x 20

marks). Students will be required to answer five questions of which question1 is compulsory.

1. Spectroscopy

 Nuclear Magnetic Resonance. Chemical shift and structure, Nuclear Shielding and deshielding, spin-spin splitting and cumpling constants, identification of kinds of protons, Areas and peaks, Interpretation

of PMR spectra of simple organic molecules such as ethyl bromide, ethanol acetaldehyde, 1, 1, 2-tribromoethane. ethyl acetate toluene and acetophenone

Problems pertaining to the structure elucidation of simple organic molecules using UV, IR and PMR spectros. copic technique.

2. Mechanism of organic reactions -

 Nucleophilic substitution at

saturated carbon atom study with reference to kinetics (SN1 and SN2)

Mechanism and Evidence, Stereochemistry, Effect and structure of organic chain, nucleophilic polarity of solvent and leavin group. Elimination Reactions- Study with reference Kinetics (E1 and E2 ).

Mechanism, Evidences, Mechanistic Variable Stereochemistry, Satnya

Zeff's rule. Hofmann's elimanation.

3. Condensed Poly nuclear Hydrocarbons - 

Napthalene. Anthracene and phenanthrene-Physic properties, Chemical properties, Structure, Synthesis Derivatives of nephthalene, anthracene and phenanthrene Molecules Overcrowding.

Heterocyclic Compounds- 

Introduction: Molecular orbital picture

and aromatic characteristics of pyrrole furan, thiophene and pyridine, Methods of synthesis and chemical reactions with particular emphasis on themechanism of electrophilic substitution. Mechanism of nucleophilic substitution reactions in pyridine derivatives. Comparison of basicity of pyridine piperidine and pyrrole

Introduction to condensed five and six membered heterocyclic, Preparation and reactions of indole, quinoline and isoquinoline with special reference to Fisher indole synthesis, Skraup's synthesis and Bischler Napieralski synthesis. Mechanism of electrophilic substitution reactions of indole, quinoline and isoquinoline.

5. Name Reaction:-

Perkin Reaction, Ma nich Reaction, Micheal Reaction, Beckmann's Rearrangement Fries Rearrangement, Caiseu

Rearrangement, Arndt- Eistert synthesis, Darzen's glycidic Ester synthesis, Hofmann's Exhaustive methylation.

6. Ureide and Uric acid-Xanthene, Caffeine.

7. Plant Pigments -Anthocynins, flavones and Isofianones

8. Amino Acids, Peptides, Proteins & Nuclic Acids -

Classification, structure and stereochemistry of amino acids, Acid-base behaviour, isoelective point and electro-phoresis. Preparation and reactions or a-amino acids.

Structure and Nomenclature of peptides and proteins. Classification of proteins, Peptide structure determination and group analysis, selective hydrolysis of peptides. Classical peptide synthesis, Solid-phase peptide synthesis. Structure of peptides and proteins. Levels of protein structure. Protein denaturation/renaturation.

Nucleic Acid-

Introduction. Constituents of nucleic acid Ribonucleside and ribonucleotides. The double helical structure of DNA.

9. Synthetic Dyes :-

Colour and constotion (electron ic concept). Classification of dyes, Chemistry and Synthesis of Methyl Orange, Congo red, Malachite green, crystal violet, Phenolthalein , Fluorescein, Alizarin and

Indigo.

 PAPER VIII (PRACTICAL)

Time-6 hours

Full Marks-100

Group-A (40 Marks)

1.Determination of molecular weight of volatile liquids by Victor Meyer

method.

2. Determination of surface tension of liquid using stalagamo meter and

calculation of Paracbor values.

3. Determination of co-efficeant of viscosity of liquids using Ostwald

Viscometer.

4. Determination of partition co-efficeant of solutes between two immiscible liquds.

5. Determination of rate constant for hydrolysis of Ester catalysed by

H+ions at room temperature.

6. Thermochemistry: Heat of solution of solute in a solvent, heat of

neutralistion.

GROUP B (40 Marks)

1. Gravimetric Analysis :- Estimations of Ag+, Ba+2, Ni+2, Cu+2, Cil-

and SO4^-2

GROUP - C

10+ 10 Marks

Record of class work and viva-voce.

Note: One experiment from Group (A) and one from Group (B) to be

set for each candidate.

Group (B) to be set for each Candidate.

CHEMISTRY HONOURS_Bsc part 2 syllabus

 CHEMISTRY PAPER III (Hons.)- Physical Chemistry

Time: 3 Hours ] Full Marks: 50

In all nine questions are to set. The Q. No. 1 will be objective 10 marks and will Screen the entire paper, Students will be required to answer five questions of which question 1 will be compulsory.

1. THERMODYNAMICS

Definition of thermodynamic terms: 

System Surroundings etc. Types of systems, intensive & extensive properties. State & path functions & their differentials, Thermodynamic process, Concept of heat & work.

First Law of Thermodynamics:

Statement, definition of internal energy & enthalpy. Heat capacity, heat capacities at constant volume & pressure & their relationship. Joul's law-Joule-Thomson coefficient & inversion temperature. Calculation of w.q. dU & dH for the expansion of ideal gases under isothermal & adiabatic conditions for reversible process.

Thermochemistry

Standard enthalpy of formation, Hess' Law of heat summation & its

applications. Heat of reaction at constant pressure & at constant volume.

Enthalpy of neutralization, Bond dissociation energy & its calculation from thermo-chemical data, temperature dependence of enthalpy, Kirchoff's equation

2. THERMODYNAMICS

Second Law of thermodynamics need for the law. different statements of the law Carnot cycle & its efficiency. Carnot theorem. Thermodynamic scale of temperature.

Concept entropy. entropy as a state function, entropy as a function of V

&T. entropy as criteria of spontaneity & equilibrium. Entropy change in ideal gases & mixing of gases.

Third law of thermodynamics

Nernst heat theorem, statements & concept of residual entropy. evaluation of absolute entropy from heat capacity data. Gibbs & Helmholtz functions. Gibbs function (G) & Helmholtz function (A) as thermodynamic quantities. A &

G as criteria for thermodynamic equilibrium & spontaneity, their advantage Over entropy change variation of G & A with P. V. & T. equilibrium constant & free energy. Reaction isotherm & reaction isoehore clapeyron equation.

Clausius Clapeyron equation) applications, Thermodynamic derivation of relation between molecular weight & elevation in boiling point & depression in freezing point.

3. LIQUID STATE:

intermolecular forces, structure of liquids (a qualitative description).

Structural differences between solids, liquids & gases.

   Liquid crystals Differences between liquid crystal, solid, liquid, Classification, Structure of nematic & phases. Thermography & seven segment cell.

4. PHASE EQUILIBRIUM:

Statements & meaning of the terms Phase, component & degree of

freedom, derivation of Gibbs phase rule, phase equilibria of one component system- water, CO2 & S system.

Phase equilibria of two componant system-Solid-liquid equilibria. simple

eutectic-bi-Cd Pb-Ag systems, desilverisation of lead.

  Solid solutions:

 Compound formation with congruent melting point (Mgzn) & in-congruent melting point. (Nac-H2o). (Fecl3-H20) system 

 Liquid Liquid mixtures

 Ideal liquid mixtures, Raoults & Henry's law Non-ideal system-azeotropes (enthanol water) system.

Partially miscible liquids - Phenol water, trimethyl amine- water systems, Lower & upper consolute temperature Effect of impurity on Consolute temperature

Immiscible Liquids, steam distillation Nernst distribution Law Thermodynamic derivation, applications.

5. ELECTRO CHEMISTY-

 Electrical transport-Conduction in metals & in electrolyte solutions, specific conductance & eguivalent conductance, measurement of equivalent conductance, variation of equivalent & specific conductance with dilution 

Migration of ions & kohlrausch law, Arrhecius theory of electrolytic

dis sociation & its limitations, weak & strong electrolytes Qustwalds, dilution law its uses & limitations Debye-Huckle-Onsagers.equn for strong electrolyte &(elementary treatment only). Transport number, definition & determination

by Hittorf method & moving boundary method

Applications of conductinity measurements, determination of degree of dissociation, determination of Ka of acids, determination of solubility. Product of sparingly soluble salt, conductomatic titration.

CHEMISTRY PAPER IV-Inorganic Chemistry

Time: 3 Hours] [Full Marks: 50

In all nine questions are to set. The Q. No. 1 will be objective 10 marks

and will Screen the entire paper, Students will be required to answer five questions of which question 1 will be compulsory.

1. Chemistry of Elements of First Transition Series

Characteristic properties of d-block elements

Properties of the elements of the first transition series their binary compounds and complexes illustrating relative stability of their oxidation states, coordination number and geometry.

2. Chemistry of Elements of Second and Third Transition Series

General Characteristics, comparative treatment with their 3rd-analogues

in respect of ioniC radii, oxidation states, magnetic behaviour, spectral

properties and stereochemistry.

3. Oxidation and Reduction

Use of redox potential data analysis of redox cycle, redox stability in

water-Frost, Latime and Pourbaix diagrams, Principles involved in the

extraction of the elements.

4. Co-ordination Compounds:

Werner's coordination theory and its experimental verification, effective

atomic number concept. chelates nomenclature of coordination compounds. isomerism in coordination compounds, valence bond theory of transition metal complexes

5. Chemistry of Lanthanide Elements:

Electronic structure, oxidation states and ionic radii and lanthanide

contraction, complex formation, occurrence and isolation, lanthanide

compounds.

6. Chemistry of Noble Gases:

Chemical properties of the Noble gases, Chemistry of Xenon, structure

and bonding in xenon compounds.

7. Non-aqueous Solvents

Physical properties of a solvent, types of solvents and their general

characteristics, reactions in non-aqueous solvents with reference to liquid NH3, and liquid SO2

8. Hard and soft acids andrbases (HSAB):

Classification of acids and bases as hard and soft, Pearson's HSAB

Concept, acid base strength and hardness and softness, symbiosis theoretical basis of hardness and softness, electronegativity and hardness and softness.

CHEMISTRY PAPER IV-ORGANIC CHEMISTRY

Time:3 Hours]

In all nine questions are to set. The a. No. 1 will be objective 10 marks

and will screen the entire paper, Students will be required to answer five questions of which question 1 will be compulsory.

1 Electromagnetic spectrum, Absorption Spectrum:

 UV absorption spectroscopy absorption laws (Beeriabert law), molar absorptivity. presentation and analysis of UV spectra, types of electronic transitions, effect of conjugation, Concept of chromophore and auxo Chrome. Bathochromic, hypsochremic, hyperchromic and hypochromic shifts. UV spectra of conjugated

enes and enones.

Infrared (R) absorption spectroscopy- molecular vibrations. Hooke's law

selection rules. intensity and position of IR bands, measurement or iR

spectrum, fingerprint region, Characteristic absorption of various functional groups and interpretation of IR spectra of simple organic compounds.

2. Mechanism: Aromatic electrophilic substitution, Directive influence of

group. Mechanism of nitration, Sulphonation and halogenation of benzene. Relative strength of acids and substituted acids. Phenols and substituted phenols, Relative strength of basicity of aliphatic amines, aromatic amines and substituted aromatic amines, Decarboxylation of acids, Synthesis of derivatives of acids, Hydrolysis of esters, Acid & Base, Catalysed opening of epoxide ring.

3. Hydroxy Acids:a, B, &y- Hydroxy acids -preparation and reactions of

lactic acid, tartaric acid and citric acid.

4. organic Synthesis era Enolates-

Acidity of hydrogen atom of a carboxylic group. Active methylene group. Keto Enol tautomerism, Ethyl acetoacetate and Diethl malonate.

5. Carbohydrates: Classification, Monosaccharides Ascending the aldose series, Descending the aldose series, Inter conversions of aldose to Ketose and vice-versa configuration of monosaccharides, mechanism of Osazone formation, Mutarotaton, Epemerisation, Erythro and threo diastereomers Structure of D (+) glucose.

6. Name reactions: Friedel- Craft's reaction Reimer Tiemann reaction,

Reformatsky reaction, Gatermann's Synthesis, Claisen Condensation,

Houben Hoeseh reaction, Kolbe's reaction, Sandmeyer's reaction)

7. Phenols: Isolation from Coal tar, Methods of prepn, Impotant rk, uses

8. Aromatic amines and Diazonium salt

9. Fats, Oils & Detergents 

Natural fats, edible and industrial oils of vegetable origin, Common fatty acids, glycerides, hydrogenation of

unsaturated oils, Saponification value, iodine value, acid, value, Soape, Synthetic detergents, alkyl and aryl sulphonates

10. Synthetic Polymers: Addition or chain-growth polymerisation. Free

radical. Vinyl polymerisation. ionic vinyl polymerization, Zieger- Natta

polymorisation and vinyl polymers condensation or step growth

polymerisation. Polyester , Polyamides, Phenols, formaldehyde resins. Urea- formaldehyde resins, Epoxy resins and polyurethanes. Natural & Synthetic rubbers.

PRACTICAL

Time:6 Hours  Full Marks: 50

1. Volumetric analysis

(a) Acidimetry and alkalimetry

(b) Use of Potassium Permanganate, Potassium Dichromate and Sodium

Thiosulphate.

2. Detection of Nitrogen, Sulphur and Halogen in Organic Compounds and identification of organic compounds containing one functional group

including monosaccharides.

3. Note Book and Viva-voce.