Instruction to Question Setter for
Semester Internal Examination (SIE 20+5=25 marks):
The Semester Internal Examination shall have two components. (a) One
Semester Internal Examination Written Test (SIE) of 20 Mark (b) Class
Attendance Score (CAS) including the behaviour of the student towards teachers
and other students of the College of 5 marks.
End Semester Examination (ESE 75 marks):
There will be two group of questions A and B. Group A is compulsory which
will contain three questions. Question No.1 will be very short answer type
consisting of five questions of 1 mark each. Question No. 2 & 3 will be
short answer type of 5 marks. Group B will contain descriptive type seven
questions of fifteen marks each, out of which any four are to be answered.
Note: There may be subdivisions in
the questions of group B.
Unit-1 Atomic
Structure: (12 Lectures)
Bohr’s theory, its
limitations and atomic spectrum of hydrogen atom. Wave mechanics: de’ Broglie
equation, Heisenberg’s Uncertainty Principle and its significance,
Schrödinger’s wave equation, significance of ψ and ψ2.
Quantum numbers and their significance. Normalized and orthogonal wave
functions. Sign of wave functions. Radial and angular wave functions for
hydrogen atom. Radial and angular distribution curves. Shapes of s, p, d and f
orbitals. Contour boundary and probability diagrams. Pauli’s Exclusion
Principle, Hund’s rule of maximum multiplicity, Aufbau’s principle and its
limitations, Variation of orbital energy with atomic number.
Unit-2 Periodicity of
Elements: (12 Lectures)
s, p, d, f block elements, the long form of periodic
table. Detailed discussion of the following properties of the elements, with
reference to s and p-block. Effective nuclear charge, shielding or screening
effect, Slater rules, variation of effective nuclear charge in periodic table. ,
Atomic radii (Vander Waals) ,Ionic and crystal radii, Covalent radii
(octahedral and tetrahedral) Ionization enthalpy, Successive ionization
enthalpies and factors affecting ionization energy. Applications of ionization enthalpy,
Electron gain enthalpy, trends of electron gain enthalpy. Electronegativity,
Pauling, Mullikan, Allred Rachow scales, electronegativity and bond order,
partial charge, hybridization, group electronegativity, Sanderson electron
density ratio.
Unit-3
Chemical Bonding: (30 Lectures)
a)
Ionic bond: General characteristics, types of ions, size effects,
radius ratio rule and its limitations. Packing of ions in crystals. Born-Lande
equation with derivation, Madelung constant, expression for lattice energy,
Kapustinskii equation. Born-Haber cycle and its application, Solvation energy.
b)
Covalent bond: Lewis structure, Valence Shell Electron Pair
Repulsion Theory (VSEPR), Shapes of simple molecules and ions containing lone
and bond pairs of electrons multiple bonding, sigma and pi-bond approach,
Valence Bond theory, (Heitler-London approach). Hybridization containing s, p
and s, p, d atomic orbitals, shapes of hybrid
orbitals, Bents rule, Resonance and resonance energy,
Molecular orbital theory, Molecular orbital diagrams of simple homonuclear and
heteronuclear diatomic molecules: N2, O2, C2,
B2, F2, CO, NO, and their ions. Covalent character in
ionic compounds; polarization, polarizing power and polarizability. Fajan
rules. Ionic character in covalent compounds: Bond moment and dipole moment,
ionic character from dipole moment and electronegativities.
c)
Metallic Bond: Qualitative idea of free electron model,
Semiconductors, Insulators.
d)
Weak Chemical
Forces: Vander Waals, ion-dipole,
dipole-dipole, induced dipole dipole-induced dipole interactions, hydrogen
bond, effects of hydrogen bonding on melting and boiling points, solubility,
dissolution
Unit-4: Oxidation-Reduction and Volumetric Analysis: (6 Lectures) Redox equations, Balancing by Ion electron method & Oxidation number method. Disproportionation Reaction. Principles involved in volumetric analysis.
Instruction to Question Setter for
Semester Internal Examination (SIE 20+5=25 marks):
The Semester Internal Examination shall have two components. (a) One
Semester Internal Examination Written Test (SIE) of 20 Mark (b) Class
Attendance Score (CAS) including the behaviour of the student towards teachers
and other students of the College of 5 marks.
End Semester Examination (ESE 75 marks):
There will be two group of questions A and B. Group A is compulsory which
will contain three questions. Question No.1 will be very short answer type
consisting of five questions of 1 mark each. Question No. 2 & 3 will be
short answer type of 5 marks. Group B will contain descriptive type seven
questions of fifteen marks each, out of which any four are to be answered.
Note: There may be subdivisions in
the questions of group B.
Unit-1 Gaseous state:
(20 Lectures)
Kinetic Molecular
model of a gas: Postulates and
derivation of the kinetic gas equation, collision frequency, collision
diameter, mean free path and viscosity of gases, their temperature and pressure
dependence, relation between mean free path and coefficient of viscosity,
calculation of σ from η, variation of viscosity with temperature and pressure.
Maxwell distribution and its use in evaluating molecular velocities (average,
root mean square and most probable) and average kinetic energy, law of
equipartition of energy, degrees of freedom and molecular basis of heat
capacities.
Behaviour of
real gases: Deviation from ideal gas
behaviour, Compressibility factor, Z , Variation of compressibility factor with
pressure at constant temperature (plot of Z vs P) for different gases ( H2,
CO2, CH4 and NH3), Causes of deviation from
ideal behaviour. van der Waals equation of state, its derivation and
application in explaining real gas behaviour. Boyle’s temperature. Isotherms of
real gases and their comparison with van der Waals isotherms, continuity of
states, critical state, critical and van der Waals constants, law of
corresponding states.
Unit-2
Liquid State: (10 Lectures)
Structure and physical properties of liquids; vapour
pressure, surface tension, viscosity, and their dependence on temperature,
Effect of addition of various solutes on surface tension, cleansing action of
detergents. Structure of water.
Unit-3:
Solid State: (10 Lectures)
Nature of the solid state, law of constancy of
interfacial angles, law of rational indices, Miller indices, elementary ideas
of symmetry, symmetry elements and symmetry operations, qualitative idea of
point and space groups, seven crystal systems and fourteen Bravais lattices,
X-ray diffraction, Bragg's law, a simple account of rotating crystal method and
powder pattern method. Analysis of powder diffraction patterns of NaCl, CsCl
and KCl. Various types of defects in crystals, Glasses and liquid crystals.
Unit -4 Ionic Equilibrium:
(20 Lectures)
Concept of Equilibrium. Le Chatlier’s principle and
its applications. Relationships between Kp, Kc and Kx
for reactions involving ideal gases (Kinetic derivation). Equilibrium between
ideal gases and a pure condensed phase.
Strong, moderate and weak electrolytes, degree of
ionization, factors affecting degree of ionization, ionization constant and
ionic product of water. Ionization of weak acids and bases, pH scale, common
ion effect, dissociation constants of mono-, di- and tri-protic acids. Salt
hydrolysis, hydrolysis constants, degree of hydrolysis and pH of different salt
solutions. Buffer solutions, Henderson equation, buffer capacity, buffer range,
buffer action, applications of buffers in analytical chemistry, Solubility and
solubility product.
Qualitative treatment of acid–base titration curves
(calculation of pH at various stages). Theories of indicators, selection of
indicators and their limitations. Multistage equilibria in polyelectrolytes.
Instructions to Question Setter for
Sessional Internal Practical Examination (SIE):
There will be one Sessional
Internal Practical Examination of 2
Hrs duration.
Evaluation of Practical Examination may be as per the following guidelines:
One Experiment = 20 marks
Attendance=5
Marks
End Semester Examination (ESE):
There will be one Practical Examination of 6 Hrs duration.
Evaluation of Practical Examination may be as per the following guidelines:
Two Experiments = 65 marks
Practical record
notebook= 5 marks
Viva-voce= 5 marks
Section -A: Inorganic Chemistry
(A)
Acid-Base Titrations
1.
Estimation of
carbonate and hydroxide present together in mixture.
2.
Estimation of
carbonate and bicarbonate present together in a mixture.
3.
Estimation of
free alkali present in different soaps/detergents
(B) Oxidation-Reduction Titrations
1.
Estimation of
Fe(II) and oxalic acid using standardized KMnO4 solution.
2.
Estimation of
oxalic acid and sodium oxalate in a given mixture.
3.
Estimation of
Fe(II) with K2Cr2O7 using internal
(diphenylamine, anthranilic acid) and external indicator.
Section
-B: Physical Chemistry
1.
Determine the
surface tension by (i) Drop number (ii) Drop weight method.
2.
Study the
variation of surface tension of detergent solutions with concentration.
3.
Study the effect
of the addition of solutes on the surface tension of water at room temperature
and explain the observations in terms of molecular interactions:
4.
(i)sugar (ii)
ethanol (iii) sodium chloride
5.
Study the variation
of surface tension with different concentration of sodium chloride solutions.
Viscosity measurements using
Ostwald’s viscometer.
1.
Determination of
viscosity of aqueous solution of (i) polymer (ii) ethanol and (iii) sugar at
room temperature.
2.
Viscosity of
sucrose solution with the concentration of solute.
Ionic Equilibrium and pH measurements
1. Preparation of buffer solutions of different pH
i. Sodium acetate-acetic acid
ii. Ammonium chloride-ammonium hydroxide
2. pH metric titration of (i) strong acid vs. strong
base, (ii) weak acid vs. strong base.
3. Determination of dissociation constant of a weak
acid.
4. Measurement of pH of different solutions like aerated drinks, fruit juices, shampoos and soaps (use dilute solutions of soaps and shampoos to prevent damage to the glass electrode) using pH-meter.
Instruction to Question Setter for
Semester Internal Examination (SIE 20+5=25 marks):
The Semester Internal Examination shall have two components. (a) One Semester
Internal Examination Written Test (SIE) of 20 Mark (b) Class Attendance Score
(CAS) including the behaviour of the student towards teachers and other
students of the College of 5 marks.
End Semester Examination (ESE 75 marks):
There will be two group of questions A and B. Group A is compulsory which
will contain three questions. Question No.1 will be very short answer type
consisting of five questions of 1 mark each. Question No. 2 & 3 will be
short answer type of 5 marks. Group B will contain descriptive type seven
questions of fifteen marks each, out of which any four are to be answered.
Note: There may be subdivisions in
the questions of group B.
Unit-1 Basics of
Organic Chemistry: (16 Lectures)
Organic Compounds:
Classification and Nomenclature, Hybridization, shape of molecules, influence
of hybridization on bond properties. Electron Displacement Effects: inductive,
electromeric, resonance and mesomeric effects. Tautomerism, hyperconjugation and
their applications. Dipole moment, Organic acids and bases, their relative
strength. Homolytic and Heterolytic fission with suitable examples. Curly arrow
rules, formal charges, Electrophiles and Nucleophiles, Nucleophilicity and
basicity, Types, shape and relative stability of reaction intermediates
(Carbocations, Carbanions, Free radicals and Carbenes). Aromaticity in
benzenoid and non-benzenoid compounds, alternant and non-alternant
hydrocarbons, Huckel’s rule, annulenes, antiaromaticity, Y-aromaticity,
homo-aromaticity, bonding in fullerenes, crown ether complexes and cryptands, inclusion
compounds, cyclodextrins, catenanes and rotaxanes. Organic reactions and their mechanism:
Addition, Elimination and Substitution reactions.
Unit-2 Stereochemistry: (12 Lectures)
Concept
of asymmetry, Fischer Projection, Newmann and Sawhorse projection formulae and
their interconversions; Geometrical isomerism: cis–trans and, syn-anti
isomerism E/Z notations with C.I.P rules. Optical Isomerism: Optical Activity,
Specific Rotation, Chirality/Asymmetry, Enantiomers, Molecules with two or more
chiral-centres, Distereoisomers, meso structures, Racemic mixtures, Relative
and absolute configuration: D/L and R/S designations. Threo & Erythreo
isomers.
Cycloalkanes
and stability, Baeyer strain theory, Conformation analysis, Energy diagrams of
cyclohexane: Chair, Boat and Twist boat forms.
Unit-3
Chemistry of Aliphatic Hydrocarbons: (16 Lectures)
a) Alkanes: Formation of alkanes, Wurtz Reaction, Corey House
Synthesis, Kolbe’s Synthesis, Free radical substitutions: Halogenation -
relative reactivity and selectivity. Lengthening and shortening of carbon chain
in alkanes.
b) Alkenes and
Alkynes: Formation of alkenes and
alkynes by elimination reactions, Mechanism of E1, E2, E1cb reactions. Saytzeff
and Hofmann eliminations. Reactions of alkenes: Electrophilic additions their
mechanisms (Markownikoff/ Anti Markownikoff addition), mechanism of
oxymercuration demercuration, hydroboration-oxidation, ozonolysis, reduction
(catalytic and chemical), syn and anti-hydroxylation (oxidation), reaction with
NBS, 1, 2- and 1, 4- addition reactions in conjugated dienes and, Diels Alder
reaction; Allylic and benzylic bromination and mechanism, e.g. propene,
1-butene, toluene, ethyl benzene. Reactions of alkynes: Acidity, Electrophilic
and Nucleophilic additions. Relative reactivity of alkenes and alkynes.
Unit-4
Chemistry of Aromatic Hydrocarbons: (16 Lectures)
a) Aromatic
Hydrocarbons: Aromaticity: Aromatic
character of arenes, cyclic carbocations/carbanions and heterocyclic compounds
with suitable examples. Electrophilic aromatic substitution: halogenation,
nitration, sulphonation and Friedel-Craft's alkylation/acylation with their
mechanism. Directing effects of substituent groups.
b) Polynuclear Hydrocarbons: Reactions of naphthalene and anthracene: Structure, Preparation and structure elucidation and important derivatives of naphthalene and anthracene.
Instructions to Question Setter for
Sessional Internal Practical Examination (SIE):
There will be one Sessional Internal Practical Examination of 2 Hrs duration.
Evaluation of Practical Examination may be as per the following guidelines:
One Experiment = 20 marks
Attendance=5 Marks
End Semester Examination (ESE):
There will be one Practical Examination of 6 Hrs duration.
Evaluation of Practical Examination may be as per the following guidelines:
Two Experiments = 65 marks
Practical record notebook= 5 marks
Viva-voce= 5 marks
Section -A: Acquaintance with Chemistry Laboratory
1. Common Laboratory Apparatus
Test
tube, Beakers, Erlenmeyer flask, Volumetric flask, graduated
cylinder, Pipette, Graduated pipette, Burette, Burette clamp. Funnel, Test tube holder, Bunsen burner, Glass
rod, Utility clamp, Spot test plate, Tripod for Bunsen burner,
Wash bottle, Spatula,
Round-bottom flasks, Glass Condenser, Filter paper, Separatory funnel, Chemical
balance, Furnaces etc.
2. Common Symbols of Laboratory Concerns
Biohazard,
Highly Flammable, Oxidizing, Corrosive, Harmful/Irritant, Radioactive,
Explosive, Toxic, Dangerous for the
Environment etc.
3. Common Laboratory Reagents
Common Acids, Common
Bases, Common Inorganic/Organic Salts, Organic Compounds, Common Solvents,
Difference between Dilute/Concentrated/Fuming liquids.
4. Chemistry Laboratory Techniques
Cutting, Bending & Rounding edge of
glass tube & glass rods, fitting glassware’s, fitting equipment for Fractional distillation, drawing liquids through
pipette, burette & measuring cylinders, Diluting a solution to a known
strength, Safe storage of chemicals. Calibration and use of apparatus. Preparation
of solutions of different Molarity/Normality of titrants. Use of primary and
secondary standard solutions.
Section -B: Organic
Chemistry
I. Common
Procedures
1. Heating/Boiling with and without condenser,
Filtration techniques, Separation techniques, Crystallization techniques.
2.
Purification of organic compounds (say naphthalene & others) by
crystallization using the following solvents:
a. Water b.
Alcohol c. Alcohol-Water d. Acetone e.
Hexane f. Toluene
3.
Determination of the melting points
a. Determination of the melting points of above compounds
and unknown organic compounds
b) (Kjeldahl method and electrically heated melting point
apparatus)
a. Effect of impurities on the melting point – mixed
melting point of two unknown organic compounds
b. Determination of boiling point of liquid compounds.
(Boiling point lower than and more than 100 °C by distillation and capillary
method).
Instruction to Question Setter for
Semester Internal Examination (SIE 20+5=25 marks):
The Semester Internal Examination shall have two components. (a) One
Semester Internal Examination Written Test (SIE) of 20 Mark (b) Class
Attendance Score (CAS) including the behaviour of the student towards teachers
and other students of the College of 5 marks.
End Semester Examination (ESE 75 marks):
There will be two group of questions A and B. Group A is compulsory which
will contain three questions. Question No.1 will be very short answer type
consisting of five questions of 1 mark each. Question No. 2 & 3 will be
short answer type of 5 marks. Group B will contain descriptive type seven
questions of fifteen marks each, out of which any four are to be answered.
Note: There may be subdivisions in
the questions of group B.
UNIT 1: Chemistry of Halogenated
Hydrocarbons: (10 Lectures)
Alkyl halides: Methods of
preparation, nucleophilic substitution reactions – SN1, SN2
and SNi mechanisms with stereochemical aspects and effect of solvent etc.
Nucleophilic substitution vs. elimination.
Aryl halides: Preparation from
diazonium salts. nucleophilic aromatic substitution, SNAr, Benzyne mechanism.
Relative reactivity of alkyl, allyl/benzyl, vinyl and aryl halides towards
nucleophilic substitution reactions.
Organometallic
compounds of Mg and Li and their use in synthesis.
UNIT 2: Alcohols,
Phenols, Ethers and Epoxides: (10 Lectures)
Alcohols: preparation,
properties and relative reactivity of 1°, 2°, 3°- alcohols, Bouveault-Blanc Reduction,
Preparation and properties of glycols and glycerol. Pinacol-Pinacolone
rearrangement.
Phenols: Preparation and
properties, Acidic nature and factors affecting it, Ring substitution
reactions, Reimer–Tiemann and Kolbe's–Schmidt Reactions, Fries and Claisen
rearrangements with mechanism.
Ethers and Epoxides: Preparation and
reaction with acids. Reaction of epoxides with alcohols, ammonia derivatives
and LiAlH4
UNIT 3: Carbonyl
Compounds: (16 Lectures)
Structure, reactivity
and preparation of Carbonyl compounds. Nucleophilic additions, Nucleophilic
addition elimination reactions with ammonia derivatives with mechanism. Aldol
and Benzoin condensation, Knoevenagel condensation, Claisen-Schmidt, Perkin,
Cannizzaro and Wittig reaction, Beckmann and Benzil- Benzilic acid
rearrangements, haloform reaction and Baeyer Villiger oxidation, α-substitution reactions, oxidations and
reductions (Clemmensen, Wolff- Kishner, LiAlH4, NaBH4, MPV, PDC and PGC), Addition
reactions of unsaturated carbonyl compounds: Michael addition.
UNIT 4: Carboxylic
Acids and their Derivatives: (8 Lectures)
Preparation, physical
properties and reactions of monocarboxylic acids, Typical reactions of
dicarboxylic acids,hydroxy acids and unsaturated acids: succinic/phthalic,
lactic, malic, tartaric, citric, maleic and fumaric acids,Preparation and
reactions of acid chlorides, anhydrides, esters and amides, Comparative study
of nucleophilic substitution at acyl group, Mechanism of acidic and alkaline
hydrolysis of esters, Claisen condensation, Dieckmann and Reformatsky
reactions, Hofmann bromamide degradation and Curtius rearrangement.
UNIT 5: Chemistry of
Active methylene groups: (4 Lectures)
Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications of diethyl malonate and ethyl acetoacetate.
Instruction to Question Setter for
Semester Internal Examination (SIE 20+5=25 marks):
The Semester Internal Examination shall have two components. (a) One
Semester Internal Examination Written Test (SIE) of 20 Mark (b) Class
Attendance Score (CAS) including the behaviour of the student towards teachers
and other students of the College of 5 marks.
End Semester Examination (ESE 75 marks):
There will be two group of questions A and B. Group A is compulsory which
will contain three questions. Question No.1 will be very short answer type
consisting of five questions of 1 mark each. Question No. 2 & 3 will be
short answer type of 5 marks. Group B will contain descriptive type seven
questions of fifteen marks each, out of which any four are to be answered.
Note: There may be subdivisions in
the questions of group B.
UNIT 1: Introduction & First Law of
thermodynamics: (8 Lectures)
Intensive and extensive properties, thermodynamic
variables, state and path functions, isolated, closed and open systems,
reversible, irreversible and cyclic processes. Zeroth law of thermodynamics.
First law of Thermodynamics: Concept of heat, q, work, w, internal energy,
enthalpy, relation between heat capacities, calculations of q, w, U and H for
reversible and irreversible processes. Expression for work done under free
expansion of gases for isothermal and adiabatic conditions.
UNIT 2:
Thermochemistry: (9 Lectures)
Heat of reactions: standard states, enthalpy of
formation of molecules and ions. Enthalpy of reactions (combustion, neutralization,
solution etc) and its applications, calculation of bond energy, bond
dissociation energy and resonance energy from thermochemical data, effect of
temperature (Kirchhoff's equations) and pressure on enthalpy of reactions.
UNIT 3:
Second & Third Law of Thermodynamics: (7 Lectures)
Concept of entropy, thermodynamic scale of
temperature, statement of the second law of thermodynamics, molecular and
statistical interpretation of entropy. Calculation of entropy change for
reversible and irreversible processes.
Third Law: Statement of
third law, concept of residual entropy, calculation of absolute entropy of
molecules.
UNIT 4: Free
Energy Functions: (6 Lectures)
Gibbs and Helmholtz energy, variation of S, G, A with
T, V, P, Free energy change and spontaneity. Relation between Joule-Thomson
coefficient and other thermodynamic parameters, inversion temperature, Gibbs Helmholtz
equation, Maxwell relations, thermodynamic equations of state.
UNIT 5:
Partial molar quantities: (8 Lectures)
Partial molar quantities, dependence of thermodynamic
parameters on composition, Gibbs- Duhem equation, chemical potential of ideal
mixtures, change in thermodynamic functions in mixing of ideal gases.
UNIT 6:
Dilute solutions: (10 Lectures)
Dilute solutions, lowering of vapour pressure,
Raoult's and Henry's Laws and their applications. Colligative properties of
solutions, abnormal colligative properties, Van’t Hoffs factor. Thermodynamic
derivation using chemical potential to derive relations between the (i)
relative lowering of vapour pressure, (ii) elevation of boiling point, (iii)
Depression of freezing point, (iv) osmotic pressure and amount of solute.
Applications in calculating molar masses of normal, dissociated and associated
solutes in solution. Azeotropes.
UNIT 7: Thermodynamics
of Chemical Equilibrium (12 Lectures)
Criteria of thermodynamic equilibrium, degree of advancement of reaction, chemical equilibria in ideal gases, concept of fugacity. Thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient. Coupling of exoergic and endoergic reactions. Equilibrium constants and their quantitative dependence on temperature, pressure and concentration. Free energy of mixing and spontaneity; thermodynamic derivation of relations between the various equilibrium constants Kp, Kc and Kx.
SEMESTER-IV
MAJOR COURSE- MJ 8: MAJOR PRACTICALS-III
Credit: Theory-04, 120 Hours, Full Marks=100, Pass Marks= 40,
Marks: 25 (Attendance=5 + 20 SIE: 1Hr) + 75 (ESE: 6Hrs) = 100, Pass Marks: Practical (SIE + ESE) = 40
Instructions to Question Setter for
Sessional Internal Practical Examination (SIE):
There will be one Sessional Internal Practical Examination of 2 Hrs duration.
Evaluation of Practical Examination may be as per the following guidelines:
One Experiment = 20 marks
Attendance=5 Marks
End Semester Examination (ESE):
There will be one Practical Examination of 6 Hrs duration.
Evaluation of Practical Examination may be as per the following guidelines:
Two Experiments = 65 marks
Practical record notebook= 5 marks
Viva-voce= 5 marks
I. Organic Chemistry
1. Detection of extra
elements in organic compounds.
2. Functional
group test for nitro, amine and amide groups
3. Functional
group tests for alcohols, phenols, carbonyl and carboxylic acid group.
4. Qualitative
analysis of unknown organic compounds containing simple functional groups
(alcohols, carboxylic acids, phenols and carbonyl compounds)
5. Organic preparations:
a.
Oxidation of
Benzaldehyde to benzoic acid.
b.
Hydrolysis of
amides and esters.
c.
Preparation of Semi
carbazone derivatives of the following compounds: acetone, ethyl methyl ketone,
cyclohexanone, benzaldehyde.
d.
Preparation of
methyl orange.
II. Thermochemistry
(a)
Determination of
heat capacity of a calorimeter for different volumes using change of enthalpy
data of a known system (method of back calculation of heat capacity of
calorimeter from known enthalpy of solution or enthalpy of neutralization).
(b)
Determination of
heat capacity of the calorimeter and enthalpy of neutralization of hydrochloric
acid with sodium hydroxide.
(c)
Calculation of the enthalpy of ionization of
ethanoic acid.
(d)
Determination of
heat capacity of the calorimeter and integral enthalpy (endothermic and
exothermic) solution of salts.
(e)
Determination of
basicity/proticity of a polyprotic acid by the thermochemical method in terms
of the changes of temperatures observed in the graph of temperature versus time
for different additions of a base. Also calculate the enthalpy of
neutralization of the first step.
(f)
Determination of
enthalpy of hydration of copper sulphate.
(g)
Study of the
solubility of benzoic acid in water and determination of Δ H.
SEMESTER-V
MAJOR COURSE-
MJ 9: ACID, BASES, SALTS,
METALLURGY, s &
p-BLOCK ELEMENTS, INORGANIC
POLYMERS
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT 1: Acids,
Bases and Salts:
(15 Lectures)
Arrhenius concept of acid and base and its
limitations, Bronsted-Lowry concept of acid and base and its limitations, Solvated proton, Relative
strengths of acids and bases,
Levelling effect and levelling
solvents, Types of acid-base reactions, Salts and their classifications, Lewis
concept of acid and base and its limitations, Classification of Lewis acids and
bases into hard and soft categories, Hard and Soft Acid Base (HSAB) principle
and its implications, Theoretical basis of hardness and softness,
Electronegativity and hardness and softness, Acid -base strength and hardness
and softness, Lux-Flood concept of acid and bases.
UNIT-2: General Principle of Metallurgy: (12 Lectures)
Standard Electrode Potential
and its application to inorganic reactions. Occurrence of metals
based on standard electrode potentials. Latimer diagrams and Frost diagrams and
their applications, Ellingham diagrams for reduction of metal oxides using
carbon or carbon
monoxide as reducing
agent. Electrolytic Reduction, Hydrometallurgy. Methods of purification
of metals: Electrolytic Kroll process, Parting process, van Arkel- de Boer
process and Mond’s process, Zone refining.
Unit-3: Chemistry of s and p Block Elements: (17 Lectures)
Inert pair effect, Relative stability of different
oxidation states, diagonal relationship and anomalous behaviour of first member
of each group. Allotropy and catenation. Complex formation tendency of s and p
block elements. Hydrides and their classification ionic, covalent and
interstitial. Basic beryllium acetate and nitrate.
Structure, bonding, preparation, properties and uses.
Boric acid and borates, boron nitrides, borohydrides (diborane) carboranes and graphitic compounds, silanes, Oxides and oxoacids of nitrogen, Phosphorus and chlorine.
Per-oxo acids of Sulphur inter-halogen compounds, poly- halide ions,
pseudo-halogens, properties of halogens.
UNIT-4: Noble Gases:
(8 Lectures)
Occurrence and uses, rationalization of inertness of noble gases, Clathrates; preparation and properties of XeF2, XeF4 and XeF6, Bonding in noble gas compounds (Valence bond and
MO treatment for XeF2), Shape of noble gas compounds (VSEPR theory).
UNIT-5: Inorganic Polymers: (8 Lectures)
Introduction, Types of inorganic polymers, comparison
with organic polymers, synthesis, structural
aspects and applications of Silicones and Siloxanes,
Borazines, Phosphazenes and Silicates.
MAJOR COURSE- MJ 10: FUNCTIONAL GROUPS CONTAINING N & S, HETROCYCLIC
COMPOUNDS, ALKALOIDS, TERPENES
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT-1: Nitrogen Containing Functional Groups (20 Lectures)
Preparation and important reactions of nitro and
compounds, nitriles and isonitriles Amines: Effect of substituent and solvent on basicity; Preparation and properties: Gabriel
phthalimide synthesis, Carbylamine reaction, Mannich reaction,
Hoffmann’s exhaustive methylation, Hofmann- elimination reaction; Distinction
between 1°, 2° and 3° amines with Hinsberg reagent and nitrous acid. Diazonium
salts: Preparation and synthetic applications.
UNIT-2: Sulphur Containing Compounds: (6 Lectures)
Preparation and reactions of thiols, thioethers including 1,3-dithiane and sulphonic acids
UNIT-3: Heterocyclic Compounds: (20 Lectures)
Classification and nomenclature, Structure,
aromaticity in 5-numbered and 6-membered rings containing one heteroatom;
Synthesis, reactions and mechanism of substitution reactions of Furan, Pyrrole
(Paal-Knorr synthesis, Knorr pyrrole synthesis, Hantzsch synthesis), Thiophene,
Pyridine (Hantzsch synthesis), Pyrimidine, Structure elucidation of indole, Fischer
indole synthesis and Madelung
synthesis), Structure elucidation of quinoline and isoquinoline, Skraup
synthesis, Friedlander’s synthesis, Knorr quinoline synthesis, Doebner-Miller synthesis, Bischler- Napieralski reaction, Pictet-Spengler reaction,
Pomeranz-Fritsch reaction Derivatives of furan: Furfural and furoic acid.
UNIT-4: Alkaloids (8 Lectures)
Natural occurrence, General structural features,
Isolation and their physiological action Hoffmann’s exhaustive methylation,
Emde’s modification, Structure elucidation and synthesis of Hygrine and Nicotine. Medicinal importance of Nicotine,
Hygrine, Quinine, Morphine, Cocaine, and Reserpine.
UNIT-5: Terpenes (6 Lectures)Occurrence, classification, isoprene rule;
Elucidation of stucture
and synthesis of Citral, Neral and α-terpineol.
MAJOR COURSE- MJ 11: MAJOR PRACTICALS-IV
Credit: Theory-04, 120 Hours,
Full Marks=100, Pass Marks= 40,
Marks: 25 (Attendance=5 + 20 SIE: 1Hr) + 75 (ESE:
6Hrs) = 100, Pass Marks:
Practical (SIE + ESE) = 40
Gravimetric
Analysis:
- Estimation of Nickel (II) using Dimethylglyoxime (DMG).
- Estimation
of Barium as BaSO4
- Estimation of
Magnesium in pyrolusite
- Estimation of Iron in Fe2O3 by precipitating
iron as Fe(OH)3.
Organic Chemistry
- Functional group test for nitro,
amine and amide groups
- Qualitative analysis of unknown organic compounds containing simple functional groups (nitro, amide, nitriles and
isonitriles, amines)
Organic
preparations:
- Acetylation of one of the following compounds: amines (aniline, o-, m-, p-toluidines and o-,
m-p-anisidine) and phenols (β-naphthol, vanillin, salicylic acid) by any one
method: (Using conventional method and Using green chemistry approach).
- Benzolyation of one of the amines (aniline,
o-, m-, p- toluidines and o-, m-, p- anisidine) and one of the phenols (β-naphthol, resorcinol, p-cresol) by Schotten-Baumann reaction.
- Oxidation of ethanol/
isopropanol (Iodoform reaction).
- Bromination (any one)
- Acetanilide by conventional methods.
- Acetanilide using green approach (Bromate-bromide method)
- Nitration: (any one)
- Acetanilide/nitrobenzene by conventional method.
- Salicylic acid by green
approach (using ceric ammonium nitrate).
- Selective reduction
of meta dinitrobenzene to m-nitroaniline.
- Reduction of p-nitrobenzaldehyde
by sodium borohydride.
- Aldol condensation with either conventional or green method.
- Benzil-Benzilic acid
rearrangement.
Collected solid samples
may be used for recrystallization, melting point and TLC.
SEMESTER-VI
MAJOR COURSE-
MJ 12: d- & f- BLOCK ELEMENTS, COORDINATION CHEMISTRY & NON-
AQUEOUS SOLVENTS
Credit: Theory-04, Full Marks=100, Pass Marks= 40,
Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT-1: d-Block Elements:
Transition Elements: (15 Lectures)
General group trends with special reference to
electronic configuration, colour, variable valency, magnetic and catalytic
properties, and ability
to form complexes. Stability of various oxidation states and e.m.f.
(Latimer & Bsworth
diagrams). Difference between
the first, second and third transition series. Oxidation
states displayed by Cr, Fe, Co, Ni and Co. A study of the following compounds (including preparation and important properties); Peroxo compounds of chromium, K2Cr2O7, KMnO4, K4[Fe(CN)6], sodium nitroprusside, [Co(NH3)6]Cl3, Na3[Co(NO2)6].
UNIT-2: f-Block elements:
Lanthanoids and Actinides: (10 Lectures)
Electronic configuration, oxidation
states, color, spectra
and magnetic behavior,
lanthanide contraction, separation of lanthanides (ion-exchange method
only).
UNIT-3: Coordination Chemistry: (25 Lectures)
Werner’s theory, EAN rule, piano-stool compounds,
valence bond theory (inner and outer orbital complexes), Crystal field theory,
d-orbital splitting, weak and strong fields, pairing energies, factors
affecting the magnitude of (Δ). Octahedral vs. tetrahedral coordination,
tetragonal distortions from octahedral geometry Jahn-Teller theorem, square planar
complexes, d orbital splitting in trigonal bipyramidal, square pyramidal and
cubic ligand field environments, CFSE, Variation of lattice energies,
enthalpies of hydration and crystal radii variations in halides of first and second row transition metal
series, Qualitative aspect
of Ligand field theory, MO diagrams of representative coronation
complexes, IUPAC nomenclature of coordination compounds, isomerism in
coordination compounds.
Stereochemistry of complexes
with the coordination number 4 and 6, Chelate
effect.
UNIT-4: Non-Aqueous Solvents:(10 Lectures)
Solvents and their
role during chemical
reactions, Classification of solvents on the basis of various criteria, General properties of
ionizing solvents, Different types of chemical reactions taking place in a solvent,
Different types of chemical reactions taking place in liquid NH3 and their comparison to those taking place in aqueous
medium , liquid SO2 as a solvent, liquid
HF as a solvent, liquid N2O4 as a solvent and
glacial acetic acid as a solvent.
MAJOR COURSE- MJ-13:
BIO-ORGANIC CHEMISTRY: AMINO
ACIDS, LIPIDS, ENZYMES, NUCLEIC ACIDS &
PHARMACEUTICAL COMPOUNDS
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
UNIT-1: Amino acids,
Peptides and Proteins:
(20 Lectures)
Amino acids: Classification of Amino Acids, α-Amino acids-
synthesis, ionic properties and reactions, Zwitter-ion structure, pKa -values, isoelectric
point and electrophoresis.
Study of peptides: Determination of primary structure
by end group analysis, Synthesis of peptides
by using N-protecting, C-protecting and C-activating groups, Merrifield solid phase
peptide synthesis.
Proteins: General characteristics, Classification of proteins,
Overview of Primary,
Secondary, Tertiary and Quaternary structure of proteins.
UNIT-2: Enzymes: (10 Lectures)
General characteristics, Mechanism of enzyme action,
factors affecting enzyme action, Coenzymes and cofactors and their role in biological reactions, Specificity of enzyme action (including stereospecificity).
Enzyme inhibitors and their importance, phenomenon of inhibition (competitive and non- competitive inhibition including
allosteric inhibition).
UNIT-3: Lipids (10 Lectures)
Introduction to lipids, classification. Oils and fats:
Common fatty acids present in oils and fats, Omega fatty acids, Trans
fats, Hydrogenation, Saponification value, Iodine number.
Biological importance of triglycerides, phospholipids, glycolipids, and
steroids (cholesterol).
UNIT-4: Nucleic Acids (10 Lectures)
Definition and general characteristics, Components of
nucleic acids, nucleosides and nucleotides,
Structure of nucleic
acids, The chemical
basis of heredity- Replication of DNA, Synthesis of adenine, guanine,
cytosine, uracil and thymine.
UNIT-5: Pharmaceutical Compounds-Structure and Importance:(10 Lectures)
Definition, Classification, Structure and Therapeutic use of
Antipyretics: Paracetamol (with synthesis)
Analgesics: Ibuprofen (with synthesis) Antimalarials:
Chloroquine (with synthesis) Antibiotics: Chloramphenicol (with synthesis)
MAJOR COURSE- MJ 14: PHASE EQUILIBRIA, CHEMICAL
KINETICS & SURFACE
CHEMISTRY
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT-1: Phase Equilibria: (28 Lectures)
Concept of phases, components and degrees of freedom,
derivation of Gibbs Phase Rule for nonreactive and reactive systems;
Clausius-Clapeyron equation and its applications to solid- liquid,
liquid-vapour and solid-vapour equilibria, phase diagram for one component
systems, with applications. Phase diagrams for systems of solid-liquid
equilibria involving eutectic, congruent and incongruent melting points, solid
solutions. Three component systems, water- chloroform- acetic acid system,
triangular plots. Binary solutions: Gibbs-Duhem-Margules equation, its derivation and applications to fractional distillation of binary miscible
liquids (ideal and nonideal),
azeotropes, lever rule, partial miscibility of liquids, CST, miscible pairs,
steam distillation. Nernst distribution law: its derivation and applications.
UNIT-2: Chemical Kinetics:(18 Lectures)
Order and molecularity of a reaction, rate laws in
terms of the advancement of a reaction, differential and integrated rate laws for first, second and fractional
order reactions, pseudo-
unimolecular reactions, determination of the order, kinetics of complex reactions (limited to first order): (i) Opposing reactions (ii)
parallel reactions and (iii) consecutive reactions and their differential rate
equations (steady-state approximation in reaction mechanisms) (iv) chain
reactions. Temperature dependence of reaction rates; Arrhenius equation;
activation energy. Collision theory of reaction rates, Lindemann mechanism,
qualitative treatment of the theory of absolute reaction rates.
UNIT-3: Catalysis: (8 Lectures)
Types of catalyst, specificity and selectivity, mechanisms of catalysed
reactions at solid
surfaces; effect of particle size and efficiency of nanoparticles as
catalysts. Enzyme catalysis, Michaelis- Menten mechanism, acid-base catalysis.
UNIT-4: Surface Chemistry: (6 Lectures)
Physical adsorption, chemisorption, adsorption
isotherms (Freundlich, Temkin, Derivation of Langmuir adsorption isotherms, surface
area determination), BET theory of multilayer adsorption (no derivation), Adsorption in
solution.
SEMESTER-V
MAJOR COURSE-
MJ 9: ACID, BASES, SALTS,
METALLURGY, s &
p-BLOCK ELEMENTS, INORGANIC
POLYMERS
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT 1: Acids,
Bases and Salts:
(15 Lectures)
Arrhenius concept of acid and base and its
limitations, Bronsted-Lowry concept of acid and base and its limitations, Solvated proton, Relative
strengths of acids and bases,
Levelling effect and levelling
solvents, Types of acid-base reactions, Salts and their classifications, Lewis
concept of acid and base and its limitations, Classification of Lewis acids and
bases into hard and soft categories, Hard and Soft Acid Base (HSAB) principle
and its implications, Theoretical basis of hardness and softness,
Electronegativity and hardness and softness, Acid -base strength and hardness
and softness, Lux-Flood concept of acid and bases.
UNIT-2: General Principle of Metallurgy: (12 Lectures)
Standard Electrode Potential
and its application to inorganic reactions. Occurrence of metals
based on standard electrode potentials. Latimer diagrams and Frost diagrams and
their applications, Ellingham diagrams for reduction of metal oxides using
carbon or carbon
monoxide as reducing
agent. Electrolytic Reduction, Hydrometallurgy. Methods of purification
of metals: Electrolytic Kroll process, Parting process, van Arkel- de Boer
process and Mond’s process, Zone refining.
Unit-3: Chemistry of s and p Block Elements: (17 Lectures)
Inert pair effect, Relative stability of different
oxidation states, diagonal relationship and anomalous behaviour of first member
of each group. Allotropy and catenation. Complex formation tendency of s and p
block elements. Hydrides and their classification ionic, covalent and
interstitial. Basic beryllium acetate and nitrate.
Structure, bonding, preparation, properties and uses.
Boric acid and borates, boron nitrides, borohydrides (diborane) carboranes and graphitic compounds, silanes, Oxides and oxoacids of nitrogen, Phosphorus and chlorine.
Per-oxo acids of Sulphur inter-halogen compounds, poly- halide ions,
pseudo-halogens, properties of halogens.
UNIT-4: Noble Gases:
(8 Lectures)
Occurrence and uses, rationalization of inertness of noble gases, Clathrates; preparation and properties of XeF2, XeF4 and XeF6, Bonding in noble gas compounds (Valence bond and
MO treatment for XeF2), Shape of noble gas compounds (VSEPR theory).
UNIT-5: Inorganic Polymers: (8 Lectures)
Introduction, Types of inorganic polymers, comparison
with organic polymers, synthesis, structural
aspects and applications of Silicones and Siloxanes,
Borazines, Phosphazenes and Silicates.
MAJOR COURSE- MJ 15: MAJOR PRACTICALS-V
Credit: Theory-04, 120 Hours, Full Marks=100, Pass Marks= 40,
Marks: 25 (Attendance=5 + 20 SIE: 1Hr) + 75 (ESE: 6Hrs) = 100, Pass Marks: Practical(SIE + ESE) = 40
Analysis of Salt
Mixture
Qualitative semi micro analysis of mixtures containing
3 anions and 3 cations. Emphasis
should be given to the understanding of the chemistry of different reactions. The following radicals
are suggested:CO3 2 -, NO2 -, S2-, SO3 2-,S2O3 2 -, CH3COO-, F-, Cl-, Br-, I-, NO3 -, BO3 3-,C2O42-, PO43-, NH4+, K+, Pb2+,
Cu2+, Cd2+, Bi3+, Sn2+,
Sb3+, Fe3+, Al3+, Cr3+,Zn2+,
Mn2+, Co2+, Ni2+, Ba2+,Sr2+,
Ca2+,
Mg2+Mixtures
should preferably contain one interfering anion, or insoluble component
(BaSO4, SrSO4, PbSO4, CaF2 or Al2O3) or combination of anions e.g. CO32- and SO32-, NO2- and NO3-, Cl- and
Br-, Cl- and I-, Br- and I-
, NO3 - and Br- , NO3- and
I-.(Spot tests should be done whenever possible.)
Phase Equilibria
and Chemical Kinetic Measurements
- Distribution of
acetic acid /benzoic acid between water & cyclohexane.
- Determination of critical solution temperature and
composition of the phenol-water system and
to study the effect of impurities on it.
- Study of equilibrium of at least one of
the following reactions by the distribution method:
I2(aq) + I- → I3-(aq) b) 𝐶𝑢++(aq) + 𝑛 𝑁𝐻3 → [Cu(NH3)n]2+
Study of
Kinetics of reaction of:
- Acid hydrolysis of methyl acetate
with HCl. b) Saponification of ethyl acetate.
Organic Chemistry
- Estimation of glycine
by Sorenson’s formalin method.
- Study of
the titration curve of glycine.
- Saponification value of an
oil or a fat.
- Determination of Iodine
number of an oil/ fat.
SEMESTER-VII
MAJOR COURSE- MJ 16: ORGANIC
SPECTROSCOPY, CARBOHYDRATES & DYES
Credit: Theory-04, 60 Hours,
Full Marks=100, Pass Marks= 40
Marks: 25 (5 Attd. + 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks:
Th (SIE + ESE) = 40
UNIT-1: Organic Spectroscopy:(30 Lectures)
General principles and introduction
to absorption and emission spectroscopy.
UV-VIS
Spectroscopy: Basic principle, Absorption
laws, Types of electronic transitions, 𝜆𝑚𝑎𝑥, Chromophores and Auxochromes, Bathochromic and Hypsochromic shifts, Intensity of absorption
bands- Hyperchromic and Hypochromic shifts, Effect of solvent on electronic
spectra,
Woodward-Fieser rules and
their applications in the calculation of 𝜆𝑚𝑎𝑥 of
α, β-unsaturated aldehydes, ketones, carboxylic acids and esters
Conjugated dienes
with or without extended
conjugation.
Distinction between
cis- and trans- isomers
IR Spectroscopy: Basic principle, Molecular
vibrations, Fingerprint region
and its significance, Group frequency region and its importance,
Infrared absorption frequencies of organic molecules with functional groups
containing O, N and S (such as ketones, aldehydes, esters, amides, acids,
anhydrides, lactones, lactams, thiols, thioethers, etc.); Effect of H-bonding,
resonance/conjugation and ring-size on IR absorptions.
NMR Spectroscopy: Basic
principle, Reference in proton magnetic
resonance spectroscopy and
Chemical shift, Chemical shifts of H atoms bonded to carbon atoms (aliphatic,
olefinic aldehydic and aromatic) and other nuclei
(alcohols, phenols, enols,
carboxylic acids, amines,
amides, mercapto), Spin-spin coupling, Chemical exchange, effect of
deuteration.
Mass Spectrometry: Basics
of fragmentations in organic compounds. Discussion of molecular ion peak, base peak and metastable ions, McLafferty rearrangement. Nitrogen rule, Index
of hydrogen deficiency. Application
of fragmentation in characterization of organic compounds.
Electronic Spectroscopy:
Franck-Condon principle, electronic transitions, singlet and triplet states,
fluorescence and
phosphorescence, dissociation and predissociation.
Atomic Absorption spectroscopy: Theory and application (with some example).
Problem Solving: Problems on structure elucidation of
organic compounds based on spectral data. Applications of IR, UV, NMR and Mass
spectra for identification of simple organic
molecules. Solving problems
for the elucidation of molecular structure with the help of mixed spectral data.
UNIT-2: Carbohydrate: (16 Lectures)
Occurrence,Definition, classification and their biological importance.
Monosaccharides: Constitution and absolute configuration of glucose and fructose, epimers and anomers, mutarotation,
determination of ring size of glucose and fructose, Haworth projections and
conformational structures, Interconversions of aldoses and ketoses, Killiani-
Fischer synthesis and Ruff degradation.
Disaccharides: Structure elucidation of maltose,
lactose and sucrose. c)Polysaccharides: Elementary treatment
of starch, cellulose
and glycogen excluding their structure elucidation.
UNIT-3: Dyes, Food Colours:(14 Lectures)
Classification, Colour and constitution, Mordant
and Vat Dyes, Chemistry of
dyeing,
Synthesis and applications of
Azo dyes: Methyl
Orange and Congo Red (mechanism of Diazo Coupling)
Triphenyl Methane Dyes: Malachite Green, Rosaniline and Crystal Violet
Phthalein Dyes: Phenolphthalein and Fluorescein,
Natural dyes –Structure elucidation and synthesis of
Alizarin and Indigotin, Natural and synthetic
food colours with examples, Natural
food colours carotenoids,chlorophyll, anthocyanin, betanin and turmeric, Preparation of Natural
food colours (Red Pink,
Green, Orange, yellow, Blue, Purle,
Brown,Tan and Black. . Synthesis and study of Tartrazine,
Quinoline yellow, Sunset yellow, Amarnanth, Erythrosine, Indigo carmine.
MAJOR COURSE- MJ 17: ELECTROCHEMISTRY, ELECTRICAL AND MAGNETIC
PROPERTIES OF MATERIALS &
POLYMERS
Credit: Theory-04, 60 Hours,
Full Marks=100, Pass Marks= 40
Marks: 25 (5 Attd. + 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks:
Th (SIE + ESE) = 40
UNIT 1: Conductance: (16 Lectures)
Arrhenius theory of electrolytic dissociation. Conductivity, equivalent and molar conductivity and their variation with dilution for weak and strong
electrolytes. Molar conductivity at infinite dilution. Kohlrausch law of
independent migration of ions. Debye-Huckel-Onsager equation, Wien effect,
Debye-Falkenhagen effect, Walden's rules. Ionic velocities, mobilities and
their determinations, transference numbers and their relation to ionic
mobilities, determination of transference numbers using Hittorf and Moving Boundary
methods. Applications of conductance
measurement: (i) degree of dissociation of weak electrolytes, (ii) ionic
product of water (iii) solubility and solubility product of sparingly soluble
salts (iv) hydrolysis constants of salts etc.
UNIT 2: Electrochemistry: (12 Lectures)
Quantitative aspects of Faraday’s law. Applications of
electrolysis in metallurgy and industry. Half-cell potential, Chemical cells, reversible and irreversible cells with examples.
Electromotive force of a cell and its measurement, Nernst equation,
Standard electrode (reduction) potential and its application of different kind
of half-cells. Electrified interfaces, overpotential, Electrocatalysis-
influence of various parameters. Hydrogen electrode.
UNIT 3: Application of EMF measurements: (12 Lectures)
Application of EMF measurements in determining (i) free energy,
enthalpy and entropy
of a cell reaction, (ii) equilibrium constants, and (iii) pH values,
using hydrogen, quinone-hydroquinone, glass and SbO/Sb2O3 electrodes. Concentration cells with and without transference, liquid
junction potential, determination of activity
coefficients and transference numbers. Qualitative discussion of potentiometric
titrations (acid-base, redox, precipitation).
UNIT 4: Electrical & Magnetic Properties of Atoms
and Molecules: (8 Lectures) Basic ideas of electrostatics, Electrostatics of dielectric media,
Clausius-Mosotti equation, Lorenz- Laurentz equation, Dipole moment and molecular
polarizabilities and their measurements.
Diamagnetism, paramagnetism, magnetic
susceptibility and its measurement, molecular
interpretation.
UNIT 5: Polymers:(12 Lectures)
Introduction: Polymers, Monomers, Polymerization
processes (addition polymerisation & Condensation polymerisation) and their
mechanism, Classification of polymers (elastomers, thermoplastics,
thermosetting plastics & fibres; natural, synthetic & semi-synthetic;
organic & inorganic; homo polymers
& copolymers, isotactic, atactic & syndiotactic), Structure of polymers (linear, branched, cross-linked
& network polymers).
Properties of polymers: Polydispersity index,
crystallinity in polymer,
Density, Melting temperature
& glass transition temperature, Co-efficient of linear thermal expansion
& volumetric thermal expansion.
Molecular weight of polymers:
Number average molecular
weight, Weight average molecular weight, Determination of
molecular weight of polymers by light scattering, osmometry, end-group analysis
& viscosity measurements
MAJOR COURSE-
MJ 18: QUANTUM CHEMISTRY, MOLECULAR
SPECTROSCOPY & PHOTOCHEMISTRY
Credit: Theory-04, Full Marks=100, Pass Marks= 40,
Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT-1: Introduction to Quantum Chemistry: (8 Lectures)
Introduction to black-body radiation and distribution of energy, photo-electric effect, concept of
quantization, wave particle duality (de-Broglie's hypothesis), Plank’s Quantum
theory. The uncertainty principle, the wavefunction: wave function and its
interpretation, conditions of normalization and Orthogonality and its
significance. Basic idea about operators, eigen function and eigen values.
UNIT 2: The Schrodinger Wave Equation (12 Lectures)
Postulates of quantum
mechanics, the Schrodinger wave equation. Discussion of solutions of the
Schrodinger equation to some model systems viz., particle in one dimensional
box, three- dimensional box, the harmonic oscillator, the rigid rotor and the
hydrogen atom. Schrodinger equation in spherical polar coordinates and
separation of R(r), Ѳ(ѳ) & Ф(ф) (radial and angular parts), degeneracies,
spherical harmonics of the hydrogen atoms.
UNIT-3: Molecular Spectroscopy:(30 Lectures)
Quantization of molecular energies, Boltzmann
distribution, Interaction of electromagnetic radiation with molecules and various types of spectra,
Born- Oppenheimer approximation. Rotation spectroscopy: The
rotation of molecules and classification of molecules on the basis of principal
moments of inertia, Rotational spectra of rigid diatomic molecules, Selection rules, Intensities of spectral lines,
Determination of bond lengths of diatomic and linear triatomic molecules, Effect of isotopic substitution on
rotational spectra, Centrifugal distortion and rotational spectra of non-rigid
rotor.
Vibrational spectroscopy: Classical equation of
vibration, computation of force constant,
amplitude of diatomic molecular vibrations, anharmonicity, Morse potential,
dissociation energies, fundamental frequencies, overtones, hot bands, degrees
of freedom for polyatomic molecules, modes of vibration, concept of group
frequencies, Breakdown of
Born-Oppenheimer approximation – interaction between rotations and vibrations
of molecules, Vibration-rotation spectroscopy, diatomic vibrating rotator, P,
Q, R branches.
Raman spectroscopy: Introduction, Raman effect, Classical
and quantum theories
of Raman effect, Rotational Raman spectra, Effect of nuclear spin on
rotational Raman spectra, Vibrational Raman spectra, Stokes & anti-Stokes
lines and their intensity difference, Rule of mutual exclusion.
Electronic Spectroscopy: Franck-Condon principle, Electronic transitions, Selection rules for
electronic transitions, Electronic spectra of diatomic molecules, Vibrational
coarse structure of electronic spectra, Rotational coarse
structure of electronic spectra, Singlet & triplet states of molecules and
their characteristics, Fluorescence and phosphorescence, Dissociation and
predissociation, Electronic spectra of polyatomic molecules.
UNIT-4: Photochemistry:(10 Lectures)
Laws of photochemistry, Quantum yield, Jablonski
diagrams, Franck-Condon principle, Law of photochemical equivalence, Quantum
efficiency, Low and high quantum efficiency, Kinetics of photochemical
reactions (H2 + Br2 = HBr, 2HI = H2 +
I2),
energy transfer in photochemical reactions (photosensitization and
quenching), fluorescence, phosphorescence, chemiluminescence, Discussion of Electronic spectra
and photochemistry (Lambert-Beer law and its
applications).
MAJOR COURSE- MJ 19: MAJOR PRACTICALS-VI
Credit: Theory-04, 120 Hours,
Full Marks=100, Pass Marks= 40,
Marks: 25 (Attendance=5 + 20 SIE: 1Hr) + 75 (ESE: 6Hrs) = 100, Pass Marks: Practical
(SIE + ESE) = 40
Conductometry
- Determination of cell constant
- Determination of equivalent conductance, degree of dissociation and dissociation constant of a weak acid.
- Perform the following conductometric titrations:
- Strong acid vs. strong base
- Weak acid vs. strong
base
- Mixture of strong
acid and weak acid vs. strong base
- Strong acid vs. weak base
- Construction of Daniell
cell and measurement of EMF.
Polymer synthesis
- Preparation of nylon 66/6
- Preparation of urea-formaldehyde resin.
Estimations
- Determination of temporary hardness in supplied
sample of water.
- Determination of permanent
hardness in supplied sample
of water.
- Determination of total hardness
of water by Complexometry.
- Estimation of Magnesium and Calcium
in a mixture by Complexometry.
- Estimation of Copper
& Zn in mixture
by Gravimetry.
- Estimation of Cu & Ni in a mixture by Gravimetry.
Preparations and Characterization
- Grignard preparation of dye (malachite green (using
methylbenoate)/crystal violet (using diethylcarbonate) (starting material as p-bromo N, N-dimethyl aniline)
(only demonstration purpose)
- Preparation of various
Schiff base-metal complexes and their identification using spectroscopy.
- Preparation of any two of the following
complexes and measurement of their conductivity measurement:
- tetraamminecarbonatocobalt (III) nitrate
- tetraamminecopper (II)
sulphate
- potassium trioxalatoferrate (III)
trihydrate.
SEMESTER-VIII
MAJOR COURSE- MJ 20: ORGANOMETALLIC AND BIOINORGANIC CHEMISTRY,OR
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT 1: Organometallic Compounds: (10 Lectures)
Definition and classification of organometallic compounds
on the basis of bond type. Concept
of hapticity of organic ligands. Metal carbonyls: 18 electron rule,
electron count of mononuclear, polynuclear and substituted metal carbonyls of
3d series. General methods of preparation (direct combination, reductive carbonylation, thermal and photochemical decomposition) of mono and binuclear carbonyls of 3d series.
UNIT 2: Synergic
effects: (14 Lectures)
EAN rule as applied to carbonyls. Preparation, structure, bonding and properties of mononuclear
and polynuclear carbonyls of 3d metals. p-acceptor behaviour of carbon
monoxide. Synergic effects (VB approach)- (MO diagram of CO can be referred to
for synergic effect to IR frequencies). Structures of mononuclear and binuclear
carbonyls of Cr, Mn, Fe, Co and Ni using VBT. pi-acceptor behaviour of CO (MO
diagram of CO to be discussed), synergic effect and use of IR data to explain
extent of back bonding. Definition and Classification with appropriate
examples based on nature of metal-carbon bond
(ionic, s, p and multicentre bonds). Structures, properties and
reactions of organometallic compounds of Mg, Al,Sn and Li –Use in synthesis of
organic compounds.
UNIT-3: Ferrocene & Zeise's salt: (10 Lectures)
Preparation and reactions (acetylation, alkylation, metallation, Mannich Condensation). Structure and aromaticity. Comparison of aromaticity and reactivity with that of benzene.
Preparation & structure of Zeise’s salt. Evidences of synergic effect
and comparison of synergic effect with that in carbonyls. UNIT-4: Metal Alkyls: (6 Lectures)
Important structural features
of methyl lithium
(tetramer) and trialkyl
aluminium (dimer), concept of multicentre bonding in these compounds. Role of triethylaluminium in polymerisation of ethene
(Ziegler – Natta Catalyst). Species present in ether solution of Grignard
reagent and their structures, Schlenk equilibrium.
UNIT-5: Bioinorganic Chemistry: (12 Lectures)
A brief introduction to bio-inorganic chemistry. Geochemical effect on distribution of metals. Role of metal ions present in biological
systems with special reference to Na+, K+ and Mg2+ ions: Na/K pump, Role of Mg2+ ions in energy production and chlorophyll.
Iron and its application in bio- systems, Haemoglobin, Myoglobin,
Storage and transfer of iron. Role of Ca2+ in
blood clotting, stabilization of protein structures and structural role
(bones).
UNIT 6: Catalysis
by Organometallic Compounds
(8 Lectures)
- Study of the following industrial processes and their
mechanism:
- Alkene hydrogenation (Wilkinsons Catalyst)
- Hydroformylation (Co
salts)
- Wacker Process
- Synthetic gasoline (Fischer Tropsch reaction)
- Synthesis gas by metal carbonyl
complexes
OR
SEMESTER-VIII
MAJOR COURSE-
MJ 20: SEMINAR & GROUP DISCUSSION
Credit: Theory-04, Full Marks=100, Pass Marks= 40,
Course Objectives:
To enhance students' communication skills through
active participation in seminars and group discussions.
To prepare students for professional and academic
settings where effective communication and collaboration are essential.
Course Outcomes:
Students will be prepared to apply the communication and collaboration skills
developed in this course to professional and academic
contexts, enhancing their overall employability and academic success.
Course Contents:
The Department Head will organize students into
various groups, assigning each group topics from different branches of
Chemistry. Under the guidance of a departmental teacher, students will
collaborate on their respective topics. Each and every student has to submit
the soft copy and the electronically typed hardbound copy of the dissertation
with the Plagiarism Report strictly adhering to the University Grants
Commission (Promotion of Academic Integrity and Prevention of Plagiarism in Higher Educational Institutions) Regulations, 2018 F. 1-18/2010(CPP- II). Published
in THE GAZETTE OF INDIA: EXTRAORDINARY [PART III—SEC. 4] dated 23rd July,2018 [web link :https://www.ugc.gov.in/pdfnews/7771545_academic-integrity- Regulation2018.pdf and the originality declarations of the
supervisor and the student along with the raw data at least a week before the
examination.
Steps of Evaluation:
Group discussion will be held within each group under
the chairmanship of Head of the Department at the department level.
Power point Presentation and the report (as per the
standard uniform format provided by the Department) submitted by the students
shall be evaluated by one external member and one internal member.
External Member will be
appointed by the Head of Department from the
following:
Permanent professors working in the postgraduate
department of the university or other colleges.
OR
Retired Professor/Associate Professor/Assistant Professor of the university.
Evaluation Process:
Evaluation of the dissertation work may be as per the following
guidelines:
Group Discussion =25
marks
Dissertation Report = 25 marks
Presentation = 50
marks
SEMESTER-VIII
ADVANCED MAJOR COURSE-
AMJ 1: ANALYTICAL CHEMISTRY
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
Unit-1: Qualitative and Quantitative Aspects
of Analysis: (4 Lectures)
Tools in
analytical chemistry and their applications, Sampling, evaluation of analytical data, errors, accuracy and precision, statistical test of data; F, Q and t-test,
rejection of data, and
confidence intervals.
UNIT-2: Spectroscopy Instrumentation (10 Lectures)
Origin of spectra,
interaction of radiation with matter, fundamental laws of spectroscopy and selection rules, validity of Beer-Lambert’s law.
Vibration spectroscopy: Basic
principles of instrumentation, sampling techniques. Application of IR spectroscopy for characterization through interpretation
of data, Effect and importance of isotope substitution. Introduction to Raman
spectra
UV-Visible Spectrometry: Basic
principles of instrumentation, principles of quantitative analysis using estimation of metal ions from aqueous solution,
Determination of composition of metal complexes using Job’s method of
continuous variation and mole ratio method.
UNIT-3: Thermal Analysis
(4 Lectures)
Theory of thermogravimetry (TG and DTG), instrumentation, estimation of Ca and Mg from their mixture.
UNIT-4: Electroanalytical Methods
(5 Lectures)
Classification of electroanalytical methods, basic principle
of pH metric, potentiometric and conductometric titrations. Techniques used for the determination of equivalence points. determination of pKa values.
UNIT-5: Separation Techniques (17 Lectures)
Solvent extraction: Classification, principle and
efficiency of the technique. Mechanism of extraction: extraction by solvation
and chelation. Technique of extraction: batch, continuous and counter current
extractions. Qualitative and quantitative aspects of solvent extraction:
extraction of metal ions from aqueous solution, extraction of organic
species from the aqueous
and non-aqueous media.
Chromatography techniques: Classification, principle
and efficiency of the technique. Mechanism of separation: adsorption, partition
& ion exchange. Development of chromatograms: frontal, elution and displacement methods.
Qualitative and quantitative aspects of chromatographic
methods of analysis using LC, GLC, TLC and HPLC.
UNIT 6: Sample Analysis: (20
Lectures)
Analysis of soil: Composition of soil, Concept
of pH and pH measurement, Complexometric titrations, Chelation, Chelating agents, use of
indicators
Determination of pH of soil samples.
- Estimation of Calcium
and Magnesium ions as Calcium
carbonate by complexometric titration.
- Analysis of water: Definition of pure water, sources responsible for contaminating water, water sampling methods, water
purification methods.
- Determination of pH,
acidity and alkalinity of a water sample.
- Determination of
dissolved oxygen (DO) of
a water sample.
- Analysis of food products:
Nutritional value of foods, idea about food processing and food
preservations and adulteration.
- Identification of adulterants in some common food items like coffee
powder, asafoetida, chilli
powder, turmeric powder, coriander powder and pulses, etc.
- Analysis of
preservatives and colouring matter.
- Analysis of cosmetics: Major and minor constituents and
their function
- Analysis of deodorants and antiperspirants, Al, Zn, boric
acid, chloride, sulphate.
- Determination of constituents of talcum powder:
Magnesium oxide, Calcium
oxide, Zinc oxide and Calcium
carbonate by complexometric titration.
SEMESTER-VIII
ADVANCED MAJOR COURSE-
AMJ 2: GREEN CHEMISTRY &
NANOCHEMISTRY
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
UNIT-1: Introduction to Green Chemistry:(3 Lectures)
What is Green Chemistry? Need for Green Chemistry.
Goals of Green Chemistry. Limitations/ Obstacles in the pursuit of the goals of
Green Chemistry.
UNIT -2: Principles of Green Chemistry and Designing Green Synthesis:(15
Lectures)
Twelve principles of Green Chemistry with their
explanations and examples; Designing a Green Synthesis using these principles;
Prevention of Waste/ by products; maximum incorporation of the materials used
in the process into the final products (Atom Economy); prevention/ minimization of hazardous/ toxic products; designing
safer chemicals – different
basic approaches to do so; selection of appropriate auxiliary substances
(solvents, separation agents), green solvents, solvent less processes,
immobilized solvents and ionic liquids.
Energy requirements for reactions
- use of microwaves, ultrasonic energy; selection of starting
materials; avoidance of unnecessary derivatization – careful use of
blocking/protecting groups; use of catalytic reagents(wherever possible) in
preference to stoichiometric reagents;
designing of biodegradable products; prevention of
chemical accidents; strengthening/ development
of analytical techniques to prevent and minimize the generation of hazardous
substances in chemical processes.
UNIT 3: Examples
of Green Synthesis/ Reactions (22 Lectures)
Green Synthesis of the following compounds: adipic
acid, catechol, BHT, methyl methacrylate, urethane, aromatic amines
(4-aminodiphenylamine), benzyl bromide, acetaldehyde, disodium iminodiacetate (alternative to Strecker synthesis), citral, ibuprofen,
paracetamol, furfural.
Microwave assisted reactions in water: Hofmann
Elimination, Hydrolysis (of benzyl chloride,
benzamide, n-phenyl benzamide, methyl benzoate to benzoic acid), Oxidation (of toluene, alcohols).
Microwave assisted reactions in organic solvents: Esterification, Fries
rearrangement, Orthoester Claisen Rearrangement, Diels-Alder Reaction,
Decarboxylation.
Microwave assisted solid
state reactions: Deacetylation, Deprotection. Saponification of esters, Alkylation of reactive
methylene compounds, reductions, synthesis of nitriles from aldehydes;
anhydrides from dicarboxylic acid; pyrimidine and pyridine derivatives; 1,2-
dihydrotriazine derivatives; benzimidazoles.
Ultrasound assisted reactions: Esterification,
saponification, substitution reactions, Alkylation, oxidation, reduction, coupling
reaction, Cannizaro reaction, Strecker synthesis,
Reformatsky reaction.
Nano chemistry
UNIT-4: Introduction to Nanoscience, Nanostructure and
Nanotechnology:(10 Lectures)
Basic idea; Overview of nanostructures and
nano-materials, classification, (cluster, colloid, nanoparticles, and
nanostructures, Spheroid, Wire, Rod, Tube, and Quantum Dot. Carbon nanotubes
and inorganic nanowires. Calculation of percentage of surface atom and surface
to volume ratio of spherical, wire, rod and disc shapes nanoparticles. Examples
of use of nanomaterials in environmental remediation, medicines and industry.
UNIT 5: Size Dependent Properties of Nanomaterials: (5 Lectures)
Basic idea with few examples only: Quantum
confinement, Electrical, Optical (Surface Plasmon resonance), variation in
colours (Blue shift & Red shift), Magnetic, thermal and catalytic properties.
UNIT 6: Synthesis
of Nanomaterials: (5 Lectures)
Brief introduction about Top-down and Bottom-up
approaches & self-assembly techniques of nanoparticles synthesis,
Solvothermal process, Examples of preparation of gold and silver metallic
nanoparticles, self-assembled nanostructures-control of nanoarchitecture-one
dimensional control. Carbon nanotubes and inorganic nanowires.
SEMESTER-VIII
ADVANCED MAJOR COURSE-
AMJ 3: MAJOR PRACTICALS-VII
Credit: Theory-04, 120 Hours,
Full Marks=100, Pass Marks= 40,
Marks: 25 (Attendance=5 + 20 SIE: 1Hr) + 75 (ESE: 6Hrs) = 100, Pass Marks: Practical(SIE + ESE) = 40
Colourimetry
- Verify Lambert-Beer’s law and
determine the concentration of
- CuSO4/KMnO4/K2Cr2O7 in a solution
of unknown concentration
- Determine the concentrations of KMnO4 and K2Cr2O7 in a
mixture.
Chromatography:
- Paper chromatographic
separation of Fe3+, Al3+, and Cr3+.
- Separation and identification of the monosaccharides present in the given mixture
(glucose & fructose) by paper chromatography. Reporting the Rf
values.
iii. Separate a mixture of Sudan yellow
and Sudan Red by TLC technique and identify them on the basis of their Rf values.
(iv) Chromatographic
separation of the active ingredients of plants, flowers and juices by TLC
Solvent Extractions:
- To separate a mixture of Ni2+ & Fe2+ by complexation with DMG and extracting the Ni2+- DMG
complex in chloroform, and determine its concentration by spectrophotometry.
- Determine the pH of the given aerated
drinks fruit juices, shampoos
and soaps.
- Determination of Na, Ca, Li in cola drinks and fruit juices
using flame photometric techniques.
Analysis of soil:
- Determination of pH
of soil.
- Total soluble salt
E Ion exchange:
- Determination of exchange capacity of cation exchange resins and anion exchange resins.
- Separation of metal ions from their binary
mixture.
- Separation of amino
acids from organic acids by ion
exchange chromatography.
F. Spectrophotometry
(i). Determination
of pKa values of indicator using spectrophotometry.
- Structural characterization of compounds by infrared spectroscopy.
- Determination of dissolved
oxygen in water.
- Determination of chemical
oxygen demand (COD).
- Determination of
Biological oxygen demand
(BOD).
- Determine the composition of the Ferric-salicylate/ ferric-thiocyanate complex
by Job’s method.
G. Green Chemistry and Nano Chemistry
- Preparation of biodiesel
from vegetable/ waste cooking
oil.
- Use of molecular
model kit to stimulate the reaction to investigate how the atom economy
illustrates Green Chemistry.
- Reactions like addition, elimination, substitution and rearrangement may also be studied for the calculation of atom economy.
- Benzoin condensation
using Thiamine Hydrochloride as a catalyst
(instead of cyanide).
- Extraction of D-limonene from orange peel using liquid
CO2 prepared form dry ice.
- Mechanochemical solvent free synthesis of azomethines
- Solvent free, microwave assisted one pot synthesis of phthalocyanine Cu(II)
complex.
- Photoreduction of benzophenone to benzopinacol in presence of sunlight.
- Synthesis of
Zinc Oxide nanoparticles.
- Synthesis of Iron Oxide nanoparticles.
- Synthesis of Nickel nanoparticle using urea decomposition method.
- Synthesis of Silver
and Gold nanoparticles
For BSc Honours with Research Degree
One Requires to Select RC-1 and RC-2 instead of AMJ-1, AMJ-2 & AMJ-3
SEMESTER-VIII
BSc (Research) Course
RC-I-RESEARCH
METHODOLOGY IN CHEMISTRY
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
Unit-1: Foundation of Research: 5 Lectures
Meaning, Objectives, Motivation, Utility. Concept of theory, empiricism, deductive and
inductive theory. Characteristics of scientific method - understanding the
language of research - Concept, Construct, definition, Variable. Research
Process
Unit-II: Problem Identification & Formulation: 7 Lectures
Definition and formulating the research problem,
Necessity of defining the problem, Importance
of literature review
in defining a problem, Research
Question - Investigation Question - Measurement
Issues - Hypothesis - Qualities of a good hypothesis - Null hypothesis &
Alternative Hypothesis. Hypothesis Testing - Logic & importance
Unit-III: Research Design: 7 Lectures
Concept and Importance in Research - Features of a good research
design - Exploratory Research Design - Concept,
Types and uses,
Descriptive Research Design - concept,
types and uses. Experimental Design - Concept of Independent &
Dependent variables.
Unit-IV: Qualitative and Quantitative Research:
Qualitative - 2 Lectures Quantitative Research
- Concept of measurement, causality, generalization, replication.
Merging the two approaches.
Unit-V: Data Collection and analysis: Execution of the
research - 3 Lectures Observation and Collection of data - Methods of data collection, hypothesis-testing -
Generalization and Interpretation.
Unit-VI: Measurement: 5 Lectures
Concept of measurement - what is measured? Problem
in measurement in research
- Validity and Reliability. Levels of measurement - Nominal, Ordinal, Interval,
Ratio.
Unit-VII: Sampling: 6 Lectures
Concept of Statistical population, Sample, Sampling
Frame, Sampling Error,
Sample size, Non-Response.
Characteristics of a good sample. Probability Sample - Simple Random Sample,
Systematic Sample, Stratified Random Sample & Multi-stage sampling.
Determining size of the
sample - Practical considerations in sampling and sample size.
Unit-VIII: Data Analysis: 4 Lectures
Data Preparation - Univariate analysis (frequency
tables, bar charts, pie charts, percentages),
Bivariate analysis - Cross tabulations and Chi-square test including testing hypothesis of association.
Unit-IX: Interpretation of Data and Paper Writing:
8 Lectures
Layout of a Research Paper, Journals in chemistry,
Impact factor of journals, When and where to publish?
Ethical issues related
to publishing, Plagiarism and Self-Plagiarism. Use of Encyclopaedias, Research Guides,
Handbook etc., Academic databases for concerned discipline. Use of tools /
techniques for Research: methods to search required information effectively,
Reference Management Software like Zotero/Mendeley, Software for paper
formatting like LaTeX/MSOffice, software for detection of Plagiarism.
Unit-X: Reporting and Thesis
writing: 7 Lectures
Structure and components of scientific reports - Types
of report - Technical reports and thesis - Significance - Different steps in
the preparation - Layout, Structure and Language of typical reports - Illustrations and tables - Bibliography, referencing and footnotes - Oral
presentation - Planning - Preparation - Practice - Making presentation - Use of visual aids -
Importance of effective communication
Unit-XI: Application of results
and ethics: 6 Lectures
Environmental impacts - Ethical issues
- ethical committees - Commercialization - Copy right - royalty - Intellectual property rights
and patent law - Trade related aspects of intellectual property Rights -
Reproduction of published material - Plagiarism - citation and acknowledgement
- citation and citation and acknowledgement - citation and acknowledgement -
Reproducibility and accountability.
SEMESTER-VIII
BSc Honours with Research
Course
RC-II- RESEARCH PROJECT
OR DISSERTATION
Credits: -08, Full Marks=200, Pass Marks= 80,
Course Objectives:
- To facilitate students in
conducting independent research projects in the field of Chemistry, allowing
them to apply theoretical knowledge to practical experimentation.
- To guide students in
developing research skills, including problem identification, formulation of
hypotheses, experimental design, data collection, analysis, and interpretation.
- To foster critical thinking
and analytical skills among students
through the exploration of research methodologies and
scientific literature.
- To enhance students' communication abilities by requiring
them to effectively present their research findings through written reports and oral
presentations.
- To cultivate ethical awareness
and responsibility in research practices, including proper citation,
acknowledgment of sources,
and adherence to ethical guidelines and regulations.
Course Outcomes:
- Students will demonstrate
proficiency in designing and conducting independent research projects in
Chemistry, from problem identification to data analysis.
- Students will develop advanced
skills in critical thinking, analytical reasoning, and problem-solving through
the exploration of complex scientific questions.
- Students will exhibit
competency in utilizing various research methodologies and techniques
appropriate for addressing specific research questions in Chemistry.
- Students will effectively communicate their research findings
through well-organized written
reports and articulate oral presentations.
- Students will demonstrate
ethical conduct in research, including proper citation practices, avoidance of
plagiarism, and adherence to ethical guidelines and regulations governing
scientific research in Chemistry.
Course Contents:
Students who achieve a minimum of 75% marks across the first six semesters and express a desire to engage in undergraduate
research may opt for a research stream during their fourth year of study. The
Head of the Department (HOD) is responsible for assigning a supervisor to these
students, chosen from the permanent faculty members holding a PhD degree.
Subsequently, students, in consultation with their supervisor, select a
research problem relevant and problem solving in nature to the local
community/Industry, environment and may be related to innovation/novel
method/idea with interdisciplinary approach to submit a synopsis or research
proposal to the department for review.
Following this, the HOD
convenes a meeting of the Departmental Research Council, where students present
their synopsis or research proposal for approval or rejection. Upon approval,
students commence their research work under the guidance of their supervisor
and in accordance with the approved proposal.
At the conclusion of the semester, Each and every
student has to submit the soft copy and the electronically typed hardbound copy
of the project thesis with the Plagiarism Report strictly adhering to the
University Grants Commission (Promotion of Academic Integrity and Prevention of
Plagiarism in Higher Educational Institutions) Regulations, 2018 F.
1-18/2010(CPP-II). Published in THE GAZETTE OF INDIA: EXTRAORDINARY [PART III—SEC. 4] dated 23rd July,2018 [web link :https://www.ugc.gov.in/pdfnews/7771545_academic-integrity-Regulation2018.pdf and the originality declarations of the
supervisor and the student along with the raw data as date notified/affixed by
the Head of the Department.
The department then forwards
the thesis to an external evaluator, who provides a report on the work. Following receipt of the external report,
the department shall
arrange an open viva voce examination for the
student, with both external and internal members present to assess the
student's work.
The Department Research Committee
shall be constituted from the following persons:
- HOD of the Department–Chairmen
- Dean, Faculty of Science-
External member
- HOD, University Department- External
member
- At list two permanent faculty member of the department (Nominated by HOD)- Members External members can be any
of the following:
- Permanent professors working
in the postgraduate department of the university or other colleges who have the
qualification to become PhD supervisors.
OR
Retired Professor/Associate
Professor/Assistant Professor of the university who has been supervising PhD
scholar/s.
OR
Professor/Associate
Professor/Assistant Professor of the outside university who has been
supervising PhD scholar/s.
Note- Minimum three external
examiner lists will be sent by HOD through concerned College Principal to the Controller of Examination, SKMU, Dumka
for final approval. In that list priority will be given as per order mentioned
above.
The project thesis shall be
evaluated under the heads as per the standard LaTex/Word format made available
by the Head of the Department which may include the following sections:
- Title Page:
- Title of the thesis
- Author's name
- Affiliation
- Date
- Abstract:
- A brief summary of the research
work, including the objectives, methods, results, and conclusions.
- Table of Contents:
- Lists all the major sections and subsections of the thesis,
along with their respective page numbers.
- List of Figures and Tables:
- Enumerates all the figures and
tables included in the thesis, along with their page numbers.
- Introduction:
- Provides background information on the research
topic.
- States the research problem
and objectives.
- Reviews relevant literature and previous research
in the field.
- Outlines the structure of the thesis.
- Experimental Methods:
- Describes the experimental procedures and methodologies used in the research.
- Includes details
on materials, equipment, and techniques employed.
- Provides sufficient information to allow for replication of the experiments.
- Results and Discussion:
- Presents the findings of the research.
- Organizes results
logically, often using figures, tables,
and graphs.
- Analyses and interprets
the results in the context of the research objectives.
- Discusses the implications of the findings
and their significance in the field.
- Conclusion:
- Summarizes the key findings
of the research.
- Restates the research objectives and addresses whether
they were achieved.
- Offers insights into the broader implications of the research.
- Suggests avenues
for future research.
- References:
- Lists all the sources cited in the thesis, following a
specific citation style (e.g., APA,
MLA, Chicago).
- Includes journal articles,
books, conference proceedings, and other relevant literature.
- Appendices:
- Contains additional
supplementary information that is relevant to the thesis but not essential to
the main text.
- Includes raw data, detailed
experimental procedures, calculations, or any
other supporting material.
Guidelines for distribution of marks may be as follows or as appropriate: Assessment of project
synopsis: 75 marks
Assessment of project thesis:
100 marks Viva-voce: 25 marks
For BSc Honours with Research Degree
One Requires to Select RC-1 and RC-2 instead of AMJ-1, AMJ-2 & AMJ-3
SEMESTER-VIII
BSc (Research) Course
RC-I-RESEARCH
METHODOLOGY IN CHEMISTRY
Credit: Theory-04, Full Marks=100, Pass Marks= 40, Lectures:60
Marks: 25 (5 Attendance+ 20 SIE: 1Hr) + 75 (ESE: 3Hrs) = 100 Pass Marks: Th (SIE + ESE) = 40
Unit-1: Foundation of Research: 5 Lectures
Meaning, Objectives, Motivation, Utility. Concept of theory, empiricism, deductive and
inductive theory. Characteristics of scientific method - understanding the
language of research - Concept, Construct, definition, Variable. Research
Process
Unit-II: Problem Identification & Formulation: 7 Lectures
Definition and formulating the research problem,
Necessity of defining the problem, Importance
of literature review
in defining a problem, Research
Question - Investigation Question - Measurement
Issues - Hypothesis - Qualities of a good hypothesis - Null hypothesis &
Alternative Hypothesis. Hypothesis Testing - Logic & importance
Unit-III: Research Design: 7 Lectures
Concept and Importance in Research - Features of a good research
design - Exploratory Research Design - Concept,
Types and uses,
Descriptive Research Design - concept,
types and uses. Experimental Design - Concept of Independent &
Dependent variables.
Unit-IV: Qualitative and Quantitative Research:
Qualitative - 2 Lectures Quantitative Research
- Concept of measurement, causality, generalization, replication.
Merging the two approaches.
Unit-V: Data Collection and analysis: Execution of the
research - 3 Lectures Observation and Collection of data - Methods of data collection, hypothesis-testing -
Generalization and Interpretation.
Unit-VI: Measurement: 5 Lectures
Concept of measurement - what is measured? Problem in measurement in research - Validity and Reliability. Levels of measurement - Nominal, Ordinal, Interval, Ratio.
Unit-VII: Sampling: 6 Lectures
Concept of Statistical population, Sample, Sampling
Frame, Sampling Error,
Sample size, Non-Response.
Characteristics of a good sample. Probability Sample - Simple Random Sample,
Systematic Sample, Stratified Random Sample & Multi-stage sampling.
Determining size of the sample - Practical considerations in sampling and sample size.
CHEMISTRY MINOR COURSES
Semester Internal Examination (SIE 10+5=15 marks):
There will be two group of
questions.
The Semester Internal Examination shall have two components. (a) One
Semester Internal Examination Written Test (SIE) of 10 Mark. Question No.1 will be very short answer type in Group A
consisting of five questions of 1 mark each. Group B will contain descriptive
type two questions of five marks each, out of which any one to answer. (b) Class Attendance
Score (CAS) including the behaviour of the student towards teachers and other
students of the College of 5 marks.
End Semester Examination (ESE 60 marks):
There will be two group of
questions. Group A is compulsory which will contain three questions. Question
No.1 will be very short answer type consisting of five questions of 1 mark
each. Question No.2 & 3 will be short answer type of 5 marks. Group B will
contain descriptive type five questions of fifteen marks each, out of which any
three are to answer.
Note: There may be subdivisions in
the questions of group B.
Section A: Physical Chemistry
UNIT I: Chemical Energetics: (8 classes
each of 60 minutes duration)
Review
of thermodynamics and the Laws of Thermodynamics.
Important
principles and definitions of thermochemistry. Concept of standard state and
standard enthalpies of formations. Calculation of bond energy, bond
dissociation energy from thermochemical data. Statement of Third Law of
thermodynamics and calculation of absolute entropies of substances.
UNIT II: Chemical Kinetics: (7 classes
each of 60 minutes duration)
The
concept of reaction rates. Effect of temperature, pressure, catalyst and other
factors on reaction rates. Order and molecularity of a reaction. Derivation of
integrated rate equations for zero, first and second order reactions (both for
equal and unequal concentrations of reactants). Half–life of a reaction.
General methods for determination of order of a reaction. Concept of activation
energy and its calculation from Arrhenius equation.
Section B: Inorganic Chemistry
UNIT III: Atomic Structure: (5 classes each of 60
minutes duration)
What
is Quantum mechanics? Time independent
Schrodinger equation and meaning of various terms in it. Significance of ψ and ψ2 , Schrodinger
equation for hydrogen atom. Radial and angular parts of the hydrogenic wave
functions (atomic orbitals) and their variations for 1s, 2s, 2p, 3s, 3p and 3d
orbitals (Only graphical representation). Radial and angular nodes and their
significance. Radial distribution functions and the concept of the most
probable distance with special reference to 1s and 2s atomic orbitals.
Significance of quantum numbers, orbital angular momentum and quantum numbers
ml and ms. Shapes of s, p and d atomic orbitals, nodal planes.
Discovery of spin, spin quantum number (s) and magnetic spin quantum number (ms).
Rules
for filling electrons in various orbitals, Electronic configurations of the
atoms. Stability of half-filled and completely filled orbitals, concept of
exchange energy. Relative energies of atomic orbitals, Anomalous electronic
configurations.
UNIT IV: Chemical Bonding and Molecular
Structure: (10 classes each of 60 minutes duration)
Ionic Bonding: General characteristics of ionic bonding. Energy
considerations in ionic bonding, lattice energy and solvation energy and their
importance in the context of stability and solubility of ionic compounds.
Polarizing power and polarizability. Fajan’s rules, ionic character in covalent
compounds, bond moment, dipole moment and percentage ionic character.
Covalent bonding: VB Approach: Shapes of some inorganic molecules and
ions on the basis of VSEPR and hybridization with suitable examples of linear,
trigonal planar, square planar, tetrahedral, trigonal bipyramidal and
octahedral arrangements.
Section
C: Organic Chemistry
UNIT V: Fundamentals of Organic
Chemistry: (3 classes each of 60 minutes duration)
Inductive
Effect, Electromeric Effect, Resonance and Hyperconjugation. Cleavage of Bonds:
Homolysis and Heterolysis. Structure, shape and reactivity of organic
molecules: Nucleophiles and
electrophiles. Reactive Intermediates: Carbocations, Carbanions and free
radicals.
Aromaticity:
Benzenoids and Hückel’s rule.
UNIT VI: Aliphatic hydrocarbons:
Alkanes: (4 classes each of 60 minutes
duration) (Upto 5 Carbons)
Preparation:
Catalytic hydrogenation, Wurtz reaction, Kolbe’s synthesis, from Grignard reagent.
Reactions: Free radical Substitution: Halogenation
Alkenes: (3 classes each of 60 minutes
duration) (Upto 5 Carbons)
Preparation:
Elimination reactions: Dehydration of alkenes and dehydrohalogenation of alkyl
halides (Saytzeff’s rule),
Reactions: cis-addition (alk.
KMnO4) and trans-addition (bromine), Addition of HX (Markownikoff’s and
antiMarkownikoff’s addition), Hydration, Ozonolysis, oxymecuration-demercuration,
Hydroboration-oxidation.
Alkynes: (3 classes each of 60 minutes
duration) (Upto 5 Carbons)
Preparation:
Acetylene from CaC2 and conversion into higher alkynes, by dehalogenation of
tetra halides and dehydrohalogenation of vicinal-dihalides.
Reactions:
Formation of metal acetylides, addition of bromine and alkaline KMnO4,
ozonolysis and oxidation with hot alkaline KMnO4.
UNIT VII: Aromatic hydrocarbons: (5
classes each of 60 minutes duration)
Preparation of benzene: from phenol, by decarboxylation, from acetylene, from benzene sulphonic acid. Reactions of benzene: Electrophilic substitution: nitration, halogenation and sulphonation. Friedel-Craft’s reaction (alkylation and acylation). Side chain oxidation of alkyl benzenes (upto 4 carbons on benzene)
There will be one Practical Examination of 3 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:
One Experiment = 15 marks
Practical record notebook = 05 marks
Viva-voce = 05 marks
Section A: Physical
Thermochemistry
1. Determination
of heat capacity of calorimeter.
2. Determination
of enthalpy of neutralization of hydrochloric acid with sodium hydroxide.
3. Determination
of integral enthalpy of solution of salts (KNO3, NH4Cl).
4. Determination
of enthalpy of hydration of copper sulphate.
Section
B: Inorganic Chemistry - Volumetric Analysis
1.
Acid-Base Titrations
a. Estimation
of oxalic acid present in the supplied sample.
b. Estimation
of sodium hydroxide present in given sample.
c. Estimation
of amount of acetic acid in vinegar solution.
d. Estimation
of carbonate and hydroxide present together in mixture.
e. Estimation
of carbonate and bicarbonate present together in a mixture.
f. Estimation
of free alkali present in different soaps/detergents.
2.
Oxidation-Reduction Titrimetry
a. Estimation
of Fe(II) in supplied solution using standardized KMnO4
solution.
b. Estimation
of oxalic acid using standardized KMnO4 solution.
c. Estimation
of percentage of Fe(II) in Iron fillings with standard K2Cr2O7
Section
C: Organic Chemistry
1. Purification
of organic compounds by crystallization (from water and alcohol) and
distillation.
2. Criteria
of Purity: Determination of melting and boiling points.
3. Recrystallisation,
determination of melting point and calculation of quantitative yields to be
done.
a. Benzoylation
of amines/phenols
b. Oxime and 2,4 dinitrophenyl hydrazone of aldehyde/ketone
Instruction to Question Setter for
Semester Internal Examination (SIE 10+5=15 marks):
There will be two group of
questions.
The Semester Internal Examination shall have two components. (a) One
Semester Internal Examination Written Test (SIE) of 10 Mark. Question No.1 will be very short answer type in Group A
consisting of five questions of 1 mark each. Group B will contain descriptive
type two questions of five marks each, out of which any one to answer. (b) Class Attendance
Score (CAS) including the behaviour of the student towards teachers and other
students of the College of 5 marks.
End Semester Examination (ESE 60 marks):
There will be two group of
questions. Group A is compulsory which will contain three questions. Question
No.1 will be very short answer type consisting of five questions of 1 mark
each. Question No.2 & 3 will be short answer type of 5 marks. Group B will
contain descriptive type five questions of fifteen marks each, out of which any
three are to answer.
Note: There may be subdivisions in
the questions of group B.
Section A: Physical Chemistry
UNIT I: Equilibrium: (15 classes each of
60 minutes duration)
Chemical Equilibria: Le Chatelier’s principle. Relationships between Kp,
Kc and Kx for reactions involving ideal gases. Free energy change in a chemical
reaction. Thermodynamic derivation of the law of chemical equilibrium.
Distinction between ΔG° and ΔG ,
Ionic
Equilibria: Strong, moderate and weak electrolytes, degree of ionization,
factors affecting degree of ionization, ionization constant and ionic product
of water. Ionization of weak acids and bases, pH scale, common ion effect. Salt
hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for
different salts. Buffer solutions. Solubility and solubility product of
sparingly soluble salts – applications of solubility product principle.
Section B: Inorganic Chemistry (8
classes each of 60 minutes duration)
MO Approach: Rules for the
LCAO method, bonding and antibonding MOs and their characteristics for s-s, sp
and p-p combinations of atomic orbitals, nonbonding combination of orbitals, MO
treatment of homonuclear diatomic molecules of 1st and 2nd periods (including
idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and NO
. Comparison of VB and MO approaches.
Section C: Organic Chemistry
UNIT II: Alkyl and Aryl Halides
Alkyl
Halides (Upto 5 Carbons) (5 classes each of 60 minutes duration)
Types of Nucleophilic
Substitution (SN1, SN2 and SNi)
reactions. Preparation: from alkenes and
alcohols. Reactions: hydrolysis, nitrite
& nitro formation, nitrile & isonitrile formation. Williamson’s ether
synthesis: Elimination vs substitution.
Aryl Halides (3 classes each of 60
minutes duration)
Preparation:
(Chloro, bromo and iodo-benzene case): from phenol, Sandmeyer & Gattermann
reactions. Reactions (Chlorobenzene):
Aromatic nucleophilic substitution (replacement by –OH group) and effect of
nitro substituent. Benzyne Mechanism: KNH2/NH3 (or NaNH2/NH3).
Reactivity
and Relative strength of C-Halogen bond in alkyl, allyl, benzyl, vinyl and aryl
halides.
Alcohols: (4 classes each of 60 minutes
duration)
Preparation: Preparation of 1o, 2о and 3o
alcohols: using Grignard reagent, Ester hydrolysis, Reduction of aldehydes,
ketones, carboxylic acid and esters.
Reactions: With sodium, HX (Lucas test),
esterification, oxidation (with PCC, alk. KMnO4, acidic dichromate,
conc. HNO3). Oppeneauer oxidation Diols: (Upto 6 Carbons) oxidation
of diols. Pinacol-Pinacolone rearrangement.
Phenols: (3
classes each of 60 minutes duration)
Preparation: Cumene hydroperoxide method, from
diazonium salts.
Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation.
Reimer- Tiemann Reaction, Gattermann-Koch Reaction, Houben–Hoesch Condensation,
Schotten – Baumann Reaction.
Ethers
(aliphatic and aromatic): (2 classes each of 60 minutes duration) Cleavage of ethers with
HI.
Aldehydes
and ketones (aliphatic and aromatic): (5 classes each of 60 minutes duration) (Formaldehye, acetaldehyde, acetone and
benzaldehyde) Preparation: from acid
chlorides and from nitriles.
Reactions– Reaction with HCN, ROH, NaHSO3,
NH2-G derivatives. Iodoform test. Aldol Condensation, Cannizzaro’s
reaction, Wittig reaction, Benzoin condensation. Clemensen reduction and Wolff
Kishner reduction. Meerwein-Pondorff Verley reduction.
End Semester Examination (ESE):
There will be one Practical Examination of 3 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:
One Experiment = 15 marks
Practical record notebook = 05 marks
Viva-voce = 05 marks
Section A: Physical Chemistry
Ionic equilibria pH measurements
1. Measurement
of pH of different solutions like aerated drinks, fruit juices, shampoos and
soaps (use dilute solutions of soaps and shampoos to prevent damage to the
glass electrode) using pH-meter.
2. Determine the
pH of the given aerated drinks fruit juices, shampoos and soaps.
3. Preparation
of buffer solutions:
a. Sodium
acetate-acetic acid
b. Ammonium
chloride-ammonium hydroxide
Section B:
Organic Chemistry
1. Detection of
hetero elements in organic compounds.
2. Functional
group tests for alcohols, phenols, carbonyl and carboxylic acid group.
3. Purification
of organic compounds by crystallization (from water and alcohol) and
distillation.
4. Criteria of Purity:
Determination of melting and boiling points.
5. Preparations:
Mechanism of various reactions involved to be discussed.
6. Recrystallisation,
determination of melting point and calculation of quantitative yields to be
done. A. Oxime of aldehyde/ketone
b.
2,4 dinitrophenylhydrazone of aldehyde/ketone
7. Analysis of
soaps and detergents.
8. Preparation
of Nylon-6, Nylon-66 9. Preparation of face cream
10. Vitamin-C preparation.
Instruction to Question Setter for
Semester Internal
Examination (SIE 10+5=15 marks):
There will be two group of questions.
The Semester Internal
Examination shall have two components. (a) One Semester Internal Examination
Written Test (SIE) of 10 Mark. Question No.1 will be very short answer
type in Group A consisting of five questions of 1 mark each. Group B will
contain descriptive type two questions of five marks each, out of which any one
to answer. (b)
Class Attendance Score (CAS) including the behaviour of the student towards
teachers and other students of the College of 5 marks.
End Semester
Examination (ESE 60 marks):
There will be two group of questions. Group A is
compulsory which will contain three questions. Question No.1 will be very short
answer type consisting of five questions of 1 mark each. Question No.2 & 3
will be short answer type of 5 marks. Group B will contain descriptive type
five questions of fifteen marks each, out of which any three are to answer.
Note: There may be subdivisions in the questions of group B.
SECTION-A: Inorganic Chemistry
UNIT I: General Principles of Metallurgy: (5 Lectures)
Chief modes of occurrence of metals based on standard
electrode potentials. Ellingham diagrams
for reduction of metal oxides using carbon as reducing agent.
Hydrometallurgy, Methods of purification of metals
(Al, Pb, Ti, Fe, Cu, Ni, Zn): electrolytic, oxidative refining, Kroll process,
Parting process, van Arkel-de Boer process and Mond’s process.
UNIT II: s-
and p-Block Elements: (5 Lectures)
Periodicity in s- and p-block elements with respect to
electronic configuration, atomic and ionic size, ionization enthalpy,
electronegativity (Pauling, Mulliken, and Alfred-Rochow scales). Allotropy in
C, S, and P.
Oxidation states with reference to elements in unusual
and rare oxidation states like carbides and nitrides), inert pair effect,
diagonal relationship and anomalous behaviour of first member of each
group.
UNIT III: Compounds
of s- and p-Block Elements: (10 Lectures) Hydrides and their classification (ionic, covalent and
interstitial), structure and properties with respect to stability of hydrides
of p- block elements. Concept of multicentre bonding (diborane). Structure,
bonding and their important properties like oxidation/reduction, acidic/basic
nature of the following compounds and their applications in industrial, organic
and environmental chemistry. Hydrides of nitrogen (NH3, N2H4,
N3H, NH2OH)
Oxoacids of P, S and Cl. Halides
and oxohalides: PCl3, PCl5, SOCl2 and SO2Cl2
Section
B: Physical Chemistry
UNIT IV: Kinetic
Theory of Gases: (15 Lectures)
Postulates of Kinetic Theory of Gases and derivation
of the kinetic gas equation. Most probable, average and root mean square
velocities (no derivation). Collision number, collision frequency, collision
diameter and mean free path of molecules. Maxwell Boltzmann distribution laws
of molecular velocities and molecular energies (graphic representation –
derivation not required) and their importance.
Deviation of real gases from ideal behaviour,
compressibility factor, causes of deviation. Van der Waals equation of state
for real gases. Boyle temperature (derivation not required). Critical
phenomena, critical constants and their calculation from van der Waals
equation. Andrews isotherms of CO2. Viscosity of gases and effect of
temperature and pressure on coefficient of viscosity (qualitative treatment
only).
UNIT V: Liquids: (4 Lectures)
Surface tension and its determination using
stalagmometer. Viscosity of a liquid and determination of coefficient of
viscosity using Ostwald viscometer. Effect of temperature on surface tension
and coefficient of viscosity of a liquid (qualitative treatment only)
UNIT VI: Solids (6 Lectures)
Forms of solids. Symmetry elements, unit cells,
crystal systems, Bravais lattice types and identification of lattice planes.
Laws of Crystallography – Law of constancy of interfacial angles, Law of
rational indices. Miller indices. X–Ray diffraction by crystals, Bragg’s law.
Structures of NaCl, KCl and CsCl (qualitative treatment only). Defects in
crystals. Glasses and liquid crystals.
End Semester Examination (ESE):
There will be one Practical Examination of 3 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:
One Experiment = 15 marks
Practical record notebook = 05 marks
Viva-voce = 05 marks
Section A: Inorganic Chemistry
Qualitative semi micro analysis
1.
Semi-micro qualitative analysis using H2S
of mixtures- not more than four ionic species (two anions and two cations and
excluding insoluble salts) out of the following:
Cations: NH4+, Pb2+, Ag+,
Bi3+, Cu2+, Cd2+, Sn2+, Fe3+,
Al3+, Co2+, Cr3+, Ni2+,Mn2+,
Zn2+, Ba2+, Sr2+, Ca2+, K+
Anions : CO3 2– , S2–,
SO2–, S2O32–, NO3 –,
CH3COO–, Cl–, Br–, I–,
NO3–,SO42-, PO43-,
BO33-, C2O4 2-, F-(Spot
tests should be carried out wherever feasible)
Section B: Physical Chemistry
(I) Surface
tension measurement (use of organic solvents excluded).
a) Determination
of the surface tension of a liquid or a dilute solution using a stalagmometer.
b) Study
of the variation of surface tension of a detergent solution with
concentration.
(II) Viscosity measurement (use of organic solvents
excluded).
a) Determination
of the relative and absolute viscosity of a liquid or dilute solution using an
Ostwald’s viscometer.
b) Study
of the variation of viscosity of an aqueous solution with concentration of
solute.
(III)Chemical
Kinetics
Study the kinetics of the following
reactions.
a. Initial
rate method: Iodide-persulphate reaction
b. Integrated
rate method:
c. Acid
hydrolysis of methyl acetate with hydrochloric acid.
d. Saponification
of ethyl acetate.
e. Compare the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of methyl acetate
MULTIDISCIPLINARY COURSE IN CHEMISTRY
Instruction to Question Setter for
End Semester Examination (ESE 75 marks):
There will be two group of
questions. Group A is compulsory which will contain three questions. Question
No.1 will be very short answer type consisting of five questions of 1 mark
each. Question No. 2 & 3 will be short answer type of 5 marks. Group B will
contain descriptive type six questions of fifteen marks each, out of which any
four are to answer.
Note: There may be subdivisions in
the questions of group B.
Unit-I: Food & Nutrition (12 Lectures)
Basic
concept on Food, Nutrition and Nutrients. Classification of Food,
Classification
of
Nutrients. Carbohydrates-Definition, sources, classification, and
properties Fatty acids-composition, properties, types. Lipids -Definition, sources,
Classification & Properties, daily requirements, function Role &
nutritional significances of PUFA, MUFA, SFA, W-3 fatty acid. Proteins-
Definition, Sources, classification & properties, daily requirements, functions.
Assessment of Protein quality (BV, PER, NPU). Vitamins- Definition, sources, classification,
diseases caused by deficiency of Vitamins. Minerals - Definition, sources, classification,
diseases caused by deficiency of minerals.
Unit-II Chemicals in Food (6 Lectures)
Introductory
idea of Food colours, Flavours and sweeteners, Fat emulsifiers and stabilizing
agents, Flour improvers - antistaling agents and bleaches, Antioxidants,
Nutritional supplements such as minerals, vitamins and amino acids.
Unit-III Food Preservation (6 Lectures)
Food
preservation: definition, objectives and principles of food preservation.
Different methods of food preservation. Preserved Products: Jelly, Marmalade,
Sauces, Pickles, Squashes, Syrups-Definitions, types, composition, storage,
uses and nutritional aspects, Food Standards: ISI, Agmark, FPO, MPO, PFA,
FSSAI.
Unit-IV Agrochemicals (6 Lectures)
Herbicides-Definition,
Classification, properties, uses and health hazards, Fungicides Definition,
Classification, properties, uses and health hazards, Insecticides- Definition,
Classification, properties, uses and health hazards, traditional pesticides.
Unit-V Drugs and Medicines (6 Lectures)
Drugs- Definition, Classification, Antacids, Antihistamines,
Tranquilizers, analgesics, antidepressant drugs, Antimicrobials, Antibiotics,
Antiseptics and disinfectants, medicinal uses of common herbs and plants.
Unit-VI Chemistry of Materials (9 Lectures)
Soaps and Detergents – Definition, Classification & their action, Biofuels – Definition, Classification ,production of biofuels and its utility as alternative fuel source, Fibers: Definition, Classification and their uses, natural fibers, cotton, wool, silk, rayon, artificial fibers, polyamides, acrylic acid, PVC, PVA; Examples of natural biodegradable polymers synthetic biodegradable polymers. Use of polymeric materials in daily life.
Comments
Post a Comment