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.
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.
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