Kuvempu
University
Sahyadri Science College (Autonomous)
New Syllabus- Autonomous-III
Implemented from academic year 2013-14
Syllabus for B.Sc course in Chemistry
I Semester—Paper I
Section A: Inorganic Chemistry
Total Hours: 20
Chapter-1: Atomic structure
10 hours (12 marks weightage)
Wave nature of electron-de Broglie equation. Heisenberg uncertainty principle. Schrodinger
wave equation (no derivation). Significance of  and 2 –atomic orbitals, Eigen values and
eigen function, radial angular wave function and probability distribution curve.
Quantum numbers and their significance. Shapes of s, p and d-orbitals and their nodal planes.
Assigning of quantum number to a given electron in an atom (I and II period elements) in the
periodic table. Pauli’s exclusion principle, energy level diagram, Aufbau principle, Hund’s
multiplicity rule, electronic configuration of elements (up to 3d- series), (n+l) rule, effective
nuclear charge, screening effect based on Slater’s rule. Problems to be solved
Chapter-2: Periodic properties
5 hours (7 marks weightage)
Atomic radii (covalent radii), vander Waal’s radii, ionic radii, variation of atomic radii in a
group, period and in isoelectronic ions.
Ionization energy: Explanation, factors influencing ionization energy, variation of ionization
energy in a group and period. Successive ionization energies, effect of ionic size and
electronic configuration (III period).
Electron affinity: Definition, explanation, variation in a group and period, explanation for
the observed trend.
Electronegativity: Definition, explanation, factors influencing electronegativity variation in
a group and period, explanation for the observed trend, Anomalies to be accounted, Pauling
scale and Mulliken’s scale of electronegativity (Problems to be solved).
Chapter 3: Volumetry
5hours(7 marks weightage)
Titrimetric method of analysis- Introduction, Primary and secondary standards, Requirement
of a primary standard substances,
Acid base titration-Types, Ostwald’s theory of acid-base indicator, choice of acid-base
indicator.
Redox titration- Theory of redox indicators with reference to diphenyl amine.
Complexometric titrations-Definitions, types of EDTA titrations, estimation of Zn2+ using
EDTA, metal indicators, principles and theory.
Iodometric titrations-Principles, applications (estimation of copper, available chlorine in
bleaching powder)
1
Reference Books:
1. Principles of Inorganic Chemistry by Puri, Sharma and Kalia.
2. Advanced inorganic Chemistry by Gurudeep Raj and Chatwal Anand.
3. Concise Inorganic Chemistry by J. D. Lee.
4. Basic Inorganic Chemistry by F. A. Cotton, G. Wilkinson and P. L. Gaus.
5. Modern Inorganic Chemistry by RD Madan
6. Advanced Practical Inorganic Chemistry by Gurudeep Raj.
7. A textbook of quantitative inorganic analysis by A. I. Vogel.
Section B: Organic Chemistry
Total Hours: 20
Chapter-1: Classification and Nomenclature of organic compounds:
5 hours (6 marks weightage)
Introduction, general classification based on structure and functional group with examples.
IUPAC names of alkanes, cycloalkanes, alkenes, dienes, alkynes, alkylhalides, alcohols,
ethers, aldehydes, ketones, carboxylic acids, esters, amines and multifunctional compounds.
(Only for Open chain compounds).
Chapter-II: Purification of organic compounds:
5 hours(6marks weightage)
Basic principle and practice (Suitable example to each method)
a) Methods of purification of solids- crystallization, fractional crystallization and sublimation
b) Methods of purification of liquids- Distillation, fractional distillation, distillation under
reduced pressure.
c) Solvent extraction- separating funnel method, soxhlet extraction method
d) Criteria of purity- melting point and boiling point (Capillary method).
Chapter-III: Composition of organic compounds:
5 hours (7 marks weightage)
a) Estimation of elements- C and H by Liebig’s method N by Kjaldahl’s method, P, S and X
(halogens) by Carius method (numerical problems).
b) Empirical and molecular formulae and their determinations with numerical problems.
Chapter-IV: Organic reactions and reaction intermediates: 5 hours(7marks weightage)
Homolysis and heterolysis, electrophilles, nueleophiles.
Types of reactions: Addition, elimination, substitution and rearrangement reactions with
suitable example.
Carbocations, carbanions and Free radicals (definition, formation, geometry, stability by
considering primary, secondary, tertiary, allylic and aromatic species).
2
Section C: Physical Chemistry
Total Hours: 20
Chapter 1: Gases
5 hours (06 Marks Weightage)
Molecular velocities-Maxwell-Boltzmann distribution of molecular velocities (no
derivation)-basic concept of Maxwell-Boltzmann equation, types of molecular velocitiesderivation of expression for RMS velocity, average velocity and most probable velocityrelationship between the three and problems to be worked out. Effect of temperature on
distribution of molecular velocities, Maxwell-Boltzmann energy distribution as a function of
temperature-degree of freedom, law of equipartition of energy and its calculation for mono,
di and tri-atomic molecule. Boltzmann factors and its importance.
Specific heat and molar heat capacities of gases, CV and CP and their relation, CP/CV ratios.
(problems to be solved).
Chapter 2: Critical Phenomena
5 hours (06 Marks Weightage)
Real gases, PV-isotherm of CO2, critical constants-Tc, Pc, and Vc definitions- vander Waal’s
equation of state for real gases-relationship of vander Waal’s constants a and b with critical
constants Tc, Pc and Vc (to be derived using isotherm of CO2) numerical problems on Tc, Pc
and Vc- experimental determination of Tc and Pc using Caignard–de-la Tours apparatus and
Vc by Cailletets and Mathias method. Law of corresponding states and reduced equation of
state (to be derived). Principle of liquefaction of gases, inversion temperature.
Chapter 3: Liquid mixtures
10 hours (14 Marks Weightage)
Classification of binary liquid mixtures into partially miscible, completely miscible and
completely immiscible liquids.
i) Completely miscible liquids
Ideal liquid mixtures-Raoult’s law, non ideal liquid mixtures showing (a) very slight +ve
deviation from ideal behaviour (type-I) from Raoult’s law (eg. C6H6+C6H5CH3)(b) very high
+ve deviation Eg: ethanol+water (type-II) system (c) –ve deviation (type-III) from Raoult’s
law- HCl + water as example, vapour pressure – composition diagram and boiling point
composition diagrams for all the three types of liquid mixtures, principle of fractional
distillation of type –I, type-II and type-III liquid mixtures and azeotropic mixtures (minimum
and maximum).
ii) Partially miscible liquid mixtures
Critical solution temperature (CST) –phenol-water system ( U-CST), trimethyl amine-water
system (L-CST) and nicotine-water (UL-CST). Mutual solubility temperature verses
composition curve to be draw for each system – effect of addition of impurity on CST with
an example (electrolyte and an organic compound impurities on phenol-water system).
Experimental determination of CST of Phenol-water system.
iii) Completely immiscible liquids
Immiscible liquid pairs with examples, steam distillation, principles, experimental,
determination of molecular weight and its application (problems to be solved).
3
I SEMESTER PRACTICALS
Volumetric Analysis
1. Calibration of burette, pipette, standard flask.
2. Estimation of NaOH using approximately 0.1N HCl solution and anhydrous sodium
carbonate
3. Estimation of HCl using approximately 0.1N NaOH solution and pot. biphthalate crystals.
4. Preparation of standard solution of oxalic acid, Standardisation of NaOH and estimation
of H2SO4 solution.
5. Estimation of Mohr’s salt using approximately 0.1N KMnO4 solution and oxalic acid
crystals.
6. Estimation of ferric chloride using approximately 0.1N K2Cr2O7 solutions and Mohr’s salt
crystals (Diphenyl amine indicator method).
7. Estimation of copper sulphate solution using approximately 0.1N sodium thiosulphate
solution and K2Cr2O7 crystals.
8. Estimation of available chlorine in bleaching powder.
9. Estimation of hardness of water using EDTA solution and ZnSO4 crystals.
4
Kuvempu
University
Sahyadri Science College (Autonomous)
New Syllabus- Autonomous-III
Implemented from academic year 2013-14
Syllabus for B.Sc course in Chemistry
II Semester—Paper II
Teaching hours: 4 Hours per week
Total Hours: 60Hours
Section A: Inorganic Chemistry
Total Hours: 20
Chapter-I: Chemical Bonding:
5 hours (7 marks waitage)
Ionic bond: Definition, lattice energy, factors controlling lattice energy, Born-Haber cycle
taking NaCl as example, Born-Lande equation (no derivation), significance of the equation,
internuclear distance between oppositely charged ions, hydration energy (solubility of ionic
solids) and its dependence on lattice energy, polarization, polarizing power, polarizability of
ions, Fazan’s rule.
Chapter-II: Covalent Bond:
4 hours (5 marks waitage)
VBT- formation of H2 molecule- (taking  wave functions of atomic orbitals)  and  bonds
with their characteristics, postulates of valance bond theory-electronegativity, polar and non
polar bonds, electronegativity differences, variation of percentage ionic character of the bond
(problems to be solved).
Chapter-III: Hybridization:
3 hours (4 marks waitage)
sp3 (CCl4), sp3d(PCl5), sp3d2(SF6).VSEPR Theory: Assumptions of VSEPR theory, shape of
SF4, BrF5, ClF3 and XeF2. Limitations of VSEPR theory
6 hours (7 marks waitage)
Molecular orbital theory: Basic principle of MOT, Linear combination of atomic orbital in
terms of wave functions, conditions for combination of atomic orbitals, energy levels of
molecular orbitals, rules for filling molecular orbitals, molecular orbital diagram and bond
order for O2, O2+,O22-.
Hetero nuclear diatomic molecules: CO, NO, CN- (prediction of magnetic properties of
these species)
Chapter IV: Metallic bonding (MOT Approach):
2 hours (3 marks waitage)
Band theory of solids (potential energy verses internuclear distance curve), conductors,
insulators, semiconductors.
5
Reference Books:
1. Principles of Inorganic chemistry by Puri, Sharma and Kalia.
2. Advanced inorganic chemistry by Gurudeep Raj and Chatwal Anand.
3. Modern Inorganic Chemistry by RD Madan
4. Theoretical principles of inorganic Chemistry by G.S.Manku
5.
Basic Inorganic Chemistry by F. A. Cotton, G. Wilkinson and P. L. Gaus.
6. Concise Inorganic Chemistry by J. D. Lee.
7. Advanced Practical Inorganic Chemistry by Gurudeep Raj.
Section B: Organic Chemistry
Total Hours: 20
Chapter-I: Hybridization
3 hours (4 marks weightage)
Overlapping of atomic orbital’s, types of overlapping SP3, SP2 and SP hybridization taking
examples of methane, ethylene and ethyne molecules. Bond length, bond angle, bond energy.
Chapter-II: Alkanes:
2 hours (3 marks weightage)
Methods of preparation: Wurtz, Kolbe and Corey-House method of synthesis. Free radical
mechanism of chlorination of methane and pyrolysis of alkanes.
Chapter-III: Alkenes:
4 hours (5 marks weightage)
Methods of preparation: By dehydration of alcohols and dehydrohalogenation of alkyl
halides, addition of bromine to ethene and its mechanism, mechanism of addition of HBr to
symmetrical and unsymmetrical alkenes (Markownkoff’s rule). Saytzeff rule, Hoffmann
elimination. AntiMarkownkoff’s rule (peroxide effect with mechanism), epoxidation,
ozonolysis (taking examples of 1-butene and 2-butene), hydroxylation and oxidation with
KMnO4.
Chapter-IV: Dienes:
3 hours (4 marks weightage)
Types with examples, synthesis of 1,3-butadiene (dehydration of diols, dehydrohalogenation
of dihalides), Resounance structre and molecular orbital picture of 1,3-butadiene.
Mechanism of addition of one mole Br2 to 1,3-butadiene, Diels-Alder reaction.
Chapter-V: Alkynes
4 hours (5 marks weightage)
Preparation by dehydrohalogenation of dihalides and dehalogenation of tetrahalides, acidity
of alkynes, formation of metal alkynides, Mechanism of electrophilic addition of propyne
with HCl, and Br2.
Nucleophilic addition of acetylene with HCN, H2O, CH3COOH, C2H5OH.
6
Chapter-VI: Arenes
4 hours (5 marks weightage)
Nomeclature of benzene derivatives (mono, di, tri substituted) Examples containing –CHO,
OH, X, NO2, SO3H etc.
M.O structure of benzene, resonance structure, resonance hybrid, resonance energy,
aromaticity, Huckel rule. Substitution reaction in benzene: mechanism of electrophilic
substitution reaction in benzene (nitration, sulphonation, halogenations and Friedel-crafts
alkylation).
Section C: Physical Chemistry
Total Hours: 20
Chapter 1: Colligative Properties
9 hours (12 Marks Weightage)
Solids in liquids, dilute solutions, i) osmotic pressure, laws of osmotic pressure,
determination of osmotic pressure by Berkeley-Hartley method. Isotonic solutions,
plasmolysis, haemolysis, turgid state, reverse osmosis.
Raoult’s law, relationship between relative lowering of vapour pressure and molar mass of
nonvolatile solute.
ii) Elevation in boiling point, Ebillioscopic constant of solvents and its units. Relation
between elevation in boiling point, lowering of vapour pressure and molar mass of
nonvolatile solute. Experimental determination of molecular weight by Walker-Lumsden
method.
iii) Depression in freezing point, cryoscopic constant, relation between depression in freezing
point, lowering of vapour pressure and molar mass of nonvolatile solute. Experimental
determination of molecular weight by Beckmann’s method. Determination of molecular
weight of volatile solute by Rast’s method.
iv) Abnormal molecular masses, Van’t Hoff factor, degree of association and dissociation,
molecular weight of electrolyte and non-electrolytes (numerical problems to be worked out).
Chapter 2: Distribution law
4 hours (05 Marks Weightage)
Nernst distribution law-statement, distribution co-efficient, conditions and its limitations. Verification
of Nernst distribution law of I2 in water and CCl4. Association and dissociation of the solute in one of
the solvent(To be derived). Application of the distribution law with respect to solvent extraction
process, de-silverisation of lead (Pattison park’s process). Solutions of gases in liquids, Henry’s law
and its limitations.
Chapter 3: Chemical Kinetics
5 hours (06 Marks Weightage)
Molecularity and order of reaction, second order reaction, differential and integrated rate
equations when a = b and a  b (to be derived), methods for determining order of reaction,
(differential, half-life, graphical and isolation methods), consecutive and parallel reactions
with examples (derivation for rate constant). Experimental determination of rate constant of
inversion of cane sugar by polarimeter method and saponification of ethyl acetate (numerical
problems).
.
7
Collision theory of reaction rates
2 hours (03Marks Weightage)
Frequency of collision and rate constant, Arrhenius concept, frequency factor. Lindeman
hypothesis for unimolecular and bimolecular reactions with derivation numerical problems
Transition state theory
Activated complex, thermodynamic functions such as G, S and H. equilibrium constant
of reactant and activated complex, comparison of collision theory and TST.
Reference Books:
1. Principles of Physical Chemistry. By Puri, Sharma, Pathania.
2. Essentials of Physical Chemistry .By B. S. Bahl, G. D. Tuli, Arun Bahl
3 Chemical Kinetics by B.K Sharma.
4. Physical Chemistry. By Archana Sharma
5. Advanced Physical Chemistry. By Bajpai.
6. Physical Chemistry By Sunakara Panda Vol.I & II
7. Advanced Physical Chemistry. By Gurudeepraj.
II SEMESTER PRACTICALS
1. Determination of density using specific gravity bottle and viscosity of the given liquid by
using Ostwald’s viscometer.
2. Determination of density and surface tension of the given liquid by using stalagmometer.
3. Determination of molecular weight of non volatile solute by Walker-Lumsden method.
4. Determination of percentage of given electrolyte in phenol water system by miscibility
temperature method.
5. Determination of percentage of given binary mixture (Glycerol-water) by viscosity
method.
6. Determination of rate constant of Fe3+ catalyzed decomposition of H2O2.
7. Determination of rate constant of saponification of ethyl acetate.
8. Determination of critical solution temperature of phenol water system.
9. Determination of transition temperature of given hydrate salt (Na2S2O3.5H2O).
10. Determination of distribution coefficient of I2 between CCl4 and water (Demonstration).
11. Determination of rate constant of inversion of cane sugar by polarimeter method.
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