UG Chemistry Syllabus 2018-21

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.
ST. JOSEPH’S COLLEGE (AUTONOMOUS)
BENGALURU-27

DEPARTMENT OF CHEMISTRY

SYLLABUS FOR UNDERGRADUATE COURSE

Re-accredited with ‘A++’ GRADE and 3.79/4 CGPA by NAAC
Recognised by UGC as College of Excellence

2018 -21

B.Sc. Syllabus Chemistry 2018-21 Page 1

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Structure of the Chemistry Course for B.Sc. Degree

The B.Sc. degree course is a three-year program divided into six semesters. Each semester
will consist of 15 weeks of instruction. In Chemistry there will be 9 Theory papers and 8
Practical papers. Continuous Internal Assessment (CIA) each is given 30% weightage and
End Semester Examination (SE) each is given 70% of the weightage in every paper. CIA is
based on written tests, seminars, assignments, quiz etc. End Semester theory and Practical
examinations will be of 3 hour duration each.

Semester Code number Title of the No of hours No of Continuous End Semester Total
I CH 118 paper
of hours of internal Examination marks
Chemistry-I
instruction teaching assessment marks

per week (CIA) marks

60 4 30 70 100

CH 1P1 Practical – I 33 3 15 35 50
CH 218 Chemistry-II 60 4 30 70 100

II CH 2P1 Practical - II 33 3 15 35 50
4 30 70 100
CH 318 Chemistry-III 60

III CH 3P1 Practical - III 33 3 15 35 50
2 15 35 50
CH 418 Chemistry-IV 30

IV CHOE 4118, CBCS 30 2 15 35 50

4218, 4318 22222222 22222222 22222222 222222222 2222222222 22222

CH 4P1 Practical - IV 33 3 15 35 50

CH 5118 (Org) Chemistry-V 45 3 30 70 100
CH 5218 (Phy) Chemistry-VI 45 3 30 70 100
V CH 5P1 (Phy) Practical - V 33 3 15 35 50
CH 5P2 (Inorg) Practical - VI 33 3 15 35 50
CH 6118 (Inorg) Chemistry-VII 45 3 30 70 100
VI CH 6218 (Bio) Chemistry-VIII 45 3 30 70 100
CH 6P1 (Org) Practical - VII 33 3 15 35 50
CH 6P2 (Bio) Practical -VIII 33 3 15 35 50

B.Sc. Syllabus Chemistry 2018-21 Page 2

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

SUMMARY OF CREDITS

Semester Code number Title of the paper No of hours of teaching per week Credit

CH 118 Chemistry-I 4 4
3 1
I CH 1P1 Practical – I 4 4
3 1
CH 218 Chemistry-II 4 4
3 1
II CH 2P1 Practical – II 2 2
2 2
CH 318 Chemistry-III 2222222222222222 222222
3 1
III CH 3P1 Practical – III 3 3
3 3
CH 418 Chemistry-IV 3 1
3 1
IV CHOE 4118, CBCS 3 3
3 3
4218, 4318 22222222222 3 1
3 1
CH4P1 Practical – IV

CH 5118 Chemistry-V

V CH 5218 Chemistry-VI

CH 5P1 Practical - V

CH 5P2 Practical – VI
CH 6118 Chemistry-VII

VI CH 6218 Chemistry-VIII

CH 6P1 Practical – VII

CH 6P2 Practical -VIII

B.Sc. Syllabus Chemistry 2018-21 Page 3

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester I
Paper code CH 118
Paper title CHEMISTRY – I
Number of teaching hrs per week
Total number of teaching hrs per 4
60
semester
Number of credits 4

1. ATOMIC STRUCTURE 11+2 hours

Historical development of atomic structure, failure of classical mechanics in the study of sub
atomic particles: black body radiation, photoelectric effect (review and recall). de Broglie
relation and Heisenberg’s uncertainty principle, problems based on these equations; thought
experiment to understand uncertainty principle.

Introduction to the principles of quantum (wave) mechanics: operators - definition, quantum
mechanical operators for position, momentum and energy; eigen functions and eigen values;
Schrodinger equation; Born interpretation of wave function (significance of ψ2); postulates of
quantum mechanics.

Quantum mechanical treatment of particle in one-dimensional box: derivation of expressions
for energy and normalized wave functions of a particle in 1D box, energy level diagram;
problems pertaining to particle in 1D box. Energy expression for a particle in 3D box (no
derivation); degeneracy.

Schrodinger equation for H-atom in cartesian coordinates and spherical polar coordinates;
qualitative explanation of the emergence of quantum numbers; radial and angular
components of the wave functions; radial distribution functions of s and p orbitals.

Self-study: Shapes of s, p and d orbitals. Polyelectron atoms: electron spin and spin quantum
number, (n+ℓ) rule, Pauli’s exclusion principle, aufbau principle, Hund’s rule, electronic
configuration of atoms.

B.Sc. Syllabus Chemistry 2018-21 Page 4

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Exchange energy, pairing energy, promotional energy, symmetric distribution of electrons in
atomic orbitals, prediction of the stable electronic configuration in p and d orbitals (Cu and
Cr as examples).

2. PERIODIC TABLE 6 hours

General electronic configurations of s, p, d and f block elements and position of elements in
the long form of periodic table.

Atomic radius: covalent, metallic and van der Waal’s radii; ionic radii. Effective nuclear
charge (qualitative treatment); periodic trends in atomic radii; comparison of ionic radii of
isoelectronic ions.

Ionization energy and electron affinity – periodic trends; electronegativity- Pauling scale,
calculation of electronegativity, periodic trends.

3. CHEMICAL BONDING 19+2 hours

Ionic bonding: lattice energy, Born-Lande equation, Born-Haber cycle, problems based on

Born-Lande equation and Born-Haber cycle, relation between lattice energy and melting

point of an ionic solid.

Covalent bonding: octet rule, Lewis structures of molecules and ions (when provided with
sequence of atoms), formal charge calculation for different atoms in molecules/ions,
deviation from octet rule.

Valence bond treatment of hydrogen molecule: qualitative discussion of wave functions,
concept of resonance.

Molecular structure: bond length, bond angle, dihedral angle and molecular geometry.
Overlapping of atomic orbitals, sigma and pi bonds.

Hybridisation: sp, sp2, sp3, sp3d, sp3d2 with examples (inorganic molecules ABn and ABnLm
type with and without π-bonds).

VSEPR theory: application to ABn and ABnLm type molecules/ions (A= s or p block element;
n ≤7)

Molecular orbital (MO) treatment of hydrogen molecule: linear combination atomic orbitals,
bonding and antibonding orbitals, energy level diagram. MO energy level diagram of

B.Sc. Syllabus Chemistry 2018-21 Page 5

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

homonuclear diatomic molecules/ions (Z ≤ 9): bond order and magnetic behaviour of these
molecules and ions, correlation of bond order with bond length and bond strength. MO
energy level diagram of heteronuclear diatomic molecules – HF and CO.

Metallic bonding: band theory (qualitative), classification of solids into conductors, insulators
and semiconductors based on band theory, electrical conductance of Li and Be.

Self-study: Partial covalent character of ionic bonds: Fajan’s rules. Partial ionic character
of covalent bonds, calculation of % ionic character.

4. STOICHIOMETRY 2+4 hours

Classification of chemical reactions, balancing chemical equations Atomic mass, gram

atomic mass, molar mass, formula mass: problems based on these concepts

Avogadro number, mole, problems based on chemical equations, concept of limiting reagent
Self-study: supplementary assignments

5. STATISTICAL THERMODYNAMICS 5 hours

Objectives of statistical thermodynamics, inputs from quantum mechanics and spectroscopy.

System in terms of energy levels and population, thermally available energy levels for

monotonic gasses. Micro and macro states, distinguishable and indistinguishable particles,

configuration and its weight, dominant configuration, ensemble and its types, thermodynamic

probability, its relationship with entropy. Postulates of statistical thermodynamics. Maxwell

Boltzmann statistics ( no derivation): assumptions. Partition function, relationship between

partition function and pressure, internal energy ( U) and entropy (S) for a monoatomic gas.

Salient features of Bose-Einstein and Fermi-Dirac statistics and comparison with Maxwell

Boltzmann statistics.

6. FIRST LAW OF THERMODYNAMICS 9 hours

Introduction to and terminology in thermodynamics: phase, system and surroundings;

Types of systems - open, closed and isolated; homogeneous and heterogeneous systems;
macroscopic properties: extensive and intensive properties; state of a system; thermodynamic
equilibrium; zeroth law of thermodynamics and absolute temperature scale; thermodynamic
processes - isothermal, adiabatic, isochoric, isobaric, cyclic, reversible, irreversible and
spontaneous processes; heat and work - sign convention; internal energy; state functions and

B.Sc. Syllabus Chemistry 2018-21 Page 6

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

path functions, exact and inexact differentials. Statement and mathematical form of first law
of thermodynamics, enthalpy of a system, heat capacity, relation between Cp and Cv.
Expressions for I law of thermodynamics for isothermal, adiabatic, isobaric, isochoric and
cyclic processes. Work done in i) irreversible isothermal expansion and compression of an
ideal gas, ii) reversible isothermal expansion and compression of an ideal gas. Kirchoff’s law
- derivation.

REFERENCE

1. Principles of Inorganic Chemistry, B R Puri; L R Sharma and K.C. Kalia;
Milestone Publishers (2011).

2. Physical Chemistry, P.W. Atkins, 6th Edition, Oxford University Press (1998).
3. Chemistry; R. Chang; 9th Edition, McGraw-Hill Higher Education (2006).
4. Principles of Physical Chemistry; B. R. Puri, L. R. Sharma, M.S. Pathania; 47th edition,

Vishal Publishing Co., (2017).

B.Sc. Syllabus Chemistry 2018-21 Page 7

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester I
Paper code CH 1P1
Paper title Practical – I
Number of teaching hrs per week
Total number of teaching hrs per 3
33
semester
Number of credits 1

Week-1 Title
Week-2 Errors & Standard Deviation
Week-3 Introduction to Volumetric Analysis-
Week-4 Estimation of NaOH using Std. HCl
Introduction to RBPT
Week-5 Estimation of HCl using Std. Na2CO3
Week-6 Redox Titration
KMnO4 <> Oxalic acid
Week-7 Define RBPT problem

Complexometric titration:
Zn2+ <> EDTA
Preparation of RBPT CHARTS.
Presentation of the charts by each group.
Discussion of materials required.
Prepare solutions

B.Sc. Syllabus Chemistry 2018-21 Page 8

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Week-8 Standardize / check solutions
Week-9 Do the main experiments individually
1)Preparation of poster
Week-10 2)Presentation of results through posters
Week-11 Repetition
Viva

B.Sc. Syllabus Chemistry 2018-21 Page 9

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester II
Paper code CH 218
Paper title CHEMISTRY– II
Number of teaching hrs per week
Total number of teaching hrs per semester 4
Number of credits 60
4

1. SECOND AND THIRD LAW OF THERMODYNAMICS 13+2 hours

Limitations of I law, scope of II law, statements of II law of thermodynamics. Spontaneous
and non-spontaneous processes, spontaneity and equilibrium. Driving forces for spontaneous
processes. Entropy; heat engine; Carnot cycle - derivation of efficiency based on entropy
concept. Entropy change in adiabatic and isothermal reversible expansion of an ideal gas.
Entropy of an ideal gas as a function of P, V and T. Entropy changes of an ideal gas for
isothermal, isochoric and isobaric processes. Entropy of phase transitions. Entropy changes
in the system and surroundings for reversible and irreversible processes; Entropy as a
criterion for spontaneity. Physical significance of entropy.

Free energy – Helmholtz free energy and Gibbs free energy, relation between work and ∆A;
work and ∆G. Standard free energy change of a reaction. Free energy and criterion of
spontaneity, variation of G with T and P; Gibbs - Helmholtz equation – derivation. van't Hoff
reaction isotherm - relation between free energy and equilibrium constant of a reaction.
Clausius–Clapeyron equation – derivation, application to liquid-vapour and solid-liquid
equilibria.

Third law of thermodynamics -statement, determination of absolute entropies of substances,
standard entropies and residual entropy.

Self-study: Problem solving

2. GASEOUS STATE 3 hours

Andrews experiments on liquefaction of CO2, critical constants. Relationship between critical
constants and van der Waals constants (no derivation) and problems. Joule – Thomson effect

for liquefaction of gases. Joule – Thomson coefficient of gases and inversion temperature.

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Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

3. CHEMICAL KINETICS 7+1 hours

Review of chemical kinetics [definitions of rate of a reaction, order, molecularity, rate
constant, rate equations for reactions of different orders, half life].

Derivation of rate expression for a 2nd order reaction when a = b and a ≠b. Methods of
determination of order of a reaction – i) integral and graphical method, ii) half life period
method; derivation of t1/2 for nth order. Effect of temperature on reaction rates - temperature
coefficient, Arrhenius theory, concept of energy barrier. Bimolecular collision theory - [final
equation given, no derivation]. Limitations of bimolecular collision theory. Transition state
theory – qualitative approach based on thermodynamics. Steady state approximation,
Lindemann theory - kinetics of unimolecular reactions.

Self study: Experimental methods of studying kinetics of reactions- Principles of volumetric
method [saponification of ester] and colorimetric method [iodination of acetone].

4. SPECTROSCOPY- THEORETICAL CONCEPTS 13+2 hours

Electromagnetic radiation (EMR)- Characteristics – Frequency, wavelength and wave

number and mathematical expressions connecting them. Types of Spectra: (Atomic and

molecular). Absorption and emission spectra: continuous, band and line. Regions of

electromagnetic spectrum. Processes and spectral techniques associated with different

regions. Different types of Molecular spectra i) Rotational (ii) vibrational and vibrational -

rotational iii) Electronic (UV & visible). Born Oppenheimer approximation. Rotational

Spectra of diatomic molecules: Rigid rotor model. Final expression for moment of inertia I =
µr2 and its significance. Calculation of reduced mass. Expression for rotational energy in
terms of joule and cm-1; EJ = h2/8 π2I [J(J+1)] joule and in cm-1 EJ / hc. Expression for
rotational constant; selection rule (gross and quantum selection rules) ∆J = ±1. Energy level

diagram for a rigid rotor and rotational spectrum. Vibrational Spectra of diatomic molecule.

Hooke’s Law. Oscillator frequency of Simple Harmonic Oscillator. Mathematical equation

for fundamental vibrational frequency and fundamental wave number in terms of force

constant, significance of force constant, effect of reduced mass on vibrational frequency.

Equation relating wave number and force constant. Potential energy curve for a diatomic

molecule of a harmonic oscillator. Selection rule. ∆v = ±1. Energy level diagram. Expression

for vibrational energy and Zero point energy. Problems on force constant, vibrational

frequency, vibrational wave number and zero point energy. Fundamental vibrations, total

B.Sc. Syllabus Chemistry 2018-21 Page 11

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

degrees of freedom (translational, rotational and vibrational) for linear and non linear
molecules. Calculation of fundamental vibrations for linear and non linear molecules (E.g.
H2O, CO2). Schematic representation of fundamental vibrations for H2O, CO2 and their IR
activity. Raman spectra – elastic and inelastic collisions, Raleigh and Raman scattering.
Raman shift, Stokes and anti stokes lines, intensity of Stokes and anti stokes lines, rule of
mutual exclusion, difference between IR and Raman spectroscopy.

Self-study: Problem solving

5. ACIDS, BASES AND SOLVENTS 7+1 hours

Theories of acids and bases : Lowry- Bronsted concept, conjugate acid –base pairs,

amphiprotic substances, relative strengths of acid-base pairs, solvent system concept of acids

and bases and examples. Lewis concept- types of molecules or species that can act as Lewis

acids and Lewis bases, Pearson’s Hard and Soft Acid- Base concept. Characteristics of hard

and soft acids and bases, HSAB principle. Applications of HSAB principle- stability of

complexes, prediction of coordination in complexes of ambidentate ligands, predicting

feasibility of a reaction, prediction of hardness and softness. Solvent properties- liquid range,

dielectric constant, solvent polarity, classification of solvents. Protic solvents – autoionisation
of protic solvents (H2O, liq. NH3). Aprotic solvents –classification with examples. Molten
salts - Classification with examples for each, and uses. Levelling effect of solvents-

explanation, levelling solvents and differentiating solvents. Liquid NH3- autoionisation, acid-
base reactions, solvation, solvolysis (comparison with H2O in each case). Liquid SO2 as
solvent- autoionisation and acid base reactions. Anhydrous HF-autoionisation, acid-base

reactions. Superacids- Hammet acidity function(equation is not required). Examples of

superacids. Applications of superacids.

Self-study: Solutions of alkali metals in liquid ammonia. Advantages and disadvantages of
liq. NH3 solvent.

6. LIQUID MIXTURES 4+1 hours

Raoults’ law, mathematical formulation, vapour pressure curves of ideal and type I
solutions, vapour pressure curves of non-ideal solutions. Vapour pressure curves of
completely miscible liquids. Boiling point - composition curves of completely miscible
liquids. Fractional distillation of binary liquid mixtures. Type II and Type III azeotropic

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Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

mixtures (minimum boiling and maximum boiling azeotropes, eg. water-ethanol and HCl-
H2O). Solubility of partially miscible liquid pairs; upper critical solution temperature
(CST): phenol-H2O system, lower CST: triethylamine-H2O system; lower CST and upper
CST: nicotine-H2O system. Effect of impurity on CST.
Self-study: immiscible liquid pairs: Nernst distribution law, effect of association and
dissociation of solute on distribution.

7. POLYMER CHEMISTRY 2+1 hours

Introduction to polymers; number average and weight average molecular weights of

polymers. Determination of molecular weights of polymers by viscosity and light scattering

methods.

Self study: Types of polymers

8. NUCLEAR CHEMISTRY 3 hours

Radioactive equilibrium. Radioactive series – first and last nuclide in all four series to be

mentioned. Nuclear reactions: nuclear reactions induced by alpha particles, protons, neutrons

deuterons and gamma radiation (one example each). Induced radioactivity. Applications of

radioactivity.

REFERENCES
1. Principles of inorganic chemistry, B.R. Puri, L. R. Sharma, K. C. Kalia. 33rded,
Vishal publishing Company (2016).
2. Basic inorganic chemistry, F. A. Cotton, G. Wilkinson, Paul L. Gaus. 3rd ed., John
Wiley and sons Cannada Pub (1995).
3. Inorganic chemistry, James H. Huheey, Ellen A. Keiter, Richard L. Keiter, 4th ed.
Pearson education (2005)
4. Inorganic Chemistry, 4th Edition, D.F. Shriver and P.W. Atkins, ELBS Oxford Univ.
Press. (2006).
5. Principles of Physical Chemistry; B. R. Puri, L. R. Sharma, M.S. Pathania; 47th
edition, Vishal Publishing Co., (2017).

B.Sc. Syllabus Chemistry 2018-21 Page 13

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester II
Paper code CH 2P1
Paper title Practical– II
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 33
1

1. Determination of density and viscosity of a given liquid using Ostwald’s viscometer.

2. Determination of percentage composition of a binary mixture by viscosity method.

3. Determination of CST of phenol- water system.

4. To show that the saponification of ethyl acetate follows second order kinetics and to
determine its rate constant at room temperature.

5. Determination of molecular diameter by surface tension measurement using a
stalagmometer.

6. Determination of percentage composition of sodium chloride solution by miscibility
temperature measurements of phenol – water system.

7. Determination of transition temperature of a salt hydrate by thermometric method.

8. Determination of the order of the reaction in iodine for the acid catalysed iodination of
acetone by colorimetric method

9. Determination of the rate constant of the saponification of an ester by conductometeric

method.

10. Determination of CST of aniline - water system.

11. Determination of the distribution coefficient of acetic acid between butanol and water.

12. Determination of the distribution coefficient of iodine between CCl4 and water.
13. To study the adsorption of a solute (acetic acid) on a dispersed solid (activated charcoal).

14. To study the adsorption of oxalic acid on activated charcoal.

15. To compare cleansing powers of two samples of detergents by surface tension method.

16. To determine the percentage composition of a given mixture of two liquids by surface
tension method.

17. To determine critical micelle concentration from surface tension measurements.

B.Sc. Syllabus Chemistry 2018-21 Page 14

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

18. Molecular weight of a polymer by viscosity method.
19. Any other suitable experiment relevant to the syllabus.

REFERENCES:
1. University Practical Chemistry, P C Kamboj; Vishal Publishing Co, (2008).
2. Advanced Practical Physical Chemistry; J B Yadav; Goel Publishing House Meerut;
(2007).
3. Practical Physical Chemistry; B Vishwanathan, P.S. Raghavan; Viva Books Pvt. Ltd.; New
Delhi (2009).

B.Sc. Syllabus Chemistry 2018-21 Page 15

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester III
Paper code CH 318
Paper title Chemistry– III
Number of teaching hrs per week
Total number of teaching hrs per semester 4
Number of credits 60
4

CHEMISTRY OF REPRESENTATIVE ELEMENTS

1. HYDROGEN 2 hours

Discussion on the position of hydrogen in the periodic table. Preparation of hydrogen,
production of hydrogen, production from fossil fuel, production from renewable resource
(water), hydrogen from solar energy. Types of hydrides–salt-like, molecular, and interstitial
hydrides. Applications and examples of hydrides. Hydrogen as a fuel for transport.

2. ALKALI METALS 3 hours

Elements, electronic configuration, oxidation state, melting point and boiling point, density,
metallic character, nature of bonds formed, photoelectric effect, hydration of ions and ionic
conductance in solution, flame coloration, electrode potential, reducing property, reaction
with water. Oxides, peroxides, superoxides - formation, reaction of each one with water.
Basic character of oxides and hydroxides. Carbonates - thermal stability, reasons for trends.
Reasons for anomalous behavior of Li. Diagonal relationship of Li & Mg.

3. ALKALINE EARTH METALS 1 + 1 hours

Compounds – basic character of oxides and hydroxides. Comparative solubilities of
hydroxides and sulphates.

Self-study: Elements, electronic configuration, oxidation state, boiling point, melting point,
density, metallic character, nature of bonds formed, flame colouration, reducing properties,
reaction with water

4. BORON FAMILY 4 hours

B.Sc. Syllabus Chemistry 2018-21 Page 16

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Electronic configuration, oxidation state, inert-pair effect, metallic character, nature of bonds
formed, basic character of oxides and hydroxides. Hydrides of boron: classification,
diborane-preparation from BCl3, properties - reactions with ammonia, Lewis acid properties.
Structure of B2H6 - explanation of bonding based on VBT. Halides - comparison of Lewis
acid character of boron trihalides. Structure and bonding in borazine; comparison with
benzene. Structure of boron nitride.

5. CARBON FAMILY 3 hours

Electronic configuration, oxidation states; inert pair effect, metallic character, nature of bonds
formed, catenation, allotropic forms of carbon: diamond and graphite-their structures,
fullerene structure of C60 (refer lecture plan), and carbon nanotubes. Carbides – salt-like,
covalent and interstitial. Silicates: Classification, ortho, pyro, chain, sheet and three
dimensional silicates with examples. Zeolites: General formula, classification - natural and
synthetic with examples, applications - catalyst, molecular sieves and ion exchangers.

6. NITROGEN FAMILY 2 + 1 hours

Some important oxides and oxyacids and corresponding salts of nitrogen and phosphorous –
important characteristics (refer lecture plan) and structures of N2O, NO, NO2, N2O5, HNO2,
HNO3, P4O6, P4O10, phosphoric and phosphorous acid series.

Self-study: Electronic configuration, oxidation state, metallic character and physical state.

7. OXYGEN FAMILY 1 + 1 hours

Oxyacids and peroxoacids of sulphur – characteristics (important ones only, refer lecture
plan), structures and corresponding salts: sulphurous acid, sulphuric acid, Caro’s acid,
Marshall’s acid, thiosulphuric acid, polythionic acid and chlorosulphonic acid. Anomalous
behaviour of oxygen.

Self-study: Electronic configuration, oxidation state, metallic character, physical state.
Allotropes of sulphur. Structure of cyclooctasulphur (S8).

8. ADSORPTION 1+1 hours

Enthalpy of adsorption, adsorption of gases on solids, adsorption isotherms, Langmuir

adsorption isotherm-derivation of the expression for the fraction of the area covered ‘θ’,

limitations. BET (Brunauer, Emmett and Teller) equation (no derivation, only interpretation),

B.Sc. Syllabus Chemistry 2018-21 Page 17

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

determination of surface area using BET equation.
Self-study: Introduction: Difference between adsorption and absorption, physisorption,
chemisorption, factors influencing adsorption.

9. CATALYSIS 4 hours

Catalysis-general characteristics of catalytic reactions, catalytic poisons, catalytic promoters,

positive and negative catalysts, auto catalysis, working of a catalyst (using an energy profile

diagram).

Types of catalysis – homogeneous and heterogeneous catalysis with examples. Kinetics and

mechanism of acid-catalysed reactions, derivation of rate expression for general and specific

acid-catalysed reactions (homogeneous).

Enzyme catalysis, derivation of Michaelis-Menten equation, qualitative description of

dependence of rate on concentration and temperature. Theories of catalysis–intermediate

complex theory (for homogenous catalysis), adsorption theory (for heterogeneous catalysis),

Langmuir-Hinshelwood mechanism.

Kinetics and mechanism of base-catalysed reactions, derivation of rate expression for general

and specific base-catalysed reactions.

10. INTRODUCTION TO ORGANIC CHEMISTRY 14 + 2 hours

Structural formulas: dash, condensed and bond-line formulas. Resonance theory, curved

arrows in resonance structures, rules for writing resonance structures, resonance contribution.
Concept of hybridization: sp3, sp2, sp hybridizations; the structures and bond lengths of

methane, ethane, ethene and ethyne. Polar covalent bonds, polar and non-polar molecules.

Physical properties and molecular structures of organic compounds, ionic compounds: ion–
ion forces, intermolecular forces (van der Waals forces), boiling points, solubilities.

Infrared (IR) spectroscopy as an instrumental method for detecting functional groups,
interpreting IR spectra, IR spectra of hydrocarbons and some functional groups containing
heteroatoms.

Use of curved arrows in illustrating reactions, heterolysis of bonds: carbocations and
carbanions, electrophiles and nucleophiles, strengths of Bronsted-Lowry acids and bases; the
acidity constant Ka; acidity and pKa; predicting the strength of bases, relationship between
structure and acidity. Effect of hybridization, inductive effect and delocalization on acidity:

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Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

carboxylic acids versus alcohols. Comparisons of conjugate acid–base strengths based on
inductive effects of other functional groups.

Self-study: Functional groups: alkyl halides, alcohols, phenols, ethers, amines, aldehydes
and ketones, carboxylic acids, esters, amides and nitriles, end chapter problems.

11. ALKANES AND CYCLOALKANES 9+1 hours

Classification of types of hydrogen atoms, nomenclature of monocyclic cycloalkanes,
alkenes, cycloalkenes and alkynes. Conformations: sigma bonds and bond rotation, Newman
projections, conformational analysis of ethane and butane. Relative stabilities and ring strain
of cyclopropane, cyclobutane and cyclopentane. Chair and boat conformations of
cyclohexane and substituted cyclohexanes: axial and equatorial hydrogens. Conformational
analysis of methyl cyclohexane, 1,3- diaxial interactions of t-butyl group.
Self-study: nomenclature of alkanes, physical properties of alkanes and cycloalkanes, end
chapter problems

12. STEREOCHEMISTRY 8 + 1 hours

Chirality and stereochemistry; isomerism: constitutional and stereoisomers; enantiomers,
diastereomers and chiral molecules. Molecules having one chirality centre, test for chirality-
plane of symmetry; R, S system of naming enantiomers. Properties of enantiomers: optical
activity and its origin, specific rotation. Polarimeter experiment. Molecules with more than
one chirality centre, meso compounds, Fischer projection formulas. Separation of
enantiomers: resolution, amines as resolving agents. Chiral molecules that do not possess
chirality centre.
Self- study: end chapter problems.

REFERENCES

1. Principles of Inorganic Chemistry, B. R. Puri, L. R. Sharma and K. C. Kalia, 33 rd
edition, Vishal publishing Co. Delhi, (2016).

th

2. Concise Inorganic Chemistry 5 edition, J. D. Lee, Blackwell Science, Oxford University
press, New Delhi (1996).

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Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

3. Inorganic Chemistry, 6th edition, Weller, Overtone, Rourke, Armstrong, Oxford
University press, New Delhi (2010).
4. Inorganic Chemistry, 5th edition, Shriver and Atkins, Oxford University press, New Delhi
(2015).
5. Principles of Physical Chemistry; B R Puri; L R Sharma and M B Pathania (47TH
edition); Vishal Chand Publishing Co., Jalandhar, New Delhi; (2016).
6. Organic Chemistry, T. W. G. Solomons, C. B. Fryhle (11th edition), Wiley India (2015).
7. Organic Chemistry, R. T. Morrison and R. N. Boyd (6th edition), Prentice hall (1992).
8. Organic Chemistry, Volume 1, I. L. Finar (6th edition), ELBS, Longman (1973).
9. Organic Chemistry, Volume 2, I. L. Finar (6th edition), ELBS, Longman (1975).

B.Sc. Syllabus Chemistry 2018-21 Page 20

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester III
Paper code CH 3P1
Paper title Practical–III
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 33
1

CH 3P1 PRACTICALS - III

Inorganic semi-micro qualitative analysis: salt mixture containing two acid and two basic
radicals.

B.Sc. Syllabus Chemistry 2018-21 Page 21

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester IV
Paper code CH 418
Paper title Chemistry–IV
Number of teaching hrs per week
Total number of teaching hrs per semester 2
Number of credits 30
2

1. ALKYL HALIDES 9 + 2 hours

Nucleophilic substitution reactions: nucleophiles; leaving groups; SN2 reaction - kinetics,
mechanism, free energy diagram and stereochemistry. SN1 reaction - mechanism, free energy
diagram and stereochemistry. Carbocations - structures and relative stabilities. Factors
affecting the rates of SN1 and SN2 reactions - structure of substrate (Hammond-Leffler
postulate), concentration and strength of nucleophile, solvent (polar protic and polar aprotic),
nature of leaving group. Substitution reactions in organic synthesis: functional group
transformations using SN2 reactions.

Elimination reactions: E2 and E1 mechanisms; dehydrohalogenation - mechanism, bases used
in dehydrohalogenation, comparison of SN2 vs E2; comparison of SN1 vs E1 in tertiary alkyl
halides.
Self-study: Nomenclature of alkyl halides, end chapter problems.

2. ALKENES AND ALKYNES 14 + 2 hours

Relative stabilities of alkenes - explanation using heats of hydrogenation. Synthesis of
alkenes via elimination reactions, Saytzeff’s rule; exception to the rule when bulky base is
used (explanation and free energy diagram excluded).

Acid-catalysed dehydration of alcohols (mechanism excluded). Rearrangement of
carbocations. Synthesis of alkynes by elimination of vicinal and geminal dihalides
(mechanism excluded). Acidity of terminal alkynes. Alkylation of terminal alkynes.
Hydrogenation of alkenes and alkynes - syn and anti addition.

B.Sc. Syllabus Chemistry 2018-21 Page 22

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Electrophilic addition of HX to alkenes - mechanism and free energy diagram,
Markovnikov’s rule, regioselectivity, peroxide effect. Stereochemistry of addition of HX to
alkenes. Addition of water to alkenes: acid-catalysed hydration - mechanism, rearrangements.
Oxymercuration-demercuration - regioselectivity, advantages. Hydroboration-oxidation -
regiochemistry and stereochemistry. Electrophilic addition of bromine and chlorine to
alkenes – mechanism and stereospecificity. Halohydrin formation - regioselectivity
(mechanism excluded). Oxidation of alkenes - syn-1,2-dihydroxylation, mechanism with
OsO4 and application to cyclopentene.

Oxidative cleavage with hot basic potassium permanganate, cleavage with ozone
(mechanistic details excluded). Electrophilic addition of bromine and chlorine to alkynes.
Addition of HX to alkynes.

1,3 butadiene - electron delocalization; electrophilic attack on conjugated dienes - 1,4
addition; kinetic vs thermodynamic control; Diels-Alder reaction.
Self-study: (E)-(Z) system for designating alkene diastereomers, Additional problems

3. ALCOHOLS, ETHERS AND EPOXIDES 3 hours

Alcohols as acids; conversion of alcohols into alkyl halides.

Synthesis of ethers by intermolecular dehydration of alcohols and Williamson ether synthesis
(mechanism excluded); Cleavage of ethers (mechanism excluded).

Synthesis of epoxides (mechanism excluded); Reactions of epoxides: acid and base catalysed
ring opening of unsymmetrical epoxides, regioselectivity - examples (mechanistic details
excluded).

REFERENCES

1. Organic Chemistry, T. W. G. Solomons, C. B. Fryhle (11th edition), Wiley India (2015).
2. Organic Chemistry, R. T. Morrison and R. N. Boyd (6th edition), Printice hall (1992).
3. Organic Chemistry, Volume 1, I. L. Finar (6th edition), ELBS, Longman (1973).
4. Organic Chemistry, Volume 2, I. L. Finar (6th edition), ELBS, Longman (1975).

B.Sc. Syllabus Chemistry 2018-21 Page 23

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester IV
Paper code CHOE 4118/ 4218/ 4318
Paper title
Number of teaching hrs per week Chemistry–IV
Total number of teaching hrs per semester 2
Number of credits 30
2

Students can choose any one of the following 30 h papers 2 credits in the IV semester.

CHOE 4118 COSMETIC CHEMISTRY 30 hours

Introduction of Cosmetic and perfumes 1 hour

Hair care products 5 hours

Shampoos – principal constituents – thickeners and foam stabilizers – perfumes –
preservatives – conditioning agents – antidandruff shampoos.

Hair cream – composition – hair dyes – types – constituents – dye removals

Skin care products 4 hours

Skin cleaners – classifications – cold cream – cleansing milk – moisturizers – hand and body
lotions – sun screen lotions – constituents.

Colour Cosmetics 5 hours

Lipstick – constituents – manufacturing methods – lip glosses – nail polish – formulation –
manufacturing- face powder – constitution

Dental Products 5 hours

Oil care product – product categories – tooth paste – tooth powder – oral rinses – mouth
washes – comparison between synthetic and herbal oral product

Bath preparations 5 hours

Bath powers – soaps and detergents – constituents of soaps and detergents – manufacture –

mechanism of cleaning actions

B.Sc. Syllabus Chemistry 2018-21 Page 24

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Essential oils and their importance in cosmetic industry 5 hours

Eugenol, geranoil, sandal oil, Eucalyptus oil, rose oil, 2-phenyl ethyl alcohol, jasmine,
civetone, muscone.

REFERENCES

1. Modern Technology of Cosmetics, Asia Pacific Press Inc, New Delhi, 2004.

2. E.Stocchi: Industrial Chemistry, Vol 1, Ellis Horwood Ltd, UK.

3. P.C. Jain , M. Jain: Engineering Chemistry, Dhanpat Rai & Sons, Delhi

4. Sharma B.K & Gaur H, Industrial Chemistry, Goel Publishing House, Meerut 1996

CHOE 4218 INDUSTRIAL AND MATERIAL CHEMISTRY 30 hours

Industrial materials 7 hours

Refractories: properties, classification, determination of PCE values. Abrasives:

Classification and application. Glass: composition, raw materials, varieties of glass
borosilicates, optical and safety glass composition and uses. Cement: raw materials, setting

of cement.

Petroleum and petrochemicals 4 hours

Origin of petroleum, composition, octane number, petrol, diesel, kerosene, naptha,

lubricants, LPG, synthetic petrol, petrochemicals.

Nanotechnology 8 hours

Definition, nano domain, properties of nanomaterial. Applications of nanomaterials i)

medicine-gold sol ii) photo voltaic cell (in solar cells) iii) self-cleaning glasses-ZnO, SnO,
TiO iv) Antibacterial materials-AgO v) Catalytic material vi) Super capacitors

Water chemistry 3 hours

Principles and applications of aqueous chemistry, water quality, parameters and standards,
hardness of water. Uses of zeolites in removal of hardness of water

Fuels 5 hours

Characteristics, calorific value, coal varieties, reserved, coke, gaseous fuels, biofuels.

Explosives and propellants 3 hours

B.Sc. Syllabus Chemistry 2018-21 Page 25

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Explosives – classification and applications
Propellants characteristics, classification and application
References
E. Stocchi: Industrial chemistry, Vol 1, Ellis Horwood Ltd. UK
Sharma BK and Gaur H, Industrial Chemistry, Goel Publishing House, Meerut, 1996.

CHOE 4318 Chemistry of food production, health and nutrition 30 hours

Chemistry of food production 8 hours

Chemicals composition of soil. Factors affecting the productivity of soil. Plant nutrients-

nonineral, primary, secondary and micronutrients and their natural sources. Nitrogen

fixation. Chemicals fertilizers: manufacture, advantages and disadvantages of ammonium

sulphate, calcium ammonium nitrate, urea and calcium superphosphate. Micronutrient

deficiencies and their remedies. Plant growth enhancers. Pesticides and their classification.

Insecticides-harmful effects of DDT and parathion. Herbicides: selective and no selective

herbicides with examples.

Chemistry of nutrition 12 hours

Nutrition and nutrients, classes of nutrients, general nutritional needs of human beings, ways

of assessing the nutritional status of a human being. Malnutrition, nutrient requirements-

recommendations – dietary allowance per day (RDA), caloric data of nutrients and

calculation of caloric value of food. Based metabolic rate (BMR). Factors affecting BMR.

Function, daily needs, food sources of carbohydrates, proteins and fats; problems associated

with excess and deficiency of carbohydrates, proteins and fats. Minerals – functions of

nutrient minerals, health issues associated with deficiency of Ca, Iodine, Fe, K and Na in

human body. Vitamins – sources and deficiency effects of vitamins A, D, E, F, K, B

complex and C.

Food additives 5 hours

Definition and classification, preservatives, antimicrobial and antioxidant preservatives,

food color, pH control in food, sequestrates, flavor enhances, sweeteners, anticaking agents,

stabilizers and thickeners, surface active agents (emulsifiers), Role of polyhydric alcohols as

B.Sc. Syllabus Chemistry 2018-21 Page 26

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

food additives.

Food adulteration 3 hours

Adulterants-definition, examples of adulterants in food and beverages, harmful effects of
food adulteration. Detection of adulteration in edible oil, milk, beverages, spices and pulses.

Chemistry of cooking 2 hours

Leavening of bread, fermentation

References
1. Chemistry: Impact of Society, M.D. Joesten. D.O. Johnston, J.T. Netterville and J. L.
Woo. Saunders College Publishing, 1998.

2. Chemistry of food and nutrition. H.C. Sharma, Agrobios (India) 2009.
3. Pesticides in the modern world: Risks and benefits, Margarita Stoitcheva, InTech, 2011.

4. E Source: Chemgeneration. Com/milestones/food-andagriculture.html

B.Sc. Syllabus Chemistry 2018-21 Page 27

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester IV
Paper code CH 4P1
Paper title Practical– IV
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 33
1

CH 4P1 PRACTICAL - IV (3 h/week)
Environmental and green chemistry

1. Estimation of copper in a water sample by colorimetry.

2. Estimation of iron in different water bodies by colorimetry.

3. Assessing the green chemistry index of oxidation reactions (benzhydrol to

benzophenone).

4. Mechanochemical synthesis of a Schiff’s base.

5. Any other appropriate experiment.

6 to 10: RBPT sessions

B.Sc. Syllabus Chemistry 2018-21 Page 28

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester V
Paper code CH 5118
Paper title Chemistry– V
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 45
3

ORGANOMETALLIC COMPOUNDS 2 hours

Preparation and reactions of RLi and RMgX compounds.

ARENES 7+1 hours

Stability of benzene based on heats of hydrogenation. Theories of structure of benzene -
resonance explanation, molecular orbital explanation (energy level diagram, without shapes
of orbitals), Hückel’s rule, aromatic, antiaromatic and nonaromatic species in benzenoid and

heterocyclic systems. Electrophilic aromatic substitution reactions - general mechanism with
free energy diagram; nitration, sulphonation, halogenation, Friedel Crafts alkylation and

acylation reactions. Reactivity and orientation: o-, p-, m- directors, activators and
deactivators. Orientation in toluene, phenol, chlorobenzene and nitrobenzene. Side chain
halogenation, oxidation of side chain.
Self-study: end chapter problems.

SPECTROSCOPY 6+1 hours

UV spectroscopy- types of electronic transitions in organic molecules, meaning of λmax, Є
and A, observed transitions in a typical UV-vis spectrum, effect of conjugation on λmax.

NMR spectroscopy- nuclear spin, origin of the signal; chemical shift, shielding and
deshielding of protons, equivalent and non-equivalent protons; integration of signal areas;
signal splitting; spin-spin coupling (effect of coupling constant excluded). Interpretation of
NMR spectra. Proton NMR and rate processes.
Problems combining UV, IR and NMR techniques.
Self-study: Additional problems

B.Sc. Syllabus Chemistry 2018-21 Page 29

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

ALDEHYDES AND KETONES 10 +1 hours

Synthesis of aldehydes by the oxidation of primary alcohols and by the reduction of
acyl chloride, esters and nitriles. Synthesis of ketones by ozonolysis, oxidation of secondary
alcohols, Friedel Craft’s reaction and using Grignard reagent.

Nucleophilic addition to carbonyl compounds: mechanism of addition using strong
nucleophiles and acid catalyzed nucleophilic addition. Relative reactivity of aldehydes
a n d ketones.

Addition of alcohols - hemiacetals and acetals, mechanism of acid-catalysed acetal
formation. Addition of amines (primary and secondary amines, hydrazine and
hydroxylamine). Addition of HCN - mechanism. Wittig reaction (no mechanism, few
examples). Oxidation of aldehydes and ketones; acidity of α-hydrogen, enolate ion. keto-
enol tautomerism; halogenation at the α-carbon, the haloform reaction

Base-catalysed aldol reaction, dehydration of aldol product (mechanism of both), crossed
aldol reactions, synthetic applications of aldol reactions. Claisen-Schmidt reaction
(mechanism excluded). Cyclisations via aldol reaction. Addition to α, β-unsaturated
aldehydes and ketones (mechanism excluded). Michael addition (mechanism excluded).
Self-study: end chapter problems

CARBOXYLIC ACIDS AND DERIVATIVES 5 + 2 hours

Preparation of carboxylic acids by the oxidation of aldehydes and primary alcohols;
hydrolysis of cyanohydrins, nitriles; and by carbonation of Grignard reagents. Nucleophilic
substitution at the carboxylic carbon - general mechanism. Relative reactivity of acid
derivatives.
β- dicarbonyl compounds: acidity, Claisen condensation with mechanism, crossed Claisen
condensation. Acetoacetic ester synthesis – alkylation and acylation. Malonic ester
synthesis – alkylation.
Self- study: Acidity of carboxylic acids, end chapter problems

B.Sc. Syllabus Chemistry 2018-21 Page 30

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

AMINES 6 + 1 hours

Basicity of amines, comparison of basicity of 1o , 2o and 3o amines in vapour and solution

phase, basicity of arylamines.

Preparation of amines by alkylation of ammonia; Gabriel synthesis; reductive amination;
reduction of nitro compounds, nitriles, oximes and amides; Hofmann’s rearrangement. Action
of nitrous acid on 1o, 2o and 3o amines. Replacement reactions and coupling reactions of
arene diazonium salts. Hofmann elimination.
Self-study: Additional problems

NATURAL PRODUCTS 3 hours

Terpenoids - introduction, isoprene rule, classification, structure elucidation and synthesis of
citral. Alkaloids - introduction, general characteristics, structural elucidation and synthesis of
nicotine.

REFERENCES
1. Organic Chemistry, T. W. G. Solomons, C. B. Fryhle (11th edition), Wiley India (2015).
2. Organic Chemistry, R. T. Morrison and R. N. Boyd (6th edition), Printice hall (1992).
3. Organic Chemistry, Volume 1, I. L. Finar (6th edition), ELBS, Longman (1973).
4. Organic Chemistry, Volume 2, I. L. Finar (6th edition), ELBS, Longman (1975).

B.Sc. Syllabus Chemistry 2018-21 Page 31

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester V
Paper code CH 5218
Paper title Chemistry– VI
Number of teaching hrs per week
Total number of teaching hrs per 3
45
semester
Number of credits 3

PHASE EQUILIBRIUM 4+1 hours

Meaning of the terms phase, component and degrees of freedom. Discussion with examples

and reasoning. Gibbs phase rule (derivation excluded), reduced phase rule for condensed

systems. Application of phase rule to one component system-water system. Effect of pressure

and temperature on triple point of water. Application of phase rule to two component

systems: solid-liquid system (KI-H2O), two component alloy system (Pb-Ag), freezing
mixtures; eutectic system - Pb–Ag system.

Self-study: Pattinson’s process of desilverisation of Pb and freezing mixtures.

ELECTROCHEMISTRY 20+2 hours

Conductance, specific conductance and molar conductance. Measurement of conductance

based on Wheatstone bridge. Cell constant and its determination; determination of molar

conductance of a strong electrolyte. Variation of specific and molar conductance with

concentration. Conductance at infinite dilution.

Kohlrausch’s law of independent migration of ions, application of Kohlrausch’s law to

determine molar conductance at infinite dilution, degree of dissociation and dissociation

constant.

Transport number, its relationship with ionic conductance and mobility of ions. Causes of

abnormal transport number observed in certain systems (Eg., Cd2+ in CdI2), transport number
of alkali metal ions, abnormal conductivities of H3O+ and OH- ions.

B.Sc. Syllabus Chemistry 2018-21 Page 32

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Conductometric titrations
Acid-base titrations (strong acidstrong base, weak acidstrong base, strong acidweak
base, weak acidweak base). Advantages of conductometric titrations.
Self-study: Arrhenius theory of electrolytic dissociation. Evidences in favour of the theory
and limitations.
Theory of strong electrolytes – qualitative account of Debye-Huckel theory (asymmetry
effect and electrophoretic effect). Debye-Huckel-Onsager (DHO) equation for aqueous
solutions of 1:1 electrolytes (derivation excluded), verification of DHO equation.
Electrode potential
Single and standard electrode potentials. Reference electrodes: (i) primary reference
electrode: standard hydrogen electrode (ii) secondary reference electrodes: saturated calomel
electrode, quinhydrone electrode.
Classification of electrochemical cells: electrolytic and Galvanic cells. Construction of
Galvanic cells - Daniel cell. Reversible and Irreversible cells, EMF of a cell and
representation of cells.
Derivation of Nernst equation for the potential of a single electrode and cells. Calculation of
cell EMF from single electrode potentials. Electrochemical series and applications.
Relationship between EMF and free energy change. Relationship between standard free
energy change and equilibrium constant for electrochemical reactions.
Different types of electrodes
Self-study: Metal-metal ion electrodes (ii) amalgam electrodes (iii) gas electrodes (iv) metal
insoluble salt electrodes (v) oxidation-reduction electrodes. Application of Nernst equation
for these electrodes.
Concentration cells
Chemical cells and concentration cells with and without transference. Definition, schematic
representation and expression for EMF for each cell. Liquid junction potential. Applications
of EMF
Calculation of (i) free energy, enthalpy and entropy changes in electrochemical reactions, (ii)
solubility product of sparingly soluble salt. pH and its determination using hydrogen and
quinhydrone electrodes. Potentiometric titrations: principle and application in redox
titrations.

B.Sc. Syllabus Chemistry 2018-21 Page 33

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

REDOX CHEMISTRY 4+1 hours

Define oxidation and reduction, calculation of oxidation number, balancing redox equations-

one example each in acid medium and basic medium-Reduction potential, standard potential

and spontaneity (Recall).

Reactions with water,stability field of water, disproportionation and comproportionation
reactions. The diagrammatic presentation of potential data -(i) Latimer diagram (chlorine).
The diagrammatic presentation of potential data -(ii)Frost diagram (oxygen and manganese)-
Construction of Frost diagram from the Latimer diagram. The diagrammatic presentation of
potential data -(iii) Pourbaix diagram (iron)- natural waters.

Self-study: Latimer diagram for manganese and Frost diagram of nitrogen in acid and basic
media and Pourbaix diagram of manganese.

SOLID STATE CHEMISTRY 5 hours

Differences between crystalline and amorphous solids – isotropy and anisotropy, interfacial
angles. Symmetry in cubic systems; space lattice and unit cell. Bravais lattices, seven
crystal systems, fourteen space lattices, law of rational indices.

Miller indices; derivation of Bragg’s equation, equation for interplanar spacing based on
Miller indices for cubic crystal systems. X-ray diffraction: experimental determination of
structure by rotating crystal method e.g. NaCl and KCl.

PHOTOCHEMISTRY 6+2 hours

Differences between thermal and photochemical reactions. Photophysical and photochemical

processes. Consequences of absorption of light radiation-luminescence, fluorescence,

phosphorescence; singlet and triplet states; explanation for fluorescence and

phosphorescence with the help of Jablonski diagram. Laws of photochemistry. Beer-

Lambert’s law – derivation, applications to colorimetry. Quantum efficiency Φ, energy

absorbed/mol (Einstein).

Study of the following photochemical reactions along with mechanism:

Between H2 and Cl2; H2 and Br2. ii) decomposition of HI in gaseous phase and iii)
dimerisation of anthracene.

Photostationary state.

B.Sc. Syllabus Chemistry 2018-21 Page 34

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

S e l f s t u d y : photosensitization (eg, decomposition of H2 in the presence of Hg vapour,
chlorophyll as sensitizer, decomposition of oxalic acid in solution in the presence of uranyl
ions), chemiluminescence, bioluminescence.

REFERENCES:
1. Principles of Physical Chemistry; B R Puri; L R Sharma and M B Pathania (43rd edition);

Vishal Chand Publishing Co. (2008).
2. Physical Chemistry for Chemical and Biological Sciences: Raymond Chang; First Indian

Edition-2015, Viva Books Pvt. Ltd.
3. Physical Chemistry; P W Atkins; (6th edition); Oxford University Press (1998).
4. Text Book of Physical Chemistry; Samuel Glasstone; Mac Millan India Ltd.
5. Principles of Inorganic Chemistry; B R Puri; L R Sharma and K.C. Kalia; Vallabh

Publications (2005).

B.Sc. Syllabus Chemistry 2018-21 Page 35

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester V
Paper code CH 5P1
Paper title Practical– V
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 33
1

CH 5P1 PRACTICAL - V 11 sessions (3 hours/week)

Physical Chemistry

Lab 1: Conductometric titration of strong acid and strong base.
Lab 2: Determination of molar conductance at infinite dilution for a given electrolyte.
Lab 3: Potentiometric titration between weak acid and strong base. Determination of pKa.
Lab 4: Determination of standard electrode potential of zinc.
Lab 5: Titration of strong acid against strong base using a pH meter. Comparison of
theoretical and experimental titration curves.
Labs 6 to 10: RBPT sessions

B.Sc. Syllabus Chemistry 2018-21 Page 36

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester V
Paper code CH 5P2
Paper title Practical– VI
Number of teaching hrs per week
Total number of teaching hrs per 3
33
semester
Number of credits 1

CH 5P2 PRACTICAL - VI 11 SESSIONS (3 hrs/week)

Inorganic Chemistry

1. Volumteric estimation of iron in haematite

2. Volumetric estimation of copper in brass

3. Volumetric estimation of calcium in limestone

4. Preparation of a suitable inorganic complex

5. Quantitative chemical analysis of the prepared inorganic complex

6. IR and UV-VIS spectral analysis of the prepared complex. (2 sessions)

7. Electrogravimetric estimation of copper

8. Gravimetric estimation of nickel as Ni(DMG)2
9. Gravimetric estimation of copper as Cu2(SCN)2
10. Gravimetric estimation of magnesium as magnesium oxinate

11. Gravimetric estimation of sulphate

12. Any other suitable inorganic quantitative analysis

B.Sc. Syllabus Chemistry 2018-21 Page 37

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester VI
Paper code CH 6118
Paper title Chemistry– VII
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 45
3

HALOGENS 5 + 2 hours

Oxidizing power of halogens and relative strength of the hydracids of halogens - explanation
using Born-Haber cycle. Oxyacids of halogens and their classification, comparative strength
of oxyacids of halogen. Interhalogen compounds: classification, structure of ClF3. - self
study) - explanation using VSEPR theory. Polyhalide ions - structure of ICl2- and ICl4- using
VSEPR theory. Anomalous behaviour of fluorine.

Self study: Electronic configuration, oxidation state, metallic character and physical state.

Structure and bonding of oxides and corresponding oxyacids of chlorine - Cl2O, ClO2, Cl2O6,
Cl2O7, HClO, HClO2, HClO3, HClO4.

Structures of BrF5, IF7.

COMPOUNDS OF NOBLE GASES 2 hours

Self-study: Bartlett experiment, classification of xenon compounds based on oxidation states
of xenon, structures of fluorides and oxides of xenon (XeF2, XeF4, XeF6, XeO3, XeO3F2) –
discussion using concept of hybridization.

d–BLOCK ELEMENTS AND COORDINATION CHEMISTRY 21+ 2 h

Terminologies in coordination chemistry. Types of ligands. IUPAC nomenclature.
Werner’s theory – explanation of the postulates using cobalt–ammine complexes. EAN
rule. Geometries of complexes with coordination number ranging from 2 to 6 with
examples. Structural isomerism: ionization, hydrate, linkage and coordination.
Stereoisomerism: geometrical isomerism in square planar and octahedral complexes, optical

B.Sc. Syllabus Chemistry 2018-21 Page 38

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

isomerism in octahedral complexes. Theories of bonding: valence bond theory (VBT) as
applied to 4 and 6 coordinate complexes, inner and outer orbital complexes, limitations of
VBT. Crystal field theory (CFT): Crystal field splitting in octahedral, tetrahedral and square
planar complexes, factors affecting 10Dq, spectrochemical series, crystal field stabilization
energy (CFSE), explanation of magnetic properties, colour and electronic spectra (d1 system
only). Jahn-Teller distortion – explanation based on octahedral Cu2+ complexes. Stability
constants – stepwise and overall formation constants and their relationship, factors affecting
thermodynamic stability. Limitations of CFT.
Self-study: Electronic configuration of first row transition elements, characteristic
properties – oxidation states, colour, magnetic properties, catalytic property, interstitial
compound formation and complex formation.

ORGANOMETALLIC CHEMISTRY 5 hours

Classification of organometallic compounds based on bond type, classification of ligands
based on hapticity, 18 electron rule, structures of and the applications of 18 electron rule to
Ni(CO)4, Fe(CO)5, Cr(CO)6, Co2(CO)8, Mn2(CO)10, Fe(C5H5)2, Cr(C6H6)2, K[PtCl3(C2H4)]
and W(CH3)6. Bonding in metal carbonyls – qualitative approach. Organometallic
compounds in catalysis – Ziegler-Natta polymerization of ethene, alkene hydrogenation
using Wilkinson’s catalyst, and Monsanto acetic acid process.

BIO-INORGANIC CHEMISTRY 3 hours

Role of metal ions in biological systems (Na, K, Ca, Mg, Fe, Zn, Cu, Mn, Mo and Co),
metalloporphyrins–haemoglobin and myoglobin in oxygen transport and storage, difference
in the binding characteristics of haemoglobin and myoglobin towards oxygen, phenomenon
of cooperativity and its mechanism.

f–BLOCK ELEMENTS 5 hours

The lanthanide series: elements and their electronic configurations, oxidation states, atomic

and ionic radii – lanthanide contraction and its consequences, colour, magnetic properties

and complex formation. Extraction of lanthanides from monazite, separation by ion

exchange method. Comparison of lanthanides and transition elements with respect to

B.Sc. Syllabus Chemistry 2018-21 Page 39

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

oxidation states, magnetic properties, electronic spectra and complex formation. Actinide
series: electronic configurations and oxidation states. Comparison of properties of
lanthanides and actinides.

REFERENCES:

1. Principles of Inorganic Chemistry, B. R. Puri, L. R. Sharma and K. C. Kalia, 33rd
edition, Vishal publishing Co. Delhi, (2016).

th

2. Concise Inorganic Chemistry 5 edition, J. D. Lee, Blackwell Science, Oxford University
press, New Delhi (1996).
3. Inorganic Chemistry, 6th edition, Weller, Overtone, Rourke, Armstrong, Oxford
University press, New Delhi (2010).
4. Inorganic Chemistry, 5th edition, Shriver and Atkins, Oxford University press, New Delhi
(2015).
5. Principles of Physical Chemistry; B R Puri; L R Sharma and M B Pathania (47th
edition); Vishal Chand Publishing Co., Jalandhar, New Delhi; (2016).

B.Sc. Syllabus Chemistry 2018-21 Page 40

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester VI
Paper code CH 6218
Paper title Chemistry– VIII
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 45
3

INTRODUCTION TO BIOCHEMISTRY 1 + 1 hours

Elemental and molecular composition of biological systems. Criteria for selection of elements

according to their biological role (CHNOPS). Different types of interactions occurring in the

biological system.

Self study: Properties and role of water in the biological system. Overview of major

functions of cell organelles.

CARBOHYDRATES 5 + 1 hours

Structure of monosaccharides (Fischer and Haworth projection formulas), homo and hetero

polysaccharides, mutarotation, glycoside formation (O-methylation) (mechanism included).

Classification (mono, oligo and polysaccharides with examples). Structure and function of

trehalose. Structure (partial and hydrolytic products) and biological importance of

homopolysaccaharides – starch and chitin. Structure (partial and hydrolytic products) and

biological importance of heteropolysaccharides – hyaluronic acid and heparin.

Self-study: Reaction of reducing sugar with Fehling’s reagent, Tollen’s reagent and

phenylhydrazine. Structure (partial and hydrolytic products) and biological importance of

glycogen and cellulose.

LIPIDS 5 + 1 hours

Lipids – definition, general functions, classification into simple, compound and derived

lipids. Concept of essesntial and non-essential fatty acids. Structures of palmitic, stearic,

oleic, linoleic, linolenic and arachidonic acids. Acylglycerols – structure and biological

importance: properties – saponification number and iodine number (reaction, definition and

significance).

B.Sc. Syllabus Chemistry 2018-21 Page 41

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Phosphoglycerides – structure and biological importance of (i) phosphatidylcholine (ii)
phosphatidylethanolamine (iii) phosphatidylserine (iv) phosphatidylinositol. Sphingolipids –
structure of sphingosine; biological importance of sphingolipids. Cerebrosides – structure of
ceramide; biological importance of cerebrosides.
Micelle and bilayer formation. Cell membranes – composition and structure (fluid mosaic
model). Lipososmes – definition and applications.
Self study: Rancidity- types of rancidity and its methods of prevention.
Steroid Hormones – β-estradiol, progesterone, testosterone, insulin, glucagon, oxytocin,
vasopressin – brief outline of biological roles (no structures only functions).

AMINO ACIDS AND PROTEINS 5+1 hours

Amino acids – general structure, classification of α-amino acids based on nature of R groups

(at pH 6.5). Ionization of amino acids: zwitterionic structure and determination of isoelectric

point taking an example from each class - glycine, aspartic acid and lysine (no titration curve

required). Peptide bond – definition and characteristics. Construction of peptides. Reactions

of amino acids with (a) ninhydrin (b) Sanger’s reagent (c) Edman’s reagent (d) CO2 –
importance of these reactions. Classification of proteins based on (a) structure (fibrous,

globular and transmembrane) (b) composition – (simple and conjugated) with examples,

functions of proteins.

Structural organisation of proteins; primary structure, secondary structure – brief description

and comparison of α-helix and β-pleated sheet, tertiary structure - forces stabilizing tertiary

structure, quaternary structure.

Self study: Naming polypeptides upto nine amino acids. Brief explanation of quaternary

structure of haemoglobin.

ENZYMES AND COENZYMES 7 hours

Concept of holoenzymes and requirement of cofactors (metal ions and coenzymes - only

names with examples). Salient features of active site. Mechanism of enzyme action – lock

and key model using carboxypeptidase A and induced fit model using lysozyme as example

(only brief qualitative explanation).

Specificity of enzymes (with reactions) – broad specificity, absolute specificity (group, bond,

stereospecificity- cis/trans and D/L).

B.Sc. Syllabus Chemistry 2018-21 Page 42

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Enzyme kinetics – effect of substrate concentration (Michaelis-Menten equation to be given-
no derivation) Lineweaver-Burke curve significance of Km and Vmax. Effect of pH and
temperature on kinetics (explanation of dumb bell shaped curve). Enzyme inhibition –
reversible and irreversible inhibitions. Brief mention of mechanism by which reversible
(competitive, non-competitive and uncompetitive inhibitons only) with suitable examples.
Lineweaver-Burke curves for these inhibitions.
Coenzyme functions of B-complex vitamins (niacin, flavin, thiamine, pyridoxal phosphate,
pantothenic acid, lipoic acid, cobalamine – no structures only descriptive treatment of the
enzymatic reactions they are involved in).
Classification and nomenclature (common and systematic names, EC number not required)
into 6 main classes with an example of a reaction catalysed by each class of enzymes.

BIOENERGETICS AND BIOLOGICAL OXIDATION 3+1 hours

Concept of coupling reactions with an example. Structure of ATP, explanation of why it’s a

high energy molecule based on its structure. Hydrolysis of ATP and energetics of the

reaction, other high energy compounds. Definition of electron transport chain; components of

ETC (no structures) and how they are successively oxidised and reduced, diagrammatic

representation of ETC - both from NADH and from reduced substrate via FADH2 (electrode
potential values and points at which ATP is produced are to be given). Oxidative and

substrate level phosphorylation. Significance of P/O ratio.

Self study: Principles of bioenergetics; bioenergetics and thermodynamics – concept of free

energy – endergonic and exergonic reactions.

Brief overview of oxidation-reduction reactions – standard electrode potentials. Relationship

between ΔG°’ and ΔE°’.

METABOLISM 7 hours

Metabolism: catabolism and anabolism – definition and comparison, glycolysis – reactions

and enzymes involved, regulation of glycolytic pathway, energy balance sheet. Reaction of

TCA cycle and energy balance sheet.

Reactions of β-oxidation of fatty acids. Energy balance sheet of fatty acid oxidation.

Metabolism of amino acids – transamination, deamination and decarboxylation with at least

B.Sc. Syllabus Chemistry 2018-21 Page 43

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

one example for each. Urea cycle – reactions, enzymes involved and significance of the
cycle.

NUCLEIC ACIDS 2+1h

Nucleic acids – nomenclature and structures of sugars, bases, nucleosides and nucleotides,

including cyclic nucleotides e.g.: cyclic AMP role in biological system. Polynucleotides -

Watson and Crick model of DNA (salient features) DNA polymorphism - mention of A, B

and Z- DNA.

Self study: Biological importance of DNA. Types of RNA and their biological role.

MOLECULAR BIOLOGY AND PROTEIN METABOLISM 4 hours

Central dogma of molecular biology. Brief account of enzymatic aspects of prokaryotic DNA

replication.

Transcription – mechanism (details of factors not required). Genetic code (general features

only).

Translation – amino acid activation, initiation, elongation and termination of protein

synthesis (details of factors not required).

Self study: Brief historical background of DNA replication-– proof of semi-conservative

mode of replication.

References
1. Biochemistry, Debajyoti Das Academic Publishers
2. Fundamentals of Biochemistry, J.L Jain, S Jain and N. Jain S Chand Publications
3. Principles of Biochemistry, A. L. Lehninger, [ CBS, New Delhi ](1993)
4. Biochemistry, L. Stryer, 2nd ed [ CBS, New Delhi ] (1986)
5. Biochemistry, J. David Rawn, Neil Patterson
6. Biochemistry, Voet and Voet, 2nd ed [ John Wiley](1995)
7. Outlines of Biochemistry, E. E. Conn and P. K. Stumpf, [Wiley Eastern] (1976)
8. Biochemistry: The Chemical Reactions of Living Cells, D. E. Metzler,[ Academic
Press] (1997)

B.Sc. Syllabus Chemistry 2018-21 Page 44

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester VI
Paper code CH 6P1
Paper title Practical– VII
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 33
1

CH 6P1 PRACTICALS - VII 11 SESSIONS (3 h/week)

Synthesis and analysis of organic compounds (spectral and qualitative analysis of reagent
and product).
Lab 1: Laboratory safety rules; determination of melting point, recrystallization
Lab 2: Bromination of phenol
Lab 3: Oxidation of benzaldehyde
Lab 4: Nitration of toluene
Lab 5 and 6: Qualitative analysis of organic compounds

Labs 7 to 10: RBPT sessions
Lab 11: Practical test and viva

B.Sc. Syllabus Chemistry 2018-21 Page 45

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Semester VI
Paper code CH 6P2
Paper title Practical– VIII
Number of teaching hrs per week
Total number of teaching hrs per semester 3
Number of credits 33
1

CH 6P2 PRACTICALS - VIII 11 SESSIONS (3 hrs/week)
BIOCHEMISTRY

(i) Estimation of creatinine by Jaffe’s method

(ii) Estimation of protein by Biuret method

(iii) Estimation of urea by DAM method

(iv) Estimation of ascorbic acid using 2,6-dichlorophenolindophenol

(v) Estimation of Inorganic Phosphate by modified Fiske-Subbarow method

(vi) Kinetics of the breakdown of starch by salivary amylase using DNS method

(vii) pH and Temperature dependence on enzymatic reaction rate of salivary amylase

(viii) Estimation of DNA by UV spectrophotometry and diphenylamine method

(ix) Thin Layer Chromatography (TLC) of amino acids

(x) Preparation of buffers and explanation on theory of buffers

(xi) Agarose Gel Electrophoresis of a DNA sample

B.Sc. Syllabus Chemistry 2018-21 Page 46

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Pattern of question paper

Part Marks allotted Total number Marks Questions to be Max. marks
for each question of questions including
answered allotted
choice
A2 8 16 6 12
48
B6 10 60 8 10
70
C5 3 15 2

Total marks 91 Total marks
including choice excluding choice

Marks allotment for I semester B.Sc.

Chapter Number of hours Maximum marks
allotted

Atomic structure 13 20

Periodic table 69

Chemical bonding 21 31

Stoichiometry 69

Statistical Thermodynamics 5 8

First Law of Thermodynamics 9 14

Total 60 91

(including choice)

B.Sc. Syllabus Chemistry 2018-21 Page 47

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Marks allotment for II semester B.Sc.

Chapter Number of hours Maximum marks
allotted
Second and Third Law of Thermodynamics 15
22

Gaseous State 35

Chemical Kinetics 8 12

Spectroscopy - Theoretical Concepts 15 23

Acids, Bases and Solvents 8 12

Liquid Mixtures 57

Polymer Chemistry 35

Nuclear Chemistry 35

Total 60 91
(including choice)

Marks allotment for III semester B.Sc.

Chapter Number of hours Maximum marks allotted
Hydrogen 2 3
Alkali metals 3 5
Alkaline earth metals 2 3
Boron family 4 6
Carbon family 3 4
Nitrogen family 3 5
Oxygen family 2 3
Adsorption 2 3
Catalysis 4 6
Introduction to organic chem 16 24
Alkanes & cycloalkanes 10 15
Stereochemistry 9 14
60 91
Total
(including choice)

B.Sc. Syllabus Chemistry 2018-21 Page 48

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Marks allotment for IV semester B.Sc.

Chapter Number of hours Maximum marks allotted
Alkyl halides 11 18
Alkenes & alkynes I 16
Alcohols, ethers & epoxides 3 27
30
Total = 5

50
(including choice)

Marks allotment for V semester B.Sc. (Organic)

Chapter Number of hours Maximum marks allotted
Organometallic compounds 2 4
8 16
Arenes 7 14
Spectroscopy 11 22
Aldehydes & ketones 7 15
Carboxylic acid & derivatives 7 14
3 6
Amines 45 91
Natural products
(including choice)
Total =

B.Sc. Syllabus Chemistry 2018-21 Page 49

Department of Chemistry St. Joseph’s College (Autonomous), Bangalore.

Marks allotment for V semester B.Sc. (Physical)

Chapter Number of hours Maximum marks allotted
Electrochemistry 22 45
Phase equilibrium 5 10
Redox chemistry 5 10
Solid state chemistry 5 10
Photo chemistry 8 16
45 91
Total
(including choice)

Marks allotment for VI semester BSc (Inorganic)

Chapter Number of hours Maximum marks allotted
7 14
Halogens 2 4
23 47
Compounds of Nobel gases
5 10
d-Block elements & 3 6
coordination chemistry 5 10
Organometallic chemistry 45 91
(including choice)
Bio-inorganic chemistry

f-Block Elements

Total

B.Sc. Syllabus Chemistry 2018-21 Page 50