KUVEMPU UNIVERSITY
DEPARTMENT OF CHEMISTRY
SAHYADRI SCIENCE COLLEGE
SHIMOGA – 577 203
INTEGRATED M.Sc. (Hons.) COURSE IN APPLIED CHEMISTRY
I – SEMESTER
Hours: 75
Inorganic chemistry
Chapter 1:Atomic Structure
11 hrs
Wave nature of electron, de-Broglie equation, (derivation of problems), Heisenberg
uncertainty principle, Schrodinger wave equation (no derivation), Significance of  and
2- atomic orbitals, Eigen function and Eigen values, radial and angular wave function
and probability distribution curve.
Quantum numbers and their significance, Shapes of s, p, d - orbitals and their nodal
planes. Assigning of quantum numbers to a given electrons 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, exchange energy, promotional energy, electronic
configuration of elements (up to 3d-series), (n + l) rule, effective nuclear charge,
screening effect based on Slater’s rule.
Chapter 2: Periodic Properties
8 hrs
Atomic radii, covalent radii, vander Waal’s radii, ionic radii, variation of atomic radii in a
group and period, iso-electronic ions.
Ionization of energy: Explanation, factors influencing ionization energies, variation of
ionization energy in a group and period, successive ionization energies, effect of ionic
size and electronic configuration (III period).
Electron affinity: Explanation, variation in a group and in a period. Explanation for the
observed trend.
Electronegativity: Explanation, factor affecting electronegativity, variation in a group and
in a period, explanation for the observed trend, anomalies to be accounted. Pauling scale
and Mullikan’s scale of electronegativity, Alfred and Rochow’s method.
Chapter 3: s-Block elements
5 hrs
Hydrogen: Atomic hydrogen-preparation and properties, ortho and para hydrogens,
definition, differences in physical properties
Alkaline earth metals: Comparative properties of alkaline earth metals, electronic
configuration, melting point, boiling point, softness and density, hydration of ions,
electropositive characters, flame coloration, comparative studies of properties of
compounds like oxides, hydroxides, carbonates, sulphates, solubility thermal
decomposition, amphoteric and basic nature. Anomalous properties of beryllium,
diagonal relationship between Be and Al.
1
Organic chemistry
Chapter 1: Introduction to analytical chemistry
11 hrs
Introduction to analytical chemistry, history, application of analytical chemistry in
clinical, pharmaceutical and chemical analysis. Statistical analytical chemistry. Errors,
types of errors, accuracy and precession. Distribution of random errors-frequency
distributions, statistical treatment of finet samples, mean, medium, range, average
deviation, standard deviation and variance. Reliability of results rejection of results,
confidence intervals. Test for significance, Q-test, F-test, Chi-isoqurane test, comparison
of means of two samples, control charts, significant fugures, least square method of
deriving calculation plots.
Introduction to qualitative analysis of inorganic salts: Common ion effect, solubility
products, principle. Application of common ion effect and solubility products, principle
in qualitative analysis.
Chapter 2: Purification of organic compounds
4 hrs
Method of purification of solids, crystallization, fractional crystallization, sublimation.
Method of purification of liquids, distillation, distillation under reduced pressure, steam
distillation, fractional distillation. Criteria of purity, melting point and boiling point.
Chapter 3:Composition of Organic Compounds
4 hrs
Estimation of elements - C, H – Liebig’s method, N - Kjeldahl’s method, P, S, X – Carius
method (with numerical problems), calculation of Empirical and Molecular formula.
Chapter 4: Types of Reactions, Reagents and Reaction Intermediates
5 hrs
Introduction to reaction, reaction mechanism, addition, elimination, substitution and
rearrangement reactions, homolysis, heterolysis, electrophiles, nucleophiles, free radicals,
carbocations, carbenes, carbanions (definition, formation, geometry, stability and
reactivity).
Chapter 5:Hybridisation
4 hrs
Overlapping of atomic orbitals, types of overlapping s-s, s-p, p-p, sp3, sp2, sp hybridization taking example of methane, ethane, ethene and ethylene molecules. Bond
length, bond angle and bond energy.
Chapter 6:Electronic effects
4 hrs
Inductive effect, electromeric effect, mesomeric effect, concept of resonance, resonance
effect and hyper conjugation effect with examples.
Chapter 7:Hydrocarbons
8 hrs
Alkanes: Nomenclature, synthesis from alkyl halides, Wurtz reaction, chlorination of
methane, free radical mechanism, pyrolysis of alkanes, pyrolysis of alkanes, knocking
property.
Alkenes: Nomenclature, types of alkenes, synthesis alkenes (dehydration and
dehydrohalogenation), chemical properties: addition of Br2 to ethene (mechanism),
mechanism of addition of HBr to symmetrical and unsymmetrical alkenes,
2
Markovnikov’s rule, peroxide effect- mechanism, oxidation reaction of alkeneshydroxylation, oxidative degradation, epoxidation, ozonolysis taking examples of
propene, 1-butene, 2-butene, 2-methyl-2-butene.
Physical chmeistry
Chapter-1: Liquid Mixtures
7 hrs
Classification of binary liquid mixtures into partially miscible, completely miscible and
completely immiscible liquids. Completely miscible liquids- Raoult’s law- ideal liquid
mixtures- -non-ideal liquid mixtures showing (a) very slight +ve deviation from ideal
behaviour (type-I) from Raoult’s law benzene, toluene as example (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 diagram and
vapour pressure temperature diagrams for all the three types of liquid mixtures, principle
of fractional distillation of type–I, type-II and type-III liquid mixtures and azeotropes.
Partially miscible liquid mixtures, mutual solubility temperature–critical solution
temperature (CST ) – mutual solubility temperature for phenol-water system
trimethylamine-water, Nicotine-water system- effect of addition of impurity on CST with
an example (electrolyte and an organic compound impurities on phenol-water system) –
completely immiscible liquids-immiscible liquid pairs with examples, weight fraction of
distillation-steam distillation and its application-problems on weight fraction of
components.
Chapter-2: Distribution law
3 hrs
Statement of Nernst distribution law, conditions for validity of distribution law,
limitations of distribution law, distribution coefficients –verification of Nernst
distribution law taking I2 in water and CCl4 as example. Association and dissociation of
the solute in one of the solvent, application of the distribution of law with respect to
solvent extraction process- de-silverisation of lead, Henry’s law and its limitations.
Chapter-3: Phase equilibrium
5 hrs
Gibb’s phase rule-statement-definition of the terms-phase, component and degree of
freedom with examples, applications- (a) phase equilibria of one component system,
water and CO2 and sulphur system
Phase equilibria of two component system-reduced phase and reduced system, solidliquid equilibria-simple eutectic system, silver-lead system and its application,
desilverisation of lead – solid solutions-compound formation with incongruent melting
point, ferric chloride- water system, KI-water system-principles of freezing point.
3
KUVEMPU UNIVERSITY
DEPARTMENT OF CHEMISTRY
SAHYADRI SCIENCE COLLEGE
SHIMOGA – 577 203
INTEGRATED M.Sc. (Hons.) COURSE IN APPLIED CHEMISTRY
II – SEMESTER
Hours: 75
Inorganic chemistry
Chapter 1: Chemical bonding
12 hrs
Ionic bond: Definition, lattice energy, factor controlling lattice energy, variation of
lattice energy with charges of ions and internuclear distance between oppositely charged
ions and internuclear distance between oppositely charged ions. Ionic size and hydration
energy, polarizing power, polarizability of ions, Fazan’s rule, covalent in ionic bonds
(problems to be solved).
Covalent bond
VBT-formation of H2 molecule- (taking  wave function of atomic orbital)  and 
bonds with their characteristics. Polar and non-polar bonds, electronegativity differences
variation of percentage ionic character of the bond (problems to be solved).
Chapter 2: Hybridization
3 hrs
2
3
3
4
3
3 2
3 3
7
sp (BF ), sp (CH ), sp d(PCl5), sp d (SF6), sp d (IF )
VSEPR Theory: shape of SF4, ClF3, XeF2, ICl, SnCl2, BO33-.
Chapter 3: Resonance
2 hrs
Concept of resonance energy calculation of resonance energy, requirements of
contributing resonance forms, resonance structures of CO2, NO, NO3-.
Chapter 4: Molecular orbital theory (MOT)
5 hrs
Linear combination of atomic orbital, in terms of wave functions, conditions for
combinations of atomic orbitals, energy levels of molecular orbitals, rules for filling
molecular orbitals, molecular orbital structure and bond order, O2, O2+, O22-, O2-.
Hetero nuclear diatomic molecules: CO, NO, CN-, HF (prediction of magnetic properties
of these species)
Chapter 5: Theory of volumetric analysis
Titrometric method of analysis-Introduction, equivalent weight, acidity, basicity. Primary
and secondary standards. Requirement of a primary standard, units of standard solutions
(normality molarity, molality, mole fraction, ppm, ppb).
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).
8 hrs
4
Organic chemistry
Chapter 1: Dienes
3 hrs
Types, with examples, synthesis of 1,3-butadiene (two methods), localized and
delocalized p-orbitals in 1,3-butadiene and 1,4-pentadiene, mechanism of addition of Br2
to 1,3-butadiene, Diels-Alder reaction.
Chapter 2: Alkynes
3 hrs
Nomenclature, preparation by dehydrohalogenation of dihalides and dehydrogenation of
tertahalides, acidity of alkynes- formation of metal alkynides, addition of water and HCl
to ethyne and propyne.
Chapter 3: Arenes and Aromaticity
8 hrs
Modern structure of benzene, resonance structures of benzene, resonance hybrid,
resonance energy, aromaticity, Huckel rule, aromatic ions and their stability, aromatic,
anti-aromatic non-aromatic and pseudo-aromatic.
Substitution reaction– mechanism of electrophilic reaction in benzene (nitration,
sulphonation, halogenation and Friedel-Craft’s alkylation mechanism of reaction
(amination, hydroxylation), derivatives of benzene- different classes of derivatives of
benzene, nomenclature, orienting influence of substituents in benzene – ortho and para
directors, meta directors, activatry effect, deactivating effect of substituent.
Chapter 4: Polynuclear Hydrocarbons
6 hrs
Fused, linked and bridged polynuclear aromatic hydrocarbons, synthesis of naphthalene
from benzene-Haworth’s method, addition, electrophilic, substitution reaction of
naphthalene, Reduction and oxidation of naphthalene, resonance structure of naphthalene,
constitution of naphthalene. Introduction to annulenes, heteroannulenes, Fullerenes –
preparation, structure and properties.
Chapter 5: Alkyl Halides
5 hrs
Classification, nucleophilic substitution reaction, SN1 and SN2 with mechanism (taking
example of t-butyl bromide and methyl bromide)
Elimination reaction- E1 and E2 reaction (taking example of t-butyl bromide and butyl
bromide), effect of solvent, alkyl halide and nucleophilic halogen of nucleophilic
substitution reaction and elimination reactions (stereochemistry of SN1 and SN2),
elimination reaction of secondary butyl bromide, Saytzeff rule and Hoffmann rule for
alkyl halides.
Chapter 6: Aryl Halides
2 hsr
Reactivity of chlorine in chlorobenzene, benzyl chloride, vinyl chloride and alkyl
chlorides, allyl chloride.
5
Chapter 1: Gases
6 hrs
Molecular velocities-Maxwell-Boltzmann distribution of molecular velocities (no
derivation)-types of molecular velocities-derivation of expression for RMS velocityderivation expression for average velocity and most probable velocity-relationship
between the three and problems based on temperature dependence-explanation of effect
of temperature on distribution of molecular velocities using distribution graph-MaxwellBoltzmann energy distribution as a function of temperature-degree of freedom-law of
equipartition of energy and its calculation for mono, di and triatomic molecule
Specific heat and molar heat of gases-the relation of molar heats of a gases with kinetic
theory.
Chapter 2: Critical Phenomena
4 hrs
Real gases, PV-isotherm of CO2- critical constants, Tc, Pc, and Vc definitionsexperimental determination of Tc and Pc using Caignard –de-la Tours apparatus and Vc
by Cailletets and Mathias method-vander Waal’s equation of state for real gasesrelationship 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 –law of
corresponding states and reduced equation of state (to be derived).
Chapter 3: Liquefaction of gases
3 hrs
Intermolecular forces- hydrogen bonding-brief account of dipole-dipole, dipole-induced
dipole and induced dipole- induced dipole interactions-vander Waal’s force of attraction
in explaining the physical properties of liquids –principle understanding liquefaction of
gases-Joule-Thomson effect, inversion temperature relation between it and vander Waal’s
constants a and b and its calculations.
Chapter 4: Colligative Properties
7 hrs
Raoult’s law of dilute solutions, osmotic pressure, relationship between relative lowering
of vapour pressure and molar mass of solute to be derived, determination of osmotic
pressure by Berkeley-Hartley method, plasmolysis, haemolysis, turgid state, reverse
osmosis, laws of osmotic pressure,. Elevation in boiling point, relation between elevation
in boiling point to molar mass (to be derived), Ebullioscopic constant, experimental
determination of molecular weight by Walker-Lumsden method.
Depression in freezing point, relation between depression in freezing point to molar mass
(to be derived), Cryoscopic constant, experimental determination of molecular weight by
Beckmann’s method. Determination of molecular weight of solute by Rast’s method.
Abnormal molecular masses-Van’t Hoff factor-degree of dissociation, (numerical
problems to be worked out).
I SEMESTER CHEMISTRY PRACTICALS
6
I Systematic semimicro qualitative analysis
Systematic semimicro qualitative analysis of inorganic mixture two simple salts
involving following anions and cations.
Anions: CO3-2, HCO3-1, SO3-2, S-2, Cl-1, Br-1, I-1, NO3-1, SO4-2, BO3-3, PO4-3.
Cations:Pb+2, Cd+2, Bi+3, Al+3, Fe+2, Fe+3, Zn+2, Mn+2, Ni+2, Ba+2, Ca+2, Sr+2, Mg+2,
+
+
NH4 , K , Na
+
II Organic preparations
Bromination:
Acylation :
Oxidation :
Nitration :
p-Bromo acetanilide from acetanilide
Acetanilide from aniline
Benzoic acid from benzyl alcohol
m-Dinitro benzene from nitro benzene
II SEMESTER CHEMISTRY 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. biphtalate
crystals.
4. Estimation of Mohr’s salt using approximately 0.1N KMnO4 solution and oxalic acid
crystals.
5. Estimation of ferric chloride using approximately 0.1N K2Cr2O7 solutions and
Mohr’s salt crystals (diphenyl amine indicator method)
6. Estimation of copper sulphate solution using approximately 0.1N sodium thiosulphate
solution and K2Cr2O7 crystals.
7. Estimation of sodium chloride using approximately 0.1N AgNO3 solution using KCl
crystal.
8. Estimation of available chlorine in bleaching powder.
7