KUVEMPU UNIVERSITY
DEPARTMENT OF CHEMISTRY
SAHYADRI SCIENCE COLLEGE (AUTONOMOUS)
SHIMOGA – 577 203
APROOVED SYLLABUS FOR B.Sc. COURSE IN CHEMISTRY
V SEMESTER
Approved Syllabus Effective From 2012
Paper-V
Inorganic Chemistry
Chapter 2
7 hrs
d-Block elements
Electronic configuration, general characteristics of transition elements, oxidation states,
atomic size, ionization potential, colour, complex formation, magnetic properties and
acidic & basic properties of oxides- explanation with reference to 3d-series.
f-Block elements
Lanthanide series-Definition, electronic configuration, oxidation states, colour, complex
formation and magnetic properties, lanthanide contraction, its causes and consequences,
separation of lanthanides by ion-exchange method, applications of lanthanides.
Actinides
General survey of actinides, properties of actinides, comparison between lanthanides and
actinides with reference to oxidation state, complex formation, colour and magnetic
properties.
Chapter 2
8 hrs
Electroplating
Theory, purpose of electroplating, nature of good deposit, factors influencing
electroplating (concentration of metal ion, pH, temperature, current density),
electroplating of chromium and gold.
Refractories
Classification, properties, hardness, pyrometric cone equivalent values.
Ceramics
Raw materials and their role, varieties of clay, production of ceramic ware, glazing
insulators.
Abrasives
Classification, properties, hardness of abrasives, Moh’s scale, manufacture and
importance of carborundum
Adhesives
Defination, classification, binding strength of adhesives, chemical factors affecting
adhesive strength, characteristics and uses of adhesives (epoxy resins and phenol
formaldehyde resin)
1
Organic Chemistry
Chapter 1
Stereochemistry
Concept of isomerism, structural isomerism, stereoisomerism and its types.
11 hrs
Optical isomerism
Elements of symmetry-plane, centric and axis of symmetry conditions for optical activity
– van’t Hoff – Lebel hypothesis, enantiomers, and diastereoisomers – Fischer projection
formulae, properties and differences, Configuration – D and L-configuration, erythrothreo configuration and R and S-configuration. Optical isomerism of lactic acid and
tartaric acid. Racemisation, resolution (mechanical, biochemical, chemical method),
Walden inversion, asymmetric synthesis (using optically active reagent)
Geometrical isomerism
Conditions for the compound to exhibit geometrical isomerism. Nomenclature – cis-trans
nomenclature, E-Z nomenclature, syn-anti nomenclature. Determination of configuration
of geometrical isomers – physical methods, chemical methods, Beckmann
rearrangement-ketoximes.
Conformational isomerism
Cause for conformational isomerism, conformers, Newmann projection formulae.
Conformational isomerism of ethane, 1,2-dichloroethane, cyclohexane-axial and
equatorial bonds.
Chapter 2
4 hrs
Heterocyclic compounds
Definition, nomenclature, classification, one method of Synthesis – pyrrole (from
acetylene and succinaldehyde), furan, thiophene, pyridine, Chemical properties of pyrrole
(Bromination, F C acetylation, nitration, sulphonation, reduction) and pyridine
(Bromination, F C acetylation, nitration, sulphonation, reduction, reaction with KOH and
NaNH2), Comparison of basicity and aromaticity (MO theory) of pyrrole and pyridine.
Physical Chemistry
Chapter 1
5 hrs
Thermodynamic-II
Spontaneous processes, heat engine, Carnot’s cycle and its efficiency, Refrigeration.
Concept of entropy. Entropy as a state function, Limitations of First law and need for the
second law. Statements of second law of thermodynamics. Entropy changes of an ideal
gas with P, V and T. Calculation of entropy changes in different processes (isothermal,
adiabatic, isochoric, isobaric and cyclic). Molecular interpretation of entropy, Physical
significance of entropy. Entropy changes in phases (problems to be solved).
2
Chapter 2
5 hrs
Thermodynamic-III
Free energy-Helmholtz free energy(A). Gibb’s free energy(G) and their relationship. Free
energy and useful work. Significance of free energy and useful work. Significance of free
energy change-criteria for equilibrium and spontaneity. Variation of free energy with P,
V, and T. Derivation of Gibbs–Helmholtz equation, Equilibrium constant and its
variation with temperature-Vant Hoff’s isotherm, Vant Hoff’s equation, ClausiusClapeyron equation and its applications (problems to be solved).
Chapter 3
5 hrs
Crystallography
Different types of crystals, Laws of crystallography, Elements of symmetry-plane, axes
and centre of symmetry. Elements of symmetry in cubic system. Crystal lattice-space
lattice and unit cell crystal systems. Bravais lattice, Miller indices, lattice planes in
different cubic systems. X-ray diffraction and Bragg’s law(to be derived). Determination
of crystal structure of rock salt by Bragg’s method. Avogadro number (Problems to be
solved).
Approved Syllabus Effective From 2012
Department of Chemistry
V SEMESTER
Paper-VI
INORGANIC CHEMISTRY
Chapter 1
6 hrs
Inorganic polymers
Silicones: Types, preparation (Linear, branched and cyclic), properties and applications.
Fluorocarbons: Definition, examples, properties, manufacture of Teflon and uses.
Phosphazenes: Preparation, properties and nature of bonding in triphosphazenes.
Borazines: Preparation, properties and uses, structure and bonding.
S-N ring compounds (S4N4 and S2N2): Preparation, properties and uses.
Chapter 2
Advantages of organic reagents in inorganic quantitative analysis
Uses of the following organic reagents in inorganic quantitative analysis
1. EDTA – Estimation of hardness of water
2. Oxine – Estimation of Magnesium
3. DMG – Estimation of Nickel
4. 1,10-phenonthraline – Estimation of Iron
3
3 hrs
Chapter 3
6 hrs
Bio-inorganic Chemistry
Elements in biological systems- metals and nonmetals, bulk metals and trace metals.
Iron: Co-ordination environment in HEAME, Role of haemoglobin in oxygen
transportation.
Zinc: Zinc containing metalloenzymes- role of carbonic anhydrase and carboxy
peptidase.
Magnesium: Co-ordination environment in chlorophyll, skeletal structure of chlorophyll,
role of chlorophyll in photosynthesis.
Cobalt: Vitamin B12 , Molybdenum: Nitrogenase.
Organic Chemistry
Chapter 1
9 hrs
Carbohydrates
Definition, Classification, Constitution of glucose and fructose (open chain and ring
structure, determination of ring size), Inter conversions – aldose to ketose and ketose to
aldose, chain lengthening and chain shortening of aldoses. Epimerisation - (conversion of
glucose to mannose). Mechanism of mutarotation. Disaccharides - Elucidation of
structure of maltose and sucrose.
Polysaccharides – Structure of starch and cellulose.
Chapter 2
3 hrs
Alkaloids
Definition, classification, method of isolation; elucidation of structure of nicotine and its
synthesis by spath process.
Chapter 3
3 hrs
Terpenes
Definition, classification and isolation; isoprene rule, structural elucidation of citral and
its synthesis from methyl heptenone.
Physical Chemistry
Chapter 1
10 hrs
Electro Chemistry-I
Conductance, specific conductance, molar conductance, equivalent conductance,
determination of equivalent conductance, variation of
specific
and equivalent
conductance with dilution. Anomaly of strong electrolytes. Debye – Huckel
theory of strong electrolytes - a qualitative treatment. Debye – Huckel – Onsagar
equation. Ionic conductivity and ionic mobility. Kohlrausch’s law and its
applications (Determination of equivalent conductance of weak electrolyte, determination
of solubility and solubility product, and determination of ionic product of water and
determination of degree of dissociation).
4
Transport numbers - anomalous transport numbers, principles of determination of
transport numbers by Hittorf’s method - both attackable and non-attackable
electrodes. Relation between ionic conductance and transport numbers. Principles
involved in conductometric titrations of i) strong acid vs strong base ii) weak acid vs
strong base
iii) strong acid vs weak base iv) weak acid vs weak base v) KCl vs
AgNO3.
Weston’s standard cell, Nernst reduction equation (to be derived), expression for
single electrode potential, reference electrodes - calomel and glass electrodes.
Determination of E.M.F. of a cell. Reversible and Irreversible cells. - Energy
calculations of a cell and thermodynamic of a chemical cell.
Concentration cells - EMF of concentration cell, concentration cells with and
without transference. Liquid junction potential and salt bridge.
Chapter 2
5 hrs
Electro Chemistry-II
Applications of EMF measurements
1. Determination of valency of ions.
2. Determination of solubility and solubility product of sparingly soluble salts.
3. Determination of pH of a solution by using
i) Quinhydrone
and
ii)
Glass electrode.
4. Potentiometric titrations.
i) Acid Base titration
ii)
Redox titrations.
Fuels cells: - Types, their construction and working of H2 –O2 fuel cell. Importance
of fuels cells.
V SEMESTER PRACTICALS
PRACTICAL V
3 hrs per week
01. Estimation of Barium in Barium chloride solution.
02. Estimation of Iron as Iron oxide in Mohr’s salt.
03. Estimation of Aluminium as aluminium oxide in potash alum solution.
04. Estimation of Nickel as Nickel dimethylglyoximate in Nickel ammonium sulphate
solution.
05. Estimation of Copper as Cuprous thiocyanate in copper sulphate solution.
06. Estimation of Zinc as Zinc Oxinate in zinc sulphate solution.
07. Estimation of Mg2+ by oxinate method.
08. Estimation of SO42- by gravity method.
09. Seperation of Cu2+, Ni2+ and Fe by paper chromatography-ascending.
10. Separation of amino acids by thin layer chromatography.
5
PRACTICAL VI
3 hrs per week
Part A - Estimation
01. Estimation of Glycine
02. Estimation of Citric acid in lemon juice.
03. Estimation of Salicylic acid in Aspirin.
04. Estimation of glucose in urine sample.
05. Estimation of phenol.
Part B – Synthesis
01. Preparation of double salt (nickel ammonium sulphate).
02. Preparation of complex compound (copper ammonium sulphate).
03. Preparation of complex compound (potassium trioxalato aluminate).
04. Preparation of organic compounds by
a) Oxidation
b) Acetylation
c) Nitration
d) Bromination
6
KUVEMPU UNIVERSITY
DEPARTMENT OF CHEMISTRY
SAHYADRI SCIENCE COLLEGE (AUTONOMUS)
SHIMOGA – 577 203
Approved Syllabus Effective From 2012
Department of Chemistry
VI SEMESTER
Paper-VII
Draft Syllabus
Inorganic Chemistry
Chapter 1
9 hrs
Metallurgy
Thermodynamics of metallurgy, Elingham’s diagrams- features, applications and
limitations, extraction of lead - self-reduction process and nickel from pentalendite,
extraction of manganese from pyrolusite from allumino thermite process extraction of
gold by hydrometallurgical process, refining of gold by quartation process, beryllium
from beryl via sodium beryllium fluoride, Thorium from Monazite sand and Uranium
from Pitch blende by aid digestion process.
Chapter 2
6 hrs
Alloys
Definition, purpose of making alloys, preparation of alloys by electro deposition method
and powder metallurgy method, advantages of powder metallurgy, influence of carbon,
manganese, nickel, chromium, tungsten, silicon and cobalt on the properties of steel, heat
treatment of steel, hardening, tempering and annealing, case hardening of steel-carbiding
and nitridins. Ferro alloys- composition and manufacture of ferromanganese and
ferrochrome.
ORGANIC CHEMISTRY
Chapter 1
3 hrs
Dyes
Definition, classification with examples, Requisites of a dye. Theory of colour and
constitution - chromophore-auxochrome theory, modern theory. Synthesis and uses of
Congo red, malachite green, indigo. Structural elucidation, synthesis and uses of alizarin.
Chapter 2
3 hrs
Drugs
Definition, Requisites of a drug, chemotherapy, sources of drugs.
Sulpha drugs – examples, mode of action, Synthesis and uses of Sulphanilamide, Sulpha
thiazole.
Antimalarial drugs – Synthesis and uses of chloroquin.
Antipyretics – Synthesis and uses of paracetamol, aspirin.
7
Chapter 3
4 hrs
Polymers
Definition, Types of polymers, stereochemistry of polymers, Addition polymers mechanism of polymerization (ionic and free radical). Synthesis and uses of PVC,
polystyrene.
Condensation polymers – polyester (Dacron), polyamides (Nylon-6,6).
Thermoplastics and thermosetting plastics – phenol formaldehyde resins and urea
formaldehyde resins.
Natural and synthetic rubber
Chapter 4
5 hrs
Active methylene compounds
Definition, acidity of active methylene compounds. Ethylacetoacetate – Synthesis
(Claisen condensation with mechanism), keto-enol tautomerism of Ethylacetoacetate ,
synthetic applications of ethylacetoacetate – Synthesis of mono and dicarboxylic acids,
keto acids, ,-unsaturated acids, amino acids, 4-methyl uracil. Diethyl malonate –
Preparation, synthetic applications of diethyl malonate - Synthesis of mono and
dicarboxylic acids, keto acids, ,-unsaturated acids, amino acids, barbituric acid.
PHYSICAL CHEMISTRY
Chapter 1
4 hrs
Spectrophotometry
Absorption spectra, Laws of absorption of light - Lambert’s law, Beer’s law,
Beer-Lambert’s law, Absorption co-efficient , molar absorption co-efficient , molar
extinction co-efficient. Construction of Spectrophotometer and determination of
absorption band. Uses of Spectrophotometer. (Problems to be solved).
Chapter 2
7 hrs
Photochemistry
Photo physical
processes, photochemical
processes, photoelectric
effect with
examples. Laws of photochemistry. (Grothus – Draper law, Einstein’s - Stark law
of photochemical equivalence) , quantum yield or efficiency. Reasons for low
and high quantum yield with examples. Primary and secondary processes.
Mechanism of the following photochemical processes.
a)
Decomposition of HI
b)
Combination of H2 and Br2
c)
Combination of H2 and Cl2
Problems based on quantum yield (Jablansky’s diagram), Chemiluminescence,
bioluminescence, fluorescence, phosphorescence, photo inhibitors, photosensitization,
photosynthesis, chemical actinometers (uranyl oxalate actinometer).
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Chapter 3
4 hrs
Radiation chemistry
Radiolysis, radiolysis of water vapour. Radiation dosimetry (units). Dosimeters
(Fricks dosimeter and ceric sulphate dosimeter). Application to some simple
organic and inorganic reactions. (C2H2 , CH4 , C6H6 , HCOOH, CH3COOH) .
Lind’s cluster theory, Erying , Hircefelder and Taylor Theory (EHT theory).
Difference between photochemistry and Radiation chemistry.
Approved Syllabus Effective From 2012
Department of Chemistry
VI SEMESTER
Paper-VIII
INORGANIC CHEMISTRY
Chapter 1
12 hrs
Co-ordination Chemistry
Double salts, complex salts, definition of terms-complex ion, ligand, co-ordination
number, co-ordination sphere. Types of ligands with example-monodentate, bidentate,
polydentate, Ambidentate and macro cyclic ligands (crown ethers, porphyrins).
Methods of detection of complex formation- conductivity, pH, colour.
Nomenclature of complex compounds,
Isomerism in complex compounds
a. Structural isomerism-Ionization isomerism, hydrate isomerism, linkage isomerism
and co-ordinate isomerism.
b. Optical and geometrical isomerism in complex compounds with co-ordination
number 4 and 6.
Stability of complex compounds- stability constant, factors influencing the stability of
complexes-Nature of metal ion, nature of ligands, chelation and macrocyclic effects.
Application of complex formation in (a) Metallurgy (in the extraction of nickel and gold)
(b) Qualitative and quantitative analysis.
Valance Bond Theory (VBT)
Valence bond theory as applied to complexes- inner and outer orbital complexes. The
structure and geometry of the following complexes to be discussed:
1. [Fe(CN)6]2- 2. [Fe(H2O)6]2+ 3. [MnCl4]2- 4. [Ni(CO)4]2- 5. [Ni(CN)4]66. [Cu(NH4))4]2+
Modification of VBT : Electroneutrality principle of [Be(H2O)]2+ and back bonding
effect with respect to [Ni(CO)4]2-.
9
Crystal Field Theory (CFT)
Splitting of d-orbitals in octahedral and tetrahedral fields, effect of weak and strong field
ligands, spectrochemical series of ligands, crystal field stabilization energy, calculation of
CFSE for different systems.
Chapter 2
3 hrs
Environmental Chemistry
Air pollution - air pollutants - oxides of carbon, nitrogen and sulphur. Global warming,
acid rain.
Photochemical smog and its effects, depletion of ozone layer-causes and its effect.
Water pollution - DO, BOD, COD.
ORGANIC CHEMISTRY
Chapter 1
6hrs
Spectroscopy
Electromagnetic radiation, interaction of electromagnetic radiation with organic
molecules, Frequency, wavelength, energy of a wave.
UV-Visible spectroscopy
Range, frequency and energy of UV radiations, interaction of UV radiation with organic
molecules, types of transitions, Concept of chromophores and auxochromes,
bathochromic shift and hypso chromic shift, hyper chromic effect and hypo chromic
effect.
Comparison of max of organic compounds taking following examples giving reasons
1. Ethylene and 1,3-butadiene
2. Cis and trans stilbene
IR spectroscopy
Range, frequency and energy of IR radiations, interaction of IR radiation with organic
molecules, molecular vibrations – stretching and bending vibrations, Hook’s law, finger
print region, Stretching frequency of functional groups in acetaldehyde, methyleamine,
methanol and methylcyanide.
Chapter 2
5 hrs
Oils, fats and waxes
Definition, chemical composition, Chemical properties - hydrogenation, hydrogenolysis,
hydrolysis, drying of oils, rancidity, Analysis of oils and fats - saponification value,
iodine and acid value, manufacture of soaps - hot process, cleansing action. Synthetic
detergents, comparison of soaps and detergents, types of detergents (cationic, anionic and
nonionic), animal and plant waxes – Defination, sources and examples.
10
Chapter 3
4 hrs
Amino acids and proteins
Definition and classification of amino acids, methods of synthesis of α-amino acidsGabriel’s phthalimide, Streckers synthesis. Zwitter ion and isoelectric point, Ninhydrin
test.
Peptides: peptide bond, carbobenzoxy method of synthesis of peptides
Protein: Classification based on composition, structure and function, primary and
secondary structures of proteins. Denaturation of proteins, Biuret test.
PHYSICAL CHEMISTRY
Chapter 1
14 hrs
Molecular Spectroscopy
Spectrum of electromagnetic radiations, interaction of electro magnetic radiations
with molecules, quantisatiation of different forms of energies in molecules.
Condition for energy absorption by
molecules, emission and absorption
spectrum.
Spectroscopic
terms, classification, Types
of
molecules - Linear
molecules, spherical top molecules, symmetric top molecules, asymmetric top
molecules.
Rotational Spectroscopy
Diatomic molecule as a rigid rotator, model, moment of inertia expression. Rotation
energy expression, wave number of rotational spectral line expression (to be
derived), Energy
level
diagram, selection rule for rotational
transitions.
Determination of moment of inertia and bond length of diatomic molecules
(CO, HCl molecules), isotopic effect on the rotational spectra, Intensity of
rotational spectral lines.
Chapter 2
Rotational - Vibrational Spectroscopy
Physical properties and molecular structure
5 hrs
Additive properties, constitutive properties, additive - constitutive properties (Molar
refraction, refractive index, molar volume - parachor).
Polarization
Induced polarization, orientation polarization, molar polarization, Classius-Mosotti
equation (No derivation) and its importance.
Dipole moment
Explanation its importance in comparison of bond polarity taking hydracids of halogens.
Shape of the molecules
a)
Tetratomic molecules ex. : PF3 , PCl3
b)
Pentatomic molecules ex. : CCl4, SiCl4
c)
Differentiating between cis and trans isomers
ex. : 1,2 dichloro ethane
11
VI SEMESTER PRACTICALS
PRACTICAL VII
3 hrs per week
Part-A
01. Determination of percentage composition of a binary mixture of organic liquids by
using Abbe’s Refractometer.
02. Determination of rate constant of inversion of cane sugar by Polarimeter.
03. Determination of cell constant (0.1N KCl solution to be prepared by students) and
determine the equivalent conductance of the given electrolyte solution by using
conductivity bridge.
04. Determination of cell constant (0.1N KCl solution to be supplied) and
determine the equivalent conductance at infinite dilution for strong electrolyte of
given
solution.
05. Potentiometric titration of Mohr’s salt solution vs Potassium dichromate solution
06. Potentiometric titration of Hydrochloric acid vs Sodium hydroxide.
Part-B
3 hrs per week
01. Conductometric titration of Sodium hydroxide vs Hydrochloric acid
02. Conductometric titration of Mixture of weak acid and strong acid vs Sodium
hydroxide.
03. Determine the pH of mixture of acetic acid and sodium acetate at different
concentrations and determination of dissociation constant of acid by using pH meter.
04. Estimation of Cu(II) in the given solution by colorimetric method.
05. Estimation of Fe(III) in the given solution by colorimetric method.
06. Conductometric titration of tertiary mixture of CuSO4 + Acetic acid + HCl using
NaOH solution.
PRACTICAL VIII
3 hrs per week
Project Work / Dissertation
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