Curriculum
2015-2016
Chemistry
course codes and Titles
YEAR
|
S.No
|
Course Code
|
Title of the Paper
|
Semester
|
2015-2016
|
1.
|
1112
|
Inorganic,Organic,Physical
and General chemistry
|
I
|
2.
|
2212
|
Inorganic,Organic,Physical
and General chemistry
|
II
|
|
3.
|
312
|
Inorganic,Organic,Physical
and General chemistry
|
III
|
|
4.
|
412
|
Inorganic,Organic,Physical
and General chemistry
|
IV
|
|
5.
|
5121
|
Inorganic
chemistry
|
V
|
|
6.
|
5122
|
organic
chemistry
|
V
|
|
7.
|
6121
|
Physical
chemistry
|
VI
|
|
8.
|
6122
|
General
chemistry
|
VI
|
|
9.
|
1112-P
|
Practical
–I
|
I
|
|
10.
|
2212-P
|
Practical-II
|
II
|
|
11.
|
312-P
|
Practical-III
|
III
|
|
12.
|
412-P
|
Practical-IV
|
IV
|
|
13.
|
6121-p
|
Practical-V
|
VI
|
|
14.
|
6122-p
|
Practical-VI
|
VI
|
DUVVURU RAMANAMMA
WOMEN’S COLLEGE GUDURU
(AUTONOMOUS)
I-B.Sc- CHEMISTRY-
SEMESTER-I- PAPER-I - SYLLABUS
UNIT-I
INORGANIC CHEMISTRY
1.
P-block elements: General characteristics
of elements of group 14 .Group 14 :
Preparation and applications of silanes and silicones,graphitic compounds.
2.
Chemical bonding : Valance bond theory, hybridization, VB theory as applied to
CIF3, Ni(CO)4,
dipolemoments-orientation of dipole in an electric field, dipolemoment, Induced dipole moment, dipolemoment and
structure of molecules. Molecular orbital theory – LCAO , construction of MO diagrams for homo-nuclear
and hetero nuclear di atomic molecules (N2,O2,COandNO).
Comparission of VB and MO theories.
UNIT-II ORGANIC CHEMISTRY
Structural
theory in organic chemistry: Types of bond fission and organic reagents
(Electophilic,Nucleophilic and freeradical reagnts including neutral molecules
like, H2O, NH3
&AlCl3). Bond
polarization : Factors influencing the polarization of covalent bonds, electro negativity- inductive effect. Applications of
inductive effect a).Basicity of amines (b)acidity of carboxylic acids (c) Stability of carbonium ions.Resonance
or mesomeric effect, application to (a)
acidity of phenol &(b) acidity
of carboxylic acid. Hyper conjugation
and its application to stability of carboniumions, free radicals and alkenes, carbanions,
carbenes & nitrenes.Types of organic reactions : Addition-electophilic,nucleophilic &
free radical.substitution-electrophilic,nucleo philic & free radical . Elimination- examples (mechanism not required).
UNIT-III Acyclic Hydrocarbons:
Allkens-preparation of alkens
(a) By dehydration of alcohols(b) by dehydro halogenation of alkyl halides(c)by
dehalogenation of 1,2 di
halides(brief mechanism),
saytzev’s rule. Properties : addition of hydrogen- heat of hydrogenation and
stability of alkenes. Addition of
halogen and its mechanism. Addition of HX,markonikov’s rule,Addition of H2o,HOX,H2SO4 with mechanism and addition of
HBr in the presence of peroxide (Ant
markonikov’s addition).Oxidation – Hydroxylation by KMnO4,OsO4,
peracids(via epoxidation)
Hydroboration,Dienes-types of dienes,reactions of conjugated dienes-1,2
and1,4 addition of HBr to 1,3 –buta
diene and Diel’s-alder reaction, Synthesis of Isoprene and Chloroprene.
Alkynes – Preparation by
dehydrohalogenation of di halides, dehalogenation of tetra halides,
properties;Acidity of acetylinic hydrogen (formation of metal
aciditylides). preparation of higher
acetylenes, metal ammonia reductions Physical properties .Chemical
reactivity-electrophilia addition of
x2,HX,H2O(tautomerism),Oxidation with KMnO4.
OsO4,Reduction and polymerization rection of acetylenes.
UNIT-IV PHYSICAL CHEMISTRY
1.Gaseous state: Compression factors, deviation
of real gases from ideal behavior. Vanderwalls equation of state. P-V Isotherms
of real gases ,Andrew’s isotherms of carbon dioxide. Continuity of state. critical phenomena. The
vanderwalls equation and the critical
state relationship between critical
constants and vanderwall’s constants. The law of corresponding states and
reduced equation of states. Joul Thomson
effect. Liquefaction of gases:1.Linde;s
method and Claude’s method.
2. Liquid state:
Intermolecular forces, structure of liquids(qualitative
description).structural differences
between solids, liquids and gases. Liquid crystals, the mesomorphic state. classification of liquid crystals into
smectic and nematic. Differences between liquid
crystal and solid or liquid.application of liquid crystals as LCD
devices.
UNIT-V GENERAL CHEMISTRY
1.Atomic structure
and elementary quantum mechanics:
Black body radiation, plancks radiation law, photo electric effect, Compton
effect, de Broglies hypothesis,
Heisenberg’s uncertainty principle. Postulates of quantum mechanics.
Wave functions and probability densities. Schrodinger wave
equation for H-atom (no derivation
qualitative treatment only). Quantum numbers and their importance.
2. Theory of
quantitative analysis:
a) principles of volumetric analysis: Theories of acid- base, redox, complexomentric, iodometric and
precipitation titrations, choice of indicators for these titrations
b) principles of gravimetric analysis:
precipitation, coagulation, peptization, co-precipitation, post precipitation,
dilution,filteration and washing of precipitate, drying and ignition,
precipitation from homogeneous
solutions, requirements of gravimetric analysis.
LABORATORY
COURSE-1( SEMESTER-1) PRACTICAL-I
Qualitative Inorganic
Analysis Qualitative
Analysis and Inorganic preparation.
Analysis
of simple salt containing the following one Anion and cation.
Analysis
of Anion: Carbonate, Sulphate, Chloride, Bromide, Iodide, Acetate,Nitrate
,Borate, Phospate. Analysis of Cation: Lead,Copper, Cadmium,Iron,Aluminum,Zinc,
Manganese, Nickel,Calcium,Stronitum.Barium,Potassium, Ammonium.
Inorganic
preparations: Any one of the following Inorganic preparations:1.Ferrous
Ammonium Sulphate
2.Tetraamine
copper(II) Sulphate.
I-B.Sc- CHEMISTRY-
SEMESTER-II- PAPER-II
UNIT-I
INORGANIC CHEMISTRY
1.P-block elements: General character sticks of elements of
groups 15&16 . Group 15 : Preparation and reactions of hydrazine, hydroxyl
amine. Group 16 : Classifications of oxides based on (i) Chemical behavior and
(ii) Oxygen conten
2.Organo metallic chemistry: Definition
and classification of organo metallic compounds, nomenclature, preparation, properties and
applications of alkyls of 1,2 and13 group elements.
UNIT-II ORGANIC CHEMISTRY-ALICYCLIC
HYDROCARBONS (CYCLO ALKENES): Nomenclature, preparation by freunds methods,
heating dicarboxylic metal salts,properties,reactivity
of ctclopropane by comparing witalkanes, stability of cycloalkanes – Baeyers strain theory, sahche
and mohr prediction and pitzer’s strain theory. conformational structures of
cyclobutane cyclopentane, cyclohexane.
UNIT-III-STEREO
CHEMISTRY OF CARBON COMPOUNDS:
Molecular representations- Wedge, Fischer, Newman and Saw-Horse formulae. Stereo isomerism, stereo isomers:
Enantiomers,diastereomers- definition and examples. Conformational and configurational
isomerism- definition. Conformational isomerism of ethane and n-butane. Enantiomers: optical activity-wave
nature of light, plane polarized light, interaction with molecules, optical
rotation and specific rotation. Chiral molecules - definition and criteria-
absence of plane, center and Sn axis of symmentry-and asymmetric and
dissymmetric molecules. Examples of
asymmetric molecules(glyceraldehydes,lactic acid, alanine) and disymetric molecules (trans 1,2-dichloro
cyclopropane).
UNIT-IV PHYSICAL CHEMISTRY
1.
Solid state : Symmetry in crystals. Law
of constancy of interfacial angles. The law of
rationality of indices. The law of symmetry. Definition of lattice
point, space lattice, unit cell. Bravis lattices and crystal system. X-ray diffraction and crystal structure. Braggs law.Determination
of crystal structure by Bragg’s method and powder method. Indexing of planes and structure NaCl and KCl
crystals. Defects in crystals.
Stoichiometric and non-stoichiometric defects. Band theory of
semi conductors. Extrinsic and intrinsic
semiconductors, n- and p-type semiconductors and their applications in
photo electrochemical cells.
2.Solutions : Liquid-liquid-ideal solutions, Raoult’s law.
Ideally dilute solutions, Henry’s law.
Non ideal solutions. Vapour pressure-composition and vapour pressure-
temperature curves. Azeotropes-HCl-H2O,
ethanol-water systems and fractional distillation. Partially miscible liquids-phenol-water, tri methyl amine-water,
nicotine-water systems. Effect of
impurity on consulate temperature. Immiscible liquids and steam
distillation. Nernst distribution
law. Calculation of the partition co-efficient. Applications of
distribution law.
UNIT-V GENERAL CHEMISTRY
1.Polymerization: Types of polymerization, free
radical, cationic and anionicpolymerization, including mechanism and
preparation of polymers by addition and
condensation with examples.
2.General principles of inorganic
qualitative analysis : Solubility
product, commonion effect, characteristic
reactions of anions, elimination of interfering anions, separation of cation into
groups, group reagents, testing of cation Evaluation of analytical data: Theoreis of
errors , idea of significant figures and its importance .Accuracy –methods of
expressing accuracy, error analysis and minimization of errors, precision –methods of expressing
precision, standard deviation and confidence limit.
LABORATORY
COURSE -II
Practical-II (At the end of
Semester-II)30 hrs (2 h / w)
Qualitative inorganic analysis
Analysis of
mixture salt containing two anions and two cations (From two different groups)
from the following:
Anions: Carbonate, sulphate, chloride,
bromide, iodide, acetate, nitrate, borate, phosphate.
Cations: Lead, copper,
iron, aluminum, zinc, manganese, calcium, strontium, barium, potassium and
ammonium.
II
B.SC -
Chemistry - SEMESTER-III- PAPER – III
UNIT-I INORGANIC CHEMISTRY-II
1. Chemistry of
d-block elements: Characteristics of d-block elements with
special reference to electronic - Configuration, variable valence, magnetic properties,
catalytic properties and ability to form
complexes. stability of various oxidation comparative states and treatment of second and thirdtransition series with their 3d
analogues
2.Theories
of bonding in metals: Valence bond theory, Explanation of metallic
properties and its limitations, Free
electron theory ,thermal and electrical conductivity of metals, limitations,
Band theory, formation of bands, explanation of conductors, semiconductors and insulators .
UNIT-II ORGANIC CHEMISTRY-II
1.Benzene and its
reactivity:Concept
of resonance, resonance energy, Heat of hydrogenation, heat of combustion of
Benzene, mention of c-c bond lengths and orbital picture of Benzene. Concept
of aromaticity – aromaticity
(definition), Huckle’s rule-application to Benzenoid (Benzene, Naphthalene) and Non- Benzenoid
compounds (cyclopropenly Cation, cyclopentadienly anion and tropylium cation).
Reactions-Gerenal mechanism of electrophilic substitution, mechanism of
nitration. Friedel craft’s alkylation and acylation. Orientation of
aromatic substitution- Definition
of ortho, para and meta directing groups. Ring activating
anddeactivating groups With examples (Electronic interpretation of various
groups like NO2 and Phenolic).
2.Halogen
compounds: Nomenclature
and classification of alkyl (into primary ,second ,tertiary), aryl, aryl
alkyl, allyl, vinyl, benzylhalides. Chemical reactivity,
formation of RMgX (Grignard products)Nucleophilic aliphatic
substitution reaction. Classification into SN1 and SN2. Energy Profile diagram of SN1 and SN2
reactions. Stereo chemistry of SN2(Walden inversion) SN2 (Recemisation). Explanation of
both by taking the example of optically
active Alkyl halide 2-bromobutane. Ease
of hydrolysis- comparison of alkyl, benzyl, alkyl,Vinyl and aryl halides.
UNIT-IIIPHYSICALCHEMISTRYII
1.Phase rule: Concept of phase, components,
degree of freedom. Derivation of Gibbs phase rule. Phase Equilibrium of one component-water system,phase equilibrium of two-component system, Solid-Liquid equilibrium. Simple eutectic diagram
of Pb-Ag system, desilverisation of lead. Solid
solutions-compound with congruent Melting point -(Mg-Zn) system,compound with
incongruent melting point –NaCl -water system. Freezing mixture
2.
Electro Chemistry-I: Specific conductance,
equivalent conductance, measurement of equivalent conductance. Variation
of equivalent conductance with dilution. Migration of ions, kohlrausch’s law Arrhenius theory of electrolyte dissociation and its limitations. Ostwald’s dilution law. Debye-Hukle-Onsagar eqation for strong
electrolytes (elementary treatment only).
Definition of transport number,
determination by Hittorf’s method. Application of conductivity measurements –determination of dissociation
constant (ka) of an acid, determination of solubility product of sparingly
soluble salt, conductometric titrations.
UNIT-IV GENERAL
CHEMISTRY
1.Stereo Chemistry of carbon
compounds: Chiral
centers: Definition - molecules with similar chiral carbon (Tartaric Acid),
definition of mesomers –molecules with dissimilar chiral carbons (2,3-di bromo pentane). Number of enantiomers
and mesomers- calculation. D,L and R,S
configuration for asymmetric and disymetric molecules. Cahn-In gold-Prelog
rules. Racemic mixture-recimisation and
resolution techniques. Diasteriomeres: definition-geometrical isomerism with
reference to alkens-cis ,trans and E,Z configuration .
2.ColloidsAndSurfaceChemistry
Definition of colloids. Solids in liquids( sols),preparation ,
purification, properties – kinetic, optical, electrical. Stability of colloids, Hardy –Schulze law, protective colloids. Liquids in liquids (Emulsions) preparation, properties, uses. Liquids in
solids(gels) preparation, uses.Adsorption;
physical adsorption , chemisorption . Freundlich, Langmuir adsorption isotherms
Applications of adsorption.
_____________________
II B.SC CHEMISTRY - IV SEMESTER – PAPER IV
UNIT-I
- INORGANIC CHEMISTRY-II
1. Chemistry of f-block elements
Chemistry of Lanthanides-
electronic structure, oxidation states, Lanthanide contraction, consequences of
Lanthanide contraction, magnetic properties, spectral properties chemistry of
actinides-electronic configuration, oxidation state, actinide contraction,
position of actinides in the periodic table, comparison with Lanthanides in
terms of magnetic properties, spectral properties and complex formation .
2.Co-ordination chemistry : IUPAC nomenclature, bonding theories –
review of Werner’s theory and Sidgwick’s
concept of coordination, Valence bond
theory, geometries of coordination numbers 4-tetrahedral and squar planar and 6-octahedral and its limitations, crystal
filed theory, splitting of d- orbitals in octahedral, tetrahedral and
squar-planar complexes-low spin and high spin complexes-factors affecting
crystal- field splitting energy ,merits
and demerits of crystal-field theory. Isomerism in coordination compounds-structural isomerism and stereo
isomerism, stereochemistry of complexes with 4 and 6 coordination numbers.
Metal Carbonyles and related compounds:
EAN Rule, classification of metal carbonyls. Stuctures and shapes of metal carbonyls of V, Cr, Mn,
Fe, Co and Ni. Metal nitrosyls and metallocenes (only Ferrocene) .
UNIT-II
ORGANIC CHEMISTRY-II
1.Hydroxy
Compounds :
Nomenclature
and classification of hydroxyl compounds. Alcohols: Preparation with hydroboration reaction,
Grignard synthesis of alcohols. Phenols: Preparation (1) from diazonium salt, (2)from Aryl sulphonates, (3)
from cumene Physical
properties-Hydrogen bonding (intermolecular and intramolecular). Effect of
hydrogen bonding on boiling point and
solubility in water. Chemical
properties: (a) acidic nature of
phenols (b)formation of alkoxides / phenoxides and their reaction with RX (C) Replacements of OH by X using Pcl5,Pcl3,
PBr3,Socl2 and with HX/Zncl2 (d)
esterification by acids (mechanism) (e) dehydration of alcohols (f) oxidation of alcohols by Cro3,
KMno4. (g) special reaction of phenols: Bromination,
Kolb- Schmidt reaction,
Riemer-Tiemann reaction, Fries
rearrangement, Azo-coupling. Identification of alcohols by oxidation with
KMno4, ceric ammonium nitrate, Lucas reagent
and phenols by reaction with Fecl3.
Polyhydroxy compounds: pinacol-
pinacolone rearrangement
2.
Carbonyl compounds :Nomenclature of aliphatic and
aromatic carbonyl compounds, structure of the carbonyls group Synthesis of
aldehydes from acid chlorides, synthesis of aldehydes and ketones using 1, 3 di
thianes,synthesis of ketones from
nitriles and from carboxylic acids.
Physical properties; absence of hydrogen bonding, keto- enol tautomerism, reactivity of carbonyl group in
aldehydes and ketones. Nucleophilic
Addition reaction with (a) NaHS03 , (b)HCN (C) RMgX
(d) NH2OH (e) PhNH NH2 (f) 2,4 -
DNPH (g) Alcohols- formation of hemiacetal and acetal.
Halogenation using PCl5 with
mechanisam. Base catalysed reactions; Aldol, Cannizzaro reaction, Perkin
reaction, Benzoin condensation, Haloform reaction, Knoevenagel reaction . Oxidation of aldehydes- Baeyer-Villiger oxidation of ketones
Reduction- clemensen reduction,Wolf- Kishner reduction, MPV Reduction, reduction with LiAlH4 and
NaBH4. Analysis of aldehydes and
ketones with a)2,4- DNP test , (B) Tollen’s test (C) Fehling test (D) Schiff test (E) Haloform test (withequation).
UNIT-III- PHYSICAL CHEMISTRY-II
1.Dilute
solutions : Colligative properties, Raoult’s law, relative
lowering of vapour pressure, its relation to molecular weight of non- volatile
solute. Elevation of boiling point and depression of freezing point. Derivation
of relation between molecular weight and elevation in boiling point anddepression
in freezing point. Experimental methods of determination. Osmosis, osmotic pressure, experimental determination. Theory of dilute
solutions. Determination of molecular weight of non-volatile solute from osmotic pressure. Abnormal
colligative properties. Van’t Hoff factor, degree of dissociation and
association.
2.Electro
chemistry-II
Types of reversible electrodes –the gas
electrode, metal-metal ion, metal-insoluble salt and
redox electrodes. Electrode reaction, Nernst equation, single electrode
potential, Standard Hydrogen electrode,
reference electrodes, , standard electrode potential, sign convention, electro
chemical series and its significance. Reversible and irreversible cells,
conventional representation of electro
chemical cells. EMF of a cell and its
measurements, computation of cell EMF. Applications of EMF
Measurements - potentiometric titrations.
UNIT-IV
- GENERAL CHEMISTRY-II
1.Molecular
symmetry:Concept
of symmetry in chemistry- symmetry
operations, symmetry elements. Rotational axis of symmetry and types of
rotational axis. Planes of symmetry and
types of planes. Improper rotational axis of symmetry. Inversion center identity element. The symmetry
operations of a molecule form a group. Flow
chart for the identification of molecular point group.
2.Infrared absorption spectroscopy :
Energy levels of simple harmonic oscillator, molecular vibrations
Hooke’s law, intensity, determination
force constant and qualitative relation of force constant bond energies ,effect of an harmonic motion and isotope on the spectrum, modes of vibrations
in poly atomic molecules, intensity and
position of IR bonds Instrumentation,
characteristic absorption bonds of various functional groups-Interpretation of
IR spectra of simple organic molecules.
LABORATORY
COURSE-III Inorganic
chemistry:
I.Titrimetric
Analysis:1.Determination
of Carbonate and bicarbonate in a mixture.
2. Determination of Fe(II)
usingKMno4 with Oxalic Acid as Primary Standard
3. Determination of Zinc using EDTA
LABORATORY
COURSE-IV
1. Determination of Fe(II) usingK2Cr2O7
2. Determination of Hardness of
Water
3. Determination of Magnesium
using EDTA
III
B.Sc-V-SEMESTER –PAPER-V- INORGANIC CHEMISTRY
1.Materials science :Superconductivity,
characteristics of superconductors, Meissner effect, types of superconductors
and applications. Nanomaterials- synthetic techniques, bottom-up-sol-gel
method, top-down- electro deposition method. Properties and applications of
nano-materials.
2. Spectral and
magnetic properties of metal complexes:
Electronic absorption spectrum of [Ti(H2O)6] 3+ ion. Types of magnetic
behavior, spin-only formula, calculation of magnetic moments, experimental
determination of magnetic susceptibility – Gouy method.
3.Reactivity of
metal complexes: Labile and inert complexes, ligand substitution
reactions – SN1 and
SN2, substitution reactions of square planar complexes – Trans effect and
applications of trans effect.
4.Stability of
metal complexes:
Thermodynamic stability and kinetic stability, factors affecting the stability
of metal complexes, chelate effect, determination of composition of complex by
Job’s method and mole ratio method.
5. Bioinorganic chemistry: Essential elements, biological significance of Na, K,
Mg, Ca, Fe, Co, Ni, Cu, Zn and chloride (Cl- ). Metalloporphyrins – hemoglobin,
structure and function, Chlorophyll, structure and role in photosynthesis.
V-SEMESTER- PAPER VI –ORGANIC CHEMISTRY
1. Nitrogen
compounds:
Amines
(Aliphatic and Aromatic): Nomenclature, Classification into 10, 20,
3OAmines and Quarternary ammonium compounds. Preparative methods -1.
Ammonolysis of alkyl halides 2. Gabriel synthesis 3. Hoffman’s bromamide
reaction (mechanism). 4. Reduction of Amides and Schmidt reaction. Physical
properties and basic character – Comparative basic strength of Ammonia, methyl
amine, dimethyl amine, trimethyl amine and aniline – comparative basic strength
of aniline, N-methylaniline and N,N-dimethyl aniline (in aqueous and
non-aqueous medium), steric effects and substituent effects. Use of amine salts
as phase transfer catalysts. Chemical properties: a) Alkylation b) Acylation c)
Carbylamine reaction d) Hinsberg separation e) Reaction with Nitrous acid of 10
, 20 , 30 (Aliphatic and aromatic amines).
2. Heterocyclic
Compounds :
Introduction
and definition: Simple 5 membered ring compounds with one hetero atom Ex.
Furan. Thiophene and pyrrole. Importance of ring system – presence in important
natural products like hemoglobin and chlorophyll. Numbering the ring systems as
per Greek letter and Numbers. Aromatic character – 6- electron system
(four-electrons from two double bonds and a pair of non-bonded electrons from
the hetero atom). Tendency to undergo substitution reactions. Resonance
structures: Indicating electron surplus carbons and electron deficient hetero
atom. Explanation of feebly acidic character of pyrrole, electrophillic
substitution at 2 or 5 position, Halogenation, Nitration and Sulphonation under
mild conditions. Reactivity of furan as 1,3-diene, Diels Alder reactions (one
example). Sulphonation of thiophene purification of Benzene obtained from coal
tar). Preparation of furan, Pyrrole and thiophene from 1,4,- dicarbonyl
compounds only, Paul-Knorr synthesis, structure of pyridine, Basicity –
Aromaticity – Comparison with pyrrole – one method of preparation and Chichibabin
Reaction.
3. Carboxylic acids
and derivative:
Nomenclature, classification and structure of
carboxylic acids. Methods of preparation by a) hydrolysis of nitriles, amides
and esters. b) carbonation of Grignard reagents. Special methods of preparation
of aromatic acids by a) oxidation of side chain. b) hydrolysis by
benzotrichlorides. c) Kolbe reaction. Physical properties: Hydrogen bonding,
dimeric association, acidity- strength of acids with examples of trimethyl
acetic acid and trichloroacetic acid. Relative differences in the acidities of
aromatic and aliphatic acids.
Chemical
properties: Reactions involving H, OH and COOH groups- salt formation,
anhydride formation, acid chloride formation, amide formation and
esterification. Degradation of carboxylic acids by Huns-Diecker reaction,
decarboxylation by Schimdt reaction, Arndt-Eistert synthesis, halogenation by
Hell-Volhard- Zelinsky reaction.
Derivatives of carboxylic acids: Reaction of
acid chlorides, acid anhydrides, acid amides, esters (mechanism of the
hydrolysis of esters by acids).
Active
methylene compounds Acetoacetic esters:
preparation by Claisen condensation, keto-enol tautomerism. Acid hydrolysis and
ketonic hydrolysis. Preparation of a) monocarboxylic acids.n-butyric acid &
Iso butyric acid b) dicarboxylic
acids.Succinic acid & Glutaric acid Reaction with urea Malonic ester:
preparation from acetic acid. Synthetic applications: Preparation of a)
monocarboxylic acids (propionic acid and n-butyric acid). b) dicarboxylic acids
(succinic acid and adipic acid). c) α,ß-unsaturated carboxylic acids (crotonic
acid). Reaction with urea.
4. Carbohydrates
:Monosaccharides: All discussion to be confined to (+) glucose as an in
support of ring structure. Evidence for cyclic structure of glucose (some
negative aldehydes tests and mutarotation). Cyclic structure of glucose.
Decomposition of cyclic structure (Pyranose structure, anomeric Carbon and
anomers). Proof for the ring size (methylation, hydrolysis and oxidation
reactions). Different ways of writing pyranose structure (Haworth formula and
chair conformationa formula).
Structure of fructose: Evidence of 2 –
ketohexose structure (formation of penta acetate, formation of cyanohydrin its
hydrolysis and reduction by HI to give 2-Carboxy-nhexane). Same osazone
formation from glucose and fructose,
cyclic structure for fructose (Furanose structure and Haworth formula).
Interconversion of Monosaccharides: Aldopentose to aldo hexose – eg: Arabinose
to DGlucose, D-Mannose (Kiliani - Fischer method). Epimers, Epimerisation –
Lobry de bruyn van Ekenstein rearrangement. Aldohexose to Aldopentose eg:
D-glucose to D- arabinose by Ruff’f degradation. Aldohexose (+) (glucose) to
ketohexose (-) (Fructose) and Ketohexose (fructose) to aldohexose (Glucose).
5. Amino acids and
proteins ;
Introduction: Definition of Amino acids, classification of Amino acids into
alpha, beta, and gama amino acids. Natural and essential amino acids –
definition and examples, classification of alpha amino acids into acidic, basic
and neutral amino acids with examples. Methods of synthesis: α- amino acids
from a) Haloginated Carboxylic acids b) Malonic ester synthesis c)Strecker’s
synthesis.(specific examples Glycin &Alanine.) Physical properties: Optical
activity of naturally occurring amino acids: L-configuration, irrespective of
sign rotation, Zwitterion structure – salt like character - solubility, melting
points, amphoteric character , definition of isoelectric point.
Chemical
properties: General reactions due to amino and carboxyl groups – lactams from
gamma and delta amino acids by heating
Peptide bond (amide linkage). Structure and nomenclature of peptides and
proteins.(Elementary treatment only)
III
B.Sc,VI SEMESTER PAPER- VII-
PHYSICAL CHEMISTRY
1.Chemical
kinetics :
Rate of reaction,. Definition of order and molecularity. Derivation of
Rate constants for first, second,
third and zero order reactions and examples. Derivation for half life equations. Methods to determine
the order of reactions. Effect of temperature on rate of reaction, Arrhenius
equation, concept of activation energy. Theories of reaction rates- collision
theory-derivation of rate constant for bimolecular reaction. The transition
state theory ( elementary treatment).
2.
Photochemistry : Differences between thermal and
photochemical processes. Laws of photochemistry- Grothus-Draper’s law and
Stark-Einstein’s law of photochemical
equivalence. Quantum yield. Ferri
oxalate actinometry. Photochemical hydrogen-chlorine hydrogen- bromine reaction. Jablonski diagram depicting various processes
occurring inthe excited state, qualitative description of fluorescence,
phosphorescence, non-radiative processes (internal conversion, intersystem crossing).
Photosensitized reactions- energy transferprocesses
(simple example).
3.
catalysis :
Homogenous and heterogeneous
catalysis, comparision with examples. Kinetic
of acid and base catalyzed reactions, - hydrolysis of an ester,
inversion of cane sugar,mutarortation of glucose. Theories of catalysis. acid –
base catalysis, enzyme catalysis and Autocatalysis Macromolecules: classification of polymers, chemistry of
polymerization chain polymerization,
step polymerization, coordination polymerization – tacticity Molecular
weight of polymers-number average and weight average molecular weight, degree
of polymerization, determination of molecular weight of polymers by viscometry,
end group analysis,. Preparation and industrial
application of Teflon, poly acrylonitrile,
terelene and Nylon-66.
4.
Thermodynamics : The first law of thermodynamics-statement,
definition of internal energyand
enthalpy. Heat capacities and their relationship. Joule-Thomson effect
co-efficient. Calculation of w, for the
expansion of perfect gas under isothermal and adiabatic conditions for
reversible processes. State function. Temperature dependence of enthalpy of
formation-Kirchoff’s equation. Second law of thermodynamics. Different
Statements of the law. Carnot cycle and its efficiency. Carnot theorem. Thermodynamic scale of temperature. Concept
ofentropy, entropy as a state function, entropy changes in reversible, and irreversible
processes. Calculation of entropy
changes with changes in V & T and
P&T. The Gibbs (G) and
Helmholtz (A) energies. Derivation of Gibb’s Helmholtz equation.
---------------------------------------------
VI
– SEMESTER-PAPER- VIII- GENERAL
CHEMISTRY
Unit – I
Physico Chemical methods of analysis
:
1. Separation techniques 1.Solvent extraction:
Principle and process, Batch extraction,continuous extraction and counter
current extraction. Application – Determination of Iron(III)
2..
Chromatography: Classification of
chromatography methods, principles of differential Migration absorption phenomenon, Nature of adsorbents, solvent systems, Rf values, factors
effecting Rf values.
(a).
Paper Chromatography: Principles, Rf values, experimental procedures, choice of
paper and solvent systems, developments
of chromatogram – ascending, descending and radial. Two dimensional chromatography, applications.
(b).
Thin layer Chromatography (TLC):
Advantages. Principles, factors effecting Rf values. Experimental procedures.
Adsorbents and solvents. Preparation of plates. Development of the
chromatogram. Detection of the spots. Applications.
(c) Column Chromatography: Principles, experimental procedures, Stationary and mobile phases,
Separation technique. Applications.
UNIT
- II 1. Spectrophotometry : General features of absorption – spectroscopy, Beer-Lambert’s law
and its limitations, transmittance, Absorbance, and molar absorptivity. Single
and double beam spectrophotometers. Application of Beer-Lambert law for
quantitative analysis of
1.
Chromium in K2Cr2O7 2.Manganese in KMnO4
UNIT
- III Molecular Spectroscopy :
i)
Mass Spectrometry: Basic principles – Molecular ion / parent ion,
fragment ions / daughter ions. Theory – formation of parent ions. Representation
of mass spectrum. Identification of parent ion, (M+1), (M+2), base peaks
(relative abundance 100%) Determination of molecular formula – Mass spectra of ethylbenzene, acetophenone,
n-butyl amine and 1- proponal.
(ii)
Electronic spectroscopy: Interaction of electromagnetic radiation with
molecules and types of molecular spectra. Potential energy curves for bonding
and antibonding molecular orbitals. Energy levels of molecules (σ,π, n) . Selection rules for
electronic spectra. Typesof electronic transitions in
molecules effect of conjugation. Concept of chromophore.
(iii)
Proton magnetic resonance spectroscopy (1H-NMR)Principles of nuclear
magnetic resonance, equivalent and non-equivalent protons, Position of signals.
Chemical shift, NMR splitting of signals – spin-spin coupling, coupling
Constants. Applications of NMR with
suitable examples – ethyl bromide, ethanol, acetaldehyde, 1,1,2 tribromo ethane, ethyl acetate, toluene and
acetophenone.
(iv)
Spectral interpretation Interpretation of 1H-NMR and mass spectral data of the
following compounds 1. Phenyl
acetylene 2. Acetophenone 3. Cinnamic Acid 4.p-nitro aniline
Unit
– IV -
Drugs & pesticides
A . Drugs :
Introduction: Drug, disease (definition), Historical
evolution, Sources – Plant, Animal synthetic, Biotechnology and human gene
therapy
1.Terminology: Pharmacy, Pharmacology, Pharma cophore, Pharmacodynamics,
2.Pharmacokinetics (ADME, Receptors – brief teartment) Metabolites and Anti- metabolites.
3. Nomenclature: Chemical name, Generic name
and trade names with examples.
4. Classification: Classification based on structures and
therapeutic activity with one example
each.
5.
Administration of Drugs
6. Synthesis: Synthesis and therapeutic activity of the
following drugs., L-Dopa, Chloroquin,
Ciprofloxacin
and Pencilline- G
7.HIV-AIDS: Immunity – CD-4 cells, CD-8 cells Retrovirus, replication in human body. Investigation
available, prevention of AIDS. Drugs available – examples with
structures: PIS: Indinavir (
Crixivan), Nelfinavir (Viracept), B . Pesticides
: Introduction to
pesticides – types – Insecticides, Fungicides, Herbicides,Weedicides, Rodenticides plant growth regulators,
Pheremones and Hormones. –examples,
Mention the Structure and uses of the following - Malathion,
Parathion, Endrin, Baygon.
LABORATORY COURSE –
V (Organic Chemistry)
1. Synthesis of Organic Compounds
i. Aromatic
electrophilic substitution Nitration: Preparation of nitro benzene .
ii. Diazotization
and coupling: Preparation of pheyl azo β-napthol
2. Organic Qualitative Analysis:
i. Identification of an organic
compound through the functional group analysis, determination
of melting point and preparation of
suitable derivatives. Alchols, Phenols, Aldehydes, Ketones,
Carboxylic acids, Aromatic Primary Amines,
Amides and Simple sugars
LABORATORY COURSE –
VI (Physical Chemistry))
1.
Chemical kinetics
i. Determination of specific
reaction rate of the hydrolysis of methyl acetate catalyzed by
hydrogen ion at room temperature.
2.
Distribution law
i. Determination of molecular status
and partition coefficient of benzoic acid in Benzene and
water.
3.
Electrochemistry
i. Determination of concentration of
HCl conductometrically using standard NaOH solution.
ii. Determination of redox potentials
of Fe2+/Fe3+ by potentiometric titration
of ferrous
ammonium sulphate vs. potassium
dichromate.
4. Adsorption
i. Surface tension and viscosity of
liquids.
ii. Adsorption of acetic acid on animal
charcoal, verification of Freundlich isotherm.
I BSC MODEL-QUESTIONPAPER
Duration:3hours
Maxmarks:70M
PART-A
Answer any Five questions. Each carries
four marks. 5x4=20M
1.
2.
3
4.
5.
6.
7.
8.
PART-B
Answer all the
questions. Each question carries ten
marks. 5x10=50M
UNIT-I
9 or10
UNIT-II
11or12
UNIT-III
13or14
UNIT-IV
15or16
UNIT-V
17or18
II &III BSC MODEL-QUESTIONPAPER
Duration:3hours
Maxmarks:70M
PART-A
Answer any six
questions. Each carries five marks. 6x5=30M
1.
2.
3
4.
5.
6.
7.
8.
PART-B
Answer all the
questions. Each question carries ten
marks.
4x10=40M
UNIT-I
9 or10
UNIT-II
11or12
UNIT-III
13or14
UNIT-IV
15or16
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