Curriculum(2016-2017)
Chemistry
course codes and Titles
YEAR
|
S.No
|
Course Code
|
Title of the Paper
|
Semester
|
2016-2017
|
1.
|
1112-A
|
Inorganic&Organic
chemistry
|
I
|
2.
|
2212-A
|
Physical&
General chemistry
|
II
|
|
3.
|
3312
|
Inorganic,Organic,Physical
and General chemistry
|
III
|
|
4.
|
4412
|
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
INORGANIC CHEMISTRY 30 hrs (2h / w)
p-block elements –I
15h
Group-13: Synthesis and
structure of diborane and higher boranes
(B4H10
and B5H9), boron-nitrogen
compounds (B3N3H6 and BN)
Group - 14: Preparation and
applications of silanes and silicone
Group - 15: Preparation and reactions
of hydrazine, hydroxylamine.
UNIT-II
Group -
16:
Classifications of oxides based on (i) Chemical behaviour and (ii) Oxygen
content.
Group-17: Inter halogen compounds and
pseudo halogens.
2.
Organometallic Chemistry 7h
Definition and
classification of Organometallic compounds, nomenclature, preparation,
properties and applications of alkyls of Li and Mg elements.
Structural theory in Organic
Chemistry 10 h
Types of bond fission and organic
reagents (Electrophilic, Nucleophilic, and free radical reagents including
neutral molecules like H2O,NH3& AlCl3).Bond
polarization : Factors influencing the polarization of covalent bonds, electro
negativity - inductive effect.
Application 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, and (b) acidity of carboxylic
acids. Hyper conjugation and its application to stability of carbonium ions,
Free radicals and alkenes, carbanions, carbenes and nitrenes.Types of Organic
reactions : Addition - electrophilic, nucleophilic and free radical.
Substitution - electrophilic, nucleophilic and free radical. Elimination-
Examples.
l. Acyclic Hydrocarbons
6 h
Alkenes - Preparation of alkenes.
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 (anti - Markonikov's addition
). Dienes - Types of dienes, reactions of conjugated dienes - 1,2 and 1,4
addition of HBr to 1,3 - butadiene and Diel's - Alder reaction.
Alkynes - Preparation by
dehydrohalogenation of dihalides, dehalogenation of tetrahalides, Properties;
Acidity of acetylenic hydrogen (formation of Metal acetylides). Preparation of
higher acetylenes, Metal ammonia reductions, Physical properties. Chemical
reactivity - electrophilic addition of X2, HX, H2O
(Tautomerism), Oxidation with KMnO4, OSO4, reduction and
Polymerisation reaction of acetylene.
2. Alicyclic hydrocarbons (Cycloalkanes)
4 h
Nomenclature, Preparation by Freunds
methods, heating dicarboxylic metal salts. Properties - reactivity of
cyclopropane and cyclobutane by comparing with alkanes, Stability of cycloalkanes
- Baeyer's strain theory, Sachse and Mohr predictions and Pitzer's strain
theory. Conformational structures of cyclobutane, cyclopentane, cyclohexane.
UNIT-V
Benzene and its
reactivity
10h
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), Huckel's rule - application to Benzenoid (Benzene, Naphthalene)
and Non - Benzenoid compounds (cyclopropenyl cation, cyclopentadienyl anion and
tropylium cation)Reactions - General 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 and deactivating groups with examples (Electronic
interpretation of various groups like NO2 and Phenolic). Orientation
of (i) Amino, methoxy and methyl groups (ii) Carboxy, nitro, nitrile, carbonyl
and sulphonic acid groups (iii) Halogens( Explanation by taking minimum of one
example from each type)
SEMESTER- II
Paper- II
(Physical & General Chemistry)
60 hrs (4 h / w)
PHYSICAL
CHEMISTRY
30 hrs (2h / w)
Solidstate
l0h
Symmetry in crystals. Law of constancy
of interfacial angles. The law of rationality of indices.wice indices, miller
indices. The law of symmetry. Definition of lattice point, space lattice, unit
cell. Bravis lattices and crystal systems. Bragg's law. Defects in crystals.
Stoichiometric and non-stoichiometric defects. And Applications.
1.Gaseous state 6
h
Compression factors, deviation of real
gases from ideal behavior. Vander Waal's equation of state. P-V Isotherms of
real gases, Andrew's isotherms of carbon dioxide, continuity of state. Critical
phenomena. The vander Waal's equation and the critical state. Law of
corresponding states.Relationship between critical constants and vander Waal's
constants. Joule Thomson effect.
2.Liquid
state 4
h
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/liquid. Application of liquid crystals as LCD devices.
Solutions
l0h
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, trimethylamine-water,
nicotine-water systems. Effect of impurity on consulate temperature. Immiscible
liquids and steam distillation.Nernst distribution law. Calculation of the
partition coefficient. Applications of distribution law.
GENERAL CHEMISTRY
30 hrs (2h / w)
l.Surface chemistry
8 h
Definition of colloids. Solids in
liquids(sols), preparation, purification, properties - kinetic, optical,
electrical. Stability of colloids, Hardy-Schulze law, protective
colloid.Liquids in liquids (emulsions) preparation, properties, uses. Liquids
in solids (gels) preparation, uses.Adsorption: Physical adsorption,
chemisorption. Freundlisch, Langmuir adsorption isotherms. Applications of
adsorption
Valence bond
theory, hybridization, VB theory as applied toClF3, Ni (CO)4, Molecular orbital
theory - LCAO method,
construction of M.O. diagrams for homo-nuclear and hetero-nuclear diatomic
molecules (N2, O2, CO and NO).
Stereochemistry of carbon
compounds
15 h
Molecular representations- Wedge,
Fischer, Newman and Saw-Horse formulae. Optical isomerism: Optical activity-
wave nature of light, plane polarised light, optical rotation and specific
rotation. Chiral molecules- definition and criteria(Symmetry elements)-
Definition of enantiomers and diastereomers – Explanation of optical isomerism
with examples Glyceraldehyde, Lactic acid, Alanine, Tartaric acid,
2,3-dibromopentane. D,L and R,S configuration methods and E,Z- configuration with examples.
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-III PHYSICAL CHEMISTRY-II
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.
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-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.
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.
LABORATORY
COURSE-III
Practical-II (At the end of
Semester-III) 30 hrs (2 h / w)
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
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 Five
questions. Each carries Six marks. 5x6=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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