CH.S.D.ST.THERESA’S AUTONOMOUS DEGREE
COLLEGE FOR WOMEN, ELURU
I BSC I SEMESTER CHEMISTRY PAPER I SYLLABUS 2017-18
TITLE:
INORGANIC & PHYSICAL CHEMISTRY
UNIT-I
P – Block elements: General Characteristics of elements of groups 13, 14,
15
Group – 13: Synthesis and
structure of diborane and higher boranes (B4H10 and B5H9),
boran – nitrogen compounds (B3N3H6 and BN)
Group – 14: Preparation
and applications of silanes and silicones.
Group – 15: Preparation and reactions of hydrazine, hydroxylamine.
UNIT-II
1.P – Block elements: General Characteristics of elements of groups 16 and
17
Group – 16: Classification of oxides based on (i) chemical
behaviour and (ii) oxygen content.
Group – 17: Inter halogen compounds and pseudo halogens.
2.Organometallic Chemistry: Definition and classification of organometallic
compounds, nomenclature, preparation, properties and applications of alkyls of Li
and Mg elements.
Physical Chemistry
UNIT-III
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
systems. X-ray diffraction and crystal structure. Bragg’s law.
Determination of crystal structure by Bragg`s method and the powder method,
indexing of planes and structure of 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 photoelectrochemical cells.
UNIT-IV
1.Gaseous state: Compression factors, deviation of real gases from
ideal behaviour. Van der Waal’s equation of state. PV-Isotherms of real gases.
Andrew’s isotherms carbondioxide, Continuity of state, critical phenomena. The
Van der Waal’s equation and the critical state. Relationship between critical
constants and Van der Waal’s constants. Joule Thomson’s effect. Liquefaction of
gases – i) Linde‘s method ii) Claude’s methods
2.Liquid state: Inter molecular 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
/liquid. Application of liquid crystals
as LCD devices.
UNIT-V
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,
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.
I BSC II SEMESTER CHEMISTRY PAPER II SYLLABUS
2017-18
TITLE:
ORGANIC & GENERAL CHEMISTRY
UNIT-I
Structural theory in Organic Chemistry: 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, electronegativity- 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.
Types of Organic reactions: Addition
electrophilic, nucleophilic and free radical.
Substitution – electrophilic, nucleophilic and free radical. Elimination – Examples (mechanism not
required).
UNIT-II
1.Acyclic Hydrocarbons:
Alkenes – Preparation of alkenes (a) by dehydration of
alcohols (b) by dehydrohalogenation of alkyl halides (c) by dehalogenation of
1, 2 dihalides , Saytzey’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, and H2SO4 with
mechanism and addition of HBr in the presence of peroxide (anti-Markonikov’s
addition). Oxidation – hydroxylation by
KMnO4, OsO4, peracids (via epoxidation) hydroboration
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):
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-III
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), Huckel’s rule –
application to Benzenoid (Benzene, Napthalene) 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 (reactions only).
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).
GENERAL
CHEMISTRY
UNIT-IV
Surface chemistry: 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.
2. Chemical
Bonding: Valence bond theory, hybridization, VB theory as applied
to ClF3, Ni(CO)4, Dipole moment- Orientation of dipoles
in an electric field, Dipole moment, induced dipole moment, dipole moment and
structure of molecules. Molecular orbital theory – LCAO method, construction of
M.O.diagrams for homo-nuclear and hetero – nuclear diatomic molecules (N2,
O2, CO and NO).
UNIT-V
Stereochemistry
of carbon compounds: Molecular representations – Molecular
representations - Wedge, Fisher, Newman and Saw – Horse formulae. Stereoisomerism, Stereoisomers: 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 symmetry – asymmetric
and dissymmetric molecules. Examples of
asymmetric molecules (Glyceraldehydes, Lactic acid, Alanine) and dissymmetric
molecules (Trans – 1, 2-dichloro cyclopropane).
Chiral
centers: definition – molecules with
similar chiral carbon (Tartaric acid), definition of mesomers – molecules with
dissimilar chiral carbons (2, 3-dibromopentane). Number of enantiomers and mesomers –
calculation. D, L and R,S configuration
for asymmetric and dissymmetric molecules.
Cahn – Ingold – Prelog rules.
Racemic mixture – racemisation and resolution techniques.
Diastereomers: definition –
geometrical isomerism with reference to alkenes – cis, Trans, and E-Z
configuration
II BSC III SEMESTER CHEMISTRY PAPER III SYLLABUS 2017-18
TITLE: SPECTROSCOPY & ORGANIC CHEMISTRY
SPECTROSCOPY 30 hrs (2h / w)
UNIT-I 6h
General features of
absorption - 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 Manganous sulphate
Electronic spectroscopy: 8h
Interaction of
electromagnetic radiation with molecules and types of molecular spectra. Energy
levels of molecular orbitals (σ, π, n). Selection rules for electronic spectra.
Types of electronic transitions in molecules effect of conjugation. Concept of
chromophore and auxochrome.
UNIT-II
Infra red spectroscopy 8h
Different
Regions in Infrared radiations. Modes of vibrations in diatomic and polyatomic molecules. Characteristic
absorption bands of various functional groups. Interpretation of
spectra-Alkanes, Aromatic, Alcohols carbonyls, and amines with one example to
each.
Proton magnetic resonance spectroscopy (1H-NMR) 8h
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.
ORGANIC CHEMISTRY
UNIT-III
1.Halogen Compounds: Nomenclature and classification of alkyl (into
primary, secondary, tertiary,), aryl, aralkyl, allyl, vinyl, benzyl halides. Chemical reactivity – formation of RMgX. Nucleophilic substitution reaction – classification into SN1
and SN2. Mechanism and
energy profile diagrams of SN1 and SN2 reactions. Stereo chemistry of SN2 (Walden
inversion), SN1 (Racemisation) explanation of both by taking the
example of optically active alkyl halide – 2 - bromobutane. Ease of hydrolysis – comparison of allyl,
benzyl, alkyl, vinyl and aryl halides.
2.Hydroxy
Compounds: Nomenclature and
classification of hydroxyl compounds, Alcohols: Preparation with hydroboration
reaction, Grignard synthesis of alcohols. Phenols: Preparation (a) from
diazoniumsalts (b) from arylsulphonates (c) from cumene. Physical properties: – Hydrogen bonding
(inter molecular and intra molecular) effect of hydrogen bonding on boiling
point and water solubility. Chemical properties: – (a) Acidic nature of phenols
(b) Formation of alkoxide/ phenoxides and their reaction with RX (c)
Replacement of OH by X using PCl5, PCl3 , PBr3,
SOCl2 and with HX/ZnCl2.(d)Esterificaion by acids
(mechanism) ,(e) Dehydration of alcohols.(f)Oxidation of alcohols by CrO3,
KMnO4.(g)Special reactions of phenols – (a) Bromination, (b) Kolbe –
Schmidt reaction, (c) Riemer Tiemann (d)
Fries rearrangement (e) Azocoupling. Identification of alcohols by oxidation –
KMnO4, Cericammonium nitrate – Lucas reagent; phenols by reaction
with FeCl3, Polyhydroxy compounds – Pinacol – pinacolone
rearrangement.
UNIT-IV
Carbonyl
Compounds:Nomenclature of aliphatic
and aromatic carbonyl compounds, structure of carbonyl group. Synthesis of
aldehydes and ketones from acid chloride by using 1, 3 – dithianes, nitriles
and from carboxylic acids.
Physical
properties: Absence of hydrogen
bonding, keto-enol tautomerism, reactivity of carbonyl group in aldehydes and
ketones. Nucleophilic addition reactions with (a) NaHSO3 (b) HCN (c)
RMgX (d) NH2OH (e) PhNHNH2
(f) 2,4 – DNP (g) alcohols formation of hemiacetols and acetols
(h)halogenations using PCl5 with mechanism. Base catalyzed reactions
with mechanism: (a) Aldol (b) Cannizaro reaction (c) Perkin reaction (d)
Benzoin condensation (e) Halo form reaction (f) Knoevenagel reaction.
Oxidation
of aldehyde Bayer-Villiger oxidation of ketones.
Reduction
without mechanism:(a) Clemmensen reduction (b)Wolf-Kushner reduction (c)MPV
reduction (d)LiAlH4 and NaBH4
Analysis
of aldehydes and ketones with (a) 2,4 DNP test (b)Tollen’s test (c)Fehling’s
test (d) Schiff test (e) Halo form test
(with equations).
UNIT-V
1.Carboxylic Acids and Derivatives: 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 the side chain. (b) Hydrolysis by benzotricholorides. (c) Kolbe
reaction.
Physical properties:- hydrogen bonding, dimeric association, acidity- strength of acids with
the examples of trimethyl acetic acid and trichloro acetic 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 (mechanism).
Degradation
of carboxylic acids by Huns-Diecker reaction, decarboxylation by Schimdt
reaction, Arndt-Eistert synthesis, halogenations 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 and bases).
2.Active methylene compounds:
Acetoacetic esters: Preparation by Claisen condensation, keto-enol
tautomerism. Acid hydrolysis and ketonic
hydrolysis. Preparation of
a) monocarboxylic acids
b) dicarboxylic acids. 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, β - unsaturated carboxylic acids (crotonic acids)
Reaction with urea
II BSC IV SEMESTER CHEMISTRY PAPER IV SYLLABUS 2017-18
TITLE:
INORGANIC & PHYSICAL CHEMISTRY
UNIT-I
1.Chemistry of d-block elements: Characteristics of d-block elements with special
reference to electronic configuration, colour, variable valence, magnetic
properties, catalytic properties and ability to form complexes. Comparative
treatment of second and third transition 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
1.Metal carbonyls and related compounds:
EAN rule, classification of metal
carbonyls, structures and shapes of metal carbonyls of V, Cr, Mn, Fe, Co and
Ni.
2.Chemistry of f-block elements:
Chemistry
of lanthanides – electronic structure, oxidation states, lanthanide
contraction, consequences of lanthanide contraction, magnetic properties, separation of lanthanides by ion exchange and
solvent extraction methods.
Chemistry
of actinides – electronic configuration, oxidation states, actinide
contraction, position of actinides in the periodic table, comparison with
lanthanides in terms of magnetic properties.
PHYSICAL CHEMISTRY
UNIT-III
Dilute solutions: Colligate properties, Raoult’s law, relative lowering
of vapour pressure (Ostwald and Walker’s method), its relation to molecular
weight of non-volatile solute. Elevation
of boiling point and depression of freezing point. Experimental determination of Elevation in
boiling point (Cottrel’s method) and depression in freezing point (Beckmann’s
method), Derivation of its(Elevation of boiling point and depression of
freezing point) relation to molecular weight of non-volatile solute. Osmosis, osmotic pressure, Experimental
determination of osmotic pressure (Berkeley-Hartley method). Theory of dilute solutions. Determination of molecular weight of
non-volatile solute from osmotic pressure.
Abnormal Colligative properties.
UNIT-IV
Electrochemistry
- I: specific conductance, equivalent
conductance, measurement of equivalent conductance, variation of specific and
equivalent conductance with dilution. Migration of ions and Kohlrausch’s law,
Arrhenius theory of electrolytic dissociation and its limitations, Ostwald’s
dilution law. Debye-Huckel- Onsagar’s equations for strong electrolytes
(elementary treatment only). Transport number, definition and determination by
Hittorf method.
Applications
of conductivity measurements: Determination dissociation constant ( Ka
)of acid, determination of solubility product of sparingly soluble salt,
conductometric titrations. Types of reversible electrodes – gas electrode,
Metal – metal ion, metal – insoluble salt and redox electrodes. Electrode
reactions, Nernst equation, single
electrode potential.
UNIT-V
1.Electrochemistry
-II
Standard
Hydrogen electrode- reference electrodes – standard electrode potential, sign
conventions, electrochemical series and its significance. Revesible and
Irrevesible cells, conventional representation of electrochemical cell . EMF of
a cell and its measurements. Computation of cell EMF. Applications of EMF
measurements – potentiometric titrations.
2.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 – NaCl - Water system.
Freezing mixtures.
III BSC V SEMESTER CHEMISTRY PAPER V SYLLABUS 2017-18
TITLE:
INORGANIC, ORGANIC & PHYSICAL CHEMISTRY
Part – A (Inorganic chemistry)
UNIT-I
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 square planar and
6-octahedral and its limitations, crystal field theory, splitting of d-
orbital in octahedral, tetrahedral and square 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,
stereochemistry of complexes with 4 and 6 coordination numbers.
UNIT-II
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.
Stability of metal complexes: Thermodynamic stability and kinetic stability,
factors affecting the stability of metal complexes, chelate effect.
Determination of composition of complex by Jobs method and mole ratio method.
Part – B (Organic Chemistry)
UNIT-III
1. Nitro hydrocarbons: Nomenclature and classification – nitro hydrocarbons
– structure. Tautomerism of nitro alkanes leading to aci and keto form. Preparation
of nitro alkanes. Reactivity – halogenations, reaction with HONO (Nitrous
acid), Nef reaction and Mannich reaction leading to Michael addition and
reduction.
Nitrogen Compounds Amines (Aliphatic and aromatic) Nomenclature,
classification into 10, 20, 30 Amines and
quaternary ammonium compounds. Preparative methods – 1. Ammonolysis of alkyl
halides 2. Gabriel synthesis 3. Hoffmann’s bromamide reaction (mechanism).
Reduction of amides & Schmidt reaction. Physical properties and basic
character – comparative basic strength of Ammonia, methyl amine, dimethyl
amine, trimethyl amine and aniline, N – methyl aniline 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)
Carbylaminereaction (d) Hinsbergseparation (5) Reaction with nitrous acid of 1o,
2º, 3º (Aliphatic and aromatic amines). Electrophilic substitutions of Aromatic
amines – Bromination and Nitration.
Oxidation of aryl and 3o Amines, Diazotisation. Cyanides and
Isocyanides: Nomenclature (aliphatic and aromatic) structure preparation of
cyanides from (a) Alkyl halides (b) from amides (c) from aldoximes. Preparation
of isocyanides from Alkyl halides and Amines.
Properties of cyanides and isocyanides (a) hydrolysis (b) addition of
Grignard reagent (iii) Reduction (IV) Oxidation.
UNIT-IV
2.Heterocyclic Compounds: Introduction and definition: Simple five membered ring
compounds with one Hetero atom ex. Furan, Thiophene and Pyrrole. 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. Electrophilic
substitution reactions at 2 or 5 positions, Halogenation, nitration and
sulphonation under mild conditions, reactivity of furan as 1, 3-diene, Diels
Alder reaction (one example). Preparation of Furan, Thiophene and Pyrrole from
1, 4 dicarbonyl compounds only. Paul-
knorr synthesis, structure of pyridine, basicity – aromaticity- comparison with
pyrrole- one method of preparation and properties- reactivity towards nucleophilic substitution
reactions- Chichibabin reaction.
Part – C Physical Chemistry
UNIT-V
1.Chemical Kinetics: Rate of a reaction, factors influencing the rate of a
reaction-concentration, temperature, light and catalyst. Definition of order and molecularity. Derivation of rate constants for first,
second, third and zero order reactions and examples. Derivation for time of half change. Methods to determine the order of
reactions. Effect of temperature on rate
of reaction. Arrhenius equation, concept
of activation energy.
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. Photochemical hydrogen –
chlorine, hydrogen – bromine reactions. Qualitative description of
fluorescence, phosphorescence, Photosensitised reactions- Energy transfer
processes (simple example).
III BSC V SEMESTER CHEMISTRY PAPER VI SYLLABUS 2017-18
TITLE:
INORGANIC, ORGANIC & PHYSICAL CHEMISTRY
UNIT- I
1.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 Tran’s effect.
2.Bioinorganic
Chemistry: Essential elements, Biological significance of Na, K, Mg, Ca, Fe,
Co, Ni, Cu, Zn, and Cl-1.
Metalloporphyrins with emphasis on hemoglobin-structure and function.
Chlorophyll -structure and role in photosynthesis.
ORGANIC CHEMISTRY
UNIT-II
1.Carbohydrates: Introduction-Classification and nomenclature –
classification into mono, oligo and polysaccharides into pentoses, hexoses etc.
into aldoses and ketoses. Mono saccharides. All discussions to be confined to
(+) glucose as an example aldohexose and (-) fructose as example of
ketohexoses. Chemical properties and structural elucidation. Evidences for
straight chain penta hydroxy aldehyde structure (Acetylation, reduction to
n-hexane, cyanohydrin formation, reduction of Tollen’s and Fehling’s reagents
and oxidation to gluconic and saccharic acids). Number of optically active
isomers possible for the structure, configuration of glucose based on D –
glyceraldehydes as primary standard (No proof for configuration is required).
Evidence for cyclic structure of glucose (some negative aldehyde tests and
mutarotation). Cyclic structure of Glucose: Proposition 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 chain
conformational formula). Structure of fructose. Evidence of 2-keto hexose
structure (formation of Penta acetate, formation of cyanohydrin, its hydrolysis
and reduction by HI to give 2-carboxy-n-hexane) same osazone formation from
glucose and fructose, Hydrogen bonding in osazones, cyclic structure for
fructose (Furanose-structure and Haworth formula). Interconversion of
monosaccharides: aldopentose to aldohexose e.g. Arabinose to D-glucose,
D-mannose. (Kiliani-Fischer method). Epimers, Epimerisation – Lobry De Bruynvan
Ekenstein rearrangement – Aldohexose-Aldopentose e.g. D-glucose to D-Arabinose
by Ruff’s degradation. Aldohexose (+) glucose to Ketohexose (-) Fructose and
Ketohexose (Fructose) to Aldohexose (Glucose).
UNIT-III
2.Amino acids and Proteins
Introduction: Definition of amino
acids, classification of amino acids into alpha beta and gamma 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: general methods of synthesis of alpha amino acids
(specific examples-glycine, alanine, valine and leucine) by following methods:
(a) From halogenated carboxylic acids (b) Malonic ester synthesis (c)
Strecker’s synthesis. Physical
properties: Optical activity of naturally occurring amino acids:
L-Configuration irrespective of sign rotation, zwitter ion 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).
PHYSICAL CHEMISTRY
UNIT-IV
Thermodynamics I: The first law of thermodynamics – statement,
definition of internal energy and enthalpy.
Heat capacities and their relationship.
Joule Thomson effect – Joule-Thomson coefficient. Calculation of W for the expansion of perfect gas under
isothermal and adiabatic conditions for reversible process. State function. Temperature dependence of
enthalpy of formation – Kirchoff’s equation.
UNIT – V
Thermodynamics II: Second law of Thermodynamics: different statements of the law. Carnot’s cycle and its efficiency, Carnot’s
Theorem. Concept of entropy, entropy as a state function, entropy changes in
reversible, and irreversible processes.
Entropy changes in spontaneous and equilibrium processes.
III BSC VI SEMESTER CHEMISTRY
ELECTIVE
PAPER VII SYLLABUS 2017-18
TITLE: GREEN
CHEMISTRY
UNIT-I 10h
Green Chemistry: Introduction- Definition of green Chemistry, need of
green chemistry, basic principles of green chemistry. Green synthesis-
Evalution of the type of the reaction i)
Rearrangements (100% atom economic), ii) Addition reaction (100% atom
economic). Organic reactions by Sonication method: apparatus required examples
of sonochemical reactions (Heck, Hundsdiecker and Wittig reactions).
UNIT-II 10h
Selection of solvent:i) Aqueous phase reactions ii) Reactions in ionic liquids,
Heckreaction, Suzuki reactions,
epoxidation. iii) Solid supported synthesis
Super critical CO2: Preparation, properties and
applications, (decaffeination, dry cleaning)
UNIT-III 10h
Microwave and Ultrasound assisted green synthesis: Apparatus required, examples of
MAOS (synthesis of fused anthro quinones, Leukart reductive amination of ketones)
- Advantages and disadvantages of MAOS. Aldol condensation-Cannizzaro
reaction-Diels-Alder reactions-Strecker's synthesis
UNIT-IV
5h
Green catalysis: Heterogeneous catalysis, use of
zeolites, silica, alumina, supported catalysis- biocatalysis: Enzymes, microbes
Phase transfer catalysis (micellar/surfactant)
UNIT V 10h
Examples
of green synthesis / reactions and some real world cases: 1. Green synthesis of
the following compounds: adipic acid , catechol , disodium imino di acetate
(alternative Strecker’s synthesis) 2. Microwave assisted reaction in water –
Hoffmann elimination – methyl benzoate to benzoic acid – oxidation of toluene
and alcohols – microwave assisted reactions in organic solvents. Diels-Alder
reactions and decarboxylation reaction. 3. Ultrasound assisted reactions –
sonochemical Simmons –Smith reaction(ultrasonic alternative to iodine)
LABORATORY
COURSE – VII
Practical Paper – Elective VII C (at the
end of semester VI) 30 hrs
(2 h/W)
1. Determination of specific reaction
rate of hydrolysis for methyl acetate catalysed
by hydrogen ion at room temperature.
by hydrogen ion at room temperature.
2.Determination of molecular status and partition
coefficient of benzoicacidin
Benzene
and water.
3.Surface
tension and viscosity of liquids.
4. Adsorption of
acetic acid on animal charcoal, verification of Freundlisch
isotherm.
III BSC VI SEMESTER CHEMISTRY
CLUSTER ELECTIVE PAPER VIII SYLLABUS 2017-18
TITLE: ORGANIC SPECTROSCOPIC TECHNIQUES
UNIT-I 10h
NUCLEAR MAGNETIC RESONANCE SPECTROSCOPY
Nuclear spin, Principles of
NMR-Classical and Quantum Mechanical methods, Magnetic moment and Spin angular
momentum. Larmour Frequency. Instrumentation. Relaxation-spin-spin & spin
lattice relaxation. Shielding constants, Chemical shifts, Shielding and
Deshielding mechanism-Factors influencing Chemical shift. Spin-Spin
interactions-AX, AX2 and AB types. Vicinal, Geminal and Long range
coupling- Factors influencing coupling constants.
UNIT – II 5h
Spin decoupling, Spin tickling,
Deuterium exchange, Chemical shift reagents and Nuclear overhauser effect.
Applications in Medical diagnostics, Reaction kinetics and Mechanically induced
dynamic nuclear polarization. FT NMR and its Advantages.
UNIT-III 10h
UV & VISIBLE SPECTROSCOPY
Electronic spectra of diatomic
molecules. The Born-oppenheimer approximation. Vibrational coarse structure:
Bond association and Bond sequence. Intensity of Vibrational-electronic
spectra: The Franck-Condon principle. Rotational fine structure of electronic
vibration transitions. Electronic structure of diatomic molecules.
Types
of transitions, Chromophores, Conjugated dienes, trienes and polyenes,
unsaturated carbonyl compounds-Woodward – Fieser rules.
UNIT – IV 10h
Analysis of Milk
and milk products: Acidity, total
solids, fat, total nitrogen, protenines,lactose, phosphate activity, casein,
choride. Analysis of food materials-
Preservatives: Sodium carbonate, sodium benzoate sorbic acid Coloring matters, - Briliant blue FCF, fast green FCF,
tertrazine, erytrhosine , sunset yellow FCF.
Flavoring agents
- Vanilla , diacetyl, isoamyl acetate, limonene, ethylpropionate , allyl
hexanoate and Adulterants in rice and
wheat, wheat floo0r, sago,coconut oil, coffee powder, tea powder, milk..
UNIT – V 10h
Clinical
analysis of blood:Composition of blood,clinical analysis,trace elements in the body.Estimation of
blood
chlolesterol,glucose,enzymes,RBC& WBC ,Blood gas analyser.
III BSC VI SEMESTER CHEMISTRY
CLUSTER ELECTIVE PAPER IX SYLLABUS 2017-18
TITLE: ADVANCED
ORGANIC REACTIONS
UNIT – I
ORGANIC PHOTOCHEMISTRY
Organic
photochemistry : Molecular orbitals, carbonyl chromophore–triplet states,
Jablonski diagram, inter–system crossing.
Energy transfer. Energies
properties and reaction of singlet and triplet states of and transitions.
Photochemical reactions : (a) Photoreduction, mechanism, influence of
temperature, solvent, nature of hydrogen donors, structure of substrates on the
course of photo reduction,.
UNIT – II
ORGNAIC PHOTOCHEMISTRY
Norrisch
cleavages, type I : Mechanism, acyclic cyclicdiones, influence of sensitizer,
photo Fries rearrangement. Norrisch type
II cleavage : Mechanism and stereochemistry, type II reactions of esters : 1: 2
diketones, photo decarboxylation., Di - π methane rearrangement, Photochemistry
– of conjugated dienes, Decomposition of nitrites – Barton reaction.
UNIT – III
PROTECTING GROUPS AND ORGANIC REACTIONS
Principles
of (1) Protection of alcohols – ether formation including silyl ethers – ester
formation, (2) Protection of diols – acetal,ketal and carbonate formation, (3)
Protection of carboxylic acids – ester formation, benzyl and t–butyl esters,
(4) Protection of amines – acetylation, benzoylation, benzyloxy carbonyl,
triphenyl methyl groups and fmoc, (5) Protection of carbonyl groups – acetal,
ketal, 1,2–glycols and 1,2–dithioglycols formation.
UNIT – IV
Synthetic
reactions : Mannich reaction – Mannich bases – Robinson annulations. The Shapiro reaction, Stork–enamine reaction.
Use of dithioacetals – Umpolung, phase transfercatalysis – mechanisms and use
of benzyl trialkyl ammonium halides.
Witting reaction.
UNIT –V : NEW SYNTHETIC REACTIONS
Baylis–Hillman
reaction, RCM olefm metathesis, Grubb catalyst, Mukayama aldol reaction,
Mitsunobu reaction, McMurrey reaction, Julia–Lythgoe olefination, and Peterson’s
stereoselective olefination, Heck reaction, Suziki coupling, Stille coupling
and Sonogishira coupling, Buchwald–Hartwig coupling. Ugi reaction, Click reaction.
III BSC VI SEMESTER CHEMISTRY
CLUSTER ELECTIVE PAPER X SYLLABUS 2017-18
TITLE: PHARMACEUTICAL
AND MEDICINAL CHEMISTRY
UNIT-I 8h
Pharmaceutical
chemistryTerminology: Pharmacy, Pharmacology, Pharmacophore,
Pharmacodynamics, Pharmacokinetics (ADME, Receptors - brief treartment)
Metabolites and Anti metabolites.
UNIT-II
Drugs: 8h
Nomenclature: Chemical name, Generic
name and trade names with examples Classification: Classification based on structures
and therapeutic activity with one example each, Administration of drugs
UNIT-III
Synthesis and therapeutic activity of
the compounds: 12h
a.
Chemotheraputic Drugs
l.Sulphadrugs(Sulphamethoxazole)
2.Antibiotics - β-Lactam Antibiotics, Macrolide Antibiotics, 3. Anti malarial
Drugs(chloroquine)
b. Psycho
therapeutic Drugs:
1.Anti pyretics(Paracetamol)
2.Hypnotics, 3.Tranquilizers(Diazepam) 4.Levodopa
UNIT-IV
Pharmacodynamic Drugs:
8h
1. Antiasthma Drugs (Solbutamol) 3.
Antianginals (Glycerol Trinitrate)
UNIT-V
HIV-AIDS: 9h
Immunity - CD-4cells, CD-8cells, Retro virus, Replication in human body,
Investigation available, prevention of AIDS, Drugs available - examples with structures: PIS: Indivanir (crixivan),
Nelfinavir(Viracept).
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