II SEMESTER
Paper2.1; Biochemistry-II
1. Introduction 6h
IUPAC nomenclature of organic compounds including bifunctional
ones. Detection and principals of
estimation of C<H<N halogens, S and P in organic
compounds. Inductive effect, reasonance and
hyperconjugation concepts. Reactive intermediates curbocations,
carbanions, carbines and free
radicals.
2. Hydrocarbons
4h
Mechanism of additional of HCL to proper.Markovnikov’s rule. I croxide effect Alkenes –
ozonolysis
and oxization. Alkenes formation of acetylides and then importance.
Dienes:Types with examples.
Conjugate dienes. 1,3 Butadiene –Stability, Mechanism of
addition of HBr. Conformational analysis of
ethane and n-butane.
3. Cycloalkanes 2h
Reactivates and relative stabilities. Baeyer strain theory.
Sachse-Mohr theory. Boat and chair forms of
cycloalkane. Axial and equatorial bonds.
4. Arenes 6h
Modern concept of structure of Benzene – Assuming Kekule’s
structure, Benzene structure according
to resonance and molecular orbital theory. Aromaticity and
aromaticity, 4n+2 rule for cycle
compounds. Nitration and Friedel Craft’s Alkylation (no
acetylation). Electronic interpretation of
orienting influence of substitutents in the electrophilicv
substitution of toluene, chlorobenzene and
nitrobenzene. Structures (inclusive of resonance structures) of
napthalene, anthracene, phenanthrene
and diphenyl (no elucidation of structures required). Oxidation
reactionof naphthalence to
naphthoquinone, phthalic anhydride and phthalic acid.
5. Alkyl halides and Organometallic compounds 3h
Alkyl halides- definition with examples, Comparison of primary,
secondary and tertiary alkyl halides
with reference to SN1 and SN2 mechanisms. Mechanistic concepts
of elimination (E1,E2) reactions- tbuty1
chloride and n-buty1 chloride as examples. Organometallic
compounds- definitation and
examples–(preparations not required) and synthetic applications
of Grignard Reagents.
6. Alcohols 3h
Definition and classification. Monohydric alcohols-general
properties – distinguishing reactions of
primary, secondary and tertiary alcohols – Lucas Test, Victor
Meyer Test, and Oxidation with
reactions. Dihydric alcohols-glycol-structure and uses.
Preparations and properties not required.
Trihydric alcohol – Glycerol- synthesis from propene.
Properties-oxidation, nitration and esterification
reactions uses of glycerol.
7. Phenols 2h
Definition and classification with structures and examples.
Electronic interpretation of acidity of
phenol. Mechanisms of Kolber’s Reimer-Tiemann reactions.
Bromination reaction without mechanism.
8. Carbonyl Compounds 4
5h
Definition and examples. General properties with list of
reactions-additions of alcohols to aldehydes
and ketones. Ketoenol tautomerism. Mechanism: addition of HCN to
acetaldehyde, Claisen and aldol
condensation. Quinones, o-and p-benzoquinones-structures and
properties.
9. Gases 3h
Postulates of Kinetic Theory of Gases. Maxwell – Boltzmann
distribution law of velocities. Van der
Waals equation with terms, no derivation required. Virial
Equation with terms, no derivation required.
Critical phenomena and determination of critical constants.
10. Solids 4h
Types-Crystalline and Amorphous. Size and Shapes. Elements of
symmetry. Law of Rational Indices
and Miller Indices with simple numericals. Definitipon of Space
Lattice and Until cell. Crystal systems
with examples.
11. Phase Rule 2h
Statement, terminology and criterion of phase equilibrium.
Application of phase rule to two
component system of liquid –Water-Phenol System. Partition
coefficient of l2 between Carbontetra chloride and water . No numericals.
required.
12.Chemical Equilibrium
4h
Reversible reactions with examples. Chemical equilibrium –
definition and characteristic.
Homogenous and heterogeneous systems with examples. Redox
equilibria with example-Fe2+ Fe3+
System.
13. Reaction Kinetics
5h
Rate equation, Velocity constant-molecularity and order of a
reaction – definitions with examples –
decomposition of PCI5 and HI, synthesis of NH3 and SO3. Factors
influencing rate of reaction –
temperature, pressure, concentration and catalyst. Kinetic
Equation of zero (k=x/1), first and second
order-No derivations required. Expression of second order
kinetics-(a=b and ab).Arrhenius hypothesis
5
–equation and its terms only. Activated complex and energy of
activation and its terms. Elementary
treatment of transition state theory (Graphical representation
to be given) Catalysis – characteristics of
of catalyst. Types of catalyst-Homo and hetero catalystswith
definition and examples. Homogeneous
examples-Invertase, SO3 formation with nitric oxide.
Heterogenous examples – Haber’s Process with
Fe, and contact process with Pt. Theory of homogenous
catalysis-intermediate compound formation
theory (No mechanisms required) pH dependence of catalyzed
reaction –Graphical representation and
its example Pepsin. Enzymes as catalysts- simple
enzymes-Chymotrypsin, Pepsin, Trypsin. Conjugated
Enzymes-Cytochromes.
14. Theromdynamics 6h
Different Statement of first and second laws of thermodynamics.
Definition of free energy, free energy
change, entrophy, chemical potential, standard free energy
change of chemical reaction, exergonic and
endergonic reactions with examples. Relationship between free
energy change and equilibrium
constant.
II SEMESTER
BIOCHEMISTRY PRACTICAL.
1. Determination of Densitys and Viscosity of the given organic
liquid.
2. Determination of Density and Surface tension of the given
liquid.
3. Partition coefficient of iodine between carbon tetrachloride
water.
4. Decomposition of hydrogen peroxide in presence and absence of
a catalyst.
5. Determination of percentage composition of binary liquid
(water/acetic acid) by viscosity
method.
6. Reaction Kinetics of Ethyl acetate Hydrolysis.
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