Calcutta University Biochemistry Syllabus

I need Calcutta University B.Sc Biochemistry course detailed syllabus for start to attend classes, so will you please provide here Calcutta University B.Sc Biochemistry course detailed syllabus???

[Quick Sam]

You are looking for Calcutta University B.Sc Biochemistry course detailed syllabus, here I am giving:

B.Sc Biochemistry

Part I
General and
Physical
Chemistry (fundamental principles)
Organic
Chemistry
Biomolecules
Physical

Module I General and Physical Chemistry
50 marks (60L)
Unit I
1. Atomic Structure
Extra nuclear structure: Bohr’s theory of atomic structure and its limitations, Summerfeld’s
modification, application of Bohr’s theory to hydrogen like atoms and ions, Spectrum of
hydrogen atom. Quantum numbers. Preliminary idea of de Broglie matter waves, concept of
atomic orbital, shapes of s, p and d orbitals, radial and angular probability of s, p and d
orbitals (qualitative idea). Many electron atoms, Pauli Exclusion Principle, Hund’s rule of
maximum multiplicity, exchange energy, Aufbau (building up) principle and its limitations,
Electronic energy levels and electronic configurations of hydrogen like and polyelectronic
atoms and ions (concept only), Ground state term symbols of atoms and ions (concept only).
2. Intermolecular forces
a. Ionic bonding
Size effects- radius ratio rules and their limitations. Packing of ions in crystals, Lattice
energy (concept only), Born- Lande equation (derivation not required) and its
applications; Born-Haber cycle (derivation not required) and its application.
Preliminary ideas of solvent energy, polarizing power and polarisibility, ionic potential
and Fajan’s rules
b. Covalent bonding
Lewis structures, formal charge, Preliminary idea of Valence Shell Electron Pair
Repulsion (VSEPR) Theory, shapes of molecules and ions containing lone pairs and
bond pairs. Partial ionic character of covalent bonds, bond moment and dipole moment,
Partial ionic character from dipole moment values and electro negativity differences,
Preliminary idea of valence Bond Theory ( Heitler- London approach). Directional
character of covalent bonds, hybridization, equivalent and non equivalent hybrid
orbital, Bent’s rule; Concept of resonance, resonance energy, resonance
structures.bonding, non-bonding,antibonding molecular orbitals( concept only)
elementary pictorial approach of H2 and O2 molecular orbitals , sigma and pi bonds,
multiple bonding. Concept of Bond order, bond length, bond strength, bond energy
c. Weak Chemical Forces
Van der Waal’s forces, ion-dipole, dipole–dipole interactions, London forces,
Hydrogen bonding; Effect of chemical forces on physical properties
CU B.Sc Biochemistry syllabus
Syllabi for three-year B.Sc. (H) in Biochemistry (BCMA) 2015
PART-I
PAPER I (F.M. 100)
Module I General and Physical Chemistry
50 marks (60L)
Unit I
1. Atomic Structure
Extra nuclear structure: Bohr’s theory of atomic structure and its limitations, Summerfeld’s
modification, application of Bohr’s theory to hydrogen like atoms and ions, Spectrum of
hydrogen atom. Quantum numbers. Preliminary idea of de Broglie matter waves, concept of
atomic orbital, shapes of s, p and d orbitals, radial and angular probability of s, p and d
orbitals (qualitative idea). Many electron atoms, Pauli Exclusion Principle, Hund’s rule of
maximum multiplicity, exchange energy, Aufbau (building up) principle and its limitations,
Electronic energy levels and electronic configurations of hydrogen like and polyelectronic
atoms and ions (concept only), Ground state term symbols of atoms and ions (concept only).
2. Intermolecular forces
a. Ionic bonding
Size effects- radius ratio rules and their limitations. Packing of ions in crystals, Lattice
energy (concept only), Born- Lande equation (derivation not required) and its
applications; Born-Haber cycle (derivation not required) and its application.
Preliminary ideas of solvent energy, polarizing power and polarisibility, ionic potential
and Fajan’s rules
b. Covalent bonding
Lewis structures, formal charge, Preliminary idea of Valence Shell Electron Pair
Repulsion (VSEPR) Theory, shapes of molecules and ions containing lone pairs and
bond pairs. Partial ionic character of covalent bonds, bond moment and dipole moment,
Partial ionic character from dipole moment values and electro negativity differences,
Preliminary idea of valence Bond Theory ( Heitler- London approach). Directional
character of covalent bonds, hybridization, equivalent and non equivalent hybrid
orbital, Bent’s rule; Concept of resonance, resonance energy, resonance
structures.bonding, non-bonding,antibonding molecular orbitals( concept only)
elementary pictorial approach of H2 and O2 molecular orbitals , sigma and pi bonds,
multiple bonding. Concept of Bond order, bond length, bond strength, bond energy
c. Weak Chemical Forces
Van der Waal’s forces, ion-dipole, dipole–dipole interactions, London forces,
Hydrogen bonding; Effect of chemical forces on physical properties
d. Co-ordination compounds
Double salts and complex salts, Werner’s theory, ambidentate and polydentate ligands,
chelate complexes, Naming of co-ordination compounds (up to two metal centres).
Isomerism of co-ordination compounds: Constitutional, geometrical and optical
isomerism in respect co-ordination numbers 4 and 6. Determination of configuration of
cis-, trans-, isomers by chemical methods,
Reference Books
1. General &Inorganic Chemistry-R.P.Sarkar
2. Inorganic Chemistry-R.L.Dutta
3. New Concise Inorganic Chemistry-J.D.Lee
Unit II:
Biophysical properties
(a) Viscosity: General features of fluid flow (streamlined and turbulent),
nature of viscous drag for streamlined motion. Definition of viscosity
coefficient. Origin of viscosity of liquids, expression for viscosity
coefficient of liquids (with derivation): Poiseuille’s equation, temperature
dependence of viscosity coefficient of liquids. Stoke’s law and terminal
velocity. Determination of viscosity coefficient of liquids. Diffusion of
solutes in solution, Fick’s law.
(b) Surface tension: Definition, angle of contact, interfacial tension,
capillary rise, determination of surface tension, temperature effect.
(c) Preliminary idea of Chemical equilibrium: Equilibrium constant, Le
Chatelier’s principle and its simple applications.
Ionic equilibrium: Standard solution, Molar, Normal, Molal, Formal and percent
strengths, Hydrolysis of weak acids and bases. pKa, pKb, pH, pOH acid- base
neutralization curves, Buffer action definition, Henderson -Hasselbalch equation
and preparation of buffers, buffer capacity, Solubility product principle and
application.
Unit-III
Electrochemistry:
Flow of electrical charge: Electrical conductance, cell constant, specific conductance and
equivalent conductance. Variation of equivalent conductances of strong and weak
electrolytes with dilution, Kohlrausch’s law of independent migration of ions, ion
conductances and ionic mobility, Equivalent conductances at infinite dilution for weak
electrolytes and determination of dissociation constants of weak electrolytes from
conductance measurements.Basic concepts of electrochemical cell and cell
reactions.EMF of cell (no derivation), types of electrode,glass electrode,determination of
pH of a solution and potentiometric titration,redox reaction.
Chemical Kinetics
(a) Concepts of rate, rate constant, order and molecularity of a reaction, integrated
form of rate expressions; half-life period and its significance.
(b) Pseudo-unimolecular reactions, multi step reactions, rate determining step, zero
and fractional orders, rate expressions for complex reactions, Steady-State
approximation. Opposing reaction, parallel reaction and consecutive reaction.
Temperature dependence of rate constant, Arrhenius’equation, Energy of
Activation; Concept of Collision theory and Transition State theory of reaction
rate.
(c) Catalytic reactions: Homogeneous catalysis, acid –base catalysis, primary salt
effects, Autocatalysis, Adsorption of gases on solids, Langmuir adsorption
isotherm, Heterogeneous catalysis, examples.
Reference Books
1. Physical Chemistry-P.C.Rakshit
2. Lehninger Principles of Biochemistry-Nelson &Cox
3. Text Book of Physical Chemistry-K.L.Kapoor(Vol-II,V)
4. Physical Chemistry-Hrishikesh Chatterjee(Vol-I)
Module II Organic Chemistry 50 marks (60L)
Unit I : Bonding and Stereochemistry of Carbon Compounds
Concept of hybridisation, resonance (including hyperconjugation), inductive effect
Huckel’s rules for aromaticity & antiaromaticity. dipole moment, bond distance,
bond angles Tautomerism: keto-enol tautomerism
Ionization of acids and bases: effect of structure, substituent and solvent on acidity and
basicity ( Simple Aliphatic and aromatic Acids, Phenols and amines).
Stereochemistry Optical activity of chiral compounds: specific rotation, measurement
of specific rotation by polarimeter, racemisation (general principle) resolution of
simple acids and bases.
Representation of molecules in saw horse, Fischer, flying-wedge and Newman formulae
and their inter translations, Configuration: stereocentres: systems involving 1, 2, 3
centres, stereogenicity, chirotopicity. pseudoasymmetric (D/L and R/S descriptor
threo/erythro and syn/anti nomenclatures ii) stereoaxis in C=C & C=N systems, cis/trans,
syn/anti, E/Z descriptors.
Coformation: Conformational nomenclature, eclipse, staggard, gauch and anti forms ;
dihedral angel, torsion angel, energy barrier of rotation; Conformational analysis of
ethane, propane and n-butane;Conformational analysis of cyclohexane(chair and boat
forms), symmetry properties, optical activity and relative stabilities of cyclohexane
systems;
.
Unit II: General treatment of reaction mechanisms
Ionic and radical reactions; heterolytic and, homolytic bond cleavage
Reactive intermediates: carbocations (carbenium and carbonium ions), carbanions,
carbon radicals, carbenes – structure using orbital picture, electrophilic/nucleophilic
behaviour, stability, generation and fate. Reaction kinetics: transition state theory,rate
constant and free energy of activation, free energy profiles for one step and two step
reactions.
Nucleophilic substitution reactions- SN1, SN2, SN
i mechanisms. Effect of substrate
structure, nucleophiles and medium on reactivity and mechanism; neighboring group
participations.
Elimination Reactions- E1, E2, and E1cB mechanisms. Saytzeff and Hofmann rules.
Elimination vs substitution reaction.
Electrophilic and Activated Nucleophilic substitution reactions of Benzene ( Nitration,
sulphonation, Halogenation and Friedel Craft reactions)
Unit-III: Specific Reactions and Heterocycles
Addition reactions to Carbon–carbon multiple bonds- Electrophilic additionsmechanisms
of halogenations, hydrohalogenation, hydration, hydroboration, epoxidation,
hydroxylation, ozonolysis.
Nucleophilic addition to carbonyl groups: relative reactivity of carbonyl compounds.
Formation of acetal, LiAlH4 and NaBH4 reductions, Grignard reactions, Cannizzaro,
aldol condensation.
Heterocycles- Structural aspects of five and six membered heterocycles containing
hetero atoms (furan, pyran, pyridine, pyrrole, furanose, pyranose, purines, pyrimidines).
Aromaticity of heterocyclic compounds; basicity of pyridine and pyrrole. Tautomerism in
heterocyclic systems.
Reference Books
1.Organic Chemistry (vol.1&2) – I.L.Finar
2.A Guide to Organic Reaction Mechanism- P. Sykes
3.Stereochemistry of Carbon Compounds- D. Nasipuri
4.Basic Stereochemistry of Organic Compounds- S. Sengupta
Paper II (F.M-100)
Module III: Biomolecules 50 marks (60L)
Unit I:
1. Amino acids
Definition,classification & structures. Physico-chemical properties of amino
acids(amphoteric molecules,ionisation, zwitterions,pk values, isoelectric point, Lambert-
Beer’s law, optical density, absorption spectra), titration of amino acids(glycine,glutamic
acid,lysine,histidine),Formol titration of glycine(only reaction and principle), reaction of
amino acids: reaction due to amino groups(reaction with mineral acids,alkyl halides,
acetyl chloride, acetic anhydride in presence of base, nitrous acid, ninhydrin and
fluorescamine), reaction due to carboxylic acid group (reaction with base,
alcohol,LiAlH4, metal oxide), separation and analysis of amino acids by paper & thin
layer chromatography and HPLC.
2. Peptides & Proteins
Peptide bond: Definition, structure and geometry of peptide bond, example of
biologically important peptide and its functions in brief (glutathione-peptide of non
protein origin), Merrifield solid-phase peptide synthesis using protection/ deprotection
protocol (brief outline). N-terminal amino acid determination(Edman degradation,
dansyl chloride reagent, Sanger’s reagent) and C-terminal amino acid determination
(carboxypeptidase and using hydrazine)
Proteins : Definition & structure, primary, secondary, tertiary and quaternary
structure(definition and example), structure of globular protein(albumin, globulin,
haemoglobin & myoglobin – Structure, function and occurrence in brief ) and fibrous
protein (keratin, collagen -role of Vitamin C in hydroxylation, elastin- Structure,
function and occurrence in brief ), Forces that stabilise structure of proteins, behaviour of
proteins in solutions, salting in and salting out, Denaturation and renaturation of proteins
(example -RNase), absorbance of proteins, example of metalloprotein, lipoprotein.Biuret
and Folin-Lowry test for protein.
Unit II:
1. Carbohydrates
Definition,classification,structure,occurrence and biological importance of
monosaccharides(aldohexose-glucose,mannose,galactose;epimers; ketohexose–fructose,;
aldopentose-riboses; deoxysugars-deoxyribose; fucose; rhamanose),Molish’s test for
carbohydrate, reaction of monosaccharides with nitric acid,bromine water,periodic acid
and phenylhydrazine,osazone formation, reaction of deoxyribose with DPA and reaction
of ribose with orcinol reagent; glycosidic linkage,disaccharides(sucrose-invert
sugar,inversion of sucrose,maltose and lactose) reducing and non-reducing sugar(tests for
reducing sugars,reaction with Benedict’s reagent,Fehling’s solution,Tollen’sreagent,
Seliwanoff test for ketose sugar, ), Configuration of D-glucose and D-fructose,anomers(_
& _- D-glucopyranose), anomeric effect,differences between anomers and isomers,
mutarotation and its mechanism;
polysaccharides(cellulose,glycogen,starch,chitin,a gar),blood group polysaccharides,
Glycoprotein,proteoglycan,glycosaminoglycan,murami c acid,sialic acid.
2. Lipids
Definition and classification(simple,complex and derived lipids with examples). Fatty
acids- definition,structure ,properties, examples of saturated and unsaturated fatty acids,
essential,non-essential fatty acids, Geometric isomerism of fatty acids, Triacyl glycerols.
Reactions and characterization of fats – hydrolysis, saponification, saponification value,
iodine number, rancidity of fats, Reichert- Meissel number. Phospholipids- Definition,
general structure (Glycerophospholipids, lecithins-phosphatidyl choline, lysolecithins,
cephalins-phosphatidyl ehanolamine , phosphatidyl serine, phosphatidyl inositol,
plasmalogens, sphingomyelines – structure,occurence and brief function). Glycolipidscerebrosides,
gangliosides(structure,occurrence and brief function),cholesterol
(structure,occurrence and brief function).test for cholesterol.
Unit III:
Nucleic acids
Definition,generalized structural plan of nucleic acids,phosphodiester bond, structure of purine
and pyrimidine bases,composition of DNA and RNA, Nucleosides and
nucleotides(definition,structure and example) , nomenclature used in writing structure of
nucleic acids, complementary base- pairings, Chargaff’s rule,features of DNA double helix
(Watson-Crick model).different forms of DNA structure(A,B & Z DNA), major and minor
groove,three major types of RNA, secondary and tertiary structure of tRNA, chemical
properties: hydrolysis(acid & alkali), absorbance of DNA & RNA, Denaturation and annealing
of DNA, melting temperature,factors affecting melting temperature,hyperchromic effect,
electrophoresis and staining of DNA(with EtBr) ,Central dogma(outline only).
Porphyrins
Porphyrin nucleus and classification. Important metalloporphyrins occurring in nature- haemoglobin, leghemoglobin (plant hemoglobin), chlorophyll, cyanocobalamin and their
brief functions (it is important to know the metal centers but memorizing the structures
are not required).
Reference Books
1.Biochemistry – Voet & Voet
2.Biochemistry – Lubert Stryer
3.Lehninger Principles of Biochemistry – Nelson & Cox
Module IV Practical Paper (Physical Chemistry and Organic Chemistry):
Unit I: Physical Chemistry 30M (One experiment 20+ Lab note book 5+ Lab Ouiz
5)
1. a. Preparation of buffer of a given pH(for example acetate buffer of
pH=4,phoshphate buffer of pH=7, glycine-NaOH buffer of pH 9.0
b. Preparation of a primary standard solution ( oxalic acid ,dichromate) of known
strength.
2. Determination of pKin value of a weak acid - base indicator by Colorimetric method.
3. pH metric titration: weak monobasic acid by strong base.
4. Conductometric titration of: Mixed acids vs strong base.
5. Potentiometric titration (Mohr vs. dichromate).
6. Determination of solubility and solubility product of a sparingly soluble salt by
titrimetric method.
7. Determination of specific rotation of a given optically active compound and
%composition of its aqueous solution using Polarimeter.
8. Determination of viscosity coefficient of a given liquid/solution with Ostwald
viscometer.
9. To study the kinetics of saponification of ester by conductometric method.
10. Estimation of protein by biuret method: application of Lambert –Beer’s law.
Unit II: Organic Chemistry 20M
(One experiment 15+ Lab note book 2.5+Lab Quiz 2.5)
1. Physical characteristics (colour, odour, texture) [1M]
2. Preliminary Tests: [2M]
(Ignition Test, litmus Test, Beilstein test for halogen, Br2 in AcOH/water or
KMnO4 in water test)
3. Detection of special elements (N, Cl, S) by Lassaigne’s tests. [2+2+1=5 M]
4. Solubility and classification [2+1=3M]
(Solvents: H2O, 5% HCl, 5% NaHCO3, 5% NaOH)
5. Detection of the following functional groups by systematic chemical tests:
(aromatic amino (–NH2), Amido (–CONH2, including imide), aromatic nitro (–
NO2), Phenolic –OH, Carboxylic acid (–COOH), Carbonyl (>C= O); only one
test for each functional group is to be reported) [6×1½=9M]
*Each student, during laboratory session, is required to carry out qualitative chemical
tests for all the special elements and the functional groups in known and unknown
organic compounds. Each student, during laboratory session, is required to analyze at
least SIX (6) unknown organic samples. In practical examination, one unknown solid
organic compound containing not more than two of the above functional groups (IV)
shall be assigned to a candidate through a single draw lottery.
B. LABORATORY RECORDS [5 M]
7. Candidates at the practical examinations are required to submit the day to day record
of all types of laboratory works prescribed in the syllabus performed by them and
duly signed by their teachers. Marks of the laboratory records shall be awarded by the
examiner at the practical examination. Candidates failing to submit their laboratory
note books may be debarred from the examination.
Practical Reference Books
(i) Advanced Practical Chemistry – Subhas Ch. Das
(ii) Handbook of Practical Chemistry – University of Calcutta
For detailed syllabus, here is attachment;