B.Sc. CHEMISTRY
DURATION OF COURSE
:
3 YEARS
ELIGIBILITY
:
+2 OR EQUIVALENT
COURSE CODE
:
181
FIRST YEAR
S. No.
Papers
Max. Marks
Exam Hrs.
1.
Tamil
100
3
2.
English
100
3
3.
Inorganic, Organic and Physical
100
3
Chemistry – I
4.
Mathematics
100
3
5.
Inorganic Qualitative Analysis and
100
3
100
3
Inorganic Preparations
6.
Practical 1: Major
SECOND YEAR
S. No.
Papers
Max. Marks
Exam Hrs.
1.
Tamil
100
3
2.
English
100
3
3.
Inorganic, Organic and Physical
100
3
Chemistry – II
4.
Physics
100
3
5.
Volumetric Estimations
100
3
6.
Practical 2: Major
100
3
7.
Practical 3: Allied
100
3
THIRD YEAR
S. No.
Papers
Max. Marks
Exam Hrs.
1.
Organic Chemistry
100
3
2.
Inorganic Chemistry
100
3
3.
Physical chemistry
100
3
4.
Pharmaceutical Chemistry
100
3
5.
Analytical Chemistry
100
3
6.
Organic Qualitative Analysis and
100
3
Organic Preparations
7.
Gravimetric Estimations
100
3
8.
Physical Chemistry Experiments
100
3
FIRST YEAR
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ENGLISH PAPER – I
Detailed Text
PROSE
1. In Prison – Jawaharlal Nehru
2. What is Science? – George Orwell
3. On Marriages – Nirad Chaudari
4. The Luncheon – N. Somerset Maugham
5. The Mourners – V. S. Naipaul
6. The Plane Crash – Juliane Koepcke
7. Better Late – R.K. Narayan
POETRY
1. Polonius’ Advice t his Son – William Shakespeare
2. Every Town a Home Town - Kaniyan Purkunran
3. The Village Schoolmaster – Oliver Goldsmith
4. The Solitary Reaper – William Wordsworth
5. On his Blindness – John Milton
6. The Tyger – William Blake
Non-Detailed
Text : THE GIFTS AND OTHER STORIES abridged and simplified by Anthony Toyne –
Oxford University Press, 1997.
The following stories
1. The Gifts – O. Henry
2. The Two Friends – Guy de Maupassant
3. The Bear Hunt – Leo Tolstoy
4. The Goblins and the Grave Digger – Charles Dickens
5. The Nightingale and the Rose – Oscar Wilde
GRAMMER
1. Articles and Prepositions
2. Infinitives and Gerunds
3. Five basic sentence patterns (SV SVC, SVO, SVOO, SVOC(A))
4. Arranging the component parts so as to form a sentence
5. Language work at the end of all lessons
6. Language work at the end of all lessons
7. Question Tag, Active and Passive Voice
8. Degrees of Comparison
COMPOSITION
1. Letter Writing (Formal and Informal)
2. Developing the hints
3. Comprehension
4. Writing Telegram
5. Completion of a passage
6. Precis Writing
Paper – 3
INORGANIC, ORGANIC AND PHYSICAL CHEMISTRY – I
UNIT I :
1.1.
Laboratory Operations and Hygiene
Storage and handling of corrosive, flammable explosive, toxic carcinogenic and
poisonous chemicals simple first aid procedure for accidents involving acids, alkalis,
Bromine burns, internal poisons cuts and wounds disposal of waste, waste chemicals and
fumes.
1.2.
Laboratory Operations
Precipitation, filtration, sample drying, transfer of precipitates, filter papers and their
use – Calibration and use of apparatus for filtration – units of weight and concentration
solvents and their purity.
1.3. Principles of Inorganic Qualitative analysis common : On effect and principles of
solubility product and its application.
UNIT – II: Chemical bonding:
2.1. Ionic bond : Types of Ions – Radius ratio and its applications – Born-Haber cycle –
calculations.
Polarising power and polarizability Transition from ionic to covalent
character – Fajan’s rule.
2.2 . Periodicity of elements :
a. Classification of elements based on electronic configuration periodicity in
properties.
b. Studies the following properties of Atomic, ionic, covalent, metallic, vander
walls radii.
c. Ionisation potential – Electron attinity . Electro-negativity – Pauling mulliken
electro-negativity scale – hydrogen bonding.
2.3. Covalent bond:
V12 and MO theories in details and comparison between them. Bonding Antibonding and non-bonding orbitals. Application of M.O. theory – configuration of molecules
and ions. F2, Li2, Co, O2 with diagram.
2.4. Shapes of Molecules – VSEPR theory. Simple inorganic molecules containing ion pairs
and bonded pairs.
2.5. Inter molecular forces – vandervaal’s and london forces. Hydrogen bond – its nature –
Types and effect on properties.
UNIT – III:
Basic concept – Hydrocarbons – halogen Compounds and Chemistry of S-Block
elements.
3.1.1. Alkanes, Isomerism – Chemical reactivity – tree radial laologenation (mechanism),
Cycloalkanes : Nomenclature – Preparation – Bayer’s strain theory.
Alkali metals – a comparative study of alkali metals and their compounds – diagonal
relationship between lithium and magnesium – Exceptional properties of Li.
3.1.2 : Alkaline earth metals – A comparative study of alkaline earth metals and their
compounds. Diagonal relationship of Be and Al. Abnormal properties of Be.
3.1.3 : Nucleophilic substitution – SN1, SN2 , SNi reactions – Effect of solvent, structure of
substrates; Nucleophilicity of Nucleophilic and nature of leaving group. Relative reactivity
of Methyl, ethyl, isoprophyl, t’-butyel vinyl and benzyl halides.
3.1.4 : Elimination reactions - E1 & E2 reactions dehydration, dehydrahalogenation –
say+zett rule – Hotmann rule.
3.1.5 : Bond dissociation energy, Bond energy – calculation from thermo-chemical data.
3.1.6 : Vitreous state – super cooled liquid – glass.
UNIT – IV :
Aromatic compounds and Hydrides.
4.1.1 :Aromatic electrophilic substitution reactions, mechanism of nitration halogenation,
sulfonation and triedel cratts alkylation and acylation orientation effects in disubstituted
benzenes.
4.1.2 : Preparation of Naphthalene and anthracene Haworths synthesis, Electrophilic
substitution, orientation and reactivity in Naphthalene and anthracene, structure of
Naphthalene and Anthracene.
4.1.3 : Aromaticity – Huckel’s rule Benzenoid and non-benzeniod compounds.
4.1.4 : Hydrides – Classification and chemistry of hydrides. Ethers and phenols.
4.1.5 : Cleavage in Ethers – Electrophilic substitution in phenols : reaction mechanism of
kolbe, Reimer Tiemann and diazocoupling reactions.
Electron displacement effects – Inductive, Inductomeric, mesomeric legonance,
hyper conjugation and steric effects – their effects on properties of compounds curved arrow
notation. Drawing electron movement with arrow half-headed and double headed arrows –
hemolytic and heterolytic fission.
UNIT – V :
Chemical Thermodynamics
5.1.1 : Definition and explanation of terms, Intensive and Extensive properties, types of
systems, thermodynamic processes, cyclic reversible process, isothermal, adiabatic
conditions.
5.1.2 : Thermodynamic functions, complete differential, zeroth law of thermodynamics,
concept of heat and work.
5.1.3 : First law of thermodynamics. Relationship between Cp and Cr – Calculations of q, w,
dE and dH for ideal gases under isothermal and adiabatic conditions for its reversible
process. Joules law. Joules thomson effect inversion Temperature and significance.
5.1.4 : Relationship between H and E. Variation of heat of reaction with temperature –
Kirchotf’s equation.
5.1.5 : Atomic structure – Bohr model – limitations sommerfield model – Blackbody
radiation – Photoelectric effect – De broglie theory – Heisernberg’s uncertainity principles.
Wave theory – Schrodinger wave equation (no derivation) significance of and wave function
and quantum numbers. Shapes of S, P and d orbitals.
PAPER – 4
MATHEMATICS
UNIT I: DIFFERENTIAL CALCULUS
Function – Limits – continuity - methods of differentiation -successive
differentiation – tangent & normals.
UNIT II: INTEGRAL CALCULUS
Elementary integration - integration by substitution - Integration by Parts and partial
fractions - Define integrals.
UNIT III: VECTOR ALGEBRA
Scalars and vectors – Addition – Product - Cross product - dot product or
scalar product.
UNIT IV: DIFFERENTIAL EQUATIONS
Ordinary differential equations – solution - variable separable method Homogeneous method - partial differential equations.
UNIT V: PROBABILITY AND STATISTICS
Measures of location and dispersion - curve fitting – correlation –regression Probability and probability Distribution - Random variable and Probability Distributions.
TEXT BOOKS:
Engineering Mathematics-Vol 1 and 2 - A.K.Gupta - Macmillan India Limited.
Paper – 5
INORGANIC QUALITATIVE ANALYSIS AND
INORGANIC PREPARATIONS
1. Inorganic qualitative analysis :
Analysis of a mixture containing two cations and two anions of which one will be an
interfering ion. Semi-micro methods using the conventional scheme with hydrogen sulphide
may be adopted.
Anions to be studied : Carbonate, nitrite, sulphide, sulphite, thiosultate, sulphate,
nitrate, fluoride, chloride, bromide, iodide, borate, oxalate, arsenite, arsenate, phosphate,
chromate, tartrate, silicate.
Cations to be studied : Silver, Mercury, read, bismuth, copper, cadmium, tin,
antimony, arsenic, iron, aluminium, chromium, barium, strontium, calsium, sodium,
potassium, magnesium, ammonium.
Note :
Note to be given for examination.
Anions – nitrite, sulphide, sulphite, thiosulfate, arsenate, tartrate, chromate and
silicate.
2. Inorganic preparations :
a. Sodium thiosulpate
b. Ferrous ammonium sulphate
c. Potassium trioxalatochromate (III)
d. Tetraammine copper (II) sulphate
e. Microcosmic salt
Not for examination : Manganous sulphate.
REFERENCE BOOKS :
I.
Inorganic chemistry :
1. Philips and williams, Inorganic Chemistry, Oxford University Press, Vol. I & II.
2. P.L. Soni Text Book of Inorganic Chemistry, Sultan Chand & Sons.
3. Puri and Sharma, Text Book of Inorganic Chemistry.
4. Madan R.D. Inorganic Chemistry, S. Chand and Co.
II.
Organic Chemistry :
1. Final 1-organic chemistry Vol. I & II – I EIBS.
2. P.L. Soni text book of Organic Chemistry, Sultan Chand and Sons.
3. Morrison and Boyd, Organic Chemistry.
4. Bhal B.S., and Arun Bhal, A text book of Organic Chemistry.
III.
Physical Chemistry :
1. Glasstone, S-Text Book Physical Chemistry Mac. Millian.
2. Gurudeep R. Chatwal, Physical Chemistry.
3. Rakshit, Thermodynamics, Science Book Agency.
4. Kundu and Jain, Physical Chemistry, S. Chand
PRACTICAL I MAJOR
Inorganic Qualitative Analysis
Analysis of a mixture containing two cations and two anions of which one will be an
interfering ion. Semimicro methods using the conventional scheme with hydrogen sulphide.
may be adopted. CATIONS TO BE STUDIED: Lead, Copper, Bismuth, Cadmium, Iron,
Aluminum, Zinc,, Manganese, Cobalt, Nickel, Barium, Calcium, Strontium,Magnesium, and
Ammonium. ANION TO BE STUDIED: Carbonate, Sulphide, Sulphate, Nitrate, Chloride,
Bromide, Fluoride, Borate, Oxalate and phosphate
Reference books:
1. Qualitative Inorganic Chemistry by A. I. Vogel.
2. Quantitative Inorganic Chemistry by A. I. Vogel.
3. Physical Chemistry of Inorganic qualitative analysis by Kuricose & Rajaram.
4. Practical manual in water Analysis by Goyal & Trivedi.
5. Basic Concepts in Analytical Chemistry by S. M. Khopkar. Wiley Eastern Ltd.
6. Practical Chemistry, Physical – Inorganic – Organic and Viva voce by Balwant Rai
Satija. Allied Publishers Private Limited.
7. College Practical Chemisty by H. N. Patel, S. R. Jakali, H. P. Subhedar, Miss. S. P.
Turakhia. Himalaya Publishing House, Mumbai.
8. College Practical Chemistry by Patel, Jakali, Mohandas, Israney, Turakhia. Himalya
Publishing house.
9. Experiments in General Chemistry by C. N. R. Rao. Affiliated East –West Press Private Ltd.,
Delhi.
1.
THIRD YEAR
Paper 11
INORGANIC CHEMISTRY
UNIT – I :
1.1.1. Nuclear chemistry
1.1.2. Fundamental particles of nucleus – concept of nuclides – Representation of nuclides
– Isotopes, Isobars and Isotones with example.
1.1.3. Forces operating between n-n and n-p and magnitude of nuclear forces.
Qualitative idea of stability of nucleas (n/p ratio)-magic numbers – stability belt.
1.1.4. Natural radioactivity – nuclear binding energy – mass defect – calculation of binding
energy and mass defect.
Artificial radioactivity or induced radioactivity – nuclear fusion and nuclear fusion
reactions.
1.1.5. Lanthanide’s – Isolation of lanthanide’s – physical and chemical properties –
Lanthanide’s contraction and consequences.
Actinides – Occurrence and synthesis – chemistry of thorium and uranium.
UNIT – II:
2.1.1. General principles and process of metallurgy.
2.1.2. Occurrence, extraction – properties and uses of Ti, Zr, V. Mo,. W, Pt and their
important compounds.
2.1.3. Group study of Ti, V and Cr groups.
UNIT – III:
3.1.1. Elements of symmetry and symmetry operations – point group – with
reference to simple molecules.
3.1.2. Nomenclature, study of complexes by precipitation and conductivity measurements
werners and sidgwick theories of bonding in complexes – factors affecting the stability of
complexes.
3.1.3. Elementary ideas of valence bond theory – explanation of geometry and magnetic
properties of complexes based on the theory – Limitations of the theory.
UNIT – IV:
1.1.1. Basic principles of Crystal field theory – Crystal field splitting in various fields –
crystal field stabilization energy in octahedral and tetrahedral complexes.
1.1.2. Explanation of Magnetic properties – Geometry and colour of the complex
compounds based on the above theory.
1.1.3. Comparison between V.B and C.F. theories.
1.1.4. Metallic carbonyls : Mono and binuclear carbonyls of Ni, Fe, Cr, Co and Mn
structure, synthesis and reactions.
1.1.5. Organo metallic compounds : Classification synthesis, properties and structure of
organo lithium and organo boron compounds.
UNIT – V:
1.1.1. Solids : Band theory of solids, metal and semi conductors and insulators.
1.1.2. Bragg’s Law and application of X-ray diffraction to crystal studies – structure of
NaCl, LiCl and Zns.
1.1.3. Defects in solids, conductors in ionic solid-electrical and magnetic properties.
PAPER – 12
ORGANIC CHEMSITRY
UNIT – I:
1.1.1. Carbohydrates – classification.
1.1.2. Monosaccharides – reaction of Glucose and Fructose – Osazone formation –
Constitution of Glucose and Fructose.
Open chain structure, configuration and ring structure – Mechanism of mutarotation
– determination of ring size – Haworth’s projection formulae – conformation of
monosaccharides.
1.1.3. Inter conversions – Epimerisation - conversion of pentose to hexose and vice-versa
– Aldose to Ketose and vice-versa.
1.1.4. Disaccharides – structural elucidation of sucrose and Maltose.
1.1.5. Polysaccharides – structre of starch and cellulose – properties – Derivatives of
Cellulose.
UNIT – II : Heterocyclic Compounds
2.1.1. Heterocyclic compounds : Introductin – Molecular Orbital picture and aromatic
characterstics of pynrole, Furan, Thiophene and Pyridine – Methods of synthesis and
chemical reactions with particular emphasis on the mechanism of electrophilic
substitution mechanism of nucleophilic substitution reactions in pyridine, piperidine
and pynrole.
2.1.2. Introduction to condensed five and six membered heterocyclics – preparation and
reactions of Indole, Quinoline and Isoquinoline with special reference to fischer –
Indole synthesis – Skraup synthesis and Bisher – Napieralski synthesis.
2.1.3. Electrophilic substitution reactions of indole, quinoline and isoquinoline.
2.1.4. Alkaloids : Classification of Alkaloids – General Methods for determination of
structure of alkaloids – Synthesis andstructural elucidation of Piperine, Coniine and
Nicotine.
UNIT – III: Stereochemistry
3.1.1
Optical Isomerism : Chiral Centre – Optical Isomerism – Elements of symmetry –
Enantiomers – Diastereoisomers – D.L. and R.S. Nomenclature.
3.1.2 Racemisation, Resolution – Asymmetric Synthesis – Walden Inversion – Projection
formulae – Optical activity of allenes, spiranes and biphenyls – optical activity of
molecules containing Nitrogem.
3.1.3 Geometrical Isomerism : E, Z system of nomenclature – methods of assigning
configuration – Geometrical isomerism in cyclic compounds 0 Maleic and fumeric
acids – structural assignments.
3.1.4 Conformational Analysis : Rotation around a single bond – preferred rotational
conformers of ethane – propane, n-butane dichlorethane, glycol, cyclohexane, mono
and disubstituted cyclohexane, 1,2 & 1,3 – interactions – Decalin-C is and trans
Decalin – Conformational isomerism.
UNIT – IV
4.1.1. Terpenes : Classification
of Terpenes – Isolation – Isoprene rule- Structural
elucidation and synthesis of citral, creraniol, alpha-terpeneol, alpha-pinene and
camphor.
4.1.2. Dyes : Classification of Dyes according to structure and methods of application.
i.
Azo dyes-Methyl orange and Bismark Brown.
ii.
Triphenylmethane dyes-malachite Green.
iii.
Phthalein dyes – Phenolphthalein.
iv.
Vat dyes – Indigo.
v.
Anthraquinone dyes – Alizarin – Structural elucidation and synthesis.
4.1.3. Vitamins – occurance and biological importance of Thiamine, Riboflavine,
Pyridoxine and Ascorbic acids.
4.1.4. Structural elucidation of Ascorbic acid and its synthesis.
4.1.5. Antibiotics – structural elucidation of penicillin-G and chloromycetin.
UNIT – V:
Important Reagents and their application in organic chemistry – AlCl3, BF3, Al2O3,
LiAlH4, NaBH4, PCl5, P2O5, Nal ethanol, Alcoholic KOH, H2 / Ni, H2 / {d – Baso4, Zn / Hg
– HCl and Ag2O.
PAPER – 13
PHYSICAL CHEMISTRY
UNIT – I:
1.1.1. Thermodynamics : Partial molal properties – partial molal volume – Chemical
potential – Gibb’s Duhem equation – effect of temperature and pressure on chemical
potential – chemical potential in a system of ideal gases – Duhem-margulus
equation.
1.1.2. Concept of fugacity – Determinaiton of fugacity of a gas – calculation of fugacity at
lower pressure – Physical significance of fugacity – Concept of activity – Activity
Co-efficient.
1.1.3. Thermodynamic derivation of equilibrium constants Kp, Kc, Ka, Kx, Kf relationship
between Kp, Ka, Kx –standard free energy change – Distribution between G and
Go – Derivation of Vanthott Reaction Isotherm.
UNIT – II:
2.1.1 Chemical Kinetics.
2.1.2 Rate of the chemical reaction – rate equation – rate constant and its unit – order and
molecularity of simple and complex reactions.
2.1.3 Derivation of the rate constant, time for half-charge and characteristics of first,
second and third and zero order reactions with examples.
2.1.4 Methods of determining order of a reaction – Experimental methods in the study of
kinetics – volumetry – monometry – polarimetry and colorimetry.
2.1.5 Effect of Temperature on reaction Rates – Derivation of Arrhenius, equation –
concept of activation energy – determination of Arrhenius frequency factor and
energy of activation.
Theory of absolute reaction rates – theorem – dynamics derivation of rate constant
for a bimolecular reaction based on ARRT – comparision between CT and ARRT –
Significance of free energy of Activiation and entropy of activation.
UNIT – III:
3.1.1 Electro Chemistry.
3.1.2 Metallic and electrolytic conductance – Definitions of specific equivalent and molar
conductance – Relations between them – Measurement of conductance cell constant.
3.1.3 Variation of conductance with dilution – Qualitative explanation – Strong and weak
electrolytes.
3.1.4 Migrations of Ions – transport number – determination by Hittort and moving
boundary methods – Kholrausch’s Law – applications calculation for weak
electrolytes and determination of transport number.
Ionic mobilities and Ionic conductances – Diffusion and ionic mobilitiy – mdar
ionic conductance and viscosity – walden rule.
3.1.5 Applications of conductance measurements – Degree of dissociation of weak
electrolytes – Determination of ionic product of water – Determination of solubility
of sparingly soluble salts – conductometric titrations.
Theory of strong electrolytes – debye Huckel – Onsager Theory – verification of
onsagar equation – Wien and Debye – Falkenhagen effect.
Ostwalds dilution Law – determination of dissociation constants – Ionic product of
water – PH value.
Hydrolysis of salts – expression for hydrolysis constant – degree of hydrolysis and
PH O+ Salt solutions for different types of salts – Determination of degree of
hydrolysis – Conductance and distribution methods.
UNIT – IV:
4.1.1. Galvanic cells – Reversible and irreversible cell – EMF and its measurement –
Weston Standard cell – types of reversible single electrodes – standard H2 electrode
– calomet electrode – Derivation of Nernst equation both for emf of cells and single
electrode potentials – Nornst theroy for single electrode potential standard reduction
potentials – electrochemical series – significance.
4.1.2. Application of emf measurements – Application of Gibb’s – Helmholtz equation to
galranic cells – calculation of thermodynamic quantities – PH using hydrogen
quiphydrone and glass electrodes – Potentiometric titrations.
4.1.3. Concentration cells with and without transference – LJP expression – applications of
concentrations cells – valency of ions – transport number – solubility product –
activity co-efficient.
4.1.4. Storage cells – lead storage battery – Mechanism of charging and discharging fuel
cells – hydrogen – oxygen cell – polarization – over voltage decomposition voltage.
UNIT – V:
1.1.1 Phase Rule : definition of terms – Derivation of phase rule.
1.1.2 One component system – H2O system – Sulphur system – Explanatin using clausius
clapeyran eequation – super cooling and sublimation.
1.1.3 Two component systems – solid – liquid equilibria – reduced phase rule – simple
eutectic simple eutectics systems – Ag – Pb only – compound formation with
congruent melting point – Mg – Zn system only.
1.1.4 Peritectic change – Fecl2 – H2O system – Kl – H2O system effloroscence –
Deliquescence.
1.1.5 C.S.T. Phenol-water system only – Effect of impurities on CST.
Paper - 14
PHARMACEUTICAL CHEMISTRY
UNIT – I:
1.1 Importance terminologies – Pharmaceutical chemistry – Definition, Drugs –
Pharmacodynamics, Pharmacokinetics, Pharmacopoea, Virus, Bacteria, fungus,
actinomycetes, metabolities, anti-metabolities, LD50, ED50, Therapeutic index their
use in selecting drugs. Assay of drugs (elementary principles only). Use of Plaster of
Paris in bone-fracture.
1.2 Antibiotics : Definition – classification as Broad and Narrow spectrum antibiotics –
peincillin, chloramphenicol, tetracycline – structure and uses only (No structure or
preparation, assay etc)
UNIT – II:
2.1.
Sulphonamindes : Mechnaism and action of sulpha drugs preparation and uses of
sulphadiazene, sulphapyridine, sulphathiazole and sulphafurazole.
2.2.
Vitamins : Classification as water soluble and liquid soluble vitamins. Sources,
deficiencies of vitamins A, B1, B2, Vitamin C. Assay of A, B1 and Vitamin C.
2.3.
Analgesics : Narcotic analgesics, Morphine – Isolation, Pharmacological action –
uses – SAR.
Heroin and Codeine – inter-relation between these. Synthetic
analgesics – Pethidine and methadone.
UNIT – III:
3.1.
Antipyretic analgesics – salicylic acid derivatives – methyl salicylate, aspirin, paminophenol derivatives – paracetamol and phenacetin.
3.2.
Antiseptics and disinfectants : Phenol as disinfectant, Phenol coefficient – Dyes,
crystal violet, acridine, organo mercurials – phenyl mercury nitrate, chlorhexidine,
cationic surfactants – Benzalkonium chloride, Formaldehyde and nitrofurazone.
3.3.
Anasthetics : Classification as General and Local Intravenous anaesthetics.
Chemistry of anaesthic ether, nitrous oxide, halothane, chloroform, Intravenouis
anaesthetics – Thiopental sodium Methohexitone. Local anaesthetics – cocaine and
benzocain.
UNIT – IV:
4.1.
Alkaloids : Detection of alkaloids – colour reagent s- Mayer, Dragendroff, Wanger,
Hager reagents – Isolation of quinine – colour reactions of quinine. SAR of Quinine,
Tranquilisers, hypnotics and sedatives – chlorpromazine, barbitone.
4.2.
Antineoplastic and Hypoglycemic agents : Detection of sugar in seru and urine –
cause and control of diabetes, Oral hypoglycemic agents – sulphonyl urea
biguanides.
Causes and control of cancer – preparation thiotepa and
cyclophosphoramide.
UNIT – V:
5.1.
Organic Pharmaceutical Aids : their role as preservatives, antioxidants – colouring,
flavouring and sweetening agents, ointment bases.
5.2.
Blood – Blood groups – Rh factor, Blood pressure normal, high and low – how to
control them.
Causes and control of anaemia, Anti anaemic drugs – Iron, Vitamin B12 and folic
acid, Coagulant and anticoagulants – Heparin, coumarins, Vitamin C.
5.3.
AIDS – causes, prevention and control.S
Paper - 15
ANALYTICAL CHEMISTRY
UNIT – I:
1.1 Data Analysis : Idea of significant figures – its importance – examples. Precision and
accuracy – error – methods of expressing accuracy – error analysis – types of errors –
minimizing error. Methods of expressing precision – Average deviation, standard
deviation and confidence limits.
1.2 Laboratory estimations : Principles of calculations involving the following estimations
– Phenol, aniline, glucose, ketone. Calculation of iodine value, saponification value,
Reichert value and RM value of an oil.
UNIT – II:
2.1.
Principles of gravimetric analysis : Theories of precipitation solubility product
principle -–Nucleation – Growth of a crystal characteristic of precipitating agent –
choice of the precipitant – conditions for precipitation.
2.2.
Specific and selective precipitants – DMG, Oxine, Cupron, Cupferron,
Salicylaldoxime Ethylenediamine – Sequestering agents – Uses.
Differences – Minimization of precipitation errors. Precipitation from homogenous
solution.
UNIT – III:
Separation and purification techniques :
3.1.
Separation by Solubility, Methods – examples – solvent extraction method –
continuous extraction – soxhlets extraction. Chemical methods of separation for
both organic and inorganic substances.
3.2.
Chromatography – Principles of adsorption, Paper and Thin layer Chromatography.
3.3.
Column Chromatography – Adsorbent, preparation of the column, elution and
recovery of substances and applications TLC – Choice of adsorbent, choice of
solvent – preparation of the plate – application.
3.4.
Paper Chromatography – principle solvent used. Development of Chromatogram –
Radial paper chromatography and circular paper chromatography – separation of
amino acid mixtures – electrophoresis Rf value – factors affecting Rf value –
importance.
3.5.
Ion exchange chromatography – principle, types of resins and requirements of a
good resin – action of ion exchange resins – application. Separation of Zn and Mg.
Chloride and Bromide ions, Co & Ni and Cd and Zn.
3.6.
Elementary idea of GLC, VPLC & HPLC and techniques.
UNIT – IV:
4.1 Purification techniques : Solids – crystallization, fractional crystallization, sublimation,
Liquids – Distillation process – simple, fractional, distillation under reduced pressure,
azeotropic and steam distillation – Principles and experimental techniques. Tests of
Purity (M.P. and B.P. methods).
UNIT – V:
5.1 Polarography : Concentration polarization – Different types of currents – migration,
residual diffusion and limiting currents
Basic experimental assembly – dropping mercury electrode – current voltage curve –
influence of oxygen on the polarogram – Influence of temperature and agitation of
diffusion layer, Ilkovic Equation (Derivation not required) and significance –
Polarography as method of qualitative and quantitative analysis.
Amperometry – Basic principles and uses.
5.2 Polarimetry : Principle – instrumentation – applications – determination of specific
rotation of a substance – estimation of glucose.
PRACTICAL - I
ORGANIC QUALITATIVE ANALYSIS AND ORGANICPREPARATIONS.
A) Organic Qualitative Analysis
Identification of at least Ten Organic compounds with reactions including two from
acids, two from phenols, two from bases and four from neutrals.
Acids – Succinic acid, Phthalic acid, Salicylic acid, Aspirin.
Phenols – Alpha-Naphthol, o-nitrophenol, p-nitrophenol.
Bases – o-,m- and p-nitroanilines, Diphenyl amine.
Neutrals – Urea, Acetanilide, carbon tetrachloride, Bromobenzene, Methyl acetate,
Nitrobenzene, Naphthalene, Anthracene, Acetophenone, Ethyl methyl ketone.
ii) Organic preparations
1) p-nitro acetanilide from acetanilide.
2) Acetanilide from aniline using sodium acetate and acetic acid.
3) Phthalimide from phthalic anhydride.
4) Benzoic acid from benzamide.
5) Preparation of phenolphthalein.
Reference Books :
1. Practical Organic Chemistry by A. I. Vogel.
2. Hand book of Organic qualitative analysis by H. T. Clarke.
3. A laboratory Hand Book of Organic qualitative analysis and separation by V. S.
Kulkarni. Dastane Ramchandra & Co.
4. Practical Organic Chemistry by F. G. Mann and B. C. Saunders. Low – priced Text
Book. ELBS. Longman.
5. Experiments in General Chemistry by C. N. R. Rao. Affiliated East-West Press Pvt.
Ltd. Delhi.
6. Advanced Practical Organic Chemistry by N. K. Vishnoi. Vikas Publishing House
Private Limited.
7. Comprehensive Practical Organic Chemistry Qualitative Analysis by V. K. Ahluwalia,
Sunita Dhingra. University Press. Distributor – Orient Longman Ltd.
8. Comprehensive Practical Organic Chemistry Preparation and Quantitative Analysis by
V. K. Ahluwalia, Renu Aggarwal. University Press. Distributor – Orient Longman Ltd.
9. Practical Chemistry – Physical – Inorganic – Organic and Viva – voce by Balwant Rai
Satija. Allied Publishers Private Limited.
10. College Practical Chemistry by H. N. Patel, S. R. Jakali, H. P. Subhedar, Miss. S. P.
Turakhia. Himalaya Publishing House, Mumbai.
11. College Practical Chemistry by Patel, Jakali, Mohandas, Israney, Turakhia. Himalaya
Publishing House, Mumbai.
12. Practice of thin layer chromatography by Joseph C. Touchstone, Murrell F. Dobbins.
A Wiley – Interscience Publication John-Wiley & Sons.
PRACTICAL - II
GRAVIMETRIC ESTIMATIONS
1. GRAVIMETRIC ANALYSIS:
1. Estimation of Sulphate as Barium Sulphate.
2. Estimation of Barium as Barium Chromate.
3. Estimation of Lead as Lead Chromate.
4. Estimation of Calcium as Calcium Oxalate.
5. Estimation of Nickel as Nickel Dimethylglyoxime.
Reference Books :
1. Qualitative Inorganic Chemistry by A. I. Vogel.
2. Quantitative Inorganic Chemistry by A. I. Vogel.
3. Physical Chemistry of Inorganic qualitative analysis by Kuricose & Rajaram.
4. Practical manual in water Analysis by Goyal & Trivedi.
5. Basic Concepts in Analytical Chemistry by S. M. Khopkar. Wiley Eastern Ltd.
6. Practical Chemistry, Physical – Inorganic – Organic and Viva voce by Balwant Rai
Satija. Allied Publishers Private Limited.
7. College Practical Chemisty by H. N. Patel, S. R. Jakali, H. P. Subhedar, Miss. S. P.
Turakhia. Himalaya Publishing House, Mumbai.
8. College Practical Chemistry by Patel, Jakali, Mohandas, Israney, Turakhia. Himalya
Publishing house.
9. Experiments in General Chemistry by C. N. R. Rao. Affiliated East –West Press Private
Ltd., Delhi.
PRACTICAL - III
PHYSICAL CHEMISTRY EXPERIMENTS
1. Determination of partition coefficient of Iodine between Carbon tetra chloride and
water.
2. Determination of partition coefficient of Iodine between Benzene and Water.
3. Determination of equilibrium constant for the reaction between potassium iodide
and Iodine.
4. Determination of rate constant of acid – catalyzed hydrolysis of an ester (Methyl
acetate or Ethyl acetate).
5. Determination of Kf / molecular weight by Rast method – Naphthalene, Diphenyl,
and m – dinitrobenzene as solvents.
6. Determination of critical solution temperature of Phenol – Water system.
7. Determination of concentration of an electrolyte ( NaCl / KCl / succinic acid).
8. Determination of transition temperature of sodium acetate, sodium thiosulphate and
SrCl2.6H2O.
9. Phase Diagram – Simple Eutectic system.
10. Determination of cell constant, specific conductivity and equivalent conductivity of
strong electrolyte.
11. Determination of dissociation constant of a weak acid ( acetic acid )
12. Conductometric titrations, strong – acid – strong base.
13. Potentiometric titrations. Acid – base HCl Vs NaOH.
Reference Books:
1. Experimental Physical Chemistry by A. Findlay. Longman.
2. Advanced Practical Physical Chemistry by J.B. Yadav. (Goel Publishing house,
Meerut).
3. Experiments in Physical Chemistry by R. C. Das and B. Behra. Tata Mc Graw Hill.
4. Advanced experimental Chemistry Vol. I. Physical by J. N. Gurtu and R. Kapoor. S.
Chand & Co.
5. Experiments in Physical Chemistry by J. C. Ghosh, Bharati Bhavan.
6. Practical book of Physical Chemistry – by Nadkarni Kothari & Lawande. Bombay
Popular Prakashan.
7. Systematic Experimental Physical Chemistry – by S. W. Rajbhoj, Chondhekar. Anjali
Publication.
8. Practical Physical Chemisty – by B. D. Khosala & V. C. Garg. R. Chand & Sons.
9. Experiments in Chemistry by D. V. Jagirdar.
10. Practical Chemistry, Physical – Inorganic – Organic and Viva – voce by Balwant Rai
Satija. Allied Publishers Pvt. Ltd.
11. College Practical Chemistry by H. N. Patel, S. R. Jakali, H. P. Subhedar, Miss. S. P.
Turakhia. Himalaya Publishing House, Mumbai.
12. College Practical Chemistry by Patel, Jakali, Mohandas, Israney, Turakhia. Himalaya
Publishing Housing, Mumbai.