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 Paper - 1 mbg;gilj;jkpo; - jhs; - 1 nra;As;> ,yf;fzf;Fwpg;G> rpWfij> nghJfl;Liu> nkhopj;jpwd; : - I. II. nra;As; : 1. jkpo;j;;jha; tho;j;J 2. jpUf;Fws; 3. gonkhopehD}W 4. ghujpahh; ftpijfs; 5. ghujpjhrd; ftpijfs; 6. ftpkzp 7. jpUf;Fw;whyf;FwtQ;rp 8. trp\;lejp 9. eh. fhkuh[d; 10. ituKj;J ,yf;fzf;Fwpg;G ( nra;As; kl;Lk; ) III. rpWfij ( Kj;Jf;fijfs; gjpd;kh; njhFg;G ) IV. nghJfl;Liu V. 1. rKjhak; 2. ,yf;fpak; 3. mwptpay; nkhopj;jpwd; Paper – 2 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.