JAI HIND COLLEGE AUTONOMOUS Syllabus for F.Y.BSc Course : Chemistry Semester : I Credit Based Semester & Grading System With effect from Academic Year 2018-19 1
List of Courses Course: Chemistry Semester: I SR. NO. COURSE CODE COURSE TITLE NO. OF LECTURES / WEEK NO. OF CREDITS FYBSc 1 2 3 SCHE101 SCHE102 SCHE1PR Semester I Concepts of Physical and Inorganic Chemistry - I Fundamentals of Organic and Inorganic Chemistry Practical Course work in Chemistry - I 3 2 3 2 6 2 4 5 6 SCHE201 SCHE202 SCHE2PR Semester II Concepts of Physical and Inorganic Chemistry - II Concepts of Organic and Co-ordination Chemistry Practical Course work in Chemistry - I 3 2 3 2 6 2 2
Semester I Theory Course: SCHE101 Concepts of Physical and Inorganic Chemistry - I (Credits: 2 Lectures/Week: 3) Course description: Concepts of the Laws of Thermodynamics, Reaction Kinetics, Atomic Structure & Basics of Quantum Mechanics Objectives: To understand the fundamental concepts of thermodynamics: interrelationships of variables and their practical applications through problem solving To understand kinetics of various reactions: parameters involved, determination of order by various methodologies and practical applications To clarify the basics of atomic structure using quantum mechanics: shapes of orbital To understand the special features of the quantum mechanical model of an atom and to define an atomic orbital in terms of its quantum numbers Unit I Unit II Unit I: Thermodynamics: a) Basic Concepts in Thermodynamics i. Types of systems ii. Properties of system iii. State and state system iv. Types of processes b) Concept of Heat and Work c) First Law of Thermodynamics i. Internal energy, Enthalpy ii. Heat capacity, Relation between Cp and Cv in gaseous state iii. Joule Thomson effect (Qualitative discussion and experimentation) iv. Work done for adiabatic and isothermal processes d) Second Law of Thermodynamics i. Carnot Cycle-Heat engine, Mechanical efficiency e) Concept of Entropy i. Relationship between Enthalpy and Entropy changes for reversible and irreversible processes ii. Physical significance of entropy iii. Entropy and spontaneity iv. Entropy changes for Fusion, Vaporization and transition (Numerical expected ) Unit II: Chemical Kinetics a) Rate of Reaction i. Definition and measurement of rate constant ii. Order of reaction iii. Molecularity of reaction iv. Integrated rate equation for zero, first and second order 3
Unit III reactions (only a = b) b) Determination of Order of Reaction i. Integration method ii. Graphical method iii. Half time method iv. Ostwald s Isolation method c) Arrhenius equation i. Effect of temperature on reaction rates ii. Energy of activation d) Types of Complex Chemical Reactions i. Reversible ii. Consecutive iii. Parallel iv. Thermal chain reaction (only examples: no derivation) e) Catalysis i. General features of a catalyst ii. Classification iii. Examples of catalyzed reactions (Numerical expected) Unit III: Atomic Structure & Basics of Quantum Mechanics in Inorganic Chemistry a) Historical perspectives of the Atomic Structure i. Bohr s theory and its limitations ii. Dual behaviour of matter and radiation iii. de Broglie s relation iv. Heisenberg s Uncertainty Principle v. Hydrogen atom spectra vi. Need for a new approach to Atomic Structure b) Basic principles of Quantum Mechanics i. Time independent Schrodinger s Equation; meaning of various terms involved ii. Significance of ψ 1 and ψ 2 iii. Schrödinger s equation for hydrogen atom (derivation not required) iv. Radial and angular parts of the hydrogenic wave function (atomic orbital) and their variations for 1s, 2s, 2p, 3s, 3p and 3d orbital (Graphical representation only) v. Radial and angular nodes and their significance vi. Radial distribution functions and concept of the most probable distance (special reference to 1s and 2s atomic orbital) vii. Significance of quantum numbers, orbital angular momentum and quantum numbers m1 and ms. 4
viii. Shapes of s, p and d atomic orbital, nodal planes ix. Discovery of spin, spin quantum number (s) and magnetic spin quantum number (ms) c) Aufbau s principle i. Rules for filling electrons in various orbitals ii. Electronic configurations of different atoms iii. Stability of half-filled and completely filled orbitals iv. Concept of exchange energy v. Relative energies of atomic orbital vi. Anomalous electronic configurations References: Unit 1 & 2 1. Barrow, G.M., Physical Chemistry, (6th Edition), Tata McGraw Hill Publishing Co. Ltd. New Delhi 2. Levine, I. N., Physical Chemistry, (6th Ed. 2010), Tata McGraw Hill 3. Puri, B. R., Sharma, L.R., Pamania, M.S., Physical Chemistry, (45 th Ed.), Vishal Publishing Co. 4. Glaston & Lewis, Principles of Physical Chemistry 5. Atkins P. W., and Paula J. De, Physical Chemistry, 10 th ed., Oxford University, 12 press (2014)5. 6. Kapoor, K.L. Textbook of Physical Chemistry, (2006) McMillan Publishers 7. K. J. Laidler, Chemical Kinetics 3 rd Ed., Pearson Education. Unit 3 1. Lee, J.D. Concise Inorganic Chemistry, (1991), ELBS 2. Douglas, B.E. and McDaniel, D.H., (1970), Concepts & Models of Inorganic Chemistry 3. Prakash,S., Tuli, G.D., Basu, S.K., Madan, R.D., Advanced Inorganic Chemistry, Volume I 4. Day, M.C. and Selbin, J., (1962), Theoretical Inorganic Chemistry, ACS Publications 5. James E. Huheey, Inorganic Chemistry, (1983), Harper & Row Publishers, Asia 6. Shriver, D.F., P.W. Atkins, C. H. Langford, 3rd edition, Inorganic Chemistry, Oxford University Press 7. Bahl, Tuli and Anand, Advanced Inorganic Chemistry, Volume I and II 8. Manas Chanda, Atomic structure and Chemical Bond: Including Molecular spectroscopy, (1972), McGraw-Hill Inc, US 5
Course: SCHE102 Fundamentals of Organic and Inorganic Chemistry (Credits: 2 Lectures/Week: 3) Course description: Nomenclature, stereo-electronic effects, stereochemistry of simple organic compounds; and modern periodic table, concept of qualitative analysis Objectives: To correlate the systematic name with the structure of organic compound; differentiate and rationalize the bond strength, bond dissociation and therefore, reactivity of different classes of organic compounds To apply the different parameters of stereo-electronic effects in organic reactions To correlate the chemical properties of elements with their position in the periodic table To apply the concept of the solubility product and ph of the medium on precipitation of ionic compounds Unit I Unit I: Fundamentals of organic chemistry, Saturated hydrocarbons and Halogenated derivatives Basic Concepts in Thermodynamics 1. General Organic Chemistry I a) Nomenclature of poly functional organic compounds on the basis of priority order, of the following classes: v. Aliphatic vi. Alicyclic vii. Aromatic compounds b) Electronic Effects i. Inductive Effect ii. Electromeric Effect iii. Mesomeric Effect iv. Hyperconjugative Effect c) Applications of stereo electronic effects in determining acidity and basicity i. Concept of Ka, Kb and pka, pkb ii. Comparative study of acidity and basicity of different classes of organic compounds: Carboxylic acids, Phenols, iii. Alcohols, Aliphatic amines, Aromatic amines Other factors affecting acid/base strength: H-Bonding, steric effects and solvation 2. Chemistry of Saturated Aliphatic Hydrocarbons a) Alkanes i. Preparation: Catalytic hydrogenation, Wurtz reaction, Kolbe s synthesis, Reduction of alkyl halides (Mechanism not expected) ii. Physical Properties b) Petroleum as an energy source i. Composition ii. Octane and Cetane number iii. Knocking & anti-knocking agents 6
iv. Alternative Green fuels c) Haloalkanes i. Nucleophilic substitution: SN 1, SN 2 & SN i ; Mechanism and Stereochemistry ii. Factors affecting nucleophilic substitution: Substrate, Solvent, Reagent, Leaving group Unit II: Stereochemistry - I Unit II 1. Stereo-chemical Modelling a) 2D models i. Projection Formula: Wedge-Dot, Fischer, Newmann, Sawhorse ii. Interconversions of projection formula b) 3D models i. Ball-stick & space fill models 2. Conformation a) Conformational analysis of alkanes i. Ethane ii. Propane iii. n-butane 3. Configuration a) Geometrical isomerism in alkenes i. Stereochemical descriptor: cis/trans; E/Z b) Optical isomerism i. Chirality, asymmetry, stereogenecity ii. Enantiomers, diastereomers & meso isomers iii. Compounds with multiple stereogenic centres- number of possible stereoisomers iv. Configurational descriptor for compounds not containing more than 2 stereogenic centres (D/L; erythro/threo; synanti; R/S) 4. Optical activity i. Plane Polarized Light ii. Polarimeter iii. Specific rotation iv. Racemic mixture (external compensation) v. Resolution (methods of resolution not expected) vi. Optical purity (calculation of ee) Unit III: General trends and Properties of Modern Periodic Table & concept of Qualitative Analysis Unit III 1. Modern Periodic Table a) Long form of Periodic Table: Classification of elements into 7
References: Unit 1 & 2 Unit 3 main group, transition elements and inner transition elements b) Periodicity in properties: i. Atomic size and Ionic size ii. Electron gain enthalpy iii. Ionization enthalpy iv. Effective nuclear charge (Slater s rule) v. Electronegativity: Pauling, Mulliken and Alred Rochow electronegativity (Numerical problems expected, wherever applicable) c) Comparative study of 's' block elements: i. Study of general trends in the properties of these elements with respect to family relationship ii. Physical and chemical properties iii. Ionic potential iv. Polarizing power and Hydration energy of their ions v. Anomalous behaviour of Li & Be vi. Diagonal relationship of Li & Mg 2. Concept of Qualitative Analysis i. Testing of Gaseous Evolutes ii. Role in qualitative analyses: Papers impregnated with reagents (Starch iodide, potassium dichromate, lead acetate, dimethyl glyoxime and oxine reagents) iii. Precipitation equilibria iv. Solubility product v. Common ion effect vi. Uncommon ions vii. Oxidation states viii. Buffer action ix. Complexing agents for precipitation of ionic compounds 1. Morrison, R. T.; Boyd, R. N. (2012). Organic Chemistry. Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). 2. Finar, I. L. (2012). Organic Chemistry (Volume 1). Dorling Kindersley (India) Pvt. Ltd. (PearsonEducation). 3. Solomons, T.W.G. (2009).Organic Chemistry. John Wiley & Sons, Inc. 4. Kalsi, P. S. (2005) Stereochemistry Conformation and Mechanism. New Age International 5. Ahluwalia, V.K.; Parashar, R.K. (2006) Organic Reaction Mechanisms. Narosa Publishing House. 6. Mukherji; Singh; Kapoor. (2002) Reaction Mechanisms in Organic Chemistry.McMillan 1. Shriver, D. F. and Atkins, P. W. 1999, Inorganic chemistry, 3 rd Ed., Oxford University Press, 8
2. Jolly, W. L., 1993, Modern inorganic chemistry, McGraw Hill Book Co. 3. Douglas, B. E. and McDaniel, H., Concepts and models in inorganic chemistry, 1994,3 rd Ed., John Wiley & Sons, Inc., New York, 4. Huheey, J.E., 1993, Inorganic Chemistry, Prentice Hall. 5. Lee, J.D., 1993, Concise Inorganic Chemistry, ELBS 6. Shriver & Atkins, ( 1994) Inorganic Chemistry, Third Edition, Oxford Press 9
Semester I Practical Course: SCHE1PR Practical Course work in Chemistry-I (Credits: 2 Practicals/Week: 2) Course description: Practical Course work on Chemical Kinetics, Thermodynamics, Titrimetric Calculations, Qualitative & Quantitative Analysis in Inorganic Chemistry, Purification of Organic Compounds and determination of Physical Constants, Factors affecting Nucleophilic Substitution reactions, Virtual Lab Experiments Learning Objectives: To determine the order of reaction; measurement of enthalpy To solve numerical problems based on basic concepts involving quantitative analysis To apply the concept of solubility product and ph in the formation of a precipitate in semi micro analysis To understand titrimetric analysis using different indicators operating at various ph ranges To determine various physical constants of an organic compound To apply the concepts of nucleophilic substitution in understanding the reactivity of different substrates PRACTICAL I A. Principles of Calculations a) Molarity, Normality, Mole fraction, Dilution of solution, ppm, ppb (Problem solving) b) Concept of primary and secondary standard c) Preparation of 0.1N succinic acid solution and subsequent standardization of the given NaOH solution B. Chemical Kinetics a) To determine the rate constant & order for hydrolysis of ester using HCl as a catalyst (graphically, calculations & using method of equifraction of times) b) To study the base catalyzed hydrolysis (saponification) of ethyl acetate and to evaluate rate constant by calculative and graphical method C. Thermodynamics a) To determine the enthalpy of dissociation of salts like NH 4Cl and CaCl 2 PRACTICAL II A. Qualitative Analysis a) Semi-micro analysis of not more than four ionic species (two cation and two anion) (Cations:NH4 +, K +, Ag +, Pb +2, Cd +2, Fe +3, Al +3, Co +2, Cr +3, Ni +2, Mn +2, Zn +2, Sn +2, Cu +2, Bi +3, Ba +2, Sr +2, Ca +2 Anions: CO3-2, NO3 -, C2O4 2-, NO2 -, S -2, SO4-2, PO4-3, BO3 2-, CH3COO -, Cl -, Br -, F -, I - ) B. Quantitative Analysis a) Estimation of the amount of sodium carbonate and sodium hydrogen 10
carbonate present in a mixture b) Estimation of Fe(II) ions by titrating it with potassium dichromate using internal indicator PRACTICAL III A. Determination of Physical Constant a) Melting point, Boiling point, Mixed melting point of organic compounds b) Specific rotation of a given optically active compound using Polarimeter B. Purification of organic compounds a) Recrystallisation using different solvents b) Confirmation of purity by Melting point C. Virtual Lab Experiment a) Nomenclature and Structure of organic compounds using Chemsketch 11
Semester II Theory Course: SCHE201 Concepts of Physical and Inorganic Chemistry - II (Credits: 2 Lectures/Week: 3) Course description: States of Matter, Ionic Equilibria, Chemical Bonding and Molecular Structure Objectives: To understand the theoretical principles of the states of matter, their properties and various applications To understand the concept of ionic equilibria, ph, theory of ionic products, theory of acids and bases, theory of indicators, solubility product & their practical applications To understand the importance of the Periodic Table of elements, historical perspective, and role in organization of chemical information To create and label models of atoms, writing and balancing of chemical equations Unit I: States of matter Unit I a) Gaseous state i. Ideal gas behaviour and kinetic theory of gases (only postulates) ii. Distribution of molecular speed (Maxwell Boltzmann s plot) iii. Real gases: Compressibility factor, Boyle s temperature, van der Waal s equation of state iv. Liquefaction of gases (Numerical expected) b) Liquid state i. Introduction ii. Liquid-vapour equilibrium (vapour pressure) iii. Surface tension: determination using stalagmometer, effect of temperature on surface tension, parachor and its applications iv. Viscosity : measurement using Ostwald s viscometer, effect of temperature on viscosity v. Refractive index: molar refraction and polarizability, determination using Abbe s refractometer vi. Liquid crystals :Introduction, classification and applications (Numerical expected) Unit II: Ionic Equilibria Unit II a) Strong, moderate and weak electrolytes: i. Ionization constant and ionic product of water ii. ph scale iii. Common ion effect iv. Dissociation constant of mono-, di- and tri-protic acid v. Buffer solution, buffer capacity and buffer action vi. Henderson s equation for acidic and basic buffer vii. Applications of buffer in biochemical processes 12
b) Hydrolysis of salts i. Hydrolysis constant, degree of hydrolysis c) Theory of acid-base indicators Action of phenolphthalein and methyl orange d) Solubility and solubility product of sparingly soluble salts i. Applications of principles of solubility product e) Ionic equilibria involving complex ions (Numerical expected) Unit III: Chemical Bonding and Molecular Structure Unit III a) Chemical bond i. Introduction ii. Octet rule b) Ionic Bonding i. General characteristics of ionic bonding ii. Energy considerations in ionic bonding; lattice and solvation energy and their importance in the context of stability and solubility of ionic compounds iii. Statement of Born-Landé equation for calculation of lattice energy iv. Born-Haber cycle and its applications v. Polarizing power and polarizability vi. Fajan s rules, ionic character in covalent compounds, vii. Bond moment, dipole moment and percentage ionic character c) Covalent bonding i. VB Approach: Shapes of some inorganic molecules and ions on the basis of VSEPR and hybridization with suitable examples of linear, trigonal planar, square planar, tetrahedral, trigonal bipyramidal and octahedral arrangements. ii. Concept of resonance and resonating structures in various inorganic and organic compounds References: Unit 1 & 2 1. Barrow, G.M., Physical Chemistry, (6th Edition), Tata McGraw Hill Publishing Co. Ltd. New Delhi 2. Levine, I. N., Physical Chemistry, (6th Ed. 2010), Tata McGraw Hill 3. Puri, B. R., Sharma, L.R., Pamania, M.S., Physical Chemistry, (45 th Ed.), Vishal Publish Co. 4. Glasston & Lewis, Principles of Physical Chemistry 13
5. Atkins P. W., and Paula J. De, Physical Chemistry, 10 th ed., Oxford University, 12 press (2014)5. 6. Kapoor, K.L. Textbook of Physical Chemistry, (2006) McMillan Publishers 7. K. J. Laidler, Chemical Kinetics 3 rd Ed., Pearson Education Unit 3 1. Lee, J.D. Concise Inorganic Chemistry, (1991), ELBS 2. Douglas, B.E. and McDaniel, D.H., (1970), Concepts & Models of Inorganic Chemistry 3. Prakash,S., Tuli, G.D., Basu, S.K., Madan, R.D., Advanced Inorganic Chemistry, Volume I 4. Day, M.C. and Selbin, J., (1962), Theoretical Inorganic Chemistry, ACS Publications 5. James E. Huheey, Inorganic Chemistry, (1983), Harper & Row Publishers, Asia 6. Shriver, D.F., P.W. Atkins, C. H. Langford, 3rd edition, Inorganic Chemistry, Oxford University Press 7. Bahl, Tuli and Anand, Advanced Inorganic Chemistry, Volume I and II 8. Manas Chanda, Atomic structure and chemical bond: Including Molecular spectroscopy, (1972), McGraw-Hill Inc, US 14
Course: SCHE202 Concepts of Organic and Coordination Chemistry (Credits: 2 Lectures/Week: 3) Course description: Reactive Intermediates, Aromaticity, Orientation effect in electrophilic aromatic substitution, Basic concepts of Coordination Chemistry and compounds of transition metal elements Objectives: To list different reactive intermediates and reason their relative stabilities To define the parameters required for aromaticity To propose the orienting influence of a group in electrophilic aromatic substitution based on electron density To relate the methods of preparation and reactions of unsaturated aliphatic hydrocarbons and oxygenated derivatives of aliphatic and aromatic systems To discuss the chemistry of formation of transition metal compounds; an introduction to coordination chemistry and to understand the salient features of coordination compounds Unit I: Reactive Intermediates & reactivity of aromatic compounds Unit I 1. General Organic Chemistry II a) Reactive Intermediates: structure shape & relative stability i. Carbocations ii. Carbanions iii. Free radicals iv. Carbenes b) Reactivity of organic molecules i. Nucleophiles & basicity ii. Electrophiles & Acidity c) Reactions involving Intermediates i. Carbocations- Acid catalysed hydration of alkenes, Friedel- Crafts alkylation reaction ii. Carbanions- homologation of terminal alkynes; iii. Free radical- Halogenation of alkane, selectivity rules (Mechanism expected) 2. Chemistry of Aromatic Compounds- I a) Aromaticity i. Conditions of aromaticity ii. Huckel's Rule iii. Aromaticity of arenes & arenium ions b) Electrophilic Aromatic Substitution i. ESR- nitration, sulphonation, halogenation (w.r.t. reagents & reaction conditions) ii. iii. Activating, deactivating groups Orientation effect (mono & disubstituted) based on electron density 15
Unit II Unit III Unit II: Unsaturated aliphatic hydrocarbons & compounds containing oxygen- I 1. Chemistry of unsaturated aliphatic hydrocarbons a) Alkenes i. Preparation- dehydration of alcohols & dehydrohalogenation of alkyl halides (Saytzeff rule) ii. Reactions: cis-addition (alkaline KMnO4, OsO4) transaddition (bromine, ring opening of epoxides); addition of HX (Markownikoff's & anti-markownikoff's addition), hydration, ozonolysis, oxymercuration-demercuration, hydroboration-oxidation b) Alkynes i. Preparation- acetylene from CaC2 (applications in fruit ripening); by dehalogenation of tetra halides & dehydrohalogenation of vicinal dihalides ii. Reactions: hydration, addition of bromine & alkaline KMnO4, ozonolysis & oxidation 2. Chemistry of alcohols, phenols & ethers a) Alcohols i. Preparation- Industrial preparation (fermentation), using Grignard reagent, using hydride reducing agents ii. Reactions- with sodium, HX (Lucas test), esterification, oxidation b) Phenols i. Preparation- Cumene hydroperoxide method ii. Reactions- O-alkylation & O-acylation; Schotten Baumen reaction, Fries rearrangement, Claisen rearrangement c) Ethers i. Preparation- Williamson's synthesis ii. Reactions- cleavage of ethers with HI iii. Uses- ethers as solvents (THF, diethyl ether) in organic synthesis Unit III: Comparative chemistry of p-block & transition elements; Co-ordination chemistry 1. Comparative chemistry of p-block elements a) Group 13 elements i. Trends in periodic properties ii. iii. Inert pair effect Chemistry of aluminium compounds: halides, oxides and alkyls b) Group 14 elements i. Trends in periodic properties ii. Catenation iii. Allotropy 16
iv. Uses and applications References: Unit 1 & 2 Unit 3 2. Chemistry of Transition Elements (3d series) i. General group trends with special reference to electronic configuration ii. Variable valency & Colour iii. iv. Magnetic and Catalytic property Ability to form complexes and Stability of various oxidation states (Latimer diagrams) for Mn, Fe &Cu 3. Coordination Chemistry a) Introduction & nomenclature i. Basic terms ii. Nomenclature of Coordination compounds iii. Types of ligands iv. Evidence for the formation of coordination compounds b) Theories of Coordination Chemistry i. Werner theory and EAN rule ii. Structural and stereo isomerism of complexes with 4 & 6 coordination numbers iii. iv. Valence Bond Theory (VBT) approach Inner and outer orbital complexes of Cr, Fe, Co, Ni and Cu (coordination numbers 4 and 6) v. Electro-neutrality principle and back bonding vi. Limitations of VBT 1. Morrison, R. T.; Boyd, R. N. (2012). Organic Chemistry. Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). 2. Finar, I. L. (2012). Organic Chemistry (Volume 1). Dorling Kindersley (India) Pvt. Ltd. (PearsonEducation). 3. Solomons, T.W.G. (2009).Organic Chemistry. John Wiley & Sons, Inc. 4. Ahluwalia, V.K.; Parashar, R.K. (2006) Organic Reaction Mechanisms. Narosa Publishing House. 5. Mukherji; Singh; Kapoor. (2002) Reaction Mechanisms in Organic Chemistry, McMillan 1. Banerjea, D., 1993, Coordination chemistry, Tata McGraw Hill, New Delhi 2. Shriver, D. F and Atkins, P. W., 1999, Inorganic chemistry, 3 rd Ed., Oxford University Press 3. W. L. Jolly, 1993, Modern inorganic chemistry, McGraw Hill Book Co. 4. Douglas, B. E. and McDaniel, H., Concepts and models in inorganic chemistry, 1994,3 rd Ed., John Wiley & Sons, Inc., New York 5. Huheey, J.E., 1993,Inorganic Chemistry, Prentice Hall 6. Lee, J.D., 1993, Concise Inorganic Chemistry, ELBS 7. Shriver & Atkins,( 1994) Inorganic Chemistry, Third Edition, Oxford Press. 17
Semester II Practical Course: SCHE2PR Practical Course work in Chemistry-II (Credits: 2 Practicals/Week: 2) Course description: Viscosity, Surface tension, Ionic Equilibria, Indicators, Gravimetric Analysis, Preparation of Inorganic Complexes, Basics of Identification of Organic Compounds, One-Step Synthesis, Chromatography Learning Objectives: To develop the skill of observation, understanding and analysis of data To apply the concept of indicators in determining the ph and strengths of solutions To perform the quantitative preparation of coordination complexes with different types of ligands To apply the concept of gravimetric analysis in determining the percentage purity of a sample To perform preliminary investigations including solubility profile and element detection of mono-functional organic compounds To develop the skills for one-step synthesis of organic compounds PRACTICAL I A. Viscosity To determine the viscosity of aqueous solutions at room temperature using Ostwald s Viscometer: (any 2) i. Polymer ii. Ethanol iii. Sugar B. Surface tension (Demonstrative experiment) To determine the surface tension of a given liquid using stalagmometer C. Ionic Equilibria To determine the ph of various concentrations of sodium acetate and acetic acid buffer solutions PRACTICAL II A. Gravimetric analysis a) To determine the percentage purity of a sample of barium sulphate, containing ammonium chloride as impurity. b) To estimate the amount of sodium carbonate & bicarbonate in a mixture gravimetrically. B. Preparation of inorganic complexes (any two) a) Tetraamine copper (II) sulphate b) Nickel DMG c) Potassium trioxalato ferrate(ii) 18
PRACTICAL III A. Basics of Identification of Organic compounds a) To determine the solubility profile and elements (N, S, X) present in a given organic compound. B. One-step synthesis a) Comparative analysis of the procedure of nitration re action on different substrates: i. Nitration of nitrobenzene ii. Nitration of acetanilide C. Chromatography (Demonstrative experiment) a) Paper chromatography b) Thin layer chromatography of ortho- and para-nitrophenol 19
Evaluation Scheme A. Evaluation scheme for Theory courses I. Continuous Assessment ( C.A.) - 40 Marks (i) C.A.-I : Test 20 Marks of 40 mins. duration (ii) C.A.-II : Assignment/ Poster for 20 marks II. Semester End Examination ( SEE)- 60 Marks B. Evaluation scheme for Practical courses I. Internal Assessment - 40 Marks: Journal/Viva/Experiment Scheme II. Semester End Examination ( SEE)- 60 Marks 20