IEC UNIVERSITY DEPARTMENT OF CHEMISTRY of...Inorganic Chemistry – IV 3 0 0 20 40 0 60 40 100 4 2. HBCH 502 Organic Chemistry-IV 3 0 0 20 40 0 60 40 100 4 3. HBCH 503 Physical Chemistry

IEC UNIVERSITY

DEPARTMENT OF CHEMISTRYSYLLABUS

BACHELOR OF SCIENCES

IN

CHEMISTRY (HONS) Session 2014-17

SCHOOL OF APPLIED AND BASIC SCIENCES

I.E.C UNIVERSITY, BADDI, SOLAN

HIMACHAL PRADESH,

PIN-174103, INDIA

Course Structure B. Sc. (Hons) ChemistryB.Sc. (Hon) Chemistry Three Years Programme Curricula

First Semester Periods Internal ExtS.

No.Sub Code Subject L T P CA MST P Total Total Sub

TotalCredits

1. HBCH-101

Inorganic Chemistry-I

3 0 0 20 40 0 60 40 100 3

2. HBCH-102

Physical Chemistry -I

3 0 0 20 40 0 60 40 100 3

3. HBCH-103

Foundation English

3 0 0 15 30 0 45 30 75 3

4. HBCH-104

Basic Mathematics

4 0 0 20 40 0 60 40 100 3

5. HBCH 151 P

Inorganic Chemistry Lab I

0 0 4 0 0 30 30 20 50 2

6 HBCH 152 P

Physical Chemistry Lab I

0 0 4 0 0 30 30 20 50 2

7 HBCH-153 P

Communication lab

0 0 4 0 0 15 15 10 25 1

Total 13 0 12 75 150 75 300 200 500 17

B.Sc. (Hon) Chemistry Three Years Programme CurriculaSecond Semester Periods Internal Ext

S. No.

Sub Code Subject L T P CA MST P Total Total Sub Total

Credits

1. HBCH 201

Organic Chemistry –I

3 0 0 20 40 0 60 40 100 3

2. HBCH 202

Analytical Methods in Chemical Analysis

3 0 0 20 40 0 60 40 100 3

3. HBCH203

Physics-I 4 0 0 20 40 0 60 40 100 3

4. HBCH 204

Biology-I 3 0 0 20 40 0 60 40 100 3

5 EVS-101

Environmental Sciences and Technology

3 0 0 20 40 0 60 40 100 3

6 HBCH 251 P

Organic Chemistry Lab-I

0 0 4 0 0 30 30 20 50 2

7 HBCH 252 P

Analytical Methods in Chemical Analysis Lab-I

0 0 4 0 0 30 30 20 50 2

8 HBCH 253 P

Physics-I lab 0 0 4 0 0 30 30 20 50 2

Total 15

0 12 100 200 90 390 260 650 22

B.Sc. (Hon) Chemistry Three Years Programme CurriculaThird Semester Periods Internal Ext

S. No.


Credits

1. HBCH 301

Inorganic Chemistry – II

3 0 0 20 40 0 60 40 100 4

2. HBCH 302

Organic Chemistry-II

3 0 0 20 40 0 60 40 100 4

3. HBCH 303

Physical Chemistry – II

3 0 0 20 40 0 60 40 100 4

4. HBCH 304

Numerical Analysis

4 0 0 20 40 0 60 40 100 4

5. HBCH 351 P

Inorganic Chemistry Lab-II

0 0 4 0 0 30 30 20 50 2

6 HBCH 352 P

Organic Chemistry Lab-II

0 0 4 0 0 30 30 20 50 2

7 HBCH 353 P

Physical Chemistry Lab-II

0 0 4 0 0 30 30 20 50 2

Total 10 0 12 80 160 90 330 220 550 22

B.Sc. (Hon) Chemistry Three Years Programme CurriculaFourth Semester Periods Internal

ExtS. No.


Credits

1.HBCH 401 Inorganic

Chemistry – III3 0 0 20 40 0 60 40 100 4

2. HBCH 402

Organic Chemistry-III

3 0 0 20 40 0 60 40 100 4

3. HBCH 403

Physical Chemistry – III

3 0 0 20 40 0 60 40 100 4

4. HBCH - 404

Physics-II 4 0 0 20 40 0 60 40 100 4

5. HBCH 451 P

Inorganic Chemistry Lab-III

0 0 4 0 0 30 30 20 50 2

6 HBCH 452 P

Organic Chemistry Lab-III

0 0 4 0 0 30 30 20 50 2

7 HBCH 453 P

Physical Chemistry Lab-III

0 0 4 0 0 30 30 20 50 2

8 HBCH 454P

Physics-II lab 0 0 4 0 0 30 30 20 50 2

Total 10 0 16 80 160 120 360 240 600 24

B.Sc. (Hon) Chemistry Three Years Programme CurriculaFifth Semester Periods Internal Ext

S. No.


Credits

1. HBCH 501

Inorganic Chemistry – IV

3 0 0 20 40 0 60 40 100 4

2. HBCH 502

Organic Chemistry-IV

3 0 0 20 40 0 60 40 100 4

3. HBCH 503

Physical Chemistry – IV

3 0 0 20 40 0 60 40 100 4

4.HBCH 504

Biochemistry and Environmental Chemistry

3 0 0 20 40 0 60 40 100 4

5. HBCH 551 P

Inorganic Chemistry Lab-IV

0 0 4 0 0 30 30 20 50 2

6 HBCH 552 P

Organic Chemistry Lab-IV

0 0 4 0 0 30 30 20 50 2

7 HBCH 553 P

Physical Chemistry Lab-IV

0 0 4 0 0 30 30 20 50 2

Total 12 0 12 80 160 90 330 220 550 22

B.Sc. (Hon) Chemistry Three Years Programme CurriculaSixth Semester Periods Internal

ExtS.

No.Sub Code Subject L T P CA MST P Total Total Sub

TotalCredits

1. HBCH 601

Inorganic Chemistry – V

3 0 0 20 40 0 60 40 100 4

2. HBCH 602

Organic Chemistry-V 3 0 0 20 40 0 60 40 100 4

3. HBCH 603

Physical Chemistry – V

3 0 0 20 40 0 60 40 100 4

4.HBCH-604

Applications of Computers in Chemistry

3 0 0 15 30 0 45 30 75 4

5. HBCH 651 P

Inorganic Chemistry Lab-V

0 0 4 0 0 30 30 20 50 2

6 HBCH 652 P

Organic Chemistry Lab-V

0 0 4 0 0 30 30 20 50 2

7 HBCH 653 P

Physical Chemistry Lab-V

0 0 4 0 0 30 30 20 50 2

8 HBCH-654 P

Computer lab 0 0 4 0 0 15 15 10 25 1

Total 12 0 16 75 150 105 330 220 550 23

Note: L= Lecture, T = tutorial, P = Practical, CA = Class assessment, MST = Mid sem test, Ext = External

Semester-I Inorganic Chemistry - I

Paper- HBCH - 101 (L:3, credits) (Max marks (60+40) Time 3 hrs

THEORY Marks: 100

Note:-

The examiner will set question paper for 100 marks having three sections. Section A containing 10

questions for 2 marks; Section B containing 2 questions, each having 6 subparts of 5 marks, (student will

attempt any 4); Section C containing 2 questions each having 4 subparts of 10 marks (student will attempt

any 2).

UNIT- IAtomic Structure: Schrodinger’s Wave equation, Significance of Ψ and Ψ2. The four quantum numbers and their significance. Radial and angular probability. The shapes of s, p, d and f orbitals. Effective nuclear charge and shielding effect, Slater rules. Calculation of screening constant.

UNIT II

The Periodic Table and Chemical Periodicity Nomenclature of Inorganic compounds:

The relationship between chemical periodicity and electronic structure of the atom. The long form of the periodic Table – Classification of elements in s, p, d and f block of elements. Periodicity in oxidation state of valence, metallic/non-metallic character, oxidizing or reducing behaviour; acidic and basic character of oxides; Anomalous behaviour of elements of 2nd short period (Li to F) compared to other members in the same groups of s & p block elements. Effect of lanthanide contraction on the elements following lanthanides. The diagonal behavior between elements. The inert pair effect; variability of oxidation states of transition elements, colour, magnetic properties and other characteristics of transition elements.

UNIT- IIIThe s-block elements: Production and uses of metals (important); chemical reactivity and trends in alkali and alkaline earth metals; structure and properties of oxides, halides and hydroxides. Organometallic compounds of alkali metals, Crown and Crypts. Behaviour of solutions in liquid ammonia.

UNIT- IV

The p-block elements

Group III (i) Boron, Al, Ga, In, Ti family: Chemical reactivity and trends. Boron : Structures of crystalline boron, electronic and/or crystal structures of borides, boranes and carboranes, metallocarboranes and their chemistry. Boron halides. Boric acid, borates, boron-nitrogen compounds, LiAlH4 – its uses as a reducing and hydrogenating reagent, structure of alumina and aluminates.

Group IV

(ii) Carbon, Si, Ge, Sn, Pb family : Chemical reactivity and group trends Carbon : Allotropic forms, graphitic compounds, graphite intercalation compounds, carbides. Silicon : Silicon carbides, silicides, silanes and silylamines structures of silicate mineral, organo silicon compounds and silicones.

Suggested Books

1. Cotton F.A., Wilkinson G.W. and Gaus P.L., Basic Inorganic Chemistry, Pubs: John Wiley & Sons ,1987.2. Lee J.D., Concise Inorganic Chemistry, 4th edition, Pubs: ELBS,1991.3. Huheey J.E., Keiter E.A., Keiter R.L., Inorganic Chemistry: Principles of Structures and Reactivity; 4th Edition, Pubs: Harper Collins, 1993.4. Greenwood N.N. and Earnshaw A., Chemistry of the Elements, 2nd edition. Pubs: Butterworth/Heinemann, 1997.FURTHER READING:1. Cotton F.A. and Wilkinson G., Murillo C.A., Bochmann M., Advanced Inorg. Chemistry, 6th Edition, Pubs: John Wiley & Sons. Inc. 1999.2. Shriver D.F., Atkins F.W. and Langford C.M., Inorganic Chemistry; 3rd Edition, Pubs: Oxford University Press, 1999.3. Douglas B., Daniel D. Mc and Alexander J., Concepts of Models of Inorganic Chemistry, Pubs: John Wiley, 1987.4. Gray H.B., Electrons and Chemical Bonding, Pubs: W.A., J Benjamin Inc., 1965.

PHYSICAL CHEMISTRY-I

Paper- HBCH 102 (L:3, credits)(Max marks (60+40) Time 3 hrs

THEORY Marks: 100

Note:-




any 2).

UNIT- IEquation of State:

Kinetic molecular theory of gases, derivation of kinetic gas equation, deduction of gas laws from kinetic gas equation, imperfection in real gases, the compressibility of real gases, isotherms of real gases, equations of state, vander Waal’s equation, effect of attractive forces, Liquification of gases, critical phenomenon, P-V isotherms of carbondioxide, principle of continuity of state, vander Waal’s equation and critical constants, principle of corresponding states.

UNIT- IIThe First Law of Thermodynamics: Thermodynamic terms and basic concepts, Intensive and extensive properties, State functions and differentials, partial derivative relations, thermodynamic processes, reversibility, irreversibility, Nature of heat and work, Conservation of energy, various statements of first law, Manipulations of first law, internal energy (U) and enthalphy (H). Work done in reversible isothermal expansion, Molar heat capacity at constant pressure Cp and at constant volume CV, relation between Cp and Cv, work of adiabatic expansion, Joule Thomson effect.

UNIT- III

Solution and Colligative Properties:

Intermolecular forces in liquids, Vapour pressure and its determination, surface tension and determination of surface tension using capillary rise method and drop formation method, viscosity and measurement of viscosity–Ostwald method, refractivity and its measurement, Optical activity and its measurement using polarimeter.

Solutions of non-volatile solutes: colligative properties, elevation in boiling point, depression in freezing point, osmosis and osmotic pressure

UNIT-IV

Chemical Kinetics

Rate of reaction, rate constant and rate laws, the order of reaction, first, second & third and zero order reactions, half-lives; determination of reaction order. Temperature dependence of reaction rates, reaction mechanism, rate-determining step approximation, steady-state approximation.

Kinetics of Complex reactions: Reversible first order reactions, consecutive first order reactions, parallel first order reactions, Chain reactions. Catalysis, homogeneous catalysis, autocatalysis, oscillation reactions, bistability. Enzyme catalysis, heterogeneous catalysis.

Suggested Books

1. Physical Chemistry by P.W. Atkins, 8th Ed., Oxford University Press, 2006 (Indian Print).2. Physical Chemistry by T. Engel & P. Reid, 1st ed., Pearson Education, 2006.FURTHER READING:1. Physical Chemistry by Castellan, 3rd Ed., Addison Wisley/Narosa, 1985 (Indian Print)2. Physical Chemistry by G. M. Barrow, 6th Ed., New York, McGraw Hill, 1996.3. Physical Chemistry by R. J. Silbey, R. A. Albert & Moungi G. Bawendi, 4th Ed., New York: John Wiley,

2005.

FOUNDATION ENGLISH-I

Paper – HBCH -103 (L:3, credits) (Max marks (60+40) Time 3 hrs THEORY Marks: 100Note:-




any 2).

Unit I

Grammar: Patterns & Parts of speech Subject, Predicate, Noun, Pronoun, Adjective, Adverb, Verb, Preposition, Conjunction, Interjection , Active and Passive voice ,Homophones and homonyms , Punctuation.

Unit IICommunication: Meaning of communication, importance of communication, process of communication, Types of communication, Barriers to effective communication, Channels of communication, Modes of Communication, Language as a tool of communication.

Unit III Writing skills: Paragraph writing , Business letters: Placing an order , Complaint Letter, Adjustment Letter, Agenda and Minutes of meeting , Advertising , Note Making , Unseen Comprehension Passage.

Unit IVNon-verbal communication- Body language, personal appearance, posture, gesture, facial expression, eye contact, proxemics, haptics. Telephonic conversation- Dealing with difficult calls and callers, skills for making& receiving a call, problems of telephonic conversation.

Text-Books: 1. Wren & Martin, High School English Grammar & Composition – S. Chand & Co. Delhi. 2. Raman Meenakshi & Sharma Sangeeta, Technical Communication-Principles & Practice – O.U.P. New Delhi. 2007. 3. Mitra Barum K., Effective Technical Communication – O.U.P. New Delhi. 2006. 4. Better Your English- A Workbook for 1st year Students- Macmillan India, New Delhi. Reference Books:

1. Horn A.S., Guide to Patterns & Usage in English – O.U.P. New Delhi.

Mathematics – I (Basic Mathematics)

Paper - HBCH 104 (L: 3, 3 credits) (Max marks (60+40) Time 3 hours

THEORY Marks: 100Note:-




any 2).

UNIT-I

Equations Reducible to Quadratic Equations: Quadratic equations, Nature of roots, Method of solving a quadratic equation and equations reducible to quadratic equations.

Functions, Limit and Continuity: Type of functions, domain and range of a function, limit of a function, properties of limits, evaluation of limit of a function, continuity of a function at a point, Types of Discontinuity.

UNIT-IIDeterminants and Matrices: Determinants, Properties of determinants, application of determinants in solving a system of simultaneous linear equations, solution of non-homogenous system by Cramer’s rule. Matrices: Matrices, Types of matrices, Addition of matrices, Subtraction and multiplication of matrices, Transpose of matrix, Adjoint of matrix, Inverse of matrix, Unit matrix, solution of systems of linear equations by matrix method.(11 Hrs)

UNIT-IIIDifferentiation and Integration: Definition of Derivatives, formation of Derivatives, Law of derivatives, Delta method, chain rule, repeated derivatives, derivative of implicit functions and explicit functions. Integration: Integration, Graphical representation, Integration of algebraic Functions, logarithmic and exponential functions, integration of functions using substitution method, Integration by parts and partial fractions . (12 Hrs)

UNIT-IVTrigonometry: Measurement of angles, trigonometric ratios, Trigonometric functions of standard angles, Trigonometric ratios of complementary angles and supplementary angles, allied angles, compound angles, multiple and sub-multiple angles; Conditional identities. (6 Hrs)

Books RecommendedNote: Recent editions of the following books to be referred

1. Schaum's Differential Equations. Singapore: Mc Graw Hill. 2. Grewal BS. Higher Engineering Mathematics. New Delhi: Khanna Publishers.

Inorganic Chemistry - I

Paper – HBCH 151 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

1. Qualitative Analysis:

Qualitative analysis of inorganic mixtures containing not more than six radicals

2. Quantitative Analysis:

Volumetric Methods

(a) Acid-base titrations – Preparation of standard hydrochloric acid and sodium hydroxide solution. Preparation of some buffers and measuring their pH value, pH titration of unknown soda ash.

Reference text:

1. Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS.

Physical Chemistry - IPaper HBCH -152 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours 1. To determine the specific reaction rate of the hydrolysis of methyl acetate/ethyl acetate catalyzed by hydrogen

ions at room temperature.2. To determine the surface tension of a given liquid by drop number method. 3. To determine the viscosity of a given liquid.4. To determine the specific refractivity of a given liquid5. To determine the solubility of benzoic acid at various temperatures and to determine the ▲H of the

dissolution process6. To determine the enthalpy of solution of solid calcium chloride.7. To study the kinetics of hydrolysis of methyl acetate in the presence of hydrochloric acid.8. To study the effect of ionic strength (primary salt effect) on the kinetics of a reduction of toluidine blue with

sodium sulfite.9. To determine the molecular weight of a non-volatile substances by a cryoscopic method

COMMUNICATION LABPaper HBCH -153P (P: 1, 1 credits) (Max marks (30+20) Time 3 hours

1 Group Discussion2 Just a minutes session: Speaking Extempore for one minutes on given topics3 Reading aloud of newspaper headlines and important articles.4 Improving pronunciation through tongue twisters.5 Mannerism or Etiquette.

6 Mock Interview

SEMESTER II

Paper- HBCH -201 (L:3, credits) (Max marks (60+40) Time 3 hrs

THEORY Marks: 100 Note:-




any 2).

UNIT-I

Structure and Bonding

Hybridization, bond lengths and bond angles, bond energy, localized and delocalized chemical bond, van der Waals interactions, inclusion compounds, clatherates, charge transfer complexes resonance, hyperconjugation, aromaticity, inductive and field effects, hydrogen bonding.

Mechanism of Organic Reactions

Curved arrow notation, drawing electron movements with arrows half-headed and double-headed arrows, hemolytic and heterolytic bond breaking. Types of reagents (electrophiles and nucleophiles). Reactive intermediates – carbocations, carbanions, free radicals,carpenes, arynes and nitrenes (with examples). Assigning formal charges on intermediates and other ionic species. Methods of determination of reaction mechanism (product analysis, intermediates, isotope effects, kinetic and stereochemical studies).

UNIT-II

Stereochemistry of Organic Compounds

Concept of isomerism. Types of isomerism. Optical isomerism – elements of symmetry, molecular chirality, enantiomers, stereogenic center, optical activity, properties of enantiomers, chiral and achiral molecules with two stereogeric centers, diastereomers, threo and erythro diastereomers, meso compounds, resolution of enantiomers, inversion, retention and racemization.

Relative and absolute configuration, sequence rules, D & L and R & S systems of nomenclature.

Geometric isomerism – determination of configuration of geometric isomers. E & Z system of nomenclature..

Conformational isomerism – conformational analysis of ethane and n-butane;

UNIT-III

Alkanes and Cycloalkanes

IUPAC nomenclature of branched and unbranched alkanes. Isomerism in alkanes, sources, methods of formation (with special reference to Wurtz reaction, Kolbe reaction, Corey-House reaction and decarboxylation of carboxylic acids). Physical properties and chemical reactions of alkanes.

Cycloalkanes – nomenclature, methods of formation, chemical reactions, Baeyer’s strain theory and its limitations. Ring strain in small rings (cyclopropane and cyclobutane), theory of strainless rings.

UNIT-IV

Alkenes, Cycloalkenes, Dienes and Alkynes

Nomenclature of alkenes, methods of formation, mechanisms of dehydration of alcohols and dehydrohalogenation of alkyl halides, regioselectivity in alcohol dehydration. The Saytzeff rules, Hofmann elimination, physical properties and relative stabilities of alkenes.

Chemical reactions of alkenes – mechanisms involved in hydrogenation, electrophilic and free radical additions, Markownikiff’s rule, hydroboration-oxidation, oxymercuration-reduction. Epoxidation, ozonolysis, hydration, hydroxylation and oxidation with KMnO4 Polymerization of alkenes. Substitution at the allylic and vinylic positions of alkenes.

Suggested Books

1. Morrison R.T. and Boyd P.S., Organic Chemistry, 5th Edn., Pubs: Allyn and Bacon Inc., Boston ,1992.2. Mukerji S. M., Singh S. P. and Kapoor R. P., Organic Chemistry Vol. I/II, Pubs: Wiley Eastern Ltd., New Delhi, 1985. FURTHER READING :1. Wade L.G.Jr., Organic Chemistry, Pubs:Prentice-Hall,1990.2. Solomons G., Fundamentals of Organic Chemistry, Pubs: John Wiley,2002.3. Carey F.A., Organic Chemistry, Pubs: McGraw-Hill, Inc, 2003.4. Streitwisser A., Jr. and Heathcock C.H., Introduction to Organic Chemistry, 3rd Edn., Pubs: MacMillan Pub. Co., N.Y,1992.


Paper HBCH 202 (L:3, credits) (Max marks (60+40) Time 3 hrs

THEORY Marks: 100

Note:-




any 2).

Unit I Qualitative and Quantitative aspects of analysis:Sampling, evaluation of analytical data, errors, accuracy and precision, methods of their expression, normal law of distribution if indeterminate errors, statistical test of data; F, Q, and T test, rejection of data, and confidence intervals.

Unit II

Optical methods of analysis: Origin of spectra, interaction of radiation with matter, fundamental laws of spectroscopy and selection rules, validity of Beer-Lambert’s law. UV-Visible Spectrometry: Basic principles of instrumentation (choice of source, monochromator and detector) for single and double beam instrument;Infrared Spectrometry: Basic principles of instrumentation (choice of source, monochromator & detector) for single and double beam instrument; sampling techniques.Flame Atomic Absorption and Emission Spectrometry: Basic principles of instrumentation (choice of source, monochromator, detector, Choice of flame and Burner designs. Techniques of atomization and sample introduction;

Unit IIIThermal method of analysis:Theory of thermogravimetry (TG), basic principle of instrumentation. Techniques for quantitative estimation of Ca and Mg from their mixture.

Unit IV Electro analytical methods:Classification of electroanalytical methods, basic principle of pH metric, potentiometric and conductometric titrations. Techniques used for the determination of equivalence point. Techniques used for the determination of pKa values.

Recommended texts:1. Vogel, Arthur I: A Test book of Quantitative Inorganic Analysis (Rev. by GH Jeffery and others) 5th Ed.

The English Language Book Society of Longman 2. Willard, Hobert H. et. al: Instrumental Methods of Analysis, 7th Ed. Wardsworth Publishing Company,

Belmont, California, USA, 1988. 3. Christian, Gary D; Analytical Chemistry, 6th Ed. New York- John Willy, 2004. 4. Harris, Daniel C: Exploring Chemical Analysis, 2nd Ed. New York, W.H. Freeman, 2001. 5. Khopkar, S.M. Basic Concepts of Analytical Chemistry New Age, International Publisher, 2009. 6. SKoog, D.A. Holler F.J. and Nieman, T.A. Principles of Instrumental Analysis, Thomson Asia Pvt. Ltd.

Singapore. 7. Mikes, O. & Chalmes, R.A. Laboratory Hand Book of Chromatographic & Allied Methods, Elles

Harwood Ltd. London. 8. Ditts, R.V. Analytical Chemistry – Methods of separation.

BIOLOGY-I

Paper HBCH 203 (L:3, credits)(Max marks (60+40) Time 3 hrs

THEORY Marks: 100

Note:-




any 2).

Cell and Cellular Processes

Unit 1. Techniques in Biology

Principles of microscopy; Light Microscope; Phase contrast microscopy; Fluorescence microscopy; Confocal microscopy; Sample Preparation for light microscopy; Electron microscopy (EM)- Scanning EM and Scanning Transmission EM (STEM); Sample Preparation for electron microscopy; X-ray diffraction analysis

Unit 2. Cell as a unit of Life

The Cell Theory; Prokaryotic and eukaryotic cells; Cell size and shape; Eukaryotic Cell components

Unit 3. Cell Organelles

• Mitochondria: Structure, marker enzymes, composition; mitochondrial biogenesis; Semiautonomous organelle; Symbiont hypothesis; Proteins synthesized within mitochondria; mitochondrial DNA

• Chloroplast Structure, marker enzymes, composition; semiautonomous nature, chloroplast DNA

• ER, Golgi body & Lysosomes Structures and roles. Signal peptide hypothesis, N-linked glycosylation, Role of golgi in O-linked glycosylation. Cell secretion, Lysosome formation.

• Peroxisomes and Glyoxisomes: Structures, composition, functions in animals and plants and biogenesis

• Nucleus: Nuclear Envelope- structure of nuclear pore complex; chromatin; molecular organization, DNA packaging in eukaryotes, euchromatin and heterochromatin, nucleolus and ribosome structure (brief).

Unit 4. Cell Membrane and Cell Wall

The functions of membranes; Models of membrane structure; The fluidity of membranes; Membrane proteins and their functions; Carbohydrates in the membrane; Faces of the membranes; Selective permeability of the membranes; Cell wall

SUGGESTED BOOKS1. Campbell, N.A. and Reece, J. B. (2008) Biology 8th edition, Pearson Benjamin Cummings, San

Francisco. 2. Raven, P.H et al (2006) Biology 7th edition Tata McGrawHill Publications, New Delhi 3. Sheeler, P and Bianchi, D.E. (2006) Cell and Molecular Biology, 3rd edition, John Wiley

& sons NY

Physics-I

Paper HBCH 204 (L:3, credits)(Max marks (60+40) Time 3 hours



questions for 2 marks; Section B contain 8 questions of 8 marks (student will attempt any 5), Section C

containing 4 questions 15 marks (student will attempt any 2).

UNIT – I

Electromagnetic fields and em wave: Gradient of a scalar, divergence and cul of a vector, Gauss’s law (integral and differential form) and its applications, Electric potential and electric field (in vector form), Dieletrics, Polarization, Electric displacement, Susceptibility and permittivity, Lorentz foce law, Magnetic field of a steady current (Biot-Savart’s law), Faraday’s law, Ampere’s circuital law and its applications, Maxwell’s equations a dn their significance, Electromagnetic Spectrum (basic idea of different regions).

UNIT – II

Quantum Theory: Need of Quantum Mechanics, Davisson-Germer Experiment and Matter waves, Group and Phase velocities. Uncertainity Principle and its applications, Time-independent and Time-Dependent Schrödinger Wave equation, Eigen values and Eigen Functions, Applications of Schrödinger Wave equation to Particle in a box (one dimensional).

UNIT – III

Lasers and Optical Fibers: Spontaneous and Stimulated Emission, Einstein’s coefficients, Population Inversion and Optical Pumping, Three-level and Four-level Lasers, Ruby, He-Ne, CO2, Semiconductor Lasers, Application of lasers, Basic theory of fiber optics, accepatance angle, numerical aperture, modes of propagation, material and pulse dispersion, application of optical fibers.

UNIT – IV

Magnetic materials and Superconductivity: Hard and soft magnetic materials and their applications, Ferrites and their applications, Phenomenon of superconductivity, Magnetic properties of superconductors (Meissner effect), Type-I and Type-II Superconductors, Applications of Superconductivity.

ENVIRONMENTAL SCIENCE


THEORY Marks: 100

Note:-




any 2).

SECTION 1: INTRODUCTION

Definition and Scope: Importance, Public awareness and education.

Natural Resources: Introduction, Renewable and non-renewable, Forest, water, mineral, food, energy

and land resources, Conservation of resources, Equitable use of resources.

Human population and the environment: Population growth, Environment and human health,

Human rights, HIV/AIDS, Value education, Women and child welfare.

SECTION 2: ECOLOGY

Ecosystems: Concept, Structure, Function, Energy flow, Ecological pyramids, Forest, grassland, desert

and aquatic ecosystems - Introduction, characteristic features, structure and function.

Biodiversity: Genetic, Species and ecological diversity, Threats to biodiversity, Conservation of

Biodiversity.

SECTION 3: SOCIAL ISSUES & ENVIRONMENTAL LEGISLATION

Social Issues: Sustainable development, Water conservation, Climatic change, Concept of Green

Computing, and Green Building

Environmental Laws: Environmental ethics, EIA, Environmental protection acts and issues.

SECTION 4: POLLUTION &WASTE MANAGEMENT

Pollution: Definition, Causes, effects and control measures of the pollution – Air, soil, Noise, Water,

Marine and Thermal and Nuclear Pollution.

Disaster management: Flood, Earthquake, Cyclone, Landslide, Drought.

Solid waste management: Waste Management hierarchy; Collection, transportation and storage of

MSW; Treatment and disposal of MSW.

SECTION 5: ENVIRONMENTAL CHEMISTRY

General Chemistry: Review of concepts like oxidation-reduction, Gas laws, pH and Buffers.

Atmospheric Chemistry: Photochemical reactions in atmosphere, Major chemical pollutants and their

effects.

Water and Wastewater Chemistry: Hardness, Residual chlorine, Dissolved oxygen, BOD, COD,

Solids.

Green Chemistry: Principles, Green materials, reactions, reagents and product.

Suggested Readings:

Text Books:

• Environmental Studies by J.P.Sharma.

• Environmental studies by Smriti Srivastava.

Reference Books:

• Environment and Ecology by H.Kaur.

• Environmental Studies by Ranjit Daniels.

• Fundamentals of Ecology by P. Odum.

Organic Chemistry - I

Paper HBCH -251 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

1. Preparation and purification through crystallization or distillation and ascertaining their purity through melting point or boiling point

(i) Iodoform from ethanol (or acetone)

(ii) m-Dinitrobenzne from nitrobenzene (use 1:2 conc. HNO3 - H2SO4 mixture if fuming HNO3 is not available)

iii) p-Bromoacetanilide from acetanilide

iv) Dibenzalacetone from acetone and benzaldehyde

v) Aspirin from salicylic acid

2. Determination of melting point Naphthalene 80-82o, Benzoic acid 121.5-122o

urea, 132.5-133o, Succinic acid 184-185o Cinnamic acid 132.5-133o, Salicylic acid 157-5-158o Acetanilide 113-5-114o, m-Dinitrobenzene 90o p-Dichlorobenzene 52o. Aspirin 135o.

3. Determination of boiling points Ethanol 78o, Cyclohexane 81.4o, Toluene 110.6o, Benzne 80o.

4. Distillation Simple distillation of ethanol-water mixture using water Condenser Distillation of nitrobenzene and aniline using air condenser.


Paper HBCH 252 P (P:2, 2 credits) (Max marks (30+20) Time 3 hoursPRACTICAL Marks: 50

Separation Techniques1. Chromatography:

(a) Separation of mixtures (i) Paper chromatographic separation of Fe3+, Al3+, and Cr3+

(ii) Separate and identify the monosaccharides present in the given mixture (glucose & fructose) by paper chromatography. Report the Rf values.

(b) Separate a mixture of Sudan yellow and Sudan Red by TLC technique and identify them on the basis of their Rf values.

(c) Chromatographic separation of the active ingredients of plants, flowers and juices by TLC 2. Solvent Extractions:

(i) To separate a mixture of Ni2+ & Fe3+ by complexing with DMG and extracting the Ni2+ DMG complex in chloroform, and determine its concentration with spectrophotometry.

(ii) Solvent extraction of zisconium with amberliti LA-1, separation from a mixture of irons and gallium.

3. Determine the pH of given aerated drinks fruit juices, shampoos and soaps. 4. Determination of Na, Ca, Li in cola drinks and fruit juices using fame photometric techniques.

5. Analysis of soil: (i) Determination of pH of soil. (ii) Total soluble salt (iii) Estimation of calcium, magnesium, phosphate, nitrate

6. Ion exchange: (i) Determination of exchange capacity of cation exchange resins and anion exchange

resins. (ii) Separation of metal ions from their binary mixture. (iii)Separation of amino acids from organic acids by ion exchange

chromatography.7. Determination of pKa values of indicator using spectrophotometry. 8. Structural characterization of compounds by Infra-Red spectroscopy. 9. Determination of dissolved oxygen in water. 10. Determination of chemical oxygen demand (COD). 11. Determination of Biological oxygen demand (BOD).

PHYSICS-IPaper HBCH 253 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICALS Marks: 50

Group A experiments

A-1. Determination of spring constant of a spring by (i) static, and (ii) dynamic methods. A-2. Study of

damped harmonic oscillator- Q factor.

A-3. Determination of temperature coefficient of resistance using platinum resistance thermometer.

A-4. Study of thermal couple calibration and inversion temperature.

A-5. LCR study of resonance Q-factor.

A-6. Kator’s pendulum- Bar pendulum.

Group B experiments

B-1. Determination of wavelength of light by Fresnel’s biprism.

B-2. Determination of wavelength of sodium light by Newton’s arrangement.

B-3. Determination of refractive index of tint glass using a spectrometer.

B-4. Determination of dispersive power of a glass prism using Cauchy’s constant. Also determine the resolving power of a prism.

B-5. Determination of wavelength of sodium light using a plane transmission grating and resolving power of a diffraction grating.

B-6. Determination of specific rotation of cane sugar solution using a polarimeter.

SEMESTER – IIIInorganic Chemistry -II

Paper HBCH -301 (L:4, credits)(Max marks (60+40) Time 3 hours

THEORY Marks: 100

Note:-




any 2).

UNIT- IChemical Bonding-I

Electronegativity and Polarity of bond : Electronegativity, different scales and methods of determination. Recent advances in electronegativity theory, variation of electronegativity, Group electronegativity. Polarities of bonds and molecules, Dipole moments. Percentage of ionic character form dipole moment and electronegativity difference.

UNIT- II

Chemical Bonding-II:

Ionic bond: Factors affecting the stability of ionic compounds. Lattice energy, Born Lande equation and its applications, Madelung constant, Born-Haber cycle, applications of lattice energy, covalent character in ionic compounds, polarizing power and polarizability, Fazan’s rules, Ionic radii, Factors affecting the radii of ions, Radii of polyatomic ions, Efficiency of packing and crystal lattices, Radius ratio rule, calculation of some limiting radius ratio values for different coordination members, Structure of crystal lattices, NaCl, CaCl, ZnS, (Zinc blende and Wurzite), fluorite, rutile and cadmium iodide. Predictive power of thermochemical calculations on ionic compounds.

UNIT-III

Valence Bond theory and Molecular Orbital Theory

Valence bond (VB) approach. Resonance structures. Bond angles and shapes of molecules and ions (containing bond pairs and lone pairs) Criterion of bond strength and bond length. Molecular orbitals (MO) approach of bonding (LCAO Method). Symmetry and overlap, symmetry of molecular orbitals, Bonding in Homonuclear molecules (H2 to Ne2) and NO, CO, CN+, CO+, CN-, HF, HCl, BeH2, CO2, Comparison of VB and MO theories.

Unit IV

The p-Block Elements

Nitrogen, P, As,Sb & Bi family : Chemical reactivity and group trends.

Nitrogen: Introduction, types of covalence in nitrogen, stereochemistry, chemical reactivity, dinitrogen complexes (basic idea only), hydrides of nitrogen, liquid NH3 as a solvent, nitrogen halides, oxides and oxoacids.

Phosphorus, As, Sb & Bi : Stereochemistry of their compounds, production of elemental P and its allotropic forms, hydrides, halides, oxides and oxy-acids, phosphorus-nitrogen compounds, some organo-metallic compounds.

Oxygen, S, Se and Te Family : Chemical Reactivity, group trends & stereochemistry, dioxygen as a ligand (basic idea only), structure of O3 and H2O2, clathrate hydrates allotropic forms of S & Se, structures of halides, oxides and oxyacids of S, Se & Te, liquid SO2 and 100% Sulphuric acid as solvent, S-N compounds (neutral) Polyatomic cations of S, Se & Te.

Suggested Books

1. Cotton F.A., Wilkinson G.W. and Gaus P.L., Basic Inorganic Chemistry, Pubs: John Wiley & Sons ,1987. 2. Lee J.D., Concise Inorganic Chemistry, 4th edition, Pubs: ELBS,1991.3. Huheey J.E., Keiter E.A., Keiter R.L., Inorganic Chemistry : Principles of Structures and Reactivity; 4th Edition, Pubs: Harper Collins, 1993.4. Greenwood N.N. and Earnshaw A., Chemistry of the Elements, 2nd edition, Pubs: Butterworth/Heinemann, 1997. FURTHER READING:1. Cotton F.A. and Wilkinson G., Murillo C.A., Bochmann M., Advanced Inorg. Chemistry, 6th Edition, Pubs: John Wiley & Sons. Inc., 1999.2. Shriver D.F., Atkins F.W. and Langford C.M., Inorganic Chemistry; 3rd Edition, Pubs: Oxford University Press, 1999.3. Douglas B., Daniel D. Mc and Alexander J., Concepts of Models of Inorganic Chemistry, Pubs: John Wiley,1987.4. Gray H.B., Electrons and Chemical Bonding, Pubs: W.A., J Benjamin Inc.,1965.

PHYSICAL CHEMISTRY-II


THEORY Marks: 100Max. Marks: 50 Time: 3 Hours

Note:-




any 2).

UNIT-I

The Second Law of Thermodynamics: Spontaneous change, Carnot Cycle, conclusions from Carnot cycle, efficiency of heat engines, second law of thermodynamics, entropy, entropy as a state function, clausius inequality, entropy as criterian of spontaneity, natural processes, different types of entropy changes under isothermal and non-isothermal conditions, entropy change in irreversible processes. Helmholtz function (A), Gibbs function (G), standard molar free energy changes, Maxwell relations, dependence of free energy functions on temperature and pressure, total differential equations. Gibbs- Helmholtz equations, thermodynamic criteria for spontaneity. Heat capacity at low temperature, Nernst heat theorem, third law of thermodynamics, third law entropies.

UNIT-II

Perfect and imperfect crystals: Intrinsic and extrinsic defects, point defects, line and plane defects, vacancies-Schottky and Frenkel defects. Thermodynamics of Schottky and Frenkel defect formation, colour centres, non-stoichiometry and defects. Metals insulators and semiconductors, Band theory, Band structure of metals, Insulators and semiconductors, intrinsic and extrinsic semiconductors, doping semiconductors, p-n junctions, and High temperature super conductors.

UNIT III

Partial Molar Properties and Fugacity: Partial molar properties. Chemical potential of a perfect gas, dependence of chemical potential on temperature and pressure, Gibbs- Duhem equation, real gases, fugacity, its importance and determination, standard state for gases.

Changes of State, Physical Transformation of Pure Materials: Stability of phases, clapeyron equation. Clausius-clapeyron equation First and second order phase transitions. Attainment of low temperature and energetics of refrigeration, adiabatic demagnetization.

UNIT-IV

Phase Equilibria: Phase rule and its thermodynamic derivation. One component systems-water, sulphur, carbon dioxide, helium. Two component systems, construction and interpretation of general phase diagrams for liquid-vapour, liquid-liquid and liquid-solid systems.

Chemical Equilibrium: Direction of spontaneous change in a chemical reaction, extent of reaction, stoichiometric coefficients, equilibrium constant in terms of G. Temperature and pressure dependence of equilibrium constant, homogeneous & heterogeneous equilibria.

Suggested Books

1. Atkins P.W., Physical Chemistry, 8th Edn., Pubs: Oxford University Press, 2006 (Indian Print).

2 Engel T. & Reid P., Physical Chemistry, 1st Edn., Pubs: Pearson Education, 2006.

FURTHER READING:

1. Castellan G.W., Physical Chemistry, 3rd Edn., Pubs: Addison Wisley/Narosa, 1985 (Indian Print).

2. Barrow G. M., Physical Chemistry, 6th Edn., Pubs: McGraw Hill, New York, 1996.

3 Silbey R. J., Albert R. A. & Bawendi Moungi G., Physical Chemistry, 4th Edn., Pubs: John Wiley, New York, 2005.

ORGANIC CHEMISTRY-II


Note:-




any 2).

UNIT-I

Arenes and Aromaticity

Nomenclature of benzene derivatives. The aryl group. Aromatic nucleus and side chain. Structure of benzene : molecular formula and Kekule structure. Stability and carbon-carbon bond lengths of benzene, resonance structure, MO picture.

Aromatic electrophilic substitution – general pattern of the mechanism, role of L-and _ complexes. Mechanism of nitration, halogenation, sulphonation, mercuration and Friedel-Crafts reaction. Energy profilediagrams. Activating and deactivating substituents, orientation and ortho/para ratio. Side chain reactions of benezene derivatives. Birch reduction.

Methods of formation and chemical reactions of alkylbenzenes and biphenyl.

UNIT -II

Alkyl and Aryl halides :Nomenclature and classes of alkyl halides, methods of formation, chemical reactions. Mechanisms of nucleophilic substitution reactions of alkyl halides, SN2 and SN1 reactions with energy profile diagrams.

Methods of formation of aryl halides, nuclear and side chain reactions. The addition-elimination and the elimination-addition mechanisms of nucleophilic aromatic substitution reactions.

Relative reactiviteis of alkyl halides vs. allyl, vinyl and aryl halides.

UNIT-III

Alcohols: Classification and nomenclature.Monohydric alcohols – nomenclature, methods of formation by reduction of aldehydes, ketones, carboxylic acids and esters. Hydrogen bonding. Acidic nature. Reactions of alcohols.Dihydric alcohols – nomenclature, methods of formation, chemical reactions of vicinal glycols, oxidative cleavage [Pb(OAc)4 and HIO4 and pinacol-pinacolone rearrangement.

Trihydric alcohols – nomenclature and methods of formation, chemical reactions of glycerol.

UNIT IV

Phenols: Nomenclature, structure and bonding. Preparation of phenols, physical properties and acidic character. Comparative acidic strengths of alcohols and phenols, resonance stabilization of phenoxide ion. Reactions of phenols – electrophilic aromatic substitution, acylation and carboxylation. Mechanisms of Fries rearrangement, Claisen rearrangement, Gatterman synthesis, Hauben-Hoesch reaction, Ledrer-Manasse reaction and Reimer-Tiemann reaction.

Ethers and Epoxides: Nomenclature of ethers and methods of their formation, physical properties. Chemical reactions – cleavage and autoxidation, Ziesel’s method. Synthesis of epoxides. Acid and base-catalyzed ring opening of epoxides, orientation of epoxide ring opening, reactions of Grignard and organolithium reagents with epoxides.

Suggested Books

1. Morrison R.T. and Boyd P.S., Organic Chemistry, 5th Edn., Pubs: Allyn and Bacon Inc., Boston (1992).

2. Mukerji S. M., Singh S. P. and Kapoor R. P., Organic Chemistry Vol. I/II, Pubs: Wiley Eastern Ltd., New Delhi, 1985.

FURTHER READING :

1. Wade L.G.Jr., Organic Chemistry, Pubs:Prentice-Hall,1990. 2. Solomons G, Fundamentals of Organic Chemistry, Pubs: John Wiley,2002.

3. Carey F.A., Organic Chemistry, Pubs: McGraw-Hill, Inc, 2003.

4. Streitwisser A., Jr. and Heathcock C.H., Introduction to Organic Chemistry, 3rd Edn., Pubs: MacMillan Pub. Co., N.Y,1992.

Mathematics – II (NUMERICAL METHODS)

HBCH 304 (L:4, credits : 4)(Max marks (60+40) Time 3 hours





any 2).

UNIT-IComputer Arithmetic: Floating-point representation of numbers, arithmetic operations with normalized floating-point numbers and their consequences, significant figures. Error in number representation-inherent error, truncation, absolute, relative, percentage and round-off error. Iterative Methods: Bisection, False position, Newton-Raphson method. Iteration method, discussion of convergence, Bairstow's method.

UNIT-IISolution of simultaneous linear equations and ordinary differential equations: Gauss-Elimination methods, pivoting, Ill-conditioned equations, refinement of solution. Gauss-Seidal iterative method, Euler method, Euler modified method, Taylor-series method, Runge-Kutta methods, Predictor-Corrector methods.

UNIT-IIIInterpolation and Approximation: Polynomial interpolation: Newton, Lagranges, Difference tables, Approximation of functions by Taylor Series. Chebyshev polynomial: First kind, Second kind and their relations, Orthogonal properties.

UNIT-IVNumerical Differentiation and integration: Differentiation formulae based on polynomial fit, pitfalls in differentiation, Trapezoidal & Simpson Rules, Gaussian Quadrature.

REFERENCE BOOKS 1. V. Rajaraman, Computer Oriented Numerical Methods, Prentice Hall, India. 2. S. S. Sastry, Introductory Methods of Numerical Analysis. 3. M. K. Jain, S.R.K. Iyengar & R. K. Jain, Numerical Methods for Scientific and Engineering Computation. 4. H. C. Saxena, Finite Differences and Numerical Analysis. 5. Modes A., Numerical Analysis for Computer Science.

Inorganic Chemistry -II

Paper - HBCH 351 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 501. Gravimetric Analysis

Quantitative estimations of, Cu2+ as copper thiocyanate and Ni2+ as Ni– dimethylglyoxime.

2. Redox titrations: Determination of Fe2+, C2O42- (using KMnO4, K2Cr2O7)

3. Iodometic titrations: Determination of Cu2+ (using standard hypo solution).

4. Complexometric titrations: Determination of Mg2+, Zn2+ by EDTA.

5. Preparation of SnI4 and its complex with pyridine

6. Preparation of Pb(OOCCH3)4 and its complex (C5H5NH2) PbCl6 Thermal analysis of Pb(OOCCH3)4

Organic Chemistry -II


PRACTICAL Marks: 50

1. To study the process of) sublimation of camphor and phthalic acid,

2 Systematic identification (detection of extra elements, functional groups, determination of melting point or boiling point and preparation of at least one pure solid derivative) of the following simple mono and bifunctional organic compounds: Naphthalene, anthracene, naphthene, benzyl chloride, p-dichlorobenzene, m-dinitrobenzene , p-nitrotoluene, resorcinol , hydroquinone, Ethyl methyl ketone, benzaldehyde, vanillin, oxalic acid, succinic acid, benzoic acid, salicyclic acid, aspirin, phthalic acid, cinnamic acid, benzamide, urea, acetanilide, benzanilide, aniline hydrochloride, p-toluidine, phenyl salicylate (salol), glucose, fructose, sucrose, o-, m-, pnitroanilines, thiourea

Physical Chemistry -II

Paper – HBCH 353 P (P:2, 2 credits) (Max marks (60+40) Time 3 hours

PRACTICAL Marks: 50

1. To determine the enthalpy of neutralisation of a weak acid/weak base vs. strong base/strong acid and determine the enthalpy of ionisation of the weak acid/weak base.

2. Determination of critical solution temperature for phenol-water system and study effect of impurities.

3. Construction of a phase diagram of a binary system (urea-benzoic acid) by cooling curves method.

Potentiometry

1. Potentiometric titration of monobasic acids (HC & CH3COOH) with NaOH.

2. Determination of mean ionic activity co-efficients of hydrochloric acid at different concentrations.

3. To study the effect of ionic strength on mean ionic activity coefficient of hydrochloric acid in a given solution and verify Debye-Huckel limiting law.

Thermo Chemistry

1. To determine heat capacity of a calorimeter and heat of solution of a given solid compound. 2. To determine heat of solution of Solid calcium chloride and calculate lattice energy of calcium chloride using Born-Haber cycle.3. To determine heat of hydration of copper sulphate

Any other experiment carried out in the class.

SEMESTER IV

Inorganic Chemistry -III

Paper- HBCH 401 (L:3, credits) (Max marks (60+40) Time 3 hours





any 2).

UNIT-I

The Halogen Family : Chemical Reactivity, group trends, chemistry of preparation of fluorine, hydrogen halides, HF as a solvent, inter-halogen compounds (their preparation and structures), polyhalide and polyhalonium ions; polyatomic cations of halogens, oxides and oxyacide of halogens.

Noble gases

Chemical reactivity and group trends, Clathrate compounds; preparation, structure & bonding of noble gas compounds.

UNIT-II

Coordination Compounds Various definitions, types of ligands : classical ligands, non-classical ligands (π-bonding or π-acid ligands); The Chelate and Microcyclic effects, Multidentate ligands, conformation of Chelate rings, stereochemistry and various coordination numbers, isomerism in coordination compounds, nomenclature, stability of coordination compounds, thermodynamic and kinetic stability, stability constants, experimental and statistical ratios of stability constants factors which influence the stability constant and chelate effect.

UNIT- III

Symmetry and group theory - I

Symmetry elements and symmetry operations, point groups, definitions of group, subgroup relation between orders of a finite group and its subgroup; group multiplication tables, conjugacy relation and classes. Schoenflies symbols, Representation of groups character of a representation.

UNIT-IV

Symmetry and group theory - II

Properties of irreducible representations, the great orthogonality theorem (without proof) and its importance. Character Tables, Symmetry criteria for optical activity, Symmetry restrictions on dipole moment, Hybridization schemes of orbitals.

Suggested Books

1. Cotton F. A.,Wilkinson G., Murillo C. A., Bochmann M., Advanced Inorg. Chemistry, 6th Edition, Pubs: John Wiley & Sons. Inc., 1999.

2. Greenwood N. N. and Earnshaw A., Chemistry of the Elements, 2nd Edition, Pubs: Butterworth/Heinemann, 1977.

3. Shriver D. F., Atkins F. W. and Langford C. M., Inorganic Chemistry, 3rd Edition, Pubs: Oxford University Press, 1999.

4. Huheey J. E., Keiter E. A., Keiter R. L., Inorganic Chemistry : Principles of Structure and Reactivity; 4th Edition, Pubs: Harper Collins, 1993.

5. Massey Allan G., Main Group Chemistry, Pubs: Ellis Horwood, NewYork 1990.

6. Cotton F. A.,Chemical applications of group theory, 3rd Edition, Pubs: John Wiley New York, 1971 [Indian print by Wiley Eastern, 1999].

7. Jaffe H. H. and Orchin M., Symmetry in Chemistry, Pubs: John Wiley NewYork, 1965.

Organic Chemistry -III

Paper- HBCH 402 (L:3, credits)(Max marks (60+40) Time 3 hours

THEORY Marks: 100

Note:-




any 2).

UNIT-I

Organic Compounds of Nitrogen:

Preparation of nitroalkanes and nitroarenes. Chemical reactions of nitroalkanes. Mechanisms of nucleophilic substitution in nitroarenes and their reductions in acidic, neutral and alkaline media. Picric acid.

Halonitroarenes: reactivity. Structure and nomenclature of amines, physical roperties. Stereochemistry of amines. Separation of a mixture of primary, secondary and tertiary amines. Structural features effecting basicity of amines. Amine salts as phase-transfer catalysts. Preparation of alkyl and aryl amines (reduction of nitro compounds nitriles), reductive amination of aldehydic and ketonic compounds. Garbriel-phthalimide reaction, Hoffmann bromamide reaction.

UNIT-II

Heterocyclic Compounds:

Introduction : Molecular orbital picture and aromatic characteristics of pyrrole, 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 derivatives. Comparison of basicity of pyridine, piperidine and pyrrole.

Introduction to condensed five and six-membered heterocycles. Preparation and reactions of indole, quinoline and isoquinoline with special reference to Fischer indole synthesis, Skraup synthesis and Bischler-Napieralski synthesis. Mechanism of electrophilic substitution reactions of indole, quinoline and isoquinoline.

UNIT-III

Carbohydrates:

Classification and nomenclature. Monosaccharides, mechanism of osazone formation, interconversion of glucose and fructose, chain lengthening and chain shortening of aldoses. Erythro and threo diastereomers. Conversion of glucose into mannose. Formation of glycosides, ethers and esters. Determination of ring size of nonosaccharides. Cyclic structure of D(+)-glucose. Mechanism of mutarotation. Structures of ribose and deoxyribose.

UNIT-IV

Amino Acids, Peptides and Proteins:

Classification, structure and stereochemistry of amino acids. Acid-base behavior, isoelectric point and electrophoresis. Preparation and reactions of _-amino acids. Structure and nomenclature of peptides and proteins. Classification of proteins.

Synthetic Dyes :

Colour and constitution (electronic concept). Classification of dyes. Chemistry and synthesis of Methyl orange, Congo red, Malachite green, Crystal violet, Phenolphthalein, Fluorescein, Alizarin and Indigo.

Suggested Books

1. Morrison R.T. and Boyd P.S., Organic Chemistry, 5th Edn., Pubs: Allyn and Bacon Inc., Boston (1992).

2. Mukerji S. M., Singh S. P. and Kapoor R. P., Organic Chemistry Vol. I/II, Pubs: Wiley Eastern Ltd., New Delhi, 1985.

FURTHER READING :

1. Wade L.G.Jr., Organic Chemistry, Pubs:Prentice-Hall,1990.

2. Solomons G, Fundamentals of Organic Chemistry, Pubs: John Wiley,2002.

3. Carey F.A., Organic Chemistry, Pubs: McGraw-Hill, Inc, 2003.

4. Streitwisser A., Jr. and Heathcock C.H., Introduction to Organic Chemistry 3rd Edn., Pubs: MacMillan Pub. Co., N.Y, 1992.

Physical Chemistry -III

Paper 1- HBCH 403 ((L:3, credits)) (Max marks (60+40) Time 3 hours





any 2).

UNIT–I

Kinetic theory of gases and transport properties

Review of kinetic molecular theory of gases, kinetic energy and temperature. Distribution of molecular speeds in an ideal gas, distribution in one dimension, distribution of speeds in three dimensions. Derivation of Maxwell-Boltzmann distribution law. Derivation of most probable speed, root mean square speed and average speed from Maxwell-Boltzmann distribution law. Collision frequency, mean free path, collision diameter, collision cross-sectionRate of effusion, Graham’s law of effusion.

Transport phenomena in gases. kinetic theory of diffusion in gases. Thermal conductivity, kinetic theory of thermal conductivity in gases. Viscosity of gases, kinetic theory of gas viscosity, molecular diameters and intermolecular force constants from viscosity.

UNIT-II

Electrochemical Cells:

Interfacial potential difference, the electrodes, potential at interfaces, electrode potentials, galvanic cells, emf, direction of spontaneous reactions. Concentration dependence of emf, equilibrium Constant from electrode potential, standard electrode potentials and their determination. Measuring activity co-efficient, thermodynamic data from cell emf. The temperature dependence of emf. Applications of emf. Measurements – solubility product, potentiometric titrations, pK and pH measurements of pK and pH. Acid-base titrations. Concentration cells with & without transference

UNIT III

Thermodynamics of diffusion

Thermodynamic view of diffusion. Relation between transport properties. Einstein relation, Nernst-Einstein relation, stoke’s Einstein relation. Diffusion in non-steady state. Fick’s second law of diffusion. Theory of diffusion in liquids.

Electro-Chemistry:Equilibrium Electrochemistry

Transport of ions in solution, conductivity, Kohlrausch’s law, Ostwald dilution law. Mobilities of ions, transport number and its measurement. Arrhenius theory of Conductivity, Debye-Huckel-Onsager theory of conductivity. Applications of conductivity: conductometeric titrations, solubility of sparingly soluble salts, degree of dissociation of weak electrolytes.

UNIT–IVDynamic Electrochemistry : Processes at electrodes,double layer at the interface, non-equilibrium electrode potentials, over potential, derivation of Butler-Volmer equation, Tafel plot, Polarization and electrolysis, concentration overpotential, diffusion current and polarography, current and cell emf, Power.

Applications of dynamic electrochemistry : Power generation (Fuel cells), power storage (batteries), photochemical cells, corrosion and passivation.

Suggested Books:

1. Atkins P.W., Physical Chemistry, 7th Edition., Pubs: Oxford University Press (2002).

2. Lavine I. N., Physical Chemistry, 3rd Edition, Pubs: Pearson Eductaion (1988). 3. Billmeyer, Textbook of Polymer Science, 2nd Edition, Pubs: Wiley Interscience (1977).

4. Friedlander G., Kennedy J.W., Macias E.S. and Miller J.M., Nuclear and Radiochemistry, 3rd Edition, Pubs: John Wiley and Sons (1981).

5. Arnikar H.J., Essentials of Nuclear Chemistry, 2nd Edition, Pubs: Wiley Eastern Limited (1987),

6. Adamson A.W., Physical Chemistry of Surfaces, Pubs: John Wiley & Sons (1982)

FURTHER READING

1. Castellan G.W., Physical Chemistry, 3rd Edn., Pubs: Addison Wisley/Narosa (1985) (Indian Print).

2. Barrow G. M., Physical Chemistry, 6th Edn., Pubs: McGraw Hill, New York (1996).

3. Sood D. D., Reddy A.V.R. and Ramamoorthy N., Fundamentals of Radiochemistry, Pubs: Indian Association of Nuclear Chemists and Allied Scientists (2004).

Physics-II

Paper HBCH - 404 ((L:4 credits) (Max marks (60+40) Time 4 hours





any 2).

UNIT – I

CRYSTAL STRUCTURE: Space lattice, Bravais lattice - unit cell, primitive cell. Lattice parameters. Crystal systems. Direction and planes in a crystal. Miller indices. Expression for inter-planar spacing. Co-ordination number. Atomic packing factor. Bragg’s Law.Determination of crystal structure by Bragg’s x-ray spectrometer. Crystal structures of NaCl, and diamond.

FREE ELECTRON THEORY: Elements of classical free electron theory and its limitations. Quantum theory of free electrons, Fermi level, density of states, Fermi-dirac distribution function, Thermionic emission, Richardson’s equation.

UNIT – II

BAND THEORY OF SOLIDS: Origin of energy bands, Periodic Potential in a crystal, Wave function in a periodic potential, kronig, Penney Model (qualitative), E-K diagrams, Brillouin Zones, Effective mass of electron, Concept of negative effective mass and holes, Classification into metals, semiconductors and insulators, fermi energy and its variation with temperature.

UNIT – III

INTERFERENCE: Coherent Sources, Two Beam Interference by Division of Wavefront- Fresnel Biprism Interference by Division of Amplitude - Newton’s Rings, Michelson Interferometer.

DIFFRACTION: Fraunhoffer Diffraction, Diffraction through Single Slit, Plane Transmission Grating, Fresnel Diffraction, Fresnel Half Period Zone, The Zone Plate.

POLARIZATION: Production of Polarized Light, Malus’s Law, Double Refraction, and Interference of polarized light: Quarter Wave Plate And Half Wave Plate.

UNIT – IV

NUCLEAR PHYSICS: Natural radioactivity, successive radioactive transformations, radioactive equilibrium, radioactive series, radiometric dating.

Nuclear force and its characteristics, Elementary description of shell model, explanation of magic numbers, liquid drop model and semi-empirical binding energy formula.

Nuclear fission, fission products, mass and energy distribution of fission products, neutron emission and energy distribution of neutrons emitted in fission, theory of fission process, nuclear reactors – classification, neutron cycle in thermal reactors and four-factor formula for neutron reproduction, nuclear fusion – controlled thermonuclear reactions.

Recommended Texts:

1. Griffiths, D. J. Introduction to Electromagnetism 3rd Ed. Prentice-Hall (1999). 2. Malvino, A.P. & Leach, D. P. Digital Principles and Applications, Tata McGraw-Hill (2008). 3. Ryder, J. D. Electronic Fundamentals and Applications: Integrated and Discrete Systems. 5th Ed. Prentice-

Hall, Inc. (2007). 4. Floyd, T. L. & Buchla, D. M. Electronics Fundamentals: Circuits, Devices and Applications (8th Ed.)

Prentice-Hall (2009).

Inorganic Chemistry -III


PRACTICAL Marks: 50

1. Preparation of any two of the following complexes and measurement of their conductivity:

(i) tetraamminecarbonatocobalt (III) nitrate

(ii) tetraamminecopper (II) sulphate

(iii) potassium trioxalatoferrate (III) trihydrate

Compare the conductance of the complexes with that of M/1000 solution of NaCl, MgCl2 and LiCl3.

2. Analysis of CaC2O4.H2O by using thermogravimetry.

3. Complexometric titrations involving EDTA for quantitative determination of individual cation/mixture of cations.

Organic Chemistry -III


PRACTICAL Marks: 50

A. CrystallizationConcept of induction of crystallization Phthalic acid from hot water (using fluted filter paper and stemless funnel) Acetanilide from boiling water Naphthalene from ethanol Benzoic acid from water.

B. Qualitative Analysis

To perform qualitative analysis of single organic compound (hydrocarbons, aldehydes, ketones, phenols, carboxylic acids/(derivative), amines, amides, nitro compounds and carbohydrates).I. Test for elements (other than C, H, O).II. Functional group determinationIII. Melting point, derivative preparation and Rf value determination.

C. Synthesis of organic compoundsI. Acetylation/benzolyation of salicylic acid, aniline, hydroquinone and glucose.II. Preparation of m-dinitrobenzene from nitrobenzene.

Physical Chemistry -III

Paper- HBCH 453 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

I. Conductometry

1. To study the effect of concentration of electrolyte on specific and molar conductance of a strong and weak electrolyte.2. Determination of degree of dissociation and dissociation constant of weak acid.

3. Conductometeric titration of a strong acid, a weak acid, mixture of a strong and weak acid and a dibasic acid with alkali.

4. To compare the relative strengths of weak acids like acetic acid and monochloroacetic acid by conductivity measurements.

5. To verify Debye-Huckel Onsager equation

III. Polarimetry1. To determine the specific and molecular rotations of an optically active substance.2. To determine the composition of an unknown solution with a polarimeter.

IV. Dipole-Metry1. To determine the dielectric constant of an unknown liquid. 2. To determine the dipole moment of a polar substance in solution.


Physics-II

Paper HBCH 454 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

1. Study of a Ballistic Galvanometer: resistance, current sensitivity, charge sensitivity, andcritical damping resistance of the galvanometer.

2. Determination of high resistance by leakage method.

3. Determination of mutual inductance by Ballistic Galvanometer.

4. Operations and measurements by Cathode Ray Oscilloscope (CRO). Calibration of DC and AC voltages, frequency and phase measurements of a signal.

5. Study of transistor characeteristics (CB, CE, CC configurations).

6. Study of power supply (rectification factor, voltage and load regulation for C, L, CL and π filters).

7. Study of basic RC coupled amplifier (frequency response and band width).

8. Study of Colpitts oscillator.

9. Self-inductance measurement by Owen’s bridge.

10. Measurement of magnetic field by search coil.

11. To verify experimentally OR, NAD, NOT, NOR, NAND gates. 12. Study of Half-Adder/ Subtractor.

SEMESTER VInorganic Chemistry -IV


THEORY Marks: 100

Note:-




any 2).

Unit I Coordination Chemistry 1

Werner’s theory, valence bond theory (inner and outer orbital complexes), electroneutrality principle and back bonding. Crystal field theory, measurement of 10 Dq ( o), CFSE in weak and strong fields, pairing energies, factors effecting the magnitude of 10 Dq ( o, t). Octahedral vs. tetrahedral coordination, tetragonal distortions from octahedral geometry Jahn-Teller theorem, square planar geometry. Qualitative aspect of Ligand field and MO Theory.

Unit II Coordination Chemistry 1I

IUPAC nomenclature of coordination compounds, isomerism in coordination compounds. Stereochemistry of complexes with 4 and 6 coordination numbers. Chelate effect, polynuclear complexes, Labile and inert complexes.

Unit IIITransition elements: General group trends with special reference to electronic configuration, colour, variable valency, magnetic and catalytic properties, ability to form complexes. Stability of various oxidation states and e.m.f. (Latimer & Bsworth diagrams). Difference between the first, second and third transition series. Chemistry of Ti, V, Cr Mn, Fe and Co in various oxidation states (excluding their metallurgy)

Unit IV Lanthanoids and actinoids: electronic configuration, oxidation states, colour, spectral and magnetic properties, lanthanide contraction, separation of lanthanides (ion-exchange method only).

Recommended Texts:

1. Purecell, K.F. and Kotz, J.C., Inorganic Chemistry W.B. Saunders Co. 1977. 2. Basolo, F, and Pearson, R.C., Mechanisms of Inorganic Chemistry, John Wiley & Sons, NY, 1967. 3. Greenwood, N.N. & Earnshaw A., Chemistry of the Elements, Butterworth-Heinemann,1997.

Organic Chemistry -IV

Paper- HBCH 502 (L:3, credits) (Max marks (60+40) Time 3 hours THEORY Marks: 100Note:-




any 2).

Unit ICarbohydrates: Occurrence, classification and their biological importance Monosaccharides: Constitution and absolute configuration of glucose and fructose, epimers and anomers, mutarotation, determination of ring size of glucose and fructose, Haworth projections and conformational structures; Interconversions of aldoses and ketoses; Killiani-Fischer synthesis and Ruff degradation;

Disaccharides – Structure elucidation of maltose, lactose and sucrose

Polysaccharides – Elementary treatment of starch, cellulose and glycogen.

Unit II Nucleic Acids Components of nucleic acids, Nucleosides and nucleotides; Structure, synthesis and reactions of: Adenine, Guanine, Cytosine, Uracil nd Thymine; Structure of polynucleotides.

Unit IIIAmino acids, Peptides, Proteins and Lipids: Amino acids, Peptides and their classification. α-Amino Acids - Synthesis, ionic properties and reactions. Zwitterions, pKa values, isoelectric point and electrophoresis;Study of peptides: determination of their primary structures-end group analysis, methods of peptide synthesis. Synthesis of peptides using N-protecting, C-protecting and C-activating groups - Solid-phase synthesisIntroduction to oils and fats; common fatty acids present in oils and fats, Hydrogenntion of fats and oils, Saponification value, acid value, iodine number. Reversion and rancidity.

Unit IVPharmaceutical Compounds: Structure and Importance: Classification, structure and therapeutic uses of antipyretics: Paracetamol (with synthesis), Analgesics: Ibuprofen (with synthesis), Antimalarials: Chloroquine (with synthesis).

An elementary treatment of Antibiotics and detailed study of chloramphenicol,

Recommended Texts:

1. Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

2. Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). 3. Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural Products),

Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). 4. Nelson, D. L. & Cox, M. M. Lehninger’s Principles of Biochemistry, Fourth Edition, W. H. Freeman. 5. Berg, J. M., Tymoczko, J. L. & Stryer, L. Biochemistry, Sixth Edition, W. H. Freeman.

Physical Chemistry -IV

Paper - HBCH 503 (L:3, credits)(Max marks (60+40) Time 3 hours THEORY Marks: 100Note:-


questions for 2 marks; Section B containing 2 questions, each having 6 subparts of 5 marks,

(student will attempt any 4); Section C containing 2 questions each having 4 subparts of 10 marks

(student will attempt any 2).

UNIT I Conductance: Arrhenius theory of electrolytic dissociation. Conductivity, equivalent and molar conductivity and their variation with dilution for weak and strong electrolytes. Molar conductivity at infinite dilution. Kohlrausch law of independent migration of ions. Debye-Hückel-Onsager equation, Walden’s rules.

Ionic velocities, mobilities and their determinations, transference numbers and their relation to ionic mobilities, determination of transference numbers using Hittorf and Moving Boundary methods. Applications of conductance measurement: (i) degree of dissociation of weak electrolytes, (ii) ionic product of water (iii) solubility and solubility product of sparingly soluble salts, (iv) conductometric titrations, and (v) hydrolysis constants of salts.

UNIT IIChemical Kinetics: Order and molecularity of a reaction, rate laws in terms of the advancement of a reaction, differential and integrated form of rate expressions up to second order reactions, experimental methods of the determination of rate laws, kinetics of complex reactions (integrated rate expressions up to first order only): (i) Opposing reactions (ii) parallel reactions and (iii) consecutive reactions and their differential rate equations (steady-state approximation in reaction mechanisms) (iv) chain reactions.

Temperature dependence of reaction rates; Arrhenius equation; activation energy. Collision theory of reaction rates, Lindemann mechanism.

UNIT III Surface chemistry: Surface chemistry: Physical adsorption, chemisorption, adsorption isotherms. nature of adsorbed state. Catalysis: Types of catalyst, specificity and selectivity, mechanisms of catalyzed reactions at solid surfaces; effect of particle size and efficiency of nanoparticles as catalysts. Enzyme catalysis, Michaelis-Menten mechanism, acid-base catalysis.

UNIT IV Photochemistry: Characteristics of electromagnetic radiation, Lambert-Beer’s law and its limitations, physical significance of absorption coefficients. Laws, of photochemistry, quantum yield, actinometry, examples of low and high quantum yields, photochemical equilibrium and the differential rate of photochemical reactions, photosensitised reactions, quenching. Role of photochemical reactions in biochemical processes, photostationary states, chemiluminescence.

Recommended Texts:

1. Atkins, P. W. & Paula, J. de Atkin’s Physical Chemistry 8th Ed., Oxford University Press (2006). 2. Ball, D. W. Physical Chemistry Thomson Press, India (2007). 3. Castellan, G. W. Physical Chemistry 4th Ed. Narosa (2004). 4. Laidler, K. J. Chemical Kinetics Pearson Education: New Delhi (2004).

Biochemistry and Environmental Chemistry

Paper– HBCH 504 (L:3, credits)(Max marks (60+40) Time 3 hours






UNIT ICarbohydrates: Biological importance of carbohydrates, Metabolism, Cellular currency of

energy (ATP), Glycolysis, Alcoholic and Lactic acid fermentations,Krebs

Proteins: classification, biological importance; Primary, secondary and tertiary structures of proteins: α-helix and β- pleated sheets, Denaturation of proteins

Enzymes: Nomenclature, Characteristics (mention of Ribozymes), Classification;Active site, Mechanism of enzyme action, Stereospecificity of enzymes,Coenzymes and cofactors, Enzyme inhibitors, Introduction to Biocatalysis:Importance in “Green Chemistry” and Chemical Industry

UNIT II

Lipids: Biological importance of triglycerides and phosphoglycerides. Lipid membrane, Liposomes and their biological functions.

Structure of DNA (Watson-Crick model) and RNA, Genetic Code, Biological roles of DNA and RNA: Replication, Transcription and Translation (overview).

UNIT III

Environment and it’s segments, Ecosystems. Biogeochemical cycles of carbon, nitrogen and sulfur

Air Pollution: Major regions of atmosphere. Chemical and photochemical reactions in atmosphere. Air pollutants: types, sources, particle size and chemical nature; Photochemical Smog: its constituents and photochemistry, Environmental effects of Ozone, Major sources of Air pollution

Effects of air pollution on living organisms and vegetation, Controls of air pollution, Climate change, Green house effect, global warming. Techniques of measuring air pollutants.

Water Pollution: Hydrological cycle, water resources, aquatic ecosystems, Sources and nature of water pollutants, Techniques for measuring water pollution, Impacts of water pollution on hydrological and ecosystems. Water purification methods

UNIT IV

Energy and Enviornment: Sources of energy: Coal, petrol and Natural gas. Nuclear Fusion / Fisson, Solar energy, Hydrogen, geothermal, Tidal and Hydel etc.

Nuclear Pollution: Disposal of nuclear waste, nuclear disaster and it’s Management

Recommended Texts:1. Berg, J.M., Tymoczko, J.L. and Stryer, L. (2006) Biochemistry. VI the Edition. W.H. Freeman and Co. 2. Nelson, D.L., Cox, M.M. and Lehninger, A.L. (2009) principles of Biochemistry.IV Edition. W.H. Freeman and Co. 3. Murray, R.K., Granner, D.K., Mayes, P.A. and Rodwell, V.W. (2009) Harper’s Illustrated Biochemistry. XXVIII edition. Lange medical Books/ McGraw-Hill 4. Manahan S.E. (2005) Environmental Chemistry, CRC Press 5. Miller, G.T. (2006) Environmental Science 11th edition. Brooks/Cole 6. Mishra, A. (2005) Environmental Studies. Selective and Scientific Books, New

Inorganic Chemistry -IV

Paper- HBCH 551 P (P:2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

(a) Quantitative Analysis: The following quantitative estimations are to be carried out.

(i) Estimation of nickel (II) using Dimethylglyoxime as the precipitant. (ii) Estimation of copper as CuSCN (iii) Estimation of iron as Fe2O3 by precipitating iron as Fe(OH)3 through (i) Heterogeneous

and (ii) Homogeneous media. (iv) Estimation of Al (III) by precipitating with oxine and weighing as Al(oxine)3

(aluminium oxinate).

(b) Inorganic Preparations

(i) Tetraammine copper (II) sulphate, [Cu(NH3)4]SO4 H2O (ii) Potassium trisoxalatochromate (III), K3[Cr(C2O4)3] (iii) Cis and trans K[Cr(C2O4)2 (H2O2] Potassium dioxalatodiaquachromate (III) (iv) Pentaammine carbonato Cobalt (III) ion

(c) Spectrophotometric estimation of Ferrous ions by using 1,10 phenanthroline

Recommended Texts:

1. Vogel, A.I. A text book of Quantitative Analysis, ELBS 1986.

Organic Chemistry -IV

Paper- HBCH 552 P (P : 2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

1. Systematic analysis of extra elements in the given unknown compounds

2. Tests for following functional groups and unsaturation

3. Qualitative analysis of the following types of unknown organic compounds

Carboxylic acids, Phenols, Alcohols, Aldehydes, Ketones, Esters

Physical Chemistry -IV


PRACTICAL Marks: 50

(I) To study changes in conductance in the following systems (i) strong acid-strong base (ii) weak acid-strong base and (iii) mixture of strong acid and weak acid-strong base

(II) Study the kinetics of the following reactions. 1. Initial rate method: Iodide-persulphate reaction 2. Integrated rate method:

(a) Acid hydrolysis of methyl acetate with hydrochloric acid, volumetrically or conductometrically.

(b) Iodide-persulphate reaction (c) Saponification of ethyl acetate.

SEMESTER VI

Inorganic Chemistry -V


THEORY Marks: 100

Note:-





UNIT ITheoretical principles:

Theoretical principles and chemistry involved in qualitative analysis of mixture of cations and anions including interfering and insolubles.

UNIT IIOrganometallic Compounds:

Definition and classification of organometallic compounds, EAN rule.

UNIT IIIMetal carbonyls:Preparation, properties, structure and bonding of mononuclear carbonyls. π-acceptor behaviour of carbon monoxide, synergic effect (MO diagram of CO) Carbonylate anions, ferrocene and its reactions.

UNIT IVBioinorganic Chemistry:Metal ions present in biological systems, classification of elements according to their action in biological system. Excess and deficiency of some trace metals. Toxicity of metal ions (Hg, Pb, Cd and As), reasons for toxicity, Use of chelating agents in medicine Iron and its application in bio-systems, Hemoglobin; Storage and transfer of iron.

Recommended Texts:

1. Purcell, K.F & Kotz, J.C. Inorganic Chemistry W.B. Saunders Co, 1977. 2. Huheey, J.E., Inorganic Chemistry, Prentice Hall, 1993. 3. Lippard, S.J. & Berg, J.M. Principles of Bioinorganic Chemistry Panima Publishing

Company 1994. 4. Cotton, F.A. & Wilkinson, G, Advanced Inorganic Chemistry. Wiley-VCH, 1999.

.Organic Chemistry -V


THEORY Marks: 100

Note:-





Unit I: Organic spectroscopy-I

General principles Introduction to absorption and emission spectroscopy.

UV Spectroscopy: Types of electronic transitions, λmax, Chromophores and Auxochromes, Bathochromic and Hypsochromic shifts, Intensity of absorption; Application of Woodward Rules for calculation of λmax for the following systems: α,β unsaturated aldehydes, ketones, carboxylic acids and esters;

UNIT-IIIR Spectroscopy: Fundamental and non-fundamental molecular vibrations; IR absorption positions of O, N and S containing functional groups; Effect of H- bonding, conjugation, resonance and ring size on IR absorptions; Fingerprint region and its significance; application in functional group analysis.

Unit III Organic spectroscopy-IINMR Spectroscopy: Basic principles of Proton Magnetic Resonance, chemical shift and factors influencing it; Spin – Spin coupling and coupling constant; Anisotropic effects in alkene, alkyne, aldehydes and aromatics, Interpetation of NMR spectra of simple compounds

Applications of IR, UV and NMR for identification of simple organic molecules.

Unit IVPolymers

Introduction and classification including di-block, tri-block and amphiphilic polymers; Number average molecular weight, Weight average molecular weight, Degree of polymerization, Polydispersity Index.Polymerisation reactions - Addition and condensation - Mechanism of cationic, anionic and free radical addition polymerization; Metallocene-based Ziegler-Natta polymerisation of alkenes;

Preparation and applications of plastics – thermosetting (phenol-formaldehyde, Polyurethanes) and

thermosoftening (PVC, polythene);

Fabrics – natural and synthetic (acrylic, polyamido, polyester);

Rubbers – natural and synthetic: Buna-S, Chloroprene and Neoprene; Vulcanization;

Biodegradable and conducting polymers with examples.

Recommended Texts:

1. Kemp, W. Organic Spectroscopy, Palgrave.

2. Kalsi, P. S. Textbook of Organic Chemistry (1st Ed.), New Age International (P) Ltd. Pub.

3. Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

Billmeyer, F. W. Textbook of Polymer Science, John Wiley & Sons, Inc.

Physical Chemistry -VPaper- HBCH 603 (L:3, credits)(Max marks (60+40) Time 3 hours






Unit IQuantum Chemistry-I

Postulates of quantum mechanics, quantum mechanical operators, Schrödinger equation and its application to free particle and “particle-in-a-box” (rigorous treatment), quantization of energy levels, zero-point energy and Heisenberg Uncertainty principle; wavefunctions, probability distribution functions, nodal properties, Extension to two and three dimensional boxes.

UNIT-IIQuantum Chemistry-II

Qualitative treatment of hydrogen atom and hydrogen-like ions: setting up of Schrödinger equation in spherical polar coordinates, radial part, quantization of energy (only final energy expression), Average and most probable distances of electron from nucleus.

UNIT IIIMolecular Spectroscopy-I:

Interaction of electromagnetic radiation with molecules and various types of spectra; Born-Oppenheimer approximation.

Rotation spectroscopy: Selection rules, intensities of spectral lines, determination of bond lengths of diatomic and linear triatomic molecules.

Vibrational spectroscopy: Classical equation of vibration, computation of force constant, amplitude of diatomic molecular vibrations, anharmonicity, dissociation energies, fundamental frequencies, overtones, hot bands, degrees of freedom for polyatomic molecules, modes of vibration, concept of group frequencies.

UNIT-IVMolecular Spectroscopy-II:

Electronic spectroscopy: Franck-Condon principle, electronic transitions, singlet and triplet states, fluorescence and phosphorescence.

Nuclear Magnetic Resonance (NMR) spectroscopy: Principles of NMR spectroscopy, Larmor precession, chemical shift and low resolution spectra, different scales, spin-spin coupling and high resolution spectra,

Electron Spin Resonance (ESR) spectroscopy: Its principle, hyperfine structure, ESR of simple radicals.

Recommended Texts:

1. Banwell, C. N. & McCash, E. M. Fundamentals of Molecular Spectroscopy 4th Ed. Tata McGraw-Hill: New Delhi (2006).

2. Chandra, A. K. Introductory Quantum Chemistry Tata McGraw-Hill (2001). 3. House, J. E. Fundamentals of Quantum Chemistry 2nd Ed. Elsevier: USA (2004).

4. Lowe, J. P. & Peterson, K. Quantum Chemistry Academic Press (2005).

Fundamental in computer and software

Paper- HBCH -604 (L:3, credits)(Max marks (60+40) Time 3 hours






UNIT-I

Introduction to Computer Systems; Data representation: Number systems, character representation codes, Binary, hex, octal codes and their inter conversions. Binary arithmetic, Floating point arithmetic, signed and unsigned numbers IEEE standards, CPU organization, ALU, registers, memory, the idea of program execution at micro level. Concept of computing, contemporary Operating Systems such as DOS, Windows, UNIX etc. (only brief user level description). Introduction to organization and architecture of mainframe, mini and micro systems.

UNIT-II

Concept of flow chart and algorithm; Algorithms to programs: specification, top-down development and stepwise refinement ,Introduction to the design and implementation of correct, efficient and maintainable programs, structured Programming, Use of high level programming Language for the systematic development of programs, programmability and programming languages, Object codes, compilers. Introduction to the Editing tools such as vi or MS-VC editors.

UNIT-III

C: Data types, Identifiers, Storage class, Constant, Operators, expression, Statements, console I/O statements, Selection statements: if-else, switch, Iteration Statements: for, while, do-while, Jump statements: return, go to, break, continue, comments. Function, Call by value, Call by reference, arguments to main(), return statements, recursion, function prototypes, reprocessor directives.

UNIT-IV

Single dimensional arrays, two dimensional arrays, multidimensional arrays, variable length arrays. Strings, array of strings. Structures: array of structures, passing structure to function, structure pointers, structure within structures. Unions, bit fields, enumerations. Pointer variables, pointer operator, pointer expression array of pointers, multiple indirection, pointers to functions, dynamic allocation functions.

Recommended Texts:

1. Noggle, J. H. Physical chemistry on a Microcomputer. Little Brown & Co. (1985). 2. Venit, S.M. Programming in Basic: Problem solving with structure and style.

Jaico Publishing House: Delhi (1996). 3. Engel, T. & Reid, P. Physical Chemistry 2nd Ed. Pearson (2010). Chapter on

Computational Chemistry.

Inorganic Chemistry -V

Paper - HBCH 651 P (P : 2 , 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

Qualitative analysis:

Using H2S /PTC/ Thioacetamide or any other reagent. Identification of cations and simple anions in a mixture of salts containing not more than six ions (Three cations and three anions) interfering anions using semimicro scheme of analysis. If combination of cations or anions is given in the mixture, insoluble should be avoided. Spot tests should be carried out for final identifications wherever feasible.

Cation : Pb2+, Bi3+ Cu2+, Cd2+, As3+, Sb3+, Sn2+ or Sn4+, Fe2+ OR Fe3+, Al3+, Cr3+,Co2+, Ni2+,Zn2+, Mn2+, Ba2+, Sr2+, Ca2+, Mg2+, NH4

+, K+

Anion : CO32-

, SO32-

, CO23, SO2-

3, S2-, NO-2, CH3 COO-, NO-

3, Cl-, Br-, I-, SO42-, PO4

3-, BO33-,

F-, C2O2-4

Organic Chemistry -V Paper - HBCH 652 P (P :2 , 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

1. Tests for following functional groups

2. Qualitative analysis of following types of unknown organic compounds 1. Carbohydrates 2. Primary, secondary and tertiary amines 3. Nitro compounds 4. Amides 5. Aryl halides

Hydrocarbons Identification of the functional groups, C-C and C-N triple bonds, sp3, sp2 and sp hybridized C-H bonds by IR spectroscopy (IR spectra to be provided)

Paper- HBCH 653 P (P : 2, 2 credits) (Max marks (30+20) Time 3 hours

PRACTICAL Marks: 50

• Colourimetry • Verification of Lambert-Beer's Law • Determination of pK (indicator) for phenolphthalein or methyl red • Study the formation of a complex between ferric and thiocyanate (or salicylate) ions. • Study the kinetics of interaction of crystal violet with sodium hydroxide colourimetrically. • Analysis of the given vibration-rotation spectrum of HCl(g) • Record the UV spectrum of p-nitrophenol (in 1:4 ethanol:water mixture). Repeat after adding a

small crystal of NaOH. Comment on the difference, if any. • Record the U.V. spectrum of a given compound (acetone) in cyclohexane

(a) Plot transmittance versus wavelength.

(b) Plot absorbance versus wavelength.

(c) Calculate the energy involved in the electronic transition in different units, i.e. cm-1, kJ/mol, kcal/mol & eV.


Note: Textbook Recommended

1. Inorganic-Chemistry B.Sc (I,II & III), By :- Prof. P.N.Kapil, Dinesh and Co.2. Organic Chemistry B.Sc (I,II & III), By :- Prof. P.N.Kapil, Dinesh and Co.3. Physical Chemistry B.Sc (I,II & III), By :- Prof. P.N.Kapil, Dinesh and Co.4. Inorganic-Chemistry B.Sc (I,II & III), By :- Prof.K.K. Bhasin, Pradeeps publications5. Organic Chemistry B.Sc (I,II & III), By :- Prof.S. N. Dhawan, Pradeeps publications.6. Physical Chemistry B.Sc (I,II & III), By :- Prof.S.C. Khetarpal, Pradeeps publications.7. Inorganic-Chemistry B.Sc (I,II & III), By :- Prof.S.P. Jauhar, Modern publishers8. Organic Chemistry B.Sc (I,II & III), By :- Prof J. M. Sehgal, Modern publishers9. Physical Chemistry B.Sc (I,II & III), By :- Prof. B.N.Kapil, Modern Piblishers10. Chemistry for degree students By :- Dr. R. L. Madan, S chand and Company

Documents

IEC UNIVERSITY DEPARTMENT OF CHEMISTRY of...Inorganic Chemistry – IV 3 0 0 20 40 0 60 40 100 4 2. HBCH 502 Organic Chemistry-IV 3 0 0 20 40 0 60 40 100 4 3. HBCH 503 Physical Chemistry