2 KANNUR UNIVERSITY (Abstract) B Sc Chemistry Programme under CCSS – Revised Scheme & Syllabus of Core & Open Courses under Choice Based Credit Semester System - Implemented - Orders issued. ACADEMIC BRANCH U.O.No.Acad/C2/754/2007 K.U.Campus,Dated, 12-06-2012 Read: 1. U.O No.Acad/C2/3838/2008 dated 07-07-2009. 2. U.O No Acad/C2/7101/2009 dated 15-06-2010, 16-09-2010 3. U.O No Acad/C2/7101/2009(2) dated 21-03-2012 4. U.O No. Acad C2/754/2007(1) dated 10-07-2009. 5. U.O.No.Acad/C2/754/2007 dated 23 -03-2011. 6. U.O.No.Acad/C2/754/2007 dated 08-05-2012 7. Letter dated 02-06-2012 from the Chairman, BoS in Chemistry (UG). ORDER 1. The Regulations for Choice Based Credit Semester System for undergraduate programmes were implemented in this University with effect from 2009 admission as per paper read (1) and certain modifications were effected to the same as per paper read (2) & (3) above. 2. The Scheme and Syllabus of B Sc Chemistry/ Polymer Chemistry/ Biochemistry (Core/ Complementary/ Open Courses) under Choice Based Credit Semester System were implemented in this University w.e.f. 2009 admission as per paper read (4) & (5) above. 3. The Chairman, Board of Studies in Chemistry (UG) vide paper read (7) above has informed that the Board of Studies has recommended the interchange of Open Courses with effect from 2010 admission and requested to revise the order(6) accordingly. 4. The Vice Chancellor after considering the matter in detail, and in exercise of the powers of the Academic Council, as per Section 11(1) of Kannur University Act, 1996 and all other enabling provisions read together with, has accorded sanction to permit the interchange of Open Courses (V & VI Semesters) of B Sc Chemistry Programme under Choice Based Credit Semester System with effect from 2010 admission onwards. 5. Orders are therefore issued implementing the revised Scheme & Syllabus of Core Courses with effect from 2012 admission and interchange of Open Courses of the Programme with effect from 2010 admission as shown below. The following portions from Module 1 in 1B01CHE METHODOLOGY OF CHEMISTRY AS A DISCIPLINE OF SCIENCE are deleted.(w.e.f.2012 Admission)
Transcript
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KANNUR UNIVERSITY
(Abstract)
B Sc Chemistry Programme under CCSS – Revised Scheme & Syllabus of Core & Open Courses under Choice Based Credit Semester System - Implemented - Orders issued.
Read: 1. U.O No.Acad/C2/3838/2008 dated 07-07-2009. 2. U.O No Acad/C2/7101/2009 dated 15-06-2010, 16-09-2010 3. U.O No Acad/C2/7101/2009(2) dated 21-03-2012
4. U.O No. Acad C2/754/2007(1) dated 10-07-2009. 5. U.O.No.Acad/C2/754/2007 dated 23 -03-2011. 6. U.O.No.Acad/C2/754/2007 dated 08-05-2012 7. Letter dated 02-06-2012 from the Chairman, BoS in Chemistry (UG).
ORDER
1. The Regulations for Choice Based Credit Semester System for undergraduate programmes were implemented in this University with effect from 2009 admission as per paper read (1) and certain modifications were effected to the same as per paper read (2) & (3) above.
2. The Scheme and Syllabus of B Sc Chemistry/ Polymer Chemistry/ Biochemistry (Core/ Complementary/ Open Courses) under Choice Based Credit Semester System were implemented in this University w.e.f. 2009 admission as per paper read (4) & (5) above.
3. The Chairman, Board of Studies in Chemistry (UG) vide paper read (7) above has informed that the Board of Studies has recommended the interchange of Open Courses with effect from 2010 admission and requested to revise the order(6) accordingly.
4. The Vice Chancellor after considering the matter in detail, and in exercise of the powers of the Academic Council, as per Section 11(1) of Kannur University Act, 1996 and all other enabling provisions read together with, has accorded sanction to permit the interchange of Open Courses (V & VI Semesters) of B Sc Chemistry Programme under Choice Based Credit Semester System with effect from 2010 admission onwards.
5. Orders are therefore issued implementing the revised Scheme & Syllabus of Core Courses with effect from 2012 admission and interchange of Open Courses of the Programme with effect from 2010 admission as shown below.
The following portions from Module 1 in 1B01CHE METHODOLOGY OF CHEMISTRY AS A DISCIPLINE OF SCIENCE are deleted.(w.e.f.2012 Admission)
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i) ‘Chemical Science in the service of man : Drugs, food, flavouring agents, sweeteners, cosmetics, soaps and detergents, paints, varnishes, textiles, dyes, fertilizers, insecticides, fuels etc.One example for each.’
ii) ‘Classification (Periodic classification of elements, classification of organic compounds in to homologous series), Analytical (qualitative and quantitative), preparation, synthesis and manufacture’.
The following Open Courses in the V and VI Semester are interchanged (Effective from 2010 admission).
i) The Course 5D03CHE ENVIRONMENTAL STUDIES is shifted to VI Semester as 6D02CHE ENVIRONMENTAL STUDIES.
ii) The Course 6D02CHE FOOD SCIENCE is shifted to V Semester as 5D03CHE FOOD SCIENCE. 6. The U.O read (6) above stands modified to this extent.
Sd/-
DEPUTY REGISTRAR (Academic)
For REGISTRAR
To The Principals of Colleges offering B. Sc. Chemistry Programme. Copy to: 1. The Examination Branch (Through PA to CE)
2. The Chairman, BoS in Chemistry (UG) 3. PS to VC/ PA to PVC/ PA to Registrar Forwarded/By Order
No Semester Course Code Title of the course Contact Hours/week
Credits
1 I 1B01CHE Methodology of Chemistry as Discipline of Science
2 2
2 I 1B02CHE Core course Practical -I Volumetric Analytics Part- I
2 -
3 II 2B03CHE Theoretical and Inorganic Chemistry
2 2
4 II 2B02CHE Core course practical -I Volumetric Analytics Part -II
2 4
5 III 3B04 CHE Inorganic Chemistry-I 3 3 6 III 3B05CHE Core Course Practical -I I
Inorganic Qualitative Analysis & Preparation Part -I
2 -
7 IV 4B06 CHE Inorganic Chemistry-II 3 3 8 IV 4B05 CHE Core Course Practical -I I
Inorganic Qualitative Analysis & Preparation Part -II
2 2
9 V 5B07 CHE Physical Chemistry –I 5 4 10 V 5B08 CHE Physical Methods in Chemistry 4 4 11 V 5B09 CHE Organic Chemistry-I 4 4 12 V 5B10 CHE Core Course Practical-III
Gravimetric Analysis 5 -
13 V 5B11 CHE Core Course Practical-IV Organic Chemistry
5 -
14 VI 6B13 CHE Physical Chemistry –II 5 4 15 VI 6B14 CHE Organic Chemistry-II 4 4 16 VI 6B15 CHE Elective
A.Environmental Chemistry B. Food Chemistry C. Industrial Chemistry D. Synthetic Organic Chemistry E. Analytical Chemistry F. Nano Materials –Synthesis & Practice
4 4
17 VI 6B10&11CHE Core Course Practicals –III&IV 5 6 18 VI 6B16 CHE Core Course Practical Physical
1 5 5D01CHE Chemistry in service to Man 2 2 2 5 5D02CHE Chemistry in everyday life 2 2 3 5 5D03CHE Food Science 2 2 4 6 6D01CHE Drugs-Use & Abuse 2 2 5 6 6D02CHE Environmental Studies 2 2 6 6 6D03CHE Nano Materials Synthesis & Practice 2 2
Scheme-Complementary Course (Chemistry)
Scheme for Open Courses
9
1B01CHE – Methodology of Chemistry as a discipline of Science
Credits-2 Contact Hours-36
Aim: To illustrate the methodology of science in chemistry
Objectives :
• To have a broad outline of the methodology of science in general and Chemistry in particular.
• To understand the important analytical and instrumental tools used for practicing chemistry.
• To learn computer based presentation and statistical analysis of data using spreadsheet software.
• To apply these skills in the analysis of experimental data in chemistry practical. •
Module - 1 Chemistry as a discipline of science (9 hrs)
What is Science? Scientific statements, Scientific methods – observation – posing a question – formulation of hypothesis – experiment theory – law. Falsification (disproving) of hypothesis, inductive and deductive reasoning, revision of scientific theories and laws. Methods of science as illustrated through the following:
i)Laws of chemical combination – Faradays laws of electrolysis – Daltons atomic theory – atom models – J.J.Thomson, Rutherford, Bohr model and quantum mechanical model of atom. ii) n-P-V-T relation of gases-gas laws – kinetic molecular theory.
Role of concepts and models in science.
Evolution of Chemistry – ancient speculations on the nature of matter, early form of chemistry – alchemy, origin of modern chemistry. Structure of chemical science: scope of chemical science, theory and experiment, branches of chemistry. Role of Chemistry as a central science connecting Physics, Biology and other branches of science. Interdisciplinary areas involving Chemistry – Nanotechnology, Biotechnology.
Methodology of chemistry: Symbols, formulae, Chemical equations. References
1. J.A.Lee, Scientific Endeavor, Addison Wesley Longman (chapters 1 and 2) 2. C.N.R. Rao, University Chemistry, Universities Press (India) Pvt. Ltd (Chapters 1 and 2)
Module –2. Research in Science (9 hours)
Selecting a topic – hypothesis – design of experiment: variables, correlation and causality, sampling, use of controls, experimental bias, analysis, results, discussion of results, models.
Summary of the scientific methods. Writing Science
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Reference
J.A.Lee, Scientific Endeavor, Addison Wesley Longman (chapters 3, 9 and Appendix 3) Module-3. Analytical and synthetic methodologies in Chemistry (9 hours) Titrimetric analysis : Fundamental concepts – mole, molarity, molality, ppm and ppb primary standard – secondary standard, quantitative dilution – problems. Acid base titrations – titration curves – pH indicators. Redox titrations – titration curve – titrations involving MnO4
- and Cr2O72-
- redox indicators. Complexometric titrations – EDTA titrations – titration curves – indicators – Gravimetric analysis: Unit operations in gravimetric analysis illustrations using iron and barium estimation. Synthetic methodologies – condensation – addition – examples. Separation and purification techniques – Filtration, Crystallization and precipitation – concept of solubility product as applied in group separation of cations – problems. Fractional distillation, Solvent extraction.
References
1. B.R.Puri, L.R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi (Chapter 40).
2. D.A.Skoog, D.M.West and S.R. Crouch, Fundamentals of Analytical Chemistry 8th edn, Brooks/Cole Nelson Chapters 12-17).
3. Vogel’s Text book of Quantitative Chemical Analysis 6th edn, Pearsons Education Ltd (Chapters 10, 11).
4. G.D.Christian, Analytical Chemistry, John Wiley and Sons (Chapters 5, 7, 8, 16, 17) Module-4. Data Analysis (9 hours) Units, significant digits, rounding, scientific and prefix notation, graphing of data – Precision and accuracy – Types of errors – Ways of expressing precision – Ways to reduce systematic errors – reporting analytical data, Statistical treatment of analytical data – population and samples – Mean and standard deviation – distribution of random errors – confidence limits – tests of significance – Correlation and regression – linear regression analysis, calculation of regression coefficients (slope, Intercept) using scientific calculator – methods of least squares.
The following section is non-evaluative for theory examination Familiarization of software packages for analysis and graphical representation of data – MS Excel, Origin, Open office calc (Physical Chemistry experiments using software packages are included in the 5th and 6th semesters), simulations, virtual experiments, drawing molecular structures using Chemsketch, ISIS Draw.
References
1. B.R. Puri, L.R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi (Chapter 40)
3. D.A.Skoog, D.M.West and S.R.Crouch, Fundamentals of Analytical Chemistry 8th edn, Brooks/Cole Nelson (Chapters 5-8)
4. Vogel’s Text book of Quantitative Chemical Analysis 6th edn, Pearsons Education Ltd
(Chapters 4). 5. G.D.Christian, Analytical Chemistry, John Wiley and Sons (Chapters 2) 6. R.Crouch and F.J.Holler, Applications of Microsoft Excel in Analytical S.Chemistry,
Brooks/Cole. Further Reading
1. J.Mills and P.Evans, Core Chemistry, Foundation books Pvt. Ltd, New Delhi (2004) 2. T.F.Gieryn,Cultural boundaries of science, University Chicago Press, 1999. 3. H.Collins and T.Pinch, The Golem, What everyone should know about science, Cambridge
University Press, 1993. 4. Hewitt, Paul G, S.Lyons, J.A.Suchocki and J.Yeh, Conceptual Integrated Science, Addison
Wesley, 2007. 5. Methods for Teaching Science as Inquiry, Allyn and Bacon, 2009. 6. K.V.S. Sarma, Statistics made simple, Prentice – Hall of India, New Delhi. 7. R.Crouch and F.J.Holler, Applications of Microsoft Excel in Analytical S.Chemistry,
Brooks/Cole. 8. R.D.Jarrard, Scientific Methods, [email protected],2001. 9. R.Sangenburg D.K.Moser, History of Science (5 Volumes), Universities Press (India) Ltd.
To impart essential theoretical knowledge on atomic structure, periodic properties,
chemical bonding, and nuclear chemistry.
Objectives:
• To study the various atom models. • To understand the important features of the quantum mechanical model of the atom. • To study the periodic properties of elements. • To explain the formation of different types of bonds. • To predict the geometry of simple molecules. • To explain the different types of hybridisation and draw shapes of simple covalent
molecules. • To understand the molecular orbital theory of diatomic molecules. • To develop interest in various branches of inorganic chemistry. • To study nuclear models and nuclear reactions. •
Module – 1. Atomic Structure (10 Hrs) Bohr model of hydrogen atom, Bohr’s equation for the energy of electron in hydrogen
atom, the hydrogen spectrum, limitations of Bohr theory, photoelectric effect, idea of de Broglie matter waves, Heisenberg’s uncertainty principle and its significance, Schrodinger wave equation (derivation not expected), wave functions, significance of Ψ (psi) and Ψ2, atomic orbitals, Nodal planes in atomic orbitals, quantum numbers (n, l, m), Zeeman effect, Stern-Gerlac experiment, spin quantum number(s), shapes of s, p and d orbitals. Aufbau and Pauli’s exclusion principles, Hund’s rule, energy level diagram of a multielectron atom, concept of effective nuclear charge, Slater’s rules and applications, Electronic configuration of atoms.
2. B.R.Puri, L.R.Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi (Chapter 1).
3. C.N.R.Rao, University General Chemistry, Macmillan, 3rd edn., John Wiley 2001 (Chapter 1).
4. F.A.Cotton, G.Wilkinson and P.L.Gans, Basic Inorganic Chemistry, 3rd edn., John Wiley (Chapter 2).
5. D.F.Shriver and P.W.Atkins, Inorganic Chemistry, 3rd edn., Oxford University Press (Chapter 1).
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6. B.Douglas, D.Me Daniel, John Alexander, Concepts and models in Inorganic Chemistry (Chapter 1).
Module – 2. Chemical Bonding (16 hrs)
Ionic bond – nature of ionic bond, properties of ionic compounds, radius ratio and coordination number, factors favouring the formation of ionic compounds. Lattice energy, Born- Lande equation with derivation, factors affecting lattice enthalpy, Born-Haber cycle and its applications, solvation enthalpy and solubility of ionic compounds.
Covalent bond – valence bond theory and its limitations, concept of resonance, resonance energy, hybridisation and shapes of simple molecules (BeF2, PCI3, SF6, CH4, Ethane, ethene and ethyne) VSEPR theory, shapes of molecules and ions (NH3, XeF6, CIF3, NH4
+, H3O+). Molecular orbital theory – LCAO method, molecular orbital energy diagram and properties of homo and hetero diatomic molecules (N2, O2, CO and NO), bond strength and bond energy. Polarisation of covalent bond, polarising power and polarisability of ions, Fajan’s rule.
Dipole moment and molecular structure – percentage ionic character from dipole moment. Metallic bonding – free electron theory, valence bond theory and band theory, explanation
of metallic properties based on these theories. Weak chemical forces – hydrogen bond, inter and intra molecular hydrogen bonds, effects
of hydrogen bonding, van der Waals forces. References
2. B.R.Puri, L.R.Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi (Chapter 4, 5).
3. C.N.R.Rao, University General Chemistry, Macmillan 3rd edn., John Wiley, 2001 (Chapter 3)
4. F.A.Cotton, G.Wilkinson and P.L.Gans, Basic Inorganic Chemistry, 3rd edn., John Wiley (Chapter 3, 4).
5. D.F.Shriver and P.W.Atkins, Inorganic Chemistry, 3rd edn., Oxford University Press (Chapter 2, 3).
Module – 2. Nuclear Chemistry (10 Hrs)
Nuclear particles, nuclear forces, nuclear size, nuclear density, stability of nucleus, binding energy, magic numbers, packing fraction, n/p ratio. Nuclear models – liquid drop model and shell model.
Natural radioactivity, modes of decay, decay constant, half life period, average life, radioactive equilibrium, Geiger-Nuttal rule, units of radioactivity, radiation dosage.
Induced radioactivity, nuclear reactions induced by charged projectiles, neutrons and γ rays fission reactions, fusion reactions, spallation reactions, preparation of transuranic elements, Q values of nuclear reactions. Fertile and fissile isotopes, chain reaction, stellar energy.
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References
1. B.R.Puri, L.R.Sharma, Kalia Principles of Inorganic Chemsitry, Milestone Publishers, New Delhi (Chapter 38).
2. H.J.Arnikar, Essentials of Nuclear Chemistry, New Age International (Chapter 3 –5). 3. R.Gopalan, Elements of Nuclear Chemistry, Vikas, Publ. House.
2. G.Wulfsberg, Inorganic Chemistry, Viva Books. 3. W.L.Jolly, Inorganic Chemistry, Ttata Mc Graw Hill. 4. J.D.Lee, New Concise Inorganic Chemistry. 5. M.N.Greenwood and A.Earnshaw, Chemistry of the elements 2nd edn., Butterworth. 6. Manas Chanda, Atomic structure and chemical bonding. 7. H.J.Emeleus, A.G.Sharpe, Modern Aspects of Inorganic Chemistry, Universal Book
Stall. 8. J.David Brown, the Chemical Bond in Inorganic Chemistry, Oxford Science
Publication.
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3B04 CHE Inorganic Chemistry I Credit – 3 Contact hours – 54
Module 1. Periodic Properties
Long form of the periodic table – periods and groups – Periodic table and electronic configuration – Division in to s, p, d and f blocks. Periodic properties – Effective nuclear charge – Screening constant – Evaluation using stater rules – Definition, factors, influencing and periodic trends in ionization energy, electron affinity and electro negativity (Pauling and Mullickan scab) – Atomic and ionic radii. ( 4 hrs)
Module 2.Chemistry of ‘s’ block elements
2.1 Hydrogen : Isotopes (separation method not needed). Ortho and parahydrogen – Hydrieds and their classification.
2.2 Alkali and alkaline earth metals : Occurrence and extraction (principle only). Comparative study based on electronic
configuration and periodic properties of hydrieds, oxides, halides, nitrides, carbides, hydrxides, carbonates and sulphates (Preparation and chemical properties of these compounds not needed). Metal solutions in liquid ammonia – characteristic properties and uses. Diagonal relationship. (5 hrs)
Module 3. Chemistry of p-block elements 3.1 Occurrence and isolation of elements (principle only) – allotropy – Comparative study
based on electronic configuration and periodic properties of binary compounds (hydrides, oxides, halides, carbides and sulphides) and oxyacids, relative stability of valencigs in these compounds, inert pair effect, metallic and non-metallic character, acid-base properties of oxides, hydrolysis of halides and exceptional behaviour of second period element in the following groups of elements – Group 13, (B, Al, Ga, In and Tl, Group 14 (C, Si, Ge, Sn and Pb) Group 15 (N, P, As, Sb and Bi) Group 16 (O, S, Se, Te and Po) and Group 17 (F, d, Br and I). (14 hrs)
3.2 Noble gases : Electronic configuration and position in the periodic table – Occurrence – Noble gas chemistry – clath rates and compounds of Xenon; XeF2, XeF4, XeF6, XeO2F2, XeOF2, XeO5, XeO4 and XeO6
4-. Preparation, use β (of elements and compounds), hybridization and geometry of these compounds. (3 hrs)
Module 4.Co-ordination Chemistry:
Introduction – Double salt and Co-ordination compounds – Werner’s Co-ordination theory, Nomenclature – Isomerism – types of ligands – Electronic interpretation of Werner’s theory – EAN rule.
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Modern theories of M-L bond – valence bond theory – hybridization in tetrahedral, square planar and octahedral complexes – explanation of magnetic properties based on VBT. Crystal field theory, Crystal field splitting ion octahedral, tetrahedral and square planar geometries. Explanation of spectral and magnetic properties –Spectro chemical series. Stability of complexes – Kinetic and thermo dynamic stability – chelate effect. Application complex formation in qualitative and quantitative analysis. ( 12 hrs)
Module 5.Organometallic Compounds :
Introduction – classification based on metal carbon bond. Metal carbonyls – preparation, properties structure and uses of mononuclear (Ni, Fe, Mn) binuclear (Fe, Mn, Co) and trinuclear (Fe) metallic carbonyl. Application of 18e- rule to predict M-M bond. Preparation properties structure and bonding in ferrocene. ( 6 hrs)
Module 6.Analytical Chemistry : Errors in Quantitative analysis – classification and
minimization of errors.Accuracy and precision. Principles of Chromatographic separations – Types of Chromatography – adsorption, partition and ion exchange chromatography – chromatographic techniques – Thin layer colum and paper chromatography – Gas chromatography. Theory of titrations – acid base titration, redox titration, precipitation titration and complexometric titration – Indicators acid-base, redox and metal – ion indicators. Gravimetric analysis – Solubility product – factors affecting solubilities of precipitates – Co-precipitation and post precipitation – errors due to precipitation. (12 hrs)
References
1. Advanced Inorganic Chemistry - Cotton and Wilkinson 2. Concise Inorganic Chemistry - J.D.Lee 3. Modern approach to Inorganic chemistry – Bell and Lott 4. University General Chemistry - CNR Rao 5. Theoretical Inorganic Chemistry – J.Huhey 6. Industries in Kerala - K.R.Rajan 7. Principles of Inorganic Chemistry – Emelns and Anderson 8. Advanced Inorganic Chemistry - S.K.Agarwala and Keemitilal
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Credits -3
Contact Hours-54
4B06CHE Inorganic Chemistry II
Module 1.Metallurgy: Occurrence of metals – minerals and ores – classification ( 8 hrs)
Concentration of ores – gravity separation, magnetic separation and froth Floatation processes with suitable examples. Metallurgical process + Pyrometallurgy – Sintering, calcination and roasting smelting (principle with one example). Hydrometallurgy – Leaching and reduction from solution with one example (Principle and chemical equations only). Electrometallurgy – molten salt electrolysis and aqueous solution electrolysis with one example (principle and chemical equations only). Reducing agents in metallurgy – C, CO, hydrogen, metals with at least one example.
Module 2. Bioinorganic Chemistry : (6 hrs)
Metal ions present in the biological system – metal ion deficiency and excess and diseases related to them – metal ion toxicity (Pd, Cd, As and Hg). Structure and functions of haemoglobin and myoglobin. Metal ion transport across cell membrane – Na/k pump.
Biochemistry of Mg and Ca. Metallo enzymes of iron and zinc (structural details not needed).
Module 3. Transition elements : (14 hrs)
Position in the periodic table. General properties – electronic configuration, Oxidation
states, spectra magnetic properties, tendency to form complexes and catalytic properties,
tendency to form alloys and formation of non-stoichiometric compounds – Comparison of
first transition series with second and third series.
Module 4. Inner transition elements (12 hrs)
Lanthanides – Occurrence and separation by ion – exchange chromatography. Electronic
configuration, oxidation states, magnetic properties and spectra of lanthanide – Lanthanide
contraction – causes and consequences.
Actinides : Electronic configuration, Oxidation states spectra and magnetic properties.
Trans actinide elements – Preparation, IUPAC nomenclature.
Comparison of transition and inner transition elements.
Module 5. Industrial Chemistry : (6 hrs)
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Chemical Industries in Kerala – Sugar, alcohol, FiO2, glass, cement, HCl, H2So4, NaOH,
Urea, Ammonium phosphates and Super phosphate of lime (Location, raw materials,
Chemistry involved in the preparation and uses) Module 6. Preparation, properties structure and uses of some inorganic compounds. ( 8 hrs)
Hydrides of boron – B2H6 and B4H10, borazine, boric acid, oxy acids of halogens, Inter
References 1. Advanced Inorganic Chemistry - Cotton and Wilkinson
2. Concise Inorganic Chemistry - J.D.Lee
3. Modern approach to Inorganic chemistry – Bell and Lott
4. University General Chemistry - CNR Rao
5. Theoretical Inorganic Chemistry – J.Huhey
6. Industries in Kerala - K.R.Rajan
7. Principles of Inorganic Chemistry – Emelns and Anderson
8. Advanced Inorganic Chemistry - S.K.Agarwala and Keemitilal
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Credits 4
Contact hrs 90
5B07CHE Physical Chemistry - 1
Module 1 The Properties of Gases (15 hrs)
Gas laws – The general gas equation – Mixture of gases – Dalton’s Law – Mole fraction and partial pressure – calculation of partial pressure – The Kinetic model of gases – Molecular Speeds – Maxwell’s distribution of molecular speeds – Calculation of most probable velocity, average velocity and root mean square velocity – Average kinetic energy – Collision diameter – Mean free path, Collision number and collision frequency – Degrees of freedom of a gaseous molecule – Principle of equipartition of energy and contribution towards heat capacity of an ideal gas. Real gases – Molecular attractions – The compression factor – virial equation of state – Van der waals equation expressed in virial form – calculation of Boyl’s temperature – Isotherm of real gases and their comparison with Van der waals isotherms – continuity of states – critical phenomenon – critical constants of a gas and its determination – Determination of molecular mass by limiting density method – Principle of corresponding states – Liquefaction of gases by Joule Thomson effect and adiabatic demagnetization.
Module II Liquid State (10 hrs)
Theory of liquids – Vacancy theory and free volume theory – Properties of liquids – vapour pressure and its determination – Heat of vapourisation – Trouton’s rule – Surface tension and its determination – Interfacial tension – surface active agents – Parachor and its applications – Viscosity and its determination – refractive index – specific and molar refraction – Measurement of refractive index – Abbe’s refractometer – optical activity and its measurement using Polarimeter.
Module III Solid State (15 hrs)
Amorphous and crystalline solids – Laws of crystallography – Crystal lattices – Unit cells – seven crystallographic systems – Bravais lattices – Spacing of lattice planes in simple cubic, body centred and face centred cubic systems – Number of particles per unit cell in each of these - Calculation of Avogadro number, density and molecular mass from crystallographic data. Determination of internal structure of crystals by X-ray diffraction methods – derivation of Bragg’s equation – Bragg’s rotating crystal method and De bye Scherrer Powder diffraction method – Crystal structure of NaCl – anomalous nature of diffraction pattern of KCl – Co-ordination Number – Efficiency of packing – Cubic and Hexagonal packing – Radius ratio rule – Tetrahedral and Octahedral voids. Classification based on cohesive forces in crystals-ionic, covalent, molecular and metallic crystals – Liquid crystals – types – Examples – applications – Properties of solids – Mechanical, Rheological and elastic – Electrical conductivity – Conductor, semiconductors
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7. CaCO3 (s) → CaO (s) + CO2 (g) 8. NH4 HS (g) → NH3 (g)+ H2S(g)
– extrinsic, intrinsic-n-type and p-type – Hall effect – super conductors – magnetic properties of solids.
Module IV Thermodynamics (25 hrs)
The first Law – the basic concepts – System – surrounding – process – open, closed and isolated system – Isothermal, Isochoric and Isobaric process – work – Heat – Energy – Internal energy – The statement of first law – the conservation of energy – Expansion work – general expression of work – free expansion – Expansion against constant pressure – reversible expansion – Heat capacity at constant volume (Cv) and at constant pressure (Cp) – relation between Cp and Cv – Thermodynamic derivation – Enthalpy definition and measurement – Adiabatic change – work of adiabatic change.
Thermo chemistry – Standard enthalpy changes – Enthalpies of physical change – Enthalpy of vapourisation, enthalpy of transition and enthalpy of fusion – enthalpy chemical changes – Thermo chemical equation – Standard enthalpy of reaction, combustion and formation – Temperature dependence of reaction enthalpies Kirchoff’s law.
The First Law – State functions and exact differentials – state and path functions – exact and inexact different differentials – internal pressure – measurement of internal pressure – Joule experiment Changes in enthalpy at constant volume – isothermal compressibility – Joule – Thomson effect – inversion temperature. (15 hrs)
The Second Law – the concepts – Spontaneous and non-spontaneous process – statement of second law – Entropy – Thermodynamic definition – Entropy as a state function – Carnot cycle – the Thermodynamic scale of temperature – Entropy changes accompanying phase transitions – variation of entropy with temperature – the Helmholtz and Gibbs free energies – their significance – Maxwell’s relations – Criteria of spontaneity – Gibbs – Duhem equation – Clausius – Clapyeyron equation applicable to solid – liquid, solid-vapour and liquid-vapour equilibria.
Third Law of thermodynamics – The Nernst heat theorem – Absolute entropy – Calculation of absolute entropies of solids, liquids and gases. (10 hrs)
Module V Chemical Equilibrium (10 hrs)
Derivation of law of mass action from kinetic theory and thermodynamics – Experimental verification – Free energy change of chemical reactions – reaction isotherm – Van’t Hoff isochore – standard free energy of reaction and equilibrium constant – Predicting the influence of temperature, pressure, concentration changes and addition of an inert gas on the equilibria of the following reactions. 1. H2 (g) + I2 (g) → 2HI(g) 2. N2 (g) + 3H2 (g) → 2NH3 (g) 3. N2 (g) + O2 (g) → 2NO(g) 4. 2SO2 (g) + O2 (g) → 2SO3 (g) 5. PCl5 (g) → PCl3 (g) + Cl2 (g) 6. N2 O4 (g) → 2 N O2 (g)
Principle of mobile equilibrium – Le-Chatliers Principle and application to the above equilibria – Degree of dissociation and dissociation constant from density measurements – Mention homogeneous and heterogeneous equilibria.
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Module VI Chemical Kinetics (10 hrs)
The rates of chemical reactions – Experimental techniques – rate laws and rate constant – Order and molecularity of reactions – Methods of determining the rate of reaction – Integrated rate laws of first order, second order and third order reactions – Half life – kinetics of consecutive parallel and opposing reactions (first order only).
Temperature dependence of reaction rates – Arrhenius equation – derivation- Interpretation of parameters – Kinetics of unimolecular reactions – steady state approximation – Lindemann’s theory.
Theories of reaction rates – collision theory – Derivation of rate equation for second order reaction from collision theory – thermodynamic approach of transition state theory – Entropy activation.
Catalysis – Homogeneous and Heterogeneous catalysis – examples – Features of homogeneous catalysis – Enzymes – Michalis – menten mechanism.
Hetyerogenous catalysis – Langmuir – Hinshelwood mechanism – Kinetics of surface reactions – unimolecular and bimolecular.
Module VII Photo Chemistry (5 hrs)
Photochemistry – consequences of light absorption – The Jablonski diagrams – Radiative and non radiative transition – Light absorption by solutions – Lambert – Beer Law – Laws of photochemistry – The Grotthus – Draper law – Stark – Einstein law – Quantum efficiency – Quantum yield – Experimental determination of quantum yield – Photochemical rate law – Energy transfer in photochemical reactions – Photo sensitisation and quenching – Chemiluminescence – Lasers – uses.
REFERENCE BOOKS
1. Atkin’s Physical Chemistry : Peter Atkins, Julio de paula 7th Edition
2. Text book of Physical Chemistry : Samuel Glasstone
3. Physical Chemistry : GM Barrow
4. Physical Chemistry : Daniel and Alberty
5. Physical Chemistry : Puri, Sharma and Pathania
6. Physical Chemistry : WJ Moose
7. Physical Chemistry : G K Vamulapaki
8. Introduction to Chemical Thermodynamics : Rastogi and Misra
9. Chemical Kinetics : K.J.Laidler
10. Physical Chemistry : PC Rakshit
11. Physical Chemistry : Glasstone & Lewis
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5B08 CHE PHYSICAL METHODS IN CHEMISTRY
Contact hours-74 Credits-4
Module –1 Spectroscopy (30 Hours)
Electromagnetic Spectrum – Ranges of different radiation, General features of Spectroscopy. Microwave Spectroscopy – Rotation spectra, Moment of inertia, Rotational Quantum numbers, Rotational Constant, Intensities of rotational spectral lines, Rotational – Vibrational Spectrum of diatomic molecules – Selection rules for rotational spectra. Infrared Spectroscopy – Theory of infrared spectra, Sampling techniques, Selection rule, Molecular vibration – Stretching and Bending modes, Calculation of stretching frequencies – Fundamental Bands and Overtones, Factors influencing vibrational frequency – Electronic effects, hydrogen bonding, solvent effect etc. Applications of IR Spectroscopy – Interpretations of the spectra of alcohols, aldehydes, ketones and esters – aliphatic and aromatic. Raman Spectroscopy – Theory , Stokes and Anti-Stokes lines, Selection Rules. UV Spectroscopy - Absorption laws, Selection Rules – Types, Electronic transitions – Position and Intensity of absorption, Molar extinction coefficient, Chromophore – Auxochrome Concept, Absorption and Intensity Shifts, Types of Absorption Bands, Interpretations of spectra of simple conjugated dienes and enons, Woodward-Fieser Rule, Application to dienes and enons. NMR Spectroscopy - Introduction, Theory of NMR, Phenomena of resonance, Modes of nuclear spin-Relaxation Process, Chemical Shift – Internal standard, δ and τ scale, Shielding Effects, Factors affecting Chemical Shift, Spin-Spin Coupling, Interpretations of spectra of hydrocarbons, alcohols, aldehydes, ketones, aliphatic and aromatic compounds. Mass Spectrometry – Basic principles, Instrumentation, Fragmentation pathway, Molecular ion- base peak, Meta stable ion, General rules for predicting the prominent peaks, Mc-Lefferty Rearrangement, Mass spectra of alkanes, cyclo alkanes, saturates alcohols and aliphatic ketones.
Module -II Instrumental Methods (25 hours)
Polarography : Dropping Mercury Electrode, Polarization – Concentration polarization, Half wave Potential and Diffusion current (Significance), Illkovic equation, Advantages of polarographic analysis – Applications. Amperometry : Amperometric Titrations, Indicators, Instrumentation-Procedure, Biamperometric Titrations – Advantages and disadvantages, Applications. Chromatography : Types of Chromatography (brief study) – Adsorption and Partition Chromatography, Thin Layer Chromatography – Rf value, HPLC, Ion Exchange Chromatography – Applications.
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Thermal methods of Analysis : Thermogravimetric analysis (TGA), Derivative Thermogravimetry (DTG) and Differential Thermal analysis (DTA) – Instrumentation, Application and Characterization of polymers. Atomic Absorption Spectroscopy : Flame Atomization and Flame Structure – Hollow Cathode lamp, Interference. Atomic Emission Spectroscopy : Direct current plasma source – Analyte atomizatio and ionization – instrumentation (brief) – Applications. Inorganic applications : Spectrophotometry : Colorimetric Methods – Theory and Applications Magnetic Properties : Types of magnetism – paramagnetism, diamagnetism and ferromagnetism Curies law, Weiss’s law, Spin only Value, Magnetic Properties of the complexes on the basis of VBT. Electronic Spectra : Crystal Field Splitting in octahedral and tetrahedral complexes – d-d transition, Spectrochemical series, Explanation of the color of complexes. Module -III Concepts and Applications of Nano Science (8 hours)
Introduction - What is Nano Science and Nano technology – Quantum Size Effect – Single electron Tunneling, Preparation, Properties and applications. Nano technology in Bio-engineering. Module – IV Computational Chemistry (9 hours)
Introduction – Methods of calculation – molecular mechanics – Quantum mechanical methods – HF-DFT Method (Qualitative treatment only), Basic functions, Slaters type Orbitals, Gaussian type Orbitals, Z Matrix of H2O and ammonia.
REFERENCE BOOKS
1. Applications of Absorption Spectroscopy of Organic Compounds - Dyer
2. Introduction to Molecular Spectroscopy - Barrow
3. Spectroscopy of Organic Compounds – P.S.Kalsi
4. Organic Spectroscopy – William Kemp
5. Molecular Spectroscopy - Banwell
6. Polarography and Allied Techniques – V.Suryanarayana Rao
7. Instrumental Methods of Chemical Analysis – B.K.Sharma
8. Computational Chemistry - Grand
9. Instrumental Methods of Chemical Analysis – Skoog and West
10. Nano technology – Richard Brooker, EARL Boyson – Wiley Dream Tech India.
11. Nano technology (Malayalam) – Anwar Sadath – DC Books
Module 1 : Introduction to Organic Chemistry (5 Hours):
Difference between Organic and Inorganic compounds, Functional groups and homologous series, IUPAC nomenclature of alkanes, cyclo alkanes, alkens, alkynes, Halogen compounds, alcohols, ethers aldehydes, ketones, carboxylic acids, nitro compounds, nitriles amines and bifunctional compounds.
Module 2: Hydrocarbons (15 hrs)
Alkanes – preparation by reduction of alkyl halides – Wurtz reaction and Kolbe’s electrolytic methods with mechanism - Chlorination of methane with mechanism. Alkenes – preparation by dehydration of alcohols, dehydrohalogenation of alkylhalides, dehalogenation of vicdihalides and by Kolbe’s electrolytic method. Reaction – Hydrogenation, addition of halogens, halogen acid and water. Oxidation with KMnO4, K2Cr2O7 and osmium tetroxide, Ozonolysis and polymerization.
Alkynes – Preparation by dehydrohalogenation of vicdihalides and gem dihalides, dehalogenation of tetrahalides and Kolbe’s electrolytic method. Reactions, addition of Hydrogen, Halogen, Halogen acid and water – oxidation using alkaline KMnO4, Acidic K2Cr2O7 and Selenium dioxide. Ozonolysis and Polymerization reactions, Specific to 1-alkyne.
Dienes – Conjugated, cumulated and isolated dienes with example, preparation of 1, 3 butadiene. By dehydration of diols, reaction of 1, 3 butadiene – Diels-Alder reaction, polymerization.
Poly nuclear Hydro carbons Synthesis of naphthalene by Haworth synthesis of Anthracene from benzyl chloride.
Cyclo Alkane – preparation by Freunds and Wislicenus. Module 3: Reaction intermediates and electron displacement effects (9 hrs)
Homolytic and Heterolytic Bond Fission – Substrate and Reagent – Electrophiles and Nucleophiles – Reaction intermediates – carbocation, carbonion, Free radicals and Carbenes – Their generation, structure and stability – Electron displacement effects – Inductive effect, Electrometric effect, Mesomeric effect, Hyper conjugation effect and Sterric effect – Their application.
Module 4 : Mechanism of Organic reactions (10 Hours) :
Nucleophilic Substitution in alkyl halides – SN1 and SN2 mechanism – Effect of structure on SN1 and SN2 as illustrated by Primary, Secondary and Tertiary alkyl halides and Benzyl halides – Stereo Chemistry of SN1 and SN2 reaction – Mechanism of Electrophilic addition of Hydrogen halides to Carbon – Carbon double bond. Markownikoff’s rule – Peroxide effect (Free radical addition of HBr on unsymmetrical double bond. Elimination – E1 and E2 mechanism –
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mechanism of dehydration of alcohol and dehydrohalogenation of alkyl halides – Saytzef’s rule and Hofmann’s rule.
Module 5 (10 hrs)
Aromaticity : Huckel’s rule and molecular orbital theory of aromaticity – mention of structures of the following non-benzenoid aromatic compound – cyclopentadienyl anion, Ferrocene and tropylium, cation – Antiaromaticity, mechanism of the following aromatic electrophilic Substitution. Halogenation, Nitration, Sulphonation, Friedal Craft’s alkylation and acylation – Aromatic nucleophilic substitution – SN Ar and Benzyne Mechanism.
Module 6 : Halogen Compound (8 hrs)
Alkyle halides – preparation form alcohol – Reaction of alkyl halides with metal Dihalides – Gem dihalides and Vic dihalides – General methods of preparation – General reaction – Trihalogen derivative of methane – Chloroform – preparation from ethanol and acetone – Haloform reaction.
Module 7 : Stereo Chemistry (15 hrs)
Classification of Stereo isomers – Geometrical isomers – Cis-trans, E-Z designation – characterization of geometrical isomers – conformation of ethane, n-butane and Cyclohexane Configuration – Wedge formula and Fischer projection formula – Newmann projection formula. Optical isomerism plane polarized light – chirality and elements of symmetry. DL designation and RS designation, Enantiomers, mesoform, erythro and threo forms and diastereoisomers.
Reference
1.Organic Chemistry : I.L. Final Volume 1 and II 2.Organic Chemistry : Pine 3.Advanced Organic Chemistry : Bhal and Bhal 4.A Text Book of Organic Chemistry : Tewari, Mehrothra, Vishnoi 5.Advanced Organic Chemistry : Jerry March 6.A Guide to mechanism in Organic Chemistry : Peter Sykes 7.Organic reaction mechanism : Raj K Bewsal
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Contact hours-90
Credits-4
6B13CHE PHYSICAL CHEMISTRY II
Module I Symmetry and Molecular Structure (6 hrs)
Elements of symmetry of molecules – Centre of symmetry, plane of symmetry, proper and improper axis of symmetry – Operations with examples – Point groups – Properties of a group – simple point groups Cnv, Cnh.
Module II Dilute Solutions (10 hrs)
Colligative properties – Lowering of vapour pressure and Raoult’s law – Calculation of molar mass. Elevation of boiling point – relation to lowering of vapour pressure – Thermodynamic derivation – Calculation of molar mass – Measurement by Beckmann’s and Landsberger’s methods – Depression of freezing point – Thermodynamic derivation – Calculation of molar mass – Measurement by Beckmann’s method – Osmotic pressure – Measurement by Berkely and Hartley’s method – Laws of Osmotic pressure – Van’t Hoff equation – Calculation of molar mass – Abnormal molar mass – Van’t Hoff factor – Degree of dissociation and association and their calculation from colligative properties.
Module III Phase Rule (15 hrs)
Statement – Explanation of terms involved – Thermodynamic derivation of phase rule – Application to water system and sulphur system – Solid – liquid equilibria involving simple eutectic system – Ag-Pb system – De silverisation of lead – Freezing mixtures – Solid – liquid equilibria involving compound formation with congruent and incongruent melting points – Solid – gas system – Dehydration of CuSO4.5 H2O-Deliquescence and efflorescence – Gas Liquid system – Absorption coefficient – Henry’s Law – Liquid systems – Completely miscible – Ideal and non- ideal solutions – Application of Raoult’s Law – Vapour pressure – composition from Raoult’s Law Azeotropic mixtures – Partially miscible liquids – Critical solution temperature – Temperature – composition curves – Fractional distillation – Derivation from Raoult’s Law – Immiscible liquids – Steam distillation – Molar mass from steam distillation – Nernst distribution Law – Derivation from phase rule and thermodynamics – Limitations of the law – Application of the law to study association and dissociation – Solvent extraction – Hydrolysis of salts – The equilibrium of KI + I2
→ KI3 Module IV Colloids, Surface Chemistry (10 hrs)
Colloids, Classification – preparation – structure and stability – The electrical double layer – Zeta potential – Properties of Colloids – Tyndall effect – Brownian movement – Coagulation of colloidal solution – Hardy – Shulz rule – Flocculation value – Electro kinetic properties – Electrophoresis – Electro-osmosis – Protective colloids – Gold number – Emulsion – Oil in water emulsion and water in oil emulsion – Emulsifying agents – Gels – Inbibition – Synerisis – Micelles – Critical micelle concentration – surface films – Physisorption and Chemisor Adsorption
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isotherms – Freundlich adsorption isotherm – effect of temperature on adsorption – Langmuir adsorption isotherm – derivation – use and limitation.
Module V Electrical Conductance (15 hrs)
Ohm’s Law – Electrical energy – volt – coulomb – Mechanism of electrical conduction – Arrhenius theory – The laws of electrolysis – Faraday’s law and its significance – Transference Number – Determination by Hittorf’s method and moving boundary method.
Equivalent conductance and Molar conductance Effect of Dilution on conductance – Effect of dielectric constants of solvents – Ionic mobilities – Kohlrausch’s Law – applications – Mobilities of Hydrogen and Hydroxyl ions – Diffusion and ionic mobility.
Activity and activity coefficient – standard state ionic activities and activity coefficient – ionic strength – Debye – Huckel Theory – Ionic atmosphere – Debye – Huckel limiting law – determination of solubilities by conductance measurements – conductometric titrations – conductance in non-aqueous solvents – Temperature dependence of ionic conductance.
Module VI Ionic Equilibria (14 hrs)
Acids and bases – Lowrry – Bronsted concept – Dissociation of acids and bases – Lewis concept of acids and bases – hard and soft acids and bases and its applications – Ionic product of water – Dissociation constants of acids and bases – pH and its determination – Heat of neutralization – Incomplete neutralization – Hydrolysis of different types of salts – Degree of hydrolysis and hydrolytic constant – and its relation with pH and pOH – Buffer solution – pH of Buffer solution – Henderson’s equation – Buffer capacity – Application of buffer – Acid – base indicators – Determination of pH of indicators.
Module VII Electromotive Force (20 hrs)
Electrochemical cell-Daniell cell – Reversible and Irreversible cell – Single electrode potential – EMF of cells – Standard potential and standard emf – Standard Hydrogen electrode and calomel electrode – Types of electrodes – electrode reaction – cell reaction Nernst equation for electrode potential and emf of the cell – Electrochemical series – IUPAC sign convention – Application of Gibb’s Helmholtz equation to galvanic cells – Calculation of ∆G, ∆H, ∆S and equilibrium constant from emf data – The standard cells – Weston Cadmium cell and its emf.
Concentration cells – Electrode and electrolytic concentration cells with and without transference and their emfs – Liquid junction potential – Elimination of liquid junction potential – salt bridge – application of potential measurements – Determination of solubility product, ionic product of water, transport number and the pH value – Hydrogen, Quinhydrone electrode and glass electrode – potentiometric titration – redox indicators – Polarisation – Over voltage – principle and applications of polorography – Fuel cells.
REFERENCE BOOKS
1. Text Book of Physical Chemistry : Glasstone 2. Atkin’s Physical Chemistry : Peter Atkins Julio de Paula VII Edn.
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3. Modern Electro Chemistry : JOM Bockris & AKN Reddy
4.
Physical Chemistry :
Puri Sharma and Pathania
5. Physical Chemistry : P.C.Rakshit 6. Physical Chemistry : Walter J Moore 7. Vogel’s Text Book of Qualitative Inorganic Analysis : AI Vogel 8. Physical Chemistry : Gillbert Casillane 9. Physical Chemistry : GK Vemulapalli 10. Physical Chemistry : Gurdeepraj 11. Prgathi’s Instrumental Methods of analysis : H Kaur 12. Group Theory in Chemistry : V.Ramakrishnan
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6B14 CHE Organic Chemistry-II
Contact hrs-72
Credits-4 Module-I, Hydroxy Compounds (7 Hours)
Alcohols – Preparation of monohydric alcohols from carbonyl compounds using Grignard reagents – Methods to distinguish 1o, 2o and 3o alcohols – Lucas method, Victor Meyer’s method and oxidation method – Ascent and descent in alcohol series.
Glycerol – Manufacture from fats and oils – Synthesis from propylene – Properties and uses .
Phenols – Preparation of phenol from cumene – Acidic character of phenol – Preparation of
cresols, nitrophenols, picric acid, dihydric phenols and naphthols – Phenolic ethers – Preparation of anisole and phenetole.
Mechanism of the following rearrangements – Pinacol – Pinacolone, Fries and Claisen rearrangements.
Module – II, Carbonyl Compounds (11 Hours)
Preparation of aldehydes and ketones – Rosenmund’s reduction, Stephen’s reduction, Etard’s reaction, Oppeanauer oxidation, Houben – Hoesh synthesis. Reactions of aldehydes and ketones. Reduction using LiA1H4 and NaBH4 MPV, Clemensen and Wolf-Kishner reduction. Reduction to pinacols – Oxidation using mild and strong oxidizing agents – SeO2 oxidation – Reaction with alcohols, KCN, sodium bisulphate and derivatives of ammonia – Distinction between acetaldehyde and benzaldehyde and acetaldehyde and acetone.
Mechanism of the following reactions – Aldol condensation , Cannizzaro’s reaction, Crossed Cannizzaro’s reaction, Reimer – Tiemann reaction, Perkin’s reaction, Benzoin condensation and Backmann rearrangement. Reaction of formal- dehyde with aldehydes containing alpha hydrogen atoms.
Preparation of acrolein, crotonaldehyde and vanillin. Quinones – Preparation and important reactions of p-benzoquinone, 1, 4 – Naphthaquinone
and 9, 10 – Anthraquione. Module – III, Carboxylic Acids, Sulphonic acids and Amino acids (14 Hours)
Carboxylic acids – Ascent and descent in aliphatic acid series, Preparation and reactions of acrylic and crotonic acids.
Hydroxy acids – Effect of heat on alpha, beta, gamma and delta hydroxyl acids – Preparation and reactions of lactic acid, tartaric acid and citric acid.
30
Dicarboxylic acids – Preparation and reactions of oxalic, malonic, succinic, maleic and fumeric acids – Blanc’s rule.
Aromatic acids – Preparation and reactions of Benzoic acids, anthranilic acid, salicylic acid, cinnamic acid and phthalic acid.
Aromatic sulphonic acids – Preparation and reactions of benzenze sulphonic acid, toluene sulphonic acids, benzenze sulphonyl chloride, ortho and para toluene sulphonyl chlorides – Preparation and uses of sccharin and chloramines-T. Preparation and properties of sulphanilic acid and sulphanilamide – Sulpha drugs – examples and uses.
Amino acids, Protiens and Nucleic acids – Classification of amino acids – Structure of glycine, alanine, phenyl alanine, tryptophan, cystine and glutamic acid (structural elucidation not expected) – Synthesis of amino acids – Gabriel, Strecker and Erlenmeyer synthesis – Zwitter ion property – Isoelectric point – Sorensen formal titration.
Module – IV, Synthetic Reagents (5 Hours)
Active methylene group – Preparation and synthetic applications of Ethyl acetoacetate, Diethyl malonate and ethil cyanoacetate. Mechanism of Claisen condensation. Preparation and synthetic uses of Grignard reagent and Frankland reagent – Mechanism of Reformatsky reaction.
Module – V, Nitrogen Compounds (12 Hours)
Cyanides and Isocyanides – Distinction between cyanides and isocyanides. Nitroalkanes – General methods of preparation and reactions of primary, secondary and tertiary nitroalkanes. Distinction between primary, secondary and tertiary nitroalkanes. Aromatic nitrocompounds – Reduction of nitrobenzene under different conditions – Preparation of dinitrobenzene, 1, 3, 5 – trinitrobenzene, nitrotoluenes and 2, 4, 6 – trinitrotoluene – Mechanism of Benzidine rearrangement.
Amines – Separation of primary, secondary and tertiary amines – Hinsberg and Hoffmann method to distinguish primary, secondary and tertiary amines. Preparation of quaternary ammonium salts.
Aromatic amines – Preparation and reactions of aniline, toluidines, phenylene diamines, diphenyl amine, N-Methyl aniline, N, N-dimethyl aniline and naphthyl amines. Distinction between benzyl amine and toluidine.
Diazonium salts – Preparation, synthetic applications and structure of benzene diazonium chloride, Diazomethane and diazoacetic ester-Ardnt-Eistert synthesis – Wolf rearrangement – mechanism.
Preparation, Properties and structure of urea, Preparation and reactions of semicarbazide and thiourea – Preparation of Urethane.
Module – VI, Heterocyclic Compounds (6 Hours)
Nomenclature of 5 and 6 – membered heterocyclic compounds – Preparation, structure and properties of Pyrrole, Pyridine, Indole, quinoline Isoquinoline, Pyrimidine and Purine – Relative
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basic character of Pyrrole, Pyridine and Piperidine – Hoffmann’s exhaustive methylation of piperidine and coniine.
Module – VII, Carbohydrates (10 Hours)
Classification and nomenclature of carbohydrates – Configurations of aldotrioses, teroses, pentoses and hexoses – Structure and configuration of glucose fructose-cyclic structure – Haworth projection formula – anomers – mutarotation – reactions of glucose and fructose - ascent and descent in aldoses – Interconversion of aldoses and ketoses – Epimer and Epimerisation – Conversion of an aldose into it’s epimer – Disaccharides – Configurational open chain ring structure of sucrose, maltose and lactose (structure elucidation not expected) – Elementary study of starch and cellulose – Industrial uses of cellulose.
Module – VIII, Dyes (3 Hours)
Classification of dyes bases on structure and application – Synthesis and use of Parared, Malachite green, Fluorescein, Eosin, Crystal violet, Fuschine, Indigo and Alizarin (Structure elucidation not expected) – Relation between colour and constitution.
Module – IX, Polymer Chemistry (4 Hours)
Classification – Natural and synthetic polymers – Thermoplastics and thermosetting plastics – Elastomers – Fibres – Liquid resins – Types of polymerization – Chain and step polymerization – Homopolymers and Co-polymers – Synthesis and application of Polythylene, Polypropylene, PVC, Polystyrene, Polyurethanes, Phenolic and Epoxy resins – Synthetic rubber – Buna-S, Buna-Neoprene, and Butyl rubber-Biodegradability.
Reference
Organic Chemistry : I.L.Finar Volume I and II
Organic Chemistry : Pine
Advanced Organic Chemistry : Fieser and Fieser
Advanced Organic Chemistry : Bhal and Bhal
A Text Book of Organic Chemistry : Tewari, Mehrothra, Vishnoi
Advanced Organic Chemistry : Jerry March.
32
SYLLABUS OF B.Sc CHEMISTRY PRACTICAL General Instructions
1. For weighing, both electronic balance and chemical balance may be used. (However,
electronic balance is preferred). 2. Organic reactions may be carried out in tiles, wherever possible. 3. Reagents should be kept in small bottles with dropper. 4. Semi-micro method may be adopted for qualitative analysis. 5. Practical examination will be conducted in even semesters (ie. 2nd, 4th and 6th Semesters).
(i) Relation of acid-base titrations with real life situations like estimation of citric acid in lemon, orange etc.
(ii) Equivalent and molecular mass of compounds. Normality and Molarity – Primary standards. Preparation of standard solution – Principles of volumetric analysis.
(iii) For acidimetry, alkalimetry and permanganometry two burette method may be used and for other volumetric analyses conventional methods can be used.
1. ACIDIMETRY AND ALKALIMETRY
a. Estimation of NaOH using standard Na2 CO3 (two burette method). b. Estimation of HCl using standard oxalic acid (two burette method). c. Estimation of bicarbonate and carbonate in a mixture.
2. PERMANGANOMETRY
a. Estimation of oxalic acid – using standard Mohr’s salt (Two burette method). b. Estimation of Fe2+ using standard oxalic acid (two burette method). c. Estimation of Ca2+
d. Estimation of nitrite. e. Estimation of percentage of Mn in pyrolusite. f. Estimation of hydrogen peroxide.
3. DICHROMETRY a. Estimation of Fe2+ - External indicator. b. Estimation of Fe3+ - Reduction of SnCl2-Internal indicator. c. Estimation of Fe2+ using internal indicator.
4. IODOMETRY AND IODIMETRY a. Estimation of Cu2+/CuSO4.5H2O b. Estimation of Potassium dichromate/Cr3+
c. Estimation of As2O3/As3+
5. PRECIPITATION TITRATION – using adsorption indicators a. Estimation of chloride in neutral medium.
PREPARATION (PART I & PART II) (i) Systematic qualitative analysis of a mixture containing two cations and two anions by semi-micro method
Study of the reactions of the following ions with a view to their identification and confirmation – Lead, Silver, Mercurous mercury, Mercuric mercury, Bismuth, Copper, Tin, Antimony, Iron, Aluminium, Chromium, Zinc, Manganese, Cobalt, Nickel, Barium, Strontium, Calcium, Magnesium, and Ammonium.
Note : Minimum ten mixtures should be analyzed and recorded.
(ii) Preparations : Any three of the following inorganic preparations. (1) Ferrous ammonium sulphate. (2) Tetraammine copper (II) sulphate. (3) Potassium trisoxalato chromate. (4) Potash alum KAl (SO4)2. 12H2O (5) Hexaammine cobalt (III) chloride.
34
Contact Hours-360
Credit-10
CORE COURSE PRACTICAL
5B10 CHE, 5B11 CHE, 6B10 CHE, 6B11 CHE, 6B16 CHE SEMESTER V & VI PRACTICALS : GRAVIMETRIC ANALYSIS
Introduction to gravimetric techniques and its highlights. 1. Determination of water of hydration in crystalline barium sulphate. 2. Determination of Ba2+ as BaSO4
3. Determination of sulphate as BaSO4
4. Determination of Fe2+) as Fe2O3
5. Determination of Ca2+ as CaCO3
6. Estimation of Ni2+ as Nickel dimethylglyxomite. 7. Determination of Cu2+ as cuprous thiocyanate. 8. Determination of Mg2+ as magnesium oxinate.
SEMESTER V & VI PRACTICALS : ORGANIC CHEMISTRY
1. Synthesis of Organic Compounds. a. Aromatic electrophilic substitution:
Nitration – Preparation of nitrobenzene and p-nitroacetanilide Halogenation – Preparation of p-bromoacetanilide, preparation of 2, 4, 6 – tribromophenol
b. Diazotization and coupling : Preparation of phenyl azo β-naphthol and methyl orange.
c. Oxidation : Preparation of benzoic acid from benzyl chloride or benzaldehyde . d. Esterification : Benzoylation of phenol to phenyl benzoate. e. Hydrolysis : Benzamide or ethylbenzoate to benzoic acid.
2. Organic Qualitative Analysis
a. Qualitative analyses with a view to characterize functional group/groups in the following compounds: Napthalene, anthracene, chlorobenzene, bromobenzene, benzyl chloride, p- dichlorobenzene, benzyil alcohol, phenol, cresols, naphthols, resorcinol, benzaldehyde, acetophenone, benzophenone, benzoic acid, phthalic acid, cinnamic acid, succinic acid, salicylic acid, ethyl benzoate, methyl salicylate, benzamide, urea, aniline, toludines, dimethyl aniline, nitrobenzene, o-nitrotoluene, glucose, sucrose.
b. Preparation of derivatives.
35
c. Separation of two component mixtures : Aniline + Naphthalene. Note : Minimum ten compounds should be analyzed and recorded. For analysis, reactions may be carried out in tiles, wherever possible.
3. Thin layer Chromatography and Column Chromatography
a. Preparation of the TLC plates – Checking the purity of the compounds by TLC – Acetylation of salicylic acid, aniline, Benzoylation of aniline and phenol, Determination of Rf. Values and identification of organic compounds by TLC, preparation and separation of 2, 4 –dinitrophenyl hydrazones of acetone and 2- butanone using toluene and light petroleum (40 :60).
b. Separation of ortho and para nitroaniline mixture by column chromatography. 4. Demonstration Experiments
Steam distillation : Separation of ortho and para nitro phenols. 5. Structure elucidation of simple organic compounds from spectra (UV, NMR, IR and
a. Determination of specific reaction rate of the hydrolysis of methyl acetate catalysed by hydrogen ion at room temperature.
b. Determination of overall order of saponification of ethyl acetate. 2. Distribution law
a. Determination of distribution coefficient of iodine between water and carbontetrachloride.
3. Electrochemistry
a. Determination of concentration of HCl conductometrically using standard NaOH solution.
b. Determination of concentration of acetic acid conductometrically using standard NaOH solution.
4. pH metry
a. Preparation of alkaline buffer solutions. b. pH metric titration of weak acid (acetic acid) with strong base
NaOH and calculation of dissociation constant. 5. Colorimetry
a. Verificatin of Beer-Labert law for KMnO4, K2CR2O7 and determination of the concentration of the given solution.
36
6. Adsorption a. Adsorption of acetic acid, oxalic acid on animal charcoal, verification of Freundlich
isotherm. 7. Phase rule
a. CST of phenol – water system. b. Transition temperature of salt hydrates.
8. Molecular weight determination
a. Determination of molecular weight by Rast’s method – determination of identity of two compounds by mixed melting points.
VIVA VOCE
Viva voce examination based on practical will be conducted on 2nd day along with the practical examination.
STUDY TOUR
Students are required to visit at least one Laboratory/factory/Research Institute of eminence during the course and present the Study Tour Report separately along with Practical Records at the time of Practical Exam (6th Semester). A bonafide Certificate for the visit should be attached with the report.
PROJECT REPORT: Students should undertake a group project work related to chemistry and submit the report along with practical records during VI semester pracicals. ( Guide lines given in Annexure I) REFERENCES 1. A.I.Vogel - A Text Book of Qualitative Analysis including semi-micro methods
5. A.O.Thomas – Practical Chemistry for B.Sc Chemistry.
6. A Findlay – Practical Physical Chemistry.
7. R.C.Das & E Behara – Experimental Physical Chemistry.
8. N.K.Vishnoi – Advanced Practical Chemistry.
37
MODEL QUESTION PAPERS FOR PRACTICALS
B.Sc CHEMISTRY PRACTICAL EXAMINATION
CORE COURSE PRACTICAL (1B2 CHE & 2B2 CHE)
SEMESTER II PRACTICAL COURSE : VOLUMETRIC ESTIMATION
Time : 4 Hours
Credit : 4 Instruction : Candidate should submit bonafide record at the time of examination
1. Write down the principle with equations for the estimation of …………………...given
……………… 2. Calculate the weight of ……………. Required for the preparation of
………….N,……………mL solution. 3. Estimate the amount of ………….. in the whole of the given solution provided with
………….solution and ………….crystals. 4. Viva Voce
38
B.Sc CHEMISTRY PRACTICAL EXAMINATION
CORE COURSE PRACTICAL (3B5 CHE & 4B5 CHE)
SEMESTER IV PRACTICAL PAPER II : INORGANIC QUALITATIVE ANALYSIS
AND PREPARATION
Time : 4 Hours
Credit: 2 Instruction : Candidate should submit bonafide record at the time of examination
1. Write briefly the principle of addition of HCl in the group II analysis/Role of addition of
NH4Cl in the group III analysis/Role of preparation of sodium carbonate extract in the
analysis of anions. 2. Write the principle and procedure used in the preparation of …………..
3. Analyse systematically the given mixture containing the anions and cations by semi-micro
method. 4. Exhibit at least 3 samples of the prepared inorganic compounds.
5. Viva Voce.
39
B.Sc CHEMISTRY PRACTICAL EXAMINATION CORE
COURSE PRACTICAL (5B10 CHE & 6B10 CHE)
SEMESTER VI PRACTICAL COURSE : GRAVIMETRIC ANALYSIS
Time : 3 Hours
Credit: 3 Instruction : Candidate should submit bonafide record at the time of examination
1. Write down the principle and procedure for the estimation of ……….. in the given
………….solution. 2. Estimate the amount of ………… in the whole of the given ……….. solution.
3. Viva Voce.
40
B.Sc CHEMISTRY PRACTICAL EXAMINATION
CORE COURSE PRACTICAL (5B11 CHE & 6B11 CHE)
SEMESTER VI PRACTICAL COURSE : ORGANIC CHEMISTRY Time : 3 Hours
Credit : 3 Instruction : Candidate should submit bonafide record at the time of examination.
1. Write down the principle for the estimation of ……………..from…………..
2. Analyse the given organic compound with a view to identify the nature of the functional
group. Suggest a suitable solid derivative. 3. Analyse the given spectra and arrive at the correct structure of the compound.
4. Convert the given………….. into……………….. Recrystallize and exhibit both crude and
recrystallized samples. 5. Viva Voce.
41
B.Sc CHEMISTRY PRACTICAL EXAMINATION
CORE COURSE PRACTICAL (6B16 CHE)
SEMESTER VI PRACTICAL COURSE : PHYSICAL CHEMISTRY
Time : 4 Hours
Credit : 4 Instruction : Candidate should submit bonafide record at the time of examination.
1. (a) Write down the principle adopted in the determination of
concentration of HCl conductometrically. (b) Principle involved in the determination of concentration
K2Cr2O7 by calorimetry.
of KMnO4 or
2. Determine the molecular mass of the given compound by Rast’s method.
3. Submit the Project Report & Report of Industrial visit
4. Viva Voce
Sd/- Dr.K.Pradeep Kumar,
Chairman,Board of Studies in Chemistry (UG)
1
42
ELECTIVE
6B15CHE – A. ENVIRONMENTAL CHEMISTRY
Credits :4 Total Contact Hrs : 72
OBJECTIVES:
1. To create awareness about the environmental issues 2. To the make students capable of analyzing the environmental problems and help the public
to take the correct stand 3. To impart knowledge about modern techniques for analyzing environmental pollutants.
Module I. Environmental segments – Atmosphere – Composition and structure – Earth’s radiation balance – Air pollution – Air pollutants – Sources, effects, and sink of CO, NOx, SO2, H2S, Hydrocarbons, particulate matter and acid rain.
Green house effect and global warming – climate change – ozone chemistry and ozone hole- photochemical smog (reactions) – El Nino phenomenon
Sampling – monitoring of air pollutants – Analysis of CO, NOx, SO2, H2S, Hydrocarbons and particulates. Control of air pollution – control by devices – Stacks, filters, electrostatic precipitators, cyclone separators, scrubbers and catalytic converters. (12 Hrs)
MODULE II : Water resourses, - Hydrolytic cycle- water pollution – sources – Industrial effluents – agriculture discharge – oil spills – heavy metals – pesticides – detergents
Eutrophication – biomagnifications and bioaccumulation – experimental determination of Dissolved oxygen, BOD and COD – Thermal Pollution – Control of water pollution – ISI/BSI standards of drinking water
Hardness of water – causes and effects – methods of estimation – removal of hardness
Module III : Lithosphere – soil formation – components of soils – Acid base and ion exchange reactions in soil – soil pollution – soil acidification – effects on plants – liming of soil – Industrial and urban wastes – plastics, Nitrates, pesticides and heavy metals in soil – garbage – biomedical waste – E waste –Municipal Solid waste management (10 Hrs)
Module IV : Noise pollution and Radioactive Pollution : Human acoustics - Noise – general features -types of Noise – Measurement of noise – sound pressure and power levels – sources and effects of noise pollution – prevention of hearing loss in industry – control of noise pollution.
Radiation chemistry – Man made and natural radiations – biological effects of radiation – radiation hazards from reactors – radioactive waste management. (10 Hrs)
43
Module V : Chemical Toxicology – Toxic chemicals in environment – Sources, effects and treatment of heavy metal poisoning – Pb, As, Cd, Hg, Cr, Cu, Zn & Co (8 Hrs)
Module VI : Pesticides – Classification – Chemistry of chlorinated organic compounds – Polychlorinated biphenyles – pesticides interfering with respiration – Lindane – polychlorinated cyclopentadiene derivatives – Auxins herbicides – long term effects of organochlorocompounds – organophospherous pesticides – Carbamates – Use of Pheramones and hormones – insect sterilization – color coding of pesticides – Handling of pesticides.
(10 Hrs)
Module VII : Instrumental techniques in Environmental analysis – Neutron activation analysis – Atomic absorption spectroscopy – X - ray fluorescence – Chemiluminescence – ion selective electrodes – Gas chromatography – HPLC – ion chromatography. (10 Hrs)
References:-
1. Environmental Chemistry, A.K.De.
2. Environmental Chemistry, P.S. Sindhu
3. Essentials of environmental studies, S.P. Misra & S.N.Pandey
4. Advanced Inorganic Chemistry Vil. II , Gurdeep Raj
5. Engineering Chemistry , Dr. B.K. Sharma
6. Engineering Chemistry, Jain & Jain
7. A Basic course in environmental studies, Surinder Deswal & Anupama Deswal.
44
ELECTIVE
6B15 CHE – B. FOOD CHEMISTRY
Credits : 4 contact hours : 72
OBJECTIVES:
1. To study about the chemical constituents in food and their role in production of energy and body building
2. To study about the chemical changes occurring during the decay of food and thereby reducing such problems
3. To provide a brief idea about the use of food additives and their harmful effects 4. To familiarize the students with the important biochemical reactions occurring in human
body.
Module I - BASIC CONCEPTS
Introduction-definition of food-terminology used in food chemistry-pH of foods- biosynthetic reactions: catalytic reactions, phosphates in biosynthesis, oxidation, condensation, acylation and rearrangement reactions
Photosynthesis: chemical reaction and mechanism 8 Hrs
Module II - WATER
Physical properties- structure of water and ice – water activity –water activity and reaction rate – water activity and food spoilage – sorption phenomena – water activity and food packaging –types of packaging and chemistry of food packaging 7 Hrs
Module III - LIPIDS
Structure and classification – Lipid oxidation: autoxidation and metal catalyzed oxidation – Rancidity in fats and oils – Measurement of lipid oxidation- predictive tests- hydrogenation of lipids-emulsions and emulsifiers – anti oxidents - Natural and synthetic. 8 Hrs
Module IV - CARBOHYDRATES
Classification and structure- mono , di and polysaccharides –important examples and uses- Lactose intolerance-source, structure and common uses of starch- structure, gelling and application s of Alginate, pectin carrageenans - Dextrans , chitin , inulin
45
and agar – nutritional role of carbohydrates – effect of sugar on health – carbohydrate metabolism
8 Hrs
Module V - PROTEINS:
Amino acids – classification- peptides and proteins- biomedical importance of peptides- functions and properties of peptides- denaturation and oxidation- classification of proteins- structure of proteins- food proteins- Browing reactions – enzymatic and non enzymatic- control 7Hrs
Module VI - ENZYMES:
General characteristics - specificity – sources - nomenclature and classification – mechanism of enzyme catalysis – factors affecting the rate of enzymatic reactions – molecular basis of enzyme action – enzyme kinetics – enzyme technology and applications
8 Hrs
Module VII - FOOD ADDITIVES:
Functions - Categories : Acidulates, preservatives, bacteriocins, emulsifying agents, textring agents, antioxidants, humectants and sequestering agents. Harmful effects of food additives – Safety concerns and legal regulations 7 Hrs
Module VIII - FOOD PIGMENTS , FLAVOURS AND SWEETENERS
Flavors – sensation of smell and taste - odor – important food flavors – fruit and vegetable flavors – spice flavors – beverage flavors – meat flavors. Off flavor in food due to chemical change and environmental contamination.
Sweeteners – classification – molecular theory of sweeteners – carbohydrate sweeteners – Artificial sweeteners: cyclamate. D-amino acids, saccharin, acesulfame-K, aspartame ,neotame and dulcin – Naturally occurring non carbonate sweeteners:
Classifications – sources, biochemical functions and deficiency symptoms of vitamin A B1,B2,B12 C,D ,E and K. 7 Hrs
References:
1. Food chemistry – H K Chopra and P S Panesar – Narosa Publishing House 2. The Chemistry of life – Harris L J – Cambridge University Press, New York 3. Organic Chemistry – Vol I and II , I L.Finar 4.
47
6B15CHE- C. INDUSTRIAL CHEMISTRY (Elective)
Credits 4 Contact Hours 72
OBJECTIVES:
1. To familiarize the students with the general and basic activities in industrial operations. 2. To study about the important raw materials used in industries. 3. To make the students capable of dealing with the environmental problems related to
industries. 4. To provide the basics about industrial management.
Module 1 Industrial aspects of Organic Chemistry ,Inorganic Chemistry and Physical chemistry
Raw materials for organic compounds-Petroleum-Natural gas-Fractionation of crude oil
Cracking-Coal-Types- Distillation of coal-Renewable natural resources-Cellulose-Starch-Properties and uses
Basic metallurgical operations-Inorganic materials of industrial importance-Alumina,Silica,Silicates,Clays,Mica,Zeolites(Structure and uses)
Catalyses: Introduction-Types-Homogenous and Heterogeneous-Basic Principles-Factors affecting the performance-Phase transfer catalysis
Emulsions-Micro emulsions-micelles-Aerosols-Effects of Surfactants 14 Hours
Module 2 Unit Operations in Chemical Industry
Distillation: Introduction-Batch and Continuous distillation-Separation of Azeotropes – Plate column and Packed column
Evaporation: Introduction- Equipments : Short tube(Standard) evaporators-Forced Circulation evaporators-Falling film evaporators-Climbing film evaporators-Wiped film evaporator
Filtration: Introduction-Filter media and filter aids-Equipments: Plate and frame filter press-Nitch filter –Bag filtrer-rotary drum filter-Sparkler filter- Candle filter- Centrifuge.
Mechanical properties of materials and change with respect tom temperature:
Meterials of constructions used in industry: Metals and alloys: Iron, Copper, Aluminium, lead, Nickel ,Titanium and their alloys-Preparation and uses
Cement: Composition-Manufacture-Application
Refractories: Classification-Application
Polymeric materials: Industrial polymer and composite materials-constitution-Chemical properties-Physical properties-Industrial application
Glass: Type-composition-Manufacture-Physical and chemical properties-Application
Corrosion: Various type of corrosion relevant to chemical industry-Preventive methods
15Hours
Module 4 Effluent treatment and waste management :
Principles and equipments for aerobic ,anaerobic treatment-adsorption -Filtration-Sedimentation-Bag filters-Electrostatic precipitator-Mist eliminator-Wet scrubbers-Solid waste management-
Industrial safety: Introduction-Definition and terms used-Accidents: Non reportable accidents-Hazard-Risk acceptance-Physical factors for accidents-Accidents ratio-Safety training-Role of supervisor in achieving high standard of safety –Supervisory training-Motivation for safety-Safety suggestion scheme –Safety committee-Safety competition-Safety contests-Safety drives-Safety exhibition and poster
15 Hours
Module 5 Industrial Organization
Concept of Scientific management in industry-Functions of management in industry-Decision making-Planning –Organizing-Directing and Control-Location of industry-Material management-Management of human resources-Selection-Incentives-Welfare-Safety 8 Hours
Books
1 Introduction to petroleum chemicals H.Steiner Pergamn Press
2 Chemistry of cellulose Heuser.E
3 Chemistry and industry of starch Kerr.R.W
4 Industrial chemistry B.K.Sharma
49
5 Principles of Physical chemistry Puri,Sharma and Pathania
6 Unit operations in chemical engineering W.L.Maccabe and J.C.Smith
7 Unit operations - I and II D.D.Kalwe Pune vidyarthi griha prakashan,Pune
8 Science of ceramics chemical processing Hench .L. L
9 Science of Ceramics Stewart G.H
10 Corrosion: Causes and Prevention Speller F.N
11 Corrosion Engineering Fontana M.G ,and Green M.D Mcgraw-Hill
Aim: To Understand the fundamentals of Analyical Chemistry
Objectives:
1.To provide knowledge about the principles involved in different analytical techniques
2. To provide knowledge about theuse of modern techniques and instruments in chemical
analysis.
Module I- Stoichiometry and Concentration systems 7hours
Statistical evaluation of analytical data - Accuracy and Precision. Errors - Determinate and Indeterminate- stoichiometry- Mole and Equivalent concepts. Stoichometric calculations .concentration systems- molarity,normality, ppm and ppt. calculations involving various types of concentration systems
ModuleII-ReviewofChemicalEquilibrium 10hours
Auto protolysis of water- acids and bases. Ionization of weak acids and bases- equilibrium constant expressions. Hydrogen ion concentration – PH scale – Calculation of PH of weak acids and bases- Buffer solutions- PH of a buffer solution-Henderson Hasselbalch equation.
ModuleIII-SolubilityEquilibria 10hours
Principles of solubility- solubility product- factors affecting solubility- temperature, solvent, common ion effect, effect of complex formation, separation of metal ions based on solubility differences- sulphide seperations. Applications of solubility product principles in qualitative and quantitative analysis. Calculation of problems involving solubility equilibria.
Definition of terms – primary standard- secondary standard solutions- equivalence point and end point of titrations- types of titrations- calculations involving volumetric titrations. Acid base titrations, redox titrations, complex formation titrations, precipitation titrations
Module V-Gravimetric methods of analysis 10hours
Principles of gravimetric analysis- gravimetric factor- gravimetric calculations- conditions of precipitation- theory of precipitation- types of precipitants- organic precipitants- advantages- purity of precipitates – co-precipitation and post precipitation. Precipitation from homogeneous solution. Crucibles- types and maintenance. Washing off the precipitates- drying and ignition of precipitates.
ModuleVI-chromatographicmethods 10hours
Theory and principles- classification of chromatographic methods
a) Column chromatography- principles and experimental procedures- adsorbants and solvent systems- applications
53
b) Thin layer chromatography- principles and procedures- adsorbents- preparation of TLC plates- Rf values- Applications- separation of dyes
c) Paper chromatography- principles and experimental procedures – ascending and descending techniques. Applications- separation of aminoacids
d) Gas liquid chromatography- principles and instrumentation- columns- detectors- applications
Module VII- instrumental methods of analysis 15 hours
a) Thermogravimetry- Principles of TGA, DTA and thermometric titrations-
b) Colorimetry and specrophotometry- Qualitative aspects of absorption of radiation- Beer- Lambert
law- deviations spectrophotometer- instrumentation – single beam and double beam instruments.
Applications of colorimetry and spectrophotometry.
c) Polarography – basic principles- DME- advantages and disadvantages. Diffusion current- the ilkovic
equation- half wave potential- experimental setup and applications
d) Solvent extraction- principles- techniques- batch and continuous extraction- soxlet extraction and
counter current extraction-applications
e) Atomic absorption and atomic emission spectroscopy- principles and application
References
1. Analytical Chemistry: (J.W) G. D. Christain 2. Introduction to chromatography : Bobbit 3. Instrumental Methods of analysis (CBS)- H.H . Willard, L.L. Mirrit, J.A. Dean 4. Instrumental Methods of Analysis : Chatwal and Anand 5. Instrumental Methods of Inorganic Analysis(ELBS) : A.I. Vogel 6. Chemical Instrumentation: A Systematic approch- H.A. Strobel 7. Principal of Instrumental Analysis- D. Skoog and D.West 8. Treatise on Analytical Chemistry: Vol Ito VII – I.M. Kolthoff 9. Analytical Chemistry S.M Khopkar - New Age International 10. Analytical chemistry - R.Gopalan - Suhan Chand 11. Fundamentals of analytical chemistry- A.Skog and M.West 12. Vogel's hand book of quantitative inorganic analysis - Longman 13. Instrumental methods of' analysis - Skog 14. Instrumental methods of analysis - Willard et al - CXBS 14. Physico-chernical techniques of analysas-P.B.Janarthanam. Vol-I and Il-Asian publishing 15. Instrumental methods of chemical analysis - B.K. Sharma - God Publications 16. Analytical Chemistry S .Usharani, Macmillan
54
ELECTIVE
6B15 CHE – F. NANOMATERIALS - SYNTHESIS AND PRACTICE
Credit:4 Contact hours:72 Hrs
(Offered By Chemistry)
Aim: To Understand the fundamentals of Nano Science and Technology
Objectives:
1. To make an objective judgment of the scientific importance and technological potential
of developments in micro- and nanotechnologies.
2. To perform a range of activities related to Nanoscience and Nanotechnology
3. To prepare the student to take the challenge of meeting national needs and
international needs
UNIT 1.Definition and Scope of Nano Science 5 Hrs
Nanotechnology- Defenition, History- Timeline and Milestones, Overview of different
nanomaterials available, Potential uses of nanomaterials in electronics, robotics, computers, sensors
in textiles, sports equipment, mobile electronic devices, vehicles and transportation. Medical
applications of nanomaterials.
UNIT 2. Nano Chemistry 15 Hrs
Novel physical chemistry related to nanoparticles such as colloids and clusters: different
equilibrium structures, quantum effects, conductivity and enhanced catalytic activity compared to
the same materials in the macroscopic state.
Exploitation of self-assembly and self-organization to design functional structures in 1D, 2D or 3D
structures. Examples to emphasize on self-assembled monolayers.
Role of polymers in lithography resists, as well as self-organization of more complicated polymer
architectures such as block copolymers and polymer brushes.
UNIT 3 Synthesis of Nanomaterials 20 Hrs
Nanomaterials (Nanoparticles, nanoclusters, quantum dots synthesis): Preparation and
Characterization: “Top-Down” and “Bottom-Up” approaches of nanomaterial (nanoparticles,
(nanoparticles, nanoclusters and quantum dots) synthesis: Top-down techniques: photolithography, other
For Physical & Biological Sciences Contact Hrs –36
Credit -2 Module I : Atomic Structure and Periodic Table (10 hrs)
Bohr atom Model (No derivation) – Atomic Spectra – limitations – wave mechanical concept of atom – Heisenberg’s Uncertainty Principle – Duel nature of electrons – De Broglie equation – quantum numbers. Orbit and orbitals – Schrodinger equation (no derivation). The periodic table – periods and groups-s, p, d and f block elements – modern concept – periodic trends – atomic radii, ionic radii & covalent radii – effective nuclear charge and screening effect – Ionization potential – electro negativity and electron affinity.
Module II : Chemical bonding (10 hrs)
Ionic, covalent and co-ordinate bonds. Lattice energy of ionic compounds – Born Haber cycle. VSEPR theory and its applications. Shape of molecules CO2, BeF2, BF3, CH4, NH3, H2O, NH4
+, PCl5, SF6, ClF3. Orbital overlapping – Hybridization sp, sp2, sp3, sp3d, sp3d2, d2sp3 and dsp2
hybridization. V B Theory. MO theory. Formation of B2, C2, N2 and O2 molecules. Hydrogen bonding, types of hydrogen bonding – examples.
Module III : Radio activity and Nuclear Chemistry (10 hrs)
Concept of nuclides – representation of nuclides – isobars, isotopes and isotones with examples – Detection of isotopes using Aston’s mass spectrograph – separation of isotopes by diffusion methods – stability of nucleus – n/p ratio. Liquid drop model, Radioactivity – natural and artificial. Decay constant and half-life period-Radioactive series – Group displacement law – radio isotopes and their applications in structural elucidation, in agriculture and in industry – Radiocarbon dating – Nuclear fission and nuclear fusion. Problems associated in the nuclear waste disposal. Derivation of decay constant – Atomic bomb and hydrogen bomb. Mass defect, Nuclear binding energy.
Module IV : Electrochemistry (6 hrs)
Electrolysis – metallic and ionic conductors. Migration of ions – relative speed of ions – Transport number – determination of transport number using Hittorf’s method. Kohlrausch’s law and applications. Conductometric titrations – advantages. Ohms law – specific conductance – molar conductance and equivalent conductance – variation with dilution.
60
2C02CHE CHEMISTRY
For Physical & Biological Sciences Contact Hrs – 36
Credit - 2
Module I : Chemical kinetics and catalysis (10 hrs)
Definition – reaction rate – factors affecting the rate of a chemical reaction – units – Zero order reactions – Order versus molecularity. Pseudo order reactions – Integrated rate equation for first order reaction – half life – determination of the order – Half life method and Graphical method – Ester hydrolysis – equation. Collission theory (qualitative) Effect of temperature on reaction rate – calculation of Ea from the values of k at two temperatures. Transition state theory (qualitative). Types of catalysis – homogeneous and heterogeneous. Characteristics of catalysis reactions – promoters and catalytic poisons. Activation energy and catalysis.
Module II : Chemical equilibrium (6 hours)
Reversible reactions – Nature of chemical equilibrium – Characteristics of chemical equilibrium – Equilibrium constant – in terms of partial pressure – thermo dynamic derivation of chemical equilibrium. Liquid systems – Le-Chatlier’s Principle – Effects of temperature, pressure and concentrations.
Module III : Photochemistry (4 hrs)
Chemical reactions Vs Photochemical Reactions. Laws of photo chemistry – Grothus – Draper Law and Stark-Einstein law of photo chemistry. Quantum yield – Hydrogen Chlorine reactions. Photo sensitized reactions – Fluorescence and Phosphorescence – Chemiluminescence and bioluminescence.
Module IV : Colloids (8 hrs)
Classification – preparation – structure and stability – The electrical double layer – zeta potential – Properties of Colloids – Tyndall effect – Brownian movement- Coagulation of colloidal solution – Hardy-Schultz rule – Flocculation value – protective colloids – Gold number – Emulsions – oil in water and water in oil type emulsions – Emulsifying agents – Gels – imbibition – syneresis – applications of colloids in food, medicine and industry.
Module V : Analytical Chemistry (8 hrs)
Analytical chemistry – classification – accuracy and precision. Errors, Solubility product – ionic product – common ion effect principle of separation of cations in various groups. pH pOH and ionic product of water. Buffer solutions – Hendersons equations. Principle of volumetric analysis – Adidimetry and alkalimetry, permanganometry, dichrometry, iodometry and iodimetry. Chromatography – column – TLC and paper. Principles and applications.
61
Contact Hrs –54
Credit – 2
3C03CHE CHEMISTRY
For Biological Sciences
Module I : Metallurgy (6 hrs)
Metallurgy of aluminium, nickel, titanium and thorium
Module II : Co-ordination Chemistry (10 hrs)
Co-ordination compounds and complex ions –co-ordination number – ligand denticity. Chelating ligands and chelates – Werners theory – Nomenclature of co-ordination compounds – Affective Atomic Number – Factors affecting the stability of complex ions – valence bond theory of complexes – application of complexes. Module III : Introduction to organic chemistry (7 hrs)
Classification of organic compounds – functional groups, homologous series – Shapes of molecules like methane, ethane, ethylene and acetylene – nomenclature of hydrocarbons. Nomenclature of organic compounds bearing functional groups – Benzene structure – Aromaticity, Huckel’s rule.
Module IV : Organic reaction mechanisms (11 hrs)
Electron displacement effects - inductive effects – Electrometric effect. Resonance – Hyper conjugative effect and steric effect. Bond fission – Homolysis and heterolysis carbonium ion-carbanion and free radicals – their stability. Classifications of organic reactions – Mechanisms of SN1 and SN2 reaction. Walden inversion. Elimination reactions - E1 and E2
reactions. Addition of hydrohalogen acids – Markownikoff’s rule – peroxide effect. Aromatic electrophilic substitution reactions. Mechanisms of chlorination, nitration, sulphonation and Friedel Crafts reaction – Orientation effect and o, p ratio.
Module V : Stereochemistry (10 hrs)
Isomerism – general – stereoisomerism – optical isomerism – chirality – plane polarized light – specific rotation – enentiomerism – recemization – diastereo isomer – optical activity of lactic acid and tartaric acid – meso tartaric acid – resolution – conformational isomerism – ethane, propane and cyclohexane – chair and boat forms- stability – geometrical isomerism – causes – maleic acid and fumaric acid – 1-butene and 2-butene stability.
Module VI : Organic spectroscopy (10 hrs)
Basic principles – UV visible spectroscopy – formation of absorption bands – Types of electronic transition. Auxochromes, Bathochromes, Hyperchromic and Hypo chromic shift – applications. IR, NMR and Mass spectrometry – Important applications in Organic chemistry (No derivations).
62
Contact Hrs –54
Credit – 2
4C04CHE CHEMISTRY
For Biological Sciences
Module I : Carbohydrates (8 hrs)
Introduction – Definition and classification. Synthesis and properties of Glucose, Fructose and Sucrose – Mutarotation – Epimers and Anomers. D and L configuration. Conversion of glucose into fructose and fructose into glucose. Cane sugar – Structure and important properties – Polysaccharides. Starch, Cellulose and Chitin – structure, properties and tests.
Module II : Heterocyclic compounds (10 hrs)
Hetrocyclic systems – 5 membered, 6 membered and condensed systems. Structure of pyrrole, Furan and Thiophene. Electrophilic substitution in pyrrole, Furan and Thiophene. Reactivity and orientation – Saturated 5 numbered heterocyclics – Structure and properties of pyridine. Electorphillic and nucleophillic substitution reactions in pyridine – Basicity and reduction. Quinoline and isoquinoline – preparation and properties.
Module III : Nucleic acids (7 hrs)
Classification – structure of DNA and RNA – Functions of Nucleic Acids – DNA replication – Bio synthesis of Proteins – Test for DNA and RNA.
Module IV : Amino acids and proteins (10 hrs)
Classification of Amino acids – Physical and Chemical Properties – Zwitter ions – Iso Electric point – Sorensons formal titration – chromatographic separation of amino acids – Peptides – Proteins classification, characterization by electrolysis – Primary, Secondary and Tertiary level structures of proteins – Tests for Proteins.
Module VI : Enzymes, Vitamins and Hormones (10 hrs)
Enzymes – General Nature – Mechanism of Enzyme action, Enzyme catalysis, Michael – Mention equation (No derivation) – Application of Enzymes, Enzyme deficiency deceases – Vitamins – Classifications structure of Vitamin A, B and C. Hormones – Classification – Structures of progesterone, Testosterone, cortisone, adrenaline and Thyroxine.
Module VII : Bio inorganic compounds (9 hrs)
Introduction – Metal ions in biological system – Metals in medicine – metal – nucleic acid interaction – biochemistry of iron – haemoglobin and myoglobin – structure and functions – mechanism of oxygen binding – Na-K pump – bio chemistry of Zn and Co- Ca in biological system.
Introduction - Types of spectra – Rotational, vibrational and electronic spectra. Moment of intertia and bond length – Vibrational – Rotational or IR spectra – Force constants. Raman’s spectra – Stokes and Anti Stokes LInes – NMR spectra.
Module II : Thermodynamics (5 Hrs)
BASIC CONCEPTS – System – surroundings – open, closed and isolated systems – Isothermal – isochloric and isobaric process – work – heat – energy – internal energy – Heat capacity at constant volume (Cv) and at constant pressure (Cp) – relation between Cp and Cv – First law First law – The second law – concepts spontaneous and non spontaneous processes – statement of second law – entropy – entropy changes accompanying phase transitions – variation of entropy with temperature.
Module II : Metallurgy (6Hrs): Metallurgy of aluminium, nickel, titanium and thorium. Module III : Co-ordination compounds (10 Hrs)
Co-ordination compounds and complex ions – co-ordination number – ligand denticity. Chelating ligands and chelates – Werners theory – Nomenclature of co-ordination compounds – Affective Atomic Number – Factors affecting the stability of complex ions – valence bond theory of complexes – application of complexes.
Module IV : Introduction to organic chemistry (7 Hrs)
Classification of organic compounds – functional groups,Homologous series – shapes of molecules like methane, ethane, ethylene and acetylene – nomenclature of hydrocarbons. Nomenclature of organic compounds bearing functional groups – Benzene structure – Aromaticity Huckel’s rule.
Reaction mechanism – electron displacement effect – inductive effects – electromeric effect – resonance – hyper conjugative effect – and sterric effect – bond fission – homolysis and heterolysis – carbonium ion – carbanion – and free radicals – their stability.
Module V: Sterochemistry (10 Hrs)
Isomerism–general–stereoisomerism –optical isomerism–chirality–plane polarized light– specific rotation –enentiomerism–recemization–diastereo isomer–optical activity of lactic acid and tartaric acid–meso tartaric acid–resolution–conformational isomerism–ethane,propane and cyclohexane–chair and boat forms–stability–geometrical isomerism–causes–maleic acid and fumaric acid – 1. Butene and 2 butene – stability.
Module VI : Organometallic compounds (8 Hrs)
Organometallic compounds – ionic compounds – compounds of elements of group 2 to 5 – compounds of transition elements – multicentric bonds with pi-bonded ligands – bonding in pi- metal complexes. Bonding in ferrocene – Reactions of C5H5 Rings – Grignard Reagent – Tetra ethyl lead.
64
Contact Hrs –54 Credit - 2
4C04CHE CHEMISTRY
For physical science
Module I: Gaseous state (6 Hrs)
Ideal gas equation – deviation of gas laws from ideal behaviour – reasons for deviation – Van der Waals equation – critical constants and experimental determination – liquefaction of gases – Linde and Claude’s processes – Velocities of gas molecules – average, most probable and RMS velocities – problems.
Module II : Crystallinestate (9 Hrs)
Solids – crystalline and amorphous solids – space lattice and unit cell- crystal planes laws of crystallography – Weiss’s indices and Miller indices - Bravais lattice – different Bravais lattices of cubic crystals – characteristic planes in these lattices – interplanar distance ratio – X-ray analysis of crystals – Bragg’s equation – problem – crystal structure of NaCl – Liquid crystals – types, properties and applications.
Module III : Electromotive force (8 Hrs)
Electro chemical cell – Daniel cell – Cell reaction – Single electrode potential – statement – explanation of Nernst equation – Standard hydrogen electrode – Calomel electrode – measurement of EMF – determination of pH using Hydrogen electrode – Potentiometric titration – concentration cells.
Module IV : Ionic equilibria (7 Hrs)
Oswald’s dilution law – Debye – Huckel theory of strong electrolytes – Relaxation effect and Electrophoretic effect. Degree of dissociation. Common ion effect – Factors influencing degree of dissociation. Solubility product. Salt hydrolysis. Quantitative aspects of salt hydrolysis – determination of degree of hydrolysis. Salts of strong acid and weak bases. Salts of weak acids and weak bases.
Module V : Binary Liquid Systems (7 Hrs)
Solutions – Types – Thermodynamic properties of a solution – condition for equilibrium between phases – ideal solutions – Raoult’s Law – Vapour pressure of ideal solutions and real solutions – Boiling point diagrams of miscible binary mixtures. Distillation of binary miscible solutions – Azeotropes – Vapour pressure and distillation of immiscible liquids.
65
Module VI : Phase rule (6 Hrs)
Statement and expression of phase rule – Phase diagrams – Study of Water and Sulphur systems – Two component systems involving simple eutectic – Lead – silver system – Desilverisation of lead – Pattinson’s process – Deliquescence efflorescence.
Module VII : Instrumental methods in Chemistry (11 Hrs)
Thermal methods of analysis – TGA mand DTA – instrumentation – application – characterisation of polymers. Spectrophotometry-basic instrumentation of UV – visible spectrophotometry – maximum optical density measurement – IR basic details – application. Electro analytical method – amperometry – amperometric titration – applications – advantages and disadvantages.
Reference Books
1. Inorganic chemistry : Puri and Sharma
2.
Inorganic chemistry :
P.L.Soni
3.
Concise inorganic chemistry :
J.D.Lee
4.
Basic inorganic chemistry :
Cotton and Wilkinson
5.
Physical Chemistry :
Puri and Sharma
6.
Organic Chemistry :
Thivari, Malhotra and Vishnoi
7.
Organic reaction mechanism :
Peter Sykes
8.
Organic reaction mechanism :
Mukherjee and Singh
9.
Pragathi’s Instrumental Methods of Analysis :
H.Kaur
66
4C05CHE COMPLEMENTARY CHEMISTRY PRACTICAL
1. Qualitative Inorganic Mixture Analysis
a. Reactions of cations:
Study of the reactions of the following cations with a view of their identification
3. A.O.Vogel – “A Text Book of Quantitative inorganic Analysis”.
68
Time : 4 Hours
Credit: 4
COMPLEMENTARY CHEMISTRY PRACTICAL
(Done at the end of the 4th Semester)
1. Identify and confirm the two cations in the given solution by systematic qualitative
analysis. Submit a record of your tests, observation and inferences along with the report.
2. Determine ……………………. 3. In the first ten minutes,
a. Write a brief outline of the procedure you would adopt for the estimation of
……………….. in the given solution, given ………………… and,
b. Calculate the mass of …………………
4. Viva Voce
Mark distribution
Sd/- Dr.K.Pradeep Kumar,
Chairman,Board of Studies in Chemistry (UG)
69
KANNUR UNIVERSITY
SCHEME & SYLLABUS
CHEMISTRY (OPEN)
Effective from 2010 Admission Onwards
UNDER
CHOICE BASED CREDIT SEMESTER SYSTEM
70
No Semester Course Code
Title of the course Contact Hr/week
Credits
1 5 5D01CHE Chemistry in service to Man 2 2 2 5 5D02CHE Chemistry in everyday life 2 2 3 5 5D03CHE Food Science 2 2 4 6 6D01CHE Drugs-Use & Abuse 2 2 5 6 6D02CHE Environmental Studies 2 2 6 6 6D03CHE Nano Materials Synthesis & Practice 2 2
Scheme for Open Courses
71
OPEN COURSE
5D01CHE : CHEMISTRY IN SERVICE TO MAN
Credits : 02 Total Hours : 36
Aim: To create interest in studying the role of chemistry in overall development
Objectives:
1. To provide knowledge about the structure, properties and uses of plastics &polymers
2. To provide a brief idea about the role of chemistry in industry and agriculture 3. To make aware about the use and abuse of chemicals in daily life 4. To study about the chemistry of medicines
5. To provide knowledge about adverse effects in using polluted water and methods of treatment
1. PLASTICS & POLYMERS
Polymers- Types of polymers natural & synthetic polymers .characteristics, examples. Cotton fibre, Silk, jute, wool etc. Monomers,. General characteristics and applications of polymers such as Polythene (LDPE &HDPE), polypropylene, PVC, Poly styrene, Poly vinyl acetate, PET, Teflon, Terrylene, Nylons (Nylon 6,Nylone 66 & Kevlar),orlone, PMMA and Bakelite. Artificial fibers –Rayon .manufacture of artificial silk.
Plastics- Thermoplastics and thermosetting plastics examples. Characteristics. Elastomers-Natural and synthetic rubbers, applications, Vulcanization, Characteristics and uses of Buna, Butyl, Chloroprene ,SBR, Silicone & Thiokol rubbers. Biodegradable polymers .examples. benefits of biodegradable plastics. Importance of plastic recycling. 6 Hours
2. FERTILIZERS & INSECTICIDES
Natural , synthetic mixed and NPK fertilizers – examples.- making of NPK mixture - Impact of excessive use of fertilizers on environment – Bio fertilizers – plant growth
72
hormones. Pesticides and their classification- examples. Excessive use of pesticides. Environmental hazards. Safe handling of pesticides. Insect repellants- Pheromones
5 Hours
3. FUELS, CELLS & BATTERIES
Defenition and classification of fuels – Characteristics of good fuel – Combustion - Calorific value – wood- coal – origin of coal- classification-characteristics- petroleum-origin –fractional distillation –different fractions, their composition & uses. Natural gas, Biogas & LPG – their composition and uses. Pollution due to burning of fossil fuels
Batteries and fuel cells – Different types – Applications in modern life.
5 Hours
4 CEMENT &GLASS
Cement- Classification – Portland cement – Raw materials – manufacture – setting and hardening – criteria of cement quality and grade.
Glass – Different types – manufacture – raw materials – manufacture of ordinary glass – annealing- varieties of glass and their composition
Chemotherapeutic agents- classification, Drug action-Bactericidal- Sulpha drugs mode of actions Importance. Examples and uses. Antibiotics- Discovery, importance, mode of action. Examples. Misuse of antibiotics.
Antipyretics & analgesic- examples-uses. Anesthetic, Antiseptic, Anti histamines and tranquillizers, narcotics- their actions and examples. Misuse of drugs .Disinfectant & germicides examples .importance and uses. 6 Hours
73
7. WATER TREATMENT
Water sources – specifications for water- impurities in water- characteristics imparted by impurities – Hardness – Disadvantages of hard water in domestic and industrial use
Softening methods-lime soda, zeolite and ion exchange methods(principle only)- Drinking water or municipal water- methods of purification- removal of micro organisms- Desalination of brackish water-electro dialysis, reverse osmosis- Importance of dissolved oxygen, BOD & COD-Municipal Sewage treatment
8 Hours
References:-
1. J Barrett: Chemistry in your environment-User friendly, Simplified Science.
2. Howard L White: Introduction to Industrial Chemistry
3. David M Targarden: Polymer Chemistry – Introduction to an indispensible
science.
4. M.S.Yadav: Synthetic drugs
5. Samuel Delvin: Dyes and Pigments
6. Alexander Findlay: Chemistry in the service of man
7. S. K Honda: Principle of pesticide chemistry
8. M.M.Chakrabarthy: Chemistry and Technology of oils and fats
9. Shalini Sareen: Chemotherapeutic agents
10. P.K.Ray: Pollution and health
11. Vanessa Good ship: Introduction to plastic recycling
12.Randy Schmetter and Perry Romanoswski: Beginning cosmetic chemistry.
13. V Jain: Organic polymer chemistry
14.V K Selva raj: Advanced polymer chemistry
15. Jr Charles E Carraher: Introduction to polymer chemistry
16. Shashi Chawla: A Text Book of Engineering Chemistry
74
17. Jain & Jain : Engineering Chemistry
OPEN COURSE
5D02CHE : CHEMISTRY IN EVERYDAY LIFE (OPEN COURSE) Credits : 02 Total Hours : 36
Aim: To create interest in studying the role of chemistry in Daily Life
Objectives:
1. To study about the chemistry of food materials
2. To provide a brief idea about the role of chemistry in Soaps, Detergents and Cosmetics.
3. To provide knowledge about the structure, properties and uses of plastics &polymers
4. To study about the chemistry of drugs and dyes
5. To provide an understanding about corrosion and the role of protective coatings in preventing it.
1. CHEMISTRY OF FOOD MATERIALS Chemicals in rice, fruits and vegetables – examples of carbohydrates, organic acids, proteins
(amino acid blocks), vitamins, fats, minerals etc in food. Functional food additives and adulteration.
---- Natural and synthetic food colours-Permitted and non permitted. Anti oxidants-Natural and
synthetic. Flavours of some important foods-Fruit and Vegetable flavours, Spice flavours and
Beverage flavours, Monosodium glutamate and its harmful effects. Methods of food preservations,
Common Preservatives, NaCl, Vinegar, Sodium Benzoate, BHA, BHT etc. Number codes given to
food additives. Sweeteners- Naturally occurring and Artificial Sweeteners with examples. Soft drinks
and their formulation 9 Hours 2. SOAPS, DETERGENTS AND COSMETICS Soap – Manufacture from oils, Different types of soaps- Toilet soap, bathing bars and
Washing soap – Ingredients-Hot and Cold processes. Cleaning action of soap, TFM- importance.
Synthetic detergents, Types of detergents-cationic, anionic and amphiphilic detergents, Difference
from soap. Detergent action, Environmental hazards. Shampoo – composition and ingredients.
Cosmetics- Cleansing cream, cold cream, bleaching and vanishing creams, perfumes,
talcum powder, deodorants and lipsticks-ingredients. Harmful chemicals in cosmetics. 7 Hours 3. PLASTICS AND POLYMERS
75
Polymers and Polymerization . Classification of polymers. Thermoplastics and
Thermosetting plastics, Properties and Uses of HDPE,LDPE,PP,PVC,PET,ABS, PMMA, Orlons,
Epoxy resins, Bakelite, melamine and Poly carbonate. Moulding constituents of plastics-Resins,
Plasticizers, fillers, colouring agents and their role and health impacts.
Recycling of plastics, Environmental hazards. Biodegradable plastics. Recycling of plastics.
Elastomers-Natural rubber, sources, processing of latex, vulcanization, grading of sheet rubber.
7 Hours 4. CHEMISTRY OF DRUGS AND DYES
Chemotherapy- Type of drugs, Antipyretics, analgesics (narcotic and non-narcotic)-, Anesthetics,
Antiseptics, Anti histamines and tranquillizers, - their actions and examples.. Disinfectant &
germicides examples, importance and uses. Antibiotics- Discovery, importance, mode of action.
Examples. Misuse of Drugs
Natural and Synthetic dyes and their classifications on the basis of application and structure.
Harmful effects of coal tar dyes, Hair dyes –Types of hair dyes, adverse effects of hair colouring.
6 Hours
5. CORROSION AND PROTECTIVE COATINGS Corrosion, Dry and wet corrosion, Electrochemical theory of wet corrosion, Factors affecting
corrosion, Corrosion control, Protective coatings and the types of protective coatings, Methods of
coating- hot dipping, cladding, spraying, cementation and electroplating. Chemical conversion
coatings- phosphate coatings, chromate coatings and chemical oxide coatings.
Organic coatings-Paints, varnishes, enamels and emulsions and their compositions. 7 Hours References:- HK Chopra and PS Panesar: Food Chemistry
Owen K Francis: Food Chemistry
CNR Rao: Understanding Chemistry, University Press
J Barrett: Chemistry in your environment-User friendly, Simplified Science.
David M Targarden: Polymer Chemistry – Introduction to an indispensible science.
M.S.Yadav: Synthetic drugs
Samuel Delvin: Dyes and Pigments
Alexander Findlay: Chemistry in the service of man
Shalini Sareen: Chemotherapeutic agents
Vanessa Good ship: Introduction to plastic recycling
Randy Schmetter and Perry Romanoswski: Beginning cosmetic chemistry.
Jr Charles E Carraher: Introduction to polymer chemistry
76
Jain and Jain :Engineering Chemistry
Shashi Chawla :A Text Book of Engineering Chemistry
77
OPEN COURSE (Offered By Chemistry)
5D03 CHE: FOOD SCIENCE
Credit : 02 Total Hours : 36
Objectives:
1. Impart Knowledge regarding the composition of various food stuffs.
2. Familiarize students with changes occurring during processing and cooking
3. Enable students to use the theoretical knowledge in various food processing
preparations and technology.
4. Orient students to potential use of various byproducts of food industry.
5. Familiarize students the various tests and standards for quality assessment,
food safety and tests used to find food adulteration.
Unit -I: Introduction
Definition- Food Science, Food Technology, Functions of food, Cooking- Objectives of cooking, cooking methods 3 Hrs.
Unit -II: Constituents of Foods
Carbohydrates-Sugars, Starch. Proteins, Fats and Oils, Additional food constituents Antioxidants, Pigments and Colours, Flavours, Natural Toxicants, Water 4 Hrs.
Unit-III: Cereals and Cereal Products
Nutritive value-Breakfast cereals, Points to remember while cooking cereals, Specific cereals – Wheat, Rice, Maize, Jowar, Ragi, Bajra & Oats 3 Hrs
Unit-IV: Pulses,
Types –Bengal gram, Black gram etc,- Nutritive value. Effect of cooking – Medicinal values
Terms Related To World Hunger. Absolute Poverty, Anemia, Daily Caloric Requirements, Hunger, Malnutrition, Poverty Line, Under nutrition. 3 Hrs
References
1. B. Srilakshmi – Foood science-New Age international Publishers
2. N. Shakuntala Manay&M. Shadaksharaswamy- Foods-Facts&Principles- New Age
international Publishers.
3. Norman N. Potter, Joseph H . Hotchkiss- Food science,-Fifth Edition-CBS Publishers,
New Delhi.
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OPEN COURSE (Offered By Chemistry)
6D01 CHE DRUGS – USE & ABUSE
Credit : 02 Total Hours : 36
Objectives:
1. Impart Knowledge regarding the history, classification uses of different drugs.
2. To provide a brief idea about the mode of action of drugs
3. To make the students aware about the side effects of modern drugs.
4. To create awareness regarding bthe misuse of drugs and its harmful effects.
INTRODUCTION
Historical aspects- Definitions - Sources of drugs.
Routes of drug administration-enteral, Parenteral, Topical. 3 Hrs
PHARMACOKINETICS CHE MISTRY
Absorption, First Pass Metabolism, Distribution, Excretion.
A brief mention of the following: Mechanism of Drug Action, Dose – Response Relationship – Drug Synergism & Antagonism. Factors that modify the effect of drugs.
Adverse drug reactions – Side effects, toxic effects, intolerance, Iatrogenic disease, drug dependence, teratogenecity, carcinogenicity. 6 Hrs
Brief mention with examples. –Mode of action, adverse effects if any of the following classes
Drugs acting on Central Nervous System, Drugs acting on Peripheral Nervous System
Drugs acting on Cardio vascular Nervous System, Drugs acting on Haemato poietic System
Drugs acting on Renal System 6 Hrs
SYNTHETIC DRUGS
80
A brief mention with Examples of Sulfa drugs, Antipyretics & analgesics, Expectorants and antitussives, anti histamines, muscle relaxants, Anti- inflammator y, anti- emetic, antimalarial, anti psychotic, anti- ulcer and antibacterial drugs. Cancer and Chemotherapy 6 Hrs
MISCELLANEOUS DRUGS
Antiseptics and disinfectants, Vaccines, chelating agents, Vitamins and Minerals, Enzymes and Hormones, Treatment in poisoning. 5 Hrs
DRUGS OF ABUSE
Study of Chemistry, Classsification and mechanism of action of the following:
Anti psychotics, Opiod Analgesics, Antidepressants, Sedatives and Hypnotics, CNS Stimulants, Hallucinog ens, alcohols. 6 Hrs
REFERENCES
1. DRUGS – G.L. David Kurupadanam,D Vijayaprasad,K VarapHIIPATrasad Rao et.al.
2. MEDICAL PHARMACOLOGY- PADMAJA UDAY AKUMAR
3. ESSEN TIALS OF MEDICINAL PHARMACOLOGY - TRIPATHI
4. MEDICINAL CHE MISTRY – ASHUTHOSH KAR
5.DISPENSING PHARMACY –KAPOOR & GUNN
6. A TEXT BOOK OF FORE NSIC PHARMACY – B.M. MITHAL.
7. A TEXT BOOK OF ORGANIC AND PHARMACEUTICAL CHE MISTRY - WILSON & GISVOLD
81
OPEN COURSE(Offered by Chemistry)
6D02 CHE : ENVIRONMENTAL STUDIES
Aim: To study about the environment, pollutants ,their effects and control measures
Objectives:
1. To provide knowledge about the environmental segments ,their structure and composition.
2. To create awareness regarding the source, effects and sink of pollutants in the environment.
3. To study about the energy recourses, the role of fuel consumption in environmental pollution, importance of energy management and search for eco-friendly and non-conventional energy sources.
4. To inculcate among the students importance of environmental protection, & environment friendly life style for a better living and better future
1. Environmental segments – Lithosphere: soil formation – components of soils. Hydrosphere: Hydrological cycle , water and river water composition. Fresh water –surface water and ground water.- Biosphere- Atmosphere.- regions of Atmosphere- temperature and composition in different regions – Troposphere, stratosphere, Mesosphere, Thermosphere. 5 Hours
2. Air pollution –Sources – pollutants –CO, NOx, Sox, Hydrocarbons, Particulates. Effect on ecosystem., Ozone layer –importance, Ozone depletion-Control measures- Acid rain-control of acid rain- Green house effect-global warming,-photochemical smog- effect pollution on plants and human beings. Control of air pollution
Noise Pollution – physiological response to noise, Noise categories- effect of noise – biological effects. 6 hours
3. Water Pollution – Sources –Industrial effluents- agriculture discharge - oil spills-heavy metal -pesticides-biomagnifications and bioaccumulations-Experimental determination of dissolved oxygen in water, chemical oxygen demand (COD) and bio chemical oxygen demand(BOD)- control of water pollution- ISI/BIS standards of drinking water. 5hours
4 Soil Pollution - Sources by industrial and urban wastes, radioactive pollutants, plastics heavy metals.Poisoning by heavy metals – Mina- matha & itai-Itai
82
diseases. Control of soil pollution.- Solid waste Management -Thermal pollution definition-sources of thermal pollution , harmful effect of thermal pollution, prevention of thermal pollution.
6 hours
5 Sources of energy- fossil fuels, nuclear fission- Solar energy – use of solar energy in space- heating and water heating.- Production of electricity using solar energy. Solar trough collections- solar pond solar energy for driving vehicles, Power from indirect solar energy – Hydro power- wind power- Biomass energy. 5hours
7 Environment and public health- climate and health-Hazardous products – occupational hazards -infectious diseases- water borne diseases, vector borne diseases -Risks due to chemicals in food, cancer and environment. 5 hours
8. Biotechnology and its application in environmental protection – Introduction, Bioinformatics, Bio technology and pollution, control bioremediation, biological de-odourisation, biological purification of contaminated air. 4 Hours
Ref:-
1. Text book of Environmental Studies for under graduate courses – Erach Bharucha
2. Essential Environmental studies- S. P. Misra – S. N. Pandey 3. Environmental chemistry and pollution control – S.S Dara (2nd edition) 4. Environmental chemistry- Peter O’ Neill 5. Environmental chemistry – B.K. Sharma 6. Fundamental concepts of environmental chemistry – G.S Sodhi 7. Environmental Chemistry. A.K De
83
OPEN COURSE 6D03 CHE – NANOMATERIALS - SYNTHESIS AND PRACTICE
Credit:2 Contact hours:36 Hrs (Offered By Chemistry)
Aim: To Understand the fundamentals of Nano Science and Technology
Objectives:
1. To make an objective judgment of the scientific importance and technological potential
of developments in micro- and nanotechnologies.
2. To perform a range of activities related to Nanoscience and Nanotechnology
3. To prepare the student to take the challenge of meeting national needs and
international needs
UNIT 1.Definition and Scope of Nano Science 7 Hrs
Nanotechnology- Defenition, History-Timeline and Milestones, Overview of different nanomaterials
available, Potential uses of nanomaterials in electronics, robotics, computers, sensors in textiles, sports
equipment, mobile electronic devices, vehicles and transportation. Medical applications of nanomaterials.
UNIT 2. Nano Chemistry 10Hrs
Novel physical chemistry related to nanoparticles such as colloids and clusters: different equilibrium
structures, quantum effects, conductivity and enhanced catalytic activity compared to the same materials in
the macroscopic state.
Exploitation of self-assembly and self-organization to design functional structures in 1D, 2D or 3D structures.
Examples to emphasize on self-assembled monolayers.
UNIT 3 Synthesis of Nanomaterials 12Hrs
Nanomaterials (Nanoparticles, nanoclusters, quantum dots synthesis): Preparation and Characterization:
“Top-Down” and “Bottom-Up” approaches of nanomaterial (nanoparticles, nanoclusters and quantum dots)
synthesis: Chemical Routes for Synthesis of Nanomaterials: Chemical precipitation and co-precipitation;
Metal nanocrystals by reduction, Sol-gel synthesis; Solvothermal synthesis; Thermolysis routes, Microwave
heating synthesis; Sonochemical synthesis;Electrochemical synthesis; , Photochemical synthesis, Synthesis in
supercritical fluids,current state-of-the-art.
UNIT 4 Applications of Nanomaterials 7Hrs
Solar energy conversion,storage and catalysis. Nanoelectronics, nanosensors, nanomedicine,
1. G.L.Hornyak, J.Dutta, H.F.Tibbals, A.K.Rao, Introduction to Nanoscience, CRC
Press, 2008, ISBN: 978-1-4200-4805-6
2. A.Nabok, Organic and Inorganic Nanostructures, Artech House 2005
3. C.Dupas, P.Houdy, M.Lahmani, Nanoscience: Nanotechnologies and
Nanophysics,Springer-Verlag Berlin Heidelberg 2007
4. Hari Singh Nalwa, Nanostructured Materials and Nanotechnology, Academic
Press,2002
5. Nanotechnology- Richard Brooker,EARL Boyson- Wiley Dream Tech India
6. Advances in Nanoscience and Nanotechnology- Dr.Ashuthosh Sharma,Dr.Bellari-
CSIR Publication 2004
7. Nanotechnology(Malayalam) – Anwar Sadath- DC Books
8. Nanochemistry: A Chemical Approach to Nanomaterials – Royal Society of
Chemistry, Cambridge, UK 2005.
9. Chemistry of nanomaterials : Synthesis, properties and applications by CNR Rao et.al. 10. ‘Handbook of Theoretical and Computational Nanotechnology, Eds. Michael Rieth
and Wolfram, Schommers, 2006.
11. ‘Handbook of Theoretical and Computational Nanotechnology, Eds. Michael Rieth and Wolfram
Schommers, 2006.
12. Nanotubes and Nanowires- CNR Rao and A Govindaraj RCS Publishing.
13. Concepts in Spintronics – Sadamichi Maekawa
14. Spin Electronics – David Awschalom
15. Carbon Nanotubes: Properties and Applications- Michael J. O'Connell
85
Annexure I
Kannur University
Board of Studies in Chemistry(UG)
Project Work Guidelines
Project work is the best way to learn how to learn. It provide the students the opportunity to familiarize with research methodology and scientific way of investigating a problem. Project work also helps in inculcating scientific temper in students which will be benefitted in both academic and real life.
General Guidelines of Project Work
1. Students should undertake the project work related to Chemistry only.
2. Students are advised to think about different problems for doing the project work and select
the suitable one taking into consideration the available facilities in the institution, access to
modern facilities available in other institutions, prospects of the project etc., in consultation
with the Project guide.
3. The UG level project work is a group activity, maximum number of students being limited to
five.
However each student should prepare and submit the project report separately. 4. Head of the Department may provide the service of a teacher for supervising the project
work of each group. A teacher can guide more than one group, if necessary.
5. The students can do the project at any period during the programme. Separate time is not
allotted for doing the same.
6. Project work can be experimental, theoretical or both.
7. No two groups in the same institution are permitted to do project work on the same
problem. Also the project should not be a repetition of the work done by students of
previous batches.
8. Each student should submit a copy of the report to the department on or before the last
working day of Semester VI. Besides each group should submit a copy to keep in the
Department.
86
9. The matter should be typed on A-4 size paper with Times New Roman font of size 12 points,
with double spacing between the lines and margins of 1.5’ at the left, 1’ at the right, 1’ each
at the top and bottom.
10. The report should be printed in plain white paper in black ink only. Color inks for charts and
graphs can be used, provided it does not hamper the readability. The logo of the college can
be displayed in the report.
11. The pages should be numbered and each chapter should begin in a new page.
12. The project report should be hard bound, spiral bound or paper back.
Format of the Project Report
Project Title
Name of the student
Department
College
Month & Year
Title Page(No page number)
emblem
87
Project Title
Project Report
submitted to Kannur University
in partial fulfillment
for the B.Sc Degree(Chemistry)
By
Name of the student
Reg. No.
Other Members of the group Name & Designation Project
1. Guide:
2.
3.
4. Signature Name and Designation
of Head of the Dept.
Examiners:
1.
2.
emblem
88
Initial Pages ; (add number as I, ii, iii, iv etc.)
Page I : Declaration ( By Project Guide)
Pageii. Acknowledgement ( By Student)
Page iii. Certificates, if any ( if done in collaboration with any other institute, industry etc.)
Page iv . Contents
Chapter Subject Page No.
1.
2.
3.
List of Tables
1.
2.
List of Figures
1.
2.
Chapter I : Introduction/Executive summary
Chapter II : Aim of the project/Problem Statement
Chapter III : Review
Chapter Iv : The Study/Present work
Chapter v : Data Analysis/ Discussion
Chapter vI :Conclusion
Chapter vii :Solutions/ Suggestions, if any
Bibliography
89
Evaluation of the Project Work:
The internal evaluation will be done at the Department level. As in the case of Core Courses , Internal evaluation of the project work carries the same weightage as the core practical course. This has to be awarded to the student on the basis of performance in the project work and presentation followed by an internal Viva- Voce conducted by a three member committee comprising of Head of the Department, supervisor and a senior faculty member.
The external evaluation will be done by Examiners appointed to conduct the practical examination of Semester VI. The evaluation is based on the report and Viva-Voce. The weightage for different components are as follows.
Component Weightage
Report 2
Presentation 2
Viva- Voce 1
Declaration of Result:
The Student should get a minimum of D grade for pass. In an instance of inability of obtaining the minimum, the project work may be done again and report submitted.
Industrial Visit
Industrial visit is part of curriculum for B.Sc. Chemistry students and it may be conducted on convenient time during III to VI semester of the programme. Visit to a Research centre/Laboratory or Industry which is related to Chemical Sciences is necessary to submit the report. The report will be subjected to both internal and external evaluation as in the case of any core course.
Each student should submit report of industrial visit prepared independently, neatly written and duly certified by Head of the Department. The report should be submitted for external evaluation along with practical records and project report during the practical examinations of semester VI. The evaluation will be solely based on the contents in the report. Those who didn’t participate in study tour are not eligible to submit the report.
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