Semester – I - JMC || Home · Web viewMolecular orbital theory - Concept – Linear combination of atomic orbital – M.O diagram for N2, O2, CO, NO, HF molecules. Comparison of

Semester – I 08UCH1301

ALLIEDPaper I – INORGANIC, ORGANIC AND

PHYSICAL CHEMISTRY

Unit – I (6 hrs)

1.1 Industrial Chemistry

Fuel gases – Water gas, Producer gas, L.P.G., Gobar gas and Natural gas. Fertilizers – N.P.K and mixed fertilizers.Soap and detergents – An elementary idea of soap and detergent. Cleansing action of soap and detergents.

Unit – II (6 hrs)

2.1 Polar Effects

Inductive effect – Relative strength of aliphatic acid and alkyl amines. Resonance – Condition for resonance, Consequences of resonance- Hyperconjugation – definition and examples.

Unit – III (6 hrs)

3.1 Halogen Containing Compounds

Important chlorohydrocarbons used as solvents and pesticides (Dichloromethane), Chloroform, Carbon tetrachloride, DDT, B.H.C.

3.2 Chemotheraphy

Sulpha drugs – Sulpha pyridine, Sulpha –thiazole and sulpha diazine – Strutural properties and uses. Antibiotics and penicillin – G and Chloromycetin formula and uses.

Unit – IV (6 hrs)

4.1 Solid State

Typical crystal lattice – Unit cell. Elements of symmetry. Bragg’s equation, Weiss indices, Miller indices, Simple, Body centred and face centred cubes.

4.2 Energetics

Second Law of theromodynamics - Carnot’s Theorem – Carnot Cycles.

4.3 Phase Rule

Phase, Component, Degree of freedom, Phase Rule – Definition. One component system – Water system.

Unit – V (6 hrs)

5.1 Chemical Equilibrium

Criteria of homogeneous and heterogeneous equilibria. Decomposition of HI and PCl5.

5.2 Chemical Kinetics

Order, Rate, Molecularity of the reaction and rate constant, Determination of order of the reaction – Activation energy, Effect of temperature on reaction rate.

Reference:

1. R.D. Madan, J.S. Tiwari and G.L. Mudhara – A text book of First year

B.Sc Chemistry: S. Chand and Co.

2. B.R. Puri and L.R. Sharma – Principles of Inorganic Chemistry: Shoban Lal,

Nagin Chand and Co., New Delhi (2000)

3. B.R Puri and L.R. Sharma – Principles of Physical Chemistry: Shoban Lal,

Nagin Chanc and Co., New Delhi.

Semester –I 08UCH1401

PART –IIICORE-I

GENERAL CHEMISTRY -I

UNIT – I (9 hrs)

1.1 VSEPR theory - Assumptions – Shapes of molecules such as NH3, H2O, CH4

1.2 Molecular orbital theory - Concept – Linear combination of atomic orbital – M.O

diagram for N2, O2, CO, NO, HF molecules. Comparison of valence bond and

molecular orbital theories.

UNIT – II (9 hrs)

2.1 Hydrides – Classification, preparation, Properties and uses.

2.2 Hydrogen peroxide – Manufacture, properties, structure, strength of H2O2 solution

– Determination, uses.

UNIT – III (9 hrs)

3.1 Nomenclature of organic compounds – IUPAC naming of simple aliphatic

compounds containing different functional groups – naming of aromatic

compounds and alicyclic compounds.

3.2 Orbital overlap – sigma and pi bonds – hybridization and geometry of molecules

methane, ethane, ethylene and acetylene.

UNIT – IV (9 hrs)

4.1 Reactive intermediates – free radical – carbocation – carbanion – generation –

chemical properties, structure and stability – homolytic and heterolytic fission of

bonds.

4.2 Electron displacement effects – inductive – electromeric – mesomeric – resonance

– hyperconjucation – and steric effects.

UNIT – V (9 hrs)5. Gaseous State:

5.1 Gas Laws-Kinetic of theory gases, Kinetic equation of gases, Molecular velocity,

Maxwells’law of distribution of molecular velocities.

5.2 Mean free path, Collision diameter, Collision number, Collision frequency,

5.3 Real gases and ideal gases, Deviation of real gases from the ideal gas laws,

Vander Waals equation to critical phenomenon, Calculation of critical constants.

References:

1. P.L.Soni & Mohankatyal – “Text Book of Inorganic Chemistry”, 20th Revised

Edition., (1992), Sultan Chand.

2. R.B.Puri & L.R. Sharma, “Principles of Inorganic Chemistry”, (1989), Sultan

Chand.

3. Morrison and Boyd – “Organic Chemistry” – 6th Edition., (1998) – Prentice_Hall of India Pvt. Ltd., New Delhi.

4. Bahl and Arun Bahl – “Advanced Organic Chemistry” – 19th Edition., (2005) – Sulthan and Chand company, New Delhi.

5. M.K. Jain – “Organic Chemistry” – 12th Ed., (2003) Sulthan and Chand Company,

New Delhi.

6. B.S. Bahl., G.D. Tuli & Arun Bahl – “Essentials of Physical Chemistry”, (1999), S.Chand & Co., New Delhi.

7. R.L. Madan, G.D. Tuli – “Simplified Course in Physical Chemistry”, (1999),

S.Chand & Co., New Delhi.

Semester – I 08UCH1402PART –III

CORE -II NUCLEAR CHEMISTRY

Unit – I (15 hrs)

1.1 Nuclear Chemistry introduction – Composition of nuclear and nuclear forces-

Meson theory.

1.2 Nuclear stability – N/P ratio – Mass defect, binding energy, packing fraction and

magic number.

1.3 Isotopes – Separation of isotopes – Thermal diffusion method – Distillation

method - Isotopic constitution of elements.

Unit – II (15 hrs)

2.1 Isobar – Isotones – Nuclear Isomers – Definition – Examples.

2.2 Nuclear reaction – Classification of Nuclear reaction – Uses of Projectiles,

nuclear fission and fusion reactions –Spallation reactions, stellar energy-

Hydrogen bomb,atom bomb- Advantages – Nuclear shell and liquid drop model.

– Nuclear power stations in India


3.1 Radioactivity – Definition – α-rays, β-rays, Gamma rays – Properties.

3.2 Detection and measurement of Radioactivity (GM Counter, Wilson cloud

champers method).

3.3 Disintegration – Modes of decay – Group displacement law – Rate of

disintegration – Half life and average life – Radioactive series.

Unit – IV (15 hrs)

4.1 Artificial Radioactivity – Definition – Examples – Preparation of transuranic

elements.

4.2 Radioactive tracer – Radio chromatography – Isotopic dilution analysis – Neutron

activation analysis.

4.3 Application of Radio Isotopes – Carbon dating – Medicine – Agriculture –

Radioactive tracers – Disposal of radio active waste.

Unit – V (15 hrs)

5.1 Nuclear reaction energy value (Q-Value) – Calculation of Q- values – Nuclear

reactor ( Breedor reactor) – Nuclear power stations in India.

5.2 The acceleration of charged particle –cyclotron, synchro cyclotron,betatron and

the electron synchrotron,proton synchrotron,linear accelerator.

Reference:

1. R.D. Madan –“Modern Inorganic Chemistry” (1987). S.Chand &Co Pvt Ltd.,

2. Arnikar – “Nuclear Chemistry”

3. B.R. Puri & L.R. Sharma – “Principle of Inorganic Chemistry”.Shoban Lal, Nagin

Chand & Co ., New Delhi (2000)

4. P.L. Soni – “Textbook of Inorganic Chemistry”. S.Chand&Co., New Delhi(1999)

5. C.V. Shekar, -“A textbook of Nuclear Chemistry”. (2005). Dominant Publisher

and Distributor.

6. Irving Kaplan - “Nuclear Physics-Narosa Publishing house.

Semester – I 08UCH1701PART-IV

SKILL BASED ELECTIVE-IINDUSTRIAL CHEMISTRY

Unit – I (6 hrs)

1.1 Water - Definition – Types – Hardness – Methods of softening water – Lime

soda, permutit process – Ionexchnage process – Expressing degree of hardness –

Estimation – EDTA – Disadvantage of hard water.

1.2 Plastics - Definition – Formation – Classification – Chemical mechanical

properties – Uses of plastics PVC, Nylon, Polythene, Balcelite.

Unit – II (6 hrs)

2.1 Rubber - Definition – Preparation of rubber from Latex – Natural rubber –

Vulcanization – Compounding of rubber – Synthetic rubber – Buna-s – Butyl

rubber – Properties and uses.

2.2 Abrasives – Definition – Scale of hardness – Classification – Natural Diamond,

Corundum, Emery, Artificial carborundum, born carbide – Metallic abrasives –

Characteristics of Abrasives.


3.1 Lubricant – Definition – Classification, Liquid – Animal oil - Vegetable oil,

mineral oil, solid – Graphite – Molebdenum sulphide – Semisolid lubricants

grease – Vaseline – Properties of good lubricants.

3.2 Fuels – Definition – Colorific value – Colorie – Gross and net colorific value –

Classification of fuels – Natural, artificial, solid, liquid, gaseous, fuels – Coal,

Petroleum, water gas, LPG and biogas – Advantage.

Unit – IV (6 hrs)

4.1 Corrosion – Definition - Types – Chemical – Electrochemical – Factors affecting

corrosion rate – Methods of prevention – Metallic coating – Hot dipping –

Cementation – ‘Electroplating – Galvanization.

4.2 Paints – Pigment – White pigment, black, blue pigment - Red pigments –

Examples – Constituents of paint – Requirement of a good paint – Paint failure –

Emulsion – Varnish.

Unit – V (6 hrs)

5.1 Refractories – Definition – Requirements – Types – acidic, basic and nutral

refractories – Example –Uses.

5.2 Cement – Definition – Important constituents – Raw materials – Manufacture –

Wet, dry process – Setting of cement – Function of compounds – Uses.

Reference:

1. B.K. Sharma –“Industrial Chemistry” 1st edition, (1983)., Goel Publication,

Meerut.

2. Jain and Jain, “Engineering chemistry” (2005)., Dhapathrai Publishing Co., New

Delhi.

Semester –II 08UCH2303ALLIED

Paper III - CHEMISTRY OF SOIL,WATER AND AIR

Unit – I (6 hrs)

1.1 Environment – Introduction – Compounds of Environment – Factors affecting

Environment – Man and Environment – Types of Environment.

1.2 Concept of Environment chemistry – Segments of Environment – Structure of

Atmosphere – Climate and weather – Hydrosphere – Lithosphere – Biosphere.

.

Unit – II (6 hrs)

2.1 Air pollution – What is Air pollution – Composition of Air –Major sources of Air

pollution.

2.2 Classification and effect of Air pollutants – Pollutants – Effects of Air pollution

on weather, climate and atmosphere process – Particulate pollutants – Fly ash –

Effects of particulate pollutants – Control of particulate emission – Effects of Air

on Human health – General methods of Air pollution control.


3.1 Noise pollution – What is Noise – Sources of Noise pollution – Characteristics of

Sound – Measurement of Noise – Unit of Sound – Measurement of Noise level

Loudness of Decibel scale – Measurement of sound power – Types of Noise.

3.2 Effects of Noise pollution – Prevention and control of Noise pollution -

Industrial Noise control

Unit – IV (6 hrs)

4.1 Water pollution – Definition of water pollution – Types of water pollution –

Physical, Chemical, Biological and Physiological pollution of water.

4.2 Types of water pollution – Harmful effects of ground water pollution – On Man,

on soil – Protecting ground water from pollution.

4.3 Sources of water pollution – Classification of water pollutants – Water treatment

– Softening of water.

Unit – V (6 hrs)

5.1 Soil – Important of soil – Life on soil – Soil formation – Factors affecting soil

formation – Composition of soil – Types of soil – Soil indicator plants – Acid soil

indicator plants – Alkaline soil indicator plants – Plants as indicators of pollution

– Bio-indicators.

5.2 Source of soil pollution – Soil pollution by soluble salts – Waster water added to

soil.Treatment of soil pollutants – Chemical methods of sewage treatment –

Control of Soil pollution.

Reference:

1. B.K. Sharma and H. Kaur- “ Environmental Chemistry” Goel Publishing house,

Meerut.

2. A.K.De “ Environmental Chemistry”:

Semester – II 08UCH2403

PART –IIICORE -III

GENERAL CHEMISTRY – II

UNIT – I (9 hrs)1.1 Halogen family – Comparative study of halogens – Basic properties – Halogen

halides – Chemistry of Astatine.

1.2 Oxides and oxy acids of halogens - Properties, comparison of oxy acid – Uses.

1.3 Inter halogen compounds – Preparation, properties structure. Pseudo halogens –

Cyanogens, thiocyanogen – Uses.

UNIT – II (9 hrs)

2.1 Group IA elements – Comparative study – Diagonal relationship between Li and

Mg – Position in the periodic table of alkali metals.

2.2 Group IIA elements – General properties – Their compounds oxides, carbonates,

sulphates – Properties and uses.


3. 1 Alkanes – preparation by Wurtz reaction – mechanism of free radical substitution

in alkanes.

3.2 Alkenes – Preparation by Wittig reaction - properties of alkenes – electrophilic

and free radical addition – Addition reactions with Hydrogen, Halogens,

Hydrogen halides (Markownikoff’s Rule), (peroxide effect) – hydroboration,

ozonolysis, hydroxylation with KMnO4 – allylic substitution of NBS.

UNIT – IV (9 hrs)

4.1 Dienes: Types of dienes – conjugated – Non conjugated and cumulated dienes –

relative stabilities of dienes and chemical reactivity – 1,2 and 1,4- additions –

kinetic and thermodynamic controlled reactions - Diels – Alder reaction.

4.2 Alkynes – preparation – properties and uses – Acidity of alkynes - formation of

metal acetylides (Li, Na and Cu) – Addition of water with HgSO4 – Halogens –

Hydrogen halides – oxidation by KMnO4 – Ozonolysis – and Hydroboration

UNIT – V (9 hrs)

5.1 Solid state – crystalline and amorphous solids, isotropic and anisotropioc solids.

Crystal systems (Cubic system only) space lattice and unit cell. Seven crystal

systems - crystal structure of NaCl, CsCl. Packing in crystals – hcp, ccp, bcc.

Bravis lattice – law of rational indices, Weiss indices and Miller indices.

5.2 X- ray diffraction - Derivation of Bragg`s equation – Determination of crystal

structure – Laue`s powder method.

References:

1. Puri, Sharma, Pathania – “Principles of Inorganic Chemistry”, (1998), Vishal

Publications, Jalandar Publications.

2. P.L. Soni – “Text Book of Inorganic Chemistry”, (1999), S.Chand & Co., New

Delhi.

3. Bahl and Arun Bahl – “Advanced Organic Chemistry” – 19th Ed., (2005) –

Sulthan and Chand company, New Delhi.

4. P.L. Soni and H.M. Chawla – “Text Book of Organic Chemistry” – 28th Ed.,

(1999) - Sulthan and Chand company, New Delhi.

5. B.S. Bahl., G.D. Tuli & Arun Bahl – “Essentials of Physical Chemistry”,

(1999), S.Chand & Co., New Delhi.



Semester –III 08UCH3404

PART –IIICORE-IV

GENERAL CHEMISTRY - III

Unit – I (15 hrs)

1.1 Elements of born family – Comparative study compounds of boron – Diborone,

boron trioxide, orthoboric acid, borax, boron halides, boron nitride,borazine.

Compounds of aluminium: Aluminium oxide, aluminium chloride, sulphate(alum)

– properties, uses.

1.2 Elements of Carbon family – Comparative study – Compounds of Carbon CO,

CO2, Phosgene, CS2, - Preparation, properties, uses.Silicon: Compounds of Si –

Structure of silicondioxide – Preparation, properties, uses.


.

2.1 Alcohols:

Classification – isomerism – general methods of preparation - properties –

Distinction between primary, secondary and tertiary alcohols by oxidation, Lucas

and Victor Meyer methods – Glycol, Glycerol - preparation, properties and uses.

2.2 Ethers:

Simple and mixed ethers – isomerism – general methods of preparation of

aliphatic ethers – Anisole – Preparation, properties and uses – Thio ether and

mustared gas

2.3 Alkyl halides:

Preparation – properties – Vicinal and gem dihalides - Grignard reagent –

preparation and synthetic applications. Aliphatic Nucleophilic substitution

reaction - mechanism of SN1, SNi reactions – Elimination reactions : -

mechanisms of E1, E2 reactions – Saytzefts and Hofmann rules.

Unit – III (15 hrs

3.1 Aromaticity and Aromatic hydrocarbons:

Aromaticity – Definition – Huckel’s rule of aromaticity of benzenoid compounds

3.2 Aromatic Electrophilic substitution reactions:

General mechanism of electrophilic reactions – Halogenation, Nitration,

sulphonation, Fridel-Craft’s alkylation and acylation reactions. Orientation effects

of various groups – ortho-para ratio. Nuclear and side chain halogenations of

toluene.

3.3 Petroleum: Thermal and catalytic process of cracking ,Synthetic petrol-Fischer

Tropschs Process-Bergius process –flash point,fire point ,smoke point-knocking-

octane number and cetane number-antiknocking reagents –Power alcohol.


4.1 Acids and bases – Arhenius , Bronsted lowry , Lewis acid base – Theories of

acid and base. Ionic Equilibria -Buffer solution – Definition, buffer capacity,

mechanism of buffer action, pH scale ,pOH, Kw, pKa and calculation of pH of

buffer mixtures by Henderson’s equations.

4.2 Hydrolysis of salts – Definition, salts of strong acids-strong base. salt of weak

acids- strong bases, salt of weak base-strong acid, salt of weak acid-weak base,

hydrolysis constant(Kh), relation between Kh, Ka and Kw, degree of hydrolysis -

salt of weak acid- strong base, salt of weak base-strong acid, salt of weak acid-

weak base.

Unit – V (15 hrs)

5.1 Basic concepts of kinetics – Rate of reaction, rate constant, factors influencing

rate constant, order of reaction, Equations of the rate constant for first, second,

third, zero order reactions, methods of determining order of reaction – Integration,

Graphical, Half life and Ostwald`s Method.

5.2 Energy of activation and its significance, influence of temperature, Arrhenius Rate

Equation and its significance. Theories of reaction rates – Simple collision theory -

Absolute Reaction Rate Theory (ARRT) to simple uni-molecular and bimolecular

processes - Comparison of collision & ARRT.

5.3 Electrical Properties of Matter:

Polar and non – Polar molecules, dipole moment, polarisastion of molecules in an

electric field - Electronic polarization, atomic polarization, orientation

polarization. Clausius Mosotti equation (no derivation), Debye equation.

(no derivation). Methods to determine dipole moment – (Temperature method,

dilute solution method) - applications of dipole moment.

References:

1. R.D. Madan, Modern Inorganic Chemistry reprint – 2003, S. Chand &

Company Ltd., New Delhi.

2. A.O. Thomas, Practical Chemistry, 8th ed., Geethanjali Offset Prints, Calicut.

3. A.K. Srivastava – “Organic Chemistry” – 1st Ed.,(2002) – New Age

International Publishers, New Delhi.

4. Morrison and Boyd – “Organic Chemistry” – 6th Ed., (1998) – Prentice_Hall of

India Pvt. Ltd., New Delhi.







Semester – III 08UCH3602PART-IV

NON MAJOR ELECTIVE-I CLINICAL CHEMISTRY

Unit – I (6 hrs)

1.1 Blood – Composition – Function – Blood groups - Rh factors.

1.2 Hemoglobin - Biological function and properties – Blood coagulation –

Mechanism. Hematological agents – Coagulants – Anti coagulants.

Unit – II (6 hrs)

2.1 Hormones – Salient feature of hormones – Biological function of hormones

– Chemical nature.

2.2 Vasoprussin, Oxytocin, Thyroxin and Insulin – Biological functions only.


3.1 Antiseptic and disinfectants – Definition ,Phenol related compounds -

Halogen compounds – Uses, Dyes – Crystal violet, Acridine – Uses,

Formaldehyde and Nitro Furazone – Uses, Distinction between antiseptic

disinfectants.

3.2 Anesthetics – General anesthetics – Local anesthetics – Examples –

Advantages.

Unit – IV (6 hrs)

4.1 Communicable diseases – Chickenpox, Diphtheria, Tuberculosis and

Leprosy causes – Clinical presentation, treatments and prevention.

4.2 Non-Communicable diseases – Cancer, Diabetes and Hypertension –

Causes – Prevention – Treatment.

Unit – V (6 hrs)

5.1 Psychopharmacology, antipsychotic drugs, anti anxiety drugs, anti

depresent drugs, sedatives and hypnotics.

5.2 Blood analysis – Blood urea – Bile pigment – Protein – Glucose.

Reference:1. J.L. Jain Sunjay Jain, and Netin Jain – “Fundamentals and

Biochemistry” (2006) S. Chand & Co ltd.

2. M.N. Chatterjee Rana Shinda – “Textbook of Medical Biochemistry”

Jaypee Brother – Medical Publisher (P) ltd – New Delhi.

3. N.S. Parmer, “Health education and community pharmacy” CBS

Publishers & Distributor – New Delhi.

4. G.R. Chatwal “Pharmaceutical chemistry Inorganic-volume-I”

Himalaya publisher.

5. Dulsy Fathima, R.P. Meyannpillai, and N. Arumugam, “Bio-chemistry”

Saras publication.

6. S. Lakshmi, “A textbook of Pharmaceutical Chemistry” 1st edition,

Sulthan Chand sons – New Delhi.

7. Jayashree Ghose,” A textbook of Pharmaceutical Chemistry “1st

edition. Shree Ghoshi, S. Chand & Company ltd. New Delhi.

8. Jayashree Ghose, “Fundamental concepts of applied chemistry” 3 rd

edition. S. Chand & Company Ltd. New Delhi.

9. I.L. Finar “Organic Chemistry II” 5th edition. Dorling Kindersley Pvt

Ltd., New Delhi.

Semester –III 08UCH3702PART – IV

SKILL BASED ELECTIVE-IICOMPUTER APPLICATIONS IN CHEMISTRY

Unit – I (6 hrs)

1.1 Introduction to computer – Characteristics of computers – Organization of a

computer – Secondary storage devices – Computer languages – Low level,

assembly and high level languages – software – System and application software

– Application of computer – Algorithms and flow charts.

Unit – II (6 hrs)

2.1 Operating system – MS-DOS, simple DOS commands – MS-Windows -

Components of Windows – Desktop, My Computer, Recycle Bin, Taskbar, My

briefcase and Network Neighborhood – Windows Accessories – Calculator,

games, Windows media player, Notepad and Imaging – Windows Explorer.

Unit –III (6 hrs)

3.1 Fundamentals of Computer Networks – Importance – Mode of Connections –

Protocol – Network Topologies – Bus, Ring and Star topologies – Network

Architecture - Network components – Hubs , cables, repeaters, routers and

bridges,

Unit – IV (6 hrs)

4.1 Internet and Intranet – Type of Networks – World Wide Web – Internet Architecture

– Domains – Applications of Internet – Electronic mail – Electronic Commerce –

Electronic date Interchange – Electronic payments – E-Journals – Search engines.

Unit – V (6 hrs)

5.1 Fundamentals of C – User friendly language – Character set – Keyword and

Identifiers – Primary data types – Constants – Variables and simple operators.

5.2 Simple C-Programming – Basic Structure of C-Programming – Conversion of

temperature from Kelvin to Celsius – Determination of molecular weight of

simple compounds – Calculation of rate constant using first order rate equation –

Calculation of root mean square velocity of the simple system.

Reference:

1. Kishor Arora –“Computer Application in Chemistry” -1st Edition – Anmol

Publications Pvt. Ltd.

2. Andrews Tenenbaum – “Computer Networks” – 4th Edition – Prentice-Hall of

India Pvt.Ltd – New Delhi -110 001.

3. E. Balagurusamy – “Programming in ANSI C” 3rd Edition – Tata McGraw-Hill-

New Delhi.

Semester – IV08UCH4602

PART - IV NON MAJOR ELECTIVE-II

FOOD AND NUTRITIONAL SCIENCE

Unit – I (6 hrs)

1.1 Food Definition – Nutritional classification of foods – Energy yielding – Body

building and protective foods – Functions – Nutrients – Types of nutrients –

Proteins, Carbohydrates, Fats, Minerals and Vitamins – Importance of nutrients –

Balanced diet( Definition only).

1.2 Nutritive Value of foods – Cereals, Wheat, rice,milk, meat, fish, egg, vegetables

and fruits.

Unit – II (6 hrs)

2.1 Minerals – Dietary sources, functions, effects of deficiency and requirements of

calcium, phosphorous, iron, fluorine, sodium and potassium.

2.2 Vitamins – Classification – vitamins – A, D, E, K, B6, B12, and C -Dietary sources,

physiological functions, effects of deficiency and daily requirements.


3.1 Meal planning for various age groups – Importance of meal planning –Importance

of mother’s milk – Balanced diets for school children and adolescents – Nutrition

of Pregnant and lactating women.

3.2 Diet during fever, dysentery, anemia, blood pressure, obesity and diabetes.

3.3 Water distribution – Water balance – Water intake and loss.

Unit – IV (6 hrs)

4.1 Food preservation – Definition, Principle and importance – Food Spoilage –

Causes of food spoilage – Fermentation, rancidity, autolysis and putrefaction –

food poisoning.

4.2 Methods of food Preservation - Freezing, canning, pickling, salting, smoking,

bottling, sterilization, refrigeration, dehydration, heating, radiation and

preservative agents.

4.3 Food additives – Broad classification – Functions and Chemical contents -

Microwave cooking – Advantages and disadvantages..

Unit – V (6 hrs)

5.1 Food adulteration – Definition – Common adulteration in food and their ill effects

– Intentional and incidental adulterants – Packing hazards.

5.2 Practical rules for good sanitation of food – food laws and standards – Bureau of

Indian standards – AGMARK – Consumer Protection act.

5.3 Evaluation of food quality – Sensory evaluation – Sensory characteristics of food

appearance, colour, odour and taste – Physical and chemical tests for detection of

food adulterants.

Reference:

1. Dr.M. Swaminathan –“Handbook of food and Nutrition” 5th edition (2005),

Bangalore printing, Bangalore -560018.

2. B. Srilaksmi – “Food Science” – 3rd edition, (2005) New Age international (P)

Ltd. – New Delhi.

3. B. Srilaksmi – “Nutrition Science” -1st edition, New Age International (P) Ltd.

New Delhi.

4. Jayashree Ghose – “Fundamental concepts of applied chemistry” – 1st edition

(2006) S. Chand and Company (P) Ltd. –New Delhi.

5. Norman N. Potter and H. Hotchkiss – “Food science” -5th edition, (2005) –CBS

Publishers – New Delhi – 110002.

Semester – V 08UCH5407

PART – IIICORE-VII

ANALYTICAL CHEMISTRY -I

Unit – I (9 hrs)

1.1 Laboratory hygiene and safety storage and handling of chemicals:

Handling of ethers, Toxic and poisonous chemicals, general precaution for

avoiding accidents, first aid techniques – acid, alkali on clothing, Burns in the

eyes, inhalation of toxic vapors, cuts from strong acids, alkalis, bromine, phenol.

Treatment for specific poisons – Acids, alkalis, methyl alcohol, arsenic

compounds, cyanides, universal antidote.

1.2 Data Analysis: The mean – median , precision, accuracy errors – Determinate

errors, indeterminate errors, minimization of errors, rejection of data-significant

figures, standard deviation.

Unit – II (9 hrs)

2.1 Volumetric Analysis: Terminology – Standard solution, titration, equivalence

point, end point, indicator. Basic requirements of a titration reaction, primary

standards, expressing concentrations of standard solutions - Normality, molarity.

2.2 Volumetric Titrations: Acid base titrations – Strong acid Vs weak base. Theory

of acid base indicators, Redox titrations – Mohr salt Vs KMnO4, oxalic acid Vs

KMnO4, FeSO4 Vs K2Cr2O7, complexometric titrations – EDTA titrations.


3.1 Gravimetric Analysis: Precipitation – Mechanism of precipitation, desirable

properties of gravimetric precipitates – Large particle size – Factors affecting the

particle size. Low solubility – Factors affecting the solubility of precipitates –

Co-precipitation – Post precipitation, digestion of the precipitate, filtration and

washing – Drying and ignition, desiccants, vacuum drying.

3.2 Principles in qualitative analysis: Common ion effect, application in qualitative

analysis, solubility, solubility product, application in qualitative analysis,

complexation reactions in qualitative analysis.

Unit – IV (9 hrs)

4.1 Purification Techniques: Principles and techniques of distillation, fractional

distillation – stream distillation and azeotropic distillation – Recrystallisation –

steps in recrystallization, solvent for recrystallisation, hot filtration, removal of

colouring matter during recrystallisation, precautions, sublimation, technique of

sublimation – Advantages of sublimation.

4.2 Criteria and tests for purity: Melting point – Definiton, Isomerisation and melting

point, determination of melting point. Boiling point definition, determination of

boiling point, precautions in determining boiling point.

Unit – V (9 hrs)

5.1 Organic estimations: Estimation of amines – Bromination method, Estimation of

phenols – Bromination method, Estimation of Ketones – Iodination method,

Estimation of Glugose – Bertrand’s method, Estimation of Ascorbic acid –

Estimation of oil and fats.

5.2 Determination of the Iodine value of an oil, Saponification value of an oil, Richert

value, RM value, Acetyl value.

Reference:

1. R.Gopalan, P.S.Subramanian, K. Rangarajan –“Elements of Analytical

Chemistry”. 1st Edition . Sultan Chand & Sons (Unit I,II, III,IV, V)

2. Puri, Shrama, Kalia – “ Principles of Inorganic Cgemistry”. Shoban Lal,

Nagin Chand & Co.,

3. U.N. Dash – “Analytical Chemistry theory and Practice”

Sultan Chand &Sons(2005)


PART –IIICORE - VIII

INORGANIC CHEMISTRY -I

Unit – I (15 hrs)

1.1 Ligands – Classification, polydendate upto hexadentate, symmetrical and

unsymmertrical ligands.

1.2 IUPAC nomenclature – Naming of complexes with all types of ligands – Bridging

– Ambidentate ligands.

1.3 Isomerism in coordination compounds – Stereoisomerism – Geometrical and

optical isomerism in 4 and 6 coordination compounds – Distinction between cis

and trans-isomers.

1.4 Application of coordination complex in qualitative and quantitative analysis –

Detection of K+ ions – Separation of Cu2+ and Cd2+ ions – Estimation of Ni2+ ions

using DMG and Al3+ using oxine, structure of EDTA and it complexes –

Applications.


2.1 Theories of coordination – Werner’s, Sidgwick and Pauling theory as applied to

Oh, Td and sq.pl. complexes. Limitations of Pauling theory, crystal field theory –

splitting of d- orbitals in Oh, Td and sq.pl. complexes – CFSE of weak, strong

fields – Factors affecting 10 Dq – measurement of 10 Dq. Applications of CFT.

2.2 Molecular orbital theory applied to octahedral complexes.


3.1 Chelates – Characteristics – Classification – Factors influencing the stability of

metal chelates – Detection of Chelates.

3.2 Stability of complexes in aqueous solution – Stability and instability constants –

Labile and inert complexes – Thermodynamic and kinetic stability.

3.3 SN1 and SN2 Reactions in Oh complexes – Acid hydrolysis – substitution reaction

in sq.pl.complexes.

3.4 Trans effect and its applications.


4.1 Metal carbonyls – Mono and polynuclear carbonyls of Ni, Fe, Cr, Co and Mn –

Preparation and properties – Application of EAN rules.

4.2 Nitrosyls – Classification, preparation and properties. Sodium nitroprusside –

Preparation, properties and structure.

4.3 Biologically important coordination compounds. Chlorophyll, hemoglobin,

Vitamin B12 - Structure, function and application.

Unit – V (15 hrs)

5.1 Clathrates - Quinol – Nobel gas and hydrates – Characteristics and structure.

5.2 Non-aqueous solvents – NH3, HF3, CH3COOH, SO2 – Properties and application.

Reference:

1. Cotton and Wilkinson - “Advanced Inorganic Chemistry” 5th edition, John Wiley

& Sons, New York.

2. R.D. Madan – “ Modern Inorganic Chemistry” (1987), S.Chand & Co Pvt Ltd.,

New Delhi

3. Gurdeep Chatwal and M.S. Yadav – “Coordination Chemistry” 1st edition,

Himalaya Publishing House.

4. James E. Huheey, EEllen A. Keier and Reichard L. Keiter, “Inorganic

Chenmistry” 4th edition., Addison – Wesley.


PART – IIICORE - IX

ORGANIC CHEMISTRY-I UNIT – I (15 hrs)

1. Carbonyl Compounds:

1.1 General methods of preparation of aliphatic and aromatic carbonyl compounds

carbonyl polarization – Reactivity of Carbonyl group – activity of alpha

hydrogen.

1.2 Mechanism of aldol, perkin, knoevenagal and Benzoin condensation, mechanisms

of Claisen, Reformatsky, Wittig and Cannizaro reactions

1.3 Mechanisms of reduction reaction: Clemmension, Rosenmund, Wolf-Kishner and

MPV reduction - Haloform reaction, Michael addition and Oppeanur oxidation.

UNIT – II (15 hrs)

2.1 Monocarboxylic acids and Dicarboxylic acids:

Acetic acid – preparation from acetylene – properties of acetic acids and uses.

Ionization of carboxylic acids – Acidity constant – Comparison of acid strengths

of substituted benzoic acids – Hammett equation.

2.2 Dicarboxylic acids – preparation and properties of oxalic, malonic, succinic,

glutaric and adipic acids.

2.3 Esters - Preparation – properties and synthetic applications of malonic,

acetoacetic esters -keto-enol tautomerism of acetoacetic esters .


3. Stereochemistry – I

3.1 Stereoisomerism – Definition – classification - optical and Geometrical

Optical isomerism:- Optical activity – conditions for optical activity.

Asymmetric centre – Chirality –- Elements of symmetry - Optical activity of

lactic and tartaric acids - Racemization – Resolution - Various methods of

resolving a racemic mixture – Asymmetric synthesis, Walden’s inversion.

3.2 R & S Notations – Cahn – Ingold – Prelog rules – Erythro and threo representations.

Fischer, Sawhorse and Newmann projection formulae of compounds containing

two asymmetric carbon atoms.

UNIT – IV (15 hrs)

4. Stereo Chemistry - II

4.1 Optical activity of compounds containing no asymmetric carbons –

Biphenyls, allenes and spiranes.

4.2 Geometrical Isomerism:- Cis-trans, syn – Anti and E – Z notations – Geometrical

isomerisms of maleic and Fumaric acids and unsymmetrical ketoximes – Methods

of determination of the configuration of geometrical isomers.

4.3 Conformation Analysis -Definition – conformation and configuration –

conformation of ethane and n-butane molecules and their stability. Conformations

of cyclohexane – energy profile diagrams.Conformation analysis of mono and

disubstituted cyclohexanes and methyl cyclohexanes and 1,2, 1,3 and 1,4-

dimethylcyclohexanes.

UNIT – V (15 hrs)

5.1 Heterocyclic compounds

Preparation, properties and uses of Furan, pyrrole, thiophene and pyridine

Comparative basic characters of pyrrole, pyridine and piperidine with alkyls

amines.Synthesis and reactions of Quinoline, Isoquinoline and Indole with special

reference to Skraup, and Fischer indole synthesis – Fischer Napieralski synthesis.

5.2 Polynuclear hydrocarbons: Naphthalene – anthracene and phenanthrene –

preparation – properties and uses.

References:

1. Dr. Jagadamba Singh – “Undergraduate Organic Chemistry” UGC

Curriculum Vol. I & Vol. II, Pragati Ed., (2007) – Pragati Prakashan, Meerut

2. M.K.Jain and S.C.Sharma, “Organic Chemistry for B.Sc students of Indian

universities” vishal Publications.

3. P.S. Kalsi – “Stereochemistry conformation and mechanism” – 6th Ed., (2005),

New Age International (P) Ltd., New Delhi.



5. Raj K. Bansal – “A Text Book of Organic Chemistry” – Revised 4th Ed.,

(2005) - New Age International Publishers, New Delhi.

6. I.L. Finar – “Stereochemistry and the Chemistry of Natural Products” – vol.

II, 5th Ed., (2006), Dorling Kindersley (India) Pvt. Ltd.


PART- IIIMAJOR BASED ELECTIVE - IPHYSICAL CHEMISTRY - I

UNIT – I (15 hrs)

1. First Law of Thermodynamics and Thermo Chemistry

1.1. Terms used in thermodynamics – Conservation of energy, internal energy, work and

heat, state function, path function, exact and inexact differentials, zeroth law of

thermodynamics, first law of thermodynamics- definition, heat capacity – Cp and

Cv. Joule-Thomson effect – definition, Joule Thomson co-efficient and inversion

temperature.

1.2. Calculation of ∆U, ∆H, q and w for ideal gases, calculation of ∆U, ∆H, q and w for

real gases - Reversible and irreversible isothermal expansion, reversible and

irreversible adiabatic expansion.


2. Second Law of Thermodynamics

2.1. Need for the law, spontaneous process, Carnot’s cycle, efficiency of Carnot’s

engine, Carnot’s theorem, thermodynamic scale of temperature, entropy - Concept

of entropy, entropy as a state function, entropy change in isothermal expansion of

ideal gas, entropy change in reversible and irreversible processes,

2.2. Entropy change accompanying change of phase – Solid to liquid, liquid to vapour

crystalline changes, isothermal, isochoric and isobaric processes, entropy of mixture

of ideal gases, entropy of mixing, physical significance of entropy.

2.3. Other state functions – Free energy, work functions, variation of G with T and P, Maxwell`s relations, Gibb’s– Helmholtz equation.

UNIT –III (15 hrs) 3. Phase Rule and Surface Chemistry

3.1. Phase Rule - Definition of the terms – Phase, components, degrees of freedom,

derivation of Gibbs`s phase rule, one component system – H2O, CO2, and Sulphur

systems, two components system – Simple eutectic system - Pb-Ag, freezing

mixture, compound formation with congruent melting points - FeCl3-H2O system,

compound formation with incongruent melting points - Na2SO4-H2O system.

3.2 Adsorptions on solids – Chemisorptions and physisorptons, potential energy

diagrams - Lannard–Jones plot, Langmuir, and BET adsorption isotherm –

Estimation of surface area, Adsorption from solution – Gibb’s adsorption isotherm.

UNIT – IV (15 hrs)4. Solutions of Non-Electrolytes 4.1. Solution of liquids in liquids – Definition, concentration units, Raoult’s Law and

Henry’s Law, ideal and non-ideal solutions, vapour pressure of ideal solution,

activity and activity coefficients component in an ideal and non-ideal solutions,

chemical potential of ideal and non-ideal solution – Gibbs-Duhem-Margules

equation, temperature dependence of vapour pressure.

4.2. Vapour pressure of non-ideal solution - deviations from Raoult’s law, vapour

pressure- composition and boiling point-composition curves, fractional distillation

of binary miscible liquids, azeotropic mixtures (HCl–H2O and ethanol–water

system).

4.3. Solubility of partially miscible liquids pairs – system with upper CST - Phenol–

Water, aniline–hexane, system with lower CST – Triethylamine-water and system

with upper and lower CSTs - Nicotine-water, effects of impurities on CST,

completely immiscible liquid pairs – Principle and application of steam distillation,

Nernst distribution law and its application to solvent extraction.

UNIT – V (15 hrs) 5. Properties of Dilute Solutions 5.1. Colligative properties – Definition, lowering of vapour pressure, relative lowering

of vapour pressure, determination of molecular weight from lowering of vapour

pressure, measurement of lowering of vapour pressure, osmosis and osmotic

pressure – Definitions, expression for calculating osmatic pressure, determination of

molecular weight from osmatic pressure, relation between osmatic pressure and

lowering of vapour pressure, experimental determination of osmatic pressure.

5.2. Elevation of boiling point – Definition, derivation of ebullioscopic constant,

determination of molecular weight from elevation of boiling point, elevation of

boiling point determination, depression of freezing point – definition, derivation of

cryoscopic constant, determination of molecular weight from depression of freezing

point, experimental determination, abnormal colligative property – Association,

dissociation and van’t Hoff factor, degree of dissociation.

References:

1. Kuriacose and Rajaram, Thermodynamics for students of chemistry, Shoban Lal Nagin

Chand & Co. Delhi – 7.

2. B.R. Puri, L.R. Sharma and M.S. Pathania – Principlles of Physical Chemistry, Vishal

Publications, Jalandhar.

3. N.Kundu and S.K.Jain, Physical Chemistry, S.Chand & Co. Ltd. New Delhi – 110 055.

4. Gurtu and Snehi, Advanced Physical Chemistry, Pragati Prakashan, Meerut-1.


PART- IIIMAJOR BASED ELECTIVE - IPHYSICAL CHEMISTRY - I

UNIT – I (15 hrs)

1. First Law of Thermodynamics and Thermo Chemistry

1.1. Terms used in thermodynamics – Conservation of energy, internal energy, work and

heat, state function, path function, exact and inexact differentials, zeroth law of

thermodynamics, first law of thermodynamics- definition, heat capacity – Cp and

Cv. Joule-Thomson effect – definition, Joule Thomson co-efficient and inversion

temperature.

1.3. Calculation of ∆U, ∆H, q and w for ideal gases, calculation of ∆U, ∆H, q and w for

real gases - Reversible and irreversible isothermal expansion, reversible and

irreversible adiabatic expansion.


2. Second Law of Thermodynamics

2.1. Need for the law, spontaneous process, Carnot’s cycle, efficiency of Carnot’s

engine, Carnot’s theorem, thermodynamic scale of temperature, entropy - Concept

of entropy, entropy as a state function, entropy change in isothermal expansion of

ideal gas, entropy change in reversible and irreversible processes,

2.2. Entropy change accompanying change of phase – Solid to liquid, liquid to vapour

crystalline changes, isothermal, isochoric and isobaric processes, entropy of mixture

of ideal gases, entropy of mixing, physical significance of entropy.

2.4. Other state functions – Free energy, work functions, variation of G with T and P, Maxwell`s relations, Gibb’s– Helmholtz equation.

UNIT –III (15 hrs) 3. Phase Rule and Surface Chemistry

3.1. Phase Rule - Definition of the terms – Phase, components, degrees of freedom,

derivation of Gibbs`s phase rule, one component system – H2O, CO2, and Sulphur

systems, two components system – Simple eutectic system - Pb-Ag, freezing

mixture, compound formation with congruent melting points - FeCl3-H2O system,

compound formation with incongruent melting points - Na2SO4-H2O system.

3.2 Adsorptions on solids – Chemisorptions and physisorptons, potential energy

diagrams - Lannard–Jones plot, Langmuir, and BET adsorption isotherm –

Estimation of surface area, Adsorption from solution – Gibb’s adsorption isotherm.

UNIT – IV (15 hrs)4. Solutions of Non-Electrolytes 4.1. Solution of liquids in liquids – Definition, concentration units, Raoult’s Law and

Henry’s Law, ideal and non-ideal solutions, vapour pressure of ideal solution,

activity and activity coefficients component in an ideal and non-ideal solutions,

chemical potential of ideal and non-ideal solution – Gibbs-Duhem-Margules

equation, temperature dependence of vapour pressure.

4.2. Vapour pressure of non-ideal solution - deviations from Raoult’s law, vapour

pressure- composition and boiling point-composition curves, fractional distillation

of binary miscible liquids, azeotropic mixtures (HCl–H2O and ethanol–water

system).

4.3. Solubility of partially miscible liquids pairs – system with upper CST - Phenol–

Water, aniline–hexane, system with lower CST – Triethylamine-water and system

with upper and lower CSTs - Nicotine-water, effects of impurities on CST,

completely immiscible liquid pairs – Principle and application of steam distillation,

Nernst distribution law and its application to solvent extraction.

UNIT – V (15 hrs) 5. Properties of Dilute Solutions 5.1. Colligative properties – Definition, lowering of vapour pressure, relative lowering

of vapour pressure, determination of molecular weight from lowering of vapour

pressure, measurement of lowering of vapour pressure, osmosis and osmotic

pressure – Definitions, expression for calculating osmatic pressure, determination of

molecular weight from osmatic pressure, relation between osmatic pressure and

lowering of vapour pressure, experimental determination of osmatic pressure.

5.2. Elevation of boiling point – Definition, derivation of ebullioscopic constant,

determination of molecular weight from elevation of boiling point, elevation of

boiling point determination, depression of freezing point – definition, derivation of

cryoscopic constant, determination of molecular weight from depression of freezing

point, experimental determination, abnormal colligative property – Association,

dissociation and van’t Hoff factor, degree of dissociation.

References:

1. Kuriacose and Rajaram, Thermodynamics for students of chemistry, Shoban Lal Nagin

Chand & Co. Delhi – 7.

2. B.R. Puri, L.R. Sharma and M.S. Pathania – Principlles of Physical Chemistry, Vishal





PART – IV

SKILL BASED ELECTIVE – IV

CHEMISTRY OF NATURAL PRODUCTS

Unit – I (6 hrs)

1. Terpenoids: Introduction – Isoprene rule, special isoprene rules, gem –

dialkyl rule - Classification, structural elucidation and synthesis of Myrcene, citral,

citronellal, geraniol, α – terpineol .

Unit – II (6 hrs)

2 Alkaloids: Introduction – Classification – General methods of isolation,

Hofmann exhaustive methylation, structural elucidation of coniine, nicotine

and piperine.


3. Carotenoids: Introduction – Classification, structural elucidation of β-

carotene, α- carotene, lycopene and xanthophylls.

Unit – IV (6 hrs)

4. Vitamins: Introduction, structural elucidation of vitamin A,B6 and C.

Unit – V (6 hrs)

5. Flavones: Introduction, properties, Isolation of flavones, structural

elucidation of flavone, Flavonol, Isoflavone.

Reference:

1. P.L. Soni, H.M. Chatwal “Textbook of Organic Chemistry” (1997),

S. Chand and Sons, New Delhi.

2. Gurdeep Chatwal “Organic Chemistry of natural products volume -1 and 2

(1986) Himalaya Publishing House.

3. I.L Finar “Organic Chemistry volume 1and 2, Stereochemistry and the

Chemistry of natural products” (2001) Pearson education Pte Hd, Delhi.

Semester – VI 08UCH6411

PART –IIICORE - XI

INORGANIC CHEMISTRY - II

Unit – I (15 hrs)

1. Metallurgy

1.1 Mineral wealth of India – Important minerals found in India (Magnetite, haematite, pyrolusite, bauxite, magnesite, dolomite, gypsum, ilmenite, monazite, pitch blende, mica, fluorspar, galena and kyanite). Minerals exported from and imported to India.

1.2 Concentration of ores and purification of metals

Froth floatation, magnetic separation, calcinations, smelting, aluminothermic process.

Electrolysis, zone refining, Van Arkel methods.


2. Tranition metals:

Group study of Ti group, V-group, Cr-group, Mn-group, Iron groups, Cu-group and Zn- group.


3. Metallurgy :

Minerals, Extraction, purification and refining of T, V, W and Mo – Uses.


4. Important compounds

Preparation, properties and uses TiO2, TiCl4, ZrO2, Zr(OH)4, ZrF4, V2O5, VF5, Tungstic acid. WO3, Ammonium molyddate and molybdenum blue.

Unit – V ( 15 hrs)

5. Lanthanides and Actinids

5.1 General study of lanthanides and actinides involving electronic configuration , oxidation states, magnetic properties and complexation behaviour.

5.2 Lanthanides Extraction, Extraction of Cerium, separation by ion exchage method – Lanthanide contraction and its effects.

Actinides – Extraction of thorium – Transuranic elements from manosite sand Uranium – Actinide contraction and its causes.

Reference:

1. R.D Madan – “Modern Inorganic Chemistry” (1987), S. Chand & Co Pvt Ltd.

2. Arnikar – “ Nuclear Chemistry”

3. B.R. Puri & L.R. Sharma – “Principles of Inorganic Chemistry” , Shoban Lal, Nagin Chand &Co., New Delhi (2000).

4. P.L. Soni – “ Text book of Inorganic Chemistry. S. Chand & Co ., New Delhi (1999).

Semester VI 08UCH6413

PART – III

CORE-XIII

Applied ChemistryUnit – I

(9 Hrs)1.1 CERAMICS

Introduction Subdivision of Ceramics Classification based on reduction on

porosity- Basic raw materials Other Ingredients Grinding of raw Materials Mixing of

Bodies-Firing-Knealing Throwing Jollying-Slit Casting- Passing- Drying.

1.2 REFRACTORIES:

Definition –classification,properties of refractories-manufacture of

refractories, fire clay bricks manufacture, uses of fire clay refractories.

UNIT-II (9 Hrs)

2.1 GLASS

Introduction-Physical and chemical properties, Raw materials-methods of

manufacture-some special glasses fused silica glass, high silica glass,optical glass,

borosilicate glass, lead glasses, soda lime glass, coloured glass, safety glass, fibre glass.

2.2 PULP AND PAPER

Introduction manufacture of pulp mechanical process chemical

process sulphate pulp, soda pulp, sulphite pulp, rag pulp, Beating,Refining,filling,

sizingand colouring, manufacture of paper.

UNIT-III (9 Hrs)

3.1 DYES:

Colour sensation-Dyes-colour and constitution classification of dyes according to

application-according to chemical structure –nitro and nitroso dyes-Triphenyl

methylene dyes Malachite green, crystal violet,Azo dyes-Aniline yellow, methyl

orange-phthaleins-Phenolphthalein, fluorescein-preparation properties and uses.

UNIT-IV

(9 Hrs)

4.1) BATTERIES:

Fundamentals of Batteries, Classification of Batteries, Sizes of Batteries,

Primary Batteries- The Le’clanche dry cell Alkaline MnO2 Batteries- The Magnesium

dry cell Secondary Batteries- The lead acid battery- Alkaline Strong Batteries- Edison

Cell.

4.1 POLYMER PROCESSING

Plastic (Thermo and thermosetting),compounding,plasticizers.colorants, flame

retardants.

UNIT-V (9 Hrs)

5. CATALYSIS:

5.1 Catalysis – Types-Importance of catalysis, types of catalysis - Homogeneous and

heterogeneous catalysis (Industrial catalyst – catalyst carrier, catalyst promoter,

catalyst inhibitor, catalytic poison, activity of catalyst). Theories of catalysis -

Intermediate complex theory and adsorption theory,Acid-base catalysis, Enzyme

catalysis - Mechanism of Enzyme catalysis, Michaelis-Menton law, influence of

substrate concentration, pH and temperature.

5.2 Magnetic properties of matter:

Magnetic flux, magnetic susceptibility, dia, para, ferro, antiferro magnetism.

Determination of magnetic susceptibility by Guoy balance method. Applications

to structural problems.

References:

1. J.C. Kuriacose, J.Rajaram-“Chemistry in Engineering and Technology- Vol-2.

2. B.K.Sharma- “Industrial Chemistry”,1st Ed., (1984),Goel Publishing House-

Meerut.

3. Jain &Jain –“Engineering Chemistry”, 15th Ed.,(2005), Dhanpath Rai

Publishing Company, New Delhi.



Semester VI 08UCH6502

PART-IIIMAJOR BASED ELECTIVE - II

ORGANIC CHEMISTRY – II

UNIT - I (15 Hrs)

1.1 Phenols and Naphthols: Nomenclature – preparation of phenols, properties

and acidic character – comparative acidic strengths of alcohols and phenols –

resonance stabilization of phenoxide ion.

1.2 Reactions of phenols – Esterfication, Nitration, Sulphonation, Halogenation,

Benzylation, Acylation, coupling reaction, Kolbe reaction, Gatterman reaction,

Hauben-Hoesch reaction and Reimer-Tiemann reactions.

1.3 Dihydric Phenols and Naphthols:

Catechol – resorcinol and quinol - preparation and reactions. Preparation –

properties – electrophilic substitution reactions of and - Naphthols.

UNIT – II (15 Hrs)

2. Nitro Compounds and amines

2.1 Preparation of Nitro benzene – Reduction of Nitro benzene in neutral, acidic and

alkaline media - TNT.

2.2 Amines: Relative basic characters of aliphatic and aromatic amines. – Ring

substitution in aromatic amines – separation of amines by Hinsburg and Hofmann

methods - diazotization and its mechanism - synthetic applications of benzene

diazonium salts and diazomethane – diazoacetic esters. .

2.3 Phenylene diamines – Preparation - sulphanilic acid, sulphanilamide, saccharin,

chloramines-T and uses.

UNIT – III (15 Hrs)

3. Amino Acids and Proteins:-

3.1 Classification of amino acids – definition of Essential and non–essential amino

acids. Preparation and properties of glycine and alanine. Zwitter ions, isoelectric

points, polypeptides, End group analysis by Sanger’s method.

3.2 Proteins – classification based on physical and chemical properties and on

physiological functions. Primary and secondary and tertiary structures of proteins.

Denaturation of proteins.

3.3 Nuclei acids: Sturctures of Nucleobases like adenine, guanine, thymine, uracil

and cytosine – nucleosides and nucleotides –polynucleosides – types of nucleic

acids – DNA and RNA biological functions.

UNIT – IV (15 Hrs)

4. Molecular rearrangement

Pinacole – Pinacolone rearrangement - migratory aptitude. Beckmann, Benzidine,

Hofmann, Curtius, Benzilic acid rearrangement (Sigmatropic rearrangement)

Claisen, para- Claisen , Fries rearrangement, Cope rearrangement and dienone –

phenol rearrangemnts.

UNIT – V (15 Hrs)

5. Carbohydrates:-

5.1 Classification, structural elucidation of glucose and fructose, Reactions of

glucose and fructose - osazone formation - mutarotaion and its mechanism -

cyclic structure – and determination of ring size - configuration of

monosaccharides. Epimerisation, Ascending and descending of aldoses and

ketones. Inter conversion of aldoses and ketoses

5.2 Disaccharides – reactions and structural elucidation of maltose and sucrose

polysaccharides starch and cellulose-manufacture,reactions, uses and structure.

[structural elucidation not necessary].

References:

1. A.K. Srivastava – “Organic Chemistry” – 1st Ed.,(2002) – New Age International Publishers, New Delhi.

2. Morrison and Boyd – “Organic Chemistry” – 6th Ed., (1998) – Prentice_Hall of India Pvt. Ltd., New Delhi.

3. Bahl and Arun Bahl – “Advanced Organic Chemistry” – 19th Ed., (2005) – Sulthan and Chand company, New Delhi.

4. Gurdeep Chatwal – “Organic Chemistry of Natural Products” – Vol. – I & Vol. II, Revised fifth ed., (2005) – Himalaya Publishing House.

5. O.P. Agarwal – “Reactions and Reagents in Organic Chemistry” – 5th Ed., (2005) – Goel Publishing House, Meerut.

6. Raj K. Bansal – “A Text Book of Organic Chemistry” – Revised 4th Ed., (2005) - New Age International Publishers, New Delhi.


PART-III

MAJOR BASED ELECTIVE - III

PHYSICAL CHEMISTRY - II UNIT – I (15 hrs)

1. Atomic Structure, Quantum Theory and Spectroscopy

1.1. de-Broglie theory of matter, experimental proof, Heisenberg`s uncertainty

principle, derivation of Schrodinger wave Equation, significance of and 2.

1.2. Electromagnetic radiations – Definition, regions of electro magnetic radiations,

quantization of energies in molecules - Translational, rotational, vibration, and

electronic energies, molecular spectra - origin of molecular spectra - Interaction

of electro-magnetic radiations with molecules.

1.3 UV visible spectroscopy – Theory of electronic spectroscopy, Frank – Condon

Principle, types of electronic transitions – Dissociation and predissociation spectra

– Application to geometrical isomerism.


2. Absorption Molecular Spectroscopy

2.1. Microwave spectroscopy - Molecular rotation, theory of microwave spectroscopy,

selection rule, effect of isotopic substitution and calculation of moment of inertia

and bond length of diatomic molecules.

2.2. Infrared spectroscopy - Molecular vibration – Modes of vibration of diatomic, tri-

atomic linear(CO2) and non linear (H2O) molecules - Stretching and bending

vibrations, selection rules, expression for vibration frequency, calculation of force

constant, factors influencing IR stretching frequency - Hydrogen bonding,

applications (important functional group identification – OH, C=O, Ar-H, NH)

and finger print region.

2.3. Raman spectroscopy – Raman effect, Rayleigh and Raman scattering – Stokes

and anti-stokes lines - Vibration Raman spectra – Modes of vibrations and

change in polarisibility of H2O and CO2, mutual exclusion principle, comparison

between Raman and IR spectroscopy, applications to covalent compounds – H2O.


3. Electronic and Resonance Spectra

3.1. NMR spectroscopy - Magnetic and non–magnetic nuclei, principle of nuclear

magnetic resonance- shielding mechanism, chemical shift, factors affecting

chemical shifts (electro negativity and anisotropic effect) number of signals –

Proton counting - Spin-spin coupling, coupling constant, NMR spectrum of ethyl

alcohol .

3.2. ESR spectroscopy - theory of ESR spectra, hyperfine splitting, ESR spectra of

methyl, benzene anion and naphthalene anion radicals.

3.3. Mass spectroscopy- Basic principle, molecular ion peak, base peak, isotopic and

meta stable peaks, nitrogen rule and mass spectra of toluene and branched

alkanes.

UNIT – IV (15 hrs)

4. Electrolytic Conductance and Transference:

4.1. Ionic mobility – Definition, experimental determination, experimental proof for

migration of ions, transport number – Definition, Hittrof`s rule, experimental

determination - Hittorf’s method, moving boundary method, effect of

concentration on transport number.

4.2. Transport of ions in solution – Debye-Huckel-Onsager (DHO) theory –

assumption and mathematical form - Validity of DHO equation, draw backs of

DHO equation, Extension of Deybe-Huckel-Onsager theory to strong electrolytes.

conductometric titrations – Acid-base titrations, precipitation titrations,

advantages of conductometric titrations.

4.3. Activity of ions in solutions – Mean ionic activity and activity coefficient, ionic

strength, Deybe-Huckel limiting law of activity coefficient, activity coefficient at

higher Concentration – Bjerrum model.

UNIT – V (15 hrs)

5. Electromotive Force of Galvanic Cells 5.1. Galvanic cell – Definition, chemical cell, concentration cell, reversible cell and

irreversible cell, types of reversible electrodes – Metal-metal ion electrodes,

amalgam electrodes, gas electrodes, metal-insoluble metal salt electrode and

oxidation-reduction electrode, single electrode potential.

5.2. E.M.F. of galvanic cell and cell reaction – Cell e.m.f., sign conventions of cell

e.m.f. and cell reaction, Nernst equation for cell e.m.f., reference electrode –

Primary and secondary reference electrode, standard electrode potential and its

determination, electro chemical series, standard cell,

5.3. Thermodynamics of galvanic cells – Relation between E.M.F. and G, H, S

and equilibrium constant(K), concentration cells – Electrode concentration cells –

Amalgam and gas concentration cells, electrolyte concentration cells -

Concentration cells without transference and its e.m.f., concentration cells with

transference and its e.m.f., liquid junction potential.

References:

1. C.N. Banwell, Fundamentals of Molecular Spectroscopy, 4th Edition, Tata McGraw-

Hill Publishing Company Ltd.

2. Manas Chanda, Structure and Chemical bonding including molecular spectra, Tata Mc

Graw-Hill Publishing company Ltd., New Delhi-2.

2. B.R. Puri, L.R. Sharma and M.S. Pathania, Principles of Physical Chemistry, Vishal





PART-IVSKILL BASED ELECTIVE - V

CHEMISTRY IN EVERY DAY LIFE

Unit – I (6 hrs)

Perfumes composition of perfume – Perfumery materials from animal and plants –

Synthetic perfumery materials – Face creams, hand lotions and creams, shampoos,

naillacquars, shaving cream – Composition and preparation. Hazards of cosmetics.

Unit – II (6 hrs)

Toilet soaps, detergents, Hair oils, Hair dyes – Composition and preparation Lipsticks –

Composition, Preparation and uses. Water quality parameters – Hard water – Types of

hardness, removal of hardness.


Fuels for home – Requirements of a good fuels – Classification – LPG gas- Health

hazards – Fire prevention and protection in house. Fire extinguisher for home and

chemical fire extinguishers.

Unit – IV (6 hrs)

Paints and pigments, varnishes – Definition and examples Dye – Classification –

Definition colour and constitution. Leather manufacture – Chrome tanning and vegetable

tannings.

Unit – V (6 hrs)

Polymers – Definition – Classification. Plastics - Types of plastics – Polythene – PVC –

Teflon – preparation , properties and uses- Health hazards of plastics Rubber – Origin

and chemical nature – Vulcanized rubbers. Synthetic rubbers – Styrene butadiene rubber

(SBR) and Butyl Rubbers.

Reference :

1. Industrial chemistry by B.K. Sharma, Goel Publishing house 1995.

2. A textbook of applied Chemistry by Thangammal Jacob, Mecmillan

company Ind Ltd 1979.

3. Fundamental concept of applied chemistry by Jayashree Ghosh. 1st

Edition (2006) S. Chand Company Ltd – New Delhi.

Semester – VI 08UCH6706PART – IV

SKILL BASED ELECTIVE - VIANALYTICAL CHEMISTRY –II

Unit – I (6 hrs)

1.1 Themogravimetric analysis (TGA) – Principles – Automatic

Thermogravimetric analysis – Factors effecting TGA – Applications –

Thermometric titrations – Differencial Thermal Analysis – Simultaneous

TGA – DTA curves.

1.2 Analytical Electrochemistry – Redox potential measurement and

applications – Interpretation of chemical behavior – Electrolytic separation.

Unit – II (6 hrs)

2.1 Chromotography – Classification – Principles – adsorption, partition, ion

exchange

2.2 Paper Chromotography – Principle, Techniques and Applications. Thin

layer Chromotography – Principle, Techniques and Applications.


3. Column Chromotography – Principle, Techniques and Applications. Ion

exchange Chromotography – Principle, Techniques and Applications.

Unit – IV (6 hrs)

4.1 Colorimetric Analysis – Laws of colorimetry – Estimation of Ni, Cu, and

Fe.

4.2 Electro gravimetry theory – Instrumentation applications – Spontaneous

(Internal) electrolysis – Coulometric analysis, coulometric titration –

Application –Potentiostatic coulometry.

Unit – V (6 hrs)

5.1 Polarography – Principles – Dropping mercury electrode – Experimental

assembly – Polarographic curves – Application of quantitative and

qualitative analysis – Concept of pulse polarography – Amperometric

titration – Principles and applications.

Reference:

4. R.Gopalan, P.S.Subramanian, K. Rangarajan –“Elements of Analytical

Chemistry”. 1st Edition . Sultan Chand & Sons (Unit I,II, III,IV, V)

5. Puri, Shrama, Kalia – “ Principles of Inorganic Cgemistry”. Shoban Lal,

Nagin Chand & Co.,

6. U.N. Dash – “Analytical Chemistry theory and Practice”

Sultan Chand &Sons(2005)

Semester –II 08UCH2302

ALLIED Paper II – INORGANIC, ORGANIC AND

PHYSICAL CHEMISTRY – II

Unit – I (15 hrs)

1.1. Coordination Chemistry

Nomenclature of mononuclear complexes – Werner, Sidgwick and Pauling’s

Theory. Biological role of Haemoglobin and Chlorophyll. Application of

complexes in qualitative and quantitative analysis.

1.2. Metallic BondElectron gas, Pauling and Band Theories. Semiconductors – Intrinsic, n and p-type.


2.1. Carbohydrates

Classification – Glucose and fructose – Preparation and properties – Sucrose –

Manufacture and properties – Starch and cellulose – Properties and uses.

2.2. Amino Acids and Proteins Amino acids – Classification, preparation and properties. Peptides (Elementary

treatment) – Proteins – Classification based on physical properties and biological

functions.


3.1. Synthetic polymers – Teflon, Alkyl and Epoxy resins, Polyesters – General

treatment only.

3.2. Types of polymerisation – Thermosetting and thermoplastics.

3.3. Heterocyclic compounds – Furan, thiophene, pyrrole and pyridine – Preparation and

properties.

3.4. Stereoisomerism – Optical isomerism – lactic and tartaric acid –

Racemic mixture and resolution – Geometrical isomerism – maleic and fumaric acid.


4.1. Surface Chemistry

Emulsions, Gels, preparation, properties and applications. Electrophoresis,

Chromatography – column, paper and thin layer chromatography.

4.2. Photochemistry

Laws of photochemistry and applications.

Unit – V (15 hrs)

5.1. Electrochemistry

Specific and equivalent conductance – their determination – Effect of dilution on

conductivities – An elementary idea about ionic theory – Ostwald’s Dilution Law,

Kohlrausch Law, Conductivity measurements.

5.2. pH and Buffer

Importance of pH and buffers in the living systems. pH determination by

colorimetric and electrometric methods.

References

1. R.D. Madan, J.S. Tiwari and G.L. Mudhara – A Textbook of First Year B.Sc.

Chemistry: S. Chand and Co.

2. B.R. Puri and L.R. Sharma – Principles of Inorganic Chemistry: Shoban Lal

Nagin Chand and Co., New Delhi (2000).

3. B.R. Puri, L.R. Sharma and S. Pathania – Principles of Physical Chemistry:

Shoban Lal Nagin Chand and Co., New Delhi.

`Semester –I 08UCH1401:P

Core – II Practical

Inorganic Qualitative Analysis – I

Analysis of Acid Radicals:

Analysis of any three Acid Radicals; (At least one must be interfering radical)

Oxalate, Phosphate, Borate, Fluoride, Sulphate, Bromide, Chloride, Nitrate, Arsenite, Sulphide, Carbonate, Arsenate.

Semester – II 08UCH2403:P

Core – II Practical

Inorganic Qualitative Analysis – II

Analysis of Basic Radicals:

Analysis any of the three Basic Radicals

Pb, Cu, Cd, Sn, Sb, Bi, Fe, Al, Mn, Ni, Zn, Co, Ca, Ba, Sr, Mg, NH4+

Semester – III 08UCH3405:P

Core – V

Volumetric Estimation Practicals

1. Estimation of Sodium Hydroxide(Na2CO3 X HCl X NaOH )

2. Estimation of Hydrochloric Acid(H2C2O4 X NaOH X HCl)

3. Estimation of Oxalic Acid(FeSO4 X KMnO4 X H2C2O4)

4. Estimation of Ferrous Sulphate(H2C2O4 X KMnO4 X FeSO4)

5. Estimation of KMnO4

(K2Cr2O7 X FAS X KMnO4)

6. Estimation of Ferric Ion (Internal Indicator)(K2Cr2O7 X Ferric Alum)

7. Estimation of Zn by EDTA(MgSO4 X EDTA X ZnSO4)

8. Estimation of Mg by EDTA

9. Estimation of Cu by iodometry(K2Cr2O7 X thio X CuSO4)

10. Estimation of Iodine (K2Cr2O7 X thio X I2)

Semester – IV 08UCH4406:P

Core – VI

Industrial Chemistry Practicals;

1. Estimation of total Hardness of Water

2. Estimation of Iodine value of an oil

3. Estimation of Saponification value of an oil

4. Estimation of acid value of an oil

5. Estimation of Vitamin C

6. Estimation of percentage purity of washing soda

7. Estimation of bleaching powder

8. Estimation of percentage of purity of Baking Soda

9. Estimation of antacid

Semester – V 08UCH5410:P

Core – X Practicals

Gravimetric Estimation Practical

Gravimetric Analysis

Sintered Crucible

1. Ni as Nickel dimethyl glyoxime

2. Zn as zinc Oxinate

3. Pb as Lead Chromate

4. Ba as Barium Chromate

5. Ca as Calcium oxalate monohydrate

Silica Crucible

1. Ca as Calcium Carbonate

2. Ca as Calcium Sulphate

3. Pb as Lead Sulphate

4. SO4 as Barium Sulphate

Semester – VI 08UCH6412:P

Core – XII

Organic Analysis and Presentation Practicals

Organic Analysis

Acids(Mono & Di Carboxylic acids), Phenols (Mono & Dihyrdric phenols) Aldehydes, Ketones, Esters Amines(Primary & Secondary), Amides(Mono & Di amides), Anilides Carbohydrates, Nitro Compounds

Preparations

1. Oxidation (benzaldehyde to benzoic acid)

2. Acetylation (aniline to acetanilide)

3. Bromination (phenol to 2,4,6- tribromophenol)

4. Nitration (nitrobenzene to 1,3- dinitrobenzene)

5. Hydrolysis (ethyl benzoate to benzoic acid)

6. Diazotization (aniline and beta naphthol coupling)

Determination of Melting point / Boiling point :

Semester – V 08UCH5407:P

Core – VIII Practical

Physical Chemistry Practical – I

1. Critical Solution temperature of Phenol Water System.

2. Determination of the strength of the electrolyte using Phenol-Water System.

3. Determination of Molecular Weight of the solute by Rast method.

4. Determination of Kf of the solvent by Rast method.

5. Ester Hydrolysis.(methyl acetate or ethyl acetate)

6. Transition temperature.

7. Phase Diagram.

8. Equilibrium constant of formation of KI3

9. Partition coefficient of iodine between carbontetrachloride and water

Semester – VI 08UCH6413:P

Core XIII Practical

Physical Chemistry Practical – II

1. Determination of equivalent conductance of strong electrolyte

2. Determination of strength of Strong acid by Conductometry

3. Determination of strength of a Strong base by Conductometry

4. Determination of strength of K2SO4 by Conductometry

5. Determination of strength of FeSO4 by Conductometry

6. Determination of strength of Strong acid by Potentiometry

7. Determination of strength of Strong base by Potentiometry

8. Determination of pH of a buffer Solution by Potentiometry

9. Estimation of FeSO4 by Potentiometry

Semester I 08UCH1301:P

Allied – I Practical

Allied Practical - I

Volumetric Analysis;

1.Estimation of Sodium Hydroxide(Na2CO3 X HCl X NaOH )

2.Estimation of Hydrochloric Acid(H2C2O4 X NaOH X HCl)

3.Estimation of Oxalic Acid(FeSO4 X KMnO4 X H2C2O4)

4.Estimation of Ferrous Sulphate(H2C2O4 X KMnO4 X FeSO4)

5.Estimation of KMnO4

(K2Cr2O7 X FAS X KMnO4)

6.Estimation of Zn by EDTA(MgSO4 X EDTA X ZnSO4)

7.Estimation of Mg by EDTA

8. Estimation of Cu by iodometry(K2Cr2O7 X thio X CuSO4)

9. Estimation of Iodine (K2Cr2O7 X thio X I2)

Semester II 08UCH2303:P

Allied III- Practical

Allied Practical II

ORGANIC ANALYSIS

A study of reactions of the following organic compounds.

1. carbohydrate

2. amide

3. aldehyde

4. ketone

5. monocarboxylic acid

6. Dicarboxylic acid

7. Amine

8. monohydric phenol

9. Dihydric phenol

10.Ester

11.Nitro

The students may be trained to perform the specific reaction like test for

element ( Nitrogen only ) , Aliphatic or aromatic , saturated or unsaturated

and functional group present and record their observation.

Documents

Semester – I - JMC || Home · Web viewMolecular orbital theory - Concept – Linear combination of atomic orbital – M.O diagram for N2, O2, CO, NO, HF molecules. Comparison of