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Semester – I
08UCH1301
ALLIED
Paper I – INORGANIC, ORGANIC AND
PHYSICAL CHEMISTRY
Unit – I
1.1
(6 hrs)
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
2.1
(6 hrs)
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
3.1
Halogen Containing Compounds
3.2
Important
chlorohydrocarbons
used
as
solvents
and
(Dichloromethane), Chloroform, Carbon tetrachloride, DDT, B.H.C.
Chemotheraphy
(6 hrs)
pesticides
Sulpha drugs – Sulpha pyridine, Sulpha –thiazole and sulpha diazine – Strutural
properties and uses. Antibiotics and penicillin – G and Chloromycetin formula
and uses.
Unit – IV
4.1
(6 hrs)
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
5.1
(6 hrs)
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 –III
CORE-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
3.1
(9 hrs)
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
4.1
(9 hrs)
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
08UCH1402
PART –III
CORE -II
NUCLEAR CHEMISTRY
Unit – I
1.1
(15 hrs)
Nuclear Chemistry introduction – Composition of nuclear and nuclear forcesMeson 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 energyHydrogen bomb,atom bomb- Advantages – Nuclear shell and liquid drop model.
– Nuclear power stations in India
Unit – III
(15 hrs)
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
4.1
(15 hrs)
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
5.1
(15 hrs)
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
08UCH1701
PART-IV
SKILL BASED ELECTIVE-I
INDUSTRIAL CHEMISTRY
Unit – I
1.1
(6 hrs)
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
2.1
(6 hrs)
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.
Unit – III
3.1
(6 hrs)
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
4.1
(6 hrs)
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
5.1
(6 hrs)
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
08UCH2303
ALLIED
Paper III - CHEMISTRY OF SOIL,WATER AND AIR
Unit – I
1.1
(6 hrs)
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
2.1
(6 hrs)
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.
Unit – III
3.1
(6 hrs)
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
4.1
(6 hrs)
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
5.1
(6 hrs)
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 –III
CORE -III
GENERAL CHEMISTRY – II
UNIT – I
1.1
(9 hrs)
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
2.1
(9 hrs)
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.
UNIT – III
3. 1
(9 hrs)
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
4.1
(9 hrs)
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
5.1
(9 hrs)
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.
6.
R.L. Madan, G.D. Tuli – “Simplified Course in Physical Chemistry”, (1999),
S.Chand & Co., New Delhi.
Semester –III
08UCH3404
PART –III
CORE-IV
GENERAL CHEMISTRY - III
Unit – I
1.1
(15 hrs)
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.
Unit – II
(15 hrs)
.
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
3.1
(15 hrs
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-knockingoctane number and cetane number-antiknocking reagents –Power alcohol.
Unit – IV
4.1
Acids and bases –
(15 hrs)
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 acidweak base.
Unit – V
5.1
(15 hrs)
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.
5. Bahl and Arun Bahl – “Advanced Organic Chemistry” – 19th Ed., (2005) –
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 – III
08UCH3602
PART-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
2.1
(6 hrs)
Hormones – Salient feature of hormones – Biological function of hormones
– Chemical nature.
2.2
Vasoprussin, Oxytocin, Thyroxin and Insulin – Biological functions only.
Unit – III
3.1
(6 hrs)
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
4.1
(6 hrs)
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
5.1
(6 hrs)
Psychopharmacology, antipsychotic drugs, anti anxiety drugs, anti
depresent drugs, sedatives and hypnotics.
Blood analysis – Blood urea – Bile pigment – Protein – Glucose.
5.2
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” 3rd
edition. S. Chand & Company Ltd. New Delhi.
9.
I.L. Finar “Organic Chemistry II” 5th edition. Dorling Kindersley Pvt
Ltd., New Delhi.
Semester –III
08UCH3702
PART – IV
SKILL BASED ELECTIVE-II
COMPUTER APPLICATIONS IN CHEMISTRY
Unit – I
1.1
(6 hrs)
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
2.1
(6 hrs)
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
3.1
(6 hrs)
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
4.1
(6 hrs)
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
5.1
(6 hrs)
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-HillNew Delhi.
Semester – IV
08UCH4602
PART - IV
NON MAJOR ELECTIVE-II
FOOD AND NUTRITIONAL SCIENCE
Unit – I
1.1
(6 hrs)
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
2.1
(6 hrs)
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.
Unit – III
3.1
(6 hrs)
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
4.1
(6 hrs)
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
5.1
(6 hrs)
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 – III
CORE-VII
ANALYTICAL CHEMISTRY -I
Unit – I
1.1
(9 hrs)
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
2.1
Volumetric Analysis:
(9 hrs)
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.
Unit – III
3.1
(9 hrs)
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
4.1
Purification Techniques:
(9 hrs)
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
5.1
(9 hrs)
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
Sultan Chand &Sons(2005)
Chemistry
theory
and
Practice”
Semester – V
08UCH5408
PART –III
CORE - VIII
INORGANIC CHEMISTRY -I
Unit – I
1.1
(15 hrs)
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.
Unit – II
2.1
(15 hrs)
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.
Unit – III
3.1
(15 hrs)
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.
Unit – IV
4.1
(15 hrs)
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.
Semester – V
08UCH5409
PART – III
CORE - 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
2.1
(15 hrs)
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 .
UNIT – III
(15 hrs)
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
4.
Stereo Chemistry - II
4.1
Optical
activity of
compounds
containing
(15 hrs)
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 1,4dimethylcyclohexanes.
UNIT – V
5.1
(15 hrs)
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.
4. Bahl and Arun Bahl – “Advanced Organic Chemistry” – 19th Ed., (2005) –
Sulthan and Chand company, 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.
Semester – V
08UCH5501
PART- III
MAJOR BASED ELECTIVE - I
PHYSICAL CHEMISTRY - I
UNIT – I
1.
(15 hrs)
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.
UNIT – II
2.
(15 hrs)
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.
3.
UNIT –III
Phase Rule and Surface Chemistry
(15 hrs)
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
4.
(15 hrs)
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
5.
(15 hrs)
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.
Semester – V
08UCH5501
PART- III
MAJOR BASED ELECTIVE - I
PHYSICAL CHEMISTRY - I
UNIT – I
1.
(15 hrs)
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.
UNIT – II
2.
(15 hrs)
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.
3.
UNIT –III
Phase Rule and Surface Chemistry
(15 hrs)
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
4.
(15 hrs)
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
5.
(15 hrs)
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.
Semester – V
08UCH5704
PART – IV
SKILL BASED ELECTIVE – IV
CHEMISTRY OF NATURAL PRODUCTS
Unit – I
1.
(6 hrs)
Terpenoids: Introduction – Isoprene rule, special isoprene rules, gem –
dialkyl rule - Classification, structural elucidation and synthesis of Myrcene, citral,
citronellal, geraniol, α – terpineol .
Unit – II
2
(6 hrs)
Alkaloids: Introduction – Classification – General methods of isolation,
Hofmann exhaustive methylation, structural elucidation of coniine, nicotine
and piperine.
Unit – III
3.
(6 hrs)
Carotenoids: Introduction – Classification, structural elucidation of βcarotene, α- carotene, lycopene and xanthophylls.
Unit – IV
4.
Vitamins: Introduction, structural elucidation of vitamin A,B6 and C.
Unit – V
5.
(6 hrs)
(6 hrs)
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 –III
CORE - 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.
Unit – II
2.
(15 hrs)
Tranition metals:
Group study of Ti group, V-group, Cr-group, Mn-group, Iron groups, Cu-group
and Zn- group.
Unit – III
3.
(15 hrs)
Metallurgy :
Minerals, Extraction, purification and refining of T, V, W and Mo – Uses.
Unit – IV
4.
(15 hrs)
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 Chemistry
Unit – 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 HouseMeerut.
3. Jain &Jain –“Engineering Chemistry”, 15th Ed.,(2005), Dhanpath Rai
Publishing Company, New Delhi.
4. B.S. Bahl., G.D. Tuli & Arun Bahl – “Essentials of Physical Chemistry”,
(1999), S.Chand & Co., New Delhi.
Semester VI
08UCH6502
PART-III
MAJOR BASED ELECTIVE - II
ORGANIC CHEMISTRY – II
UNIT - I
1.1
Phenols and Naphthols:
(15 Hrs)
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
4.
(15 Hrs)
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
5.
Carbohydrates:-
5.1
Classification, structural elucidation of glucose and fructose,
(15 Hrs)
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,
structure.[structural elucidation not necessary].
uses
and
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.
Semester – VI
08UCH6503
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.
UNIT – II
(15 hrs)
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, triatomic 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.
UNIT – III
(15 hrs)
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 McGrawHill 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
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.
Semester – VI
08UCH6705
PART-IV
SKILL 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.
Unit – III
(6 hrs)
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
08UCH6706
PART – IV
SKILL BASED ELECTIVE - VI
ANALYTICAL CHEMISTRY –II
Unit – I
1.1
Themogravimetric
analysis
(6 hrs)
(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
2.1
(6 hrs)
Chromotography – Classification – Principles – adsorption, partition, ion
exchange
2.2
Paper Chromotography – Principle, Techniques and Applications. Thin
layer Chromotography – Principle, Techniques and Applications.
Unit – III
3.
(6 hrs)
Column Chromotography – Principle, Techniques and Applications. Ion
exchange Chromotography – Principle, Techniques and Applications.
Unit – IV
4.1
(6 hrs)
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
5.1
(6 hrs)
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
Sultan Chand &Sons(2005)
Chemistry
theory
and
Practice”
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 Bond
Electron gas, Pauling and Band Theories. Semiconductors – Intrinsic, n and p-type.
Unit – II
(15 hrs)
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.
Unit – III
(15 hrs)
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.
–
Unit – IV
(15 hrs)
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.