DEPARTMENT OF CHEMISTRY Semester wise …drvskrishnagdc.edu.in/syllabus/chemistry_2014_15.pdfDEPARTMENT OF CHEMISTRY Semester wise syllabus & Model Question Papers With Effect from

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DEPARTMENT OF CHEMISTRY

Semester wise syllabus&

Model Question Papers

With Effect from 2014-15

Dr. V. S. KRISHNA GOVT.DEGREE (A)& P. G. COLLEGE

VISAKHAPATNAM- 13

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ALLOCATION OF CREDITS AT SUBJECT LEVEL -Draft Final Format

College: Dr.V.S.Krishna Govt. Degree College (A); Course: Science;

Subject: CHEMISTRY

S.No

Semester PaperNature

Paper Name Max.Mark

s

Hours Credits

1 1 Core-1 COURSE IInorganic & Organic Chemistry-I

100 4 03

2 2 Core-2 COURSE IIPhysical & General Chemistry -I

100 4 03

Practicals Semi Micro qualitative analysis 50 3 023 3 Core-3 COURSE III

Inorganic & Organic Chemistry-II100 4 03

4 4 Core-4 COURSE IVPhysical & General Chemistry-II

100 4 03

Practicals Volumetric and Gravimetricanalysis

50 3 02

5 5 Advanced-1 COURSE VAdvanced Inorganic, Organic &

Physical Chemistry-III

100 3 03

6 5 Advanced-2Elective-1

OrElective-2

COURSE VAMolecular Spectroscopy &

Catalysis-IVOr

COURSE VBDrugs, Formulations, Green

Chemistry & Material Science-IV

100 3 02

7 6 Applied-1 COURSE VIInorganic, Organic & PhysicalChemistry-III

100 3 02

8 6 Applied-2Elective-1

Or

Elective-2

COURSE VIASeparation Techniques, SpectroPhotometry & Natural Products-IV

OrCOURSE VIB

Pesticides, Macro molecules &Petro Chemicals-IV

100 3 02

Practicals Organic Chemistry Practicals-III 50 3 02Practicals Physical Chemistry Practicals-IV 50 3 02

Total 30

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CORE-I

B. Sc., Chemistry

Model Curriculum – Course -I structure

B. Sc., First year

Course -I(Inorganic & Organic Chemistry-I)

Semester –I 60 hrs (15 weeks)

MODULE- I (Inorganic Chemistry-I) 30 hrs (2h / w)

1. s- Block Elements 3 h

2. p-Block Elementrs 20 h

3. Organometallic Compounds 7 h

MODULE- II (Organic Chemistry-I) 30 hrs (2h / w)

1. Structural Theory in organic Chemistry 10 h

2. Acyclic Hydro carbons 8 h

3. Alycyclic Hydrocarbons 4 h

4. Benzene & Its reactivity 6 h

5. Poly Nuclear Hydrocarbons 2 h

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Dr. V.S. Krishna Govt. Degree College (A), VISAKHAPATNAMCOURSE-I

I B.Sc., Semester – I, Chemistry Syllabus for the Academic Year 2014 – 2015(Inorganic and Organic Chemistry - I)

(w. e. f. 2014 – 2015)

MODULE – I (Inorganic Chemistry – I)

1. s-block elements:General characteristics of groups I & II elements, diagonal relationship between Li & Mg, Be

& Al.

2. p-block elements:Group – 13: Synthesis and structure of diborane and higher boranes (B4H10 and B5H9),

Boron- Nitrogen compounds (B3N3H6 and BN)Group – 14: Preparation and applications of silanes and silicones, graphitic compounds.Group – 15: Preparation and reactions of hydrazine, hydroxylamine, phosphazenes.Group – 16: Classifications of oxides based on (i) Chemical behaviour and (ii) Oxygen content.Group – 17: Inter halogen compounds and pseudo halogens

3. Organometallic ChemistryDefinition and classification of organometallic compounds, nomenclature, preparationproperties, and applications of alkyls of 1, 2 and 13 group elements.

MODULE-II (Organic Chemistry-I)

1. Structural theory in Organic ChemistryTypes of bond fission and organic reagents (Electrophilic, Nucleophilic, and free radical

reagents including neutral molecules like H2O, NH3 & AlCl3). Bond polarization: Factorsinfluencing the polarization of covalent bonds, electro negativity – inductive effect. Application ofinductive effect (a) Basicity of amines (b) Acidity of carboxylic acides (c) Stability of carboniumions. Resonance or Mesomeric effect, application to (a) acidity of phenol, and (b) acidity ofcarboxylic acids. Hyper conjugation and its application to stability of carbonium ions, Free radicalsand alkenes, carbanions, carbenes and nitrenes.

Types of Organic reactions: Addition – electrophilic, nucleophilic and free radical.Substitution– electrophilic, nucleophilic and free radical. Elimination- Examples (mechanism notrequired).

2. Acyclic HydrocarbonsAlkanes– IUPAC Nomenclature of Hydrocarbons. Methods of preparation: Hydrogenation

of alkynes and alkenes, Wurtz reaction, Kolbe’s electrolysis, Corey- House reaction.Chemicalreactivity – inert nature, free radical substitution mechanism. Halogenation example-reactivity,selectivity and orientation.

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Alkenes – Preparation of alkenes (a) by dehydration of alcohols (b) by dehydrohalogenationof alkyl halides (c) by dehalogenation of 1, 2 dihalides (brief mechanism), Saytzev’s rule.Properties: Addition of hydrogen – heat of hydrogenation and stability of alkenes. Addition ofhalogen and its mechanism. Addition of HX, Markonikov’s rule, addition of H2O, HOX, H2SO4

with mechanism and addition of HBr in the presence of peroxide (anti – Markonikov’s addition ).Dienes – Types of dienes, reactions of conjugated dines – 1, 2 and 1, 4 addition of HBr to 1,3 –butadiene and Diel’s – Alder reaction.Alkynes – Preparation by dehydrohalogenation of dihalides, dehalogenation of tetrahalides,Properties; Acidity of acetylenic hydrogen (formation of Metal acedtylides). Preperation of higheracetylenes, Metal ammonia reductions Physical properties. Chemical reactivity – electrophilicaddition of X2, HX, H2O (Tautomerism).

3. Alicyclic hydrocarbons (Cycloalkanes)Nomenclature, Preparation by Freunds methods, heating dicarboxylic metal salts. Properties –

reactivity of cyclopropane and cyclobutane by comparing with alkanes, Stability of cycloalkanes –Baeyer’s strain theory, Sachse and Mohr predictions and Pitzer’s strain theory. Conformationalstructures of cyclobutane, cyclopentane, cyclohexane.

4. Benzene and its reactivityConcept of resonance, resonance energy.

Concept of aromaticity – aromaticity (definition), Huckel’s rule – application to Benzenoid(Benzene, Napthalene) and Non – Benzenoid compounds (cyclopropenyl cation, cyclopentadienylanion and tropylium cation)Reactions – General mechanism of electrophilic substitution, mechanism of nitration. FriedelCraft’s alkylation and acylation. Orientation of aromatic substitution – Definition of ortho, para andmeta directing groups. Ring activating and deactivating groups with examples (Electronicinterpretation of various groups like NO2 and Phenolic). Orientation of (i). Amino, methoxy andmethyl groups (ii). Carboxy, nitro, nitrile, carbonyl and Sulfonic acid groups. (iii). Halogens(Explanation by taking minimum of one example from each type).

5. Polynuclear HydrocarbonsStructure of naphthalene and anthracene (Molecular Orbital diagram and resonance energy)

Any two methods of preparation of naphthalene and reactivity. Reactivity towards electrophilicsubstitution. Nitration and sulfonation as examples.

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Guidelines to the Paper Setter: The syllabus I Semester consists of Inorganic &organic chemistry. The I Semester question paper consists of 3 sections.

In Section – A: consists of 5 very short answers questions in which 5 are to be answered eachquestion carries 2 marks. The examiner has to choose 2 question from organic & 3 questions fromInorganic partIn Section – B: consists of 8 short answer questions carries 5 marks out of which 5 are to beanswered. The examiner has to choose 4 questions from Inorganic & 4 questions from organic part.In section – C: 8 essay questions are to be set each question carrying 10 marks out of which 4questions are to be answered. The examiner has to set 4 eassy questions from Inorganic & 4questions from Organic chemistry.

The examiner is requested to set question in such a way that the entire syllabus is reflected inthe question paper set by him.

B. Sc., First YearCourse -I

(Inorganic & Organic Chemistry-I)Semester-I

BLUE PRINT

Sl. No Name of the chapter 2 marks 5 marks 10marks

Module-I (Inorganic Chemistry – I)1. s- Block Elements 1 1

2. p-Block ElementsGroup – 13 1

Group – 14 1 1

Group – 15 1

Group – 16 2

Group – 17 13. Organo Metallic Compounds 1 1

Module-II (Organic Chemistry-I)

1. Structural TheoryIn organic chemistry

1 1 1

2. Acyclic Hydrocarbons 1 1 1

3. Alicyclic Hydrocarbons 1 1

3. Benzene & Its reactivity 1

4. Poly Nuclear Hydrocarbons 1

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CHEMISTRYI B.Sc., Semester– I,

COURSE-I(Inorganic and Organic Chemistry - I)

Time: 3 Hours Model Paper Max. Mark: 75(w. e. f. 2014-15)

SECTION – A

Answer ALL questions. Each question carries 2 Marks. (5 X 2 = 10 Marks)

1. Write two synthetic applications of organo-lithium compounds?

2. Why berilium and magnesium do not give flame test?

3. Write any one method of preparation of phosphazene with equation?

4. What is Markonikov’s rule and give an example?

5. Write about Inductive effect?

SECTION – B

Write any FIVE questions. Each question carries 5 Marks. (5 X 5 = 25 Marks)

6. Discuss the diagonal relationship between Li & Mg?

7. Write any three methods of preparation of Hydrazine with equation?

8. What are carbides and write a brief note on ionic carbides?

9. What are Organo Metallic compounds. Write any three important reactions of Grignard reagent?

10. What is meant by Hyperconjugation. How does it explain the stability of carbonium ion?

11. Write a short note on (a) Inductive effect (b) Mesomeric effect.

12. Write any three important reactions of acetylene with equations.

13. Write a short note an ozonolysis.

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SECTION – C

Answer any FOUR questions. Each question carries 10 Marks. (4 X 10 = 40 Marks)

14. (a). What is Inorganic benzene? Discuss the structure and preparation of Inorganic Benzene.(b). Discuss the structure of diborane.

(OR)

Write any two methods of preparation of silicones, and discuss about any 4 applications of it.

15. What are Inter Halogen Compounds and discuss the structure of IF5 and IF7.

(OR)

Explain the classification of Oxides on the basis of oxygen content and chemical nature?

16. Write an essay about types of organic reactions. Explain them by giving suitable examples toeach reaction.

(OR)

What is meant by aromaticity and discuss the structure of Benzene.

17. What are cycloalkanes.Give two methods of preparation of cycloalkanes with equation andhow does Sachse- Mohr explain the stability of cycloalkanes.

(OR)

Write two methods of preparation and four chemical properties of alkanes?

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CORE-II

B.Sc., Chemistry

Model Curriculum-Course structureB.Sc., First year

COURSE-II(Physical & General Chemistry-I)

(w. e. f. 2014 – 2015)

Semester –II 60 hrs (15 weeks)

MODULE- III (Physical Chemistry-I) 30 hrs (2h / w)

1. Gaseous State 6 h

2. Liquid State 2 h

3. Salid State 10 h

4. Solutions 6 h

5. Colloids & Surface chemistry 6 h

MODULE- IV (General Chemistry-I) 30 hrs (2h / w)

1. Atomic Structure &Elementary Quantum Mechanics 8 h

2. Chemical Bonding 8 h

3. Streo Chemistry of Carbon compounds 10 h

4. General Principles of Inorganic & Qualitative Analysis 4 h

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Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13CORE - II

I B.Sc., SEMESTER- II, CHEMISTRY SYLLABUSCOURSE – II

(Physical & General Chemistry-I)(w. e. f. 2014 – 2015)

MODULE – III: (Physical Chemistry – I)

1 Gaseous stateCompression factors, deviation of real gases from ideal behavior. Van der Waal’s equation of state.Critical phenomena. The van der Waal’s equation and the critical state. Relationship betweencritical constants and van der Waal’s constants. The law of corresponding states and reducedequation of states. Joule Thomson effect. Liquefaction of gases: i) Linde’s method and ii) Claude’smethod.

2 Liquid stateIntermolecular forces, structure of liquids (qualitative description). Structural differences betweensolids, liquids and gases. Liquid crystals, the mesomorphic state. Classification of liquid crystalsinto Smectic and Nematic. Differences between liquid crystal and solid/liquid. Application of liquidcrystals as LCD devices.

3 Solid stateSymmetry in crystals. Law of constancy of interfacial angles. The law of rationality of indices. Thelaw of symmetry. Definition of lattice point, space lattice, MODULE cell. Bravis lattices andcrystal systems. X-ray diffraction and crystal structure. Bragg’s law. Defects in crystals.Stoichiometric and non-stoichiometric defects. Band theory of semoconductors. Extrinsic andintrinsic semiconductors, n- and p-type semiconductors and their applications in photoelectrochemical cells.

4 SolutionsLiquid-liquid - ideal solutions, Raoult’s law. Ideally dilute solutions, Henry’s law. Non-idealsolutions. Azeotropes-HCl-H2O, ethanol-water systems and fractional distillation. Partially miscibleliquids-phenol-water, trimethylamine-water, nicotine-water systems. Effect of impurity on consulatetemperature. Immiscible liquids and steam distillation.Nernst distribution law. Applications ofdistribution law.

5 Colloids and surface chemistryDefinition of colloids. Solids in liquids(sols), preparation, purification, properties -kinetic,optical,electrical. Stability of colloids, Hardy-Schulze law, protective colloid. Liquids inliquids (emulsions) preparation, properties, uses. Liquids in solids (gels) preparation, uses.Adsorption: Physical adsoption, chemisorption. Freundlich, Langmuir adsorption isotherms.Applications of adsorption

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MODULE – IV (General Chemistry-I)

1. Atomic Structure and elementary quantum mechanics:

Blackbody radiation, Planck’s radiation law, photoelectric effect, Compton effect, de Broglie’shypothesis, Heisenberg’s uncertainty principle. Postulates of quantum mechanics. Schrodingerwave equation and a particle in a box, energy levels, wave functions and probability densities.Schrodinger wave equation for H-atom. Separation of variables, Radial and angular functions,hydrogen like wave functions, quantum numbers and their importance.

2. Chemical Bonding:

Valence bond theory, hybridization, VB theory as applied to ClF3, BrF5, Ni(CO)4, XeF2. Dipolemoment – orientation of dipoles in an electric field, dipole moment, induced dipole moment, dipolemoment and structure of molecules. Molecular orbital theory – LCAO method, construction ofM.O. diagrams for homo-nuclear and hetero-nuclear diatomic molecules (N2, O2, HCl, CO andNO).

3. Stereochemistry of carbon compounds:Molecular representations- Wedge, Fischer, Newman and Saw-Horse formulae.Stereoisomerism,Stereoisomers: enantiomers, diastereomers- definition and examples.Conformational andconfigurational isomerism- definition. Conformational isomerism of ethane and n-butane.Enantiomers: Optical activity- wave nature of light, plane polarised light, interaction withmolecules, optical rotation and specific rotation. Chiral molecules- definition and criteria- absenceof plane, center, and Sn axis of symmetry- asymmetric and disymmetric molecules. Examples ofasymmetric molecules (Glyceraldehyde, Lactic acid, Alanine) and disymmetric molecules (trans -1,2-dichloro cyclopropane).Chiral centers: definition- molecules with similar chiral carbon (Tartaric acid), definition ofmesomers- molecules with dissimilar chiral carbons (2, 3-dibromopentane). Number of enantiomersand mesomers- calculation.

D, L and R, S configuration for asymmetric and disymmetric molecules. Cahn-Ingold-Prelog rules.Racemic mixture- racemisation and resolution techniques.Diastereomers: definition- geometrical isomerism with reference to alkenes- cis, trans and E, Z-configuration.

4. General Principles of Inorganic qualitative analysisSolubility product, common ion effect, characteristic reactions of anions, elimination of interferinganions, separation of cations into groups, group reagents, testing of cations

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Guidelines to the Paper Setter: The syllabus Semester II consists of Physical &General chemistry. The Semester II question paper consists of 3 sections.

In Section – A: consists of 5 very short answers questions in which 5 are to be answered eachquestion carries 2 marks. The examiner has to choose 3 questions from Physical & 2 questions fromGeneral chemistry partIn Section – B: consists of 8 short answer questions carries 5 marks out of which 5 are to beanswered. The examiner has to choose 4 questions from Physical & 4 questions from Generalchemistry part.In section – C: consists of 8 essay questions are to be set each question carrying 10 marks out ofwhich 4 questions are to be answered. The examiner has to set 4 eassy questions from Physical & 4questions from General chemistry.

The examiner is requested to set question in such a way that the entire syllabus is reflected inthe question paper set by him.

B. Sc., First YearCOURSE-II

(Physical & General Chemistry-I)Semester-II

BLUE PRINT


Module-III (Physical Chemistry-I)1. Gaseous state 1 1 1

2 Liquid state 13 Solid state 1 14 Solutions 1 1 15 Colloids and surface

chemistry1 1

Module-IV (General Chemistry-I)

1.Atomic Structure andelementary quantummechanics

1 1 1

2. Chemical Bonding 1 2

3. Stereochemistry of carboncompounds

1 1

4.General Principles ofInorganic qualitativeanalysis

1 1

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Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13CORE - II

I B.Sc., SECOND SEMESTER EXAMINATIONS

CHEMISTRYCOURSE – II

(Physical & General Chemistry-I)Time: 3 Hours MODEL PAPER Max. Marks: 75

(w. e. f. 2014 – 2015)

SECTION-A

Answer any FIVE questions. Each question carries TWO Marks. (5 X 2 = 10 Marks)

1. What are critical constants?

2. Define Unit cell and space lattice?

3. Define Henry’s Law and state the conditions under which Henry’s law is valid?

4. What is meant by radial probability?

5. Define solubility and common ion effect?

SECTION-B

Answer any FIVE questions. Each question carries FIVE Marks. (5 X 5 = 25 Marks)

6. Define and explain the law of corresponding states?

7. Write a short note on schottky and frenkel defects in solids?

8. What are protective colloids, explain? Give their uses?

9. What are liquid crystals? Write about their classification?

10. Write the Schrodinger’s wave equation and explain the significance of Ψ and Ψ2?

11. Discuss the structure of Ni (CO) 4 with the help of valance bond theory

12. Explain enantiomers and diastereomers with one example?

13. Write any two Applications of complexes in qualitative analysis?

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SECTION-C


14. Derive the vander wall’s equation of state for real gases? How does it explain the behaviour ofreal gases?

OrWhat is critical solution temperature? Explain the phenol-water system in terms of C.S.T.?

15. (a) Define semi conductors? How are they classified?(b) Write a detailed note on n-type and p-type semi conductors.

Or(a) Discuss Debroglies wave theory? Calculate debroglies wavelength, if the velocity ofelectron is 2.2X103cm/sec.

(b) State and explain Heisenberg’s uncertainity principle?

16. (a) Explain the paramagnetic behaviour of oxygen with the help of molecular orbital energyDiagram.

Or(b) Draw the molecular orbital energy diagram of carbon monoxide and explain its bond order?

17. (a) Write any two methods of preparations of colloids?(b) Explain Kinitic and Optical properties of colloids?

OrWhat is conformational isomerism? Draw and explain the various types of conformers of ethaneand n- butane?

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Dr. V.S. Krishna Govt. Degree College (A), VISAKHAPATNAM-13Chemistry Practical Examinations at the END OF I Year / Sem-II

Time: 3 Hours Max. Marks: 50

LABORATORY COURSE – I 90 hrs (3 h / w)

Practical PAPER – I (Inorganic Chemistry)

Qualitative Analysis and Inorganic preparations:

Analysis of mixtures containing two anions (one simple and one interfering) and two cations (ofdifferent groups) from the following:

Anions: Carbonate, sulfide, sulphate, chloride, bromide, iodide, acetate, nitrate, oxalate, tartrate,borate, phosphate, arsenate* and chromate*.

Cations: Lead, copper, bismuth, cadmium, tin, antimony, iron, aluminum, zinc, manganese, nickel,cobalt, calcium, strontium, barium, potassium and ammonium.

*not to be given for examination.

Preparations: Any three of the following inorganic preparations:

1) Ferrous ammonium sulphate2) Tetrammine copper (II) sulphate3) Potassium trisoxalato chromate4) Potash alum KAl(SO4)2. 12H2O5) Hexammine cobalt (III) chloride.

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CORE-III

B.Sc., Chemistry

Model Curriculum-Course structure

B.Sc., Second yearCOURSE-III

(Inorganic & Organic Chemistry-II)

Semester –III 60 hrs (15 weeks)

MODULE- I (Inorganic Chemistry-II) 30 hrs (2h / w)

1. Chemistry of d-Block Elements 9 h

2. Chemistry of f- Block Elements 8 h

3. Theories of Bonding in Metals 6 h

4. Metal Carbonyls & Related Compounds 7 h

MODULE- II (Organic Chemistry-II) 30 hrs (2h / w)

1. Halogen Compounds 4 h

2. Hydroxy Compounds 6 h

3. Carbonyl Compounds 12 h

4. Carboxylic acids & Derivatives 5 h

5. Active Methylene Compounds 3 h

________________________________________________________________

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Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13CORE - III

II B.Sc., 3rd – SEMESTER CHEMISTRY SYLLABUSCOURSE- III

(Inorganic and Organic Chemistry - II)(w. e. f. 2015 – 2016)

MODULE – I: (Inorganic Chemistry – II)

1. Chemistry of d – Block elements:Characteristics of d-block elements with special reference to electronic configuration, variablevalence, magnetic properties, catalytic properties and ability to form complexes. Study of Cutraid in respect of electronic configuration and reactivity of different oxidation states.

2. Chemistry of f-Block elements:Chemistry of lanthanides – electronic structure, oxidation states, lanthanide contraction,consequences of lanthanide contraction, magnetic properties, spectral properties and separation oflanthanides by ion exchange and solvent extraction methods. Chemistry of actinides– electronicconfiguration, oxidation states, actinide contraction, position of actinides in the periodic table,comparison with lanthanides in terms of magnetic properties, spectral properties and complexformation.

3. Theories of bonding in metals :Valence bond theory, Explanation of metallic properties and its limitations, Free electrontheory, thermal and electrical conductivity of metals, limitations, Band theory, formation ofbands, explanation of conductors, semiconductors and insulators.

4. Metal carbonyls and related compounds :EAN rule, classification of metal carbonyls, structures and shapes of metal carbonyls of Fe, Co andNi. Metal nitrosyls and ferrocene.

MODULE- II: (Organic Chemistry – II)

1. Halogen compounds:Nomenclature and classification of alkyl (into primary, secondary, tertiary), aryl, aralkyl, allyl,vinyl, benzyl halides. Chemical Reactivity, formation of RMgX .Nucleophilic aliphatic substitutionreaction- classification into SN1 and SN2. Energy profile diagram of SN1 and SN2 reactions.Stereochemistry of SN2 (Walden Inversion) SN1 (Racemisation). Explanation of both by taking theexample of optically active alkyl halide – 2bromobutane. Ease of hydrolysis – comparision of alkyl,benzyl, alkyl, vinyl and aryl halides

2. Hydroxy compoundsNomenclature and classification of hydroxy compounds. Alcohols: Preparation with hydroborationreaction, Grignard synthesis of alcohols. Phenols: Preparation i) from diazonium salt, ii) from arylsulphonates, iii) from cumene. Physical properties- Hydrogen bonding (intermolecular andintramolecular). Effect of hydrogen bonding on boiling point and solubilitiy in water.Chemical properties:

a. acidic nature of phenols.b. formation of alkoxides/phenoxides and their reaction with RX.

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c. oxidation of alcohols by CrO3, KMnO4.

d. special reaction of phenols: Bromination, Kolb-Schmidt reaction, Riemer-Tiemann reaction,Fries rearrangement, azocoupling.Identification of alcohols by oxidation with KMnO4, ceric ammonium nitrate, lucas reagentand phenols by reaction with FeCl3.Polyhydroxy compounds: Pinacol-Pinacolone rearrangement.

3. Carbonyl Compounds :Nomenclature of aliphatic and aromatic carbonyl compounds, structure of the carbonyl group.Synthesis of aldehydes from acid chlorides, synthesis of aldehydes and ketones using 1, 3-dithianes,synthesis of ketones from nitriles and from carboxylic acids.Base catalysed reactions: a) Aldol, b) Cannizzaro reaction, c) Perkin reaction, d) Benzoincondensation, e) Haloform reaction, f) Knoevenagel reaction.Oxidation of aldehydes- Baeyer-Villiger oxidation of ketones.Reduction: Clemmensen reduction, Wolf-Kishner reduction, MPV reduction, reduction with LiAlH4

and NaBH4.Analysis of aldehydes and ketones with a) 2,4-DNT test, b) Tollen’s test, c) Fehling test, d) Schifftest, e) Haloform test (with equation).

4. Carboxylic acids and Derivatives :Nomenclature, Classification and structure of carboxylic acids.Physical properties: Relative differences in the acidities of aromatic and aliphatic acids.Chemical properties: Reactions involving H, OH and COOH groups- salt formation, anhydrideformation, acid chloride formation, amide formation and esterification (mechanism). Degradation ofcarboxylic acids by Huns-Diecker reaction, decarboxylation by Schimdt reaction, Arndt-Eistertsynthesis, halogenation by Hell-Volhard- Zelinsky reaction.Derivatives of carboxylic acids: Reaction of acid chlorides, acid anhydrides, acid amides, esters(mechanism of the hydrolysis of esters by acids and bases).

5. Active methylene compounds:

Acetoacetic esters: preparation by Claisen condensation, keto-enol tautomerism. Acid hydrolysisand ketonic hydrolysis.Preparation of a) monocarboxylic acids.

b) dicarboxylic acids.Reaction with urea

Malonic ester: preparation from acetic acid.Synthetic applications: Preparation of

a) monocarboxylic acids (propionic acid and n-butyric acid).b) dicarboxylic acids (succinic acid and adipic acid).

c) α,ß-unsaturated carboxylic acids (crotonic acid).

Reaction with urea.

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Guidelines to the Paper Setter: II B.Sc., Chemistry Syllabi is devided into Two parts forSemester III and IV. Semester – III Syllabi consists of Inorganic and Organic Chemistry. Semester– III Syllabis consists of 3 Sections, Section – A, Section – B and Section – C.

In Section – A, Five Very Short Answer Questions are to be set. Choosing Two from Inorganicand Three from Organic. Five to be answered. Each question carries 2 Marks.In Section – B , Eight Short Answer Questions are to be set. Choosing Four from Inorganic and

Four from Organic. Out of which Five are to be answered. Each question carries 5 Marks.In Section – C, Eight Essay Questions are to be set. Choosing Four from Inorganic and Four from

Organic. Each question carries 10 Marks and Four are to be answered.

The examiner is requested to set question in such a way that the entire syllabus is reflected in thequestion paper set by him.

CORE-IIIB. Sc., Second Year

Semester-IIICOURSE-III

(Inorganic & Organic Chemistry-II)BLUE PRINT


Module-V (Inorganic Chemistry – II)

1.Chemistry of d – Blockelements

1 1

2 Chemistry of f-Blockelements

1 1 1

3 Theories of Bonding inmetals

1 1 1

4 Metal Carbonyls andrelated compounds

1 1

Module-VI (Organic Chemistry – II)

1. Halogen compounds 1 1

2. Hydroxy compounds 1 1 13. Carbonyl compounds 1 1 1

4.Carboxylic acids andderivatives

1

5.Active methylenecompounds

1 1

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Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13CORE - III

II B.Sc., THIRD SEMESTER - END EXAMINATIONSCHEMISTRY

(COURSE – III)(Inorganic & Organic Chemistry-II)

Time: 3 Hours MODEL PAPER Max. Marks: 75(w. e. f. 2015 – 2016)

S E C T I O N – A

Answer any FIVE questions. Each question carries 2 Marks. (5 X 2 = 10 Marks)

1. What is Lanthanide Contraction?

2. Write a short note on Conductors?

3. How do you prepare benzyl chloride from benzene?

4. Explain intermolecular and intramolecular hydrogen bonding with one example.

5. Explain wolf-kishner reduction?

S E C T I O N – B


6. Write a brief note on keto-enol tautomerism.

7. Write and explain the reaction mechanism of Benzoin condensation.

8. Write a brief note on Pinacol – Pinacolone rearrangement?

9. Write and explain Cannizaro reaction.

10. What are Metal Carbonyls? Discuss the structure of Nickel tetra carbonyl?

11. Write any five differences between Lanthanides and Actinides?

12. Explain the Catalytic properties of d-block elements.

13. State and explain Valance bond theory of bonding in metals.

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S E C T I O N – C


14. What are transition elements? Describe their variable oxidation states, Magnetic properties andcapacity of forming Complexes?

(OR)Explain the procedure involved in the separation of Lanthanides by Ion exchange and solvent

extraction methods?

15. Explain Band theory of metals?(OR)

What are metal carbonyls? Explain the classification of metal carbonyls?

16. Explain SN1 and SN2 reaction mechanisms with the help of energy profile diagrams?

(OR)Write a brief note on:

a) Acidic nature of phenol b) Riemer – Tiemann reaction c) Kolbe’s Reaction

17. How do you prepare Aceto acetic ester and write any three synthetic applications of it?(OR)

Explain the following: a) Aldol condensation b) Perkin reaction.

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CORE-IV

B.Sc., ChemistryModel Curriculum- Course structure

B.Sc., Second year, Semester –IVCOURSE-IV

(Physical & General Chemistry-II)

Semester –IV 60 hrs (15 weeks)

MODULE- III (Physical Chemistry-II) 30 hrs (2h / w)

1. Phase rule 5 h

2. Dilute Solutions 8 h

3. Electro Chemistry 17 h

MODULE- IV (General Chemistry-II) 30 hrs (2h / w)

1. Molecular Symmetry 5 h

2. Theory of Quantitative Analysis 8 h

3. Evaluation of Analytical Data 4 h

4. Introductory Treatment to

a) Peri cyclic reactions 5 h

b) Synthetic Stratagies 4 h

c) Asymmetric Synthesis 4 h

23

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13CORE - IV

II B.Sc., IV – SEMESTER CHEMISTRY SYLLABUS(COURSE - IV: Physical & General Chemistry - II)

(w. e. f. 2015– 2016)

MODULE - III (Physical chemistry – II)

1. Phase rule

Concept of phase, components, degree of freedom. Derivation of Gibbs phase rule. Phaseequilibrium of one component – water system. Phase equilibrium of two-component system,solid-liquid equilibrium. Simple eutectic diagram of Pb-Ag system, desilverisation of lead. Solidsolutions- compound with congruent melting point- (Mg-Zn) system, compound withincongruent melting point – NaCl- water system. Freezing Mixtures.

2. Dilute solutions

Colligative properties. Raoult’s law, relative lowering of vapour pressure, its relation tomolecular weight of non-volatile solute. Elevation of boiling point and depression of freezingpoint. Relation between molecular weight and elevation in boiling point and depression infreezing point. Experimental methods of determination. Osmosis, osmotic pressure,experimental determination. Theory of dilute solutions. Determination of molecular weight ofnon-volatile solute from osmotic pressure. Abnormal Colligative properties. Van’t Hoff factor,degree of dissociation and association.

3. Electrochemistry

Specific conductance, equivalent conductance, measurement of equivalent conductance.Variation of equivalent conductance with dilution. Migration of ions, Kohlrausch’s law.Arrhenius theory of electrolyte dissociation and its limitations. Ostwald’s dilution law. Debye-Huckel-Onsagar’s equation for strong electrolytes (elementary treatment only). Definition oftransport number. Application of conductivity measurements-determination of dissociationconstant (Ka) of an acid, determination of solubility product of sparingly soluble salt,conductometric titrations. Standard Hydrogen electrode, reference electrodes,

Electrode reactions, Nernst equation, single electrode potential, standard electrode potential,sign convention, electrochemical series and its significance. Reversible and irreversible cells,conventional representation of electrochemical cells. EMF of a cell and its measurements.Computation of cell EMF. Applications of EMF measurements.

MODULE IV (General chemistry-II)

1. Molecular symmetry

Concept of symmetry in chemistry-symmetry operations, symmetry elements. Rotational axis ofsymmetry and types of rotational axes. Planes of symmetry and types of planes. Improperrotational axis of symmetry. Inversion centre. Identity element. The symmetry operations of amolecule form a group.

2. Theory of quantitative analysis

a) Principles of volumetric analysis. Theories of acid-base, redox, complexometric, iodometricand precipitation titrations.

24

b) Principles of gravimetric analysis: precipitation, coprecipitation, post precipitation,

3. Evaluation of analytical data.

Theory of errors, idea of significant figures and its importance, accuracy – methods ofexpressing accuracy, precision – methods of expressing precision, standard deviation.

4. Introductory treatment to:

a) Pericyclic ReactionsConcerted reactions, Molecular orbitals, Symmetry properties HOMO, LUMO, Thermal andphotochemical pericyclic reactions. Types of pericyclic reactions – electrocyclic,cycloaddition and sigmatropic reactions – one example each.

b) Synthetic strategiesTerminology – Disconnection (dix), Symbol ( ), synthon, synthetic equivalent (SE),Functional group interconversion (FGI), Retrosynthesis of the following molecules 1)acetophenone 2) cyclohexene.

c) Asymmetric (Chiral) synthesisDefinitions-Asymmetric synthesis, enantiomeric excess, diastereomeric excess.

25

Guidelines to the Paper Setter: II B.Sc., Chemistry Syllabi is devided into Two parts forSemester III and IV. Semester – IV Syllabi consists of Physical and General Chemistry. Semester –IV Syllabis consists of 3 Sections, Section – A, Section – B and Section – C.

In Section – A, Five Very Short Answer Questions are to be set. Choosing Three from Physicaland Two from General Chemistry. Five to be answered. Each question carries 2 Marks.

In Section – B , Eight Short Answer Questions are to be set. Choosing Four from Physical and Fourfrom General Chemistry. Out of which Five are to be answered. Each question carries 5 Marks.

In Section – C, Eight Essay Questions are to be set. Choosing Four from Physical and Four fromGeneral Chemistry. Each question carries 10 Marks and Four are to be answered.

The examiner is requested to set question in such a way that the entire syllabus is reflected in thequestion paper set by him.

B. Sc., Second Year – CORE-IVCOURSE-IV

(Physical & General Chemistry-II)Semester-IVBLUE PRINT


Module-VII (Physical Chemistry-II)1. Phase rule 1 1 1

2 Dilute solutions 1 1 1

3 Electrochemistry 1 2 2

Module-VIII (General Chemistry-II)

1. Molecular symmetry 1 1

2.Theory of quantitative

analysis1 1 1

3.Evaluation of analytical

data1 1 1

4.

Introductory treatment to:

Pericyclic reactions

Synthetic strategies

Asymmetric synthesis

1 1

26

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13CORE-IV

II B.Sc., FOURTH SEMESTER EXAMINATIONS 2014 – 2015.CHEMISTRYCOURSE– IV

(Physical and General Chemistry – II)Time: 3 Hours MODEL PAPER Max. Marks: 75

(w. e. f. 2015 – 2016)

SECTION – A


1. State Raoult’s Law.

2. Define specific conductance?

3. What is freezing mixture? Give one example.

4. What is electro chemical series?

5. Write the Retro synthesis of Acetophenone?

SECTION – B

Answer any FIVE questions. Each question carries 5 Marks. (5 X 5 = 25 marks)

6. What is Eutectic Point and explain desilverisation of lead?

7. State and explain Ostwald dilution law.

8. What is Vanthoff’s factor? Write its one application.

9. State and explain Nernest Equation?

10. Write a short note on Coprecipitation?

11. Write a short note on Asymmetric Synthesis?

12. What are complexometric titrations? Explain with one example

13. What are symmetry properties and explain?

27

SECTION – C

Answer any FOUR questions. Each question carries 10 Marks. (4X 10 = 40 Marks)

14. State and explain Gibbs phase rule and explain the following terms with examples.

a) Phase b) Degrees of freedom c) Number of Components(OR)

Define Osmotic Pressure and determine the molecular weight of non-volatile solute fromOsmotic pressure?

15. Explain Debye Huckel theory?(OR)

Explain conductometric titrations?

16. What are Symmetry elements and explain the following terms with examples?

a) Plane of Symmetry b) Axis of Symmetry c) Centre of Symmetry d) Rotational axis ofSymmetry

(OR)

Explain the principle involved in Acid – Base Titrations and explain the choice of indicators?

17. Explain different types of pericyclic reactions with exampls?(OR)

What is an error and explain different types of errors?

28

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13Chemistry Practical Examinations at the END OF II Year / Sem-IV

Time: 3 Hours Max. Marks: 50

LABORATORY COURSE – II 90 hrs (3 h / w)

Practical PAPER – II (Inorganic Chemistry)

I. Titrimetric analysis:

1) Determination of carbonate and bicarbonate in a mixture2) Determination of Fe(II) using K2Cr2O7

3) Determination of Fe(II) using KMnO4 with oxalic acid as primary standard.4) Determination of Cu(II) using Na2S2O3 with K2Cr2O7 as primary standard5) Determination of Zinc using EDTA6) Determination of hardness of water7) Determination of Zinc by ferrocyanide

II. Gravimetric analysis (any three of the following)

1) Determination of barium as barium sulphate2) Determination of sulphate as barium sulphate3) Determination of lead as lead chromate4) Determination of nickel as Ni-DMG complex5) Determination of magnesium as magnesium pyrophosphate.

29

ADVANCED-I

B.Sc., Chemistry

Model Curriculum -Course structure

B.Sc., Third YearCourse- V

(Inorganic, Organic & Physical Chemistry-III)

Semester –V 60 hrs (15 weeks)

MODULE- I (Inorganic Chemistry-III) 15 hrs (1 h / w)

1. Co-ordination Chemistry 10 h

2. Spectral & Magnetic properties of

Metal Complexes 5 h

MODULE II (Organic Chemistry-III) 15 hrs (1 h/w)

1. Nitrogen Compounds 9 h

2. Heterocyclic Compounds 6 h

MODULE III (Physical Chemistry-III) 15 hrs (1 h/w)

1. Thermodynamics 15 h

30

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13ADVANCED-I

III B.Sc., V – SEMESTER CHEMISTRY SYLLABUS FOR THE ACADEMIC YEAR 2014 – 2015(Course – VA: Inorganic, Organic and Physical Chemistry-III)

(w. e. f. 2016 – 2017)

MODULE – I (Inorganic Chemistry – III):

1. Coordination Chemistry: 10h

IUPAC nomenclature, bonding theories – review of Werner’s theory and Sidgwick’s concept ofcoordination, Valence bond theory, geometries of coordination numbers 4-tetrahedral and squareplanar and 6-octahedral and its limitations, crystal field theory, splitting of d-orbitals inoctahedral, tetrahedral and square-planar complexes – low spin and high spin complexes – factorsaffecting crystal-field splitting energy, merits and demerits of crystal-field theory. Isomerism incoordination compounds – structural isomerism and stereo isomerism, stereochemistry ofcomplexes with 4 and 6 coordination numbers.

2. Spectral and magnetic properties of metal complexes: 4h

Electronic absorption spectrum of [Ti(H2O)6]3+ ion. Types of magnetic behaviour, spin-only

formula, calculation of magnetic moments, experimental determination of magnetic susceptibility– Gouy method.

MODULE – II (Organic Chemistry – III):

1. Nitrogen Compounds: 9h

Nitro hydrocarbons: Nomenclature and classification – nitro hydrocarbons – structure. Tautomerismof nitroalkanes leading to aci and keto form. Preparation of Nitroalkanes. Reactivity – halogenation,reaction with HONO (Nitrous acid), Nef reaction and Mannich reaction leading to Michael additionand reduction.

Amines (Aliphatic and Aromatic): Nomenclature, Classification into 10, 20, 30 Amines andQuarternary ammonium compounds. Preparative methods -1. Ammonolysis of alkyl halides 2.Gabriel synthesis 3. Hoffman’s bromamide reaction (mechanism).4. Reduction of Amides andSchmidt reaction. Physical properties and basic character – Comparative basic strength ofAmmonia, methyl amine, dimethyl amine, trimethyl amine and aniline – comparative basic strengthof aniline, N-methylaniline and N,N-dimethyl aniline (in aqueous and non-aqueous medium), stericeffects and substituent effects. Use of amine salts as phase transfer catalysts. Chemical properties:a) Alkylation b) Acylation c) Carbylamine reaction d) Hinsberg separation e) Reaction with Nitrousacid of 10, 20, 30 (Aliphatic and aromatic amines). Electrophilic substitutions of Aromatic amines –Bromination and Nitration. oxidation of aryl and 30 Amines. Diazotization Cyanides andisocyanides: Nomenclature (aliphatic and aromatic) structure. Preparation of cyanides from a) Alkylhalides b) from amides c) from aldoximes. Preparation of isocyanides from Alkyl halides andAmines. Properties of cyanides and isocyanides, a) hydrolysis b) addition of Grignard reagent iii)reduction iv) oxidation.

31

2. Heterocyclic Compounds: 6h

Introduction and definition: Simple 5 membered ring compounds with one hetero atom Ex.Furan. Thiophene and pyrrole. Importance of ring system – presence in important natural productslike hamoglobin and chlorophyll. Numbering the ring systems as per Greek letter and Numbers.Aromatic character – 6- electron system (four-electrons from two double bonds and a pair of non-bonded electrons from the hetero atom). Tendency to undergo substitution reactions.Resonancestructures: Indicating electron surplus carbons and electron deficient hetero atom. Explanation offeebly acidic character of pyrrole, electrophillic substitution at 2 or 5 position, Halogenation,Nitration and Sulphonation under mild conditions. Reactivity of furan as 1,3-diene, Diels Alderreactions (one example). Sulphonation of thiophene purification of Benzene obtained from coal tar).Preparation of furan, Pyrrole and thiophene from 1,4,- dicarbonyl compounds only, Paul-Knorrsynthesis, structure of pyridine, Basicity – Aromaticity – Comparison with pyrrole – one method ofpreparation and properties – Reactivity towards Nucleophilic substitution reaction – chichibabinreaction.

MODULE – II1 (Physical Chemistry –III):

1. Thermodynamics: 16h

The first law of thermodynamics-statement, definition of internal energy and enthalpy. Heatcapacities and their relationship. Joule’s law-Joule-Thomson coefficient. Calculation of w, q, dUand dH for the expansion of perfect gas under isothermal and adiabatic conditions for reversibleprocesses. State function. Temperature dependence of enthalpy of formation-Kirchoff’s equation.

Second law of thermodynamics. Different Statements of the law. Carnot cycle and its efficiency.Carnot theorem. Thermodynamic scale of temperature. Concept of entropy, entropy as a statefunction, entropy changes in cyclic, reversible, and irreversible processes and reversible phasechange. Calculation of entropy changes with changes in V & T and P&T. Entropy of mixing inertperfect gases. Entropy changes in spontaneous and equilibrium processes.

The Gibbs (G) and Helmholtz (A) energies. A & G as criteria for thermodynamic equilibrium andspontaneity-advantage over entropy change. Gibbs equations and the Maxwell relations. Variationof G with P, V and T.

32

Guidelines to the Paper Setter: V Semester syllabi consist of Inorganic, Organic and PhysicalChemistry. Paper – III consists of 3 Sections, Section – A, Section – B and Section – C.

In Section – A : Five very short answer questions are to be set choosing two from Inorganic 2from Organic and 1 from Physical out of which 5 questions are to be answered each questioncarries 2 Marks. (2 X 5 = 10 Marks)In Section - B: Eight short answer questions are to be set choosing 3 questions from Inorganic, 3from Organic and 2 from Physical out of which 5 questions are to be answered each question carries5 Marks. (5 X 5 = 25 Marks)In Section – C: Eight essay questions are to be set choosing three from Inorganic, three fromOrganic and two from physical with internal choice. Each question carries 10 Marks and fourquestions are to be answered. (4 X 10 = 40 Marks)

B.Sc Third Year – COURSE-V(Inorganic, Organic & Physical Chemistry-III)

Semester-VBLUE PRINT

S.No Name of the chapter 2 marks 5 marks 10 marks

Unit- I (Inorganic Chemistry-III)

1. Co-ordination chemistry 1 2 2

2. Spectral & Magneticproperties of Metal complexes

1 1 1

Unit- II (Organic Chemistry-III)

3. Nitrogen compounds 1 2 2

4. Heterocyclic compounds 1 1 1

Unit- III (Physical Chemistry-III)

5. Thermodynamics 1 2 2

33

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13ADVANCED - I

III B.Sc., V SEMESTER - END EXAMINATIONS 2013 - 2014CHEMISTRYCOURSE-V

(Inorganic, Organic and Physical Chemistry-III)Time: 3 Hours MODEL PAPER Max. Marks: 75

(w. e. f. 2016 – 2017)

Answer only FIVE questions from Section – A; Only FIVE questions from Section – B; andanswer all FOUR questions from Section – C.

S E C T I O N – A

Answer all FIVE questions. Each question carries two Marks. (5 X 2 = 10 Marks)

1. What is effective atomic number and calculate the EAN of ‘Pt’ in [Pt(NH3)2cl2].

2. Why square plannar complexes do not exhibit optical Isomerism.

3. Which is more basic among N, N –dimethyl aniline and Aniline.

4. Furan gives Diels-Alder reaction. Where as pyrrole and Thiophene does not give why?

5. Write any one definitions of second law of thermodynamics.

S E C T I O N – B


6. Write the postulates of Werner’s theory.

7. Write a brief note on structural isomerism in coordination compounds with one example each.

8 Explain(i) Why pyrrole undergoes nucleophilic substitution predominsntly at 2-position (i.e. α-position)

(ii) How do you separate Thiophene from Benzene obtained from coaltar.

9. Explain how amine salts are used as phase-Transfer catalyst.

10. Write a short note on Joule - Thomson effect.

11. Derive Gibbs Helmholtz’s equation and explain its importance.

12. Write about the factors that influence crystal field splitting energy

13. Dicuss the basicity of Pyridine?

34

S E C T I O N – C

Answer all questions. (4 X 10 = 40 Marks)

14. Write the important postulates of Valence Bond Theory and on the basis of VBThow will you explain that [Ni(CO)4] is Tetrahedral while[Ni(CN)4]

2- Square planar.

(O R)

Explain crystal Field Theory. Discuss the splitting of d-orbitals in Octahedral and Tetrahedralcomplexes by taking any one example.

15. (a). Explain Tautomerism in nitroalkanes with one example.

(b). Write any two methods of preparation of nitro alkanes.

©. Write any three properties of nitroalkanes.

(O R)

(a). How do you prepare primary amines by Hoffmann Bromamide reaction method and give it’s

mechanism.

(b). How do you separate the mixture of primary, Secondary and tertiary amines by Hinsberg’s

method.

©. Write the reaction of 10, 20, 30 amines with HNo2.

16. Deduce the following relations.

(a). PVr = constant for an aadiabatic expansion of an ideal gas.

(b). Derive Cp - Cv =R

(O R)(a). Write an essay on Carnot’s cycle?

(b). Explain the significance of entropy.17. Explain the absorption spectrum of [Ti (H2O)6] with suitable diagram?

(O R)Explain the aromatic character of Furan, pyrrole and thiophene and write the preparationmethods for the above compounds

35

ADVANCED-II / ELECTIVE-1COURSE-VA

B.Sc., Chemistry Third year

Model Curriculum- Course structure

COURSE-VA(Molecular Spectroscopy & Catalysis-IV)

Semester –V 30 hrs (15 weeks)

MODULE I

1. Molecular Spectroscopy 18 h

MODULE II

1. Catalysis 12 h

36

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13ADVANCED-II / ELECTIVE-1

III B.Sc., V – SEMESTER CHEMISTRY SYLLABUSCOURSE – VA

(Molecular Spectroscopy, Catalysis-IV)(w. e. f. 2016 – 2017)

Molecular Spectorscopy: 18h

MODULE I

Electronic spectroscopy:Interaction of electromagnetic radiation with molecules and types of molecular spectra. Potentialenergy curves for bonding and antibonding molecular orbitals. Energy levels of molecules (σ,π, n) .Selectio rules for electronic spectra. Types of electronic transitions in molecules effect ofconjugation. Concept of chromophore.

MODULE II

Infra red spectroscopy:Energy levels of simple harmonic oscillator, molecular vibration spectrum, selection rules.Determination of force constant. Qualitative relation of force constant to bond energies.Anharmonic motion of real molecules and energy levels. Modes of vibrations in polyatomicmolecules. Characteristic absorption bands of various functional groups. Finger print nature ofinfrared spectrum.

MODULE III

Raman spectroscopy:Concept of polarizability, selection rules, pure rotational and pure vibrational Raman spectra ofdiatomic molecules, selection rules.

MODULE IV

Proton magnetic resonance spectroscopy (1H-NMR):Principles of nuclear magnetic resonance, equivalent and non-equivalent protons, position ofsignals. Chemical shift, NMR splitting of signals – spin-spin coupling, coupling constants.Applications of NMR with suitable examples – ethyl bromide, ethanol, acetaldehyde, 1,1,2-tribromo ethane, ethyl acetate, toluene and acetophenone.

MODULE V

Spectral interpretation:Interpretation of IR, UV-Visible, 1H-NMR and mass spectral data of the following compounds 1.Phenyl acetylene 2. Acetophenone 3.Cinnamic Acid 4. para-nitro aniline.

37

MODULE II

Catalysis: 12h

Homogeneous and heterogeneous catalysis, comparision with examples. Kinetics of specific acidcatalyzed reactions, inversion of cane sugar. Kinetics of specific base catalyzed reactions, basecatalyzed conversion of acetone to diacetone alcohol. Acid and base catalyzed reactions- hydrolysisof esters, mutarotation of glucose. Catalytic activity at surfaces. Mechanisms of heterogeneouscatalysis. Langmuir-Hinshelwood mechanism.

Enzyme catalysis: Classification, characteristics of enzyme catalysis. Kinetics of enzyme catalyzedreactions-Michaelis Menton law, significance of Michaelis constant (Km) and maximum velocity(Vmax). Factors affecting enzyme catalysis- effect of temperature, pH, concentration and inhibitor.Catalytic efficiency. Mechanism of oxidation of ethanol by alcohol dehydrogenase.

38

Guidelines to the Paper Setter:

ADVANCED-II / ELECTIVE-1III B.Sc., V – SEMESTER CHEMISTRY SYLLABUS

COURSE – VA(Molecular Spectroscopy, Catalysis-IV)

V Semester Syllabi consist of molecular spectroscopy and catalysis.Paper – IV consists of 3 sections, Section – A, Section – B and Section –C.

In Section – A: 5 very short answer questions are to be set out of which 5 questions are to beanswered each question carries 2 Marks. (2 X 5 = 10 Marks)

In Section – B: 8 short answer questions are to be set out of which 5 questions are to be answeredeach question carries 5 Marks. (5 X 5 = 25 Marks)

In Section – C: 8 Essay Questions are to be set choosing one question from each chapter. Eachquestion carries 10 Marks and four questions are to be answered. (4 X 10 = 40 Marks)

ADVANCED-II / ELECTIVE-1B. Sc., Third Year, V – SEMESTER

COURS – VA(Molecular Spectroscopy and Catalysis-IV)

BLUE PRINT

Sl.No Name of the chapter

Very ShortQuestion2 marks

ShortQuestion5 marks

EssayQuestion10 marks

Molecular Spectorscopy

1. Electronic Spectroscopy 1 1 1

2. IR Spectroscopy 1 1 1

3. Raman Spectroscopy 1 1 1

4. PMR Spectroscopy 1 1 2

5. Spectral Interpretation - 1 1

Catalysis6. Catalysis 1 3 2

39

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13III B.Sc.., FIFTH SEMESTER

(ADVANCED-II / ELECTIVE-1)COURSE – VA

(Molecular Spectroscopy, Catalysis-IV)Time: 3 Hours MODEL PAPER Max. Marks: 75

(w. e. f. 2017 – 2018)

SECTION-A

Answer any FIVE questions each question carries 2 Marks 5 x 2 = 10 marks

1. Define chromophore and give one example

2. What is finger print region?

3. What is Raman Effect?

4. What is coupling constant?

5. Write Michaelis Manton law?

SECTION-B


6. Explain energy levels of molecules. Write selection rules of electronic spectroscopy

7. Write and explain the NMR spectrum of Ethyl Bromide

8. Explain concept of polarisability

9. Explain Langmuir-Hinshelwood mechanism of catalysis

10. Explain various factories effecting enzyme catalysis

11. Derive force constant in simple Harmonic oscillation

12. Explain the kinetics of acid catalyzed Inversion of cane sugar

13. Explain the interpretation of IR, UV, ‘H NMR and mass spectral data of Acetophenone.

40

SECTION-C

Answer any all questions. Each question carries 10 Marks 4 x 10 = 40 marks

14. Explain different types of electronic transitions in molecules.with examples

(OR)

(a) Explain different modes of vibrations in poly atomic molecules.

(b) Explain characteristic absorption bands of alcohols, aldehyde, and carboxylic acid.

15. (a) Explain the principle of nuclear magnetic resonance spectroscopy.

(b)Explain equivalent and non-equivalent protons with examples.(OR)

Explain the following terms

(A) Chemical Shift

(B) Splitting of signals due to spin-spin coupling

(C) Applications of NMR.

16. (a) Explain Homogeneous and Heterogeneous catalysis with examples.

(b) Explain acid base catalysis with examples.

(OR)

(a) Explain enzyme catalysis with examples. Write the characteristics of enzyme catalysis

(b) Explain the kinetics of enzyme catalysis.

17. Explain Raman spectra and its applications

(OR)

Explain the interpretation of IR, UV, ‘H NMR and mass spectral data of Cinnamic Acid andpara-nitro aniline

41

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13

ADVANCED-2 / ELECTIVE-2B.Sc., Chemistry

Model Curriculum- Course structureB.Sc., Third year, Semester-V

COURSE-5B(Drugs, Formulations, Green Chemistry & Material Science-IV)

Semester –V, Elective-2 30 hrs (15 weeks)

MODULE I

1. Drugs- Formulations 17 h

MODULE II

2. Green Chemistry 5 h

MODULE III

3. Material Science 8 h

42


ADVANCED-2 / ELECTIVE-2III B.Sc., V – SEMESTER CHEMISTRY SYLLABUS

COURSE-VBDrugs, Formulations, Green Chemistry & Material Science-IV)

(w. e. f. 2017 – 18)

MODULE – I

Drugs 17 h

Introduction: Drug, disease (definition), Historical evolution, Sources – Plant, Animal synthetic,Biotechnology and human gene therapy.Terminology: Pharmacy, Pharmacology, Pharmacophore,Pharmacodynamics, Pharmacokinetics (ADME, Receptors – brief teartment) Metabolites and Antimetabolites.Nomenclature: Chemical name, Generic name and trade names with examplesClassification: Classification based on structures and therapeutic activity with one example each.Synthesis: Synthesis and therapeutic activity of the following drugs., L-Dopa, Chloroquin,Omeprazole, Albuterol and ciprofloxacin.Drug Development: Pencillin, Separation and isolation, structures of different pencillinsHIV-AIDS: ImmMODULEy – CD-4 cells, CD-8 cells Retrovirus, replication in human body.Investigation available, prevention of AIDS. Drugs available – examples with structures: PIS:Indinavir (Crixivan), Nelfinavir (Viracept), NNRTIS: Efavirenz (Susrtiva), Nevirapine (Viramune)NRTIs: Abacavir (Ziagen), Lamivudine (Epivir, 3TC) Zidovudine (Retravir, AZT, ZDV)Monographs of drugs: Eg Paracetamol, Sulpha methoxazole (Tablets)

MODULE – II

Formulations 3 hNeed of conversion of drugs into medicine. Additives and their role (brief account only).Differenttypes of formulations

MODULE – III

1. Green Chemistry 5hIntroduction: Definition of green Chemistry, need of green chemistry, basic principles of greenchemistry

Green synthesis: Evalution of the type of the reaction i) Rearrangements (100% atom economic),ii) Addition reaction (100% atom economic), Pericyclic reactions (no by-product).Selection ofsolvent: i) Aqueous phase reactions ii) Reactions in ionic liquids iii) Solid supported synthesisiv)Solvent free reactions (solid phase reactions) ii) Green catalysts: i) Phase transfer catalysts(PTC) ii) Biocatalysts, Microwave and Ultrasound assisted green synthesis:Aldol condensation,Cannizzaro reaction, Diels-Alder reactions, Strecker synthesis, Willaimson synthesis, Dieckmanncondensation

2. Materials science 5h

Superconductivity, characteristics of superconductors, Meissner effect, types of superconductorsand applications.Nanomaterials- synthetic techniques, bottom-up-sol-gel method, top-down- electro

43

deposition method. Properties and applications of nano-materials. Composites-definition, generalcharacteristics, particle reinforce and fiber reinforce composites and their applications.


V Semester Syllabi consist of Drugs, Formulations, Green Chemistry and Material Science.Paper – IV consists of 3 sections, Section – A, Section – B and Section –C.

In Section – A: 5 very short answer questions are to be set out of which 5 questions are to beanswered each question carries 2 Marks. (2 X 5 = 10 Marks)

In Section – B: 8 short answer questions are to be set out of which 5 questions are to be answeredeach question carries 5 Marks. (5 X 5 = 25 Marks)

In Section – C: 8 Essay Questions are to be set choosing one question from each chapter. Eachquestion carries 10 Marks and four questions are to be answered. (3 X 10 = 40 Marks)

ADVANCED-2 / ELECTIVE-2III B.Sc., V – SEMESTER CHEMISTRY SYLLABUS

Course-VB(Drugs, Formulations, Green Chemistry and Material Science)

BLUE PRINT

Sl. No Name of the chapterVery ShortQuestion2 marks



1. Drugs 2 3 3

2. Formulations 1 2 1

3. Green Chemistry 1 2 1

4. Material Science 1 1 3

44


ADVANCED-2 / ELECTIVE-2III B.Sc., V – SEMESTER CHEMISTRY

Course-VB(Drugs, Formulations, Green Chemistry and Material Science-IV)


SECTION-A

Answer any FIVE questions. Each question carries 2 Marks 5 x 2 = 10 marks

1. What are metabolites and anti metabolites?

2. Write any two drugs used in treatment of HIV-AIDS?

3. What is meant by formulation?

4. Give one example to 100% atom economy?

5. Write Meissner effect?

SECTION-B


6. Explain the monograph of Paracetamol

7. Write short notes on CD4 and CD8 cells

8. Write about the need of conversion of drug into medicine

9. Write about phase transfer catalysts

10. Write about the separation and isolation of penicillin

11. Explain different types of superconductors

12. Explain the following reactions with special reference to green chemistry.

(a) Aldol condensation (b) Diels-Alder reaction

13. What are additives? Explain their role?

45

SECTION-C

Answer any All questions. Each question carries 10 Marks 4 x 10 = 40 marks

14. Explain the classification of drugs based on structure and therapeutic activity with examples.

(OR)

Explain the synthesis and therapeutic activity of the following.

(a) Omeprazole (b) L-DOPA

15. Explain different types of formulations with examples.

(OR)

Explain basic principles of Green Chemistry.

16. What are superconductors? Explain the characteristics and applications of superconductors.

(OR)

Explain the synthetic techniques and properties of nanomaterials.

17. Explain the charectristics properties of Composites and their applications.

(OR)

Explain the synthesis and therapeutic activity of the following drugs

(a) Chloroquin and (b) Ciprofloxacin

46

APPLIED-IIII B.Sc., Semester-VI Chemistry

Model Curriculum- Course structure

COURSE-VI(Inorganic, Organic & Physical Chemistry-III)

(w. e. f. 2016 – 2017)

Semester –VI A 45 hrs (15 weeks)

MODULE- I (Inorganic Chemistry-III) 15 hrs (1h / w)

1. Reactivity of Metal Complexes 4 h

2. Stability of Metal Complexes 4 h

3. Hard & Soft acids bases (HSAB) 4 h

4. Bio-Inorganic Chemistry 4 h

MODULE- II (Organic Chemistry-III) 15 hrs (1h / w)

1. Carbohydrates 6 h

2. Amino Acids & Proteins 5 h

3. Mass Spectrophotometry 4 h

MODULE- III (Physical Chemistry-III) 15 hrs (1h / w)

1. Chemical Kinetics 9 h

2. Photo Chemistry 6 h

47

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13APPLIED - I

III B.Sc., VI – SEMESTER CHEMISTRYCOURSE - VI

(Inorganic, Organic and Physical Chemistry-III)(w. e. f. 2016– 2017)

MODULE – I (Inorganic Chemistry-III)

1. Reactivity of metal complexes:Labile and inert complexes, ligand substitution reactions – SN1 and SN2, substitution reactions ofsquare planar complexes – Trans effect and applications of trans effect. 4h

2. Stability of metal complexes: 4 hThermodynamic stability and kinetic stability, factors affecting the stability of metal complexes,chelate effect, determination of composition of complex by Job’s method and mole ratio method.

3 Hard and soft acids bases (HSAB):Classification, Pearson’s concept of hardness and softness, application of HSAB principles –Stability of compounds / complexes, predicting the feasibility of a reaction. 4 h

4. Bio-inorganic chemistry: 4 hEssential elements, biological significance of Na, K, Mg, Ca, Fe, Co, Ni, Cu, Zn and chloride (Cl-

).Metalloporphyrins – hemoglobin, structure and function, Chlorophyll, structure and role inphotosynthesis.

MODULE II: (Organic Chemistry-III)

1. Carbohydrates: 6h

Monosaccharides: All discussion to be confined to (+) glucose as an example of aldo hexoses and (-) fructose as example of ketohexoses. Chemical properties and structureal elucidation: Evidencesfor straight chain pentahydroxy aldehyde structure (Acetylation, reduction to n-hexane, cyanohydrinformation, reduction of Tollen’s and Fehling’s reagents and oxidation to gluconic and saccharicacid). Number of optically active isomers possible for the structure, configuration of glucose basedon D-glyceraldehyde as primary standard (no proof for configuration is required). Evidence forcyclic structure of glucose (some negative aldehydes tests and mutarotation). Cyclic structure ofglucose. Decomposition of cyclic structure (Pyranose structure, anomericCarbon and anomers). Proof for the ring size (methylation, hydrolysis and oxidation reactions).Different ways of writing pyranose structure (Haworth formula and chair conformationa formula).Structure of fructose: Evidence of 2 – ketohexose structure (formation of penta acetate, formation ofcyanohydrin its hydrolysis and reduction by HI to give 2-Carboxy-n-hexane). Same osazoneformation from glucose and fructose, Hydrogen bonding in osazones, cyclic structure for fructose(Furanose structure and Haworth formula).

Interconversion of Monosaccharides: Aldopentose to aldo hexose – eg: Arabinose to D-Glucose, D-Mannose (Kiliani - Fischer method). Epimers, Epimerisation – Lobry de bruyn van Ekensteinrearrangement. Aldohexose to Aldopentose eg: D-glucose to D-arabinose by Ruff’f degradation.

48

Aldohexose (+) (glucose) to ketohexose (-) (Fructose) and Ketohexose (fructose) to aldohexose(Glucose)

2. Amino acids and proteins 5 h

Introduction: Definition of Amino acids, classification of Amino acids into alpha, beta, and gamaamino acids. Natural and essential amino acids – definition and examples, classification of alphaamino acids into acidic, basic and neutral amino acids with examples. Methods of synthesis:General methods of synthesis of alpha amino acids (specific examples – Glycine, Alanine, valineand leucene) by following methods: a) from halogenated carboxylic acid b) Malonic ester synthesisc) strecker’s synthesis.

Physical properties: Optical activity of naturally occurring amino acids: L-configuration,irrespective of sign rotation, Zwitterion structure – salt like character - solubility, melting points,amphoteric character , definition of isoelectric point.

Chemical properties: General reactions due to amino and carboxyl groups – lactams fromgamma and delta amino acids by heating peptide bond (amide linkage). Structure and nomenclatureof peptides and proteins.

3. Mass Spectrometry: 4 h

Basic principles – Molecular ion / parent ion, fragment ions / daughter ions. Theory – formation ofparent ions. Representation of mass spectrum. Identification of parent ion, (M+1), (M+2), basepeaks (relative abundance 100%) Determination of molecular formula – Mass spectra ofethylbenzene, acetophenone, n-butyl amine and 1- proponal.

MODULE-III (Physical chemistry-III)

1. Chemical kinetics 9 h

Rate of reaction, factors influencing the rate of a reaction-concentration, temperature, pressure,solvent, light, catalyst. Experimental methods to determine the rate of reaction. Definition of orderand molecularity. Derivation of rate constants for first, second, third and zero order reactions andexamples. Derivation for time half change. Methods to determine the order of reactions. Kinetics ofcomplex reactions (first order only): opposing reactions, parallel reactions, consecutive reactionsand chain reactions. Effect of temperature on rate of reaction, Arrhenius equation, concept ofactivation energy. Theories of reaction rates- collision theory-derivation of rate constant forbimolecular reaction. The transition state theory (elementary treatment)

2. Photochemistry 5 h

Difference between thermal and photochemical processes. Laws of photochemistry-Grothus-Draper’s law and Stark-Einstein’s law of photochemical equivalence. Quantum yield. Ferrioxalateactinometry. Photochemical hydrogen- chlorine, hydrogen-bromine reaction. Jablonski diagramdepicting various processes occurring in the excited state, qualitative description of fluorescence,phosphorescence, non-radiative processes (internal conversion, intersystem crossing).Photosensitized reactions- energy transfer processes (simple example)

49

Guidelines to the Paper Setter:VI A: Semester syllabi consist of Inorganic, Organic and PhysicalChemistry. Paper – III consists of 3 Sections, Section – A, Section – B and Section – C.

In Section – A : Five very short answer questions are to be set choosing two from Inorganic 2from Organic and 1 from Physical out of which 5 questions are to be answered each questioncarries 2 Marks. (2 X 5 = 10 Marks)In Section - B: Eight short answer questions are to be set choosing 2 questions from Inorganic, 3from Organic and 3 from Physical out of which 5 questions are to be answered each question carries5 Marks. (5 X 5 = 25 Marks)In Section – C: Eight essay questions are to be set choosing three from Inorganic, three fromOrganic and two from physical with internal choice. Each question carries 10 Marks and fourquestions are to be answered. (4 X 10 = 40 Marks)

APPLIED - IIII B.Sc., VI – SEMESTER CHEMISTRY

COURSE - VI(Inorganic, Organic and Physical Chemistry-III)

BLUE PRINT

S.No Name of the chapter 2 marks 5 marks 10 marks

Unit- I (Inorganic Chemistry)

1. Reactivity of Metal complexes 1 1

2. Stability of Metal complexes 1 1

3. Hard and Soft Acids Bases 1

4. Bio-inorganic chemistry 1 1

Unit- II (Organic Chemistry)

5. Carbohydrates 1 1 1

6. Amino acids and proteins 1 1

7. Mass Spectrometry 1 1 1

Unit- III (Physical Chemistry)

8. Chemical kinetics 2 1

9. Photochemistry 1 1 1

50

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13APPLIED – I

III B.Sc.., SIXTH SEMESTER - END EXAMINATIONS 2016 - 2017CHEMISTRYCOURSE– VI

(Inorganic, Organic and Physical Chemistry-III)Time: 3 Hours MODEL PAPER Max. Marks: 75

(w. e. f. 2016 – 2017)

Answer only FIVE questions from Section – A; Only FIVE questions from Section – B; andanswer all FOUR questions from Section – C.

S E C T I O N – A

Answer any FIVE questions. Each question carries 2 Marks (5 X 2 = 10 Marks)

1. What is Chelate?

2. What is HSAB Principle?

3. What is Molisch Test?

4. What is peptide bond?

5. Explain the Chemileuminnescnce?S E C T I O N – B

Answer any FIVE questions. Each question carries 5 Marks (5X5 = 25 Marks)

6. Explain the Trans Effect?

7. Explain the concept of Activation energy?

8. How Glucose and Fructose give same osozone?

9. Explain the Principle of Mass Spectroscopy?

10. Explain the Jablonski Diagram?

11. Write the Differences between Fluorescence and phosphorescence?

12. Write the importance of the Mg & Zn elements?

13. What are essentional amino acids, give two examples?

51

S E C T I O N – C

Answer all questions. (4 X 10 = 40 Marks)

14. Explain the Ligand substitution reactons in SN1 & SN2 Mechanism?

(OR)

Explain the determination of composition of complexes byi) Job’s method and ii) Mole ratio method

15. Discuss the structure of Glucose?

(OR)

Write the classification of Amino Acids and write any three methods of preparaton of Aminoacids?

16. Derive the rate constant of First Order Reaction?

(OR)

Write the laws of Photo Chemistry and Determination of Quantum yield of a reaction?

17. Write about the different applications of Hard- Soft, acid base rule?

(OR)Explain the fragmentations processes of Ethylbenzene, Acetophenone and draw their mass spectra?

52

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13Applied-2 / Elective-I

III B.Sc., V I– SEMESTER CHEMISTRY

COURSE-6A(Separation techniques, Spectrophotometry, Natural Products-IV)

(w. e. f. 2016 – 2017)

Semester –VI 30 hrs (3 h/w)

MODULE I (Physico Chemical Methods of Analysis)

1. Separation Techniques 13 h

MODULE II

2. Spectrophometry 5 h

MODULE III (Natural Products) 12h

3. Alkaloids

4. Terpenoids

5. Steroids

53

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13Applied-2 / Elective-I



(w. e. f. 2016 – 2017)

MODULE – I : Physico Chemical methods of analysis:

1. Separation techniques: 13h

1. Solvent extraction: Principle and process, Batch extraction, continuous extraction and countercurrent extraction. Application – Determination of Iron (III)

2. Chromatography: Classification of chromatography methods, principles of differential migrationadsorption phenomenon, Nature of adsorbents, solvent systems, Rf values, factors effecting Rfvalues.

a) Paper Chromatography: Principles, Rf values, experimental procedures, choice of paper andsolvent systems, developments of chromatogram – ascending, descending and radial. Twodimensional chromatography, applications.

b) Thin layer Chromatography (TLC): Advantages. Principles, factors effecting Rf values.Experimentalprocedures. Adsorbents and solvents. Preparation of plates. Development of the

chromatogram. Detection of the spots. Applications.c) Column Chromatography: Principles, experimental procedures, Stationary and mobile

Phases, Separation technique. Applicationsd) High Performance Liquid Chromatography (HPLC): Principles and Applications.e) Gas Liquid Chromatography (GLC): Principles and Applications

MODULE IISpectrophotometry: 5h

General features of absorption – spectroscopy, Beer-Lambert’s law and its limitations,transmittance, Absorbance, and molar absorptivity. Single and double beam spectrophotometers.Application of Beer-Lambert law for quantitative analysis of

1. Chromium in K2Cr2O7

2. Manganese in manganous sulphate3. Iron (III) with thiocyanate.

MODULE IIIIntroduction to Natural Products 12h

Alkaloids1. Introduction and functions of alkaloids.2. Synthesis and biologica properties of piperine, nicotine.Terpenoids1: Introduction, Isoprene Rule. 2. Synthesis of citral, camphor.Steroids:Introduction, stereochemistry and nomenclature. synthesis & Biological importance of cholesterol.

54


VI Semester syllabi consist of Separation techniques, Spectrophotometry, Natural Products. Paper– IV B consists of 3 Sections, Section – A, Section – B and Section – C.

In Section – A : Five very short answer questions are to be set choosing two from Separationtechniques 2 from Natural Products and 1 from Spectrophotometry 5 questions are to beanswered each question carries 2 Marks.

(2 X 5 = 10 Marks)In Section - B: Eight short answer questions are to be set choosing 3questions from Separationtechniques, 2 from Spectrophotometry and 3from Natural Products out of which 5 questions are tobe answered each question carries 5 Marks.

(5 X 5 = 25 Marks)In Section – C: Eight essay questions are to be set choosing three from Separation techniques, two

from Spectrophotometry and three from Natural Products with internal choice. Each questioncarries 10 Marks and four questions are to be answered.

(4 X 10 = 40 Marks)

Applied-2 / Elective-I



BLUE PRINT




1. Separation techniques 2 3 3

2. Spectrophotometry 1 2 2

3. Natural Products 2 3 3

55


Applied-2 / Elective-IIII B.Sc., V I– SEMESTER CHEMISTRY



Section –A

Answer all questions. Each question carries 2 Marks. 2 x 5 = 10 marks

1. Define Rf value?

2. Write Isoprene rule?

3. What is Chromotogram?

4. Write the structure of Cholesterol?

5. Define Transmittance?

Section –BAnswer any FIVE questions. Each question carries 5 Marks. 5 x 5 = 25 marks

6. Describe double beam spectro photometer?

7. Explain the principle of HPLC?

8. Explain the classification of chromatography?

9. Explain ascending and descending paper chromatography?

10. Define absorbance and molar absorptivity?

11. What are the functions of Alkaloids?

12. Explain the biological importance of Cholesterol?

13. Explain the biological importance of Piperine?

Section –C

Answer any All questions. Each question carries 10 Marks. 4 x 10 = 40 marks

14. Explain the principle, experimental procedure of solvent extraction.explain the application of

solvent extraction in determinstion of Fe (III)?

(OR)

Explain the principle, experimental procedure and applications of Thin Layer chromatography?

56

15. Explain the principle, experimental procedure and applications of Column chromatography?

(OR)

State and explain Beer-Lambert law and its limitations? Explain the applications of Beer-

Lambert law for quantitative analysis of (a) chromium in K2Cr2O7 (b) Manganese in Manganece

sulphate?

16. What are Alkaloide? Explain the synthesis of Nicotine?

(OR)

What are Terpenoides? Explain the synthesis of Citral?

17. Explain about single and double beam spectrophotometers.

(OR)

Explain Synthesis and biologica importance of piperine?

57


Applied-2 / Elective-II

III B.Sc., V I– SEMESTER CHEMISTRYCOURSE – VI B

(Pesticides, Macromolecules & Petrochemicals-IV)

Semester –VI B 30 hrs (3 h/w)

MODULE I

1. Pesticides 6 hrs

MODULE II

2. Macromolecules 12 hrs

MODULE III

3. Petrochemicals 12 hrs

58

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13Applied-2 / Elective-II


(Pesticides, Macromolecules & Petrochemicals-IV)(w. e. f. 2016 – 2017)

MODULE I

Pesticides 5 h1. Introduction to pesticides – types – Insecticides, Fungicides, Herbicides, Weedicides,

Rodenticides plant growth regulators, Pheremones and Hormones. Brief discussion withexamples, Structure and uses.

2. Synthesis and presnt status of the following.DDT, BHC, Malathion, Parathion, Endrin, Baygon, 2,4-D and Endo-sulphon

MODULE II

Macromolecules 10hClassification of polymers, chemistry of polymerization, chain polymerization, steppolymerization, coordination polymerization – tacticity. Molecular weight of polymers-numberaverage and weight average molecular weight, degree of polymerization, determination ofmolecular weight of polymers by viscometry, Osmometry and light scattering methods. Kineticsof free radical polymerization, derivation of rate law. Preparation and industrial application ofpolyethylene, PVC, Teflon, polyacrylonitrile, terelene and Nylon66. Introduction tobiodegradability.

MODULE III

Petro chemicals 14h1. Introduction to petro chemicals -definition and classification of petro chemicals.2. Petroleum composition- Nature of crude oil -fractional distillation of crude oil3. CrackingThermal and catalytic cracking- knocking- octone number-aviation gasoline-kerosene-cetanenumber-LPG its composition.4. First generation petro chemicals- Types of compounds and importanceSecond generation petro chemicals- Types of compounds and importanceThird generation petro chemicals- Types of compounds and importance

59


VI Semester syllabi consist of Pesticides, Macromolecules & Petrochemicals. Paper – 6B consistsof 3 Sections, Section – A, Section – B and Section – C.

In Section – A : Five very short answer questions are to be set choosing 2 from Pesticides, 2from Macromolecules and 1 from Petrochemicals 5 questions are to be answered each questioncarries 2 Marks. (2 X 5 = 10 Marks)

In Section – B: Eight short answer questions are to be set choosing two from Pesticides, three fromMacromolecules and three from Petrochemicals with internal choice. Each question carries 5Marks and Five questions are to be answered.

(5 X 5 = 25 Marks)In Section -C: Eight essay questions are to be set choosing two from Pesticides, three fromMacromolecules and three from Petrochemicals with internal choice. Each question carries 10Marks and four questions are to be answered.

(4 X 10 = 40 Marks)



(Pesticides, Macromolecules & Petrochemicals-IV)BLUE PRINT




1. Pesticides 2 2 2

2. Macromolecules 2 3 3

3. Petrochemicals 1 3 3

60

B. Sc., Third Year – Paper-IV



(Pesticides, Macromolecules & Petrochemicals-IV)


Section –A

Answer all questions. Each question carries 2 Marks. 2 X5=10 marks.

1. Write the structure of 2, 4 D?

2. What are weedicides? Give example?

3. Write the Industrial applications of Teflan?

4. Write the preparation of Terylene?

5. Define Octane Number?

Section –B

Answer any Five questions. Each question carries 5 Marks 5X5=25 marks.

6. Write the synthesis and present statues of Melethion?

7. Explain about Tacticity?

8. Explain about coordination polymerisation?

9. Write the preparation and Industrial applications of Nylon 66?

10. What is Knocking and Cetane Number?

11. Write about third generation petro chemicals?

12. Explain different types of cracking?

13. Explain about plant growth regulators?

Section –C

Answer ALL questions. Each question carries 10 Marks 4X10=40 marks.

14. What are Pesticides? Explain the classification of Pesticides with examples?

(OR)

Explain the synthesis and present status of the following

(a) D D T (b) B H C

61

15. What are Polymers? Explain the classification of polymers with examples?

(OR)

Define number average molecular weight and weight overage molecular weight? Explain one

method of determining molecular weight of a polymer.

16. Explain the fractional distillation of crude oil?

(OR)

Expain about first generation petro chemicals with examples?

17.Explain chain polymerization and step polymerization with suitable examples?

(OR)

Write about Second generation petro chemicals?

62

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13Practical PAPER – III (Organic Chemistry-III)

Chemistry Practical Examinations at the END OF III Year / Sem-VITime: 3 Hours Max. Marks: 50

LABORATORY COURSE – III 90 hrs (3 h / w)

Practical PAPER – III (Organic Chemistry) 90 hrs (3 h / w)

1. Synthesis of Organic Compounds

i. Aromatic electrophilic substitution Nitration: Preparation of nitro benzene and p-nitroacetanilide, Halogenation: Preparation of p-bromo acetanilide – preparation of 2,4,6-tribromo phenol.

ii. Diazotization and coupling: Preparation of pheyl azo β-naptholiii. Oxidation: Preparation of benzoic acid from benzoyl chlorideiv. Reduction: Preparation of m-nitro aniline from m-dinitro benzenev. Esterfication: Preparation of methyl p-nitro benzoate from p-nitro benzoic acid.vi. Methylation: Preparation of β-napthyl methyl ether

Condensation: Preparation of benzilidine aniline and Benzoyl aniline.

2. Thin layer Chromatography & Column Chromatography

i. Preparation of the TLC plates. Checking the purity of the compounds by TLC:Acetylation of salicyclic acid, aniline, Benzoylation of Aniline and PhenolDetermination of Rf values and identification of organic compounds by TLC: preparationand separation of 2,4-dinitrophenyl hydrazones of acetione and 2-butanone using tolueneand light petroleum(40:60)

ii. Separation of ortho & para nitro aniline mixture by column chromatography

3. Organic Qualitative Analysis:

i. Identification of an organic compound through the functional group analysis, determinationof melting point and preparation of suitable derivatives.

ii. Separation of two component mixtures1) Aniline + Naphthalene 2) Benzoic acid + Benzophenone 3) p-Cresol +

Chlorobenzene.

4. Demonstration experiments:

1. Steam distillation experiment: separation of ortho and para nitro phenols 2) Microwaveassisted Green synthesis, two examples: 1. Hydrolysis of Benzamide 2. Oxidation of Toluene

63

Dr. V.S. Krishna Govt. Degree College, VISAKHAPATNAM-13Practical PAPER – IV (Physical Chemistry-IV)

Chemistry Practical Examinations at the END OF III Year / Sem-VITime: 3 Hours Max. Marks: 50LABORATORY COURSE – IV 90 hrs (3 h / w)

LABORATORY COURSE - IV

Practical Paper IV (Physical Chemistry) 90hrs (3 h / w)

1. Chemical kinetics

i. Determination of specific reaction rate of the hydrolysis of methyl acetate

catalyzed by hydrogen ion at room temperature.

ii. Determination of rate of decomposition of hydrogen peroxide.

iii. Determination of overall order of saponification of ethyl acetate

2. Distribution law

i. Determination of distribution coefficient of iodine between water and carbon

Tetrachloride.

ii. Determination of molecular status and partition coefficient of benzoic acid in

Toluene and water.

3. Electrochemistry

i. Determination of concentration of HCl conductometrically using standard NaOHsolution.

ii. Determination of concentration of acetic acid conductometrically using standard NaOHsolution.

iii. Determination of dissociation constant (Ka) of acetic acid by conductivitymeasurements.

iv. Determination of solubility and solubility product of BaSO4.

v. Determination of redox potentials of Fe2+/Fe3+by potentiometric titration of ferrousammonium sulphate vs. potassium dichromate.

4. pH metry

i. Preparation phosphate buffer solutionsii. pH metric titration of weak acid, acetic acid with strong base NaOH and calculation of

dissociation constant.5. Colorimetry

i. Verification of Beer-Lambert law for KMnO4 , K2Cr2O7 and determination ofconcentration of the given solution.

ii. Verification of Beer-Lambert law for CuSO4 and determination of concentration of thegiven solution.

iii. Composition of complex of Cu2+ - EDTA disodium salt

6. Adsorption

i. Surface tension and viscosity of liquids.ii. Adsorption of acetic acid on animal charcoal, verification of Freundlich isotherm.

64


Project Work

Collection of spectral data of a minimum of six compounds belonging to different functionalgroups (other than those included in the syllabus) and submission of the report at the END ofIII Year / Semester VI.

65


General Elective Food Science syllabi consist of 5 modules.This paper consists of 3 Sections,Section – A, Section – B and Section – C.

In Section – A: Six very short answer questions are to be set choosing one from MODULE I, 3from MODULE 2, 1 from MODULE 4 and 1 from MODULE 5 out of which 5 questions are tobe answered each question carries 2 Marks.

(2 X 5 = 10 Marks)In Section - B: Eight short answer questions are to be set choosing 1 from MODULE I, 4 fromMODULE 2, 1 from MODULE 3 and 2 from MODULE 4 out of which 5 questions are to beanswered each question carries 5 Marks.

(5X 5 = 25 Marks)In Section – C: Six essay questions are to be set choosing 1 from MODULE I, 4 from MODULE 2

and 1 from MODULE 5. Each question carries 10 Marks and four questions are to be answered.(4 X 10 = 40 Marks)

FOOD SCIENCE(General Elective for B. Sc., B. A., B. Com., students)

BLUE PRINT

Sl. No Name of the chapter 2 marks 5 marks 10 marksMODULE I: Introduction

1.Food 12.Water 13.Milk 1

MODULE 2: Constituents of foods1.Proteins 1 1 12 Carbohydrates 13.Lipids 14.Minerals 1 1 15 Vitamins 1 1 1

MODULE 3:Foods and Food Additives: 1 1

MODULE 4:Nutrition and Balanced Diet 2 1

MODULE 5:Food Adulteration and Hygiene 1 1

66

FOOD SCIENCEGeneral Elective for B. Sc., B. A., B. Com., students

No. of Credits: 2 No. of hours per week: 2Semester – IV Hours: 30 hrs

Objective: This Introductory course provides students with basic knowledge in Food Science

MODULE I: Introduction (4 h)

1.1 Food: Source, functions of food1.2 Water: Quality of Potable Water1.3 Milk: Composition and effectiveness as a diet. Fat content in milk, whole and skimmed.

MODULE 2: Constituents of foods (12 h)

2.1 Proteins: amino acids – peptides – proteins, modification of food products through heatprocessing.Effect of cooking, Sources & Functions of Proteins. Enzymes: Sources & Functions

2.2 Carbohydrates: Classification – Mono-saccharides glucose, fructose, Oligo(Di) -saccharidessucrose, maltose, lactose and Poly-saccharides starch.Artificial sweetening agents. Sources,Functions & Energy Cycle.

2.3 Lipids: Nomenclature and classification rancidity of fats & oils – function and storage of fats.

2.4 Minerals: Sources, functions, bioavailability and deficiency of the following minerals (calcium, iron, iodine, fluorine, sodium and potassium (elementarytreatment).

2.5 Vitamins - classification, sources, functions and deficiencies of fat- soluble vitamins – A, D, Eand K, water-soluble vitamins – C, thiamin, niacine, riboflavin, B-complex

MODULE 3: Foods and Food Additives: (8 h)

3.1 Food additives: Artificial sweeteners – saccharin, asparatame – food flavours . Antioxidants.Food colours – changes in cooking. Restricted use. Spurious colours. Preservatives – leaveningagents.Baking powder –Yeast. Taste enhancers – MSG-vinegar

MODULE 4: Nutrition and Balanced Diet (3 h)

4.1 Diseases associated with protein malnutrition. Nutritional value of carbohydrates. – Fibers in thediet, dietary sugars – nutritional aspects of lipids. Low cost nutrient supplements.

MODULE 5: Food Adulteration and Hygiene (3 h)

5.1 Adulterants: Common adulterants in different foods – milk and milk products, vegetable oils,and fats, spices and cereals, pulses, sweetening agents and beverages.

67


FOOD SCIENCE

General Elective for B.Sc., B.A., B. Com., students


Section –AAnswer all questions 2X5=10 marks

1. Write the composition of milk?

2. What are amino acids? Give one example?

3. Write two artificial sweetening agents?

4. What is florosis?

5. Write the dificency disease of vitamin C?

Section –BAnswer any Five questions 5X5=25 marks

6. What are the qualities of potable water?

7. What are enzymes. Explain the functions of enzymes with examples?

8. Write about the deficiency diseases of Calcium, Iron and Iodine?

9. Explain about classification of vitamins with examples?

10. Explain about diseases associated with protein malnutrition?

11. Write about food colors?

12. Explain about functions and storage of fats?

13. Explain about the importance of fibres in diet?

Section –CAnswer any FOUR questions 4X10=40 marks

14. Write about food sources and functions of food?

or

What are Proteins. Explain their functions?

15. Explain the classification of carbohydrates with examples?

or

Explain the sources, biological functions of sodium and potassium?

16. Explain the sources functions of vitamin A, B, C, D, E?

or

68

Write about the food adulteration of milk, oils, fats and pulses?

17. Write an essay on Artificial sweeteners?

or

Write an essay on low cost nutrient supplements?

69

Recommended Text Books and Reference Books:

Inorganic Chemistry:

1. Concise Inorganic Chemistry by J.D.Lee2. Basic Inorganic Chemistry by Cotton and Wilkinson3. Advanced Inorganic Chemistry Vol-I by Satyaprakash, Tuli, Basu and Madan4. Inorganic Chemistry by R R Heslop and P.L. Robinson5. Modern Inorganic Chemistry by C F Bell and K A K Lott6. University Chemistry by Bruce Mahan7. Inorganic Chemistry by J.E.Huheey8. Inorganic Chemistry by Chopra and Kapoor9. Coordination Chemistry by Basalo and Johnson10. Organometallic Chemistry – An introduction by R.C.Mehrotra and A.Singh11. Inorganic Chemistry by D.F.Shriver, P.W.Atkins and C.H.Langford12. Inorganic Chemistry by Philips and Williams, Lab Manuals13. Introduction to inorganic reactions mechanisms by A.C.Lockhart14. Theoretical inorganic chemistry by McDay and J.Selbin15. Chemical bonding and molecular geometry by R.J.Gillepsy and P.L.Popelier16. Advanced Inorganic Chemistry By Gurudeep Raj17. Analytical chemistry by Gary D Christian, Wiley India18. Analytical Chemistry by G.L.David Krupadanam, et al, Univ. Press19. Selected topics in inorganic chemistry by W.D.Malik, G..D.Tuli, R.D.Madan20. Concepts and models of Inorganic Chemistry by Bodie Douglas, D.McDaniel and

J.Alexander21. Modern Inorganic Chemistry by William L. Jolly22. Concise coordination chemistry by Gopalan and Ramalingam23. Satyaprakash’s modern inorganic chemistry by R.D.Madan.24. Qualitative Inorganic analysis by A.I.Vogel25. A textbook of qualitative inorganic analysis by A.I. Vogel

Organic Chemistry:

1. Organic Chemistry By R T Morrison and R.N.Boyd2. Organic Chemistry by T.J.Solomons3. Organic Chemistry by L.G.Wade Sr4. Organic Chemistry by D.Cram, G.S.Hammond and Herdricks5. Modern Organic Chemistry by J.D.Roberts and M.C.Caserio6. Text book of Organic Chemistry by Ferguson7. Problems and their solutions in organic Chemistry by I.L.Finar8. Reaction mechanisms in Organic Chemistry by S.M.Mukherji and S.P.Singh9. A guide book to mechanisms in Organic Chemistry by Peter Sykes10. Organic spectroscopy by J.R.Dyer11. Organic Spectroscopy by William Kemp12. Fundamentals of organic synthesis amd retrosynthetic analysis by Ratna Kumar Kar13. Comprehensive practical organic qualitative analysis by V.K.Ahluwalia & Sumta Dhingra

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14. Comprehensive practical organic chemistry: Preparation and quantitative analysis byV.K.Ahluwalia and Reena Agarwal.

15. Organic Chemistry by Janice Gorzynski16. Organic Chemistry by Stanley H Pine17. Fundamentals of Organic Chemistry by John Mc Murray, Eric Simanek18. Organic Chemistry by Francis A Carey19. Text book of Organic Chemistry by K.S.Mukherjee20. Organic Chemistry by Bhupinder Meha & Manju Mehta21. Organic Chemistry by L.G.Wade Jr, Maya Shankar Singh22. Elementary organic spectroscopy by Y.R. Sharma23. Chemistry & Industry by Gurdeep R. Chatwal24. Applied Chemistry by Jayashree Ghosh25. Drugs by David Krupadanam26. Pharmacodynamics by R.C.Srivastava, Subit Ghosh27. Analytical Chemistry by David Krupadanam28. Green Chemistry – V.K.Ahluwalia29. Organic Synthesis by V.K.Ahluwalia and R.Agarwal30. New trends in Green Chemistry –by V.K.Ahluwalia & M.Kidwai31. Industrial Chemistry by B.K.Sharma32. Industrial Chemistry by Banerji33. Industrial Chemistry byM.G.Arora34. Industrial Chemistry by O.P.Veramani & A.K.Narula35. Synthetic Drugs by O.D.Tyagi & M.Yadav36. Medicinal Chemistry by Ashutoshkar37. Medicinal Chemistry by P.Parimoo38. Pharmacology & Pharmacotherapeutics by R.S Satoshkar & S.D.Bhandenkar39. Medicinal Chemistry by Kadametal P-I & P.II40. European Pharmacopoeia41. Vogel’s Qualitative organic analysis.42. Laboratory manual of Organic Chemistry by Raj K Bansal

Physical chemistry books:

1. Physical chemistry A molecular approach by Donald A. Mcquarrie andJohn D. Simon.

2. Physical chemistry by G M Barrow3. Principles of physical chemistry by Prutton and Marron4. Physical chemistry by Peter Atkins, Julio D. Paula5. Physical Chemistry by Ira N Levine

6. Elements of Physical Chemistry by Peter Atkins, Julio D. Paula

7. Text book of Physical Chemistry by P.L.Soni, O.P.Dharmarha and Q.N.Dash

8. Solid State Chemistry and its applications by Anthony R. West9 Text book of physical chemistry by K L Kapoor

10. Thermodynamics for Chemists by S Glasston

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11. Chemical Kinetics by K J Laidler12. An Introduction to Electrochemistry by S Glasston13. Physical chemistry through problems By S K Dogra14. Thermodynamics by J Jayaram and J C Kuriakose15. Introductory Quantum Chemistry by A K Chandra16. Physical Chemistry by J W Moore17. Kinetics and mechanism by J W Moore and R G Pearson18. Fundamentals of photochemistry by K K Rohtagi Mukharjee19. Chemical thermodynamics by R P Rastogi and S S Misra20. Advanced physical chemistry by Gurudeep Raj21. Physical chemistry by G W castellan22. Physical chemistry by Silbey, Alberty and Bawendi.23. Elements of physical chemistry by Glasstone and Lewis24. Text book of physical chemistry by S Glasstone25. Fundamentals of Molecular spectroscopy by C.N.Banwell and E.M.McCash26. Nanochemistry by Geoffrey Ozin and Andre Arsenault27. Catalysis: Concepts and green applications by Gadi Rotherberg28. Green Chemistry: Theory and practice by P.T.Anastas and J.C.Warner29. Polymer Science by Gowriker, Viswanathan and Jayadev Sridhar30. Introduction polymer Chemistry By G.S.Misra31. Polymer Chemistry by Bilmayer32. Kinetics and Mechanism of Chemical Transformations by Rajaram and Kuriacose.33. Senior practical physical chemistry by Khosla

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DEPARTMENT OF CHEMISTRYDr. V. S. KRISHNA GOVT.DEGREE (A) & P. G. COLLEGE, VISAKHAPATNAM.

List of paper setters and paper evaluators

S.No Name of the Faculty Name of the college

1. Sri. Y. Vamsi kumar M.R. College, Vizanagaram

2. Dr. G. Venkateswara Rao Mrs. A.V.N. College, Visakhapatnam

3. Sri E.V.Subramanyam P.R.College, Kakinada

4. Sri G.Satyanarayana P.R.College, Kakinada

5 Mahaboob Pachcha P.R.College, Kakinada

6. Dr. Sambasiva Rao Govt. Arts College, Rajahmundry

7. Sri Machi Raju Govt. Arts College, Rajahmundry

8. Dr. Ranga Rao Govt. Arts College, Rajahmundry

9. Sri. T.Narisimha Murthy Govt. Arts College, Rajahmundry

10. Smt. D.Sunita Govt. Arts College, Rajahmundry

11. Dr.G.Vayu Kumar GDC(M), Srikakulam

12. I.Neelam Naidu GDC(M), Srikakulam

13. Sri. D.Satya Prasad GDC(M), Srikakulam

14. Sri. M.Upendra Rao GDC, Sabbavaram

15. Smt.Ch. Anuradha GDC (W), Visakha patnam

16. Sri. A.V. Ramesh GDC, Chodavaram

17. Smt J.Lakshmi Mangamma. S.G.A.G.D.C.Yellamanchili

Documents

DEPARTMENT OF CHEMISTRY Semester wise …drvskrishnagdc.edu.in/syllabus/chemistry_2014_15.pdfDEPARTMENT OF CHEMISTRY Semester wise syllabus & Model Question Papers With Effect from