B.Sc. Chemistry Question paper

“Loyola College B.Sc. Chemistry April 2008 Physics For Chemistry – II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FG 9

 

THIRD SEMESTER – APRIL 2008

PH 3202 / 3200 – PHYSICS FOR CHEMISTRY – II

 

 

 

Date : 05/05/2008                Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART-A

 

Answer all questions                                                                                            10×2=20marks

  1. What are flip flops?
  2. What is the difference between full and half adder.
  3. State Pauli’s exclusion principle.
  4. Give any two industrial applications of x-rays.
  5. Calculate the binding energy of a Deutron. Given 1P1=1.0081amu, 0n1=1.00893amu,

1H2=2.01473amu.

  1. Describe Proton and Neutron using quark model.
  2. State the laws of transverse vibrations of strings.
  3. Mention two properties of ultra sonic waves.
  4. State Heisenberg’s uncertainty principle.
  5. Mention two situations where classical mechanics fails.

 

PART-B

Answer any four questions                                                                               4×7.5=30marks

 

  1. Explain the working of a 3 bit counter using flip flops.
  2. Explain the main aspects of photo electric effect using Einstein’s equation.
  3. What are elementary particles? How they are classified?
  4. How will you determine the velocity of sound waves in gas?
  5. Obtain the energy of a particle in a one dimensional box.

 

PART-C

Answer any four questions                                                                               4×12.5=50marks

  1. Explain the truth table of a full adder with a neat circuit.
  2. State the postulates of Bohr atom model. Obtain expressions for the radius and energy of

the nth orbit.

 

  1. Explain semi empirical mass formula for the binding energy of the nucleus.
  2. a) Explain how ultra sonic waves are generated by using piezo electric effect? (9.5)
  3. b) Mention any two uses of ultra sonic waves. (3)
  4. a) With relevant theory, explain Davison and Germer experiment for diffraction of

electrons.(10)

 

  1. b) Calculate De Broglie wave length of an electron accelerated through a potential of

150 volts.(2.5)

 

 

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“Loyola College B.Sc. Chemistry April 2008 Physical Chemistry – II Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

           B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 18

FIFTH SEMESTER – APRIL 2008

CH 5500 – PHYSICAL CHEMISTRY – II

 

 

 

Date : 28-04-08                  Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

part – a

            Answer all questions.                                                            (10 ´ 2 = 20 marks)

 

  1. Why can’t you use NaCl in salt bridge preparation of a galvanic cell?
  2. For the cell reaction at 25° C, Zn½Zn2++½½Cu2+½Cu     E°cell = 1.10 V

Calculate equilibrium constant for the  reaction.

  1. Define molar conductance of a solution.
  2. What is transport number?
  3. Calculate the ionic strength of 0.01 M KNO3
  4. 30% of a zero order is complete in 100 min. How long will it take for 60% completion of the reaction?
  5. Mention the steps involved in a chain reaction
  6. Differentiate adsorption from absorbtion
  7. Mention the significance of the equation q =
  8. State Grotthus – Drapper’s law.

 

PART – B

            Answer any EIGHT questions.                                            (8 x 5 = 40 marks)

 

  1. Derive Nernst equation for a cell reaction.
  2. Calculate E°cell, Ecell, DG°cell and DGcell for

Cu½Cu2+(0.01 M)½½Ag+(0.001 M)½Ag at 298 K.  E°red  Cu2+½Cu and Ag+½Ag are 0.34 V

and 0.8 V respectively.

  1. Explain the construction and working of calomel electrode.
  2. State and explain Kohlrausch’s law of independent migration of ions.
  3. Write the electrode reactions and the net reaction of lead storage cell when it serves as source of current.
  4. Explain the principle of conductometric acid-base titrations with an example.
  5. Explain the mechanism of bimolecular surface reaction.
  6. How does Λ vary with concentration for

(i) strong electrolyte        (ii) weak electrolyte

  1. The rate of a reaction is doubled on increasing the temperature from 25° C to 35°  Calculate the activation energy of the reaction.  (R = 8.314 JK-1mol-1).
  2. Derive an expression connecting rate constant and concentration of a II order5 reaction of the type 2A ®
  3. Differentiate (i) order from molecularity (ii) EMF and potential difference.           (3 + 2)
  4. Define quantum yield of a photochemical reaction. How is it determined?                        (2 + 3)

 

 

 

PART-C

   Answer any FOUR questions.                                                            (4 ´ 10 = 40 marks)

 

23.(a) Explain any two methods of determining order of a reaction.       (6)

(b) t1/2 of C-14 is 5770 years.  Calculate the rate constant.  Starting from 100 mg
of  C-14 how much of it will remain at the end of 17,310 years.              (4)

  1. Discuss the kinetics of unimolecular reaction with relevant derivation of the rate law.
  2. Explain any two of the following: (5 + 5)

(a) Quinhydrone electrode and its use.

(b) Evaluation of thermodynamic quantities from EMF data.

(c) H2-O2 fuel cell.

(d) Determination of Ksp using conductometry.

  1. (a) Explain how transport number of an ion be determined using moving
    boundary method?

(b) Explain the functioning of glass electrode.

  1. Explain any two of the following:

(a) Electrochemical series

(b) Cells with transference

(c) Determination of EMF

(d) Weston Cadmium cell

28.(a) Explain the postulates of Langumir adsorption isotherm and hence derive the
equation.

(b) Write briefly on photosensitisation.

 

 

 

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“Loyola College B.Sc. Chemistry April 2008 Physical Chemistry – I Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 10

 

THIRD SEMESTER – APRIL 2008

CH 3500 – PHYSICAL CHEMISTRY – I

 

 

 

Date : 26/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

part – a

            answer ALL the questions.                                                 (10 ´ 2 = 20 marks)

 

  1. Write van der Waal’s equation for ‘n’ moles of the gas and mention the terms involved.
  2. Calculate DS for the vapourisation of 1 mole of H2O(l) at 373 K.

DHvap = 9720 cal/mol.

  1. State Hess’s law of constant heat summation.
  2. What is the effect of pressure on the system PCl5(g) ⇌ PCl3g) + Cl2g) at equilibrium?
  3. What is chemical potential? Is it extensive or intensive?
  4. State reduced phase rule equation.
  5. State Henry’s law.
  6. What are colligative properties? Give two examples.
  7. Define partition coefficient.
  8. What is meant by thermodynamic equilibrium constant?

 

PART – B                             (8 ´ 5 = 40 marks)

              Answer any EIGHT questions.

 

  1. State any five postulates of kinetic theory of gases.
  2. Derive Gibb’s-Helmohltz equation.
  3. Draw the phase diagram for water system and apply the phase rule equation to any one point, one line and one area.
  4. 1 mole of an ideal, monoatomic gas expands isothermally and reversibly at 27°C from 10 to 100 lit. Calculate q, w, DE, DH and D
  5. Differentiate bond energy from bond dissociation energy with a specific example.
  6. State Raoult’s law and explain positive deviation from it.
  7. How is osmotic pressure of a solution determined experimentally?
  8. Derive the relation DG = DG° + RT ln Q and hence deduce an expression for thermodynamic equilibrium constant.
  9. State III law of thermodynamics and explain.
  10. Explain the phase diagram of phenol-water system.
  11. Calculate the freezing point of 0.01 m aqueous solution of K4[Fe(CN)6] assuming 80% ionization. kf for H2O is 1.86 K kg mol-1.
  12. Derive Nernst distribution law.

 

 

PART – C

            Answer any FOUR questions.                                 (4 ´ 10 = 40 marks)

 

  1. Derive Maxwell equations from first principle.
  2. Deduce van der Waal’s equation.

 

  1. Derive any two of the following. (5 + 5)

(a) PVg = constant                              (b) Kirchoff’s equation

(c) relation between Kp and Kc             (d)

  1. Draw the phase diagram of a simple eutectic system and discuss its salient features.
  2. Derive thermodynamically the relation connecting elevation of boiling point of a solution and molality.
  3. Explain any two of the following: (5 + 5)

(a) Gibb’s phase rule equation            (b) Azeotropes

(c) Joule-Thomson coefficient           (d) van’t Hoff factor.

 

 

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“Loyola College B.Sc. Chemistry April 2008 Organic Functional Groups – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 11

 

THIRD SEMESTER – APRIL 2008

CH 3502 – ORGANIC FUNCTIONAL GROUPS – I

 

 

 

Date : 26/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

                                                                        (10 x 2 = 20 marks)

Answer ALL the questions.

  1. Explain why 10 alkyl halides undergo nucleophitic substitution only by SN2.
  2. Name the products obtained in the addition of HBr to propere in the absence and presence of peroxide.
  3. What happens when acetophenone is treated with I2 / NaOH?
  4. Why p-nitrophenol has higher boiling point than o-nitrophenol?
  5. What are mixed ethers? Give examples.
  6. How is anisole prepared? What happens when anisole is treated with excess of HI?
  7. Name the products obtained form 2-hexanone in Norrish type II reaction.
  8. What is Cannizzaro’s reaction?
  9. Compare and account for the acidity of acetic acid, prop ionic acid and chloroacetic acid.
  10. What is the action of heat on malonic and succinic acids?

 

PART – B

                                                                        (8 x 5 = 40 marks)

Answer any EIGHT questions.

  1. Give any two methods of preparation of chlorobenzene. Starting from chlorobenzene how are the following compounds prepared?
  1. a) o-dichlorobenzene b) aniline      c) DDT
  1. Discuss the effect of nature of substrate, nucleophile and solvent in nucleophilic substitution.
  2. a) Account for the acidity of phenol
  1. b) How would you prepare the following compounds from phenol?
  2. i) o – Cresol ii) Benzene iii) Phenyl acetate.
  1. Explain the nitration of Phenol with Mechanism.
  2. How are alcohols prepared by hydroboration method? Give the mechanism of the reaction.
  3. a) Why are ethers less reactive than epoxides?
  1. b) How is ethylene oxide prepared? How does it react with methanol and ammonia?
  1. a) Write the IUPAC names of ethyl methyl ether and anisole.
  1. b) Give any two methods of preparation of diethyl ether. Mention a reaction where ether behaves as a Lewis base.
  1. What is Reformatsky reaction? How is it useful in organic synthesis?
  2. Discuss Norrish type I reaction.
  3. Give the products of the following reactions.
  1. Benzaldehyde +
  2. Acetaldehyde + Malonic ester
  3. Benzaldehyde
  4. Acetone +
  5. Acetaldehyde +Malonic ester

 

  1. a) What is meant by transesterification?
  1. b) Discuss the action of heat on and – amino acids.
  1. Give any two methods of preparation of adipic acid. Write its IUPAC name. How would you convert adipic acid into cyclopentanone and NYLON-6,6?

 

PART – C

                                    (4 x 10 = 40 marks)

Answer any FOUR questions.

  1. Explain E1 mechanism of dehydrohalogenation of alkyl halides. Discuss the orientation and reactivity of alkyl halides in dehydrohalogenation.
  2. a) Identify the products in the following sequence of reactions

Isopropyl alcohol ABC D

  1. b) Discuss the following reactions of phenol
  2. i) Coupling reaction ii) Reimer – Tiemann reaction
  1. a) Explain Williamson’s synthesis of ethers with mechanism.
  1. b) Discuss the cleavage of ethers with HI
  1. Discuss the following reactions with mechanism
  1. a) Wittig reaction b) Benzoin condensation
  1. a) How do you convert benzaldehyde into cinnamaldehyde? Explain with mechanism.
  1. b) Arrange the following compounds in the increasing order of acidity. Give reason. Benzoic acid, p-toluic acid, p-nitrobenzoic acid and p-chlorobenzoic acid.
  1. a) How is acetyl chloride prepared from acetic acid? How are the following compounds prepared from acetyl chloride?
  1. Acetaldehyde ii) Acetophenone  iii) Acetone
  2. b) Give the mechanism of esterification.

 

 

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“Loyola College B.Sc. Chemistry April 2008 Organic Chemistry – II Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 54

 

FOURTH SEMESTER – APRIL 2008

CH 4500 – ORGANIC CHEMISTRY – II

 

 

 

Date : 26/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 
Part-A

                                                     Answer ALL questions.                              (10 ´ 2 = 20)

 

  1. ‘cyclopropane is more reactive than cyclohexane’. Why?
  2. What are the conformers possible for cyclohexane? Which one is more stable? Why?
  3. How would you distinguish methanol from ethanol by means of chemical tests?
  4. ‘Williamson’s synthesis is useful for the preparation of both simple and mixed ethers’. Justify this statement with suitable examples.
  5. Arrange the following in the increasing order of their acidity. Justify your answer.

Monochloroacetic acid, Dichloroacetic acid, Acetic acid, Formic acid and Trichloro acetic acid.

  1. What happens when maleic acid is treated with bromine? Identify the stereochemistry of the product obtained?
  2. Name the electrophile in nitration of benzene. What are the evidences for its existence?
  3. ‘Aniline does not undergo Friedel-Craft’s reaction’. Why?
  4. How would you prepare the following from benzene diazonium chloride?
    (i) Benzene   and  (ii) Benzoic acid
  5. Give the mechanism of Reimer-Tiemann reaction.

 

Part-B

                                                 Answer any EIGHT questions.                      (8 ´ 5 = 40)

 

  1. Explain Baeyer’s strain theory in the stability of cycloalkanes.
  2. How are alcohols prepared from hydroboration-oxidation method? Explain with mechanism.
  3. An amide(A) having molecular formula C3H7ON on hydrolysis gives an acid C3H6O2(B). (B) on chlorination in the presence of red phosphorus produces a chloroacid(C).The latter on boiling with aqueous NaOH and subsequent acidification forms lactic acid(D).Write the reactions and identify the structure of A, B, C and D.
  4. What happens when benzaldehyde is heated with alcoholic KCN solution? Explain the mechanism.
  5. How would you prepare 4-methylpentanoic and 3-methylbutanoic acid using diethyl malonate?
  6. Explain the mechanism of Hofmann-bromamide reaction. Name the intermediate in this reaction.
  7. ‘Nitration of benzene is irreversible while sulphonation of benzene is a reversible reaction.’ Explain.
  8. What are sulpha drugs? Explain the mechanism of action of  sulpha durgs.
  9. What happens when 3-bromo-2, 3-dimethyl pentane is treated with alcoholic KOH? Identify the different products obtained and explain with mechanism.
  10. Explain the mechanism of Baeyer-Villiger rearrangement.
  11. Explain the synthetic utility of acetoacetic ester with examples.
  12. Explain aromaticity, antiaromaticity and nonaromaticity with suitable examples.

 

 
 
Part-C

                                                 Answer any FOUR questions.                       (4 ´ 10 = 40)

 

  1. a) Explain the mechanism of reduction of CH3COOC2H5 by LiAlH4.
  2. b) Compare the stereochemistry of products obtained in Sn1 and Sn2 reactions.
  3. a) How are grignard reagents used in the preparation of primary, secondary and     tertiary alcohols? Explain with suitable examples.
  4. b) Explain the mechanism of preparation of ethers by oxymercuration-    demercuration method.
  5. a) How are the following compounds prepared?
    (i) acrylic acid             (ii) cinnamic acid      (iii) maleic acid
  6. b) Explain the action of heat on a-, b- and g-hydroxy acids and identify the     products obtained.
  7. a) Explain the mechanism of sulphonation of benzene
  8. b) ‘Halogens are deactivating groups but o-, p- directing’.
  9. a) How will you synthesise the following compounds from benzaldehyde?

(i) Mandelic acid         (ii) m-Benzaldehydesulphonic acid

  1. b) Write a note on: (a) Cannizaro reaction (b) Perkin reaction
  2. a) Explain Claisen and abnormal Claisen rearrangements with mechanism.
  3. b) How would you convert m-nitrophenol from nitrobenzene? Explain all the steps involved in this process.

 

 

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“Loyola College B.Sc. Chemistry April 2008 Natural Products Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 24

 

SIXTH SEMESTER – APRIL 2008

CH 6604 – NATURAL PRODUCTS

 

 

 

Date : 23/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer all the questions.                                          (10  ´ 2   = 20)

 

  1. Write the products obtained when anthracene is reduced using sodium –amalgam and isopentanol.
  2. Give the name and structure of any two very potent cancer producing polycyclic hydrocarbons.
  3. Give the products obtained when pyridine reacts with sodium amide.
  4. How wil you determine the number of double bonds present in the alkaloid piperine.
  5. What is isoprene rule ? Indicate the isoprene units in the structure of citral.
  6. How will you synthesize α- terpineol from α -pinene.
  7. What are purines ? Write the structure of Caffeine.
  8. Give any two biological importance of anthocyanins.
  9. Write the products obtained when uric acid is oxidized using dil.HNO3.
  10. Write the structure of cyanidine chloride

 

PART – B

Answer any Eight questions                     (8  ´  5   = 40)

 

  1. How will you synthesize anthracene from Phthalic anhydride using Friedel – Craft’s reaction.
  2. Complete the following reactions.

 

  1. i. How is thiophene manufactured from acetylene ?
  2.       How will you synthesise quinoline using Skraup’s synthesis method.
  3. i. Explain why are pyrrole,furan and thiophene classified as aromatic compounds.
  4.          How will you prepare pyridine from pyrrole.
  5. Identify the products in the following reactions.
  6. Quinoline               A
  7. Pyridine   +   Acetyl chloride     B

iii.     Pyridine   +  C6H5 Li     C

  1. i. What happens when citral is subjected to oxidation with Alk. KMnO4 followed by chromic acid? Write the name and structure of the products formed.
  2. What happens when menthol is heated with KHSO4
  3. Briefly discuss the constitution of Geraniol.
  4. i. What are terpenes ?  How are they classified ?
  5.   How will you establish the position of double bonds in citral.
  6. Write short notes on Flavones and Flavonoids.
  7. Give any one method for the synthesis of cyanidine chloride.
  8. How will you synthesize Xanthine from urea using Traube’s method.
  9. i. What are the products obtained when Caffeine is oxidized using potassium chlorate in HCl.
  10.   How will you synthesize Caffeine from uric acid using Fischer method.
PART – C

Answer any four questions.                                 ( 4 ´ 10 = 40 )

 

  1. Elucidate the structure of phenanthrene. Confirm it by Haworth and Pschorr’s synthesis.
  2. i. Deduce the orbital structure of pyrrole.
  3. Give any one method for the synthesis of piperine.
  4. Elucidate the structure of menthol.
  5. What are anthocyanins? Discuss the structure and any two general methods of synthesis of anthocyanins.
  6. Establish the structure of iso-quinoline.
  7. Elucidate the structure of uric acid.

 

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“Loyola College B.Sc. Chemistry April 2008 Main Group Elements & Solid State Chemistry Question Paper PDF Download”

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FG 12

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

           B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2008

    CH 3503 – MAIN GROUP ELEMENTS & SOLID STATE CHEMISTRY

 

 

 

Date : 29-04-08                  Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART – A

Answer ALL the questions.                                                             (10 x 2 = 20 marks)

  1. Indicate two uses of Lithium compound.
  2. What is the role of K+ ion in biological systems.
  3. Explain the amphoteric behaviour of Aluminium.
  4. What are the raw materials used in manufacture of glass.
  5. Explain the basicity of orthophosphoric acid.
  6. How do you prepare Caro’s acid? Write its structure.
  7. F2o is called as oxygen difluoride while Cl2O is named as chrorine oxide. Give reasons.
  8. Discuss the structure of IF5.
  9. Draw 110, 111 planes.
  10. What is the importance of radius ratio in ionic crystal? Give an example.

 

PART – B

Answer any EIGHT questions.                                            (8 x 5 = 40 marks)

  1. How does Li differ from other elements of first group?
  2. Describe ‘Wrap Around’ complexes of alkali metal ions.
  3. What are election deficient compounds? Discuss the bonding and structure of diborane.
  4. Write a note on classification of carbides.
  5. How do you prepare (a) Hydrazine  (b) Hydroxylamine in the laboratory? Indicate two chemical reactions for each.
  6. Write the manufacture of (a) Superphosphate of lime  (b)  triple superphosphate.
  7. Describe the preparation of Marshall’s acid by anodic oxidation of H2SO4. Write its structure.
  8. Write a note on Psuedohalogens.
  9. Discuss the structure of Oxoacids of halogens? What is their relative acid strength?
  10. Derive Bragg’s equations.
  11. Describe the structure of (a) zinc blende  (b)  wurtzite.
  12. What are Frankel defects? Explain with two examples.

 

PART – C

Answer any TWO questions.                                                           (2 x 20 = 40 marks)

  1. (a) Describe the extraction of Beryllium from its ore.                                    (5)

(b) Write a note on organometallic compounds of Li and Be.                       (5)

  1.  What are silicates? How are they classified? Describe the structure of various types of silicates.
  2. How do you prepare (a) Hyponitrous acid (b) Pernitric acid  (c)  Pyrophosphoric acid  (d) metaphosphoric acid.  (e)  dithionic acid?
  3. a) How is ozone prepared? Describe its structure                                           (4)
  1. b) State different types of oxides with one example each. (6)
  1. a) Discuss the preparation and structure of
  1. ICl (ii) BrF3  (iii) BrF5                                                   (6)
  2. b) How do you estimate available chlorine in bleaching powder? (4)
  1. (a) Discuss the structure of (i) Rutile (ii) Fluorite                                           (5)

(b) What are different crystal systems. Give an example for each.                (5)

 

 

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“Loyola College B.Sc. Chemistry April 2008 Inorganic Chemistry – II Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 55

 

FOURTH SEMESTER – APRIL 2008

CH 4501 – INORGANIC CHEMISTRY – II

 

 

 

Date : 29/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

            PART-A

Answer all the questions                                                           (10 ´ 2 = 20)

  1. What are the basic chemical changes observed in roasting of an ore?
  2. Give any two examples for reduction of an oxide ore.
  3. Why do d-block elements exhibit variable oxidation states?
  4. What happens to the mercuric salt when it acts as a reductant?
  5. Write the IUPAC nomenclature of the following complexes.

(i)  K[Ag(CN)2]  and   (ii)  [Pt(NH3)4NO2Cl]CO3

  1. Define electroneutrality principle.
  2. What is induced radioactivity? Give an example.
  3. Write the role of moderators in nuclear reactor.
  4. Give any two differences between amorphous and crystalline substances.
  5. How are silicates classified?

PART-B

Answer any eight questions                                                    (8 ´ 5 = 40)

  1. Write a note on Ellingham diagram.
  2. What are the various processes used in the concentration of ores? How would you concentrate an ore using froath floatation process?
  3. What are transition metals? Discuss their position in the periodic table.
  4. How is uranium extracted from its ore?
  5. Explain the following with an example.
  6. Ionization isomerism
  7. Ligand isomerism
  8. Explain the postulates of valence bond theory of coordination complexes.
  9. What are Magic numbers? What are their importance in the stability of nuclei?
  10. Discuss the precipitation and conductivity methods for the study of complexes.
  11. Describe the methods involved in the detection of radioactivity?
  12. What is meant by nuclear fission? Write a note on chain reaction.
  13. Explain the conductance and metallic luster of metals using metallic bond theory.
  14. Derive Bragg’s law.

PART-C

Answer any four questions                                                   (4 ´ 10 = 40)

 

  1. Explain the different techniques employed for refining of metals.
  2. a) Discuss the lanthanide contraction and its consequences. (7)
  3. b) Give the equations for the application of Cr(VI) and Mn(VII) as oxidants.                        (3)
  4. a) State the postulates of Werner’s theory of coordination compounds. Illustrate with one

example                                                                                                                         (6)

  1. b) Calculate EAN of the metals in the following complexes.

(i) K4[Fe(CN)6]                                 (ii) [Ni(CO)4]                           (4)

  1. a) What are the assumptions of Crystal field theory? (4)
  2. b) Discuss the splitting of d- orbitals in the case of square planar complexes.              (6)
  3. Discuss the application of nuclear energy in various fields.
  4. a) How will you find the following for fcc and bcc crystals?                                      (6)
  • Number of atoms in a unit cell
  • Packing fraction
  • Coordination number
  1. b) Draw and explain (100), (111), (101) and (001) planes.                                           (4)

 

 

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“Loyola College B.Sc. Chemistry April 2008 Inorganic Chemistry – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 1

 

FIRST SEMESTER – APRIL 2008

CH 1500 – INORGANIC CHEMISTRY – I

 

 

 

Date : 03/05/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

                                                                        (10 x 2 = 20 marks)

Answer ALL the questions.

  1. What is the relationship between ionization potential of the element and election affinity of an element in formation of an ionic bond between the elements?
  2. Is it possible to have anion, Why?
  3. What is the shape of ClF3? Draw the structure.
  4. He2 does not exist. Why?
  5. What are clathrates? Give example.
  6. The boiling point of HCl is –85.00C while that of HF is + 19.40C. Explain.
  7. Label as Acid or Base: Cl–, BF3, Ag+, AlCl3.
  8. What are aprotic solvents? Give two examples.
  9. How do you prepare pernitric acid? Write its structure.
  10. What is oleum? How is it prepared?

PART – B

                                                                        (8 x 5 = 40 marks)

Answer any EIGHT questions.

  1. Define lattice energy? Explain the factors which affect lattice energy.
  2. Discuss the relationship between electronegativity difference and partial covalent character of an ionic compound. What is its effect in molecules?
  3. Describe the hybridizations involved and structure of (a) BeF2         (b) PCl5
  4. Draw MO energy lavel diagram for NO molecule. Calculate the bond order in NC.
  5. State VSEPR theory. Explain the structure of ICl4 using VSEPR theory.
  6. Write a note on van der Waal’s forces.
  7. What are different types of Hydrogen bonding? Explain their influence on the properties of compounds with proper examples.
  8. Explain the Solvent-System concept of an acid and a base. What are its limitations?
  9. Discuss any four types of reactions using liquid ammonia as a solvent.
  10. How do you prepare (a) N2O3    (b) Hyponitrous acid. Discuss their structure.
  11. How do you prepare Marshall’s acid from Sulphuric acid? Draw its structure.
  12. Give an comparitive account of the hydrides and halides of Nitrogen group elements.

PART – C

                                    (4 x 10 = 40 marks)

Answer any FOUR questions.

  1. (a)  For HCl molecule the internuclear distance is 127 pm; actual dipole moment

is 3.44 x 10-30 coulomb meter. Calculate the percent ionic character of HCl.(5)

(b) How do you determine the lattice energy of an ionic compound using Bon-Haber cycle?    (5)

  1. (a)  Draw MO energy level diagram of CO molecule. Calculate the bond order (5)

(b)  Using VSEPR theory, describe the structure of (i) SF6 (ii) XeF6                  (5)

  1. (a)  Of the species O2, O2+, O2– and O22-, which will have maximum bond strength? Explain. (5)

 

(b) What is the action of heat on

(i) Phosphorus acid        (ii) orthophosphoric acid

(iii) metaphosphoric acid                                                                 (5)

  1. (a)  What is band theory of a metal?                                                                    (2)

(b)  How does band theory explain the property of a metal, semiconductor and insulator?                                                                                                                                           (8)

  1. (a) Explain conjugate acid – base concept with two examples                            (5)

(b) Write a note on hard and soft acids and basis.

  1. (a) Write a note on nitrogen fixation.                                                                  (4)

(b) Complete the following with balanced equation.                                          (6)

  • Sulphuric acid + Phosphorus pentachloride ®?

(ii) Potassium persulphate + Con. Sulphuric acid®?

(iii) Zinc + dil. nitric acid®?

 

 

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“Loyola College B.Sc. Chemistry April 2008 Hydrocarbons And Stereochemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 7

 

SECOND SEMESTER – APRIL 2008

CH 2502 – HYDROCARBONS AND STEREOCHEMISTRY

 

 

 

Date : 23/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

Answer ALL the questions                                                                            (10 x 2 = 20 marks)

 

  1. Define homolytic cleavage with an example.
  2. Explain why nitromethane is soluble and nitrobenzene is insoluble in NaOH.
  3. How would you covert n-butane into isobutane?
  4. Arrange the following alkanes in the increasing order of their boiling points

n– hexane, n-pentane, 2-methyl pentane.

  1. Name the products obtained when 2-methyl -2- butene is subjected to ozonolysis.
  2. Explain why is the chair form of cyclohexane more stable than the boat form.
  3. Among ortho, meta and para-dichlorobenzenes, which isomer has the highest dipole moment?  Why?
  4. Write down the combustion reaction of benzene.
  5. Write the E, Z notation of the following compounds.

 

 

  1. Mention any two differences between tautomerism and resonance.

 

                                                                        PART – B

Answer any EIGHT questions                                                                 (8 x 5 = 40 marks)

 

  1. What are the requirements for a compound to be aromatic?
  2. Discuss keto-enol tautomerism with an example.
  3. Explain Dieckmann’s ring closure reaction.
  4. Discuss Baeyer’s strain theory of ring compounds.
  5. Discuss on the relative stability of dienes.
  6. Explain the Saytzeff’s rule in elimination reactions.
  7. How is acetylene prepared?  How does it react with   a) HCN   b) Excess of HBr
  1. c) Acetic acid
  1. Give the preparation, properties and uses of naphthalene.
  2. Explain why – OH group is activating and o, p-directing where as -No2 group is deactivating and m-directing.
  3. Discuss the conformations of n-butane.
  4. What are geometrical isomers?  How do the two isomers differ in their physical and chemical properties?
  5. What are conformers?  How many conformers are possible for ethane?  Comment on their relative stabilities.

PART – C

Answer any FOUR questions                                                                  (4 x 10 = 40 marks)

 

  1. a) Compare the basicities of 1o, 2o and 3o amines with that of NH3.  Give reason.           (6)

 

  1. b) Arrange primary, secondary and tertiary carbocations in the increasing order of their

stabilities and explain.                                                                                                   (4)

 

  1. a) How are alkanes prepared by Wurtz and House – Corey methods?                             (4)

 

  1. b) How are the following conversions effected? (6)
    1. n-hexane into benzene
    2. methane into nitromethane
  • propene into n-propyl bromide
  1. Ethylene into ethylene glycol.

 

  1. Write notes on the following:
  1. Markownikoff’s rule
  2. Allylic bromination by NBS
  • Hydroboration
  1. Diels – Alder reaction

 

  1. a) How is benzene prepared and purified in the laboratory?                                             (6)
  1. b) Starting form benzene how are the following compounds prepared?
  2. i) Acetophenone
  3. ii) 1,3,5-Trinitrobenzene                              (4)

 

  1. Explain the following with examples
  1. Addition polymerization        (3)
  2. Zeigler – Natta polymerization        (4)
  • Dehydrohalogenation        (3)

 

  1. Discuss on the conformers of disubstituted cyclohexane and explain 1,2 and 1,3 interactions.

 

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“Loyola College B.Sc. Chemistry April 2008 General Chemistry For Physics & Maths Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034B.Sc. DEGREE EXAMINATION – MATHEMATICS & PHYSICSSECOND SEMESTER – APRIL 2008CH 2102 – GENERAL CHEMISTRY FOR PHYSICS & MATHS (Also Equal CH 2100/3100)
Date : 25/04/2008 Dept. No.         Max. : 100 Marks                 Time : 1:00 – 4:00                                               PART-A                                                          Answer ALL the questions        (10 × 2 = 20)1. Write the IUPAC nomenclature for the following complexes.a. [Co(en)2Cl2]+          b.  K4[Fe(CN)6]2. Why the transition metal ions are coloured?3. Which type of substitution reaction do the primary alkyl halides undergo? Give reason.4. Tertiary amines are comparatively less basic than secondary amines. Give reason.5. Calculate the degrees of freedom for the following reaction.                                   CaCO3(s)    ⇌   CaO(s)+ CO2(g)6. State Beer-Lambert’s law.7. Draw the structure of thyroxine and mention any two functions.8. Mention the functions of different  types of RNA.9. How is Neoprene prepared?10. What are the drawbacks of crude natural rubber?PATR-B                                                      Answer any EIGHT questions      (8 × 5 = 40)11. Draw the structure of haemoglobin and explain its role in blood.12. Predict the hybridization and geometry of the following complexes.a. [Fe(CO)5]                b.    [Ni(NH3)6]2+13. How is hardness of water determined using EDTA method?14. Discuss the conformation of cyclohexane.15. Predict the product and give its mechanism

 

16. Derive the rate constant of first order reaction.17. Distinguish between thermal and photochemical reactions.18. Write briefly on Pattinson’s process.19. Differentiate between DNA and RNA.20. Write the structure and functions of adrenaline and oxytocin.21. How do you prepare the following polymers?a. PUF                                     b. Terylene22. Differentiate the following with suitable examples.a. Step growth and Chain growth polymerization.b. Thermoplastic and Thermosetting plastics.
PART-CAnswer any FOUR questions (4×10=40)23. a ) How many geometrical isomers are possible for [Co(en)2(NH3)Cl]2+? Draw their structures.b ) Predict the magnetic nature of the following complexes.(i) [Ni(CN)4]2-                       (ii) [Co(NH3)6]3+24. a ) Discuss the mechanism of SN1 reaction.b ) Explain the optical isomerism of tartaric acid.25. a ) Arrange the following molecules based on acidity.(i)

(ii)

 

 

b ) Explain the deviation of solution from its ideal behavior.26. State and apply the phase rule to one component system.27. a ) Mention any four applications and two possible risk of genetic engineering.b ) Explain the Watson and Crick model of DNA.28. a ) How do you prevent  corrosion by cathodic protection ?b ) Explain vulcanization of rubber. Mention its uses.
* * * * *

 

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“Loyola College B.Sc. Chemistry April 2008 Electrochemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 15

 

FOURTH SEMESTER – APRIL 2008

CH 4502 – ELECTROCHEMISTRY

 

 

 

Date : 26/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

Answer ALL the questions                                                                            (10 x 2 = 20 marks)

 

  1. Write down the reactions taking place at the anode and cathode separately

Cu½ Cu2+ ½½ Ag+ ½ Ag

  1. What is meant by primary reference electrode?
  2. What is LJP?  How can it be minimized?
  3. Explain why quinhydrone electrode cannot be used for alkaline solution.
  4. Calculate the ionic strength of 0.01 M Cu SO4 solution.
  5. Compare the transference numbers of chloride ion in HCl and NaCl.
  6. Mention any two advantages of conductometric titrations.
  7. What is meant by activity of an electrolyte?  How is it related to activity coefficient of an electrolyte?
  8. Define overvoltage.
  9. What is concentration polarization?

 

PART – B

 

Answer any EIGHT questions                                                                 (8 x 5 = 40 marks)

 

  1. Describe the following types of electrodes with examples and write the electrode reactions.      a) Metal – Metal ion electrode  b) gas electrode.

 

  1. Describe the construction and working of a calomel electrode.

 

  1. How will you determine the standard electrode potential of zinc electrode?

 

  1. The standard oxidation potentials of Ce3+– Ce4+ and Fe2+– Fe3+ systems are – 1.61 and

-0.771 respectively.  Calculate the equilibrium constant at 25oC for the reversible process     Fe2+ + Ce4+  Ce3+ + Fe3+.

  1. Describe any one method of determination of pH of a solution by EMF measurement.

 

  1. Derive expressions for DG, DH and DS in terms of EMF of a cell.

 

  1. Differentiate between a strong and a weak electrolyte from the variation of conductance with concentration.

 

  1. Calculate the equivalent conductance at infinite dilution of NH4OH, if the equivalent conductance at infinite dilution of Ba(OH)2, BaCl2 and NH4Cl are 228.8, 120.3 and 129.8 ohm-1 cm2 eqiv—1 respectively.

 

  1. How is Ka of a weak acid determined by conductance measurement?

 

  1. Discus the conductometric titrations of a) a strong acid with a strong base b) a strong acid with a weak base.

 

  1. What are the applications of overvoltage?

 

  1. How is the decomposition voltage in an aqueous solution measured?

 

 

PART – C

 

Answer any FOUR questions                                                                        (4 x 10 = 40 marks)

 

  1. Define EMF.  How is solubility product of a sparingly soluble salt determined from EMF measurement?
  2. What is a standard cell?  Discuss the working of Weston standard cell.
  3. What are concentration cells? Derive an expression for the EMF of an electrolyte concentration cell without transference.
  4. The cell Cd½Cd Cl2 ½½ Ag Cl ½ Ag  has an emf of 0.675 V at 25oC and the temperature coefficient of emf is – 0.00065 V deg-1.  Calculate DG, DH and DS for the cell reaction.
  5. What is meant by transference number of an ion?  Describe the moving boundary method for the determination of transference number of an ion.
  6. a)  Give a account of Debye – Huckel theory of strong electrolytes.                         (6)
  1. b) Discuss the principle of polarography. (4)

 

 

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“Loyola College B.Sc. Chemistry April 2008 Coordination Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 21

 

SIXTH SEMESTER – APRIL 2008

CH 6601 – COORDINATION CHEMISTRY

 

 

 

Date : 21/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

                                                                           PART – A                                                           

Answer all the questions:                                                                  10 x 2 = 20

 

  1. Calculate CFSE value for high spin Mn2+ octahedral complex.
  2. What is meant by spin – orbit coupling?
  3. ‘The electron transfer from [Co(NH3)6]2+ to [Co(NH3)6] 3+ is extremely slow’. Explain
  4. Give two examples for photoredox reactions.
  5. How is ferrocene prepared? Draw its structure.
  6. Explain cis effect with an example.
  7. Write two examples for Metal template synthesis.
  8. Draw the structure of (a) Fe3(CO)12 (b) Co4(CO)12
  9. What is the biological significance of peroxidases?
  10. What are the contrast agents used in MRI?

PART – B

Answer any Eight questions:                                                   8 x 5 = 40

 

  1. Describe the CF splitting of metal d – orbitals in tetrahedral field of ligands.
  2. State John-Teller theorem. Explain why Cu2+ does not form regular octahedral complex while Ni2+
  3. What are the experimental evidences for overlapping between metal and ligand orbitals? Explain with examples.
  4. Discuss the splitting of metal d-orbitals in square planar complex.
  5. Explain dissociative mechanism of ligand substitution reactions in octahedral complex with suitable example.
  6. What are photoisomerisation reactions? Explain with two examples.
  7. How are cis-and trans – isomers of [Pt(NH3)2Cl2] prepared?
  8. Write the name and draw the structure for the following
    • [Pt(C6H5-C º C-C6 H5) (PPh3) 2]
    • Be(C5H5) 2
  9. What is Wilkinson’s catalyst? Describe the hydrogenation an alkene using it.
  10. Discuss the bonding in (a) metal carbenes (b) Metal alkyls.
  11. Write a note on iron-molybdenum center in nitrogenase enzyme.
  12. Explain chelate therapy with examples.

 

 

PART – C

Answer any FOUR Questions:                                                         4 x 10 = 40

 

  1. What are the principles of MO theory as applied to complexes? Construct MO energy level diagram for  [Co(NH3)6]3+ and explain why it is a diamagnetic complex.
  2. Define inner-sphere electrom transfer reaction. Explain the mechanism involved with a suitable example.  What are the experimental evidences for inter sphere electron transfer reactions?
  3. (a) Describe the factors affecting crystal field stabilization Energy in complexes.

(b) What are complimentary and non-complimentary electron transfer reactions?  Give two examples.

  1. (a) Write a note on cis-and trans-effect in synthesis of octahedral complex.

(b) Describe template synthesis of metal phthalocyanins.

  1. Describe in detail about bonding in metal carbonyls.
  2. (a) Write a note on Zeigler-Natta catalyst and its synthetic application.

(b) Discuss the structure and functions of carboxypeptidase – A.

 

 

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“Loyola College B.Sc. Chemistry April 2008 Concepts In Inorganic Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

GH 3

           B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2008

CH 1503 (CONCEPTS IN INORGANIC CHEMISTRY)

 

 

 

Date : 06-05-08                  Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer ALL the questions.                                                                         (10 x 2 = 20 marks)

  1. State Heisenberg uncertainity principle.
  2. Explain diagonal relationship of elements in the Periodic Table.
  3. Write election dot formula for (i) PCl5 (ii) O2
  4. Describe the structure of XeF6 using VSEPR theory.
  5. What is the relationship between ionization porential of an element and election affinity of an element in favouring the formation of an ionic compound between them?
  6. Bromides and iodides have higher lattice energies than expected from theoretical calculations. Give reasons.
  7. What are Hume – Rothory rules?
  8. Why does ice float in water?
  9. Label as acid or base; AlCl3, HSO4–, Ag+
  10. What are aprotic solvents? Give 2 examples.

 

PART – B

Answer any EIGHT questions.                                                        (8 x 5 = 40 marks)

  1. What are radial and angular wave functions? What information can we get from these functions.
  2. How do you determine the electronegativity of elements using Pauling method?
  3. Explain with example electrolytic reductions in aqueons and non-aqueous media.
  4. How is the lattice energy of a solid determined from Born-Haber cycle?
  5. What are Fajan’s rule? How do they help in explaining covalent character of ionic compounds?
  6. Using VSEPR theory illustrate the structure of (a) ICl2–   (b) XeF4
  7. Draw MO energy diagram for CO molecule. Calculate the bond order in CO molecule.
  8. Discuss resonance e– dot structures of carbonate ion.
  9. Discuss the crystal structure of CsCl.
  10. Write a note on clathrates.
  11. Balance the following chemical reactions by oxidation number method.

(a)

(b)

  1. Describe (a) Lux-flood concept  (b) Solvent – system Concept of acid, bases.

 

PART – C

Answer any FOUR questions.                                                         (4 x 10 = 40 marks)

  1. What are quantum numbers? Explain how they are derived. Describe the significance of quantum numbers.
  2. How are the following factors affect the ionization potential of an element?

(a) atomic size (b) nuclear charge   (c) screening effect   (d) electronic configuration.

  1. (a) Draw MO energy diagram for NO molecule. Calculate the bond order.

(b) Of the species O2, O2+, O2–, O22-, which will have maximum bond strength? Explain based on MO theory.

  1. (a) Explain with two examples, the exception to octet rule.

(b) Discuss the hybridization involved and structure of (i) NH3   (ii) SF4

  1. (a) How does band theory explain the property of metal, semi-conductor and insulator?

(b) What are types of hydrogen bonding? Explain with examples.

  1. What are the characteristic of liq Ammonia as a solvent? Describe any four types of reactions taking place in liq. NH3 with two examples each.

 

 

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“Loyola College B.Sc. Chemistry April 2008 Chemistry Of Materials Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

RO 31

 

SIXTH SEMESTER – APRIL 2008

CH 6602 – CHEMISTRY OF MATERIALS

 

 

 

Date : 23/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

Answer all the questions.                                (10 ´2 = 20)

  1. What is primitive cell ?
  2. Draw a neat sketch for cubic Zinc sulfide crystal structure.
  3. What is known as hydrothermal method.
  4. What is the principle of working of scanning electron microscope.
  5. How conductivity varies with temperature in
  6. Conductors
  7. Semiconductors
  8. What is photoluminescence?
  9. What are Ferrites ?
  10. Define Neel temperature.
  11. What is isotopic effect in super conductivity ?
  12. What are Polarons ?

PART – B

Answer any Eight questions                     (8  ´ 5   = 40)

  1. What are Miller Indices ? Explain how Miller indices is determined for a crystal plane.
  2. With a neat diagram , explain the NaCl structure.
  3. Discuss in detail about Bravais Lattices.
  4. How is zone refining technique used to purify the material?
  5. Explain the principle of working of thermogravimetric analysis.
  6. Explain about point defects in crystalline solids.
  7. Discuss in detail about the classification of ferroelectric crystals .
  8. Distinguish between dia, para and ferromagnetic materials.
  9. Explain the origin of ferromagnetic domains.
  10. What is Meissner effect? What are Type – I &  Type – II super conductors.
  11. Explain the principle, construction and working of high energy Lithium battery.
  12. Discuss about the classification of liquid crystal and give their applications.

PART – C

Answer any four questions.                                 ( 4 ´ 10 = 40 )

  1. What is hexagonal closed packed structure? Find the properties of hexagonal closed packed structure.
  2. Discuss in detail about the growth of crystal from Czochraski method.
  3. a). What are intrinsic and extrinsic semiconductors?

b). Derive an expression for intrinsic carrier concentration.

  1. Write short notes on

a).Curie point and the exchange integral.

b).Temperature dependence of saturation magnetization.

c).Saturation magnetization at absolute zero.

  1. Explain the occurrence of super conductivity based on Bardeen Cooper and Schrieffer theory.
  2. Write short notes on a) Spinel
  3. b) Perorakite structures
  4. c) High temperature super conductors

 

 

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“Loyola College B.Sc. Chemistry April 2008 Chemistry For Biologists – II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

             B.Sc. DEGREE EXAMINATION – PLA. BIO&BIOTEC.&ADV.ZOO.&BIOTE.

GH 14

 

FOURTH SEMESTER – APRIL 2008

CH 4204 / 4202 – CHEMISTRY FOR BIOLOGISTS – II

 

 

 

Date : 24/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer ALL the questions.                                                               (10 X 2 = 20)

  1. What is feed back inhibition ? Give an example.
  2. Define iodine value of oil.
  3. Give any two differences between DNA and RNA.
  4. How will you prepare BHC ?
  5. Explain about vanslyke method.
  6. What is apoenzyme ?
  7. Draw the structure of flavones.
  8. How will you prepare glucaric acid from glucose ?
  9. Give the structure of the following. i) Citral ii) a- Pinene
  10. What is absolute specificity ?

 

PART – B

Answer any EIGHT questions only.                                                   (8 X 5 = 40)

 

  1. How will you form Gly-Ala peptide bond by Fisher’s third method ?
  2. Explain about Lobryde Bruyn Van Elestein rearrangement.
  3. Give the difference between plant and animal fatty acids.
  4. Explain about hydrogen bonding between the nitrogenous bases in DNA.
  5. How will you analyse C- terminal of aminoacid by enzymatic method ?
  6. What is an alkaloid ? Give it’s classification.
  7. Write short notes on superphosphate.
  8. Show that D- glucose and D- fructose form the same osazone.
  9. What are the steps involved in citric acid cycle ? Calculate the net ATP’s gained.
  10. How did Haworth establish the presence of six membered ring in glucose.
  11. What are the factors which affect the activity of the enzyme ? Explain any two.
  12. Write short notes on rancidity.

 

 

 

PART – C

Answer any FOUR questions only.                                      (4 X 10 = 40)

 

  1. How will you convert the following :-
  2. a) Aldohexose into aldopentose (6)
  3. b) Aldopentose into aldohexose.                       (4)
  4. Give the role of macro nutrients and explain each with examples.
  5. Explain the mechanism of enzyme action.
  6. What are fungicides ? Explain it with two examples.
  7. Derive Michelis- Menton equation and explain each terms involved.
  8. Discuss the following :-
  9. a) Manufacture of Urea                                                                        (6)
  10.  b) Three types of RNA                                                                         (4)

 

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“Loyola College B.Sc. Chemistry April 2008 Chemistry For Biologist – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

             B.Sc. DEGREE EXAMINATION – PL.BIO.&BIOTEC.&ADV.ZOO&BIOTECH.

GH 8

THIRD SEMESTER – APRIL 2008

CH 3104/ 3102 – CHEMISTRY FOR BIOLOGIST – I

 

 

 

Date : 07-05-08                  Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART-A

Answer ALL the questions.                                              (10 x 2 =20 marks)

 

  1. Predict the hybridization and shape of the following molecules.

(a) BF3            (b) PCl5

  1. Draw the structure of the following complexes.

(a) tetraamminecopper(II) sulphate   (b) Potassium hexacyanoferrate(III)

  1. Calculate the normality of a solution having 9.8g of H2SO4 in 2 litre water.                (Equivalent weight of H2SO4 = 49)
  2. Define pH of a solution .What is the pH of pure water
  3. Differentiate order and molecularity of a reaction.
  4. Synthesis of ammonia is a heterogeneous catalysis reaction. Justify.
  5. Mention the optical properties of colloids.
  6. What is meant by coagulation? Give an example.
  7. How will you synthesise Terylene? Mention its use.
  8. Why tertiary carbonation is more stable than secondary and primary? Give reasons.

 

PART-B

 

Answer any EIGHT questions.                                           (8 x 5 = 40 marks)

 

  1. Write a note on vander Waals forces.
  2. Explain the structure and function of hemoglobin.
  3. Discuss the structure of methane based on hybridization.
  4. (a) State the law of volumetric analysis.                                                           (2)

(b) 20ml of oxalic acid requires 19.8 ml of 0.095N of NaOH. Calculate the weight

of crystalline oxalic acid present in 500ml of the given solution.                    (3)

  1. What is a buffer solution? Discuss the buffer action of a mixture of ammonium hydroxide hydroxide and ammonium chloride.
  2. Derive the rate expression for the rate constant of a first order reaction.
  3. (a) Define t1/2 of a second order reaction.                                                          (3)

(b) What is a zero order reaction? Give an example.                                         (2)

  1. Write a note on electro osmosis.
  2. (a) How will you prepare ferric hydroxide sol by peptisation method?            (3)

(b) Write any two applications of colloids.                                                        (2)

  1. Define inductive effect. Mention its types with examples.
  2. What are polymers? Explain the classification of high polymers giving one example of each.
  3. Discuss the optical activity in lactic acid.

 

PART-C

 

Answer any FOUR questions.                        (4 ´ 10 = 40 marks)

 

  1. (a) Explain Werner’s theory of coordination complexes.            (6)

(b) Draw all possible isomers of  [Rh(en)2Br2]+ complex.                                  (4)

  1. (a) Discuss the types of hydrogen bonding with suitable examples.            (6)

(b) Discuss the structure of NaCl unit cell.                                                        (4)

  1. (a) What are primary and secondary standard solutions.           (4)

(b) What is common ion effect? Give an example.                                            (3)

(c) Is NaOH a primary standard? Explain your answer.                                    (3)

  1. Discuss the kinetics of enzyme catalysed reaction.
  2. (a) Define the following:

[1] Enantiomers  [2] Diastereomers  [3] Resolution of racemic mixtures    (2+2+2)

(b) Explain the isomerism exhibited by maleic and fumaric acids.                    (4)

  1. (a) What are the defects of crude natural rubber? Explain with equation how are they overcome? (6) (b) Discuss any two method of expressing the concentration of a solution.           (4)

 

                        

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“Loyola College B.Sc. Chemistry April 2008 Bio Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 17

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

FIFTH SEMESTER – APRIL 2008

CH 5401 – BIO CHEMISTRY

 

 

 

Date : 06/05/2008                Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

            PART A

Answer all the questions                                                                                                         10 x 2 = 20

  1. What are the functions of nucleus?
  2. What is Zwitter ion?
  3. What are ligases? Give an example.
  4. Draw the structure of cholesterol.
  5. What are the products obtained by the oxidation of fructose?
  6. What are the differences between cellulose and starch?
  7. Write a note on biological oxidation?
  8. What is the role of ubiquinone in electron transport mechanism?
  9. What are purine and pyrimidine bases?
  10. Write down the various types of RNA.

PART B

Answer any eight questions                                                                                        8 x 5 = 40

  1. Explain the primary structure of proteins.
  2. How is N-terminal of an amino acid determined by Sanger’s method?
  3. How is alanyl glycine prepared?
  4. Explain the factors affecting the enzyme activity.
  5. Discuss β-Oxidation of fatty acids.
  6. Discuss any three important phospholipids.
  7. Explain the cyclic structure of D-glucose.
  8. Explain the classification of carbohydrates with examples.
  9. Discuss the mechanism of oxidative phosphorylation.
  10. Draw the structure of hemoglobin. Write any two the functions of hemoglobin.
  11. Explain the clover leaf model of t-RNA.

22     Discuss the replication of DNA.

PART C

Answer any four questions                                                                               4 x 10 = 40

  1. a) Explain the secondary structure of proteins.
  2. b) Describe any two methods of preparation of amino acids.
  3. a) Explain the steps involved in absorption and digestion of proteins.
  4. b) What are the differences between animal and plant fats?
  5. Describe different types of enzyme inhibition.
  6. Explain the overall process of glycolysis with enzymes involved in each step and energy yield.
  7. Explain the role of RNA involved in protein biosynthesis.
  8. Explain the double helical structure of DNA.

 

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“Loyola College B.Sc. Chemistry April 2008 Analytical Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

           B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 19

FIFTH SEMESTER – APRIL 2008

CH 5501 – ANALYTICAL CHEMISTRY

 

 

 

Date : 30-04-08                  Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

Answer the following:                                                                       (10×2=20)

  1. Distinguish between ‘precision’ and ‘accuracy’ of analytical data.
  2. What are antidotes? Cite two examples.
  3. What are drying agents? Cite two examples
  4. What are Rf values? Mention their significance.
  5. Define the term Normality.
  6. What are redox indicators? Give two examples.
  7. What is solubility product? What is its application?
  8. Define the term peptization.
  9. State the Beer-Lamberts law. Give its use.
  10. What is the wave number corresponding to 10.

 

PART – B

Answer any EIGHT of the following:                                             (8×5=40)

  1. How are pipettes and standard flasks Calibrated?
  2. Explain the types of error. Give the methods of minimising them.
  3. Explain the chemical methods of purification and test of purity.
  4. Explain the principle and procedure for Ion-exchange chromatography.
  5. Derive the Henderson’s equation.
  6. Explain the primary and secondary standards.
  7. Explain how Erio-chrome black.T functions as an indicator in EDTA titrations.
  8. The solubility product of AgCl at 250C is 1.78 x 10-10. Calculate its solubility in morality.
  9. Distinguish between co precipitation and post precipitation.
  10. Explain the following: (a) Line width in a spectrum. (b) Auxochromes.
  11. What are selection Rules? Give them for electonic (Uv-vis) spectorscopy.
  12. Describe the types of vibrational modes of a non-linear triatomic molecule.

 

PART – C

Answer any FOUR of the following:                                              (4×10=40)

  1. How is Standard Deviation calculated for a set of analytical data.
  2. Discuss on the principle and experimental techniques of Fractional distillation.
  3. (a) Explain the principle and preparation of TLC.

(b) How will you determine the relative strength of acids from Ka values.

  1. (a) Explain the various types of titrations?

(b) Explain the use of phenolphthalein and methyl orange as indicator.

  1. Write notes on:

(i) Sequestering agent             (iii) Nucleation

(ii) Common – ion effect        (iv) Homogenous precipitation

  1. Discuss on the functional group analysis in IR spectroscopy.

 

 

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“Loyola College B.Sc. Chemistry April 2008 Analytical Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 2

 

FIRST SEMESTER – APRIL 2008

CH 1502 – ANALYTICAL CHEMISTRY

 

 

 

Date : 03/05/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

                                                                        (10 x 2 = 20 marks)

Answer ALL questions.

  1. The metal content in a mineral was reported as 30%. Taking the acceptable value as 32%, calculate the absolute error and relative error in ppt.
  2. What first aid should be given for spillage of concentrated acid and strong alkali on a person?
  3. Differentiate between eluent and eluate.
  4. What is the difference between direct titration and a back titration?
  5. Why would a reprecipitation be employed in a gravimetric analysis?
  6. What quantity is measured in TGA and in DTA?
  7.  What are the advantages of DTA over TGA?
  8. What are metallochromic indicators? Give an example.
  9. What is a secondary standard? Mention its properties.
  10. Compare the solubility of lead iodide in
  1. i) pure water ii) 0.1 M aq KNO3 and iii) 0.1 M aq KI.

 

PART – B

                                                                        (8 x 5 = 40 marks)

Answer any EIGHT questions.

  1. What are the general rules observed in the storage and handling of chemicals?
  2. How is a burette calibrated?
  3. What are the possible errors in weighing? How can they be minimized?
  4. Explain the principle of solvent extraction and extraction using a second solvent.
  5. Discuss the principle of distillation under reduced pressure.
  6. Explain the principle behind the separation of a mixture using paper chromatography.
  7. A sample of pure sodium carbonate weighing 0.3542g is dissolved in water and titrated with a solution of hydrochloric acid. A volume of 30.23 mL is required to reach the methyl orange end point. Calculate the normality of the acid solution.
  8. How is selection of proper indicator effected in acid-base titrations?
  9. What characteristics should a substance possess to be used as a primary standard for acid or base solutions?
  10. Explain the terms coprecipitation and post precipitation. Differentiate between them.
  11. Discuss the factors that affect the size of particles of precipitate in gravimetric analysis.
  12. Write briefly on the factors that affect the thermogram.

 

PART – C

                                    (4 x 10 = 40 marks)

Answer any FOUR questions.

  1. The normality of a solution is determined by four separate titrations, the results being 0.2041, 0.2049, 0.2039 and 0.2043. Calculate the mean, median, range, average deviation and standard deviation and coefficient of variation.
  2. a) Discuss the principle and applications of GC.                                            (5)
  1. b) Explain the functioning of FID in GC. (5)
  1.  Explain the principle and methodology behind the separation of ions using

ion exchange chromatography.

  1. a) List out the reasons for the versatility of EDTA as titrant.                                    (3)
  1. b) Explain how EDTA is used in direct, back and indirect titration methods.(7)
  1. a) How is chloride determined by Volhard method?                                     (6)
  1. b) What are adsorption indicators? Explain (4)
  1. Using a block diagram, discuss the various components of TGA and DTA apparatus.                                                                                                                                             (5+5)

 

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