Loyola College Question Paper 2006

Loyola College M.Sc. Chemistry April 2006 Heterocyclics & Natural Products Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 42

FOURTH SEMESTER – APRIL 2006

                                 CH 4954 – HETEROCYCLICS AND NATURAL PRODUCTS

(Also equivalent to CH 4951)

 

 

Date & Time : 25-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

Part- A

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

  1. How is isoquinoline synthesized?
  2. Write the retrosynthesis of pyrimidine.
  3. How is luciferin synthesized? What is its function?
  4. How is the configuration of steroid nucleus defined? How does it affect the stability of nucleus?
  5. During the synthesis of cholesterol, how is the B ring introduced?
  6. What happens when quinoline is subjected to Hofmann’s exhaustive methylation method?
  7. ‘Nametskin rearrangement plays a key role in the biological conversion of Terpenes”. Explain.
  8. How would you convert acetophenone into tropic acid?
  9. Convert: Carvone into Cadelene.
  10. How are terpenes classified? Give an example for each.

Part – B

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

  1. How do pericyclic reactions help in the synthesis of heterocyclic compounds? Mention any two examples.
  2. Predict the products in the following reactions.

 

 

  1. Write a note on the electrophilic substitution reactions in thiazole with suitable example.
  2. Explain Traube’s synthesis of uric acid.
  3. How is oestriol synthesized from (±)-oestrone?
  4. Describe any two ring closing reactions during synthesis of cholesterol.
  5. Establish the structure of peepuloidin by synthesis.
  6. How would you establish the structure of veratric acid?
  7. Establish the structure of abietic acid by synthesis.
  8. Give the structure of cocaine. How would you establish and confirm the structure of cocaine by synthesis?
  9. How would you confirm the structure of papaverine by synthesis?
  10. Establish the structure of camphoric acid.

 

Part-C

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

23     a) What happens when chromone is treated with hydrazine? Write the mechanism of the reaction.

  1. b) Heterocyclic compounds are highly reactive than the corresponding homocyclic compounds. Give suitable explanation with examples.

24     a) Draw the resosnance structures of the following

  1. i) isoquinoline              ii) pyridine                   iii) purine
  2. b) How are the following heterocyclic compounds useful biologically
  3. i) coumarin                  ii) flavone
  4. c) What is Cornforth rearrangement?

25     a) How is the following conversion effected during the synthesis of cortisone?

 

  1. b) What is the biological importance of steroids? Give any two examples.
  2. a) Establish the structure of vitamin-A.
  3. b) What are the functional groups present in heptaphylline? How would you confirm its structure?
  4. a) Establish the structure of gibberelic acid.
  5. b) How would you establish the structure of atropine by synthesis?
  6. How would you convert the following:
  • Tropine into 2-ethylpyridine
  • 1,4-butanedial into ecgonine
  • Camphoric acid into camphor
  • 2,5-dimethoxytetrahydrofuran into tropinone.

 

 

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Loyola College M.Sc. Chemistry April 2006 Electrochemistry Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 40

FOURTH SEMESTER – APRIL 2006

                                               CH 4805/CH 4803 – ELECTROCHEMISTRY

 

 

Date & Time : 20-04-2006/FORENOON     Dept. No.                                                       Max. : 100 Marks

 

 

 

Part–A (20 Marks)

 

Answer ALL questions (10 x 2 = 20)

  1. Calculate the thickness of ionic atmosphere in 0.1M aqueous lanthanum sulphate.
  2. Compare the ion-solvent interaction of the following
    1. 1M aq KCl
    2. 1M aq Al2(SO4)3
  3. λ H+ is the highest among cations in aqueous solution. Why?
  4. How is the capacitance related to the thickness of double layer in Helmholtz Perrin

model?

  1. What are surfactants? Give example.
  2. What do you mean by a polarisable electrode? State the condition for its ideal

polarisability.

  1. What is reaction resistance? Calculate its value of an electrode having equilibrium

current density  2 .08 μA cm.

  1. Nernst equation is a special case of Butler-Volmer equation.Explain.
  2. Determine whether Cu form 0.01 M Cu2+ will be deposited or not.

( SRP :  Cu2+/ Cu = 0.34V )

  1. Obtain the relation between rate and current density of an electro-chemical reaction

from Faraday’s laws.

Part-B (40 Marks)

 

Answer any EIGHT questions (8 x 5 = 40)

  1. 11. What are electro capillary curves? What is its importance?
  2. Derive an expression for the interfacial tension applying parallel plate condenser

model.

  1. Apply Born’s model to find out the energy of ion solvent interaction.
  2. 14. Discuss the evidences for the existence of ionic atmosphere.
  3. 15. The measured emf for the cell Ag, AgBr,KBr || Hg2Br2 | Hg are 0.06839V at 25ºC

and 0.07048V at 30ºC. Write the reaction involved and calculate ∆H, ∆G and ∆S

for the reaction at 25ºC

  1. A 0.2m lead nitrate solution freezes at -0.10ºC. Calculate the dissociation constant

if Kf of water is 1.86 K molal-1

  1. Derive the Butler-Volmer equation for a one electron electrode process.
  2. 18. Define transfer coefficient. How is it determined experimentally?
  3. 19. The reversible potential and c.d of an electrode are 0.22 V and 7.2×10 -4 A cm-2

        respectively. Calculate the c.d across it   at 0.74 V if it has 40% cathodic tendency.

 

  1. 20. The tafel anodic and cathodic slopes of “applied potential vs logi ” of an

electrode process were found to be 0.04 & 0.12 respectively.  Calculate the

ransfer coefficients.

 

  1. 21. Explain the applications of Tafel equations.

 

  1. 22. The exchange current density of Pt/Fe, Feis 2.5 mA cm. Calculate the

current density across the electrode at 25C maintained at 1V when [Fe] = 0.1

M and [Fe]= 0.2 M (SRP = 0.77IV, β = 0.58)

 

Part-C (40 Marks)

 

Answer any FOUR questions (4 x 10 = 40)

 

  1. 23. Discuss sterns model of double layer structure.
  2. 24. Describe ‘Electrokinetic Phenomena’.
  3. 25. Derive Debye Huckel limiting law. How is it verified?
  4. 26. For the system Pt /Fe3+, Fe2+ at 298K the i were measured as shown below:

(mV):             50       80      100     120        150     200

(mA cm)   :  8.01  16.1    25.17    41         82.4   264

Evaluate  io and β

  1. 27. Consider the following mechanism for the deposition iron.

 

Fe2+ + H2O           FeOH+ + H+   eq const K1 ……. (1)

 

                                   FeOH+ + e            FeOH             eq const K2 ……. (2)

 

FeOH + H+ + e          Fe + H2O    eq const K3   ……. (3)

 

Derive the expression for rate if step-2 is rds

  1. Discussion of Butler -Volmer equation for different values of over potentials.

 

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Loyola College M.Sc. Chemistry April 2006 Analytical Chemistry Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 26

FIRST SEMESTER – APRIL 2006

                                                    CH 1809 – ANALYTICAL CHEMISTRY

 

 

Date & Time : 25-04-2006/1.00-4.00 P.M.   Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

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

  1. Triethylamine is a good titrant for the estimation of Cu2+ but not ammonia. Why?
  2. In what way is HPLC is different from GC?
  3. Define confidence interval.
  4. How is the indicator chosen for redox titration?
  5. 00 ml of well water is found to contain10-3 moles of ca2+. Express the concentration of Ca2+ in well water in ppm.
  6. Mention two applications of differential thermal analysis (DTA).
  7. What are the three electrodes used in cyclic voltametric experiment?
  8. What is the significance of molar absorption coefficient?
  9. What is hollow cathode lamp? Where is it used?
  10. Suggest a method for the determination of (a) quinine (b) Na+ (c) Fe3+ in a tap water.

PART – B

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

  1. What is thermogram? Explain with an example.
  2. Show that the fraction of completely ionized form of EDTA is a measure of pH.
  3. A 50.00 ml of aliquot of a water sample containing Fe3+ required 13.75 ml of

1.2X10-2 M EDTA when titrated at pH 2.0. Express scientifically the             concentration of Fe3+ in water sample in ppm.

  1. 6000g sample consisting of only CaC2O4 and MgC2O4 is heated at 500 ֯C converting the salts to CaCO3 and MgCO3. The sample then weighs 0.4650g. If the sample had been heated at 900 ⁰C, where the products are CaO and MgO, what would be the mixture of oxides have weighed?
  2. Find out the pH of the following solutions:
    1. Mixture of 20.00 ml of 0.0250 M acetic acid and 40.00 ml of 0.01250 M of sodium hydroxide. Ka of acetic acid is 10-5.
    2. Mixture containing 20.00 ml of 0.0250 M sodium hydroxide and 20.00 ml of 0.0300 M HCOOH. Ka of HCOOH is 10-2.
  3. How will you proceed to collect authentic results for research?
  4. How is sulphate determined by turbidimetric method?
  5. How is Ni2+ estimated by spectrophotocoloriometric method?
  6. How is florescence method more useful than the absorption method in some cases?
  7. Write a note on anodic stripping voltammetry.
  8. Write a note on deviations from Lambert-Beers law.
  9. How is potassium estimated by flame photometric method?

 

PART – C

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

  1. Discuss the principle and instrumentation of Gas Chromatography.
  2. The sulphate concentration I natural water can be determined by measuring the turbidity that results when excess BaCl2 is added to a measured quantity of the sample. A turbidimeter was calibrated with a series of standard sodium sulphate solutions. The following data were obtained in the calibration.

mg/L                           Reading

0.0                               0.06

0.5                               1.48

  • 28
  • 98

20.0                             4.61

Assuming a linear relationship, derive the equation for the best straight line though these points. Assuming the turbidimeter reading 3.67 for the unknown sample which is the mean of 3 readings, calculate the standard deviation of the result and the concentration of sulphate in the sample.

  1. Discuss the applications of Thermogravimetry. (6)
  2. Explain how the concentration of analyte and products are estimated at the equivalence point in redox titration.
  3. How is thermogravimetry recorded? Mention the factors that affect the thermo gravimetric curves.
  4. Describe the estimation of copper by electrogravimetric method.
  5. Describe the principle and instrumentation involved in atomic absorption method. How is Ca2+ in ppm levels estimated by this method?

 

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Loyola College M.Sc. Chemistry April 2006 Analytical Chemistry-III Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2006

                                                 CH 3805 – ANALYTICAL CHEMISTRY – III

 

 

Date & Time : 18-04-2006/AFTERNOON   Dept. No.                                                       Max. : 100 Marks

Part–A (20 Marks)

Answer ALL questions (10 x 2 = 20)

  1. How large a sample to be taken for analysis using a chemical balance so that the maximum relative uncertainty in the sample weight is 5 ppm?
  2. Explain replacement titration with an example.
  3. Compute the equivalent point potential for titration of
    A2+ vs B4+ (SRP: B4+ / B2+ = 1.44 V ;  A4+ / A2+ = 0.15V )
  4. How is an indicator chosen for a red ox titration?
  5.  Calculate the equilibrium constant for the following reaction:

HCN + OH–   ⇌  CN– + H2O; Ka (HCN) = 1 x 10 -10

  1. How does coulometer differ from potentiometric technique?
  2. Explain how the addition of nitrate ion avoids the liberation of hydrogen?
  3. State an expression for the residual current and explain the terms in it.
  4. Explain the effect of added CN–  on the electrode deposition of Ag.
  5. Mention any two applications of DTA.

 

Part–B (40 Marks)

 

Answer any EIGHT questions (8 x 5 = 40)

  1. Show that the equivalence point for the titration of Fe2+ vs MnO4– is pH dependant.
  2. Explain diverse ion effect
  3. Draw  the titration curves for the follwing:
  • 20 mL of 0.1 M NaOH vs 0.1M CH3COOH
  • 20 mL of 0.1 M NaOH vs 0.1M H2SO4.
  1. Write a note on homogeneous precipitation.
  2. Exactly 0.3525 g of 96.5% Na2SO4 required 37.7 mL of a solution of BaCl2. Calculate the concentration and express the concentration of BaCl2 in scientific notation.
  3. The values of Ka1, Ka2, Ka3 & Ka4 for EDTA (H4Y) are 1x 10-2 , 1x 10-3 , 1x 10-8  & 1x 10-12 ,  respectively. Calculate the conditional stability constant for the following process in 1x 10-2 M HCl.

Fe3+ + Y4-     ⇌       FeY–     ; Kobs = 1 x 1025

    1. How will you estimate Cu2+ by electro gravimetric method?

 

  1. Draw a typical polarogram and indicate the following on the diagram.
  1. Residual current.
  2. Limiting current
  3. Diffusion current
  4. How are they related to each other?
  1. A certain Pb2+ solution gives id = 1.00 mA . To 10 ml of the solution 0.5 ml of 0.04 M of Pb2+ was added. The id of the solution was found to be 1.5 mA. Calculate the concentration of Pb2+ in the unknown solution.
  2. Draw and explain the ampereometric titration curves for the following titrations if the applied potential is maintained at half wave potential of Pb2+
  1. Pb2+ vs CrO42- b . CrO42- vs Pb2+
  1. Explain how the cyclic voltometric technique can be used to determine the electrochemical reversibility and stability of a red-ox  system.
  2. Explain the following with an example.

(i) Fluorimetric estimation of metal ions

(ii) Chemiluminescence

 

Part-C (40 Marks)

 

Answer any FOUR questions (4 x 10 = 40)

  1. The following are peak areas for chromatogram of standard solutions of methyl vinyl ketone (MVK)
Conc. MVK

mmol-1

 Relative peak Area
0.500 3.76
1.50 9.16
2.50 15.03
3.50 20.42
4.50 25.33
5.50 31.97

Apply method of last squares to determine the Conc. of MVK in a sample which yielded relative peak area 6.3, which is the mean of 4 measurements. Also calculate the standard deviation of the result.

  1. Give a critical account of acid-base titration in non-aqueous solvents.
  2. a) Determine the concentration of Fe2+, Fe3+, Ce4+ and Ce3+ in the mixture containing 20.00mL of 0.1000M Ce4+ and 40.00ml of 0.0500M Ce2+ in acidic medium.

(Eº Fe3+/Fe2+ = 0.8V, EºCe4+/ Ce3+ =1.4V)

  1. b) Discuss the factors which influence ∆Pm at the equivalence point.
  1. a) Explain the components of spectro flurometer with a neat diagram.
  1. b) What is hollow cathode? How does it work?
  1. a) Bring out the difference between TG and DTA.
  1. b) How will you prove the liberation of CO in a thermal analysis?
  1. A metal carbonate, MCO3.4H2O (at.wt of metal = 74) on thermal analysis becomes  dihydrate at  160˚C , monohydrate at 200˚C , anhydrous at 260˚C and MO at 550˚C Construct a TG, using graph sheet if 0.725 mg of the salt hydrate is heated from 40˚C to 750˚C.

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Loyola College M.Sc. Chemistry April 2006 Chemistry Of Main Group Elements Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 30

SECOND SEMESTER – APRIL 2006

                                     CH 2809 – CHEMISTRY OF MAIN GROUP ELEMENTS

 

 

Date & Time : 21-04-2006/FORENOON     Dept. No.                                                       Max. : 100 Marks

Part-A

Answer all questions. Each question carries two marks

  1. Both Li and Mg can be used to remove N2 from other gases. Rationalize.
  2. What are electrides? Cite an example.
  3. Europium is frequently found in nature in group II minerals. Comment.
  4. Compounds of alkaline earth metal ions are colorless, but [Be(bpy)(C2H5)2] is bright red in color. Account for this observation.
  5. What are pyrazaboles? Cite an example.
  6. Cite the cyclohexane chair conformational analogue of phosphinoborane.
  7. What are silanes? How do they act as a strong reducing agents for halogens?
  8. What is ZSM-5 catalyst? Mention any two applications.
  9. What is the basic unit of silica present in pyroxene mineral? Draw its structure.
  10. Mention the general trend observed in the hydrolysis of interhalogen compounds.

Part-B

Answer eight questions. Each question carries five marks

  1. Explain the structure of B5H9 using PSEPT theory.
  2. Give an account of the preparation, properties, and structure of C2B10H12.
  3. Write brief notes on (a) silylamines and (b) inorganic rubber.
  4. Explain the role of zeolites as molecular sieves.

15a.  Explain the principle involved in the qualitative estimation of CO by using I2O5.

  1. Complete the following reactions: I2O5 + H2S  ?; I2O5 + HCl  ?

I2O5 + F2BF3   ?

  1. Explain the synthesis of linear phosphazenes and their reactivity toward amines, alkoxides, aryloxides, and organometallic reagents.
  2. Give an account of hexagonal and cubic boron nitrides and their analogy toward graphite and diamond.
  3. Give a brief account of natutrally occurring azamacrocycles.
  4. Explain the chlorinating and oxidising reactions of any two oxides of chlorine.
  5. Give an account of the chemistry of phosphorus compounds with P-P double bonds.
  6. Give an account of the synthesis of aluminium alkyls and their synthetic importance. Comment upon the structures of aluminium alkyls and aluminium aryls.
  7. How is phosphorus sulfides prepared? Depict their cyclic structures.

Part-C

Answer four  questions. Each question carries ten marks

  1. Discuss the bonding in boranes. How can this be extended to cover higher boranes?

24a.  Explain the polyhedral rearrangements of closo-carboranes.                             (5)

  1. Explain the preparation, properties, and structure of borazine.                         (5)

25a.  Give a brief account of the chemistry of oxohalogen fluorides.                       (7)

  1. Write a note on heteropoly blues.                                                                      (3)

26a.  Explain the special equipments and fundamental techniques employed

in the synthesis of main group nonmetal compounds.                                       (6)

  1. Explain the use of hexamethyldisilazane as a silylating agent for organic and inorganic compounds with examples. (4)

27a.  Give an account of naturally occurring ionophores and their interaction with the alkali and alkaline earth metal ions.                                                                    (6)

  1. Explain the mechanism of ion transport across  cell membranes.                      (4)

28a.  Explain the synthesis, reactivity, and structural aspects of rings and cages involving

Si-Si multiple bonding.                                                                                      (6)

  1. Give an account of heterocyclic inorganic ring systems involving Si-O and N-S bondings.                                                                                                       (4)

 

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Loyola College M.Sc. Chemistry April 2006 Advanced Coodination Chemistry Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 44

FOURTH SEMESTER – APRIL 2006

                                     CH 4953 – ADVANCED COORDINATION CHEMISTRY

(Also equivalent to CH 4950)

 

 

Date & Time : 25-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

Part-A

Answer all questions. Each question carries two marks

  1. Organometallic compounds of transition metals are invariably colorless. Give reason.
  2. Cl-occupies the lower end of the spectrochemical series, yet the Do value of [RuCl6]3- is comparable to that of [Ru(H2O)6]2+. Offer a reasonable explanation.
  3. How is low-spin and high-spin complexes of d5 metal ion differentiated by electronic spectroscopy?
  4. Mention the causes of tetragonal distortion in transition metal complexes. How is it inferred from epr spectroscopy?
  5. How is the covalent character in transition metal complexes quantified?
  6. What is the oxidation state and spin state of iron centers in Fe_S proteins?
  7. How is p-acceptor series constructed?
  8. What is zero field splitting? Mention its causes in transition metal complexes.
  9. How does angular overlap of metal and ligand aos alter the magnitude of es- and ep-parameters?
  10. Illustrate transmetallation reaction with an example.

Part-B

Answer eight questions. Each question carries five marks

  1. Explain the structural features and biological roles of Fe-S proteins.

12     What is crystal field splitting parameter Dt? How is it manifested when Dqxy > Dqz and Dqxy < Dqz?

  1. How is nitro- and nitrito complexes differentiated by IR spectroscopy?

14     Explain the features of Tanabe-Sugano diagrams. In these diagrams the lowest energy excited state for a high-spin metal ion in a given geometry becomes the ground state for the low-spin state. Explain.

15     What is nitrogen fixation. Explain its mechanism

16     What are coupled chemical reactions? How are they classified? How do you infer  such a process from cyclic voltammetry?

  1. Explain the structural aspects and biological roles of cytochromes.
  2. Give an account of the structural features of biological electron transfer agents.
  3. What is chelation therapy? Mention the specific disease which is cured by this therapy.

20     Explain the principle of AC polarography. How is the reversibility of a redox couple evaluated by this technique?

  1. What are optically trasparent thin layer electrodes? Mention their importance.
  2. What is static dynamic Jahn Teller distortion? How is it studied by esr spectroscopy?

Part-C

Answer four questions. Each question carries ten marks

23a   Explain the electronic spectral features of low-spin and high-spin Oh complexes of d6 metal ion.                                                                         (4)

b     Explain the electronic spectral features of tetragonally distorted Oh complex of low-spin d6   metal   ion and the method of evaluating the crystal field parameters. (6)

24a.  Derive Marcus-Hush equation to compute the rate constant of electron transfer reactions. (7)

  1. How do you differentiate inner- and outer-sphere electron transfer reactions?            (3)

25a.  Explain hyperfine and superhyperfine splittings.                                                (3)

  1. The epr spectrum of a high spin Mn(II) complex, doped onto a diamagnetic host, consists of 30 epr lines when there is no hyperfine splitting by the ligand. Interpret the spectrum with the help of a qualitative hyperfine splitting diagram. (7)

26a.  p-Donation by ligands lowers 10Dq values whereas p-back bonding increases 10Dq values and facilitates M-L bonding. Explain with the help of MO theory with qualitative MO energy level diagrams.                                           (5)

  1. Account for the difference in the properties of metal carbonyls and complexes of nitrogen donor ligands in the light of MO theory.                                        (5)

27a.  Explain the principles of angular overlap model.

  1. Show that  Dt =  4/9Do with the help of this model.

28a.  Illustate coordination template effect with examples.                                      (4)

  1. What are compartmental ligands? Explain the method of synthesizing dinuclear macrocyclic and macroacyclic compartmental ligands with illustrative examples.(6)

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Quantum Chemistry Question Paper PDF Download

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                     LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034    M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 11

FIRST SEMESTER – NOV 2006

         CH 1800 – QUANTUM CHEMISTRY

 

 

 

Date & Time : 26-10-2006/1.00-4.00          Dept. No.                                                              Max. : 100 Marks

 

 

 

Part-A   ANSWER ALL QUESTIONS (10 x 2 = 20)

 

  1. Explain the Ultraviolet catastrophe.
  2. The size of an atomic nucleus is 10-14 Calculate the uncertainty in momentum of the electron if it were to exist inside the nucleus.
  3. The accepted wave function Φ for a rigid rotor is Nexp(±imφ) for 0≤φ≤2π.

Determine N.

  1. Show that the function Ψ(x,y,z) = cosax cosby coscz (where a,b,c are constants) is an

eigen function of the Laplacian Operaator ∇2. What is its eigen value?

  1. Show that the energy E = 14h2/8ma2 of a particle in a cubic box of side ‘a’ is triply degenerate.
  2. What is a well-behaved or acceptable wave function in quantum mechanics?
  3. Explain the radial plot and the radial probability density plot for 2s electron.
  4. What is Born-Oppenheimer approximation?
  5. Write the Hamiltonian operator for the H2+ molecular ion in atomic units defining

each term  involved in it.

  1. Write the Slater determinant for the ground state of He atom which takes into account the antisymmetric condition of Pauli Exclusion Principle for electrons.

 

 

Part-B   ANSWER ANY EIGHT QUESTIONS (8 x 5 = 40)

 

 

  1. Discuss the failures of classical mechanics and the success of quantum theory in the explanation of black body radiation. .
  2. What are quantum mechanical postulates? Explain briefly any two of the postulates.
  3. The work function for Cesium is 2.14 eV. What is the kinetic energy and the speed of the electrons emitted when the metal is irradiated with the light of 300 nm?
  4. What is a hermitian operator? Show that the eigen value of a hermitian operator is real.                                                                                                                 (2+3)
  5. The normalized wave function for the 1s orbital of Hydrogen atom is

ψ = (1/√π)(1/a0)3/2exp(-r/a0). Show that the most probable distance of the electron is    a0.

  1. Explain Bohr’s correspondence principle with a suitable example.
  2. Write the Schroedinger equation for 1-D harmonic oscillator. Verify ψ = (2a/π)1/4exp (-ax2) is an eigenfunction of the Hamiltonian operator for the 1-D harmonic oscillator.

 

 

  1. What is a node? Draw the first three wave functions and probability plots for the Particle in a 1-D box and Simple Harmonic Oscillator models and compare them.

(1+4)

 

 

 

  1. The spacing between adjacent rotational lines in the spectrum of HCl molecule is

6.33 x 1011s-1. Calculate the moment of inertia of HCl molecule and the internuclear spacing  if the atomic masses are H = 1.008 and Cl = 34.97.

  1. (a) Explain the conditions under which an electron may give a continuous or a discrete spectrum.
    • The continuous probability distribution Gaussian function is given by

f(x) = Aexp(-x2/2a2) with interval (-∞, +∞). Show that <x> = 0.                (2+3)

  1. In solving the H2+ problem using the LCAO method, the lowest energy obtained is given by E+ = (HAA + HAB) / (1+SAB) where A and B refer to the two hydrogen nuclei. Explain each of the integrals in the above equation and their significance.
  2. With a suitable example explain the quantum mechanical tunneling.

 

 

Part-C   ANSWER ANY FOUR QUESTIONS (4 x 10 = 40)

 

  1. (a) Write the Schroedinger equation to be solved for H atom and solve it for its energy using a simple solution, which assumes the wave function to depend only on the distance r and not on the angles θ and φ

(b) In the Compton experiment, a beam of x-rays with wave length 0.0558 nm is scattered through an angle of 45˚. What is the wavelength of the scattered beam?

(7+ 3)

  1. (a) Apply the variation method to get an upper bound to the ground state energy of hydrogen atom using the trial function φ(r) = exp(-αr2). Compare your result with the true value.

(b) Discuss the Pauli Principle of antisymmetric wave function.             (6+4)

  1. Set up the Schroedinger equation for a rigid rotor in polar coordinates and solve it for its energy and wave function.

26  (a) Set up and solve the Schroedinger wave equation for a 1-D particle in a box model for its energy and wave function.

(b) For the hexatriene molecule, calculate λmax on the basis of particle in a one dimensional box of length equal to 7.3Ǻ                                                     (7+3)

  1. Discuss the Molecular Orbital treatment of H2 molecule and explain how the Valence

Bond (Heitler-London) method overcomes some of the difficulties of MO theory.

  1. (a) What are the three important approximations of Huckel-LCAO-MO theory?

(b) Using this theory set up the secular equation and secular determinants for

allyl radical and hence obtain its energy levels.                                            (3+7)

 

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Loyola College M.Sc. Chemistry Nov 2006 Quantum Chemistry & Group Theory Question Paper PDF Download

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                     LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034    M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 16

FIRST SEMESTER – NOV 2006

CH 1808 – QUANTUM CHEMISTRY & GROUP THEORY

 

 

 

Date & Time : 26-10-2006/1.00-4.00               Dept. No.                                                              Max. : 100 Marks

 

 

 

 

 

Part-A   ANSWER ALL QUESTIONS (10 x 2 = 20)

 

  1. Show that Ae-ax is an eigen function of the operator d2/dx2. What is the eigen value?
  2. Define an orthonormal function.
  3. The energy of a particle moving in a cubic box of side ‘a’ is 3h2/2ma2. What is its degeneracy?
  4. What is a node? Draw the radial distribution plot for 3s orbital of H-atom and indicate where the nodes are.
  5. What is the value of [x,px]? What is its physical significance?
  1. What is a fermion? Give an example.
  2. Set up the Schroedinger wave equation to be solved for the rigid rotor in spherical

polar coordinates.

  1. Define the Variation Principle and mention its significance.
  2. Identify the point groups for the following molecules:

(a) POCl3         (b) SF6   (c) Br2            (d) Ni(CN)42- (square planar)

  1. The following irreducible representations are parts of the C4v and C2h character

tables. What do x and y in these tables mean and in what way they differ from

each other?

 

C4v    E    2C4    C2     2σv   2σd                   C2h           E     C2           i      σh

 

 

E      2      0    -2     0     0       (x, y)       Bu         1     -1      -1        1        x,y

 

 

Part-B   ANSWER ANY EIGHT QUESTIONS (8 x 5 = 40)

 

11 Apply variation theorem to the problem of particle in a 1-D box of length a, by taking

ψ = x(a-x) as a trial function for 0≤x≤a.

 

  1. What is a hermitian operator? What is its significance in quantum mechanics?

Show that the eigen value of a hermitian operator is real

 

  1. Show that the wave functions describing 1s and 2s electron for He atom are

orthogonal to each other, given Ψ1s = (1/4π)1/2 2(2/a0)3/2 exp(-2r/a0)   and

Ψ2s = (1/4π)1/2 (1/a0)3/2 (2 – 2r/a0) exp (-r/a0).

 

  1. What is a Slater determinant? Write the four Slater determinants for the excited state

of He atom (1s,2s)

 

 

 

 

  1. The force constant of 79Br is 240 Nm-1. Calculate the fundamental vibrational

frequency and the zero-point energy of the molecule.

 

 

  1. Explain briefly with a suitable example:

(a) Bohr’s correspondence principle (b) Born –Oppenheimer approximation.      (3+2)

 

  1. The wave function of 1s orbital of Li2+ is given by Ψ1s = (1/√π) (Z/a0)3/2 exp(-Zr/a0),

where a0 is the most probable distance of the electron from the nucleus. Show that the

average distance is a0/2.  [Help:  0ò¥ xn e-qx dx = n! / qn+1]

 

  1. (a) Show that [x, d/dx] = -1

(b) What are the values of [x,px] and [L2,Lx]? What is their physical significance?

(2+2+1)

 

  1. Write the Schroedinger equation to be solved for H atom and solve it for its

energy using a simple solution, which assumes the wave function to depend only

on the distance r and not on the angles θ and φ.

 

  1. Explain the following with a suitable example:

(a) A ‘Class’ in group theory (b) Principle of mutual exclusion                  (3+2)

 

  1. Explain ‘quantum mechanical tunneling’ with a suitable example.

 

  1. Find the number, symmetry species of the infrared and Raman active vibrations of

CCl4, which belongs to Td point group by reducing the following reducible

representation. State how many of them are coincident.

Td          E       8C3            3C2             6S4            6σd

GCCl4         15        0              -1                 -1             3

 

Td         E          8C3      3C2      6S4       6σd

A1        1          1          1          1          1                             x2+y2+z2

A2        1          1          1          -1         -1

E          2        -1           2          0          0                            (2z2-x2-y2, x2-y2)

T1         3          0          -1         1          -1         (Rx,Ry,Rz)

T2         3          0          -1         -1         1         (x,y,z)         (xy,xz,yz)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Part-C   ANSWER ANY FOUR  QUESTIONS (4 x 10 = 40)

 

  1. (a) Derive the wave function and energy for the particle in a 1-D box.

(b) A cubic box of 10Å on the side contains 8 electrons. Applying the simple particle in a box model, calculate the value of ΔE for the first excited state of this system.

 

  1. (a) What are the three important approximations of Huckel-LCAO-MO theory?

(b) Using this theory set up the secular equation and secular determinant for

ethylene and hence obtain its energy levels and corresponding wave functions.

 

  1. What is a permutation operator? State and illustrate the Pauli Exclusion Principle for

the ground state of He atom that wave functions must be antisymmetric in the

interchange of any two electrons.

 

  1. (a) Derive the time-independent Schroedinger equation from the time-dependent

equation and show that the property such as electron density is time independent

although the wave function describing an electron is time dependent.

(b) The microwave spectrum of the CN radical shows a series of lines spaced by a

nearly constant amount of 3.798 cm-1. What is the bond length of CN?        (6+4)

 

  1. (a) In solving the H2+ problem using the LCAO method, the lowest energy obtained is

given by E+ = (HAA + HAB) / (1+SAB) where A and B refer to the two hydrogen

nuclei. Explain each of the integrals in the above equation and their significance

(b) Outline the salient features of VB (Heitler-London) theory as applied to H2

                 molecule                                                                                                         (5+5)

 

  1. The MoO4 belongs to the Td point group. Find the reducible representation for the

molecule using the four Mo – O bonds as bases and reduce this into irreducible

representation using the Td character table given below and show that the bonds in

MoO4 are more likely to be sd3 hybrids.

 

Td          E          8C3      3C2      6S4       6σd

 

 

A1        1          1          1         1         1                                 x2+y2+z2

A2        1          1          1         -1         -1

E         2          -1         2         0         0                                 (2z2-x2-y2, x2-y2)

T1        3          0          -1         1         -1         (Rx,Ry,Rz)

T2         3          0          -1         -1         1         (x,y,z)              (xy,xz,yz)

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Photochemistry & Organic Synthesis Question Paper PDF Download

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                            LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 22

THIRD SEMESTER – NOV 2006

         CH 3808 – PHOTOCHEMISTRY AND ORGANIC SYNTHESIS

 

 

Date & Time : 25-10-2006/9.00-12.00   Dept. No.                                                       Max. : 100 Marks

 

 

 

 

Part A

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

 

  1. What is benzoin reaction?
  2. Draw the Frontier Molecular Orbital interaction of 1,3-butadiene and ethylene under photochemical conditions.
  3. How will you effect the following isomerisation? Write the mechanism.

 

  1. Write the Woodward Hoffmann rules for electrocyclization reaction.
  2. Explain the change in the geometry of excited state molecule in a photochemical process and the variation in its physical property.
  3. What is Norrish type I and II cleavage reactions? Give suitable examples.
  4. What are the important guidelines to be followed while choosing alternate synthetic route?
  5. Explain the umpolung concept of synthesis with suitable example.
  6. Explain the mechanism of the following reaction.

 

  1. What are the products formed when benzene is subjected to Birch reduction?

 

Part B

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

 

  1. Explain Michel addition reaction with an example.
  2. Draw correlation diagram for the electrocyclization of 1,3,5-hexatriene for the dis-rotatory approach. State whether the reaction is feasible by thermal or photochemical means.
  3. Predict the products in the following pericyclic reactions and explain the mechanism with proper stereochemistry.

 

 

 

 

 

 

 

 

  1. Predict the mechanism of the following reaction.

 

  1. Explain the mechanism of Paterno Buchii reaction. How does this take place in case of an alkyne?
  2. Explain the mechanism of photochemical rearrangement of 4,4-diphenylcyclo- hexenone.
  3. Describe a general scheme of synthesizing various mono functionalized compounds starting from alcohols.
  4. Describe a suitable method to prepare the following compounds.

 

 

 

  1. What is chemoselectivity? How well are chemoselective reactions performed? Explain with any two examples.
  2. Explain the mechanism of electroorganic synthesis with an example.
  3. How is cubane synthesized? Explain the mechanism.
  4. Explain the mechanism of oxidation using
  5. a) mercuric acetate and b) SeO2.

 

Part C

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

 

  1. a) Explain the mechanism of following reactions.
  2. i) Hydroboration of carbonyls ii) Darzens reaction.
  3. b) Predict the reaction mechanism of the following reaction.

 

 

 

  1. a) Predict the product in the following sigmatropic rearrangement reactions.

 

 

 

  1. b) Explain the effect of substituents on the cycloaddition reactions.

 

 

 

 

 

 

 

 

 

  1. a) Predict the product and explain the mechanism of following reactions.

 

 

 

  1. b) Derive Stern Volmer expression for photochemical quenching.
  2. Explain the complete retrosynthetic analysis and subsequent synthesis of longifolene.
  3. Explain the mechanism of following reactions.
  4. a) Wolf Kishner reduction
  5. b) Claisen-Schmidt reaction
  6. c) Stobbe reaction with aromatic ketones
  7. Explain the retrosynthetic analysis of the following compounds

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Organic Reaction Mechanism & Stereochemistry Question Paper PDF Download

by

                        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 14

FIRST SEMESTER – NOV 2006

CH 1806 – ORGANIC REACTION MECHANISM & STEREOCHEMISTRY

 

 

Date & Time : 28-10-2006/1.00-4.00     Dept. No.                                                       Max. : 100 Marks

 

 

 

PART A

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

 

  1. What is transition state theory? Mention its importance.
  2. What are the various kinetics experiments to study the mechanism of a particular reaction?
  3. Classify the rearrangement reactions and give example for each.
  4. What is memory effect? Explain with an example.
  5. Write a short note on catalytic dehydrogenation.
  6. Explain Cram’s rule with a suitable example.
  7. Explain why meso-stilbene dichloride on heating with pyridine at 200°C gives no product while dl-isomer gives alkene readily.
  8. What is epimerisation? Give an example.
  9. Explain Walden inversion with a suitable example.
  10. Explain the racemization via cations with a suitable example.

 

 

PART B

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

 

  1. How trapping of intermediate, cross-over experiments and isotopic labeling studies help to show that a reaction is intermolecular? Explain with suitable examples. (5)
  2. How does the kinetics study in chain and parallel reactions help to design the reaction mechanism? Explain with suitable examples. (5)
  3. Explain the mechanism of the following rearrangement reactions. (2 ´ 2½)
  4. a) Beckman rearrangement b) Baeyer Villiger rearrangement
  5. a) Why secondary amides do not undergo Hoffmann degradation? Give reasons. (2½)
  6. b) Explain the mechanism of Claisen rearrangement with suitable example. (2½)
  7. Explain the mechanism of NaBH4 reduction. How is it chemoselective? Explain with an example.                                                                                                    (5)
  8. How direct electron transfer can bring in reduction? Explain the mechanism with any two examples.                                                                                                    (5)
  9. Predict the Cotton effect by the sign of the most occupied octant in the following compounds:

(i) (+)-trans-1-methyl-2-decalone            (ii) 5a-cholestan-6-one.   Explain.                  (2 ´ 2½)

  1. Dehydrobromination of diastereoisomeric a-phenyl-b-bromo-b-benzoylpropionic acids with    hot pyridine give different products.  Explain.
  2. Write notes on: a) asymmetric destruction  and  b) asymmetric synthesis
  3. ‘The cotton effect curves of (+)-3-methylcyclopentanone in methanol shows only a 24%                 reaction upon addition of acid’.  Explain.
  4. Give an example for first order and second order asymmetric transformations. Explain.
  5. What are the different methods of resolution of racemic mixture? Explain any two methods.

 

 

PART C

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

 

  1. a) How does the kinetics study help to design the reaction mechanism in the following      reactions?                                                                                                    (2 ´ 2½)
  2. i) Aldol condensation ii) Benzidine rearrangement
  3. b) How stereochemical study and isotopic labeling study help to design a reaction      mechanism as intramolecular? Explain with suitable examples.                                   (5)
  4. a) Explain the mechanism of                                                             (2 ´ 2½)
  5. i) Fischer Indole synthesis and      ii) Favorskii rearrangement
  6. b) Predict the products in the following reactions. Give suitable reasons. (5)

 

  1. a) Explain the reductive coupling of carbonyl compounds with any two examples. (5)
  2. b) How does specific dehydrogenation in steroids take place? Explain the mechanism with an (5)
  3. a) Explain the octant rule with a suitable example.
    b) Predict the Cotton effect by the sign of the most occupied octant in the following     compounds:

(i) 3-bromo-4-methoxycyclohexanone           (ii) 3-methylcyclohexanone

  1. Explain the following:
    a)  trans-4-t-butylcyclohexane carboxylic acid is more stronger than cis-isomer.
    b) erythro-3-bromo-2-butanol with HBr gives meso product
    c) Dehydrochlorination of 1,2-diphenyl-1-chloroethane gives trans product fastly but cis     product slowly.
  2. a) Explain the following with suitable example.
    a)      Asymmetric destruction
    b)      Bredt’s rule
  3. c) Axial haloketone rule
  4. Prelog’s rules

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Organic Chemistry-III Question Paper PDF Download

by

                            LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 18

THIRD SEMESTER – NOV 2006

                              CH 3800 – ORGANIC CHEMISTRY – III

 

 

Date & Time : 25-10-2006/9.00-12.00      Dept. No.                                                    Max. : 100 Marks

 

 

 

Part A

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

  1. Write a short note on [4+2]-cycloaddition in dipolar compounds.
  2. What is a cheletropic reaction? Give an example.
  3. What is Alder’s endo rule. Explain with an example.
  4. Define the following. a) Photo quenching b) II law of photochemistry
  5. Write a short note on the fate of the excited state molecules in a photochemical reaction.
  6. Explain retro synthetic approach with an example.
  7. What are annelation reactions? Give an example.
  8. How would you plan the synthesis of 3-methyl-6-hepten-2-one by span technique?
  9. Give a synthesis based on umpolung concept of seebach.
  10. What are the importance of three component system in Clemmensen reduction?

 

 

Part B

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

  1. Draw a correlation diagram for the cycloaddition reaction of 1,3-butadiene and ethylene. State whether the reaction is thermally or photochemically feasible.
  2. Predict the products in the following pericyclic reactions and explain the mechanism with proper stereochemistry.

 

 

  1. Predict the mechanism of the following reaction.

 

  1. Derive Stern Volmer expression for photochemical quenching.
  2. Explain the photochemical rearrangement of 4,4-diphenylcyclohexenone.
  3. What is Barton reaction? Explain its reaction mechanism in a steroidal compound.

 

 

 

17.    Explain the mechanism of Birch reduction. Identify the products obtained when the following are subjected to this reduction: (a) Benzoic acid and (b) Anisole.  Justify your answer.

18.    Explain the importance of electroorganic synthesis over the conventional synthesis in synthesizing bridged compounds with suitable examples.

19.    Explain the synthesis of reserpine.

20.    Explain the mechanism of Reformatsky reaction.  How is this reaction useful in organic synthesis?

21.    Oxymercuration-demercuration reactions follow Markownikov’s addition while Hydroboration-oxidation follows Anti-Markownikov’s addition. Why?  Explain with two suitable examples.

22.    What are stereospecific control elements?  How are they useful in organic  synthesis?

Part C

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

  1. Predict the reaction mechanism of the following reactions.

a)

 

b)

 

 

  1. a) Predict the products of following reactions.

 

 

  1. b) “Cycloaddition reactions are regioselective.” Explain with any two examples.

 

 

 

 

 

 

 

  1. a) Photo reduction of benzophenone with diphenylmethanol involves a quantum     yield of 1 compared to that of 2-propanol with 2. Explain.
  2. b) Explain the photochemical rearrangement of 4,4-diphenylcyclohexen-2,5-    dienone.
  3. a) How would you synthesise Norethisterone?
  4. b) What are the advantages of selenium dioxide oxidation? Explain the mechanism      with suitable examples.
  5. a) Explain the steps involved in the synthesis of longifoline.
  6. b) Identify the product in the following. Explain with mechanism.
    Me2C=CH-CO-CH3      A   +   B
  7. Explain the following:
  8. Perkin reaction is most widely used in the synthesis of coumarin.
  9. Benzaldehyde is condensed with ketonic ester in retrograde aldol condensation reaction.
  10. Alkylation of active methylene group is an important step in organic synthesis in increasing carbon skeleton.

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Organic Chemistry-I Question Paper PDF Download

by

                        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 12

FIRST SEMESTER – NOV 2006

CH 1801 – ORGANIC CHEMISTRY – I

 

 

Date & Time : 28-10-2006/1.00-4.00 Dept. No.                                                       Max. : 100 Marks

 

 

 

PART – A

Answer all the questions                                                                            (10 × 2 = 20 marks)

 

  1. Explain Prelog’s rule with a suitable example.
  2. In 4-t-butylcyclohexanecarboxylic acid, trans form is more acidic than cis isomer in 66% aquesous DMF.
  3. What is mutarotation? Give an example.
  4. Dehydrobromintion of threo-1-bromo-1,2-diphenylpropane is faster than erythro.
  5. Write the most stable conformation of
    (a) 1,2,2,6,6-pentamethol-4-hydroxy-4-phenylpiperidine
    (b) 1,3-di-t-butylcyclohexane
  6. Arrange the following compounds in the decreasing order of basicity. Justify your answer.

i)methylamine  ii) ethylamine  iii) n-propylamine  iv) iso-propylamine

  1. How does DS‡ factor help in understanding the kinetics of chemical reactions?
  2. Write the mechanism of Chichibabin reaction.
  3. What are consecutive reactions? Apply conditions and derive specific rate expression.
  4. How does trapping method help in determining the mechanism of a chemical reaction?

 

 

PART – B

Answer EIGHT the questions                                                                       (8 × 5 = 40 marks)

 

  1. Dehydrobromination of diastereoisomeric a-phenyl-b-bromo-b-benzolypropionic acids with hot pyridine give different products.
  2. Explain the determination of configuration of (-)mandelic acid and (-)phenylmethylcarbinol with respect to (+)lactic acid.
  3. Acetolysis of  diastereoisomeric   3-phenyl-2-pentyltosylate   and 2-phenyl-3-pentyltosylate give different products.   Account for your answer and explain the formation of the products.
  4. Explain Walden inversion with two suitable examples.
  5. Explain the racemization via cations and anions with suitable examples.
  6. Write notes on: a) asymmetric destruction  and  b) asymmetric synthesis
  7. How do inductive and field effects affect the second substitution in aromatic systems? Explain with suitable examples.
  8. Write the mechanism of following name reactions.
  9. a) Bucherer reaction     b) Fischer-Hepp rearrangement
  10. Account for the following
  11. a) Diazotization of aniline follows third order kinetics.
  12. b) 2,6-Dimethyl-4-nitroaniline is weaker base than 2,5-dimethyl-4-nitroaniline.
  13. Compare the ipso-attack in aromatic electrophilic substitution with the SNAr mechanism.    Explain with an example.
  14. The diazotization of aniline in moderately concentrated acid has been found to be

second order in HNO2. Explain.

 

 

  1. Predict the products in the following reactions.
  2. i)  2,4,5-trimethyliodobenzene  +  NaNH2                  ¾®   ?
  3. ii) 2,6-dimethyl-1,4-dinitrobenzene  +  C2H5O–         ¾®   ?

 

 

PART – C

Answer FOUR the questions                                                                                     (4 × 10 = 40 marks)

 

  1. a) How would you resolve (±)-alcohol mixture by a suitable resolving agent?
  2. b) ‘Mandelic acid is racemized by a base easily but not atrolactic acid’.
  3. a) How do isotopic labeling and stereochemistry help in predicting suitable reaction                  mechanisms? Give examples.
  4. b) How are the following conversions effected?
  5.                i)          benzene                                   ¾®    naphthalene
  6.             ii)         sodium phenylsulphonate       ¾®    sodium phenoxide
  7. a) Prove that Hammett equation is LFER. How is the orientation and reactivity of

electrophiles normally studied? Briefly explain with examples.

  1. b) How do cross over experiments help in determining the mechanism of a chemical

reaction. Explain with an example.

  1. a) Explain the octant rule with a suitable example.
    b) Predict the Cotton effect by the sign of the most occupied octant in the following     compounds:

(i) (+)-trans-1-methyl-2-decalone            (ii) 3-methylcyclohexanone

  1. Explain the following:
    a) meso-stilbene dichloride on heating with pyridine at 200°C gives no product while
    dl-isomer gives alkene readily.
    b) erythro-3-bromo-2-butanol with HBr gives meso product
    c) Dehydrochlorination of 1,2-diphenyl-1-chloroethane gives trans product fastly but cis     product slowly.
  2. Explain the following:
    a) The cotton effect curves of (+)-3-methylcyclopentanone in methanol shows only a 24%     reaction upon addition of acid.
  3. b) meso form of stilbene dichloride has a dipole moment 1.27D while the dl-pair has 2.75D.
    c) Debromination of meso-2,3-dibromobutane by iodide ion is faster than its dl–pair

 

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Loyola College M.Sc. Chemistry Nov 2006 Molecular Spectroscopy Question Paper PDF Download

by

                          LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 24

THIRD SEMESTER – NOV 2006

CH 3810 – MOLECULAR SPECTROSCOPY

 

 

Date & Time : 30-10-2006/9.00-12.00      Dept. No.                                                   Max. : 100 Marks

 

 

PART A

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

  1. Convert 0.15 nm to Hz and state what sort of transition this corresponds to.
  2. What are stokes and anti-stokes lines?
  3. Name two techniques to enhance the sensitivity of the spectral lines.
  4. What is the basic principle of Mossbauer spectroscopy?
  5. From the relative abundance of the (M+2)+ peaks in the mass spectra, can you distinguish chloro compounds from Bromo compounds?
  6. State the principle of PES. What is the essential difference between XPES and UV-PES?
  7. A free electron is placed in a magnetic field of strength 1.3 T. If ge is 2.0023 and βe is 9.274 x 10-24 JT-1. Find the ESR frequency in GHz.
  8. What are the advantages of using TMS as the standard in NMR experiments?
  9. Compare the 1H and 13C NMR spectra in terms of the range of chemical shifts and intensity of the peaks (peak areas)
  10. What is spin-spin relaxation?

PART – B

Answer ANY EIGHT questions                                          (8 x 5 = 40 Marks)

  1. What are the factors that affect the width of the spectral lines? Explain any two of them.
  2. The observed infrared absorption and Raman spectral lines of Chlorate ion (ClO3–) are given below. Predict the structure of Chlorate ion.
Raman Frequencies (cm-1 )                        IR Frequencies (cm-1

450 (depolarized)                                           434 (^)

610 (polarized)                                               624 (||)

940  (depolarized)                                          950 (^)

982 (polarized)                                               994 (||)

 

  1. The frequencies of vibration of the following molecules in their v = 0 states are HCl: 2885 cm-1; D2: 2990 cm-1; DCl: 1990 cm-1 and HD: 3627 cm-1, calculate the energy change in the reaction HCl + D2 à DCl + HD.
  2. The mass spectrum of a compound having the empirical formula C11H12O2, shows the following peaks at m/e : 78,105 (Base peak), 122, 135,176 (Molecular Peak). Identify the compound and account for the fragments.
  3. At what temperature will the number of I2 molecules in the v=1 level be one-tenth of that in the v=0 level? Given = 214.6 cm-1;xe = 0.6 cm-1 and k = 1.38 x 10-23J K-1.
  4. Explain Quadrupole mass spectrometer.
  5. Explain what is Zero Field or Crystal Field Effect in the fine structure of ESR

and the factors that contribute to that.

  1. State and explain Franck-Condon Principle. With diagrams explain the

variations in intensity of electronic spectra explained by this principle?

  1. What is population inversion? Prove that a population inversion cannot

be achieved in a two level system while it is possible in a three level system.

  1. (a) With an example explain Diamagnetic Anisotropy.

(b) The chemical shift of the CH3 protons in diethyl ether is ∂ = 1.16 ppm and that of the CH2 protons is 3.36 ppm. What is the difference in local magnetic fields between the two regions of the molecule when the applied field is 16.5 T?

  1. Predict

(a) the spin-spin splitting pattern for the protons of neopentane molecule

and the peaks’ intensity distribution.

(b) the hyperfine splitting of the ESR spectrum of ۰CD3 and ۰CHD2 radicals.

[note: the spin of D is 1]

  1. Explain the principle of 2D NMR highlighting its advantages.

PART – C

Answer ANY FOUR questions                                            (4 x 10 = 40 Marks)

  1. a) Three consecutive lines in the rotational spectrum of a diatomic molecule are observed at 84.544, 101.355 and 118.112 cm-1.  Assign these lines to their appropriate J’’ àJ’ transitions and deduce the values of B and D.
  2. b) How are meta stable ions produced and how are they useful in identifying the molecular formula of a compound?
  3. a) The fundamental band of HCl is centered at 2886 cm-1.  Assuming that the internuclear distance is 12.76 nm, calculate the wave number of the first two lines of each of the P and R branches of HCl.
  4. b) Explain the pure rotational spectra of symmetric top molecules.
  5. a) Explain the fact that the Mossbauer spectrum of [Fe(CN)5NO]2- gives two lines whereas [Fe(CN)6]4- spectrum gives one line.
  6. b) In the rotational Raman spectrum of HCl, the displacements from the exciting lines are represented by Dn = ± (62.4 + 41.6 J) cm-1.  Calculate the moment of inertia of the HCl molecule.
  7. Explain the following with a suitable example:

(a) spin-spin coupling in 1H-NMR

(b) mechanism of spin-spin coupling for geminal protons

(c) the multiplicity and intensity distribution represented by the ‘coupling tree’

 

  1. (a) Explain briefly: (a) spin-spin relaxation (b) Fourier Transformation Technique.

(b) Sketch the esr spectrum of °CH3 and explain its nuclear hyperfine splitting.

 

  1. (a) What are asymmetry electric field gradient and asymmetry parameter, η? How

are they related? What is the significance of η?

(b) Taking any laser as example explain the three most important components

of a laser?

 

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Loyola College M.Sc. Chemistry Nov 2006 Material Science Question Paper PDF Download

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                        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 25

THIRD SEMESTER – NOV 2006

CH 3875 – MATERIAL SCIENCE

 

 

Date & Time : 06-11-2006/9.00-12.00   Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

Answer all the questions                                  (10 x 2 = 20)

 

  1. What are “glide planes”?
  2. Give the expression for Brinell Hardness number.
  3. Mention few applications of single crystals.
  4. List the thermodynamical properties that can be measured using TG/DSC methods.
  5. Write a note on “electron charge density maps”.
  6. What is Meissner effect?
  7. What is Hall effect?
  8. What is breakdown diode? What are its uses?
  9. What is Josephson’s effect?
  10. What are ferrites? What is the role of this compound in super conductivity?

 

 

PART – B

 

Answer any eight questions                                 (8 x 5 = 40)

 

  1. Outline the principle, instrumentation and applications of thermogravimetric method.
  2. State Brags’s law. Discuss the powder method of X-ray diffraction.
  3. With neat sketch explain the Bridgman-Stockbarger method of crystal growth from melt.
  4. What are Miller indices? Illustrate their formation in different planes of a cube.
  5. Discuss the role of modulus as an essential parameter in the structural design.
  6. Describe the slow evaporation technique of growing crystals with Manson jar apparatus.
  7. How are cooper pairs formed? Explain BCS theory of superconductivity.
  8. Describe the role of TaS2 in high temperature superconductivity.
  9. Describe domain theory to account for the Hysteresis behaviours of magnetic materials.
  10. Write short notes on a) LED b) Photo voltaic cell.
  11. Explain qualitatively how a p-n junction functions as a rectifier.
  12. Distinguish between Zenner breakdown and avalanche breakdown.

 

 

 

PART – C

 

Answer any four questions                                                 (4 x 10 = 40)

 

  1. Describe (i) Chemical reaction (ii) Chemical reduction (iii) Complex decomplexion and (iv)    solubility reduction methods of growing single crystals by gel.
  2. Outline the essential features of rubber like elasticity. Obtain the equation of            state for           the rubbering material.
  3. What is meant by symmetry operation? Describe point group and space group        symmetry        elements with necessary diagram.
  1. Explain the working of a p-n junction. Discuss forward and reverse biasing of p-n junction.
  2. Describe the behaviour and properties of conductors, insulators and semiconductors on the    basis of band theory.
  3. Write short notes on a) 1-2-3 oxides b) Chevral phases c) hard and soft magnetic materials.

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Instrumental Analysis Question Paper PDF Download

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                        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – PHYSICS

AD 26

THIRD SEMESTER – NOV 2006

CH 3900 – INSTRUMENTAL ANALYSIS (FOR PHYSICS)

 

 

Date & Time : 03-11-2006/9.00-12.00     Dept. No.                                                    Max. : 100 Marks

 

 

PART – A

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

 

  1. A sample of well water is found to contain 0.5000 g CaCO3 in 1 kg water sample.  Find out the concentration of calcium in mg mL-1.
  2. What is the pH of a solution containing 400 mg NaOH in 100 mL H2O.
  3. Explain red shift with an example.
  4. Mention the cell and detector used in IR spectroscopy.
  5. Compare the solubility of Agcl(s) in (i) pure H2O  (ii) 0.1 M aq. KCl and (iii) 0.1 m aq. KNO3.
  6. Mention factors which influence the quality of crystals obtained during recrystallization.
  7. How is adsorption different from absorption?
  8. What is retention factor in chromatography?  What is its significance?
  9. Why is low pressure distillation used to purify some compounds?
  10. Give the general principles of thermal analytical techniques.

 

PART – B

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

 

  1. How is 1.0000 m HCl prepared from con. HCl?
  2. Drive Beer Lambert’s law.  How is it verified?
  3. Explain the principle of flame photometry.
  4. Determine the solubility of lead iodide in 0.0100 m aq. Pb(NO3)2 . Ksp of pbI2 is 1 ´ 10-10 mol3 dm-9.
  5. A solution containing 8.75 ppm KMnO4 has a transmittance of 0.743 in a 1 cm cell at 520 nm.  Calculate the molar absorptivity of KMnO4.
  6. What is the molarity of commercial H2SO4, containing 98% by weight with specific gravity 1.84 g mL-1.
  7. What is fractional distillation?  What are its advantages and limitations?
  8. Explain mobile phase, immobile phase, eluent and detection of compounds in paper chromatography.
  9. How is column for column chromatography prepared?  What are substances generally used to prepare these columns?
  10. How are compounds extracted from parts of plants?
  11. Discuss factors affecting DTA curves.
  12. Write notes on (i) sublimation (ii) thermometric titrations.

 

PART – C

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

 

  1. How is the pH of a solution determined using potentiometer?
  2. Draw the flow sheet diagram of UV-visible double beam spectrophotometer and explain the function of the components.
  3. (a) Draw the thermogram of CaC2O4.H2O(s) and explain.

(b) Explain the factors affecting thermogram.

  1. Explain steam distillation taking isomers of nitrophenol as examples.
  2. Write an essay on ion-exchange chromatography and its applications.
  3. Write notes on:

(i)  Molarity and Normality

(ii) Common ion effect

(iii)Thermal Conductivity Detector                                                                (3 + 3 + 4)

 

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Loyola College M.Sc. Chemistry Nov 2006 Coordination Chemistry Question Paper PDF Download

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                            LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 20

THIRD SEMESTER – NOV 2006

CH 3802 – COORDINATION CHEMISTRY

 

 

Date & Time : 27-10-2006/9.00-12.00   Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

 

Answer the following:                                                                                    (10 x 2 = 20 marks)

 

  1. Draw the structure of optically inactive isomer of the following, giving reasons for optical inactivity [Co (ox)2 Cl2]-3 ion (ox = oxalato).
  2. Give the IUPAC names of (i) ferrocene (ii) nickeltetracarbonyl.
  3. What are the defects of VBT?
  4. Mention the assumption used by crystal field theory?
  5. What is nephelauxetic effect?
  6. What is CRSE?  Calculate CFSE of a d8 metal ion containing coordination compound.
  7. What are complimentary and non-complimentary electron transfer reactions?
  8. What are thermodynamically stable and kinetically stable coordination compounds?
  9. Explain 18 electron rule with an example.
  10. Give structures of any two industrially useful coordination compounds.

 

PART – B

 

Answer any EIGHT of the following                                                            (8 x 5 = 40 marks)

 

  1. What is chelate effect?  Give thermodynamic explanation for this effect.
  2. Why does electronic spectrum of [Ti (H2O)6]3+ show a shoulder, though Ti3+ is a d’ system?
  3. Why is [Cu(en)3]2+ less stable than [Cu(en)2 Cl2]+?
  4. Explain the theoretical basis of trans effect.
  5. How is esr spectrum useful in proving covalency in M-L bond?
  6. Explain Job’s method of continuous variation?  What is inferred from this experiment?
  7. Draw and explain various types of overlap of orbitals of central atom/ion and ligand to from a p bond in an octahedral molecule.
  8. How is Mossbauer spectroscopy useful in deducing geometry of Fe3(CO)12?
  9. Discuss bonding nature of p – electron delocalized ligands with central atom/ion.
  10. What is the central metal atom present in Vitamin B12?  What is its oxidation state?  What is the use of this vitamin?
  11. Give an account of orgamometallic compounds.
  12. Explain any two uses of coordination compounds in laboratories.

 

PART – C

 

Answer any FOUR of the following                                                                         (4 x 10 = 40 marks)

 

  1. What are the factors affecting CFSP of coordination compound?  Explain each factor.
  2. Draw energy level diagram and explain the formation of a square planar molecule according to CFT.
  3. What are the differences between Tanabe-Sugano diagram and Orgel diagram?
  4. Discuss SN1, SN2 and SN CB mechanisms of an octahedral coordination compound.
  5. List and explain various photochemical and photo physical processes of coordination compounds.
  6. Write short notes on (i) Marcus – Hush Theory       (ii) Oxygen transport.                 (5+5)

 

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Loyola College M.Sc. Chemistry Nov 2006 Chemical Kinetics Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034  M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 19

THIRD SEMESTER – NOV 2006

         CH 3801 – CHEMICAL KINETICS

 

 

Date & Time : 01-11-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

PART – A                          (10 ´ 2 = 20 marks)

 

Answer ALL the questions.

 

  1. Differentiate time order from true order.
  2. The half life of C–14 is 5770 years. Starting with 100 mg of C–14, how much of
    it would remain after 17,310 years.  Also calculate the decay constant.
  3. What is the effect of ionic strength on the rate constant of the following reaction
    in solution?

[Fe(CN)6]4– + S2O82– ®  products

  1. Show that the Collision theory of activation energy is less than the energy of
    activation calculated from Arrhenius equation.
  2. Write down the expression for the rate constant of a reaction between two linear
    molecules forming a linear activated complex on the basis of ARRT.
  3. What are “Skrabal plots”?
  4. For an enzyme catalysed reaction KM = 25 ´ 10­–3 M and the turnover number

is 4 ´ 107 s–1, calculate the limiting rate of the reaction if [E]0­ = 1.6 ´ 10–8 M.

  1. Mention all the steps involved in the thermal decomposition of acetaldehyde
    following a chain reaction.
  2. “Adsorption if spontaneous is generally exothermic”. Explain.
  3. Explain why conventional methods cannot be used for the study of kinetics of
    very rapid reactions.

 

PART – B

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

 

  1. The rate of a reaction of the type A + B ® products was studied in solution phase
    at 298 K with initial concentration of each reactant at 0.02 M.  From the
    following data determine the order of the reaction and calculate the rate constant.

Time (min.)                                 20                            30                 40

Conc. of ‘A’ reacted

in ‘t’  (mol’/l)                      8.76 ´ 10-3              1.07 ´ 10–2    1.21 ´ 10–2

  1. Derive an expression for the total number of collisions of all molecules of ‘A’
    with all molecules of ‘B’.
  2. Explain the kinetics of unimolecular gaseous reaction using Lindemann’s theory.
  3. For hydrolysis of sulphamic acid the rate constant is 1.16 ´ 10–3 l mol–1 s–1 at
    90°C with Ea = 127.61 kJ mol–1.  Calculate DG±,  DH±  and  DS± of the reaction
    occurring in solution phase.
  4. Explain the significance of potential energy surfaces with an example.
  5. What is the importance of “volume of activation” in the study of kinetics of
    reactions in solution.  Explain.
  6. Explain the concept of Arrhenius and Van’t Hoff type intermediates.

 

 

 

  1. Show that “Bronsted–Catalytic law” is a form of LFER (Linear Free Energy
    Relation)
  2. The decomposition of PH3(g) on a tungsten filament follows first order kinetics at
    low gas pressure and zero order kinetics at very high pressure.  Explain.
  3. 227Ac has a half life of 21.8 years with respect to radioactive decay. The decay
    follows two parallel paths one leading to Th–227 and the other to Fr–223.  The
    percentage yields of these two daughter nuclides are 1.2% and 98.8%
    respectively.    Calculate the rate constant in y–1 for each of the paths.
  4. How is surface area of a solid determined using “BET equation”.
  5. Explain the principle of “flash photolysis”.

 

 

PART – C

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

 

23.(a)How is order of a reaction determined using dimensionless parameters.
Explain.                                                                                                  (6)

(b)Calculate the translational partition function of CO(g) in the standard state of
1 mol/l at 27° C.                                                                                    (4)

24.(a) Explain the “single sphere model” for a reaction between two ions in

solution.                                                                                                            (5)

(b) Discuss the importance of Hammett equation with one example.       (5)

  1. Explain the kinetics of bimolecular surface reactions with a specific example.

Derive the relevant rate laws in each mechanism.                               (5 + 5)

  1. Discuss the kinetic scheme for a single substrate enzymatic reaction and

Explain how the kinetic parameters can be evaluated.                        (5 + 5)

  1. Explain any two of the following: (5 + 5)

(a) Kinetics of reversible reactions (both I order)

(b) Determination of   kH+  for an acid catalysed reaction.

(c) Expression for relaxation time for a I order reaction

(d) Stern–Volmer equation

  1. (a) The decomposition of ozone 2O3 ® 3O2 proceeds through the mechanism

 

(i) O3 Û O2 + O with k1 is the rate constant for the forward reaction and k2 is the rate constant for the backward reaction

(ii) O3 + O  Û 2O2 (slow step)

Derive expression for the rate of reaction using

  • equilibrium approach for step (i)
  • Steady state treatment for O . (7)

(b) How is the energy of activation for the overall reaction above related to the
energies of activation for the individual steps?                                 (3)

 

 

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Loyola College M.Sc. Chemistry Nov 2006 Analytical Chemistry-III Question Paper PDF Download

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                           LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

AD 21

THIRD SEMESTER – NOV 2006

CH 3805 – ANALYTICAL CHEMISTRY – III

 

 

Date & Time : 08-11-2006/9.00-12.00   Dept. No.                                                   Max. : 100 Marks

 

 

 

PART – A

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

 

  1. How many litres of water can be chlorinated using 1 kg bleaching powder containing 30% available chlorine.  Assume the allowable limit of cl2 in water is 2 ppm.
  2. Can ‘trien’ be used as a titrant to estimate Cu+2? Why?
  3. How are indicators chosen for redox titration?
  4. Compare the solubility of lead iodide in (i) pure H2O  (ii) 0.1 M aq. KNO3
    (iii) 0.1 M aq. KI.
  5. Define confidence interval.
  6. How does potentiometry differ from voltametry.
  7. Differentiate electrogravimetry and coulometry.
  8. Draw the plot of Emf vs Time for
  • Linear sean
  • Differential pulse.
  1. What is supporting electrolyte?  Explain its role.
  2. Define quantum yield.  Account for the high quantum yield of the reaction between H2 and Cl2.

 

PART – B

 

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

 

  1. How will you proceed to collect authentic data from research?
  2. Explain the importance of vonweimarnn ratio in gravimetric analysis.
  3. Discuss the factors which influence Dpm/Dv in complexometry.
  4. describe the salient features of acid base titration in non-aqueous solvents?
  5. Show that the equivalence point potential for the titration of Fe+2 vs MnO in acidic medium is dependent on pH.
  6. Draw the titration curve for the titration of 20.00mL of 0.1000 m CH3COOH vs
    0.0500 m NaOH.  Ka of CH3COOH is 10-5.
  7. a) How will you determine electrode discharge potential.
  1. b) Explain the factors that may affect the nature of electro deposition.
  1. Draw a typical cyclic voltagram and indicate ip(a) , ip(c), Ep(a) and Ep(c) on the diagram.
  2. Explain how polarographic method can be used in quantitative studies.
  3. Explain the following briefly
    a) Flame photometry      b) Atomic absorption spectroscopy.
  4. Explain the construction and working of hallocathode.
  5. How will you prove the liberation of carbon monoxide.  Illustrate with an example.

 

 

 

 

PART – C

 

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

 

  1. Cone common way to determine phosphorus in Urine is to treat the sample, after removing the protein, with molybdenum (VI) and then reduce the resulting
    12-molybdophosphate complex with ascorbic acid to give an intense blue coloured species called molybdenum blue.  The absorbance of molybdenum blue can be measured at 650 nm.  A patient produced 1122 mL of Urine in 24 hours.  A 1.00 mL aliquot of the sample was treated with Mo(VI) and ascorbic acid and was diluted to a volume of
    50.00 ml.  A calibration curve was prepared by treating 1.00 mL aliquots of phosphate standard solutions in the same manner as the urine sample. The absorbances of the standards and the urine sample were obtained at 650 nm and the following results were obtained.
Solution ppm of  P. Absorbance at 650 nm
1.00 0.230
2.00 0.436
3.00 0.638
4.00 0.848
Urine sample 0.518

Apply the method of least squares to fine the slope, intercept and the standard deviation

of the results Determine the concentration of  P in ppm in Urine sample.

 

  1. A 0.3284 g sample of brass (containing Pb, Zn, Cu, Sn,) was dissolved in HNO3.  The sparingly soluble SnO2.4H2O was removed by filtration and the combined filtrated and washings were then diluted to 500.00 mL.  A 10.00 mL aliquot was suitably buffered; titration of the pb, Zn, Cu in this aliquot required 37.56 mL of 0.002500 M EDTA.  The copper in a 25.00 mL  aliquot was masked with tholulfate;  the Pb and Zn were then titrated with 27.60 mL of the EDTA solution.  Cyanide ion was used to mask the Cu and Zn in a 100.00 mL aliquot; 10.80 mL of the EDTA solution was needed to titrate the Pb ion.  Determine the composition of the brass sample;  evaluate the percentage of Sn by difference.

 

  1. a) Find out the gravimetric factor if Fe+3 is precipitated as Fe(OH)3 and weighed asFe2O3.
  1. b) A 0.6407 g sample containing Cl– and I– gave silver halide precipitate weighing
    4430 g. This precipitate was than strongly heated in a stream of Cl2 gas to convert the AgI to Agcl; On completion of this treatment, the precipitate weighted 0.3181 g. Calculate the percentage of Cl– and I– in the sample.

 

  1. a) Draw a typical polarogram and indicate (i) residual current (ii) limiting current
    (iii)diffusion current on the graph drawing.
  1. b) State Ilkovic equation. Explain the terms in it and its applications.

 

  1. a) Explain how cyclic voltametry is usefull to determine (i) reversibility
    (ii) Electro chemical stability of a reaction.
  1. b) Write a note on chemiluminescence.
  1. a) Explain a and differentiate the following  (i) TGA & DTGA  (ii) DSC & DTA
  1. b) Calcium oxalate mono hydrate loses H2O at 100 – 250o Co (at 400 – 500oC) and

CO2 (at 650 – 660o C) Draw its TGA when 0.25 g is heated to 700oC at fixed

Atmosphere.

 

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Loyola College M.Com Nov 2003 Income Tax Law & Practice-II Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034

M.Com., DEGREE EXAMINATION – COMMERCE

THIRD SEMESTER – NOVEMBER 2004

CO 3952 – INCOME TAX LAW & PRACTICE – II

02.11.2004                                                                                                           Max:100 marks

1.00 – 4.00 p.m.

 

SECTION – A

 

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

 

  1. Define the term Business as per IT Act.
  2. What do you mean by Block of Assets?
  3. What do you mean by clubbing of Income?
  4. What is Intra – Head Adjustment of Loss?
  5. Define the term TRUST.
  6. What is the meaning of change in the constitution of a firm?
  7. What is meant by Partnership firm assessed as Association of persons?
  8. What is Residence of Company?
  9. How the minor’s Income is treated under Income – Tax Act?
  10. Give the order of set off of carried forward of losses.

 

SECTION – B

 

Answer any FIVE questions                                                                         (5 ´ 8 = 40 marks)

 

  1. Explain the various points to be considered while allowing depreciation on the Assets.

 

  1. Discuss the Deemed Incomes under section 69.

 

  1. Following are the particulars submitted by Mr.Kuldeep for the year ending 21st march 2004. Compute his total income:

(i) Income from House property:                                   Rs.

  1. a) Income from house ‘A’    –        60,000
  2. b) Loss from house ‘B’ (Both are let out) –       20,000

(ii) Income from Business or profession:

  1. a) Income from cloth business    –        30,000
  2. b) Loss from Hardware business    –        60,000
  3. c) Loss from speculation business    –        10,000

(iii) Income from other sources:

  1. a) Income from Lottery    –        25,000
  2. b) Loss from maintenance of race horses –          7,000
  3. c) Interest on securities    –        10,000

(iv) Cross salary                                                 –        66,000

 

  1. Discuss the Admissibility of following expenses/losses:
  • Loss by embezzlement by employees and theft by outsiders or through negligence of employees.
  • Membership fee paid to the Indian Institute of foreign trade.
  • Premium paid on ‘loss of profit (on account of strike, lock-out etc) policy.
  • Professional Tax paid to local Authority.
  • Amount paid to the employee under the profit – sharing scheme adopted by the employer.
  • Interest charged to a partner on debit balance.

 

  1. Calculate depreciation allowance for the assessment year 2004 – 05 from the details given below by Mr.X:
  • The written value of the Assets on April, 2003 was:

Rs.

Office Building                       –           2,00,000

Factory Building                     –           3,00,000

Workers Recreation Room      –              29,000

Machinery                               –           1,50,000

Furniture                                 –              25,000

Type writer                              –              11,000

Tractor                                     –              25,000

  • A new machine costing Rs.50,000 was installed on 20th July 2003.
  • A new typewriter was purchased for Rs.5,000 on 1st 2003.
  • A new foreign car purchased for Rs.2,30,000 on 1-2-2004.
  • Extension at a cost of Rs.50,000 was made during the year in the office building.
  • Furniture of the written – down value of Rs.3,500 was discounted on 1st Jan 2004. It has been sold for Rs.1,400 on 1-2-2004.

 

  1. Explain the exempted incomes in case of charitable or religious trusts.

 

  1. Explain the provisions of minimum alternative tax on companies u/s 115 JA.

 

  1. Write a note on Expenditure incurred in the field of Scientific Research.

 

SECTION – C

 

Answer any TWO questions                                                                          (2 ´ 20 = 40 marks)

 

  1. Explain the incomes of other persons included with the total income of the Assessee under sec 60 – 64.

 

  1. A, B, and C are partners in a firm, sharing profits and losses in the ratio of 2 : 2 : 1 respectively.  The profit and loss Account for the year ended 31st march, 2004 is as follows:

Rs.                                                                   Rs.

To Sunday Trade expenses           1,02,000          By Cross Profit                       2,78,200

To Interest on Capital @ 13%                              By interest on securities             10,000

A         13,000                                                             (gross)

B           6,500

C           6,500

———                26,000

To Rent to B                                    30,000

To Salary to B                                  72,000

To Commission to C                        36,000

To Net profit                                    22,200

————                                                        ————-

2,88,200                                                          2,88,200

————                                                        ————-

Compute the total income of the firm and Taxable Income of the three partners in the firm.

B and C are working partners.

 

  1. X is a registered medical practitioner. She keeps her books on cash basis.  The summarized cash Account for the year ended 31st march 2004 is as under.

Rs.                                                                   Rs.

Opening Balance                     2,700              Cost of medicines                   20,000

Bank Loan                              6,000              Surgical equipment                   6,000

Sale of medicines                   30,500              Motor car                                12,000

Consultation fees                   10,000              Salary                                        1,200

Visiting fees                            8,000              Rend of Dispensary                  1,200

Interest on Investments          9,000              General expenses                         600

Rent from property                 7,200              Personal expenses                     3,600

Sale of Building                     15,000              L.I.C. premium                         2,000

Sale of Furniture                     5,000              Interest on Bank Loan                             360

Property insurance                       400

fixed deposit in bank              30,000

Closing Balance                      14,240

———–                                                         ———–

93,400                                                             93,400

———–                                                         ———–

keeping in view the following additional information,  Compute her income from

profession for the p.y 2003 – 04:

 

  1. 1/3 Car expenses are for personal use.
  2. Written down value of the house property on 1st April, 2003 was Rs.20,000 and that of furniture was Rs.4,000. There were no other assets in these books.
  3. Rate depreciation of the new car is @ 20% and on surgical equipment’s 25%.

 

 

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Loyola College M.Com April 2006 Organizational Behaviour Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Com. DEGREE EXAMINATION – COMMERCE

TH 34

FIRST SEMESTER – APRIL 2006

                                               CO 1809 – ORGANISATIONAL BEHAVIOUR

 

 

Date & Time : 25-04-2006/1.00-4.00 P.M.   Dept. No.                                                       Max. : 100 Marks

 

 

PART – A     

Explain the following concepts in five lines each.                  (10 ´ 2 = 20 marks)

  1. Organizational Behaviour.
  2. Personality
  3. Social learning
  4. Perception
  5. Cognitive dissonance
  6. Stress
  7. Organizational Culture
  8. Re-freezing
  9. Power
  10. Collaborating

PART – B

Answer any FIVE questions.  Answer should not exceed 2 pages.   (8 ´ 5 = 40 marks)

  1. To what extent do social sciences influence the study of organizational behaviour?
  2. How will you measure the climate of an organization?
  3. Distinguish between groups and teams. Explain the characteristics of a team.
  4. Explain the various sources of power available to a leader. What are the qualities of a good leader?
  5. What are the consequences of stress? Explain the various kinds of Stress Management Strategies.
  6. How are attitudes related to job satisfaction? What are the various factors related to job satisfaction?
  7. What are the various factors correlated with perception? What strategies would you use for impression management?
  8. How will you deal with inter group conflict?

PART – C

Answer any TWO questions (Answer should not exceed 4-6 pages each)

(2 x 20 = 40 marks)

  1. Why is change necessary? What are the external and internal sources of change in an Organization?  How will you introduce and manage in your organization?
  2. What are the characteristics of organizational Behaviour. Explain any organizational behaviour model and also highlight the various variables appearing in that model.
  3. Explain any three situational theories of leadership. How do leaders use politics in an Organization.

 

 

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