B.Sc. Chemistry Question paper

Loyola College B.Sc. Chemistry April 2003 Physical Chemistry I Question Paper PDF Download

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LOYOLA  COLLEGE (AUTONOMOUS), CHENNAI-600 034.

B.Sc. DEGREE  EXAMINATION  – chemistry

third  SEMESTER  – APRIL 2003

CH  3500/ che 504 physical chemistry – I

04.04.2002

1.00 – 4.00                                                                                          Max: 100 Marks

 

 

 

PART – A                                         (10 ´ 2 = 20) )

Answer ALL questions

 

  1. What is an adiabatic process?
  2. Examine whether dP is a complete differential for a system with the equation of state P(V-b) =RT where b,R are constats.
  3. State: Trouton’s law.
  4. What is the effect of pressure on the gaseous system PCl5 PCl3+Cl2 at equilibrium?
  5. Define enthalpy of combustion.
  6. Mention the importance of the following.

(i)  plait point          (ii) tie line.

  1. Calculate the number of components and degree of freedom in an aqueous solution

of Nacl.

  1. Prove that a congruent melting point is an invariant point.
  2. Define : Henry’s law.
  3. Calculate the osmotic pressure of a 5% aqueous solution of glucose at 25°C

(mol.wt. of glucose=180 g mol-1)

 

PART  – B                                         (8 ´5 = 40)

Answer any eight only

 

  1. State and explain Hess’s law with an example.
  2. Show that PVr = constant.
  3. 10 moles of an ideal gas expand isothermally and reversibly at 27°C from 10 lit to 100 lit. Calculate q, w, DE, DH and D
  4. The standard free energy change of a chemical reaction at 100k is -104

Calculate the equilibrium constant for the reaction.

 

  1. Differentiate
  • intensive and extensive variables.

(ii) bond energy and bond dissociation  energy.

  1. How is absolute entropy of a gas determined using third law of thermodynamics?
  2. State phase rule and discuss its derivation.

 

 

 

 

 

  1. Explain the Pattinson’s process of desilverisation of lead.
  2. Obtain a relation between osmotic pressure and uapour pressure lowering of an ideal solution.
  3. State Raoult’s law and discuss it for a solution showing positive deviation.
  4. The molar heat of vaporisation of water at 100°C is 40.585 kJ.  At what temperature

will a solution containing 5.60g of glucose per 1000g of water boil?(Mol. wt. of glucose = 180 gmol–1)

 

 

 

PART  – C                            (4 ´ 10 = 40 Marks)

Answer any four only

 

  1. Deduce four Maxwell’s equation from first principles. (10)
  2. Derive (i) Kirchoff’s equation (5)

(ii) an expression for entropy of mixing of gases.                                    (5)

  • a) For the reaction of the type

aA + bb cC +dD

derive the relation connecting DG and reaction quotient and deduce an expression for equilibrium constant.                                                                              (5)

 

  1. b) Derive Gibbs-Helmboltz equation.  Mention its significance.                      (5)

 

  1. State the distribution law. Discuss its thermodynamic derivation and explain

how it is altered during the association of the solute in one of the solvents.     (10)

 

  1. Derive thermodynamically an expression connecting elevation of boiling point

of a solution and molality.

  1. a) Discuss the salient features of the phase diagram of sulphur system.           (6)

 

  1. How will you explain the variation of the mutual solubility of water and

phenol with temperature?                                                                              (4)

 

 

 

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Loyola College B.Sc. Chemistry April 2003 Organic Chemistry I Question Paper PDF Download

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LOYOLA  COLLEGE (AUTONOMOUS), CHENNAI-600 034.

B.Sc. DEGREE  EXAMINATION  – chemistry

second SEMESTER  – APRIL 2003

CH  2500/ che 502 organic chemistry – I

23.04.2002

9.00 – 12.00                                                                                        Max: 100 Marks

 

 

PART – A                      (10 ´ 2 = 20 Marks)

                                                 Answer ALL the questions.

 

  1. Which alcohol of the following pair would you expect to be more

easily dehydrated? Why?

(CH3) C(OH) CH2 CH3 (or)  (CH3)2 CH CH (OH)  CH3.

  1. State and explain Markonikov’s rule.
  2. How would you distinguish 1-butyne from 2-butyne?
  3. Identify the product in the following.

R-CH = CH2  +  CCl4             ?

  1. Anti-Markonikov’s rule is possible only for the addition of HBr in presence of

peroxides to an unsymmetrical alkene  and not for HCl or HI.  Why?

  1. ‘The presence of a small amount of O2 slows down the chlorination of methane’.
  2. In a study of Chlorination of  propane, four products of formula C3 H6 Cl2

were isolated.  What are their structures?

  1. Acidity of the following Carboxylic acids is in the following order.

Cl2 CH COOH   >  F CH2 COOH  >  Cl CH2 COOH.  Explain.

  1. Many -but not all molecules – that contain a cheral centre are chiral.
  2. How do the properties of diasteromers compare?

 

PART – B                          (8 ´ 5 = 40 Marks)

Answer any eight questions

  1. Identify the products of obtained in the dehydration of 3 -methy1-2 butanol.

Which one is major?  Justify your answer.

  1. Arrange the following compounds in order of reactivity toward dehydrohalogenation  by strong base.   Account for your answer.

1-bromobutone, 1-brome-2,2 – dimethyl propane,

1-bromo-2 methylbutane, 1-bromo-3-methylbutane.

  1. Account for the following

(i)         trans -alkene is more stable than cis -alkene.

(ii)        NBS is preferred for allylic halogenation.

  1. 98% H2 SO4 is required to hydrate ethylene while 63% H2 SO4 is enough for

isobutylene.  Explain

  1. Explain with mechanism the addition of HBr to 1,3-butadiene as 1,2-  Vs 1,4 addition.
  2. How would you prepare cis and trans alkenes from alkynes?

Explain with an example.

  1. Give the mechanism of chlorination of methane is the presence of uv light.

Explain the relative reactivities of F2, Cl2, Br2 & I2 towards methane.

 

 

 

 

 

 

  1. How do you prepare the following?

(i)         n-nonane starting with CH3 Br.

(ii)        3- methyl octane starting with sec-butyl chloride.

  1.    In the halogenation of alkanes, bromine atom is much more selective than

chlorine atom.  Explain [ relative rate factors of  1600: 82:1 for Br2 Vs 5.0: 3.8:1 for Cl2 for the reaction at tertiary: secondary: primary hydrogen]

  1.    Account for the following.

(a)        Chlorination of ethane is  400 times  faster than that of methane when         equimolar   amounts of  both are reacted with  a small amount of C12 .

(b)        chlorination of propane gives 45% of CH3 CH2 CH2 Cl and
55%  of CH3CH(Cl) CH3.

  1.    Draw and specify as  R or S, the enantiomers of

(i)  CH3 CH (OH) COOH  (ii) Sec-butyl chloride
(iii)   Bromo chloro iodomethane

  1.    What is a racemic modification?  Discuss any two methods of resolving a

recemic modification.

 

 

PART – C                           (4 ´ 10 = 40 Marks)

Answer any FOUR questions.

  1. a) Explain the stability of conjugated dienes based  on hydrogenation data.
  2. b) Explain the acidity of acetylene compared with water, ammonia and
  3. Account for the following
  4. Hydration of acetylene gives CH3
  5. Industrially acetylene is prepared from coal.
  6. Propene reacts with HOCl gives propylene chloro hydrin.
  7. 2-methyl-l-butanol on dehydration mainly gives 2-methyl 2-
  8. Sec-butyl trimethyl ammonium ion on treatment with strong base              undergoes elimination.
  9. a) Explain the mechanism of addition of halogens to alkene.
  10. b) Explain the mechanism of anti-Markonikov’s rule.
  11. Explain homogenous and heterogeneous hydrogenation of alkenes with an     Discuss the mechanism for both in detail.
  12. Draw the different conformation of ethane and n-butane, considering the

rotations about the bonds shown.  CH3-CH3 and CH3CH2-CH2CH3.  Draw the

potential energy Vs rotation curve for both and explain the strain and rotational  barrier involved.

  1. Draw the stereocherical formulas of the dichlorobutanes obtained by the

free-radical chlorination of (i) (S) -Sec-batyl chloride,  (ii) (R) -Sec-butyl chloride and  (iii)  racemic-Sec-butyl chloride.  Give  the ratios of the different 2,3-dichlorobutanes obtained in the case of  (i),(ii) & (iii) and Explain.  Also comment on the optical activity of the mixtures of 2,3-dichlorobutanes  obtained in (i)  ,(ii), & (iii).

 

               

 

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Loyola College B.Sc. Chemistry Nov 2003 Polymer Chemistry Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034

B.Sc., DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2003

CH – 5400/CHE400/CH518 – POLYMER CHEMISTRY

07.11.2003                                                                                                          Max:100 marks

1.00 – 4.00

 

PART-A

 

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

 

  1. What are chain transfer agents? Give an example.
  2. What are plasticizers? Give an example.
  3. Define CMC.
  4. Mention two disadvantages of bulk polymerization.
  5. When rubber is masticated in an atmosphere of nitrogen, the degradation does not occur, but when the process is repeated in the presence of air, the degradation is very quick and significant – Explain.
  6. Mention the polymer used for the following:
  • Articles that can be sterilized.
  • Attractive sign boards and durable lenses.
  1. What are Kevlar fibres?
  2. What is compounding?
  3. Mention the uses of FRP.
  4. How is the monomer of PAN prepared?

 

PART-B

 

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

 

  1. A polymer sample consists of 5 moles of molecular weight 30,000, five moles of molecular weight 40,000 and 10 moles of molecular weight 50,000. Calculate  and .
  2. Discuss the polymerization of acetonitrile in the presence of Li NH2.
  3. Explain gas phase polymerization with an example.
  4. Stilbene and maleic anhydride fail to undergo self polymerization but these two react to give exclusively alternating co-polymer.
  5. What are epoxy polymers? How are these prepared?
  6. Give an example of photostabilizer and mention its requirement.
  7. Write a note on Fibre Reinforcing Plastics.
  8. Define cohesive energy and account for the high cohesive energy of polyamide.
  9. What should be the criteria of conducting polymers? Give two examples of conducting polymers.

 

  1. Give an example for each:
  • Man made fibre
  • Natural fibre
  • Natural rubber
  • Synthetic rubber
  • Thermosetting plastic.

 

PART-C

 

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

 

  1. Discuss the secondary bond forces in polymers.
  2. What are stereoregular polymers? Give examples. How are these obtained?  Discuss the mechanism for the preparation stereoregular polymers.
  3. Discuss emulsion polymerization.
  4. Give an account of thermal degradation of polymers.
  5. Write notes on
  • Injection moulding
  • Callendering
  1. (i) Distinguish homopolymes and co-polymers.

(ii) Give the preparation and the uses of polystyrene and phenolformaldehyde resin.

 

 

 

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Loyola College B.Sc. Chemistry Nov 2003 Physical Chemisrty – II Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034

B.Sc., DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2003

CH – 5500/CHE508 –  PHYSICAL CHEMISRTY – II

03-11-2003                                                                                                     Max:100 marks

1.00 – 4.00

 

PART – A                                           (10X2=20 marks)

Answer ALL questions.

 

  1. Write the electrode reaction occurring in a saturated calomel electrode when it serves as cathode.
  2. NaCl cannot be used in salt bridge preparation. Why?
  3. Calculate Ecell for Cu | Cu2+ (10-2‑M) || Ag+ (10-3M)| Ag at 298 K. Eo red for Cu2+ | Cu is 0.34V, Ag+ | Ag 0.8V.
  4. Write the electrode reactions occurring in a lead storage battery when it serves as a source of current.
  5. Define molar conductance of an electrolytic solution.
  6. 30% of a zero order reaction is complete in 100 min. Calculate i) rate constant ii) half life.
  7. Mention the steps involved in a thermal chain reaction with one example.
  8. Predict the effect of ionic strength on the rate constant of the following reaction and account for your answer.

S2O82- + 2I–    2SO42- + I2

  1. Adsorption if spontaneous must be exothermic.
  2. Why is quantum yield for H2 + Cl2   2 HCl very high?

 

PART – B                                           (8X5=40 marks)

Answer any EIGHT questions.

 

  1. Explain the construction and working of Weston saturated standard cell. Write the electrode reactions involved.
  2. Eo cell for Pt | H2 HCl (aq) | HgCl­2(s) | Hg­ is 0.2699V at 293 K and 0.2669 V at 303 K. Evaluate the thermodynamic parameters DGo, DHo and DSo at 298 K.  (Assume two electron transfer)
  3. How is pH of a solution determined using quinhdrone electrode?
  4. Eo red for Ag-AgCl electrode is 0.22V and for Ag+ | Ag is 0.8 V at 298 K. Calculate the solubility product of AgCl and the solubility of it in water in g/l.  (Molecular mass of AgCl : 143.5).
  5. How is Ka of a weak acid determined experimentally using conductance measurements?
  6. For a reaction with an activation energy of 50 kJ/mol the temperature is increased from 25oC to 37o Calculate the ratio of the rate constants (R = 8.314 JK-1 mol-1).
  7. The following mechanism is proposed for the decomposition of ozone in the atmosphere.
  8. k­1

03            O2 + O

k2

  1. ii) O + O3 k3 O2 + O2    (slow step)

 

Derive an expression for the rate of decomposition of O3 using steady state

approximation with O treated as the intermediate.  Show that when the second step is

slow, the rate is second order in O3 and  first order in  O2.

  1. The pre-exponential factor for a bimolecular gaseous reaction at 300oC is 7.4 X 1010 l mol-1 s-1. Calculate DS¹.
  2. Differentiate physisorption form Chemisorption (five points).
  3. Explain a) Photosensitization b) Parallel reaction with one example for each.
  4. The quantum yield is 2 for the photolysis of HI(g) to H2 + I2 by light of wavelength 253.7 nm. Calculate the number of moles of HI that will be decomposed if 300 J of energy of this wavelength is absorbed.
  5. Explain Langumir – Hinshelwood mechanism with one example.

 

PART – C                                           (4X10=40 marks)

Answer any FOUR questions.

 

  1. a) Derive Nernst equation for a cell reaction and hence deduce an expression relating equilibrium constant and Eo         (4+2)
  2. b) Explain the significance of electromotive series. (4)
  3. Derive an expression for E cell for a concentration cell with transference and hence deduce an expression for liquid junction potential.          (7+3)
  4. a) Explain the principle of polarography. (5)
  5. b) How is transport number of an ion determined experimentally? (5)
  6. a) Account for the variation of equivalent conductance with concentration for i) strong electrolyte ii) weak electrolyte. (5)
  7. b) Derive an expression for rate constant of a second order reaction of the type 2A                                                                                                       (5)
  8. a) Explain any two methods of determining order of a reaction. (4)
  9. b) Derive Langumir adsorption isotherm equation and apply it to a moderately adsorbed system.         (5+1)
  10. a) Compare collision theory with ARRT (5)
  11. b) Explain the principle of flash photolysis. (5)
  12. Explain the kinetics of enzyme catalysed reaction involving a single substrate. How are the kinetic parameters for the enzymatic reaction evaluated?                                         (10)

 

 

 

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Loyola College B.Sc. Chemistry Nov 2003 Physical Chemisrty – I Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034

B.Sc., DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – NOVEMBER 2003

CH – 3500/CHE504 –   PHYSICAL CHEMISRTY – I

04-11-2003                                                                                                     Max:100 marks

9.00 – 12.00

 

PART – A                                           (10X2=20 marks)

Answer ALL questions.

 

  1. Define Molar heat capacity at constant volume.
  2. State the third law of thermodynamics.
  3. Heat supplied to a Cornot engine is 1897.86 kJ. How much useful work can be done by the engine which works between 0oC and 100oC?
  4. Mention the criteria of reversibility interms of S and G.
  5. For the reaction C(graphite) + 1/2 O2 (g) CO (g) at 298k and at 1 atm pressure, DH = 110.60 kJ.  Calculate D
  6. Define Ebullioscopic constant of a liquid?
  7. What are isotonic solutions? Give an example.
  8. Mention the importance of critical Solution Temperature.
  9. Express the conditions for the validity of the distribution law.
  10. Determine the number of degrees of freedom for the following equilibrium at 1 atm premure.

Water (liquid)  water (vapour).

 

 

PART – B                                           (8X5=40 marks)

Answer EIGHT questions.

 

  1. Show that for an ideal gas
  2. a) (= 0.    b)   ( = 0.
  3. Internal energy and enthalpy remain constant in the isothermal expansion of an ideal gas – Explain.
  4. For the reaction N2 (g) + 3H2 (g) 2 NH3(g).  Kp is 1.64 x 10-4 at 673 k.  Calculate DG when the partial pressure of N2, H2 and NH3 are 10 atm, 30 atm and 3 atm respectively. Is the reaction spontaneous?
  5. Discuss the effect of temperature on enthalpy change of a reaction.
  6. Obtain an expression for the equilibrium constant thermodynamically.
  7. Explain with an example the positive deviation from Raoult’s law.
  8. How will you determine the molecular weight by Beckmann’s method.
  9. Highlight the salient features of the phase diagram of water system.
  10. Derive thermodynamically the distribution law.
  11. Draw and explain the phase diagram of a system having both UCST and LCST.
  12. An immisible mixture of water and quinoline boils at 98.9oC under a pressure of 740 torr. The distillate contains 77.9 g of quinoline and 1 kg of water.  At the given boiling point the vapour pressure of quinoline is 7.96 torr. Calculate the molar mass of quinoline?
  13. Derive any two Maxwell’s relationships.

 

PART – C                                           (4X10=40 marks)

Answer FOUR questions.

 

  1. Obtain expressions for w, Du and DH for the reversible isothermal expansion of real gas.
  2. a) How is Joule-Thomson coefficient calculated? Mention the importance of inversion

temperature.                                                                                                                  (7)

  1. b) Calculate the ratio of Kp to Kc at 27oC for the following equilibrium. (R = 0.082 lit

atm K-1 mol-1)

COCl2 (g) CO(g) + Cl2(g).                                                                              (3)

  1. a) Discuss the application of Lechatelier’s principle to the formation of ammonia. (6)
  2. b) Two moles of an ideal gas undergo isothermal reversible expansion from 15 litres to 30

litres at 300 K. Calculate the work done and change in entropy.                                (4)

  1. a) Draw the vapour pressure – composition and boiling point – composition curves of

completely miscible binary solutions.                                                                          (5)

  1. b) Explain the principle of steam distillation. (5)
  2. Derive phase rule equation and explain the terms involved in it with one example.
  3. a) How will you determine osmotic pressure of a solution by Berkely – Hartley method? (5)
  4. b) A 0.5% aqueous solution of kCl was found to freeze at -0.24o Calculate the van’t

Hoff factor and the degree of dissociation of the solute at this concentration (kf = 1.86 K

kg mol-1).                                                                                                                        (5)

 

 

 

 

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Loyola College B.Sc. Chemistry Nov 2003 Inorganic Chemistry – I Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034

B.Sc., DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – NOVEMBER 2003

CH – 1500/CHE500 – INORGANIC CHEMISTRY – I

07-11-2003                                                                                                          Max:100 marks

9.00 – 12.00

 

PART-A                                 (10×2=20 marks)

Answer ALL the questions.                                                                             

 

  1. What are the factors favouring the formation of ionic compounds?
  2. Arrange the solubility of the following silver halides in the decreasing order: AgF, AgCl, AgBr, AgI and account for your answer.
  3. What are the essential conditions for LCAO?
  4. Explain why CO is diamagnetic while NO is paramagnetic?
  5. Why is density of ice lesser than that of water?
  6. What is protonic and aprotic solvents? Give one example for each.
  7. [AgI2] – is stable but [AgF2] – is not. Why?
  8. What are clathrates? Give any one example.
  9. What is oleum? How is it obtained?
  10. Give the reaction of Na2O2 as an oxidizing agent on moist Cr(OH)3.

 

PART-B                                             (8×5=40 marks)

Answer any EIGHT questions.                                                                       

 

  1. Construct Born-Haber cycle for the formation of salt MX and calculate the lattice energy of the salt MX from the data given below:

Heat of formation of MX = -550 KJmol-1

Heat of sublimation of M = +80 KJmol-1

Heat of dissociation of X2 = +155 KJmol-1

Ionization energy of M = +374 KJmol-1

Electron affinity of X = -343 Kjmol-1

  1. Calculate the electronegativity of silicon using Allred Rochow method. (covalent radius of  Si atom is 1.175 ).
  2. Explain Fajan’s rule with an example.
  3. Explain the structures of PCl5 and SF6 using hybridisation.
  4. Describe the reactions of liq. NH3 as solvent with respect to (i) acid – base reactions (ii) precipitation reactions.
  5. What are hard and soft acids and bases? Give two examples for each. How does HSAB principle explain the ambidentate nature of the ligand SCN– ?
  6. Explain the types of hydrogen bonding with suitable examples and explain two of its consequences.
  7. What are levelling and differentiating solvents? Explain with an example.
  8. Write briefly about the classification of oxides with suitable examples.
  9. Write the various oxides and oxyacids of nitrogen and give the structure of any two oxyacids of nitrogen.
  10. Give the reaction of hydrazine with (i) O2 (ii) HNO2  and indicate the significance of this reaction.

 

PART-C                                            (4×10=40 marks)

Answer any FOUR questions.                                                            

 

  1. Define lattice energy. How is lattice energy calculated theoretically?  What are the factors that affect lattice energy?
  2. Explain the postulates of VSEPR theory with special reference to (i) ClF3   (ii) NH3.
  3. Construct molecular orbital diagram for O2 molecule and hence discuss the relative stabilities of O2, O, O and O2 2+.
  4. Explain band theory as applicable to metals.
  5. Explain i) Similarities among nitrogen group elements
  6. ii) Differences between nitrogen and other members of the family
  7. a) Explain any two methods of estimating H2O2.
  8. b) How is the structure of H2O2 established?

 

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Loyola College B.Sc. Chemistry Nov 2003 Bio-Chemistry Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034

B.Sc., DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2003

CH – 5401/520/CHE 401 – BIO-CHEMISTRY

10-11-2003                                                                                                     Max:100 marks

1.00 – 4.00

PART – A

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

  1. Define isoelectric point.
  2. How is aninoacid tested using Ninhydrin? Indicate the reaction.
  3. What are the two tertiary structures possible for a polypeptide? Give one example for each.
  4. What is transamination reaction? Mention one example.
  5. What is ATP? Give its structure.
  6. What is ‘allosteric’ enzymes? How does it affect the rate of a reaction?
  7. Suggest a chemical test for cholesterol.
  8. What is the reaction of glucose with an amine?
  9. Indicate the hydrogen bonding between A – T, G-C.
  10. Mention any two differences between DNA and RNA?

 

PART – B

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

  1. Suggest a synthetic route for ala-gly-ph ala.
  2. Explain one method for C-terminal analysis of a polypeptide?
  3. Explain all the steps involved in the ‘b-oxidation of fattyacid’.
  4. How is the ring size of glucose determined?
  5. Write briefly about competitive inhibition of enzymes.
  6. How are enzymes classified? How is the enzyme action affected by pH?
  7. Explain the mechanism of oxidative phosphorylation and explain the steps involved in this process.
  8. Bring out the salient features of secondary structure of DNA.
  9. Define genetic code. How is genetic information decoded for protein synthesis?
  10. Write all the steps involved in the bio-synthesis of fattyacids.
  11. Explain how blood is coagulated?

 

PART – C

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

  1. a) Define anabolism and catabolism. How are amino acids catabolyzed?
  2. b) Discuss the advantage of preparing polypeptides by solid phase synthesis.
  3. Explain how Michalis-Menton model helps in understanding the characteristics of enzyme catalysis. Derive the expression for the rate of enzyme catalysis.
  4. Out line the steps in the bio-synthesis of cholesterol.
  5. Describe the secondary structure of proteins.
  6. Describe the steps involved in a) tricarboxylic acid cycle b) Glycolysis and energetics of glycolysis.
  7. Explain the mechanism of transport of oxygen by blood.

 

 

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Loyola College B.Sc. Chemistry Nov 2003 Allied Chemistry Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI-600 034.

B.Sc. DEGREE EXAMINATION – MATHEMATICS/PHYSICS

THIRD SEMESTER – NOVEMBER 2003

CH 3100 / CHE 100  – ALLIED CHEMISTRY

 

08.11.2003

09.00 to 12.00                                                                                             Max. 100 Marks.

PART – A

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

 

  1. Draw the resonance structures of phenol.
  2. State Raoult’s law.
  3. Define ‘degrees of freedom’.
  4. Write the structure of PVC.
  5. N,N-Dimethyl-o-toluidine is a stronger base than N,N-Dimethyltoluene. Why?
  6. What are the advantages of variable oxidation states of transition metals?
  7. Name the following coordination compounds.
  8. a) [Ni(CO)4]         b) [Cr(NH3)4Cl2]Cl
  9. Draw the structure of the following compounds.
  10. a) adenine         b) ribose sugar
  11. Define the order of a chemical reaction.
  12. State Grotthus-Draper Law.

 

PART – B

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

 

  1. Draw the optical isomers of tartaric acid and explain.
  2. Draw the conformational isomers of n-butane and explain.
  3. What is an SN2 reaction? Explain its mechanism.
  4. Explain positive deviation from Raoult’s Law with an example.
  5. Draw the phase diagram of water. Apply the phase rule to any one point, line and

area.

  1. Write a note on vulcanization of rubber.
  2. Using valence bond theory, bring out the structures of
  3. a) [ Cu(NH3)4]Cl2   b) [Cr(H2O)6]Cl3
  4. What is EAN rule? Apply it to a) K3[Fe(CN)6] and b) [Ni(CO)4]
  5. Explain Watson-Creek model of DNA.
  6. Write short notes on the following hormones?
  7. a) Prostaglandins b) Thyroxine
  8. Write the relation connecting rate constant and concentration for a) I order and
    b) II  order reactions.
  9. How is copper estimated by photoelectric colorimetry?

PART – C

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

 

  1. a) Explain the phase diagram of phenol-water system.
  2. b) Write the mechanism of nitration of benzene.
  3. a) How is terylene manufactured? Write the equation.
  4. b) How will you determine pH by using a glass electrode?
  5. What is corrosion? Write the electrochemical mechanism of it. How will you

prevent corrosion by galvanization and cathodic protection?

  1. a) Give a short note on the magnetic properties of transition elements?
  2. b) Discuss on the geometrical and optical isomerisms in the coordination compounds  with an example for each.
  3. a) “DNA forms RNA; RNA makes proteins- Explain?
  4. b)  Write a short notes on “adrenaline”.
  5. a) “What is replication of DNA”. Explain the mechanism.
  6. b)  Explain heterogeneous catalysis with two examples.

 

 

 

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Loyola College B.Sc. Chemistry April 2006 Synthetics Org.Chem. & Org. Spectroscopy Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 18

SIXTH SEMESTER – APRIL 2006

                           CH 6603 – SYNTHETICS ORG.CHEM. & ORG. SPECTROSCOPY

(Also equivalent to CHE 603)

 

 

Date & Time : 26-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

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

  1. What are protecting groups? Give an example of a protecting group for amines and alcohols.
  2. What is raney nickel and Adam’s catalyst?
  3. Distinguish between linear and convergent method of synthesis.
  4. Predict the product and reason for the formation of the product.
  5. Add the necessary reagents for the forward and reverse reactions.
  6. Identify the base peak when acetone undergoes fragmentation during mass spectral study.
  7. Define hyperchromic shift. How does it arise in the electronic spectrum of an organic compound?
  8. Name the methods by which non-first order NMR spectrum is resolved into a first order spectrum.
  9. Calculate the frequency regions for N=O stretching vibrations.
  10. Define the following a) auxochromes         b)  shielding effect

 

PART – B

                                                Answer any eight questions            (8 × 5 = 40 marks)

  1. How are the following conversions effected?
  2. Predict which of the following products would be got in Baeyer-Villiger oxidation of cyclohexylmethyl ketone.Why?

 

  1. Give the reterosynthesis and the synthesis of 2-aminocyclohexanone using umpolung concepts.
  2. Give the reterosynthesis and the synthesis of the following.
  3. Explain a) Aldol condensation b) Michael addition reaction
  4. What are the diene and the dienophile used in the synthesis of the following compounds?
  5. What is solvent cut-off region? How do solvents affect the lmax of any compound? Explain with suitable examples.
  6. Write the various fragmentation pattern for an arbitrary compound A–B-C–D.
  7. What are the advantages of FT-IR over dispersive IR spectrophotometer? Give suitable evidences to mark the differences.
  8. Assign the IR spectral regions and calculate lmax of the following compound

 

  1. What are the factors that affect the coupling constants of NMR signals? Explain any three in detail.
  2. Explain the following with respect to 13C-NMR spectroscopy
  3. a) Deuterium coupling b) nuclear overhauser effect


PART – C

Answer any four questions            (4 × 10 = 40 marks)

  1. Predict the product with mechanism
  2. Give the reterosynthesis and the synthesis of the following
  3. a) Predict the product with mechanism for the reaction of EAA with traces of
    sodium hydrogen carbonate.
    b) How are the following conversions effected?
  4. a) Predict the number of NMR signals with increasing order of d values for each of the following compounds.
  5. i) phenylacetic acid
  6. ii) o-hydroxyacetophenone
  7. b) Of the given pairs of isomers which will show the longest wavelength of UV absorption. Give reasons.
  8. i) 1,2-pentadiene and 1,3-pentadiene
  9. ii) 4-hept-1-enone and 4-hept-2-enone
  10. For the given compound predict the following
  11. a) IR vibrational frequencies for various groups present
  12. b) Mass spectral fragmentation pattern
  13. c) Proton NMR spectral data with splitting and chemical shift values.

CH3-CH(CH3)-CH2-COOH

  1. Elucidate the structure of the given organic compound from the following spectral data (Annexure-I). The molecular formula of the compound is C6H10O2

 

 

 

 

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Loyola College B.Sc. Chemistry April 2006 Organic Chemistry – II Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 9

FOURTH SEMESTER – APRIL 2006

                                                     CH 4500 – ORGANIC CHEMISTRY – II

(Also equivalent to CHE 507)

 

 

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

 

 

Part A

Answer all the questions.                                                                          10´2=20

  1. Give an evidence for the resonance structure of benzene.
  2. What is aldol condensation?
  3. Cyclopropane readily undergoes ring-opening reactions. Explain
  4. Why is tropylium cation aromatic?
  5. What will be the major product formed on dehydrohalogenation of 2-bromo-2,3-dimethylbutane.
  6. Name the following alcohols by carbinol and IUPAC system:
    • CH3-CHOH-CH=CH2
    • CH3-CH2-C(CH3)(OH)-CH2-CH2-CH3
  1. C-O-C bond angle in diethyl ether is greater than H-O-H bond angle in water. Explain.
  2. Arrange the following in the order of increasing acidity.

p-toluic acid, phenyl acetic acid, m-nitrobenzoic acid, benzoic acid.

  1. Accont for the lower boiling point and decreasing water solubility of o-nitrophenol as compared with their m- and p- isomers.
  2. What is coupling reaction? Give an example.

Part B

Answer any eight questions.                                                                      8´5=40

  1. Aromatic electrophilic substitution in phenol takes place at ortho and para positions. Explain.
  2. Design a synthesis that would convert phenol primarily to a) o-bromophenol
    b)p-bromophenol.
  3. Give the major products of the following reactions with reason.
  1. bromination of p-fluorotoluene
  2. nitration of p-nitrotoluene
  3. Explain the stability of cyclohexane on the basis of Sache Mohr theory and the potential energy diagram.
  4. Give reasons for the following:
    1. p-chloronitrobenzene has less dipole moment than p-nitrotoluene.
    2. Nitrobenzene and not benzene is used as a solvent for Friedel-Craft’s    alkylation of bromobenzene.
    3. c) Halogens are o-p directors but are deactivating.
    4. Explain the mechanism of Cannizaro reaction.
    5. Explain the mechanism of hydroboration-oxidation of alkenes.
    6. Write the mechanism of nitration of methyl phenyl ether.
    7. Convert the following:
  5. Phenol into salicylic acid
  6. Salicylic acid into a-chloro benzoyl chloride.
  7. Explain Gabriel phthalimide synthesis.  How would you use this method in the preparation of glycine and n-propyl amine?
  8. What is diazodisation? How is benzene diazonium chloride prepared? Give its

mechanism.

  1. Discuss the mechanism of pinacol-pinacolone rearrangement.

Part C

Answer any four questions.                                                                     4´10=40

  1. a) Explain the mechanism of formation of 2,4-dinitrophenylhydrazone derivative from acetone.
  2. b) Compound A with the molecular formula C5H8O2 on reduction forms n-pentane and forms dioxime with hydroxylamine. It gives positive test with Tollen’s reagent and also forms iodoform. Suggest a suitable structure of the compound.
  3. a) Two isomeric hydrocarbons A and B have molecular formula C8H10. A on oxidation gives benzoic acid while a dicarboxylic acid is formed by the oxidation of B which later on heating forms anhydride. Suggest the structures of A and B.
  4. b) CH3-CH (X) – CH2– CH2– CH3 on dehydrohalogenation forms 2-pentene and 1-

pentene. The major and minor product varies with respect to the substituents.

Explain the reactions with reason.

Substituents 2-pentene 1-pentene
Br 80% 20%
Cl 75% 25%
F 65% 35%
S+R2 30% 70%
N+R3 30% 70%

 

  1. a) When nitrobenzene is nitrated m-dinitrobenzene is formed as the major product whereas anisole on nitration forms a mixture of o- and p-nitro compounds. Explain.
  2. How are the following conversions done?
    1. phenol to cyclohexane
    2. cyclopropane to butanoic acid.       (6+2+2)
    3. i) Explain the mechanism of Reimer-Tiemann’s reaction. (4+6)

ii)Identify the products ( A, B, C and D) in the following sequence of reactions.

Isopropyl alcohol   A

B   C  D

  1. a)Write any two methods of preparation of each primary, secondary and tertiary

amines.                                                                                                               (6)

b)Phenol is less acidic than trinitrophenol and carboxylic acids.  Explain.       (4)

  1. a) Explain the mechanism of Hofmann rearrangement. (6)
  2. b) How will you convert phenol into salicylaldehyde? Give the mechanism.   (4)

 

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Loyola College B.Sc. Chemistry April 2006 Organic Chemistry – I Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 4

SECOND SEMESTER – APRIL 2006

                                                     CH 2500 – ORGANIC CHEMISTRY – I

(Also equivalent to CHE 502)

 

 

Date & Time : 24-04-2006/1.00-4.00 P.M.   Dept. No.                                                       Max. : 100 Marks

PART – A

                                                Answer all questions                         (10 ×2 = 20 marks)

  1. Draw the sawhorse and Newman projection structures of propane.
  2. Arrange the following in the increasing order of stability.
    1, 3-butadiene, 1, 2-butadiene, 1, 4-butadiene.
  3. Draw the structure of
    (a) (Z)-3-isopropyl-2-heptene (b) (E)-1-bromo-2-chloropropene.
  4. Define the following (a) racemic mixture (b) resolution.
  5. Arrange the following in the increasing order of reactivity towards Diel’s-Alder reaction.
  6. What are the factors that affect the free radical halogenation of alkanes?
  7. What is Baeyer’s test?
  8. What happens when calcium carbide is treated with water?
  9. What is Wurtz reaction?
  10. Draw the structure of the following compounds
  11. a) 2,6-dimethyl-4-ethyl-2,4-heptadiene
  12. b) 3,5-diethyl-1,7-octadiyne.

PART – B

                                                Answer any eight questions             (8 × 5 = 40 marks)

  1. What are conformers? How are they different from configuraitonal isomers? Give an example.
  2. Predict the product with mechanism for the reaction of 2, 4-hexadiene with HCl.
  3. The specific rotation of R-(+)-glyceraldehyde is + 8.7°. If the observed rotation of a mixture of R-glyceraldehyde and s-glyceraldehyde is +1.4°, what percent of glyceraldehydes is present as the R enantiomer?
  4. Draw the various stereoisomers of 3-chloro-2-butne and indicate which of them are entantiomers and diastereomers.
  5. Predict the product with mechanism
  6. Define the following
    a) asymmetric synthesis b) chemoselectivity c) regioselectivity.
  7. Compare the free radical chlorination and bromination of methane for reactivity and quantum yield.
  8. Why the alternative mechanism of chlorination of methane is not possible? Explain with proof.
  9. What is Kolbe’s synthesis? How is butane synthesized by above method?
  10. How is ozonolysis used to differentiate 1-butene and isobutene. Write the mechanism of the above reaction.
  11. What are the products formed when 1-butyne is subjected to hydroboration and oxidation. Explain the mechanism of the reaction.
  12. Give the mechanism of addition of bromine to ethylene.

PART – C

                                                Answer any four questions   (4 × 10 = 40 marks)

  1. Indicate whether the following pairs of compounds are identical or enantiomers or constitutional isomers.
  2. Perform a conformational analysis of rotation of C2-C3 bonds in n-butane and explain using a potential energy diagram.
  3. a) Dienes undergo free radical reactions faster than alkenes. Why?
    b) What are atropisomers? Give suitable example.
    c) Which of the following conjugated dienes would not react with a dienophile in
    Diel’s-Alder reaction? Why?
  4. Explain in detail the chlorination reaction of methane. How many products are formed? Discuss the rate of the reaction and the reaction mechanism of the reaction.
  5. a) A hydrocarbon reacts with conc. H2SO4 to form an alkyl hydrogen sulphates which on hydrolysis yields tert-butyl alcohol. What is the structural formula of the hydrocarbon? Write the equations.
  6. b) Write the structure of the alkene, which on ozonolysis gives 2-butananone and 2-mehtylpropanaldehyde. Write the mechanism of the reactions.
  7. a) compound A, C4H6 gave the following tests
  8. i) A + Br2 / CCl4 ® B (C4H6Br4)
  9. ii) A + H2 / Pt® C (C4H10)

Identify A, B and C

  1. b) What are the uses of the following compounds?
  2. i) ethylene ii) acetylene iii) propene

 

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Loyola College B.Sc. Chemistry April 2006 Natural Products Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 19

SIXTH SEMESTER – APRIL 2006

                                                        CH 6604 – NATURAL PRODUCTS

(Also equivalent to CHE 604)

 

 

Date & Time : 24-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

PART – A

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

  1. Explain isoprene rule with respect to geraniol.
  2. Draw the structure of piperonylic acid and caffeine.
  3. Predict the product for the reaction between anthracene and maleic anhydride.
  4. How is the presence of unsaturation tested in alkaloids?
  5. How is urea converted into parabanic acid?
  6. Give the resonance structure of naphthalene.
  7. Apply Huckel’s rule to predict the aromatic character of thiophene and explain.
  8. How is 2-aminopyridine obtained from pyridine?
  9. What is nicotinic acid? How is it obtained?
  10. What are alkaloids? Give an example for pyridine alkaloid.

PART – B

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

  1. Explain Hoffmann’s exhaustive methylation of coniine.
  2. Naphthalene on sulphonation at 50 ⁰C and at 150 ⁰C yields different products. Explain.
  3. What are carcinogens? Explain the carcinogenic activity of polynuclear hydrocarbons.
  4. How is anthracene obtained by Haworth’s synthesis?
  5. Resonance energy of benzene is 36 kcal mol-1 while that of naphthalene is 61 kcal mol-1. Explain.
  6. Electrophilic substitution of pyridine yields 3- substituted product. Explain.
  7. Explain the synthesis of uric acid.
  8. Write note on anthocyanins.
  9. How are the following obtained from pyrrole:
  10. Pyrrole-2-carboxylic acid. b. 2-Formylpyrrole.
  11. How is the presence of two benzene rings established in naphthalene?
  12. Account for the products of oxidation of quinoline with acidified potassium permanganate.
  13. How are terpenes isolated?

 

PART – B

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

  1. Establish the structure of uric acid.
  2. Elucidate the structure of nicotine.
  3. Describe the constitution of citral.
  4. a. Discuss the structure of piperic acid.
  5. Write a note on flavones.
  6. Explain the following:
  7. Skraup’s synthesis b. Conversion of thiophene to thiophene-2-carboxylic acid.

 

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Loyola College B.Sc. Chemistry April 2006 Molecular Dynamics Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 15

SIXTH SEMESTER – APRIL 2006

                                                     CH 6600 – MOLECULAR DYNAMICS

(Also equivalent to CHE 600)

 

 

Date & Time : 19-04-2006/FORENOON     Dept. No.                                                       Max. : 100 Marks

 

 

                                                            PART – A                            

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

 

  1. State the de Broglie relation. Explain the condition under which it is applicable.
  2. Normalise eax in the interaval (0,1).
  3. What are the possible values for angular momentum according to Bohr’s postulate?
  4. Give the expressions for wave function and energy for the third p-energy level of 1,3-
  5. Evaluate ln N! when N = 1030 using Stirling’s formula.
  6. Calculate the number of ways of distributing four particles among five energy levels if the particles are electrons.
  7. Write Boltzmann equation connecting entropy and thermodynamic probability.
  8. What is intersystem crossing?
  9. Define quantum yield of a photochemical reaction.
  10. Mention any four relaxation methods used in the kinetic study of fast reactions.

 

PART – B                 

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

 

  1. Determine the kinetic energy of the electrons emitted by a light of 100 nm if the threshold frequency of the metal is 9.0 ´ 1014
  2. Calculate the ionization energy per mole of H atom.
  3. Derive the expression for Hamiltonian operator in cartesian coordinates.
  4. Examine whether “A sin ax” is Eigen function for the second order differential operator. If so, state the Eigen value.
  5. Calculate the wave length of transition for a conjugate olefin containing 3 double bonds.
  6. Explain how partition functions can be separated.
  7. Calculate the ratio of translational partition function of D2(g) to H2(g)  at the same temperature and volume.
  8. Write Sackur-Tetrode equation and mention the terms involved.
  9. Derive the relation connecting internal energy(E) and molecular partition function(Q).
  10. Explain the principle of flash photolysis.
  11. Explain the factors affecting phosphorescence emission.
  12. Explain photosensitisation with two examples.

 

PART – C

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

 

  1. Obtain an expression for the radius of “H” atom on the basis of the Bohr’s model of atom.
  2. Obtain the expressions for the energy and wave function of a free particle in a one dimensional box.
  3. State the postulates of Maxwell-Boltzmann distribution law and hence derive an expression for most probable distribution.
  4. Explain any two of the following
    (a) Fluorescence and structure
  • Kinetics of H2-Br2 (photochemical) reaction.
  • Chemical actinometer.
  1. Draw Jablonski diagram and explain in detail.
  2. Derive the following

(a)  E = RT2

(b)  Etranslation =

 

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Loyola College B.Sc. Chemistry April 2006 Microbial Biotechnology Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY, ZOOLOGY

IB 7

FOURTH SEMESTER – APRIL 2006

                                                PB 4202 – MICROBIAL BIOTECHNOLOGY

 

 

Date & Time : 22-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

Part A

Answer all the questions                                                                         (20 marks)

  1. Choose the correct answer (5 x 1 = 5 )
  1. ________ are enzymes which acts on proteins.
  1. a) amylases b) pectinases             c) proteases     d) lipases
  1. The viral surface antigen of the hepatitis B virus is .
  1. a) HbsAg b) HbcAg c)  HbeAg       d)  HbdAg
  1. Malt extract contains ………… % of nitrogen.
  1. a) 5 b) 5.5               c) 8.5               d)  80
  1. The production of malt beverages is known as …….
  1. a) Malting       b) Mashing            c) Brewing      d) Ripening
  1. Which of the following one is an exopolysaccharide?
  1. a) Xanthan            b) Inulin          c) Renin           d) Pectin

 

  1. State whether the following statements are True or False (5 x 1  = 5 )
  1. An endocellular enzyme is not secreted in the fermentation medium.
  2. Immunizing agents that stimulate immunity to toxins are called toxoids.
  3. Microorganisms can be preserved by Lyophilization.
  4. Spirulina contains carotene pigments.
  5. Biosensor is used for the quantitative estimation of important substances in body fluid

III. Complete the following                                                                              (5 x 1 = 5)

  1. ______ is the first discovered antibiotic.
  2. _______ are used in removal of starch sizing from woven cloth.
  3. The technology used for the cultivation of eukaryotic cells in large scale is called as __________
  4. The moisture content of soft cheese is  ________
  5. VAM  refers to ________    __________   _________.
  1. Answer the following in one or two sentences. (5 x 1 = 5)
  1. What is a constitutive enzyme ?.
  2. What is acquired immunity ?.
  3. What is Beerwort?
  4. Define transgenic microbe
  5. What is single cell protein?

Part B

Answer any five of the following each in about 350 words. Draw necessary diagrams.                                                                                         (5 x 8 = 40)

  1. Explain the microbial production of pectinase.
  2. List out any 5 applications of microbial enzymes.
  3. Explain the transformation of steroids.
  4. Mention the different sources of Nitrogen and Carbon energy in fermentation industry.
  5. Describe the methodology of wine production. Add a note on types of wine.
  6. Define Bioplastics. Write notes on  Xanthan production and its applications.
  7. With the flow chart, explain the steps involved in cheese production.
  8. What is biosensor? Explain its working principle and its application.

Part C

Answer the following  questions each within 1500 words. Draw necessary diagrams

(2 x 20 = 40)

  1. a) i) Describe the different stages of fermentation process (10 marks)
  2. ii) Describe in detail the cultivation of mushroom. Add a note on their nutritional  composition (10 marks).

OR

  1. b) i) Define Biofertilizer. Explain the method of mass cultivation of Azolla and Rhizobium. Add a note on their significance (12 marks).
  2. ii) Define biopesticide. Why Bacillus thuringiensis is called as biopesticide?    (8 marks)
  3. a) What are antibiotics ?. What are its properties ?. Give an account on the industrial production of penicillin.

OR

  1. b) Give an account on the applications of aminoacids and explain the industrial production of L glutamic acid.

 

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Loyola College B.Sc. Chemistry April 2006 Inorganic Chemistry – II Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 10

FOURTH SEMESTER – APRIL 2006

                                                   CH 4501 – INORGANIC CHEMISTRY – II

(Also equivalent to CHE 506)

 

 

Date & Time : 27-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

Part – A

Answer all the questions                    (10 ´ 2 = 20)

 

  1. Name any two alloys of copper and give the composition.
  2. How does KMnO4 on acidic medium act as an oxidizing agent? Give the chemical equation.
  3. ‘Zinc does not show variable oxidation state’. Explain.
  4. What is EAN rule? Calculate EAN for K3[Fe(CN)6].
  5. What is the source of the presence of crystal defects in regular solids?
  6. Give the structure of EDTA and indicate the coordination sites.
  7. What are fertile and fissile isotopes? Give examples.
  8. Half life of Po210 is 140 days. Calculate the number of days after which 1/4g of Po210 will be left undisintegrated from 1g of the isotope?
  9. What are isotopes and isotones? Give an example for each.
  10. Account for the fact that the conductivity of the metal decreases if the temperature is increased.

Part – B

Answer any eight questions                 (8 ´ 5 = 40)

 

  1. Explain the zone refining and cyanide processes of refining of metals.
  2. What is lanthanide contraction? How are individual lanthanides separated by ion-exchange chromatography techniques.
  3. Predict the geometry of [Co(CN)6]3-(diamagnetic) and [CoF6]3-(paramagnetic) using VB theory.
  4. What are electron capture process and spallation reaction? Give an example for each.
  5. Explain the various steps involved in the extraction of Uranium (Give chemical reactions wherever necessary).
  6. Calculate the CFSE for octahedral, high and low spin d4 and d7
  7. a) Differentiate hydrogen bomb and atom bomb
    b) Complete the nuclear reaction:

                                                       12Mg24 (2He4, 0n1 )    ;      17Cl35( 0n1, 1H1)

  1. Derive the relationship between half-life period,t1/2 and decay constant, K of a radioactive element.
  2. Explain Geiger-Nuttal rule with suitable example.
  3. (a) Calculate the density of nucleus of 81Br isotope.
    (b) In a period of time 236U was found to have permitted 7 alpha particles and four beta particles. Find the final product.
  4. Explain the conducting behaviour of metals using band theory.
  5. Define unit cell. Discuss the structure of Nacl unit cell.

 

Part – C

Answer any four questions                 (4 ´ 10 = 40)

 

  1. Explain the significances of Ellingham diagram in the conversion of metallic oxide to metal in the metallurgical process?
  2. Discuss (a) hydrate (b) linkage   (c) ionization and (d) geometrical isomerism exhibited by coordination compounds with suitable examples.
  3. Discuss the splitting of d-orbitals of metals in square planar environment of ligands.
  4. Discuss the factors affecting the stability of a nucleus.
  5. Explain the working principles of a nuclear reactor and breeder reactor. Describe the working of a nuclear reactor to generate electricity.
  6. (a) What is the principle of X-ray diffraction techniques? (b) Explain the single crystal diffraction technique.

 

.

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Loyola College B.Sc. Chemistry April 2006 Industrial Chemistry Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 20

SIXTH SEMESTER – APRIL 2006

                                                     CH 6605 – INDUSTRIAL CHEMISTRY

(Also equivalent to CHE 605)

 

 

Date & Time : 26-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

Part A

Answer the following                                                                             10×2 = 20

  1. What are renewable and nonrenewable energy resources?
  2. How is producer gas manufactured?
  3. How are chemical fuels classified?
  4. What are herbicides? Cite two examples.
  5. Give approximate chemical composition of any one mixed fertilizer.
  6. What are the ions responsible for making water hard?
  7. How are suspended impurities in water removed?
  8. What is acid rain? What are its consequences?
  9. Explain origin of poisoning of ground water by cyanide ions.
  10. Give any two differences between paints and dyes.

 

Part B

Answer any eight of the following:                                                       8×5 = 40

 

  1. Define calorific value of a fuel. State advantages and disadvantages (two each) of gaseous fuels over solid fuels.
  2. What is coal? Explain its preparation, properties and uses.
  3. Write short notes on primary and secondary fuels.
  4. Explain the role of micronutrients in agriculture.
  5. What is triple superphosphate? How is it prepared?
  6. Give the preparation and two uses of lime – sulphur.
  7. Explain differences between temporary hardness and permanent hardness of water
  8. Describe reverse osmosis, with special reference to desalination of sea water.
  9. Explain (ii) green house effect and (ii) ozone layer depletion
  10. What are the ways of reducing carbonmonoxide pollution in atmospheric air?
  11. What are plastics? What are their advantages? How do they affect environment?
  12. Write notes on food industry.

Part C

 

Answer any four of the following:                                                        4×10 = 40

 

  1. Explain the significance of the following constituents of coal (i) moisture (ii) volatile matter (iii) carbon (iv) ash.
  2. Explain of petroleum. Discuss advantages of catalytic cracking over thermal cracking.
  3. Write notes on (i) phosphatic fertilizers (ii) annealing of glass
  4. Discuss the use of complexometric titrations in estimating hardness of water.
  5. How is river water converted into potable water?
  6. Discuss methods to treat industrial waste water and gases.

 

 

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Loyola College B.Sc. Chemistry April 2006 General Chemistry For Physics & Maths Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS & MATHEMATICS

LM 03

SECOND SEMESTER – APRIL 2006

                               CH 2100 – GENERAL CHEMISTRY FOR PHYSICS & MATHS

(Also equivalent to CH 3100)

 

 

Date & Time : 26-04-2006/1.00-4.00 P.M.   Dept. No.                                                       Max. : 100 Marks

 

 

                                 PART-A                                                             (10×2=20)

   Answer all questions.

 

  1. Write any four characteristics of d-block elements.
  2. Write the IUPAC name of the following.

a)[ CoCl(NH3)5] Cl2          b)[ Pt(NH3)6] Cl4

  1. What is Friedel-Craft’s alkylation?
  2. Differentiate enantiomers and diastereomers.
  3. State Henry’s law.
  4. What is degree of freedom?
  5. Define quantum yield.
  6. Draw the structure of the following.
  7. Adenine b) Cytosine
  8. What is vulcanisation of rubber?
  9. How is Buna-s rubber prepared?

 

                                                    PART – B

Answer any eight questions.                                                              (8 x 5 = 40)

 

  1. a) Transition metal compounds are generally coloured. Why?
  2. b) Differentiate primary valency and secondary valency of coordination compounds.

12     Draw the structure of hemoglobin and explain its functions.

  1. Which of the following exhibit geometrical isomerism? Explain
  2. 2-butene b) 1,2-dichloro propane c) 2,3-butenedioic acid.
  3. Compare the stereochemistry of SN1 and SN2 reaction.
  4. Explain the optical isomerism of lactic acid.
  5. Draw the phase diagram of phenol-water system and explain.
  6. Derive the rate expression of first order reaction.
  7. State a) Grotthus-Draper law b) Stark-Einstein’s law.
  8. Write a note on replication of DNA.
  9. Draw the structure and give any two functions of the following.
  10. a) Oxytocin   b) Adrenaline

 

 

  1. Define the following.
  2. a) polymer      b) degree of polymerization     c) Elastomers
  3. What are the causes of corrosion?

 

PART-C

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

  1. a) What is EAN principle? Apply it to the following compounds and explain their

stability.

  1. i) [Co(NH3)6]3+                       ii) K3[Fe(CN)6  ]                                   (6)
  2. b) Predict the geometry, hybridization and magnetic properties of [Co(CN)6]3-                                                                                                                  (4)

24        a)  Give the mechanism of halogenation of benzene.                                     (4)

  1. Define the following term:
  2. i) racemic mixture ii) resolution iii) optical isomerism                               (6)
  3. a) What are the conditions of ideal solutions.                         (4)
  4. b) Draw the phase diagram of simple eutectic system. Explain.                    (6)
  5. Derive the rate expression for the reaction 2A¾® products. Find the value of half life period.                                                             (6+4)
  6. Discuss the double stranded helical structure of DNA. (10)
  7. a) Write a note on “galvanisation”. (4)
  8. b) Explain the mechanism of step growth and chain growth polymerization with any one example.                                                                         (6)

 

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Loyola College B.Sc. Chemistry April 2006 Coordination Chemistry Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 16

SIXTH SEMESTER – APRIL 2006

                                                 CH 6601 – COORDINATION CHEMISTRY

(Also equivalent to CHE 601)

 

 

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

 

 

PART – A

Answer All the questions                                                                                10×2=20

  1. Draw the structure of salicyldoxime? How is it prepared?
  2. Calculate the CFSE value for [Cr(NH3)6]3+ complex.
  3. How is ferrocene prepared? Draw is structure.
  4. Show that Ni(CO)4 obeys EAN rule.
  5. Draw the structures of (a) Co2(CO)8 (b) Mn2(CO)10
  6. What are metal-arene complexes? Give one example.
  7. What is cisplatin? Mention its use.
  8. Give the IUPAC name of (a) K[PtCl3(C2H4)] (b) Fe2(CO)9
  9. How is ‘salen’ ligand prepared?
  10. Mention any two uses of crown ethers.

 

PART – B

Answer any Eight only                                                                                   8×5=40

  1. Apply ligand field theory to [Fe(CN)6]4- and [Fe(H2O)6]3+
  2. How are cis and trans – [Pt(NH3)2Cl2] prepared?
  3. Give the evidence for the bridge mechanism in inner sphere electron transfer      mechanism.
  4. Describe the splitting of d orbitals in the tetrahedral ligand field.
  5. Give any two reactions indicating the metal template synthesis.
  6. Explain the Wackers process of converting ethylene to ethanal.
  7. Discuss the photosubstitution reactions in metal carbonyls.
  8. How is ‘Do’ influenced by the nature of the central metal atom?
  9. Draw the structures of (a) Ni(DMG)2 (b) [Zn(EDTA)]-1
  10. Write a note on biological significance of alkali and alkaline earth metals.
  11. Write a note on iron-molybdenum centre in nitrogenase enzyme

 

 

 

 

PART – C

Answer any Four only                                                                                   4×10=40

  1. State Jahn-Teller theorem. Explain the d-orbital splitting due to elongation and compression along the z-axis in the octahedral complexes. Give one evidence for such a distorted structure.
  2. Discuss the association and dissociation mechanism of the substitution reactions in octahedral complexes.
  3. Discuss the bonding in metal carbonyls. Give any two evidences supporting the bonding scheme.
  4. Describe the hydrogenation of alkene using Wilkinson catalyst. State the merits of this method.
  5. Discuss the structure and function of carboxypeptidase-A.
  6. Write a note on (a) Crown Ethers (b) Color in transition metal compounds

 

 

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Loyola College B.Sc. Chemistry April 2006 Chemistry Of Materials Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 17

SIXTH SEMESTER – APRIL 2006

                                                  CH 6602 – CHEMISTRY OF MATERIALS

(Also equivalent to CHE 602)

 

 

Date & Time : 24-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

Part A

Answer all the questions.                                                                          10×2=20

  1. What are Bravais lattices?
  2. Differentiate type I and type II semiconductors.
  3. What are intrinsic semiconductors? Give an example.
  4. What is Curie-Weiss law?
  5. What is Meissner effect?
  6. Give two examples each of n-type or p-type metal oxide semiconductor.
  7. Define piezoelectric ceramics.
  8. How is radius ratio rule useful in determining the crystal structure?
  9. Define magnetic susceptibility.
  10. What is CVD technique?

Part B

Answer any eight questions.                                                                      8×5=40

  1. What are liquid crystals? Explain the different types of liquid crystals.
  2. How is the structure of compounds determined by powder method?
  3. Explain the crystal structure of perovksite with a neat diagram.
  4. Mention any five differences between hard and soft magnetic materials.
  5. What are ferromagnetic and antiferromagnetic materials? Give examples.
  6. How is solar energy harnessed using photovoltaic cells?
  7. Describe the technique of crystal growth from solutions.
  8. An alkali metal crystallizes in a cubic lattice. The edge of the unit cell is 4.16Ao. The density is 975kg/m3 and its atomic weight is 23. Find the number of atoms in the unit cell and give your comment about the type of cubic cell.
  9. Draw and explain the crystal structure of NaCl.
  10. Describe the principle and fabrication of a transistor using n-p junction.
  11. How are TG and DTA useful in the structural determination of crystals? Give    examples.
  12. What is Frenkel defect? Explain with an example.

Part C

Answer any four questions.                                                                     4X10=40

  1. What are the types of non-stoichiometric defects? Explain with examples.
  2. Draw and explain the structures of wurtzite and zinc blende. Mention the     differences between them.
  3. Describe the hydrothermal growth and growth from melt methods for preparing    crystals.
  4. Write a note on photoelectrocatalytic splitting and photo reduction of water.
  5. Explain BCS theory and Kirkendall effect.
  6. a) Mention any four types of Bravais lattices available depending upon the shapes of the unit cells? Explain with suitable examples.
  7. b) Explain photo galvanic studies using a heterobinuclear complex.

 

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Loyola College B.Sc. Chemistry April 2006 Bio-Chemistry For Biologist Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PLANT BIOLOGY & ZOOLOGY

LM 08

FOURTH SEMESTER – APRIL 2006

                                             CH 4202 – BIO-CHEMISTRY FOR BIOLOGIST

(Also equivalent to CHE 202)

 

 

Date & Time : 22-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

 

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

  1. What is isoelectric point?
  2. Give the structure of lecithin.
  3. How is C- terminal of a peptide determined?
  4. What are enzymes? How are they named?
  5. Mention the roles of the various types of RNA.
  6. What is a reducing sugar? Cite an example.
  7. Give the net reaction of glycolysis.
  8. Explain the enfleurage process.
  9. List the uses of camphor.
  10. Draw the structures of BHC and DDT.

PART – B

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

  1. Discuss the secondary structures of proteins.
  2. Why do almost all enzyme catalyzed reactions show a pH optimum?
  3. Write a short note on the classification of lipids.
  4. What are anomers? Draw the anomeric structures of D-glucose and compare their stability.
  5. Mention the monosaccharide units present in the following sugars:
  6. Maltose b. Cellobiose   c. Lactose        d. Sucrose       e. Starch.
  7. Discuss the different types of soil found in India.
  8. Write a short note on N, P and K fertilizers.
  9. Compare and contrast the two nucleic acids in their composition, secondary structure, bases present and their abundance in the body.
  10. Illustrate the importance of hydrogen bonding in the base pairs of nucleic acids.
  11. Write a short note on flavanoids.
  12. What is isoprene rule? Explain it with an example.
  13. Draw the geometrical isomers of citral. List the uses of citral.

 

 

PART – C

 

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

  1. Discuss the kinds of enzyme inhibition.
  2. Discuss the citric acid cycle in detail.
  3. a. Calculate the net gain of ATP in glycolysis of one mole glucose.             (3)
  4. Write a short note on muta rotation.             (4)
  5. What is denaturation of proteins? What are the factors influencing it? (3)
  6. a. How are terpenoids classified? Give an example each. (5)
  7. Explain the structure, physical properties and uses of α- pinene. (5)
  8. a. What are cofactors? Brief the three kinds of cofactors with an example. (6)
  9. What is iodine value of oil? How is it determined? What is its significance?  (4)
  10. “DNA makes RNA and RNA makes proteins” – establish this with respect to the      biosynthesis of proteins.

 

 

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