B.Sc. Chemistry Question paper

“Loyola College B.Sc. Chemistry April 2009 Polymer Chemistry Question Paper PDF Download”

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        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 15

FIFTH SEMESTER – April 2009

CH 5402 / CH 5400 – POLYMER CHEMISTRY

 

 

 

Date & Time: 28/04/2009 / 1:00 – 4:00  Dept. No.                                                     Max. : 100 Marks

 

 

PART-A                                      

Answer ALL questions.                                                                                               (10 x 2 = 20)

 

  1. Write any two stereo-isomers of polypropylene.
  2. Why does the melting point of Teflon high?
  3. How is polyester prepared? Give an example.
  4. What is living polymerization?
  5. Mention the importance of benzoyl  peroxide in the polymerization reaction with an example.
  6. Give any two drawbacks of solution polymerization.
  7. Differentiate LDPE and HDPE with any four points?
  8. How is polymethyl metha acrylate synthesized?
  9. What are fire retardants?
  10. What are fire reinforcing plastics?

PART-B                                     

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

 

  1. Write short notes on: (a) Elastomers    (b) Polyisoprene rubber
  2. Explain the role of secondary bond forces in polymers.
  3. Discuss the cationic polymerization with mechanism.
  4. Distinguish between number average molecular mass and weight average molecular mass with suitable example.
  5. Explain the process of bulk polymerization.
  6. Derive the rate constant for anionic polymerization.
  7. Write the order of thermal stability of the following polymers and give reasons for the order you select.

Polytetraflouroethylene, Polyphenylene, Polytetraphenylene.

  1. Write and explain the mechanism of phenol formaldehyde polymer.
  2. How are the following polymers synthesized?

(a)Polystyrene   (b) Buna-S

  1. Explain any two methods of polymer degradation?
  2. Explain the process of injection moulding.
  3. Write short notes on: (a) Antioxidants (b) Fillers

PART-C                                    

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

  1. Define the following with example.

(a) Oligomers  (b)Degree of polymerization  (c) Isotactic polymer

(d) Syndiotactic polymer

  1. Discuss the mechanism and its importance of Ziegler Natta polymerization.
  2. Explain the emulsion polymerization with diagram.
  3. What is gas phase polymerization? Explain the mechanism.
  4. What are conducting polymers? Discuss the characteristics of conducting polymers.
  5. Explain the process of calendaring with its applications and limitations.

 

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“Loyola College B.Sc. Chemistry April 2009 Physical Chemistry – II Question Paper PDF Download”

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      LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 01

FIFTH SEMESTER – April 2009

CH 5500 – PHYSICAL CHEMISTRY – II

 

 

 

Date & Time: 16/04/2009 / 9:00 – 12:00    Dept. No.                                              Max. : 100 Marks

 

 

PART – A

Answer ALL questions                                                                                               (10 x 2 = 20)

  1. Write calomel electrode reaction as reduction.
  2. NaCl cannot be used in salt bridge. Why?
  3. Eocell is 1.10V for Zn + Cu2+ → Zn2+ + Cu. Calculate ∆Go cell at 298K.
  4. What are concentration cells? Give one example.
  5. Define transport number of an ion.
  6. 30% of a first order reaction is complete in 100 min. Calculate the rate constant of the reaction.
  7. What is the effect of ionic strength on the rate constant of a reaction of the type A– + B– →

products in solution phase.

 

  1. Mention the steps involved in a thermal chain reaction.

 

  1. “Adsorption is spontaneous and mostly exothermic”.
  2. Define quantum yield of a photochemical reaction.

PART – B

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

  1. Derive Nernst equation for a cell reaction and hence deduce an expression for equilibrium constant for the cell reaction.
  2. Calculate Eo cell, Ecell, ∆Go cell and ∆G cell for Zn|Zn2+ (0.01M) ||Ag+ (0.01M) |Ag at 298k. Eored Zn+2|Zn – 076V and Ag+|Ag 0.8V.  Assume n = 2.  Write the electrode reactions.
  3. Write down the electrode reactions in a) lead storage cell   b) H2 – O2 fuel cell.  Mention one salient feature for each.                                                                                 (3+2)
  4. What is Weston – Cadmium cell? Explain its construction and indicate the electrode reactions.                                                                                                                      (2+2+1)
  5. How is transport number of an ion determined experimentally?
  6. Explain the variation of equivalent conductance with concentration for
  7. a) strong electrolyte b) weak electrolyte in water with suitable graph. (2+2+1)
  8. Differentiate order form molecularity.
  9. Explain the principle of conductometric titrations with one example.
  10. The rate of a first order reaction is doubled on increasing the temperature from 27oC to 37oC (R=8.314 JK-1 mol-1.)   Calculate the activation energy of the reaction.
  11. State the postulates of Langumir adsorption isotherm and hence derive the equation. (2+3)
  12. Write briefly on i) photosensitization ii) chemiluminescence.
  13. Derive an expression for rate constant of a second order reaction of the type 2A →products.

PART – C

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

23) a) Explain how ∆Go, ∆Ho, ∆So of a cell reaction be determined using EMF measurements.    (6)

  1. b) Explain the significance of electromotive series.                 (4)
  2. Give an account of any two of the following a) types of electrodes with the relevant Nernst

equations.  b) determination of Ksp of a salt using EMF.  c) Principle for potentiometric acid –

base titrations.  d) standard hydrogen electrode.

  1. a) Derive an expression for Ecell for a chemical cell with transference (6)
  2. b) How is Ka of weak acid determined using conductance measurements?                         (4)
  3. a) Explain any two methods of determining order of a reaction (6)
  4. b) Discuss the mechanism of SN2 reaction with an example. (4)
  5. Explain the kinetics of single substrate enzymatic reaction. How are the kinetic parameterms

evaluated?                                                                                                                               (6+4)

  1. Write notes on any two of the following (5+5)
  2. a) Debye-Huckel theory of strong electrolytes
  3. b) Principle of polarography
  4. c) Quinhydrone electrode & its use.
  5. d) Parallel reactions.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Physical Chemistry – I Question Paper PDF Download”

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      LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 09

THIRD SEMESTER – April 2009

CH 3500 – PHYSICAL CHEMISTRY – I

 

 

 

Date & Time: 06/05/2009 / 9:00 – 12:00  Dept. No.                                                   Max. : 100 Marks

 

 

 

PART – A

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

 

  1. Distinguish Cp and Cv of an ideal gas.
  2. Define: Integral heat of dilution.
  3. Deduce the relationship between Kp and Kc for the following reaction

2NO(g) + O2(g)     2NO2(g)

  1. Dissociation of NH4Cl is represented by the equation

2NH4Cl(s)      NH3(g) + HCl(g)

What is the number of components for it if a start is made with (i) pure NH4Cl    (ii) NH4Cl  and either product of dissociation

  1. State Le Chatelier’s principle.
  2. Apply phase rule to the triple point of water.
  3. State Hess’s law of heat of summation.
  4. Calculate the root mean square velocity of O2 molecule at 27°C.
  5. “Addition of a non-volatile solute lowers the vapour pressure of a solution” – Offer a theoretical explanation for this statement.
  6. State the Nernst distribution law.

PART – B

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

 

  1. Show that the entropy of mixing of ideal gases is positive.
  2. The standard enthalpy of formation of HCl gas at 25°C is -22.06 kcalmole-1. Calculate the ΔE of formation at 250C.
  3. State third law of thermodynamics. Explain how the absolute entropy of a substance can be determined on the basis of the third law of thermodynamics.
  4. State and derive Gibb’s phase rule.
  5. Water gas reaction is represented by the equation

C(s) + H2O(g)     CO(g) + H2(g)

  1. What is the equilibrium law expression for the reaction?
  2. State, giving reasons, how this equilibrium will shift if
  3. all pressures are doubled
  4. the temperature is increased

 

  1. Deduce gas laws on the basis of the kinetic theory of gases.
  2. State and explain Henry’s law. What are the limitations of this law?

 

 

 

 

  1. What is meant by critical solution temperature? How can it be determined for phenol-water system? Explain the effect of addition of NaCl on the critical solution temperature.
  2. How can the molecular mass of a nonvolatile solution be determined from freezing point measurements?
  3. A 0.1formal solution of NaCl is found to be isotonic with a 1.10% solution of urea. Calculate the apparent degree of dissociation of NaCl.
  4. Apply phase rule to Lead-Silver system and discuss the desilverisation of lead from this system.
  5. Draw and explain the phase diagram of any three component system having one partially miscible pair.

PART – C

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

 

  1. Derive Maxwell’s equations from basic thermodynamic ralations.
  2. a. Derive Gibbs-Helmholtz equation.
  3. The measured heats of neutralization of acetic acid, formic acid, hydrocyanic acid and hydrogen sulphide are 13.20, 13.40, 2.90 and 3.80 kcal per geq. respectively. Arrange these acids in the decreasing order of strength.
  4. Draw the phase diagram of FeCl3-H2O system and describe its complete labeling. Explain, What do you understand by the isothermal evaporation of the solution.
  5. a. State and explain Raoult’s law.
  6. What are azeotropic mixtures? Give examples.
  7. a. What are abnormal colligative properties? How will you calculate the vant Hoff factor and degree of dissociation of a solute from the measurement of colligative properties?
  8. 0.9g of a solute was dissolved in 100ml of benzene at 25°C when its density is 0.879g/ml. The solution boiled 0.250°C higher than the boiling point of benzene. Molal elevation boiling point constant for benzene is 2.52 Kkgmol-1. Calculate the molecular weight of the solute.

 

  1. Derive thermodynamically the relation connecting elevation in boiling point of a solution of a non-volatile solute in a volatile solvent and its molality.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Phase Equilibria And Kinetics Question Paper PDF Download”

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       LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 25A

FIFTH SEMESTER – April 2009

CH 5507 – PHASE EQUILIBRIA AND KINETICS

 

 

 

Date & Time: 24/04/2009 / 1:00 – 4:00   Dept. No.                                                      Max. : 100 Marks

 

 

 

PART – A

Answer ALL questions                                                                                 (10 X 2 = 20)

 

  • Identify the number of phases and components at equilibrium

CaCO3(s)                       CaO(s)   +   CO2(g)

2)      Apply phase rule equation at the triple point of water.

3)      What are isotonic solutions?

4)       A solution of 0.1 M NaCℓ aqueous solution has a boiling point of 101.04o C. What will be the boiling point of 0.2 M urea solution Kb = 0.52K kg mol -1?

5)      Define rate constant of a reaction.

6)      What is a zero order reaction?

7)      Calculate the ionic strength of 0.1 m BaCℓ2 solution at 25o C

8)      Enzyme catalysis decelerates at high temperatures.  Why?

9)      What is Wilkinson’s catalyst?

10) Distinguish between adsorption and absorption.

PART – B

Answer ANY EIGHT questions only                                                                      (8 X 5 = 40)

 

  • Draw and describe phase diagram of Pb – Ag system

12)  Explain the phase behavior of a three component system.

13)  What is an azeotrope?  Explain azeotropic distillation with an example.

14)  Derive Nernst Distribution law.

15)  What are chain reactions. Explain with an example.

16)  There is a first order dependence on concentration of KI and K2S2O8.  If the initial concentration of K2S2O8 is ‘a’ moles dm-3 and KI is ‘2a’ moles dm-3.   Derive the expression for the rate constant of the reaction.

17)  Explain the terms order, molecularity and stoichiometry of a reaction with a suitable example.

18)  Explain the kinetics of parallel reactions with an example.

19)  State steady state approximation.  Illustrate with an example

20)  The specific rate of decomposition of HI at 556 K & 781 K are 3.517 X10-7 dm3 mol-1 s-1 and     3.954 X 10-2 dm3 mol-1 s-1 respectively.  Calculate energy of activation in cal mol-1 and Arrhenius pre-exponential factor A in dm3 mol-1 s-1.

 

 

21)  Explain the kinetics of acid catalysed ester hydrolysis.  How the order with respect to each reactant is determined.

22)   Distinguish between physisorption and chemisorption.

 

PART C

Answer ANY FOUR questions only                                                                       (4 X 10 = 40)

 

23)  Draw the phase diagram of FeCℓ3 – water system and apply phase rule.

24)  Derive the relation between elevation of boiling point and morality of the solution, thermodynamically.

25)  Explain any two of the following:                                                                                                        a) Phase diagram of partially miscible liquid pair exhibiting both UCST & LCST                                  b) Application of distribution law to KI  +  I2              KI3 equilibrium                                               c) Raoults law and its deviations                                                                                                        d) Application of Clapeyron equation

26)  A) Describe Van’t Hoff differential method of determination of order of a reaction                                              B) Explain one mechanism of bimolecular surface reaction.

27)  Discuss the kinetics enzyme catalysis as propounded by Michaelis Menton in detail.

How the rate constants of individual steps are evaluated.

28)  State the postulates of Langumir adsorption isotherm and hence derive the equation and explain.

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“Loyola College B.Sc. Chemistry April 2009 Organic Functional Groups II Question Paper PDF Download”

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CH 5505 – ORGANIC FUNCTIONAL GROUPS II

PART – A

Answer ALL the questions                                                                        (10 x2 = 20 marks)

  1. Write the isomers of nitrobutane.
  2. What is diazotization?
  3. Explain with example D and L notation.
  4. Mark R and S configuration for the following compounds
  1.             ii)

 

  1. Write the synthesis of acetoacetic ester by Claisen condensation.
  2. How is diazomethane prepared?
  3. What is Isoprene rule?
  4. What is Fries rearrangement?
  5. What are sulpha drugs?
  6. Draw the structures of the following compounds  (i) α-pinene          ii) Camphor

 

PART – B

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

  1. Explain the mechanism of Gomberg reaction.
  2. Which of the following is more basic? p-nitro aniline or  p-Toludine.  Explain
  3. Give an account of the optical activity of biphenyls.
  4. Explain Walden inversion.
  5. Establish keto-enol tautomerism exhibited by acetoacetic ester.
  6. How will you synthesise the following from acetoacetic ester (i) Acetyl acetone  (ii) Crotonic acid?
  7. Write briefly on Beckmann rearrangement.
  8. How is isoquinoline prepared?
  9. How does pyridine react with         i) NaNH2      ii) n-ButylLithium        iii) CH3 COCl/A1C13.
  10. Explain the electrophillic substitution of reactions of pyrrole.
  11. How will you prepare 1, 3, 5 trinitrobenzene?
  12. Explain asymmetric synthesis.

 

 

 

PART – C

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

  1. (i) How will you separate the mixture of amines by Hinsberg method.

(ii)Explain the coupling reactions of benzene diazonium chloride.

  1. Explain the various methods of Resolution of a racemic mixture.
  2. Write the preparation, properties and uses of diazoacetic ester.
  3. Explain any two following rearragngements with mechanism

(i) Benzilic      (ii) Cope                     (iii) Curtius

  1. i) Name the following compounds based on R and S configuration and represent it in

flying wedge,  sawhorse and Newmann projection formula.

 

 

(ii) Differentiate of enantiomersfrom diastereomers.

  1. (i) Explain Hoffmann’s rearrangement.

(ii) Outline the synthetic utility of Benzene diazonium chloride.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Organic Functional Groups – I Question Paper PDF Download”

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 LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 10

THIRD SEMESTER – April 2009

CH 3502 – ORGANIC FUNCTIONAL GROUPS – I

 

 

 

Date & Time: 02/05/2009 / 9:00 – 12:00       Dept. No.                                                       Max. : 100 Marks

 

 

PART-A                                      

Answer ALL questions.                                                                                  (10 x 2 = 20)

 

  1. What is Saytzeff rule? Give an example?
  2. What happens when n-propyl bromide is treated with alcoholic KOH?
  3. How will you distinguish between methyl alcohol and ethyl alcohol?
  4. Write any two drawbacks of Friedal-Crafts reaction with an example.
  5. How will you synthesise diethyl ether from ethyl alcohol?
  6. Give the general mechanism of nucleophilic addition reactions of carbonyl compounds.
  7. Write the mechanism of Cannizzaro reacton.
  8. Arrange the following compounds in order of increasing acidity and explain you answer.

HCOOH,   ClCH2COOH, CH3COOH

  1. How will you synthesise succinic acid from ethylene?

 

PART-B                                     

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

 

  1. a) What happens when propene treated with HBr in the presence of organic peroxides?

Explain.

  1. b) Discuss the mechanism of E2 reaction of alkyl halides.
  2. a) Why do aryl halides are less reactive towards nucleophilic displacement reactions?
  3. b) Write the general mechanism of aromatic electrophilic substitution reaction.
  4. How will you convert primary alcohol into tertiary alcohol? Explain.
  5. Discuss the mechanism of sulphonation reaction of phenol.
  6. Write a note on: Kolbe Reaction.
  7. Explain the mechanism of the reaction between aromatic aldehydes and aqueous alcoholic KCN.
  8. Write a note on: Norrish II reaction.
  9. How will you synthesis cinnamic acid from benzaldehyde? Give the mechanism.
  10. a) n-Butyl ether(bp 118 °C) has a much higher boiling point than its isomer diethylether (bp 35 °C).Explain.
  11. b) Write a note on: Cleavage of ethers by acids.
  12. Discuss the effect of the substituents on acidity of carboxylic acids.
  13. Write the mechanism of esterification reaction.
  14. How is adipic acid synthesized from cyclohexane?

 

 

 

 

 

PART-C                                    

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

 

  1. a) Write any five differences between SN1 and SN2 reaction mechanism. (5)
  2. b) Discuss the mechanism of E2 and explain any three evidences. (5)
  3. Complete the following reactions with mechanism. (5+5)
  4. a) Write the mechanism of wittig reaction. (5)
  5. b) Write a note on: Michael addition. (5)
  6. a) What is Williamson’s synthesis? (3)
  7. b) What happens when glycerol treated with KHSO4? (3)
  8. c) How will you convert acetaldehyde into paraldehyde?                            (2)
  9. d) Give the product when acetone undergoes the condensation in dry HCl. (2)
  10. Write the complete reaction for the following conversions.                           (4 x2.5)
  11. a) Ethylene bromide into succinic acid b) Butene into maleic acid
  12. c) Ethyl acetoacetate into crotonic acid d) Allyl alcohol into acrylic acid
  13. Predict the products of the following reactions. (5×2)

 

 

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“Loyola College B.Sc. Chemistry April 2009 Molecular Dynamics Question Paper PDF Download”

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    LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 19

SIXTH SEMESTER – April 2009

CH 6606 / 6600 – MOLECULAR DYNAMICS

 

 

 

Date & Time: 18/04/2009 / 9:00 – 12:00     Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

 

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

 

  1. Define the term orbit and orbitals.

 

  1. State Pauli’s exclusion principle.

 

  1. Define the term degeneracy of an energy level.

 

  1. What is Quantum Yield?

 

  1. Give the significance of φ2.

 

  1. Find the value of ln NA!, ( Where  NA   is Avagadro’s number )using Stirlings

approximation.

 

  1. State the Stark-Einistien’s law.

 

  1. Define Chemiluminescence.

 

  1. What are thermal reactions? Give an example.

 

  1. Mention any two methods of studying fast reactions.

 

PART – B

 

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

 

  1. How is photoelectric effect explained by quantum theory.

 

  1. Calculate the radius of the electron in the first orbit of hydrogen atom.

 

  1. Derive the expression for the energy of an electron in the nth shell of hydrogen.

 

  1. State the postulates of quantum mechanics and explain any one of them.

 

  1. Define the Laplacian operator and Hamiltonian operator.

 

  1. Explain Sackur-Tetrode equation and mention the terms involved.
  2. A system of N particles has among others, two energy levels with g1 = 2,

g2 = 3, E1 = 41.84 kJmol-1  and  E2 = 58.58 kJmol-1.   Calculate the ratio of the number of particles in the two energy states at 1000K.

 

  1. Derive the relation between partition function and energy.

 

  1. Explain Photo sensitisation.

 

  1. Explain the primary and secondary processes in a photochemical reaction.

 

  1. Describe flash photolysis.

 

  1. Explain the kinetics of photochemical reaction between  H2  and  Br2.

 

PART – C

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

 

  1. Explain (i) Black body radiation (ii) Separation of partition function.

 

  1. Derive the expression of Eigen value ‘E’ and Eigen function  ‘ψ ‘ for a particle

in one dimensional box.

 

  1. (i) Derive an expression for translation partition function.

(ii)        Calculate the translational partition function for benzene in a volume of

1 m3 at 25oC.

 

  1. Derive the Maxwell – Boltzmann distribution law.

 

  1. Explain any tow of the following

(i)         Radiationless transition.

(ii)        Phosphorescence

  • Actinometers
  • Zeemann effect

 

  1. (i) Derive the Stern-Volmer equation.

(ii)        Explain Jablanski diagram.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Mathematics For Chemistry Question Paper PDF Download”

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       LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

ZA 72

THIRD SEMESTER – April 2009

MT 3103 / 3101 – MATHEMATICS FOR CHEMISTRY

 

 

 

Date & Time: 17/04/2009 / 1:00 – 4:00   Dept. No.                                                        Max. : 100 Marks

 

 

SECTION A

Answer ALL questions:                                                                               (10 x 2 = 20)

  1. If, find.
  2. Solve.
  3. Integrate with respect to x.
  4. Solve
  5. Show that .
  6. Define characteristic roots.
  7. Expand tan 7θ in terms of tanθ.
  8. Find the real and imaginary parts of.
  9. Find the arithmetic mean of the following frequency distribution:

x:         1          2          3          4          5          6          7

f:          5          9          12        17        14        10        6

  1. Write the moment generating function of Poisson distribution.

SECTION B

Answer any FIVE questions:                                                                       (5 x 8 = 40)

  1. Find the maxima and minima of the function.
  2. Find the equation of the tangent to the ellipse at.
  3. Evaluate.
  4. If a,b,c denote three consecutive integers show that
  5. Sum to infinity the series.
  6. Show that
  7. Prove that.
  8. A coffee connoisseur claims that he can distinguish between a cup of instant coffee and a cup of percolator coffee 75% of the time. It is agreed that his claim will be accepted if he correctly identifies at least 5 of the 6 cups. Find his chances of having the claim (i) accepted, (ii) rejected, when he does have the ability he claims.

SECTION C

Answer any TWO questions:                                                                       (2 x 20 = 40)

 

  1. (a) For the curves  and, find the angle of intersection.

(b) Differentiate.                                                                      (12 + 8)

  1. (a) Evaluate .

(b) Integrate  with respect to x.

(c) Solve .                                                       (7 + 5 + 8)

  1. (a) Sum to infinity the series .

(b) Find the characteristic roots and the characteristic vectors of the matrix

.                                                                                           (8 + 12)

  1. (a) Prove that.

(b) Obtain a Fourier expansion for the function.  (10 + 10)

 

 

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“Loyola College B.Sc. Chemistry April 2009 Main Group Elements & Solid State Chemistry Question Paper PDF Download”

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        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 11

THIRD SEMESTER – April 2009

CH 3503 – MAIN GROUP ELEMENTS & SOLID STATE CHEMISTRY

 

 

 

Date & Time: 05/05/2009 / 1:00 – 4:00  Dept. No.                                                    Max. : 100 Marks

 

 

 

PART – A                                                                              (10 x 2 = 20)

ANSWER ALL THE QUESTIONS

 

  1. Why do group I elements have the lowest first ionization energy values ?
  2. Write the structure of beryllium chloride in the gaseous and solid state.
  3. Write the reaction of aluminum with dilute mineral acid.
  4. How does diborane react with ammonia at different conditions ?
  5. How is tripe super phosphate obtained ?
  6. Write the structure of perdisulphuric acid.
  7. Fluorine is the most reactive of all the elements. Why ?
  8. What are pseudohalides ?  Give examples.
  9. What are Miller indices ?
  10. Define isotropy.

 

PART – B                                                                        (8 x 5 = 40)

ANSWER ANY EIGHT QUESTIONS

 

  1. How lithium differs from the other group I elements ?
  2. What are the uses of the compounds of group I elements ?
  3. How are amorphous and crystalline boron extracted ?
  4. What are the different types of silicates ?
  5. How is hydroxylamine prepared ?  Write the reaction of it with HCl and H2SO4.  Mention its uses.
  6. Draw the structures of phosphorous trioxide and pentoxide.
  7. How is hydrazine prepared ? Give two of its reactions.
  8. How is dichlorine monoxide prepared ?  Mention its reactions and structure.
  9. Mention one method of preparation of a) HClO3    b) HClO4
  10. Mention the different types of crystals.  Give one example each.
  11. What is crystal defect ?  Explain one of it.
  12. Draw and explain simple cubic, face centered cubic and body centered cubic system.

 

PART – C                                                                                    (4 x 10 = 40)

 

ANSWER ANY FOUR QUESTIONS

  1. a) How is sodium metal extracted ?                                                              (5)
  2. b) How beryllium differs from the other group II elements (5)
  3. a) Write a note on the structure of borates.
  4. b) Explain the different types of carbides
  5. a) What are the different types of oxoacids of phosphorus ?

Draw their structures.                                                                                (2+4)

  1. b) How are oxides classified ? Explain. (4)
  2. a) Compare the properties of phosphorous trichloride and phosphorous penta

chloride.

  1. b) Write the preparation and properties of nitric acid.
  2. a)   What is an interhalogen compound ?  Mention their different types.  Give one

example of each.

  1. b) Write the chemical properties of ClF, ClF3    and  I F7
  2. a)  How is X-ray diffraction technique used in the study of crystals ?
  3. b) Derive Bragg’s equation for diffraction of X-rays by crystals.

 

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“Loyola College B.Sc. Chemistry April 2009 Industrial Chemistry Question Paper PDF Download”

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      LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 24

SIXTH SEMESTER – April 2009

CH 6611 / 6605 – INDUSTRIAL CHEMISTRY

 

 

 

Date & Time: 25/04/2009 / 9:00 – 12:00  Dept. No.                                                   Max. : 100 Marks

 

 

PART – A

Answer ALL questions:                                                                               (10 x 2 = 20)

 

  1. Define calorific value of fuels.
  2. Explain: Gobar electric cell.
  3. How is 2, 4-D manufactured?
  4. Give two examples for biofertilisers.
  5. Define Break point chlorination.
  6. Which dissolved salts contribute for permanent hardness?
  7. What is acid rain? How is it caused?
  8. Describe the toxicity of mercury.
  9. What are the constituents of portland cement?
  10. What is a luminous paint? Give an example.

PART – B

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

 

  1. Write a note on Producer gas.
  2. How are coals classified? Give the composition of each type.
  3. What is DDT? How is it manufactured? Indicate its uses.
  4. Write a note on micronutrients and their role in the growth of plants.
  5. How do you estimate calcium hardness in water by EDTA method?
  6. How is water softened by zeolite process?
  7. Explain the principle involved and application of reverse osmosis.
  8. Describe how ozone depletion takes place in stratosphere.
  9. Give an account of BOD determination in waste water.
  10. What are the international standards for drinking water quality? How do they compare with ISI specifications?
  11. Write a note on perfumes and flavouring agents.
  12. Explain the functioning of molybdenum sulphide as a solid libricant.

PART – C

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

 

  1. a) Describe the determination of calorific value of a fuel by Bomb calorimeter (6).
  2. b) What are the uses of ETBE and MTBE (4).
  3. a) How are (a) Super phosphate of lime (b) Triple superphosphate manufactured? Which is superior? Why?  (7)
  4. b) What is BHC? How is it manufactured? (3)
  5. a) Outline the process of refining of Petroleum (5)
  6. b) How do you prepare Bordeaux mixture? What is its composition? Mention its use. (5)
  7. a) How is total hardness of water estimated. (5)
  8. b) How are suspended impurities and micro organism removed from water used for drinking purpose? (5)
  9. a) Write a note on air pollution (5)
  10. b) Explain the biochemical effects of nitrogen oxides (5)
  11. a) What are abrasives? How are they classified? Give examples (5)
  12. b) Write a note on pharmaceutical industries in India.

 

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“Loyola College B.Sc. Chemistry April 2009 Hydrocarbons And Stereochemistry Question Paper PDF Download”

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       LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 06

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – April 2009

CH 2504 / 2502 – HYDROCARBONS AND STEREOCHEMISTRY

 

 

 

Date & Time: 23/04/2009 / 1:00 – 4:00 Dept. No.                                                   Max. : 100 Marks

 

 

PART – A

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

 

  1. Write the structural formula for the following compounds.
  2. 3,3-Dimethyl-1-butene; b) But-2-en-1-ol.
  3. Classify the following into +M and –M group

2 ,   2 ,   ,

  1. What happends when ethylchloride reacts with sodium metal.
  2. What is aromaticity Explain with an example?
  3. Specify the E and Z notation to the following compounds.
  4. a) b)

 

  1. What alkyl halide would yield each of the following pure alkene up on dehydro halogenation by a strong base. a) Isobutylene b) 3-methyl-l-butene.
  2. In Fridel-craft’s alkylation of benzene using n-propyl chloride gave only Isopropyl benzene rather than n-propyl benzene. Explain.
  3. Indicate which ring you would expect undergo nitration in phenylbenzoate.
  4. Write the structure of (i) Cis-4-tert-butylmethyl cyclohexane.                           (ii) cis-1, 2-dimethyl cyclohexane
  5. What are polynuclear aromatic compounds? Give two examples.

 

PART – B

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

 

  1. Write various possible structural formula of alkanes with molecular formula, C5H12 and write their IUPAC names.
  2. Discuss the different factors affecting the stabilities of carbocation (1o, 2o and 3o)
  3. Explain Bayer’s strain theory.
  4. How will you prepare cyclopentane using Dieckmann’s Synthesis.
  5. What are different conformation of cyclohexane. Draw their structure and explain the stabilities.
  6. How is ethylene prepared in the laboratroy? How does it react with
  7. i) Bromine water ii) Conc. H2SO4 iii) HCl                                                            (2+3)
  8. Explain the mechanism of Nitration of benzene.
  9. What is tautomerism. Explain mitro-acinitro tautomerism exhibited by Nitroethane.
  10. Explain by resonance structure that NO2 is meta directing, where as –OH group is Ortho-para directing towards electrophillic aromatic substitution.
  11. Explain the mechanism of Markownikoff’s Propene.

 

  1. i) How will you differentiate 1-butyne from 2-butyne.
  2. ii) Explain the mechanism of Hydroboration of propene.
  3. Write the structure of the product for the following reaction.
  4. Napthalene
  5. Napthalene
  • 2-butene
  1. Nitrobenzene
  2. Phenol

PART – C

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

 

  1. a) Explain the type of hybridisation in the following
  2. i) Benzene ii) 1, 3 – buta-diene iii) cyclohexane                       iv) l-butyne.
  3. Which is more basic ethylamine or Aniline Explain.
  4. a) Explain Hyper conjugation.
  5. Arrange the compound in the increasing order of acid strength and Explain.
  6. CCl3 COOH ii) CH3 COOH,           iii) CH3 CH2 CH2 COOH       iv)CH2Cl OOH
  7. A hydrocarbon ‘A’ adds one mole of hydrogen in the presences of a platinum catalyst to form n-hexane. When A is oxidised vigourously with KMnO4, a single carboxylic acid containing three carbon atoms is isolated. Give the structure and name of A. Show your reasoning including equation for all reactions.
  8. i) Explain 1,2 – and 1,4 – addition of HBr with 1,3-butadiene.
  9. Write the mechanism Fridel – Craft’s Acylation
  10. i) Predict the product of Bromination of
  11. Acetanilide b) cinnamic acid
  12. Explain Diel’s Alder reaction taking suitable example.
  13. Draw various possible conformation of n-butane explain their stabilities based on energy level diagram?

 

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“Loyola College B.Sc. Chemistry April 2009 General Chemistry For Physics & Maths Question Paper PDF Download”

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        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 04

B.Sc. DEGREE EXAMINATION – MATHEMATICS & PHYSICS

SECOND SEMESTER – April 2009

CH 2102 / 2100 – GENERAL CHEMISTRY  FOR PHYSICS & MATHS

 

 

 

Date & Time: 25/04/2009 / 1:00 – 4:00  Dept. No.                                                 Max. : 100 Marks

 

 

                                                                      PART-A                  

 Answer ALL questions.                                                                   (10 x 2 = 20)

 

  1. Write the IUPAC names of the following complexes.

(i) Na2[Fe(CN )6]      (ii)    [Co(en)3]Cl 3                                                                                                                                  2. The expected and actual configuration of Cr and Cu differs. Why?

  1. Write the following acids in increasing order of their acidity. Justify your answer.

ClCH2COOH, CH3COOH, CCl3COOH, Cl2CHCOOH

  1. Mention the type of isomerism exhibited by maleic and fumaric acids. Give their structures.
  2. State Beer-Lambert’s Law.
  3. Differentiate homogeneous and heterogeneous catalysis with suitable examples. 7. What are the types of RNA? Mention their functions.
  4. What are the diseases associated with abnormal metabolism of thyroxine? What are its

symptoms?

  1. What is meant by vulcanization?

10 How corrosion is prevented by electroplating?

 

PART-B

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

 

  1. Explain the postulates of Werner’s theory of coordination complexes. 12. Explain the structure and functions of chlorophyll.
  2. Write all possible isomers of (i) [RhCl2(en)2]+ (ii)  [CoCl3(NH3)3]+
  3. Discuss the various conformers of butane.
  4. Explain the optical isomerism in tartaric acid. 16. Derive the expression for rate constant of first order reactions.                                                            17. Compare thermal and photochemical reactions.                                                                                      18.  Draw the structure and give any two functions of the following.
  5. a) Oxytocin   b) Testosterone
  6. What are the various achievements of genetic engineering and give any two possible

dangers of it.                                                                                                                                     20. Explain the electrochemical mechanism of corrosion.                                                                                                    21. State Raoult’s law. Discuss the positive deviations of real solutions from their ideal  behaviour.   22. Differentiate the following with suitable examples.

(a) Step growth and chain growth polymerization

(b) Thermoplastics and thermosetting plastics

 

PART-C

Answer any FOUR questions                                                          (4 x10 = 40)  

  1. i) Discuss the postulates of VB theory.   (4+6)
  2. ii) Predict the geometry, structure and magnetic property of [CoF6]3-
  3. i) Compare SN1 and SN2 reactions (5+5)
  4. ii) Give the mechanism of nitration of benzene.
  5. Discuss the application of phase rule to water system.
  6. i) What is the effect of temperature on the rate of a reaction? (4+6)
  7. ii) Discuss the variation of mutual solubility of phenol and water with temperature.
  8. Discuss the double helical structure of DNA. (5 + 5).
  9. How do the following polymers prepared? Give any two uses of them.

(a) Buna-S     (b) Bakelite     (c) PET                 (3+4+3)

 

 

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“Loyola College B.Sc. Chemistry April 2009 Electrochemistry Question Paper PDF Download”

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       LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 14

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – April 2009

CH 4502 – ELECTROCHEMISTRY

 

 

 

Date & Time: 24/04/2009 / 9:00 – 12:00  Dept. No.                                                   Max. : 100 Marks

 

 

                                                                      PART – A                   

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

 

  1. Define electromotive series. Give its application.
  2. What is a reversible cell?
  3. What is LJP? How can it be minimised?
  4. What are Fuel cells? Give its application.
  5. State Faraday’s first law of electrolysis.
  6. Distinguish between Strong and Weak electrolyte.
  7. Define the term activity of an electrolyte.
  8. Explain the principle involved in the conductometic titration of AgNO3.
  9. Define the term limiting current.
  10. Define Overvoltage.

 

PART – B

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

 

  1. Explain the following with an example.

(i)         Metal – Metal ion electrode.

(ii)        Amalgam electrode.

  1. Describe the construction and working of Weston cell.
  2. Calculate the EMF of the concentration cell

Pt;  H2(P1),  HCl,  H2(P2);  Pt at 25oC.

If P1 = 600 torr and P2 = 400 torr.

  1. How will you determine the standard electrode potential of copper electrode.
  2. How will you determine the pH of a solution using glass electrode.
  3. Derive expressions for ΔG; ΔH  and  ΔS  in terms of EMF of a cell.
  4. How is transport number determined by moving boundary method?
  5. Calculate the equivalent and molar conductivities of 0.08N H2SO4  solution

having specific conductivity  1.72 x 10-3  Scm-1.

  1. How is Kb of a weak base determined by conductance measurement?
  2. Discuss the principle and procedure for conductometric titration of a

Strong acid with a strong base.

  1. Discuss on the applications of decomposition potential.
  2. Explain the electrochemical theory of corrosion.

 

                                                                      PART – C

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

 

  1. How is solubility of sparingly soluble salt determined by EMF measurements.
  2. (i) Derive the Nernst electrochemical equation.

(ii)        Calculate the reduction potential of the electrode

Pt/Cl2(g)  (1.15)atm/2Cl– (0.01M).

Given that EoCl2/2Cl– = 1.8V.

  1. What are concentration cells? Derive an expression for the EMF of an electrolyte  for a concentration cell without transference.
  2. Explain any four applications of EMF.
  3. (i) Discuss the Arrhenius theory of electrolytic dissociation.

Give its limitations.

  • Explain the principle involved in the potentiometric titrations.
  1. (i) Discuss on the Debye-Huckel theory of strong electrolytes.

(ii)        Explain the principle of polarography.

 

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“Loyola College B.Sc. Chemistry April 2009 Coordination Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 20

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – April 2009

CH 6607/CH 6601 – COORDINATION CHEMISTRY

 

 

 

Date & Time: 21/04/2009 / 9:00 – 12:00      Dept. No.                                                          Max. : 100 Marks

 

 

PART – A

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

 

  1. Calculate CFSE value for octahedral complex.
  2. Predict whether an octahedral complex formed by a ion is perfect or distorted. Explain.
  3. on treatment with gives trans . Account for.
  4. Give two examples for photo substitution reaction.
  5. What is the principle involved in Metal template Synthesis? Give an example.
  6. What are non-complementary electron transfer reactions? Give an example.
  7. Explain the role of rhodium metal in Wilkinson’s catalysis.
  8. Draw the structure of .
  9. What is meant by chelate therapy? Mention its advantage.
  10. What is the biological role of catalases in nitrogen fixations?

 

PART – B

 

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

 

  1. Describe with a neat diagram, the splitting of metal d-oribals in a square planar complex.
  2. What are the experimental evidences for metal-ligand orbitals overlapping?
  3. State Jahn Teller theorem. The octahedral complex formed by is distorted. Explain.
  4. Discuss the mechanism of inner-sphere electron transfer reaction with a suitable example.
  5. Explain associative mechanism of ligand substitution reactions in octahedral complexes.
  6. Write a note on photoisomerisation reactions.
  7. Describe the polarization theory of trans effect in synthesis of square planar complexes.
  8. How do you prepare Schiff bases using template synthesis? Explain with two examples.
  9. The IR spectrum of consists of two CO stretching bands at 1857 cm-1 and 1897 cm-1. Rationalize this.
  10. Explain the polymerization of olefins using Ziegler-Natta catalyst.
  11. What is the significance of contrast agents in MRI? Give three examples.
  12. Write a note on iron-molybdenum center in nitrogenase enzyme.

 

 

PART – C

Answer any FOUR questions:                                                                                             (4 x10 = 40)

 

  1. (a) Construct Metal orbitals and LGO suitable for and – bonding in Octahedral geometry  (5)

(b) Construct MO energy level diagram for .                                                            (5)

 

  1. Define outer-sphere electon transfer reaction. Explain the mechanism with an example. What are the experimental evidences for outer sphere electron transfer?

 

  1. (a) Explain dissociative mechanism of ligand substitution reactions in octahedral complexes.  (5)

(b) Describe the CF split of metal d-orbitals in octahedral geometry.                                              (5)

 

  1. (a) Predict the stability of .                    (5)

(b) Draw the structure of (i) Fe3 (CO)12   (ii)Mn2(CO)10.                                                                 (5)

 

  1. (a) What is meant by Cis effect? Explain with two examples.          (5)

(b) Describe the template synthesis of metal phthalocyanins.                                                         (5)

 

  1. (a) Write a note on Wilkinson’s catalyst and hydrogenation of alkene using it.          (6)

(b) Write the structure of carboxypeptidase-A. What is its biological importance?                      (4)

 

 

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“Loyola College B.Sc. Chemistry April 2009 Concepts In Inorganic Chemistry Question Paper PDF Download”

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          LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 03

FIRST SEMESTER – April 2009

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

Date & Time: 22/04/2009 / 1:00 – 4:00       Dept. No.                                                       Max. : 100 Marks

 

 

 

PART – A

Answer ALL the questions:                                                             10 x 2 = 20       

 

  1. Define inert-pair effect with an example.
  2. State Pauli’s exclusion principle.
  3. Among and , which has more electron affinity? Why?
  4. is less soluble than Give reason.
  5. Calculate the bond order in .
  6. Describe the structure of based on VSEPR Theory.
  7. Among O-chloro phenol and p-chlorophenol, which is more volatile? Explain.
  8. Explain ion dipole – dipole interactions of molecules.
  9. Label the following as Acid or base. .
  10. What are aprotic solvents? Give two examples.

 

PART – B

Answer any EIGHT questions:                                                                   8 x 5 = 40

 

  1. Write a note on magnetic separation of ore dressing.
  2. (a) Write the Schrodinger wave equation and explain the terms.

(b) What is the significance of wave function?

  1. Discuss the diagonal relationship between and .
  2. State and explain Fajan’s rules to explain the Covalent character of ionic compounds with examples.
  3. Explain the trend in ionisation potential values of elements belonging to Second Period.
  4. Apply MO theory and draw MO energy level diagram for ‘NO’ molecule. Calculate bond order.
  5. Based on Valence Bond Theory, discuss the geometry of (a) (b) .
  6. Explain the structure of (a) (b) using VSEPR Theory.
  7. Write a note on clathrates.
  8. What are Hume-Rothery rules? What are their significance in the structure of alloys?
  9. Balance the following chemical reactions by oxidation number method.
  1. Write a note on Lewis theory of acids and bases.

PART – C

Answer any FOUR questions:                                                                     4 x 10 = 40

 

  1. Discuss various factors affecting the formation of ionic compounds with suitable examples.
  2. How is electro negativity determined by (a) Pauling Method (b) Mulliken – Jaffe Method.
  3. Write electron dot formula for
  4. Describe the conditions for the combinations of atomic orbitals to produce Molecular Orbitals.
  5. How does band theory explain the conducting properties of metals, Semi-conductor and insulator?
  6. Describe the role of liquid ammonia as a solvent for various types of reactions with examples.

 

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“Loyola College B.Sc. Chemistry April 2009 Chemistry Of Natural Products Question Paper PDF Download”

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     LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 23

SIXTH SEMESTER – April 2009

CH 6610 / 6604 – CHEMISTRY OF NATURAL PRODUCTS

 

 

 

Date & Time: 23/04/2009 / 9:00 – 12:00  Dept. No.                                                  Max. : 100 Marks

PART – A

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

  1. What is Zeisels method?
  2. Predict the product of complete Hoffmann’s exhaustive methylation of piperidine.
  3. What are flavones?
  4. Explain the geometrical isomerism exhibited by citral.
  5. Write down the Robinsons Synthesis of anthocyandin.
  6. Predict the product of KoH fusion of cyandine chloride.
  7. What happends when uric acid treated with Conc. HNO3.
  8. How will you convert uric acid to Theophylline.
  9. Write the structure of alizarin.
  10. What will be the product selenium distillation of cholestrol.

PART – B

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

  1. How will you synthesis piperine.
  2. What are anthocyanisis? Give exmaples.
  3. What are the various conformation exhibited by Menthol.
  4. Predict the Ozonolysis product of b–ionone.
  5. What happens when Geranic acid is treated with cold alkaline potassium permanganate solution.
  6. How flavones are prepared by Baker-Venkatraman Synthesis.
  7. Write down the Traubes Synthesis of Caffeine.
  8. Write down the synthesis of Camphornic acid.
  9. Explain the nature and position of side chain in cholestrol.
  10. Write the synthesis of Alizarin.
  11. Briefly elucidate the structure of Indigoitin.
  12. What are purines? What are all its biological importance.

PART – C

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

  1. Elucidate the structure of papaverine.
  2. Explain the general methods of structural clucidation of alkaloids with suitable examples.
  3. Explain any two of the following:
  4. Cartenoids
  5. Biological properties of papaverine
  6. Spectral properties of steroids
  7. Isoprene rule.
  8. Write down the synthesis of Oestrone.
  9. Write the synthesis of any two (i) Conine (ii) Nicotine     (iii) Indigotin
  10. Write the importance and structural determination Quercetin.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Chemistry For Biologist – I Question Paper PDF Download”

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       LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – ADV.ZOO. & PLAN. BIO&BIOTECH.

WD 07

THIRD SEMESTER – April 2009

CH 3104 / 3102 – CHEMISTRY FOR BIOLOGIST – I

 

 

 

Date & Time: 17/04/2009 / 1:00 – 4:00    Dept. No.                                         Max. : 100 Marks

 

 

PART A

Answer all the questions.                                                                                      10×2=20

  1. Define molarity.
  2. How are (i) ionic and (ii) covalent bonds formed?
  3. What is tyndall effect?
  4. How is Nylon-6 prepared?
  5. Differentiate lyophilic and lyophobic colloids.
  6. What is enzyme catalysis?
  7. Give the principle of volumetric analysis.
  8. What are enantiomers? Give an example.
  9. Mention the properties of a primary standard substance.
  10. What is electron affinity? What is its significance?

PART B

Answer any eight questions.                                                                                  8×5=40

  1. How are         a) PVC       b) Teflon prepared?
  2. Explain the following with example
  3. a) Inductive effect        b) Resonance effect.
  4. Explain the structure and functions of hemoglobin.
  5. Explain geometrical isomerism of square planar co- ordination complex.
  6. Discuss the postulates of VSEPR theory.
  7. Give any two methods of the separation of racemic mixture.
  8. Explain the properties of primary and secondary valencies of a coordination

compound

  1. a) How will you prepare 250mL of 0.05N NaOH solution (molecular weight-40)
  2. b) What is the amount of H2SO4 required (in grams) to prepare 500mL of

N/10 H2SO4 (molecular weight –98)

  1. What are the properties of ionic and covalent compounds?
  2. Write short notes on a) peptisation       b) polymerisation.
  3. Derive an expression for the half life period for first order reaction from its rate

Expression.

  1. a) Arrange the following in the increasing order of strength of acid giving reasons:

(i) CH3COOH      (ii) CCl3COOH       (iii) CF3COOH       (iv) HCOOH

  1. b) Arrange the following in the increasing order of strength of the base giving

reasons:

(i) NH3                      (ii) CH3NH2           (iii) (CH3)2NH         (iv) (CH3)3N

 

                                                                                             PART C

Answer any four questions.                                                                                 4X10=40

  1. Draw and explain the crystal structures of NaCl and CsCl.
  2. a) Write short notes on Dissociation constant of acids.
  3. b) What is buffer solution? Derive Henderson equation for acidic buffer.
  4. Derive the rate constant for the second order reaction involving same initial concentration of the reactant.
  5. Discuss any three methods of preparation of colloids.
  6. Explain the hybridization in NH3, H2O and BeCl2 and predict the geometry of these molecules.
  7. a) Explain the intermolecular and intramolecular hydrogen bonding.
  8. b) Discuss the application of colloids.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Chemistry Of Materials Question Paper PDF Download”

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      LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 21

SIXTH SEMESTER – April 2009

CH 6608 / 6602 – CHEMISTRY OF MATERIALS

 

 

 

Date & Time: 23/04/2009 / 9:00 – 12:00     Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

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

 

  1. Define coordination number in ionic crystals.
  2. Sketch the unit of fcc and bcc structures.
  3. What is CVD?
  4. Give any two types of thermograms in TGA.
  5. With an example, explain photoluminescence.
  6. Mention any two organic semiconductors.
  7. What is Curie temperature?
  8. Indicate the following as diamagnetic or paramagnetic and give reason.
  • (ii)
  1. Cite any two examples for super conducting oxides.
  2. What are Polarons?

PART – B

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

 

  1. With a neat diagram explain the structure of wurtzite.
  2. Discuss the different types of indices used in crystallography.
  3. What is hexagonal close packed structure? Explain.
  4. Write a note on Czochralski method of crystal growth.
  5. Enlist the applications of SEM.
  6. Derive an expression for intrinsic carrier concentration.
  7. Explain the types of ferroelectric crystals.
  8. Discuss curve point and exchange integral.
  9. Bringout the differences between ferro and ferri magnetic substances.
  10. Discuss Bardeen, Cooper and Schrieffer theory.
  11. Listout the applications of superconducting materials.
  12. Explain the working of (i)    Sodium-sulphur battery

(ii)    Lithium battery

 

PART – C

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

 

  1. Discuss the types and applications of liquid crystals.
  2. What is magnetic susceptibility? How is it determined?
  3. Explain the types of defects in solid state.
  4. Explain the principle and application of TGA and DTA.
  5. a) Tabulate the Bravais lattices in crystal systems with examples.
  6. b) Write briefly on solar energy conversion. (5+5)
  7. Write notes on            any two of the following
  • Meissner effect
  • X-ray diffraction
  • Liquid crystals (5+5)

 

 

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“Loyola College B.Sc. Chemistry April 2009 Analytical Chemistry Question Paper PDF Download”

by

      LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 02

FIRST SEMESTER – April 2009

CH 1502 – ANALYTICAL CHEMISTRY

 

 

 

Date & Time: 20/04/2009 / 1:00 – 4:00       Dept. No.                                                       Max. : 100 Marks

 

 

PART –A

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

  1. Mention the threshold limits of a vapour concentration of mercury, chromic acid, hydrogen sulphide and formaldehyde.
  2. Repeated estimation of the percentage of carbon in a certain organic compound yielded the result, 38.42, 38.02 and 38.22 in three trials. What is the ‘spread’ of the above set of data?
  3. State any two conditions for a good fractionation.
  4. What is meant by partition chromatography?
  5. If 0.4 g of NaOH is dissolved in water to give 500 ml solution what will be molarity of the solution?
  6. Distinguish a primary standard from a secondary standard.
  7. Define ‘Concentration solubility product’.
  8. What are masking agents?
  9. What are the properties measured in TG and DTG methods?
  10. What do you understand by the term ‘reaction interval’ in thermal analysis?

PART – B

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

  1. Describe the calibration of a burette and a volumetric flask.
  2. List out any five advantages of using a standard glass joint apparatus.
  3. Assess the average deviation from the ‘mean’ and also from the ‘median’ of the percentage of chloride obtained in three trials, namely, 24.39, 24.19 and 24.36.
  4. Describe ‘hot filtration’ and give its significance.
  5. Outline the preparation and development of ‘plates’ for a TLC study.
  6. Explain, briefly, the various steps involved in recrystallization of a solid.
  7. What are metallochoromic indicators? Outline the principle and conditions for using such indicators.
  8. Calculate the pH of the solution obtained by mixing 5.0 g of acetic acid and 7.5 g of sodium acetate and making the volume equal to 500 mL. Given: the dissociation constant of acetic acid is 1.75 x 10-5 at 298 K.
  9. Write an account of complexometric titrations.
  10. Find out the solubility of magnesium hydroxide in g L-1 if its solubility product is

1.20 x 10-11 at 25oC.  (Mg = 24, O=16, H=1).

  1. Discuss the factors affecting solubility of precipitates.
  2. Sketch and account for the DTA analysis of calcium oxalatemonohydrate.

 

PART – C

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

 

  1. Write a detailed account of various kinds of determinate and indeterminate errors in analysis.
  2. Discuss the principle, experimental technique and applications of ion-exchange

chromatography.

  1. Write notes on: (i) reduced pressure distillation (ii) electron capture detector in GC.
  2. Discuss the theory of acid-base indicators with two examples.
  3. (i) Describe post precipitation. (ii) How is post precipitation different from coprecipitaion?

(iii) Mention any three requisites of a wash liquid.

  1. Discuss the factors that influence a thermogram.

 

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“Loyola College B.Sc. Chemistry April 2009 Bio Chemistry Question Paper PDF Download”

by

   LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 16

FIFTH SEMESTER – April 2009

CH 5404 / CH 5401 – BIO CHEMISTRY

 

 

 

Date & Time: 30/04/2009 / 1:00 – 4:00       Dept. No.                                                       Max. : 100 Marks

 

 

PART A

Answer all the questions.                                                                                   10 x 2 = 20

  1. Give any two functions of the nucleus.
  2. How is glycine prepared by Strecker synthesis?
  3. Define catabolism.
  4. How is C-terminal of an amino acid determined?
  5. What are coenzymes?
  6. Define iodine number of an oil.
  7. What will happen when glucose and fructose are oxidized by conc. HNO3?
  8. Draw the structure of purine and pyrimidine bases in DNA.
  9. Define oxidative phosphorylation.
  10. Mention any two differences between amylose and amylopectin.

PART B

Answer any eight questions.                                                                                8 x 5 = 40

  1. How is N-terminal of an amino acid determined by Sanger’s method?
  2. Describe the synthesis of glycyl alanine by t-BOC method?
  3. Explain the biosynthesis of fatty acids.
  4. Discuss the b-oxidation theory of fatty acids.
  5. Mention differences between prokaryotic and eukaryotic cells.
  6. What are phosopholipids? How are they classified? Explain.
  7. Discuss the mechanism of electron transport reaction.
  8. Draw and explain the structure of t-RNA.
  9. Briefly explain the replication of DNA.
  10. What is genetic code? Mention any four important characteristics of the genetic code?
  11. Describe the role of hemoglobin in the chemistry of respiration.
  12. What are the factors affecting the enzymatic activity?

PART C

Answer any four questions.                                                                              4 x 10 = 40

  1. What are the different chemical bonds involved in protein structure? Explain.
  2. Define enzyme inhibition. Explain the types of inhibition with examples.
  3. a) Define biological oxidation. Give any five salient features of biological oxidation.
  4. b) Mention any five differences between plant and animal fats. (5+5)
  5. How is glucose converted to pyruvate? Explain.
  6. Draw and explain the citric acid cycle with all the steps involved.
  7. Discuss the biosynthesis of proteins in brief.

 

 

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