B.Sc. Chemistry Question paper

“Loyola College B.Sc. Chemistry April 2012 Organic Functional Groups – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2012

CH 3502 – ORGANIC FUNCTIONAL GROUPS – I

 

 

 

Date : 24-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

       Answer all the questions:                                                                                   (10 x 2 = 20 marks)

  1. Vinyl halides are less reactive towards nucleophilic substitution reaction. Why?
  2. Arrange the following bromides in the order of ease of dehydrohalogenation by alc. KOH.

 

 

 

  1. What happens when propanone reacts with CH3MgBr followed by hydrolysis?
  2. Convert aniline to phenol.
  3. Give the IUPAC names of the following ethers:

 

 

  1. What happens when anisole( methoxy benzene) is hydrolysed with HI? Write the reaction.
  2. Identify the compounds A and B:

H2/Pd, BaSO4                         HCN

C6H5COCl  ——————–→  A  ——————–→ B.

 

  1. Two isomeric compounds A and B, with molecular formula C3H6O , form oxime with hydroxyl

amine.  Tollens test is answered by compound B only and iodoform  test is answered by compound

A only. Give the structures of A and B and state reason.

 

  1. What is trans-esterification reaction.

 

  1. Why is α-chloroacetic acid more acidic than chloroacetic acid ?

 

SECTION – B

Answer any eight questions:                                                                                    (8 X 5 = 40 marks)

  1. Explain the reactions involved in the free radical chlorination of methane.
  2. Predict the major product of the following reaction and explain.

(CH3)3 C CH= CH2    + HBr  ————→ ?

  1. Explain Reimer-Tiemann reaction.
  2. Convert phenol to : i). benzaldehyde, ii) benzoic acid.                                           (2.5 + 2.5)
  3. Describe the mechanism of hydroboration-oxidation of propene to 1-propanol.
  4. What happens when tert-butyl methyl ether is hydrolysed using HI? Explain.
  5. Write the mechanism of acid catalysed ring opening of ethylene oxide.
  6. Explain Wittig reaction with a suitable example. Bring out the advantage of this reaction.

 

 

  1. What are the products formed when acetophenone reacts with each of the following compounds?

Write the reactions.

  1. i) LiAlH4 in THF followed by hydrolysis ,        ii) HCN.                                                      (2 x 2.5)
  2. Write a short note on Norrish type I reactions.
  3. Differentiate between maleic and fumaric acids.
  4. Write a brief account on the action of heat on α, β hydroxy acids.

SECTION – C

Answer any four questions:                                                                                     (4 X 10= 40 marks)

  1. a) Describe E1 mechanism with an example.
  2. b) 2, 4 –dinitro chloro benzene undergoes nucleophilic substitution much faster than              Explain your answer.
  3. a) Explain Kolbe’s reaction with mechanism.
  4. b) Carry out the following conversions:
  5. i) (CH3)2 CH CH2OH ——–→  (CH3)3COH
  6. ii) (CH3)3CBr ——————-→    (CH3)2 CH CH2                                                 (2.5 + 2.5)
  7. a) Describe alkoxymercuration and demercuration procedure for the synthesis of ethers

with an example.

  1. b) How are the following compounds prepared from ethylene oxide?
  2. i) butan-1-ol             ii)  2-methoxy ethanol.                                                                        (2+3)
  3. Write a short note on :
  4. a) Michael reaction b) Perkin’s reaction                                                                             (5+5)
  5. Provide any one method to prepare the following compounds.
  6. i) succinic acid ii) cinnamic acid iii) crotonic acid         iv) phenyl acetate
  7. v) phthalic anhydride                                                                                                                      (5 x 2)
  8. Compound A with molecular formula C7H6O on treatment with con.NaOH gives compounds B and
  9. B on oxidation gives back A. A answers Tollens test but not Fehing’s test. Compound C on

acidification gives D (C7H6O2). D gives brisk effervescence with aqueous NaHCO3 and reaction with

ethanol in the presence of dil.H2SO4 gives a sweet smelling compound E. Identify A, B, C, D and E

and write the reactions involved.  Write all possible isomers of A.

 

 

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“Loyola College B.Sc. Chemistry April 2012 Molecular Dynamics Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2012

CH 6606/CH 6600 – MOLECULAR DYNAMICS

 

 

 

Date : 16-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

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

 

  1. Define the terms orbit and orbitals.
  2. Calculate the energy of the photon associated with light of wavelength 3200 Ao.
  3. Define the term degeneracy of an energy level.
  4. What are operators? Give an example.
  5. What are microstates?
  6. Define the term partition function.
  7. Explain internal conversion.
  8. What is quantum yield?
  9. State the Grotthus-Draper’s law of photochemistry.
  10. Define molar extinction coefficient.

 

PART – B

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

 

  1. Explain the difference between classical mechanics and quantum mechanics.
  2. Explain the energy distribution in Black Body radiation.
  3. Explain Zeeman effect.
  4. State the postulates of quantum mechanics.
  5. Explain the significance of eigen functions.
  6. Derive Sackur-Tetrode equation and explain the terms involved.
  7. Discuss the most probable distribution of particles.
  8. Explain the spin-orbit coupling.
  9. Explain the primary and secondary processes in a photochemical reaction.
  10. Radiation of wave length 2500 Ǻ was passed through a cell containing 10 ml of a

solution which was 0.05 molar in oxalic acid and 0.01 molar in uranyl sulphate.   After absorption of

80 Joules of radiation energy, the concentration of oxalic acid was reduced to 0.04 molar.   Calculate

the quantum yield for the photochemical decomposition of oxalic acid at the given wave length.

  1. Explain the kinetics of fast reaction by relaxation techniques.
  2. Discuss the kinetics of photochemical reaction between H2 and Br2.

PART – C

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

 

  1. (i) What are quantum numbers?  Give its significance.

(ii)  A photon of wave length 4000 Ǻ strikes a metal surface, the work function of the

metal being 2.13 eV.   Calculate the energy of the photon in eV.

 

  1. (i) State Pauli’s exclusion principle and explain.

(ii)  Derive the expressions for eigen value and eigen function for a particle in one

dimensional box.

 

  1. Explain the separation of partition functions and its significance.

 

  1. Derive Maxwell-Boltzmann statistics.

 

  1. Explain any two of the following:

(i)    Chemical Actinometers                           (ii)    Fluorescence

(iii)  Chemiluminescence                                 (iv)   Flash photolysis

 

  1. Derive Stern-Volmer equation. Give its applications.

 

 

 

 

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“Loyola College B.Sc. Chemistry April 2012 Mathematics For Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2012

MT 3103 – MATHEMATICS FOR CHEMISTRY

 

 

Date : 28-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 

Part A. Answer all the questions. Each question carries two marks.                               (10 x 2 = 20)

  1. Find  for x = a(+sin ); y = a(1-cos),
  2. Find  if
  3. Evaluate
  4. Evaluate
  5. Prove that
  6. If
  7. If, show that the angle  is 3o approximately
  8. Prove that sinh 3x = 3 sinh x + 4 sinh3 x

 

  1. If the probability of defective bolt is 0.1; find the mean and standard deviation for the distribution of defective bolts in a total of 500.

 

  1. What are the significance of normal distribution.

 

Part B. Any 5 questions only. Each question carries 8 marks.                                          (5 x 8=40)

 

  1. Find the equation of the tangent and normal for y2= 4ax at (at2,2at).

 

  1. Prove that the tangents to the curve y = x2 -5x + 6 at the points (2,0) and (3,0) cut at right angles.

 

  1. Solve (3D2– 4D + 5) y = 3 e2x
  2. Prove that
  3. If x is large, prove that  nearly.
  4. Prove that
  5. Find the standard deviation for the following data:
Age (x) 20-25 25-30 30-35 35-40 40-45 45-50
No of frequencies (f) 170 110 80 45 40 35

 

  1. Ten percent of the tools produced in a certain manufacturing process turn out to be defective. Find the probability that in a sample of 10 tools chosen at random, exactly two will be defective by using (a) Binomial distribution and (b) the Poisson approximation to the binomial distribution.

 

 

 

 

 

 

Part C. Any two questions only. Each question carries 20 marks.                                   (2 x20 = 40)

  • a) Prove that

19) b)  Solve xp + yq = x

 

20)a) Evaluate

20)b) Evaluate

 

21) Find the Fourier series to the function f(x) = in the interval (0,2).

 

 

  • a) Find the maximum or minimum values of xy + 1/x +1/

 

22) b) A family has six children. Find the probability P that there are (a) three boys and three girls and (b) fewer boys than girls.

 

 

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“Loyola College B.Sc. Chemistry April 2012 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

THIRD SEMESTER – APRIL 2012

CH 3503 – MAIN GROUP ELEMENTS & SOLID STATE CHEMISTRY

 

 

 

Date : 26-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. When sodium is shaken with naphthalene in nonaqueous solution, it turns paramagnetic.

Why?

  1. Explain why Mg(OH)2 is a weaker base than NaOH.
  2. What are fullerenes? How are they prepared?
  3. What are aluminates?
  4. How is sodium thiosulphate prepared?
  5. Give the preparation of Caro’s acid.
  6. What happens when dichlorine monoxide is dissolved in water?
  7. What are pseudohalogens? Why are they called so?
  8. Distinguish between amorphous and crystalline solids.
  9. What are Miller indices? Sketch the plane in a cube having Miller indices 110.

 

PART – B

 

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

 

  1. How are peroxides and superoxides formed by s block elements? Comment on their

magnetic properties.

  1. How does Beryllium differ from other elements of Group 2? Discuss the main points of

difference.

  1. How is ozone prepared? Establish its structure.
  2. Apply Wade’s rules to B4H10 and predict the structure.
  3. How is nitric oxide prepared? How does it react with acidified potassium permanganate?
  4. Write a note on three dimensional silicates.
  5. How is orthophosphoric acid prepared? Write its structure.
  6. How is available chlorine in bleaching powder determined?
  7. How are chlorine dioxide and iodine pentoxide prepared?
  8. Draw the projection of unit cells of zinc blende and explain the salient features of its

structure.

  1. Derive Bragg’s equation.
  2. Write a note on Frenkel defects and its consequences.

 

 

PART – C

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

 

  1. What are carbides? How are they classified? Explain with an example for each class.
  2. a) How are organometallic compounds of lithium prepared? Mention their synthetic

applications.                                                                                                                              (6)

  1. b) What happens when alkali metal oxides react with water? How does the basic

strength of hydroxides of alkali metals vary down a group?                                             (4)

  1. a) How are hydrazine and hydrazoic acid prepared?   (5)
  2. b) Give a brief description of sulphides of phosphorus.                                                       (5)
  3. a) Write briefly on bismuth trioxide and pentoxide.    (4)
  4. b) Give a brief account of phosphatic fertilizers.                                                                     (6)
  5. What are interhalogen compounds? How are they classified? Explain the structures

of ClF3 and IF5.

  1. a) Describe any two types of cubic unit cells among the Bravais lattices. Calculate the

number of atoms per unit cell in each case.                                                                          (6)

  1. b) Show that the limiting radius ratio for an octahedral site is 0.414.                              (4)

 

 

 

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“Loyola College B.Sc. Chemistry April 2012 Industrial Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2012

CH 6611/CH 6605 – INDUSTRIAL CHEMISTRY

 

 

 

Date : 23-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

 

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

 

  1. Mention the composition of gobar gas.
  2. List out the characteristics of anthracite coal.
  3. What are mixed fertilizers?
  4. What are the advantages of saccharin as a sugar substitute?
  5. What is break point chlorination?
  6. How is the use of secondary treatment related to COD to BOD ratio?
  7. What is acid rain? How is it caused?
  8. Assigning reasons, list out the conditions for the dilution of wastewater sample in the

determination of its BOD.

  1. How are refractories classified?
  2. What are bonded abrasives?

PART – B

 

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

 

  1. How is calorific value of a fuel determined?
  2. What is meant by knocking in internal combustion engines? How is it related to octane

number?

  1. How is DDT manufactured?
  2. Explain the process of refining and grading of sugar.
  3. How is water softened by lime soda process?
  4. Explain the process of reverse osmosis.
  5. What are the disadvantages of using hard water?
  6. Explain the biochemical effect of carbon monoxide.
  7. How does nitric oxide contribute to the stratospheric ozone depletion? Explain using

equations.

  1. What is enhanced green house effect? Compare the green house effect potentials of

different green house gases.

 

  1. What are the chief constituents of a paint? What are their functions?
  2. Describe the manufacture of carborundum and boron carbide.

 

PART – C

 

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

 

  1. What is meant by cracking process with respect to petroleum industry? How is catalytic

cracking carried out?

  1. Explain with a help of a block diagram, the refining process of crude oil.
  2. Describe the process of production of ethanol from molasses by fermentation.
  3. How is temporary hardness of water determined by EDTA method?
  4. Define COD. How is COD of a sample of wastewater determined?
  5. a) What are primary and secondary explosives? Give an example for each. (5)
  6. b) How 2,4 D manufactured?                                                                                                         (5)

 

 

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“Loyola College B.Sc. Chemistry April 2012 Hydrocarbons And Stereochemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – APRIL 2012

CH 2504/CH 2502 – HYDROCARBONS AND STEREOCHEMISTRY

 

 

 

Date : 16-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

ANSWER ALL THE QUESTIONS:                                                                      (10 x 2 = 20 marks)

 

  1. Give the IUPAC name of CH3-(CH2) 3-CH=CH-(CH2) 3-CH3
  2. What is hyper conjugation effect?
  3. How will you prepare n-butane from ethyl chloride?
  4. Draw the structures of isopentane and neopentane.
  5. How does ethylene react with chlorine in water?
  6. What happens when propene is treated with HBr?
  7. Mention the electrophiles in the sulphonation and Friedel- Craft’s acylation reactions.
  8. Name the products obtained when naphthalene is reduced in presence of Ni.
  9. Draw any two conformational isomers for ethane and name them.
  10. How does conformation differ from configuration?

 

PART – B

Answer any EIGHT Questions:                                                                            (8 x 5 = 40 marks)

 

  1. What is meant by inductive effect? Explain the stabilities of 10, 20 and 30 carbocations using inductive effect.
  2. Discus the type of hybridizations ethane, ethene and ethyne.
  3. What is meant by a) aromatization and b) cracking.
  4. Explain Dieckmann’s cyclization reaction.
  5. What are the two alkenes obtained when neopentyl alcohol is dehydrated? Which of them is the major product and why?
  6. What is peroxide effect? Explain why peroxide effect is observed in the addition of HBr only and not HCl & HI.
  7. Explain ozonolysis reaction with an example.
  8. Explain why OH group is activating and o, p-directing an aromatic electrophilic substitution reaction.
  9. Discuss the mechanism of nitration of benzene.
  10. Discuss the conformational analysis of n-butane.
  11. What is geometrical isomerism? Discuss any two methods of differentiating geometric isomers.
  12. Discuss the relative stabilities of chair and boad conformations of cyclohexane.

 

PART – C

Answer any FOUR Questions:                                                                            (4 x 10 = 40 marks)

 

  1. a) Explain keto-enol tautomerism by taking acetoacetic ester as an example
  2. b) Write the mechanism of keto-enol tautomerism. (5+5)
  3. a) Expalin the mechanism of halogenations of alkanes.
  4. b) Explain Baeyer’s strain theory. (5+5)
  5. a) What is meant by allylic substitution? Give the mechanism of the reaction.
  6. b) Comapre the acid strengths of ethane. Ethylene and acetylene. (5+5)
  7. a) Explain Diels-Alder reaction and mention its synthetic applications.
  8. b) Explain aromaticity of benzene using Huckel’s rule. (5+5)
  9. a) Outline Haworth’s synthesis of naphthalene.
  10. b) Name the products obtained when naphthalene is oxidized with
  11. i) KMnO4      ii) V2O5 iii) CrO3                                                                                                             (5+5)
  12. a) Explain why equatiorial conformation of methylcyclohexane is more stable than the

corresponding axial conformation.

  1. b) What is 1,3-diaxial interaction? (7+3)

 

 

 

 

 

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“Loyola College B.Sc. Chemistry April 2012 General Chemistry For Physics & Maths Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – APRIL 2012

CH 2102 – GENERAL CHEMISTRY FOR PHYSICS & MATHS

 

 

Date : 23-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 

 

Part – B

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

  1. Why do transition elements show variable valencies?
  2. Mention the biological importance of Chlorophyll.
  3. Define inductive effect with an example.
  4. Draw the optical isomers of tartaric acid.
  5. State Raoult’s law.
  6. Draw the structure of testosterone.
  7. What is an auto catalyst? Give an example.
  8. Mention the uses of Buna-S rubber.
  9. What is meant by hyper thyroidism?
  10. How will you prepare polyethylene?

Part – B

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

  1. Draw the geometrical isomers exhibited by square planar complexes.
  2. Calculate EAN of the metal ion in the following complexes.
  3. i) ) [Co(NH3)6] 2+   ii) )  [Fe(CN) 6]4-
  4. Explain the SN1 mechanism of alkyl halides.
  5. Why phenol is more acidic than ethyl alcohol?
  6. How will you distinguish between maleic and fumaric acids?
  7. Describe Beer – Lambert’s law.
  8. Mention any five characteristics of a catalyst.
  9. Write a note on following:
  10. Activation energy b) Grotthus Drapper’s law.
  11. Explain the replication of DNA.
  12. List the application and risks of genetic engineering.
  13. Discuss chain growth and step growth polymerization.
  14. Give the synthesis of PET and give its uses.

Part-C

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

 

  1. a) How is hardness of water determined using EDTA?
  2. b) What is a bidentate ligand? Give an example. (7+3)

 

  1. a) Discuss the optical isomerism exhibited by octahedral complexes.

b)Write Friedel Crafts alkylation reaction with mechanism.                              (6+4)

  1. a) Explain the conformational isomers of n-butane.
  2. How will you determine the pH of a solution by glass electrode?

 

  1. Derive an expression for the rate constant of a second order reaction involving two different reactants.

 

  1. a) Compare thermal and photochemical reaction. b) Give equation for the preparation of following
  2. i) PVC            ii) Buna-S                                                                 (6+4)

 

  1. a) How is poly acrylate synthesized? Mention its uses.
  2. b) Explain the Galvanization method of prevention of corrosion. (5+5)

 

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“Loyola College B.Sc. Chemistry April 2012 General Chemistry II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – APRIL 2012

CH 207 / 209 – GENERAL CHEMISTRY  II

 

 

 

Date : 16-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

Part A

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

 

  1. What are semiconductors?
  2. How are ortho and para-nitrophenols separated?
  3. What is the product obtained by the nitration of naphthalene?
  4. Define chromophores.
  5. Draw the structure of aspirin.
  6. State I law of thermodynamics.
  7. What is the catalyst used in Haber’s process?
  8. State Beer Lambert’s law.
  9. Define entropy.
  10. How is PVC prepared?

 

Part B

Answer any EIGHTquestions:                                                                                          (8 x 5 = 40 Marks)

 

  1. Differentiate inter and intramolecular hydrogen bonding with examples.
  2. Explain lanthanide contraction.
  3. Discuss the mechanism of nitration of furan.
  4. How is congo red prepared?
  5. Discuss the vulcanization of rubber.
  6. State Kohlrausch’s law. Give an example.
  7. Mention any two applications and any two risks of genetic engineering.
  8. Derive rate constant for a first order reaction.
  9. How is nickel estimated by photocolorimetry?
  10. Explain any two methods of prevention of corrosion.
  11. Differentiate homo and heterogeneous catalysis with examples.
  12. Explain the replication of DNA with a neat diagram.

 

Part C

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

 

  1. Explain the optical isomerism in square planar and octahedral complexes.
  2. What are buffer solutions? Derive an expression for Henderson equation for an acidic buffer.
  3. Explain electrophoresis with a suitable diagram.
  4. Define steric acceleration and steric hindrance. Explain with an example for each.
  5. How are the following prepared?

(i) nylon           (ii) terylene      (iii) neoprene               (iv) PVC

  1. Explain in detail the optical isomerism of tartaric acid.

 

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“Loyola College B.Sc. Chemistry April 2012 Fundamentals Of Spectroscopy Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5508 – FUNDAMENTALS OF SPECTROSCOPY

 

 

 

Date : 03-05-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. Arrange the following spectral regions in the increasing order their frequencies (a) UV   (b) IR

(c) X – ray (d) Microwave (e) cosmic rays.

  1. Distinguish between absorption and emission spectrum.
  2. Write the mathematical expression for Beer – Lamberts law.
  3. What is the wavelength of UV, IR regions in the electromagnetic spectrum?
  4. What is finger print region?
  5. How are CH₃CH₂COCH₃ and CH₃CH₂CH₂OH distinguished using IR spectroscopy?
  6. What is coupling constant?
  7. Why TMS is used as a reference in NMR spectroscopy?
  8. Define base peak.
  9. Name the parts of a mass spectrometer.

 

PART – B

 

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

 

  1. Describe the factors that determine the intensity of spectral lines.
  2. Discuss various types of electronic transition with a suitable diagram.
  3. State and explain Frank – Condon principle.
  4. Discuss the instrumentation of photocolorimeter.
  5. Explain Rayleigh and Raman effects.
  6. State Mutual exclusion principle and discuss the geometry of CO₂ and N₂O.
  7. Write any 5 differences between IR and Raman spectrum.
  8. Discuss the instrumentation of NMR spectroscopy.
  9. Explain spin – spin coupling.
  10. How many signals appear in the NMR spectrum of a) toluene b) propyl alcohol   c) acetone
  11.  d) ethyl alcohol    e) acetaldehyde?
  12. Explain nitrogen rule in mass spectrometry.
  13. Write notes on metastable peak.

PART – C

Answer any FOUR questions:                                                                                        (4×10=40 Marks)

 

  1. Explain the following terms with suitable examples.
  2. a) chromophore   b) Bathochromic shift     c) auxochrome.                                                     (10)
  3. Discuss the principle, instrumentation and application of flame Photometry.      (10)
  4. a) Discuss stretching and bending vibrations.                         (5+5)
  5. b) Discuss the selection rules of Raman spectrum.
  6. a) Explain the sampling techniques in IR spectroscopy.    (5+5)
  7. b) Distinguish the following using IR spectra:
  8. i) CH₃CH₂CHO and CH₃COCH₃
  9.    ii) CH₃CONH₂ and CH₃NH₂

iii) C₂H₅OH and C₂H₅Cl.

  1. a) Explain McLafferty rearrangement.    (5+5)
  2. b) Write notes on shielding and deshielding effects.
  3. a) Discuss the basic principles of mass spectrum.    (5+5)
  4. b) Determine the structure of the compound whose m/e values in the mass spectrum

are 100, 85, 71, 57, 43(base) 41, 29 and 27.

 

 

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“Loyola College B.Sc. Chemistry April 2012 Electrochemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2012

CH 4502 – ELECTROCHEMISTRY

 

 

 

Date : 21-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

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

 

  1. Define electromotive series.
  2. What is a primary reference electrode?
  3. Write the relationship between ΔG and  EMF.
  4. What are commercial cells? Give its applications.
  5. What is Van’t Hoff factor?
  6. Define ionic mobility.
  7. Define equivalent conductance at infinite dilution.
  8. What is cell constant?
  9. What is meant by polarisation?
  10. Write down the Ilkovic equation and mention the terms involved in it.

 

PART – B

 

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

 

  1. What is meant by standard electrode potential? How could you determine the standard

electrode potential of Copper electrode?

  1. State Faraday’s law of electrolysis. and explain.
  2. What is the reduction potential of a half-cell consisting of zinc electrode in 0.015M ZnSO4

solution  at 25oC, Eo­­red of zn2+ ½zn -0.763 v.

  1. Explain the principle involved in the precipitation titration by potentiometry.
  2. Derive Nernst equation.
  3. Explain the classification of electrochemical cells with one example for each
  4. A moving boundary experiment was carried out with a 0.01 M solution of KCl

(қ=1.29 Sm-1), using CdCl2 as the indicator electrolyte.  A current of 5.21 mA was passed through the

tube of 0.230 cm2 cross-sectional area.  It was observed that the boundary moved through 4.16 cm in

one hr.   Calculate the mobility of the K+ ion.

  1. Explain the variation of specific conductance with concentration.
  2. How will you determine the solubility of a sparingly soluble salt by conductivity

measurements?

  1. Discuss Debye Huckel theory of strong electrolytes.
  2. Describe how the electrolytic separations of metals are carried out.
  3. State and explain kohlrausch’s law.

 

PART – C

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

 

  1. Explain the following :

(i)   Amalgam electrode

(ii)  Saturated calomel electrode

 

  1. Explain any four applications of EMF.

 

  1. How the pH of a solution can be determined using a glass electrode? Explain.

 

  1. What are concentration cells? Derive an expression for the EMF of a concentration

cell without transference.

 

  1. (i) Discuss Arrhenius theory of electrolytic dissociation.

(ii) How will you determine the transference number by moving boundary method?

 

  1. (i) Explain any two applications of conductivity measurements.

(ii)   Explain the principle of polarography.

 

 

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“Loyola College B.Sc. Chemistry April 2012 Coordination Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2012

CH 6607/CH 6601 – COORDINATION CHEMISTRY

 

 

 

Date : 18-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

 

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

 

  1. Calculate CFSE for [Co(NH3)6]2+ .
  2. Write the oxidation number and coordination number of iron in K3[Fe(CN)6].
  3. Define outer sphere mechanism with an example.
  4. Draw the structure of Fe(CO)5.
  5. What is nephelauxetic effect?
  6. Mention the applications of radiopharmaceuticals.
  7. Define metal template synthesis with a suitable example.
  8. Give the biological role of peroxidase.
  9. What is chelate therapy?
  10. Give an example for non-complementary electron transfer reaction.

PART – B

 

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

 

  1. Write a note on photoredox reactions.
  2. What is Trans effect? Mention its applications.
  3. Among the complex ions [Fe(H2O)6 ]2+and [Fe(H2O)6]3+  which is expected to give greater splitting of d orbitals.
  4. Discuss the structure and function of carboxypeptidase
  5. How does Zeigler Natta Catalyst catalyze the polymerization of ethylene?
  6. State and explain Jahn Teller theorem with a suitable example. What are its consequences?
  7. What are the experimental evidences for metal – ligand overlapping?
  8. [Co(CN)6]3– is diamagnetic but [Co(F)6]3– is paramagnetic. Account for difference in magnetic properties of these two octahedral complexes using CFT.

 

  1. Explain metal template synthesis of Schiff bases with suitable examples.
  2. Discuss the mechanism of inner sphere electron transfer reaction with suitable examples.
  3. Describe the structure and bonding in Metal alkyls      ii. carbenes.
  4. Explain the following apoenzymes   ii. coenzymes.

 

PART – C

 

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

 

  1. What are π–acceptor ligands? Discuss in detail the nature of bonding involved in

Fe3(CO)12   and Cr(CO)6.

  1. Discuss the σ and π metal –ligand bonding in transition metal complexes with reference

to octahedral geometry.

  1. a) Explain invivo and invitro nitrogen fixation.
  2. b) Give the importance of contrast agents in MRI.
  3. a)Explain the 18 electron rule with two examples.
  4. b) Discuss the structure and bonding of ferrocene.
  5. What do you understand by nucleophilic substitution mechanism reactions for

octahedral complexes? Discuss associative and dissociative mechanism of ligand

substitution for octahedral complexes.

  1. a) Giving a neat diagram explain Crystal Field splitting of d orbitals when a transition

metal ion is placed in a tetrahedral field.

  1. b) Discuss the mechanism of hydrogenation of olefins using Wilkinson’s catalyst.

 

 

 

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“Loyola College B.Sc. Chemistry April 2012 Concepts In Inorganic Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2012

CH 1503/CH 1500 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

Date : 02-05-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

Answer ALL questions:                                                                                           10 x 2 = 20 Marks

 

  1. State Heisenberg’s Uncertainty Principle.
  2. What is meant by Diagonal Relationship? Give an example.
  3. Which among the following are ionic compounds i) Sodium Bromide ii) Calcium Fluoride

iii) Carbon tetrachloride iv) Magnesium Oxide.

  1. Distinguish Electronegativity from Electron affinity.
  2. Define Bond Order.
  3.  Mention the bond angle and hybridization of  BF3.
  4. How do you classify solids based on their electrical conductivity?
  5. Differentiate Substitutional Alloy from Interstitial Alloy.
  6. Give any two examples each of Oxidizing and Reducing agents
  7. Classify the following as Bronsted acid or bases i) HCl   ii) NH3  iii) +NH4 iv) Cl–

 

PART – B

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

 

  1. What are the limitations of Bohr’s theory?
  2.  a) State the Modern Periodic law.
  1. b) Write the electronic configuration of chromium (z = 24).                                     (3 +2)
  2. a) What is meant by Inert Pair effect?
  3. b) Distinguish Calcination from Roasting                                     (2+3)
  4. Mention the essential criteria for the formation of an ionic bond
  5. What is Covalency? Mention the factors which enhance covalency?
  6. What are the postulates of Valence Bond Theory. Predict the shape of [PtCl4]2- and [NiCl4]2-.
  7. Arrange the following in increasing Bond order O2, O2+, O2– and  O22-.  Justify your answer.
  8. Explain the structure and geometry of XeF6 molecule based on VSEPR Theory.
  9. What is meant by isoelctronic species? Arrange the following ions in the order of

increasing size and justify your answer. Na+, Mg2+, F–, Al3+ and Si4+.

 

 

  1. Using suitable example distinguish intermolecular hydrogen-bonding from intra

Molecular  hydrogen-bonding? Why is the boiling point of para nitro phenol higher than that of ortho nitro phenol.

  1. Classify the following as Monoprotonic acids, Polyprotonic acids, Monoprotonic bases and Polyprotonic bases from the following: i) Hydrofluoric acid ii) Oxalic acid iii) Hydrogen Sulphide iv) Acetic acid v) SO42-.
  2. a) Define Acid-Base Behaviour proposed by Usanovich.                                        (2)
  3. b) What is meant by Lewis Base? Give any two examples.                         (2+1)

 

PART – C

 

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

 

  1. a) What is the significance of wave function Y and Y2?                        (3)

 

  1. b) Explain the term i) Covalent Radius ii) Ionization Potential (4)

 

  1. c) What is the oxidation state of: i) Cr in Potassium dichromate
  2. ii) Mn inPotassium permanganate iii) Pt in H2[PtCl6].                         (3)

 

  1. a) What is Born-Lande equation and explain the terms involved.                                            (5)

 

  1. b) Explain in brief the factors influencing the magnitude of electronegativity. (5)

 

  1. a) Explain in brief the Sidgwick rule of Maximum covalency.                                      (6)

 

  1. b) Draw the structure of i) Carbon monoxide ii) Sulphur dioxide iii) Ammonia
  2. iv) Phosphorus pentachloride.                                                                                                  (4)

 

  1. a) Sketch the Molecular Orbital diagram of Nitrogen molecule and calculate the bond order. (6)

 

  1. b) Distinguish Bonding from Anti bonding molecular orbital.                                                      (4)
  2. Write notes on:
  3.       a) Conditions determining the formation of solid solution.                                                         (5)
  4. b) van der walls forces.                                                                 (5)

 

  1. a) Give any two examples each of i) Acid-Base reactions   ii) Redox reactions.                          (4)

 

  1. b) Discuss the role of liquid Ammonia as a solvent.                                                                       (6)

 

 

 

 

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“Loyola College B.Sc. Chemistry April 2012 Chemistry Of Materials Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2012

CH 4204 – CHEMISTRY FOR BIOLOGISTS – II

 

 

Date : 19-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

 

Part- A

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

  1. What is a dipeptide? Give an example.
  2. Define isoelectric point of an amino acid
  3. Draw the structure of fructose.
  4. What are fungicides? Give any two examples.
  5. Give the compositions of NPK fertilizers.
  6. What are isomerases? Give an example.
  7. Give an example for the optical specificity of an enzyme.
  8. Define iodine value of a fat.
  9. What are PUFA? Give any two examples.
  10. Draw the structure of papavarine and citral.

Part – B

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

  1. Discuss in detail the primary structure of proteins.
  2. Give any two methods of synthesis of amino acids.
  3. How will you convert a hexose into  pentose?
  1. Give a brief over view of Citric acid cycle.
  1. What are fertilizers? List the importance of the fertilizers.
  2. How are the following synthesized?

(a) 2,4-D          (b) 2,4,5-T

  1. Explain the process of transcription in brief.
  1. What are coenzymes? Explain the significance of coenzymes in enzyme action.
  2. Mention the difference between plant and animal fats.
  3. Define rancidity of a fat? What are the two types of rancidity? Explain.
  4. What are lecithins and cephalins? Explain.
  5. Explain the factors affecting the enzymatic activity.

 

 

Part-C

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

  1. Discuss the classification of proteins based on their function.
  2. Describe in detail the different types of soil
  3. List the uses of insecticides. Give the method of synthesis of the following
  4. a) DDT b)   BHC    c)  Organophosphates                                    (3+4+3)
  5. What is enzyme inhibition? Discuss competitive and non-competitive inhibitions with examples.
  6. a.) Explain the classification of lipids with examples.

b.) Discuss the classification of alkaloids.

  1. Draw and explain the double helical structure of DNA.

 

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“Loyola College B.Sc. Chemistry April 2012 Chemistry For Biologists – II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2012

CH 4204 – CHEMISTRY FOR BIOLOGISTS – II

 

 

Date : 19-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

 

Part- A

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

  1. What is a dipeptide? Give an example.
  2. Define isoelectric point of an amino acid
  3. Draw the structure of fructose.
  4. What are fungicides? Give any two examples.
  5. Give the compositions of NPK fertilizers.
  6. What are isomerases? Give an example.
  7. Give an example for the optical specificity of an enzyme.
  8. Define iodine value of a fat.
  9. What are PUFA? Give any two examples.
  10. Draw the structure of papavarine and citral.

Part – B

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

  1. Discuss in detail the primary structure of proteins.
  2. Give any two methods of synthesis of amino acids.
  3. How will you convert a hexose into  pentose?
  1. Give a brief over view of Citric acid cycle.
  1. What are fertilizers? List the importance of the fertilizers.
  2. How are the following synthesized?

(a) 2,4-D          (b) 2,4,5-T

  1. Explain the process of transcription in brief.
  1. What are coenzymes? Explain the significance of coenzymes in enzyme action.
  2. Mention the difference between plant and animal fats.
  3. Define rancidity of a fat? What are the two types of rancidity? Explain.
  4. What are lecithins and cephalins? Explain.
  5. Explain the factors affecting the enzymatic activity.

 

 

Part-C

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

  1. Discuss the classification of proteins based on their function.
  2. Describe in detail the different types of soil
  3. List the uses of insecticides. Give the method of synthesis of the following
  4. a) DDT b)   BHC    c)  Organophosphates                                    (3+4+3)
  5. What is enzyme inhibition? Discuss competitive and non-competitive inhibitions with examples.
  6. a.) Explain the classification of lipids with examples.

b.) Discuss the classification of alkaloids.

  1. Draw and explain the double helical structure of DNA.

 

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“Loyola College B.Sc. Chemistry April 2012 Chemistry For Biologists – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PLANT BIOLOGY & ADV. ZOOLOGY

THIRD SEMESTER – APRIL 2012

CH 3104 – CHEMISTRY FOR BIOLOGISTS – I

 

 

Date : 28-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

Part A

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

 

  1. What is intermolecular hydrogen bonding? Give an example.
  2. Why the bond angle of water is reduced to 104° when compared with the normal tetrahedral angle?
  3. Calculate the pH of 0.001N HCl.
  4. Define the rate of a reaction.
  5. Mention any two differences between order and molecularity.
  6. Give any two examples for enzymes used in industries.
  7. Draw the resonance structures of phenol.
  8. Define Brownian movement.
  9. How is maleic acid differentiated from fumaric acid?
  10. Why is chlorophenol more acidic than phenol?

 

Part B

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

 

  1. Explain the hybridization and shape of PCl5.
  2. State the postulates of Werner’s theory of coordination compounds.
  3. Draw the structure of chlorophyll and explain any three functions.
  4. Explain any five requirements for a primary standard solution.
  5. Differentiate homogeneous and heterogeneous catalysis with examples.
  6. Derive an expression for the rate constant of a first order reaction.
  7. What is peptisation? Explain with an example.
  8. Explain any two methods for the separation of a racemic mixture.
  9. Discuss the optical isomerism of lactic acid.
  10. Explain the types of polymerization with an example for each.
  11. What is electro-osmosis? Explain.
  12. Explain the vulcanization of rubber in detail.

 

 

 

 

Part C

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

 

  1. Explain the optical isomerism in square planar and octahedral complexes.
  2. What are buffer solutions? Derive Henderson equation for an acidic buffer.
  3. Explain electrophoresis in detail.
  4. Define steric acceleration and steric hindrance. Explain with an example for each.
  5. How are the following prepared?
  6. i) nylon ii) terylene iii) neoprene                iv) PVC
  7. Explain in detail the optical isomerism of tartaric acid.

 

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“Loyola College B.Sc. Chemistry April 2012 Bio Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5404 – BIO CHEMISTRY

 

 

Date : 30-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

Part A

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

 

  1. What is a peptide bond?
  2. Define denaturation of a protein.
  3. Give an example for the geometric specificity of an enzyme.
  4. Mention the significance of enzymes in the kinetics of the reaction.
  5. Define RM value of a fat.
  6. Draw the structure of cholesterol.
  7. Mention the differences between amylose and amylopectin.
  8. What are disaccharides? Give an example.
  9. Mention any two differences between DNA and RNA.
  10. Define genetic code.

 

Part B

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

 

  1. How is Sanger’s method useful for the determination of amino acid sequence?
  2. Mention the differences between plant and animal fats.
  3. Briefly discuss the primary structure of proteins.
  4. What are the factors affecting the enzyme activity? Explain.
  5. What are phospholipids? Explain the types of phospholipids.
  6. Explain the mechanism of electron transport chain.
  7. What is payoff phase? Explain the steps involved.
  8. Discuss briefly the translation process.
  9. Mention any five salient features of biological oxidation.
  10. Draw and explain the replication of DNA.
  11. Define rancidity? Explain the types of rancidity.
  12. Draw and explain the structure of t-RNA.

 

Part C

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

 

  1. Explain the secondary structure of proteins.
  2. What is enzyme inhibition? Explain any two types of enzyme inhibition.
  3. ) Discuss the β-oxidation theory of fatty acids.

b.) Explain the coenzyme action in brief.                                           (5 + 5)

  1. Draw and explain the steps involved in TCA cycle.
  2. Explain in detail the characteristics of enzymes.
  3. Draw and explain the double helical structure of DNA.

 

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“Loyola College B.Sc. Chemistry April 2012 Analytical Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2012

CH 1502/CH 5501 – ANALYTICAL CHEMISTRY

 

 

 

Date : 28-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

 

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

 

  1. Distinguish accuracy from precision.
  2. Mention any two filtration techniques.
  3. Name two drying agents.
  4. Under what conditions distillation under reduced pressure is necessary?
  5. Give any two advantages of thin layer chromatography over paper chromatography.
  6. What is a buffer solution? Give an example.
  7. Write two limitations of volumetric analysis.
  8. Define solubility product.
  9. Sketch the expected thermogram of calcium oxalate monohydrate in TGA.
  10. What is gravimetric factor?

PART – B

 

Answer any EIGHT questions:                                                                                       (8X5=40)

 

  1. Write the differences between co-precipitation and post-precipitation
  2. How will you calibrate pipette and burette?
  3. Find the number of significant figures in the following

(a)6.023X1023  (b) 0.112  (c) 423.6            (d) 3.1X1010   (e) 0.00014

  1. What are the first – aid procedures to be followed in the laboratory
  2. Give the common methods employed to test the purity of the compound
  3. Discuss the applications of Rf value.
  4. Explain the precautions to be carried out during preparing a column.
  5. Enlist the requirements for a good primary standard.
  6. Methyl orange cannot be used for all acid-base titrations. Why?
  7. Give the applications of adsorption indicators.
  8. Discuss the factors that affect solubility.
  9. Sketch the block diagram of DTA apparatus.

 

 

PART – C

 

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

 

  1. a) Discuss the factors that affect the thermogram.

 

  1. b) Write the inferences that could be drawn from DTA.

 

  1. Explain: a) Volhard’s method

 

  1. b) Von Weiman ratio.

 

  1. a) Deduce an expression connecting solubility and Ksp for Ag2CrO4.

 

  1. b) What are metal ion indicators?

 

  1. a) Write the significance of Henderson equations.

 

  1. b) Give the definitions of (i) Normality          (ii) Formality             (iii) ppm      (iv) millimole.

 

  1. Discuss the principle and applications of a) ion exchange chromatography
  2. b) gas chromatography.

 

  1. a) Explain the types of errors. (6)
  2. b) Mention methods of minimizing errors. (4)

 

 

 

 

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“Loyola College B.Sc. Chemistry April 2012 Advanced Maths For Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2012

MT 4204 / 4201 – ADVANCED MATHS FOR CHEMISTRY

 

 

Date : 19-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

Part A (Answer ALL the questions)                                                                       (10×2=20)

  1. Evaluate .
  2. Show that.
  3. Find .
  4. Find.
  5. If are the roots of the equation , then show that are the roots of the equation .
  6. Find the equation whose roots are the roots of with signs changed.
  7. Define Null hypothesis.
  8. Write the normal equations for the curve .
  9. Solve the system of equations 5x–y+6=0 & x-2y+3=0.
  10. Write down Newton backward formula.

Part B (Answer any FIVE questions)                                                                     (5×8=40)

 

  1. Evaluate and .
  2. By changing the order of integration, evaluate .
  3. Find the Laplace transform of
  4. Solve the equation  of which one root is .
  5. If, show that.
  6. Fit a straight line for the following data.
X 1 2 3 4 5 6 7 8 9 10
Y 52.5 58.7 65 70.2 75.4 81.1 87.2 95.5 102.5 108.4
  1. Solve the following equations by Gauss-Seidel method:,, .
  2. Find a root of the equation correct to three decimal places by using bisection method.

 

Part C (Answer any TWO questions)                                                                     (2×20=40)

 

  1. (a) Evaluate  over the region in the first quadrant bounded by the hyperbolas  and  and the circles  and  .

(b) Prove that .                                                                                   (10+10)

 

  1. (a) Find and .

(b) Using Laplace transform solve  given that .

(10+10)

  1. (a) Solve the equation.

(b) Find the condition that the roots of the equation   may be in geometric progression. Hence solve the equation                                                                                                                                                          (10+10)

  1. (a) Obtain the equations of two lines of regressions for the following data.

X  :           65        66        67        67        68        69        70        72

Y  :           67        68        65        68        72        72        69        71

(b) Solve the following system of equations , ,  using Cramer’s rule.                                                                   (10+10)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

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“Loyola College B.Sc. Chemistry Nov 2012 Transition Elements And Nuclear Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2012

CH 5506 – TRANSITION ELEMENTS AND NUCLEAR CHEMISTRY

 

 

 

Date : 03/11/2012             Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. How is (CH3)2 Hg prepared? Mention one of its uses.
  2. Inspite of its high negative electrode potential, chromium is not a reducing agent. Why?
  3. Orbital contributions to magnetic moments of lanthanide ions are significant. Why?
  4. f-f transitions are used for fingerprinting of Ln (III) ions. Account.
  5. Write down the systematic name for each of the following complexes.
  6. a) K[Cr(oxal)2(H2O)2] .3H2O b) [NiCl(en)2(NH3)]Cl
  7. Draw the geometrical and isomers of [RhCl2(en)2]+.
  8. What is K-electron capture?
  9. What are leptons and hardons?
  10. What is critical mass with respect to nuclear fission?
  11. Why 238 U is not suitable for nuclear fission reaction?

 

PART – B

 

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

 

  1. How is potassium dichromate prepared?
  2. Discuss the various oxidations states exhibited by titanium. Which is the most stable oxidation state?
  3. How are lanthanides separated by on exchange method?
  4. What is lanthanide contraction? What are its consequences?
  5. Using VB theory explain the geometry and magnetism of [CoF6]3–and [Co(CN)6]3– .
  6. What is EAN rule ? Which of these complexes obey EAN rule? i.[Zn(NH3)4]2+ ii. [Co(NH3)6]2+.
  7. How are d-orbitals split, when a transition metal ion is placed in an octahedral field?
  8. The half life of 220Rn is 54.5 s. What mass of this nucleus is equivalent to 1 millicurie?
  9. What is binding energy? How is related to the stability of nuclei?
  10. Write a note on shell model of the nucleus.
  11. What type of materials can be used as moderators and coolants in a nuclear reactor? Explain.
  12. How is radioactive dating carried out using carbon-14?

PART – C

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

 

  1. How does tungsten occur in nature? How is the metal extracted?
  2. Write a note on occurrence, isolation and uses of uranium.
  3. Define crystal field stabilization energy. Calculate its value for the following systems and explain.
  4. d5 low spin octahedral ii.d5 high spin octahedral.
  5. What are the basic postulates of valence bond theory of coordination compounds. What are its

limitations?

  1. Explain the functioning of Geiger counter and scintillation counter.
  2. a. Explain the principle and application of neutron activation analysis. (5)
  3. Write a brief note on nuclear reactors in India.                                                                       (5)

 

 

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“Loyola College B.Sc. Chemistry Nov 2012 Thermodynamics Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – NOVEMBER 2012

CH 3504/3500 – THERMODYNAMICS

 

 

Date : 15/11/2012             Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 

 

PART – A

 

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

 

  1. Define isothermal and isobaric processes.
  2. Define the adiabatic process.
  3. What is meant by calorific value?
  4. Define heat of transition.
  5. What is the need for the second law of thermodynamics?
  6. Define the term efficiency of an engine.
  7. State the law of mass action.
  8. What is a homogenous mixture?
  9. Give the Van’t Hoffs isotherm. Explain the terms.
  10. What are the exceptions to third law of thermodynamics?

 

PART – B

 

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

 

  1. Derive Vander Walls equation of state.
  2. Compare Wrev and Wirrev.for an isothermal process.
  3. Derive the Kirchoff’s equation.Give its application.
  4. State Hess’s law of constant heat of summation and explain its application.
  5. For a certain gas Cp = 8.58. J mol-1 Two moles of the gas are expanded adiabatically from an initial

temperature of 20oC to  a final temperature of -45.4oC.   Calculate the work done.

  1. Explain the method for the determination of enthalpy of combustion.
  2. Explain the thermodynamic principle of the working of refrigerator.
  3. Derive the equation for the entropy of mixing of gases at constant temperature.
  4. Derive the relationship between Kp and Kc.
  5. Derive Van’t Hoffs isochore.
  6. Discuss the dissociation of ammonia by applying Le-chatlier principle.
  7. Explain the Nernst heat theorem.

 

 

 

PART – C

 

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

 

  1. a) Explain the postulates of the kinetic theory of gases. (5)
  2. b) Discuss Joule Thompson effect.                                                                      (5)

 

  1. a) Discuss the thermodynamics of Carnot cycle.                                                (5)
  2. b) Explain the bond energy.                                                                                (5)

 

  1. a) Derive Gibbs Helmholtz equation. (5)
  2. b) Discuss the criteria for spontaneous process.                                                  (5)

 

  1. a) Explain the properties of equilibrium constant. (5)
  2. b) Calculate the equilibrium constant for a equilibrium reaction at 310K

whose  DGo  value at this temperature is  30 kJ mol-1.                                    (5)

 

  1. a) Apply law of mass action for the formation of HI. (5)
  2. b) Explain the factors which alter the state of equilibrium for the above

reaction.                                                                                                          (5)

 

  1. a) Explain Lewis Randall formulation of third law. (5)
  2. b) How will you determine the absolute entropy of oxygen gas?                      (5)

 

 

 

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