loyolacollege.edu Chemistry Sample Question Paper : Loyola College

Organisation : Loyola College (Autonomous), Chennai
Exam: M.Sc.Degree Examination
Subject: Chemistry
Year : 2017
Document Type : Model Question Paper
Website : https://www.loyolacollege.edu/
Download Model Question Paper :
Inorganic Chemistry : https://www.pdfquestion.in/uploads/24999-CH1MC02.pdf
Analytical Chemistry : https://www.pdfquestion.in/uploads/24999-CH1MC04.pdf
Biomolecules : https://www.pdfquestion.in/uploads/24999-CH2ES01.pdf

Chemistry Sample Question Paper

M.Sc.Degree Examination
Chemistry First semester
April 2017
16PCH1MC02 / CH 1813

Related : Loyola College Advanced Zoology & Biotechnology Question Paper : www.pdfquestion.in/24995.html

Date: 05-05-2017
Max. : 100 Marks
Time: 09:00-12:00

Concepts In Inorganic Chemistry

Part-A :
Answer ALL questions. : (10 × 2= 20)
1. Calculate the effective nuclear charge felt by the 2p electron of fluorine atom.
2. Why is the second ionization energy of sodium is very high as compared to its first ionization energy?
3. Compare the O-O bond length in O22+ and O2.
4. Predict the type of hybridization in PCl5 and SF6.
5. Differentiate intrinsic and extrinsic semiconductors.
6. What are the different types of close packing in solids?
7. Mention the factors affecting Lattice energy.
8. How are noble gases liquefied?
9. Define acids based on
(i) Bronsted-Lowry (ii) Lux-Flood.
10. What are the characteristics of a hard acid?

Part-B :
Answer any EIGHT questions.: (8 × 5= 40)
11. How does atomic radii vary in a group and period? How is it related with ionization energy and electronegativity?
12. Calculate the electronegativity of carbon using Allred –Rochow procedure ( rC = 0.77Å)
13. How does molecular orbital theory explain the stability and magnetic properties of NO and NO+?
14. How does valence bond theory explain the formation of NH3 molecule?
15. Discuss the structure of ClO4- using hybridization.
16. What do you mean by HOMO and LUMO? Explain with CO as an example..
17. Define radius ratio. Explain its significance.
18. How does lattice energy influence the solubility of an ionic crystal?
19. Explain Kesom forces citing an example.
20. How are solvents classified?
21. What are London forces? How do they affect the properties of noble gases?
22. Account for the fact that [Ni(dmg)2] is formed in ammoniacal medium but neither in NaOH nor in HCl media.

Part-C :
Answer any FOUR questions. :(4 × 10= 40)
23. How does band theory explain the conducting 2ehavior of conductors, insulators and semiconductors?
24. Discuss the postulates of VSEPR theory and apply to the following ions to predict the actual geometry i) CO32- ii) SO42- iii) I3-
25. How does molecular orbital theory explain the formation of HF and N2 molecules?
26. Discuss Fajan’s Rules citing suitable examples.
27. Give a detailed account on the hydrogen bonds, types and their influence on the properties of compounds.
28 . Discuss HSAB principle and the theoretical basis of the same.

Analytical Chemistry

Part-A :
Answer ALL questions. :(10 × 2= 20)
1. Mention the common errors encountered in precipitation titrations.
2. The standard deviation from one set of determinations was 0.250, while from another set, it was found to be 0.650. Is there any significant difference between the precision of these two sets of results? (Table value = 2.3)
3. Define Eddy diffusion.
4. What are the impurities present in the solvents used in HPLC? How are they removed?
5. Mention any two advantages of electrophoresis over other chromatographic techniques.
6. Define autoprotolysis constant of solvents.
7. How is an indicator chosen for a redox titration?
8. What is the role of supporting electrolyte in an electrochemical cell?
9. State the principle of DSC.
10. Mention the principle of nephelometry.

Part-B :
Answer any EIGHT questions. :(8 × 5= 40)
11. What are additive and proportional errors? Explain with suitable examples.
12. Discuss any five factors affecting the fluorescence.
13. What is electro-osmotic flow? Explain its role in electrophoresis.
14. Explain any three types of column packing in HPLC.
15. Discuss the working principle of flame ionization detector witha neat diagram.
16. Describe the significance of partition columns in gas chromatography.
17. Write short notes on the chemical interferences in FES
18. When a monochromatic light is passed through a cell of 1cm length the intensity of the radiation is reduced to 10%. What is the transmittance if the same radiation is passed through a cell of length 8 cm? Calculate the length of a cell in order to have 25% absorbance.
19. How do enzymatic or biochemical electrodes work?
20. How will you estimate copper electrogravimetrically?
21. Explain the classification ofnon aqueous solvents.
22. What is the molarity and molality of a 13% solution by weight of sulphuric acid? Its density is 1.090 g/ml. To what volume should 100 ml of this acid be diluted in order to prepare 1.5 N solution?

Part-C :
Answer any FOUR questions.: (4 × 10= 40)
23a. Draw Jablonski diagram and discuss the phenomena in brief. (5)
b. Analysis of a sample of alloy gave the following % values of iron content. 9.16, 9.14, 9.08, 9.09, 9.12, 9.21, 9.14, and 9.11. Calculate the average and standard deviations.(5)
24. Write a short note on the three methods of sample injection and derivatisation in gas chromatography.
25a. How is fluorimetry used for the determination of codeine and morphine in a mixture?
(6) b. Discuss the solvent delivery system using pumps in HPLC. (4)

Biomolecules And Natural Products

Part-A :
Answer ALL questions. :(10 x 2= 20)
1. Mention the biological importance of cellulose.
2. How is the fatty acid oxidation switched off when the active synthesis of fatty acid is in process?
3. Differentiate between miRNA and siRNA?
4. What is single nucleotide polymorphism?
5. What is the active form of thiamine? Give the coenzyme role of thiamine.
6. Name any two nutrients that play antioxidant role.
7. Briefly write notes on the use of NMR technique in the characterization of N- Methyl groups in Belladine.
8. How does atropine undergo hydrolysis with mild alkali?
9. Identify the product of dehydrogenation of cadinene with sulphur.

Part-B :
Answer any EIGHT questions. :(8 x 5= 40)
11. Discuss the synthesis of sucrose.
12. Why does maltose undergo mutarotation and reduce Tollen’s reagent but sucrose does not?
13. Enumerate the steps involved in the ß-oxidation of fatty acids.
14. Explain the chemical synthesis of DNA by phosphoramidite method.
15. Describe the components of nucleic acid.
16. What are epinephrine and nor-epinephrine? Draw their structure and mention their hormonal activity.
17. How are free radicals formed in a biological system?
18. Write a note on the electronic structure and stability of singlet oxygen.
19. Explain the stereochemistry of cocaine.
20. Describe Zerewitinoff method of determination of active hydrogen.
21. How are the positions of double bonds in cadinene determined using Ruzicka’s method?
22. Using Wagner-Meerwein rearrangement, establish the position of carboxyl group in Abietic acid.

Part-C :
Answer any FOUR questions. : (4 x 10= 40)
23. Describe the steps involved in TCA cycle. Calculate the energetics of TCA cycle.
24. Write a short note on the following. (5+5)
a. catalytic RNA
b. fluorescently labeled nucleotides

25 a. Discuss the mechanism of hormonal activity on biological functions. (6)
b. How is vitamin D produced in the body? (4)
26 a. Describe uric acid cycle. (5)
b. Convert the following