LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 55

FOURTH SEMESTER – APRIL 2008

CH 4501 – INORGANIC CHEMISTRY – II

 

 

 

Date : 29/04/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

            PART-A

Answer all the questions                                                           (10 ´ 2 = 20)

1. What are the basic chemical changes observed in roasting of an ore?
2. Give any two examples for reduction of an oxide ore.
3. Why do d-block elements exhibit variable oxidation states?
4. What happens to the mercuric salt when it acts as a reductant?
5. Write the IUPAC nomenclature of the following complexes.

(i)  K[Ag(CN)₂]  and   (ii)  [Pt(NH₃)₄NO₂Cl]CO₃

6. Define electroneutrality principle.
7. What is induced radioactivity? Give an example.
8. Write the role of moderators in nuclear reactor.
9. Give any two differences between amorphous and crystalline substances.
10. How are silicates classified?

PART-B

Answer any eight questions                                                    (8 ´ 5 = 40)

11. Write a note on Ellingham diagram.
12. What are the various processes used in the concentration of ores? How would you concentrate an ore using froath floatation process?
13. What are transition metals? Discuss their position in the periodic table.
14. How is uranium extracted from its ore?
15. Explain the following with an example.
16. Ionization isomerism
17. Ligand isomerism
18. Explain the postulates of valence bond theory of coordination complexes.
19. What are Magic numbers? What are their importance in the stability of nuclei?
20. Discuss the precipitation and conductivity methods for the study of complexes.
21. Describe the methods involved in the detection of radioactivity?
22. What is meant by nuclear fission? Write a note on chain reaction.
23. Explain the conductance and metallic luster of metals using metallic bond theory.
24. Derive Bragg’s law.

PART-C

Answer any four questions                                                   (4 ´ 10 = 40)

 

23. Explain the different techniques employed for refining of metals.
24. a) Discuss the lanthanide contraction and its consequences. (7)
25. b) Give the equations for the application of Cr(VI) and Mn(VII) as oxidants.                        (3)
26. a) State the postulates of Werner’s theory of coordination compounds. Illustrate with one

example                                                                                                                         (6)

1. b) Calculate EAN of the metals in the following complexes.

(i) K₄[Fe(CN)₆]                                 (ii) [Ni(CO)₄]                           (4)

26. a) What are the assumptions of Crystal field theory? (4)
27. b) Discuss the splitting of d- orbitals in the case of square planar complexes.              (6)
28. Discuss the application of nuclear energy in various fields.
29. a) How will you find the following for fcc and bcc crystals?                                      (6)

• Number of atoms in a unit cell
• Packing fraction
• Coordination number

1. b) Draw and explain (100), (111), (101) and (001) planes.                                           (4)

 

 

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 1

FIRST SEMESTER – APRIL 2008

CH 1500 – INORGANIC CHEMISTRY – I

 

 

 

Date : 03/05/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

                                                                        (10 x 2 = 20 marks)

Answer ALL the questions.

1. What is the relationship between ionization potential of the element and election affinity of an element in formation of an ionic bond between the elements?
2. Is it possible to have anion, Why?
3. What is the shape of ClF₃? Draw the structure.
4. He₂ does not exist. Why?
5. What are clathrates? Give example.
6. The boiling point of HCl is –85.0⁰C while that of HF is + 19.4⁰C. Explain.
7. Label as Acid or Base: Cl^–, BF₃, Ag⁺, AlCl₃.
8. What are aprotic solvents? Give two examples.
9. How do you prepare pernitric acid? Write its structure.
10. What is oleum? How is it prepared?

PART – B

                                                                        (8 x 5 = 40 marks)

Answer any EIGHT questions.

1. Define lattice energy? Explain the factors which affect lattice energy.
2. Discuss the relationship between electronegativity difference and partial covalent character of an ionic compound. What is its effect in molecules?
3. Describe the hybridizations involved and structure of (a) BeF₂         (b) PCl₅
4. Draw MO energy lavel diagram for NO molecule. Calculate the bond order in NC.
5. State VSEPR theory. Explain the structure of ICl₄ using VSEPR theory.
6. Write a note on van der Waal’s forces.
7. What are different types of Hydrogen bonding? Explain their influence on the properties of compounds with proper examples.
8. Explain the Solvent-System concept of an acid and a base. What are its limitations?
9. Discuss any four types of reactions using liquid ammonia as a solvent.
10. How do you prepare (a) N₂O₃    (b) Hyponitrous acid. Discuss their structure.
11. How do you prepare Marshall’s acid from Sulphuric acid? Draw its structure.
12. Give an comparitive account of the hydrides and halides of Nitrogen group elements.

PART – C

                                    (4 x 10 = 40 marks)

Answer any FOUR questions.

1. (a)  For HCl molecule the internuclear distance is 127 pm; actual dipole moment

is 3.44 x 10^-30 coulomb meter. Calculate the percent ionic character of HCl.(5)

(b) How do you determine the lattice energy of an ionic compound using Bon-Haber cycle?    (5)

1. (a)  Draw MO energy level diagram of CO molecule. Calculate the bond order (5)

(b)  Using VSEPR theory, describe the structure of (i) SF₆ (ii) XeF₆                  (5)

1. (a)  Of the species O₂, O₂⁺, O₂^– and O₂^2-, which will have maximum bond strength? Explain. (5)

 

(b) What is the action of heat on

(i) Phosphorus acid        (ii) orthophosphoric acid

(iii) metaphosphoric acid                                                                 (5)

1. (a)  What is band theory of a metal?                                                                    (2)

(b)  How does band theory explain the property of a metal, semiconductor and insulator?                                                                                                                                           (8)

1. (a) Explain conjugate acid – base concept with two examples                            (5)

(b) Write a note on hard and soft acids and basis.

1. (a) Write a note on nitrogen fixation.                                                                  (4)

(b) Complete the following with balanced equation.                                          (6)

• Sulphuric acid + Phosphorus pentachloride ®?

(ii) Potassium persulphate + Con. Sulphuric acid®?

(iii) Zinc + dil. nitric acid®?

 

 

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 01

FIRST SEMESTER – November 2008

CH 1500 – INORGANIC CHEMISTRY – I

 

 

 

Date : 12-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

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

 

1. How does Ionisation potential vary across a period?
2. Arrange the following in the increasing order of ionic character: .
3. Why an anion is always bigger and a cation is always smaller than the parent atom?
4. Calculate the bond order of N₂.
5. Why H₂S is a gas whereas H₂O is a liquid at 298k.
6. What are London forces? Give its origin?
7. Arrange the following acids according to their increasing acid strength with relevant explanation:
8. Give an example each for protic and aprotic solvents.
9. How Caro’s acid can be prepared.
10. Complete the reactions:

 

 

PART – B

Answer any Eight                                                                           (8 x 5 = 40 marks)

 

11. What is Lattice energy? How is it determined for the formation of NaCl using Born Haber cycle.
12. Calculate the electornegativity of Si following allred-rochow procedure. Covalent radius of Si=1.75 Ǎ.
13. Like compounds dissolve in like solvents – comment.
14. Discuss the hybridization and structure of SF₆ and BeF₂.
15. Give the importance of LCAO method.
16. What are clathrates? Explain with an example.
17. What is difference between Valence Band and Conduction band.
18. What is conjugate acid-base pair? Give two examples.
19. Complete the reaction

 

 

 

20. Compare the stability of NH₃ and PH₃.
21. How Hydrazine is prepared? Give any three of its reactions.
22. Write notes on the various allotropic forms of sulphur.

 

 

 

PART – C

Answer any four                                                                             (4 x 10 = 40 marks)

 

23. (a) Discuss Fajan’s rule with suitable examples.

(b) Calculate the lattice energy of sodium chloride using Born-Haber cycle.

Heat of sublimation of sodium (S) = 108.5kJ/ Mol

Dissociation energy of Cl₂(D) = 243.0kJ/ Mol

Ionization energy of sodium (I.E) = 495.2 kJ/Mol

Electron affinity of Chlorine (EA) = -348.3 kJ/ Mol

Enthalpy of formation of NaCl(ΔH_f)=-381.8 kJ/Mol

24. Arrange the following species in the order of increasing order of bond strength and explain:

O₂⁺, O₂^–, O₂ ,O₂ ²⁺, O₂^2-

25. (a). Based on VB theory predict the magnetic property of Oxygen molecule.

(b). Give the preparation, properties and uses of Hydrazine.

26. How does band theory of metals explain the conduction property of metals.
27. Explain HSAB theory. Mention any four applications.
28. Write in detail the properties and structures of various oxides of sulphur.

 

 

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