LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc.  DEGREE EXAMINATION – CHEMISTRY

LM 12

FOURTH SEMESTER – APRIL 2007

CH 4501  – INORGANIC CHEMISTRY – II

 

 

Date & Time: 24/04/2007 / 9:00 – 12:00         Dept. No.                                                     Max. : 100 Marks

 

 

 

PART- A

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

1. Write the exceptional electronic configuration of any four d-block elements.

1. Calculate the EAN and give the stability of the following complex.

1. i) [Pt Cl ₆ ] ^2-    ii) [Pd (NH₃) ₆ ] ⁴⁺
2. Write a note on hydrate isomerism with example.
3. Give the important oxidation states of lanthanides. How would you

account for them?

5. Calculate the CFSE for octahedral high and low spin d⁴ and d⁶– configurations.
6. How is radius of nucleus calculated?
7. What is meant by carbon dating?
8. What are isotopes and isotones? Give an example to each.
9. What are differences between amorphous and crystalline solids?
10. Show that 1a.m.u. = 1.66´10^-27 Kg = 931.5 MeV

 

PART- B

Answer any EIGHT questions                                                                         (8 ´ 5 = 40)

11. Draw the structures and write the names of all possible isomers of.
12. i) [Co (NH ₃) ₅ (NO₂)] ²⁺        ii) [Cr (SCN) (NH ₃) ₅] Cl ₂
13. a) Explain the colours in the compounds of the following.
14. i) Mn ²⁺ ii) Cr ³⁺ iii) Zn ²⁺                                                                     (2)
15. b) What are chelates? Give its any one application.                                             (3)
16. a) Write a note on Roasting and Calcinations processes. Give their chemical

equations.                                                                                                           (2)

1. b) How is nickel purified by Mond’s process? (3)
2. Discuss the term “dressing” of the ore? Describe any one method carried out for the concentration of the ore.

 

 

15. a) Define the term oxidation and reduction in terms of oxidation number.
16. b) Explain the oxidizing and reducing properties of Fe²⁺ and Fe³⁺
17. Explain the Ellingham diagram for the metal oxides for different elements.

17.How are mesons classified? Why are mesons needed inside the nucleus?

18. Actual mass of ¹²⁷ I nucleus was found to be 126.941 a.m.u. Calculate the binding

energy of this nucleus and predict whether the nucleus is stable or not.

19. Write a note on Geiger- Muller counter.
20. Derive Bragg’s equation for X- ray crystallography.
21. Discuss the structure of CsCl and calculate the number of atoms per unit cell.
22. Draw the (100), (110), (111), and (200) planes in a cubic cell.

 

PART-C

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

 

23. a) Discuss the crystal field splitting in square planar complex. (5)
24. b) Find out hybridization and the value of µ expected for following complex. (5)
25. i) [Fe (CN) ₆]^3- ii) [Pt Cl ₆]^2-
26. a) Explain the optical isomerism in coordination compounds with coordination

number 6.  Discuss any three types.                                                                     (5)

8. b) Describe the any one structure and hybridization of Co₂ (CO) ₈. Do

these compounds obey EAN rule.

25. a) What is lanthanide contraction? Give its causes and consequences? (7)
26. b) Discuss the catalytic properties of transition elements                                (3)

• a) Using band theory, explain the various types of semiconductors. (7)

1. b) Write a note on lattice energy. (3)
2. Discuss the following nuclear processes.
3. a) b⁺ Emission
4. b) Electron capture
5. c) g – Emission
6. Explain the working of a conventional nuclear reactor. What is breeder reactor?

 

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 01

FIRST SEMESTER – APRIL 2007

CH 1500 – INORGANIC CHEMISTRY – I

 

 

Date & Time: 24/04/2007 / 1:00 – 4:00 Dept. No.                                                Max. : 100 Marks

 

 

PART – A

Answer all the questions                                  (10 x 2 = 20)

1. Differentiate electron affinity from electro negativity.
2. Why is an anion always bigger and a cation always smaller in size than the parent atom?
3. Which are readily soluble in water (a) CaCO₃ (b) K₂CO₃? Give reasons.
4. Why is the electron affinity of nitrogen almost zero while that of fluorine is high?
5. Explain why the bond angle in water is less than that of methane?
6. Explain the term covalency. What is the maximum covalency which the element of  fifth group

can exhibit?

7. Name the types of hybridization in (a) SF₆    (b) BeF
8. What are protic and aprotic solvents? Explain with an example.
9. Give any two oxoacids of nitrogen and indicate the oxidation state of nitrogen.
10. How is hydrazine prepared? Mention any two uses.

PART – B

      Answer any eight questions                                 (8 x 5 = 40)

11. Construct Born Haber’s cycle for the formation of NaCl and explain the terms involved in

calculating the lattice energy.

12. Explain the structure of HF and H₂O using valence bond theory.
13. Explain the types of hydrogen bonding and explain any two of its consequences.
14. Discuss the structure of (a) PCl₅ (b) COCl₂ using hybridization theory.
15. What are London forces? How do these originate?
16. Explain the concepts of acids and bases by a) Lewis b) Bronsted- Lowry system.
17. Explain n-type and p-type semicondutors with suitable examples.
18. Write short notes on nitrogen fixation.
19. Explain the anomalous behaviour of oxygen from the rest of the elements in its group.
20. Give the preparation, properties and uses of hydroxylamine.
21. Explain how H₂O₂ acts both as oxidizing and reducing agent with two examples
22. Explain how does O₃ react with a) PbS  b) KI

 

PART – C

 

Answer any four questions                                                 (4 x 10 = 40)

23. (a) Define electronegativity. How is it determined by different scales of  electronegativity?

Explain with examples the factors affecting it.                                                        (2+ 5+3)

24. Construct a qualitative MO energy level diagram for N₂ Write the MO electronic

configuration, bond order and predict the magnetic nature.

25. Explain the postulates of VSEPR theory and explain the structure of
26. a) ClF₃        b) ICl₄^–                                                                             (4+3+3)
27. Write short notes on:    a) leveling effect of solvent    b) symbiosis
28. c)  precipitation reaction in liq. ammonia.                                              (4+3+3)
29. Write short notes on hydrides and halides of
30. Explain the classification of oxides and their properties.

 

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