LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc.

LM 03

DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2007

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

Date & Time: 26/04/2007 / 1:00 – 4:00          Dept. No.                                                     Max. : 100 Marks

 

 

 

 

Part A

Answer all the questions.                                                                                      10×2=20

1. State Mulliken’s scale of electro negativity.
2. How are the molecular shapes predicted using Sidgwick-Powell theory?
3. Why is 4s orbital lower in energy than 3d orbital?
4. Which of the following sets of quantum numbers are not allowed?
   1. n = 3, l = 4, m = -1 , s = +1/2
   2. n = 2, l = 2, m = 0 , s = +1/2
5. What is intra molecular hydrogen bonding? Give an example.
6. Calculate the amount of energy required to convert 1.5g of potassium atoms in the gaseous state to form potassium ions. Ionization energy of potassium is 419 kJ mol^-1 and atomic mass of potassium is 39 amu.
7. Why the bond angle of water is reduced to 104° from the normal tetrahedral angle?
8. Give Lewis definition of acid and base with an example.
9. Write the electronic configuration of Mn²⁺ and Al³⁺.
10. Write the expression for Schrodinger wave equation and define the terms involved.

 

Part B

Answer any eight questions.                                                                                  8×5=40

11. Discuss the hybridization of IF₅ with the help of VSEPR theory.
12. Write notes on Zone refining and Mond’s process?
13. Normalize the wave function y = sinx between the limits +p to -p
14. Draw the molecular orbital diagram of CO and calculate the bond order.
15. How is the lattice energy of a solid obtained from Born-Haber cycle?
16. State and explain Fajan’s rules to explain the covalent character in ionic compounds with examples.
17. Discuss the crystal structure of CsCl.
18. Explain symbiosis with examples.
19. Discuss the variation in electron affinity along the period and down the group.

 

 

20. Explain the following:
21. a) Electron affinities of halogens are very high.
22. Ionic radius of K⁺ is smaller than that of Cl^– but both are isoelectronic.
23. MgS is harder than LiCl.
24. Using band theory of metals explain the nature of conductors, insulators and semiconductors.
25. Explain ‘leveling effect’ with two examples.

 

Part C

Answer any four questions.                                                                                 4x 10=40

23. Discuss the salient features of the periods in the modern periodic table.
24. How are the following factors affect the ionization energy
25. a) atomic size b) nuclear charge
    c) screening effect                   d) electronic configuration
26. Draw and explain the molecular orbital diagram of oxygen and calculate the bond order of O₂, O₂^–, O₂^2- and O²⁺.
27. Explain the hybridization of a) SF₄ b) SF₆
28. Draw and explain Ellingham diagram for the reduction of metal oxide by carbon.
29. Discuss the following reactions in liquid ammonia giving two examples of each type:
30. a) acid-base reactions b)ammonolysis
    c)complex formation               d) precipitation reactions

 

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