LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

 

DB 03

FIRST SEMESTER – November 2008

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

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. Why orbitals like 1 p and 3 f are not possible?
2. Define inert pair effect. Give an example.
3. State Hume Rothery’s ratio rule.
4. HF is a liquid whereas HCl, HBr and HI are gases at 298k.
5. Define oxidation and reduction in terms of electronic concept.
6. Classify the following as Lewis acids or bases.
7. BF₃ ii) NH₃ iii) Cl^– iv) Zn²⁺
8. Of the following species which has the shortest bond length? NO or NO⁺
9. Give Born – Lande equation for lattice energy.
10. Electron affinities of halogens are high. Give reason.
11. What are bonding and anti bonding orbitals?

 

PART – B

 

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

 

1. Discuss Mulliken Jaffee concept of electronegativity.
2. Differentiate between Zone refining and electrolytic refining
3. What is ( n+l ) rule? Why is 4s orbital is lesser in energy than 3d orbital?                                  (2+3)
4. Discuss the structure of XeF₄ on the basis of VSEPR theory.
5. Draw the molecular orbital energy diagram for CO molecule.
6. Nitrogen molecule is diamagnetic while oxygen molecule is paramagnetic. Explain on the basis of Molecular Orbital diagram.
7. What are clathrates? Give any three applications.                                                                  (2+3)
8. Explain the nature of conductors, insulators and semi conductors using band theory.
9. Explain the terms polarization, polarizing power and polarizability.
10. State giving reasons which cation will have greater polarizing power.

1. Na⁺ or Mg²⁺             ii) Cu²⁺ or Ca²⁺                        iii) Pb²⁺ of Pb⁴⁺

1. What are hard and soft acids and bases? Give examples.
2. Discuss the crystal structure of CsCl.

PART C

 

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

 

1. Define the following and explain their trends in a period and in a group.                             (3 + 7)

1. Electron affinity ii) Ionization energy                ii) Atomic radius

1. Mention the hybridization and bond angle for the following geometries.

1. Octahedral ii) Trigonal planar        ii) Trigonal bipyramidal           iv) Tetrahedral
2. v) Pentagonal bipyramidal

1. Differentiate the following                                                                                                     (2 x 5)

1. Inter and Intramolecular hydrogen bonding with a suitable example.
2. Cubic close packing and hexagonal close packing.

1.  a) What is lattice energy? Discuss the factors affecting lattice energy.                                   (2 + 4)

1. b) State and explain Fajan’s rule.                       (4)

 

27. a) How does inductive effect and resonance effect contribute to the strength of Lewis acids?    (6)
28. b) Discuss the following reactions in liquid ammonia as solvent.
29. i) Acid – Base reaction            ii) Precipitation reaction                                                      (4)

 

28. a)  Explain the hybridization and geometry of SF₄.                                                                        (5)

 

1. b) How are the molecular shapes predicted by Sidgwick – Powell theory?                                 (5)

 

 

 

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