LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

GH 3

           B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2008

CH 1503 (CONCEPTS IN INORGANIC CHEMISTRY)

 

 

 

Date : 06-05-08                  Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer ALL the questions.                                                                         (10 x 2 = 20 marks)

1. State Heisenberg uncertainity principle.
2. Explain diagonal relationship of elements in the Periodic Table.
3. Write election dot formula for (i) PCl₅ (ii) O₂
4. Describe the structure of XeF₆ using VSEPR theory.
5. What is the relationship between ionization porential of an element and election affinity of an element in favouring the formation of an ionic compound between them?
6. Bromides and iodides have higher lattice energies than expected from theoretical calculations. Give reasons.
7. What are Hume – Rothory rules?
8. Why does ice float in water?
9. Label as acid or base; AlCl₃, HSO₄^–, Ag⁺
10. What are aprotic solvents? Give 2 examples.

 

PART – B

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

1. What are radial and angular wave functions? What information can we get from these functions.
2. How do you determine the electronegativity of elements using Pauling method?
3. Explain with example electrolytic reductions in aqueons and non-aqueous media.
4. How is the lattice energy of a solid determined from Born-Haber cycle?
5. What are Fajan’s rule? How do they help in explaining covalent character of ionic compounds?
6. Using VSEPR theory illustrate the structure of (a) ICl₂^–   (b) XeF₄
7. Draw MO energy diagram for CO molecule. Calculate the bond order in CO molecule.
8. Discuss resonance e^– dot structures of carbonate ion.
9. Discuss the crystal structure of CsCl.
10. Write a note on clathrates.
11. Balance the following chemical reactions by oxidation number method.

(a)

(b)

1. Describe (a) Lux-flood concept  (b) Solvent – system Concept of acid, bases.

 

PART – C

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

1. What are quantum numbers? Explain how they are derived. Describe the significance of quantum numbers.
2. How are the following factors affect the ionization potential of an element?

(a) atomic size (b) nuclear charge   (c) screening effect   (d) electronic configuration.

1. (a) Draw MO energy diagram for NO molecule. Calculate the bond order.

(b) Of the species O₂, O₂⁺, O₂^–, O₂^2-, which will have maximum bond strength? Explain based on MO theory.

1. (a) Explain with two examples, the exception to octet rule.

(b) Discuss the hybridization involved and structure of (i) NH₃   (ii) SF₄

1. (a) How does band theory explain the property of metal, semi-conductor and insulator?

(b) What are types of hydrogen bonding? Explain with examples.

1. What are the characteristic of liq Ammonia as a solvent? Describe any four types of reactions taking place in liq. NH₃ with two examples each.

 

 

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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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