LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2012

CH 1503/CH 1500 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

Date : 02-05-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

Answer ALL questions:                                                                                           10 x 2 = 20 Marks

 

1. State Heisenberg’s Uncertainty Principle.
2. What is meant by Diagonal Relationship? Give an example.
3. Which among the following are ionic compounds i) Sodium Bromide ii) Calcium Fluoride

iii) Carbon tetrachloride iv) Magnesium Oxide.

1. Distinguish Electronegativity from Electron affinity.
2. Define Bond Order.
3.  Mention the bond angle and hybridization of  BF₃.
4. How do you classify solids based on their electrical conductivity?
5. Differentiate Substitutional Alloy from Interstitial Alloy.
6. Give any two examples each of Oxidizing and Reducing agents
7. Classify the following as Bronsted acid or bases i) HCl   ii) NH₃  iii) ⁺NH₄ iv) Cl^–

 

PART – B

Answer any EIGHT questions:                                                                                     (8 x 5 = 40 Marks)

 

1. What are the limitations of Bohr’s theory?
2.  a) State the Modern Periodic law.

1. b) Write the electronic configuration of chromium (z = 24).                                     (3 +2)
2. a) What is meant by Inert Pair effect?
3. b) Distinguish Calcination from Roasting                                     (2+3)
4. Mention the essential criteria for the formation of an ionic bond
5. What is Covalency? Mention the factors which enhance covalency?
6. What are the postulates of Valence Bond Theory. Predict the shape of [PtCl₄]^2- and [NiCl₄]^2-.
7. Arrange the following in increasing Bond order O₂, O₂⁺, O₂^– and  O₂^2-.  Justify your answer.
8. Explain the structure and geometry of XeF₆ molecule based on VSEPR Theory.
9. What is meant by isoelctronic species? Arrange the following ions in the order of

increasing size and justify your answer. Na⁺, Mg²⁺, F^–, Al³⁺ and Si⁴⁺.

 

 

20. Using suitable example distinguish intermolecular hydrogen-bonding from intra

Molecular  hydrogen-bonding? Why is the boiling point of para nitro phenol higher than that of ortho nitro phenol.

21. Classify the following as Monoprotonic acids, Polyprotonic acids, Monoprotonic bases and Polyprotonic bases from the following: i) Hydrofluoric acid ii) Oxalic acid iii) Hydrogen Sulphide iv) Acetic acid v) SO₄^2-.
22. a) Define Acid-Base Behaviour proposed by Usanovich.                                        (2)
23. b) What is meant by Lewis Base? Give any two examples.                         (2+1)

 

PART – C

 

Answer any FOUR questions:                                                                                    (4 x 10 = 40 Marks)

 

23. a) What is the significance of wave function Y and Y²?                        (3)

 

1. b) Explain the term i) Covalent Radius ii) Ionization Potential (4)

 

1. c) What is the oxidation state of: i) Cr in Potassium dichromate
2. ii) Mn inPotassium permanganate iii) Pt in H₂[PtCl₆].                         (3)

 

24. a) What is Born-Lande equation and explain the terms involved.                                            (5)

 

1. b) Explain in brief the factors influencing the magnitude of electronegativity. (5)

 

25. a) Explain in brief the Sidgwick rule of Maximum covalency.                                      (6)

 

1. b) Draw the structure of i) Carbon monoxide ii) Sulphur dioxide iii) Ammonia
2. iv) Phosphorus pentachloride.                                                                                                  (4)

 

26. a) Sketch the Molecular Orbital diagram of Nitrogen molecule and calculate the bond order. (6)

 

1. b) Distinguish Bonding from Anti bonding molecular orbital.                                                      (4)
2. Write notes on:
3.       a) Conditions determining the formation of solid solution.                                                         (5)
4. b) van der walls forces.                                                                 (5)

 

28. a) Give any two examples each of i) Acid-Base reactions   ii) Redox reactions.                          (4)

 

1. b) Discuss the role of liquid Ammonia as a solvent.                                                                       (6)

 

 

 

 

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