LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – NOV 2006

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

Date & Time : 03-11-2006/1.00-4.00     Dept. No.                                                       Max. : 100 Marks

PART – A

Answer all the questions                                  (10 x 2 = 20)

1. Write the Schrodinger wave equation and discuss the significance of wave function.
2. What is inert pair effect? Explain with an example.
3. Give the electronic configuration of manganese and its variable oxidation states.
4. Which of the following element has higher ionization energy? Give reasons:
   (a) oxygen (b)
5. What is galvanization? What is the role of standard electrode potential in this process?
6. Arrange the following acids in the increasing acid strength with suitable explanation,
   HOCl,          HClO₃,        HClO₂,       HClO₄.
7. What are the differences between roasting and calcination?
8. Write the Lewis dot formula for ammonia molecule and give the number of bonded and lone   pairs of electron.
9. Mention the hybridization and geometry of PCl₅
10. Why the density of ice is lesser than that of water?

PART – B

Answer any eight questions                                 (8 x 5 = 40)

11. Explain a) Heisenberg uncertainity principle b) Hund’s rule of maximum multiplicity.
12. Write short notes on a) froth floatation process b) Van-Arkel process in metallurgy.
13. Explain the diagonal relationship in the periodic table with an example.
14. What is lattice energy? How is it determined for the formation of CaF₂ using Born Haber’s
15. Calculate the electronegativity of carbon (r_C = 0.71 A^o) using Allred –Rochow method.
16. Explain the types of hydrogen bonding and explain any two of its consequences.
17. Discuss the structure of (a) SF₆ (b) COCl₂ using hybridization theory.
18. What is levelling effect? How does HNO₃ behave as a base in concentrated sulphuric acid?    Give the chemical equation.
19. What are clathrates? What are their characteristics?
20. What are conjugate acid base pairs? Give an example.
21. What is symbiosis? Give examples.
22. What are the different types of forces in non-polar molecules?

PART – C

Answer any four questions                                                 (4 x 10 = 40)

23. Describe the role of Ellingham diagram for the reduction of metal oxides

to metals in metallurgy.

24. Explain the structure of the following compounds using VSEPRtheory

(i) SF₄                      (ii) H₂O               (iii) ClF₃              (iv) ICl₄^–

25. Construct a qualitative MO energy level diagram for O₂ Write the MO electronic    configuration and bond order for O₂, O₂⁺, O₂²⁺ O^2-, O₂^2-molecule
26. Discuss fajan’s rule with suitable examples.
27. How does band theory of metals explain the conducting properties of metals and n-type and p-   type semicondctors?
28. Explain HSAB theory. Mention any four applications.

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc.

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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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

           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

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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          LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – April 2009

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

Date & Time: 22/04/2009 / 1:00 – 4:00       Dept. No.                                                       Max. : 100 Marks

PART – A

Answer ALL the questions:                                                             10 x 2 = 20       

1. Define inert-pair effect with an example.
2. State Pauli’s exclusion principle.
3. Among and , which has more electron affinity? Why?
4. is less soluble than Give reason.
5. Calculate the bond order in .
6. Describe the structure of based on VSEPR Theory.
7. Among O-chloro phenol and p-chlorophenol, which is more volatile? Explain.
8. Explain ion dipole – dipole interactions of molecules.
9. Label the following as Acid or base. .
10. What are aprotic solvents? Give two examples.

PART – B

Answer any EIGHT questions:                                                                   8 x 5 = 40

11. Write a note on magnetic separation of ore dressing.
12. (a) Write the Schrodinger wave equation and explain the terms.

(b) What is the significance of wave function?

13. Discuss the diagonal relationship between and .
14. State and explain Fajan’s rules to explain the Covalent character of ionic compounds with examples.
15. Explain the trend in ionisation potential values of elements belonging to Second Period.
16. Apply MO theory and draw MO energy level diagram for ‘NO’ molecule. Calculate bond order.
17. Based on Valence Bond Theory, discuss the geometry of (a) (b) .
18. Explain the structure of (a) (b) using VSEPR Theory.
19. Write a note on clathrates.
20. What are Hume-Rothery rules? What are their significance in the structure of alloys?
21. Balance the following chemical reactions by oxidation number method.

22. Write a note on Lewis theory of acids and bases.

PART – C

Answer any FOUR questions:                                                                     4 x 10 = 40

23. Discuss various factors affecting the formation of ionic compounds with suitable examples.
24. How is electro negativity determined by (a) Pauling Method (b) Mulliken – Jaffe Method.
25. Write electron dot formula for
26. Describe the conditions for the combinations of atomic orbitals to produce Molecular Orbitals.
27. How does band theory explain the conducting properties of metals, Semi-conductor and insulator?
28. Describe the role of liquid ammonia as a solvent for various types of reactions with examples.

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – NOVEMBER 2010

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

Date : 12-11-10                     Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART – A

Answer ALL the questions:                                                                          (10 × 2 = 20 marks)

1. Size of Cl^– ion is greater than that of Chlorine atom – Explain.
2. Define Ionisation energy.
3. What is Aufbau principle?
4. What is inert pair effect?
5. Define bond order.
6. What is Lewis concept of acids and bases?
7. What are interstitial compounds?
8. Explain why O₂ is paramagnetic whereas O₂^2– is diamagnetic.
9. Which is more soluble in water MgSO₄ or BaSO₄? Why?
10. Find the oxidation number of

• Mn in KMnO₄ 2) S in  H₂S₂O₈.

PART – B

Answer any EIGHT questions:                                                                    (8 × 5 = 40 marks)

11. Explain the following processes
12. Smelting  b) Froth floatation.                                                                                              (2+3)
13. Define Electron affinity. Explain its trend across the period and down the group of periodic table.
14. Describe the factors favouring the formation of covalent bond in reference to Fajan’s rule.
15. Explain ‘Ellingham diagrams’.
16. Lithium shows greater resemblance with magnesium than with other alkali metals.
17. What are the postulates and limitations of Valence bond theory?
18. Draw the M.O diagram for NO molecule and explain its magnetic behavior.
19. What do you mean by inter and intra molecular hydrogen bonding?Discuss the effect of H-bonding on melting point and boiling point of substances.
20. What are bonding and antibonding molecular orbitals?

20. Write a note on clathrates.
21. Explain Pearsons’s concept of hard and soft acids. Give examples.
22. Balance the following chemical reaction by ion- electron method

MnO₄^– + C₂O₄^2– à Mn²⁺ + CO₂   (in acidic medium).

PART – C

Answer any FOUR questions:                                                                                (4 × 10 = 40  marks)

23. What is electronegativity? How do you calculate electronegativity on the basis of
24. Pauling’s approach        b) Mulliken’s approach                                                        (2+4+4)

24. Define lattice energy and solvation energy. Describe how lattice energy of ionic solids is evaluated by Born-Haber cycle.

25. Define Hybridisation. On the basis of hybridization discuss the geometry of the following molecules.

• SF₆        2) PCl₅            3) NH₃            4) XeF₄                                                                   (2+8)

26. a) Explain the postulates of VSEPR theory.                                                                                  (6)

1. b) Differentiate between a σ bond and a π bond. With an example.             (4)

27. a) Distinguish between cubic close packing and hexagonal close packing of spheres. (6)

1. b) Give reasons for the following:

1) H₂S is a gas H₂O is a liquid

2) Diamond is a hard substance while graphite is soft.                                                       (4)

27. Describe the following reactions in liquid ammonia giving suitable examples.

1. a) Acid-base reactions
2.    b) Precipitation reactions
3.    c) Complex formation reactions
4. d) Ammonolysis

3LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2011

CH 1503/CH 1500 – CONCEPTS IN INORGANIC CHEMISTRY

Date : 06-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART – A

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

1. What are the possible values of quantum numbers n, l ,m and s for an electron in 3d orbital?
2. The metallic character increases in the order As< Sb <Bi. Substantiate.
3. What would be the effect on lattice energy of increasing the charge on M ⁿ⁺?
4. What is inert pair effect?
5. Explain the shape of beryllium chloride, using the concept of hybridization,
6. He₂ ⁺ exists while He₂ does not. Why?
7. What are London forces?
8. Why is sodium in liquor ammonia blue?.
9. HgO is soluble in HCl but HgS is not. Reason out using HSAB principle.
10. What are aprotic solvents? Give one example.

PART – B

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

11. Describe the method of froth floatation.
12. How is electronegativity expressed using Mulliken-Jaffé and Allred -Rochow scales? Explain.
13. What is electrochemical series? Give one application of this series.
14. State and explain Fajan’s rules.
15. Using VSEPR theory arrive at the structures of XeF₄ and XeF₆ .
16. Explain the factors that affect lattice energy.
17. State and explain isoelectronic principle.
18. Construct the qualitative MO energy level diagram of oxygen and account for its paramagnetism.
19. State and explain Hume – Rothery rules.
20. What are interstitial solid solutions? Explain.
21. What are the characteristics of hard and soft acids and bases?
22. What are leveling and differentiating solvents? Explain with an example for each.

PART – C

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

23.What is an Ellingham diagram? With the help of this diagram, fix the criterion for

1. Reduction of metal oxide by carbon at a given temperature
2. Reduction of oxide X₂O₃ by a metal Y and

iii. Reduction of metal oxide by hydrogen.

24. a) Construct and explain, Born-Haber cycle for determination of lattice energy of sodium chloride. (6)

1. b) What is Born – Lande equation.              (4)

25. Using the molecular orbital diagram, explain the magnetic properties and stabilities of CO and N₂.

26. Write a comparative account of the VB and MO theories of bonding.

27. Distinguish between conductors, semiconductors and insulators on the

basis of band theory.

28. Describe the following reactions in liquid ammonia giving an example for each:
29. Acid-base reactions ii. Precipitation reactions  iii. Complex formation reactions and
30. Ammonolysis.                                                                                                 (10)

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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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