1. What is the coordination number of each type of ions in a rock-salt type crystal structure?
2. Define the term ‘order of reaction’ for chemical reactions.
3. What causes Brownian movement in a colloidal solution?
4. In which one of the two structures, NO2 + and NO2 the bond angle has a higher value?
5. Write the IUPAC name of the following compound:
.
6. Arrange the following compounds in an increasing order of their acid strengths:
(CH3)2 CHCOOH, CH3 CH2 CH (Br) COOH, CH3 CH (Br) CH2 COOH
7. Write a chemical reaction in which the iodide ion replaces the diazonium group
8. Name a substance that can be used as an antiseptic as well as a disinfectant
9. Explain as to why haloarenes are much less reactive than haloalkanes towards nucleophilic
substitution reactions.
OR
Which compound in each of the following pairs will react faster in SN2 reaction with –
OH? Why?
(i) CH3 Br or CH3 I
(ii) (CH3)3 CCl or CH3Cl
10. (a) State the IUPAC name of the following compound:
(b) Complete the following chemical equations:
CH3 CH2 CH=CH2 + HBr Peroxide ……….
11. State Henry’s law correlating the pressure of a gas and its solubility in a solvent and
Mention two applications for the law.
12. A first order decomposition reaction takes 40 minutes for 30% decomposition. Calculate
its t ½ value.
13. What is meant by the ‘rate constant, k’ of a reaction? If the concentration be expressed in
Mol L-1 units and time in seconds, what would be the units for k(i) for a zero order
reaction and (ii) for a first order reaction?
14. Define the following terms in relation to proteins:
(i) Peptide linkage
(ii) Denaturation
15. List the reactions of glucose which cannot be explained by its open chain structure.
16. Assign a reason for each of the following statements:
(i) Ammonia is a stronger base than phosphine.
(ii) Sulphur in vapour state exhibits a paramagnetic behavior.
17. Draw the structures of the following molecules:
(i) SF4
(ii) XeF4
18. What are biodegradable and non-biodegradable detergents? Give one example of each
class.
19. What is semiconductor? Describe the two main types of semiconductors and explain
mechanisms for their conduction.
20. Calculate the temperature at which a solution 54g of glucose, (C6H12O6), in 250g of water
will freeze.
(Kf for water = 1.86 k mol-1kg)
21. What are lyophilic and lyophobic sols? Give one example of each type. Which one of
These two types of sols is easily coagulated and why?
22. State briefly the principles which serve as basis for the following operations in
metallurgy:
(i) Froth floatation process
(ii) Zone refining
(iii) Reining by liquation
23. Write chemical equations for the following processes:
(i) Chlorine reacts with a hot concentrated solution of sodium hydroxide
(ii) Orthophosphorous acid is heated
(iii) PtF6 and xenon are mixed together
OR
Complete the following chemical equations:
(i) Ca3P2(s) + H2O (1)_ …….
(ii) Cu2+ (aq) + NH2 (aq) _……..
(iii) F2 (g) + H2O (1) _…….
24. (a) What is a ligand? Give an example of a bidentate ligand.
(b) Explain as to how the two complexes of nickel, [Ni (CN) 4]2- and Ni (CO)4, have
different structures but do not differ in their magnetic behavior. (Ni = 28)
25. Name the reagents which are used in the following conversions:
(i) A primary alcohol to an aldehyde
(ii) Butan-2-one to butan-2-ol
(iii) Phenol to 2, 4, 6-tribtomophenol
26. Account for the following observations:
(i) pKb for aniline is more than that for methylamine.
(ii) Methylamine solution in water reacts with ferric chloride solution to give a
precipitate of ferric hydroxide.
(iii) Aniline does not undergo Friedel-Crafts reaction.
27. Write the names and structures of the monomers of the following polymers:
(i) Buna-S
(ii) Neoprene
(iii) Nylon-6
28. Conductivity of 0.00241M acetic acid solution is 7.896´ 10-5 Scm-1. Calculate its molar
conductivity in this solution. If 0 m Ù for acetic acid be 390.5 S cm2 mol-1, what
would be its dissociation constant?
OR
Three electrolytic cells A, B and C containing solutions of zinc sulphate, silver nitrate and
copper sulphate, respectively are connected in series. A steady current of 1.5 ampere was
passed through them until 1.45g of silver were deposited at the cathode of cell B. How
long did the current flow? What mass of copper and what mass of zinc were deposited
in the concerned cells? (Atomic masses of Ag = 108, Zn = 65.4, Cu = 63.5)
29. Assign reasons for the following:
(i) The enthalpies of atomisation of transition elements are high.
(ii) The transitions metals and many of their compounds act as good catalyst.
(iii) From element to element the actinoid contraction is greater than the lanthanoid
contraction.
OR
(a) What may be the possible oxidation states of the transition metals with the following d
electronic configuration in the ground state of their atoms:
3d3 4s2, 3d54s2 and 3d64s2. Indicate relative stability of oxidation states in each
case.
(b) Write steps involved in the preparation of (i) Na2 CrO4 from chromite ore and
(ii) K2MnO4 from pyrolusite ore.
30. (a)
(b) Describe the following reactions:
(i) Cannizaro reaction
(ii) Cross aldol condensation
Iii) Etard reaction IV) Stephen reaction V) wurts reaction
OR
(a) How would you account for the following:
(i) Aldehydes are more reactive than ketones towards nucleophiles.
(ii) The boiling points of aldehydes and ketones are lower than of the corresponding acids.
(iii) The aldehydes and ketones undergo a number of addition reactions.
(b) Give chemical tests to distinguish between:
(i) Acetaldehyde and benzldehyde
(ii) Propanone and propanol
