Q. 1. (a) Write the names of the following complexes according to IUPAC system of nomenclature :
(i) [Co (en)2 (ONO) Cl] Cl
(iii) Image no.4
(iv) [(CH3)4 N] [Rh (NH3)2 (SCN)4]
(v) [Pt (NH3) Py Cl Br].
(b) Write the formulae of the following complexes :
(i) Dichlorobis (methylamine) iron (III) chloride;
(ii) Hexaammnine Chromium (II) hexafluorocobaUate (III).
Q. 2. (a) Write all possible isomers for a complex of the type M (AA)2 B2±n.
(b) The compound Ir Br3.4H2O contains only one Cl- ion that will be precipitated immediately upon addition of Ag+ ions. Draw the structure on the basis of Werner’s theory.
(c ) The complex ion [MnBr4]2 and [Ni (CN) 4]2- are found to be paramagnetic and diamagnetic respectively. What is the geometry that can be assigned to these complex ions on the basis of Valence Bond Theory ?
Q. 3. (a) What is green house effect ? How does it affect the global climate ?
(b) A black-coloured compound of manganese (A), when fused with KOH under atmospheric oxygen formed (B), a green coloured compound. (B), on electrolytic oxidation in alkaline medium gave a purple coloured solution (C) which on treatment with cone. H2SO4 gave green oily liquid (D). Identify A to D and give the sequence of reactions.
Q. 4. (a) What happens when (Give chemical equations) ?
(i) A 30% solution of H2O2 is added to an alkalin’e solution of K2CrO4;
(ii) Cuprous Chloride is heated with acetylene,
(iii) CoCI2 is treated with KNO2 in the presence of ace tic acid.
(iv) Xenon and fluorine are mixed in a sealed vessel a 673 K in 1 : 20 ratio.
(b) Explain the industrial preparation of superphosphate of lime.
Q. 5. (a) Complete the following reactions :
(i) AgNO3+KNHz ——————-
(ii) SOCI2+Cs2SO3 ——————-
(iii) NH4NO3+ KNH2 ————–
(iv) CH3COOAg+ SOCI2 —————
(b) How will you distinguish between the following pairs of somers ?
(i) cis and trans [Pt(NH3)zCI2]
(ii) [Co (NH3)5 SO4 ] I and [Co (NH3)51] SO4.
Q. 6. Account for the following :
(i) The density of the third transition seris elements is almost twice that of the second transition series elements.
(ii) Solubility of noble gases in water increases as their atomic number increases.
(iii) Though transition elements possess very, high electrode potential but they are not good reducing agent.
(iv) TiO2 is colourless whereas Ti2O3 is coloured.