A. Very short answer question
1. How many moles of AgCl will be precipitated when a solution containing one mole of [CoCl(NH3)5]Cl2is treated with an excess of an AgNO3 solution?
2. What is the primary valency of Cr in [Cr(NH3)6]Cl3?
3. What is the coordination number of Cr3+in [Cr(NH3)6]3+ and [CrCl2(NH3)4]+?
4. What is the coordination number of Cu in [Cu(en)2]2+?
5. Will Cr3+ ion form an outer orbital octahedral complex?
6. Can a chromium (III) complex be diamagnetic?
7. How many unpaired electrons does Cu have in [CuCl4]2-?
8. Why are ligands considered to be negative point charges in CFT?
9. Can a low spin state of a d2system exist in a coordination entity?
10. Why is a zinc (II) complex colourless?
B. Short answer questions
1. Will 1 mole of the compound CoCl3.6NH3give the same number of moles of AgCl as PtCl4.5NH3 does when treated with an excess of an AgNO3 solution?
2. Is the electrolyte nature of CoCl3.5NH3the same as that of PtCl4.4NH3?
3. How many moles of HCl will be liberated from one mole of CoCl3.5NH3 when treated with concentrated H2SO4?
4. What is the oxidation state of metal in
a. Na2[PtCl2(NH3)4]
b. K3[Cr(NCS)6]
c. [Co(en)3]Cl3
d. [Pt(gly)2]
e. Na[Co(edta)]
f. [Cr(acac)3]
5. What is the coordination number of Fe in
a. [Fe(acac)3]
b. [Fe(CO)5]
c. [Fe(H2O)2(ox)2]-
6. Can the NH4+ ion act as a ligant? Why?
7. Can the NO3-ion act as N-donor ligand? Why?
8. Give an example of an N, O-donor ligand along with its structure. How many members will the ring, it will form with the metal, have?
9. Give an example of a flexidentate ligand along with its structure. Why it is called a flexidentate ligand?
10. What kind of isomers are the following pairs of compounds?
a. [CrCl(py)5]SO4and [Cr(py)(SO4)]Cl
b. [CrCl(H2O)5]Cl2.H2O and [CrCl2(H2O)4]Cl.2H2O
c. [Co(NH3)5(NO2)]SO4and [Co(NH3)5(ONO)]SO4
d. [Cr(en)3][Co(CN)6] and [Co(en)3][Cr(CN)6]
11. Draw the structure of the geometrical isomers of [Co(en)2(NH3)2]3+.
12. Diagrammatically show one element of symmetry each in the fac- and mer-isomers of an appropriate coordination entity.
13. Why does [CoCl2(en)2]+show cis-trans isomerism but [Co(en)3]3+ does not?
14. Why does cis-[ CoCl2(en)2]+show optical isomerism but trans-[CoCl2(en)2]+does not?
15. Give the configuration of a d6 metal ion in an outer-orbital and in inner-orbital complex. How many unpaired electrons are there in them?
16. Show that the inner-orbital/ outer-orbital situation does nor arise in an octahedral nickel (II) coordination entity.
17. Why the metal ions normally in a spin are free state in a tetrahedral crystal fiels?
18. Why copper (II) coordination entities are coloured but copper (I) entities colourless?
C. Long Answer questions
1. Mention the main reactions of CoCl3.6NH3, CoCl3.5NH3, CoCl3.4NH3 which led to the correct formulation of these compounds.
2. Show how the SCN- ion is an ambidentate ligand but not a bidentate one.
3. A NiSO4 solution, when treated with an excess of concentrated HCl, gives the coordination ion A, and with an excess of a NaCN solution, B. Gives IUPAC names of A and B.
4. Suggest the methods to identify the
a. Ionization isomerism of CoBrSO4.5NH3
b. Hydrate isomerism of CoCl3.6H2O
5. Apply VBT to explain the bonding in [Cr(NH3)6]3+.
6. Explain using VBT, how [CuCl4]2-is tetrahedral whereas [Cu(NH3)4]2+ is square-planar.
7. Show how the magnetic behavior of d4to d7 system in Oh fields can be explained by considering the relative value of the crystal field splitting parameter and the pairing energy for a metal ion.
8. Explain the synergic bonding in metal carbonyls.
9. How are the bonding parameters of the CO molecule changed on being bonded to a metal?
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