Download Q. 1. (a) What is a Difference between a double salt and a complex

Q. 1. (a) What is a Difference between a double salt and a complex.
(b). Explain the following with suitable examples: Homoleptic and Heteroleptic ligands,
Coordination number.
Q. 2. What is meant by unidentate, didentate and ambidentate ligands? Give examples for each.
Q. 3. (a)Specify the oxidation numbers of the metals in the following coordination entities
i.
ii.
iii.
iv.
v.
[Co(H2O)(CN)(en)2]2+
[PtCl4]2–
[Cr(NH 3)3Cl3]
[CoBr2(en)2]+
K3[Fe(CN)6]
Q. 4. (a) Using IUPAC norms write the formulae for the following:
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
x.
xi.
xii.
xiii.
xiv.
xv.
Tetrahydroxozincate(II) ion
pentaamminenitrito-N-cobalt (III)
Potassiumtri(oxalato) chromate (III)
Diamminedichloridoplatinum (II)
Hexaammine cobalt (III) sulphate
Potassiumtetrachloridopalladate (II)
Hexaammineplatinum (IV)
potassiumtetracyanonickelate (II)
Tetrabromido cuprate (II)
pentaamminenitrito-O-cobalt (III)
Tetraammineaquachloridocobalt (III) chloride
Potassiumtetrahydroxozincate (II)
Potassiumtrioxalatoaluminate (III)
Dichloride bis (ethane-1, 2-diamine) cobalt (III)
Tetracarbonylnickel (0)
(b) Write the formulas for the following coordination compounds:
1.
2.
3.
4.
5.
6.
Tetraamminediaquacobalt(III) chloride
Potassium tetracyanonickelate(II)
Tris(ethane–1, 2–diamine) chromium(III) chloride
Amminebromidochloridonitrito-N-platinate(II)
Dichloridobis(ethane–1, 2–diamine)platinum(IV) nitrate
Iron(III) hexacyanoferrate(II)
Q. 5. (a) Write the IUPAC names of the following coordination compounds:
i.
ii.
iii.
[Pt (NH3)4Cl(NO2)]+
K3[Cr (C2O4)3]
[CoCl2 (en) 2]Cl
iv.
v.
vi.
vii.
viii.
ix.
x.
xi.
xii.
xiii.
xiv.
xv.
xvi.
xvii.
xviii.
xix.
xx.
[Co (NH3)5(CO3)]Cl
Hg [Co (SCN)4]
[Co (NH3)6)]Cl3
[Co (NH3)5Cl]Cl2
K3 [Fe (CN) 6]
K3 [Fe (C2O4)3]
K2 [PdCl4]
[Pt (NH3)2Cl (NH2CH3)]Cl
[NiCl4]2[Ni (CO) 4]
[Co (en) 3]3+
[Co (NH3)6] Cl3
[Co (NH3)4Cl (NO2)]Cl
[Ni (NH3)6]Cl2
[Mn (H2O)6]+
[Co (en) 3]3+
[Ti(H2O)6]3+
(b) Write the IUPAC names of the following coordination compounds:
i.
ii.
iii.
iv.
v.
vi.
[Co(NH3)6]Cl3
[Co(NH3)5Cl]Cl2
K3[Fe(CN)6]
K3[Fe(C2O4)3]
K2[PdCl4]
[Pt(NH3)2Cl(NH2CH3)]Cl
Q. 6. The oxidation number of cobalt in K[Co(CO)4] is
a.
b.
c.
d.
+1
+3
-1
-3
Q. 7. What is understood by following, explain giving examples:
i.
ii.
iii.
iv.
Linkage Isomerism
Ionization isomerism
Coordination isomerism
Solvate(Hydrate)isomerism
Q. 7. What is understood by geometrical and optical isomers?
Q. 8. Draw all the structures of optical isomers of
a. [CrCl(en)2(NH3)]2+
b. [CrCl2(en)2]+
c.
d.
e.
f.
g.
h.
[Cr(C2O4)3]3[PtCl 2(en)2]+
[CrCl2 (en) (NH3)2]2+
[CoCl (en) 2(NH3)] 2+
K[Cr (H2O) 2(C2O4)2]
[Co(en)3]Cl3
Q. 9. Draw all the structures of geometrical isomers of:
a.
b.
c.
d.
e.
f.
g.
[Pt(NH3)2Cl2]
[ Co(NH3)4Cl2]+
[ CrCl(en)2(NH3)]2+
[ CrCl2 (en) 2] +
[ Pt (NH3) (H2O) Cl2]
[ CoCl (en) 2(NH3)] 2+
[ CrCl2 (en)(NH3)2]2+
Q. 10. Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these will
exhibit optical isomers?
Q. 11. Why is geometrical isomerism not possible in tetrahedral complexes having two different
types of unidentate ligands coordinated with the central metal ion ?
Q. 12. Draw structures of geometrical isomers of [Fe(NH3)2(CN)4]–
Q. 13. Indicate the types of isomerism exhibited by the following complexes and draw the
structures for these isomers:
i.
ii.
iii.
iv.
K[Cr(H2O)2(C2O4)2
[Co(en)3]Cl3
[Co(NH3)5(NO2)](NO3)2
[Pt(NH3)(H2O)Cl2]
Q. 14. Give evidence that [Co(NH3)5Cl] SO4 and [Co(NH3)5SO4]Cl are ionization isomers.
Q. 15. Using VBT Predict the Magnetic behaviour, Hybridization, Shape of following
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
x.
[ Fe (CN)6]4[ Fe F6]3[ Co F6]3[ Co(C2O4)3]3[ Ni(CN)4]2[ NiCl4]2[ Ni (CO)4]
[ Fe (H2O) 6]3+
[ Fe (CN)6]3[ Co (NH3)6] +3
xi.
xii.
[ Ni (NH3)6] +2
[ Ti(H2O)6]3+
Q. 16. Account for the Following:
a. [ Ni (CN)4]2- ion with square planar structure is diamagnetic and the [ NiCl4]2- ion with
tetrahedral structure is paramagnetic .
b. [ NiCl4]2- is paramagnetic while [ Ni (CO)4] is diamagnetic though both are tetrahedral.
c. [ Fe (H2O) 6]3+is strongly paramagnetic while [Fe(CN)6]3- is weakly paramagnetic.
d. [ Co (NH3)6]+3 is an inner orbital complex whereas [Ni(NH3)6]+2 is an outer complex.
e. [ Cr (NH3)6] +3is paramagnetic while [Ni (CN)4]2- is diamagnetic.
f. A solution of [Ni (H2O) 6]2+ is green but a solution of [Ni (CN)4]2- is colourless.
g. [ Fe (CN)6]3- and [Fe(H2O) 6]3+ are of different colours in dilute solutions.
Q. 17. The spin only magnetic moment of [MnBr4]2– is 5.9 BM. Predict the geometry of the
complex ion.
Q. 18. 4. Predict the number of unpaired electrons in the square planar [Pt(CN)4]2– ion.
Q. 19. Draw diagram to show splitting of d – orbital in octahedral crystal field. Explain the two
patterns of filling d4 in octahedral crystal Field.
Q. 20. Draw diagram to show splitting of d – orbital in a tetrahedral crystal field.
Q. 21. The Hexaaquomanganese (II) ion contains five unpaired electrons, while the Hexacyano
manganese (II) ion contains only one unpaired electron. Explain using CFT.
Q. 22. (a)Write down the IUPAC name for each of the following complexes and indicate the
oxidation state, electronic configuration and coordination number. Also give stereochemistry and
magnetic moment of the complex:
i.
ii.
iii.
iv.
K[Cr(H2O)2(C2O4)2]3H2O
[CrCl3(py)3] (v) K4[Mn(CN)6]
[Co(NH3)5Cl]Cl2
Cs[FeCl4]
(b) Give the oxidation state, d orbital occupation and coordination number of the central metal ion
in the following complexes:
i.
ii.
iii.
iv.
K3[Co(C2O4)3]
(NH4)2[CoF4]
cis-[Cr(en)2Cl2]Cl
[Mn(H2O)6]SO4
Q. 23. Explain the bonding in coordination compounds in terms of Werner’s postulates
Q. 24. Discuss the role of coordination chemistry in
a.
b.
c.
d.
Biological systems
Analytical Chemistry
Medicinal Chemistry
metallurgy / Extraction of metals
Q. 25. What is the coordination entity formed when excess of aqueous KCN is added to an
aqueous solution of Copper sulphate? Why is it that no precipitates of Copper sulphide is
obtained when H2S (g) is passed through this solution.
Q. 26. What is spectrochemical series? Explain the difference between a weak field ligand and a
strong field ligand.
Q. 27. What is crystal field splitting energy? How does the magnitude of ∆0 decide the actual
configuration of d-orbital in a coordination entity?
Q. 28. What is meant by stability of a coordination compound in solution? State the factors which
govern stability of complexes.
Q. 29. What is meant the chelate effect? Give an example.
Q. 30. Discuss the nature of Bonding in metal carbonyls.
Q. 31. Multiple choice questions
(a). How many ions are produced from the complex Co(NH3)6Cl2 in solution?
i.
ii.
iii.
iv.
6
4
3
2
(b). Amongst the following ions which one has the highest magnetic moment value?
i.
ii.
iii.
[Cr(H2O)6]3+
[Fe(H2O)6]2+
[Zn(H2O)6]2+
(c). Amongst the following, the most stable complex is
i.
ii.
iii.
iv.
[Fe(H2O)6]3+
[Fe(NH3)6]3+
[Fe(C2O4)3]3–
[FeCl6]3–
Q. 32. What will be the correct order for the wavelengths of absorption in the visible region for
the following: [Ni(NO2)6]4–, [Ni(NH3)6]2+, [Ni(H2O)6]2+ ?