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Questions on coordination chemistry
1-Sketch the structures of isomers Co(en)33+ complex ion to show that they are mirror
images of each other.
2- What are the coordination number and the oxidation state, respectively, of the cobalt
atom in the compound [Co(NH3)5Cl]Cl2?
3- Coordination compounds which contain cyanide, CN-, ligands tend to be yellow
whereas coordination compounds which contain water, H2O, ligands tend to be blue or.
Explain why?
4-Consider the coordination compound, Na3[Co(CN)6]. Would you expect this compound
to be diamagnetic or paramagnetic? Explain your reasoning assuming that the CN- ligand
is a strong-field ligand.
5-What are the oxidation number of the iron atom, coordination number and geometric
shape, respectively, for the complex ion, [Fe(CN)6]4-?
6- For the complex ion, [Co(en)2(OH2)CN]2+, what are the coordination number (C.N.)
and the oxidation number (O.N.) of the central metal atom?
7- The hexaquo manganese(II) ion contains five unpaired electrons, while the hexacyanoion contains only one unpaired electron. Explain, using Crystal Field Theory.
8- 5) Give an example of each of the following:
a. Metal Chelate
b. Low spin complex
c. High spin complex
9- ) Write down the systematic name for each of the following complexes and indicate
the coordination number, oxidation state, of the central ion.
a. K4[Mn(CN)6]
b. [CoCl(NH3)5]Cl2
c. [NiCl(NH3)(en)2]Cl
d. [Cu(NH3)4(H2O)]SO4
10- Co in [CoF6]3- is a high spin complex. Show the distribution of d electrons for Co3+ in
the octahedral d energy level diagram.
11- Using crystal field theory, draw the crystal field d orbital energy level diagram for
each of the following complexes by assigning electrons to 3d orbitals.
[Co(en)2]2+ (square planar)
[FeF6]3- (octahedral)
12- The crystal field splitting energy affects the dorbital occupancy and the magnetic properties of the
complex. Explain with example.
13- What is the relationship between the following two complex ions?
I. [Co(NH3)4(NO2)Cl]+
II. [Co(NH3)4(ONO)Cl]+
14-Calculate the crystal field stabilization energy for the high-spin complex Fe(H2O)63+.
15- Which of the following compounds would be paramagnetic?
a.
b.
c.
d.
Sc(NH3)63+ (high spin)
Zn(OH)42- (tetrahedral)
Co(NH3)63+ (high spin)
Fe(CN)64- (low spin)
-Mark Questions
1. Write the IUPAC name of each of the following complexes. (1 mark
each)
(a) [CrBr(H2O)5]SO4
(b) [Co Cl (en)2 (ONO)] NO3
(c) [Fe(C2O4)3]3(d) [Cr(H2O)5(SCN)]Cl2
(e) Na3[Cr F4(OH)2]
(f) [Pt(NH3)4][PtIICl6]
(g) K4[Fe(CN) ]
h. [RhCl(PPh3)3]
(i) [Ni(CO)4]
(j) [CoCl(en)2(NH3)]2+
(k) [CrCl2(OX)2]3(l) K3[Fe(C2O4)3]
(m) [Pt Cl (NH2CH3) (NH3)2]NO2
n. [CoIIICl(NH3)4(NO2)] [Au(CN)2]
(o) K2[HgI4]
(p) Xe[PtF6]
2. Using IUPAC norms, write the formulae for the following: (1 mark
each)
(a) potassiumtetrachloropalladate(II)
(b) pentaamminenitrito-O-cobalt(III)chloride
(c) tetraaquadichlorochromium(III)chloridedihydrate
(d) bis(ethylenediamine)nitrito-N-thiocyanato-S-cobalt(III)ion
(e) hexaamminechromium(III)sulphate
(f) pentaamminenitrito-N-cobalt (III) chloride
(g) tetrachlorocuprate(II)
h. potassiumtetracyanonickelate(II)
(i) potassiumhexacyanocobaltate(III)
(j) bis(ethylenediamine)nitrito-N-thiocyanato-S-cobalt(III) ion
(k) tetraaquadichlorochromium(III)chloridedihydrate.
3. The equilibrium constants of [Cu(NH3)4]2+ and [Co(NH3)6]3+ are 1.0 x
10-12 and
6.2 x 10-36 respectively. Which compound is more stable and why?
4. Give one use of Ziegler catalyst.
5. Which of these cannot act as a ligand:NH3, H2O, CO, CH4
6. (a) Write the IUPAC name of the ionisation isomer of
[Ni(NH3)5(NO3)]Cl. (1 mark each)
(b) Write the IUPAC name of the linkage isomer of [Co(NH3)5(SCN)] Cl2
(c) Write the IUPAC name of the coordination isomer of [ PtII(NH3)4 ] [
CuCl4 ]
7. What is meant by ‘denticity’?
8. Compare the molar conductivities of the following complexes:
[Pt(NH3)2Cl2] and [Pt(NH3)4][PtIICl6]
9. Name the type of isomerism exhibited by the following isomers:
[PtII(NH3)4][PtCl6] and [PtIV(NH3)4Cl2][PtCl4]
2-Mark Questions
10. Mention four applications of coordination complexes.
11. How will you distinguish [Co(NH3)5 (SO4)] Br and [CoBr(NH3)5] SO4
What kind of isomerism do they exhibit?
12. Which among [Ag(NH3)2]Cl, [Ni(CN)4]2-, [NiCl4]2(i) has square planar geometry and (ii) remains colourless in aqueous
solution.
13. Using valence bond approach, explain the shape and magnetic
behaviour of [Fe(CN)6]3-.
14. Write all isomers of Na[Co(en)2( ox)2]
15. What do the terms ‘inner octahedral’ and ‘outer octahedral’ mean?
16. Explain how [ PtCl2(NH3)2 ] and [ Pt(NH3)6 ] Cl4 will differ in their
electrolytic conductance. Give the hybridization and oxidation states of
Pt in these complexes.
17. Draw the structures of each of the following:
(a) [ Cr(C2O4)3 ] 3(b) [Fe(CO)5]
18. Draw a figure to show the splitting of degenerate d-orbitals in an
octahedral crystal field. How does the magnitude of ?o decide the actual
configuration of d-orbitals in a complex entity?
19. Discuss the nature of bonding in [Ni(CO)4]
20. What is the coordination entity formed when excess of aqueous
KCN is added to an aqueous solution of copper(II) sulphate? Why is it
that no precipitate of copper sulphide obtained when H2S is passed
through this solution?
21. Using valence bond approach, predict the shape of each of the
following: (2 mark each)
(a) [CuCl4]2- (paramagnetic)
(b) [Ni(CN)4]2- (diamagnetic)
(c) [Cu(NH3)4]2+ (diamagnetic)
(d) [Ag(NH3)2]+ (diamagnetic)
(e) [Ni(NH3)6]2+ (paramagnetic)
3-Mark Questions
22. Explain the terms:
(a) ambidentate ligand
(b) chelate complexes
(c) coordination number.
23. (a) A coordination compound has the formula CoCl3.4NH3. It does
not liberate NH3 but forms a precipitate of AgCl on treatment with
AgNO3 solution. Write the structure and IUPAC name of the complex.
(b) Name two properties of the central metal ion which enable it to form
stable complex entities.
(c) The formation of complex compounds finds application in the
extraction of some metals. Furnish one example to support the above
statement
24. Draw the structures of:
(a) cis-dichlorotetracyanochromate(III)
(b) mer-triamminetrichlorocobalt(III)
(c) fac-triaquatrinitrito-N-cobalt(III).
25. Explain the role of coordination compounds in:
(a) medicine
(b) extraction of metals
(c) analytical chemistry
26. Account for the following:
(a) Though CO is a weak Lewis base, yet it forms a number of stable
metal carbonyls.
(b) K3[Fe(CN)6] shows very low paramagnetism while K3[FeF6] is highly
paramagnetic.
(c) Aqueous silver nitrate forms precipitate with [Co(NH3)6] Cl2 but does
not form precipitate with [Pt(NH3)2Cl2].
27. (a) What are the factors on which the stability of a complex
depends?
(b) Write the IUPAC nomenclature of the K3[Cr(NO)NH3(CN)4] complex
along with its hybridization and structure [K3[Cr(NO)NH3(CN)4], ?=1.73
BM]
(c) With the help of crystal field theory, predict the number of unpaired
electrons in [Fe(CN)6]4- and [Fe(H2O)6]2+ complexes
29. (a) Give the IUPAC name of the ionization isomer of
[Co(H2O)(NH3)4(NO3)]SO4
(b) Explain the meaning of chelate complexes with an example.
30 (a) Draw the geometrical isomers of [Pt(NH3)4Cl2]2+.
(b) Account for the following:
(i) The complex [Co(en)(NH3)4]Cl3 is more stable than
[Co(NH3)6]Cl3.
(ii) In an octahedral complex eg set of d-orbitals is raised in energy
as compared to t2g set.
Last modified: Tuesday, 6 November 2007, 11:51 PM
Questions on Transition metals
Give reasons for the following questions related to transition elements:
1. Transition metals form alloys with other transition metals easily.
2. Melting points of transition metals increase up to the middle of the series
and then decrease.
3. Transition metals and their compounds are good catalysts.
4. Zn, Cd and Hg are softer and volatile metals.
5. Cr and Cu exhibit exceptional electronic configurations.
6. Transition metals have high melting points.
7. Transition metals compounds are mostly coloured.
8. Sc3+ and Zn2+ are colourless in aqueous solutions.
9. Transition metals exhibit variable oxidation states.
10. Transition metal series exhibit fewer oxidation states at their extreme ends. (Sc,
Ti, Cu)
11. Density of zinc is lower than that of copper.
12. Transition metals have high enthalpy of atomisation.
13. Generally speaking, the enthalpies of atomisation and melting points transition
metals of 3d, 4d and 5d series increase steadily down the group
14. Transition metals and their compounds show paramagnetic behaviour.
15. Hydrated copper sulphate is blue where as anhydrous copper sulphate is white.
16. The magnetic moments of the transition metals increase up to the middle of the
series
and then decrease.
17. Transition metals generally form complex compounds.
18. Transition metals form interstitial compounds.
19. The third ionisation enthalpies of Mn & Zn are quite high in comparison to Fe.
20. Zn has little tendency to form complexes.
21. Zn, Cd and Hg are not considered as true transition metals.
22. [Ti(H2O)6]3+ is coloured while [Sc(H2O)6]3+ is colourless.
23. Mn2+ compounds are more stable than Fe2+ compounds towards oxidation to +3
state.
24. The decrease in atomic radius in the case of any d-series is not as large as that in
period 2 or 3.
25. A transition metal exhibits higher oxidation states in oxides and fluorides.
26. The d1 configuration is very unstable in ions of d-Block elements.
27. Scandium(II) is virtually unknown.
28. The magnetic moment of Co3+ is higher than that of Co2+.
29. The lowest oxide of transition metal is basic, the highest is acidic.
30. The densities of post-lanthanoid elements are very high.
31. The atomic sizes of corresponding elements of 4d and 5d series are almost the
same.
32. La3+ and Lu3+ are colourless while rest of lanthanoids are coloured in the solid
as well as in aqueous state.
33. The first-ionisation enthalpies of the 5-d transition elements are higher than those
of
the 4-d metals.
34. Cu+ is diamagnetic whereas Cu2+ is paramagnetic.
35. The ionisation enthalpy of Hf (6th period) is higher than that of Zr (5th period).
36. The most common oxidation state of lanthanoids is +3. However cerium and
europium form additional oxidation states of +4 and +2 respectively.
37. Ce4+ is a good oxidant.
38. Eu2+ is a good reducing agent.
II.
1.
2.
III.
1.
2.
3.
4.
5.
Describe the large scale preparation of:
Potassium dichromate from chromite ore (FeCr2O4).
KMnO4 manufactured from pyrolusite.
Write the chemical reactions involved.
Acidified potassium dichromate with (a) KI solution (b) FeSO4 solution.
Acidified potassium permanganate with (a) oxalate solution (b) Sn2+ solution.
Pr + H2O
Ce + N2
heated
Lu + O2
IV.
Compare the chemistry of actinoids with that of the lanthanoids with special
reference to:
1.
2.
3.
4.
V.
VI.
1.
2.
3.
4.
5.
6.
7.
electronic configuration
oxidation state
atomic sizes
chemical reactivity.
What is lanthanoid contraction? How would you account for it?
What are its important consequences?
Short Questions:
What are transition elements?
What is misch-metal?
Which is more stable – Mn2+ or Mn4+?
What are coinage metals?
Write the outer shell configuration of inner transition metals.
Calculate the magnetic moment of Mn2+.
Draw the structures of , Cr2O72- and CrO42-
8. Name the metal with the highest melting point.
9. Name the actinoid with no 5f electron.
10. Name the lanthanoid with the maximum paramagnetism.
11. What are the uses of lanthanoids?
12. What are transuranic elements?