CBSE Guess > Papers > Important Questions > Class XII > 2013 > Chemistry > Coordination compounds By Mr. R. Srinivas Vasudevamurthy
CBSE CLASS XII
Coordination compounds - 3 Marks Questions
1. Write IUPAC names of the following compounds
a) [Co (NH3 )5 Cl ] Cl2
b) [Cr(NH3 )6 ]3+
c) [Ni(NH3 )6 ] Cl2
d) [CoCl(NO2)(NH3)4 ] Cl
e) [Co(en)2(ONO)2] Cl
f) [Cr(NH3 )5(H2O)]3+
g) K3 [Co(C2O4)3 ]
h) Na3 [Cr(OH)2F4 ]
i) [Co(NH3 )6] [Cr(CN)6 ]
j) [Pt(NH3 )2Cl(NH2CH3)] Cl
k) [Ni(CO)4 ]
l) [CrCl3 (Py)3 ]
2. Write the IUPAC name of ionization isomer of [Co(NH3)5Br ]SO4
3. Write the IUPAC name of linkage isomer of [Co(en)2(ONO)2 ]Cl
4. Write the formula of the following coordination compounds:
a) Tris (ethane-1,2-diamine)cobalt(III)sulphate
b) Amminebromidochloridonitrito-N- platinate(II)
c) Pottasiumtetrachloridopalladate(II)
d) Tetrahydroxozincate5. Explain the following with suitable examples
a) coordination entity
b) ligand
c) coordination number
d) coordination polyhedron
e) homoleptic
f) heterolrptic6. What is meant by unidentate, bidentate and ambidentate ligands? Give two examples each.
7. Give an example of hexadentate ligand.
8. Explain chelation with a suitable example.
9. Write the IUPAC name and indicate the oxidation state,electronic configuration and coordination number of the central metal in the complex [Co (NH3)5 Cl ] Cl2 Also give the primary and secondary valency of the metal. Give the stereochemistry and magnetic moment of this complex.
10. Mention the limitations of valence bond theory.
11. Using valence bond theory, predict the structure and the magnetic behavior of the below given complexes:
a) [Fe(CN)6 ]4-
b) [Fe(CN)6 ]3-
c) [NiCl4]2-
d) [Ni(CN)4]2-
e) [Cr(NH3)6 ]3+
f) [Co(NH3)6 ]3+
g) [Ni(CO)4]
h) [Fe(CO)5]
i) [MnCl4]2-
j) [CoF6 ]3-
k) [Co(en)3]3+
m) [Co(C2O4)3]3-
n) [Mn(CN)6 ]3-
o) [Ni(NH3)6 ]3+
p) [Fe(H2O)6 ]3+
q) [Mn(CN)6 ]4-
r) [FeF6]3-
s) [MnCl6]3-
t) [MnBr4]2-
12. Name two properties of central metal ion which enables it to form stable complex entities.
13. A coordination compound has the formula CoCl3.4NH3. It does not liberate ammonia but gives precipitate of AgCl with AgNO3 solution. Give the structural formula and IUPAC name of the complex.
14. Account for the following:
a) [Fe(CN)6]4- is diamagnetic while [Fe(CN)6]3- is paramagnetic.
b) [NiCl4]2 is tetrahedral while [Ni(CN)4]2- is square planar.
c) Hydrated copper sulphate is colored while anhydrous copper sulphate is colorless.
d) [Ti(H2O)6]3+ become colorless on heating.
e) [Ni(H2O)6]2+ is green while [Ni(CN)4]2- is colorless.
f) [Fe(CN)6]4- and [Fe(H2O)6]2+ show different colors in aqueous solution..
g) [Cr(NH3)6]3+ is paramagnetic while[Ni(CN)4]2- is diamagnetic.
h) Tetrahedral complex do not exhibit geometrical isomerism.
15. What is the difference between inner orbital and outer orbital complexes? Illustrate with one example each.
16. How the given factor affect the stability of complex
a) charge on cation
b) nature of ligand.17. Illustrate the following with an example each:
a) linkage isomerism
b) ionization isomerism
c) coordination isomerism
d) hydrate isomerism
e) geometrical isomerism
f) optical isomerism18. Draw the geometrical isomers of [Co(NH3)3(NO2)3] and label them.
19. Give a chemical test to distinguish between [Co (NH3)5 Cl ] SO4 and [Co (NH3)5 SO4 ] Cl What type of isomerism does they exhibit?
20. Draw the structure of optical isomers of
a) [Co(en)3]3+
b) [Cr(C2O4)3]3-
c) [PtCl2(en)2 ]2+
d) [Cr(NH3)2 Cl2(en)]+
21. Draw the structure of all the isomers (geometrical and optical) of
a) [CoCl2(en)2]+
b) [Co(NH3)2Cl2(en)]+
c) [Co(NH3) Cl (en)2]2+
22. A metal ion Mn+ having d4 configuration combine with three didentate ligand to form a complex compound. Assuming D0>P
i) Draw the diagram showing d orbital splitting during this complex formation.
ii) Write the electronic configuration of the valence electron of the metal Mn+ ion in terms of t2g and eg.
iii) What type of hybridisation will Mn+ ion have?
iv) Draw the structure of isomers exhibited by this complex.23. Draw the figure to show the d orbital splitting in tetrahedral complex.
24. Mention the limitations of crystal field theory.
25. What is spectrochemical series? Explain the difference between strong and weak ligand.
26. Calculate the overall complex dissociation constant of the complex [Cu(NH3)4]2+ b4 for the complex is 2x1013.
27. The spin only magnetic moment of the complex[MnBr4]2- is 5.9B.M. Predict the geometry of the complex.
28. Calculate the spin only magnetic moment of the complex
a) [Fe(CN)6]4-
b) [CoF6]3-
29. Aqueous copper sulphate gives green precipitate with KF(aq) but bright green solution with KCl(aq). Explain these results.
30. What is the coordination entity formed when excess of KCN is ttreated with aqueous copper sulphate. Why is that no precipitate of copper sulphide is formed when H2S is passed through this solution?
31. Give one application each of coordination compounds in
a) analytical chemistry
b) biological system
c) medicine
d) extraction of metal/metallurgy
e) estimation of hardness of water.32. Draw the structures of
a) [Ni(CO)]4
b) [Fe(CO)]5
c) [ Cr(CO)]6
d) [Mn2(CO)]10
e) [Co2(CO)]8. Explain the bonding in metal carbonyls.
Submitted By : Mr. R. Srinivas Vasudevamurthy
Email: [email protected]
