Engineering Chemistry S Datta

TRANSITION METAL CHEMISTRY 307
5. Give an expression for K ins
and state its significance.
6. Give main postulates of Werner’s theory.
7. What is a ligand?
8. What is co-ordination number?
9. Mention main drawback of co-ordination theory.
10. What are chelate compounds? Give examples.
11. What are inner metallic complexes?
12. What do you mean by ambident ligands?
13. Give examples of each:
(a) Cationic complex (b) Anionic complex.
14. Give an example of bridging ligand complex.
15. Mention the types of isomerism found in complex compounds. Give one example of each type.
16. Show the hybridisation of an octahedral complex.
17. Give the state of hybridisation of a square planar complex.
18. What is the main postulate of CFT?
19. What do you mean by crystal field splitting of d-orbitals?
20. What is CFSE?
21. What is spectrochemical series?
22. What are low spin and high spin complexes?
23. What is the main outcome of CFT?
24. Give some uses of ligands.
25. Calculate the magnetic moment µ for one unpaired electron. [Ans. 1.732 Bµ]
26. Calculate the magnetic moment µ for 2, 3, 4, 5, 6 and 7 unpaired electrons.
[Ans. 2.83; 3.87; 4.9; 5.92; 6.93 and 7.93 Bµ respectively]
EXERCISES
1. State the postulates of Werner’s co-ordination theory and discuss the structure of K 4
Fe(CN) 6
on
the basis of this theory.
2. Explain geometrical and optical isomerisms of octahedral complexes.
3. Discuss the geometrical as well as optical isomerism in complexes with co-ordination number 4
and 6.
4. State the postulates of crystal field theory. On the basis of this theory predict whether the complexes
[CoF 6
] –3 and [Co(NH 3
) 6
] +3 are paramagnetic or diamagnetic.
5. Explain with example the valence bond theory regarding complex molecules.
6. Cite some fields of application of ligands in our daily lives.
7. Give IUPAC nomenclature of the following:
(a) CoCl 2
.6NH 3
, (b) Pt(NH 3
) 2
Cl 2
, (c) [Co(en) 2
Cl 2
] + II
(d) (en)
2Co
NH 2
O 2
IV
Co (en) 2
(e) [Fe(CN) 6
] –3 . (f )[Cr(H 2
O) 5
Cl] 2+ ( g) [Cr(H 2
O) 4
Cl 2
] + (h) [Cr(H 2
O) 6
]Cl 3
(i) [Pt(NH 3
) 4
Cl 2
]Br 2
( j ) [Pt(NH 3
) 4
Br 2
]Cl 2
(k) [Co(NH 3
) 4
Cl 2
]NO 2
8. Draw the structures of the following:
(a) Tetraaquo dihydro aluminium ion.
(b) Ammonium diamine tetrathiocyano chromate (III)
(c) Triamine aquo dichloro cobalt (III) chloride
(d) Sodium hexa nitrito cobaltate (III).