Coordination Compounds
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9.31 [Fe(CN)6] 4– and [Fe(H2O)6] 2+ are of different colours in dilute solutions. Why?
9.31 [Fe(CN)6] 4– and [Fe(H2O)6] 2+ are of different colours in dilute solutions. Why?
The colour of the particular complex compound depends on the crystal field splitting energy (CFSE). This CFSE depends on the nature of the ligand attached to the metal atom. In case of [Fe (CN)6]4– and [Fe (H2O)6]2+ the colour differs due to differences in CFSE .
CN- is a strong field ligand so will
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9.30 A solution of [Ni(H2O)6] 2+ is green but a solution of [Ni(CN)4] 2– is colourless. Explain.
9.30 A solution of [Ni(H2O)6] 2+ is green but a solution of [Ni(CN)4] 2– is colourless. Explain.
In case of [Ni (H2O)6]2+ H2O is a weak field ligand, so it does not cause the pairing of the unpaired electron of Ni2+ ion. Thus there is possibility of the intra d-d transition from the d orbital of lower energy to that of higher energy. Thus the light is absorbed from the visible region and compli
Upvote 9.29 [Cr(NH3)6] 3+ is paramagnetic while [Ni(CN)4] 2– is diamagnetic. Explain why?
9.29 [Cr(NH3)6] 3+ is paramagnetic while [Ni(CN)4] 2– is diamagnetic. Explain why?
Overall charge balance in [Cr (NH3)6]3+ complex:
X + 6 (0) = + 3 X = + 3
Cr is in + 3 oxidation state.
Electronic configuration of Cr in + 2 state: 3d3 . Now ammonia is a weak field ligand so it not causes pairing of the unpaired electron and undergoes hybridisation to form 6 sp3d2 hybrid orbitals fill
Upvote 9.28 What is crystal field splitting energy? How does the magnitude of ?o decide the actual configuration of d orbitals in a coordination entity?
9.28 What is crystal field splitting energy? How does the magnitude of ?o decide the actual configuration of d orbitals in a coordination entity?
The difference between the energies of the two set of the d orbitals is called as crystal field splitting energy (CFSE). The degenerate d orbitals split into two levels i.e t2g and eg level due to the presence of the ligands. This splitting of the degenerate orbitals due to the ligand is called as c
Upvote 9.27 What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
9.27 What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
The strong ligands have higher splitting power of d orbitals of the central metal ion, whereas weak ligand has relatively lower splitting power of d orbitals of the central metal ion. The energy difference between t2g and eg sets of d orbitals is CFSE. The strength of the ligands depend on the magni
Upvote 9.26 Draw figure to show the splitting of d orbitals in an octahedral crystal field.
9.26 Draw figure to show the splitting of d orbitals in an octahedral crystal field.
In octahedral complex the splitting of the d orbital will be such a way that the dx2-y2 and dz2 orbitals which face towards the axes along the direction of the ligand will experience more repulsion and will be raised in the energy and the other three orbitals which are directed between the axes are
Upvote 9.25 Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:
(i) [Fe(CN)6] 4–
(ii) [FeF6] 3–
(iii) [Co(C2O4)3] 3–
(iv) [CoF6] 3–
9.25 Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:
(i) [Fe(CN)6] 4–
(ii) [FeF6] 3–
(iii) [Co(C2O4)3] 3–
(iv) [CoF6] 3–
(i) In the coordination entity iron exists in + 2 oxidation state. Overall charge balance:
X + 6 (-1) = -4 X = + 2.
Its electronic configuration is: 3d6
CN- is strong field ligand so it causes pairing of the unpaired electron and undergoes hybridisation to form 6 d2sp3 hybrid orbitals to be filled by
Upvote 9.24 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 precipitate of copper sulphide is obtained when H2S(g) is passed through this solution?
9.24 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 precipitate of copper sulphide is obtained when H2S(g) is passed through this solution?
CuSO4 + KCN? K2 [Cu (CN)4] + K2SO4
[Cu (H2O)4]2+ + 4CN-? [Cu (CN)4]2- + 4H2O
The coordination entity formed is K2 [Cu (CN)4] .
IUPAC name of the coordination entity is potassium tetracyanocuprate (II). It is a very stable complex. The copper atom present inside the coordination sphere does not separat
Upvote 9.23 Aqueous copper sulphate solution (blue in colour) gives: (i) a green precipitate with aqueous potassium fluoride and (ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.
9.23 Aqueous copper sulphate solution (blue in colour) gives: (i) a green precipitate with aqueous potassium fluoride and (ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.
Copper sulphate exists as [Cu (H2O)4]SO4 . It is blue in colour due to presence of the [Cu (H2O)4]2+ ions.
When KF is added water is replaced by fluoride ion and green colour is due to [Cu (F)4]2- ions.
When KCl is added water is replaced by chloride ion and bright green colour is due to presence of [
Upvote 9.22 Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these optical isomers?
9.22 Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these optical isomers?
There are four different types of ligands present in the complex. So, by fixing the position of 2 ligands we get 2 geometrical isomers and by changing the position of fixed isomer we get one more geometrical isomer.
Since it is tetrahedral complex so it should be optically active . But however it has
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