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Coordination Compounds

Question
CBSEENCH12011327
Wired Faculty App

On the basis of the following Eo values; the strongest oxidising agent is

[Fe(CN)6]4- → [Fe(CN)6]3-] +e- ;
Eo = -0.35 V

Fe2+ → Fe3+  +e-; E = -0.77 V

  • [Fe(CN)6]4-

  • Fe2+

  • Fe3+

  • [Fe(CN)6]3-

Solution

C.

Fe3+

Oxidised form + ne- → Reduced Form
The substance which has lower reduction potential are stronger reducing agent while the substances which have higher reduction potential are a stronger oxidising agent.
[Fe(CN)6]3- + e- →[Fe(CN)6]4- ; Eo = 0.35 V
Fe3+ + e- → Fe2+ ;                      Eo = 0.77 V
The reduction potential of Fe3+/ Fe2+ is higher, hence, Fe3+ is a strongest oxidising agent.

Some More Questions From Coordination Compounds Chapter

Indicate the type of isomerism exhibited by the following complexes and draw structures for these isomers:
(i)    K[Cr(H2O)2(C2O4)2],                      (ii) [Co(en)3Cl3,
(iii) [Co(NH3)5(NO2)]|NO3]2,                 (iv) [Pt(NH3)(H2O)Cl2]

Explain on the basis of valence bond theory that [Ni(CN)4]2–  ion with square planar is diamagnetic and the [NiCl4]2– ion with tetrahedral geometry is paramagnetic.

Predict the number of unpaired electrons in the square planar [Pt(CN)4,]2– ion.

The hexaquo manganese(II) ion contains five unpaired electrons, while the hexacynoion contains only one unpaired electron. Explain using crystal field theory.

Calculate the overall complex dissociation equilibrium constant for the Cu(NH3)42+ion, given β4 for this complex is 2.1 x 1013.

Identify the ligands from the following coordination compounds:
(a)    [Co(en)2Cl(NO2)2]
(b)    K[Co(CN)(CO2)(NO)]
(c)    K3[Al(OH)6]
(d)    [Co(H2O)2(NH3)4](OH)3

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