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Coordination Compounds

Question
CBSEENCH12011208
Wired Faculty App

The d- electron configurations of Cr3+, Mn2+ , Fe2+, and Co2+ are d4 ,d5, d6 and d7 respectively. Which one of the following will exhibit minimum paramagnetic behaviour?

(At. no. Cr = 24, Mn = 25, Fe =26, Co = 27) 

  • [Fe(H2O)6]2+

  • [Co(H2O)6]2+

  • [Cr(H2O)6]2+

  • [Mn(H2O)6]2+

Solution

B.

[Co(H2O)6]2+


Therefore, [Co(H2O)6]2+ has a minimum number of unpaired electrons and thus, minimum paramagnetic behaviour.

Some More Questions From Coordination Compounds Chapter

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

Write IUPAC name of the following complexes:
(a)    [Fe(H2O)6]SO4
(b)    [Cu(en)2(NO3)2

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