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InterviewSolution
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What can be inferred from the magnetic moment values of the following complex species ?`{:("Example","Magnetic",(BM)),(K_(4)[Mn(CN)_(6)),2.2),([Fe(H_(2)O)_(6)]^(2+),5.3),(K_(2)[MnCl_(4)],5.9):}` |
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Answer» Magnetic moment `(mu)` is given as `mu=sqrt(n(n+2))` For value n = 1, `mu=sqrt(1(1+2))=sqrt(3)=1.732` For value n = 2, `mu=sqrt(2(2+2))=sqrt(8)=2.83` For value n = 3, `mu=sqrt(3(3+2))=sqrt(15)=2.87` For value n = 4, `mu=sqrt(4(4+2))=sqrt(24)=4.899` For value n = 5, `mu=sqrt(5(5+2))=sqrt(35)=5.92` (i) `K_(4)[Mn(CN)_(6)]` For in transition metals, the magnetic moment is calculated from the spin-only formula. Therefore,b `sqrt(n(n+2))=2.2` We can see from the above calculation that the given value is closest to n=1. Also, in this complex, Mn is in the +2 oxidation state. This means that Mn has 5 electrons in the d-orbital. Hence, we can say that `CN^(−)` is a strong field ligand that causes the pairing of electrons (ii) `[Fe(H_(2)O)_(6)]^(2+)` `sqrt(n(n+2))=5.3` We can see from the above calculation that the given value is closest to n=4. Also, in this complex, Fe is in the +2 oxidation state. This means that Fe has 6 electrons in the d-orbital. Hence, we can say that `H_(2)O` is a weak field ligand and does not cause the pairing of electrons. (iii) `K_(2)[MnCl_(4)]` `sqrt(n(n+2))=5.9` We can see from the above calculation that the given value is closest to n=5. Also, in this complex, Mn is in the +2 oxidation state. This means that Mn has 5 electrons in the d-orbital. Hence, we can say that `Cl^(-)` is a weak field ligand and does not cause the pairing of electrons. |
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