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प्रश्न
[Fe(H2O)6]3+ is strongly paramagnetic whereas [Fe(CN)6]3− is weakly paramagnetic. Explain.
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उत्तर १
In both [Fe(H2O)6]3+ and [Fe(CN)6]3− Fe exists in the +3 oxidation state i.e., in d5 configuration.
| ↑ | ↑ | ↑ | ↑ | ↑ |
Since CN− is a strong field ligand, it causes the pairing of unpaired electrons. Therefore, there is only one unpaired electron left in the d-orbital.
| ↑↓ | ↑↓ | ↑ |
∴ μ = `sqrt(n(n+2))`
= `sqrt(1(1+2))`
= `sqrt3`
= 1.732 BM
On the other hand, H2O is a weak field ligand. Therefore, it cannot cause the pairing of electrons. This means that the number of unpaired electrons is 5.
∴ μ = `sqrt(n(n+2))`
= `sqrt(5(5+2))`
= `sqrt35`
= 6 BM
Thus it is evident that [Fe(H2O)6]3+ is strongly paramagnetic, while [Fe(CN)6]3− is weakly paramagnetic.
उत्तर २
In the presence of CN– (strong field ligand), the 3d-electrons pair up leaving only one unpaired electron. An inner orbital complex with d2sp3 hybridisation is formed. Hence, [Fe(CN)6]3− is weak paramagnetic. In the presence of HO (weak field ligand), the 3d-electrons are not paired, i.e., the hybridisation is sp3 which forms an outer orbital complex having five unpaired electrons; hence, [Fe(H2O)6]3+ is strong paramagnetic.
Notes
Students can refer to the provided solutions based on their preferred marks.
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संबंधित प्रश्न
For the complex [Fe(CN)6]3–, write the hybridization type, magnetic character and spin nature of the complex. (At. number : Fe = 26).
Write the hybridization and magnetic behaviour of the complex [Ni(CO)4].
(At.no. of Ni = 28)
[NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?
Write the hybridisation and magnetic character of [Co(C2O4)3]3–.
(At. no. of Co = 27)
Why is [NiCl4]2− paramagnetic while [Ni(CN)4]2− is diamagnetic? (Atomic number of Ni = 28)
Write the hybridization type and magnetic behaviour of the complex [Ni(CN)4]2−. (Atomic number of Ni = 28)
Write the hybridization and magnetic character of the following complexes:
[Fe(H2O)6]2+
(Atomic no. of Fe = 26)
Which of the following options are correct for \[\ce{[Fe(CN)6]^{3-}}\] complex?
(i) d2sp3 hybridisation
(ii) sp3d2 hybridisation
(iii) paramagnetic
(iv) diamagnetic
Explain why \[\ce{[Fe(H2O)6]^{3+}}\] has magnetic moment value of 5.92 BM whereas \[\ce{[Fe(CN)6]^{3-}}\] – has a value of only 1.74 BM.
Why do compounds having similar geometry have different magnetic moment?
Assertion: \[\ce{[Fe(CN)6]^{3-}}\] ion shows magnetic moment corresponding to two unpaired electrons.
Reason: Because it has d2sp3 type hybridisation.
[Ti(H2O6]3+ T is paramagnetic is nature due to
Low oxidation state of metals in their complexes are common when ligands ______.
Explain [Fe(CN)6]3− is an inner orbital complex, whereas [FeF6]3− is an outer orbital complex.
[Atomic number: Fe = 26]
Given below are two statements:
Statement I: Ferromagnetism is considered as an extreme form of paramagnetism.
Statement II: The number of unpaired electrons in a Cr2+ ion (Z = 24) is the same as that of a Nd3+ ion (Z = 60).
In the light of the above statements, choose the correct answer from the options given below:
