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प्रश्न
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[FeF6]3−
Explain the structure of [FeF6]3− on the basis of valence bond theory.
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उत्तर
- In this complex, the oxidation state of Fe is +3.
- Orbitals of Fe+3 ion:
- The complex ion [FeF6]3− is explained on the basis of valence bond theory as follows: Iron in this complex is in the +3 oxidation state, so the electronic configuration of Fe3+ is [Ar] 3d5. The fluoride ion (F−) is a weak field ligand and does not cause the pairing of electrons in the d-orbitals.
- As a result, the five 3d electrons in Fe3+ remain unpaired. Since there are six ligands, the geometry of the complex is octahedral, requiring six hybrid orbitals.
- Due to the weak field nature of F−, the complex uses outer d-orbitals (4d) for bonding, resulting in sp3d2 hybridization.
- The [FeF6]3− complex is an outer orbital octahedral complex. Because of the presence of five unpaired electrons, the complex is paramagnetic in nature.
- The sp3d2 hybridized orbitals of Fe are:
Hence, the geometry of the complex is found to be octahedral.
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संबंधित प्रश्न
On the basis of valence bond theory explain the nature of bonding in [CoF6]3 ion.
Explain on the basis of valence bond theory that [Ni(CN)4]2− ion with square planar structure is diamagnetic and the [NiCl4]2− ion with tetrahedral geometry is paramagnetic.
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[Fe(CN)6]4−
[Cr(NH3)6]3+ is paramagnetic while [Ni(CN)4]2− is diamagnetic. Explain why?
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[Co(C2O4)3]3−
Using valence bond theory, explain the following in relation to the complexes given below:
\[\ce{[Mn(CN)6]^{3-}}\]
(i) Type of hybridisation.
(ii) Inner or outer orbital complex.
(iii) Magnetic behaviour.
(iv) Spin only magnetic moment value.
Using valence bond theory, explain the following in relation to the complexes given below:
\[\ce{[FeCl6]^{4-}}\]
(i) Type of hybridisation.
(ii) Inner or outer orbital complex.
(iii) Magnetic behaviour.
(iv) Spin only magnetic moment value.
The type of hybridization involved in Octahedral complexes is ______.
If orbital quantum number (l) has values 0, 1, 2 and 3, deduce the corresponding value of principal quantum number, n.
How many radial nodes for 3p orbital?
Which of the statement given below is incorrect about H2O2?
Which of the following methods is used for measuring bond length?
Write the hybridisation and magnetic behaviour of [CoF6]3−.
[Given: Atomic number of Co = 27]
The magnetic moment of [NiCl4]2− is ______.
[Atomic number: Ni = 28]
[Ni(CO)4] has tetrahedral geometry while [Ni(CN)4]2− has square planar, yet both exhibit diamagnetism. Explain.
[Atomic number: Ni = 28]
During chemistry class, a teacher wrote \[\ce{[Ni(CN)4]^2-}\] as a coordination complex ion on the board. The students were asked to find out the magnetic behaviour and shape of the complex. Pari, a student, wrote the answer paramagnetic and tetrahedral whereas another student Suhail wrote diamagnetic and square planer.
Evaluate Pari’s and Suhail’s responses.
Given below are two statements:
Statement I: Both [Co(NH3)6]3+ and [CoF6]3− complexes are octahedral but differ in their magnetic behavior.
Statement II: [Co(NH3)6]3+ is diamagnetic whereas [CoF6]3− is paramagnetic.
In the light of the above statements, Choose the correct answer form the options given below:
