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प्रश्न
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[Fe(CN)6]4−
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उत्तर
The oxidation state of iron in this complex ion is +2.
Electronic configuration of Fe = [Ar] 3d64s2
Electronic configuration of Fe2+ = [Ar] 3d6
The iron (II) ion must provide six vacant orbitals to accommodate the six electron pairs from the six cyanide ions. This can be achieved by the hybridisation method, in which the d-subshell electrons pair, since CN– ions are strong-field ligands.
Hence, six electron pairs from six cyanide ions occupy six hybrid orbitals of the iron (II) ion. Thus, no unpaired electrons are in any orbital, so [Fe(CN)6]4− shows diamagnetism. Hence, [Fe(CN)6]4− is diamagnetic and octahedral.
संबंधित प्रश्न
[NiCl4]2− is paramagnetic, while [Ni(CO)4] is diamagnetic, though both are tetrahedral. Why? (Atomic number of Ni = 28)
Predict the number of unpaired electrons in the square planar [Pt(CN)4]2− ion.
[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:
[CoF6]3−
Explain the geometry of `[Co(NH_3)_6]^(3+)` on the basis of hybridisation. (Z of Co = 27)
[NiCl4]2- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why? (Atomic no. Ni = 28)
Using valence bond theory, explain the following in relation to the complexes given below:
\[\ce{[Co(NH3)6]^{3+}}\]
(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.
In a coordination entity, the electronic configuration of the central metal ion is t2g3 eg1
Is the coordination compound a high spin or low spin complex?
If orbital quantum number (l) has values 0, 1, 2 and 3, deduce the corresponding value of principal quantum number, n.
Which of the following methods is used for measuring bond length?
Which of the following has square planar structures?
Valence bond theory is based on the assumption that the bonds formed between the metal ions and ligands are ______
Using Valence bond theory, explain the following in relation to the paramagnetic complex [Mn(CN)6]3−
- type of hybridization
- magnetic moment value
- type of complex – inner, outer orbital complex
According to the valence bond theory, the hybridization of central metal atom is dsp2 for which one of the following compounds?
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]
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:
