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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
On the basis of valence bond theory explain the nature of bonding in [CoF6]3 ion.
[NiCl4]2− is paramagnetic, while [Ni(CO)4] is diamagnetic, though both are tetrahedral. Why? (Atomic number of Ni = 28)
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:
[Co(C2O4)3]3−
Using valence bond theory, explain the following in relation to the complexes given below:
\[\ce{[Cr(H2O)6]^{3+}}\]
(i) Type of hybridisation.
(ii) Inner or outer orbital complex.
(iii) Magnetic behaviour.
(iv) Spin only magnetic moment value.
Write the hybridization and shape of the following complexes:
[Ni(CN)4]2−
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.
As the s-character of hybridised orbital increases, the bond angle
Which of the following methods is used for measuring bond length?
What is the no. of possible isomers for the octahedral complex [Co(NH3)2(C2O4)2]?
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
Using valence bond theory, predict the hybridization and magnetic character of the following:
[CoF6]3– [Atomic number of Co = 27]
[Ni(CO)4] has tetrahedral geometry while [Ni(CN)4]2− has square planar, yet both exhibit diamagnetism. Explain.
[Atomic number: Ni = 28]
The geometry and magnetic behaviour of the complex [Ni(CO)4] are ______.
Which of the following are paramagnetic?
- [NiCl4]2−
- Ni(CO)4
- [Ni(CN)4]2−
- [Ni(H2O)6]2+
- Ni(PPh3)4
Choose the correct answer from the options given below:
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:
