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प्रश्न
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.
Explain on the basis of valence bond theory, the experimental finding that [Ni(CN)4]2− ion with a square planar structure is diamagnetic and the [Ni(Cl)4]2− ion with tetrahedral geometry is paramagnetic.
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उत्तर
Nickel in [Ni(CN)4]2− is in the +2 oxidation state, i.e., nickel is present as Ni2+ ion and dsp2 hybrid orbitals.
| [Ni(CN)4]2− | Ni(28): 4s2 3d8 |
| Ni2+(28): 4s0 3d8 |
CN− is a strong field ligand, so it causes the pairing of electrons.
The strong ligand CN− facilitates electron pairing. The complex is diamagnetic because it contains no unpaired electrons.
In [NiCl4]2−, the formation of the above complex can be explained by hybridization. Ni in the above compound is in the +2 oxidation state, i.e., Ni2+.
As Cl− is a weak ligand, pairing of electrons does not take place. sp3 hybridisation of orbitals takes place, giving rise to tetrahedral geometry. As there are two unpaired electrons in the complex, it is paramagnetic.
It is paramagnetic due to the presence of unpaired electrons.
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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)
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)
Write the hybridisation and number of unpaired electrons in the complex `[CoF_6]^(3-)`. (Atomic No. of Co = 27)
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:
\[\ce{[Co(NH3)6]^{3+}}\]
(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 ______.
Write the hybridization and shape of the following complexes:
[Ni(CN)4]2−
If orbital quantum number (l) has values 0, 1, 2 and 3, deduce the corresponding value of principal quantum number, n.
When the hybridization state of carbon changes from sp3 to sp2 and finally to sp, the angle between hybridized orbital will
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?
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]
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.
The geometry and magnetic behaviour of the complex [Ni(CO)4] are ______.
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:
