Advertisements
Advertisements
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.
Advertisements
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.
APPEARS IN
संबंधित प्रश्न
Predict the number of unpaired electrons in the square planar [Pt(CN)4]2− ion.
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:
[FeF6]3−
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[Co(C2O4)3]3−
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:
\[\ce{[FeCl6]^{4-}}\]
(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.
How many radial nodes for 3p orbital?
As the s-character of hybridised orbital increases, the bond angle
Valence bond theory is based on the assumption that the bonds formed between the metal ions and ligands are ______
Using valence bond theory, predict the hybridization and magnetic character of the following:
[CoF6]3– [Atomic number of Co = 27]
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]
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:
