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प्रश्न
[Cr(NH3)6]3+ is paramagnetic while [Ni(CN)4]2− is diamagnetic. Explain why?
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उत्तर
Formation of [Cr(NH3)6]3+: The oxidation state of chromium in [Cr(NH3)6]3+ ion is +3. The electronic configuration of chromium is [Ar] 3d54s1. The hybridisation is shown in the following diagram:
The Cr3+ ion provides six vacant orbitals to accommodate six electron pairs from six ammonia molecules. As a result, the complex [Cr(NH3)6]3+ has d2sp3 hybridisation and is octahedral. The presence of three unpaired electrons in the complex explains its paramagnetic property.
Formation of [Ni(CN)4]2−: In [Ni(CN)4]2− the oxidation state of Ni is +2 and its electronic configuration is 3d8. Hybridisation can be explained as follows:
Each hybridised orbital accepts a pair of electrons from the cyanide ion. The absence of unpaired electrons confirms the diamagnetic behaviour of [Ni(CN)4]2−.
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संबंधित 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.
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[Fe(CN)6]4−
[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:
\[\ce{[Mn(CN)6]^{3-}}\]
(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.
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.
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.
When the hybridization state of carbon changes from sp3 to sp2 and finally to sp, the angle between hybridized orbital will
Which of the following methods is used for measuring bond length?
Which of the following has square planar structures?
In Fe(CO)5, the Fe – C bond possesses
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
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]
