Advertisements
Advertisements
Question
[NiCl4]2- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why? (Atomic no. Ni = 28)
Advertisements
Solution
[NiCl4]2-
Ni is in + 2 oxidation state.
3d8 configuration 
Cl- is weak field ligand. So, pairing doesnot occur.
sp3 hybridised orbitals of 2 Ni2+ 
[ ] NiCl is paramagnetic as n = 2
4 [ ( ) ] Ni CO Ni is in ‘0’ oxidation state
In presence of ‘CO’ pairing of e– takes place ‘CO’ is strong field ligand. So, with ‘CO
[Ni(CO)4] → 
[Ni(CO)4] → 
So, [Ni(CO)4] is diamagnetic as n = 0.
APPEARS IN
RELATED QUESTIONS
On the basis of valence bond theory explain the nature of bonding in [CoF6]3 ion.
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.
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:
[CoF6]3−
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?
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]?
Using valence bond theory, predict the hybridization and magnetic character of the following:
[CoF6]3– [Atomic number of Co = 27]
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.
