Among Ni(CO)_4, [Ni(CN)_4]^{2-} and [NiCl_4]^ | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) $1$. In $Ni(CO)_4$,the oxidation state of $Ni$ is $0$. The configuration is $[Ar] 3d^8 4s^2$. Since $CO$ is a strong field ligand,it causes pairin

Vedclass · Accepted Answer

$Ni(CO)_4$ and $[Ni(CN)_4]^{2-}$ are diamagnetic and $[NiCl_4]^{2-}$ is paramagnetic.

Vedclass · Answer

(C) $1$. In $Ni(CO)_4$,the oxidation state of $Ni$ is $0$. The configuration is $[Ar] 3d^8 4s^2$. Since $CO$ is a strong field ligand,it causes pairing of electrons,resulting in $3d^{10}$ configuration. Thus,it is diamagnetic.$2$. In $[Ni(CN)_4]^{2-}$,the oxidation state of $Ni$ is $+2$. The configuration is $[Ar] 3d^8$. $CN^-$ is a strong field ligand,causing pairing of electrons in $3d$ orbitals,resulting in $d^8$ configuration with no unpaired electrons. Thus,it is diamagnetic.$3$. In $[NiCl_4]^{2-}$,the oxidation state of $Ni$ is $+2$. The configuration is $[Ar] 3d^8$. $Cl^-$ is a weak field ligand,so it does not cause pairing. There are $2$ unpaired electrons in the $3d$ orbitals. Thus,it is paramagnetic.

Among $Ni(CO)_4, [Ni(CN)_4]^{2-}$ and $[NiCl_4]^{2-}$,which of the following statements is correct?

Similar Questions

Which of the following statements is incorrect for the complex $[Cr(NH_3)_6]Cl_3$?

$NiCl_2\{P(C_2H_5)_2(C_6H_5)\}_2$ exhibits temperature-dependent magnetic behaviour (paramagnetic/diamagnetic). The coordination geometries of $Ni^{2+}$ in the paramagnetic and diamagnetic states are respectively

Which of the following complexes exhibits outer orbital hybridization?

The geometries of some complex ions are given below. Select the correct answer.
$(1) [Ag(NH_3)_2]^+ - \text{Linear}$
$(2) [MnCl_4]^{2-} - \text{Tetrahedral}$
$(3) [Cu(NH_3)_4]^{2+} - \text{Square planar}$
$(4) [Ni(CN)_4]^{2-} - \text{Square planar}$

What is the number of unpaired electrons present in $[CoF_6]^{3-}$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module