The hybridisation of Ni centre in [Ni(PPh_3)_ | vedclass

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Question

(A) The oxidation number of $Ni$ in both $[Ni(PPh_3)_2Cl_2]$ and $[NiCl_4]^{2-}$ is $+2$. The electronic configuration of $Ni(II)$ is $[Ar] 3d^8 4s^0$

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$dsp^2$ and $sp^3$

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(A) The oxidation number of $Ni$ in both $[Ni(PPh_3)_2Cl_2]$ and $[NiCl_4]^{2-}$ is $+2$. The electronic configuration of $Ni(II)$ is $[Ar] 3d^8 4s^0$.In $[Ni(PPh_3)_2Cl_2]$,$PPh_3$ is a strong field ligand,which forces the electrons in the $3d$ orbital to pair up,leaving one $3d$ orbital vacant. This allows for $dsp^2$ hybridisation,resulting in a square planar geometry.In $[NiCl_4]^{2-}$,$Cl^-$ is a weak field ligand,which does not cause pairing of electrons in the $3d$ orbital. Thus,the $4s$ and $4p$ orbitals are used for $sp^3$ hybridisation,resulting in a tetrahedral geometry.Therefore,the hybridisation of $Ni$ in $[Ni(PPh_3)_2Cl_2]$ and $[NiCl_4]^{2-}$ are $dsp^2$ and $sp^3$ respectively.

List-$I$ (Complex)	List-$II$ (Hybridization)
$A. Ni(CO)_4$	$I. sp^3d^2$
$B. [Ni(CN)_4]^{2-}$	$II. d^2sp^3$
$C. [Co(NH_3)_6]^{3+}$	$III. dsp^2$
$D. [CoF_6]^{3-}$	$IV. sp^3$

The hybridisation of $Ni$ centre in $[Ni(PPh_3)_2Cl_2]$ and $[NiCl_4]^{2-}$,respectively are

Similar Questions

Match the complexes in List-$I$ with their hybridization in List-$II$.
List-$I$ (Complex) List-$II$ (Hybridization)
$A. Ni(CO)_4$ $I. sp^3d^2$
$B. [Ni(CN)_4]^{2-}$ $II. d^2sp^3$
$C. [Co(NH_3)_6]^{3+}$ $III. dsp^2$
$D. [CoF_6]^{3-}$ $IV. sp^3$

Which of the following has a non-zero magnetic moment and $sp^3d^2$ hybridization?

$[PdCl_2(PMe_3)_2]$ is a diamagnetic complex of $Pd(II)$. How many unpaired electrons are present in the analogous complex of $Ni(II)$?

In an octahedral structure,which pair of $d$-orbitals is involved in ${d^2}sp^3$ hybridization?

The $Cl-Co-Cl$ bond angle values in a $fac-[Co(NH_3)_3Cl_3]$ complex is/are:

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