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(A) $1$. For $[Ni(CO)_4]$: $Ni$ is in $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing of electrons. The hybridization

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$[Ni(CO)_4]$ $-$ Tetrahedral,Paramagnetic

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(A) $1$. For $[Ni(CO)_4]$: $Ni$ is in $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing of electrons. The hybridization is $sp^3$,resulting in a tetrahedral geometry and diamagnetic nature (all electrons paired).$2$. For $[Ni(CN)_4]^{2-}$: $Ni$ is in $+2$ oxidation state $(3d^8)$. $CN^-$ is a strong field ligand,causing pairing. The hybridization is $dsp^2$,resulting in a square planar geometry and diamagnetic nature.$3$. For $[NiCl_4]^{2-}$: $Ni$ is in $+2$ oxidation state $(3d^8)$. $Cl^-$ is a weak field ligand,no pairing occurs. The hybridization is $sp^3$,resulting in a tetrahedral geometry and paramagnetic nature (two unpaired electrons).$4$. Comparing these with the options,statement $A$ is incorrect because $[Ni(CO)_4]$ is diamagnetic,not paramagnetic.

List-$I$ (Compound)	List-$II$ (Hybridization of Central atom)
$A. [Ni(NH_3)_6]^{2+}$	$1. sp^3$
$B. [PtCl_4]^{2-}$	$2. sp^3d^2$
$C. [Ni(CO)_4]$	$3. dsp^2$
$D. [Co(ox)_3]^{3-}$	$4. d^2sp^3$

$A. sp^3$	$(i). [Co(NH_3)_6]^{3+}$
$B. dsp^2$	$(ii). [Ni(CO)_4]$
$C. sp^3d^2$	$(iii). [Pt(NH_3)_2Cl_2]$
$D. d^2sp^3$	$(iv). [CoF_6]^{3-}$
	$(v). [Fe(CO)_5]$

Which of the following statements is incorrect?

Similar Questions

An octahedral complex of $Co^{3+}$ is diamagnetic. The hybridisation involved in the formation of the complex is

$A$ complex involving $dsp^2$ hybridization has:

Match the following hybridization in Column $I$ with the corresponding coordination complexes in Column $II$.
$A. sp^3$ $(i). [Co(NH_3)_6]^{3+}$
$B. dsp^2$ $(ii). [Ni(CO)_4]$
$C. sp^3d^2$ $(iii). [Pt(NH_3)_2Cl_2]$
$D. d^2sp^3$ $(iv). [CoF_6]^{3-}$
$(v). [Fe(CO)_5]$

Which of the following systems in an octahedral complex has the maximum number of unpaired electrons?

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