Match the complexes in List-I with their hybr | vedclass

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(C) $A. Ni(CO)_4$: $Ni$ is in $0$ oxidation state. $CO$ is a strong field ligand. $Ni(0) = [Ar] 3d^8 4s^2$. Due to $CO$,electrons pair up to give $3d^

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$I-D, II-C, III-B, IV-A$

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(C) $A. Ni(CO)_4$: $Ni$ is in $0$ oxidation state. $CO$ is a strong field ligand. $Ni(0) = [Ar] 3d^8 4s^2$. Due to $CO$,electrons pair up to give $3d^{10}$. Hybridization is $sp^3$ $(IV)$.$B. [Ni(CN)_4]^{2-}$: $Ni$ is in $+2$ oxidation state. $CN^{-}$ is a strong field ligand. $Ni^{2+} = [Ar] 3d^8$. Electrons pair up,leaving one $3d$ orbital vacant. Hybridization is $dsp^2$ $(III)$.$C. [Co(NH_3)_6]^{3+}$: $Co$ is in $+3$ oxidation state. $NH_3$ is a strong field ligand. $Co^{3+} = [Ar] 3d^6$. Electrons pair up,leaving two $3d$ orbitals vacant. Hybridization is $d^2sp^3$ $(II)$.$D. [CoF_6]^{3-}$: $Co$ is in $+3$ oxidation state. $F^{-}$ is a weak field ligand. $Co^{3+} = [Ar] 3d^6$. No pairing occurs. Hybridization is $sp^3d^2$ $(I)$.Therefore,the correct match is $A-IV, B-III, C-II, D-I$,which corresponds to option $C$ $(I-D, II-C, III-B, IV-A)$.

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

$LIST-I$	$LIST-II$
$P. dsp^2$	$1. [FeF_6]^{4-}$
$Q. sp^3$	$2. [Ti(H_2O)_3Cl_3]$
$R. sp^3d^2$	$3. [Cr(NH_3)_6]^{3+}$
$S. d^2sp^3$	$4. [FeCl_4]^{2-}$
	$5. Ni(CO)_4$
	$6. [Ni(CN)_4]^{2-}$

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

Similar Questions

Which of the following statements is correct regarding the $[Fe(CN)_6]^{4-}$ complex?

The hybridization of $[Ni(CO)_4]$ is:

Match each set of hybrid orbitals from $LIST-I$ with complex(es) given in $LIST-II$. The correct option is

$LIST-I$ $LIST-II$

$P. dsp^2$ $1. [FeF_6]^{4-}$

$Q. sp^3$ $2. [Ti(H_2O)_3Cl_3]$

$R. sp^3d^2$ $3. [Cr(NH_3)_6]^{3+}$

$S. d^2sp^3$ $4. [FeCl_4]^{2-}$

$5. Ni(CO)_4$

$6. [Ni(CN)_4]^{2-}$

State the limitations of valence bond theory.

Which among the following complexes has square pyramidal geometry?

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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$