Identify the hybridization of the central met | vedclass

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(A) $1$. The central metal atom is $Fe$ (atomic number $26$). The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$.$2$. In $[Fe(CO)_5]$, $CO$ is a

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$dsp^3$

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(A) $1$. The central metal atom is $Fe$ (atomic number $26$). The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$.$2$. In $[Fe(CO)_5]$, $CO$ is a strong field ligand, which causes pairing of electrons in the $3d$ orbital.$3$. The $Fe$ atom in $[Fe(CO)_5]$ is in the $0$ oxidation state.$4$. Due to the strong field ligand $CO$, the $4s$ electrons pair up into the $3d$ orbitals, leaving one $4s$, three $4p$, and one $3d$ orbital vacant.$5$. These five orbitals hybridize to form five $dsp^3$ hybrid orbitals, resulting in a trigonal bipyramidal geometry.

List-$I$ (Complex/ion)	List-$II$ (Shape/geometry)
$A$. $[Pt(Cl)_2(NH_3)_2]$	$I$. Octahedral
$B$. $[Co(NH_3)_6]Cl_3$	$II$. Trigonal bipyramidal
$C$. $[NiCl_4]^{2-}$	$III$. Square planar
$D$. $[Fe(CO)_5]$	$IV$. Tetrahedral

Identify the hybridization of the central metal atom in the $[Fe(CO)_5]$ complex.

Similar Questions

Which of the following complexes exhibits $sp^{3}d$ hybridization?

The hybridization of the central atom in $NH_3, [PtCl_4]^{2-}, PCl_5$,and $BCl_3$ respectively is:

Match List-$I$ with List-$II$:
List-$I$ (Complex/ion) List-$II$ (Shape/geometry)
$A$. $[Pt(Cl)_2(NH_3)_2]$ $I$. Octahedral
$B$. $[Co(NH_3)_6]Cl_3$ $II$. Trigonal bipyramidal
$C$. $[NiCl_4]^{2-}$ $III$. Square planar
$D$. $[Fe(CO)_5]$ $IV$. Tetrahedral

The hybridization observed in the $[PtCl_6]^{2-}$ ion is .......

What is the geometry of $[Ni(CO)_4]$?

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