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/Species)	List-$II$ (Shape and magnetic moment)
$A$. $[Ni(CO)_4]$	$I$. Tetrahedral,$2.8 \ BM$
$B$. $[Ni(CN)_4]^{2-}$	$II$. Square planar,$0 \ BM$
$C$. $[NiCl_4]^{2-}$	$III$. Tetrahedral,$0 \ BM$
$D$. $[MnBr_4]^{2-}$	$IV$. Tetrahedral,$5.9 \ BM$

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

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