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(D) The number of $90^{\circ}$ bond pair-bond pair angles for different geometries are as follows:$1$. $dsp^2$ hybridization (Square planar): There ar

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$sp^3d^2$ hybridization

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(D) The number of $90^{\circ}$ bond pair-bond pair angles for different geometries are as follows:$1$. $dsp^2$ hybridization (Square planar): There are $4$ angles of $90^{\circ}$ between adjacent bond pairs.$2$. $sp^3d$ hybridization (Trigonal bipyramidal): There are $6$ angles of $90^{\circ}$ (three between equatorial and axial bonds,and three more between the other equatorial and axial bonds).$3$. $sp^3d^2$ hybridization (Octahedral): There are $12$ angles of $90^{\circ}$ between adjacent bond pairs.Comparing these,$sp^3d^2$ hybridization has the maximum number of $90^{\circ}$ angles. Therefore,the correct option is $D$.

Column-$I$	Column-$II$
$A$. Boron in $[B(OH)_4]^-$	$1$. $sp^2$
$B$. Aluminum in $[Al(H_2O)_6]^{3+}$	$2$. $sp^3$
$C$. Boron in $B_2H_6$	$3$. $sp^3d^2$
$D$. Carbon in Buckminsterfullerene
$E$. $Si$ in $SiO_4^{4-}$
$F$. $Ge$ in $[GeCl_6]^{2-}$

The maximum number of $90^{\circ}$ angles between bond pair-bond pair of electrons is observed in

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