Match the species given in Column-$I$ with the hybridizations given in Column-$II$.

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 $[GeCl_6]^{2-}$

(A-2, B-3, C-2, D-1, E-2, F-3) $A-2, B-3, C-2, D-1, E-2, F-3$
$A$. Boron is the central atom and is surrounded by $4$ bond pairs only,hence it is $sp^3$ hybridized.
$B$. In $[Al(H_2O)_6]^{3+}$,the coordination number of $Al$ is $6$ and the geometry is octahedral,which corresponds to $sp^3d^2$ hybridization.
$C$. In $B_2H_6$,each $B$ atom is bonded to $4$ other atoms (two terminal $H$ and two bridging $H$),using $sp^3$ hybrid orbitals.
$D$. In Buckminsterfullerene $(C_{60})$,each carbon atom is bonded to three other carbon atoms and undergoes $sp^2$ hybridization.
$E$. The basic structural unit of silicates is $SiO_4^{4-}$,in which the silicon atom is bonded to four oxygen atoms in a tetrahedral fashion,indicating $sp^3$ hybridization.
$F$. In $[GeCl_6]^{2-}$,$Ge$ has a coordination number of $6$,resulting in octahedral geometry and $sp^3d^2$ hybridization.