In an octahedral structure, the pair of $d$ orbitals involved in $d^2 s p^2$ hybridisation is:
In an octahedral structure, the pair of $d$ orbitals involved in $d^2 s p^2$ hybridisation is:
$d_{x^2-y^2} \cdot d_{z^2}$
$d_{x z} d_{x^2-y^2}$
$d_{z 2} \cdot d_{x z}$
$d_{x y^{\prime}} d_{y z}$
Solution
$s p^3 d^2$ or $d^2 s p^3$ are hybridisation for the octahedral geometry. In octahedron, the bonds are formed parallel to the $x, y$, and $z$-axes, hence $d x^2-d y^2$ and $d z^2$ will be used to form the hybrid orbitals.
