Question

In an octahedral structure, the pair of d orbitals involved in $d^{2}s{p}^3$ hybridization is :

• A. $d_{xz},d_{x^2-y^2}$
• B. $d_z^2,d_{xz}$
• C. $d_{xy},d_{yz}$
• D. $d_{x^2-y^2},d_{z^2}$

Answer 1

Answer: (C)

$d_{xy},d_{yz}$

$d^{2}s{p}^3$ or $s{p}^3{d}^2$ are hybridizations for the octahedral geometry and we know that the bonds are in the shape of an octahedron with the bonds parallel to the x,y and z axes.

Hence the $2$ d orbitals involved in the formation of the hybrid orbitals are $d{x}^2-y^2$ and $d{z}^2$

The other $3$ d orbitals (i.e., dxy,dxz and dyz are not parallel to the axis. They are formed in between the axes)

(Image )

$\therefore$ $d{x}^2-y^2$ and $d{z}^2$ are d-orbitals that are involved in $d^{2}s{p}^3$ hybridization.

Therefore, option D is correct.