Question

What is the spatial orientation of ${\mathrm{sp}}^3{\mathrm{d}}^3$ hybrid orbitals?

Answer 1

Hybridization:

• “Hybridization is the mixing of atomic orbitals that have a similar energy to form hybrid atomic orbitals. The formed hybrid orbitals have an entirely different energy, shape, etc.”
• The possible mixing of atomic orbitals is two “s” orbitals and two “p” orbitals or an “s” orbital and a “p” orbital or a mixing of “s” orbital and “d” orbital.

${\mathrm{sp}}^3{\mathrm{d}}^3$ hybridization and its spatial orientation:

• The overlapping of one s-orbital, three p-orbital, and three-d-orbitals forms the ${\mathrm{sp}}^3{\mathrm{d}}^3$ hybridized orbitals. That is, seven hybridized orbitals are formed.
• The molecule with ${\mathrm{sp}}^3{\mathrm{d}}^3$ hybridization possesses pentagonal bipyramidal geometry. Five bonds are created in the X-Y plane, while the remaining two are produced along the Z-axis, one above and one below the plane. The angle between every five bonds in the X-Y plane is $72°$. Whereas the angle between the bond along Z-axis and X-Y plane is $90°$.
• The s-orbital, which is non-directional, is found in the plane. The three orbitals of the p- subshell are directed along the X-, Y-, and Z-axes, respectively.
• The d-subshell, on the other hand, has five orbitals. The lobes of the $\mathrm{dxy},\mathrm{dyz},\mathrm{dzx}$- orbitals are positioned between their designated axes. The remaining two orbitals, the ${\mathrm{dx}}^2-{\mathrm{y}}^2$ orbitals, have their lobes on the X-Y plane, while the ${\mathrm{dz}}^2$ orbitals, which have a unique shape, have their lobes on both the Z-axis and the X-Y plane.
• Only the $\mathrm{s},\mathrm{px},\mathrm{py},{\mathrm{dx}}^2{\mathrm{y}}^2,\mathrm{dxy}$orbitals in the X-Y plane and the $\mathrm{pz}$ and ${\mathrm{dz}}^2$ orbitals perpendicular to the X-Y plane along the Z-axis may achieve the provided geometry.

Example:

• ${\mathrm{IF}}_7$is an example of ${\mathrm{sp}}^3{\mathrm{d}}^3$ hybridization.
• The Iodine $\left(\mathrm{I}\right)$ atom will be in the center, five fluorine $\left(\mathrm{F}\right)$ atoms will be in the X-Y plane, and the remaining two F will be along the positive and negative Z-axis.
• The angle between the iodine atom and fluorine atom in the X-Y plane will $72°$. While the angle between the iodine atom and the $\mathrm{F}$ (along z-axis) has$90°$.