Electron sp3d2
hybridization with suitable example.

The electron sp3d2 hybridization is a type of hybridization that occurs when six atomic orbitals, consisting of one s orbital, three p orbitals, and two d orbitals, combine to form six hybrid orbitals. This hybridization is commonly observed in compounds with octahedral geometry.

One example of a compound that exhibits sp3d2 hybridization is sulfur hexafluoride (SF6). In SF6, the central sulfur atom forms six sigma bonds with six fluorine atoms, resulting in an octahedral arrangement around the sulfur atom. The electronic configuration of sulfur (S) is 1s2 2s2 2p6 3s2 3p4. During hybridization, one s orbital, three p orbitals, and two d orbitals of sulfur combine to form six sp3d2 hybrid orbitals.

The hybridization process can be explained as follows:

Sulfur's 3s orbital and three 3p orbitals hybridize to form four sp3 hybrid orbitals. These orbitals are involved in bonding with four of the fluorine atoms.
Sulfur's 3d orbitals (3dxz, 3dyz, 3dx^2-y^2, and 3dz^2) are involved in hybridization as well. Two of the d orbitals (3dxz and 3dyz) combine with two of the p orbitals in a process called dsp2 hybridization, forming two additional hybrid orbitals.
The resulting six sp3d2 hybrid orbitals of sulfur overlap with the 2p orbitals of the six fluorine atoms, forming six sigma bonds.
Overall, the sp3d2 hybridization in sulfur hexafluoride allows for the formation of six strong sigma bonds, resulting in the compound's stable octahedral geometry.