Molecule obtained by sp³d² hybridization has bond angle (s) of

Concept: 

Hybridization:

• It is the phenomenon of intermixing atomic orbitals of slightly different energies and shape to form new hybrid orbitals.
• The hybrid orbitals have equivalent energies and identical shapes to that of parent orbitals.
• Hybrid orbitals are effective in forming stable bonds than atomic orbitals.
• They are directed in space in some preferred direction to have a stable arrangement.

Types of Hybridization:

Types of hybridization	Atomic orbitals involved	Structure of molecule	Geometry	Examples
sp	one s + one p		Linear	BeCl2, BeH2, C2H2
sp2	one s + two p		Triagonal planar	BF3, BCl3, C2H4
sp3	one s + three p		Tetrahedral	CH4, CCl4, SnCl4
dsp2	one d (dx2-y2) + one s + two p		Square planar	[PtCl42-], [NiCN42-]
sp3d	one s + three p + one d (dz2)		Triagonal bipyramidal	PF5, PCl5
sp3d2	one s + three p + two d (dx2-y2and dz2)		Octahedral	SF6, [CrF6]3-
sp3d3	one s + three p + dxy, dyz, dxz		Pentagonal bipyramidal	IF7

Explanation:

sp³d² hybridization:

• The hybridization of one s, three p, and two d orbitals (d_x²_-y²and d_z²) results in 6 sp³d² hybrid orbitals.
• The electron density lobes of these 6 sp³d² orbitals are directed towards the vertices of an octahedron.
• The angle between each pair of sp³d² hybrid orbitals is 90°.
• The bonds in the central square plane make angles of 90° between adjacent pairs and also with the axial bonds.
• Compounds of the typeAX₆, AX₅E, AX₄E₂ are sp³d² hybridized.

The figure below is the graphical representation of sp3d2 hybridization in a molecule:

Hence, the Molecule obtained by sp³d² hybridization has a bond angle (s) of 90°.