Difference Between sp3d2 and d2sp3 Hybridization

Key Difference – sp3d2 vs d2sp3 Hybridization
 

There are hypothetical structures known as orbitals in an atom in which electrons reside. Different scientific discoveries have proposed different shapes for these orbitals. Atomic orbitals can undergo a process known as hybridization. Hybridization of orbitals occurs in order to obtain suitable shapes required for chemical bonding. Hybridization is the mixing of atomic orbitals to form hybrid orbitals. sp³d² and d²sp³ are such hybrid orbitals. The key difference between sp³d² and d²sp³hybridization is that sp³d² hybridization involves atomic orbitals of same electron shell whereas d²sp³ hybridization involves atomic orbitals of two electron shells.

CONTENTS

1. Overview and Key Difference
2. What is sp3d2 Hybridization
3. What is d2sp3 Hybridization
4. Similarities Between sp3d2 and d2sp3 Hybridization
5. Side by Side Comparison – sp3d2 vs d2sp3 Hybridization in Tabular Form
6. Summary

What is sp3d2 Hybridization

sp³d² hybridization is the mixing of s, p and d atomic orbitals of the same electron shell to form sp³d² hybrid orbitals. There, one s atomic orbital, three p atomic orbitals and two d atomic orbitals mix with each other. This mixing results in six hybrid orbitals of same size and shape but different from their orientation.

The sp³d² hybrid orbitals are arranged in octahedral arrangement. These hybrid orbitals have 90^o angles between two orbitals in the octahedral arrangement. The octahedral arrangement displays a square plane having four hybrid orbitals and the two remaining orbitals are oriented above and below of this square plane (perpendicular to this plane).

Example

Let us consider an example in order to understand the sp³d² hybridization. Ex: SF6 molecule has an octahedral shape because the 3s, 3p and 3d atomic orbitals of the sulfur atom (S) are mixed to formsp³d² hybrid orbitals.

As shown in the above image, the hybridization results in six unpaired electrons that can participate in chemical bonding with six fluorine atoms. Most importantly, all the atomic orbitals involved in this hybridization are in the same electron shell (in above example, it is n=3 electron shell).

What is d2sp3 Hybridization?

d²sp³ hybridization is the mixing of s and p atomic orbitals of the same electron shell with d orbitals of another electron shell to form d²sp³ hybrid orbitals. This hybridization results in six hybrid orbitals. These hybrid orbitals are arranged in an octahedral geometry.

Most importantly, in this hybridization, the d atomic orbitals come from a different electron shell (n-1 electron shell) whereas s and p atomic orbitals are of the same electron shell. Let us consider an example to understand this hybridization. Most of the metal ion complexes are composed of d²sp³ hybridized orbitals.

Example

For example, take Co(NH₃)³⁺ complex.

As shown in the above image, there are six empty hybrid orbitals in cobalt atom after hybridization. These empty orbitals can participate in coordination chemical bond formation with ligands (here ammonia ligands = NH₃).

What are the Similarities Between sp3d2 and d2sp3 Hybridization?

• Both sp3d2 and d2sp3 Hybridizations result in octahedral geometry.
• Both sp3d2 and d2sp3 Hybridization geometries have 90^o angle between hybrid orbitals.
• Both sp3d2 and d2sp3 Hybridization result in six hybrid orbitals.

What is the Difference Between sp3d2 and d2sp3 Hybridization?

Summary – sp3d2 vs d2sp3 Hybridization

sp³d² hybridization and d²sp³ hybridization are confusing terms that are most of the times used interchangeably by mistake. These are different in many ways. The key difference between sp³d² and d²sp³hybridization is that, sp³d² hybridization involves atomic orbitals of same electron shell whereas d²sp³ hybridization involves atomic orbitals of two electron shells.

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Reference:

1.“8.2: Hybrid Atomic Orbitals.” Chemistry LibreTexts, Libretexts, 30 Aug. 2017. Available here