What is the Difference Between Pure and Hybrid Orbitals?

The key difference between pure and hybrid orbitals lies in their formation and the number of atomic orbitals involved. Here are the main differences:

1. Formation: Pure orbitals are the original atomic orbitals that contain electrons of the atom, whereas hybrid orbitals form from the mixing of two or more atomic orbitals.
2. Hybridization: Pure orbitals are not hybridized, while hybrid orbitals form via orbital hybridization.
3. Nomenclature: Pure orbitals are named as s, p, d, and f orbitals, while hybrid orbitals are named as sp, sp², sp³, etc.
4. Stability: Hybridized orbitals are generally more stable than pure orbitals because they allow for better overlap between atomic orbitals, leading to stronger chemical bonds.
5. Spatial Arrangement: The spatial arrangement of hybrid orbitals can vary depending on the combination of atomic orbitals involved. For example, sp³ hybrid orbitals point at the vertices of a tetrahedron, oriented at 109.5° from each other.

In summary, pure orbitals are the original atomic orbitals that do not undergo hybridization, while hybrid orbitals are the result of mixing two or more atomic orbitals. Hybrid orbitals are more stable than pure orbitals due to better overlap, and their spatial arrangement depends on the combination of atomic orbitals involved.

Comparative Table: Pure vs Hybrid Orbitals

Here is a table comparing pure and hybrid orbitals:

In summary, pure orbitals are atomic orbitals that do not mix, while hybrid orbitals are formed by combining atomic orbitals to create new, equivalent orbitals with specific spatial arrangements. Hybrid orbitals are often used in bonding due to their optimized energy levels and ability to minimize electron repulsion.