Orbital hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals suitable for bonding. When atoms form covalent bonds, their atomic orbitals (s, p, d) can combine to create equivalent hybrid orbitals that have different shapes and energies than the original atomic orbitals.

This hybridization model, developed by Linus Pauling, helps explain molecular geometries and bonding characteristics that cannot be explained by simple atomic orbital theory. The type of hybridization directly determines the geometry of molecules and the angles between bonds, making it essential for understanding molecular structure.

To determine the hybridization of a central atom, first count the number of sigma bonds (single bonds, or one bond from double/triple bonds) and lone pairs around the central atom. The sum of these gives the steric number, which directly corresponds to the hybridization type.

For example, in water (H₂O), the oxygen atom has 2 sigma bonds (to hydrogen atoms) and 2 lone pairs, giving a steric number of 4. This means oxygen is sp³ hybridized with a tetrahedral electron geometry, though the molecular geometry is bent due to the lone pairs pushing the bonds closer together.

Hybridization predictions are based on VSEPR theory and steric number calculations. While this model works well for many molecules, it has limitations. Actual hybridization may vary due to resonance structures, molecular orbital delocalization, or complex electronic effects in transition metal compounds.

This calculator provides idealized predictions based on classical hybridization theory. For accurate analysis of complex molecules, especially those involving d-block elements or extensive conjugation, more advanced computational methods or experimental data should be consulted.