Hybridization

Hybridization

The process by which atomic orbitals mix to form new hybrid orbitals.
Used to make σ bonds
Involves end-to-end overlapping (hence why π bonds are not hybridized)

σ bond

A bond that is cylindrical symmetrical, involves end-to-end overlap along the bond axis.

π bond

A bond formed by side-to-side overlap of p orbitals, which locks rotation.

sp hybridization

Hybridization involving one s and one p orbital, resulting in a linear structure.

sp² hybridization

Hybridization involving one s and two p orbitals, resulting in a trigonal planar structure.

sp³ hybridization

Hybridization involving one s and three p orbitals, resulting in a tetrahedral structure.

sp³d hybridization

Hybridization resulting from one s, three p, and one d orbital, creating a trigonal bipyramidal structure.

sp³d² hybridization

Hybridization resulting from one s, three p, and two d orbitals, resulting in an octahedral structure.

Covalent bond

A bond formed by the overlapping of atomic orbitals.

End-to-end overlap

The overlap that occurs along the bond axis, characteristic of σ bonds.

Side-to-side overlap

The overlap that occurs above and below the internuclear axis, characteristic of π bonds.

Molecular structure of single bond

Consists of 1 σ bond.

Molecular structure of double bond

Consists of 1 σ bond and 1 π bond.

Molecular structure of triple bond

Consists of 1 σ bond and 2 π bonds.