Pi (π) bonding molecular orbital

Definition

A pi (π) bonding molecular orbital is formed by the lateral overlap of atomic orbitals. This type of bonding occurs in molecules where electrons are shared above and below the plane of the nuclei.

5 Must Know Facts For Your Next Test

1. Pi (π) bonds are generally weaker than sigma (σ) bonds due to less effective overlap of orbitals.
2. In a π bond, the electron density is concentrated above and below the internuclear axis.
3. Pi bonds usually form between p orbitals that are parallel to each other.
4. Molecules with double or triple bonds have both σ and π bonds; one σ bond and one or two π bonds respectively.
5. The formation of a π bond restricts rotation around the bond axis, leading to cis-trans isomerism.

Review Questions

• What type of orbital overlap results in a pi (π) bonding molecular orbital?
• How does the strength of a π bond compare to that of a σ bond?
• Why do π bonds restrict rotation around the bond axis?

Related terms

Sigma (σ) Bond: A sigma (σ) bond is formed by the end-to-end overlap of atomic orbitals, resulting in electron density along the internuclear axis.

Molecular Orbital Theory: A theory that describes the distribution of electrons in molecules in terms of combination and interaction of atomic orbitals forming molecular orbitals.

Cis-Trans Isomerism: \text{Isomerism arising from restricted rotation around double bonds or cyclic structures, leading to different spatial arrangements.}