What is the Difference Between Localised and Delocalised Chemical Bonds?

The main difference between localized and delocalized chemical bonds lies in the distribution of electrons between atoms.

Localized chemical bonds involve sharing electrons between two atoms, with electrons being associated with specific atom pairs and not free to move throughout the molecule. These bonds usually occur due to the overlapping of molecular orbitals, such as sigma bonds and pi bonds. Localized bonds have a well-defined bond length determined by the distance between the participating atoms.

Delocalized chemical bonds involve electrons that are not confined to specific atom pairs but are shared among multiple atoms or regions. These bonds form due to side overlapping of p orbitals and are commonly found in molecules with extended pi systems or resonance structures. Delocalized bonds may not have a specific bond length since the electrons are distributed over a larger molecular structure.

In summary, localized bonds are characterized by electrons that are confined to specific atom pairs, whereas delocalized bonds involve electrons that are shared among multiple atoms or regions.

Comparative Table: Localised vs Delocalised Chemical Bonds

The difference between localised and delocalised chemical bonds lies in the distribution of electrons between atoms. Here is a comparison table highlighting the key differences:

In summary, localised chemical bonds are normal sigma and pi bonds or lone electron pairs that exist on a single atom, with electrons concentrated in a limited region of a molecule. On the other hand, delocalised chemical bonds involve electrons that are shared over an extended region of space, often involving multiple atoms, and are free to move throughout the molecule.