What is the Difference Between Localised and Delocalised Chemical Bonds?
🆚 Go to Comparative Table 🆚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:
Localised Chemical Bonds | Delocalised Chemical Bonds |
---|---|
Occur due to frontal overlapping between s orbitals, p orbitals, or s and p orbitals | Form when several localised bonds mix with each other |
Exist on a single atom | Involve more than one atom in a molecule |
Electrons are limited to a particular region between two separate atoms | Electrons spread throughout the molecule, free to move |
Examples include sigma and pi bonds | Examples include resonance structures in benzene |
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.
- Localized vs Delocalized Electrons
- Delocalization vs Resonance
- Ionic vs Covalent Bonds
- Ionic Bonding vs Metallic Bonding
- Electrovalent vs Covalent Bond
- Covalent vs Noncovalent Bonds
- Double Bond vs Single Bond
- Bond Enthalpy vs Lattice Enthalpy
- Hydrogen Bond vs Ionic Bond
- Enthalpy of Atomisation vs Bond Dissociation
- Coordinate Covalent Bond vs Covalent Bond
- Intermolecular vs Intramolecular Hydrogen Bonding
- Hydrogen Bond vs Covalent Bond
- Bonding vs Antibonding Molecular Orbitals
- Antibonding vs Nonbonding
- Electrovalency vs Covalency
- Bond Dipole vs Molecular Dipole
- Saturated vs Unsaturated Bonds
- Supramolecular Chemistry vs Molecular Chemistry