Polar Bond
| Formula / Notation | Polar bond: δ+ — δ−; Δχ > 0.4; partial charges |
|---|---|
| Also Known As | Polar covalent bond, dipolar bond, δ+−δ− bond |
What is Polar Bond?
A covalent bond between two atoms of different electronegativities in which electrons are unequally shared. The more electronegative atom carries a partial negative charge (δ-), and the less electronegative atom carries a partial positive charge (δ+). Water's O-H bonds are polar.
Formula & Notation
Other Names / Synonyms: Polar covalent bond, dipolar bond, δ+−δ− bond
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A covalent bond between two atoms of different electronegativities in which electrons are unequally shared. The more electronegative atom carries a partial negative charge (δ-), and the less electronegative atom carries a partial positive charge (δ+). Water's O-H bonds are polar.
Polar bonds determine: molecular polarity (affects solubility, boiling point, intermolecular forces), reactivity (polar bonds are susceptible to nucleophilic/electrophilic attack), spectroscopy (IR-active vibrations change dipole moment), and drug-receptor interactions (polar groups form hydrogen bo…
Highly polar bonds (H-F, O-H) create strong hydrogen bonding, explaining why HF and H₂SO₄ are more viscous and corrosive than expected. Polar bonds in solvent molecules determine their ability to stabilise charge intermediates — polar aprotic solvents (DMSO, DMF) enhance nucleophile reactivity and m…
The formula or notation for Polar Bond is: Polar bond: δ+ — δ−; Δχ > 0.4; partial charges