Dipole-Dipole Interactions
| Formula / Notation | ΔE = μ₁μ₂(1−3cos²θ)/(4πε₀r³); stronger with greater μ and smaller r |
|---|---|
| Also Known As | Keesom force (orientational), dipole-dipole force, polar intermolecular force |
What is Dipole-Dipole Interactions?
Intermolecular attractive forces between polar molecules that arise from electrostatic interactions between permanent dipoles. The positive end of one molecule is attracted to the negative end of another. These forces are stronger than London dispersion forces but weaker than hydrogen bonds.
Formula & Notation
Other Names / Synonyms: Keesom force (orientational), dipole-dipole force, polar intermolecular force
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
Intermolecular attractive forces between polar molecules that arise from electrostatic interactions between permanent dipoles. The positive end of one molecule is attracted to the negative end of another. These forces are stronger than London dispersion forces but weaker than hydrogen bonds.
Dipole-dipole forces explain the higher boiling points of polar molecules compared to nonpolar molecules of similar molecular weight. They govern the miscibility of polar solvents, the solubility of drugs in biological fluids, and the physical properties of liquid crystals.
Polar solvents with strong dipole-dipole interactions (acetone, DMF, DMSO) dissolve a wide range of chemicals and can enhance skin absorption of dissolved toxins. Handle solutions in polar solvents with appropriate PPE.
The formula or notation for Dipole-Dipole Interactions is: ΔE = μ₁μ₂(1−3cos²θ)/(4πε₀r³); stronger with greater μ and smaller r