Dipole-Dipole Forces
Part of the Structure and Bonding section of Coddy's Chemistry journey. Lesson 29 of 49.
Polar molecules have lasting δ+ and δ− ends that attract each other: dipole-dipole forces.
The δ+ end of one polar molecule attracts the δ− end of the next
They act on top of London forces, so a polar substance boils higher than a non-polar one of similar size.
Challenge
Hydrogen chloride, HCl. Is the molecule polar, and what is the strongest force between its molecules?
Try it yourself
Shape viewerDescribe the molecule HCl
Test yourselfThis lesson includes a short quiz. Start the lesson to answer it and track your progress.
All lessons in Structure and Bonding
1Ionic Bonding
Why Atoms BondForming IonsThe Ionic BondIonic FormulasPolyatomic IonsIonic LatticesRecap - Salt Factory2Covalent Bonds
Sharing ElectronsCounting Valence ElectronsDrawing Lewis StructuresDouble and Triple BondsLone PairsFormal ChargeLewis Structures of IonsRecap - Molecule Builder5Forces Between Molecules
London ForcesDipole-Dipole ForcesHydrogen BondsBoiling PointsLike Dissolves LikeRecap - Boiling Contest