London Dispersion: All molecules have these.Just remember, there will be a partially-positive atom that interacts with a partially-negative atom of a neighboring molecule. The concept is the same as above except on a smaller scale since the dipoles will not be as large. Dipole-Dipole: These can be basically thought of as weaker hydrogen bonds that do not contain F,O, or N as the electronegative atoms.Partially-positive hydrogens will interact with partially-negative F,O, or Ns of neighboring molecules. The large contrast in electronegativities between the hydrogen and these other F, O, N atoms creates large dipoles. Hydrogen Bonding: requires a hydrogen to be covalently bound to F, O, or N.(example: the positive cation of NaCl will be surrounded be water’s oxygens which have a negative dipole). Ion-Dipole: the interaction between an ion and an oppositely charged dipole.Here are the four intermolecular forces you should know in order of DECREASING strength: IntERmolecular forces are the interactions that occur between neighboring particles and have a large effect on a compound’s physical properties such as the melting point, boiling point, viscosity, etc. covalent bonds, metallic bonds, ionic bonds). We’re talking about intermolecular forces, not to be confused with intRAmolecular forces, which bind the atoms within a single particle (i.e.

Here’s a general chemistry concept that frequently appears on the DAT.

Metallic bonds and dispersio force