All intermolecular forces are Van der Waals forces.

They are not true bonds in the sense of sharing or transferring electrons, but are weaker attractive forces.  These forces include dipole-dipole forces, hydrogen bonding, and ionic interactions:

• Dipole-dipole forces exist between polar regions of different molecules.  The presence of a dipole means that the molecule has a partially positive end and a partially negative end.  Opposite partial charges attract each other, whereas like partial charges repel.  Biological systems utilise a special type of dipole-dipole force, known as hydrogen bonding.
• Hydrogen bonding involves hydrogen.  The hydrogen atom must be bonded to either an oxygen atom or a nitrogen atom.  Hydrogen bonding is significantly stronger than a “normal” dipole-dipole force and is very much stronger than London dispersion forces (very weak and short-lived attractions between molecules that arise due to the nucleus of one atom attracting the electron cloud of another atom).  Hydrogen bonding may be either intra-molecular or intermolecular.
• Ionic interactions may serve as intermolecular or intra-molecular forces in biological systems.  In some cases, these may involve metal cations, such as Na⁺, or anions, such as Cl^–.  In many cases, the cation is an ammonium ion from an amino group.  The anion may be from a carboxylic acid.  Oppositely charged ions attract each other strongly.