The situation that leads to Hydrogen bonding arises with a normal bond between a Hydrogen atom and a neighbour. Since any other atom will bind the electron from the Hydrogen atom more tightly, the electron will spend more time with the other atom. Hydrogen bonding between water molecules makes ice less dense than water so, in winter, rivers freeze down from the top and not up from the bottom, enabling life to survive. Hydrogen bonding is also one of the major forces responsible for the attraction between chains in polymers. The dipoles involved in Van der Waals bonding come from fluctuations in the symmetry of the electron distribution surrounding the nucleus of an atom.
Ionic bonds tend to form between elements at the edges.
Covalent bonds tend to form between elements in the middle. Secondary bonds are the result of electric dipole interaction. Hydrogen bonds form with permament dipoles. Van der Waals bonds form with fluctuating dipoles. Covalent crystals tend to be brittle because of the directional restriction.