Question

What is intermolecular hydrogen bonding?

Answer 1

Hint: Hydrogen bond is defined as an attractive force between partially positive charged atoms with partially negative charged atoms. This is very weak in nature as compared to the strength of covalent bonds. Hydrogen bonds are usually shown as dotted lines between the atoms. 

Complete answer:
Intermolecular forces for example dipole-dipole interactions or hydrogen bonding are one of the important concepts while learning the concept of solvation.  Molecules that are polar in nature will form hydrogen bonds with other molecules when they have hydrogen atoms which are further covalently bonded with highly electronegative elements like ammonia in which hydrogen molecules get bonded with nitrogen atoms or hydrogen atoms bonded with each other. Where the polar nature of the molecule makes the molecules capable of dissolving in water. Other polar molecules which do not have hydrogen atoms will be attracted to other molecules with the help of dipole-dipole interactions. The fact that they are polar also means that they will dissolve in water. If the main intermolecular force between molecules is dispersion forces or London forces then the molecule is nonpolar in nature and will not dissolve properly in polar solvents like water.
Hydrogen bonding is mainly of two types known as intermolecular hydrogen bonding and intramolecular hydrogen bonding. Intermolecular hydrogen bonding can be explained by hydrogen bonding taking place between different molecules of the same or different compounds. The main example of intermolecular hydrogen bonding is water, ammonia etc.

Note: Intermolecular forces are those forces which binds the molecules of matter together. Intermolecular forces are higher in case of solid then in liquid and very less in gaseous state. Solid state has definite shape, liquid state takes the shape of the container in which it is kept and gaseous state has no shape as it has a great tendency to flow.