Examples of compounds that can form hydrogen bonds are:
Ammonia can form a maximum of one hydrogen bond per molecule
Hydrogen bonds are strong intermolecular forces which are harder to break causing water to have a higher melting and boiling point than would be expected for a molecule of such a small size
The high enthalpy change of evaporation of water suggests that instantaneous dipole-induced dipole forces are not the only forces present in the molecule – there are also strong hydrogen bonds, which cause the high boiling point
The surface molecules are pulled downwards due to the hydrogen bonds with other molecules, whereas the inner water molecules are pulled in all directions
The ‘more open’ structure of molecules in ice causes it to have a lower density than liquid water
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