Hydrogen bonds are present in water structure. Presence of hydrogen bonds gives a characteristic property to water, which is :
High melting and high boiling points
Each water molecule can form up to four hydrogen bonds (two through its hydrogen atoms and two through the lone pairs on oxygen), giving an extensive three-dimensional network in ice and liquid water.
Extra energy is needed to break this network before the molecules can separate, so both the solid-to-liquid and the liquid-to-vapour transitions need more heat than expected for a molecule of molar mass 18.
Compared with the related hydrides H2S, H2Se and H2Te, which lack strong hydrogen bonding, water melts at 0 °C and boils at 100 °C, both far higher than the trend in the group would predict.
Therefore hydrogen bonding raises both the melting point and the boiling point of water; combinations with a low value for either transition do not fit.
Hence, High melting and high boiling points.
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