Hydrogen-bonded molecules response

That the molecules in solid and liquid water interact by hydrogen bonding and that hydrogen bonding is responsible for the anomalous properties of water compared with the other hydrides of Group 16... 

The amine may enter into hydrogen bonding interaction with a surface hydroxyl (figure 9.23 a). The hydrogen bond formation is responsible for the fast adsorption of the silane molecules onto the silica surface, as discussed above. The basic amine function may abstract a proton from a silanol and form an ionic bond (figure 9.23 b). This type of interaction is much more stable than the first one. The hydrogen bonded molecules may self-catalyse the condensation of the silicon side of the silane molecule (figure 9.23 c). Thus, a covalent siloxane bond is formed. 

The fact that water molecules are usually held to each other by hydrogen bonds is responsible for the success of our planet and of life-forms themselves. Hydrogen bonding in water is the reason that frozen water is less dense than liquid water. Not only does ice float, but more importantly, floating ice permits water below the surface in ponds and lakes to remain in a liquid state during the winter and therefore allows for the continuity of life in these waters. On a more aesthetic note, hydrogen bonding is responsible for the six-sided nature of snowflakes. 

The N—H N hydrogen bond is responsible for the formation of the complexes between aniline and aliphatic amines (ammonia, methylamine, dimethylamine and tri-methylamine) which act as proton acceptors. Infrared photodissociation spectra and DFT calculation indicate208 that the clusters [aniline/ammonia]+ and [aniline/methylamine]+ have a non proton transferred (without the proton donation from the aniline moiety to the amine molecule) structure, while the complexes [aniline/dimethylamine]+, [aniline/ trimethylamine]+ possess a proton transferred structure. Reasonably, the proton transfer increases on increasing the proton affinity of the amine used as solvent. 

The ability to form strong hydrogen bonds is responsible for the many unique characteristics of water, such as its very high melting point and boiling point for a molecule of its size. 

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