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Hydrogen-hond interactions

Notice in Figure 15.2 that the water molecules in liquid water are associated with each other by hydrogen-honding interactions. For a solute to dissolve in water, a "hole" must be made in the water structure for each solute particle. This will occur only if the lost water-water interactions are replaced by similar water-solute interactions. [Pg.524]

It is important to notice that the united-atom simplification cannot be applied to functional hydrogens which are involved in the formation of a hydrogen hond or a salt bridge. This would destroy interactions important for the structural integrity of the protein. Removing the hydrogen at the u-carbon of the peptide backbone is also dangerous, because it prevents racemization of the amino acid. [Pg.363]

Crystal solvates exhibit a wide range of behaviour depending on the interaction between the solvent and the crystal stmcture. With some solvates the solvent plays a key role in holding the crystal together for example, it may he part of a hydrogen-honded network within the crystal stmcture. These solvates are very stable and are difficult to desolvate. When these crystals lose their solvent they collapse and recrystallise in a new crystal form. We can think of these as polymorphic solvates. In other solvates, the solvent is not part of the crystal bonding and merely occupies... [Pg.19]

Fig. 2.7. The effective interaction potential between two oxygen atoms joined by a hydrogen hond O-H... O as calculated from the model of Lippincott Schroeder (1955). Fig. 2.7. The effective interaction potential between two oxygen atoms joined by a hydrogen hond O-H... O as calculated from the model of Lippincott Schroeder (1955).
The electrostatic interaction plays a particularly important role because it is of a long-range character as well as very sensible to relative orientation of the subsystems. The hydrogen hond X-H... Y represents an example of the domination of the electrostatic interaction. This results in its directionality, linearity and a small (as compared to typical chemical bonds) interaction energy of the order of —5 kcal/mol. [Pg.879]

The quantitative analysis of molecular interactions is of fundamental interest, and the development of computer software has made it easy to calculate the theoretical properties of molecules. Feasibility can be demonstrated using simple, small molecules. Alkanes have demonstrated van der Waals energy contribution, and alkanols demonstrated the additional hydrogen-honding energy contribution. Ion-ion interactions were related to the electrostatic energy contribution, and amino acids demonstrated the contribution of steric hindrance. [Pg.15]

D1.3VhD58 E5.2VlY49 interactions include one additional van der Waals contact each. These results show the importance of local environment, in addition to hond geometry, in determining the relative strengths of different types of hydrogen bonds. [Pg.140]


See other pages where Hydrogen-hond interactions is mentioned: [Pg.28]    [Pg.2414]    [Pg.1088]    [Pg.451]    [Pg.223]    [Pg.28]    [Pg.2414]    [Pg.1088]    [Pg.451]    [Pg.223]    [Pg.221]    [Pg.53]    [Pg.67]    [Pg.166]    [Pg.1077]    [Pg.25]    [Pg.83]    [Pg.162]    [Pg.17]    [Pg.83]    [Pg.254]    [Pg.986]    [Pg.536]    [Pg.457]    [Pg.12]    [Pg.38]   
See also in sourсe #XX -- [ Pg.205 ]




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Hydrogen interactions

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