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Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group 16 hydrides, which have little capability to hydrogen bond. Intramolecular hydrogen bonding is partly responsible for the secondary , tertiary , and quaternary structures of proteins and nucleic acids .
The normal boiling point is the boiling point at atmospheric pressure, ... and materials with stronger intermolecular forces, such as most solids, ...
Non-covalent interactions have a significant effect on the boiling point of a liquid. Boiling point is defined as the temperature at which the vapor pressure of a liquid is equal to the pressure surrounding the liquid. More simply, it is the temperature at which a liquid becomes a gas. As one might expect, the stronger the non-covalent ...
Melting and boiling points of metallic, ionic, covalent, and molecular solids ... many molecular solids have directional intermolecular forces. [11] ...
Interestingly, for homogeneous systems, the intermolecular forces that are calculated from the LJ and the LJTS potential at a given distance are the same (since / is the same), whereas the potential energy and the pressure are affected by the shifting. Also, the properties of the LJTS substance may furthermore be affected by the chosen ...
These two definitions are equivalent: the boiling point is the temperature at which the increased entropy of the gas phase overcomes the intermolecular forces. As a given quantity of matter always has a higher entropy in the gas phase than in a condensed phase ( Δ v S {\displaystyle \Delta _{\text{v}}S} is always positive), and from
The intermolecular force between noble gas atoms is the very weak London dispersion force, so their boiling points are all cryogenic, below 165 K (−108 °C; −163 °F). [ 2 ] The noble gases' inertness , or tendency not to react with other chemical substances , results from their electron configuration : their outer shell of valence ...
Melting (blue) and boiling (orange) points of the first 16 n-alkanes in °C. Alkanes experience intermolecular van der Waals forces. The cumulative effects of these intermolecular forces give rise to greater boiling points of alkanes. [18] Two factors influence the strength of the van der Waals forces: