Question

Why are van der waals forces critical for micelle formation and what is the role of entropy in the process?

Answer 1

Hydrophobic tails when bound inside, still have interchanges, which is alright because it is more stable and favorable. Think of how bonds structure and phase as the water stays together to maximize stronger bonds and does not adhere with nonpolar because of less stable bonds. Van der Waals forces are very weak so they discourage strong bonds from forming between polar and nonpolar compounds, aiding the construction of more stable like-like interactions, and aiding the formation of micelles.

Entropy is a role as the system minimizes the numeral ordered water molecules required to surround hydrophobic portions of solute molecules. In molecular physics, the van der Waals force, quoted after Dutch physicist Johannes Diderik van der Waals, is a distance-dependent interaction between atoms or molecules. Contrary to ionic or covalent bonds, these attractions do not result from a chemical electronic bond; they are comparatively weak and therefore more susceptible to annoyance. The van der Waals force quickly vanishes at longer distances between interacting molecules.

Learn more about the Van der Waals force:

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