BIOL 301 Chapter Notes - Chapter 2.1: Hydrogen Bond, Electronegativity, Boiling Point

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In liquid water, the average number of hydrogen bonds per molecule is lower due to disorganized motion of liquid water. It weakens ( screens ) the interactions between the na+ and cl- ions by hydrating them, which prevents their arrangement in a lattice: for charged molecules, it replaces solute-solute hydrogen bonds with solute- water hydrogen bonds. It is effective at screening electrostatic interactions due to its high dielectric constant, a function of the number of dipoles in solvent. The solvation of crystalline substances increases entropy: the ions of nacl acquire greater freedom of motion when leaving the lattice structure, this explains why formation of the solution in water is thermodynamically favorable. Nonpolar gases do not dissolve readily in water: e. g. Co2, o2, n2: the movement of molecules from gas phase to aqueous phase leads to less disorder among gas molecules and in the motion of water molecules, this is a decrease in entropy, which is not favorable.

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