MBB 222 Lecture Notes - Lecture 4: Lone Pair, Boiling Point, Sodium Chloride
20 Dec 2018
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Document Summary
Hydrogen bonds are key to water"s properties and to its role as a solvent. This polarity makes h-bonding between water molecules very favorable. Water has a very high melting point, boiling point and heat of vaporization compared to other solvents. These properties are due to its hydrogen-bonding tendency, which hold the molecules together, requiring significant energy input to separate them. Because of its polarity, water is also as an excellent solvent. Water forms hydration spheres around ions, proteins and other macromolecules. Ions and polar molecules are hydrophilic love water. Water is highly polar, thus an excellent solvent for ionic and nonionic-but-polar compounds. Water can also solubilize polar compounds by forming h bonds with these solutes. In a vacuum, two oppositely charged species interact very tightly. However, when ions are solvated their charges are dampened. The ability of a solvent to interact with a solute and decrease the electrostatic attraction between ions is a measure of its dielectric constant, d.
