1. Water

2. Water in the Liquid State A water molecule is polar.

3. Water in the Liquid State Polar molecules are attracted to one another by dipole interactions. The negative end of one molecule attracts the positive end of another molecule.

4. Water in the Liquid State The intermolecular attraction among water molecules results in the formation of hydrogen bonds.

5. Surface Tension

6. Water in the Liquid State A surfactant is any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension.

7. Water in the Liquid State –Vapor Pressure Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure. Because hydrogen bonds hold water molecules to one another, the tendency of these molecules to escape is low, and evaporation is slow.

8. Water in the Solid State

10. Homogeneous vs. Heterogeneous Mixtures Guided note, 3. HomogeneousHeterogeneous Mixture that is uniform in composition. Components are evenly distributed throughout the mixture and not easily distinguished. Mixture that is not uniform in composition. Components are not evenly distributed throughout the mixture

11. Solvents and Solutes Guided note: 4. SolventDissolving medium in a solution SoluteDissolved particles in a solution Solution homogeneous mixture, consisting of a solute dissolved in a solvent

12. The Solution Process Guided note: 7. The dissolving process is a result of random molecular motion. The process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules is called solvation.

13. Solution Formation The compositions of the solvent and the solute determine whether a substance will dissolve. Guided notes: 8. The factors that determine how fast a substance dissolves are »stirring (agitation) »temperature »the surface area of the dissolving particles

14. Solubility – Saturation Guided Notes – 9. Saturated Solution UnSaturated Solution contains the maximum amount of solute for a given quantity of solvent at a given temperature and pressure.

15. Solubility

16. Solubility - Expression Guided Note: 9. Solubility definition –Solubility is often expressed in grams of solute per 100 g of solvent at a specific temperature and pressure to produce a saturated solution. 16.1

17. Factors Affecting Solubility Guided note: 10. –Temperature affects the solubility of solid, liquid, and gaseous solutes in a solvent; –Both temperature and pressure affect the solubility of gaseous solutes.

18. Temperature vs. Solubility

19. Supersaturation A supersaturated solution contains more solute than it can theoretically hold at a given temperature. (Guided notes, 9.) The crystallization of a supersaturated solution can be initiated if a very small crystal, called a seed crystal, of the solute is added.

20. Factors Affecting Solubility –Pressure Changes in pressure have little effect on the solubility of solids and liquids, but pressure strongly influences the solubility of gases. Gas solubility increases as the partial pressure of the gas above the solution increases.

21. Factors Affecting Solubility Henry’s law states that at a given temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas above the liquid.

22. Strong Electrolytes Guided note: 5. An strong electrolyte is a compound that conducts an electric current when it is in an aqueous solution or in the molten state. –All ionic compounds are electrolytes because they dissociate into ions.

23. Weak Electrolytes A weak electrolyte conducts electricity poorly because only a fraction of the solute in the solution exists as ions.

24. Nonelectrolytes A compound that does not conduct an electric current in either aqueous solution or the molten state is called a nonelectrolyte.

25. Suspensions and Colloids A suspension is a mixture from which particles settle out upon standing. –A suspension differs from a solution because the particles of a suspension are much larger and do not stay suspended indefinitely. Colloids have particles smaller than those in suspensions and larger than those in solutions.

26. Colloids

27. Colloids

28. Colloids