1. Chapter 15 “Water and Aqueous Systems”

2. The Water Molecule l Each O-H bond is highly polar, –high electronegativity of the oxygen l Water is bent, /\, –O-H bond polarities do not cancel. water as a whole is polar.

3. The Water Molecule l Water’s bent shape and ability to hydrogen bond gives it many special properties! l Water molecules are attracted to one another by dipole interactions l This hydrogen bonding gives water: a) its high surface tension, b) its low vapor pressure.

4. High Surface Tension l liquid water acts like it has a “skin” –glass of water bulges over the top –This explains the pain of a ‘belly flop’

5. Surface Tension l One water molecule can hydrogen bond to another because of this electrostatic attraction. l Also, hydrogen bonding occurs with other molecules surrounding them on all sides. H H O ++ ++ -- H H O ++ -- ++

6. Surface Tension l A water molecule in the middle of a solution is pulled in all directions.

7. Surface Tension l Not true at the surface. l Only pulled down and to each side. l Holds the molecules at the surface together tightly. l This causes surface tension.

8. Surface Tension l Water drops are rounded, because all molecules on the edge are pulled to the middle- not outward to the air!

9. Surface Tension / capillary action l Glass has polar molecules. l Glass can also hydrogen bond. l This attracts the water molecules. l Some of the pull is up a cylinder.

10. Meniscus l Water curves up along the side of glass. l This makes the meniscus, as in a graduated cylinder l Plastics are non- wetting; no attraction

11. Meniscus In Glass In Plastic

12. Surface tension l All liquids have surface tension –water is just higher than most others l How can we decrease surface tension? –Use a surfactant - surface active agent –Also called a wetting agent, like detergent or soap –Interferes with hydrogen bonding

13. Low vapor pressure Hydrogen bonding also explains water’s unusually low vapor pressure. –Holds water molecules together, so they do not escape easily –This is a good thing, because lakes and oceans would evaporate very quickly due to their large surface area!

14. Ice l Most liquids contract (get smaller) as they are cooled. –They get more dense. l When they change to solid, they are more dense than the liquid. l Solid metals sink in their own liquid metal. –But, ice floats in water.

15. Ice l 10% lower density than water. l Water freezes from the top down. –The layer of ice on a pond acts as an insulator for water below l Why is ice less dense than liquid water? –The structure of ice is a regular open framework of water molecules arranged like a honeycomb.

16. Solvents and Solutes l Solution - a homogenous mixture, that is mixed molecule by molecule. l Solvent - the dissolving medium, the larger amount l Solute -the dissolved particles, the smaller amount l Aqueous solution- a solution with water as the solvent.

17. 1. Solute A solute is the dissolved substance in a solution. A solvent is the dissolving medium in a solution. 2. Solvent Salt in salt waterSugar in soda drinks Carbon dioxide in soda drinks Water in salt waterWater in soda Parts of a Solution:

18. Concentrated vs. Dilute

19. Aqueous Solutions l Water dissolves ionic compounds and polar covalent molecules best. l The rule is: “like dissolves like” l Polar dissolves polar. l Nonpolar dissolves nonpolar. l Oil is nonpolar. –Oil and water don’t mix. l Salt is ionic- makes salt water.

20. The Solution Process l Called “solvation”. l Water breaks the + and - charged pieces apart and surrounds them.

21. How Ionic solids dissolve in water H H O H H O H H O H H O H H O H H O H H O H H O H H O These ions have been surrounded by water, and are now dissolved! These ions have been pulled away from the main crystal structure by water’s polarity.

22. l Solids dissolve if attractive force of water is stronger than attractive force of solid. l If not, the solids are insoluble. l Water doesn’t dissolve nonpolar molecules (like oil) because it can’t hold onto them. l The water molecules hold onto other water molecules, and separate from the nonpolar molecules. l Nonpolars? No repulsion between them

23. Electrolytes and Nonelectrolytes l Electrolytes- compounds that conduct an electric current in aqueous solution, or in the molten state –all ionic compounds are electrolytes because they dissociate into ions (they are also called “salts”) l barium sulfate- will conduct when molten, but is insoluble in water!

24. Electrolytes and Nonelectrolytes l Do not conduct? = Nonelectrolytes. –Most are molecular materials, because they do not have ions l Not all electrolytes conduct to the same degree –there are weak electrolytes, and strong electrolytes –depends on: degree of ionization

25. The ammeter measures the flow of electrons (current) through the circuit. If the ammeter measures a current, and the bulb glows, then the solution conducts. If the ammeter fails to measure a current, and the bulb does not glow, the solution is non- conducting. Electrolytes vs. Nonelectrolytes

26. Electrolytes and Nonelectrolytes l Strong electrolytes exist as nearly 100 % ions l Weak electrolytes have only a fraction of the solute that exists as ions

27. Electrolyte Summary l Substances that conduct electricity when dissolved in water, or molten. l Must have charged particles that can move. l Ionic compounds break into charged ions: NaCl  Na 1+ and Cl 1- l These ions can conduct electricity.

28. l Nonelectrolytes do not conduct electricity when dissolved in water or molten l Polar covalent molecules such as methanol (CH 3 OH) don’t fall apart into ions when they dissolve. l Weak electrolytes don’t fall completely apart into ions. l Strong electrolytes do ionize completely.

29. Water of Hydration (or Water of Crystallization) l Water molecules are chemically bonded to solid salt molecules (not in solution) l These compounds have fixed amounts of water. l The water can be driven off by heating: l CuSO 4. 5H 2 O CuSO 4 + 5H 2 O l Called copper(II)sulfate pentahydrate. - heat + heat

30. Hydrates l Since heat can drive off the water, the forces holding it are weak l If a hydrate has a vapor pressure higher than that of water vapor in air, the hydrate will effloresce by losing the water of hydration

31. Hydrates l Some hydrates that have a low vapor pressure remove water from the air to form higher hydrates- these are called hygroscopic –used as drying agents, or dessicants –packaged with products to absorb moisture

32. Hydrates l Some compounds are so hygroscopic, they become wet when exposed to normally moist air - called deliquescent –remove sufficient water to dissolve completely and form solutions:

33. Mixtures that are NOT Solutions l The colloid particles are the dispersed phase, and are spread throughout the dispersion medium l The first colloids were glues. Others include mixtures such as gelatin, paint, aerosol sprays, and smoke l Table 15.3, p.460 list some common colloidal systems and examples

34. Mixtures that are NOT Solutions l Many colloids are cloudy or milky in appearance when concentrated, but almost clear when dilute –do not settle out –can not be filtered out l Colloids exhibit the Tyndall effect- the scattering of visible light in all directions. –suspensions also show Tyndall effect

35. The Tyndall Effect Colloids and suspensions scatter light, making a beam visible, due to their large particle size. Solutions do not scatter light, because of their small particle size. Which glass contains a colloid? solution colloid

36. - Page 461 Note that you can easily see the “sunbeam”, probably due to the presence of fog in the forest

37. Mixtures that are NOT Solutions l Flashes of light are seen when colloids are studied under a microscope- light is reflecting- called Brownian motion to describe the chaotic movement of the particles. Observed by Robert Brown. l Table 15.4, p.462 summarizes the properties of solutions, colloids, and suspensions

38. Mixtures that are NOT Solutions l Emulsions- dispersions of liquid in liquid (2 immiscible liquids + an emulsifier) –an emulsifying agent is essential for maintaining stability; it has one polar end, and the other end is nonpolar –oil and water not soluble; but with soap or detergent added, they will be. l Oil + vinegar in dressing – are they soluble? –What makes up Mayonnaise? Margarine?