1. Should we control a chemical that: u Causes excessive sweating and vomiting. u Is a major component in acid rain. u Can cause severe burns in its gaseous state.

2. u Accidental inhalation can kill you. u Contributes to erosion. u Decreases the effectiveness of car brakes. u Has been found in tumors of terminal cancer patients.

3. What is the chemical? u Dihydrogen monoxide u Otherwise known as H 2 O

4. Chapter 3 Water and the Fitness of the Environment

5. Question? What molecule Is the most common In living Cells? Water - most cells are 70 - 95% water.

6. The Water Planet

7. Properties Of Water u Be ready and able to discuss several of the following properties. u Focus on definitions and examples. u Review water structure and H-bonds from Chapter 2.

8. Liquid Water Is Cohesive u Water sticks to water. u Why? Because the polarity of water results in hydrogen bonding.

9. Liquid Water is Adhesive u Water sticks to other molecules. u Why? Hydrogen bonding.

10. Water transport in trees uses Cohesion and Adhesion

11. Water Has A High Surface Tension u The surface of water is difficult to stretch or break. u Why? Hydrogen bonding.

12. Water Has A High Specific Heat u Specific Heat - the amount of heat needed to raise 1 g of the substance 1 degree C. u Why? Hydrogen bonding.

13. Heat u Total quantity of kinetic energy due to molecular motion.

14. Temperature u Measures the average speed of the molecules.

15. Celsius Scale u Will be used for most of our temperature measurements. u O o C - water freezes u 100 o C - water boils u 37 o C - human body

16. Water Stabilizes Temperature u Water can absorb and store a huge amount of heat from the sun. u Result - climate moderation u Result - organisms are able to survive temperature changes.

17. Fig. 3-5 San Diego 72° 40 miles Pacific Ocean 70s (°F ) 80s 90s 100s Santa Barbara 73° Los Angeles (Airport) 75° Burbank 90° San Bernardino 100° Riverside 96° Santa Ana 84° Palm Springs 106°

18. Water Has A High Heat Of Vaporization u Heat of Vaporization: the quantity of heat a liquid must absorb for 1g of it to convert to a gaseous state.

19. Evaporative Cooling

20. Result: u Water cools organisms from excessive heat buildup. u Why? Hydrogen bonding

21. Water Expands When It Freezes u The distance between water molecules INCREASES from the liquid to the solid form. u Why? u Hydrogen bonding

25. Ice forms a Hexagonal Lattices Snow crystals form when water vapor condenses directly into ice

26. Solids and Liquids WaterBenzene Floats Sinks

27. Solid LiquidGas States of Matter

28. Result u Aquatic life can live under ice.

29. Hydrophilic Materials u Materials that dissolve in water. u Hydro - water u philic - to like or love u Have ionic or polar regions (polar covalent bonds) on their molecules for H + bonds.

32. Hydrophobic u Materials that repel water. u Hydro - water u phobic - to fear u Have non-polar covalent bonds. Ex - lipids.

33. Without Water Life Would Not Be Possible!!

34. How can this be?

35. Van de Waals Bonds u Due to polarity in specific regions of nonpolar covalent substances

36. Water Is A Versatile Solvent u Water will form a solution with many materials. u Why? Hydrogen bonding

37. Solution u Homogeneous mixture of two or more substances.

38. Solvent u The dissolving agent. u The material in the greater quantity.

39. Solute u The substance that is dissolved. u The material in the lesser quantity.

40. Solution Concentration u Usually based on Molarity. u Molarity - the number of moles of solute per liter of solution.

41. Moles u The molecular weight of a substance in grams. u One Avogadro’s number of molecules. 6.02 X 10 23

42. One Mole of each Sulfur Sugar Copper Sulfate Mercury Oxide Copper Sodium Chloride

43. Dissociation of Water u Water can sometimes split into two ions. u In pure water the concentration of each ion is 10 -7 M

44. u Adding certain solutes disrupts the balance between the two ions. u The two ions are very reactive and can drastically affect a cell.

45. Acids u Materials that can release H + u Example: HCl HCl H + + Cl -

46. Acid Rain

48. Bases u Materials that can absorb H + u Often reduce H + by producing OH - u Example: NaOH NaOH Na + + OH -

49. Neutrals u Materials that are neither acids nor bases.

50. pH Scale u A logarithmic scale for showing H + concentration pH = - log [H + ]

51. pH Scale

52. Example: For a neutral solution: [H + ] is 10 -7 or - log 10 -7 or - (-7) or 7

53. u Acids: pH <7 etc. u Bases: pH >7 etc. u Each pH unit is a 10x change in H +

54. Comment u [H + ] + [OH - ] = 14 u Therefore, if you know the concentration of one ion, you can easily calculate the other.

55. Fig. 3-9 Neutral solution Acidic solution Basic solution OH – H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ Neutral [H + ] = [OH – ] Increasingly Acidic [H + ] > [OH – ] Increasingly Basic [H + ] < [OH – ] pH Scale 0 1 2 3 4 5 6 7 8 Battery acid Gastric juice, lemon juice Vinegar, beer, wine, cola Tomato juice Black coffee Rainwater Urine Saliva Pure water Human blood, tears Seawater 9 10 Milk of magnesia Household ammonia Household bleach Oven cleaner 11 12 13 14

56. Buffers u Materials that have both acid and base properties. u Resist pH shifts. u Cells and other biological solutions often contain buffers to prevent damage.

57. Blood Buffers- Carbonic-acid-bicarbonate u HCO 3 -CO 2 u BaseAcid u In water Carbonic acid

58. Summary u Be able to discuss the properties of water. u Be able to measure solution concentrations in Molarity. u Be able to work pH scale questions.