1. 1 - 1 © Chemeketa Community College: CH117 CH117 Chemistry in the Kitchen Unit 1: States & Solutions Measurements; Metric Units Phase Changes Water Solutions Polarity

2. 1 - 2 © Chemeketa Community College: CH117 MetricSICommonConversions Length Volume Mass Temperature Energy Units of Measurement meter (m) 1 m = 1.09 yd liter (L) 1 L = 1.06 qt gram (g) 1 kg = 2.2 lb Celsius ( o C) C = (F-32)/1.8 Kelvin (K) K = C + 273

3. 1 - 3 © Chemeketa Community College: CH117 180 o 100 o Temperature

4. 1 - 4 © Chemeketa Community College: CH117 MetricSICommonConversions Length Volume Mass Temperature Energy Units of Measurement meter (m) 1 m = 1.09 yd liter (L) 1 L = 1.06 qt gram (g) 1 kg = 2.2 lb Celsius ( o C) C = (F-32)/1.8 Kelvin (K) K = C + 273 calorie (cal) 1Kcal = 1000 cal = 1Cal Joule (J) 1 cal = 4.18 J

5. 1 - 5 © Chemeketa Community College: CH117 Changes of State Melting Pt = Freezing Pt Boiling Pt Solid Liquid Vapor CondenseCondense FreezeFreeze MeltMelt VaporizeVaporize Slow, close, Fixed arrangement Moderate, close, Random arrangement Fast, far apart, Random Crystalline Amorphous

6. 1 - 6 © Chemeketa Community College: CH117 Common Melting/Boiling Pts Freezing/ Melting Pt o C ( o F) Boiling Pt o C ( o F) Water0 (32)100 (212) Ethanol-114 (-173)78 (173) Salt801 (1474)1413 (2575) Sucrose Dec 186 (367) Canola Oil-10 (14) Smokes 204 (400) Olive Oil-6 (21) Smokes 190 (374) Coconut Oil25 (77) Smokes 177 (351) Many molecules can’t change phases.

7. 1 - 7 © Chemeketa Community College: CH117 Water Purification Desalination – remove salt http://glossary.periodni.com/glossary.php?en=distillation Distillation – water boils at 100 o C; the impurity (salt) at 800 o C Water boils first – cools –condenses pure

8. 1 - 8 © Chemeketa Community College: CH117 Water Purification Solar Still

9. 1 - 9 © Chemeketa Community College: CH117 Solid Liquid Vapor Changes of State Frost DepositDeposit SublimeSublime Freeze Dry (At reduced Pressure)

10. 1 - 10 © Chemeketa Community College: CH117 Temperature stays constant Temperature rises Heating Curve Temp stays constant Changes of State

11. 1 - 11 © Chemeketa Community College: CH117 Temperature at Boiling Pt is Constant. Boiling Point Double Boiler: To melt chocolate or wax without burning. Dry Meat before Browning: Wet meat can’t get hot enough to brown. Dried meat browns; wet meat steams. Applications:

12. 1 - 12 © Chemeketa Community College: CH117 Temperature at Boiling Pt is Constant. Boiling Point Cooling for Nuclear Reactor: To generate energy without “meltdown”. Applications:

13. 1 - 13 © Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure

14. 1 - 14 © Chemeketa Community College: CH117 We live at the bottom of an ocean of air Atmospheric Pressure Atmosphere: A sea of colorless, odorless gases surrounding the earth Boiling Point

15. 1 - 15 © Chemeketa Community College: CH117 At higher elevations, there is less air so the P is less. Boiling Point Atmospheric Pressure

16. 1 - 16 © Chemeketa Community College: CH117 Boiling Point = Boiling Point = Temp where molecule’s Vapor Pressure = Atmospheric Pressure Sea Level 760 torr Denver (5280’) 630 torr Mt. Evans,CO(14,000’) Mt. Everest(20,000’) 467 torr 270 torr H2OH2OH2OH2O = 100 o C = 95 o C = 87 o C = 73 o C If P goes down Boiling Pt goes down

17. 1 - 17 © Chemeketa Community College: CH117 Compound Interest: Compoundchem.com http://www.compoundchem.com/2016/03/22/boiling-point/_ http://www.compoundchem.com/2016/03/22/boiling-point/_

18. 1 - 18 © Chemeketa Community College: CH117 PT V If P goes up Boiling Pt goes up Boiling Point Pressure cookers Autoclaves

19. 1 - 19 © Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Ethyl alcohol (drinking alcohol) Isopropyl alcohol (rubbing alcohol) Mass = 46Mass = 60 Bp = 78 o CBp = 83 o C

20. 1 - 20 © Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Polarity (water vs ethanol) WaterEthyl alcohol (drinking alcohol) Acetone (polish remover) Hexane (in gasoline) Mass = 18Mass = 46Mass = 58Mass = 86 Bp = 100 o CBp = 78 o CBp = 56 o CBp = 69 o C

21. 1 - 21 © Chemeketa Community College: CH117 Hydrogen Bonding of Water HH O ++++ ++++ ---- HH O ++++ ++++ ---- HH O ++++ ++++ ---- Hydrogen Bonds HH O ++++ ++++ ---- Polar Attraction Water beads, Water bends

22. 1 - 22 © Chemeketa Community College: CH117 Hydrogen Bonding of Water Hydrogen Bonds Causes Surface Tension Water beads, Water bends

23. 1 - 23 © Chemeketa Community College: CH117 Hydrogen Bonding of Water Frozen H 2 O: Slow moving molecules H-Bond in patterns (Hexagonal Ring Crystals)

24. 1 - 24 © Chemeketa Community College: CH117 Frozen H 2 O Floats: Hydrogen Bonding of Water 4 o C (water most dense) 0oC0oC0oC0oC

25. 1 - 25 © Chemeketa Community College: CH117 Hydrogen Bonding of Ethanol Hydrogen Bonds Polar Attraction CH O ++++ ---- C H H H H H CH O ++++ ---- C H H H H H CH O ++++ ---- C H H H H H

26. 1 - 26 © Chemeketa Community College: CH117 Hydrogen Bonding of Water Hydrogen Bonds Causes Surface Tension Surfactants reduce Surface Tension by disrupting H-bonding (soaps, detergents etc.; make water “wetter”)

27. 1 - 27 © Chemeketa Community College: CH117 Solutions Na + Cl - Na + Cl - Solvent Solvent : greater component in greater amount (The dissolver) Water Alcohol (in some medicines) Solute Solute: lesser component in lesser amount (The dissolved) Alcohol (in beverages) NaCl (in saline or ocean) Sugar (in beverages) A solution A solution = A homogeneous mixture of components.

28. 1 - 28 © Chemeketa Community College: CH117 Saturation Unsaturated: Unsaturated: (Dilute) Can dissolve more. Saturated: Saturated: (very concentrated) Have dissolved all possible Undissolved Solids in equilibrium w/ dissolved particles Undissolved Solids in equilibrium w/ dissolved particles

29. 1 - 29 © Chemeketa Community College: CH117 Solutions Supersaturated: Temporarily dissolves more than normal at given Temp. Precipitate Excess solute that falls out of solution Application: Rock Candy On pipe cleaner: 7:22 https://search.yahoo.com/search?fr=mcafee&type=B211 US0D20150525&p=sugar+crystals https://search.yahoo.com/search?fr=mcafee&type=B211 US0D20150525&p=sugar+crystals Canadian guy: 14:35 https://search.yahoo.com/search?fr=mcafee&type=B211 US0D20150525&p=sugar+crystals https://search.yahoo.com/search?fr=mcafee&type=B211 US0D20150525&p=sugar+crystals

30. 1 - 30 © Chemeketa Community College: CH117 Solutions Solid solutions Gelatin, Jelly 14K gold (58% Au ), Brass (Zn in Cu), Steel (C in Fe), Liquid solutions Gaseous solutions Air Air, Solid in Solid Liquid in SolidSoda, Vodka, Tea, Gas in Liquid Liquid in Liquid Solid in Liquid Gas in Gas

31. 1 - 31 © Chemeketa Community College: CH117 Solubility How much solute will dissolve in a solvent grams solute mls solution mls solution grams solute mls solution mls solution Factors affecting solubility PolarityPolarity TemperatureTemperature

32. 1 - 32 © Chemeketa Community College: CH117 Polarity vs Solubility Like Dissolves Like NaCl Sugar H 2 O NaCl & Sugar dissolve in H 2 O C 6 H 14 But not in C 6 H 14 NaCl Sugar H 2 O NaCl & Sugar dissolve in H 2 O C 6 H 14 But not in C 6 H 14 OilC 6 H 14 Oil dissolves in C 6 H 14 H 2 O But not in H 2 O OilC 6 H 14 Oil dissolves in C 6 H 14 H 2 O But not in H 2 O Polar Attracts Polar Nonpolar Attracts Nonpolar Factors affecting solubility PolarityPolarity Nonpolar Oil Polar H 2 O

33. 1 - 33 © Chemeketa Community College: CH117 Solubility Polar water attracts to Polar particles Polar water attracts to Polar particles When polar solid dissolves in water, the polar solvent removes The particles from the crystal lattice. Like Dissolves Like

34. 1 - 34 © Chemeketa Community College: CH117 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 -- ++ ++ Solubility

35. 1 - 35 © Chemeketa Community College: CH117 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 - + 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 - + Solubility

36. 1 - 36 © Chemeketa Community College: CH117 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 - + H - H O + H H O - + H H O - + H H O - + H H O - + Solubility

37. 1 - 37 © Chemeketa Community College: CH117 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 - + 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 - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

38. 1 - 38 © Chemeketa Community College: CH117 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 + 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 - + Solubility

39. 1 - 39 © Chemeketa Community College: CH117 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 - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

40. 1 - 40 © Chemeketa Community College: CH117 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 - + 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 - + 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 - + H H O - + Solubility

41. 1 - 41 © Chemeketa Community College: CH117 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 - + 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 - + Solubility

42. 1 - 42 © Chemeketa Community College: CH117 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 - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

43. 1 - 43 © Chemeketa Community College: CH117 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 - + 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 - + H H O - + H H O - + “Like Dissolves Like” Solubility

44. 1 - 44 © Chemeketa Community College: CH117 Temperature vs Solubility

45. 1 - 45 © Chemeketa Community College: CH117 Gases & most liquids less soluble when T increases Solids more soluble SolT T Sol Temperature vs Solubility

46. 1 - 46 © Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Polarity Solution Concentration

47. 1 - 47 © Chemeketa Community College: CH117 Boiling point elevation Adding solute raises the boiling point. 100 o C H 2 O Applications Cooking pasta or hard boiled eggs w/ salt Making Fudge/Candy/Brittle Antifreeze More Solute  Higher Temp (Until solution is saturated) NaCl H 2 O More NaCl

48. 1 - 48 © Chemeketa Community College: CH117 Adding solute lowers the freezing point. H2OH2O 0oC0oC Freezing point depression Applications “Salting” roads in winter Making ice cream Frozen Juice concentrates More Solute  Lower Temp (Until solution is saturated) NaCl H 2 O

49. 1 - 49 © Chemeketa Community College: CH117 The more impurities the more unorganized so the solution needs to be cooler to freeze solid. Freezing point depression

50. 1 - 50 © Chemeketa Community College: CH117

51. 1 - 51 © Chemeketa Community College: CH117 Salt on Ice Solute particles interfere, causing the hydrogen bonding To get disrupted and the ice to melt. Solute particles interfere, causing the water molecules to slow down more. This reduces the temperature. The Sci Guys: Melting Points: Ice cream in a Bag https://www.youtube.com/watch?v=s1CpSrXa1EI&index=4&list=PL7VnnL-CJ- z6LO56_OCnKUTOsnH-7MwC_ https://www.youtube.com/watch?v=s1CpSrXa1EI&index=4&list=PL7VnnL-CJ- z6LO56_OCnKUTOsnH-7MwC_

52. 1 - 52 © Chemeketa Community College: CH117 Compound Interest: Compoundchem.com https://www.youtube.com/watch?v=s1CpSrXa1EI&index=4&list=PL7VnnL-CJ- z6LO56_OCnKUTOsnH-7MwC_ https://www.youtube.com/watch?v=s1CpSrXa1EI&index=4&list=PL7VnnL-CJ- z6LO56_OCnKUTOsnH-7MwC_

53. 1 - 53 © Chemeketa Community College: CH117 Crystallization The more impurities the more unorganized so the more difficult to get large crystals. In Candy: Mix of Sucrose, Glucose, Fructose resists stacking into crystals Single molecular shapes can stack into crystals Mix of molecular shapes resist uniform stacking

54. 1 - 54 © Chemeketa Community College: CH117 Crystallization Smooth ice cream: Mix of Sugars, proteins, Fats, etc. resists stacking into crystals

55. 1 - 55 © Chemeketa Community College: CH117 Crystals

56. 1 - 56 © Chemeketa Community College: CH117 Energy Energy Energy = The capacity to cause change Heat Light

57. 1 - 57 © Chemeketa Community College: CH117 Temperature stays constant Temperature rises Heating Curve Temp constant Remember Changes of State Remember Changes of State Energy

58. 1 - 58 © Chemeketa Community College: CH117 Potential Energy stored Energy Potential Energy = stored Energy (Has potential for motion) Kinetic Energy Energy in motion Kinetic Energy = Energy in motion (Fulfilling its potential) X Energy

59. 1 - 59 © Chemeketa Community College: CH117 Energy calorie: E to raise 1 g H 2 0 by 1 o CE to raise 1 g H 2 0 by 1 o C H2OH2O 1 1 cal 1g 1 o C 1 1 cal 1g 1 o C Specific Heat 1oC1oC

60. 1 - 60 © Chemeketa Community College: CH117 Energy Units of Energy = caloriecal kilocaloriekcal 1000 cal = 1 kcal CalorieCal Cal = kcal jouleJ 4.18 J = 1 cal British Thermal Unit BTU

61. 1 - 61 © Chemeketa Community College: CH117 80 cal to melt ice g 1.00 cal to heat water g o C g o C 540 cal to vaporize g water g water Heat of Vaporization Specific Heat of H 2 O Heat of Fusion Heating Curve Energy

62. 1 - 62 © Chemeketa Community College: CH117 E to raise Temp of 1g substance by 1 o C Fe0.11 Cu 0.093 H 2 O 1.00 Ag 0.057 Au 0.031 Sand 0.19 Al 0.22 cal 1g 1 o C cal 1g 1 o C 0 o C = start Add 1 cal Specific Heat

63. 1 - 63 © Chemeketa Community College: CH117 Specific Heat Fe0.11 Cu 0.093 Ag 0.057 Au 0.031 Sand 0.19 Al 0.22 0 o C = start H 2 O 1.00 E to raise Temp of 1g substance by 1 o C cal g o C cal g o C 1o1o 10 o 30 o 20 o Add 1 cal

64. 1 - 64 © Chemeketa Community College: CH117 High SpHt; Resists change Specific Heat Fe0.11 Cu 0.093 Ag 0.057 Au 0.031 Sand 0.19 Al 0.22 H 2 O 1.00 1o1o 10 o 30 o 20 o Low SpHt; Heats quickly

65. 1 - 65 © Chemeketa Community College: CH117 Specific Heat 30 o C = start Energy gets given back with cooling 1o1o 10 o 30 o 20 oFe0.11 Cu 0.093 H 2 O 1.00 Ag 0.057 Au 0.031 Sand 0.19 Al 0.22

66. 1 - 66 © Chemeketa Community College: CH117 Specific Heat Fe0.11 Cu 0.093 Ag 0.057 Au 0.031 Sand 0.19 Al 0.22 H 2 O 1.00 Energy gets given back with cooling cal g o C cal g o C 70 o 90 o 100 o 99 o 80 o 95 o High SpHt; Resists change Low SpHt; cools quickly

67. 1 - 67 © Chemeketa Community College: CH117 Specific Heat Sand 0.19 H 2 O 1.00 Resists change Stays cold Heats quickly Gets hot Hydrated person Resists change in body temp Dehydrated person Body temp rises quickly & Lowers quickly