1. Chemistry of Life Unit When water, H2O, is created, hydrogen and oxygen share the electrons The oxygen has a slightly negative charge The hydrogen’s have a slightly positive charge This uneven pattern of charge creates a polar molecule = has a positive side and negative side

2. Water Molecule

3. Hydrogen Bonding Hydrogen Bond = an attraction between a slightly positive hydrogen atom and a slightly negative atom, often oxygen or nitrogen

4. Hydrogen Bonding

5. Properties Related to Hydrogen Bonding Life depends on hydrogen bonds in water High Specific Heat = water resists changes in temp. - helps regulate cells

6. Properties Related to Hydrogen Bonding (cont) Cohesion = attractive forces between particles of the same kind - example: surface tension of water

7. Surface Tension

8. Surface Tension – Floating Paper Clips

9. Catching Fleas with Soapy Water

10. Properties Related to Hydrogen Bonding (cont) Adhesion = the attractive forces between unlike substances - example: meniscus curve in a graduated cylinder

11. Meniscus Curve

12. Properties Related to Hydrogen Bonding (cont) Capillarity = the ability of water to move up through narrow tubes against gravity - due to cohesion and adhesion - example: carnations turning a different color in colored water

13. Carnations in Colored Water

15. Solutions The polarity of water makes it very effective at dissolving many substances Solvent + Solute = Solution Concentration [ ] = amount of solute in a given amount of solvent Saturated = no more solute will dissolve in the solvent

16. Solvent + Solute = Solution

17. Mosquito injects a solution into your body that prevents clotting

18. Other Types of Solutions Solutions can involve different states of matter (not just solvents that are liquids and solutes that are solids). Here are some examples….

19. Other Types of Solutions – Air Air is a gas mixture of mostly Nitrogen (78%), Oxygen (~ 21%), and other gases (~ 1%)

20. Other Types of Solution - Brass Brass is a solid mixture of Copper (~67%) and Zinc (~33%)

21. Other Types of Solutions - Vinegar Vinegar is a liquid solution of two liquids: 95 % Water And 5% Acetic Acid

22. Solutions (cont) Water is the universal solvent. All processes necessary for life take place in water.

23. Acids and Bases Acid = compound that releases a hydrogen ion (H+) when dissolved in water - increases the H+ [ ] Base = compound that remove H+ ions from a solution - lowers the H+ [ ]

24. Acids and Bases (cont) pH scale = amount of H+ ions in a solution 0 to 6 = acidic 7 = neutral 8 to 14 = basic buffer = compound that regulates H+ [ ] - maintains homeostasis

25. Examples of Buffers

26. pH Scale

30. Car Analogy for Organic Compounds Toyota Camry Toyota Supra

31. Organic Compounds Carbon is the building block of life - can form multiple bonds (up to 4), including other carbon atoms More than 90 % of the mass of all living things are composed of combinations of just 4 elements 1) Carbon ( C) 2) Hydrogen (H) 3) Oxygen (O) 4) Nitrogen (N)

33. 1) Carbohydrates Examples sugars starches cellulose glycogen Specifics - contain C, H, and O - main source of usable chemical energy for cells - major part of plant cell wall (made of cellulose) - most basic are simple sugars = monosaccharides (glucose) - bond to form polysaccharides

34. 1) Carbohydrates

35. Field of Cotton

36. 2) Lipids Examples Fats Oils Cholesterol Specifics - contain C, H, and O - store large amounts of energy - cell membrane made up of phospholipids - regulate body responses and control sexual development - are nonpolar molecules (don’t dissolve in water)

38. Saturated Fats (solid at room temp)

39. Unsaturated Fats (liquid at room temp)

40. 3) Proteins Examples Specifics - contain C, H, O, and N - made of monomers called amino acids - 20 different amino acids build proteins - specific sequence determines structure and function

41. Red Blood Cells and Sickle Cell Anemia (SEM 3500x)

42. 4) Nucleic Acids - work together to make proteins Functions: – stores info to build proteins – helps build proteins Types: 1) DNA 2) RNA

43. Chemical Reactions = change substances into different substances by breaking and forming chemical bonds

44. 6O 2 + C 6 H 12 O 6 6CO 2 + 6H 2 O 1. Reactants = substances changed during a chemical reaction (left side) 2. Direction 3. Products = substances made during a chemical reaction (right side)

45. * Chemical reactions release or absorb energy

46. Types of Chemical Reactions Activation Energy = the amount of energy needed to start a reaction - is very high in most chemical reactions (especially in the body)

47. Activation Energy

48. Types of Chemical Reactions (cont) Exothermic = chemical reaction that releases more energy than it absorbs - gives off heat (hot) - ex: cellular respiration

49. Exothermic Reaction

50. Glowsticks

51. Bioluminescence

52. Types of Chemical Reactions (cont) Endothermic = chemical reaction that absorbs more energy than it releases - absorbs heat (cold) - ex: photosynthesis

53. Endothermic Reaction

54. Cold packs

55. Exothermic ReactionEndothermic Reaction

56. Enzymes Catalyst = substance that reduces the amount of activation energy that is needed to start a chemical reaction Catalysts are not changed during a chemical reaction Enzymes = a type of catalyst in living things

57. Enzymes (cont) - almost all are proteins - work best in normal body conditions (temp. and pH) - specific shape allows only certain reactants to bind - fit like a lock and key

58. Lock and Key Model - Enzymes

61. Enzymes (cont) - functions: 1) help bring substrates together and chemical reactions occur 2) decrease the activation energy of the reaction 3) increase the rate of the reaction

62. Enzymes reduce Activation Energy

63. Enzymes (cont) - Reaction 1 requires more activation energy than Reaction 2 - Reaction 3 has less activation energy due to a catalyst being used

64. Enzymes in Your Life