1. Chemicals of Life A Unit on Biochemistry

2. Important terms: Atoms: Basic building block of matter.

3. Composition of an atom: Made up of three subatomic particles: Protons + in the nucleus Neutrons neutral in the nucleus Electrons --- electron shell

4. Elements: Substance made up of all one type of atom. Six most common elements found in living organisms: C, H, N, O, P, S hyperlink

6. Molecules/compounds: Two or more atoms bonded together to create a new substance with new properties..

8. Molecules/compounds: Two or more atoms bonded together to create a new substance with new properties. Example: NaCl /Sodium Chloride Sodium White crystal Solid Explosive in water Chlorine Green Gas Very poisonous Sodium Chloride White crystal Solid Not explosive Not poisonous Table Salt

9. Most common compounds in a living organism: Carbohydrates Lipids Proteins Nucleic Acids Water

10. Two types of compounds: Inorganic compounds:  Do not contain carbon  Can not be decomposed  Must be recycled  Examples:  Sand, glass, styrofoam  Soil, rocks, metals and  water

11. Organic Compounds:  Contain carbon  Are decomposed or broken down and nutrients returned to soil  Examples:  Anything living or once living  Dead plants and animals  Proteins, lipids, carbs and nucleic acids

12. Inorganic Compounds found in all living organisms: WATER

13. Water: H 2 O 1. Made up of two hydrogen atoms bonded to one oxygen atom. 2. Atoms bond to form an angular molecule

14. 3. Water is classified as a polar molecule. Polar because like the Earth or a bar magnet it has a partial positive and a partial negative end. + -

15. One of the most important rules in biology is that:

16. Opposites attract:

17. Therefore, one molecule of water’s positive end is attracted to another molecule of water’s negative end giving water many unique properties. Weak Hydrogen bonds hold the molecules together. + - + -

19. Water’s unique characteristics: -1. Water is an inorganic molecule -Contains no carbon -2. Water covers 75% of the Earth’s surface -3. Water makes up 70% to 80% of a living organism -4. Water is made up of two hydrogen atoms and one oxygen atom -5. Water forms an angular molecule -6. Water is a POLAR MOLECULE -has a + and a – end + -

20. 7. Water occurs in three phases -Solid -molecules have a small amount of energy -molecules have just a little movement (just vibrating against each other) -molecules are close together and held in place with hydrogen bonds. -Liquid -molecules gain some energy and some movement -Hydrogen bonds are broken -molecules begin to spread out -Gas -molecules gain a lot of energy - molecules have a lot of rapid movement (enough to escape the surface into the air as a gas ) -molecules widely spaced out

22. PHASE DIAGRAM OF WATER

23. 8. Water displays cohesion: Co= together hesion or hesive = to stick Cohesion is the attraction between like molecules. (one water molecule attracted to another water molecule). This occurs due to the fact that water is a polar molecule and opposites attract. + - + -

24. 9. Water displays adhesion Adhesion – is the tendency of certain dissimilar molecules to cling together due to attractive forces.

25. The water molecules are attracted to the “sides” of the graduated cylinder causing the water to raise up on the sides. Water forms a concaved meniscus. The water molecules are attracted to the sides of the glass container.

26. 10. Water expands when frozen. When frozen, the water molecules slow down and due to their polarity they will line themselves up + to – end thus taking up more volume and lowering it’s density.

27. O H.. O HH H H H H O O SolidLiquid Occupies more volume Occupies less volume

28. 11. Water is known as the UNIVERSAL SOLVENT: It dissolves more substances than any other substance on Earth. To dissolve means that the molecules of one substance are picked up and totally surrounded by water molecules.

29. Demo of salt dissolving In water.

30. Mini Experiment #1 What is cohesion? -waters attraction to other water molecules

31. Mini Experiment #2:

32. Water Alcohol Mini Experiment #3 Cup 1 Cup 2 Ice in water Ice in alcohol Reason why this occurred?

33. Mini Experiment #4 SubstanceSoluble/dissolves Insoluble/does not dissolve Salt Sugar Oil Powder soap

34. Mini Experiment #5 Using the two terms you defined, adhesion and cohesion, explain why the water is able to travel down the string from position A to position B. STRING DEMO

35. 13. Due to its polarity, water is excellent at making two types of mixtures 1. Suspensions 2. Solutions

36. What is a mixture: - 2 or more substances combined but not chemically. -each substance retains it’s own properties. -each substance can be separated from the other. Examples???????

37. Suspensions: A substance is mixed with water and the 2 substances separate. The less dense substance is “suspended above” the more dense substance. Example: Oil and water This happens because water is polar and oil is NONPOLAR (no + or – ends)

38. Blood is a suspension:

39. Solutions: One substance dissolves into another substance. Examples: Kool aid Salt water

40. Cytoplasm is a solution:

41. The Rule : Likes dissolves likes: Polar substances dissolve other polar substances Water dissolves salt Nonpolar substances dissolve other nonpolar substances Gasoline or lighter fluid dissolves oil

42. Parts of a solution: Substance doing the dissolving. (water) Solute: Substance being dissolved. (salt) Solution: Created when the solute DISSOLVES in the solvent. (salt water)

43. Aqueous solution: water is the solvent Saline solution: salt is the solute

44. 3 types of water solutions: Acids, Bases and Neutral

45. Acids: A substance that releases +H ions when dissolved in water.

46. Acidic Solutions: HCl is Hydrogen Chloride

47. – H is +1 and Cl is – 1 therefore it is neutral – Not dangerous to us and our tissues – When HCl is dissolved into water, the H and Cl ions separate. HCl is now known as Hydrochloric Acid – It is now very dangerous to us and our tissues

48. Base: A substance that releases -OH ions when dissolved in water.

49. Basic Solution: NaOH is Sodium Hydroxide

50. Na is +1 and OH is – 1 therefore it is neutral Not dangerous to us When NaOH is dissolved into water, the Na and OH ions separate. NaOH, sodium hydroxide is now very dangerous to us and our tissues

51. Neutral: A substance that release no +H or –OH ions when dissolved in water A substance that releases and equal amount of both the +H and the – OH ions and they cancel each other out. OR

52. Neutral Solution:

53. pH Scale: -measures the strength and weaknesses of an acid (%H+) and of bases (%OH-) -based on a scale of 0 to 14

54. pH scale:

55. pHpH and common substances:

56. Neutralization Reaction: When an acid and a base of equal strength are mixed and cancel each other out creating a neutral substance. HCl + NaOH ----  NaCl + HOH Strong Strong neutral neutral acid base no H or OH H = OH

57. Buffer: A substance which guards against shifts in the pH level. Our blood is an example of a buffer. Blood uses extra H+ and OH- ions substances to help resist pH changes in our body.

58. Lab: Using Acid-Base Indicators

59. Indicator Test: -special chemicals that can show whether a substance is an acid, a base or is neutral. -Two type of indicators: -pH paper: Used to determine the strength or weakness of an acid or a base. -litmus paper: Used to determine the presence of either or both H+ or –OH ions.

60. pH paper:

61. Litmus Paper: -Two types of litmus paper. -RED and BLUE

62. Litmus Paper: Red Litmus Paper - stays red when H+ ions are present. -turns blue when OH- Ions are present. Blue Litmus Paper - turns red when H+ ions are present. -stays blue when OH- Ions are present.

63. Item Result of Test Blue Litmus Red or Blue Red Litmus Red or Blue pH paper Color and Number Strong Acid, Weak Acid Strong Base, Weak Base 1.Benedict’s solution