1. Chapter 2 The Chemistry of Life

2. Objectives 2-1 1.Differentiate between atoms and elements. 2.Analyze how compounds are formed. 3.Distinguish between covalent bonds, ionic bonds, and hydrogen bonds.

3. I. Nature of Matter A. Atoms – Smallest unit of matter that cannot be broken down by chemical means. 1. All matter consists of atoms.matter 2. Atoms consist of protons, neutrons and electrons.Atoms

4. I. Nature of Matter Cont. a. Protons – positive charge in nucleus b. Electrons – tiny, negative charge outside nucleus c. Neutrons- neutral charge in nucleus

5. The Atom

6. I. Nature of Matter Cont. B. Elements – pure substance made of one kind of atomElements 1. Represented by symbols 2. Elements differ in the number of protons. 3. Isotopes – atoms of the same element with different numbers of neutrons

7. Periodic Table of Elements

8. I. Nature of Matter Cont. C. Chemical bond – force that joins more than one atom 1. Compound – Two or more elements chemically joinedCompound 2. Covalent Bonds – two or more atoms share electrons a. A molecule is held together with covalent bonds.

9. I. Nature of Matter Cont. b. Electrons are grouped in different levels. i. The outer level determines bonding. ii. The max. outer level for hydrogen and helium has two electrons. iii. The max. outer level for all other elements is eight.

10. CovalentCovalent bond

12. I. Nature of Matter Cont. c. An atom is stable when its outer electron level is full. d. Atoms react readily when outer electron level is not full. 3. Hydrogen Bonds – weak chemical bonds between polar molecules.Hydrogen molecules

13. I. Nature of Matter Cont. a. Polar molecule – partially negative end and partially positive endPolar b. Partial positive end of one molecule is attracted to the partial negative end of another.

15. I. Nature of Matter Cont. 4. Ionic Bonds – attraction between positively charged ions and negatively charged ions.Ionic

16. I. Nature of Matter Cont. a. Atoms that lack full outer electrons levels will donate or accept electrons to have a full outer electron level. b. Ion – atom with an unequal number of protons and electrons.Ion

17. Ionic Bond

18. II. Water and Solutions Objectives –Analyze the properties of water. –Describe how water dissolves substances. –Distinguish between acids and bases.

19. II Water and Solutions A.Water in living things 1. Storage of energy a. Changes in water temperature happen slowly. b. Aids in maintaining homeostasis.

20. 2. Cohesion and adhesionCohesion A. Cohesion- attraction between substances of the same kind due to hydrogen bonding. B. Adhesion- attraction between different substance due to polarity. ex: Capillary action

21. Cohesion

22. Adhesion

23. B. Aqueous Solutions- one substance is evenly distributed through water.Solutions 1. Polarity a. Ionic compounds and polar molecules dissolve in water. b. Ions become surrounded by water. c. Nonpolar molecules do not dissolve in water.

24. Surface Tension

25. Hydrogen Bonding

26. Nonpolar vs. Polar

27. Cell Membrane

28. 2. Acids and BasesAcids a. Hydrogen ion (H + ) – Broken water molecule forms a positively charged ion b. Hydroxide ion (OH - ) – Broken water molecule forms a negatively charged ion c. Acid- a compound that forms hydrogen ions in water

29. Acids and Bases

30. 2. Acids and bases cont. d. Base – a compound that forms hydroxide ions in water or decreases the number of hydrogen atomsBase e. pH scale – 0 to 14pH i. 0 to 7- acidic ii. 7 – neutral iii. 7-14 – basic iv. Factor of 10 scale

31. pH Scale

32. III. Chemistry of Cells

33. 2-3 Objectives Summarize the characteristics of organic molecules. Compare the structure and function of organic macromolecules.

34. Carbon Compounds: Most non-water matter in your body is made of organic compounds containing carbon.

35. 4 Classes of Organic Compounds: Carbohydrates Lipids Proteins Nucleic Acids

36. A. Carbohydrates:Carbohydrates: 1) Organic compounds made of Carbon, Hydrogen, & Oxygen in a 1:2:1 ratio

38. A. Carbohydrates: 2) Key source of energy 3) Found in most foods, including fruits, vegetables, and grains

40. A. Carbohydrates: 4) Made of single sugars called monosaccharides…2 sugars are disaccharides. monosaccharidesdisaccharides 5) Starch is a carbohydrate that stores energy in plants

41. A. Carbohydrates: 6. Glycogen is a carbohydrate made by animals to store energy

42. A. Carbohydrates: 7. Cellulose is an indigestible carbohydrate that provides structural support for plants

43. B. Lipids:Lipids 1. Mostly insoluble in water 2. Include fats, phospholipids, steroids, and waxesfats

45. B. Lipids: 3. Important part of cell membranes 4. Fats are lipids that store energy

47. Fats a. Contain 3 fatty acids bonded to a glycerol molecule backbonefatty

48. Fats b. Glycerol is a 3-carbon organic molecule c. A fatty acid is a long chain of carbon atoms with attached hydrogen atoms

49. Fats d. Unsaturated fats – liquid at room temperature. Contain double bonds. e. Saturated Fats – Solid at room temperature. No double bonds.

50. Fat

51. C. Proteins 1.Protein – large molecule formed by linked amino acids.Protein 2.Twenty amino acids make up all proteins.amino a. Order and number of amino acids determine protein. b. Amino acids fold and twist into a compact protein.

52. Hemoglobin

53. C. Proteins 3. Importance a. Structural b. Enzymes- speed up chemical reactions c. Immune system d. Muscle contraction

54. Actin and Myosin

55. D. Nucleic Acids 1. Nucleic Acid – long chain of nucleotides, codes for genetic information.Nucleic 2. Nucleotides – contains a sugar phosphate back bone and a base.Nucleotides a. There are 4 bases b. Variation on pattern and number of bases creates genetic variation.

56. DNA

57. D. Nucleic Acid 3. DNA – deoxyribonucleic acid, two strands form a double helix. Contained in chromosomes.DNA 4. RNA – Ribonucleic acid, single or double stranded, involved in manufacture of proteins.RNA

58. E. ATP 1. ATP – Adenosine Triphosphate, Energy storage molecule used by all living things. 2. Cells require ATP to function.

59. ATP

60. IV. Energy and Chemical Reactions Objectives Evaluate the importance of energy to living things. Relate energy and chemical reactions. Describe the role of enzymes in chemical reactions.

61. IV. Energy and Chemical Reactions Energy- the ability to change or move matter. Types- heat, light, mechanical, chemical, Chemical reactions convert store or release energy.

62. A. Energy a. Depicted by chemical equations B. written: reactants  products i. reactant is starting material ii. Product- newly formed substance

63. B. Energy in Chemical Reactions 1. Energy is absorbed or released during a chemical reaction.Energy 2. Metabolism is the sum total of all chemical reactions.

65. C. Activation Energy 1. Activation energy – energy needed to begin a chemical reaction.Activation

66. Activation Energy

67. D. Enzymes 1. Enzymes – substance that increase the speed of a chemical reaction or lower the activation energy. a. Most are proteins. b. Without enzymes chemical reaction would not happen quickly enough to sustain life.

68. Enzymes

69. D. Enzymes Ex: CO 2 + H 2 O  H 2 CO 3\ c. Carbonic anhydrase converts carbon dioxide and water to hydrochloric acid and back.

70. D. Enzymes 2. Enzymes are highly specific.Enzymes a. Substrate- the substance on which an enzyme acts. b. Active site – deep fold on enzyme at which the substrate attaches.

71. D. Enzymes c. Process i. Substrate(s) attach(es) to enzymes active site changing the enzymes shape. ii. Enzyme reduces the activation energy of the reaction iii. Substrate leaves and enzyme returns to the starting position.

72. D. Enzymes d. Factors that affect an enzymes shape affect its activity.Factors i. Temperature ii. pH

73. Temp. affects enzymes