1. CH. 1 THE CHEMICAL LEVEL OF ORGANIZATION

2. REVIEW OF Ch. 1 1 a-d. Identify the indicated regions of the body. 1a. 1b. 1c. 1d.

3. 2. What is the primary organ found in the right hypochondriac region? 3. Name an organ found in hypogastric region?

4.  4. When the response to the effect of a stimulus is in the opposite direction it is called _______________ Feedback.

5. CH. 2 THE CHEMICAL LEVEL OF ORGANIZATION 2.1 Elements and Atoms– the Building Blocks of Matter A. Matter :  States of matter: B. Energy : 1. Types

6. 2. Forms of Energy (Text pp. 62-63)  Chemical:  Electrical:  Mechanical:  Radiant or electromagnetic

7. C. Elements & Compounds  Elements:  92, others created  Atomic Symbol  4 elements = 96% of body

8.  Major Elements:  Trace Elements  Derived from: Text Page 51

9. Elemental Deficiencies  Iron (Fe): anemi  Iodine (I): goiter

10. D. Atoms & Subatomic Particles 1. Atom = 2. Atomic Structure & Energy  Nucleus  Protons (p + )  Neutrons (n 0 )  Electrons (e - ) Figure 2.1 E. Atomic Number & Mass 1.Atomic Number: # electrons 2.Atomic Mass TEXT PAGE 25

11. Examples

12. F. Isotopes (text p. 53)  Protons:  Neutrons:  Symbol: H-1 or ¹H  Atomic weight -- Figure 2.3

13. Radioisotopes  *Radioisotope:  Radioactivity—process of spontaneous atomic decay  PET Scan using glucose

14. G. IONS (Text pp. 57-58)  Cations  Anions  Importance:  Know: atoms tend to want 2 or 8 electrons in their outer shell; Omit details on electron shells Example  ATOMION Na Na+ = Cation

15.  IONS …  Anions ATOM ION Cl Cl-

16.  IONS & IONIC COMPOUNDS  Opposite charges attract each other ATOMS IONS  Ionic Compound Na ClNa+ Cl-

17. 2.2 Chemical Bonds  Bonds:  Molecules  Compound Figure 2.4

18. A. Ions and Ionic Bonds Figure 2.6, step 2 Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Cl Na

19. Crystals Figure 2.6, step 3 +– Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Sodium ion (Na + )Chloride ion (Cl – ) Sodium chloride (NaCl) ClNaCl Na cationanion

20. B. Covalent Bonds: Figure 2.7a

21. 2 Types of Covalent Bonds 1. Non-polar covalent: 2. Polar bonds:  Polar Molecule:  Why chemicals dissolve in water: Figure 2.8

22. Example: double bond ( Text p. 52) Figure 2.7b

23. Comparison of Ionic, Polar & Nonpolar Covalent Bonds Figure 2.9

24. C. Hydrogen Bonds (p. 35) Figure 2.9 Between: Molecules/compounds, not individual atoms in one molecule or compound Created by: Polarity Strength of Bond:

25. 2.3 Chemical Reactions A. The Role of Energy in Chemical Reactions - chemical energy Figure 2.10a

26. B. Characteristics of Chemical Reactions - Reactants - Products - Chemical Equations Na + Cl  NaCl Figure 2.10a Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Sodium ion (Na + )Chloride ion (Cl – ) Sodium chloride (NaCl) ClNaCl Na

27. C. Types of Chemical Reactions 1. Synthesis Reactions Figure 2.10a

28. 2. Decomposition Reactions: Figure 2.10b

29. 3. Exchange reaction (AB + C  AC + B) Figure 2.10c

30. D. Reversibility of Chemical Reactions A + B  ----  AB  Changing the concentration of one or more chemicals in the reaction affects the direction of the reaction.  If increase concentration of a chemical on one side, makes reaction go more to the opposite side (more of the chemicals on the opposite side are made).  If decrease the concentration of a chemical on one side, makes reaction go more to that same side (more of the chemicals on the same side are made). Example: H 2 CO 3  -----  HCO 3 - + H+ -If more H+ (acid) is added, then more Carbonic Acid (a weak acid) is produced -If decrease H+ by adding OH- (they react to produce water), then makes more bicarbonate and H+.

31. E. Factors Influencing the Rate of Chemical Reactions Temperature Concentration Pressure Catalysts - Enzymes

32. 2.4 Inorganic Compounds Essential to Human Functioning Types of Chemicals  Organic compounds:  Examples:  Biochemicals  Inorganic compounds:

33. 2.4 Inorganic Compounds Essential to Human Functioning A. WATER = 60-80%  Functions  Lubricant/cushioning  Heat Sink  Chemical Reactions ( text p. 59)  Dehydration Synthesis  Hydrolysis  Solvent of living things  Solutioins  Solvent  Solute  Concentration of Solutions: % solute = (amount solute) (total amount) X 100%

34.  *Colloids  *Suspensions

35. B. SALT: ionic compounds not having H+ or OH- C. ACIDS and BASES 1. Have H+ and OH- 2. Proton (H+) donors and acceptors 3. pH  pH scale

36. Figure 2.12 4. BUFFERS—chemicals that can regulate pH change  Are composed of a weak acid and its weak base  Example: Carbonic acid—Bicarbonate system H 2 CO 3  -----  HCO 3 - + H+ If H+ is added to the solution: If OH- is added to the solution:

37. 2.5 Organic Compounds Essential to Human Functioning  Carbon & Covalent Bonding  Macromolecules  Polymers and Monomers:  Functional Groups  Text page 64, Table 2.1 A. Carbohydrates 1. Elements: 2. Functions:  ATP  Cell Recognition 3. Saccharides = Sugars

38. 4. Three Forms  Monosaccharides  Examples (Text p. 65)  Disaccharieds  Examples (Text p. 66)  Polysaccharides  Examples (Text p. 67)

39. 5. Isomers Isomers Glucose   Glucose

40. 7. Combined w other biochemicals  Glycolipids  Glycoproteins Lipid Galactose Glycolipid

41. B. Lipids 1. Contain Elements:  Ratio 2. In water 3. Functions:

42. 4. Types  Triglycerides = Neutral Fats  Composition  Saturated vs. Unsaturated vs. Trans Fats  Omega-3 fatty acids  Phospholipids =  Function  Steroids  Prostaglandins P

43. C. Proteins 1. Subunit =  Elements:  NH 2 (amine) and COOH (carboxyl)  R- group: 2. Peptide Bond: dehydration synthesis Figure 2.16 Structure of amino acid R

44. 3. Structural Levels of Proteins (Text p. 73) Figure 2.18a–c Secondary tend to be fibrous and so form structures Primary = the sequence of amino acids. Proteins do not remain in this form

45. Structural Levels of Proteins … Figure 2.18b,d,e Tertiary have a unique shape that is important to their function

46. 4. Protein Denaturation = Figure 2.19b

47. 5. over half body’s organic matter 6. Combine with other biochemicals  Glycoproteins & Proteoglycans  Lipoproteins 7. Functions:  Build Structures  Hormones  Carry Oxygen & Carbon Dioxide  Buffers  Transport substances across the cell membrane  Enzymes  details next slide Hemoglobin Collagen

48. 7. Enzymes and Enzyme Activity  Enzymes =  General Function–Catalyst  Characteristics of Enzymes  Shape  Recycling  Cofactors  Coenzymes  “ase” ending  Mechanism of Action  Next Slide Enzyme Reactants Products

49. Figure 2.21 Active site Amino acids Enzyme (E) Enzyme-substrate complex (E-S) Substrates (S) H2OH2O + Mechanism of Enzyme Activity ( Steps on pp. 74) Substrate Active Site Energy of Activation

50. Figure 2.21 Active site Amino acids Enzyme (E) Enzyme-substrate complex (E-S) Internal rearrangements leading to catalysis Substrates (S) H2OH2O +

51. Figure 2.21 Active site Amino acids Enzyme (E) Enzyme-substrate complex (E-S) Internal rearrangements leading to catalysis Dipeptide product (P) Free enzyme (E) Substrates (S) Peptide bond H2OH2O +

52. D. Nucleic Acids (Text pp. 74-76) 1. Nucleic Acids = 2. Types: DNA and RNA 3. Elements 4. Nucleotides:  Phosphate  Monosaccharide  Nitrogenous Base  Purines: Adenine and Guanine  Pyrimidines: Cytosine, Thymine, and Uracil 5. Dehydration Synthesis: sugar of one nucleotide to phosphate of another nucleotide 6. Overview of DNA and RNA

53. DNA  Nitrogenous Bases: A, G, C, T  Sugar =  Double Helix  Complementary bases  Function RNA  Sugar =  U replaces T  Single stranded  Function Released mRNA

54.  Function: -Hydrolysis of phosphates Food + O2 + ADP + Pi ATP + CO2 -Phosphorylation ATP + H2O ADP/AMP + Pi + Energy energy transfer energy released 7. Other Related Chemicals Adenosine Triphosphate (ATP) (Text p. 77)

55. Figure 2.21 + ADP Solute Contracted muscle cell Product made Relaxed muscle cell Reactants Transport work Mechanical work Chemical work Membrane protein Solute transported Energy liberated during oxidation of food fuels used to regenerate ATP ATP P P P X Y (a) (b) (c) YX P P + Adenosine Triphosphate (ATP) … Released Energy is used for:

56. END

57. REVIEW QUESTION 1. What is the atomic number and atomic mass of each of the above atoms?

58. 4.What sort of chemical reactions do you suppose would be happening during digestion? What about when your body is making more bone? Review Question

59. 5. What are the 4 major groups of biological organic molecules? What is a major function of each? Review Question

61. REVIEW QUESTION  What are 2 variables that can distort the active site of an enzyme and what is the distortion process called? Dysfunctional Enzyme