1. Important Biological Molecules Biology 1114

2. Important Inorganic Compounds Water Acids, Bases, Salts

3. Inorganic Compounds Small Ionic Bonds Water Acids Bases Salts

4. Water Most Abundant Substance in Cells 98% Body Mass Polar Molecule Solvent Reactant / Decomposition Reactions Cohesive Properties Expands upon Freezing Acts as Acid/Base Temperature Buffer Thermal Conductance

5. Water occurs in three states. Ice is less dense than liquid water and therefore ice floats.

6. Acids, Bases, Salts Acids Dissociate into H +1 and anions HCl  H +1 + Cl -1 Bases dissociate into OH -1 and cations NaOH  OH -1 + Na +1 Salts dissociate into anions and cations neither of which is H +1 or OH -1 NaCl  Na +1 + Cl -1

7. pH = -log[H +1 ]

8. To clean a toilet: Pour a can of Cola into the toilet bowl. Let the "real thing" sit for one hour, then flush clean. The citric acid in Coke removes stains from vitreous china. To remove rust spots from chrome car bumpers: Rub the bumper with a crumpled-up piece of Reynolds Wrap aluminum foil dipped in Cola. To clean corrosion from car battery terminals: Pour a can of Cola over the terminals to bubble away the corrosion. To loosen a rusted bolt: Applying a cloth soaked in Cola to the rusted bolt for several minutes.

11. pH Buffer Stabilizes the pH inside a cell Can be either an Acid or a Base

12. This figure shows the major organs that help control the blood concentrations of CO 2 and HCO -3, and thus help control the pH of the blood. Removing CO 2 from the blood helps increase the pH. Removing HCO -3 from the blood helps lower the pH.

13. Important Organic Compounds Carbohydrates Lipids Proteins Nucleic Acids

14. Organic Compounds Contain Carbon and Hydrogen Carbon has Four Bonding Sites Covalently Bonded Large Molecules

15. Functional Groups

16. Living Cells Synthesize By Functional Group Transfer Electron Transfer Rearrangement Condensation Cleavage

17. Carbohydrates 1.Synthesis of Amino Acids and Fats 2.Function as Food Reserves 3.Fuel Cell Activities

18. Monosaccharide

19. Formation of Sucrose Disaccharide

20. In this molecule, sugar monomers (e.g. glucose; red hexagons) are fastened together with covalent bonds (black lines) to form a larger molecule called a Polysaccharide.

21. Sample Carbohydrates 1.Carbon, Hydrogen and Oxygen 2.CH 2 O 3.Sugars 4.Starches 5.Cellulose

22. Isomers Glucose C 6 H 12 O 6 Fructose C 6 H 12 O 6 Isomers are two or more molecules with the same chemical formula but different structures and properties.

23. Uses Short Term Energy Storage Intermediate Energy Storage Composing Cellular Components

24. Lipids 1.Long Term Energy Storage 2.Carbon, Hydrogen, Oxygen 3.Lack 1:2:1 Ratio 4.Nonpolar

25. Simple Lipids Fats and Glycerides Containing an Alcohol Called Glycerol and a Fatty Acid. Monoglyceride = 1 Molecule Glycerol + 1 Molecule Fatty Acid Diglyceride? Triglyceride?

26. Phospholipid

27. These Molecules Twist so that the Polar End Turns Toward Water and the Nonpolar End Turns Away from Water

31. Linda Hamilton Terminator I

32. Linda Hamilton Terminator II

35. Cholesterol and Artherioschlerosis

36. 1 is Lumen Opening 2 is Plaque (Fat) 3 is Artery Wall

40. Saturated has all single bonds between adjacent carbons. These are hard to break. Unsaturated has double or even triple bonds between some of the adjacent carbon atoms. These are relatively easy to break.

42. Uses Building Blocks of Cell Membranes Information Transfer Through Hormones Energy Storage Units

43. Proteins 1.Carbon, Hydrogen, Oxygen and Nitrogen (Sulfur) 2.Accounts for 50% Dry Weight of Living Organisms 3.Functions Include a. Structure b. Transport c. Regulatory d. Catalysis e. Locomotion

44. Amino Acid with Alpha Carbon

47. Denaturation occurs when the normal bonding patterns are disturbed causing the shape of the protein to change. This can be caused by changes in temperature, pH, or salt concentration. For example, acid causes milk to curdle and heat (cooking) causes egg whites to coagulate because the proteins within them denature.pH

48. Nucleic Acids 1.Energy Currency 2.Information Transfer 3.Built From Smaller Building Blocks Called Nucleotides

49. Nucleotide is made of a nitrogenous base, a sugar, and a phosphate group.

50. Nucleotides Form Genes Genes Determine Hereditary Traits Purine or Pyrimidine Pentose Sugar (Deoxyribose or Ribose) Phosphates (1 to 3)

51. Nucleotides Depending on the Number of Phosphates and the Identity of the Base Nucleotides are Abbreviated. ATP= Adenine Triphosphate CDP= ? GMP= ?

52. Nucleotides Purines 1. Double Ring Structure 2. Adenine and Guanine Pyrimidine 1. Single Ring Structure 2. Thymine, Uracil, and Cytosine

55. Nucleoside Base Distribution in DNA Organism Base Composition (mole %)Base Ratios Ratio (A+T)/(G+C) AGTCA/TG/C Human30.919.929.419.81.051.001.52 Chicken28.820.529.221.51.020.951.38 Yeast31.318.732.917.10.951.091.79 Clostridium perfringens 36.914.036.312.81.011.092.70 Sarcina lutea 13.437.112.437.11.081.000.35

56. Differences DNA 1. Double Stranded 2. Deoxyribose 3. A-T and G-C RNA 1. Single Stranded 2. Ribose 3. A-U and G-C

57. Types of RNA Messenger RNA –Directs the incorporation of amino acids into proteins. Ribosomal RNA –Type of RNA molecule that forms ribosomes Transfer RNA –Type of RNA that brings amino acids to the ribosomal site where they are incorporated into proteins.

58. Review

59. Remember we also need minerals and vitamins for good health.