2. Macromolecules Most confusing of concepts. What are they? Use of Macromolecules Differentiate Human need

3. Etymology 1886, from macro- + molecule. Apparently coined in "On Macro-molecules, with the Determinations of the Form of Some of Them," by Anglo-Irish physicist G. Johnstone Stoney (1826–1911). Originally of crystals.

4. Etymology Macro- meaning “large,” “long,” “great,” “excessive,” AND…. Molecule – Combination of elements Meaning "molecule composed of many atoms" is from 1935, from German makromolekul (1922).

5. A macromolecule - is a very large molecule commonly created by polymerization of smaller subunits. In biochemistry, the term is applied to the four conventional Biopolymersmolecule polymerization biochemistry nucleic acids proteins carbohydrates as well as non-polymeric molecules with large molecular mass such as lipids and macrocycles.lipids macrocycles

6. The individual constituent molecules of macromolecules are called monomers (mono=single, meros=part).monomers

7. SPONCH What is SPONCH?

8. SPONCH S= Sulfur P= Phosphorus O= Oxygen N= Nitrogen C= Carbon H= Hydrogen 6 most important elements to life

9. Matter Anything that occupies space and has mass

10. Element Simplest form of matter, cannot be broken down chemically into a simpler kind of matter

11. Periodic Table of Elements Organized table of elements discovered so far Organized according to atomic structure and chemical characteristics

12. Atoms and Atomic Structure Atoms are the simplest form of an element that keeps all the properties of the element

13. Model of the Atom Parts of the atom: –Protons (+), Neutrons and Electrons (-) –Nucleus: central core of the atom that contains Protons Neutrons –Electrons orbit the nucleus

14. Determining Atomic Structure Using the Periodic Table Atomic number = # of protons and is smaller number by the symbol Atomic mass number = # of protons + # of neutrons Assume for now that protons =electrons

15. Practice Element# protons# neutrons# electrons hydrogen101 helium carbon oxygen sodium chlorine argon sulfur

16. Practice Element# protons# neutrons # electrons hydrogen101 helium222 carbon666 oxygen888 sodium111211 chlorine171817 argon182218 sulfur16

17. Types of Bonds COVALENT – strong bond between elements IONIC- attraction between elements due to opposite charges (weaker than covalent) HYDROGEN – weakest type of bond

18. Covalent Sharing of electrons to fill the valence shell Examples– methane (CH 4 ) and carbon dioxide (CO 2 )

19. Ionic One element gains electrons becoming ____ The other element loses electrons becoming _____________ Opposites attract Ionic compounds Dissolve easily in water –EX. NaCl

20. Hydrogen bonds Caused by partial positive and negative charges Water is best example ﮦ - ﮦ +

21. How does salt dissolve in water? Na+ and Cl – Ions become attracted to the partial charges on water

22. Biology I know the following… *atomic mass *atomic number *how to find # of protons *how to find # of neutrons *how to find # of electrons *atomic structure (drawings) *types of bonds Today’s Agenda:

23. QUIZ on Basic Chem. 2-1

24. Chemistry Basics Quiz ElementAtomic Mass Atomic Number # of protons # of neutron s # of electron s Li Lithium He Helium B Boron Na Sodium

25. Draw the following atoms CarbonOxygen WATER H 2 O

26. CARBON – the building block of life! DRAW Carbon Carbon is able to covalently bond with up to four other elements or form double and triple bonds with other carbon atoms.

27. Carbon Carbon chains make up many structures of living organisms. Varying carbon chains’ structure and/or adding various atoms and molecules to the carbon chain will change it’s function

28. MAKE CH 4 * MAKE C 2 H 6 * MAKE C 2 H 4

29. Group of 4 Make… C 4 H 10 – two different ways

30. Ring Forms of Carbons Make C 4 H 8 with NO DOUBLE BONDS

31. FUNCTIONAL GROUPS Add a hydroxyl group (-OH) to a 2 carbon chain You just made ethanol – an alcohol that destroys liver cells

32. MACROMOLECULES 4 Large Molecules Important to Life –Carbohydrates –Lipids –Proteins –Nucleic Acids

33. Stuff to know! Chapter 2-1 Atomic # Atomic mass Atomic structure Ionic bonds Covalent bonds Hydrogen bonds Water chemistry –Solutions,Solvents,pH – polarity Chapter 2-3 Carbon chem Carbohydrates Lipids Proteins Nucleic Acids

34. CARBOHYDRATES (CH 2 O) n Monomers = monosaccharides –Examples = glucose, fructose and galactose (all 3 = C 6 H 12 O 6 so they are isomer) Functions= provides energy (glucose is energy source for cells

35. Two linked = disaccharides –Examples = sucrose (glucose and fructose) and lactose

36. Polymer = polysaccharides –Examples =glycogen (animals) starch (plants)

37. Why “bulk-up” on carbs? Why not eat carbs?

38. CONDENSATION REACTION

39. HOW WOULD THIS GET BROKEN DOWN? HYDROLYSIS H20H20

40. PROTEINS Monomers = amino acids All amino acids have –Amine group (NH 2 ) –Carboxyl group (COOH) R-groups differ

41. Dipeptide

42. FUNCTIONS of PROTEINS Structural Hormones Transport Histones ENZYMES!!!

43. Lock and Key Model

44. What symptoms would you have if you had sickle cell anemia?

45. 1 amino acid is wrong in the hemoglobin sequence = mis-shaped RBCs

46. LIPIDS MONOMERS = fatty acids Saturated Unsaturated

47. COMPLEX TRIGLYCERIDES PHOSPHOLIPIDS WAXES

48. FUNCTIONS TRIGLYCERIDES – insulation and energy storage PHOSPHOLIPDS – main component in cell membranes

49. HARDENING OF THE ARTERIES Fats such as cholesterol and saturated fatty acids build up in arteries What other factors contribute to arteriosclerosis?

50. include that consist of which contain that consist of which contain Section 2-3 Concept Map

51. Carbon Compounds include that consist of which contain that consist of which contain Section 2-3 Concept Map CarbohydratesLipidsNucleic acidsProteins Sugars and starches Fats and oilsNucleotidesAmino Acids Carbon, hydrogen, oxygen Carbon, hydrogen, oxygen Carbon,hydrogen, oxygen, nitrogen, phosphorus Carbon, hydrogen,oxygen, nitrogen,

52. WATER CHEMISTRY 2-2

53. 2–2 Properties of Water A.The Water Molecule 1.Polarity 2.Hydrogen Bonds B.Solutions and Suspensions 1.Solutions 2.Suspensions C.Acids, Bases, and pH 1.The pH Scale 2.Acids 3.Bases 4.Buffers Section 2-2 Section Outline

54. Hydrogen bonds Caused by partial positive and negative charges Water is best example ﮦ - ﮦ +

55. Cl - Water Cl - Na + Water Na + Section 2-2 Figure 2-9 NaCI Solution

56. Section 2-2 Figure 2-9 NaCI Solution Cl - Water Cl - Na + Water Na +

57. Solutions Ions break away from each other and form hydrogen bonds with water (because its polar) Solute- the substance that is dissolved Solvent- almost always water, substance in which the solute is dissolved Ex. Koolaid –Solute- koolaid powder –Solvent- water

58. Suspension Materials do not dissolve when placed in water, instead the water molecules keep them floating Blood- cells are floating in water solution

59. H2O sometimes breaks down into H+ and OH-

60. Oven cleaner Bleach Ammonia solution Soap Sea water Human blood Pure water Milk Normal rainfall Acid rain Tomato juice Lemon juice Stomach acid Neutral Increasingly Basic Increasingly Acidic Section 2-2 pH Scale indicates the concentrion of H+ ions in water Acids have higher concentration of H+, bases have higher concentration of OH- The higher the pH, the more BASIC the solution. The lower the pH, the more ACIDIC the solution.

62. Buffers Weak acids and bases that reacts with other acids and bases to change the pH. In the body, buffers help maintain homeostasis Ex. Blood needs to stay within 6.5 to 7.5. Stomach needs to stay around 3. Peptobismo (buffer) raises stomach acid if your stomach is too acidic.

63. 1. What are the reactants when wood burns? Reactants are oxygen and cellulose. 2. What are the products when wood burns? Products are carbon dioxide and water 3. What kinds of energy are given off when wood burns? Light and heat are given off. Some students may also mention sound (the crackling of a fire). 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy? To start a fire, you must light it with a match and kindling. You are giving the wood some energy in the form of heat. 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire? Once the fire gets going, it gives off enough heat to start more of the wood burning. Section 2-4 Interest Grabber continued

64. 2–4Chemical Reactions and Enzymes A.Chemical Reactions B.Energy in Reactions 1.Energy Changes 2.Activation Energy C.Enzymes D.Enzyme Action 1.The Enzyme-Substrate Complex 2.Regulation of Enzyme Activity Section 2-4 Section Outline

65. Reaction pathway without enzyme Activation energy without enzyme Activation energy with enzyme Reaction pathway with enzyme Reactants Products Section 2-4 Effect of Enzymes

66. Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions

67. Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions

68. Enzyme/Substrate Complex

69. CATALASE AND H 2 O 2