Macromolecules

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

2. 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.

3. 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).

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

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

6. SPONCH What is SPONCH?

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

8. Matter • Anything that occupies space and has mass

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

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

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

12. 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

13. 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

14. Practice

15. Practice

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

17. Covalent • Sharing of electrons to fill the valence shell • Examples– methane (CH4) and carbon dioxide (CO2)

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

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

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

21. Today’s Agenda: 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

22. QUIZ on Basic Chem. • 2-1

23. Chemistry Basics Quiz

24. Carbon Oxygen Draw the following atoms WATER H2O

25. 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.

26. 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

27. MAKE CH4 * MAKE C2H6 * MAKE C2H4

28. Group of 4 Make… • C4H10 – two different ways

29. Ring Forms of Carbons • Make C4H8 with NO DOUBLE BONDS

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

31. MACROMOLECULES • 4 Large Molecules Important to Life • Carbohydrates • Lipids • Proteins • Nucleic Acids

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

33. CARBOHYDRATES (CH2O)n • Functions= provides energy (glucose is energy source for cells • Monomers = monosaccharides • Examples = glucose, fructose and galactose (all 3 = C6H12O6 so they are isomer)

34. Two linked = disaccharides • Examples = sucrose (glucose and fructose) and lactose

35. Polymer = polysaccharides • Examples = glycogen (animals) starch (plants)

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

37. CONDENSATION REACTION

38. HOW WOULD THIS GET BROKEN DOWN? H20 HYDROLYSIS

39. PROTEINS • Monomers = amino acids • All amino acids have • Amine group (NH2) • Carboxyl group (COOH) • R-groups differ

40. Dipeptide

41. FUNCTIONS of PROTEINS • Structural • Hormones • Transport • Histones • ENZYMES!!!

42. Lock and Key Model

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

44. 1 amino acid is wrong in the hemoglobin sequence = mis-shaped RBCs

45. LIPIDS • MONOMERS = fatty acids • Saturated • Unsaturated

46. COMPLEX • TRIGLYCERIDES • PHOSPHOLIPIDS • WAXES

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

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

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

50. Carbohydrates Lipids Nucleic acids Proteins Sugars and starches Fats and oils Nucleotides Amino Acids Carbon, hydrogen, oxygen Carbon, hydrogen, oxygen Carbon, hydrogen,oxygen, nitrogen, Carbon,hydrogen, oxygen, nitrogen, phosphorus Concept Map Section 2-3 Carbon Compounds include that consist of that consist of that consist of that consist of which contain which contain which contain which contain