People and the Earth's Ecosystem for students.pptx

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1. MODULE 1 BIOCHEMISTERY PREPARED BY: PK BESANA, RMT, MLS (ASCPI)CM

2. “Towards a Better Living”

3. OBJECTIVES Understanding the chemical processes in living cells at a molecular level Understanding the origin of life on earth. Integrate biochemical knowledge to maintain heat. Understand and treat diseases effectively

4. Science of the chemical basis of life Study of chemical constituents of living cells and the reactions and processes they undergo WHAT IS BIOCHEMISTRY?

5. CELLS are highly organized. Living processes consist of thousands of chemical reactions. certain fundamental reaction pathways are found in all living organisms. All organisms use the same types of molecules. The instructions for growth, development and reproduction are encoded in each organisms’ nucleic acids. PRINCIPLES IN UNDERSTANDING LIVING ORGANISMS

6. The biochemistry of the nucleic acids lies at the heart of genetics. Harmonious balance of biochemical reactions Disease reflects abnormalities

7. CELLULAR ORGANIZATION All living cells are made up of cells and DNA MOVEMENT All organism can engage in movement which may occur internally or even in a cellular level REPRODUCTION Organisms can multiply through sexual or asexual reproduction METABOLISM A term which is applied to the collection of different chemical reactions occurring in the body or a cell HOMEOSTASIS Organism is capable of maintaining a stable internal environment CHARACTERISTICS OF LIVING THINGS

8. HEREDITY Genetic information can be passed on from one generation to another SENSITIVITY Response to a stimuli GROWTH & DEVELOPMENT Increase of the size of the living things and change in bodily function over time EVOLUTION Body adapts with the change in the environment CHARACTERISTICS OF LIVING THINGS

9. THE CELL Basic morphological and functional unit of all living things Smallest living part of the body Comprises the tissue that make up the organs of multicellular organisms Cells comprising the human body form a tightly knit and highly organized society

10. THE CELL CELLS TISSUE ORGANS ORGAN SYSTEM

11. PROKARYOTIC No nucleus , no organelles, small amount of DNA Pro means before; karyon means nucleus or kernel TYPES OF CELLS

12. EUKARYOTIC Nucleated, w/ multiple organelles and more DNA arranged in multiple, linear chromosomes Eu means to true; karyon means nucleus or kernel. TYPES OF CELLS

13. DNA helices for dna unwinding Polymerase for manufacturing new DNA strands follows a semi-conservative replication pattern Lagging strands Starts with new DNA strand with a small primer RNA SIMILARITIES OF PROKARYOTIC & EUKARYOTIC CELLS

14. Average eukaryotic cell has 25 times more DNA Major difference between the two types is replication DIFFERENCES OF PROKARYOTIC & EUKARYOTIC CELLS

15. Prokaryotes Eukaryotes Faster, one point of origin Slower, multiple points of origin 2 opposing directions Unidirectional Occurs in the cytoplasm Occurs in the nucleus Telomere replication at the ends of their chromosome No ends to synthesize Short, continuous Only during S-phase 1 or 2 polymerases 4 or more polymerase

16. ELEMENTAL COMPOSITION OF LIVING CELLS

17. FAMILY NAME: ALKANES FUNCTIONAL GROUPS GROUP NAME: ALKENE FAMILY NAME: DOUBLE BOND

18. GROUP NAME: HYDROXYL FAMILY NAME: ALCOHOL FUNCTIONAL GROUPS FAMILY NAME: PHENOLS

19. GROUP NAME: CARBONYL FAMILY NAME: ALDEHYDES FUNCTIONAL GROUPS GROUP NAME: CARBONYL FAMILY NAME: KETONES

20. GROUP NAME: CARBOXYLIC ACID FAMILY NAME: ACIDS FUNCTIONAL GROUPS GROUP NAME: ESTER FAMILY NAME: ESTERS

21. FAMILY NAME: ETHERS FUNCTIONAL GROUPS GROUP NAME: AMINO FAMILY NAME: AMINE

22. GROUP NAME: AMIDO FAMILY NAME: AMIDE FUNCTIONAL GROUPS GROUP NAME: THIOL FAMILY NAME: THIOLS

23. Nucleic Acids Proteins Polysaccharides Lipid FOUR CLASSES OF MACROMOLECULES WITHIN LIVING CELLS

24. All living organisms consist of chemical reactions catalyzed by Enzymes . Collectively, the reactions in a living organism is known as Metabolism . BIOCHEMICAL PROCESSES & REACTIONS

25. BIOCHEMICAL PROCESSES & REACTIONS

26. Acquisition and utilization of energy Synthesis of molecules needed for cell structure and functioning Removal of wastes products PRIMARY FUNCTIONS OF METABOLISM

27. Nucleophilic Substitution Elimination Addition Isomerization Oxidation Reduction Hydrolysis BIOCHEMICAL REACTIONS

28. Nucleophile : electron-rich species that reacts with an electron poor species Substitution : one group replaces another Electrophiles : atoms or groups that are transferred from one nucleophile to another NUCLEOPHILIC SUBSTITUTION

29. NUCLEOPHILIC SUBSTITUTION

30. A double bond is formed when 2 atoms in a molecule are removed. ELIMINATION

31. 2 molecules combine to form a single molecule Hydration is the most common addition reaction ADDITION

32. Intramolecular shift of atoms or groups ISOMERIZATION

33. “Redox Reactions” Transfer of electrons from a donor (reducing agent) to an electron acceptor (oxidizing agent) When reducing agents donate they become oxidized . When oxidizing agents accepts electrons they are reduced . OXIDATION REDUCTION

34. OXIDATION

35. REDUCTION

36. Cleavage of covalent bond by H2O Involves nucleophilic substitution at a saturated carbon or carbonyl carbon HYDROLYSIS

37. HYDROLYSIS

38. Weak attraction between an electronegative atom in one molecule & a H+ atom in another molecule H+ in a H2O molecule is attracted to unshared pairs of electron of another H2O molecule HYDROGEN BOND

39. Electrostatic interaction Van der Waals forces Hydrophobic interaction NON-COVALENT BONDING

40. Between oppositely charged atoms or group Involved in hydration of ions Salvation Spheres ELECTROSATIC INTERACTION

41. Between oppositely charged atoms or group Involved in hydration of ions Salvation Spheres VAN DER WAALS FORCES

42. DIPOLE-DIPOLE INTERACTIONS Between polar molecules - (+) end of one molecule directed toward the (-) end of another VAN DER WAALS FORCES

43. DIPOLE-INDUCED DIPOLE INTERACTIONS A permanent dipole induces a transient dipole in a nearby molecule by distorting its electron distribution Between a polar molecule and nonpolar molecule VAN DER WAALS FORCES

44. INDUCED DIPOLE-INDUCED DIPOLE INTERACTIONS A transient dipole in one molecule polarizes the electrons in neighboring molecules VAN DER WAALS FORCES

45. Occurs between H2O and a nonpolar substance Allows the fats to have minimal contact with H2O HYDROPHOBIC INTERACTIONS

46. Ion H2O, a proton combines with a H2O molecule to form hydrated ion H3O IONIZATION OF WATER

47. the dissociation of water may be expressed according to the concept of Law of Mass action as follows: IONIZATION OF WATER  

48. Thus, the equation may be written as: IONIZATION OF WATER  

49. Since the equilibrium constant for the reversible ionization of water is equal to 1.8 x 10 -16 M, the above relationship yields: IONIZATION OF WATER =  

50. When a solution contains equal amounts of hydrogen and hydroxyl ion, it is said to be neutral Dissolved when an ionic or polar substance is dissolved in water, it may change the relative numbers of hydrogen and hydroxyl ion IONIZATION OF WATER

51. Hydrogen ion concentration: 10 to 10 -14 pH scale has been devised acid: H+ donor base: H+ acceptor Strong acids and strong bases dissociates completely in H2O ACID, BASES, AND PH

52. Organic acids (with carboxyl group ) Do not completely dissociate with H2O WEAK ACIDS WEAK BASES Contain amino group

53. STRENGTH OF A WEAK ACID Note: Ka acid dissociation constant

54. Ka values vary over a wide range, therefore: pKa = - logKa STRENGTH OF A WEAK ACID

55. Concentration of H+ Measure of the proton [H+ ] concentration of a solution pH = -log[H+] pH

56. H + or OH- added to solutions to resist pH changes Essential to maintain pH Combine with H+ ion or release H+ under different conditions Conjugate base of a weak acid BUFFERS

57. Alternatively, if the pH increases the weak acid can releases H+ Buffer is created by neutralizing acetic acid with base NaOH When more OH- ions are added, more acidic acid dissociates furnish additional H+ ions to form water BUFFERS

58. Directly proportional to the concentration of the buffer component The more molecules pH buffer present, the more H+ and OH- ion can be absorbed BUFFERING CAPACITY

59. Expresses the relationship between pH and pKa Derived from the equilibrium expression: HENDERSON-HASSELBALCH EQUATION

60. As the pH of the solution changes, the charges of the molecules in the solution can change. Changing charges on biological molecules can drastically affect how they work and even they work at all. WHY DO WE REALLY CARE FOR PH?