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Transcript
Ch. 2 The Chemistry of Life Name __________________________ Per. ___________ California State Standard covered within this chapter: Cell Biology 1. The fundamental life processes of plants and animals depend on a variety of chemical reactions that occur in specialized areas of the organism's cells. As a basis for understanding this concept: b. Students know enzymes are proteins that catalyze biochemical reactions without altering the reaction equilibrium and the activities of enzymes depend on the temperature, ionic conditions, and the pH of the surroundings. h. Students know most macromolecules (polysaccharides, nucleic acids, proteins, lipids) in cells and organisms are synthesized from a small collection of simple precursors. Read the appropriate section in the textbook and look at the lecture notes before answering the following questions. You must put all answers and definitions in your own words for full credit. Section 2-1 The Nature of Matter Define the following terms in your own words. 1. atom: 2. nucleus: 3. electron: 4. proton: 5. neutron: 6. Diagram and label the structure of an atom. 7. element: The atomic number of an element is the number of protons in the atom. It is also the number of electrons. The atomic mass is determined by adding together the mass of the protons and the mass of the neutrons. Periodic Table of Elements Use the Periodic Table of Elements above and in the back cover of your book to complete the following table. Write the chemical symbol for each of the following elements. Chemical Element 8. Oxygen 9. Carbon 10. Calcium 11. Hydrogen Chemical Element 12. Nitrogen 13. Sodium 14. Chlorine 15. Phosphorus Chemical Symbol O Chemical Symbol It is most important to know what the subatomic particles are, where they are located in an atom, and that atoms of different elements differ because they contain different numbers of protons. First, use the Periodic Table of Elements above to fill in the number of protons, neutrons and electrons. Then sketch each atom’s electron configuration, labeling and coloring protons red, neutrons gray, and electrons blue. Element Atomic Number 16. Hydrogen 1 17. Carbon 18. Oxygen Number Number Number of of of Electron Configuration protons neutrons electrons 1 0 1 19. isotope: 20. radioactive isotope: 21. Describe two beneficial uses of radioactive isotopes. 22. chemical compound: List 2 examples: Describe the different kinds of chemical bonds. Chemical Bond Description 23. Ionic bond 24. Covalent bond 25. Polar covalent bond (p. 40) 26. Hydrogen bond (p. 41) 27. ion: 28. molecule: 29. matter: Section 2-2: Properties of Water Define the following terms in your own words. 30. cohesion: 31. adhesion: 32. mixture: 33. solution: 34. solute: 35. solvent: 36. Describe the properties of water that make it such an important substance for life. Use your lecture notes to assist you in your description. Property Description a. Heat capacity of water b. Cohesion c. Adhesion d. “universal solvent” e. Polarity of water f. exists in all 3 states of matter g. solid form is less dense than liquid 37. Name a substance that would not dissolve well in water. Explain why. 38. How might the fact that ice is less dense that liquid water be important to living things? 39. What does the pH scale actually measure? 40. Complete the table. Proportion of ions Acid hydrogen Contains more _________________ ions Neutral Contains _________________________ Base Contains more _________________ ions pH range Example 0-6.99 Hydrochloric acid Stomach acid Note: A buffer maintains a stable pH in a solution. If there are too many H+ ions (because an acid is added), the buffer will remove H+ ions from the solution. If there are too few H+ ions (because a base is added), the buffer will add H+ ions to the solution. Section 2-3: Chemistry of Cells 41. organic compounds: 42. Carbon has _____ electrons in its outer energy level. As such, carbon is _____ electrons short of filling the outer energy level and being stable. Therefore, carbon readily forms four _____________ bonds with other elements. 43. monomers: 44. polymer: Note: • Polymers of living things are constructed from monomers by a series of reactions called condensation reactions (dehydration reactions). These reactions result in covalent bonds between monomers. • The reverse of a condensation reaction is a hydrolysis reaction. These reactions use water to break apart polymers to produce monomers. Biological Molecules Carbohydrates 45. Carbohydrates can be found in three forms. Complete the following table be providing a description and two examples of each form. Form Description a. monosaccharide b. disaccharide c. polysaccharide 2 Examples for each i. C6H12O6 – glucose ii. i. ii. i. ii. 46. Sucrose is a disaccharide composed of ________________ and __________________, formed through a __________________ reaction. 47. What is the primary function of carbohydrates? Note: Carbohydrates readily dissolve in water and are said to be hydrophilic. 48. Describe the function of each of the following molecules. Carbohydrate Function a. starch b. glycogen c. cellulose Lipids 49. Unlike other organic compounds, lipids do not dissolve in ________________. As such, lipids are said to be hydrophobic. 50. fatty acid: 51. Lipids come in a variety of forms which have different functions. Pay special attention to additional information supplied to you in the table. Form a. Fat Structure Example Function Phosphate head (hydrophilic) attached to 2 fatty acid tails (hydrophobic) Cell membrane (phospholipid bilayer) Separates cell interior from external environment b. Steroid c. Phospholipid 52. Explain the difference between a saturated and an unsaturated fat. 53. How do lipids store energy efficiently? Nucleic Acids 54. What is the monomeric unit for nucleic acids? 55. Draw the basic structure of a nucleotide and label the three different parts of the molecule. 56. Describe the function of the 2 forms of nucleic acids. Form a. DNA which stands for Function ______________________________ b. RNA which stands for ______________________________ Proteins 57. amino acid: 58. Draw the basic structure of an amino acid and label the major functional groups. 59. The covalent bond formed between a nitrogen atom and a carbon atom is called a ________________________. 60. Describe three functions of proteins. 61. Identify each of the levels of protein structure in the diagrams. Include a description of each structure mentioning what type of bond(s) is/are responsible for each. a. ____________________________ ____________________________ b. ____________________________ ____________________________ c. ____________________________ ____________________________ d. ____________________________ ____________________________ Study Tip: Make a Comparative Table for the Macromolecules. An example of some key headings might be the following: Type of Functions of Polymeric Monomeric Unit Polymeric Forms Macromolecule Forms Section 2-4: Chemical Reactions and Enzymes 62. chemical reaction: 63. Products are on the ____________ side of the equation. 64. Reactants are on the _____________ side of the equation. 65. potential energy: 66. kinetic energy: Note: Chemical reactions either store or release energy – Endergonic reactions—absorb and store energy in a reaction – Exergonic reactions—energy is released from reaction 67. activation energy: 68. Draw energy profiles for the following types of reactions. Be sure to label them. Exergonic (energy-releasing) reaction Endergonic (energy-absorbing) reaction 69. Enzymes are proteins that act as ____________________, to speed up chemical reactions. 70. How does an enzyme speed up a chemical reaction? 71. Diagram a model of one of the ways scientists think that enzymes might work (Induced fit Model). Be sure to label the steps of the model (p. 52). 72. Proteins are sensitive to their environment. Changes in pH, temperature, or other qualities can cause a protein to denature. What does it mean for a protein to be denatured? 73. Why does a denatured protein no longer function? 74. Why do extreme high temperatures cause enzymes to denature?