3. Table of Contents – pages iv-v Unit 1: What is Biology? Unit 2: Ecology Unit 3: The Life of a CellThe Life of a Cell Unit 4: Genetics Unit 5: Change Through Time Unit 6: Viruses, Bacteria, Protists, and Fungi Unit 7: Plants Unit 8: Invertebrates Unit 9: Vertebrates Unit 10: The Human Body

4. Table of Contents – pages iv-v Unit 1: What is Biology? Chapter 1: Biology: The Study of Life Unit 2: Ecology Chapter 2: Principles of Ecology Chapter 3: Communities and Biomes Chapter 4: Population Biology Chapter 5: Biological Diversity and Conservation Unit 3: The Life of a CellThe Life of a Cell Chapter 6: The Chemistry of LifeThe Chemistry of Life Chapter 7: A View of the Cell Chapter 8: Cellular Transport and the Cell Cycle Chapter 9: Energy in a Cell

5. Table of Contents – pages iv-v Unit 4: Genetics Chapter 10: Mendel and Meiosis Chapter 11: DNA and Genes Chapter 12: Patterns of Heredity and Human Genetics Chapter 13: Genetic Technology Unit 5: Change Through Time Chapter 14: The History of Life Chapter 15: The Theory of Evolution Chapter 16: Primate Evolution Chapter 17: Organizing Life’s Diversity

6. Table of Contents – pages iv-v Unit 6: Viruses, Bacteria, Protists, and Fungi Chapter 18: Viruses and Bacteria Chapter 19: Protists Chapter 20: Fungi Unit 7: Plants Chapter 21: What Is a Plant? Chapter 22: The Diversity of Plants Chapter 23: Plant Structure and Function Chapter 24: Reproduction in Plants

7. Table of Contents – pages iv-v Unit 8: Invertebrates Chapter 25: What Is an Animal? Chapter 26: Sponges, Cnidarians, Flatworms, and Roundworms Chapter 27: Mollusks and Segmented Worms Chapter 28: Arthropods Chapter 29: Echinoderms and Invertebrate Chordates

8. Table of Contents – pages iv-v Unit 9: Vertebrates Chapter 30: Fishes and Amphibians Chapter 31: Reptiles and Birds Chapter 32: Mammals Chapter 33: Animal Behavior Unit 10: The Human Body Chapter 34: Protection, Support, and Locomotion Chapter 35: The Digestive and Endocrine Systems Chapter 36: The Nervous System Chapter 37: Respiration, Circulation, and Excretion Chapter 38: Reproduction and Development Chapter 39: Immunity from Disease

9. Unit Overview – pages 138-139 The Life of a Cell The Chemistry of Life A View of the Cell Cellular Transport and the Cell Cycle Energy in a Cell

10. Chapter Contents – page viii Chapter 6 The Chemistry of LifeThe Chemistry of Life 6.1: Atoms and Their InteractionsAtoms and Their Interactions 6.1: Section CheckSection Check 6.2: Water and DiffusionWater and Diffusion 6.2: Section CheckSection Check 6.3: Life SubstancesLife Substances 6.3: Section CheckSection Check Chapter 6 SummarySummary Chapter 6 AssessmentAssessment

11. Chapter Intro-page 140 What You’ll Learn You will relate an atom’s interactions with other atoms to its structure. You will explain why water is important in life. You will compare the role of biomolecules in organisms.

12. 6.1 Section Objectives – page 141 Relate the structure of an atom to the identity of elements. Section Objectives: Relate the formation of covalent and ionic chemical bonds to the stability of atoms.

13. 6.1 Section Objectives – page 141 Section Objectives: Distinguish mixtures and solutions. Define acids and bases and relate their importance to biological systems.

14. An element is a substance that can’t be broken down into simpler chemical substances. Section 6.1 Summary – pages 141-151 Elements Everything – whether it is a rock, frog, or flower – is made of substances called elements.

15. Section 6.1 Summary – pages 141-151 Of the naturally occurring elements on Earth, only about 25 are essential to living organisms. Carbon, hydrogen, oxygen, and nitrogen make up more than 96 percent of the mass of a human body. Natural elements in living things

16. Section 6.1 Summary – pages 141-151 Trace elements Trace elements such as iron and copper, play a vital role in maintaining healthy cells in all organisms. Plants obtain trace elements by absorbing them through their roots; animals get them from the foods they eat.

17. Section 6.1 Summary – pages 141-151 Table 6.1 Some Elements That Make Up the Human Body ElementSymbol Percent By Mass in Human Body Element Symbol Percent By Mass in Human Body Molybdenum Oxygen Carbon Hydrogen Nitrogen Calcium Phosphorus Potassium Sulfur Sodium Chlorine Magnesium Selenium Iron Zinc Copper Iodine Manganese Boron Chromium Cobalt Fluorine O C H N Ca P K S Na Cl Mg 65.0 18.5 9.5 3.3 1.5 1.0 0.4 0.3 0.2 0.1 Fe Zn Cu I Mn B Cr Mo Co Se F trace

18. An atom is the smallest particle of an element that has the characteristics of that element. Section 6.1 Summary – pages 141-151 Atoms: The Building Blocks of Elements Atoms are the basic building blocks of all matter.

19. All nuclei contain positively charged particles called protons (p + ). The center of an atom is called the nucleus (NEW klee us). Section 6.1 Summary – pages 141-151 The structure of an atom Most contain particles that have no charge, called neutrons (n 0 ).

20. Section 6.1 Summary – pages 141-151 The Structure of an atom Nucleus Electron energy levels The region of space surrounding the nucleus contains extremely small, negatively charged particles called electrons (e - ) This region of space is referred to as an electron cloud.

21. Section 6.1 Summary – pages 141-151 The Structure of an atom Because opposites attract, the negatively charged electrons are held in the electron cloud by the positively charged nucleus.

22. Section 6.1 Summary – pages 141-151 Electron energy levels Electrons exist around the nucleus in regions known as energy levels. The first energy level can hold only two electrons. The second level can hold a maximum of eight electrons. The third level can hold up to 18 electrons. Nucleus 8 protons (p+) 8 neutrons (n 0 ) Oxygen atom

23. Section 6.1 Summary – pages 141-151 Electron energy levels Atoms contain equal numbers of electrons and protons; therefore, they have no net charge.

24. Section 6.1 Summary – pages 141-151 Atoms of the same element always have the same number of protons but may contain different numbers of neutrons. Isotopes of an Element Atoms of the same element that have different numbers of neutrons are called isotopes (I suh tophs) of that element.

25. Section 6.1 Summary – pages 141-151 A compound is a substance that is composed of atoms of two or more different elements that are chemically combined. Compounds and Bonding Table salt (NaCl) is a compound composed of the elements sodium and chlorine.

26. Section 6.1 Summary – pages 141-151 Atoms combine with other atoms only when the resulting compound is more stable than the individual atoms. How covalent bonds form For many elements, an atom becomes stable when its outermost energy level is full. Sharing electrons with other atoms is one way for elements to become stable.

27. Section 6.1 Summary – pages 141-151 Two hydrogen atoms can combine with each other by sharing their electrons. How covalent bonds form Each atom becomes stable by sharing its electron with the other atom. Hydrogen molecule

28. Section 6.1 Summary – pages 141-151 How covalent bonds form Click image to view movie.

29. Section 6.1 Summary – pages 141-151 How covalent bonds form The attraction of the positively charged nuclei for the shared, negatively charged electrons holds the atoms together. Hydrogen molecule

30. Section 6.1 Summary – pages 141-151 A covalent bond holds the two hydrogen atoms together. How covalent bonds form A molecule is a group of atoms held together by covalent bonds. It has no overall charge. Water molecule

31. Section 6.1 Summary – pages 141-151 An atom (or group of atoms) that gains or loses electrons has an electrical charge and is called an ion. An ion is a charged particle made of atoms. How ionic bonds form The attractive force between two ions of opposite charge is known as an ionic bond. Click image to view movie.

32. Section 6.1 Summary – pages 141-151 Chemical reactions occur when bonds are formed or broken, causing substances to recombine into different substances. Chemical Reactions Ionic bond + Sodium atom + Chlorine atom Sodium + Ion + Chlorine ― ion Na atom: 11p + 11e ― Cl atom: 17p + 17e ― Na + ion: 11p + 10e ― Cl ― ion: 17p + 18e ―

33. All of the chemical reactions that occur within an organism are referred to as that organism’s metabolism. Section 6.1 Summary – pages 141-151 Chemical Reactions Ionic bond + Sodium atom + Chlorine atom Sodium + Ion + Chlorine ― ion Na atom: 11p + 11e ― Cl atom: 17p + 17e ― Na + ion: 11p + 10e ― Cl ― ion: 17p + 18e ―

34. Section 6.1 Summary – pages 141-151 In a chemical reaction, substances that undergo chemical reactions, are called reactants. Writing chemical equations Substances formed by chemical reactions, are called products.

35. Section 6.1 Summary – pages 141-151 A molecule of table sugar can be represented by the formula: C 12 H 22 O 11. Writing chemical equations The easiest way to understand chemical equations is to know that atoms are neither created nor destroyed in chemical reactions. They are simply rearranged.

36. A mixture is a combination of substances in which the individual components retain their own properties. Section 6.1 Summary – pages 141-151 Mixtures and Solutions Neither component of the mixture changes.

37. Section 6.1 Summary – pages 141-151 A solution is a mixture in which one or more substances (solutes) are distributed evenly in another substance (solvent). Mixtures and Solutions Sugar molecules in a powdered drink mix dissolve easily in water to form a solution.

38. Section 6.1 Summary – pages 141-151 Chemical reactions can occur only when conditions are right. Acids and bases A reaction may depend on: - energy availability - temperature - concentration of a substance - pH of the surrounding environment

39. Section 6.1 Summary – pages 141-151 The pH is a measure of how acidic or basic a solution is. Acids and bases A scale with values ranging from below 0 to above 14 is used to measure pH. More acidic NeutralMore basic

40. Section 6.1 Summary – pages 141-151 Substances with a pH below 7 are acidic. An acid is any substance that forms hydrogen ions (H + ) in water. Acids and bases A solution is neutral if its pH equals seven. More acidic NeutralMore basic

41. Section 6.1 Summary – pages 141-151 Substances with a pH above 7 are basic. A base is any substance that forms hydroxide ions (OH - ) in water. Acids and bases pH 11

42. Section 1 Check Question 1 Which of the following is an element? D. water C. sodium chloride B. carbon A. chlorophyll CA: Biology/Life Sciences 1f

43. Section 1 Check The answer is B. An element can't be broken down into simpler chemical substances. Chemical elements combine in different ways to form a variety of substances useful to living things. CA: Biology/Life Sciences 1f

44. Section 1 Check Table 6.1 Some Elements That Make Up the Human Body ElementSymbol Percent By Mass in Human Body Element Symbol Percent By Mass in Human Body Molybdenum Oxygen Carbon Hydrogen Nitrogen Calcium Phosphorus Potassium Sulfur Sodium Chlorine Magnesium Selenium Iron Zinc Copper Iodine Manganese Boron Chromium Cobalt Fluorine O C H N Ca P K S Na Cl Mg 65.0 18.5 9.5 3.3 1.5 1.0 0.4 0.3 0.2 0.1 Fe Zn Cu I Mn B Cr Mo Co Se F trace CA: Biology/Life Sciences 1f

45. Section 1 Check The smallest particle of an element that has the characteristics of that element is a(n) __________. Question 2 D. atom C. nucleus B. electron A. proton CA: Biology/Life Sciences 1h

46. Section 1 Check The answer is D. Atoms are the basic building blocks of all matter and have the same general structure, including a nucleus and electrons. Elements found in both living and nonliving things are made of atoms. Nucleus Electron energy levels An atom has a nucleus and electrons in energy levels. CA: Biology/Life Sciences 1h

47. Section 1 Check Which of the following can contain two types of particles? D. electrons Question 3 B. protons C. neutrons A. nucleus CA: Biology/Life Sciences 1h

48. Section 1 Check The answer is A. The nucleus is the center of the atom and may contain both positively charged particles and particles that have no charge. Nucleus 8 protons (p+) 8 neutrons (n 0 ) Oxygen atom CA: Biology/Life Sciences 1h

49. Section 1 Check Question 4 B. Sodium and chlorine atoms have no overall electrical charge. A. Sodium and chlorine are sharing electrons in their outer energy levels. Sodium and chlorine combine to form table salt. What do you know to be true? CA: Biology/Life Sciences 1h

50. Section 1 Check Question 4 D. Sodium and chlorine atoms in table salt have full outer energy levels. C. Sodium and chlorine are less stable in the compound sodium chloride. Sodium and chlorine combine to form table salt. What do you know to be true? CA: Biology/Life Sciences 1h

51. Section 1 Check The answer is D. Sodium and chlorine atoms combine because the resulting compound, table salt, is more stable than the individual atoms. Sodium loses an electron in its outer energy level, chlorine gains that electron in its outer energy level, and an ionic bond is formed. CA: Biology/Life Sciences 1h

52. Section 2 Objectives – page 152 Section Objectives Identify how the process of diffusion occurs and why it is important to cells. Relate water’s unique features to polarity.

53. Summary Section 2 – pages 152-156 Water is perhaps the most important compound in living organisms. Water and Its Importance Water makes up 70 to 95 percent of most organisms.

54. Summary Section 2 – pages 152-156 Water is Polar Sometimes, when atoms form covalent bonds they do not share the electrons equally. This is called a polar bond.

55. Summary Section 2 – pages 152-156 Water is Polar A polar molecule is a molecule with an unequal distribution of charge; that is, each molecule has a positive end and a negative end. Water is an example of a polar molecule. Water can dissolve many ionic compounds, such as salt, and many other polar molecules, such as sugar.

56. Summary Section 2 – pages 152-156 Water is Polar Water molecules also attract other water molecules. Weak hydrogen bonds are formed between positively charged hydrogen atoms and negatively charged oxygen atoms. Hydrogen atom Oxygen atom

57. Summary Section 2 – pages 152-156 Water resists changes in temperature. Therefore, water requires more heat to increase its temperature than do most other common liquids. Water resists temperature changes

58. Summary Section 2 – pages 152-156 Water expands when it freezes Water is one of the few substances that expands when it freezes. Ice is less dense than liquid water so it floats as it forms in a body of water.

59. Summary Section 2 – pages 152-156 Early observations: Bownian motion In 1827, Scottish scientist Robert Brown used a microscope to observe pollen grains suspended in water. He noticed that the grains moved constantly in little jerks, as if being struck by invisible objects. This motion is now called Brownian motion. Today we know that Brown was observing evidence of the random motion of atoms and molecules.

60. Summary Section 2 – pages 152-156 The process of diffusion Diffusion is the net movement of particles from an area of higher concentration to an area of lower concentration. Diffusion results because of the random movement of particles (Brownian motion). Three key factors—concentration, temperature, and pressure—affect the rate of diffusion.

61. Summary Section 2 – pages 152-156 The results of diffusion When a cell is in dynamic equilibrium with its environment, materials move into and out of the cell at equal rates. As a result, there is no net change in concentration inside or outside the cell. Material moving out of cell equals material moving into cell

62. Summary Section 2 – pages 152-156 Diffusion in living systems The difference in concentration of a substance across space is called a concentration gradient. Ions and molecules diffuse from an area of higher concentration to an area of lower concentration, moving with the gradient. Dynamic equilibrium occurs when there is no longer a concentration gradient.

63. Section 2 Check Explain why water is important to living organisms. Question 1 Living organisms must have water for life processes, because critical molecules and ions must be free to move and collide, which only happens when they are dissolved in water. Water also transports materials in living organisms, such as in blood or sap. Answer CA: Biology/Life Sciences 1a

64. Section 2 Check How does water's chemical structure impact its role in living organisms? Question 2 Positively charged end Negatively charged end + + ― CA: Biology/Life Sciences 9a, 9g

65. Section 2 Check Because water is polar, it can dissolve many ionic compounds and polar molecules. Water has the property of capillary action that enables plants to get water from the ground. Water also resists temperature changes, which allows cells to maintain homeostasis. CA: Biology/Life Sciences 9a, 9g

66. Section 2 Check Which of the following best describes diffusion? Question 3 B. net movement of particles from area of low concentration to area of high concentration A. slow process resulting from random movement of particles CA: Biology/Life Sciences 1a

67. Section 2 Check D. net movement of particles from high to low concentrations that accelerates when pressure decreases C. rapid process that is unaffected by increases in temperature Which of the following best describes diffusion? Question 3 CA: Biology/Life Sciences 1a

68. Section 2 Check The answer is A. Diffusion is a slow process resulting from the random movement of particles, and is the net movement of particles from areas of high concentration to areas of lower concentration. CA: Biology/Life Sciences 1a

69. 6.3 Section Objectives – page 157 Classify the variety of organic compounds. Section Objectives: Describe how polymers are formed and broken down in organisms. Compare the chemical structures of carbohydrates, lipids, proteins, and nucleic acids, and relate their importance to living things. Identify the effects of enzymes.

70. 6.3 Section Summary 6.3 – pages 157-163 A carbon atom has four electrons available for bonding in its outer energy level. In order to become stable, a carbon atom forms four covalent bonds that fill its outer energy level. The Role of Carbon in Organisms

71. 6.3 Section Summary 6.3 – pages 157-163 The Role of Carbon in Organisms Two carbon atoms can form various types of covalent bonds—single, double or triple. Single Bond Double BondTriple Bond

72. 6.3 Section Summary 6.3 – pages 157-163 Carbon compounds vary greatly in size. Molecular chains When carbon atoms bond to each other, they can form straight chains, branched chains, or rings.

73. 6.3 Section Summary 6.3 – pages 157-163 Molecular chains Small molecules bond together to form chains called polymers. A polymer is a large molecule formed when many smaller molecules bond together.

74. 6.3 Section Summary 6.3 – pages 157-163 A carbohydrate is a biomolecule composed of carbon, hydrogen, and oxygen with a ratio of about two hydrogen atoms and one oxygen atom for every carbon atom. The structure of carbohydrates

75. 6.3 Section Summary 6.3 – pages 157-163 The largest carbohydrate molecules are polysaccharides, polymers composed of many monosaccharide subunits. (ie. potatoes, liver) The structure of carbohydrates The simplest type of carbohydrate is a simple sugar called a monosaccharide (mah noh SA kuh ride). (ie. glucose, fructose)

76. 6.3 Section Summary 6.3 – pages 157-163 Lipids are large biomolecules that are made mostly of carbon and hydrogen with a small amount of oxygen. (ie. fats, oils, waxes) The structure of lipids They are insoluble in water because their molecules are nonpolar and are not attracted by water molecules.

77. 6.3 Section Summary 6.3 – pages 157-163 A protein is a large, complex polymer composed of carbon, hydrogen, oxygen, nitrogen, and sometimes sulfur. The structure of proteins

78. 6.3 Section Summary 6.3 – pages 157-163 The structure of proteins The basic building blocks of proteins are called amino acids. There are about 20 common amino acids that can make literally thousands of proteins.

79. 6.3 Section Summary 6.3 – pages 157-163 Peptide bonds are covalent bonds formed between amino acids. The structure of proteins

80. 6.3 Section Summary 6.3 – pages 157-163 Proteins are the building blocks of many structural components of organisms. The structure of proteins

81. 6.3 Section Summary 6.3 – pages 157-163 The structure of proteins Enzymes are important proteins found in living things. An enzyme is a protein that changes the rate of a chemical reaction. They speed the reactions in digestion of food. Click image to view movie.

82. 6.3 Section Summary 6.3 – pages 157-163 A nucleic (noo KLAY ihk) acid is a complex biomolecule that stores cellular information in the form of a code. The structure of nucleic acids Nucleic acids are polymers made of smaller subunits called nucleotides.

83. 6.3 Section Summary 6.3 – pages 157-163 The structure of nucleic acids Nucleotides are arranged in three groups—a nitrogenous base, a simple sugar, and a phosphate group. Phosphate Sugar Nitrogenous base

84. 6.3 Section Summary 6.3 – pages 157-163 DNA, which stands for deoxyribonucleic acid is a nucleic acid. The structure of nucleic acids Phosphate Sugar Nitrogenous base

85. 6.3 Section Summary 6.3 – pages 157-163 The structure of nucleic acids The information coded in DNA contains the instructions used to form all of an organism’s enzymes and structural proteins. Another important nucleic acid is RNA, which stands for ribonucleic acid. RNA is a nucleic acid that forms a copy of DNA for use in making proteins.

86. Section 3 Check How many covalent bonds does a carbon atom need to form in order to become stable? Question 1 D. 4 C. 3 B. 2 A. 1 CA: Biology/Life Sciences 1h

87. The answer is D. A carbon atom has four electrons available for bonding in its outer energy level and needs to form four covalent bonds in order to become stable. Section 3 Check CA: Biology/Life Sciences 1h

88. A __________ is a biomolecule composed of carbon, hydrogen, and oxygen with a ratio of about two hydrogen atoms and one oxygen atom for every carbon atom. Question 2 D. fatty acid C. protein B. lipid A. carbohydrate Section 3 Check CA: Biology/Life Sciences 1h

89. The answer is A. Lipids are made mostly of carbon and hydrogen, and proteins contain nitrogen in addition to carbon, hydrogen and oxygen. Section 3 Check CA: Biology/Life Sciences 1h

90. In which type of molecule will you find peptide bonds? Question 3 D. fatty acid C. protein B. lipid A. carbohydrate Section 3 Check CA: Biology/Life Sciences 1h

91. The answer is C. Amino acids are the basic building blocks of proteins and are linked together by peptide bonds. Section 3 Check CA: Biology/Life Sciences 1h

92. What biomolecule is represented in this diagram? Question 4 D. lipid C. protein B. nucleotide A. carbohydrate Phosphate Sugar Nitrogenous base Section 3 Check CA: Biology/Life Sciences 1h

93. The answer is B. Nucleotides are the smaller subunits that make up nucleic acids. Nucleotides are composed of three groups: a nitrogenous base, a simple sugar, and a phosphate group. Phosphate Sugar Nitrogenous base Section 3 Check CA: Biology/Life Sciences 1h

94. Describe an enzyme and its function. Question 5 Section 3 Check CA: Biology/Life Sciences 1b

95. An enzyme is a protein that enables other molecules to undergo chemical changes to form new products. Enzymes increase the speed of reactions that would otherwise proceed too slowly. Substrate Active site Section 3 Check CA: Biology/Life Sciences 1b

96. Chapter Summary – 6.1 Atoms are the basic building block of all matter. Atoms and Their Interactions Atoms consist of a nucleus containing protons and usually neutrons. The positively charged nucleus is surrounded by rapidly moving, negatively charged electrons. Atoms become stable by bonding to other atoms through covalent or ionic bonds.

97. Chapter Summary – 6.1 Components of mixtures retain their properties. Atoms and Their Interactions Solutions are mixtures in which the components are evenly distributed. Acids are substances that from hydrogen ions in water. Bases are substances that form hydroxide ions in water.

98. Chapter Summary – 6.2 Water is the most abundant compound in living things. Water and Diffusion Water is an excellent solvent due to the polar property of its molecules. Particles of matter are in constant motion. Diffusion occurs from areas of higher concentration to areas of lower concentration.

99. Chapter Summary – 6.3 All organic compounds contain carbon atoms. Life Substances There are four principal types of organic compounds, or biomolecules, that make up living things: carbohydrates, lipids, proteins, and nucleic acid. The structure of a biomolecule will help determine its properties and functions.

100. Chapter Assessment Question 1 What is the difference between a compound and an element? Answer A compound is a substance that is composed of atoms of two or more different elements that are chemically combined. An element is a substance that can't be broken down into simpler chemical substances. CA: Biology/Life Sciences 1h

101. Question 2 What is it called when atoms share electrons? D. diffusion C. hydrogen bonding B. ionic bonding Water molecule A. covalent bonding Chapter Assessment CA: Biology/Life Sciences 1h

102. The answer is A. Covalent bonds differ from ionic bonds in that the shared electrons move about the nuclei of both atoms of the covalent compound. Water molecule Chapter Assessment CA: Biology/Life Sciences 1h

103. Question 3 Which of the following combinations will produce a solution? D. oil and vinegar C. powdered drink mix and water B. sand and sugar crystals A. chocolate chips and cookie dough Chapter Assessment CA: Biology/Life Sciences 1h

104. The answer is C. All of the combinations are mixtures because the individual components retain their own properties. A solution is a mixture in which one or more substances is dissolved in another and will not settle out of solution. Water molecules Sugar molecules Sugar crystal Chapter Assessment CA: Biology/Life Sciences 1h

105. Question 4 What type of substance forms hydrogen ions in water? D. polar C. base B. acid A. enzyme Chapter Assessment CA: Biology/Life Sciences 1h

106. The answer is B. Any substance that forms hydrogen ions (H + ) in water is an acid. The pH of a substance is a measure of how acidic or basic a solution is. Chapter Assessment CA: Biology/Life Sciences 1h

107. Question 5 Which of the following best describes a molecule with an unequal distribution of charge? D. diffuse C. basic B. acidic A. polar Chapter Assessment CA: Biology/Life Sciences 1h

108. The answer is A. Each polar molecule has a positive end and a negative end. Polar water molecules attract ions and other polar molecules, and can dissolve many ionic compounds. Chapter Assessment CA: Biology/Life Sciences 1h

109. Question 6 Name the chemical reaction illustrated in the diagram. B. condensation Glucose Fructose Sucrose CH 2 OH O OH CH 2 OH HO OH HO O HOCH 2 CH 2 OH + H2OH2O O OH HO OH O HOCH 2 OH HO O + CH 2 OH D. glycolysis C. Protein synthesis A. hydrolysis Chapter Assessment CA: Biology/Life Sciences 1h

110. The answer is B. In condensation reactions, small molecules bond together to produce a polymer and water. Glucose Fructose Sucrose CH 2 OH O OH CH 2 OH HO OH HO O HOCH 2 CH 2 OH + H2OH2O O OH HO OH O HOCH 2 OH HO O + CH 2 OH Chapter Assessment CA: Biology/Life Sciences 1h

111. Question 7 An oxygen atom has 8 protons and 8 neutrons. How many electrons does it have? D. 0 C. 32 B. 18 A. 8 Chapter Assessment CA: Biology/Life Sciences 1h

112. The answer is A. Atoms contain equal numbers of electrons and protons and have no net charge. Nucleus 8 protons (p+) 8 neutrons (n 0 ) Oxygen atom Chapter Assessment CA: Biology/Life Sciences 1h

113. Question 8 Based on your knowledge of biomolecules, which of the following substances would be most effective at breaking down this polymer? B. lipase CH 2 OH O OH HO OH O HOCH 2 OH HO O CH 2 OH D. water C. pepsin A. nuclease Chapter Assessment CA: Biology/Life Sciences 1h

114. The answer is D. This is a sucrose molecule, formed from glucose and fructose in a condensation reaction. The products of this reaction are the sucrose molecule and water. If water is added to sucrose, hydrolysis occurs and breaks the covalent bonds between the subunits. Chapter Assessment CA: Biology/Life Sciences 1h

115. Photo Credits Aaron Haupt Corbis Digital Stock Elaine Shay Mark Thayer PhotoDisc Alton Biggs Photo Credits

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