1. Go to Section: 2–1The Nature of Matter A.Atoms B.Elements and Isotopes 1.Isotopes 2.Radioactive Isotopes C.Chemical Compounds D.Chemical Bonds 1.Ionic Bonds 2.Covalent Bonds 3.Van der Waals Forces Section 2-1 Section Outline

2. Go to Section: Matter –Anything that has mass and occupies space 1 The basic unit of matter is called the atom.

3. Go to Section: Nonradioactive carbon-12Nonradioactive carbon-13Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 8 neutrons 6 electrons 6 protons 7 neutrons Section 2-1 Figure 2-2 Isotopes of Carbon 2, 3 Atomic Nuclei contain protons and neutrons. Protons1+ chargesize 1 amunucleus Neutrons0 charge size 1 amuin nucleus Electrons1- chargesize 1/1840 amuin electron cloud

4. Go to Section: 4 Atoms are neutral because they contain the same # of electrons & protons.

5. Go to Section: 5 Chemical elements are groups of atoms having the same atomic number, that is, atoms having the same number protons. These are all atoms of Carbon. All have atomic # 6.

6. Go to Section: 6 C 12.011 Section 2-1 An Element in the Periodic Table 6. Proton # = 6 : shown by the atomic number Also, C atoms have 6 electrons: Since atoms are neutral, if you know proton #, you also know electron #!

7. Go to Section: Nonradioactive carbon-12Nonradioactive carbon-13Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 8 neutrons 6 electrons 6 protons 7 neutrons Section 2-1 Figure 2-2 Isotopes of Carbon 7 Isotopes are forms of the same element that have the same number of protons but a different number of neutrons.

8. Go to Section: Nonradioactive carbon-12Nonradioactive carbon-13Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 8 neutrons 6 electrons 6 protons 7 neutrons Section 2-1 Figure 2-2 Isotopes of Carbon 8Isotopes are identified by isotopic notation: Carbon-12, carbon-13, carbon-14 OR 12 C 13 C 14 C 6 6 6

9. Go to Section: 9 Isotopes of the same element have the same properties because they have the same atomic number (the same number protons) 12 C 13 C 14 C 6 6 6

10. Go to Section: 10 Chemical compounds are groups of atoms held together by chemical bonds. Chemical compounds are more stable than individual atoms (except for noble gas atoms which have stable ---filled— valence electron shells. Chemical compounds allow atoms to obey the “octet rule”. (2 electrons in the outer electron shell in H and He, but 8 for other elements.

11. Go to Section: 11 Chemical formulas show the numbers of different kinds of atoms bonded together in a single formula unit of a compound NaClone Na ion bonded to one Cl ion Why do we know it’s composed of ions? Because Na is a metal—an electron donor—and Cl is a nonmetal—an electron acceptor if a metal is present to give it an electron.

12. Go to Section: 12 Atoms in compounds are held together by chemical bonds—either ionic or covalent.

13. Go to Section: Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na + )Chloride ion (Cl - ) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Section 2-1 Figure 2-3 Ionic Bonding 13 Ionic bonds: attraction of negative ions to positive ions because a metal donates its electrons to a nonmetal atom, forming stable ions with complete valence shell octets.

14. Go to Section: 13 Covalent bonds form when nonmetal atoms share electrons to fill their valence octets, linking atoms because both nuclei attract the shared electrons.

15. Go to Section: Sodium atom (Na)Chlorine atom (Cl)Sodium ion (Na + )Chloride ion (Cl - ) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Section 2-1 Figure 2-3 Ionic Bonding 14 Ions are atoms carrying a charge after losing or gaining valence electrons.

16. Go to Section: 15. False. Atom that loses electrons becomes a positive ion.

17. Go to Section: 16 Molecules (Not ionic compounds!) form when atoms are joined with covalent bonds.

18. Go to Section: 17 A is false—2 shared electrons is a single covalent bond ACAC b D covalent bonds are formed when atoms share electrons http://academic.brooklyn.cuny.edu/biology/bio4fv/page/covalent_bonds.html

19. Go to Section: 18 Van Der Waals forces and dipole-dipole interactions hold atoms of nearby molecules together. Occasionally, valence electrons are nearer one atom than the other in a covalent bond, creating areas partial charge. http://www.chem.unsw.edu.au/coursenotes/CHEM1/nonunipass/Haine sIMF/images/dipoledipole.jpg

20. Go to Section: Lesson 3: Chapter 2 The chemistry of Life 1.Watch movie on water, then answer questions on the worksheet together in your lab group BEFORE beginning the lab. Teacher will select one worksheet for grading, by random drawing. 2.Complete water lab, then turn in one copy per lab group. Teacher will select one student’s report. 3.Discuss the water movie & labs, and complete the 2.2 guided reading questions 1—8 as a class. Homework: guided reading & study workbook questions, pages 15—16, #9—21.

21. Go to Section: 2–2 Properties of Water, the strangest and most important molecule on earth! Section 2-2 Section Outline http://www.wsi.nrcs.usda.gov/products/i mages/wq_drop.jpg

22. Go to Section: http://www.sumanasinc.com/webcontent/ani mations/content/propertiesofwater/water.html Watch this movie from beginning to end. Then, the teacher will advance the movie one question at a time, giving time for you to write the answers to each question.

23. Go to Section: Guided reading & study workbook for section 2.2, p 15--16 1. Water molecules contain 10 electrons, 1 for each H and eight for O. Water molecules also contain 10 protons True or False. Water molecules are neutral. 1.True 2.False

24. Go to Section: 2. Because water molecules have O at one end and H at the other, the entire molecule: 1.Is positively charged 2.Is negatively charged 3.Is polar, with partial + & - charges.

25. Go to Section: 3. Water is a polar covalent molecule because: 1.More electronegative O atoms are bonded to less electronegative H atoms 2.O carries a δ- charge & H’s a δ+ charge 3.The shared electrons of each O—H covalent bond are more strongly attracted to the O 4.All of the above 5.None of the above

26. Go to Section: Strongesttriple covalent bond 2nd strongestdouble covalent bond 3rd strongestsingle covalent bond 4 th strongestionic bond 5 th strongestHydrogen bonds 6 th strongestDipole dipole interactions (polar molecules attracted δ+ to δ- ) OTHER than Hydrogen bonds 7 th strongest Van der Waals forces (hydrophobic interactions of nonpolar compounds)

27. Go to Section: 4. Which statement is True? 1.Hydrogen bonds are stronger than ionic bonds. 2.Attraction of the H in one water molecule to O in another is a Hydrogen bond 3.Hydrogen bonds are stronger than covalent bonds 4.Hydrogen bonds are the strongest bonds BETWEEN different neutral molecules. 5.Choices 2 and 5 are true

28. Go to Section: cohesion

29. Go to Section: 5. Cohesion is: 1.Attraction of δ+ and δ- atoms of water molecules to atoms or ions of other substances, like the glass in a graduated cylinder 2.Attraction of δ+ H and δ- O of water molecules atoms in adjacent water molecules

30. Go to Section: 5. Adhesion (exhibited by water adhering to the spider web) is: 1.Attraction of δ+ and δ- atoms of water molecules to atoms or ions of other substances, like the glass in a graduated cylinder 2.Attraction of δ+ H and δ- O of water molecules atoms in adjacent water molecules

31. Go to Section: 6. Water is cohesive (shown by water’s forming droplets) because: 1.δ+ H and δ- O atoms of water molecules are attracted to each other in the same molecule 2.δ+ H and δ- O atoms of water molecules are attracted to each other in adjacent molecules

32. Go to Section: Surface tension versus capillary action

33. Go to Section: 7. The rise of water in a narrow tube (like water rising in a thermometer) against the force of gravity is: 1.surface tension 2. capillary action 3. specific heat

34. Go to Section: 8 In plants capillary action: 1.Draws water upwards from the roots into the leaves through thin tubes called xylem 2.Pulls sugar downwards from the leaves into the roots through thin tubes called phloem

35. Go to Section: 10-1-09 Lesson on solutions and suspensions with homework correction slides Lesson on acids and bases Complete water labs & questions & acid/base questions. Tear off lab & questions through end page. Put rest back in notebooks. Homework: prep for a quiz on ch 2.1,2.2, tomorrow

36. Go to Section: Mixture: 2 or more substances combined but not chemically bonded. They can be separated without another chemical reaction (a physical separation). e.g., sand and water can be separated with a filter inks in markers can be separated with chromatography Salt can be removed from water by evaporating the water

37. Go to Section: 9. True or False. Sucrose (C 6 H 12 O 6 ) is a mixture. 1.True 2.False

38. Go to Section: 9. True or False. Sucrose (C 6 H 12 O 6 ) dissolved in water is a mixture. 1.True 2.False

39. Go to Section: Mixtures may be heterogenous (nonuniform throughout) or homogenous (uniform throughout) Another name for a homogeneous mixture is solution. Another name for a heterogeneous mixture is suspension.

40. Go to Section: 10. This picture shows bananas mashed up in water. This mixture is a 1.suspension 2.solution

41. Go to Section: 11. World’s greatest solvent: water! Water is known as the universal solvent because it can dissolve ionic compounds and polar covalent compounds. Ionic and polar covalent compounds are hydrophillic (water loving) Water can not dissolve nonpolar covalent compounds. Nonpolar compounds are hydrophobic (water hating)

42. Go to Section: 12. A suspension is a: 1.Homogeneous mixture 2.Heterogeneous mixture 3.Unstable (particles settle out over time) 4.Stable (a solution whose solutes do not settle out) 5.2 and 3

43. Go to Section: Parts of Solutions: Solvent: more abundant—does the dissolving Solute: less abundant—gets dissolved

44. Go to Section: 13. Two liters water are mixed with 0.3 liters salt. The water is the 1.solution 2.solute 3.solvent

45. Go to Section: 14. Two liters water are mixed with 0.3 liters salt. The salt is the 1.solution 2.solute 3.solvent

46. Go to Section: concentration Molarity (M) = # moles solute/#L solution 3 Moles/0.5 L = 6 M 1 mole NaCl = 58.4 g 29.2 g/0.25 L = 0.5 moles/0.25 L= 2M

47. Go to Section: Aqueous solutions can be neutral, acidic, or basic. These descriptions depend refer to the behavior of the solute when it is dissolved in water and to how this behavior alters the molar concentrations of these two ions in the aqueous solution: H + protons OH 1- hydroxide ions

48. Go to Section: 1 out of over 500 million water molecules dissociates to H + hydronium, OH - hydroxide Neutral aqueous solutions and pure water contain equal numbers of both ions. 2H 2 O (l) → H 3 O + (aq) + OH – (aq)

49. Go to Section: 14. Two water molecules can react to form: 2H 2 O (l) → H 3 O + (aq) + OH – (aq) 1.Nonpolar compounds 2.Hydronium & hydroxide ions

50. Go to Section: 15. Water is neutral because it: 1.Is polar covalent 2.Forms Hydrogen bonds 3.Has equal numbers of hydronium & hydroxide ions 4.Is nonpolar covalent

51. Go to Section: Acids increase the H 1+ content of water in aqueous solutions. Bases increase the OH 1- HCl  H + + Cl - NaOH  Na 1+ + OH 1-

52. Go to Section: 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 The more H + ions, the more acidic, the lower pH. The more OH 1- ions, the more basic, the higher pH. pH measures whether either H + ions are greater (acidic) or the OH 1- ions are greater (basic)

53. Go to Section: 16. The pH scale indicates: 1.The acidity of an aqueous solution 2.The basicity of an aqueous solution 3.The concentration of H+ ions present relative to concentration of the OH- ions 4.All of these.

54. Go to Section: 17. Which of these aqueous solutions is most acidic? 1.pH9 2.pH11 3.pH7 4.pH5 5.pH3

55. Go to Section: 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 pH 7 has 10 times less H+ than pH6 and 100 times less than pH5 The pH scale is logarithmic. So, pH 0 has 10 times more H+ than pH1 and 100 times more than pH2.

56. Go to Section: 18. How many more H+ ions does a solution with pH 4 have than one with pH 5? 1.1X more 2.10X more 3.100X more 4.It has 1X less than pH5

57. Go to Section: 19. Which statement is false? 1.Acidic solution pH is < 7 2.Acids add H+ to solutions 3.Strong acids make solutions whose pH is 11--14 4.Acidic solutions have higher concentrations of H+ than pure water

58. Go to Section:

59. pH

60. Go to Section: Life’s Backbone Most of the compounds that make up living things contain carbon. In fact, carbon makes up the basic structure, or “backbone,” of these compounds. Each atom of carbon has four electrons in its outer energy level, which makes it possible for each carbon atom to form four bonds with other atoms. As a result, carbon atoms can form long chains. A huge number of different carbon compounds exist. Each compound has a different structure. For example, carbon chains can be straight or branching. Also, other kinds of atoms can be attached to the carbon chain. Section 2-3 Interest Grabber

61. Go to Section: 1. On a sheet of paper, make a list of at least ten things that contain carbon. 2. Working with a partner, review your list. If you think some things on your list contain only carbon, write “only carbon” next to them. 3. If you know other elements that are in any items on your list, write those elements next to them. Section 2-3 Interest Grabber continued

62. Go to Section: 2–3Carbon Compounds A.The Chemistry of Carbon B.Macromolecules C.Carbohydrates D.Lipids E.Nucleic Acids F.Proteins Section 2-3 Section Outline

63. Go to Section: 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,

64. Go to Section: MethaneAcetyleneButadieneBenzeneIsooctane Section 2-3 Figure 2-11 Carbon Compounds

65. Go to Section: Starch Glucose Section 2-3 Figure 2-13 A Starch

66. Go to Section: General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

67. Go to Section: General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

68. Go to Section: General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

69. Go to Section: Amino acids Section 2-3 Figure 2-17 A Protein

70. Go to Section: Matter and Energy Have you ever sat around a campfire or watched flames flicker in a fireplace? The burning of wood is a chemical reaction—a process that changes one set of chemicals into another set of chemicals. A chemical reaction always involves changes in chemical bonds that join atoms in compounds. The elements or compounds that enter into a chemical reaction are called reactants. The elements or compounds produced by a chemical reaction are called products. As wood burns, molecules of cellulose are broken down and combine with oxygen to form carbon dioxide and water vapor, and energy is released. Section 2-4 Interest Grabber

71. Go to Section: 1. What are the reactants when wood burns? 2. What are the products when wood burns? 3. What kinds of energy are given off when wood burns? 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy? 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire? Section 2-4 Interest Grabber continued

72. Go to Section: 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

73. Go to Section: Reaction pathway without enzyme Activation energy without enzyme Activation energy with enzyme Reaction pathway with enzyme Reactants Products Section 2-4 Effect of Enzymes

74. Go to Section: Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions

75. Go to Section: Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions

76. Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

77. Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

78. Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

79. Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

80. Video Contents Click a hyperlink to choose a video. Atomic Structure Energy Levels and Ionic Bonding Covalent Bonding Enzymatic Reactions Videos

81. Video 1 Click the image to play the video segment. Video 1 Atomic Structure

82. Video 2 Click the image to play the video segment. Video 2 Energy Levels and Ionic Bonding

83. Video 3 Click the image to play the video segment. Video 3 Covalent Bonding

84. Video 4 Click the image to play the video segment. Video 4 Enzymatic Reactions

85. Internet Career links on forensic scientists Interactive test Articles on organic chemistry For links on properties of water, go to www.SciLinks.org and enter the Web Code as follows: cbn-1022.www.SciLinks.org For links on enzymes, go to www.SciLinks.org and enter the Web Code as follows: cbn-1024.www.SciLinks.org Go Online

86. Section 1 Answers 1.Give an example of solid matter. Sample answers: books, desks, chairs 2. Give an example of liquid matter. Sample answers: water, milk 3. Give an example of gaseous matter. Sample answers: air, helium in a balloon 4. Is all matter visible? No 5. Does all matter take up space? Yes Interest Grabber Answers

87. Section 2 Answers 1. Working with a partner, make a list of ten things that have water in them. Possible answers: bodies of water, rain and snow, soft drinks and other beverages, juicy foods such as fruits, and so on. 2. Exchange your list for the list of another pair of students. Did your lists contain some of the same things? Did anything on the other list surprise you? Students’ answers will likely be similar, but not exactly alike. 3. Did either list contain any living things? Students’ lists may include plants, animals, or other living things. Interest Grabber Answers

88. Section 3 Answers 1. On a sheet of paper, make a list of at least ten things that contain carbon. Students will likely know that charcoal and coal contain carbon. They may also list carbohydrates (starches and sugars), oil, gasoline, wood, or carbon dioxide. 2. Working with a partner, review your list. If you think some things on your list contain only carbon, write “only carbon” next to them. Students will say that charcoal and coal contain only carbon. While these materials do contain small amounts of other elements, such as sulfur, they are composed mostly of carbon. 3. If you know other elements that are in any items on your list, write those elements next to them. Students may know that many carbon compounds also contain oxygen and/or hydrogen. Interest Grabber Answers

89. Section 4 Answers Interest Grabber Answers 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.

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