1. Professor’s eyes only… You may be surprised to learn… …that over 25% of all undergraduate students do not utilize their required course material. …student retention is dropping nationwide and while the higher education community has done a remarkable job of opening the doors of college to more and more students, we have not seen equal strides in the number of students who actually complete four-year degrees. (Education Trust, 2004) See the next slide on what you can do… Professor: Course/Section:

2. Professor’s eyes only… What you can do… The top factors motivating a student to use their adopted books all involve whether the material is immediately used, referred to, or assessed from in the classroom. Please take a few minutes the first day of class to explain and demonstrate why you adopted your book and accompanying technology. The next few slides show the book, technology products, and messaging to students that indicates they will be responsible for the content. Feel free to customize the information or delete from your slide set. Professor: Course/Section:

3. Solomon/Berg/Martin Biology, 8e Professor: Course/Section: This is your required course material You will need this material for: - tests and quizzes - homework and reading assignments

4. Some of the reasons why you need to use the new edition… Professor: Course/Section: Based on instructor and student feedback, text and illustrations throughout this edition have been extensively revised, honed, and reorganized. Would you like to monitor your progress quickly and easily? Track your progress with ease using innovative resources like ThomsonNOW Foremost is a self-assessment diagnostic tool--ThomsonNOW for Biology-- with automatic grading, which saves you time and helps you learn concepts more efficiently.

5. ThomsonNow for Biology is a powerful online learning tool that helps you assess your unique study needs, and available with each new copy of Solomon/Berg/Martin’s Biology, 8e. On-line assessments/exams Animations/interactivities Point-of-use eBook study less, learn more!

6. Personalized Study

7. How Do I Prepare?

8. Professor: Course/Section: InfoTrac College Edition Do your research 24/7! Easy access to over 10 million full-text articles Nearly 5000 academic journals, magazines, and periodicals. Do your research from home, work, or your dorm room! InfoTrac can be used for ALL of your courses! Includes InfoWrite, a web-based training tool designed to help you develop your writing skills.

9. HOW TO SEARCH THE DATABASE There are 3 ways to search: Subject Guide Keyword Search Advanced Search There is also a Limit Search function, which limits the search by date, journal, or keyword.

10. IT’S EASY TO SEARCH BY SUBJECT OR KEYWORD! IT’S EASY TO SEARCH BY SUBJECT OR KEYWORD! STEP 1 Type in a subject or keyword. STEP 2 Click on View to see search results, or click on Narrow to narrow down the search. STEP 3 Once the article is located, click on the title to view.

11. InfoWrite offers the following benefits: Facilitates the writing process Assists with the organization and presentation of ideas Helps you articulate key concepts Improves grammar, spelling and correct word usage Aids your creativity Also included: Critical Thinking with InfoTrac APA vs. MLA documentation style Essay Topics Research and the Internet …and much more! INFOWRITE INFOWRITE InfoTrac College Edition, your Online Research and Learning Center, includes InfoWrite, a web-based training tool designed to help you develop your writing skills.

12. Professor: Course/Section: On-line live tutoring from biology experts!

14. Buy ISBN # 0534375952 Essential Study Skills for Science Students Written specifically for science students, this book discusses how to develop good study habits, sharpen memory, learn more quickly, get the most out of lectures, prepare for tests, produce excellent term papers, and improve critical-thinking skills.

15. Your book may come with an access card for Biology’s e-resources. Access your e-Resources

16. Go to www.thomsonedu.com www.thomsonedu.com Create or sign into your Thomsonedu account. Enter the access code found in the card. Access your e-Resources

17. You should now have access to your e-resources for Biology. To access resources in ThomsonNOW, click on the ThomsonNOW link. Access your e-Resources

18. Enter Your School Name First-time users: Set up your ThomsonNOW account. It will link up to your Thomsonedu account.

19. New ThomsonNOW Account

20. Student Homepage

21. Enter a Course Key

22. Students Please Read… If your textbook doesn’t already come with the helpful study aids we’ve discussed, go to your local college bookstore or go on-line to the textbook URL … http://www.thomsonedu.com/biology Professor: Course/Section:

23. Atoms and Molecules: The Chemical Basis of Life Chapter 2

24. Learning Objective 1 What principal chemical elements are found in living things? What principal chemical elements are found in living things? What are the most important functions of these elements? What are the most important functions of these elements?

25. Element A substance that cannot be decomposed into simpler substances by normal chemical reactions A substance that cannot be decomposed into simpler substances by normal chemical reactions

26. The Periodic Table

27. KEY CONCEPTS Carbon, hydrogen, oxygen, and nitrogen are the most abundant elements in living things (about 96% of mass) Carbon, hydrogen, oxygen, and nitrogen are the most abundant elements in living things (about 96% of mass)

28. Element Functions Carbon Carbon backbone of organic molecules backbone of organic molecules Hydrogen and oxygen Hydrogen and oxygen components of water components of water Nitrogen Nitrogen component of proteins and nucleic acids component of proteins and nucleic acids

29. Learning Objective 2 Compare the physical properties (mass and charge) and locations of electrons, protons, and neutrons Compare the physical properties (mass and charge) and locations of electrons, protons, and neutrons What is the difference between the atomic number and the mass number of an atom? What is the difference between the atomic number and the mass number of an atom?

30. Atom Nucleus Nucleus protons (positive) protons (positive) neutrons (uncharged) neutrons (uncharged) Electrons Electrons encircle the nucleus encircle the nucleus negative negative

31. Atomic Number and Mass Each atom is a particular element Each atom is a particular element identified by number of protons (atomic number) identified by number of protons (atomic number) Atomic mass Atomic mass sum of protons and neutrons sum of protons and neutrons

32. AMU Atomic Mass Unit Atomic Mass Unit Mass of a single proton or neutron Mass of a single proton or neutron Mass of an electron Mass of an electron about 1/1800 amu about 1/1800 amu

33. Isotopes

34. Fig. 2-2, p. 28 Carbon-12 ( 12 C) (6p, 6n) 6 Carbon-14 ( 14 C) (6p, 8n) 6

35. Learning Objective 3 What are orbitals and electron shells? What are orbitals and electron shells? How are electron shells related to principal energy levels? How are electron shells related to principal energy levels?

36. KEY CONCEPTS Chemical properties of an atom are determined by its highest-energy (valence) electrons Chemical properties of an atom are determined by its highest-energy (valence) electrons

37. Orbitals Electrons move rapidly in electron orbitals Electrons move rapidly in electron orbitals Outside the nucleus Outside the nucleus Electron shell Electron shell Electrons in orbitals at the same principal energy level Electrons in orbitals at the same principal energy level Electron in shell far from nucleus has more energy than electron in shell close to nucleus Electron in shell far from nucleus has more energy than electron in shell close to nucleus

38. Atomic Orbitals

39. Fig. 2-4a, p. 30 (a) The first principal energy level contains a maximum of 2 electrons, occupying a single spherical orbital (designated 1s). The electrons depicted in the diagram could be present anywhere in the blue area. Nucleus

40. Fig. 2-4b, p. 30 (b) The second principal energy level includes four orbitals, each with a maximum of 2 electrons: one spherical (2s) and three dumbbell-shaped (2p) orbitals at right angles to one another.

41. Fig. 2-4c, p. 30 (c) Orbitals of the first and second principal energy levels of a neon atom are shown superimposed. Note that the single 2s orbital plus three 2p orbitals make up neon's full valence shell of 8 electrons. Compare this more realistic view of the atomic orbitals with the Bohr model of a neon atom at right.

42. Learning Objective 4 How does the number of valence electrons of an atom relate to its chemical properties? How does the number of valence electrons of an atom relate to its chemical properties?

43. Valence Electrons Electron in the outer shell Electron in the outer shell most energetic electrons most energetic electrons Number and arrangement of an atom’s valence electrons Number and arrangement of an atom’s valence electrons determine its chemical properties determine its chemical properties

44. Valence Electrons An atom tends to lose, gain, or share electrons to fill its valence shell An atom tends to lose, gain, or share electrons to fill its valence shell Electrons needed to fill valence shell Electrons needed to fill valence shell Most atoms: 8 electrons Most atoms: 8 electrons Hydrogen or helium: 2 electrons Hydrogen or helium: 2 electrons

45. Learning Objective 5 What is the difference between simplest, molecular, and structural chemical formulas? What is the difference between simplest, molecular, and structural chemical formulas?

46. Compounds Atoms are joined by chemical bonds to form compounds Atoms are joined by chemical bonds to form compounds A chemical formula gives the types and relative numbers of atoms in a substance A chemical formula gives the types and relative numbers of atoms in a substance

47. Chemical Formulae Simplest formula Simplest formula smallest whole-number ratio of component atoms smallest whole-number ratio of component atoms Molecular formula Molecular formula actual numbers of each type of atom actual numbers of each type of atom Structural formula Structural formula the arrangement of atoms in a molecule the arrangement of atoms in a molecule

48. KEY CONCEPTS A molecule consists of atoms joined by covalent bonds A molecule consists of atoms joined by covalent bonds Other important chemical bonds include ionic bonds and hydrogen bonds Other important chemical bonds include ionic bonds and hydrogen bonds

49. Learning Objective 6 Why is the mole concept so useful to chemists? Why is the mole concept so useful to chemists?

50. Avogadro’s Number Avogadro’s number 6.02 x 10 23 Avogadro’s number 6.02 x 10 23 One mole (atomic or molecular mass in grams) of any substance contains 6.02 x 10 23 atoms, molecules, or ions One mole (atomic or molecular mass in grams) of any substance contains 6.02 x 10 23 atoms, molecules, or ions Enables scientists to “count” particles by weighing a sample Enables scientists to “count” particles by weighing a sample

51. Learning Objective 7 What is the difference between covalent bonds, ionic bonds, hydrogen bonds, and van der Waals interactions? What is the difference between covalent bonds, ionic bonds, hydrogen bonds, and van der Waals interactions? How does each differ in the mechanisms by which they form and in relative strength? How does each differ in the mechanisms by which they form and in relative strength?

52. Covalent Bonds Strong, stable bonds Strong, stable bonds Formed when atoms share valence electrons Formed when atoms share valence electrons Form molecules Form molecules May rearrange the orbitals of valence electrons (orbital hybridization) May rearrange the orbitals of valence electrons (orbital hybridization)

53. Covalent Bonds

54. Fig. 2-5, p. 32 Molecular hydrogen (H2) HH HH or Hydrogen (H) (a) Single covalent bond formation. Two hydrogen atoms achieve stability by sharing a pair of electrons, thereby forming a molecule of hydrogen. In the structural formula on the right, the straight line between the hydrogen atoms represents a single covalent bond. Molecular oxygen (O2) (double bond is formed) O O O O Oxygen (O) or (b) Double covalent bond formation. In molecular oxygen, two oxygen atoms share two pairs of electrons, forming a double covalent bond. The parallel straight lines in the structural formula represent a double covalent bond.

55. Nonpolar and Polar Covalent Bonds Covalent bonds are Covalent bonds are nonpolar if electrons are shared equally between the two atoms nonpolar if electrons are shared equally between the two atoms polar if one atom is more electronegative (greater electron affinity) than the other polar if one atom is more electronegative (greater electron affinity) than the other

56. Ionic Bonds Form between a positively charged cation and a negatively charged anion Form between a positively charged cation and a negatively charged anion Are strong in the absence of water but relatively weak in aqueous solution Are strong in the absence of water but relatively weak in aqueous solution

57. Ionic Bonds

58. Fig. 2-9a, p. 35 + 11 protons 11 electrons Sodium (Na) 17 electrons Chlorine (Cl) 17 protons and 18 electrons Chloride ion (Cl – ) 10 electrons Sodium ion (Na + ) Sodium chloride (NaCl) –

59. Hydrogen Bonds Relatively weak bonds Relatively weak bonds Form when Form when A hydrogen atom with a partial positive charge A hydrogen atom with a partial positive charge Is attracted to an atom (usually O or N) with a partial negative charge Is attracted to an atom (usually O or N) with a partial negative charge Already bonded to another molecule or part of the same molecule Already bonded to another molecule or part of the same molecule

60. Hydrogen Bonds

61. Fig. 2-11, p. 35 Electronegative atoms Hydrogen bond H H H H H –+ O N

62. KEY CONCEPTS Hydrogen bonds and van der Waals interactions are weak attractions Hydrogen bonds and van der Waals interactions are weak attractions

63. van der Waals interactions Weak forces Weak forces Based on fluctuating electric charges Based on fluctuating electric charges

64. Learning Objective 8 What are oxidation and reduction reactions? What are oxidation and reduction reactions? How do oxidation and reduction reactions relate to the transfer of energy? How do oxidation and reduction reactions relate to the transfer of energy?

65. Redox Reactions Oxidation and reduction reactions Oxidation and reduction reactions Electrons (energy) are transferred from a reducing agent to an oxidizing agent Electrons (energy) are transferred from a reducing agent to an oxidizing agent

66. Oxidation and Reduction Oxidation Oxidation Atom, ion, or molecule loses electrons (energy) Atom, ion, or molecule loses electrons (energy) Reduction Reduction Atom, ion, or molecule gains electrons (energy) Atom, ion, or molecule gains electrons (energy)

67. KEY CONCEPTS The energy of an electron is transferred in a redox reaction The energy of an electron is transferred in a redox reaction

68. Learning Objective 9 How do hydrogen bonds between adjacent water molecules govern the properties of water? How do hydrogen bonds between adjacent water molecules govern the properties of water?

69. Polar Molecules Water is a polar molecule Water is a polar molecule One end has a partial positive charge and the other has a partial negative charge One end has a partial positive charge and the other has a partial negative charge Because it is polar, water is an excellent solvent for ionic or polar solutes Because it is polar, water is an excellent solvent for ionic or polar solutes

70. Polar Molecules

71. Fig. 2-7, p. 34 Hydrogen parts Hydrogen (H)Oxygen (O) Hydrogen (H) Partial negative charge at oxygen end of molecule Oxygen part Water molecule (H 2 O) Partial positive charge at hydrogen end of molecule

72. Fig. 2-7, p. 34 Hydrogen (H)Oxygen (O) Hydrogen (H) Partial negative charge at oxygen end of molecule Water molecule (H 2 O) Partial positive charge at hydrogen end of molecule Oxygen part Hydrogen parts Stepped Art

73. Cohesion and Adhesion Water molecules exhibit cohesion because they form hydrogen bonds with one another Water molecules exhibit cohesion because they form hydrogen bonds with one another Water molecules exhibit adhesion by hydrogen bonding to substances with ionic or polar regions Water molecules exhibit adhesion by hydrogen bonding to substances with ionic or polar regions

74. Hydrogen Bonds in Water

75. Specific Heat Water has high specific heat Water has high specific heat Hydrogen bonds must break to raise water temperature Hydrogen bonds must break to raise water temperature Specific heat of water helps Specific heat of water helps organisms maintain relatively constant internal temperature organisms maintain relatively constant internal temperature keep large bodies of water (ocean) at a constant temperature keep large bodies of water (ocean) at a constant temperature

76. Heat of Vaporization Water has a high heat of vaporization Water has a high heat of vaporization Hydrogen bonds must break for molecules to enter vapor phase Hydrogen bonds must break for molecules to enter vapor phase Molecules carry heat, causing evaporative cooling Molecules carry heat, causing evaporative cooling

77. Ice Hydrogen bonds between water molecules make ice less dense than liquid water Hydrogen bonds between water molecules make ice less dense than liquid water Because ice floats, the aquatic environment is less extreme Because ice floats, the aquatic environment is less extreme

78. Three Phases of Water

79. KEY CONCEPTS Water molecules are polar, with partial positive and negative charges Water molecules are polar, with partial positive and negative charges Form hydrogen bonds with one another and other charged substances Form hydrogen bonds with one another and other charged substances

80. Learning Objective 10 What is the difference between an acid and a base? What is the difference between an acid and a base? What are the properties of acids and bases? What are the properties of acids and bases?

81. Acids and Bases Acids Acids proton (hydrogen ion, H + ) donors proton (hydrogen ion, H + ) donors dissociate in solution to yield H + and an anion dissociate in solution to yield H + and an anion Bases Bases proton acceptors proton acceptors dissociate in solution to yield hydroxide ions (OH - ) dissociate in solution to yield hydroxide ions (OH - )

82. KEY CONCEPTS Acids are hydrogen ion donors Acids are hydrogen ion donors Bases are hydrogen ion acceptors Bases are hydrogen ion acceptors The pH scale measures the hydrogen ion concentration of a solution The pH scale measures the hydrogen ion concentration of a solution

83. Learning Objective 11 How does the hydrogen ion concentration (moles per liter) of a solution relate to its pH value? How does the hydrogen ion concentration (moles per liter) of a solution relate to its pH value? How do buffers help minimize changes in pH? How do buffers help minimize changes in pH?

84. pH The negative log of the hydrogen ion (H +) concentration of a solution The negative log of the hydrogen ion (H +) concentration of a solution (measured in moles per liter)

85. pH of Solutions Neutral solution Neutral solution equal concentrations of H + and OH - equal concentrations of H + and OH - (10 -7 mol/L), pH 7 (10 -7 mol/L), pH 7 Acidic solution Acidic solution pH less than 7 pH less than 7 Basic solution Basic solution pH greater than 7 pH greater than 7

86. Buffers Buffering system Buffering system based on a weak acid or a weak base based on a weak acid or a weak base Buffer Buffer resists changes in pH of a solution when acids or bases are added resists changes in pH of a solution when acids or bases are added

87. Learning Objective 12 What is the composition of a salt? What is the composition of a salt? Why are salts are important in organisms? Why are salts are important in organisms?

88. Salts Salt Salt a compound in which the hydrogen atom of an acid is replaced by some other cation a compound in which the hydrogen atom of an acid is replaced by some other cation Salts provide many mineral ions essential for life functions Salts provide many mineral ions essential for life functions

89. CLICK TO PLAY How Atoms Bond

90. Spheres of Hydration CLICK TO PLAY

91. The pH Scale CLICK TO PLAY

92. The Shell Model of Electron Distribution CLICK TO PLAY