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2. Resources Chapter Presentation Visual Concepts Transparencies Standardized Test Prep

3. Section 1 Composition of Matter Chapter 2 Objectives • Definethe term matter. • Explainthe relationship between elements and atoms. • Draw and label a model of the structure of an atom. • Explain howcompounds affect an atom’s stability. • Contrast covalent and ionic bonds.

4. Chapter 2 Chemistry of Life Table of Contents Section 1 Composition of Matter Section 2 Energy Section 3 Water and Solutions

5. At the Bell Review 1) Major characteristics all living things have in common are • metabolism b. response to stimuli • both a and b d. neither a nor b 2) 750 grams = _____ kg. • 7,500 b. 7.50 • 0.750 d. 0.0750 3) The ocular lens in a microscope has a 10x magnification and the objective lens has a 40x magnification. The total magnification is • 4x b. 40x c. 400x d. 4,000x 4) Describe how natural selection causes adaptations in organisms. 5) Pairs of electrons are shared between atoms in a covalent bond. TRUE or FALSE

6. Big Ideas • Life emerges due to the chemical organization of matter into cells. • Structure is related to function at all biological levels of organization. • Eukaryotic cells can differentiate and organize making it possible for multicellularity.

7. Section 1 Composition of Matter Chapter 2 Matter • Matteris anything that occupies space and has mass. • Massis the quantity of matter an object has.

8. Section 1 Composition of Matter Chapter 2 Elements and Atoms • Elementsare made of a single kind of atom and cannot be broken down by chemical means into simpler substances. • Atoms are composed of protons, neutrons, and electrons. • http://ptable.com/

9. Section 1 Composition of Matter Chapter 2 Elements and Atoms, continued • The Nucleus • Protons and neutrons make up the nucleus of the atom.

10. Section 1 Composition of Matter Chapter 2 Elements and Atoms, continued • Electrons • Electronsmove about the nucleus in orbitals. • An orbital is a three-dimensional region around a nucleus that indicates the probable location of an electron.

11. Section 1 Composition of Matter Chapter 2 Elements and Atoms, continued • Isotopes • Atoms of the same element that have a different number of neutrons are calledisotopes.

12. Section 1 Composition of Matter Chapter 2 Compounds • Compoundsconsist of atoms of two or more elements that are joined by chemical bonds in a fixed proportion.

13. Section 1 Composition of Matter Chapter 2 Keystone Bio Question Carbon is found in all known forms of life. Which statement best describes why carbon is uniquely suited to forming macromolecules such as those found in living organisms? A. Carbon forms large, flat compounds that have increased surface area available for reactions. B. Carbon forms large, three-dimensional compounds that are not chemically reactive. C.Carbon forms strong, stable bonds with up to four other atoms, including carbon atoms. D. Carbon forms weak bonds with other atoms that can be easily broken to release energy.

14. Section 1 Composition of Matter Chapter 2 Compounds, continued • Covalent Bonds • A covalent bond is formed when two atoms share electrons.

15. Section 1 Composition of Matter Chapter 2 Compounds, continued • Ionic Bonds • An ionic bond is formed when one atom gives up an electron to another. The positive ion is then attracted to a negative ion to form the ionic bond.

16. Section 1 Composition of Matter Chapter 2 Ionic Bonding

17. Section 2 Energy Chapter 2 Objectives • Describethe physical properties of each state of matter. • Describethe role of reactants and products in chemical reactions. • Explainthe relationship between enzymes and activation energy. • Explainhow oxidation and reduction reactions are linked.

18. Section 2 Energy Chapter 2 Energy and Matter • States of Matter • Addition of energy to a substance can cause its state to change from a solid to a liquid and from a liquid to a gas.

19. Section 2 Energy Chapter 2 Energy and Chemical Reactions • Reactantsare substances that enter chemical reactions. • Products are substances produced by chemical reactions.

20. Section 2 Energy Chapter 2 Energy and Chemical Reactions

21. Section 2 Energy Chapter 2 Energy and Chemical Reactions, continued • Activation Energy • Enzymes lower the amount of activation energy necessary for a reaction to begin in living systems. • Enzymes are • Biological catalysts. • (reduce amount • of energy needed • for reaction to take place)

23. Section 2 Energy Chapter 2 Energy and Chemical Reactions, continued • Oxidation Reduction Reactions • A chemical reaction in which electrons are exchanged between atoms is called an oxidation-reduction reaction. • Oxidation: a reactant loses one or more electrons (becomes more positive) • Reduction: a reactant gains one or more electrons (becomes more negative)

24. Section 3 Water and Solutions Chapter 2 Objectives • Describethe structure of a water molecule. • Explainhow water’s polar nature affects its ability to dissolve substances. • Outline the relationship between hydrogen bonding and the different properties of water. • Identify the roles of solutes and solvents in solutions. • Differentiate between acids and bases.

25. Section 3 Water and Solutions Chapter 2 Polarity • Water = polarmolecule • due to anuneven distribution of charge • Electrons in a water molecule are shared unevenly between hydrogen and oxygen.

26. Section 3 Water and Solutions Chapter 2 Polarity, continued • Solubility of Water • polarity of water makes it effective at dissolving other polar substances • Ex. sugars, ionic compounds, and some proteins

27. Section 3 Water and Solutions Chapter 2 Hydrogen Bonding • hydrogen bond= force of attraction between a hydrogen molecule with a partial positive charge and another atom or molecule with a partial or full negative charge

28. Section 3 Water and Solutions Chapter 2 Hydrogen Bonding, continued • Cohesion and Adhesion • Cohesion = attractive force that holds molecules of a single substance together • Ex. Group of water molecules • Adhesion= attractive force between two particles of different substances • Ex. water molecules & glass molecules

29. Section 3 Water and Solutions Chapter 2 Solutions • solution= solute + solvent • Ex. Solute = Kool-aid • Ex. Solvent = water

30. Section 3 Water and Solutions Chapter 2 Acids and Bases • Ionization of Water • Water ionizes intohydronium ions(H3O+) and hydroxide ions (OH–). • …because of the exchanging of protons, H2O dissociates into these ions…

31. Section 3 Water and Solutions Chapter 2 Acids and Bases, continued • Acids • Acidic solutions= more hydronium ions • Bases • Basic solutions= more hydroxide ions

32. Section 3 Water and Solutions Chapter 2 Acids and Bases, continued • pH • pH scale – compares concentrations of hydronium ions to hydroxide ions in a solution • ranges from 0 (acidic) to 14 (basic) • 7 = neutral

33. Section 3 Water and Solutions Chapter 2 The pH Scale

34. Section 3 Water and Solutions Chapter 2 Acids and Bases, continued • Buffers • Buffers= neutralize • either by adding acid or base

35. Chapter 2 Standardized Test Prep Multiple Choice 1. The way in which elements bond to form compounds depends on which of the following? A. the model of the atom B. the structural formula of the compound C. the dissociation of the ions in the compound D. the number and arrangement of electrons in the atoms of the elements

36. Chapter 2 Standardized Test Prep Multiple Choice, continued 1. The way in which elements bond to form compounds depends on which of the following? A. the model of the atom B. the structural formula of the compound C. the dissociation of the ions in the compound D. the number and arrangement of electrons in the atoms of the elements

37. Chapter 2 Standardized Test Prep Multiple Choice, continued 2. If an atom is made up of 6 protons, 7 neutrons, and 6 electrons, what is its atomic number? F. 6 G. 7 H. 13 J. 19

38. Chapter 2 Standardized Test Prep Multiple Choice, continued 2. If an atom is made up of 6 protons, 7 neutrons, and 6 electrons, what is its atomic number? F. 6 G. 7 H. 13 J. 19

39. Chapter 2 Standardized Test Prep Multiple Choice, continued The graph below shows the energy in a chemical reaction as the reaction progresses. Use the graph to answer the questions that follow. 3. The amount of energy needed for this chemical reaction to begin is shown by the line rising from the reactants. What is this energy called? A. chemical energy B. electrical energy C. activation energy D. mechanical energy

40. Chapter 2 Standardized Test Prep Multiple Choice, continued The graph below shows the energy in a chemical reaction as the reaction progresses. Use the graph to answer the questions that follow. 3. The amount of energy needed for this chemical reaction to begin is shown by the line rising from the reactants. What is this energy called? A. chemical energy B. electrical energy C. activation energy D. mechanical energy

41. Chapter 2 Standardized Test Prep Multiple Choice, continued The graph below shows the energy in a chemical reaction as the reaction progresses. Use the graph to answer the questions that follow. 4. Suppose that this reaction needs a catalyst to proceed. In the absence of a catalyst, the activation energy would be which of the following? F. larger than what is shown G. the same as what is shown H. smaller than what is shown J. not much different from what is shown

42. Chapter 2 Standardized Test Prep Multiple Choice, continued The graph below shows the energy in a chemical reaction as the reaction progresses. Use the graph to answer the questions that follow. 4. Suppose that this reaction needs a catalyst to proceed. In the absence of a catalyst, the activation energy would be which of the following? F. larger than what is shown G. the same as what is shown H. smaller than what is shown J. not much different from what is shown

43. Chapter 2 Standardized Test Prep Multiple Choice, continued The graph below shows the energy in a chemical reaction as the reaction progresses. Use the graph to answer the questions that follow. 5. What is an aqueous solution that contains more hydroxide ions than hydronium ions called? A. a gas B. a base C. a solid D. an acid

44. Chapter 2 Standardized Test Prep Multiple Choice, continued The graph below shows the energy in a chemical reaction as the reaction progresses. Use the graph to answer the questions that follow. 5. What is an aqueous solution that contains more hydroxide ions than hydronium ions called? A. a gas B. a base C. a solid D. an acid

45. Chapter 2 Standardized Test Prep Multiple Choice, continued 6. Oxidation : loss :: reduction : F. win G. gain H. take J. forfeit

46. Chapter 2 Standardized Test Prep Multiple Choice, continued 6. Oxidation : loss :: reduction : F. win G. gain H. take J. forfeit

47. Chapter 2 Standardized Test Prep Multiple Choice, continued The illustration below is a space-filling model of water. Use the model to answer the following question. 7. The covalent bonds on the water molecule depicted in the picture above has partial positive charges on the hydrogen atom and a partial negative charge on the oxygen atom. What do the partial positive and partial negative charges on this water molecule mean? A. Water is an ion. B. Water is a polar molecule. C. Water needs a proton and two electrons to be stable. D. Oxygen atoms and hydrogen atoms have opposite charges.

48. Chapter 2 Standardized Test Prep Multiple Choice, continued The illustration below is a space-filling model of water. Use the model to answer the following question. 7. The covalent bonds on the water molecule depicted in the picture above has partial positive charges on the hydrogen atom and a partial negative charge on the oxygen atom. What do the partial positive and partial negative charges on this water molecule mean? A. Water is an ion. B. Water is a polar molecule. C. Water needs a proton and two electrons to be stable. D. Oxygen atoms and hydrogen atoms have opposite charges.

49. Chapter 2 Standardized Test Prep Short Response Covalent bonding is a sharing of electrons between atoms. Why do some atoms share electrons?

50. Chapter 2 Standardized Test Prep Short Response, continued Covalent bonding is a sharing of electrons between atoms. Why do some atoms share electrons? Answer: Sharing electrons achieves a stable number of electrons in the orbitals that correspond to the highest energy level for each atom.