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2. Standardized Test Prep
Resources
Chapter Presentation
Visual Concepts
Transparencies
Standardized Test Prep

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

4. Chapter 2 Objectives Define the term matter.
Section 1 Composition of Matter
Chapter 2
Objectives
Define the term matter.
Explain the relationship between elements and atoms.
Draw and label a model of the structure of an atom.
Explain how compounds affect an atom’s stability.
Contrast covalent and ionic bonds.

5. Chapter 2 Matter Matter is anything that occupies space and has mass.
Section 1 Composition of Matter
Chapter 2
Matter
Matter is anything that occupies space and has mass.
Mass is the quantity of matter an object has.

6. Section 1 Composition of Matter
Chapter 2
Matter

7. Chapter 2 Elements and Atoms
Section 1 Composition of Matter
Chapter 2
Elements and Atoms
Elements are 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.

8. Section 1 Composition of Matter
Chapter 2
Element

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

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

11. Elements and Atoms, continued
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 called isotopes.

12. Section 1 Composition of Matter
Chapter 2
Compounds
Compounds consist 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
Compounds

14. Chapter 2 Compounds, continued Covalent Bonds
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
Covalent Bonding

16. Chapter 2 Compounds, continued Ionic Bonds
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.

17. Section 1 Composition of Matter
Chapter 2
Ionic Bonding

18. Section 1 Composition of Matter
Chapter 2
Ionic Bonding

19. Section 2 Energy
Chapter 2
Objectives
Describe the physical properties of each state of matter.
Describe the role of reactants and products in chemical reactions.
Explain the relationship between enzymes and activation energy.
Explain how oxidation and reduction reactions are linked.

20. Chapter 2 Energy and Matter States of Matter
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.

21. Section 2 Energy
Chapter 2
Energy

22. Energy and Chemical Reactions
Section 2 Energy
Chapter 2
Energy and Chemical Reactions
Reactants are substances that enter chemical reactions.
Products are substances produced by chemical reactions.

23. Energy and Chemical Reactions
Section 2 Energy
Chapter 2
Energy and Chemical Reactions

24. Energy and Chemical Reactions, continued
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.

25. Activation Energy and Chemical Reactions
Section 2 Energy
Chapter 2
Activation Energy and Chemical Reactions

26. Energy and Chemical Reactions, continued
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.

27. Chapter 2 Objectives Describe the structure of a water molecule.
Section 3 Water and Solutions
Chapter 2
Objectives
Describe the structure of a water molecule.
Explain how 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.

28. Section 3 Water and Solutions
Chapter 2
Polarity
Water is considered to be a polar molecule due to an uneven distribution of charge.
The electrons in a water molecule are shared unevenly between hydrogen and oxygen.

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

30. Chapter 2 Hydrogen Bonding
Section 3 Water and Solutions
Chapter 2
Hydrogen Bonding
A hydrogen bond is the force of attraction between a hydrogen molecule with a partial positive charge and another atom or molecule with a partial or full negative charge.

31. Hydrogen Bonding, continued
Section 3 Water and Solutions
Chapter 2
Hydrogen Bonding, continued
Cohesion and Adhesion
Cohesion is an attractive force that holds molecules of a single substance together, such as water molecules.
Adhesion is the attractive force between two particles of different substances, such as water molecules and glass molecules.

32. Comparing Cohesion and Adhesion
Section 3 Water and Solutions
Chapter 2
Comparing Cohesion and Adhesion

33. Hydrogen Bonding, continued
Section 3 Water and Solutions
Chapter 2
Hydrogen Bonding, continued
Temperature Moderation
Water has the ability to absorb a relatively large amount of energy as heat and the ability to cool surfaces through evaporation.

34. Hydrogen Bonding, continued
Section 3 Water and Solutions
Chapter 2
Hydrogen Bonding, continued
Density of Ice
Solid water is less dense than liquid water due to the shape of the water molecule and hydrogen bonding.

35. Section 3 Water and Solutions
Chapter 2
Solutions
A solution consists of a solute dissolved in a solvent.

36. Chapter 2 Acids and Bases Ionization of Water
Section 3 Water and Solutions
Chapter 2
Acids and Bases
Ionization of Water
Water ionizes into hydronium ions (H3O+) and hydroxide ions (OH–).

37. Acids and Bases, continued
Section 3 Water and Solutions
Chapter 2
Acids and Bases, continued
Acids
Acidic solutions contain more hydronium ions than hydroxide ions.

38. Acids and Bases, continued
Section 3 Water and Solutions
Chapter 2
Acids and Bases, continued
Bases
Basic solutions contain more hydroxide ions than hydronium ions.

39. Section 3 Water and Solutions
Chapter 2
Bases

40. Acids and Bases, continued
Section 3 Water and Solutions
Chapter 2
Acids and Bases, continued pH
Scientists have developed a scale for comparing the relative concentrations of hydronium ions and hydroxide ions in a solution. This scale is called the pH scale, and it ranges from 0 to 14.

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

42. Acids and Bases, continued
Section 3 Water and Solutions
Chapter 2
Acids and Bases, continued
Buffers
Buffers are chemicals that neutralize the effects of adding small amounts of either an acid or a base to a solution.

43. Section 3 Water and Solutions
Chapter 2 pH

44. Chapter 2 Multiple Choice
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

45. Multiple Choice, continued
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

46. Multiple Choice, continued
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

47. Multiple Choice, continued
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

48. Multiple Choice, continued
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

49. Multiple Choice, continued
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

50. Multiple Choice, continued
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

51. Multiple Choice, continued
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

52. Multiple Choice, continued
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

53. Multiple Choice, continued
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

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

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

56. Multiple Choice, continued
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.

57. Multiple Choice, continued
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.

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

59. Short Response, continued
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.

60. Chapter 2 Extended Response
Standardized Test Prep
Extended Response
Pure water contains equal numbers of hydronium ions and hydroxide ions and is therefore a neutral solution.
Part A What is the initial cause of the dissociation of water molecules into hydrogen and hydroxide ions? Explain the process.
Part B After water dissociates, hydronium ions are formed. Explain this process.

61. Extended Response, continued
Chapter 2
Standardized Test Prep
Extended Response, continued
Answer:
Part A Water molecules collide as they move about. Some collisions result in the loss of a hydrogen nucleus. Thus, the water molecule gives rise to a hydrogen ion and a hydroxide ion.
Part B The hydrogen ion from the initial dissociation of water combines with another water molecule to form a hydronium ion.

62. Section 1 Composition of Matter
Chapter 2
Elements and Atoms

63. Section 1 Composition of Matter
Chapter 2
Elements and Atoms

64. Section 1 Composition of Matter
Chapter 2
Compounds

65. Section 2 Energy
Chapter 2
Energy and Matter

66. Section 3 Water and Solutions
Chapter 2
Hydrogen Bonding