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2. Standardized Test Prep
Resources
Chapter Presentation
Bellringer
Transparencies
Sample Problems
Visual Concepts
Standardized Test Prep

3. Chapter 1 Table of Contents Section 1 What Is Chemistry?
The Science of Chemistry
Table of Contents
Section 1 What Is Chemistry?
Section 2 Describing Matter
Section 3 How Is Matter Classified?

4. Chapter 1
Section 1 What Is Chemistry?
Bellringer
Make a list of all the chemicals that you can think of.
Which ones on that list could you live without?
Which ones on the list could you not live without?

5. Chapter 1
Section 1 What Is Chemistry?
Objectives
Describe ways in which chemistry is a part of your daily life.
Describe the characteristics of three common states of matter.
Describe physical and chemical changes, and give examples of each.

6. Chapter 1 Objectives, continued
Section 1 What Is Chemistry?
Objectives, continued
Identify the reactants and products in a chemical reaction.
List four observations that suggest a chemical change has occurred.

7. Working with the Properties and Changes of Matter
Chapter 1
Section 1 What Is Chemistry?
Working with the Properties and Changes of Matter
A chemical is any substance that has a definite composition.
A chemical reaction is the process by which one or more substances change to produce one or more new substances.

8. Chapter 1
Visual Concepts
Chemical

9. Physical States of Matter
Chapter 1
Section 1 What Is Chemistry?
Physical States of Matter
The states of matter are the physical forms of matter which are solid, liquid, gas, and plasma.
Macroscopic refers to what you can see with the unaided eye.
Microscopic refers to what you would see if you could see individual atoms.

10. Physical States of Matter, continued
Chapter 1
Section 1 What Is Chemistry?
Physical States of Matter, continued
Properties of the Physical States
Solids have a fixed volume and shape that result from the way their particles are arranged.
Liquids have a fixed volume but not a fixed shape.
Gases have neither fixed volume nor shape.

11. Chapter 1
Section 1 What Is Chemistry?
Water in Three States

12. Chapter 1
Visual Concepts
Solid, Liquid and Gas

13. Chapter 1 Changes of Matter
Section 1 What Is Chemistry?
Changes of Matter
Physical changes are changes in which the identity of a substance doesn’t change.
Changes of state are physical changes.
Chemical changes occur when the identities of substances change and new substances form.

14. mercury(II) oxide  mercury + oxygen
Chapter 1
Section 1 What Is Chemistry?
Changes of Matter, continued
Chemical Changes
mercury(II) oxide  mercury + oxygen
Reactants are the substances are the left-hand side of the arrow.
They are used up in the reaction.
Products are the substances are the right-hand side of the arrow.
They are made in the reaction.

15. Evidence of a Chemical Change
Chapter 1
Section 1 What Is Chemistry?
Evidence of a Chemical Change

16. Changes of Matter, continued
Chapter 1
Section 1 What Is Chemistry?
Changes of Matter, continued
Evidence of a Chemical Change
Evidence that a chemical change may be happening generally falls into one of the following categories.
the evolution of a gas
the formation of a precipitate
the release or absorption of energy
a change in temperature or the giving off of light energy
a color change in the reaction system

17. Chapter 1
Visual Concepts
Chemical Reaction

18. Chapter 1 Bellringer Look at the list of words below:
Section 2 Describing Matter
Bellringer
Look at the list of words below:
peanut butter, water, fish, light, garbage, time, motion, the human brain, carbon dioxide, air, yourself, an idea, tree, energy
Sort the words into three categories: matter, not matter, or not sure.
Why is a clear definition of matter important to the study of chemistry?

19. Chapter 1
Section 2 Describing Matter
Objectives
Distinguish between different characteristics of matter, including mass, volume, and weight.
Identify and use SI units in measurements and calculations.
Set up conversion factors, and use them in calculations.

20. Chapter 1 Objectives, continued
Section 2 Describing Matter
Objectives, continued
Identify and describe physical properties, including density.
Identify chemical properties.

21. Matter Has Mass and Volume
Chapter 1
Section 2 Describing Matter
Matter Has Mass and Volume
Matter is anything that has mass and volume.
Volume is the space an object occupies.
Mass is the quantity of matter in an object.
Devices used for measuring mass in a laboratory are called balances.
Weight is the force produced by gravity acting on a mass.

22. Comparing Mass and Weight
Chapter 1
Visual Concepts
Comparing Mass and Weight

23. Chapter 1 Units of Measurement
Section 2 Describing Matter
Units of Measurement
When working with numbers, be careful to distinguish between a quantity and its unit.
Quantity describes something that has magnitude, size, or amount.
Unit is a quantity adopted as a standard of measurement.

24. Units of Measurement, continued
Chapter 1
Section 2 Describing Matter
Units of Measurement, continued
Scientist Express Measurements in SI Units
Scientists worldwide use a set of units called the Système Internationale d’Unités or SI.

25. Units of Measurement, continued
Chapter 1
Section 2 Describing Matter
Units of Measurement, continued
Scientist Express Measurements in SI Units, continued
Base units can be too large or too small for some measurements, so the base units may be modified by attaching prefixes.

26. SI (Système Internationale d’Unités )
Chapter 1
Visual Concepts
SI (Système Internationale d’Unités )

27. Chapter 1
Visual Concepts
Conversion Factor

28. Unit of Measurement, continued
Chapter 1
Section 2 Describing Matter
Unit of Measurement, continued
Converting One Unit to Another
A conversion factor is a simple ratio that relates two units that express a measurement of the same quantity.
example: You can construct conversion factors between kilograms and grams as follows:

29. Using Conversion Factors
Chapter 1
Section 2 Describing Matter
Using Conversion Factors

30. Chapter 1 Converting Units Sample Problem A
Section 2 Describing Matter
Converting Units
Sample Problem A
Convert L to milliliters.

31. Sample Problem A Solution
Chapter 1
Section 2 Describing Matter
Sample Problem A Solution
The equality that links the two units is 1000 mL = 1 L. (The prefix milli- represents 1/1000 of a base unit.)
The conversion factor needed must cancel liters and leave milliliters. Thus, liters must be on the bottom of the fraction and milliliters must be on the top.

32. Chapter 1
Section 2 Describing Matter
Derived Units
Many quantities you can measure need units other than the seven basic SI units.
These units are derived by multiplying or dividing the base units.
Speed is distance divided by time.The derived unit of speed is meters per second (m/s).
A rectangle’s area is found by multiplying its length (in meters) by its width (also in meters).
Its unit is square meters (m2).

33. Derived Units, continued
Chapter 1
Section 2 Describing Matter
Derived Units, continued
Volume is another commonly used derived unit.
The volume of a book can be found by multiplying its length, width, and height.
The unit of volume is the cubic meter (m3).
This unit is too large and inconvenient in most labs. Chemists usually use the liter (L).
1L = 1000 mL = 1000 cm3

34. Chapter 1 Properties of Matter Physical Properties
Section 2 Describing Matter
Properties of Matter
Physical Properties
A physical property of a substance is a characteristic that does not involve a chemical change.
Physical properties of a substance can be determined without changing the nature of a substance.
Physical properties include texture, state, melting point, and boiling point.

35. Properties of Matter, continued
Chapter 1
Section 2 Describing Matter
Properties of Matter, continued
Density is the Ratio of Mass to Volume
The density of an object is the mass of the object divided by volume of the object.
Densities are expressed in derived units such as g/cm3 or g/mL.
Density is calculated as follows:

36. Properties of Matter, continued
Chapter 1
Section 2 Describing Matter
Properties of Matter, continued
Density of an Object
The density of a substance is the same no mater what the size of the sample is.

37. Chapter 1
Visual Concepts
Equation for Density

38. Properties of Matter, continued
Chapter 1
Section 2 Describing Matter
Properties of Matter, continued
Density Can Be Used to Identify Substances
Because the density of a substance is the same for all samples, you can use this property to help identify substances.

39. Properties of Matter, continued
Chapter 1
Section 2 Describing Matter
Properties of Matter, continued
Chemical Properties
A chemical property a property of matter that describes a substance’s ability to participate in chemical reactions.
A chemical property of many substances is that they react with oxygen.
example: rusting
Some substances break down into new substances when heated.

40. Comparing Physical and Chemical Properties
Chapter 1
Visual Concepts
Comparing Physical and Chemical Properties

41. Signs of a Chemical Reaction
Chapter 1
Visual Concepts
Signs of a Chemical Reaction

42. Chapter 1
Section 3 How Is Matter Classified?
Bellringer
Make a list of the ways you have seen things organized.
Which of these methods was the easiest to use and provided the greatest success?

43. Chapter 1 Objectives Distinguish between elements and compounds.
Section 3 How Is Matter Classified?
Objectives
Distinguish between elements and compounds.
Distinguish between pure substances and mixtures.
Classify mixtures as homogenous or heterogeneous.
Explain the difference between mixtures and compounds.

44. Chapter 1 Classifying Matter
Section 3 How Is Matter Classified?
Classifying Matter
An atom is the smallest unit of an element that maintains the properties of that element.
Matter exists in many different forms but there are only 110 types of atoms.
Atoms are joined together to make up all the different kinds of matter.

45. Chapter 1 Pure Substances
Section 3 How Is Matter Classified?
Pure Substances
A pure substance is a sample of matter, either a single element or a single compound, that has definite chemical and physical properties.
Elements are pure substances that only contain one kind of matter. They cannot be separated or broken down into simpler substances by chemical means.
Each element has its own unique set of physical and chemical properties.

46. Chapter 1
Section 3 How Is Matter Classified?
Pure Substances

47. Elements are Pure Substances
Chapter 1
Section 3 How Is Matter Classified?
Elements are Pure Substances
Each elements is represented by a distinct chemical symbol.

48. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Elements as Single Elements or Molecules
A molecule is the smallest unit of a substance that keeps all of the physical and chemical properties of that substance.
A molecule usually consists of two or more atoms combined in a definite ratio.
Diatomic elements exist as two atoms of the same element joined together.

49. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Some Elements Have More Than One Form
Some elements, such as oxygen, phosphorus, sulfur, and carbon, have many different molecular forms.
An allotrope is one of a number of different molecular forms of an element.
The properties of allotropes vary widely.

50. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Some Elements Have More Than One Form, continued
Oxygen exists as allotropes.
Oxygen gas (O2) is colorless and odorless.
Ozone (O3) is toxic and pale blue.

51. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Compounds are Pure Substances
Pure substances that are not elements are compounds. Compounds are composed of more than one kind of atom.
example: carbon dioxide (CO2)
There may be easier ways of preparing them, but compounds can be made from their elements.
Compounds can be broken down into their elements, though often with great difficulty.

52. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Compounds are Represented by Formulas
Because every molecule of a compound is made up of the same kinds of atoms arranged the same way, a compound has characteristic properties and composition.
Compounds can be represented by an abbreviation or formula.
A formula has subscripts which represent the ratio of different atoms in the compound.
example: H2O has 2 hydrogen atoms and one oxygen atom

53. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Compounds are Represented by Formulas, continued
Molecular formulas give information only about what makes up a compound.
example: the molecular formula for aspirin is C9H8O4
A structural formula shows how the atoms are connected
This two-dimensional model does not show the molecule’s true shape.

54. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Compounds are Represented by Formulas, continued
A ball-and-stick model shows the distances between atoms and the angles between them in three dimensions.
A space-filling model attempts to represent the actual sizes of the atoms and not just their relative positions.
A hand-held model can provide more information than models shown on the flat surface of the page.

55. Pure Substances, continued
Chapter 1
Section 3 How Is Matter Classified?
Pure Substances, continued
Compounds are Represented by Formulas, continued
These models convey different information about acetylsalicylic acid (aspirin).

56. Chapter 1
Section 3 How Is Matter Classified?
Mixtures
A mixture is a combination of two or more substances that are not chemically combined.
Air is a mixture of mostly nitrogen and oxygen.
All the different gases in air are physically mixed.
The proportions of the gases can vary.
Water is not a mixture.
The H and O atoms are chemically bonded
The ratio of H to O atoms is always 2 to 1.

57. Chapter 1 Mixtures, continued
Section 3 How Is Matter Classified?
Mixtures, continued
Mixtures Can Vary in Composition and Properties
The proportion of the materials in a mixture can change.
The properties of the mixture may vary.
An alloy is a solid mixture.
example: An alloy of gold and other metal atoms is stronger than pure gold.
18-karat gold contains 18 grams of gold per 24 grams of alloy.
14-karat gold contains 14 grams of gold per 24 grams of alloy.

58. Chapter 1
Particle Models for Gold and Gold Alloy

59. Chapter 1 Mixtures, continued Homogenous Mixtures
Section 3 How Is Matter Classified?
Mixtures, continued
Homogenous Mixtures
A homogenous mixture describes something that has uniform structure or composition throughout.
examples: gasoline, syrup, and air
Because any two samples of a homogenous mixture will have the same proportions of ingredients, homogenous mixtures have the same properties throughout.

60. Chapter 1 Mixtures, continued Heterogeneous Mixtures
Section 3 How Is Matter Classified?
Mixtures, continued
Heterogeneous Mixtures
A heterogeneous mixture describes something that is composed of dissimilar components.
example: A mixture of sand and water is a heterogenous mixture.
Any two samples of a heterogeneous mixture will have the different proportions of ingredients.
Heterogeneous mixtures have different properties throughout.

61. Chapter 1 Examples of Mixtures
Section 3 How Is Matter Classified?
Examples of Mixtures
Mixtures are either homogenous or heterogeneous.

62. Chapter 1
Section 3 How Is Matter Classified?
Types of Mixtures

63. Chapter 1 Mixtures, continued Distinguishing Mixtures from Compounds
Section 3 How Is Matter Classified?
Mixtures, continued
Distinguishing Mixtures from Compounds
The properties of a mixture reflect the properties of the substances it contains.
The properties of a compound often are very different from the properties of the elements that make it up.
A mixture’s components can be present in varying proportions.
A compound has a definite composition in terms of the masses of its elements.

64. Chapter 1
Section 3 How Is Matter Classified?
Classifying Matter

65. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
1. Which of the following is best classified as a homogeneous mixture?
A. blood
B. copper wire
C. pizza
D. hot tea

66. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
1. Which of the following is best classified as a homogeneous mixture?
A. blood
B. copper wire
C. pizza
D. hot tea

67. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
2. Which of the following statements about compounds is true?
F. A compound contains only one element.
G. A compound can be classified as either heterogeneous or homogeneous.
H. A compound has a defined ratio by mass of the elements that it contains.
I. A compound varies in chemical composition depending on the sample size.

68. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
2. Which of the following statements about compounds is true?
F. A compound contains only one element.
G. A compound can be classified as either heterogeneous or homogeneous.
H. A compound has a defined ratio by mass of the elements that it contains.
I. A compound varies in chemical composition depending on the sample size.

69. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
3. Which of the following is an element?
A. BaCl2
B. CO
C. He
D. NaOH

70. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
3. Which of the following is an element?
A. BaCl2
B. CO
C. He
D. NaOH

71. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
4. Is photosynthesis, in which light energy is captured by plants to make sugar from carbon dioxide and water, a physical change or a chemical change? Explain your answer.

72. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
4. Is photosynthesis, in which light energy is captured by plants to make sugar from carbon dioxide and water, a physical change or a chemical change? Explain your answer.
Answer: Photosynthesis is a chemical change because the products of the change are different substances than the starting materials.

73. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
5. A student checks the volume, melting point, and shape of two unlabeled samples of matter and finds that the measurements are identical. He concludes that the samples have the same chemical composition. Is this a valid conclusion? What additional information might be collected to test this conclusion?

74. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
5. A student checks the volume, melting point, and shape of two unlabeled samples of matter and finds that the measurements are identical. He concludes that the samples have the same chemical composition. Is this a valid conclusion? What additional information might be collected to test this conclusion?
Answer: The conclusion is not valid because volume and shape give no information about identity and two different substances can have the same melting point. Additional information could include determining additional physical properties or chemical properties.

75. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
6. Describe the physical and chemical changes that occur when a pot of water is boiled over a campfire.

76. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
6. Describe the physical and chemical changes that occur when a pot of water is boiled over a campfire.
Answer: A physical change is the conversion of liquid water to vapor. A chemical change is the reaction between wood and oxygen that generates heat while forming carbon dioxide and ash.

77. Chapter 1 Reading Skills Standardized Test Preparation
Read the passage below. Then answer the questions.
Willow bark has been a remedy for pain and fever for hundreds of years. In the late eighteenth century, scientists isolated the compound in willow bark that is responsible for its effects. They then converted it to a similar compound, salicylic acid, which is even more effective. In the late nineteenth century, a German chemist, Felix Hoffmann, did research to find a pain reliever that would help his father’s arthritis, but not cause the nausea that is a side effect of salicylic acid. Because the technologies used to synthesize chemicals had improved, he had a number of more effective ways the work with chemical compounds than the earlier chemists. The compound that he made, acetylsalicylic acid, is known as aspirin. It is still one of the most common pain relievers more than 100 years later.

78. Chapter 1 Reading Skills
Standardized Test Preparation
Reading Skills
7. The main reason willow bark has been used as a painkiller and fever treatment is because
F. chemists can use it to make painkilling compounds.
G. it contains elements that have painkilling effects.
H. it contains compounds that have painkilling effects.
I. no other painkillers were available long ago.

79. Chapter 1 Reading Skills
Standardized Test Preparation
Reading Skills
7. The main reason willow bark has been used as a painkiller and fever treatment is because
F. chemists can use it to make painkilling compounds.
G. it contains elements that have painkilling effects.
H. it contains compounds that have painkilling effects.
I. no other painkillers were available long ago.

80. Chapter 1 Reading Skills
Standardized Test Preparation
Reading Skills
8. Why is aspirin normally used as a painkiller instead of salicylic acid?
A. Aspirin tends to cause less nausea.
B. Aspirin is cheaper to make than salicylic acid.
C. Only aspirin can be isolated from willow bark.
D. Salicylic acid is less effective as a painkiller.

81. Chapter 1 Reading Skills
Standardized Test Preparation
Reading Skills
8. Why is aspirin normally used as a painkiller instead of salicylic acid?
A. Aspirin tends to cause less nausea.
B. Aspirin is cheaper to make than salicylic acid.
C. Only aspirin can be isolated from willow bark.
D. Salicylic acid is less effective as a painkiller.

82. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
The table and graph below show a relationship of direct
proportionality between mass (grams) versus volume (cubic centimeters). Use it to answer questions 9 through 12.

83. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
9. Based on information in the table and the graph, what is the relationship between mass and volume of a sample of aluminum?
F. no relationship
G. a linear relationship
H. an inverse relationship
I. an exponential relationship

84. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
9. Based on information in the table and the graph, what is the relationship between mass and volume of a sample of aluminum?
F. no relationship
G. a linear relationship
H. an inverse relationship
I. an exponential relationship

85. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
10. From the data provided, what is the density of aluminum?
A g/cm3
B. 1.0 g/cm3
C. 2.0 g/cm3
D. 2.7 g/cm3

86. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
10. From the data provided, what is the density of aluminum?
A g/cm3
B. 1.0 g/cm3
C. 2.0 g/cm3
D. 2.7 g/cm3

87. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
11. Someone gives you a metal cube that measures 2.0 centimeters on each side and has a mass of 27.5 grams. What can be deduced about the metal from this information and the table?
F. It is not pure aluminum.
G. It has more than one element.
H. It does not contain any aluminum.
I. It is a compound, not an element.

88. Interpreting Graphics
Chapter 1
Standardized Test Preparation
Interpreting Graphics
11. Someone gives you a metal cube that measures 2.0 centimeters on each side and has a mass of 27.5 grams. What can be deduced about the metal from this information and the table?
F. It is not pure aluminum.
G. It has more than one element.
H. It does not contain any aluminum.
I. It is a compound, not an element.

89. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
12. The density of nickel is 8.90 g/cm3. How could this information be applied, along with information from the graph, to determine which of two pieces of metal is aluminum, and which is nickel?

90. Understanding Concepts
Chapter 1
Standardized Test Preparation
Understanding Concepts
12. The density of nickel is 8.90 g/cm3. How could this information be applied, along with information from the graph, to determine which of two pieces of metal is aluminum, and which is nickel?
Answer: From the table, you can calculate the density of aluminum. Aluminum is much less dense than nickel, so if the pieces of metal are the same size, the lighter one is aluminum.