1. CHEMISTRY Matter and Change
Chapter 3: Matter—Properties and Changes

2. Table Of Contents Section 3.1 Properties of Matter
CHAPTER3
Table Of Contents
Section 3.1 Properties of Matter
Section 3.2 Changes in Matter
Section 3.3 Mixtures of Matter
Section 3.4 Elements and Compounds
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3. Properties of Matter Identify the characteristics of a substance.
SECTION3.1
Properties of Matter
Identify the characteristics of a substance.
Distinguish between physical and chemical properties.
Differentiate among the physical states of matter.
density: a ratio that compares the mass of an object to its volume

4. Properties of Matter states of matter solid liquid gas vapor
SECTION3.1
Properties of Matter
states of matter
solid
liquid
gas
vapor
physical property
extensive property
intensive property
chemical property
Most common substances exist as solids, liquids, and gases, which have diverse physical and chemical properties.

5. Properties of Matter Substances
SECTION3.1
Properties of Matter
Substances
Matter is anything that has mass and takes up space.
Matter is everything around us.
Matter with a uniform and unchanging composition is a substance.

6. Properties of Matter States of Matter
SECTION3.1
Properties of Matter
States of Matter
The physical forms of matter, either solid, liquid, or gas, are called the states of matter.
Solids are a form of matter that have their own definite shape and volume.
Liquids are a form of matter that have a definite volume but take the shape of the container.

7. States of Matter (cont.)
SECTION3.1
Properties of Matter
States of Matter (cont.)
Gases have no definite shape or volume. They expand to fill their container.
Vapor refers to the gaseous state of a substance that is a solid or liquid at room temperature.

8. Physical Properties of Matter
SECTION3.1
Properties of Matter
Physical Properties of Matter
A physical property is a characteristic that can be observed or measured without changing the sample’s composition.

9. Physical Properties of Matter (cont.)
SECTION3.1
Properties of Matter
Physical Properties of Matter (cont.)
Extensive properties, such as mass, length, and volume, are dependent on the amount of substance present.
Intensive properties, such as density, are dependent on the what the substance is not how much there is.

10. Chemical Properties of Matter
SECTION3.1
Properties of Matter
Chemical Properties of Matter
The ability of a substance to combine with or change into one or more other substances is called a chemical property.
Iron forming rust
Copper turning green in the air

11. Observing Properties of Matter
SECTION3.1
Properties of Matter
Observing Properties of Matter
A substance can change form–an important concept in chemistry.
Both physical and chemical properties can change with specific environmental conditions, such as temperature and pressure.

12. Density is what kind of property?
SECTION3.1
Section Check
Density is what kind of property?
A. atomic
B. intensive
C. extensive
D. dependent

13. Section Check What defines a gas?
A. Gases have a definite volume and shape.
B. Gases have a definite volume but take the shape of their container.
C. Gases have no definite volume or shape.
D. Gases have a definite shape but no definite volume.

15. SECTION3.2
Changes in Matter
Define physical change and list several common physical changes.
Define chemical change and list several indications that a chemical change has taken place.
Apply the law of conservation of mass to chemical reactions.
observation: orderly, direct information gathering about a phenomenon

16. Changes in Matter physical change phase change chemical change
SECTION3.2
Changes in Matter
physical change
phase change
chemical change
law of conservation of mass
Matter can undergo physical and chemical changes.

17. Changes in Matter Physical Changes
SECTION3.2
Changes in Matter
Physical Changes
A change that alters a substance without changing its composition is known as a physical change.
A phase change is a transition of matter from one state to another.
Boiling, freezing, melting, and condensing all describe phase changes in chemistry.

18. Changes in Matter Chemical Changes
SECTION3.2
Changes in Matter
Chemical Changes
A change that involves one or more substances turning into new substances is called a chemical change.
Decomposing, rusting, exploding, burning, or oxidizing are all terms that describe chemical changes.

19. Changes in Matter Conservation of Mass
SECTION3.2
Changes in Matter
Conservation of Mass
The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction, it is conserved.
The mass of the reactants equals the mass of the products.
massreactants = massproducts

20. SECTION3.2
Section Check
When one substances turns into another, what kind of change has taken place?
A. chemical reaction
B. physical reaction
C. extensive reaction
D. nuclear reaction

21. The law of conservation of mass states that:
SECTION3.2
Section Check
The law of conservation of mass states that:
A. Matter can be created and destroyed.
B. Matter can be created but not destroyed.
C. The products of a reaction always have a greater mass than the reactants.
D. The products of a reaction must have the same mass as the reactants.

23. Mixtures of Matter Contrast mixtures and substances.
SECTION3.3
Mixtures of Matter
Contrast mixtures and substances.
Classify mixtures as homogeneous or heterogeneous.
List and describe several techniques used to separate mixtures.
substance: a form of matter that has a uniform and unchanging composition; also known as a pure substance

24. Mixtures of Matter mixture heterogeneous mixture homogeneous mixture
SECTION3.3
Mixtures of Matter
mixture
heterogeneous mixture
homogeneous mixture
solution
filtration
distillation
crystallization
sublimation
chromatography
Most everyday matter occurs as mixtures—combinations of two or more substances.

25. Mixtures of Matter Mixtures
SECTION3.3
Mixtures of Matter
Mixtures
A mixture is a combination of two or more pure substances in which each pure substance retains its individual chemical properties.
A homogenous mixture is a mixture where the composition is constant throughout.

26. Mixtures of Matter Mixtures (cont.)
SECTION3.3
Mixtures of Matter
Mixtures (cont.)
Homogeneous mixtures are also called solutions.
A heterogeneous mixture is a mixture where the individual substances remain distinct.

27. SECTION3.3
Mixtures of Matter
Mixtures (cont.)

28. Mixtures of Matter Separating Mixtures
SECTION3.3
Mixtures of Matter
Separating Mixtures
Filtration is a technique that uses a porous barrier to separate a solid from a liquid in a heterogeneous mixture.
Distillation is a separation technique for homogeneous mixtures that is based on the differences in boiling points of substances.
Crystallization is a separation technique for homogenous mixtures that results in the formation of pure solid particles from a solution containing the dissolved substance.

29. Separating Mixtures (cont.)
SECTION3.3
Mixtures of Matter
Separating Mixtures (cont.)
Sublimation is the process of a solid changing directly to a gas, which can be used to separate mixtures of solids when one sublimates and the other does not.
Chromatography is a technique that separates the components of a mixture on the basis of tendency of each to travel across the surface of another material.

30. Which is NOT a technique for separating a homogenous mixture?
SECTION3.3
Section Check
Which is NOT a technique for separating a homogenous mixture?
A. crystallization
B. distillation
C. filtration
D. chromatography

31. Which of the following is a heterogeneous mixture?
SECTION3.3
Section Check
Which of the following is a heterogeneous mixture?
A. seawater
B. silver mercury amalgam
C. atmosphere
D. salad dressing

33. Elements and Compounds
SECTION3.4
Elements and Compounds
Distinguish between elements and compounds.
Describe the organization of elements in the periodic table.
Explain how all compounds obey the laws of definite and multiple proportions.
proportion: the relation of one part to another or to the whole with respect to quantity

34. Elements and Compounds
SECTION3.4
Elements and Compounds
element
periodic table
compound
law of definite proportions
percent by mass
law of multiple proportions
A compound is a combination of two or more elements.

35. Elements and Compounds
SECTION3.4
Elements and Compounds
Elements
An element is a pure substance that cannot be separated into simpler substances by physical or chemical means.
92 elements occur naturally on Earth.
Each element has a unique name and a one, two, or three-letter symbol.
The periodic table organizes the elements into a grid of horizontal rows called periods and vertical columns called groups.

36. Elements and Compounds
SECTION3.4
Elements and Compounds
Elements (cont.)
The periodic table organizes the elements into a grid of horizontal rows called periods and vertical columns called groups.
Elements in the same group have similar chemical and physical properties.
The table is called periodic because the pattern of similar properties repeats from period to period.

37. Elements and Compounds
SECTION3.4
Elements and Compounds
Compounds (cont.)
A compound is a made up of two or more elements combined chemically.
Most of the matter in the universe exists as compounds.
Table salt, NaCl, and water, H2O, are compounds.
Unlike elements, compounds can be broken into smaller components by chemical means.

38. Elements and Compounds
SECTION3.4
Elements and Compounds
Compounds (cont.)
Separating a compounds into its elements often requires external energy, such as heat or electricity.
This figure shows electrolysis of water to form hydrogen and oxygen gas.

39. Elements and Compounds
SECTION3.4
Elements and Compounds
Compounds (cont.)
The properties of a compound are different from its component elements.

40. Elements and Compounds
SECTION3.4
Elements and Compounds
Law of Definite Proportions
The law of definite proportions states that a compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample.
Ex. Water is always composed of 2 Hydrogen to 1 Oxygen

41. Elements and Compounds
SECTION3.4
Elements and Compounds
Law of Definite Proportions (cont.)
The relative amounts are expressed as percent by mass, the ratio of the mass of each element to the total mass of the compound expressed as a percentage.

42. Elements and Compounds
SECTION3.4
Elements and Compounds
Law of Definite Proportions (cont.)
This table demonstrates that the percentages of elements in sucrose remain the same despite differences in sample amount.

43. Elements and Compounds
SECTION3.4
Elements and Compounds
Law of Multiple Proportions
The law of multiple proportions states that when different compounds are formed by a combination of the same elements, different masses of one element combine with the same relative mass of the other element in whole number ratios.
Ex. Peroxide, H2O2, and water, H2O.
Different compounds formed from the same elements.
Hydrogen mass the same in both compounds but oxygen mass is a 2:1 ratio in peroxide to water.

44. Elements and Compounds
SECTION3.4
Elements and Compounds
Law of Multiple Proportions (cont.)

45. What is a period on the periodic table of the elements?
SECTION3.4
Section Check
What is a period on the periodic table of the elements?
A. a vertical columns
B. even numbered elements only
C. horizontal rows
D. the last vertical column only

46. An element is a substance that cannot be
SECTION3.4
Section Check
An element is a substance that cannot be
A. divided into simpler substances by physical or chemical means.
B. combined to form a mixture.
C. combined to form an element.
D. different phases.

48. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Resources
Chemistry Online
Study Guide
Chapter Assessment
Standardized Test Practice

49. Properties of Matter Key Concepts
SECTION3.1
Properties of Matter
Study Guide
Key Concepts
The three common states of matter are solid, liquid, and gas.
Physical properties can be observed without altering a substance’s composition.
Chemical properties describe a substance’s ability to combine with or change into one or more new substances.
External conditions can affect both physical and chemical properties.

50. Changes in Matter Key Concepts
SECTION3.2
Changes in Matter
Study Guide
Key Concepts
A physical change alters the physical properties of a substance without changing its composition.
A chemical change, also known as a chemical reaction, involves a change in a substance’s composition.
In a chemical reaction, reactants form products.
The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction; it is conserved.
massreactants = massproducts

51. Mixtures of Matter Key Concepts
SECTION3.3
Mixtures of Matter
Study Guide
Key Concepts
A mixture is a physical blend of two or more pure substances in any proportion.
Solutions are homogeneous mixtures.
Mixtures can be separated by physical means. Common separation techniques include filtration, distillation, crystallization, sublimation, and chromatography.

52. Elements and Compounds
SECTION3.4
Elements and Compounds
Study Guide
Key Concepts
Elements cannot be broken down into simpler substances by physical or chemical means.
Elements are organized in the periodic table of the elements.
Compounds are chemical combinations of two or more elements and their properties differ from the properties of their component elements.

53. Elements and Compounds
SECTION3.4
Elements and Compounds
Study Guide
Key Concepts
The law of definite proportions states that a compound is always composed of the same elements in the same proportions.
The law of multiple proportions states that if elements form more than one compound, those compounds will have compositions that are whole-number multiples of each other.

54. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Chapter Assessment
Which of the following is NOT a physical property of water?
A. Ice melts at 0°C.
B. Water boils at 100.
C. Water reacts violently with pure sodium.
D. Water is a liquid at room temperature.

55. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Chapter Assessment
28.0 grams of nitrogen gas reacts completely with 6.0 grams of hydrogen to form 34.0 grams of ammonia. What does this demonstrate?
A. the law of conservation of energy
B. sublimation
C. distillation
D. the law of conservation of mass

56. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Chapter Assessment
What is the best way to separate salt dissolved in water?
A. sublimation
B. crystallization
C. freezing
D. filtration

57. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Chapter Assessment
Two or more elements chemically joined form what?
A. substance
B. heterogeneous mixture
C. homogenous solution
D. compound

58. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Chapter Assessment
What is the ratio of oxygen to carbon in carbon dioxide (CO2)?
A. 2:1
B. 1:2
C. 1:1
D. 1:3

59. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Standardized Test Practice
Which is NOT a chemical reaction?
A. a car rusting
B. dissolving sugar in water
C. wood burning
D. a banana ripening

60. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Standardized Test Practice
Which describes a substance that is in the liquid state?
A. It has a definite shape.
B. It has no definite volume.
C. It can be compressed into a smaller volume.
D. It has a definite volume.

61. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Standardized Test Practice
Elements in the same group are likely to have similar ____.
A. physical properties
B. densities
C. chemical properties
D. melting points

62. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Standardized Test Practice
Filtration is an easy way to separate what?
A. heterogeneous mixture
B. homogeneous mixture
C. compounds
D. solutions

63. Matter—Properties and Changes
CHAPTER3
Matter—Properties and Changes
Standardized Test Practice
Compounds can be broken into their component elements by which of the following?
A. crystallization
B. distillation
C. filtration
D. chemical reaction

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