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 *

8. Physical Properties of Matter
SECTION3.1
Properties of Matter
Physical Properties of Matter
A physical property is a *

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 *
Intensive properties, such as density, are dependent * .

10. Chemical Properties of Matter
SECTION3.1
Properties of Matter
Chemical Properties of Matter
* 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.

13. 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

14. 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.

15. Changes in Matter Physical Changes * is known as a physical change.
SECTION3.2
Changes in Matter
Physical Changes
* 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.

16. Changes in Matter Chemical Changes * is called a chemical change.
SECTION3.2
Changes in Matter
Chemical Changes
* is called a chemical change.
Decomposing, rusting, exploding, burning, or oxidizing are all terms that describe chemical changes.

17. Changes in Matter Conservation of Mass
SECTION3.2
Changes in Matter
Conservation of Mass
The law of conservation of mass states that *.
The mass of the reactants equals the mass of the products.
massreactants = massproducts

19. 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

20. 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.

21. Mixtures of Matter Mixtures A mixture is a *.
SECTION3.3
Mixtures of Matter
Mixtures
A mixture is a *.
A homogenous mixture is a mixture where the *.

22. 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.

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

24. Mixtures of Matter Separating Mixtures
SECTION3.3
Mixtures of Matter
Separating Mixtures
Filtration is a technique that *
Distillation is a separation technique *
Crystallization is a separation technique for *

25. 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 *

27. 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

28. 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.

29. Elements and Compounds
SECTION3.4
Elements and Compounds
Elements
An element is a *
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 *

30. Elements and Compounds
SECTION3.4
Elements and Compounds
Elements (cont.)
The periodic table organizes *
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.

31. Elements and Compounds
SECTION3.4
Elements and Compounds
Compounds (cont.)
A compound is a *.
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.

32. 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.

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

34. 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

35. Elements and Compounds
SECTION3.4
Elements and Compounds
Law of Definite Proportions (cont.)
The relative amounts are expressed as percent by mass, the *.

36. 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.

37. 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.

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

39. 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.

40. 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

41. 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.

42. 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.

43. 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.