3. Chapter Menu Matter—Properties and Change Section 3.1Section 3.1Properties of Matter Section 3.2Section 3.2 Changes in Matter Section 3.3Section 3.3 Mixtures of Matter Section 3.4Section 3.4 Elements and Compounds Exit Click a hyperlink or folder tab to view the corresponding slides.

4. Section 3-1 Section 3.1 Properties of Matter Identify the characteristics of a substance. density: a ratio that compares the mass of an object to its volume Distinguish between physical and chemical properties. Differentiate among the physical states of matter.

5. Section 3-1 Section 3.1 Properties of Matter (cont.) states of matter solid liquid gas vapor Most common substances exist as solids, liquids, and gases, which have diverse physical and chemical properties. physical property extensive property intensive property chemical property

6. Section 3-1 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.

7. Section 3-1 States of Matter The physical forms of matter are called the states of matter. The most common forms on Earth are solid, liquid, and gas. states of matter Solids are a form of matter that have their own definite shape and volume.Solids Liquids are a form of matter that have a definite volume but take the shape of the container.Liquids

8. Section 3-1 States of Matter (cont.) Gases have no definite shape or volume. They expand to fill their container.Gases Vapor refers to the gaseous state of a substance that is a solid or liquid at room temperature.Vapor

9. Section 3-1 Physical Properties of Matter A physical property is a characteristic that can be observed or measured without changing the sample’s composition.physical property

10. Section 3-1 Physical Properties of Matter (cont.) Extensive properties are dependent on the amount of substance present, such as mass, length, or volume.Extensive properties Intensive properties are independent of the amount of substance present, such as density.Intensive properties

11. Section 3-1 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.chemical property Iron rusting Copper forming patina

12. Section 3-1 Observing Properties of Matter A substance can change form–an important concept in chemistry. Physical and chemical properties can change with specific environmental conditions, such as temperature and pressure.

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15. A.A B.B C.C D.D Section 3-1 Section 3.1 Assessment Density is what kind of property? A.atomic B.intensive C.extensive D.dependent

16. A.A B.B C.C D.D Section 3-1 Section 3.1 Assessment 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.

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18. Section 3-2 Section 3.2 Changes in Matter Define physical change and list several common physical changes. observation: orderly, direct information gathering about a phenomenon Define chemical change and list several indications that a chemical change has taken place. Apply the law of conservation of mass to chemical reactions.

19. Section 3-2 Section 3.2 Changes in Matter (cont.) Matter can undergo physical and chemical changes. physical change phase change chemical change law of conservation of mass

20. Section 3-2 Physical Changes A change that alters a substance without changing its composition is known as a physical change. physical change A phase change is a transition of matter from one state to another.phase change Boiling, freezing, melting, subliming, and condensing all describe phase changes in chemistry.

21. Section 3-2 Chemical Changes A change that involves one or more substances turning into new substances is called a chemical change.chemical change Decomposing, rusting, exploding, burning, or oxidizing are all examples of terms that describe chemical changes.

22. Section 3-2 Chemical Changes We describe chemical reactions with chemical equations. Chemical equations begin with reactants and end with products. Iron reacts with oxygen to make rust.

23. Section 3-2 Conservation of Mass The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction, it is conserved.law of conservation of mass The mass of the reactants equals the mass of the products. mass reactants = mass products

24. An iron nail has a mass of 12.00 g. It is left exposed to air and it rusts (forms iron oxide). The rusty nail has a mass of 16.35 g. What mass of oxygen was consumed in the reaction? iron + oxygen = iron oxide 12.00 g+ ?= 16.35 g Oxygen = 4.35 g

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27. A.A B.B C.C D.D Section 3-2 Section 3.2 Assessment 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

28. A.A B.B C.C D.D Section 3-2 Section 3.2 Assessment 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.