1. Matter - Properties and Change

2. Section 3.1Properties of MatterProperties of Matter Section 3.2Changes in MatterChanges in Matter Section 3.3Mixtures of MatterMixtures of Matter Section 3.4Elements and CompoundsElements and Compounds Exit CHAPTER 3 Table Of Contents Click a hyperlink to view the corresponding slides.

3. 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. SECTION 3.1 Properties of Matter

4. 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 SECTION 3.1 Properties of Matter

5. A substance, also known as a chemical, is matter that has a definite composition. 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. SECTION 3.1 Properties of Matter Substances

6. 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. SECTION 3.1 Properties of Matter States of Matter

7. 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. Plasma - It does not occur naturally on earth except in the form of lightning bolts. Similar to gas in which a certain portion of the particles are ionized. SECTION 3.1 Properties of Matter States of Matter (cont.)

8. A physical property is a characteristic that can be observed or measured without changing the sample’s composition. SECTION 3.1 Properties of Matter Physical Properties of Matter

9. Extensive properties, are dependent on the amount of substance present. Intensive properties, are dependent on the what the substance is not how much there is. SECTION 3.1 Properties of Matter Physical Properties of Matter (cont.)

10. Extensive Properties Intensive Properties

11. 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 SECTION 3.1 Properties of Matter Chemical Properties of Matter

12. 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. SECTION 3.1 Properties of Matter Observing Properties of Matter

13. Density is what kind of property? A.atomic B.intensive C.extensive D.dependent Section Check SECTION 3.1

14. 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. Section Check SECTION 3.1

15. Changes in Matter

16. 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. SECTION 3.2 Changes in Matter

17. Matter can undergo physical and chemical changes. physical change phase change chemical change law of conservation of mass SECTION 3.2 Changes in Matter

18. 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. SECTION 3.2 Changes in Matter Physical Changes

19. 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. SECTION 3.2 Changes in Matter Chemical Changes

20. 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. mass reactants = mass products SECTION 3.2 Changes in Matter Conservation of Mass

21. 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 Section Check SECTION 3.2

22. 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. Section Check SECTION 3.2

23. Mixtures of Matter

24. Contrast mixtures and substances. substance: a form of matter that has a uniform and unchanging composition; also known as a pure substance Classify mixtures as homogeneous or heterogeneous. List and describe several techniques used to separate mixtures. SECTION 3.3 Mixtures of Matter

25. Most everyday matter occurs as mixtures—combinations of two or more substances. mixture heterogeneous mixture homogeneous mixture solution filtration distillation crystallization sublimation chromatography SECTION 3.3 Mixtures of Matter

26. A mixture is a combination of two or more pure substances in which each pure substance retains its individual chemical properties. A heterogeneous mixture is a mixture where the individual substances remain distinct. Two types – colloid and suspension SECTION 3.3 Mixtures of Matter Mixtures

27. A homogenous mixture is a mixture where the composition is constant throughout. Homogeneous mixtures are also called solutions. SECTION 3.3 Mixtures of Matter Mixtures (cont.)

28. SECTION 3.3 Mixtures of Matter Mixtures (cont.)

29. 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. SECTION 3.3 Mixtures of Matter Separating Mixtures

30. 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. SECTION 3.3 Mixtures of Matter Separating Mixtures (cont.)

31. Which is NOT a technique for separating a homogenous mixture? A.crystallization B.distillation C.filtration D.chromatography SECTION 3.3 Section Check

32. Which of the following is a heterogeneous mixture? A.seawater B.silver mercury amalgam C.atmosphere D.salad dressing SECTION 3.3 Section Check

33. Elements and Compounds

34. Distinguish between elements and compounds. proportion: the relation of one part to another or to the whole with respect to quantity Describe the organization of elements in the periodic table. Explain how all compounds obey the laws of definite and multiple proportions. SECTION 3.4 Elements and Compounds

35. A compound is a combination of two or more elements. element periodic table compound law of definite proportions percent by mass law of multiple proportions SECTION 3.4 Elements and Compounds

36. 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. SECTION 3.4 Elements and Compounds Elements

37. 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. SECTION 3.4 Elements and Compounds Elements (cont.)

38. 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, H 2 O, are compounds. Unlike elements, compounds can be broken into smaller components by chemical means. SECTION 3.4 Elements and Compounds Compounds (cont.)

39. 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. SECTION 3.4 Elements and Compounds Compounds (cont.)

40. The properties of a compound are different from its component elements. SECTION 3.4 Elements and Compounds Compounds (cont.)

41. Comparison of Mixture and a Compound MixtureCompound Properties of the components Properties of the elements are not changedare changed No heat needed to make a mixtureHeat is usually needed to make a compound A mixture can be fairly easilyDifficult to separate into its separatedelements Variable composition Fixed composition - chemical formula can be written

42. 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 SECTION 3.4 Elements and Compounds Law of Definite Proportions

43. 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. SECTION 3.4 Elements and Compounds Law of Definite Proportions (cont.)

44. This table demonstrates that the percentages of elements in sucrose remain the same despite differences in sample amount. SECTION 3.4 Elements and Compounds Law of Definite Proportions (cont.)

45. The law of multiple proportions states that if elements form more than one compound, those compounds will have compositions that are small, whole number multiples of each other Ex. Fe 2 O 3 and FeO –Ex. Peroxide, H 2 O 2, and water, H 2 O. –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. SECTION 3.4 Elements and Compounds Law of Multiple Proportions

46. The law of multiple proportions states that if the elements X and Y form two compounds, the different masses of Y that combine with a fixed mass of X can be expressed as a ratio of small whole numbers. Mass ratio compound I Mass ratio compound II

47. SECTION 3.4 Elements and Compounds Law of Multiple Proportions (cont.)

48. 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 SECTION 3.4 Section Check

49. 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. SECTION 3.4 Section Check

51. Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Resources CHAPTER 3 Matter—Properties and Changes

52. 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. SECTION 3.1 Properties of Matter Study Guide

53. 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. mass reactants = mass products Study Guide SECTION 3.2 Changes in Matter Key Concepts

54. 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. Study Guide SECTION 3.3 Mixtures of Matter Key Concepts

55. 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. Study Guide SECTION 3.4 Elements and Compounds Key Concepts

56. 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. SECTION 3.4 Elements and Compounds Study Guide Key Concepts

57. 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 roomtemperature. Chapter Assessment CHAPTER 3 Matter—Properties and Changes

58. 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 Chapter Assessment CHAPTER 3 Matter—Properties and Changes

59. What is the best way to separate salt dissolved in water? A.sublimation B.crystallization C.freezing D.filtration Chapter Assessment CHAPTER 3 Matter—Properties and Changes

60. Two or more elements chemically joined form what? A.substance B.heterogeneous mixture C.homogenous solution D.compound Chapter Assessment CHAPTER 3 Matter—Properties and Changes

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

62. Which is NOT a chemical reaction? A.a car rusting B.dissolving sugar in water C.wood burning D.a banana ripening CHAPTER 3 Matter—Properties and Changes Standardized Test Practice

63. 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. CHAPTER 3 Matter—Properties and Changes Standardized Test Practice

64. Elements in the same group are likely to have similar ____. A.physical properties B.densities C.chemical properties D.melting points CHAPTER 3 Matter—Properties and Changes Standardized Test Practice

65. Filtration is an easy way to separate what? A.heterogeneous mixture B.homogeneous mixture C.compounds D.solutions CHAPTER 3 Matter—Properties and Changes Standardized Test Practice

66. Compounds can be broken into their component elements by which of the following? A.crystallization B.distillation C.filtration D.chemical reaction CHAPTER 3 Matter—Properties and Changes Standardized Test Practice

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