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Chapter 3: Matter—Properties and Changes

CHEMISTRY Matter and Change. Chapter 3: Matter—Properties and Changes. Table Of Contents. CHAPTER 3. 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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Chapter 3: Matter—Properties and Changes

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

  2. Table Of Contents CHAPTER3 Section 3.1 Properties of Matter Section 3.2 Changes in Matter Section 3.3 Mixtures of Matter Section 3.4 Elements and Compounds Click a hyperlink to view the corresponding slides. Exit

  3. Properties of Matter SECTION3.1 • 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 SECTION3.1 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 SECTION3.1 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.

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

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

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

  9. Properties of Matter SECTION3.1 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. Properties of Matter SECTION3.1 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. • Iron forming rust • Copper turning green in the air

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

  13. Section Check SECTION3.1 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.

  14. Changes in Matter SECTION3.2 • 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

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

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

  17. Changes in Matter SECTION3.2 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.

  18. Changes in Matter SECTION3.2 Conservation of Mass • The law of conservation of massstates 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

  19. Section Check SECTION3.2 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

  20. Section Check SECTION3.2 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.

  21. Mixtures of Matter SECTION3.3 • 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

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

  23. Mixtures of Matter SECTION3.3 Mixtures • A mixtureis 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.

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

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

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

  27. Mixtures of Matter SECTION3.3 Separating Mixtures(cont.) • Sublimationis 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. • Chromatographyis a technique that separates the components of a mixture on the basis of tendency of each to travel across the surface of another material.

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

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

  30. Elements and Compounds SECTION3.4 • 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

  31. Elements and Compounds SECTION3.4 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.

  32. Elements and Compounds SECTION3.4 Elements • An elementis 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 tableorganizes the elements into a grid of horizontal rows called periods and vertical columns called groups.

  33. Elements and Compounds SECTION3.4 Elements (cont.) • The periodic tableorganizes 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.

  34. Elements and Compounds SECTION3.4 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.

  35. Elements and Compounds SECTION3.4 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.

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

  37. Elements and Compounds SECTION3.4 Law of Definite Proportions • The law of definite proportionsstates 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

  38. Elements and Compounds SECTION3.4 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.

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

  40. Elements and Compounds SECTION3.4 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.

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

  42. Section Check SECTION3.4 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

  43. Section Check SECTION3.4 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.

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

  45. Properties of Matter SECTION3.1 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.

  46. Changes in Matter SECTION3.2 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

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