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Properties and Changes in Matter

Learn about the properties of matter, different states of matter, physical and chemical changes, and techniques to separate mixtures.

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Properties and Changes in Matter

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

  2. Section 3.1 Properties of Matter • Identify the characteristics of a substance. • Distinguish between physical and chemical properties. • Differentiate among the physical states of matter. Section 3-1

  3. Section 3.1 Properties of Matter (cont.) Most common substances exist as solids, liquids, and gases, which have diverse physical and chemical properties. Section 3-1

  4. Matter • is anything that has mass and takes up space. • is everything around us. • with a uniform and unchanging composition is a substance. Section 3-1

  5. 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. Section 3-1

  6. States of Matter • 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. Section 3-1

  7. Physical Properties of Matter • A physical propertyis a characteristic that can be observed or measured without changing the sample’s composition. • Color, Density, Melting point, etc. Section 3-1

  8. Physical Properties of Matter (cont.) • Physical properties can be classified as extensive or intensive. • Extensive propertiesdepend on the amount of substance present, such as mass, length, or volume. • Intensive propertiesare independent of the amount of substance present, such as density. Section 3-1

  9. Volume • Boiling point • Density • Mass • Length • Diameter • Circumference • Melting point • Area • Taste • Color • State of matter • Weight Extensive or Intensive?

  10. 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. Tells HOW a chemical will interact with something else. • Iron forming rust • Copper turning green in the air • Chemical properties can change with specific environmental conditions, such as temperature and pressure. Section 3-1

  11. Flammability • Density • Boiling point • Volume • Ability to rust • Ductility • Reactivity • Reacts with vinegar • Length • Combustibility • Melting point • Tendency to corrode • Texture Chemical or Physical property? If it is a physical property, determine if it is intensive or extensive.

  12. Section 3.2 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. Section 3-2

  13. Section 3.2 Changes in Matter (cont.) physical changephase change chemical changelaw of conservation of mass Matter can undergo physical and chemical changes. Section 3-2

  14. 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, evaporation, sublimation, and condensing all describe phase changes in chemistry. Section 3-2

  15. Chemical Changes • A change that involves one or more substances turning into newsubstances is called a chemical change. • Decomposing, rusting, exploding, burning, etc. are all terms that describe chemical changes. Section 3-2

  16. Production of heat or light Production of gases or solids Production of an odor Color change (not always) Indications of a Chemical Change:

  17. Iron rusts Water freezes A sodium pellet is sliced in two Water and sodium react producing hydrogen gas Pancakes cook Sugar dissolves Water evaporates Lunch is digested Water is absorbed by a paper towel Identify the following as a physical or chemical change

  18. 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 Section 3-2

  19. Example: 10.0g of a HgO is heated and the substance decomposes into its individual elements. If 9.26g of Hg is formed, how much oxygen is also produced? Example: A 12.2g sample of X reacts with a sample of Y to form 78.9g of XY. What is the mass of Y that reacted?

  20. Section 3.3 Mixtures of Matter • Contrast mixtures and substances. • Classify mixtures as homogeneous or heterogeneous. • List and describe several techniques used to separate mixtures. Section 3-3

  21. Section 3.3 Mixtures of Matter (cont.) Most everyday matter occurs as mixtures—combinations of two or more substances. Section 3-3

  22. Mixtures • A mixtureis a combination of 2 or more pure substances in which each pure substance retains its individual chemical properties. Section 3-3

  23. Mixtures • A homogenous mixture is a mixture where the composition is constant throughout. (aka solution) • A heterogeneous mixture is a mixture where the individual substances remain distinct. Section 3-3

  24. Sugar water Ice tea Trail mix Ranch salad dressing Black coffee Vinegar Air Polluted air Oil & water Salt water Rocky road ice cream Identify the following as Homogeneous or Heterogeneous

  25. Mixtures (cont.) Section 3-3

  26. Separating Mixtures • Filtrationis a technique that uses a porous barrier to separate a solid from a liquid in a heterogeneous mixture. Section 3-3

  27. Separating Mixtures • Distillationis a separation technique for homogeneous mixtures that is based on the differences in boiling points of substances. Section 3-3

  28. Separating Mixtures • Crystallizationis 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

  29. 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. Section 3-3

  30. Separating Mixtures (cont.) • 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. Section 3-3

  31. Sand and water • Sugar and water • Oil and water • Sand and gravel • A mixture of heptane (bp 98oC) and heptanol (bp 176oC) • A mixture of iodine solid and sodium chloride (HINT: Iodine is not soluble in water) How would you separate the following mixtures?

  32. Section 3.4 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. Section 3-4

  33. Section 3.4 Elements and Compounds (cont.) 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. Section 3-4

  34. 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. Section 3-4

  35. Compounds • 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. Section 3-4

  36. Compounds (cont.) • Elements can never be separated. (and retain the properties of that element) • Compounds can be broken into components by chemical means. • The properties of a compound are different from its component elements. Section 3-4

  37. Compounds (cont.) Section 3-4

  38. Sodium • Water • Soil • Coffee • Oxygen • Cake batter • Table salt • Soup • Air • Salt water • Eggs • Blood • Nitrogen • Carbon dioxide Mixture or Pure Substance?

  39. 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. • Water is always H2O Section 3-4

  40. 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. Section 3-4

  41. Example: A sample of baking soda contains 34.48g Na, 1.51g H, 18.02g C, & 72.00gO. What is the total mass of the sample? What is the percent by mass of each element in baking soda?

  42. Example: A sample of baking soda contains 34.48g Na, 1.51g H, 18.02g C, & 72.00gO. What is the total mass of the sample? = 34.48g + 1.51g + 18.02g + 72.00g = 126.01g

  43. Example: A sample of baking soda contains 34.48g Na, 1.51g H, 18.02g C, & 72.00gO. What is the percent by mass of each element in baking soda?

  44. Example: A sample of baking soda contains 34.48g Na, 1.51g H, 18.02g C, & 72.00gO.

  45. Law of Definite Proportions (cont.) • This table demonstrates that the percentages of elements in sucrose remain the same despite differences in sample amount. Section 3-4

  46. 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. • H2O2 and H2O • Copper(I) chloride and copper(II) chloride Section 3-4

  47. What: Memorize the correct spelling and symbol for elements #1 – 100. • When: Test on Fri. Oct. 17th • Flashcards: name on one side & symbol on the other side; worth +5 on the test • Sheldon: http://www.google.com/url?sa=t&rct=j&q=&esrc=s&source=web&cd=1&cad=rja&uact=8&ved=0CB4QtwIwAA&url=http%3A%2F%2Fwww.youtube.com%2Fwatch%3Fv%3DAmhWwSJDkaw&ei=Wy8TVITFN4e7ogS2iIH4Bg&usg=AFQjCNHs59LSHDDXfgF5UeGLdmYgCqyoog&bvm=bv.75097201,d.aWw • Element Song: Periodic Table TEST

  48. A B C D Section 3.3 Assessment Which is NOT a technique for separating a homogenous mixture? A.crystallization B.distillation C.filtration D.chromatography Section 3-3

  49. A B C D 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. Section 3-2

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