1 / 65

Properties and Changes in Matter

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

ninab
Télécharger la présentation

Properties and Changes in Matter

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related