1. Chapter 16.2

2. What we know so far… Matter is made of atoms

3. Atoms are submicroscopic

4. Matter exists in phases Solid

5. Liquid

6. Gas

7. In the SOLID phase Particles are attracted to one another Held together in a tightly packed and fixed 3-d arrangement

8. Microscopic View of a Solid The atoms vibrate but stay close to one another Solids maintain their shape and volume Not easily compressible

9. Intereactive 3-D Diamond Molecule

10. Snowflake Ice Interactive Ice Molecule

11. In the LIQUID phase Particles can move and slide across one another Can assume the shape of their container

12. Microscopic View of a Liquid The atoms vibrate and particles can flow easily past one another Liquids assume the shape of their container

13. Liquids Particles in liquids flow easily across one another

14. Liquids – take the shape of their containers

15. In the GASEOUS PHASE The atoms are moving rapidly, and easily across one another. Lots of free space between the particles They assume the shape of their container.

16. Microscopic View of a Gas The atoms are moving rapidly, and easily across one another. Lots of free space between the particles Compressible

17. Gases Conform to the shape of their containers Easily compressed

18. Gases Particles easily flow and move over one another

19. Let’s Review YouTube - States of Matter

20. Phase Changes Chapter 16.3

21. Substances can change phases GasesLiquidsSolidsLiquids

22. Substances can change phases GasesLiquidsSolidsLiquids Condensation Freezing Evaporation Melting

23. Substances can change phases GAS SOLID Sublimation

24. Changing Phases

25. Water Cycle – Hydrologic Cycle

26. Boiling on the atomic level CLICK The Beaker

27. Boiling Point CLICK The Beaker

28. Heat of Vaporization The amount of energy required to change a liquid to a gas (and vice versa). 2256J/g

29. Heat of Fusion The amount of energy needed to change any substance from solid to liquid ( and vice versa) Water = 334J/g

30. Chapter 16.4

31. Physical Properties Describe the look or feel of a substance Density Texture Phase

32. Every substance has its own set of physical properties

33. Physical Properties CAN Change However…… The substance’s identity remains the same SolidGasLiquid

35. Chemical Properties Characterize the ability of a substance to react with other substances, or to transform from one substance to another.

36. How Substances React or Transform

37. Chemical Changes Change how atoms are Chemically bonded to one another.

38. When we cook with gas……..

39. Take another look CH 4 + 2 O 2 CO 2 + 2H 2 O Chemical Reaction

40. During a chemical reaction… Changes are made in the way atoms bond together New materials are formed CH 4 + 2O 2 CO 2 + 2H 2 O

41. Chapter 16.6

42. Remember….. Periodic table is a listing of all the known elements Atomic number Symbol Atomic Mass He 2 4.003

43. The way the table is organized tells a lot about the elements’ properties

44. Metals are on the left side of the periodic table

45. Most of the known elements are metals Malleable Can be hammered and bent into different shapes without breaking

46. Most of the known elements are metals Ductile Can be drawn into thin wires

47. Most of the known elements are metals Good Conductors Heat Electricity Most solid at room temperature

48. Non-metals are on the right side of the periodic table

49. Non-Metals Poor conductors Not malleable Not ductile Can be solid, liquid or gas at room temperature Shatter when hammered Brittle

51. Metalloids

52. B - Boron Si - Silicon Ge - Germanium As - Arsenic Sb - Antimony Te - Tellurium

53. Metalloids Have both metallic and nonmetallic properties

54. Metalloids Weak conductors “Semi- conductors”

57. Across a period properties gradually change Periodic Trend

58. Smaller Easily lose e- Larger Do not easily lose e-

59. Columns have remarkably similar properties

60. The elements are “grouped” or in “families”

62. Element Families/Grouops

63. Inner Transition Metals

66. Chapter 16.7

67. Elements are made of atoms The element gold ( Au) is made entirely of gold atoms

68. The element silver (Ag) is made entirely of silver atoms

69. The element neon, Ne, is composed entirely of neon atoms

70. Elemental Formula “A notation that uses the atomic symbol and sometimes a numerical subscript to show how atoms of an element are bonded together.” ……confused?

71. Elemental Formula Tell you how the atoms of an element are arranged. ……take a look

72. Elemental Gold The smallest unit of the element gold, as it occurs in nature, is the gold atom itself. Use the element’s symbol Au

73. The smallest unit of the element silver is the silver atom itself Use the symbol Ag Elemental Silver

74. The smallest unit of the element nitrogen is a nitrogen molecule Use the symbol and subscript numbers Elemental Nitrogen N2N2

75. The smallest unit of the element oxygen is an oxygen molecule Use the symbol and subscript numbers Elemental Oxygen O2O2

76. The smallest unit of the element sulfur is a sulfur molecule Use the symbol and subscript numbers Elemental Sulfur S8S8

77. Compound Material composed of different elements bonded to each other

79. Compounds Salt NaCl Sodium chloride

80. Chemical formula Salt NaCl Sodium chloride

81. Chemical formula Water H 2 O water

82. Chemical formula Ammonia NH3 ammonia N H H H

83. Compounds have their own identities and properties

84. Chapter 16.8

85. IUPAC International Union for Pure and Applied Chemistry

86. Developed a chemical naming system  Name reflects the elements a compound contains  How the elements are combined

87. 3 Basic Guidelines #1 The name of the element farthest to the left on the periodic table is followed by the name of the element father to the right, with the suffix “-ide” added to the latter.

88. Examples of Guideline #1 NaCl - Sodium chloride Li 2 O - Lithium oxide CaF 2 - Calcium fluoride The name of the element farthest to the left on the periodic table is followed by the name of the element father to the right, with the suffix “-ide” added to the latter. HCl - Hydrogen chloride MgO - Magnesium oxide Sr 3 P 2 - Strontium phosphide

89. 3 Basic Guidelines #2 Use prefixes to designate numbers of elements in compounds Mono-one Di – two Tri - three

90. Examples of Guideline #2 Carbon & Oxygen Nitrogen & Oxygen CO – Carbon monoxide CO 2 – Carbon dioxide NO2 – Nitrogen dioxide N2O4 – Dinitrogen tetroxide

91. Try this sulfur & oxygen example….. SO 2 SO 3 Sulfur dioxide Sulfur trioxide

92. 3 Basic Guidelines #3 Many compounds have common names

93. Examples of Guideline #3 H2OH2O CH 4 Dihydrogen monoxide ? Water Carbon tetrahydride? Methane

94. You completed Chapter 16! Congratulations!