1. Matter What is Matter? Section 2.1

2. Matter Matter is what the world is made of. Matter is what the world is made of. Matter has mass and volume Matter has mass and volume All objects consists of matter. All objects consists of matter.

3. Mass A measure of the quantity of matter in an object A measure of the quantity of matter in an object Measured by grams (g) and kilograms (kg) Measured by grams (g) and kilograms (kg) Doesn’t change due to location Doesn’t change due to location

4. Weight Weight is the response of mass to the pull of gravity. Metric unit of weight is the Newton (N). Weight is the response of mass to the pull of gravity. Metric unit of weight is the Newton (N). Does change due to location Does change due to location

6. Mass vs. Weight Weight = mass x acceleration of gravity Weight = mass x acceleration of gravity Mass kg X 9.8 m/s 2 = Weight (on earth) N Mass kg X 9.8 m/s 2 = Weight (on earth) N What is your weight on earth? (Remember 1 kg = 2.2 lbs) What is your weight on earth? (Remember 1 kg = 2.2 lbs)

7. What is your weight on earth? mass X 9.8 m/s 2 = Weight (on earth) mass X 9.8 m/s 2 = Weight (on earth) (Remember 1 kg = 2.2 lbs) (Remember 1 kg = 2.2 lbs)

8. Volume The amount of space an object takes up is called its volume. The amount of space an object takes up is called its volume. Volume is measured in liters (L), milliliters (mL), and cubic centimeters (cm 3 ) Volume is measured in liters (L), milliliters (mL), and cubic centimeters (cm 3 )

9. Chemistry The study of matter and how it changes The study of matter and how it changes

10. Element A substance that cannot be broken down into simpler substances A substance that cannot be broken down into simpler substances Everything Everything is made of is made of elements elements

11. Atom Smallest particle of an element Smallest particle of an element Has all the properties of that element Has all the properties of that element Unique Unique

12. Molecule Smallest unit of a compound that exhibits all the properties and characteristic of that compound Smallest unit of a compound that exhibits all the properties and characteristic of that compound  Element a substance that cannot be broken down into simpler substances a substance that cannot be broken down into simpler substances

13. Compound A substance made of atoms of more than one element bound together A substance made of atoms of more than one element bound together

14. Earth’s Composition

15. Chemical Formula Chemical symbols and numbers indicating the atoms contained in the basic unit of a substance Chemical symbols and numbers indicating the atoms contained in the basic unit of a substance A formula that represents one molecule of a compound A formula that represents one molecule of a compound Empirical formula is the simplest formula of a compound Empirical formula is the simplest formula of a compound Molecular formula is a simple multiple of its empirical formula Molecular formula is a simple multiple of its empirical formula

16. Elements in the Human Body

17. Chemical Formula Examples Examples  C 16 H 10 N 2 O 2 Indigo  C 12 H 22 O 11 Sugar

18. Classifying Matter

24. Classification of Matter

25. Pure Substance Any matter that has a fixed composition and definite properties Any matter that has a fixed composition and definite properties

26. Mixture A combination of more than one pure substance A combination of more than one pure substance Blending together of pure substances Blending together of pure substances

27. Mixture Homogeneous Homogeneous  Same kind  Uniform in structure or composition throughout

28. Mixture Heterogeneous Heterogeneous  Different kinds  Not complete mixed  Consists of dissimilar elements or parts Marble

29. Mixtures Miscible Miscible  Able to dissolve into each other in various proportions

30. Mixtures Immiscible Immiscible  describes two or more liquids that do not mix into each other Oil and Water

31. Platform Holly Oil Spill November 1981

32. Matter Matter and Energy Section 2.2

33. Matter and Energy 1. Think about the properties of ice. It is somewhat hard and cannot be compressed easily. Which drawing do you think represents a solid? Why?

34. Matter and Energy 2. Think about the properties of gases. They are not hard, and they can be compressed. Which drawing represents a gas? Why?

35. Matter and Energy 3. In which state(s) of matter are the particles touching?

36. Matter and Energy 4. In which drawing do you think the particles have the least effect on one another? Why?

37. Kinetic Theory All matter is made up of atoms and molecules that act like tiny particles All matter is made up of atoms and molecules that act like tiny particles Tiny particles are always in motion. The higher the temperature the faster they move Tiny particles are always in motion. The higher the temperature the faster they move At the same temperature heavier particles move slower than lighter particles At the same temperature heavier particles move slower than lighter particles

38. States of Matter Four phases of matter Four phases of matter  Solid  Liquid  Gas  Plasma

39. Gases Do not have a regular shape Do not have a regular shape Nor a regular volume Nor a regular volume Take on the shape of their container Take on the shape of their container

40. Particles of a Gas Move fast enough to overcome nearly all of the attraction between them Move fast enough to overcome nearly all of the attraction between them The particles move independently of one another The particles move independently of one another

41. Gas

42. Pressure Force exerted per unit area on a surface Force exerted per unit area on a surface P = F / A P = F / A

43. Pressure Gas particles exert pressure by hitting the walls of a balloon. Gas particles exert pressure by hitting the walls of a balloon. The balloon pops because the internal pressure is more than the balloon can hold. The balloon pops because the internal pressure is more than the balloon can hold.

44. Liquids Have a definite volume Have a definite volume Do not have a definite shape Do not have a definite shape Take on the shape of their container Take on the shape of their container Viscosity Viscosity  The resistance of a liquid to flow

45. Particles of a Liquid Move fast enough to overcome some of the attraction between them Move fast enough to overcome some of the attraction between them The particles are able to slide past one another The particles are able to slide past one another

46. Liquid

47. Solids definite shape definite shape definite volume definite volume Crystalline Solids Crystalline Solids  In many solids, the particles are arranged in a regular, repeating pattern called a crystal. (i.e. salt, quartz)

48. Crystals

49. Solids Amorphous solids Amorphous solids  lose their shape under certain conditions (i.e. tar, candle wax, glass) (i.e. tar, candle wax, glass)

50. Amorphous Solids: Candle Wax

51. Particles of a solid Do not move fast enough to overcome the strong attraction between them Do not move fast enough to overcome the strong attraction between them So they are held tightly in place. So they are held tightly in place. The particles vibrate in place. The particles vibrate in place.

52. Plasma Rare on earth. (lightning) Rare on earth. (lightning) Most common phase in the universe Most common phase in the universe Stars, like our Sun Stars, like our Sun Matter in plasma phase is high in energy, and is dangerous to living things Matter in plasma phase is high in energy, and is dangerous to living things

53. Plasma

54. Plasma

55. Energy Ability to change or move matter Ability to change or move matter

56. Phase Changes Melting Melting Freezing Freezing Vaporization Vaporization Condensation Condensation Sublimation Sublimation

57. Phase Changes are Physical Changes

58. Melting The change from solid to liquid The change from solid to liquid

59. Freezing Liquid To Solid Liquid To Solid When a liquid loses heat energy When a liquid loses heat energy

60. Liquid to Gas Vaporization Vaporization  change from a liquid to a gas Evaporation Evaporation  Vaporization at the surface of a liquid

61. Boiling Process by which particles inside the liquid travel into the air. Process by which particles inside the liquid travel into the air.

62. Condensation The change of a substance from a gas or vapor to a liquid The change of a substance from a gas or vapor to a liquid

63. Sublimation To change phase (from a solid or gas) without becoming a liquid To change phase (from a solid or gas) without becoming a liquid

64. Vaporization To be converted from a liquid into vapor/gas To be converted from a liquid into vapor/gas

65. Evaporation Vaporization that occurs at the surface of a liquid Vaporization that occurs at the surface of a liquid

66. Changes of State Graph For Water

67. Conservation of Mass

68. Law of Conservation of Mass Mass cannot be created Mass cannot be created or destroyed or destroyed

69. Law of Conservation of Energy Energy cannot be created or destroyed Energy cannot be created or destroyed

70. Matter Properties of Matter Section 2.3

71. Chemical Properties describes the way a substance reacts with others to change into a different substance describes the way a substance reacts with others to change into a different substance

72. Chemical Changes

73. Reactivity the ability of a substance to combine chemically with another substance the ability of a substance to combine chemically with another substance

74. Physical Properties characteristics that can be observed or measured characteristics that can be observed or measured without changing the identity of the object. without changing the identity of the object.  Shape, color, odor, texture…

75. Melting Point Temperature at which a solid changes to a liquid. Temperature at which a solid changes to a liquid. Aluminum M.P. = 660 °C Aluminum M.P. = 660 °C 0 0 C for water at sea level 0 0 C for water at sea level

76. Freezing Point Temperature at which a liquid changes to a solid Temperature at which a liquid changes to a solid Water F.P. = 0 °C at sea level Water F.P. = 0 °C at sea level

77. Boiling Point Temperature a liquid boils at. Temperature a liquid boils at. B.P. of a liquid is related to pressure above it. B.P. of a liquid is related to pressure above it. Water BP = 100 °C Water BP = 100 °C Table Salt BP = 1413 °C Table Salt BP = 1413 °C Diamond BP = 4200 °C Diamond BP = 4200 °C

78. General Properties of Matter include Mass Mass Weight Weight Volume Volume and density and density

79. Density Density is the mass per unit volume Density is the mass per unit volume

80. Density density = mass / volume density = mass / volume  Or DMV Units Units  Mass – g  Volume – cm 3  Density – g/ cm 3

81. Problem If 96.5 grams of gold has a volume of 5 cubic centimeters, what is its density? If 96.5 grams of gold has a volume of 5 cubic centimeters, what is its density?

82. Solution Step 1 Write the formula d=m/v Step 1 Write the formula d=m/v Step 2 Substitute given numbers and units d = 96.5 g/ 5 cm 3 Step 2 Substitute given numbers and units d = 96.5 g/ 5 cm 3 Step 3 Solve for unknown variable d= 19.3 g / cm 3 Step 3 Solve for unknown variable d= 19.3 g / cm 3

83. Practice Problems 1. If 96.5 grams of aluminum has a volume of 35 cm 3, what is the density of aluminum? 1. If 96.5 grams of aluminum has a volume of 35 cm 3, what is the density of aluminum? 2. If the density of a diamond is 3.5 g / cm 3, what would the mass be if the volume is 0.5 cm 3 ? 2. If the density of a diamond is 3.5 g / cm 3, what would the mass be if the volume is 0.5 cm 3 ?

84. Solution Step 1 d=m/v Step 1 d=m/v Step 2 rearrange d. v= m Step 2 rearrange d. v= m Step 3 Substitute given numbers and units 3.5 g/cm 3..5cm 3 = m Step 3 Substitute given numbers and units 3.5 g/cm 3..5cm 3 = m Step 4 Solve for unknown variable m= 1.75 g Step 4 Solve for unknown variable m= 1.75 g

85. Buoyancy The force with which a more dense fluid pushes a less dense substance upward. The force with which a more dense fluid pushes a less dense substance upward.

86. Archimedes’ Principle The buoyant force on an object is equal to the weight of the fluid displaced by the object. The buoyant force on an object is equal to the weight of the fluid displaced by the object. Therefore if an object increases it’s density it will sink, and if decreases it’s density it will float. Therefore if an object increases it’s density it will sink, and if decreases it’s density it will float.

87. Density Lab Does it Float?

88. The density of water is 1 gram per milliliter, 1g/mL. The density of water is 1 gram per milliliter, 1g/mL. If the object’s density is greater than 1g/mL, then the object will sink. If the object’s density is greater than 1g/mL, then the object will sink. If the object’s density is less than 1g/mL then it will float. If the object’s density is less than 1g/mL then it will float.

89. Does it Float? In this activity you will measure the mass and volume of several objects to obtain their densities. In this activity you will measure the mass and volume of several objects to obtain their densities. density = mass / volume density = mass / volume Volume of cube=length x width x height Volume of cube=length x width x height Volume of cylinder=  r 2 h Volume of cylinder=  r 2 h   =3.14

90. Remember 1 cubic centimeter = 1 mL

91. Volume of Cylinder Volume =  r 2 h Volume =  r 2 h

92. Volume of a Cube Volume= L x W x H Volume= L x W x H

93. Lab Report Format Descrip tion Mas s (g) Volu me (mL) Densi ty (g/m L) Does it float ?

95. Quiz What kind of solid is in the picture? What kind of solid is in the picture?

96. Quiz What kind of matter phase is in the picture? What kind of matter phase is in the picture?

97. Name the Phase

101. Gas – Pressure, Temperature and Volume Boyle’s Law – if volume is reduced, pressure will increase. P 1 V 1 = P 2 V 2 or P 1 /P 2 = V 2 /V 1 Boyle’s Law – if volume is reduced, pressure will increase. P 1 V 1 = P 2 V 2 or P 1 /P 2 = V 2 /V 1 Charles’s Law – if temperature of a gas changes but pressure is the same, then volume of the gas changes. T 1 V 2 =T 2 V 1 or T 1 /T 2 =V 1 /V 2 Charles’s Law – if temperature of a gas changes but pressure is the same, then volume of the gas changes. T 1 V 2 =T 2 V 1 or T 1 /T 2 =V 1 /V 2