1. Matter

3. 1.3 An apparently empty test tube is submerged, mouth downward in water. Only a small volume of water rises into the tube, which is actually filled with invisible matter –air.

4. Physical States of Matter

6. A solid can be either crystalline or amorphous . Which one it is depends on the internal arrangement of the particles that constitute the solid. Solid Amorphous Solid Crystalline Solid Particles lack a regular internal arrangement Particles exist in regular, repeating three-dimensional geometric patterns . Glass, plastics, gels Diamond, metals, salts

14. Classifying Matter

15. Matter refers to all of the materials that make up the universe.

19. Homogeneous Heterogeneous

23. Example Sugar and fine white sand. The amount of sugar relative to sand can be varied. The sugar and sand each retain their own properties. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases.

25. liquid phase Heterogeneous Mixture solid phase 2 solid phase 1

26. Mixture of iron and sulfur Compound of iron and sulfur Formula Has no definite formula: consists of Fe and S. FeS Composition Contains Fe and S in any proportion by mass. 63.5% Fe and 36.5% S by mass. Separation Fe and S can be separated by physical means. Fe and S can be separated only by chemical change.

28. 1.6 Classification of matter: A pure substance is always homogeneous in composition, whereas a mixture always contains two or more substances and may be either homogeneous or heterogeneous.

29. Elements

30. An element is a fundamental or elementary substance that cannot be broken down into simpler substances by chemical means.

34. Compounds

35. A compound is a distinct substance that contains two or more elements combined in a definite proportion by weight.

37. There are two types of compounds: molecular and ionic .

38. Metals, Nonmetals and Metalloids

39. Metals

42. Examples of Metals gold iron lead

45. Nonmetals

47. Solid Physical State at Room Temperature sulfur selenium phosphorous carbon iodine

48. liquid Physical State at Room Temperature bromine

49. gas Physical State at Room Temperature helium, neon, argon, krypton, xenon, radon nitrogen, oxygen fluorine, chlorine

50. Metalloids

51. Metalloids have properties that are intermediate between metals and nonmetals

53. Metals are found to the left of the metalloids Nonmetals are found to the right of the metalloids.

54. Properties of Substances

56. Physical Properties

59. Chemical Properties

63. Physical Changes

65. Chemical Changes

66. In a chemical change new substances are formed that have different properties and composition from the original material.

67. Heating a copper wire in a Bunsen burner causes the copper to lose its original appearance and become a black material. Formation of Copper(II) Oxide Heating a copper wire in a Bunsen burner causes the copper to lose its original appearance and become a black material. The black material is a new substance called copper(II) oxide. Copper is 100% copper by mass. Copper (II) oxide is: 79.94% copper by mass 20.1% oxygen by mass. The formation of copper(II) oxide from copper and oxygen is a chemical change. The copper (II) oxide is a new substance with properties that are different from copper.

68. Formation of Copper(II) Oxide Copper(II) oxide is made up of Cu 2+ and O 2- 4.2 Neither Cu nor O 2 contains Cu 2+ or O 2- A chemical change has occurred.

69. Water is decomposed into hydrogen and oxygen by passing electricity through it. Decomposition of Water The composition and physical appearance of hydrogen and oxygen are different from water. The hydrogen explodes with a pop upon the addition of a burning splint. The oxygen causes the flame of a burning splint to intensify. They are both colorless gases. But the burning splint is extinguished when placed into the water sample.

70. Chemical Equations

71. Water decomposes into hydrogen and oxygen when electrolyzed. reactant products yields

72. Chemical symbols can be used to express chemical reactions

73. Water decomposes into hydrogen and oxygen when electrolyzed. reactant yields 2H 2 O 2H 2 O 2 products

74. Copper plus oxygen yields copper(II) oxide. yield product reactants heat

75. Copper plus oxygen yields copper(II) oxide. heat yield product reactants 2Cu O 2 2Cu 2 O

77. Conservation of Mass

78. No change is observed in the total mass of the substances involved in a chemical change.

79. sodium + sulfur  sodium sulfide 78.1 g 78.1 g product mass products 78.1 g reactant -> 46.0 g 32.1 g mass reactants =

80. Energy

81. Energy is the capacity to do work

83. Potential Energy Energy that an object possesses due to its relative position.

84. The potential energy of the ball increases with increasing height. increasing potential energy 50 ft 20 ft increasing potential energy

85. Potential Energy Stored energy

87. Kinetic Energy Energy matter possesses due to its motion.

92. Heat

94. Units of Heat Energy

96. An Example of the Difference Between Heat and Temperature A form of energy associated with small particles of matter. A measure of the intensity of heat, or of how hot or cold a system is.

97. Twice as much heat energy is required to raise the temperature of 200 g of water 10 o C as compared to 100 g of water. 200 g water 20 o C A 100 g water 20 o C B heat beakers temperature rises 10 o C 100 g water 30 o C 200 g water 30 o C 4184 J 8368 J

98. Conservation of Energy

100. 4.3 H 2 + O 2 have higher potential energy than H 2 O Electrolysis of Water Burning of Hydrogen in Air energy is given off energy is absorbed higher potential energy lower potential energy

101. Law of Conservation of Energy Energy can be neither created nor destroyed, though it can be transformed from one form of energy to another form of energy.