1. Chapter 3: Matter and Energy Classification of Matter Properties of Matter Temperature Energy Specific Heat

2. Chapter 3 - Slide 2 of 48 Matter Is the material that makes up all things. Has mass and occupies space. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

3. Chapter 3 - Slide 3 of 48 Matter Anything that has mass and takes up space. Matter Pure Substance Mixture

4. Chapter 3 - Slide 4 of 48 Classification of Matter Pure Substances: A form of matter that always has a definite and constant composition. Properties always the same under a given set of conditions (temperature & pressure)

5. Chapter 3 - Slide 5 of 48 A pure substance is classified as An element when composed of one type of atom. A compound when composed of two or more different elements combined in a definite ratio. Pure Substances

6. Chapter 3 - Slide 6 of 48 Pure Substances: Elements Element –Pure substance that can not be broken down into simpler substances by chemical means. Copper (Cu) Lead (Pb) Aluminum (Al) –The most basic form of matter. –Each element can be found on the periodic table.

7. Chapter 3 - Slide 7 of 48 Pure Substances: Compounds Compounds –A chemical combination of 2 or more different elements. –A pure substance that can be broken down into simpler substances by chemical means. Salt (NaCl) Table sugar (C 12 H 22 O 11 ) Water (H 2 O) Carbon monoxide (CO) NOTE: CO is different from the element Co

8. Chapter 3 - Slide 8 of 48 Elements in a Compound “Table salt” is a compound that contains the elements sodium and chlorine. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

9. Chapter 3 - Slide 9 of 48 Pure Substances Elements and Compounds Elements and compounds have definite compositions, and each has a set of properties that are unique. Which pairs of symbols / formulas represent elements and compounds respectively? (A) (B) (C) (D) (E) P-1

10. Chapter 3 - Slide 10 of 48 Mixtures A mixture is a type of matter that consists of Two or more substances that are physically mixed, not chemically combined. A physical combination of two or more pure substances in which each substance retains its own chemical identity. Two or more substances in different (variable) proportions. Substances that can be separated by physical methods.

11. Chapter 3 - Slide 11 of 48 Mixtures Example of a mixture: Pasta and water can be separated by using a strainer. Uses a physical method to separate the components. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

12. Chapter 3 - Slide 12 of 48 Homogeneous Mixtures In a homogeneous mixture, The composition is uniform throughout. The different components of the mixture are not visible or discernable, one from the other. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

13. Chapter 3 - Slide 13 of 48 Heterogeneous Mixtures In a heterogeneous mixture, The composition of substances is not uniform. The composition varies from one part of the mixture to another. The different parts of the mixture are visible. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

14. Chapter 3 - Slide 14 of 48 Classification of Matter Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

15. Chapter 3 - Slide 15 of 48 Elements v. Compounds v. Mixtures Identify the following as an

16. Chapter 3 - Slide 16 of 48 Matter Has characteristics called physical and chemical properties.

17. Chapter 3 - Slide 17 of 48 Physical Properties Physical properties are: Characteristics observed or measured without changing the identity of a substance. Shape, physical state, odor, boiling and freezing points (Changes of state), density, and color of that substance.

18. Chapter 3 - Slide 18 of 48 Physical Properties of Copper Copper has the following physical properties: Reddish-orange Very shiny Excellent conductor of heat and electricity Solid at 25  C Melting point 1083  C Boiling point 2567  C Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

19. Chapter 3 - Slide 19 of 48 A physical change occurs in a substance if there is A change in the state. A change in the physical shape. No change in the identity and composition of the substance. Physical Change

20. Chapter 3 - Slide 20 of 48 States of Matter The states of matter are Solid Definite volume and shape Liquid Definite volume, but take the shape of its container Gas No definite volume or shape Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

21. Chapter 3 - Slide 21 of 48 Examples of States of Matter Solids Rocks, shells, baseballs, tennis racquets, books Liquids Lakes, rain, melted gold, mercury in a thermometer Gases Air, helium in a balloon, neon in a neon tube

22. Chapter 3 - Slide 22 of 48 Examples of Changes of State Some changes of state for water: Solid water (ice) melts and forms liquid water. Liquid water boils and forms gaseous water (steam). Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

23. Chapter 3 - Slide 23 of 48 Examples of Physical Changes Examples of physical changes: Paper torn into little pieces (change of size) Copper hammered into thin sheets (change of shape) Water poured into a glass (change of shape ) Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

24. Chapter 3 - Slide 24 of 48 Chemical Properties Chemical properties describe the ability of a substance To interact with other substances To change into a new substance Example: Iron has the ability to form rust when exposed to oxygen. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

25. Chapter 3 - Slide 25 of 48 Chemical Change In a chemical change, a new substance forms that has A new composition New chemical properties New physical properties Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

26. Chapter 3 - Slide 26 of 48 Some Chemical Changes Silver tarnishes Shiny metal reacts to form black, grainy coating. Wood burns A piece of wood burns with a bright flame to form ash, carbon dioxide, water vapor, and heat. Iron rusts A shiny nail combines with oxygen to form orange-red rust.

27. Chapter 3 - Slide 27 of 48 Classify each of the following changes as physical or chemical A.Burning a candle. B. Ice melting on the street. C. Toasting a marshmallow. D. Cutting a pizza. E. Iron rusting in an old car. Learning Check

28. Chapter 3 - Slide 28 of 48 Temperature Is a measure of how hot or cold an object is compared to another object. Indicates that heat flows from the object with a higher temperature to the object with a lower temperature. Is measured using a thermometer. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

29. Chapter 3 - Slide 29 of 48 Temperature Scales Temperature scales Are Fahrenheit, Celsius, and Kelvin. Have reference points for the boiling and freezing points of water. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

30. Chapter 3 - Slide 30 of 48 Learning Check P-2

31. Chapter 3 - Slide 31 of 48 On the Fahrenheit scale, there are 180°F between the freezing and boiling points and on the Celsius scale, there are 100°C. 180°F = 9°F =1.8°F 100°C 5°C 1°C In the formula for calculating the Fahrenheit temperature, adding 32 adjusts the zero point of water from 0°C to 32°F. T F = 9/5 T C + 32  orT F = 1.8 T C + 32  Fahrenheit Formula

32. Chapter 3 - Slide 32 of 48 Solving for °F Temperature A person with hypothermia has a body temperature of 34.8°C. What is that temperature in °F? T F = 1.8 T C + 32  T F = 1.8 (34.8°C) + 32° exact tenth's exact = 62.6 + 32° = 94.6°F tenth’s Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

33. Chapter 3 - Slide 33 of 48 T C is obtained by rearranging the equation for T F. T F = 1.8T C + 32 Subtract 32 from both sides. T F - 32 = 1.8T C ( +32 - 32) T F - 32 = 1.8T C Divide by 1.8 =°F - 32 = 1.8 T C 1.8 1.8 (T F - 32 )= T C 1.8 Celsius Formula

34. Chapter 3 - Slide 34 of 48 The normal temperature of a chickadee is 105.8°F. What is that temperature on the Celsius scale? 1) 73.8 °C 2) 58.8 °C 3) 41.0 °C Learning Check HW

35. Chapter 3 - Slide 35 of 48 A pepperoni pizza is baked at 455°F. What temperature is needed on the Celsius scale? 1) 423°C 2) 235°C 3) 221°C Learning Check HW

36. Chapter 3 - Slide 36 of 48 On a cold winter day, the temperature is –15°C. What is that temperature in °F? 1) 19 °F 2) 59°F 3) 5°F Learning Check HW

37. Chapter 3 - Slide 37 of 48 The kelvin temperature Has 100 units between freezing and boiling points. 100 K = 100°Cor 1 K = 1 °C Adds 273 to the Celsius temperature. T K = T C + 273 0 K (absolute zero) is the lowest possible temperature. 0 K = –273 °C Kelvin Temperature Scale

38. Chapter 3 - Slide 38 of 48 Temperatures Table 3.6 Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

39. Chapter 3 - Slide 39 of 48 Learning Check

40. Chapter 3 - Slide 40 of 48 Energy Makes objects move. Makes things stop. Is needed to “do work ”. Energy

41. Chapter 3 - Slide 41 of 48 Work Work is done when You climb. You lift a bag of groceries. You ride a bicycle. You breathe. Your heart pumps blood. Water goes over a dam. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

42. Chapter 3 - Slide 42 of 48 Potential Energy Potential energy is energy stored for use at a later time. Examples are Water behind a dam. A compressed spring. Chemical bonds in gasoline, coal, or food. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

43. Chapter 3 - Slide 43 of 48 Kinetic Energy Kinetic energy is the energy of matter in motion. Examples are Swimming. Water flowing over a dam. Working out. Burning gasoline. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

44. Chapter 3 - Slide 44 of 48 Learning Check Identify the energy as potential or kinetic. 1. Roller blading. 2. A peanut butter and jelly sandwich. 3. Mowing the lawn. 4. Gasoline in the gas tank.

45. Chapter 3 - Slide 45 of 48 Forms of Energy Energy can take many forms. Heat (thermal) Mechanical (movement) Light Electrical Chemical Nuclear

46. Chapter 3 - Slide 46 of 48 Changes in Forms of Energy Energy can change from one form to another. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

47. Chapter 3 - Slide 47 of 48 Heat is measured in joules or calories. 4.184 Joules (J) = 1 calorie (cal) Exact by definition 1 kJ = 1000 J 1 kilocalorie (kcal) = 1000 calories (cal) Units for Measuring Energy or Heat

48. Chapter 3 - Slide 48 of 48 Examples of Energy In Joules Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings