1. Matter takes up space. All matter is made up of 4 general properties: Mass, Weight, Volume and Density.

2. Properties of matter http://studyjams.scholastic.com/studyjams/ja ms/science/matter/properties-of- matter.htmhttp://studyjams.scholastic.com/st udyjams/jams/science/matter/properties-of- matter.htmhttp://studyjams.scholastic.com/st udyjams/jams/science/matter/properties-of- matter.htm

3. GENERAL PROPERTIES SPECIFIC Properties Masscolor Weighttexture Volumeshape Density Size Odor Hardness malleable, ductile

4. mass-amount of matter in an object. Weight-measure of the pull of gravity on an object. Volume-amount of space an object or liquid takes up. Density-mass per unit volume; D=M/V

5. Units for mass, weight, volume and density Mass: Kg Weight: newtons Volume: L for a liquid ; cm ³ for a solid Density: g/mL, Kg /KL-liquids g/ cm ³, Kg/ m ³ -solids

7. Weight is different from mass To understand this, you must first understand gravity… Gravity is a force of attraction between objects that is due to their masses ☺ This attraction causes objects to exert a pull on other objects Because all matter has mass, all matter experiences gravity

8. The amount of gravitational attraction between objects depends on two things: 1.The masses of the objects 2. The distance between them

9. Gravitational force is smaller between objects with smaller masses that are close together vs. larger masses close together Smaller vs. larger masses close together How Mass & Distance Affect Gravity Between Objects

10. An increase in distance reduces gravitational force between two objects Gravitational force is smaller when further away vs. closer together

11. Weight is a measure of gravitational force exerted on an object ☺ For example: The brick vs. the sponge Larger mass; Larger force; Larger weight Smaller mass; Smaller force; Lower weight

12. Liquid Volume Measured in liters Use a graduated cylinder The curve that you see at the liquid’s surface has a special name meniscus ☺

13. Solid Volumes Measured in cubic units, such as cm 3 or m 3 Cubic means “having three dimensions”—L X W X H 1 mL = 1 cm 3 = 1 g For rectangular or square objects: Volume = Length x width x height Height Length Width

14. Measuring an irregular solid( object ) Graduated cylinder or over flow can, and convert displaced water in mL to cm3

15. Water displacement worksheet Do the water displacement worksheet and correct

16. ANSWERS TO WATER DISPLACEMENT 1. 9 cm³ 2. 5 cm³ 3. 4 cm³ 4..4 cm³ 5. 3.5 cm³ 6. 1 cm³ 7. 1.8 cm³ 8. 7 cm³ 9. 4 cm³ 10. 15 cm³ 11. 3 cm³ 12. 9.5 cm³ 13. 8.5 cm³ 14. 3 cm³ 15. 3 cm³ 16..7 cm³ 17. 8.5 cm³ 18. 1 cm³ 19. 1.1 cm³ 20. 7 cm³ 21. 10 cm³ 22. 14 cm³ 23. 5 cm³ 24. 6 cm³

17. Volume lab

18. Measuring the Volume of Gases How do you measure the volume of a gas? You cannot: hold a ruler up to a gas So it’s impossible….right? Think again ! Gas molecules move:________________ A gas expands to fill its container, so … –I–If you know the volume of the container the gas is in –T–Then you know the volume of the gas

19. density Density is the relationship between mass and volume. It is a proportion. Mass and volume need to be calculated. Formula: D = m/v http://teachertube.com/viewVideo.php?video _id=93322http://teachertube.com/viewVideo. php?video_id=93322http://teachertube.com/viewVideo. php?video_id=93322

20. DENSITY PROBLEMS 1.A coke can has a volume of 355 mL. Its mass is 50 g. What is its density? 2.Titanium has a density of 4.5 g/cubic cm. Mass of a titanium Cube is 4500 g. What is its volume? 3.What is the density of a cork that has a mass of 0.24 g and a volume of 2.0 cubic cm? D = 4. What is the mass of an ice cube that has a volume of 8.0 cubic cm? ( density of ice is 0.92 g/cubic cm ) Mass =

21. Answers to problems : D =.14 g/mL V = 1000 cubic cm³ D =.12 cm³ M = 7.4 g

22. Density worksheet 1 and 2 Answers to ws. # 1: 1..2 g/cm³ 2. 1 g/mL 3. 12.72 g 4.11.4 g/cm³ lead 5.3.7 g/cm³ aluminum 6.1.9 g/cm³ bone 7..68 g/cm³ gasoline

23. Density worksheet # 2 answers: 1. 2.54 g/cm³ 2. 4.67 g/cm³ 3. 6.11 g/cm³ 4. 0.639 g/cm³ 5. 0.168 g/cm³ 6. 2.52 g/cm³ 7. 0.281 g/cm³ 8. 4.88 g/cm³ 9. 1.32 g/cm³ 10. 7.55 g/cm³ 11. 3.36 g/cm³ 12. a) 1.398 g/ mL; b) no. Water’s density is 1 g/mL 13. 4.046 or 4.05 g/cm³

24. Part 2 – phases of matter

25. What is not matter? Light, Sound,Electricity. They are all forms of energy. Phases of matter ( or States ) What is steam? Invisible gas. The water boils at 212 degrees, and it cannot get hotter. So,the additional energy condenses it to water droplets, or vapor. To change water into a solid? Freeze it. To change ice into water? Melt it.

26. Two Pieces of matter cannot occupy the same space at the same time. There are 4 States or Phases of Matter. They are :Solid, liquid, gas and Plasma.

27. Short video http://www.brainpop.com/science/matterand chemistry/statesofmatter/http://www.brainp op.com/science/matterandchemistry/statesof matter/http://www.brainp op.com/science/matterandchemistry/statesof matter/

29. 1 1 Image Bank Solid Particles

31. Glass of Liquid

32. Liquid Particles

33. Gas Particles

34. Definite Shape Definite Volume Solid Yes Yes Liquid No Yes Gas No No Plasma No No

35. Theory of Moving Particles (Kinetic-Molecular Theory) States of Matter Particle Distance Particle Speed Solid No Space between particles Part. vibrate in place Liquid Particles slide Particles moving around OVER EACH OTHER quicker than solid. Gas Particles are far apart Particles moving very fast Plasma Widely Separated particles Fastest moving particles

36. http://phet.colorado.edu/en/simulation/states-of-matterphet.colorado.edu/en/simulation/states-of-matter

38. Bill nye video and worksheet

39. Solids—have a variety of shapes. Crystalline solids—definite repeating pattern and shape. ex: salt, sugar, sand, snow Amorphous solids–a solid that can flow under certain conditions. Acts like a liquid, and loses its shape. ex: wax, tar, rubber, glass Liquids - -----flow differently—some flow quickly, some slowly. Viscosity—resistance of liquid to flow. Honey, ketchup,,lava.

40. Physical Property- the characteristics of a substance that can be measured or observed. ex. GP, SP Physical Change- affects the physical properties of the substance (same substance)

41. Temperature and Phase Changes Temperature— A measure of how fast/slow the molecules are moving in a phase of matter. When Temp. rises, heat is being added. When it goes down, heat is being taken away. Phase Change: A physical change where heat energy is added or taken away to change form. It is STILL the same substance.

42. 5 Phase Changes—Physical Properties Energy is what causes particles to move. Adding or taking away heat energy is what causes matter change phase. These are physical changes. The matter changes from 1 form to another, but the substance is still the same.

43. http://www.miamisci.org/af/sln/p hases/watersolid.htmlhttp://www.miamisci.org/af/sln/phases/wat ersolid.htmlhttp://www.miamisci.org/af/sln/phases/wat ersolid.html HAND OUT: INTERNET LAB ON PHASE CHANGES

45. Air Pressure in Volleyball

47. Frozen pond

48. Freezing—Change of a liquid to a solid. (loss of heat energy). The freezing point of a substance is = to its melting point. Water to ice Melting---- Change of a solid to a liquid. (gain of heat energy). The melting point of a substance is = to its freezing point. Ex: ice to water Condensation—When a gas changes to a liquid. ( loss of heat energy) ex: steam to water Vaporization—Change from a liquid to a gas. (gain of heat energy)—Evaporation-at surface of liquid. Ex: water to steam Sublimation---When a solid goes directly to a gas, and skips the liquid state. (gain of heat energy) ex: dry ice, snow. Ex: snow, dry ice, glaciers Deposition: when gas goes to solid, skipping liquid state.

49. Solid CO2 Not crystal like Not brittle White Below freezing Sublimes - 75 degrees C Solid H2O molecules Crystal like Brittle Clear ( usually ) Freezing pt of water Melts 0 degrees C Dry ice water ice In common

50. DRAW endothermic exothermic endothermic exothermic

51. Endothermic ---gain ( absorption ) of heat energy Exothermic -- loss ( release ) of heat energy

52. And heat energy !! Add in

53. Ck this out: substa:Melting pt/freezing pt condensationpt/vaporization pt. A 14degrees C 120 degrees C B 75 degrees C 85 degrees C C - 45 degrees C 15 degrees C 1.Which is a solid at 65 degrees C? 2.What phase is B at 90 degrees C? 3. Which substance, A, B or C is a liquid at 60 degrees C?

54. ANSWERS: 1.B IS A SOLID AT 65 DEGREES 2.B IS A GAS AT 90 DEGREES 3.A IS A LIQUID AT 60 DEGREES

55. Recap of phase changes OR, changes of state http://studyjams.scholastic.com/studyjams/ja ms/science/matter/solids-liquids- gases.htmhttp://studyjams.scholastic.com/stu dyjams/jams/science/matter/solids-liquids- gases.htmhttp://studyjams.scholastic.com/stu dyjams/jams/science/matter/solids-liquids- gases.htm

58. November 26, 2012 Is something New created?

59. http://studyjams.scholastic.com/studyjams/jams/science/matt er/changes-of-matter.htm PART 3: chemical changes of matter

60. c hemical change – the process by which a new substance is created. Ex: brownie mix cooks—becomes brownies. c hemical reaction– same as a chemical change involves chemically combining substances, to produce a new substance. chemical Property– describes how a substance changes into a new substance Ex: paper has the ability to burn and create ash.

61. SIGNS OF CHEMICAL REACTIONS: Is it rusting ? Ex: Is it tarnishing?( reaction to oxygen in air) Ex: is it Flammable ? Ex: hairspray ability to burn( oxygen supports burning, but carbon dioxide does not!) -- is it burning ? Ex: wood on fire -- is it giving off a gas? Ex: alka seltzer and water Is it fizzing? Ex: alka seltzer and water Is it changing color? Ex: leaves changing color Is it Bubbling? Ex: alka seltzer and water

63. Recap of chemical and physical Properties and changes Chem prop. Chem changes phys.Prop phys changes

64. brain pop -property changes – use worksheet http://www.brainpop.com/science /matterandchemistry/propertycha nges/ http://www.brainpop.com/science /matterandchemistry/propertycha nges/

65. Gas Laws--- only work with a sealed ( fixed ) amount of gas. Volume, temp. and pressure Boyle’s Law— Inverse Relationship between Volume and Pressure on a fixed amount of gas. Volume increases as Pressure decreases. P 1 V 1 = P 2 V 2 Charles’s Law--- Volume varies directly with the temperature of the gas with a fixed amount of gas. Volume increases as Temperature increases. V 1 V 2 ------ = ------ T 1 T 2

66. BOYLE’S GAS LAW

67. Volume Decreases-Pressure Increases

68. CHARLES’S GAS LAW

69. Pressure and Temperature

70. Gas law formulas: Boyles : P 1 V 1 =P 2 V 2 Charles’s: V 1 V 2 ------ = ------ T 1 T 2

71. LET’S DO GAS LAW PROBLEMS!