1. M ATTER Physical and Chemical Properties of Matter

2. Vocabulary 1/21 – Matter 1/22 – volume 1/23 – plasma 1/26 – Bose- einstein condensate 1/28 – density 1/29 – Regular solid 1/30 – Irregular solid 2/2 – Archimedes principle I can ……. 1/21 – Explain the difference between ice and water. 1/22 – Explain the difference between mass and volume. 1/23 – Contrast a liquid and a solid 1/26 – Name the states of matter in order of increasing energy! 1/28 – Name the 2 types of properties 1/29 – Calculate the volume of a regular solid(unit?) 1/30 – Calculate the volume of an irregular solid. 2/2 – Calculate the density of an object

3. W HAT DO YOU O BSERVE IN THE PICTURE

4. W HAT IS M ATTER ? Anything that has mass and takes up space (volume). Examples of matter:

5. MATTER CANNOT BE CREATED OR DESTROYED IT JUST CHANGES FROM ONE FORM TO ANOTHER. () (MATTER GETS RECYCLED) LAW OF CONSERVATION OF MATTER

6. THEORY OF KINETIC ENERGY ATOMS ARE 1. ATOMS ARE ALWAYS MOVING THE MORE ENERGY TO THE ATOMS, THE & APART THEY MOVE 2. THE MORE ENERGY ADDED TO THE ATOMS, THE FASTER & FARTHER APART THEY MOVE ENERGY ADDED

7. M ATTER Matter can be described by using physical and chemical properties. These are characteristics the matter has that make it unique. Physical Properties: Are properties that can be observed or measured. (color, mass, length, volume, density, state, etc). Physical Properties can be either: Observable or Measurable

8. O BSERVABLE P HYSICAL P ROPERTIES Observable Physical Properties: Properties you can use your senses to get information about an object. If you can describe the matter based on what it looks, feels, smells or tastes like, you are describing the physical properties.

9. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES State of Matter: Matter can either be a solid, liquid, gas, or plasma. We observe this by using our senses.

10. STATES OF MATTER MATTER CAN BE FOUND IN 4 MATTER CAN BE FOUND IN 4 STATES (PHASES) SOLID SOLID LIQUID LIQUID GAS GAS PLASMA PLASMA State of matter is a physical property!!!! http://www.harcourtschool.com/activity/states_of_matter/

11. PARTICLES of a SOLID (Physical Property) Pattern: ATOMS (PARTICLES) ARE ARRANGED CLOSELY PACKED TOGETHER Movement: VIBRATE Shape/Volume: HAS FIXED SHAPE & FIXED VOLUME Examples – ice, rock, book

12. – THE OBJECT IS HARDER – THE MORE DIFFICULT IT IS TO BREAK THEM APART BREAK THEM APART – THE MORE ENERGY NEEDED TO CHANGE FROM A SOLID TO A CHANGE FROM A SOLID TO A LIQUID LIQUID In Solids, the particles are very tightly packed SO:

13. The particles in a LIQUID: Pattern: none Movement: atoms roll or slide over each other and move faster than a solid. Shape: No fixed shape, takes shape of container Volume: Fixed Examples: water, milk, soda

14. The particles in a GAS: Pattern: none Movement: PARTICLES MOVE VERY FAST & AS FAR APART AS THEY CAN GET Shape: NO FIXED SHAPE, takes shape of container Volume: No fixed volume Examples – oxygen, helium

15. W E ALL KNOW ABOUT : LIQUIDS SOLIDS GASES Higher Temperatur e Lower Temperatur e

16. Two states of matter they didn ’ t teach you about in school… Until Now!

17. P LASMA Bose-Einstein Condensate

18. But what happens if you raise the temperature to super-high levels… between 1000°C and 1,000,000,000°C ? Will everything just be a gas?

19. NO! If the gas is made up of particles which carry an electric charge ( “ ionized particles ” ), but the entire gas as a whole has no electric charge, and if the density is not too high, then we can get The 4 th state of matter: PLASMA

20. The particles in PLASMA: Pattern: none Movement: Particles move very fast and are therefore very HOT Shape/Volume: NO FIXED SHAPE OR VOLUME Facts : Most common state of matter in the universe. Most Uncommon state of matter on Earth. Found in lightning, fluorescent lights and stars (Sun)

22. Some places where plasmas are found… 1. Flames

23. 2. Lightning

24. 3. Aurora (Northern Lights)

25. 4. Neon lights

26. 5. Stars Stars make up 99% of the total matter in the Universe. Therefore, 99% of everything that exists in the entire Universe is in the plasma state.

27. The Sun is an example of a star in its plasma state

28. 6 6. Clouds of gas and dust around stars

29. S O NOW WE KNOW ALL ABOUT FOUR STATES OF MATTER : LIQUIDS SOLIDS GASES Higher Temperatur e Lower Temperatur e PLASMAS (only for low density ionized gases)

30. But now what happens if you lower the temperature way, way, down to 100 nano degrees above “Absolute Zero” (-273°C) Will everything just be a frozen solid?

31. N OT N ECESSARILY ! In 1924 (82 years ago), two scientists, Albert Einstein and Satyendra Bose predicted a 5 th state of matter which would occur at very very low temperatures. EinsteinBose +

32. The 5 th state of matter: Bose-Einstein Condensate Finally, in 1995 (only 11 years ago!), Wolfgang Ketterle and his team of graduate students (like me) discovered the 5 th state of matter for the first time. Ketterle and his students

33. I N A B OSE -E INSTEIN CONDENSATE, ATOMS CAN NO LONGER BOUNCE AROUND AS INDIVIDUALS. I NSTEAD THEY MUST ALL ACT IN EXACTLY THE SAME WAY, AND YOU CAN NO LONGER TELL THEM APART !

34. Here is a picture a computer took of Bose-Einstein Condensation The big peak happens when all the atoms act exactly the same way! (We can ’ t see Bose-Einstein condensation with our eyes because the atoms are too small)

35. Some other computer images of Bose-Einstein Condensates…

38. B OSE EINSTEIN CONDENSATES Pattern: ATOMS (PARTICLES) ARE ARRANGED IN A PATTERN Movement: NONE Shape/Volume: HAS FIXED SHAPE & FIXED VOLUME When temperatures get that low, you can create a BEC with a few special elements. Cornell and Weiman did it with rubidium (Rb).

39. The whole process happens at temperatures within a few billionths of a degree, so you won't see this at home. When the temperature becomes that low, the atomic parts can't move at all. They lose almost all of their energy. Since there is no more energy to transfer (as in solids or liquids), all of the atoms have exactly the same levels, like twins. The result of this clumping is the BEC. The group of rubidium atoms sits in the same place, creating a " super atom." There are no longer thousands of separate atoms. They all take on the same qualities and, for our purposes, become one blob.

40. E XAMPLES OF B OSE EINSTEIN CONDENSATES Two examples of Bose-Einstein condensates include superfluids, such as cold liquid helium, or superconductors, such as the nucleons inside a neutron star. Bose-Einstein condensates are another state of matter, similar to solids but with less energy. They were not directly observed until the 1990s, even though Einstein predicted their existence in the 1920s.

41. T O REALLY UNDERSTAND B OSE -E INSTEIN CONDENSATE YOU NEED TO KNOW Quantum Physics

42. In 2002, Ketterle and two other scientists received the highest award in science for discovering Bose-Einstein condensate: The Nobel Prize

43. T HE FIVE STATES OF MATTER : LIQUIDS SOLIDS GASES Higher Temperatur e Lower Temperatur e PLASMAS (only for low density ionized gases) BOSE- EINSTEIN CONDENSATE

44. OTHER OBSERVABLE PHYSICAL PROPERTIES

45. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Color: The color of object can be seen and is a physical property of matter. Color can help identify a substance. For example, sulfur is usually yellow in color, iodine is usually red in color. Sulfur Iodine

46. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Smell: The smell or odor an object gives off can also help identify a substance. For example, sulfur has a rotten egg smell, vinegar has a very acidic smell, and chlorine has a very strong bleach smell.

47. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Malleability: the ability of a substance to be pounded into thin sheets.

48. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Conduction of heat or electricity: The ability for heat and electricity to pass through an object easily. Metals are usually the best conductors of heat and electricity.

49. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Insulator of electricity or heat: when an object passes heat and electricity poorly. Nonmetals are usually good insulators.

50. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Ductility: the ability to be drawn or pulled into a wire. Metals usually are ductile.

51. E XAMPLES OF O BSERVABLE P HYSICAL P ROPERTIES Solubility: The ability to dissolve in a nother substance. Examples: sugar dissolves in water.

52. P HYSICAL P ROPERTIES - E XAMPLES Color Hardness Odor Taste State of matter Texture Luster (shine) Flexibility Heat conductivity Electrical conductivity Solubility (ability to dissolve in water.) Shape Viscosity Ductility Malleability

53. P HYSICAL P ROPERTIES - E XAMPLES Examples of physical properties include: Density Melting point Boiling point

54. P ROPERTIES OF M ATTER Matter can be described by using physical and chemical properties. These are characteristics the matter has that make it unique. Physical Properties: Are properties that can be observed or measured. (color, mass, length, volume, density, state, etc). NAME 2 OBJECTS!!!!!

55. M EASURABLE P ROPERTIES OF M ATTER Measurabe Properties: Properties that must be measured with a tool (ruler, beaker, graduated cylinder, scale, etc.). Ruler Graduated Cylinder Beaker Triple Beam Balance Scale

56. M EASURABLE P ROPERTIES OF M ATTER Mass: is the amount of atoms contained in a substance. Calculate: Using a triple beam balance or a scale. Unit: in science ALWAYS use grams (g) or kilograms (kg).

57. M EASURABLE P ROPERTIES OF M ATTER Weight: is the amount gravity is pulling on an object. Different on the MOON!!! Other wise it is measured the same as MASS!!

58. M EASURABLE P ROPERTIES OF M ATTER Volume : the amount of space an object takes up. Measured by : different for regular solid, irregular solid and liquids. Examples of Regular Solids : any solid you can measure the length, width and height of. Examples of Irregular Solids : any solid you cannot measure the length, width and height of. Examples of Liquids: any object that has no definite shape but does have a definite volume.

59. Measuring the Volume of Liquids: How to calculate: Use a graduate cylinder to find the volume at the meniscus. Material: graduated cylinder, beaker, flask How to read a graduated cylinder Must be at eye level to read. Must read to bottom of the curve Must read to bottom of the curve. MENISCUS - bottom of the curve. Unit: mL or L Measurable Properties of Matter

60. M EASURABLE P ROPERTIES OF M ATTER Measuring Volume of Regular Solids : measure the length, width and height with ruler and multiply them together. Length X Width X Height = Volume of Regular Solid cm X cm X cm = cm 3 *ALWAYS USE CENTIMETERS IN SCIENCE!!!! UNIT: cm 3

61. M EASURABLE P ROPERTIES OF M ATTER Measuring Volume of Irregular Solids: Water displacement. Put water into a graduated cylinder and record volume. Place irregular solid into cylinder with water and record second volume. Subtract the two amounts. Initial volume (water only) – volume with irregular solid = volume of solid UNIT: measured in mL but, since it is a solid use cm 3. 1 mL = 1 cm 3

62. M EASURABLE P ROPERTIES OF M ATTER Density: the amount of matter in a given space or volume. Density is used to describe matter because everything has a different density.

63. M EASURABLE P ROPERTIES OF M ATTER Measure by: dividing and objects mass by it’s volume. Calculate: Density = Mass/Volume m D = ------- V Mass divided by Volume UNIT: since mass is measured in grams and volume is measured in cm 3 or mL the unit for density has to have those two units. So, the unit for density is g/mL or g/cm 3. D m V

64. BELLRINGER Calculate the density for the following objects: a.Mass= 10 Volume= 5 b.Mass= 16 Volume= 8 c.Mass= 5 Volume= 10 d.Mass= 12 Volume= 12 Which object is water? Which object will float in water? Which objects will sink in water? 2g/ml sinker 2g/cm 3 sinker 0.5g/ml floater 1g/cm 3 water

65. W HICH IS GOLD ? H OW WOULD YOU KNOW ?

66. W HO WAS ARCHIMEDES ???? VIDEO!!!!!

67. Archimedes Principle – measuring density with water displacement The density of water is ALWAYS 1.0 g/mL. Anything less than 1.0 g/mL will FLOAT. Anything greater than 1.0 g/mL will sink.

68. These are two, unopened full cans of soda. Explain why one is floating and one has sunk.

69. Why are some objects less dense than other objects? As the molecules of a substance spread apart, the density of the substance is lowered. What causes molecules to spread? Adding energy so the movement of the molecules increases.

70. Objects float in other substances because they are less dense than the substance they are floating in. Why does ice float in water? They are both the same substance, right?

71. Notice how tightly packed the atoms are in the liquid water vs the solid water? The spaces between the atoms make solid water less dense. Is this true for all solids? NO WAY!!! This is a unique quality of water. Most solids are always more dense than their liquid forms.

72. Why does this happen? Hot air balloon rises Basketball goes flat in winter Perfume can be smelled all over the room Atmosphere changes as you climb a mountain

73. DENSITY When does an objects density change? If heat is added or taken away!!!! HEAT – spreads out molecules – LESS dense Take AWAY heat – molecules come together – MORE dense. Hot objects are less dense than cool objects!!!!

74. C HEMICAL P ROPERTIES OF M ATTER Chemical Properties- Properties that determine whether or not a substance will react chemically. Flammability: the ability to burn. Reactivity: The ability for a substance to react with another. Simply, when two substances get together, something can happen.

75. C HEMICAL PROPERTIES - E XAMPLES Examples of chemical properties include: The ability to burn Ability to tarnish Ability to rust Ability to decompose Ability to react with other chemicals Instability Ability to do acid/base reactions

76. C HEMICAL PROPERTIES List as many chemical properties as you can for this item.

77. Chemical and physical properties – So what? Titanium is very strong and doesn’t rust, so it is often used in jet engines. Titanium is also nonallergenic. This, combined with the fact that it is rust proof makes it great for artificial joints as well as piercings.

78. Chemical and physical properties – So what? Tungsten is usually used as the filament in lightbulbs because it has the highest melting point of any metal. It glows red hot when electricity runs through it, and it gives off both heat and light.

79. Chemical and physical properties – So what? Vanadium is heavier and harder than titanium, so mixing a tiny bit of vanadium with steel can make cheap tools that are still very strong.

80. Chemical and physical properties – So what? Helium is almost completely nonreactive (inert). It is lighter than air, so it’s great for floating balloons (or making funny voices.) When electricity runs through helium, it glows a creamy pale peach color.

81. Chemical and physical properties – So what? In 1943, all US pennies were made of zinc plated steel because copper was being used in the war. The pennies had to be coated with zinc because steel will rust, but zinc won’t.

82. Chemical and physical properties – So what? Sulfur smells awful. Rotten eggs, onions, and garlic all have sulfur in them. Stink bombs use sulfur to create a bad smell. Sulfur is also flammable, and it is one of the 3 main ingredients in gun powder.

83. Chemical and physical properties – So what? Chromium is famous for its intense luster. Chrome plated tools, jewlery, silverware, or car parts are very popular.

84. Chemical and physical properties – So what? Most bullets are made of lead because lead is a very dense metal. These bullets are required, by international law, to be coated with a different metal because lead has such a low melting point and is so malleable.

85. Chemical and physical properties – So what? The most dense elements are Iridium and osmium which have a density of about 22.6 g/cm3

86. Physical and Chemical Changes 7 th Grade Science

87. Physical Changes Matter is always changing form, size, shape, color, etc. There are 2 types of changes that matter undergoes. PHYSICAL OR CHEMICAL CHANGE I. Physical Changes: a change of matter without changing the identity of the substance. IN OTHER WORDS A CHANGE IN STATE A CHANGE IN SIZE, SHAPE, MASS DOES NOT CHANGE THE CHEMICAL MAKE UP OF THE MATTER YOU HAVE WHAT YOU STARTED WITH, JUST IN A DIFFERENT FORM

88. Examples of Physical Changes - Verbs used to describe physical changes – grind, dissolve, erode, rip, tear, break, phase change (melt, freeze, condense, etc)

89. Other Physical Change Examples PAPER TORN INTO PIECES SUGAR DISSOLVED INTO TEA SALT DISSOLVED INTO WATER NAILS OR HAIR CUT

90. Chemical Changes The other way that matter can be changed is call a CHEMICAL CHANGE. II. CHEMICAL CHANGE – occurs when 2 or more substances are combined into entirely new substance with all new properties. CANNOT CHANGE IT BACK!!!!!

91. Chemical Change Verbs Chemical Change Verbs: rusting, rotting, curdling, burning, cooking, light sensitivity, digesting, tarnishing.

92. Kinetic Theory of Matter THEORY OF KINETIC ENERGY A. ATOMS ARE ALWAYS MOVING B. THE MORE ENERGY ADDED TO THE ATOMS, THE FASTER & FARTHER APART THEY MOVE

93. WHEN MOLECULES MOVE FASTER, THEY PRODUCE MORE FRICTION AND THEREFORE MORE HEAT. THEY SPREAD FARTHER APART & EXPAND WHEN MOLECULES MOVE SLOWER, THEY CAUSE LESS FRICTION AND THEREFORE LESS HEAT & CLOSER TOGETHER & CONTRACT

94. MATTER CHANGES FROM ONE STATE OF MATTER TO ANOTHER WHEN HEAT (ENERGY) IS ADDED WHEN HEAT (ENERGY IS TAKEN AWAY

95. CHANGING STATES DOES NOT CHANGE THE CHEMICAL MAKE UP OF THE MATTER YOU HAVE WHAT YOU STARTED WITH JUST IN A DIFFERENT FORM ICE  WATER  WATER VAPOR H 2 O H 2 O H 2 O

96. Phase Changes are PHYSICAL PHYSICAL!!!!! Types of Phase Changes: 1. Melting 2. Freezing 3. Evaporation 4. Boiling 5. Condensation 6. Sublimation 7. Deposition ALL phase changes are caused by ADDING or TAKING away energy!!!

97. Melting 1. MELTING – matter changing FROM A SOLID TO A LIQUID. Energy is added When more heat (energy) is added to matter the particles move faster till the bonds break. Decrease density except ice to water.

98. Evaporation/Vaporization 2. EVAPORATION Matter changing FROM A LIQUID TO A GAS AT THE SURFACE ENERGY IS ADDED TO SURFACE OF LIQUID THE PARTICLES AT THE SURFACE MOVE FASTER breaking bonds. Decreases density. VAPORIZATION- a general term for any substance changing to a gas.

99. Boiling 3. BOILING matter changing FROM A LIQUID TO A GAS ALL THROUGHOUT THE LIQUID ENERGY IS ADDED TO ALL OF LIQUID PARTICLES MOVE FASTER ALL THROUGH THE LIQUID SOME PARTICLES MOVE FAST ENOUGH TO CHANGE TO GAS WHILE THEY ARE IN THE MIDDLE OF THE LIQUID DENSITY DESCREASES Water boils at 212 F, 100C. EX: pan of liquid on the stove VAPORIZATION- a general term for any substance changing to a gas.

100. VAPORIZATION!!! Remember that vaporization is a general word for any substance changing to a gas. Boiling, evaporation, and sublimation are ALL examples of vaporization!!!

101. Condensation 4. CONDENSATION Matter CHANGING FROM A GAS TO A LIQUID ENERGY IS REMOVED THE PARTICLES MOVE SLOWER THE ATTRACTION BETWEEN THE PARTICLES BEGAN TO PULL THE PARTICLES CLOSER TOGETHER & THE MATTER TURNS INTO A LIQUID DENSTITY INCREASES Ex: dew in the lawn, water running down mirror, ring on table under glass.

102. Freezing 5) FREEZING CHANGING FROM A LIQUID TO A SOLID CHANGING FROM A LIQUID TO A SOLID ENERGY IS REMOVED ENERGY IS REMOVED THE PARTICLES MOVE EVEN SLOWER THE ATTRACTION BETWEEN THE PARTICLES BEGAN TO PULL THE PARTICLES CLOSER TOGETHER & THE MATTER TURNS INTO A SOLID Increase density. Water freezes at 32 F, 0 C EX: water to ice, wax or chocolate hardening

103. SOLIDIFICATION!!!! Solidification is a general word for any substance changing to a solid. Freezing and deposition are examples of SOLIDIFICATION!

104. Sublimation 6) Sublimation: matter changes straight from a solid to a gas!!!! Heat added rapidly Molecules speed up and spread out rapidly decrease density Examples of Sublimation: dry ice, shrinking ice in a freezer, air freshener.

105. Deposition 7) Deposition- when matter changes from a gas directly to a solid. -Heat is taken away rapidly - Density increases -Molecules slow down and get closer together. Examples: Snowflakes, frost on a wind shield

106. WHAT HAS TO HAPPEN FOR THESE CHANGES OF STATES TO OCCUR?

108. DRAW THIS DIAGRAM IN YOUR NOTES!!!!

109. Let’s Sing!!!! Phase changes are physical, physical… Melting is physical…. Freezing is physical. BOYS: Let me see some condensation. GIRLS: (in high pitch voice) It’s physical. BOYS: Let me see some sublimation. GIRLS: (in high pitch voice) It’s physical. Phase changes are physical, physical… Boiling is physical… BOYS: Let me see some deposition. GIRLS: (in high pitch voice) It’s physical BOYS: Let me see some evaporation. GIRLS: (in high pitch voice) It’s physical

110. Chemical Changes The other way that matter can be changed is call a CHEMICAL CHANGE. II. CHEMICAL CHANGE – occurs when 2 or more substances are combined into entirely new substance with all new properties. CANNOT CHANGE IT BACK!!!!!

111. Chemical Change Verbs Chemical Change Verbs: rusting, rotting, curdling, burning, cooking, light sensitivity, digesting, tarnishing.

112. Chemical Changes SOME SIGNS OF A CHEMICAL CHANGE FIZZES OR BUBBLES COLOR CHANGE HEAT GIVEN OFF LIGHT GIVEN OFF ODOR HEAT REQUIRED FOR REACTION NEW SUBSTANCE FORMED Precipitate (solid) Precipitate (gas bubbles)

113. CHEMICAL CHANGE EXAMPLES BAKING BREAD – NO LONGER HAVE FLOUR, EGGS, MILK, YEAST ALKASELTER BAKING SODA & VINEGAR RUST TARNISH