Are these things matter?

1. Are these things matter? • Your book, your desk, your lunch, the air that you breathe and the water you drink? • How do you know?

2. Matter is anything that has mass and volume.1. Mass is the amount of matter an object has.2.Volumeis the amount of space an object takes up. • Question: Will an inflated balloon weigh more, less, or the same as the same balloon deflated? • Make a hypothesis, then test it. • Obtain the mass of a balloon, then inflate it, and then obtain the new mass.

4. Homogeneous Mixture (Solution) uniform(same) throughout in composition Examples: coffee air (mixture of gases) Alloys like: brass (Cu & Zn) steel (Fe & C) Heterogeneous Mixture not uniform (different)throughout in composition Examples: sand in water tea with ice cubes oil in water chicken noodle soup Mixtures:contain more than one type of matter and are physically combined. What are some mixtures found in your kitchen?

5. Homogeneous When you don’t see the gas bubbles. Heterogeneous When you see the gas bubbles. What is soda?Heterogenous or Homogeneous? But if asked, say homogeneous!

6. Separation of Mixtures Mixtures can be separated by physical means. a) Filtration b) Centrifuge c) Chromatography d) Distillation e) Crystallization Separate sand and salt?

7. Compounds made from more than one kind of atom A molecule is the smallest particle of a compound that retains its properties. Compoundscannotbe separated by physical means! (only by chemical reactions) Ex: salt, distilled water, sugar Elements made of only one kind of atom. Anatomis the smallest part of an element). Ex: Pure Substances:contain only one typeof matter.

8. Separation of Compounds Compoundscan be separated chemical means. Examples: a) Electrolysis of water water  hydrogen gas and oxygen gas b) Chemical Reactions Magnesium + Acid  hydrogen gas Mg + HCl (acid)  MgCl2 + H2 So the properties of compounds may be similar or different than the properties of their elements!

9. Classify MatterElement, Compound, Homogenous mixture, or Heterogeneous mixture Homogeneous mixture Element (molecule) Compound Homogeneous mixture Heterogeneous mixture

10. Classify each of the following as either: (E) – Element (HomM) – Homogeneous Mixture (C) – Compound (HetM) – Heterogeneous Mixture E Complete the classification chart now. Skip the classification cards diagram below for now. You will do it later. Its due at end of class HetM E HomM

11. Starter • Classify the following compounds • Finish the yellow homework (exit ticket)

12. Chemical properties: characteristics of a substance’s “ability”to change into a different substance. Gasoline is combustible and flammable Properties of MatterProperty – a characteristic • Physical properties: • characteristics that can be observed or measured without changing the identity of the substance. • Gasoline has a distinct odor, it is colorless, and a liquid at room temperature.

13. Physical Properties Hardness- resistance to scratching. More examples luster – shine Solubility – ability to dissolve in water Elasticity– ability to be stretched or bounce Which would you rather play “basketball” with? A) bowling ball B) volleyball

14. Physical Properties More examples Brittleness –tendency to shatter Malleability –be pounded into thin sheets. Ductility– be drawn into thin wire. Tensile Strength – the tension it can withstand before breaking.

15. Physical Properties More examples Phase Change –change to and from solids, liquids and gasses. Viscosity –the resistance to flow Magnetism– attracted by a magnet. Color – the current color. Odor – the Smell.

16. Chemical Properties More examples CombustibilitY & Flammability – capable of catching fire and burning. pH– measure of acidity. reactivity – ability to react to form a new substance.

17. combustibility flammability reactivity pH (acidity) Ex: Silver will tarnish because of reactivity How many properties did you come up with? Chemical Physical density hardness luster solubility elasticity brittleness malleability ductility tensile strength Electrical conductivity melting point boiling point freezing point viscosity magnetism odor color solid liquid gas

18. Chemical Changes: A change that does produce a new substance. Usually not reversible. Ex: Iron rusts forming iron oxide. Changes of Matter • Physical Changes: • A change that does notproduce a new substance. • Usually reversible. • Ex: Ice melts into water.

19. How do you know a chemical change has occurred? Evidence of a Chemical Change: • Energy (Heat): • absorbed energy (endothermic) • released energy (exothermic) • Gas is produced (bubbles) • Solid (precipitate) forms • Odor or colorchange occurs New substances are formed

20. Physical Plant loses water through evaporation Toothpick is broken Sugar dissolves Ice cube melts Food coloring Copper wire is cut Chemical Energy  ATP Match burns Bike rusts Gasoline burns Silver tarnishes Leaves change color Food is digested Acid + Base  Salt Physical & Chemical Changes

21. Why are these chemical changes?

22. Tea Party Properties • In an envelope provided by the teacher are • Physical and Chemical Properties (Orange Cards) • Physical and Chemical Changes (Blue or White Cards) • Organize the orange cards into two piles: Physical and Chemical Properties.

23. Identify the following as a physical property, a chemical property, a physical change, or a chemical change. Physical change Chemical change Physical property Physical property Chemical property Physical change Chemical property Chemical change Do Worksheets

24. Starter • Quiz today Pick up white and green handout. Pick up returned HW. • What are each of these? HomM, HetM, Compound or Element? What are each of these? ChemC, PhysC, ChemP or PhysP? • aluminum is malleable __________ • ability of sodium to react with chlorine__________ • leaf turning red __________ • a pond freezes over__________ • iron rusting __________ • paper being torn __________ • TNT is explosive __________ • acetone is volatile (vaporizes easily)__________

25. Video: States of Matter Oobleck PLASMA MythBusters

26. States of Matter Plasma – “charged gas”.

27. Plasma • Plasma is a gas containing charged particles such as electrons and ions. • It is the most common state of matter in the universe.

28. Changes of State Solid Liquid Gas Molecular Motion Increases

29. What is meant by “change of state”?

30. Change of State:a physical change between states of matter. • Temperature influences changes of state. • As temperature increases, the internal energy increases. • S L  G (Boiling) Temperature Click Here and run applet

31. The Phase Change Graph L & G Temp is constant • Phase changes require a gain or loss of Energy. • During a phase change, the temperature does NOT change. • When can two states coexist? During a phase change. S & L Temp is constant

32. Solid: Substance with a definite shape and volume • Liquid: Substance with a definite volume but not a definite shape • Gas: Substance with no definite volume or shape • Plasma: Substance that is extremely high in energy and is rare on earth but common in stars

33. Phase changes in matter are: • Melting: change from a solid to a liquid • Freezing: change from a liquid to a solid • Vaporization: the change from liquid to gas • Evaporization: vaporization from the surface of a liquid. • Boiling: vaporization from within as well as from the surface of a liquid • Condensation: change from a gas to a liquid • Sublimation: change from a solid to a gas • Deposition: change from gas to solid

34. Real World Experiences! • How does it feel when you put rubbing alcohol on your skin? Why? • What happens to “dry ice” when left on the counter? Why? • What happens to “moth balls” left in storage trunks? Your skin feels cold because when alcohol evaporates, it absorbs heat energy from your skin. “Dry ice” (solid carbon dioxide) does not disappear, but it sublimes into a gas. “Moth balls” (solid napthalene) do not disappear, but it sublimes into a gas. The fumes kill the moths.

35. Starter Pick up green handout. Pick up homework and grades back tables. Turn in white notes from last class and green demo lab pick up a calculator 1. In which of these materials do particles have the slowest motion and MOST ordered arrangement? • a gas such as nitrogen C. a solid compound such as baking soda • a liquid such as salt water D. a mixture such as coke a cola 2. How can scientists separate elements in compounds and in mixtures? • By heating them to their gaseous state. • By chemical reactions that recombine or rearrange atoms • They separate elements in compounds by chemical reactions, and elements in mixtures by physical processes. • They separate elements in compounds by physical reactions and elements in mixtures by physical processes. 3. At a Halloween party students observe dry ice at room temperature. The solid sublimes directly to the gas state. This sublimation is accompanied by which change in the carbon dioxide? • decrease in volume C. increase in mass • decrease in particle number D. increase in particle motion

37. Matter is anything that has mass and volume.1. Mass is the amount of matter an object has.2.Volumeis the amount of space an object takes up. • Question: Will an inflated balloon weigh more, less, or the same as the same balloon deflated? • Make a hypothesis, then test it. • Obtain the mass of a balloon, then inflate it, and then obtain the new mass.

38. Amount of matter Use a balance Kg Doesn’t change with location Pull of gravity Use a scale Newton Does change with location Mass vs. Weight

39. Which has more mass?A) 1 kilogram of feathersB) 1 kilogram of bricks They are the same! 1 kg = 1 kg

40. Which takes up more space?A) 1 kilogram of feathersB) 1 kilogram of bricks The Feathers

41. Measure matter by finding the density! Which has the greater density?A) steel bar B) steel paper clip The density of steel is the same! Size doesn’t matter!

42. Density of Steel steel bar

43. Units for Density Metric Units: Solid: g/cm3 Liquid: g/mL Density of water is 1g/mL (at 4º C) Memorize This!

44. Which one floats? Why? • Density of Water: 1.00 g/mL • Density of Ice: 0.92 g/mL Ice! Because it is less dense.

45. Which of the following will float on water?Why is it good to know the density? Density helps you identify a substance All those less than 1.0 g/mL

46. Predict the correct “floating order” of the substances as they would appear in the “Density Column”.

47. Make your own density column • Get out your density column handout. • Get some colored pencils, scissors and glue sticks • Color and arrange your density columns with the least dense on top and most dense on bottom • You have 15 minutes

48. Calculating Density • Obtain mass using a balance. • Obtain volume by any of these methods. • Ruler: Volume = L x W x H • Graduated cylinder • Water displacement d = m/vm = d x vv = m/d m “Magic Circles” d v

49. Is the bar really gold or fool’s gold?Find the density of the bar if the mass is 1891.4 g and the dimensions are 3.5 cm by 3.5 cm by 8.0 cm. • Gold has a density of 19.3 g/cm3 V = L x W x H D = M/V 1891.4 g / 98 cm3 = 19.3 g/cm3 Yes it’s gold! m d v

50. Is this liquid water, alcohol, or kerosene? Find the density of the liquid if the mass is 16.98 g? Water 1.0 g/mLAlcohol 0.79 g/mLKerosene 0.82 g/mL • Read the volume  D = M/V 16.98 g / 21.5 mL = 0.79 g/mL It is alcohol! m d v