1. Introduction to Matter Matter? Does it Matter? What’s the Matter?

2. Essential Question   How are particles in solids, liquids, and gases arranged and how does that affect their properties?

3. So, What is Matter ?  Matter is defined as anything that has Mass Mass Takes up space (volume) Takes up space (volume)

4. Physical Property  Any quality or condition of a substance that can be observed or measured without changing the substances identity. Examples: color, solubility, odor, hardness, melting point, and state of matter

5. Physical States of Matter There’s 4 of them !  SOLIDS Have definite (or fixed) shape and volume Have definite (or fixed) shape and volume The particles in a solid are held fairly rigidly in place. The particles in a solid are held fairly rigidly in place.

6. Physical States of Matter There’s 4 of them !  LIQUIDS Have a definite volume but no fixed shape. Have a definite volume but no fixed shape. The particles in a liquid are free to flow around each other The particles in a liquid are free to flow around each other

7. Physical States of Matter There’s 4 of them !  GASES Have neither definite or fixed shape or volume. Have neither definite or fixed shape or volume. The particles in a gas are: widely disbursed, The particles in a gas are: widely disbursed, interact weakly, interact weakly, move independently at high speed, move independently at high speed, and completely fill any container they occupy. and completely fill any container they occupy.

8. 4 th Type of Matter PLASMA Gases whose particles are so hot they have acquired an electrical charge. Gases whose particles are so hot they have acquired an electrical charge.

9. Changes of State

10. Physical Changes in Matter  change in a substance that doesn’t change the identity of the substance  Ex. grinding, cutting, melting, boiling  Includes all changes of state (physical changes of a substance from one state to another)

11. Chemical Property  Ability of a substance to combine with or change into one or more other substances Examples: Rusting, flammability, reactivity, etc.

12. Chemical Changes in Matter  a change in which a substance IS converted into a different substance  same as chemical reaction  doesn’t change the amount of matter present  reactants – substances that react  products – substances that form

13. Signs of Chemical Change  Energy is always absorbed or given off  Change in color or odor  Production of a gas (bubbling)  Irreversibility

14. Chemical or Physical?  Cookies are baked  Water boils  Salt dissolves in water  Milk spoils  A metal chair rusts  Paper is torn  A tree burns down Chemical Physical Chemical Physical Chemical

15. Law of Conservation of Mass  In any physical change or chemical reaction, mass is neither created nor destroyed; it is conserved.

16. Law of Conservation of Mass Total mass of substances before reaction = Total mass of substance after reaction From the law of conservation of mass: Can you find the amount of oxygen that reacts? Mercury + oxygen red-orange residue 2.53g2.73g 0.20 g

18. Intensive vs. Extensive Properties

19. CLASSIFICATION OF MATTER

20. EQ’s EQ’s   How is matter classified?

21. A. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes ColloidsSuspensions

22. Pure Substances  Every sample has same: characteristic properties characteristic properties composition composition  Are made of: 1 type of atom: element 1 type of atom: element Ex: iron, gold, arsenicEx: iron, gold, arsenic 2 or more types of atoms: compound (molecules too) 2 or more types of atoms: compound (molecules too) Ex: salt, sugar, water, ammonia (NH 3 )Ex: salt, sugar, water, ammonia (NH 3 )

23. Which are pure substances?

24. Mixtures  Blend (mix) of 2 or more types of matter  Each component keeps its own identity and properties  The components are only physically mixed  Can be separated using physical means  Properties of the mixture are a combination of the componenent’s properties

25. Homogeneous Mixtures  Also called solution  Uniform in composition  No visible parts Ex:  vinegar  clear air  salt water  brass

26. Mixtures

27. Heterogeneous Mixtures  Not uniform in composition  Visible parts Ex:  soil  concrete  blood  chocolate chip cookies  sand in water  iced tea with ice

28. Practice Determine whether each of the following is element, compound, homogeneous mixture or heterogeneous mixture.  air  zinc  chlorine  granite  aluminum  sugar in water  blood  sucrose  stainless steel  sodium chloride  brass  whole milk  apple  table salt  soft drinks  vinegar  concrete  sodium  baking soda (NaHCO 3 )  gravel Homogeneous Heterogeneous Element Heterogeneous Element Homogeneous Element Compound Homogeneous Compound Homogeneous Heterogeneous Compound Homogeneous Heterogeneous Element Compound Heterogenous

29. Substance or Mixture?  A homogeneous mixture looks like a substance  Is the material in question always a single kind of material? For instance, there are different grades of gasoline and different kinds of cough syrup  Is the material in question physically separable?

30. Separation Techniques of Mixtures

31. EQ’s  What are five physical separation techniques that can be used with mixtures?

32. Physical Separation Techniques  Filtration- solid part is trapped by filter paper and the liquid part runs through the paper  Vaporization- where the liquid portion is evaporated off to leave solid

33. Physical Separation Techniques  Decanting- when liquid is poured off after solid has settled to bottom  Centrifuge- machine that spins a sample very quickly so that components with different densities will separate

34. Physical Separation Techniques  Paper Chromatography- used to separate mixtures because different parts move quicker on paper than other

35. Classify the following as a substance or a mixture  Silver  Alphabet soup  Salt water  Table salt (sodium chloride)  Motor oil

37.  How do you separate different substances from a mixture? You have just been given the latest creation of your science teacher. The teacher presents you with a mixture of sawdust, iron filings, salt, and sand. He needs to separate the mixture and wants your help. You are to separate the mixture and find the total mass of each of the substances in the mixture!  You are to describe your proposed separation plan. Present your plan to your teacher for approval.  You will then conduct the experiment and separate the mixture  Upon completion of the experiment each member of the group will submit a final paper

38. Data Table MaterialOriginal Mass (g) Recovered Mass (g) Percent Error Salt Sand Iron Filings Sawdust

39. Possible Errors  Too much water to evaporate  Wet wood chips when finding the mass after separation  Using a beaker instead of a graduated cylinder when finding the volume of water  Forgetting to zero out scale before massing  Massing the cup and not subtracting  Water did not dry out from sand  Substances lost in the “transport” from lab table to scale

40. The Final Paper Must Include the Following: *Introduction: Define the mixture and properties of the ingredients in this mixture *Materials: List of ALL lab equipment used *Procedures: Numbered step by step procedures that you performed to separate the mixture

41. The Final Paper Must Include the Following: *Results: Mass of each substance before and after separation (data table) *Conclusion: A description of problems you encountered while conducting the lab and percent error calculations for each substance Ideas as to how you could improve your methods to better separate each ingredient and reduce your percent error. Ideas as to how you could improve your methods to better separate each ingredient and reduce your percent error.