MATTER the stuff of the universe

1. MATTER the stuff of the universe

2. Matter • Matter: ______________________________ _____________________________________ • Mass: the amount of ____________________ • Weight: ______________________________ • on Earth, this is the same as mass • Law of Conservation of Matter: “__________ ________________________________”…but it can be rearranged (via chemical or physical reactions)

3. Atoms Matter is composed of _________ • Atoms: ___________________________ _________________________________ _________________________________ • can not be further divided and still have _________ ___________ • Are composed of _________, ___________, and ___________

4. Pure Substance • A substance with • Ex:___________________ _______________________ • __________ and ______________are both considered to be pure substances

5. Solid Liquid Gas States of Matter

6. Condensed States: Solids • Solids • Have a ___________________ __________________________ • Molecules are • Tightly ________ • Moving _________________________ ____________________ • ________________attracted to each other • Not _________________

7. Condensed States: Liquids • Liquids • Have NO set__________but definite __________ • Molecules are • ____________than in a solid at the same temperature • _________________________ • _________ attracted to each other • Not _______________

8. Expanded States: Gas • Gas (vapor) • Have no ________________ • Depends on the container • Have ________________ • Varies depending on _______________ and ___________ • Molecules are • ______________________attracted to each other • ________________than those in a liquid at the same temperature • As a result are • _________________as far as possible • __________________past each other • _____________________

9. Expanded States: Plasma • Plasmas • Occur at extremely ____________________ • Are ________________ • May be some atoms or molecules but mostly • ________________ floating around not attached • Usually are __________________________ • Most ________________ form of matter in the universe • ______________ • Here on Earth: _______________________________ ___________________________________________

11. What is a non-Newtonian fluid? You have to pull the trigger on a water pistol to get the water to squirt out. To make the water to come out faster, you have to pull the trigger harder. Fluids resist flow. The resistance to flow arises because of the friction between these layers. This phenomenon is known as viscosity. Newton devised a simple model for fluid flow that could be used to relate how hard you have to pull the trigger to how fast the liquid will squirt out of the pistol. Picture a flowing liquid as a series of layers of liquid sliding past each other. The slower one layer slides over another, the less resistance there is, so that if there was no difference between the speeds the layers were moving, there would be no resistance. Fluids like water and gasoline behave according to Newton's model, and are called Newtonian fluids. But ketchup, blood, yogurt, gravy, pie fillings, mud, and cornstarch paste DON'T follow the model. They're non-Newtonian fluids because doubling the speed that the layers slide past each other does not double the resisting force. It may less than double (like ketchup), or it may more than double (as in the case of quicksand and gravy). That's why stirring gravy thickens it, and why struggling in quicksand will make it even harder to escape. For some fluids (like mud, or snow) you can push and get no flow at all- until you push hard enough, and the substance begins to flow like a normal liquid. This is what causes mudslides and avalanches.

12. Physical and Chemical Properties and Changes

13. Physical Property • Characteristic of a substance that can be observed ________________ ________________________________________________________________ • Examples: • ______________ • ______________ • ______________ • ______________ • ______________ • ______________

14. Chemical Property • Ability of a substance to _____________ _________________________________ • You must change the identity _________ __________________________________________________________________ • Examples: • ______________ • ______________ with acids and bases

15. Intrinsic v. Extrinsic Properties • Intrinsic (intensive) Property: A property that _______________ __________________________ of substance changes • _____________ • _____________ • _____________ • _____________

16. Intrinsic v. Extrinsic Properties • Extrinsic (extensive) property: A property that ___________________ ____________________________________________________________ • _____________ • _____________ • _____________ • _____________

17. Density…Intrinsic or Extrinsic? • Density data for a sample of gold. • Density= mass/ volume • Units are g/mL or g/cm3

18. Physical Change • Change in the _________________substance, not in its chemical nature • No chemical bonds ___________________________ • The chemical formula is the same before and after the change • ________________________________are made or broken, not the molecules themselves • Examples: • __________________ • __________________ • __________________ • __________________

19. Chemical Change (___________) • Change__________________________________________________________ • Atoms are __________________ • Bonds are ______________________ in new ways • Examples: • __________________ • __________________ • _______________ • __________________

20. Signs of Chemical Change • Change in: • ___________________ • Forming a _______________ (solid made from liquids) • ___________________________ • __________ • ________________ • _________ (exothermic) • _________ (endothermic) • _____________ • giving off ___________

21. What is an element? • Element: • A substance made up of only one type of atom is an _____________________

22. How do we represent elements? • Represented by symbols on the periodic table • Usually comes from the ___________, a _____________, or a _____________ • One or two letters for those with official names • ___________________________________ • ___________________________________ • Unofficially named elements have three letters, starting with a capital ____

23. Elements in Nature • ____90 naturally occurring • Of the __________on the Periodic Table, only ___ and ____ are not naturally occurring • Some elements are _________________ __________________, but commonly are found in compounds • ex: ______________is virtually non-existent in pure form, but is found in common_______, a compound we call table salt.

24. Elements

25. When elements were discovered

26. Allotropes • Allotropes are ___________________ __________________________ • Shown here are allotropes of carbon • ______________, ______________, and ______________ • Difference is how the atoms are __________________________

27. Molecules • Two (2) or more _______________ _____________________ • O2 • H2 • H2O • C6H12O6

28. Compounds • Two (2) or more ___________________ ________________________________ _________________________________ • Has own, unique: • ________ (law of__________________) • properties • ___________________________________ • Need a ___________________to separate them into the elements it is made from • 2 H2O -> 2H2 and O2

29. Law of Definite Proportions • In samples of any chemical compound, the ________________________________ _________________________________ • ________________________________ • H2O is always H2O, and never H2O2 • Once the formula is different, the materials and the properties are different

31. What is the difference between compounds and molecules? • The term molecule is more _________, compound is more _________. • Molecules can be _______________ like ___________ • Compounds by definition ________ _______________

32. Separation of compounds into their elements • Compounds can be broken into their elements by _______________, such as • ______________. This is the decomposition of a substance (here, water) into it’s elements by an ______________.

33. Mixture • A blend of 2 or more____________ • Have __________ compositions • No _____________________ • Examples:

34. Air: A Mixture

35. Types of Mixtures • Homogeneous • ________________ • __________________ • cannot see ________________ • Examples • ___________ • ___________ • ___________ • ___________

36. Types of mixture, con’t • Heterogeneous • ______________ • not __________________ • can see ______________ • Examples: • _________________ • _________________ • _________________ • _________________

37. Subtypes of mixtures... • Solutions: one thing dissolved in another; they do not ___________________or when filtered (particles are molecules) • Two parts: • Solvent-______________________________ • Solute- _______________________________ Ex: Salt water – water is the ________, salt the _______ • Can be any state of matter • Alloys are _____________________(a solid solution)

38. Subtypes of mixtures... • Suspensions: • Heterogeneous mixture of two or more substances • may look like a solution but can ____________________________ ____________________________ • particles are not dissolved • particles are larger than molecules; sometimes they can be seen by the naked eye

39. Subtypes of mixtures... • Colloid- microscopically mixed homogeneous solutions that will _______________ (____________) • They will ________________out upon standing • Emulsion- a type of colloid made from of two liquids that normally will not mix (are_________________________)

41. Tyndall Effect

42. Twenty-four-karat gold is an _____________ • Eighteen-karat gold is an ________. • Fourteen-karat gold is an ___________. • (Alloys are homogeneous mixtures- specifically solutions- of metals) • What is the solvent in 18K and 14K gold? • What is/ are the solute(s) in 18K and 14K gold?

43. Classification of Matter

44. Separating Mixtures • Mixtures can be separated by _________________________ • No chemical reactions or changes needed • 5 main methods are based on physical properties • _________________ • _________________ • _________________ • _________________ • _________________

45. Separating Mixtures • Evaporation: ____________________ ________________________________ • Crystallization: ___________________ __________________________________________________________ • Usually paired • _____________ • _____________ • _____________ • _____________

46. Chromatography: “color writing” • Using how ______________________to separate them • Use specific ratios of movement through a medium (paper, water, column) based on how some molecules move through the medium • Phases: • Stationary phase • _____________________(paper, the column) • ____________________of the mixture _________________ • Mobile phase • moves over the stationary phase • _________________________of the mixture • Rf values constant for component of a mixture • Ratio of ________________________________________ _______________________________________________ • Ex: running colors in ink when wet

47. chromatograms

48. Gas and Column Chromotography

49. Filtration • Use a funnel and ________ _____________ • Separates a __________________________ • Based on _____________

50. Distillation • Separates _______ ________________ • One liquid has to have a lower _____ ________________ • Heat both; the one with the lower BP is boiled out first • Can use _______________ to collect materials as they boil out • Used with crude oil (______________) to isolate separate products