1. Matter Chapter 3

2. I. Properties of Matter A. Physical B. Chemical C. Phases II. Changes of Matter A. Physical B. Chemical C. Law of Conservation III.Classifying Matter A. Pure Substance B. Mixtures IV.Overview of the Periodic Table A. Metals B. Non Metals C. Metalliods D. Noble Gases

3. I.Properties A. Physical Property that can be observed or measured without altering identity of matter Property that can be observed or measured without altering identity of matter examples: blue, soft, 78˚C, smelly, 10L examples: blue, soft, 78˚C, smelly, 10L 1. Intensive – does not change with amount 2. Extensive – changes with amount

4. Examples: Examples:lengthcolormassvolumedensityphaseconductivitytexture I.Properties A. Physical

5. I.Properties B. Chemical Describes ability of substance to change into another substance Describes ability of substance to change into another substance Examples: rust, burn, bubbles, precipitate Examples: rust, burn, bubbles, precipitate

6. I.Properties C. Phases A physical property A physical property 1. Solid – particles very close together particles vibrate in a fixed position

7. 2. Liquid – particles are intermediate in distance particles glide past each other I.Properties C. Phases

8. 3. Gas – particles are far apart particles are separated from eachother particles move quickly I.Properties C. Phases STOP

9. Clip 1: Physical Changes Clip 1: Physical Changes II.Changes A. Physical

10. Changes which do not result in a new substance Changes which do not result in a new substance Ice  water Ice  water Start with H 2 O, end with H 2 O Start with H 2 O, end with H 2 O Examples: all phase changes, rip, cut Examples: all phase changes, rip, cut

11. II.Changes A. Physical

12. Solid Liquid Gas Melt Vaporize (boil or evaporate) Condense Freeze

13. Clip 2 – Chemical changes in matter Clip 2 – Chemical changes in matter II.Changes B. Chemical

14. Changes that result in a new substance Changes that result in a new substance a.k.a chemical reaction a.k.a chemical reaction 1. Word equation: hydrogen + oxygen  water reactants product copper + silver nitrate  silver + copper nitrate II.Changes B. Chemical

15. 2. Formula Equation Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag AgNO 3 + KCrO  KNO 3 + AgCrO II.Changes B. Chemical (be able to identify reactants and products)

16. 3. Indications of chemical changes: –New substances form –Color change (sometimes) –Odor results –Release of light and heat light and heatlight and heat –Release of gas bubbles –Formation of a precipitate (solid that forms when two liquids are mixed) KI and Pb(NO 3 ) 2 II.Changes B. Chemical

17. II.Changes C. Law of Conservation of Mass Mass is neither created nor destroyed during a chemical or physical change Mass is neither created nor destroyed during a chemical or physical change Mass Reactants = Mass Products All chemical reactions follow the Law of Cons. of Mass….that’s why we balance them All chemical reactions follow the Law of Cons. of Mass….that’s why we balance them

18. 20g of lithium reacts with chlorine to form 244g of lithium chloride. How much chlorine reacted? 20g of lithium reacts with chlorine to form 244g of lithium chloride. How much chlorine reacted? Write a word equation: Write a word equation: lithium + chlorine  lithium chloride 20g+x=244g x =224g 224g of chlorine reacted II.Changes C. Law of Conservation of Mass

19. A 2.4g sample of X reacts with 12.8g of Y to form X 2 Y. What mass of product forms? A 2.4g sample of X reacts with 12.8g of Y to form X 2 Y. What mass of product forms? X+Y  X 2 Y 2.4g+12.8g =x X = 15.2g II.Changes C. Law of Conservation of Mass

20. III. Classification of Matter Matter Pure Substance ElementCompound Mixtures HomogeneousHeterogeneous Combine to form

21. Composition is always the same, whatever the source…never varies Composition is always the same, whatever the source…never varies 1. Element – –Simplest form of matter –Made up of identical atoms –All listed on PTOE (92 natural) –Au, Na, O 2, S 8 are all elements –Cannot be broken down III.Classification of Matter A. Pure Substance

23. 2. Compounds –Combination of more than one type of element joined by bonds (CO 2, NaCl) –Components separated by chemical rxn –Represented with a chemical formula  Letters indicate type of element  Subscripts tell how many III.Classification of Matter A. Pure Substance

24. CaCO 3 1 calcium atom 3 oxygen atoms 1 carbon atom Chemical Formulas: 5 atoms total

25. 1. Molecule – combination of more that one atom held by covalent bonds (all elements in a molecule are nonmetals) O 2 is a molecule of the oxygen element O 3 is a molecule of the oxygen element CO 2 is a molecule and a compound NaCl is NOT a molecule but a compound III.Classification of Matter A. Pure Substance

26. Clip: elements and compounds Clip: elements and compounds

27. –Law of Definite Composition (1779) by Joseph L. Proust –In any compound, the elements are present in a fixed proportion by weight.

28. –According to the Law of Definite Composition (aka Definite Proportions): –Water, by mass, is always 11.2% hydrogen and 88.8% oxygen no matter what the source is. Water = H 2 O Mass of hydrogen = 1.01 Mass of oxygen = 16.00

29. % hydrogen = mass of hydrogen mass of water mass of water =(2) (1.01) x 100% 18.02 18.02 = 11.2%

30. –Given CH 4 (methane), determine the percent composition % C = 12.01 x 100 16.06 16.06 = 74.8% = 74.8%

31. III.Classifying Matter B. Mixtures Combination of two or more pure substances Combination of two or more pure substances Composition of mixtures varies from source to source Composition of mixtures varies from source to source Components can be separated by physical means (magnet, filter, distillation) Components can be separated by physical means (magnet, filter, distillation)distillation No chemical formula No chemical formula List of ‘ingredients’ List of ‘ingredients’

32. 1. Homogenous Mixtures –Uniform composition throughout one sample –Also known as solutions –Solutions can be solid, liquid or gas –Aqueous solutions have water as solvent III.Classifying Matter B. Mixtures

34. Sometimes you need additional information

35. 2. Heterogenous Mixture –Composition varies within one sample III.Classifying Matter B. Mixtures

36. Aluminum Aluminum Paper Paper Gold Gold Orange juice Orange juice Fruit on the bottom yogurt Fruit on the bottom yogurt Iced tea Iced tea Diamond Diamond Buckminsterfullerene Buckminsterfullerene Air Air Octane (C 8 H 18 ) Octane (C 8 H 18 ) Glucose Glucose Oil and water Oil and water Hand lotion Hand lotion

37. IV. The Periodic Table of Elements 18 columns (group or family) containing elements with similar properties 18 columns (group or family) containing elements with similar properties 7 rows (periods) containing elements with same number of electron shells 7 rows (periods) containing elements with same number of electron shells I abbreviate it…PTOE I abbreviate it…PTOE

39. IV.PTOE A. Metals 1. Types –Alkali earth metals (group 1) –Alkaline earth metals (group 2) –Transition metals (group 3-12) –Lanthanides (bottom period 6) –Actinides (bottom period 7) –Others (some in groups 13-16)

42. 2. Properties –Luster –Conductors of heat and electricity –Solids (except Hg) –Malleable –Ductile –Tensile strength IV.PTOE A. Metals

43. Properties Properties –Vary according to metalloid –All are semi-conductors –B, Si, Ge, As, Sb, Te, Po IV.PTOE B. Metalloids

46. Properties Properties –Poor conductors –Brittle –Solids: C, P, S, Se, I, At –Liquid: Br –Gases: N, O, F, Cl IV.PTOE C. Non Metals

49. Properties Properties –All are gases –Stable, do not react naturally IV.PTOE D. Noble gases