1. Matter and Change Mrs. McGuire Chemistry

2. Classification of Matter Some Criteria for the Classification of Matter ______________ _________(solid, liquid, gas) _______________

3. Properties Intensive -Do not depend on amount of matter. Ex: __________, ________________, ____________ Extensive -Depend on amount of matter. Ex: ________, ______________, ______________

4. Intensive and Extensive Properties Sulfur

5. Properties Physical: observed _________ ______________of the substance. Chemical: the ability of a substance to _______________ ___________________________

6. Examples of Physical Properties

7. SubstanceStateColor Melting Point (C°) Boiling Point (C°) Density (g/cm 3 ) OxygenO2O2 GasColorless-218-1830.0014 MercuryHgLiquidSilvery- white -3935713.5 BromineBr 2 LiquidRed-brown-7593.12 WaterH2OH2OLiquidColorless01001.00 Sodium Chloride NaClSolidWhite80114132.17 Example: Physical Properties

8. States of Matter Solid __________________________ __________________________ Liquid _________________________ __________________________ Gas _________________________

10. STATES of matter

11. Bromine Gas (Vapor) Liquid

12. Change of Phase Condensationgas  liquid Freezingliquid  solid Deposition gas  solid Meltingsolid  liquid Evaporationliquid  gas Sublimationsolid  gas Boiling: Evaporation occurring beneath the liquid’s surface.

13. Chemical Properties and Chemical Changes Is changing phase a physical or chemical change? ___________________Explain:

14. H 2 O composition is fixed- compound Gaseous PhaseLiquid Phase

15. Chemical Properties The ability of a ____________ _______________________(to undergo a chemical change). Example: Magnesium ______ with oxygen to form magnesium oxide.

16. Magnesium Mg

17. Burning of Magnesium 2Mg+ O 2  2MgO

18. Physical Changes Physical change: a _________ in the ___________________of a substance. Composition does not change. May be reversible or irreversible. Examples: Reversible: Irreversible:

19. Chemical Change A change that produces matter with a different composition than the original matter. Atoms rearrange themselves into new combinations.

20. Burning of Methane CH 4 +2O 2  CO 2 + 2H 2 O

21. Burning of Methane __________________________

22. Recognizing a Chemical Change _________ exchange production of a ______ _______ change*** formation of a ____________

23. Formation of a Precipitate Cu(OH) 2 Precipitate

24. The Law of Conservation of Mass (Antoine Lavoisier) In any chemical or physical change, ________________ _______________________ Mass is CONSTANT

25. Classification of Matter (by composition)

26. (Pure) Substance Matter that has a uniform and definite composition. Elements: _________________ _________________________ Compounds: _______________ ___________________________

27. c) Elements and Compounds Pure substances Elements can NOT be decomposed by chemical means, but compounds can.

28. Elements The ___________substances. ________________into simpler substances. Building blocks of all matter. More than 100 known elements. Represented by ___________symbols.

29. Chemical Symbols of Elements System started by Jons Berzelius (Sweden, 1779-1848) One or two first letters of name of the element. Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

30. Examples: Americium, ____ Einsteinium, Es Bromine, ____ Helium, He Lead(Plumbum), Pb Niobium, _____ Iron (Ferrum), Fe Mendelevium, _____

31. Compound A substance that contains _________ _____________________________. Compounds have different properties from the individual substances. (Ex: ______)

32. Example: H 2 O

34. The law of definite proportions states that a compound is always composed of the same elements in the same proportions.

35. Percent composition

36. Substance or mixture? If composition is fixed and may not change  substance

38. Mixture: a physical blend of two or more substances that are not chemically combined. Homogeneous:_____________ ________________________ _________________________ Heterogeneous ___________ _________________________

39. Mixtures A _________ blend of two or more substances.

40. Mixtures Homogeneous Heterogeneous

41. Example: Stainless Steel A homogeneous mixture of: -Iron (Fe) -Chromium (Cr) -Nickel (Ni)

42. Heterogeneous Mixtures ______________________ _____________________ Example: Oil and vinegar

43. Example: Gaseous Mixture Elements argon and nitrogen and a compound (water vapor). Choice ?

44. Note: Mixtures can be physically separated. Mixtures exhibit physical properties similar to the components of the mixture.

45. Separation Methods Use differences in the physical properties of the components of the mixture.

46. Example: Separate iron filings from sulfur using a _________.

47. Filtration: separates a _____ from a ________ in a heterogeneous mixture

48. Distillation: - separate dissolved _____ from a _____ -uses _________ and ______________.

49. Distillation of Crude Oil (Refining) Crude Oil is a ____________________

50. Distillation of Crude Oil