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Matter and Change

This text provides a review of the criteria for the classification of matter, including properties, states (solid, liquid, gas), and composition. It discusses physical and chemical properties, as well as the classification of substances and mixtures. The text also explores methods of separating mixtures and the concepts of elements and compounds. Finally, it explains chemical properties and changes, including the law of conservation of mass.

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Matter and Change

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  1. Matter and Change Ms. Miller 8th SSI

  2. A) Classification of Matter • Review of prior knowledge: • Talk with your shoulder partner, how is matter classified?

  3. Some Criteria for the Classification of Matter • Properties • State (solid, liquid, gas) • Composition

  4. Properties Intensive -DOES NOT depend on amount of matter. Extensive -DOES depend on amount of matter present.

  5. Intensive and Extensive Properties Sulfur

  6. Properties • Physical: observed without without changing the composition of the substance. • Chemical: the ability of a substance to undergo a specific chemical change

  7. Examples of Physical Properties • Color, odor, hardness, density, melting point, boiling point, state, solubility.

  8. Example: Physical Properties

  9. States of Matter • Solid • fixed shape and volume, incompressible • Liquid • fixed volume, takes the shape of its container • Gas • takes the volume and shape of its container

  10. Solid Liquid Gas http://www.chem.purdue.edu/gchelp/atoms/states.html

  11. Bromine Gas (Vapor) Liquid

  12. Change of Phase Melting solid  liquid Condensation gas  liquid Freezing liquid  solid Evaporation liquid  gas Sublimation solid  gas Boiling: Evaporation occurring beneath the liquid’s surface.

  13. Is changing phase a physical or chemical change? Review of prior knowledge: Talk with your shoulder partner and be prepared to share out

  14. Classification of Matter(by composition)

  15. (Pure) Substance • Matter that has a uniform and definite composition. • Elements • Compounds

  16. Mixture: a physical blend of two or more substances that are not chemically combined. • Homogeneous • Heterogeneous

  17. Mixtures • Homogeneous • Heterogeneous

  18. Homogeneous mixture (solution) • Uniform composition throughout. • One phase.

  19. Copper II Sulfate and its solution in water.

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

  21. Example: Gaseous Mixture • Elements argon and nitrogen and a compound (water vapor).

  22. Heterogeneous Mixtures Example: Oil and vinegar • Non-uniform composition throughout the mixture • Two or more phases.

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

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

  25. Example: Separate iron filings from sulfur using a magnet.

  26. Filtration: separates a solid from a liquid in a heterogeneous mixture

  27. Distillation: -separate dissolved solids from a liquid -uses boiling and condensation.

  28. Distillation of Crude Oil (Refining) • Crude Oil is a mixture of Hydrocarbons

  29. Distillation of Crude Oil

  30. c) Elements and Compounds

  31. Elements • The simplest substances. • Can not be separated into simpler substances. • Building blocks of all matter. • More than 100 known elements. • Represented by chemical symbols.

  32. 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.

  33. Americium, Am Einsteinium, Es Bromine, Br Helium, He Lead(Plumbum), Pb Niobium, Nb Iron (Ferrum), Fe Mendelevium, Md Examples:

  34. Compound • A substance that contains two or more elements chemically combined. • Compounds have different properties from the individual substances. (Ex: H2O)

  35. Example: H2O

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

  37. d) Chemical Properties and Chemical Changes

  38. H2O composition is fixed- compound Gaseous Phase Liquid Phase

  39. Chemical Properties • The ability of a substance to transform into a new substance (to undergo a chemical change). • Example: Magnesium reacts with oxygen to form magnesiumoxide.

  40. Magnesium Mg

  41. Burning of Magnesium2Mg+ O2 2MgO

  42. Physical Changes • Physical change: a change in the physical properties of a substance. • Composition does not change. • May be reversible or irreversible. • Examples: Reversible: Irreversible:

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

  44. Burning of MethaneCH4 +2O2 CO2 + 2H2O

  45. Burning of MethaneCH4 + 2O2 CO2 + 2H2O

  46. Recognizing a Chemical Change • energy exchange • production of a gas • color change • formation of a precipitate

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

  48. The Law of Conservation of Mass (Antoine Lavoisier) • In any chemical or physical change, mass is neither created or destroyed • Mass is CONSTANT

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