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Unit 1. Matter and Change

Unit 1. Matter and Change. Chapter 1 and 3. Do Now:. What is matter as described in Chemistry?. Chapter 1 & 3 Objective . Distinguish between: intensive and extensive properties Physical & chemical changes/properties Classify matter. Matter and its Properties. It’s Classified!

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Unit 1. Matter and Change

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  1. Unit 1. Matter and Change Chapter 1 and 3

  2. Do Now: • What is matter as described in Chemistry?

  3. Chapter 1 & 3Objective • Distinguish between: • intensive and extensive properties • Physical & chemical changes/properties • Classify matter

  4. Matter and its Properties • It’s Classified! • But first what is Scientific Method and what does it involve?

  5. Properties & Changes in Matter • Extensive vs. Intensive • Physical vs. Chemical

  6. A. Extensive vs. Intensive • Extensive Property • depends on the amount of matter present • ex,.- • Intensive Property • depends on the identity of substance, not the amount • Ex.-

  7. A. Extensive vs. Intensive • Extensive Property • depends on the amount of matter present • ex,.- Volume, mass, Energy • Intensive Property • depends on the identity of substance, not the amount • Ex.- melting point, boiling point, conduct electricity or heat • WHAT ABOUT DENSITY??

  8. A. Extensive vs. Intensive • Examples: • boiling point • volume • mass • density • conductivity

  9. A. Extensive vs. Intensive • Examples: • boiling point…… intensive • Volume …. extensive • Mass ….. extensive • Density ….. intensive • Conductivity ….. intensive

  10. PROPERTYB. Physical vs. Chemical • Physical Property • can be observed without changing the identity of the substance • Chemical Property • describes the ability of a substance to undergo changes in identity

  11. B. Physical vs. Chemical physical chemical physical physical chemical • Examples: • melting point • flammable • density • magnetic • tarnishes in air

  12. CHANGEC. Physical vs. Chemical • Physical Change • changes the form of a substance without changing its identity • properties remain the same • Chemical Change • changes the identity of a substance • products have different properties

  13. B. Physical vs. Chemical • Signs of a Chemical Change • change in color or odor • formation of a gas • formation of a precipitate (solid) • change in light or heat

  14. B. Physical vs. Chemical • Examples: • rusting iron • dissolving in water • burning a log • melting ice • grinding spices

  15. B. Physical vs. Chemical chemical physical chemical physical physical • Examples: • rusting iron • dissolving in water • burning a log or charcoal • melting ice • grinding spices?

  16. Properties and Changes in Matter In the example of burning of charcoal, carbon and oxygen are the reactants in the combustion reaction. Carbon dioxide is the product. carbon + oxygen carbon dioxide C + O2 CO2 (reactants) (product)

  17. Homework • Review Scientific Method: Read page 12 – 16 Q 17 Complete - Work sheet

  18. STATE OF MATTER Chapter 3

  19. Do Now • Name the State of Matter • How do they differ?

  20. States of Matter • There are Four state of matter • A. Solid • B. Liquid • C. Gas • D. Plasma • State of matter depends on Kinetic Energy between the particles

  21. A. Kinetic Molecular Theory • KMT • Particles of matter are always in motion. • The kinetic energy (speed) of these particles increases as temperature increases.

  22. Four States of Matter • A. Solids • very low KE - particles vibrate but can’t move around • fixed shape • fixed volume

  23. Four States of Matter • B. Liquids • low KE - particles can move around but are still close together • variable shape • fixed volume

  24. Four States of Matter • C. Gases • high KE - particles can separate and move throughout container • variable shape • variable volume

  25. Four States of Matter • D. Plasma • very high KE - particles collide with enough energy to break into charged particles (+/-) • gas-like, variableshape & volume • stars, fluorescentlight bulbs, CRTs

  26. SOLUTIONS AND MIXTURES

  27. Objective: • Classification of Matter • DO NOW: • What is a solution? • Describe the difference between a heterogeneous and homogenous mixture

  28. A. Pure Substances • Element • composed of identical atoms • EX: copper wire, aluminum foil

  29. A. Pure Substances • Compound • composed of 2 or more elements in a fixed ratio • properties differ from those of individual elements • EX: table salt (NaCl)

  30. A. Pure Substances • Law of Definite Composition • A given compound always contains the same, fixed ratio of elements. • Law of Multiple Proportions • Elements can combine in different ratios to form different compounds.

  31. A. Pure Substances • For example… Two different compounds, each has a definite composition.

  32. Pure Substances(constant composition) • Elements • Listed on the Periodic Table • Cannot be broken down into unique components • Na, Cl, Al, O2, S8 • Compounds • Made of elements that are chemically joined • Can be broken down • NaCl, H2O, AlCl3, H2SO4

  33. B. Mixtures • Variable combination of 2 or more pure substances. Heterogeneous Homogeneous

  34. B. Mixtures(variable composition) • Homogeneous – Solutions • evenly distributed • Heterogeneous • not evenly distributed

  35. Tyndall Effect B. Mixtures • Solution • homogeneous • very small particles • no Tyndall effect

  36. B. Mixtures • Colloid • heterogeneous • medium-sized particles • Tyndall effect • particles don’t settle • EX: milk

  37. B. Mixtures • Suspension • heterogeneous • large particles • Tyndall effect • particles settle • EX: fresh-squeezed lemonade

  38. C. Mixtures • Examples: • mayonnaise • muddy water • fog • saltwater • Italian salad dressing

  39. C. Mixtures colloid suspension colloid solution suspension • Examples: • mayonnaise • muddy water • fog • saltwater • Italian salad dressing

  40. MIXTURE PURE SUBSTANCE yes no yes no Is the composition uniform? Can it be chemically decomposed? Colloids Suspensions A. Matter Flowchart MATTER yes no Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

  41. A. Matter Flowchart • Examples: • graphite • pepper • sugar (sucrose) • paint • soda

  42. A. Matter Flowchart element hetero. mixture compound hetero. mixture solution • Examples: • graphite • pepper • sugar (sucrose) • paint • soda

  43. Tea – Homogeneous Mixture

  44. Air – Homogeneous Mixture

  45. Alloys – Homogeneous Mixtures

  46. Cereal – Heterogeneous Mixture

  47. Sand – Heterogeneous Mixture

  48. Separating Mixtures Only a physical change- no new matter • Filtration - separate solids from liquids with a barrier (filter paper) • Distillation - separate liquids because of different boiling points • Heat mixture • Catch vapor in cooled area • Chromatography - different substances are attracted to paper or gel, so move at different speeds

  49. Separating Mixtures cont…. • Crystallization - results in formation of solid particles of a substance from a solution containing the dissolved substance • Sublimation – separation when a solid changes to a vapor without melting or going through a liquid phase

  50. Filtration Distillation Chromatography

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