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Ch. 1 - Matter

Ch. 1 - Matter. I. States of Matter (p.12) Kinetic Molecular Theory States of Matter. A. Kinetic Molecular Theory. KMT Particles of matter are always in motion. The kinetic energy (speed) of these particles increases as temperature increases. B. Four States of Matter. Solids

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Ch. 1 - Matter

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  1. Ch. 1 - Matter I. States of Matter (p.12) Kinetic Molecular Theory States of Matter

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

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

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

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

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

  7. Ch. 1 - Matter II. Classification of Matter (p.15-17, 397-398) Matter Flowchart Pure Substances Mixtures C. Johannesson

  8. Warm-Up • What is the difference between a homogeneous and heterogeneous mixture? (how can you tell the difference?) C. Johannesson

  9. 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 C. Johannesson

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

  11. B. Pure Substances • Element • composed of identical atoms • EX: copper wire, aluminum foil C. Johannesson

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

  13. B. 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. C. Johannesson

  14. B. Pure Substances • For example… Two different compounds, each has a definite composition. C. Johannesson

  15. C. Mixtures • Variable combination of 2 or more pure substances. Heterogeneous Homogeneous C. Johannesson

  16. Tyndall Effect C. Mixtures • Solution • homogeneous • very small particles • no Tyndall effect • particles don’t settle • EX: rubbing alcohol C. Johannesson

  17. C. Mixtures • Colloid • heterogeneous • medium-sized particles • Tyndall effect • particles don’t settle • EX: milk C. Johannesson

  18. C. Mixtures • Suspension • heterogeneous • large particles • Tyndall effect • particles settle • EX: fresh-squeezed lemonade C. Johannesson

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

  20. Ch. 1 - Matter III. Properties & Changes in Matter (p.11-14) Extensive vs. Intensive Physical vs. Chemical C. Johannesson

  21. A. Extensive vs. Intensive • Extensive Property • depends on the amount of matter present • Intensive Property • depends on the identity of substance, not the amount C. Johannesson

  22. A. Extensive vs. Intensive • Examples: • boiling point • volume • mass • density • conductivity intensive extensive extensive intensive intensive C. Johannesson

  23. B. 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 C. Johannesson

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

  25. B. 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 C. Johannesson

  26. 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 C. Johannesson

  27. B. Physical vs. Chemical • Examples: • rusting iron • dissolving in water • burning a log • melting ice • grinding spices chemical physical chemical physical physical C. Johannesson

  28. MATTER Ch. 9 - Classification of Matter I. Describing Matter (p.254-261) Physical Property Physical Change Chemical Change Chemical Property

  29. A. Physical Property • A characteristic of a substance that can be observed without changing its identity. • can be used to separate mixtures • EX: magnetism, density

  30. B. Physical Change • A change in the form of a substance without changing its identity. • properties remain the same • reversible • can be used to separate mixtures • EX: dissolving, grinding

  31. C. Chemical Change • A change in the identity of a substance. • properties change • irreversible • Signs: color change, formation of a gas/solid, release of light/heat • EX: burning, rusting

  32. D. Chemical Property • A characteristic that indicates whether a substance can undergo a specific chemical change. • EX: flammability, reactivity

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