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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

  8. 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

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

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

  11. 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)

  12. 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.

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

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

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

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

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

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

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

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

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

  22. 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

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

  24. 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

  25. 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

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

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