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Ch. 1 - Matter

Ch. 1 - Matter. I. States of Matter 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. Five States of Matter. Bose-Einstein Condensate

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Ch. 1 - Matter

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  1. Ch. 1 - Matter I. States of Matter 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. Five States of Matter • Bose-Einstein Condensate • Atoms mount on top of each other

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

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

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

  7. 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

  8. Ch. 1 - Matter II. Classification of Matter Matter Flowchart Pure Substances Mixtures

  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

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

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

  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) • Ionic vs Molecular compounds

  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.

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

  15. C. Mixtures • Variable combination of 2 or more pure substances. • Can be separated by physical means. • Distillation, density, filtration, magnetism, boiling points Homogeneous Heterogeneous

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

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

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

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

  20. Ch. 1 - Matter III. Properties & Changes in Matter Extensive vs. Intensive Physical vs. Chemical

  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

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

  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

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

  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

  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

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

  28. Intro to periodic table • Groups (Families) • Periods • Noble Gases • Metals vs. Nonmetals • Metalloids (B, Si, Ge, As, Sb, Te) • Alkali Metals • Halogens

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