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Chemistry Ch 13 Pg 385

Chemistry Ch 13 Pg 385. Kinetic Theory – all matter in motion Particle collisions are elastic Solids – atoms crowded, move slightly while staying in crystalline structure

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Chemistry Ch 13 Pg 385

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  1. Chemistry Ch 13 Pg 385 • Kinetic Theory – all matter in motion • Particle collisions are elastic • Solids – atoms crowded, move slightly while staying in crystalline structure amorphous solid – cools without crystallizing, makes random shards not crystals, ex: glass, plastic, rubber, asphalt Pg 399 • Liquids – atoms farther and faster • Gas – farthest and fastest, most compressible, least dense

  2. Atmospheric Pressure – from collisions of air molecules, less molecules = less pressure (mountaintops, airplanes) • Barometer – measures air pressure • 1 atm = 760 mm Hg = 101.3 kPa • Pg 387 #1,2

  3. Kinetic Energy – energy of motion • Average Kinetic Energy = temperature • Graph Pg 388***** • Absolute Zero – all atoms stop moving, theory, zero K = - 273 C K = C + 273 • Pg 389 #6*** • Evaporation – room temp, surface • Boiling – added energy, bubbles at bottom = liquid changing to gas

  4. High Pressure RAISES Boiling Pt (pressure cooker) and LOWERS Cooling Pt (cloud in bottle) • Low Pressure LOWERS Boiling Pt (Pg 394) and RAISES Freezing Pt (instant soda freeze at room temp) Pg 395 #12-14 & Writing Activity

  5. Ionic Compounds • transfer electrons • solid • high melting pt • stronger than covalent (shared electrons) • salts • crystalline structure (allotropes – same element, diff crystal, ex: carbon in layers = graphite in pencils, carbon in body centered = diamond, carbon in sphere = soot Pg 398) Pg 399 #17,19 Pg 403 and 404 #25

  6. Gases Ch 14 Pg 418 Boyle’s LawPV=PV marshmallow in syringe, graph Pg 418 Charles’ LawV/T=V/T hot objects expand, cold contracts , ex: expansion joints in sidewalk, graph Pg 420 Gay-Lussac’s LawP/T = P/T pressure increases if trapped air heated, ex: pressure cooker, tires in summer, spray cans ( can explode if P too high) Pg 419 #7,8 Pg 421 #9,10 Pg 423 #11,12

  7. Combined Gas LawPV/T = PV/T Pg 424 #13,14 • Ideal Gas Law – based on IF all gases behaved perfectly, but they don’t – they are more attracted to each to each other at low temp or high pressure, so volume not always correct Pg 426-8 PV = nRT Pg 427 #23,24

  8. Dalton’s Law – total pressure = sum of pressure of each gas Pg 434 #31,32 Chart Pg 432 Pictures Pg 433 and 434

  9. Graham’s Law Pg 436 Diffusion – movement from high to low concentration Effusion – gas escaping through a hole, smaller molecules escape faster, ACT ex. Formula Pg 436, practice Key Equations Pg 438

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