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 – cools without crystallizing, makes random shards not crystals, ex: glass, plastic, rubber, asphalt Pg 399 a morphous 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 1.transfer electrons 2.solid 3.high melting pt 4.stronger than covalent (shared electrons) 5.salts 6.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 1.Boyle’s Law PV=PV marshmallow in syringe, graph Pg 418 2.Charles’ Law V/T=V/T hot objects expand, cold contracts, ex: expansion joints in sidewalk, graph Pg 420 3.Gay-Lussac’s Law P/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 Law PV/T = PV/T Pg 424 #13,14Combined Gas Law PV/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 #23,24Ideal 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