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Chapter 10

Chapter 10. States of Matter. KMT. Kinetic Molecular Theory- describes matter as being constantly in motion Kinetic energy- energy in motion Yes, solids are moving Will explain difference of motion of atoms through song examples (fast, medium, slow)

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Chapter 10

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  1. Chapter 10 States of Matter

  2. KMT • Kinetic Molecular Theory- describes matter as being constantly in motion • Kinetic energy- energy in motion • Yes, solids are moving • Will explain difference of motion of atoms through song examples (fast, medium, slow) • Gas-fast, liquid = medium, solid = slow (plasma = fastest)

  3. Gases • Ideal gas- hypothetical gas that perfectly fits each of the following assumptions • Gases consist of large numbers of tiny particles that are far apart relative to their size • Collisions between gas particles and between particles and container walls are elastic (no net KE lost) • Particles in continuous, rapid, random motion (have KE) • *no forces of attraction between particles • Temperature depends on average KE (KE = ½ mv^2 (see board for example problems)

  4. Gases • Drunken Sailor • Expansion- gas fills any container • Fluidity- not attracted, so glide apart • Low density • Compressibility- come together • Diffusion- spread across room • Effusion- go through tiny hole • Gases are usually not ideal • High P, low T, particles are close together (noble gases ideal)

  5. Liquid • Fluid (flow) • When gases make inelastic collisions (stick) • Relatively high density • Relatively incompressible • Can diffuse (food dye in water) • Surface tension- neighbors stick together, decrease surface area, can push back • Capillary action- liquid attracted to solid, goes against gravity (water tree) • Adhesion vs. cohesion • Evaporation vs. freezing

  6. Solid • Particles vibrate • 2 types: crystalline vs. amorphous • Crystalline- orderly pattern, Amorphous- random • Definite shape, volume, melting point, high density, incompressible, low diffusion rate • Crystal unit cells • Cubic, trigonal, tetragonal, orthorhombic, hexagonal, monoclinic, triclinic

  7. Crystals • Ionic • Covalent • Metallic • Covalent Molecular (weaker forces) • Dessicates- take in water • Hydrates- have water • Anhydrous- no water in

  8. Phase changes • Volatile liquid- goes to gas quickly • P. 344-345 pics • Deposition vs. sublimation • Phase diagram picture on board (label solid, liquid, gas, triple point, critical point, critical temperature and critical pressure)

  9. Phase Conversion Problems • See board • Q = m(tf –ti)Cp • Q = mHfus • Q = mHvap • Qtotal = Q1+Q2+Q3+Q4+Q5 • Cp = 4.18 kJ/kgC • Hfus = 334 kJ/kg • Hvap = 2260 kJ/kg

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