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Solids, Liquids and Gases
Chapter 16
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Section 1 – Kinetic Theory
States of matter you saw at lunch? Kinetic Theory – explanation of how particles in matter behave All matter is composed of small particles (atoms, molecules, ions)
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Kinetic Theory Particles in constant, random motion Particles are colliding Energy that particles lose from collisions is negligible
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Average Kinetic Energy
Temperature is measure of average kinetic energy. Warmer – particles have MORE energy Move faster Cooler – particles have LESS energy Move slower
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Solid State – H2O Particles in fixed position
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Liquid State Particles in solid gain energy and move faster break out of fixed position Melting point: temperature where solid begins to liquefy Heat of fusion: amount of energy needed to change a solid to liquid
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Liquids Flow Particles have energy to break SOME attraction and flow
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Gas State Particles have energy to escape ALL attraction
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Vaporization Liquid particles gain enough energy to escape to gas phase Evaporation: vaporization at the surface of liquid, spontaneously Boiling point: applying heat, temperature at which pressure of vapor is equal to external pressure, liquid to gas Heat of vaporization: amount of energy needed for liquid to be a gas
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Gases fill their Container
Diffusion: spreading of particles throughout until they are mixed
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Heating Curve of a Liquid
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Heating Curve of a Liquid
a and c – increasing in energy b and d – energy used to break attraction between particles
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Plasma Def: consists of positive and negative particles
Very HIGH temperature Particles moving so fast e- are stripped off Lightning, sun, neon lights
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Thermal Expansion
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Thermal Expansion Spaces are expansion joints Prevent cracks
Absorbs heat – expands Cools – shrinks
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Expansion of Matter Thermal Expansion: increase in the size of a substance when the temperature is increased Warmer = less attraction b/ particles = move freer Cooler = more attraction = closer together
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Expansion of Matter
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Expansion of Matter
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Strange Water Ice is less dense than liquid water
(+) and (-) ends arrange themselves next to each other Create empty spaces
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Strange Water
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Solid or Liquid? Amorphous Solids: “without” form, change to liquid over range of temperatures Ex: glass, plastic Liquid turned to solid too quickly
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Solid or Liquid Liquid crystals: change to liquid but don’t lose their ordered form Ex: liquid crystal display (LCD) calculators, etc.
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Properties of Fluids Section 2
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How do ships float? Buoyancy: ability of fluid to exert upward force on object. If force equal to weight = float
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Archimedes’ Principle
Def: buoyant force on an object is equal to the weight of the fluid displaced by the object
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Density Same size blocks - wood and steel
Displace same amount of water BUT, wood block floats and steel block sinks Different densities – object has less density than density of fluid to float
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Archimedes’ Principle
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Pascal’s Principle Pressure: force exerted per unit area
Pressure applied to fluid is exerted throughout the fluid Used in hydraulic lifts – use your weight to lift something much heavier
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Bernoulli’s Principle
Def: as velocity of fluid increases pressure of fluid decreases
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Fluid Flow Viscosity: the resistance of a fluid to flow
Syrup – high viscosity Water – low viscosity
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Behavior of Gases Section 3
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Pressure Result of gas particle collisions with the container
More collisions = More pressure Pressure unit = Pascal (Pa) How do we get high pressure?
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Boyle’s Law Relationship between pressure and volume
volume, size of container, what will pressure do? Pressure Inversely related: as one goes the other goes , or vice versa
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Charles’s Law Relationship between volume and temperature
“Keep away from heat” on pressurized can temperature what will volume do? volume Directly related: as one goes the other goes , or vice versa
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Kelvin Scale All (+) numbers
0K = absolute zero – all particle motion stops 0K = -273oC K = oC + 273
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