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Solids, Liquids, & Gases I. States of Matter Kinetic Molecular Theory Four States of Matter Thermal Expansion MATTER
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A. Kinetic Molecular Theory KMT All matter is composed of small particles (atoms, molecules, ions). These particles are in constant, random motion. Motion is dependent on temperature. Higher temp. = higher KE.
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Thermal energy Total energy of a material’s particles KE – vibration and movement between particles PE – results from forces acting within or between particles Thermal Energy (Heat) = KE + PE A. Kinetic Molecular Theory
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B. Four States of Matter Solids low KE - particles vibrate but can’t move around definite shape & volume crystalline - repeating geometric pattern amorphous - no pattern (e.g. glass, wax)
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B. Four States of Matter Liquids higher KE - particles can move around but are still close together indefinite shape definite volume
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B. Four States of Matter Gases high KE - particles can separate and move throughout container indefinite shape & volume
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B. Four States of Matter Plasma very high KE - particles collide with enough energy to break into charged particles (+/-) gas-like, indefinite shape & volume stars, fluorescent light bulbs, TV tubes
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C. Thermal Expansion Most matter expands when heated & contracts when cooled. Temp causes KE. Particles collide with more force & spread out. EX: thermostats (bimetallic strip), sidewalks
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Solids, Liquids, & Gases II. Changes in State Phase Changes Heating Curves MATTER
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A. Phase Changes Melting solid to liquid Freezing liquid to solid melting point = freezing point
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A. Phase Changes Vaporization (boiling) liquid to gas at the boiling point Evaporation liquid to gas below the boiling point Condensation gas to liquid
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A. Phase Changes Sublimation solid to gas EX: dry ice, freeze drying, iodine
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A. Phase Changes
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B. Heating Curves Kinetic Energy motion of particles related to temperature Potential Energy space between particles related to phase changes
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B. Heating Curves Solid - KE Melting - PE Liquid - KE Boiling - PE Gas - KE
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B. Heating Curves Heat of Fusion energy required to change from solid to liquid some attractive forces are broken
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B. Heating Curves Heat of Vaporization energy required to change from liquid to gas all attractive forces are broken EX: steam burns, sweating, and… the drinking bird HEATING CURVE
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Solids, Liquids, & Gases III. Properties of Fluids Archimedes Principle Pascal’s Principle Bernoulli’s Principle Fluid Flow MATTER
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A. Archemides Principle Buoyant force of an object in a fluid is equal to the weight of the fluid displaced
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A. Pascal’s Principle Pressure applied to a fluid is transmitted unchanged throughout the fluid.
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A. Bernoulli’s Principle Pressure exerted by a fluid decreases as its velocity increases.
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Solids, Liquids, & Gases IV. Behavior of Gases Pressure Boyle’s Law Charles’ Law Gay-Lussac’s Law MATTER
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A. Pressure Which shoes create the most pressure?
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A. Pressure Key Units at Sea Level 101.325 kPa (kilopascal) 1 atm 760 mm Hg 14.7 psi
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A. Pressure Barometer Atmospheric Pressure Manometer Contained Pressure
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A. Pressure Effect on Boiling Point When atmospheric pressure increases, the boiling point of a liquid increases. EX: high altitude cooking, boiling cold water
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B. Boyle’s Law When the volume of a gas decreases, its pressure increases (at constant temp). P V PV = k INVERSE
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V T C. Charles’ Law When the temperature of a gas increases, its volume also increases (at constant pressure). DIRECT
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C. Charles’ Law Absolute Zero - Temp at which... the volume of a gas would equal zero. all particle motion would stop. -273°C or 0 K
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P T C. Gay-Lussac’s Law The pressure and absolute temperature (K) of a gas are directly related at constant mass & volume
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