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Ch 13: States of Matter

Ch 13: States of Matter. Kinetic theory- tiny particles that make up matter are in constant motion Gas particles move rapidly in constant random motion, travel in straight paths, and move independently of each other Collisions between gas particles are perfectly elastic.

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Ch 13: States of Matter

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  1. Ch 13: States of Matter • Kinetic theory- tiny particles that make up matter are in constant motion Gas particles move rapidly in constant random motion, travel in straight paths, and move independently of each other Collisions between gas particles are perfectly elastic

  2. Gas pressure- force exerted by a gas per unit surface area of an object. The result of simultaneous collisions of billions of rapidly moving gas particles within an object Vacuum- empty space with no particles and no pressure

  3. Atmospheric pressure- collisions of air molecules with objects Pascal- SI unit of pressure 1 atm = 760 mm Hg = 101.3 kPa STP

  4. 13.2 Nature of Liquids • Liquids: Indefinite shape, definite volume do not have enough kinetic energy to overcome the intermolecular forces to escape into a gas Vaporization-conversion of a liquid to a gas, has enough energy to overcome the intermolecular forces Evaporation- conversion of a liquid to a gas at the surface of a liquid that is not boiling

  5. 13.2 Nature of Liquids • Vapor Pressure- force of a gas above a liquid evaporation Liquid - Vapor condensation At constant pressure, the rate of evaporation equals the rate of condensation As temperature increases, vapor pressure increases

  6. 13.2 Nature of Liquids • Boiling point: temperature at which the vapor pressure of a liquid is equal to the external pressure. pressure increases, boiling point increases Ex: pressure cooker high altitude cooking Normal boiling pt: boiling point of a liquid at STP

  7. 13.3 Nature of solids • Melting point: the temperature at which a solid turns into a liquid. Solids- definite shape and definite volume molecules are packed closely together in organized patterns dense and incompressible Crystals- solid substance arranged in an orderly, repeating, three-dimensional pattern

  8. 13.3 Nature of solids • p. 397- 7 patterns -Cubic -Tetragonal -Orthorhombic -Monoclinic -Triclinic -Hexagonal -Rhombohedral

  9. 13.3 Nature of solids • Allotropes- two or more different molecular forms of the same element in the same physical state • Amorphous solids- solid without an ordered internal structure

  10. Ch 13 Study Guide melting point normal boiling point boiling point amorphous solid sublimation allotrope evaporation crystal lattice vaporization kinetic theory barometer atmospheric pressure kinetic energy vapor pressure

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