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Liquids & Solids
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Objectives 12-1 describe the motion of particles of a liquid and the properties of a liquid using KMT define and discuss vaporization define and discuss freezing
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KMT of Liquids FLUID - a substance that can flow and therefore take the shape of its container Particles have lower KE than gases Attractive forces between molecules is greater More ordered than gases
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Properties of Liquids Relative to gases have a much higher density Relatively incompressible Can diffuse Surface tension –(force that pulls molecules together giving a smaller surface area) –Capillary action – attraction between the surface of a liquid and a solid (meniscus) Vaporization – changing from liquid to gas –Evaporation – particles escaping from the surface of a non- boiling liquid Boiling – changing of liquid to bubbles of vapor that appear throughout a liquid Freezing – change of a liquid to a solid by the removal of heat
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Objectives 12-2 describe the motion of particles of a solid and the properties of a solid using KMT differentiate between crystalline and amorphous solids describe crystal symmetry and define crystal structure and unit cell
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KMT of Solids Higher density than liquids More ordered Very strong intermolecular forces –London dispersion –Dipole-dipole –Hydrogen bonding Crystalline solids (very organized) Amorphous solids (not organized)
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Properties of Solids Definite shape and volume Definite melting point –Supercooled liquids – amorphous solids have the ability to flow over a range of temperatures High density/incompressibility Low rate of diffusion
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Crystalline Solids
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Ionic Crystals Cations and anions arranged in a pattern Group 1 & 2 bonded with Group 16 & 17 Hard and brittle High melting points Good insulators
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Covalent network crystals Single atoms bonded to its neighbor Can be very large Usually hard and brittle High melting points Non-conductors or semiconductors
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Metallic crystals Metal atoms surrounded by a sea of electrons Good conductors Melting points vary
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Covalent molecule crystals Covalently bonded molecules held together by intermolecular forces –If non-polar, only LDF (weak) –If polar, held together by LDF, dipole-dipole, and maybe hydrogen bonds Low melting points Relatively soft Easily vaporized Good insulators
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Amorphous solids “without shape” Plastics and glass
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Changes of State
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Equilibrium Dynamic condition in which two opposing changes occur at the same rate in a closed system
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Equilibrium and Changes of State Solid to liquid melting Solid to gas sublimation Liquid to solid freezing Liquid to gas vaporization Gas to liquid condensation Gas to solid deposition
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LeChatelier’s Principle When a system in equilibrium is stressed, it attains a new equilibrium which will minimize stress
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Stresses Addition of liquid Removal of liquid Addition of vapor Removal of vapor Decrease in volume Increase in volume Decrease in temp Increase in temp
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Equilibrium Vapor Pressure The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature
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Phase Diagrams Triple point – the temperature and pressure at which all 3 phases can exist Critical point – indicates critical pressure and temperature –Critical Temp: temp at which a substance cannot exist in the liquid state –Critical Pressure: the lowest pressure at which a substance can exist as a liquid at the critical temperature
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Volatile vs. Non-volatile Volatile liquids evaporate easily (i.e – lower temperatures)
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12-4: Water
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Physical Properties of Water Clear Colorless Odorless Tasteless Molar heat of fusion is 6.009 kJ/mol (amount of heat energy needed to melt one mole of water) Molar heat of vaporization is 40.79 kJ/mol (amount of heat energy needed to vaporize one mole of water)
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