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Ch. 13 States of Matter

Need I to Know Fuzzy Learn. Describe the assumptions of the kinetic theory as it applies to solid, liquids, and gases. Define the relationship between Kelvin temperature and average kinetic energy .

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Ch. 13 States of Matter

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  1. Need I to Know Fuzzy Learn Describe the assumptions of the kinetic theoryas it applies to solid, liquids, and gases. Define the relationship betweenKelvin temperature and average kinetic energy. Identify the conditions for freezing, melting, evaporation, condensation, boiling, and sublimation. Describe the equilibrium between a liquid and its vapor. Describe how equilibrium conditions are represented in a phase diagram. Ch. 13 States of Matter

  2. 13.3 Liquids and Solids Not fixed Not fixed Definite Definite Relatively high Extremely low Extremely low Low does not flow flows rapid medium none

  3. Kinetic Theory and the Nature of Gases What is kinetic energy? energy of motion The Kinetic Theory states: 1) Matter is composed of _________. 2) The particles move _____in constant random motion. 3) All collisions are perfectly __________.

  4. Gas Pressure What causes pressure? result of _________of particles What is a vacuum? no _________in a empty space

  5. Atmospheric Pressure What instrument measures atmospheric pressure? ____________ There are a variety of units used for pressure SI unit - 101.3 kPa(____________) other units of __________pressure at sea level 760 mm Hg = 29.9" (weatherman) 760 torrs 1 atm (atmosphere) 14.8 psi (pounds per square inch - tires)

  6. Conversion of Pressure How many kilopascals (kPa) in 1.5 atm? 1.5 atm |__________| = | | 1.5 atm | 101.3 kPa | = ________kPa | 1 atm |

  7. Kinetic Energy and Kelvin Temperature What is meant by average Kinetic Energy? Not all __________ are moving exactly the same speed If Kinetic Energy increases, how will it effect the temperature? > K.E. > temperature What is absolute zero? (0 K = -273 oC) all particles stop __________ K.E. and temp. are directly related to the Kelvin scale. 100 K --> 200 K x K.E. = 2x K.E.

  8. Standard Temperature Standard temperature is 0oC What is STP? Standard Temperature and Pressure 0oC and 101.3 kPa Remember ______L of any gas at STP

  9. The Nature of Liquids Liquids and gases flow, but liquids are more strongly attracted by intermolecular forces. Liquids cannot be ______________.

  10. Evaporation or Vaporization What is evaporation? The conversion of a liquid to a gas below its normal boiling point. Only molecules with certain amount of K.E. can _______from the surface. Evaporation is known as a ________process. Why? molecules with the highest amount of K.E. escape, leaving the molecules with the lowest K.E. behind. Ex. perspiration sweat with higher K.E. evaporates, leaving cooler sweat, which cools you off

  11. Evaporation in a closed container Evaporation in a closed container ex. terrarium particles collide with the walls of a sealed container and produce a vapor pressure above the liquid. What is dynamic equilibrium? ____________rate = ___________rate increase temperature --> increases vapor pressure

  12. Boiling Point of a Liquid When does a liquid boiling? Boiling point occurs when the ______pressure equals external air pressure. bubbles form because the pressure _____the bubbles equals the ____pressure. What is normal boiling point? refers to the boiling point at standard pressure. Boiling point decreases as external air pressure decreases sea level = 100oC Denver = 95oC Mt. Everest = 60oC

  13. Solids Are solid particles moving? vibrating about a fixed point Solids are dense and incompressible What is melting point? temp. at which a solid turns into a liquid solid melting> liquid <freezing

  14. I2, H2O,NH3, CO2, C12H22O11 Very soft, very low melting point and poor conductivity Inter- molecular _________ Atoms connected by ______bonds Fairly soft, low melting point, and poor conductivity Diamond and quartz Intra- molecular Very hard, high melting point, and poor conductivity NaCl, KBr, CaCO3 _______ Intra- molecular Atoms surrounded by mobile valence e- Soft to hard, low to high melting point, and excellent conductivity All metallic elements Intra- molecular

  15. Solid - Crystals What are crystals? atoms, ions, or molecules are arranged in an orderly, repeating 3D pattern lattice - array of _______ unit cell - smallest group of particles within a crystal that retains the ________ shape

  16. Allotropes What is an ___________? 2 or more different molecular forms of the same _________in the same physical state Ex. carbon diamond - 4 C graphite - 6 C buckey balls - 60 C Ex. arsenic gray or white

  17. Amorphous What is Amorphous? solids _______an order to their internal structure ex. rubber, plastic, glass glass is supercooled, no definite melting point, it gradually softens when heated

  18. Sublimation What is sublimation? change a substance from a solid to a gas or vapor without passing through the _____state Ex. iodine, air fresheners, moth balls Ex. dry ice --> CO2

  19. Phase Diagram Shows the relationship between the solid, liquid, and gas state and how temp and pressure affects them. What is triple point? all _______phases can exist at equilibrium

  20. Water Phase Diagram

  21. Plasma Plasma: The Fourth State of Matter gaseous mixture of electrons and positive ions partial plasma ex. fluorescent light, lightening bolts, neon signs "cold plasma" 50,000 -100,000 K "hot plasma" 10,000,000-1,000,000,000 K (stars)

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