Ch. 13 States of Matter Need Need I to I to Know Fuzzy Learn Know Fuzzy Learn 1. Describe the assumptions of the kinetic theory as it applies to solid, liquids, and gases. 1. Describe the assumptions of the kinetic theory as it applies to solid, liquids, and gases. 2. Define the relationship between Kelvin temperature and average kinetic energy. 2. Define the relationship between Kelvin temperature and average kinetic energy. 3. Identify the conditions for freezing, melting, evaporation, condensation, boiling, and sublimation. 3. Identify the conditions for freezing, melting, evaporation, condensation, boiling, and sublimation. 4. Describe the equilibrium between a liquid and its vapor. 4. Describe the equilibrium between a liquid and its vapor. 5. Describe how equilibrium conditions are represented in a phase diagram.

13.3 Liquids and Solids GasLiquidSolid Shape (e.g. fixed or not fixed) Volume (e.g. definite or indefinite) Density (relatively high, medium, or extremely low) Compressibility (e.g. relatively high, low, or extremely low) Fluidity (e.g. flows or does not flow) Not fixed Definite Extremely low Relatively high Low Extremely low flows does not flow Diffusion (e.g. rapid, medium, or none) rapid mediumnone

Kinetic Theory and the Nature of Gases What is kinetic energy? 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 __________.

Gas Pressure What causes pressure? result of _________ of particles What is a vacuum? no _________ in a empty space

Atmospheric Pressure What instrument measures atmospheric pressure? ____________ There are a variety of units used for pressure SI unit 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)

Conversion of Pressure How many kilopascals (kPa) in 1.5 atm? 1.5 atm |__________| = | | | | 1.5 atm | kPa | = ________ kPa | 1 atm | | 1 atm |

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 o C)all particles stop __________ (0 K = -273 o C)all particles stop __________ K.E. and temp. are directly related to the Kelvin scale. 100 K --> 200 K x K.E. = 2x K.E. x K.E. = 2x K.E.

Standard Temperature Standard temperature is 0 o C What is STP? Standard Temperature and Pressure 0 o C and kPa Remember ______ L of any gas at STP

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

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

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

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. refers to the boiling point at standard pressure. Boiling point decreases as external air pressure decreases sea level = 100 o C Denver = 95 o C Mt. Everest = 60 o C

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 temp. at which a solid turns into a liquid solid melting> liquid liquid <freezing

Type of Solid Unit particles CharacteristicsExamples Molecular Covalent Network Ionic Metallic _________ Atoms connected by ______ bonds _______ Atoms surrounded by mobile valence e- Very soft, very low melting point and poor conductivity Fairly soft, low melting point, and poor conductivity Very hard, high melting point, and poor conductivity Soft to hard, low to high melting point, and excellent conductivity I 2, H 2 O, NH 3, CO 2, C 12 H 22 O 11 Diamond and quartz NaCl, KBr, CaCO 3 All metallic elements Forces Inter- molecular Intra- molecular Intra- molecular Intra- molecular

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

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

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

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 --> CO 2

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 all _______phases can exist at equilibrium

Water Phase Diagram

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 K "hot plasma" 10,000,000-1,000,000,000 K (stars)