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Kinetic Molecular Theory All matter is made up of tiny atoms and molecules that interact physically Molecules are separated by empty space All molecules are in constant motion (kinetic energy) Kinetic energy increases as heat is added and decreases as heat is removed
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Physical Science
Heat and Matter
MatterMatter
Anything that occupies space and has mass
Ex. AirLaw of Conservation of Matter
Matter is neither created or destroyed
It is only changed from one form to another
Solid, liquid, gas, and plasma are states or phases of matter
Kinetic Molecular Theory
All matter is made up of tiny atoms and molecules that interact physicallyMolecules are separated by empty spaceAll molecules are in constant motion (kinetic energy)Kinetic energy increases as heat is added and decreases as heat is removed
Phases of Matter - Solids
Definite shape and volume
Rigid 3-D structure
Atoms/molecules bonded in place
Allowed motions restricted to vibration in place only
Phases of Matter - Liquids
Definite volume, indefinite shape
Only weak cohesive bonds between component molecules
Constituent molecules mostly in contact
Allowed motionsVibrationRotation
Phases of Matter - Gases
Indefinite volume and shapeMolecules mostly not in contact Allowed motions
Vibration and rotation (molecules with more than one atom)
Random, mostly free paths
Phases of Matter - Plasma
PlasmaA very hot gas consisting of atoms that have been stripped of their electrons because of high kinetic energies
For a picture, see the link belowhttp://www.rialian.com/rnboyd/plasma2.jpg
Phase ChangesSolid/liquid
Liquid/gas
Solid/gas
Temperature(Direction ->)
Melting Boiling Sublimation
Temperature(Direction <-)
Freezing Condensation
Sublimation
Evaporation and Condensation
Individual molecules can change phase any time
Evaporation:Energy required to
overcome phase cohesionHigher energy molecules
near the surface can then escape
Condensation: Gas molecules near the
surface lose KE to liquid molecules and merge
HeatA form of energy transfer
between two objectsEnergy always moves from
higher temperature regions to lower temperature regions
Calorie (cal) – unit of energy needed to raise temperature of 1 g of water 1 degree Celsius
TemperatureA measure of the internal energy of an object
ThermometersUsed to measure temperature
Temperature measured in degrees2 temperature scales
Celsius: water freezes at 00 and boils at 1000 Fahrenheit: water freezes at 320 boils at 2120
WaterMajor constituent of living things“Universal solvent”Dissolves most moleculesSolid phase less dense than liquid
Ice floats!High specific heat
Amount of heat (energy) needed to increase the temperature of 1 gram of water 1 degree Celsius
Cohesion Attractive forces between like molecules
Adhesion Attractive forces between unlike molecules
http://www.physicalgeography.net/fundamentals/8a.html
http://www.uni.edu/~iowawet/H2OProperties.html
Heat flow Three mechanisms for heat
transfer due to a temperature difference
1. Conduction2. Convection3. Radiation
Natural flow is always from higher temperature regions to cooler ones
ConductionHeat flowing through
matter (solids)Mechanism
Hotter atoms collide with cooler ones, transferring some of their energy
Direct physical contact required; cannot occur in a vacuum
Poor conductors = insulators (Styrofoam, wool, air…)
Convection Energy transfer
through the bulk motion of hot material (liquids and gases)
ExamplesSpace heaterGas furnace
(forced)Natural convection
mechanism - “hot air rises”
Radiation Radiant energy - energy associated with
electromagnetic wavesCan operate through a vacuum All objects emit and absorb radiationTemperature determines
Emission rateIntensity of emitted lightType of radiation given off
Temperature determined by balance between rates of emission and absorptionExample: Global warming
Study Websites What Is Matter?: Properties and Classification of
Matter http://www.learner.org/resources/series200.html#
The Particle Nature of Matter: Solids, Liquids, and Gases http://www.learner.org/resources/series200.html#
Physical Changes and Conservation of Matter http://www.learner.org/resources/series200.html#
Chemical Changes and Conservation of Matter http://www.learner.org/resources/series200.html#
Density and Pressurehttp://www.learner.org/resources/series200.html#
Rising and Sinking http://www.learner.org/resources/series200.html#
Water Propertieshttp://www.uni.edu/~iowawet/H2OProperties.html
Heat and Temperature http://www.uni.edu/~iowawet/H2OProperties.html
GACE II Information- ECE/MG
Water Freezing point
Kinetic energy of molecules reduced enough to allow crystallization
Presence of solute particles interferes with crystal formation lowers the freezing point (freezing point depression)
Example: Salt excluded from ice as seawater freezesIce is practically pure waterSalinity of seawater increases
Example: Antifreeze, ethylene glycolBoiling point
Normal boiling pointTemperature where vapor pressure = average sea level
atmospheric pressureVapor pressure over a solution less than that of the pure
solventSolute particles displace solvent particles on surface,
hindering vaporization Leads to higher boiling point
GACE II Information- MGInterpreting Diagrams that Illustrate Changes in the Physical States of Matterhttp://dthschemistry.com/ch_12%20Phase%20Diagrams.doc