Solids, Liquids, & Gases I. States of Matter  Kinetic Molecular Theory  Four States of Matter  Thermal Expansion MATTER

A. Kinetic Molecular Theory  KMT  All matter is composed of small particles (atoms, molecules, ions).  These particles are in constant, random motion.  Motion is dependent on temperature. Higher temp. = higher KE.

 Thermal energy  Total energy of a material’s particles  KE – vibration and movement between particles  PE – results from forces acting within or between particles  Thermal Energy (Heat) = KE + PE A. Kinetic Molecular Theory

B. Four States of Matter  Solids  low KE - particles vibrate but can’t move around  definite shape & volume  crystalline - repeating geometric pattern  amorphous - no pattern (e.g. glass, wax)

B. Four States of Matter  Liquids  higher KE - particles can move around but are still close together  indefinite shape  definite volume

B. Four States of Matter  Gases  high KE - particles can separate and move throughout container  indefinite shape & volume

B. Four States of Matter  Plasma  very high KE - particles collide with enough energy to break into charged particles (+/-)  gas-like, indefinite shape & volume  stars, fluorescent light bulbs, TV tubes

C. Thermal Expansion  Most matter expands when heated & contracts when cooled.   Temp causes  KE. Particles collide with more force & spread out.  EX: thermostats (bimetallic strip), sidewalks

Solids, Liquids, & Gases II. Changes in State  Phase Changes  Heating Curves MATTER

A. Phase Changes  Melting  solid to liquid  Freezing  liquid to solid melting point = freezing point

A. Phase Changes  Vaporization (boiling)  liquid to gas at the boiling point  Evaporation  liquid to gas below the boiling point  Condensation  gas to liquid

A. Phase Changes  Sublimation  solid to gas  EX: dry ice, freeze drying, iodine

A. Phase Changes

B. Heating Curves  Kinetic Energy  motion of particles  related to temperature  Potential Energy  space between particles  related to phase changes

B. Heating Curves Solid - KE  Melting - PE  Liquid - KE  Boiling - PE  Gas - KE 

B. Heating Curves  Heat of Fusion  energy required to change from solid to liquid  some attractive forces are broken

B. Heating Curves  Heat of Vaporization  energy required to change from liquid to gas  all attractive forces are broken  EX: steam burns, sweating, and… the drinking bird HEATING CURVE

Solids, Liquids, & Gases III. Properties of Fluids  Archimedes Principle  Pascal’s Principle  Bernoulli’s Principle  Fluid Flow MATTER

A. Archemides Principle  Buoyant force of an object in a fluid is equal to the weight of the fluid displaced

A. Pascal’s Principle  Pressure applied to a fluid is transmitted unchanged throughout the fluid.

A. Bernoulli’s Principle  Pressure exerted by a fluid decreases as its velocity increases.

Solids, Liquids, & Gases IV. Behavior of Gases  Pressure  Boyle’s Law  Charles’ Law  Gay-Lussac’s Law MATTER

A. Pressure Which shoes create the most pressure?

A. Pressure  Key Units at Sea Level kPa (kilopascal) 1 atm 760 mm Hg 14.7 psi

A. Pressure Barometer Atmospheric Pressure Manometer Contained Pressure

A. Pressure  Effect on Boiling Point  When atmospheric pressure increases, the boiling point of a liquid increases.  EX: high altitude cooking, boiling cold water

B. Boyle’s Law  When the volume of a gas decreases, its pressure increases (at constant temp). P V PV = k INVERSE

V T C. Charles’ Law  When the temperature of a gas increases, its volume also increases (at constant pressure). DIRECT

C. Charles’ Law  Absolute Zero - Temp at which...  the volume of a gas would equal zero.  all particle motion would stop. -273°C or 0 K

P T C. Gay-Lussac’s Law  The pressure and absolute temperature (K) of a gas are directly related  at constant mass & volume