Adv. Chem Ch 13 - Beitko

gas

no defenite volume or shape

do gasses have high ot low densities

low; particles are so much farther away from each other because gasses take up a lot of space

gas particles

flow and mix by random motion (diffusion)

1st part of kinetic molecular theory

gases consist of large \#s of tiny particles

2nd part of kinetic molecular theory

the particles of a gas are in constant motion, moving rapidly in straight lines in all directions, and thus possess kinetic energy

3rd part of kinetic molecular theory

the collisions between particles of a gas and container walls are elastic collisions

in gasses, when kenetic energy is transferred between two particles

the total energy of the particles remain the same. there is no net loss of kinetic energy

4th part of kinetic molecular theory

there are no forces of attraction or repulsion between particles of gas

5th part of kinetic molecular theory

the average kinetic energy of the particles of a gas is directy proportional to the kelvin temperature of gas

pressure

the force exerted per unit p \= f/a

pressure units

atmospheres (atm) pascals (pa) bars (bar) torr (torr) millimeters of mercury (mm hg) pounds per square inche (psi)

standard temperature and pressure (stp)

0 degrees celsius, 273 kelvin, 760 mm hg

particles would have no kinetic energy at

absolute zero

barometer

measures atomspheric pressure

manometer

measues the pressure in a container

liquids

definite volume no definite shape

have stronge intermolecular forces than gases

liquids

why do liquids have a higher density than gases

because particles are closer together

can liquids diffuse slower or faster than gasses

slower

how are particles arranged in liquids

they are not in fixed positions and can slide past eachother

soilds

defenite shape and volume

solids have the strongest and highest

intermolecular forces and densities (water is an exception)

how are particles arranged in a solid

in a relatively fixed position. they can vibrated a little, but not much

crystalline

particles are arrnaged in a competing pattern (salts)

amorphous

particles are arranged randomly (waxes, plastics, glass)

vaporizaion

the process by which a liquid or a solid changes into a gas

in vaporization, particles gain enough energy to

overrcome the attractive forces holding them together

evaporation

the process by which particles escape the surface of a nonboiling liquid and enter the gas state

condensation

the process by which a gas changes into a liquid

boiling

the change of a liquid to a gas

boiling point

the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure

freezing

the physical change of a liquid to a solid by the removal of heat

freezing point

the temperature at which solid and liquid are at equuilibrium

melting

the physical change of a solid to a liquid by the addition of heat

during melting, particles gain enough energy to

overcome the attractive forces holding them together

sublimation

change of state from a solid directly to a gas (dry ice)

deposition

change the state from a gas directly to a solid (frost)

phase diagram

a graph of pressure versus temperature that shows the condition under which the phases of a substance exit

triple point

the temp and pressure at which all 3 states can coexist at equilibrium

critical point

temp and pressure where only a gas can exit

normal boiling point

boiling point at standard pressure

normal freezing/melting point

the freezing/melting point at standard pressure