ch2 Flashcards
3 things that Kinetic Particle Theory states
- All matter, made out, particles
- Particles, always, constant, random motion
- Kinetic energy of particles, increases when heated
When temp is constant during boiling, what does it mean?
change of state occuring
NOT TO BE CONFUSED w/ pure substance
substance X pure: 90 deg
substance X impure 80deg - 89deg
substance X pure during boiling, experiment repeated 5x observation is the same: stays constant 90deg until fully boiled
Substance X impure during boiling experiment repeated 5x, temp stays constant at different experiment timings
Solid
- Arrangement
- Motion of particles
- Orderly, very closely packed
- Vibrate, rotate, fixed positions (can’t change location)
Solid particles
- Amount of Energy
- Density
- Low
- Very Dense
Arrangement of liquid particles
Disorderly, Closely packed, less closely packed compared to solid
Liquid particles motion
Rolls, slide past one another
Liquid particles level of kinetic energy
Forces of attraction in liquid state particles
Moderate
Forces of attraction in liquid state particles
Strong
Level of density in liquid state particles
Dense
Motion of gaseous state particles
Movement: Moves around, random, high speed, all directions
Creates Pressure:, collide, each other, sides, container
Arrangment of Gaseous state particles
Very Far apart, disorderly
Kinetic energy of gaseous state particles
Very High
Density of gaseous state particles
very low density
Can copper be crystallised/evaporated?
Is copper soluble in water?
No.
“wet” copper is not a solution. (does not exist)
What affects evaporation
- volatile (evaporate quickly, rtp)
- large surface area
- high temp surface of liquid
fractional distillation
State 2 similarity between melting and boiling
Temperature stays constant
both phys change, involve state change
Why does temperature stay constant during melting/boiling?
- thermal energy absorbed by particles used, overcome forces, attraction, holding particles together
- instead, raising temperature
forces of attraction
ionic bonds
covalent bonds
metallic bonds
overcome forces,
and break bonds
3 differences between boiling and evaporation
- Boiling occurs -> boiling pt. only
evaporation occurs -> temperatures BELOW boiling pt. - Boiling occurs throughout liquid
Evaporation occurs at surface, liquid only - Boiling, faster process than evaporation
think of evaporation like much slower boiling below boiling pt, they’re 2 different words for a reason :)
2 characteristics of matter
- takes up space, has mass
- 3 states solid liquid gas
- melt/freeze exact
boil/condense too
definition of physical changes
- change in physical states
- does not produce new substances
evidence of movement of particles?
diffusion,
shows constant, random motion of particles
2 factors affecting diffusion
-
Mr
- shows total mass, all atoms, substance -
Temperature
- affect kinetic energy, particles -> more KE -> faster constant random motion
gravity DOES NOT AFFECT DIFFUSION!!!
affect chemical properties of atom
proton, neutron, electron?
electrons
isotopes sim diff
(besides proton, neutron count)
different
- mass number (different no. neutrons)
- physical properties
liquid, gas in container, how it acts
liquid: adopt shape, container
gas: fills container
y gas can be compressed
compressed, much smaller volume
- a lot of space btwn particles
describe boiling
- heat, causes bubbles of gas form
- below, surface of liquid
- allow liquid particles escape
- from surface, within liquid
what does heating/cooling curve show
how change in temp affect change in state
bascially dis the axes for the graph
when is there flat line in cooling/heating curve
when
- state change
- no temp change
describe heating from solid -> liquid
Kinetic Theory of Matter: Substances heated, particles absorb thermal energy converted kinetic energy
- Heat solid causes particles vibrate more
- as temp increase,
- vibrate so much that solid expands
- structure breaks
- solid melts
