chem unit 5

Solid

Particles compact, close together, & vibrate - lowest energy

definitive shape and volume 😶

liquid

particles flow past each other - medium energy

indefinite shape, definite volume

gas

partcles fast(electrons can’t keep up), have charges(ionize) - high energy - far apart

indefinite shape + volume

temperature

average kinetic energy of particles in a substance.

what happens when increase in temp.?

increase of energy + motion of atoms in molecules of a substance

kinetic molecular theory?

1) elastic collisions: molecules collide w/ each other - no energy loss

2) gas particles in continuous motion - possess kinetic motion

3) temp. measured as avg. kinetic energy of ALL gas particles(some fast, some slow, take avg.)

4)gases consits of many tiny molecules

5) no forces of attraction bw particles

plasma

particles ionize(have charges), fast so electrons can’t keep up, highest energy

supercrital fluid

exist at high temp. + pressue AND past critical point

has properties of liquids and gases

exothermic reaction

release heat → forms bond → temp. of substance decreases

endotermic reaction

absorbs heat → breaks bonds → temp. of substance increases

sublimination

solid → gas

deposition

gas → solid

freezing

liquid → solid

melting

solid → liquid

condensation

gas → liquid

vaporizing

liquid → gas

recombination

plasma → gas

ionization

gas → plasma

IMFs?

forces of attraction/repulsion between molecules

hydrogen bonding

strongest imf ig, highest boiling + melting point(taught it was 2nd to ion dipole but wtv)

Hydrogen bonded with NOF(nitrogen, oxygen, flourine)

high diff. in electronegativiety

(+) hydrogen and partial (-) NOF → strong attraction or permanant dipole mwah

contains dipole-dipole and LDF

dipole dipole

2nd strongest imf → medum rise in melting + boiling point

between 2 polar molecules only

comtains ldf

LDF(London dispersion forces)

Weakest IMF → weakest rise in melting + boiling points

every molecule has it

partial attraction bw polar or nonpolar molecules

temporray dipole

cer example(writtenberry approved)

ethanol has a heigher boiling point than ethane because ethanol has stronger IMFs of HB, DD, and LDF. This means that it takes more energy to OVERCOME the IMFs in ethanol leading to a higher boiling point.

vapor pressure

random molecules w/ high kinetic energy escape as liquids → it is the PRESSURE above liquids

chemicals w/ weaker imfs mean?

stronger vapor pressure → easier to evaporate

covalent bond networks

crystallized form of element or compound → structure allows for bonding → increases boiling point + durability

collgetive properties

substances dissolve differently based on solute and solvent

like dissolve like

polar dissolve polar

nonpolar dissolve nonpolar

soluble

solid will dissolve

insoluble

solid no dissolve womp womp

miscible

liquid will mix

inmiscible

liquid not mix womp womp

adhesion

propert of water to stick to other surfaes due to high polarity

cohesion

property of water sticking to itself → creates surface tension in water

ionic solubility

water polar molecule → able dissolved in ionic compound

partially (+) hydrogen pull on (-) anion

partially (-) oxygenpull on (+) cations

chemical salt

any ionic compound that dissolves in water

vant hoffs factor

estimates how many ions created when smth dissolves

measured using i= # of particles made

if ionic - add up subscripts

unsaturated

solvent can dissolve more solute

saturated

 solvent is at its maximum amount of solute dissolved, any more added will fall out

supersaturated

• solvent forced to dissolve more than can handle

• solvent must be heated so it is unsaturated or saturated. Then, it must cool down to a point such that there is more solute than allowed.

• extremely delicate and fragile, slightest disturbance break and turn into a crystal instead.