AP Chemistry Memorization

Use this to memorize things for your upcoming AP Exam

A/C

e- move through the wire from anode to cathode

Salt Bridge

Anion to cathode and cation to cathode

ΔH- and ΔS+

TDF @ all temp

ΔH+ and ΔS-

never tdf

ΔH+ and ΔS+

TDF at high temperatures.

ΔH- and ΔS-

TDF at low temperatures.

@ half equivalence point…

pH=Pka

ΔG +

Not TDF

ΔG -

TDF

Hydrogen bonding happens when H+ is bonded with…

O, N, and F

Strong Acids are _____ bonded with H+

Cl, Br, I, ClO4, SO4, and NO3

Strong Bases are _____ bonded with OH-

Group 1 and 2 hydroxides

phosphate

PO4 3-

Nitrate

NO3 -1

Acetate

C2H3O3 - or CH3COO -

Sulfate

SO4 2-

Chlorate

ClO3-

Carbonate

CO3 2-

Hydroxide

OH-

Ammonium

NH4+

Compounds containing what are fully soluable?

Na+, K+, NH4+, NO3-

Microwave

Rotation

Infared

Vibration

UV/Visible

Electronic Transition

Which is the most abundant on a mass spectrometry graph?

The one with the highest relative abundance

Using a mass spectrometry graph, how do you find the element?

Multiply all mass #s by percentage (decimal form) and then add all

How do you find average atomic mass using a mass spectrometry graph?

Add all masses and then divide by the number of different masses

Ideal gas law equation

PV=nRT

Moles

Grams/molar mass

Moles @ STP

liters/22.4

% composition

(element mass/ compound mass) X 100

Empirical Formula

mass or % divided by molar mass to get moles and then divide the moles by the smallest number of moles

Molecular Formula

Mass divided by empirical mass and then multiply empirical formula subscripts by that #

Coulomb’’s Law

The closer e- are to the nucleus, the stronger the attraction

Going up energy levels…

absorbs Energy

Going back down to energy levels…

emits energy

incoming radiation=

binding + kinetic energy

More protons=

more attraction

what is zinc metals only charge?

+2

what is silver metals only charge?

+1

Bigger atoms have…

more e- shielding

as metals go more to the right

the less metallic they behave

atomic radius increases

left and down

ionization energy increases

right and up

electronegativity increases

right and up

stronger bonds have a…

greater charge and smaller ion

losing e- results in

smaller atom

gaining e- results in

bigger atom

Substitutional alloy

similar sized combined metals

interstitial alloys

different sized metals combine

larger atoms=

longer bond length

bonds in decreasing length…

single, double, triple

perfect distance to bond is at the

lowest hump in a PE diagram

most common network covalents

graphite, diamond, quartz

ionic bond conductivity

only when aq or liquid

molecular covalent conductivity

never

network covalent conductivity

never

metallic conductivity

solid and liquid

conductivity increases with

more ions and higher [ ]

Strength and length of bond=

bond order / # of resonance structure

Which elements only need 2 valence e-

H and He

Which element(s) only needs 6 valence e-

B

Which elements can have 8+ valence e-

Si,P,S,Cl

formal charge=

(# of valence e-) - (bonds + lone e-)

2 domains 0 LP

Linear 180

3 domains 0 LP

trigonal planar 120

4 domains 0 LP

tetrahedral 109.5

5 domains 0 LP

trigonal bipyramidal 90 & 120

6 domains 0 LP

octahedral 90

3 domains 1 LP

bent 120

4 domains 1 LP

trigonal bipyramidal 109.5

4 domains 2 LP

bent 109.5

5 domains 1 LP

Seesaw 90 and 120

5 domains 2 LP

T shape 90

6 domains 1 LP

square pyramidal ~90

6 domains 2 LP

square planar 90

4 electron domain hybridization

Sp3

3 electron domain hybridization

Sp2

2 electron domain hybridization

Sp

dipole moment arrows point to…

more electronegative element

inter

between molecules

intra

within molecules

more e-

stronger LDFs

IMF strength

ion-dipole, hydrogen, dipole-dipole, LDF

Stronger IMFs=

lower vaporization

retention factor (rf)=

distance travelled by solute/ distance traveled by solvent front

the higher the temp…

the higher the variation of velocity in particles

Fast, high temps, and smaller molecules result in

more effusion

the combined gas law used when moles are held constant

p1v1/t1=p2v2/t2

ideal gases behave at

high temp low pressure

% error

(expiremental-expected)/(expected) X 100

LEO

Losing E- oxidization

GER

gaining e- reduction

acids

donate H+

bases

accept H+

0 order rate law

rate=k

1st order rate law

rate=k[a]

2nd order rate law

rate=k[a]²

0 order graph

[A] with a -slope

first order graph

ln[A] with a -slope