Pre-AP Chemistry Charts
oxidation chart & info
--atoms in a pure element have an ox # of zero
--the more electroneg element will have a neg ox # equal to how many e- it needs to be stable
--the less electroneg. # will have a pos ox # equal to how many e- it would give up to be stable
--F has an ox # of -1
--O has an ox # of -2 with a few exceptions (cmpds with halogens ox #= +2, peroxides H2O2
ox # -1)
--H has an ox # of +1 w/nonmetals & an ox # of -1 with metals
--sum of ox #’s in a neutral cmpd = 0
--sum of ox #’s in a polyatomic ion = charge on ion
--ox # for a monatomic ion is the same as the charge
SOLUBILITY RULES FOR IONIC CMPDS
(1) all compounds whose cation is Group IA or ammonium are
soluble, no matter what the anion is.
(2) all nitrates, chlorates, perchlorates, acetates are soluble,
no matter what the cation is.
(3) all chlorides, bromides and iodides are soluble except Ag,
Pb (II) & Hg (I)
(4) all sulfates are soluble except Ag, Pb (II) and Hg (I), Ca, Sr
& Ba
(5) all hydroxides are insoluble except Ca, Sr, Ba
(6) everything else in INSOLUBLE rule 1 supersedes all
Equations
Formula mass is the same as molar mass which is the same as formula weight.
molar mass = (mass of 1st element x # of atoms) + (mass of 2nd element x # of atoms) + …
Percent error
=
(observed - actual value) x 100
actual value.
actual = calculated or from a chart
observed is what you get in the lab
If your answer is negative you were under the calculated value.
If your answer is positive you were over the calculated value.
Density
mass
 density
volume
measured in: liquid = g/mL
solid = g/cm3
gas = g/L
Average Atomic Mass = (% isotope #1)(mass of #1) + (% isotope #2)(mass of #2) + . . . . .
grams to moles
#grams
moles to grams
# moles
1 mol
molar mass in grams
molar mass in grams
1 mole
moles to molecules or atoms
percent composition
# moles
=
6.022 x 1023 atoms or molecules
1 mole
mass of element in 1 mol of cmpd
formula mass of cmpd
x 100
percent comp. to empirical formula
assume 100g sample
convert each element from grams to moles
moles element # 1: moles element #2
divide each element by the element with the smallest # of moles
ratio! element #1: element #2
must be in whole numbers (so 1:2.5 would be 2:5)
percent yield = observed yield
x 100
theoretical yield
(observed is from lab theoretical is calculated)
Equation Stoichiometry
MASS-MASS problem
mass of given
moles of unknown from formula mass of
1 mol given
balanced equation
unknown
= mass of unknown
molar mass
moles of given from
1 mol unknown
of given
balanced equation
MASS-MOLE problem
mass of given
1 mol given
molar mass
of given
moles of unknown from
balanced equation
moles of given from
balanced equation
= moles of unknown
MOLE-MASS problem
moles of given
moles of unknown from molar mass of
balanced equation
unknown
moles of given from
1 mol unknown
balanced equation
= mass of unknown
MOLE-MOLE problem
moles of given
moles of unknown from
balanced equation
= moles of unknown
moles of given from
balanced equation
MASS-VOLUME problem with a gas at STP
moles of unknown from 22.4 L of
mass of given
1 mol given
balanced equation
unknown
molar mass of moles of given from
1 mol unknown
given
balanced equation
= vol of unknown
VOLUME-MASS problem with a gas at STP
moles of unknown from molar mass of
vol of given
1 mol given
balanced equation
unknown
= mass of unknown
22.4 L of
moles of given from
1 mol unknown
given
balanced equation
VOLUME-MASS problem with a liquid
moles of unknown from
vol of given
# mol given in M
balanced equation
1 L given
moles of given from
balanced equation
molar mass of
unknown
1 mol unknown
= mass of unknown
Reactions
Synthesis reactions A + X → AX
Combustion reaction - substance combines with oxygen releasing a
*activity series p. 266
amt of E combustion of a hydrocarbon produces water & carbon dioxide
Decomposition Reactions AX → A + X
*a single cmpd reacts to form 2 or more simpler substances
*6
kinds of decomp reactions
a. metallic carbonates when heated form metallic oxides & CO2
b. (many) metallic hydroxides when heated form metallic oxides & water
c. metallic chlorates when heated form metallic chlorides & oxygen
d. (some) acids when heated form nonmetallic oxides & water
e. (some) oxides when heated decompose
f. electrolysis
Single Replacement Reactions
A + BX → AX + B
use activity chart for metals
Double Replacement Reactions
AX + BY → BX + AY
typical reactions
a. metallic carbonates when heated form metallic oxides & CO2
Li2CO3 → Li2O + CO2
b. (many) metallic hydroxides when heated form metallic oxides & water
LiOH → Li2O + H2O
c. metallic chlorates when heated form metallic chlorides & oxygen
LiClO3 → LiCl + O2
d. (some) acids when heated form nonmetallic oxides & water
H2CO3 → CO2 + H2O
e. (some) oxides when heated decompose
HgO → Hg + O2
f. electrolysis
g. a metal in a cmpd is replaced by a more active metal
Al + Pb(NO3)2 → Pb + Al(NO3)3
h. (1/2) the hydrogen in water replaced by a metal
Na + H2O → NaOH + H2
i. hydrogen replaced by metal in an acid
Mg + HCl → MgCl2 + H2
j. a halogen in a cmpd is replaced by a more active halogen
Cl2 + KBr → KCl + Br2
k. combustion of H produces water vapor
l. combustion of a hydrocarbon produces carbon dioxide & water
large
IONS AND OXIDATION NUMBERS
POSITIVE IONS (cations)
Hydrogen
H 1+
Lithium
Li 1+
Sodium
Na 1+
Potassium
K 1+
Cesium
Cs 1+
Silver
Ag 1+
Copper ( I )
Cu 1+
Mercury ( I )
Hg2 2+
( ion always “diatomic” )
Ammonium
NH41+
Barium
Magnesium
Calcium
Strontium
Zinc
Cadmium
Copper ( II )
Iron ( II )
Lead ( II )
Mercury ( II )
Tin ( II )
Ba 2+
Mg 2+
Ca 2+
Sr 2+
Zn 2+
Cd 2+
Cu 2+
Fe 2+
Pb 2+
Hg 2+
Sn 2+
Aluminum
Iron ( III )
Al 3+
Fe 3+
Tin ( IV )
Lead ( IV )
Sn 4+
Pb 4+
NEGATIVE IONS (anions)
Bromide
Chloride
Fluoride
Iodide
Br 1Cl 1F 1I 1-
Oxide
Sulfide
O 2S 2-
Nitride
Phosphide
N 3P 3-
Acetate
C2H3O2 1Cyanide
CN 1Hydroxide
OH 1Nitrite
NO2 1Nitrate
NO31Chlorate
ClO31Perchlorate
ClO41Bisulfite
HSO31(aka hydrogen sulfite)
Bisulfate
HSO41(aka hydrogen sulfate)
Bicarbonate
HCO31(aka hydrogen carbonate)
Permanganate MnO41-
Carbonate
Chromate
Dichromate
Sulfite
Sulfate
Oxalate
CO32CrO42Cr2O72SO32SO42C2O42-
Phosphite
Phosphate
PO33PO43
Pre-AP Chemistry Equations
KE= ½ mv2 (kinetic energy = ½ mass x velocity2)
F = ma (force = mass x acceleration)
a = Vf - Vi
acceleration = (velocity final – velocity initial)/ time
t
d = m/v (density = mass/volume)
M = m/n (Molar Mass = mass/moles)
Combined Gas Laws: P1V1T2 = P2V2T1
1 atm = 760mm Hg
1 atm = 760 torr
1 atm = 1.013 x 105 Pa
1 atm = 101.325 kPa
1 atm = 14 psi
Ideal Gas Law PV = nRT
(gas constant R = .0821 if atm are used, 8.314 is Pa are used & 62.4 if mm Hg are used)
M = m/n
(Molar Mass = mass/moles)
Solutions:
molarity (M) 
moles of solute
Liters of solution
1 kg water = 1 L water
1g of water = 1 mL of water
molality (m) 
moles of solute
kg of solvent
Dilution of solutions:
M1V1  M 2V2