THE EQUATION SHEET
Constants:
Basic Equations:
Avogadro’s Number (NA)
Universal Gas Constant (R)
Planck’s constant (h)
Rydberg Constant (RH)
Speed of Light (c)
Charge of an Electron (q)
Boltzmann Constant (kB)
Molar Volume (Vmol)
Mass of Earth
Specific Heat Capacity of Water (C)
Ionic Product Constant of Water (Kw)
Faraday’s constant (F)
STP conditions
Acid-Base Chemistry:

pH   log H 3O
H O  10

3


 pH
pK a  pK b  pK w
pK b   log K b
OH  10

pH Buffer
Q
# mol
M Enthalpy   ( E k E p )
Q
T
Q  mcT

 pOH
 [ HA] 

 pKa  log
 [ A ] 


 

H rxn
  H f ( P)   H F ( R)


H rxn   D(broken )   D( formed )
S  k ln W 
q H

 S System  S Surroundin g
T
T

S rxn
  S (P)  S (R)
% atom ecomony 
Rate1

Rate 2
n H  e
1atm = 760 torr = 760 mm Hg
0°C = 273 K
1 amu = 1.66 x 10-27 kg
Chemical Kinetics:
c
RateRe action 
t
E 
RateRe action  k Am Bn
c  v
At
0.693
k
1

k A]
Quantum
Mechanics:
hc
ln
 kt  [A]
k 1 Ea  1
1
   
k 2 R  T 2 T1 
[Prodtcts]nB
[Re ac tan ts]nA
K P  KC RT n
G   RT ln K
Redox:
Ch arg e  Current  Time


Ecell
 Ecathode
 E Anode
M2
M1
G   nFE 
0
1
Extras
Solubility:
Qc
<
=
>
Kc
Prod Fav
EQ
React Fav
Q
<
=
>
Ksp (Precipitate)
No
No
Yes (Super Saturated)
Aufbau Principle: Build up electrons one by one.
1K(2)2L(8)3M(18)4N(32)5O(50)6P(72)7Q(98)
Formations:
1. Acid + Metal = Salt + Hydrogen Gas
Ex. 2HCl(aq) + Zn(s)  ZnCl2(s) + H2(g)
2. Acid + Base = Salt + Water
Ex. HCl(aq) + NaOH(aq)  NaCl(s) + H2O(l)
3. Acid + Metal Carbonate = CO2 + H2O + Salt
Ex. CaCO3(s) + HCl(aq)  H2O(l) + CO2(g) + CaCl(s)
4. Metal Oxide + Acid  Salt + Water
Ex. MgO(s) + HCl(aq)  MgCl2(s) + H2O(l)
Periodic Table of Electronegativities

 1
1 
E  R H  2  2 
n

 f ni 
E  hf
nλ = 2dsinθ
lnAt  kt  lnA
Gas:
4
U  234
 0Th 2 He
molar mass of desired product
 100%
molar mass of all reac tan ts
Conversion factors:
1L atm = 101.3 J
1nm = 10-9 m
1dm3 = 1L
PV  nRT
238
92
c1V1  c 2V2
K SP  Kc (Aqueous)
V

22.4mol / L
KC 
Nuclear Chemistry:
2
1
1
n gas
PV  nRT
k  Ae  Ea / RT

Grxn
  G(P)   G(R)
1
0
Order of reaction m  n
t1 / 2

n  cV
m
MR
t1 / 2 
G   H   TS 
E  mc
n
k
E A   RT ln  
 A
C
pK b  14  pK a

q  H at constant pressure
1
Ek  mv 2
2
pK a   log K a
pOH   log OH 
Thermodynamics:
H rxn  H P  H R
H  
K w  K a  Kb
pH  pOH  14
6.02 × 1023
8.314 J/molK or 0.0821 Latm/molK
6.626 × 10-34 Js
2.18 × 10-18 J
3.00 × 108 m/s
1.602 × 10-19
1.381 × 10-23 J/K
22.4 L/mol
5.97 x 1024 kg
4.18 J/gK or 4.18 kJ/kgK
1.00 × 10-14 (mol/L)2 at 298 K (25°C)
96 500 C/mol
273 K and 100 kPa
Polyatomic Ions:
−
Acetate
CH3COO or C2H3O2− Hydroxide
OH−
Aluminate
AlO2−, Al2O42−
Hypobromite
BrO−
Amide
NH2−
Hypochlorite
ClO−
Ammonium
NH4+
Hypoiodite
IO−
Antimonate
SbO43−
Hypophosphite
PO23−
Antimonite
SbO33−
Hyposulfite
SO22−
Arsenate
AsO43−
Iodate
IO3−
Arsenite
AsO33−
Iodite
IO2−
Bicarbonate (hydrogen carbonate)
HCO3−
Manganate
MnO42−
Bromate
BrO3−
Nitrate
NO3−
Bromite
BrO2−
Nitrite
NO2−
Carbide
C22−
Oxalate
C2O42-
Carbonate
CO32−
Ozonide
O3−
Chlorate
ClO3−
Perbromate
BrO4−
Chlorite
ClO2−
Perchlorate
ClO4−
Chromate
CrO42−
Periodate
IO4−
Chromite
CrO2−
Permanganate
MnO4−
Cyanate
OCN−
Peroxide
O22−
Cyanide
CN−
Phosphate
PO43−
Dichromate
Cr2O72−
Phosphite
PO33−
Dihydrogen arsenate
H2AsO4−
Plumbate
PbO32−
Dihydrogen phosphate
H2PO4−
Plumbite
PbO22−
Dihydrogen phosphite
H2PO3−
Stannate
SnO32−
Disulfide
S22−
Stannite
SnO22−
Ferrate
FeO42−
Sulfate
SO42−
Hydrogen arsenate
HAsO42−
Sulfite
SO32−
Hydrogen carbonate (bicarbonate)
HCO3−
Superoxide
O2−
Hydrogen phosphate
HPO42−
Tartrate
(CH(OH)COO)22−
Hydrogen phosphite
HPO32−
Tellurate
TeO42−
Hydrogen sulfate
HSO4−
Tellurite
TeO32−
Hydrogen sulfite
HSO3−
Thiocyanate
SCN−
Hydronium
H3O+
Thiosulfate
S2O32−