THE EQUATION SHEET
Constants:
Basic Equations:
Avogadro’s Number (N A )
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 /SATP
Acid-Base Chemistry:
[
pH = − log H 3 O
[H O ] = 10
+
3
+
]
− pH
pK a + pK b = pK w
pK b = − log K b
[
[OH ] = 10
−
−Q
# mol
M Enthalpy = ∑ ( E k +E p )
]
− pOH
 [ HA] 

pH Buffer = pKa − log
 [ A− ] 


Order of reaction = m + n
V
ngas =
22.7mol / L
% atom ecomony =
[
] [
t1/ 2
]
K SP = Kc (Aqueous)
0.693
=
k
1
=
k [ A]]ο
Quantum
Mechanics:
∆E =
hc
λ
c = λv
 1
1
∆E = RH  2 − 2 
n

 f ni 
E = hf
n? = 2dsin?
k = Ae − Ea / RT
ο
∆H rxn
= ∑ D(broken) − ∑ D( formed )
∆S = k ln W =
c1V1 = c 2V 2
molar mass of desired product
× 100%
molar mass of all reac tan ts
k 
E A = − RT ln 
 A
ο
∆H rxn
= ∑ ∆H οf ( P) − ∑ ∆H οF ( R )
PV = nRT
Conversion factors:
1 atm = 100 kPa
1atm = 760 torr = 760 mm Hg
1nm = 10-9 m
0°C = 273.15 K
1dm3 = 1L= 1 x 10-3 m3 = 1 x 103 cm3 = 1 x 103 mL
1 amu = 1.66 x 10-27 kg
t1 / 2
Q
∆T
Q = mc∆T
n = cV
m
MR
Rate Re action = k [A]m [B ]n
C=
pK b = 14 − pK a
n=
Chemical Kinetics &
Equilibrium:
∆c
Rate Re action =
∆t
1
E k = mv 2
2
pK a = − log K a
pOH = − log OH −
Thermodynamics:
∆H rxn = H P − H R
q = ∆H at constant pressure
∆H ο =
K w = Ka × Kb
pH + pOH = 14
6.02 × 1023
8.314 J/molžK or 0.0821 Lžatm/molžK
6.626 × 10-34 Jžs
2.18 × 10-18 J
3.00 × 108 m/s
1.602 × 10-19
1.381 × 10-23 J/K
22.7 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 / 298 K and 100 kPa
q ∆H
=
= S System + S Surroundin g
T
T
∆S οrxn = ∑ S (οP) − ∑ S (οR )
[A]t = − kt + [ A]ο
ln[A]t = − kt + ln[A]ο
ln
∆G ο = ∆H ο − T∆S ο
k 1 Ea  1
1
=
 − 
k2 R T 2 T1
KC =
ο
∆Grxn
= ∑ ∆G(οP) − ∑ ∆ G(οR )
[Pr odtcts]nB
[Re ac tan ts]nA
K P = KC (RT )∆n
∆G ο = − RT ln K
Nuclear Chemistry:
E = mc
U=
238
92
1
0
Gas:
2
234
+0
PV = nRT
Th+ He
4
2
P1V1 P2V 2
=
T1
T2
Rate1
=
Rate 2
M2
M1
STP conditions= 273 K and 100 kPa
SATP conditions= 298 K and 100 kPa
n→11H + −01 e
ngas =
Redox:
Ch arg e = Current × Time
ο
ο
E cell
= E cathode
− E οAnode
∆G ο = −nFE ο
V
22.7mol / L
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) à ZnCl2(aq) + H2(g)
2. Acid + Base = Salt + Water
Ex. HCl(aq) + NaOH(aq) à NaCl(aq) + H2O(l)
3. Acid + Metal Carbonate = CO2 + H2O + Salt
Ex. CaCO 3(s) + 2HCl(aq) à H2O(l) + CO2(g) + CaCl2(aq)
4. Metal Oxide + Acid à Salt + Water
Ex. MgO (s) + 2HCl(aq) à MgCl2(aq) + H2O(l)
Periodic Table of Electronegativities
Polyatomic Ions:
-
Acetate
CH3COO or C2H3O2- Hydroxide
OH-
Aluminate
AlO2- , Al 2O42-
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
MnO 42-
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
MnO 4-
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 carbonate (bicarbonate)
HCO3-
Sulfite
SO32-
Hydrogen arsenate
HAsO42-
Superoxide
O2-
Hydrogen phosphate
HPO 42-
Tartrate
(CH(OH)COO) 22-
Hydrogen phosphite
HPO 32-
Tellurate
TeO42-
Hydrogen sulfate
HSO 4-
Tellurite
TeO32-
Hydrogen sulfite
HSO 3-
Thiocyanate
SCN-
Hydronium
H3O+
Thiosulfate
S2O32-