Formations:
1. Acid + Metal = Salt + Hydrogen Gas
Ex. 2HCl(aq) + Zn(s) Æ ZnCl2(aq) + H2(g)
2. Acid + Base = Salt + Water
Ex. HCl(aq) + NaOH(aq) Æ NaCl(aq) + H2O
3. Acid + Metal Carbonate = CO2 + H2O + Salt
Ex. CaCO3(s) + HCl(aq) Æ H2O + CO2(g) + CaCl2(aq)
4. Metal Oxide + Acid Æ Salt + Water
Ex. MgO(s) + HCl(aq) Æ MgCl2(aq) + H2O
Polyatomic Ions:
Acetate
Aluminate
Amide
Ammonium
Antimonate
Antimonite
Arsenate
Arsenite
Bicarbonate (hydrogen carbonate)
Bromate
Bromite
Carbide
Carbonate
Chlorate
Chlorite
Chromate
Chromite
Cyanate
Cyanide
Dichromate
Dihydrogen arsenate
Dihydrogen phosphate
Dihydrogen phosphite
Disulfide
Ferrate
Hydrogen carbonate (bicarbonate)
Hydrogen arsenate
Hydrogen phosphate
Hydrogen phosphite
Hydrogen sulfate
Hydrogen sulfite
CH3COO− or C2H3O2−
AlO2−, Al2O42−
NH2−
NH4+
SbO43−
SbO33−
AsO43−
AsO33−
HCO3−
BrO3−
BrO2−
C22−
CO32−
ClO3−
ClO2−
CrO42−
CrO2−
OCN−
CN−
Cr2O72−
H2AsO4−
H2PO4−
H2PO3−
S22−
FeO42−
HCO3−
HAsO42−
HPO42−
HPO32−
HSO4−
HSO3−
Hydronium
Hydroxide
Hypobromite
Hypochlorite
Hypoiodite
Hypophosphite
Hyposulfite
Iodate
Iodite
Manganate
Nitrate
Nitrite
Ozonide
Perbromate
Perchlorate
Periodate
Permanganate
Peroxide
Phosphate
Phosphite
Plumbate
Plumbite
Stannate
Stannite
Sulfate
Sulfite
Superoxide
Tartrate
Tellurite
Thiocyanate
Thiosulfate
H3O+
OH−
BrO−
ClO−
IO−
PO23−
SO22−
IO3−
IO2−
MnO42−
NO3−
NO2−
O3−
BrO4−
ClO4−
IO4−
MnO4−
O22−
PO43−
PO33−
PbO32−
PbO22−
SnO32−
SnO22−
SO42−
SO32−
O2−
(CH(OH)COO)22−
TeO32−
SCN−
S2O32−
THE EQUATION SHEET
Constants:
Avagadro’s Number (NA)
Universal Gas Constant (R)
Planck’s constant (h)
Rydberg Constant
Speed of Light (c)
Charge of an Electron (q)
Boltzmann Constant (kB)
Molar Volume (Vmol)
Compton Wavelength of the Electron (λc)
Specific Heat Capacity of Water (C)
Faraday’s Constant (F)
6.02 × 1023
8.314 J/molxK
6.626 × 10-34 Jxs
2.18 × 10 -18 J
3.00 × 10 8 m/s
1.602 × 10-19
1.381 × 10-23 J/K
22.4 L/mol
2.42631 × 10-12 m
4.18J/gxmol
9.64846 × 104 C/mol
Conversion factors:
1A = 1C/s
1C = 1 J/Vxmol
1L atm = 101.3J
1nm = 10-9m
1atm = 760 torr = 760mm Hg
0°C = 273 K
Basic Equations:
n=
n gas =
The Equations:
Acid-Base Chemistry:
[
pH = − log H 3 O
[H O ] = 10
+
3
+
]
∆H rxn = H P
q = ∆H
− pH
pK b = 14 − pK a
[OH ] = 10
−
t1 / 2 =
]
[
] [
ο
∆H rxn
= ∑ ∆H οf ( P ) − ∑ ∆H Fο ( R )
k
ln 
 A
EA = −
RT
1
t1 / 2 =
k [A]]ο
]
ο
∆H rxn = ∑ D(broken) − ∑ D( formed )
− pOH
0.693
k
Rate Re action = k [A]m [B ]n
Ek =
pK b = − log K b
c1V1 = c 2V 2
Chemical Kinetics:
∆c
Rate Re action =
∆t
Thermodynamics:
−HR
at constant pressure
1 2
v
2
Q
C=
∆T
Q = mc∆T
pK a = − log K a
[
V
22.4mol / L
−Q
# mol
M Enthalpy = ∑ ( E k +E p )
pK a + pK b = pK w
pOH = − log OH −
n = cV
∆H ο =
K w = Ka × Kb
pH + pOH = 14
m
MR
q ∆H
∆S = k ln W = =
= S System + S Surrounding
T
T
ο
∆S rxn
= ∑ S (οP ) −∑ S (οR )
k = Ae − Ea / RT
[A]t
= − kt + [ A]ο
1
1
= kt +
[A]
[A]ο
ln[A]t = −kt + ln[A]ο
∆G ο = ∆H ο − T∆S ο
ο
∆G rxn
= ∑ ∆G (οP ) − ∑ ∆G (οR )
Quantum Mechanics:
hc
E=
λ
c = fλ


1 
 1
∆E = R H 
−

 ni2 n 2f 


E = hf
Nuclear Chemistry:
E = mc
2
4
U = 234
+ 0Th + 2 He
238
92
1
0
n→11H + −10 e
Gas:
PV = nRT
Redox:
Ch arg e = Current × Time
ο
ο
E cell
= E cathode
− E οAnode