PERIODIC TABLE OF THE ELEMETS
1
2
H
He
1.0079
4.0026
3
4
5
6
7
8
9
10
Li
Be
B
C
O
F
e
6.941
9.012
10.811
12.011
14.007
16.00
19.00
20.179
11
12
13
14
15
16
17
18
a
Mg
Al
Si
P
S
Cl
Ar
22.99
24.30
26.98
28.09
30.974
32.06
35.453
39.948
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
i
Cu
Zn
Ga
Ge
As
Se
Br
Kr
39.10
40.08
44.96
47.90
50.94
52.00
54.938
55.85
58.93
58.69
63.55
65.39
69.72
72.59
74.92
78.96
79.90
83.80
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
b
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
85.47
87.62
88.91
91.22
92.91
95.94
(98)
101.1
102.91
106.42
107.87
112.41
114.82
118.71
121.75
127.60
126.91
131.29
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
*La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.91
137.33
138.91
178.49
180.95
183.85
186.21
190.2
192.2
195.08
196.97
200.59
204.38
207.2
208.98
(209)
(210)
(222)
87
88
89
104
105
106
107
108
109
110
111
112
Fr
Ra
(223)
226.02
†
Ac
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
§
227.03
(261)
(262)
(266)
(264)
(277)
(268)
(271)
(272)
(277)
*Lanthanide Series
†
Actinide Series
§ Not yet named
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce
Pr
d
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
140.12
140.91
144.24
(145)
150.4
151.97
157.25
158.93
162.50
164.93
167.26
168.93
173.04
174.97
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Th
Pa
U
p
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
o
Lr
232.04
231.04
238.03
237.05
(244)
(243)
(247)
(247)
(251)
(252)
(257)
(258)
(259)
(262)
2 FCo2+
Au(s)
2 Cl2 H2O(l)
2 BrHg22+
Hg(l)
Ag(s)
2 Hg(l)
Fe2+
2 ICu(s)
Cu(s)
Cu+
Sn2+
H2S(g)
H2(g)
Pb(s)
Sn(s)
Ni(s)
Co(s)
Cd(s)
Cr2+
Fe(s)
Cr(s)
Zn(s)
H2(g) + 2 OHMn(s)
Al(s)
Be(s)
Mg(s)
Na(s)
Ca(s)
Sr(s)
Ba(s)
Rb(s)
K(s)
Cs(s)
Li(s)
Half-Reaction
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
→
E°(V)
2.87
1.82
1.50
1.36
1.23
1.07
0.92
0.85
0.80
0.79
0.77
0.53
0.52
0.34
0.15
0.15
0.14
0.00
-0.13
-0.14
-0.25
-0.28
-0.40
-0.41
-0.44
-0.74
-0.76
-0.83
-1.18
-1.66
-1.70
-2.37
-2.71
-2.87
-2.89
-2.90
-2.92
-2.92
-2.92
-3.05
STADARD REDUCTIO POTETIALS I AQUEOUS SOLUTIO AT 25°C
F2(g) + 2 eCo3+ + eAu3+ + 3 eCl2(g) + 2 eO2(g) + 4 H+ + 4 eBr2(l) + 2 e2Hg2+ + 2 eHg2+ + 2 eAg+ + eHg22+ + 2 eFe3+ + eI2(s) + 2 eCu+ + eCu2+ + 2 eCu2+ + eSn4+ + 2 eS(s) + 2 H+ + 2 e2 H+ + 2 ePb2+ + 2 eSn2+ + 2 eNi2+ + 2 eCo2+ + 2 eCd2+ + 2 eCr3+ + eFe2+ + 2 eCr3+ + 3 eZn2+ + 2 e2 H2O(l) + 2 eMn2+ + 2 eAl3+ + 3 eBe2+ + 2 eMg2+ + 2 eNa+ + eCa2+ + 2 eSr2+ + 2 eBa2+ + 2 eRb+ + eK + + eCs+ + eLi+ + e-
o
f
o
f
o
f
‫ = ܧ‬energy
ν = frequency
p = momentum
λ = wavelength
moles A
total moles
GASES, LIQUIDS, AD SOLUTIOS
ቆܲ +
PV = nRT
݊ଶ ܽ
ቇ ሺܸ − ܾ݊ሻ = ܴ݊ܶ
ܸଶ
߭ = velocity
n = principal quantum number
D=
=
m
V
݉߭ ଶ
3RT
M
ଵ
3
RT
2
ଶ
KE per mole =
M2
M1
[C] c [D] d
[A] a [B]b
q
t
log K =
nE °
0.0592
‫ܧ‬ୡୣ୪୪ = ‫ܧ‬°ୡୣ୪୪ −
I=
Q =
ܴܶ
0.0592
ln ܳ = ‫ܧ‬°ୡୣ୪୪ −
log ܳ @ 25 ℃
݊‫ܨ‬
݊
, where a A + b B → c C + d D
OXIDATIO-REDUCTIO; ELECTROCHEMISTRY
A = abc
π = iMRT
molarity, M = moles solute per liter solution
molality = moles solute per kilogram solvent
∆Tf = iKf × molality
∆Tb = iKb × molality
r1
=
r2
‫ ܧܭ‬per molecule =
3kT
m
P1V1 P2V2
=
T1
T2
m
n=
M
K = ° C + 273
Ptotal = PA + PB + PC + ...
PA = Ptotal × X A , where X A =
Speed of light, c = 3.0 × 108 m s-1
Planck’s constant, h = 6.63 × 10-34 J s
Boltzmann’s constant, k = 1.38 × 10-23 J K-1
Avogadro’s number = 6.022 × 1023 mol-1
Electron charge, e = -1.602 × 10-19 coulomb
1 electron volt per atom = 96.5 kJ mol-1
Equilibrium Constants
Ka (weak acid)
Kb (weak base)
Kw (water)
Kp (gas pressure)
Kc (molar concentrations)
S° = standard entropy
H° = standard enthalpy
G° = standard free energy
E° = standard reduction potential
T = temperature
n = moles
m = mass
q = heat
c = specific heat capacity
Cp = molar heat capacity at constant pressure
Ea = activation energy
k = rate constant
A = frequency factor
Faraday’s constant, F = 96,500 coulombs per mole
of electrons
Gas constant, R = 8.31 J mol-1 K-1
= 0.0821 L atm mol-1 K-1
= 8.31 volt coulomb mol-1 K-1
u rms =
m = mass
ADVACED PLACEMET CHEMISTRY EQUATIOS AD COSTATS
ATOMIC STRUCTURE
c = λν
E = hv
h
λ=
p = mυ
mυ
−2.178 × 10 −18
joule
n2
En =
[OH - ][ HB + ]
[ B]
EQUILIBRIUM
[H + ][A - ]
Ka =
[HA]
Kb =
K w = [OH − ][H + ] = 1.0 × 10 −14 @ 25° C
= Ka × Kb
[A - ]
[ HA]
pK b
Kb
pH = - log [H + ], pOH = - log [OH - ]
14 = pH + pOH
pH = pK a + log
= - log
Ka ,
[HB + ]
pOH = pK b + log
[ B]
= - log
pK a
K p = K c ( RT ) ∆n ,
where ∆n = moles product gas – moles reactant gas
THERMOCHEMISTRY/KIETICS
o
f
∆S ° = ∑ S ° products - ∑ S ° reactants
∆H ° = ∑ ∆H products - ∑ ∆H reactants
∆G ° = ∑ ∆G products - ∑ ∆G reactants
∆G° = ∆H °− T∆S °
= − RT ln K = - 2.303 RT log K
= −݊‫ܧܨ‬°
∆G = ∆G°+ RT ln Q = ∆G° + 2.303 RT log Q
∆H
=
∆T
q = mc∆T
Cp
ln[A] t - ln[A] 0 = - kt
−‫ܧ‬௔ 1
൬ ൰ + ln ‫ܣ‬
ܴ ܶ
1
1
−
= kt
[A] t [A] 0
ln ݇ =
P = pressure
V = volume
T = temperature
n = number of moles
D = density
m = mass
߭= velocity
urms = root-mean-square speed
KE = kinetic energy
r = rate of effusion
M = molar mass
π = osmotic pressure
i = van’t Hoff factor
Kf = molal freezing-point depression constant
Kb = molal boiling-point elevation constant
A = absorbance
a = molar absorptivity
b = path length
c = concentration
Q = reaction quotient
I = current (amperes)
q = charge (coulombs)
t = time (seconds)
E° = standard reduction potential
K = equilibrium constant
Gas constant, R = 8.31 J mol-1 K-1
= 0.0821 L atm mol-1 K-1
= 8.31 volt coulomb mol-1 K-1
Boltzmann’s constant, k = 1.38 × 10-23 J K-1
Kf for H2O = 1.86 K kg mol -1
Kb for H2O = 0.512 K kg mol -1
1 atm = 760 mm Hg
= 760 torr
STP = 0.000°C and 1.000 atm
Faraday’s constant, F = 96,500 coulombs per mole
of electrons