Chemistry 12
Data Page 1
39
(226)
(223)
(227)
Actinium
Ac
Yttrium
(261)
Rutherfordium
Rf
Zirconium
Values in parentheses
are the masses of the most
stable or best known isotopes for
elements which do not occur naturally.
Based on mass of C12 at 12.00.
Radium
Francium
104
89
88
138.9
Barium
137.3
Cesium
132.9
Ra
Hafnium
178.5
Lanthanum
56
Ba
55
Cs
87
72
Hf
57
La
87.6
Fr
91.2
88.9
Strontium
85.5
41
91
Pa
Protactinium
231.0
90
Thorium
232.0
140.9
Th
Neodymium
Praseodymium
Cerium
140.1
238.0
Uranium
U
92
144.2
60
Nd
59
Pr
58
Ce
Bohrium
(262)
Seaborgium
Bh
107
186.2
Rhenium
Re
75
(98)
Technetium
Tc
43
54.9
Manganese
Mn
25
28.1
28.1
Silicon
Silicon
Si
Si
14
14
7
(263)
(262)
Dubnium
Sg
106
105
Db
183.8
Tungsten
W
74
95.9
Molybdenum
Mo
42
52.0
Chromium
Cr
24
6
180.9
Tantalum
Ta
73
92.9
Niobium
Nb
40
Zr
Rubidium
Y
38
Sr
37
Rb
50.9
Vanadium
V
23
5
47.9
Titanium
45.0
40.1
Scandium
Calcium
39.1
22
Ti
Potassium
21
4
Sc
20
Ca
24.3
23.0
K
Magnesium
Sodium
3
19
12
Mg
9.0
6.9
11
Beryllium
Lithium
Na
4
Be
3
2
Li
1.0
Hydrogen
H
1
1
9
27
93
(237)
Neptunium
Np
(244)
Plutonium
Pu
94
150.4
Samarium
Promethium
(145)
Sm
62
(266)
Meitnerium
Mt
109
192.2
Iridium
Ir
77
102.9
Rhodium
Rh
45
58.9
Cobalt
Co
Pm
61
(265)
Hassium
Hs
108
190.2
Osmium
Os
76
101.1
Ruthenium
Ru
44
55.8
Iron
Fe
26
Atomic Number
Symbol
Name
Atomic Mass
8
48
Platinum
(243)
Americium
Am
95
152.0
Europium
Eu
63
195.1
(247)
Curium
Cm
96
157.3
Gadolinium
Gd
64
197.0
Gold
Au
79
Pt
78
Silver
107.9
(247)
Berkelium
Bk
97
158.9
Terbium
Tb
65
200.6
Mercury
Hg
80
112.4
Cadmium
Cd
47
Ag
65.4
Zinc
Zn
30
12
63.5
Copper
Cu
29
11
106.4
Palladium
Pd
46
58.7
Nickel
Ni
28
10
PERIODIC TABLE OF THE ELEMENTS
(251)
Californium
Cf
98
162.5
Dysprosium
Dy
66
204.4
Thallium
Tl
81
114.8
Indium
In
49
69.7
Gallium
Ga
31
27.0
Aluminum
Al
13
10.8
Boron
B
5
13
(252)
Einsteinium
Es
99
164.9
Holmium
Ho
67
207.2
Lead
Pb
82
118.7
Tin
Sn
50
72.6
Germanium
Ge
32
28.1
Silicon
Si
14
12.0
Carbon
C
6
14
(257)
Fermium
Fm
100
167.3
Erbium
Er
68
209.0
Bismuth
Bi
83
121.8
Antimony
Sb
51
74.9
Arsenic
As
33
31.0
Phosphorus
P
15
14.0
Nitrogen
N
7
15
(258)
Mendelevium
Md
101
168.9
Thulium
Tm
69
(209)
Polonium
Po
84
127.6
Tellurium
Te
52
79.0
Selenium
Se
34
32.1
Sulphur
S
16
16.0
Oxygen
O
8
16
(259)
Nobelium
No
102
173.0
Ytterbium
Yb
70
(210)
Astatine
At
85
126.9
Iodine
I
53
79.9
Bromine
Br
35
35.5
Chlorine
Cl
17
19.0
Fluorine
F
9
17
(262)
Lawrencium
Lr
103
175.0
Lutetium
Lu
71
(222)
Radon
Rn
86
131.3
Xenon
Xe
54
83.8
Krypton
Kr
36
39.9
Argon
Ar
18
20.2
Neon
Ne
10
4.0
Helium
He
2
18
ATOMIC MASSES OF THE ELEMENTS
Based on mass of C12 at 12.00.
Values in parentheses are the mass number of the most stable or best
known isotopes for elements that do not occur naturally.
Element
Actinium
Aluminum
Americium
Antimony
Argon
Arsenic
Astatine
Barium
Berkelium
Beryllium
Bismuth
Boron
Bromine
Cadmium
Calcium
Californium
Carbon
Cerium
Cesium
Chlorine
Chromium
Cobalt
Copper
Curium
Dubnium
Dysprosium
Einsteinium
Erbium
Europium
Fermium
Fluorine
Francium
Gadolinium
Gallium
Germanium
Gold
Hafnium
Helium
Holmium
Hydrogen
Indium
Iodine
Iridium
Iron
Krypton
Lanthanum
Lawrencium
Lead
Lithium
Lutetium
Magnesium
Manganese
Mendelevium
Data Page 2
Symbol
Atomic
Number
Atomic
Mass
Ac
Al
Am
Sb
Ar
As
At
Ba
Bk
Be
Bi
B
Br
Cd
Ca
Cf
C
Ce
Cs
Cl
Cr
Co
Cu
Cm
Db
Dy
Es
Er
Eu
Fm
F
Fr
Gd
Ga
Ge
Au
Hf
He
Ho
H
In
I
Ir
Fe
Kr
La
Lr
Pb
Li
Lu
Mg
Mn
Md
89
13
95
51
18
33
85
56
97
4
83
5
35
48
20
98
6
58
55
17
24
27
29
96
105
66
99
68
63
100
9
87
64
31
32
79
72
2
67
1
49
53
77
26
36
57
103
82
3
71
12
25
101
(227)
27.0
(243)
121.8
39.9
74.9
(210)
137.3
(247)
9.0
209.0
10.8
79.9
112.4
40.1
(251)
12.0
140.1
132.9
35.5
52.0
58.9
63.5
(247)
(262)
162.5
(252)
167.3
152.0
(257)
19.0
(223)
157.3
69.7
72.6
197.0
178.5
4.0
164.9
1.0
114.8
126.9
192.2
55.8
83.8
138.9
(262)
207.2
6.9
175.0
24.3
54.9
(258)
Element
Mercury
Molybdenum
Neodymium
Neon
Neptunium
Nickel
Niobium
Nitrogen
Nobelium
Osmium
Oxygen
Palladium
Phosphorus
Platinum
Plutonium
Polonium
Potassium
Praseodymium
Promethium
Protactinium
Radium
Radon
Rhenium
Rhodium
Rubidium
Ruthenium
Rutherfordium
Samarium
Scandium
Selenium
Silicon
Silver
Sodium
Strontium
Sulphur
Tantalum
Technetium
Tellurium
Terbium
Thallium
Thorium
Thulium
Tin
Titanium
Tungsten
Uranium
Vanadium
Xenon
Ytterbium
Yttrium
Zinc
Zirconium
Symbol
Atomic
Number
Atomic
Mass
Hg
Mo
Nd
Ne
Np
Ni
Nb
N
No
Os
O
Pd
P
Pt
Pu
Po
K
Pr
Pm
Pa
Ra
Rn
Re
Rh
Rb
Ru
Rf
Sm
Sc
Se
Si
Ag
Na
Sr
S
Ta
Tc
Te
Tb
Tl
Th
Tm
Sn
Ti
W
U
V
Xe
Yb
Y
Zn
Zr
80
42
60
10
93
28
41
7
102
76
8
46
15
78
94
84
19
59
61
91
88
86
75
45
37
44
104
62
21
34
14
47
11
38
16
73
43
52
65
81
90
69
50
22
74
92
23
54
70
39
30
40
200.6
95.9
144.2
20.2
(237)
58.7
92.9
14.0
(259)
190.2
16.0
106.4
31.0
195.1
(244)
(209)
39.1
140.9
(145)
231.0
(226)
(222)
186.2
102.9
85.5
101.1
(261)
150.4
45.0
79.0
28.1
107.9
23.0
87.6
32.1
180.9
(98)
127.6
158.9
204.4
232.0
168.9
118.7
47.9
183.8
238.0
50.9
131.3
173.0
88.9
65.4
91.2
Chemistry 12
NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS
* Aqueous solutions are readily oxidized by air.
** Not stable in aqueous solutions.
Positive Ions
(Cations)
Al3+
Aluminum
Pb4+
NH4+
Ammonium
Li+
Lead(IV), plumbic
Lithium
Ba2+
Barium
Mg2+
Magnesium
Ca2+
Calcium
Mn2+
Manganese(II), manganous
Cr2+
Chromium(II), chromous
Mn4+
Manganese(IV)
Cr3+
Chromium(III), chromic
Hg22+
Mercury(I)*, mercurous
Cu+
Copper(I)*, cuprous
Cu2+
Hg2+
K+
Copper(II), cupric
Mercury(II), mercuric
Potassium
Hydrogen
Ag+
Silver
Hydronium
Na+
Sodium
Fe2+
Iron(II)*, ferrous
Sn2+
Tin(II)*, stannous
Fe3+
Iron(III), ferric
Sn4+
Tin(IV), stannic
Pb2+
Lead(II), plumbous
Zn2+
Zinc
Bromide
OH–
Hydroxide
CO32–
Carbonate
ClO–
Hypochlorite
ClO3–
Chlorate
I–
Cl–
Chloride
HPO42–
ClO2–
Chlorite
NO3–
Nitrate
Chromate
NO2–
Nitrite
H+
H3O+
Negative Ions
(Anions)
Br–
CrO42–
CN–
Cyanide
Cr2O72–
Dichromate
H2PO4–
Dihydrogen phosphate
CH3COO –
F–
HCO3–
Ethanoate, acetate
C2O42–
O2–
ClO4–
MnO4–
Iodide
Monohydrogen phosphate
Oxalate
Oxide**
Perchlorate
Permanganate
Fluoride
PO4 3–
Phosphate
Hydrogen carbonate, bicarbonate
SO42–
Sulphate
S2–
Sulphide
HC2O4–
Hydrogen oxalate, binoxalate
HSO4–
Hydrogen sulphate, bisulphate
SO32–
Sulphite
HS–
Hydrogen sulphide, bisulphide
SCN–
Thiocyanate
HSO3–
Chemistry 12
Hydrogen sulphite, bisulphite
Data Page 3
SOLUBILITY OF COMMON COMPOUNDS IN WATER
The term soluble here means > 0.1 mol/L at 25°C.
or
Solubility of
Compounds
All
Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+
Soluble
All
Hydrogen ion: H+
Soluble
All
Ammonium ion: NH4+
Soluble
Nitrate, NO3–
All
Soluble
All others
Soluble
Chloride, Cl–
–
Bromide, Br
Iodide, I–
2–
or
Positive Ions
(Cations)
Negative Ions
(Anions)
2–
Sulphide, S
Sulphate, SO4
Hydroxide, OH
or
or
–
Phosphate, PO43–
2–
Carbonate, CO3
Sulphite, SO32–
Data Page 4
Ag+, Pb2+, Cu+
All others
Low Solubility
Soluble
Ag+, Ca2+, Sr2+, Ba2+, Pb2+
Alkali ions, H+, NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+
Low Solubility
Soluble
All others
Alkali ions, H+, NH4+, Sr2+
Low Solubility
Soluble
Low Solubility
All others
Alkali ions, H+, NH4+
All others
Soluble
Low Solubility
Chemistry 12
SOLUBILITY PRODUCT CONSTANTS AT 25°C
Chemistry 12
Name
Formula
K sp
Barium carbonate
BaCO3
2.6 10–9
Barium chromate
BaCrO4
1.2 10–10
Barium sulphate
BaSO4
1.1 10–10
Calcium carbonate
CaCO3
5.0 10–9
Calcium oxalate
CaC2O4
2.3 10–9
Calcium sulphate
CaSO4
7.1 10–5
Copper(I) iodide
CuI
1.3 10–12
Copper(II) iodate
Cu(IO3)2
6.9 10–8
Copper(II) sulphide
CuS
6.0 10–37
Iron(II) hydroxide
Fe(OH)2
4.9 10–17
Iron(II) sulphide
FeS
6.0 10–19
Iron(III) hydroxide
Fe(OH)3
2.6 10–39
Lead(II) bromide
PbBr2
6.6 10–6
Lead(II) chloride
PbCl2
1.2 10–5
Lead(II) iodate
Pb(IO3)2
3.7 10–13
Lead(II) iodide
PbI2
8.5 10–9
Lead(II) sulphate
PbSO4
1.8 10–8
Magnesium carbonate
MgCO3
6.8 10–6
Magnesium hydroxide
Mg(OH)2
5.6 10–12
Silver bromate
AgBrO3
5.3 10–5
Silver bromide
AgBr
5.4 10–13
Silver carbonate
Ag2CO3
8.5 10–12
Silver chloride
AgCl
1.8 10–10
Silver chromate
Ag2CrO4
1.1 10–12
Silver iodate
AgIO3
3.2 10–8
Silver iodide
AgI
8.5 10–17
Strontium carbonate
SrCO3
5.6 10–10
Strontium fluoride
SrF2
4.3 10–9
Strontium sulphate
SrSO4
3.4 10–7
Zinc sulphide
ZnS
2.0 10–25
Data Page 5
RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES
in aqueous solution at room temperature.
STRONG
Name of Acid
Iodic
Oxalic
H2C2O4
H 2 SO 3
Hydrogen sulphate ion
HSO 4 −
Phosphoric
H 3 PO 4
Citric
Nitrous
Hydrofluoric
Methanoic, formic
Fe(H 2 O)6 3 +
H 3C 6 H 5O 7
HNO 2
HF
HCOOH
Hexaaquochromium ion, chromium( III ) ion
Cr(H 2 O)6 3 +
Benzoic
C 6 H 5COOH
Hydrogen oxalate ion
Ethanoic, acetic
HC 2 O 4 −
CH 3COOH
Dihydrogen citrate ion
H 2 C 6 H 5O 7 −
Hexaaquoaluminum ion, aluminum ion
Al(H 2 O)6 3 +
Carbonic (CO 2 + H 2 O)
Monohydrogen citrate ion
Hydrogen sulphite ion
Hydrogen sulphide
Dihydrogen phosphate ion
Boric
Ammonium ion
Hydrocyanic
Phenol
Hydrogen carbonate ion
H 2 CO 3
HC 6 H 5O 7 2 −
HSO 3 −
H 2S
H 2 PO 4 −
H 3BO 3
NH 4 +
HCN
C 6 H 5OH
HCO 3 −
→
→
→
→
→
→
→
←
H+
H+
H+
H+
H+
H+
H+
+ ClO 4 −
+ I−
+ Br −
+ Cl −
+ NO 3 −
+ HSO 4 −
+ H2O
−
+
→
← H + IO 3
−
+
→
← H + HC 2 O 4
−
+
→
← H + HSO
6.0 × 10 − 3
7.1 × 10 − 4
+
2+
→
← H + Cr(H 2 O)5 (OH)
+
−
→
← H + C 6 H 5COO
2−
+
→
← H +C O
1.5 × 10 − 4
2
3.5 × 10 − 4
1.8 × 10 − 4
4
6.5 × 10 − 5
6.4 × 10 − 5
+
−
→
← H + CH 3COO
2−
+
→
← H + HC 6 H 5O 7
+
2+
→
← H + Al(H O) (OH)
1.8 × 10 − 5
−
+
→
← H + HCO 3
3−
+
→
← H + C 6 H 5O 7
2−
+
→
← H + SO
4.3 × 10 − 7
2
5
3
−
+
→
← H + HS
2−
+
→
← H + HPO 4
−
+
→
← H + H BO
2
3
1.7 × 10 − 5
1.4 × 10 − 5
4.1 × 10 − 7
1.0 × 10 − 7
9.1 × 10 − 8
6.2 × 10 − 8
7.3 × 10 −10
+
→
← H + NH 3
+
−
→
← H + CN
+
−
→
← H + C 6 H 5O
2−
+
→
← H + CO
5.6 × 10 −10
2.4 × 10 −12
3
← H + + O2 −
NH 3
+
← H + NH 2
4.9 × 10 −10
1.3 × 10 −10
5.6 × 10 −11
2.2 × 10 −13
1.0 × 10 −14
very small
−
very small
STRONG
OH −
Data Page 6
7.5 × 10 − 3
4.6 × 10 − 4
Hydroxide ion
Ammonia
7
1.2 × 10 − 2
+
→
← H + NO 2
+
−
→
← H +F
+
−
→
← H + HCOO
H2O
HPO 4 2 −
1.5 × 10 − 2
6 5
−
Water
Monohydrogen phosphate ion
H2O2
5.9 × 10 − 2
+
→
← H + SO 4
−
+
→
← H + H 2 PO 4
+
2+
→
← H + Fe(H 2 O)5 (OH)
−
+
→
← H +H C H O
2
large
large
large
large
large
large
1.7 × 10 −1
3
2−
−
+
→
← H + HO 2
3−
+
→
← H + PO 4
+
−
→
← H + OH
Hydrogen peroxide
very
very
very
very
very
very
1.0
STRENGTH OF BASE
STRENGTH OF ACID
HIO 3
Sulphurous (SO 2 + H 2 O)
Hexaaquoiron ion, iron( III ) ion
WEAK
HClO 4
HI
HBr
HCl
HNO 3
H 2 SO 4
H 3O +
Ka
Base
WEAK
Perchloric
Hydriodic
Hydrobromic
Hydrochloric
Nitric
Sulphuric
Hydronium Ion
Acid
Chemistry 12
ACID-BASE INDICATORS
Indicator
Chemistry 12
pH Range in Which
Colour Change Occurs
Colour Change
as pH Increases
Methyl violet
0.0 – 1.6
yellow to blue
Thymol blue
1.2 – 2.8
red to yellow
Orange IV
1.4 – 2.8
red to yellow
Methyl orange
3.2 – 4.4
red to yellow
Bromcresol green
3.8 – 5.4
yellow to blue
Methyl red
4.8 – 6.0
red to yellow
Chlorophenol red
5.2 – 6.8
yellow to red
Bromthymol blue
6.0 – 7.6
yellow to blue
Phenol red
6.6 – 8.0
yellow to red
Neutral red
6.8 – 8.0
red to amber
Thymol blue
8.0 – 9.6
yellow to blue
Phenolphthalein
8.2 – 10.0
colourless to pink
Thymolphthalein
9.4 – 10.6
colourless to blue
Alizarin yellow
10.1 – 12.0
yellow to red
Indigo carmine
11.4 – 13.0
blue to yellow
Data Page 7
STANDARD REDUCTION POTENTIALS OF HALF-CELLS
Ionic concentrations are at 1M in water at 25°C.
Oxidizing Agents
F2 (g) + 2 e −
STRONG
+ 2e
−
H 2 O 2 + 2H + + 2e −
MnO 4 − + 8H + + 5e −
Au 3+ + 3e −
BrO 3 − + 6H + + 5e −
ClO 4 − + 8H + + 8e −
Cl 2 (g) + 2 e −
Cr2 O 7
1
2
2−
+ 14H + + 6e −
O 2 (g) + 2 H + + 2 e −
MnO 2 (s) + 4H + + 2 e −
IO 3 − + 6H + + 5e −
Br2 () + 2 e −
AuCl 4 − + 3e −
NO 3 − + 4H + + 3e −
Hg 2 + + 2 e −
1
2
O 2 (g) + 2 H (10
+
−7
M) + 2e −
2 NO 3 − + 4H + + 2 e −
Ag + + e −
Hg 2 2 + + e −
Fe 3+ + e −
O 2 (g) + 2 H + + 2 e −
MnO 4 − + 2 H 2 O + 3e −
I 2 (s) + 2 e −
Cu + + e −
H 2 SO 3 + 4H + + 4e −
Cu 2 + + 2 e −
SO 4 2 − + 4H + + 2 e −
Cu
2+
+e
−
Sn 4 + + 2 e −
S(s) + 2 H + + 2 e −
2H + + 2e −
Pb 2 + + 2 e −
Sn 2 + + 2 e −
Ni 2 + + 2 e −
H 3 PO 4 + 2 H + + 2 e −
Co 2 + + 2 e −
Se(s) + 2 H + + 2 e −
Cr 3+ + e −
2H 2 O + 2e −
Overpotential
Effect
Fe
2+
+ 2e
−
Ag 2 S(s) + 2 e −
Cr 3+ + 3e −
Zn 2 + + 2 e −
Te(s) + 2 H + + 2 e −
2H 2 O + 2e −
Mn 2 + + 2 e −
Al 3+ + 3e −
Mg 2 + + 2 e −
Na + + e −
Ca 2 + + 2 e −
WEAK
Ba 2 + + 2e −
Data Page 8
K+ + e−
Rb + + e −
Cs + + e −
Li + + e −
3+
→
← 2Cr + 7H 2 O
→
← H2O
2+
→
← Mn + 2 H O
2
1
→
← 2 I 2 (s) + 3H 2 O
−
→
2
← Br
→
(
) + 4Cl −
Au
s
←
→
← NO(g) + 2 H 2 O
→
← Hg()
→
← H O
2
→
← N 2 O 4 + 2H 2 O
→
← Ag(s)
→
← Hg()
2+
→
← Fe
→
H
←
2O2
−
→
MnO
←
2 (s) + 4OH
−
→
← 2I
→
← Cu(s)
→
← S(s) + 3H 2 O
→
← Cu(s)
→
← H 2 SO 3 + H 2 O
+
→
← Cu
2+
→
Sn
←
→
← H S(g)
2
→
← H 2 (g)
→
← Pb(s)
→
← Sn(s)
→
← Ni(s)
→
← H 3 PO 3 + H 2 O
→
← Co(s)
+ 2.01
+1.78
+1.51
+1.50
+1.48
+1.39
+1.36
+1.23
+1.23
+1.22
+1.20
+1.09
+1.00
+ 0.96
+ 0.85
+ 0.82
+ 0.80
+ 0.80
+ 0.80
+ 0.77
+ 0.70
+ 0.60
+ 0.54
+ 0.52
+ 0.45
+ 0.34
+ 0.17
+ 0.15
+ 0.15
+ 0.14
+ 0.00
− 0.13
− 0.14
− 0.26
− 0.28
− 0.28
→
← H 2 Se
2+
→
← Cr
→
H
+ 2 OH − (10 −7 M )
←
− 0.40
→
← Fe(s)
2−
→
← 2 Ag(s) + S
→
← Cr(s)
− 0.45
2
→
← Zn(s)
→
← H 2 Te
−
→
← H 2 (g) + 2 OH
→
← Mn(s)
→
← Al(s)
→
← Mg(s)
→
← Na(s)
→
← Ca(s)
→
← Sr(s)
→
← Ba(s)
→
← K(s)
→
← Rb(s)
→
← Cs(s)
→
← Li(s)
Overpotential
Effect
− 0.41
− 0.41
− 0.69
− 0.74
− 0.76
− 0.79
− 0.83
−1.19
−1.66
− 2.37
− 2.71
− 2.87
− 2.89
− 2.91
− 2.93
− 2.98
− 3.03
STRONG
Sr 2 + + 2e −
1
→
← 2 Br2 () + 3H 2 O
−
→
← Cl + 4H 2 O
−
→
← 2Cl
+ 2.87
STRENGTH OF REDUCING AGENT
STRENGTH OF OXIDIZING AGENT
1
2
−
→
← 2F
2−
→
← 2SO 4
→
← 2H 2 O
2+
→
← Mn + 4H 2 O
→
(
Au
s)
←
E° (Volts)
WEAK
S2 O 8
2−
Reducing Agents
− 3.04
Chemistry 12