Title | Data booklet |
---|---|
Course | Structural Chemistry With Application To Chemistry Of The Elements |
Institution | The University of British Columbia |
Pages | 8 |
File Size | 290 KB |
File Type | |
Total Downloads | 95 |
Total Views | 160 |
Data booklet...
Chemistry 12
PERIODIC TABLE OF THE E LEMENTS 1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
1 2
H
He
Hydrogen
Helium
1.0 14 3
4
Li
Be
Silicon
Lithium
Beryllium
28.1
6.9
9.0
Si
4.0
Atomic Number Symbol Name Atomic Mass
5
6
7
8
9
10
B
C
N
O
F
Ne
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
10.8
12.0
14.0
16.0
19.0
20.2
11
12
13
14
15
16
17
18
Na
Mg
Al
Si
P
S
Cl
Ar
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulphur
Chlorine
Argon
23.0
24.3
27.0
28.1
31.0
32.1
35.5
39.9
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
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
39.1
40.1
45.0
47.9
50.9
52.0
54.9
55.8
58.9
58.7
63.5
65.4
69.7
72.6
74.9
79.0
79.9
83.8
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Rubidium
Strontium
Yttrium
Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellur ium
Iodine
Xenon
85.5
87.6
88.9
91.2
92.9
95.9
(98)
101.1
102.9
106.4
107.9
112.4
114.8
118.7
121.8
127.6
126.9
131.3
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
Cesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury
Thallium
Lead
Bismuth
Polonium
Astatine
Radon
132.9
137.3
138.9
178.5
180.9
183.8
186.2
190.2
192.2
195.1
197.0
200.6
204.4
207.2
209.0
(209)
(210)
(222)
109
87
88
89
104
105
106
107
108
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Francium
Radium
Actinium
Ruther fordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
(223)
(226)
(227)
(261)
(262)
(263)
(262)
(265)
(266)
12
Based on mass of C at 12.00. Data Page 1
Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally.
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
140.1
140.9
144.2
(145)
150.4
152.0
157.3
158.9
162.5
164.9
167.3
168.9
173.0
175.0
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Californium
Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
232.0
231.0
238.0
(237)
(244)
(243)
(247)
(247)
(251)
(252)
(257)
(258)
(259)
(262)
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
Element
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)
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 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
Atomic Number 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
Atomic Mass 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+ +
NH4 Ba
2+
Ca
2+
Cr
2+
Cr
3+
Cu
+
2+
Cu
+
H
+
H3O
Fe2+ Fe
3+
2+
Pb
Pb4+
Aluminum
+
Li
Ammonium
Lithium
2+
Magnesium
Mn
2+
Manganese(II), manganous
Mn
4+
Manganese(IV)
Hg2
2+
Mercury(I)*, mercurous
Hg
2+
Mercury(II), mercuric
Mg
Barium Calcium Chromium(II), chromous Chromium(III), chromic
Lead(IV), plumbic
Copper(I)*, cuprous
+
Potassium
+
Silver
+
Sodium
K
Copper(II), cupric
Ag
Hydrogen Hydronium
Na
Iron(II)*, ferrous
Sn2+ Sn
Iron(III), ferric
Tin(IV), stannic
2+
Zinc
Zn
Lead(II), plumbous
Tin(II)*, stannous
4+
Negative Ions (Anions) Br
–
CO32–
Carbonate
ClO3–
Chlorate
–
Chloride
Cl
ClO2– CrO4
2– –
CN
Cr2O72– H2PO4
–
CH3COO
–
F
–
HCO3– HC2O4
–
HSO4
– –
HS
HSO3 – Chemistry 12
Bromide
Chlorite Chromate Cyanide Dichromate Dihydrogen phosphate Ethanoate, acetate
–
Hydroxide
–
Hypochlorite
–
Iodide
OH
ClO I
HPO42–
Monohydrogen phosphate
NO3
–
Nitrate
NO2
–
Nitrite
C2O42– O2– ClO4– MnO4– 3–
Oxalate Oxide** Perchlorate Permanganate Phosphate
Fluoride
PO4
Hydrogen carbonate, bicarbonate
SO42–
Sulphate
2–
Sulphide
2–
Sulphite
Hydrogen oxalate, binoxalate Hydrogen sulphate, bisulphate Hydrogen sulphide, bisulphide
S SO3
–
SCN
Thiocyanate
Hydrogen sulphite, bisulphite
Data Page 3
SOLUBILITY OF C OMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/L at 25°C. Negative Ions (Anions)
+
+
+
Soluble
All
Ammonium ion: NH4 +
Soluble
All
Soluble
All others
Soluble
+
Bromide, Br
–
Iodide, I–
–
–
Hydroxide, OH
Chloride, Cl
–
2–
+
2+
Ag , Pb , Cu
Low Solubility
Soluble
All others +
2+
Phosphate, PO4
Carbonate, CO32– Sulphite, SO32–
Soluble
+
2+
2+
Ag , Ca , Sr , Ba , Pb
2+
+
Alkali ions, H , NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+
Low Solubility Soluble
Low Solubility
All others
+
Alkali ions, H , NH4+, Sr2+
Soluble
Low Solubility
All others
3–
Data Page 4
+
Hydrogen ion: H
Sulphide, S
or
+
All
Sulphate, SO42–
or
+
Alkali ions: Li , Na , K , Rb , Cs , Fr
or
Solubility of Compounds
All
Nitrate, NO3
or
Positive Ions (Cations)
+
Alkali ions, H , NH4 + All others
Soluble
Low Solubility
Chemistry 12
SOLUBILITY P RODUCT C ONSTANTS 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
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
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
–9
–13
Data Page 5
R ELATIVE STRENGTHS OF BRØNSTED- LOWRY ACIDS AND B ASES in aqueous solution at room temperature.
STRONG
Name of Acid
Perchloric Hydriodic Hydrobromic Hydrochloric Nitric Sulphuric Iodic
HIO 3
Hydrogen sulphate ion Phosphoric Hexaaquoiron ion, iron ( III ) ion Citric Nitrous Hydrofluoric Methanoic, formic
H2C 2O 4 H 2SO 3 HSO 4
−
H 3PO 4 Fe( H2 O)6
3+
H 3C 6H 5O 7 HNO 2 HF HCOOH 3+
Cr (H2 O )6
Benzoic
C6 H5 COOH
→ ← → ← → ← → ← → ← → ←
Ka
H+ H+ H+ H+ H+ H+
very large
+ ClO4 − + I− + Br − + Cl− + NO 3 − + HSO 4 − + H + H2 O
very large very large very large very large very large 1.0
H + + IO 3 −
1.7 × 10 − 1
+
H + HC 2O 4 +
H + HSO 3 +
H + SO 4
−
5.9 × 10 − 2
−
1.5 × 10 − 2
2−
+
H + H 2PO 4
1.2 × 10 − 2 7.5 × 10 − 3
−
+ H + Fe( H2 O)5 (OH )2 + +
H + H 2C 6H 5O 7 +
−
−
H + NO 2 → H+ + F− ← → H + + HCOO − ← + 2+ → ← H + Cr( H2 O)5 (OH ) + − → ← H + C H COO 6
5
H 2O
Hydroxide ion
OH −
Ammonia
NH 3
+ − ← H + NH 2
Ethanoic, acetic Dihydrogen citrate ion Hexaaquoaluminum ion, aluminum ion Carbonic (CO2 + H2 O ) Monohydrogen citrate ion Hydrogen sulphite ion Hydrogen sulphide Dihydrogen phosphate ion Boric Ammonium ion Hydrocyanic Phenol Hydrogen carbonate ion Hydrogen peroxide Monohydrogen phosphate ion
Data Page 6
HC 2 O 4
CH 3COOH H 2 C 6 H 5O 7 − Al( H 2O) 6
3+
H2 CO3 HC6 H5 O 7 2
...