Download Chemistry Data Booklet

Chemistry Data Booklet
Higher and Advanced Higher
For use in National Qualification Courses
Publication date: 2014
Publication code: BB6753
ISBN: 978 1 910180 00 6
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Page two
Contents
Relationships for Higher and Advanced Higher Chemistry . . . . . . . . . . . . . . . . . . . . . . . . . . 4
Names, Symbols, Relative Atomic Masses and Densities . . . . . . . . . . . . . . . . . . . . . . . . . . . 5
Melting and Boiling Points of Selected Elements . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 6
Covalent Radii of Selected Elements . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 7
Electron Arrangements of Elements . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 8
Melting and Boiling Points of Selected Oxides . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 9
Melting and Boiling Points of Selected Chlorides . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 9
Melting and Boiling Points of Selected Organic Compounds . . . . . . . . . . . . . . . . . . . . . . . . . 9
Enthalpies of Formation and Combustion of Selected Substances . . . . . . . . . . . . . . . . . . . 10
Selected Bond and Mean Bond Enthalpies . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 10
Enthalpy of Sublimation of Carbon . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 10
Ionisation Energies and Electronegativities of Selected Elements . . . . . . . . . . . . . . . . . . . 11
Electrochemical Series: Standard Reduction Potentials . . . . . . . . . . . . . . . . . . . . . . . . . . 12
Electrolysis of Water . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 12
Dissociation Constants of Selected Species . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 13
Infra-red Correlation Table . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 14
Spectral Lines and Flame Colours . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 15
Proton NMR Spectra Correlation Chart . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 16
Ionic Radii of Selected Ions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 17
Standard Entropy Values for Selected Substances . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 17
Standard Molar Enthalpies of Atomisation of Selected Elements . . . . . . . . . . . . . . . . . . . . 18
Lattice Enthalpies of Selected Compounds . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 18
Electron Affinities of Selected Elements . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 19
Hydration Enthalpies of Selected Ions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 19
Colour Wheel . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 20
Acid-base Indicators . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 20
Formulae of Selected Ions containing more than one kind of Atom . . . . . . . . . . . . . . . . . . 21
Solubilities of Selected Compounds in Water . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 21
Systeme Internationale Units . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 22
Physical Constants . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 22
Properties of Water . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 22
SI Prefixes and Multiplication Factors . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 22
Conversion Factors . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 22
Page three
Relationships for Higher and Advanced Higher Chemistry
Eh = cm ∆T
% yield =
Actual yield
×100
Theoretical yield
% atom economy =
Mass of desired product(s)
×100
Total mass of reacc tants
n = cV
c1V1 c2V2
=
n1
n2
n=
m
GFM
rate =
∆ quantity
∆t
reaction rate =
% by mass =
1
t
m
×100
GFM
c = fλ
pH + pOH = 14
E = Lhf
 H 3O +   I n − 
K In =
[HI n ]
c
d
C ] [ D]
[
K=
[ A]a [ B ]b
for aA + bB cC + dD
pH = p K In ±1
pH = − log10  H + 
∆ H ° = ∑ ∆ H °f (products) − ∑ ∆ H °f (reactants)
p K a = − log10 K a
∆ S° = ∑ S°(products) − ∑ S°(reactants)
pH = 12 p K a − 12 log10 c
pH = p K a − log10
[acid ]
[salt ]
∆G = ∆H − T ∆S
∆ G° = ∑ ∆ Gf° (products) − ∑ ∆ Gf° (reactants)
∆ G° = ∆ H °− T ∆ S°
KW =  H +  OH − 
pOH = − log10 OH − 
Page four
Names, Symbols, Relative Atomic Masses and Densities
(Relative atomic masses, also known as average atomic masses, have been rounded to the nearest 0·1)
Element
Actinium
Aluminium
Americium
Antimony
Argon
Arsenic
Astatine
Barium
Berkelium
Beryllium
Bismuth
Boron
Bromine
Cadmium
Calcium
Californium
Carbon
Cerium
Caesium
Chlorine
Chromium
Cobalt
Copper
Curium
Dysprosium
Einsteinium
Erbium
Europium
Fluorine
Francium
Gadolinium
Gallium
Germanium
Gold
Hafnium
Helium
Holmium
Hydrogen
Indium
Iodine
Iridium
Iron
Krypton
Lanthanum
Lead
Lithium
Lutetium
Magnesium
Symbol
Ac
Al
Am
Sb
Ar
As
At
Ba
Bk
Be
Bi
B
Br
Cd
Ca
Cf
C
Ce
Cs
Cl
Cr
Co
Cu
Cm
Dy
Es
Er
Eu
F
Fr
Gd
Ga
Ge
Au
Hf
He
Ho
H
In
I
Ir
Fe
Kr
La
Pb
Li
Lu
Mg
Relative
atomic
mass
227·0
27·0
243·1
121·8
39·9
74·9
210·0
137·3
247·1
9·0
209·0
10·8
79·9
112·4
40·1
251·1
12·0
140·1
132·9
35·5
52·0
58·9
63·5
247·1
162·5
252·1
167·3
152·0
19·0
223·0
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
207·2
6·9
175·0
24·3
Density
(g cm-3)
10·1
2·70
13·7
6·68
0·0018
5·78
unknown
3·62
14·8
1·85
9·79
2·47
3·12
8·69
1·54
unknown
*
6·77
1·93
0·0032
7·15
8·86
8·96
13·3
8·55
unknown
9·07
5·24
0·0017
unknown
7·90
5·91
5·32
19·3
13·3
0·0002
8·80
0·00009
7·31
4·95
22·5
7·87
0·0037
6·15
11·3
0·53
9·84
1·74
*The density of carbon as graphite is 2·27 g cm−3
The density of carbon as diamond is 3·51 g cm−3
Element
Symbol
Relative
atomic
mass
Density
(g cm-3)
Manganese
Mercury
Molybdenum
Neodymium
Neon
Neptunium
Nickel
Niobium
Nitrogen
Osmium
Oxygen
Palladium
Phosphorus
Platinum
Plutonium
Polonium
Potassium
Praseodymium
Promethium
Protactinium
Radium
Radon
Rhenium
Rhodium
Rubidium
Ruthenium
Samarium
Scandium
Selenium
Silicon
Silver
Sodium
Strontium
Sulfur
Tantalum
Technetium
Tellurium
Terbium
Thallium
Thorium
Thulium
Tin
Titanium
Tungsten
Uranium
Vanadium
Xenon
Ytterbium
Yttrium
Zinc
Zirconium
Mn
Hg
Mo
Nd
Ne
Np
Ni
Nb
N
Os
O
Pd
P
Pt
Pu
Po
K
Pr
Pm
Pa
Ra
Rn
Re
Rh
Rb
Ru
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
54·9
200·6
96·0
144·2
20·2
237·0
58·7
92·9
14·0
190·2
16·0
106·4
31·0
195·1
244·1
209·0
39·1
140·9
144·9
231·0
226·0
222·0
186·2
102·9
85·5
101·1
150·4
45·0
79·0
28·1
107·9
23·0
87·6
32·1
180·9
97·9
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
7·47
13·5
10·2
7·01
0·0009
20·2
8·90
8·57
0.0013
22·6
0·0014
12·0
1·82
21·5
19·7
9·20
0·89
6·77
7·26
15·4
5·00
0·0097
20·8
12·4
1·53
12·1
7·52
2·99
4·81
2·33
10·5
0·97
2·64
2·09
16·4
11
6·25
8·23
11·8
11·7
9·32
7·26
4·51
19·3
19·1
6·00
0·0059
6·90
4·47
7·14
6·52
Page five
Group
1
1
Hydrogen
Melting and Boiling Points of Selected Elements
Group
0
11
181
1342
Lithium
3
650
1090
Magnesium
12
1287
2471*
Beryllium
4
Scandium
21
40
1668
3287
Titanium
22
Niobium
41
1910
3407
Vanadium
23
42
1907
2672
Chromium
24
43
1246
2061
Manganese
25
Ruthenium
44
1538
2861
Iron
26
1964
3695
Rhodium
45
1495
2927
Cobalt
27
78
1555
2963
Palladium
46
1455
2913
Nickel
28
Gold
79
962
2162
Silver
47
1085
2562
Copper
29
—39
357
Mercury
80
321
767
Cadmium
48
420
907
Zinc
30
304
1473
Thallium
81
157
2072
Indium
49
30
2204
Gallium
31
660
2519
Aluminium
13
2075
4000
Boron
5
328
1749
Lead
82
232
2602
Tin
50
938
2833
Germanium
32
1414
3265
Silicon
14
†3825
Carbon
6
271
1564
Bismuth
83
631
1587
Antimony
51
*817
†616
Arsenic
33
44
280
Phosphorus
15
—210
—196
Nitrogen
7
254
962
Polonium
84
449
988
Tellurium
52
221
685
Selenium
34
115
445
Sulfur
16
—219
—183
Oxygen
8
302
Astatine
85
114
184
Iodine
53
—7
59
Bromine
35
—101
—34
Chlorine
17
—220
—188
Fluorine
9
—71
—62
Radon
86
—112
—108
Xenon
54
—157
—153
Krypton
36
—189
—186
Argon
18
—249
—246
Neon
10
Group
7
Sodium
20
1541
2836
Zirconium
2333
4150
77
Platinum
1064
2856
Group
6
98
883
Calcium
39
2157
4265
76
Iridium
1768
3825
Group
5
19
842
1484
Yttrium
2623
4639
75
Osmium
2446
4428
Group
4
Potassium
38
2477
4744
74
Rhenium
3033
5012
Group
3
2
Helium
63
759
Strontium
1855
4409
73
Tungsten
3185
5596
Group
2
Atomic number
37
1522
3345
72
Tantalum
3422
5555
—272
—269
Rubidium
777
1382
57
Hafnium
3017
5458
Key
Name of element
39
688
56
Lanthanum
2223
4602
—259
—253
55
Barium
920
3464
Melting point/ºC
Caesium
727
1897
Molybdenum Technetium
Boiling point/ºC
28
671
* at 28 atmospheres
† sublimes
Page six
26
Cobalt
27
Nickel
28
Copper
29
Zinc
30
120
Gallium
31
130
Aluminium
13
90
Boron
5
Group
3
Tin
50
122
Germanium
32
117
Silicon
14
77
Carbon
6
Group
4
143
Antimony
51
121
Arsenic
33
110
Phosphorus
15
75
Nitrogen
7
Group
5
135
Tellurium
52
117
Selenium
34
102
Sulfur
16
73
Oxygen
8
Group
6
133
Iodine
53
114
Bromine
35
99
Chlorine
17
71
Fluorine
9
Group
7
Covalent Radii of Selected Elements
4
Iron
120
49
140
Group
2
Beryllium
25
118
48
150
Indium
Group
1
3
129
Manganese
113
47
140
Cadmium
Atomic number
Lithium
12
24
114
46
136
Silver
Key
134
Magnesium
Chromium
114
45
126
Palladium
196
Potassium
19
154
38
174
Calcium
20
39
141
Scandium
21
147
Zirconium
40
132
Titanium
22
133
Niobium
41
122
42
Covalent radius/pm
37
162
Yttrium
37
Hydrogen
1
11
23
116
44
122
Rhodium
Name of element
Sodium
145
Vanadium
119
43
122
Ruthenium
191
Strontium
55
198
Barium
56
169
Lanthanum
57
142
Hafnium
72
133
Tantalum
73
131
Tungsten
74
127
128
Rhenium
75
—
126
Osmium
76
124
Iridium
77
127
Platinum
78
130
Gold
79
141
Mercury
80
157
Thallium
81
155
Lead
82
151
Bismuth
83
—
Polonium
84
140
Astatine
85
Molybdenum Technetium
216
Rubidium
235
Caesium
Page seven
Group 1
(1)
Group 2
Key
Electron Arrangements of Elements
Atomic number
1
H
Symbol
Group 0
Hydrogen
Be
4
(2)
Cr
24
2,8,13,2
Mn
25
2,8,14,2
Fe
26
2,8,15,2
Co
27
2,8,16,2
Ni
28
2,8,18,1
Cu
29
2,8,18,2
Zn
30
(12)
Gallium
2,8,18,3
Ga
31
Aluminium
2,8,3
Al
13
Boron
2,3
B
5
(13)
Germanium
2,8,18,4
Ge
32
Silicon
2,8,4
Si
14
Carbon
2,4
C
6
(14)
Arsenic
2,8,18,5
As
33
Phosphorus
2,8,5
P
15
Nitrogen
2,5
N
7
(15)
Selenium
2,8,18,6
Se
34
Sulfur
2,8,6
S
16
Oxygen
2,6
O
8
(16)
53
Bromine
2,8,18,7
Br
35
Chlorine
2,8,7
Cl
17
Fluorine
2,7
F
9
(17)
54
Krypton
2,8,18,8
Kr
36
Argon
2,8,8
Ar
18
Neon
2,8
Ne
10
Group 7
3
2,2
23
2,8,13,1
Zinc
52
Group 6
Li
Beryllium
V
Copper
51
Group 5
2,1
12
22
2,8,11,2
Nickel
50
Group 4
Lithium
Mg
Ti
Cobalt
49
Group 3
(18)
2
11
2,8,2
21
2,8,10,2
Iron
48
2
He
Na
Magnesium
Sc
Manganese
47
(5)
Name
(6)
(8)
Transition Elements
(7)
Xe
Helium
2,8,1
20
2,8,9,2
Chromium
46
Electron arrangement
Sodium
Ca
Vanadium
45
(11)
19
2,8,8,2
Titanium
Rh
(10)
K
Scandium
44
(9)
2,8,8,1
Calcium
Ru
(4)
1
(3)
Potassium
43
I
Tc
Te
42
2,8,18,
18,8
86
Xenon
2,8,18,
18,7
Iodine
2,8,18,
18,6
Tellurium
Sb
Mo
Sn
41
Nb
In
40
Cd
Y
39
Ag
38
Pd
Sr
Zr
37
2,8,18,
18,4
Antimony
85
Rn
84
At
83
Po
Meitnerium Darmstadtium Roentgenium Copernicium
2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32,
18,9,2
32,10,2
32,11,2
32,12,2
32,13,2
32,14,2
32,15,2
32,17,1
32,18,1
32,18,2
Pb
Bi
Au
2,8,18,
18,5
Rb
2,8,18,
18,3
Tl
2,8,18,
18,2
Hg
2,8,18,
18,1
Rhodium
Pt
2,8,18,
18,0
Ir
77
2,8,18,13, 2,8,18,13, 2,8,18,15, 2,8,18,16,
1
2
1
1
76
2,8,18,
12,1
Os
2,8,18,
10,2
75
2,8,18,9,2
Re
2,8,18,8,1 2,8,18,8,2
74
Tin
Niobium
W
71
Indium
73
Lu
Cadmium
Zirconium
Ta
70
Silver
Yttrium
72
Polonium
Yb
Palladium
Strontium
Hf
69
Molybdenum Technetium Ruthenium
Rubidium
57
Bismuth
Tm
Radon
2,8,18,
32,18,8
68
Ce
Thulium
Ytterbium
Lutetium
Terbium
Erbium
Gadolinium
Holmium
Europium
98
Dysprosium
Samarium
Cf
Praseodymium Neodymium Promethium
97
2,8,18,21, 2,8,18,22, 2,8,18,23, 2,8,18,24, 2,8,18,25, 2,8,18,25, 2,8,18,27, 2,8,18,28, 2,8,18,29, 2,8,18,30, 2,8,18,31, 2,8,18,32, 2,8,18,32,
8,2
8,2
8,2
8,2
8,2
9,2
8,2
8,2
8,2
8,2
8,2
8,2
9,2
Astatine
Er
2,8,18,
32,18,7
67
2,8,18,
32,18,6
Ho
La
Cerium
Bk
Lr
96
103
Cm
No
95
102
Am
101
94
Md
Pu
100
93
Fm
Np
99
U
92
Es
91
90
Pa
Th
Berkelium
89
Curium
Ac
Lanthanum
Lead
66
82
La
Thallium
Dy
2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32,
12,2
13,2
14,2
15,2
17,1
65
81
56
112
Mercury
Tb
80
Ba
111
Gold
64
79
55
110
Platinum
Gd
78
Cs
109
Iridium
63
2,8,18,
32,18,5
108
Osmium
Eu
2,8,18,
32,18,4
107
Rhenium
Hs
62
2,8,18,
32,18,3
106
Tungsten
Hassium
Sm
2,8,18,
32,18,2
105
Tantalum
Bh
61
2,8,18,
32,18,1
104
Hafnium
Bohrium
Pm
2,8,18,
32,11,2
89
Lanthanum
Sg
60
Cn
Db
Seaborgium
Nd
Rg
Rf
Dubnium
59
Ds
Ac
Rutherfordium
Pr
Mt
Actinium
58
2,8,18,18, 2,8,18,32,
9,2
10,2
88
Barium
Ra
2,8,18,18, 2,8,18,18,
8,1
8,2
87
Caesium
Fr
Radium
2,8,18,32, 2,8,18,32,
18,8,1
18,8,2
57
2,8,18,
20,8,2
Lanthanides
Francium
2,8,18,
18,9,2
Actinides
Americium
Mendelevium
Plutonium
Fermium
Neptunium
Protactinium
Uranium
Thorium
Californium Einsteinium
Nobelium
Lawrencium
2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32, 2,8,18,32,
18,9,2
18,10,2
20,9,2
21,9,2
22,9,2
24,8,2
25,8,2
25,9,2
27,8,2
28,8,2
29,8,2
30,8,2
31,8,2
32,8,2
32,9,2
Actinium
Page eight
Melting and Boiling Points of Selected Oxides
Element
hydrogen
Formula
of oxide
H2O
mp/ºC
bp/ºC
0
100
Melting and Boiling Points of Selected Chlorides
Element
Formula of
chloride
mp/ºC
bp/ºC
lithium
LiCl
610
1383
beryllium
BeCl2
405
482
lithium
Li2O
1438
beryllium
BeO
2578
3900
boron
BCl3
—107
boron
B2O3
1860
carbon
CCl4
—23
carbon
CO2
nitrogen
NCl3
—40
nitrogen
N2O4
450
sublimes at
—78·5
—9
fluorine
FCl
—155
—100
fluorine
F2O
—224
—144
sodium
NaCl
801
1465
magnesium
MgCl2
1412
aluminium
Al2Cl6
silicon
SiCl4
714
Sublimes
at 180
—70
phosphorus
PCl3
—93
sulfur
SCl2
—78
potassium
KCl
770
75·5
decomposes
at 59
1680
calcium
CaCl2
775
21
sublimes at
1134
2825
3600
2054
2977
1713
sublimes at
300
—75
2950
—121
2
sodium
Na2O
magnesium
MgO
aluminium
Al2O3
silicon
SiO2
phosphorus
P4O10
sulfur
SO2
chlorine
Cl2O
potassium
K2O
740
calcium
CaO
2614
—10
57·6
1935
2850
Melting and Boiling Points of Selected Organic Compounds
Name of compound
mp/ºC
bp/ºC
Name of compound
methane
—182·5
—162
methanol
ethane
—183
—89
ethanol
—114
78
propane
—188
—42
propan-1-ol
—124
97
butane
—138
—1
propan-2-ol
—88
82
pentane
—130
36
butan-1-ol
—84
118
hexane
—95
69
butan-2-ol
—89
100
heptane
—91
98
methanal
—92
—19
octane
—57
126
ethanal
—123
20
cyclobutane
—91
13
propanal
—81
49
cyclopentane
—93
49
butanal
—97
75
81
propanone
butanone
—95
—86·5
56
79·5
cyclohexane
6.5
ethene
—169
—104
propene
—185
—48
but-1-ene
—185
—6
ethanoic acid
pent-1-ene
—165
30
hex-1-ene
—140
benzene
5·5
methanoic acid
mp/ºC
—97·5
bp/ºC
65
8
101
17
118
propanoic acid
—21
141
63
butanoic acid
—5
164
80
methoxyethane
ethoxyethane
Page nine
—139
—116
7·5
34·5
Enthalpies of Formation and Combustion of Selected Substances
Standard enthalpy of
formation /kJ mol−1
Standard enthalpy of
combustion/kJ mol−1
hydrogen
−
−286
carbon (graphite)
−
−394
sulfur (rhombic)
−
−297
methane
−75
−891
ethane
−84
−1561
propane
−104
−2219
butane
−126
−2878
benzene
49
−3628
ethene
52
−1411
ethyne
227
−1301
methanol
−239
−726
ethanol
−278
−1367
propan-1-ol
−303
−2021
methanoic acid
−425
−255
ethanoic acid
−484
−874
Substance
Selected Bond and Mean Bond Enthalpies
Bond Enthalpies
Mean Bond Enthalpies
Bond
Enthalpy/kJ mol−1
H − H
436
O = O
498
N ≡ N
945
F − F
Mean Enthalpy/
kJ mol−1
Bond
Si − Si
226
C − C
348
159
C = C
612
Cl − Cl
243
838
Br − Br
194
I − I
151
C ≡ C
C C
(aromatic)
H − F
570
H − Cl
432
H − Br
366
H − I
298
}
H − O
463
H − N
388
C − H
412
C − O
360
C = O
743
C − F
484
C − Cl
338
C − Br
276
C − I
238
Enthalpy of Sublimation of Carbon
The energy required to convert 1 mole solid carbon into 1 mole
gaseous carbon atoms is 716 kJ at 298 K (25 ºC). The equation is
C(s) → C(g) ∆H = 716 kJ
Page ten
518
Ionisation Energies and Electronegativities of Selected Elements
Notes: T
he first ionisation energy for an element E refers to the reaction E(g) → E+(g) + e− ; the second ionisation energy
refers to E+(g) → E2+(g) + e− ; etc.
hydrogen
helium
H
He
1312
2372
—
5251
—
—
—
—
Electronegativity
(Pauling scale)
2·2
—
lithium
beryllium
boron
carbon
nitrogen
oxygen
fluorine
neon
Li
Be
B
C
N
O
F
Ne
520
900
801
1086
1402
1314
1681
2081
7298
1757
2427
2353
2856
3389
3374
3952
11815
14849
3660
4620
4578
5300
6050
6122
—
21007
25026
6223
7475
7469
8408
9371
1·0
1·5
2·0
2·5
3·0
3·5
4·0
—
sodium
magnesium
aluminium
silicon
phosphorus
sulfur
chlorine
argon
Na
Mg
Al
Si
P
S
Cl
Ar
496
738
578
787
1012
1000
1251
1521
4562
1451
1817
1577
1907
2252
2298
2666
6910
7733
2745
3232
2914
3357
3822
3931
9543
10543
11577
4356
4964
4556
5159
5771
0·9
1·2
1·5
1·9
2·2
2·5
3·0
—
potassium
calcium
scandium
titanium
vanadium
chromium
manganese
iron
cobalt
nickel
copper
zinc
gallium
germanium
arsenic
bromine
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Br
419
590
633
659
651
653
717
762
760
737
745
906
579
762
944
1140
3052
1145
1235
1310
1410
1591
1509
1562
1648
1753
1958
1733
1979
1537
1794
2083
4420
4912
2389
2653
2828
2987
3248
2957
3232
3395
3555
3833
2965
3302
2735
3473
5877
6491
7091
4175
4507
4743
4940
5287
4950
5297
5536
5731
6102
4411
4837
4564
0·8
1·0
1·3
1·5
1·6
1·6
1·5
1·8
1·8
1·9
1·9
1·6
1·8
2·0
2·2
2·8
rubidium
strontium
silver
tin
antimony
iodine
Rb
Sr
Ag
Sn
Sb
I
403
549
731
709
831
1008
2633
1064
2072
1412
1605
1846
3859
4138
3361
2943
2441
3184
5075
5500
—
3930
4260
—
0·8
1·0
1·9
1·8
2·1
2·6
caesium
barium
gold
lead
Cs
Ba
Au
Pb
376
503
890
716
2234
965
1949
1450
—
—
—
3081
—
—
—
4083
0·8
0·9
2·4
1·8
Element
Symbol
Ionisation Energies/kJ mol—1
First
Second
Third
Fourth
Page eleven
Electrochemical Series: Standard Reduction Potentials
Note: The data given below are reduction potentials applicable to standard state conditions.
Reaction
+
Eº/V
Li (aq) + e
−

Li(s)
−3·04
+
−

Cs(s)
−3·03
+
−

Rb(s)
−2·98

K(s)
−2·93

Sr(s)
−2·90

Ca(s)
−2·87

Na(s)
−2·71

Mg(s)
−2·37

Al(s)
Cs (aq) + e
Rb (aq) + e
+
K (aq) + e
−
2+
Sr (aq) + 2e
−
2+
Ca (aq) + 2e
+
Na (aq) + e
−
−
2+
Mg (aq) + 2e
−
Al3+(aq) + 3e−
−
−1·66
−

H2(g) + 2OH (aq)
−0·83
2+
−

Zn(s)
−0·76
3+
−

Cr(s)
−0·74
2+
−

Fe(s)
−0·45
2+
−

Ni(s)
−0·26
2+
−

Sn(s)
−0·14
2+
−

Pb(s)
−0·13
3+
−

Fe(s)
−0·04

H2(g)
0·00
2H2O() + 2e
Zn (aq) + 2e
Cr (aq) + 3e
Fe (aq) + 2e
Ni (aq) + 2e
Sn (aq) + 2e
Pb (aq) + 2e
Fe (aq) + 3e
+
−
4+
−
2H (aq) + 2e
Sn (aq) + 2e
2+
Cu (aq) + e

−
2−
+
SO4 (aq) + 2H (aq) + 2e
−
Cu2+(aq) + 2e−
O2(g) + 2H2O() + 4e
I2(s) + 2e
−
−
3+
Fe (aq) + e
+
Ag (aq) + e
−
−
2+
Hg (aq) + 2e
Br2() + 2e
−
−
+
O2(g) + 4H (aq) + 4e
2−
−
+
Cr2O7 (aq) + 14H (aq) + 6e
Cl2(g) + 2e
−
−
+
MnO4 (aq) + 8H (aq) + 5e
F2(g) + 2e
−
−
−
2+
0·15
+
Sn (aq)

Cu (aq)
0·15

2−
SO3 (aq) + H2O()
0·17

Cu(s)
0·34

−
0·40
4OH (aq)
−

2I (aq)
0·54

2+
Fe (aq)
0·77

Ag(s)
0·80

Hg()
0·85

−
2Br (aq)
1·07

2H2O()
1·23

3+
1·36

−
2Cl (aq)
1·36

2+
1·51

2Cr (aq) + 7H2O()
Mn (aq) + 4H2O()
−
2F (aq)
Electrolysis of Water
Reduction reactions at the negative electrode
2H2O() + 2e− → H2(g) + 2OH−(aq)
2H+(aq) + 2e− → H2(g)
Oxidation reactions at the positive electrode
2H2O() → O2(g) + 4H+(aq) + 4e−
4OH−(aq) → 2H2O() + O2(g) + 4e−
Page twelve
2·87
Dissociation Constants of Selected Species
Equilibrium in aqueous solution
methanoic acid
ethanoic acid
propanoic acid
butanoic acid
pKa
Ka
 H+ + HCOO−
HCOOH
+
CH3COOH
−
 H + CH3COO
CH3CH2COOH
CH3(CH2)2COOH
+
−
 H + CH3CH2COO
+
−
 H + CH3(CH2)2COO
+
−
1·8 × 10−4
3·75
1·7 × 10
−5
4·76
1·3 × 10
−5
4·87
1·5 × 10
−5
4·83
−5
4·20
benzoic acid
C6H5COOH
 H + C6H5COO
6·3 × 10
phenol
C6H5OH
 H+ + C6H5O−
1·0 × 10−10
9·99
hydrofluoric acid
HF
 H+ + F −
6·8 × 10−4
3·17
boric acid
H3BO3
 H+ + H2BO3−
5·4 × 10−10
9·27
hydrocyanic acid
HCN
 H+ + CN−
6·2 × 10−10
9·21
carbonic acid
H2O + CO2
 H+ + HCO3−
4·5 × 10−7
6·35
hydrogencarbonate ion
HCO3−
 H+ + CO32−
4·7 × 10−11
10·33
sulfurous acid
H2SO3
 H+ + HSO3−
1·4 × 10−2
1·85
hydrogensulfite ion
HSO3−
 H+ + SO32−
6·3 × 10−8
7·19
hydrogen sulfide
H2S
 H+ + HS−
8·9 × 10−8
7·05
hydrogensulfide ion
HS−
 H+ + S2−
2·73 × 10−20
phosphoric acid
H3PO4
 H+ + H2PO4−
6·9 × 10−3
2·16
dihydrogenphosphate ion
H2PO4−
 H+ + HPO42−
6·2 × 10−8
7·21
hydrogenphosphate ion
HPO42−
 H+ + PO43−
4·8 × 10−13
12·32
ammonium ion
NH4+
 H+ + NH3
5·8 × 10−10
9·24
methylammonium ion
CH3NH3+
 H+ + CH3NH2
2·2 × 10−11
10·66
phenylammonium ion
C6H5NH3+
 H+ + C6H5NH2
1·3 × 10−5
4·87
Page thirteen
19·00
Infra-red Correlation Table
Wave number range/cm−1 Type of compound
Infra-red absorption due to
3570−3200
alcohols and phenols
hydrogen bonded O − H stretch
3650−3590
alcohols and phenols
not hydrogen bonded O − H stretch
3500−3300
amine, not hydrogen bonded
N − H stretch
3300
alkyne
C − H stretch in C ≡ C − H
3095−3010
alkene
C − H stretch in C = C − H
3100−3000
benzene ring
C − H stretch
2962−2853
alkane
C − H stretch
2900−2820
aldehyde
C − H stretch in −CHO
2775−2700
aldehyde
C − H stretch in −CHO
3500−2500
carboxylic acid
hydrogen bonded O − H stretch in −COOH
2260−2215
nitriles
C ≡ N stretch
2260−2100
alkynes
C ≡ C stretch
1750−1735
ester
C = O stretch
1740−1720
aldehyde
C = O stretch
1730−1717
aromatic ester
C = O stretch
1725−1700
caboxylic acid
C = O stretch
1700−1680
aromatic and alkyl ketones
aromatic carboxylic acid
1680−1620
alkene
C = C stretch
1600,1580,1500 and 1450
benzene ring
C
1485−1340
alkane
C − H bend
1275−1200
aromatic ether
C − O stretch
1150−1070
alkyl ether
C − O stretch
}
Page fourteen
C = O stretch
C (aromatic) stretch
Spectral Lines and Flame Colours
Gas Discharge Lamps
Element
hydrogen
(Balmer series)
helium
Wavelength/nm
Colour
656
red
486
blue-green
434
blue-green
410
violet
397
ultra-violet
389
ultra-violet
706
red
667
red
588
orange-yellow
Metal Vapour Lamps
Element
cadmium
mercury
sodium
Wavelength/nm
Colour
644
red
509
green
480
blue
579
577
}
yellow doublet
546
green
436
blue-violet
405
violet
310
ultra-violet
589·0
589·6
}
orange-yellow
doublet
Flame Colours
Note: The data refers to prominent spectral lines.
Element
Wavelength/nm
Colour
barium
554
green
calcium
620
orange-red
copper
325
blue-green
lithium
671
crimson
potassium
405
lilac
sodium
589
orange-yellow
strontium
650
red
Page fifteen
R2CHC ≡ C−
10·0
10·0−9·4
10·5−9·7
10·0
11·0−10·0
11·0
9·0
9·0
Proton NMR Spectra Correlation Chart
8·0
7·0
8·0−6·6
7·0
9·4−5·0
11·0−4·5
8·0
6·0
6·0
5·0
6·0−4·5
5·0
4·0
5·0−3·0
3·0
3·0−2·3
2·0
2·7−2·0
2·5−2·0
5·0−1·0
3·0
2·0
1·0
1·0
1·5−0·9
3·0−1·1
3·1−1·8
2·8−1·7
2·6−1·6
3·0−2·5
4·2−2·2
3·9−3·5
4·0
0·0
0·0
δ (ppm)
X =halogen
Ar = aryl (aromatic) group
R = alkyl group
δ (ppm)
Note: Approximate chemical shift values of hydrogen atoms in different structural environments relative to tetramethylsilane (TMS) for which δ = 0 ppm
RCH3, R2CH2, R3CH
ArCH3, ArCH2R, ArCHR2
O
O
O
CH3C− , RCH2C− , R2CHC−
(aldehyde, ketone, acid, ester, amide)
CH3O−, RCH2O−, R2CHO−
(alcohol, ether)
CH3X, RCH2X, R2CHX
CH3CN, RCH2CN, R2CHCN
CH3N , RCH2N , R2CHN
RCH2C ≡ C−,
CH3C C , RCH2C C , R2CHC C
CH3C ≡ C−,
C CH2 , C CH
−C ≡ CH
ArH
O
RC−H
O
ArC−H
O
O
RC−OH, ArC−OH
ROH
ArOH
RNH2 , RNH
ArNH2, ArNH
O
O
−C−NH2 , −C−NH
11·0
Page sixteen
Ionic Radii of Selected Ions
Ion
Radius/pm
H−
208
+
76
Be2+
27
N3−
132
O2−
140
F−
133
Na+
102
Mg2+
72
Al3+
54
P3−
198
S2−
184
Cl−
181
K+
138
Ca2+
100
Ti3+
67
V3+
64
Cr2+
73
Cr3+
62
Mn2+
83
Fe2+
61
Fe3+
55
Co2+
65
Co3+
55
Li
Standard Entropy Values for Selected Substances
Substance
Standard Entropy
/J K−1 mol−1
H2(g)
131
He(g)
126
Li(s)
29
B(s)
5·9
C(s) (graphite)
5·7
C(s) (diamond)
2·4
N2(g)
192
O2(g)
205
F2(g)
203
Na(s)
51
Mg(s)
33
Al(s)
28
Si(s)
19
Cl2(g)
223
K(s)
65
Ca(s)
42
Fe(s)
27
Ni(s)
30
Cu(s)
33
Br2()
152
Ag(s)
43
I2(s)
116
Cs(s)
85
2+
69
Ba(s)
63
Cu
+
60
Au(s)
47
Cu
2+
73
Hg()
76
2+
74
H2O()
70
H2O(g)
189
Ni
Zn
−
196
+
152
CO2(g)
214
2+
126
MgO(s)
27
+
115
Al2O3(s)
51
2+
112
SO2(g)
248
Br
Rb
Sr
Ag
Sn
I
−
220
CaO(s)
38
+
174
BaO(s)
72
2+
135
NaCl(s)
72
2+
102
CaCl2(s)
108
Pb2+
120
CsCl(s)
99
Cs
Ba
Hg
Page seventeen
Standard Molar Enthalpies of Atomisation
of Selected Elements
−1
Lattice Enthalpies of Selected Compounds
Compound
Lattice Enthalpy/kJ mol−1
Element
∆Hº/kJ mol
Li2O
−2799
H
218
BeO
−4514
Li
159
Na2O
−2481
Be
326
MgO
−3795
B
565
Al2O3
−15916
C
716
K2O
−2238
N
472
CaO
−3414
O
249
FeO
−3795
F
79
CoO
−3837
Na
107
NiO
−3908
Mg
147
CuO
−4135
Al
330
ZnO
−4142
Si
450
SrO
−3217
P
317
Ag2O
−3002
S
277
BaO
−3029
Cl
121
LiCl
−834
K
88
NaCl
−769
Ca
178
MgCl2
−2477
Sc
378
KCl
Ti
473
CaCl2
−2268
V
515
CoCl2
−2707
Cr
397
NiCl2
−2753
Mn
283
CuCl
−992
Fe
414
CuCl2
−2774
Co
427
SrCl2
−2142
Ni
430
AgCl
−910
Cu
337
BaCl2
−2046
Zn
130
LiF
−1030
Br
112
NaF
−910
Rb
81
MgF2
−2926
Sr
163
KF
Ag
285
CaF2
−2640
Sn
301
NiF2
−3098
I
107
SrF2
−2476
Cs
77
AgF
−953
Ba
178
BaF2
−2347
MgS
−3406
CaS
−3002
BaS
−2713
NiS
−3528
ZnS
−3692
LiBr
−730
NaBr
−732
KBr
−671
Page eighteen
−701
−808
NiBr2
−2729
CuBr2
−2715
AgBr
−897
Electron Affinities of Selected Elements
Element
H
O
(O−)
F
S
(S−)
Cl
Br
I
Electron Affinity/
kJ mol−1
−72
−141
+844
−328
−201
+456
−349
−324
−295
The electron affinity for an element E refers to the reaction E(g) + e− → E−(g).
The second electron affinity refers to the reaction E−(g) + e− → E2−(g).
Hydration Enthalpies of Selected Ions
Ion
Li+
Na+
K+
Mg2+
Al3+
Ca2+
Fe2+
Fe3+
Cu2+
Zn2+
Rb+
Sr2+
Ag+
Cs+
Ba2+
OH−
F−
Cl−
Br−
I−
Hydration Enthalpy/kJ mol−1
−520
−405
−321
−1920
−4690
−1650
−1950
−4430
−2100
−2050
−300
−1480
−446
−277
−1360
−460
−506
−364
−337
−296
The hydration enthalpy for the ion of an element E refers to the changes represented by
En+(g) → En+(aq) and En−(g) → En−(aq).
Page nineteen
Colour Wheel
orange
600−640 nm
red
640−700 nm
yellow
560−600 nm
violet
400−450 nm
green
480−560 nm
blue
450−480 nm
Acid-base Indicators
Acid-base indicator
bromophenol blue
pH range
3·0−4·6
methyl orange
3·2−4·4
methyl red
4·8−6·0
phenolphthalein
8·2−10·0
bromocresol green
3·8−5·4
bromocresol purple
5·2−6·8
bromothymol blue
6·0−7·6
cresol red
0·0−1·0; 7·0−8·8
p−nitrophenol
5·4−6·6
phenol red
6·6−8·0
thymol blue
1·2−2·8; 8·0−9·6
thymolphthalein
9·4−10·6
screened methyl orange
2·9−4·4
azolitmin (litmus)
4·5−8·3
Page twenty
Formulae of Selected Ions containing more than one kind of Atom
one positive
one negative
two negative
Ion
Ion
Ion
ammonium
Formula
NH4+
Formula
CH3COO−
ethanoate
chromate
−
dichromate
−
sulfate
hydrogencarbonate HCO3
hydrogensulfate
hydrogensulfite
HSO4
HSO3
OH−
hydroxide
nitrate
NO3
permanganate
−
Formula
CO 32−
carbonate
−
three negative
Ion
Formula
phosphate
PO43−
sulfate
oxide
hydroxide
CrO4
2−
Cr2O 7 2−
SO42−
SO 32−
sulfite
S 2O32−
thiosulfate
MnO4−
Solubilities of Selected Compounds in Water
The table shows how some compounds behave in cold water
vs
means very soluble (a solubility greater than 10 g l−1)
s
means soluble
(a solubility of between 1 and 10 g l−1)
i
means insoluble
(a solubility of less than 1 g l−1)
−
no data
bromide carbonate chloride iodide nitrate phosphate
aluminium
vs
−
vs
vs
vs
i
vs
i
i
ammonium
vs
vs
vs
vs
vs
vs
vs
−
−
barium
vs
i
vs
vs
vs
i
i
vs
vs
calcium
vs
i
vs
vs
vs
i
s
s
s
copper(II)
vs
i
vs
−
vs
i
vs
i
i
iron(II)
vs
i
vs
vs
vs
i
vs
i
i
iron(III)
vs
−
vs
−
vs
i
vs
i
i
lead(II)
s
i
s
i
vs
i
i
i
i
lithium
vs
vs
vs
vs
vs
i
vs
vs
vs
magnesium
vs
i
vs
vs
vs
i
vs
i
i
nickel
vs
i
vs
vs
vs
i
vs
i
i
potassium
vs
vs
vs
vs
vs
vs
vs
vs
vs
i
i
i
i
vs
i
s
i
−
sodium
vs
vs
vs
vs
vs
vs
vs
vs
vs
tin(II)
vs
i
vs
s
−
i
vs
i
i
zinc
vs
i
vs
vs
vs
i
vs
i
i
silver
Note: Some of the compounds in the table hydrolyse significantly in water.
Page twenty-one
Systeme Internationale (SI) Units
Quantity
Name of Unit
Symbol
length
metre
m
mass
kilogram
kg
time
second
s
electric current
ampere
A
temperature
degree celsius
ºC
energy
joule
J
electric charge
coulomb
C
electric potential difference
volt
V
amount of substance
mole
mol
Physical Constants
Quantity
Symbol
Value
−
1·60 × 10−19 C
charge on electron
e
Avogadro constant
L
6·02 × 1023 mol−1
Faraday constant
F
9·65 × 104 C mol−1
Planck constant
h
6·63 × 10−34 J s
speed of light in vacuum
c
3·00 × 108 m s−1
Properties of Water
Quantity
Value
specific heat capacity of liquid water
4·18 kJ kg−1 ºC−1
ionic product of water
10−14 at 24 ºC
SI Prefixes and Multiplication Factors
SI Prefix
Symbol
Multiplication
tera
T
1012
giga
G
109
mega
M
106
kilo
k
103
deci
d
10−1
centi
c
10−2
milli
m
10−3
micro
μ
10−6
nano
n
10−9
pico
p
10−12
Conversion Factors
For Volume
For Thermodynamic Temperature
3
3
1 litre = 1 dm = 1000 cm
0 ºC = 273 K
1000 litres = 1000 dm3 = 1 m3
Page twenty-two