Download Chemistry Data Booklet Higher and Advanced Higher

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
Published by the Scottish Qualifications Authority
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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
Melting and Boiling Points of Selected Elements
Group
2
Group
3
Group
4
Group
5
Group
6
Group
7
Group
0
1
2
Hydrogen
Helium
Key
—259
—253
Atomic number
—272
—269
Name of element
3
4
Lithium
Beryllium
181
1342
1287
2471*
Melting point/ºC
Boiling point/ºC
5
6
7
8
9
10
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
2075
4000
†3825
—210
—196
—219
—183
—220
—188
—249
—246
11
12
13
14
15
16
17
18
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
Argon
98
883
650
1090
660
2519
1414
3265
44
280
115
445
—101
—34
—189
—186
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
63
759
842
1484
1541
2836
1668
3287
1910
3407
1907
2672
1246
2061
1538
2861
1495
2927
1455
2913
1085
2562
420
907
30
2204
938
2833
*817
†616
221
685
—7
59
—157
—153
42
43
37
38
39
40
41
Rubidium
Strontium
Yttrium
Zirconium
Niobium
39
688
777
1382
1522
3345
1855
4409
2477
4744
Molybdenum Technetium
2623
4639
2157
4265
44
45
46
47
48
49
50
51
52
53
54
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon
2333
4150
1964
3695
1555
2963
962
2162
321
767
157
2072
232
2602
631
1587
449
988
114
184
—112
—108
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Caesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury
Thallium
Lead
Bismuth
Polonium
Astatine
Radon
28
671
727
1897
920
3464
2223
4602
3017
5458
3422
5555
3185
5596
3033
5012
2446
4428
1768
3825
1064
2856
—39
357
304
1473
328
1749
271
1564
254
962
302
—71
—62
* at 28 atmospheres
† sublimes
Page six
Group
1
Covalent Radii of Selected Elements
Group
2
1
Group
3
Key
Hydrogen
Group
4
Group
5
Group
6
Group
7
Atomic number
Name of element
37
Covalent radius/pm
3
4
5
6
7
8
9
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
134
129
90
77
75
73
71
11
12
13
14
15
16
17
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
154
145
130
117
110
102
99
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
196
174
141
132
122
119
116
114
114
113
118
120
120
122
121
117
114
42
43
37
38
39
40
41
Rubidium
Strontium
Yttrium
Zirconium
Niobium
216
191
162
147
133
Molybdenum Technetium
127
—
44
45
46
47
48
49
50
51
52
53
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
122
122
126
136
140
150
140
143
135
133
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
Caesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury
Thallium
Lead
Bismuth
Polonium
Astatine
235
198
169
142
133
131
128
126
124
127
130
141
157
155
151
—
140
Page seven
Group
1
Electron Arrangements of Elements
Group 2
Group 3
Group 4
Group 5
Group 6
Group 7
Group 0
(1)
(18)
Key
1
H
1
Hydrogen
(2)
3
4
Li
Be
2
Atomic number
He
Symbol
(13)
Electron arrangement
Name
(14)
(15)
(16)
2
(17)
Helium
5
6
7
8
9
10
B
C
N
O
F
Ne
2,1
2,2
2,3
2,4
2,5
2,6
2,7
2,8
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
11
12
Na
Mg
Transition Elements
2,8,1
2,8,2
Sodium
Magnesium
(3)
(4)
(5)
(6)
(7)
(8)
(9)
(10)
(11)
(12)
2,8,3
2,8,4
2,8,5
2,8,6
2,8,7
2,8,8
Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
Argon
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
2,8,8,1
2,8,8,2
2,8,9,2
2,8,10,2
2,8,11,2
2,8,13,1
2,8,13,2
2,8,14,2
2,8,15,2
2,8,16,2
2,8,18,1
2,8,18,2
2,8,18,3
2,8,18,4
2,8,18,5
2,8,18,6
2,8,18,7
2,8,18,8
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
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
2,8,18,8,1 2,8,18,8,2
2,8,18,9,2
2,8,18,
10,2
2,8,18,
12,1
2,8,18,13, 2,8,18,13, 2,8,18,15, 2,8,18,16,
1
2
1
1
2,8,18,
18,0
2,8,18,
18,1
2,8,18,
18,2
2,8,18,
18,3
2,8,18,
18,4
2,8,18,
18,5
2,8,18,
18,6
2,8,18,
18,7
2,8,18,
18,8
Rubidium
Strontium
Yttrium
Zirconium
Niobium
Rhodium
Palladium
Silver
Cadmium
Tin
Antimony
Tellurium
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
Caesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
87
88
89
104
105
106
107
108
109
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Francium
Radium
Actinium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
57
58
59
60
61
62
63
64
Pr
Nd
Pm
Sm
Eu
Samarium
Europium
2,8,18,18, 2,8,18,18,
8,1
8,2
2,8,18,32, 2,8,18,32,
18,8,1
18,8,2
2,8,18,18, 2,8,18,32,
9,2
10,2
2,8,18,
32,11,2
Molybdenum Technetium Ruthenium
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
2,8,18,
32,18,1
2,8,18,
32,18,2
110
111
112
Ds
Rg
Cn
Indium
2,8,18,
32,18,3
2,8,18,
32,18,4
2,8,18,
32,18,5
65
66
67
Gd
Tb
Dy
Gadolinium
Terbium
Dysprosium
Gold
Mercury
Thallium
Iodine
Xenon
2,8,18,
32,18,6
2,8,18,
32,18,7
2,8,18,
32,18,8
68
69
70
71
Ho
Er
Tm
Yb
Lu
Holmium
Erbium
Thulium
Ytterbium
Lutetium
Lead
Bismuth
Polonium
Astatine
Radon
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
Lanthanides
La
2,8,18,
18,9,2
Lanthanum
Actinides
Ce
2,8,18,
20,8,2
Cerium
Meitnerium Darmstadtium Roentgenium Copernicium
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
Praseodymium Neodymium Promethium
89
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Actinium
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Fermium
Mendelevium
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
Californium Einsteinium
Page eight
Group 1
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
Proton NMR Spectra Correlation Chart
Note: Approximate chemical shift values of hydrogen atoms in different structural environments relative to tetramethylsilane (TMS) for which δ = 0 ppm
11·0
10·0
9·0
8·0
7·0
6·0
5·0
4·0
3·0
2·0
1·0
0·0
RCH3, R2CH2, R3CH
3·0−2·3
ArCH3, ArCH2R, ArCHR2
O
O
O
CH3C− , RCH2C− , R2CHC−
2·7−2·0
(aldehyde, ketone, acid, ester, amide)
CH3O−, RCH2O−, R2CHO−
R = alkyl group
3·9−3·5
Ar = aryl (aromatic) group
(alcohol, ether)
X =halogen
4·2−2·2
CH3X, RCH2X, R2CHX
2·5−2·0
CH3CN, RCH2CN, R2CHCN
3·0−2·5
CH3N , RCH2N , R2CHN
Page sixteen
2·6−1·6
CH3C C , RCH2C C , R2CHC C
2·8−1·7
CH3C ≡ C−, RCH2C ≡ C−, R2CHC ≡ C−
6·0−4·5
C CH2 , C CH
3·1−1·8
−C ≡ CH
8·0−6·6
ArH
O
RC−H
10·0−9·4
O
ArC−H
O
O
RC−OH, ArC−OH
δ (ppm)
1·5−0·9
10·5−9·7
11·0−10·0
5·0−1·0
ROH
11·0−4·5
ArOH
3·0−1·1
RNH2 , RNH
5·0−3·0
ArNH2, ArNH
O
O
−C−NH2 , −C−NH
9·4−5·0
11·0
10·0
9·0
8·0
7·0
6·0
5·0
4·0
3·0
2·0
1·0
0·0
δ (ppm)
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