Aylward and Findlay's SI Chemical Data E-Text
About the authors iv
Preface iv
Acknowledgements v
Section 1: General: Physical constants, units and symbols
1 The International System of Units (SI) 3
2 SI derived units commonly used in chemistry 3
3 Fundamental constants (revised 2010) 4
4 Common conversion factors 4
5 The Greek alphabet 5
6 Numerical prefixes 5
7 Decimal fractions and multiples 6
Section 2: The elements
8 Ground state electronic configurations of the elements 9
9 Properties of the elements 14
10 Properties and applications of some common radioisotopes
22
11 Electronegativities of the elements (Pauling scale) 24
12 Enthalpies of melting, vaporisation and atomisation of the
elements 25
13 First ionisation enthalpies (Ei1) of the elements 27
14 Successive ionisation enthalpies (Ein) of the elements 29
15 Electron affinities (Eea) of the elements 31
Section 3: Inorganic compounds
16 Properties of elements and inorganic compounds 35
17 Some crystal forms 84
18 Shapes of some molecules and ions 87
19 Bond lengths 88
20 Average bond enthalpies 89
21 Lattice enthalpies of ionic crystals 89
22 Stability constants of complex ions 90
23 Solubility products 91
Section 4: Organic compounds
24 Some important organic functional groups 95
25 Properties of organic compounds 97
26 Properties of amino acids 120
27 Properties of solvents 123
28 Miscibility of solvents 125
29 Boiling temperature elevation and freezing temperature
depression constants 126
30 Critical constants and triple points 127
Section 5: Spectroscopic data
31 The spectral energies 131
32 Infrared absorption frequencies 131
33 NMR chemical shifts 132
34 Chemical shifts and multiplicities of residual protons in
deuterated NMR solvents 132
35 NMR chemical shifts of common solvents in a variety of
deuterated NMR solvents 133
36 Important NMR-active nuclei 137
37 Common singly charged (z = 1) fragments detected by mass
spectrometry 137
Section 6: Properties of acids and bases
38 Dissociation constants of acids and hydrated metal ions
141
39 Aqueous concentrations of common acids 142
40 Common acid-base indicators 143
41 Common buffers 143
42 Buffering ranges of some common biological buffers (0.1 m)
144
Section 7: Properties of aqueous solutions
43 Ionic properties of water 149
44 Molar conductivities of aqueous solutions at 298 K 149
45 Ionic molar conductivities at
infinite dilution at 298 K 149
46 Solubility of gases in water 150
47 Vapour pressure and density of water and mercury at different
temperatures 150
48 Densities of aqueous solutions at 298 K 151
Section 8: Electrochemistry
49 Standard electrode potentials and redox equilibria in aqueous
solution 155
50 Potentials of common reference electrodes at 298 K 159
51 Conversion factors (mV) between common reference electrodes in
acetonitrile 160
Section 9: Appendices
52 Globally Harmonised System of Classification and Labelling of
Chemicals (GHS) 163
53 Interpretation of a material safety data sheet (MSDS) 165
54 Common formulae and definitions 173
References 176
Index 181
Preface iv
Acknowledgements v
Section 1: General: Physical constants, units and symbols
1 The International System of Units (SI) 3
2 SI derived units commonly used in chemistry 3
3 Fundamental constants (revised 2010) 4
4 Common conversion factors 4
5 The Greek alphabet 5
6 Numerical prefixes 5
7 Decimal fractions and multiples 6
Section 2: The elements
8 Ground state electronic configurations of the elements 9
9 Properties of the elements 14
10 Properties and applications of some common radioisotopes
22
11 Electronegativities of the elements (Pauling scale) 24
12 Enthalpies of melting, vaporisation and atomisation of the
elements 25
13 First ionisation enthalpies (Ei1) of the elements 27
14 Successive ionisation enthalpies (Ein) of the elements 29
15 Electron affinities (Eea) of the elements 31
Section 3: Inorganic compounds
16 Properties of elements and inorganic compounds 35
17 Some crystal forms 84
18 Shapes of some molecules and ions 87
19 Bond lengths 88
20 Average bond enthalpies 89
21 Lattice enthalpies of ionic crystals 89
22 Stability constants of complex ions 90
23 Solubility products 91
Section 4: Organic compounds
24 Some important organic functional groups 95
25 Properties of organic compounds 97
26 Properties of amino acids 120
27 Properties of solvents 123
28 Miscibility of solvents 125
29 Boiling temperature elevation and freezing temperature
depression constants 126
30 Critical constants and triple points 127
Section 5: Spectroscopic data
31 The spectral energies 131
32 Infrared absorption frequencies 131
33 NMR chemical shifts 132
34 Chemical shifts and multiplicities of residual protons in
deuterated NMR solvents 132
35 NMR chemical shifts of common solvents in a variety of
deuterated NMR solvents 133
36 Important NMR-active nuclei 137
37 Common singly charged (z = 1) fragments detected by mass
spectrometry 137
Section 6: Properties of acids and bases
38 Dissociation constants of acids and hydrated metal ions
141
39 Aqueous concentrations of common acids 142
40 Common acid-base indicators 143
41 Common buffers 143
42 Buffering ranges of some common biological buffers (0.1 m)
144
Section 7: Properties of aqueous solutions
43 Ionic properties of water 149
44 Molar conductivities of aqueous solutions at 298 K 149
45 Ionic molar conductivities at
infinite dilution at 298 K 149
46 Solubility of gases in water 150
47 Vapour pressure and density of water and mercury at different
temperatures 150
48 Densities of aqueous solutions at 298 K 151
Section 8: Electrochemistry
49 Standard electrode potentials and redox equilibria in aqueous
solution 155
50 Potentials of common reference electrodes at 298 K 159
51 Conversion factors (mV) between common reference electrodes in
acetonitrile 160
Section 9: Appendices
52 Globally Harmonised System of Classification and Labelling of
Chemicals (GHS) 163
53 Interpretation of a material safety data sheet (MSDS) 165
54 Common formulae and definitions 173
References 176
Index 181
Allan Blackman is an Associate Professor of Chemistry in
the Department of Chemistry, University of Otago, Dunedin, New
Zealand. He has a PhD in Physical Inorganic Chemistry, and his
research interests include coordination chemistry and chemical
kinetics. He has 22 years' experience in both teaching and
research, is the co-author of a best-selling Australasian-focused
first-year Chemistry textbook, and has won teaching awards at his
home university. His monthly musings on things chemical can be
found at http://neon.otago.ac.nz/chemistry/magazine/.
Lawrence R. Gahan is a Professor of Chemistry in the
School of Chemistry and Molecular Biosciences, The University of
Queensland, Australia. He has a PhD in Chemistry, has active
research interests in bioinorganic chemistry, and has published
extensively in international journals. Professor Gahan has 30
years' experience in university teaching with various
teaching and learning grants, and local and national awards for his
teaching. In addition, he has been awarded competitive grants to
support his chemistry research.
the Department of Chemistry, University of Otago, Dunedin, New
Zealand. He has a PhD in Physical Inorganic Chemistry, and his
research interests include coordination chemistry and chemical
kinetics. He has 22 years' experience in both teaching and
research, is the co-author of a best-selling Australasian-focused
first-year Chemistry textbook, and has won teaching awards at his
home university. His monthly musings on things chemical can be
found at http://neon.otago.ac.nz/chemistry/magazine/.
Lawrence R. Gahan is a Professor of Chemistry in the
School of Chemistry and Molecular Biosciences, The University of
Queensland, Australia. He has a PhD in Chemistry, has active
research interests in bioinorganic chemistry, and has published
extensively in international journals. Professor Gahan has 30
years' experience in university teaching with various
teaching and learning grants, and local and national awards for his
teaching. In addition, he has been awarded competitive grants to
support his chemistry research.
