Aylward and Findlays SI Chemical Data

SI Chemical Data, 7th edition, is a supplementary text for students in undergraduate chemistry courses and in high school subjects specialising in chemistry. The chemicals included have been chosen specifically to cover those typically studied in these courses. New to this edition The adoption of the Globally Harmonised System of Classification and Labelling of Chemicals (GHS) has necessitated extensive revision of the hazard codes that were elaborately detailed in earlier editions. Now, instead of listing individual hazard codes for each element and chemical, the GHS is explained in detail, along with how to interpret a material safety data sheet (MSDS). This information provides students with the skills to discover and understand the hazards that may be associated with the chemicals they use. In addition to this major change, the order of the tables of data has been rearranged to systematise the sequence of presentation. The values of the fundamental constants have been updated, data have been updated based on the most recent published compendia and, in some cases, data have been presented in different formats to those in previous editions. New tables have been included to provide data and information on: common radioisotopes common amino acids the miscibility of common solvents 1H chemical shifts of residual protons in deuterated NMR solvents 1H and 13C chemical shifts of common solvents common biological buffers the potentials and conversion factors for common reference electrodes.

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

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.