29 Appendix
30 Short end-of-chapter answers
31 Index
List of Tables
1 Chapter 0Table 0.1 Base SI quantities used in chemistry with symbols and units.Table 0.2 Commonly used derived units.Table 0.3 Some common prefixes and their values with quantities and symbols.Table 0.4 Symbols and charges for some common cations and anions.Table 0.5 State symbols commonly used in chemical equations.
2 Chapter 1Table 1.1 Properties of subatomic particles.Table 1.2 The maximum number of electrons in the first four energy levels.Table 1.3 Arrangement of electrons in the first 11 elements of the periodic t...Table 1.4 Electron configurations for the first 36 elements.
3 Chapter 2Table 2.1 The names, molecular formulae, dot‐and‐cross diagrams, and display ...Table 2.2 Approximate strengths of different types of bonds and intermolecula...
4 Chapter 4Table 4.1 A summary of the properties of ionic, covalent, and metallic compou...Table 4.2 Physical properties of the halogens.Table 4.3 Properties of noble gases.
5 Chapter 6Table 6.1 Values of mean bond energies.Table 6.2 Calculation of enthalpy of reaction using mean bond energies.Table 6.3 Standard molar entropy values for selected elements and compounds.Table 6.4 Combinations of possible enthalpy and entropy changes for a reactio...
6 Chapter 7Table 7.1 Summary of the effect of changes in reaction conditions upon the eq...Table 7.2 Some common acids and the ions they form when dissolved in water.Table 7.3 Some common bases and the ions they form when dissolved in water.Table 7.4 Some weak acids and theirKa and pKa values.
7 Chapter 8Table 8.1 Concentration, rate, and time data for the reaction of bromine with...Table 8.2 Some chemical reactions and their related rate expressions and over...Table 8.3 Initial rates data for the reaction 2NO(g) + O2(g) → 2NO2(g).Table 8.4 Kinetics data for the decomposition of NO2 at varying temperatures....
8 Chapter 9Table 9.1 Standard reduction potentials for metal/metal ion half‐cells.Table 9.2 List of some common standard reduction potentials in numerical orde...Table 9.3 Comparison of galvanic and electrolytic cells.
9 Chapter 10Table 10.1 Electron affinity values for Group 7 (17) elements.Table 10.2 The electronic configurations and number of protons for selected e...Table 10.3 Names and charges of monatomic anions.Table 10.4 The bonding, structures, and melting and boiling points of the Per...
10 Chapter 11Table 11.1 Physical properties of Group 1 metals.Table 11.2 Electron configurations of the elements of Group 1.Table 11.3 Physical properties of the Group 2 elements.Table 11.4 Electron configurations of Group 2 elements.Table 11.5 The solubilities of Group 2 metal hydroxides increase down the gro...Table 11.6 Electron configurations of the halogen elements.Table 11.7 Colours of elemental halogens in polar and non‐polar solvents.Table 11.8 Standard reduction potentials of the halogens.Table 11.9 Displacement reactions of halogens.Table 11.10 Oxyanions of chlorine.Table 11.11 Results from tests to identify halide ions.Table 11.12 The electron configurations of Period 4 elements and stable ions....Table 11.13 Maximum stable oxidation states and most common oxidation states ...
11 Chapter 12Table 12.1 Some commonly encountered homologous series and examples. Note: R ...Table 12.2 The names and structures of the first five hydrocarbon chains.Table 12.3 The name, structural formulae, and prefixes of the first 10 hydroc...Table 12.4 The hierarchy of some commonly encountered functional groups.
12 Chapter 14Table 14.1 A comparison of boiling points between alkanes and the correspondi...
13 Chapter 19Table 19.1 Characteristic absorptions of some functional groups commonly enco...Table 19.2 The chemical shifts for different1H environments.Table 19.3 A table summarising the most commonly encountered peak (resonance)...
List of Illustrations
1 Chapter 0Figure 0.1 The shape of a water molecule, H2O.Figure 0.2 (a) 25 cm3 measuring cylinder; (b) 25 cm3 pipette; (c) 50 cm3 bur...Figure 0.3 (a) Cube of volume 1 m3. (b) Flask of volume 1 L.(c) Cube of ...
2 Chapter 1Figure 1.1 Simplified structure of the atom (not to scale).Figure 1.2 (a) General representation of mass number and atomic number for t...Figure 1.3 The standard modern form of the periodic table. Source: Universit...Figure 1.4 The energy levels (EL) in an atom. The integers represent the pri...Figure 1.5 The structure of neon.Figure 1.6 (a) The 1s orbital; (b) the 2s orbital; (c) the 3s orbital.Figure 1.7 (a) The 2px orbital; (b) the 2py orbital; (c) the 2pz orbital.Figure 1.8 (a) The dxy orbital; (b) the dxz orbital; (c) the dyz orbital; (d...Figure 1.9 The relative energies of the orbitals in an atom. Relative energi...Figure 1.10 Electron arrangements in lithium, oxygen, and chlorine. Outer sh...
3 Chapter 2Figure 2.1 (a) Eight hydrogen atoms; (b) four hydrogen molecules.Figure 2.2 Bonding in sodium metal.Figure 2.3 Addition of an electron to a fluorine atom to generate a fluoride...Figure 2.4 Arrangement of electrons in (a) a sodium atom; (b) a sodium ion....Figure 2.5 Bonding in NaCl. Note: only outer‐shell electrons are shown for c...Figure 2.6 The sodium chloride lattice. Source: Based on https://www.chemgui...