Efnisyfirlit

• Contents
• Syllabus roadmap
• Authors’ introduction to the third edition
• Introduction to ‘Skills in the study of chemistry’
• Structure
  • Structure 1: Models of the particulate nature of matter
    • Structure 1.1: Introduction to the particulate nature of matter
      • Structure 1.1.1 – Elements, compounds and mixtures
      • Structure 1.1.2 – The kinetic molecular theory
      • Structure 1.1.3 – Kinetic energy and temperature
    • Structure 1.2: The nuclear atom
      • Structure 1.2.1 – The atomic model
      • Structure 1.2.2 – Isotopes
      • Structure 1.2.3 – Mass spectra
    • Structure 1.3: Electron confi gurations
      • Structure 1.3.1 and 1.3.2 – Emission spectra
      • Structure 1.3.3, 1.3.4 and 1.3.5 – Electron configuration
      • Structure 1.3.6 and 1.3.7 – Ionization energies
    • Structure 1.4: Counting particles by mass: The mole
      • Structure 1.4.1 – The mole as the unit of amount
      • Structure 1.4.2 – Relative atomic mass andrelative formula mass
      • Structure 1.4.3 – Molar mass
      • Structure 1.4.4 – Empirical and molecular formulas
      • Structure 1.4.5 – Molar concentration
      • Structure 1.4.6 – Avogadro’s law
    • Structure 1.5: Ideal gases
      • Structure 1.5.1 – The ideal gas model
      • Structure 1.5.2 – Real gases
      • Structure 1.5.3 and 1.5.4 – The ideal gas laws
  • Structure 2: Models of bonding and structure
    • Structure 2.1: The ionic model
      • Structure 2.1.1 and 2.1.2 – The ionic bond
      • Structure 2.1.3 – Ionic structures and properties
    • Structure 2.2: The covalent model
      • Structure 2.2.1 – Covalent bonding, the octet rule and Lewis formulas
      • Structure 2.2.2 – Single, double and triple covalent bonds
      • Structure 2.2.3 – Coordination bonds
      • Structure 2.2.4 – The Valence Shell Electron Pair Repulsion (VSEPR) model
      • Structure 2.2.5 – Bond polarity
      • Structure 2.2.6 – Molecular polarity
      • Structure 2.2.7 – Covalent network structures
      • Structure 2.2.8 and 2.2.9 – Intermolecular forces
      • Structure 2.2.10 – Intermolecular forces and chromatography
      • Structure 2.2.11 – Resonance structures
      • Structure 2.2.12 – Benzene
      • Structure 2.2.13 – Molecules with an expanded octet
      • Structure 2.2.14 – Formal charge
      • Structure 2.2.15 – Sigma and pi bonds
      • Structure 2.2.16 – Hybridization
    • Structure 2.3: The metallic model
      • Structure 2.3.1 and 2.3.2 – The metallic bond
      • Structure 2.3.3 – Transition elements
    • Structure 2.4: From models to materials
      • Structure 2.4.1 – The bonding triangle
      • Structure 2.4.2 – Application of the bonding triangle
      • Structure 2.4.3 – Alloys
      • Structure 2.4.4 – Polymers
      • Structure 2.4.5 – Addition polymers
      • Structure 2.4.6 – Condensation polymers
  • Structure 3: Classification of matter
    • Structure 3.1 :The periodic table: Classification of elements
      • Structure 3.1.1 – Periods, groups and blocks
      • Structure 3.1.2 – Periodicity and electron configuration
      • Structure 3.1.3 – Periodicity in properties of elements
      • Structure 3.1.4 – Periodicity in reactivity
      • Structure 3.1.5 – Metal and non-metal oxides
      • Structure 3.1.6 – Oxidation states
      • Structure 3.1.7 – Discontinuities in patterns of first ionization energy
      • Structure 3.1.8 – Characteristic properties of transition elements
      • Structure 3.1.9 – Variable oxidation states
      • Structure 3.1.10 – Coloured complexes
    • Structure 3.2: Functional groups: Classification of organic compounds
      • Structure 3.2.1 – Structural representations of organic compounds
      • Structure 3.2.2 – Functional groups and classes of compounds
      • Structure 3.2.3 and 3.2.4 – Homologous series
      • Structure 3.2.5 – IUPAC nomenclature
      • Structure 3.2.6 – Structural isomers
      • Structure 3.2.7 – Stereoisomers
      • Structure 3.2.8 – Mass spectrometry
      • Structure 3.2.9 – Infrared spectroscopy
      • Structure 3.2.10 and 3.2.11 – Nuclear magnetic resonance spectroscopy
      • Structure 3.2.12 – Combining analytical techniques
• Reactivity
  • Reactivity 1: What drives chemical reactions?
    • Reactivity 1.1: Measuring enthalpy changes
      • Reactivity 1.1.1 – Chemical reactions involve heat transfers
      • Reactivity 1.1.2 – Endothermic and exothermic reactions
      • Reactivity 1.1.3 – Energetic stability and the direction of change
      • Reactivity 1.1.4 – Measuring enthalpy changes
    • Reactivity 1.2: Energy cycles in reactions
      • Reactivity 1.2.1 – Bond enthalpy
      • Reactivity 1.2.2 – Hess’s law
      • Reactivity 1.2.3 – Standard enthalpy changes of combustion and formation
      • Reactivity 1.2.4 – Calculating enthalpy changes
      • Reactivity 1.2.5 – Born–Haber cycles
    • Reactivity 1.3: Energy from fuels
      • Reactivity 1.3.1 – Combustion reactions
      • Reactivity 1.3.2 – Incomplete combustion of organic compounds
      • Reactivity 1.3.3 – Fossil fuels
      • Reactivity 1.3.4 – Biofuels
      • Reactivity 1.3.5 – Fuel cells
    • Reactivity 1.4: Entropy and spontaneity
      • Reactivity 1.4.1 – Entropy
      • Reactivity 1.4.2 – Gibbs energy
      • Reactivity 1.4.3 – ΔG and spontaneity
      • Reactivity 1.4.4 – ΔG and equilibrium
  • Reactivity 2: How much, how fast and how far?
    • Reactivity 2.1: How much? The amount of chemical change
      • Reactivity 2.1.1 – Chemical equations
      • Reactivity 2.1.2 – Using mole ratios in equations
      • Reacti vity 2.1.3 – The limiting reactant and theoretical yield
      • Reactivity 2.1.4 – Percentage yield
      • Reactivity 2.1.5 – Atom economy
    • Reactivity 2.2: How fast? The rate of chemical change
      • Reactivity 2.2.1 – Rate of reaction
      • Reactivity 2.2.2 – Collision theory
      • Reactivity 2.2.3, 2.2.4 and 2.2.5 – Factors that influence the rate of reaction
      • Reactivity 2.2.6, 2.2.7 and 2.2.8 – Reaction mechanisms
      • Reactivity 2.2.9 and 2.2.10 – Rate equations
      • Reactivity 2.2.11 – The rate constant, k
      • Reactivity 2.2.12 and 2.2.13 – The Arrhenius equation
    • Reactivity 2.3: How far? The extent of chemical change
      • Reactivity 2.3.1 – Dynamic equilibrium
      • Reactivity 2.3.2 and 2.3.3 – Equilibrium law
      • Reactivity 2.3.4 – Le Châtelier’s principle
      • Reactivity 2.3.5 – The reaction quotient, Q
      • Reactivity 2.3.6 – Quantifying the composition of equilibrium
      • Reactivity 2.3.7 – Measuring the position of equilibrium
  • Reactivity 3: What are the mechanisms of chemical change?
    • Reactivity 3.1: Proton transfer reactions
      • Reactivity 3.1.1 and 3.1.2 – Brønsted–Lowry acids and bases
      • Reactivity 3.1.3 – Amphiprotic species
      • Reactivity 3.1.4 – The pH scale
      • Reactivity 3.1.5 – The ion product constant of water
      • Reactivity 3.1.6 – Strong and weak acids and bases
      • Reactivity 3.1.7 – Neutralization reactions
      • Reactivity 3.1.8 – pH curves
      • Reactivity 3.1.9 – The pOH scale
      • Reactivity 3.1.10 and 3.1.11 – Acid and base dissociation constants
      • Reactivity 3.1.12 – pH of salt solutions
      • Reactivity 3.1.13 – pH curves revisited
      • Reactivity 3.1.14 and 3.1.15 – Acid–base indicators
      • Reactivity 3.1.16 – Buffer solutions
      • Reactivity 3.1.17 – Buffer composition and pH
    • Reactivity 3.2: Electron transfer reactions
      • Reactivity 3.2.1 – Redox reactions
      • Reactivity 3.2.2 – Half-equations
      • Reactivity 3.2.3 – Trends in ease of oxidation and reduction of elements
      • Reactivity 3.2.4 – Oxidation of metals by acids
      • Reactivity 3.2.5 – Comparing voltaic and electrochemical cells
      • Reactivity 3.2.6 – Primary (voltaic) cells
      • Reactivity 3.2.7 – Secondary (rechargeable) cells
      • Reactivity 3.2.8 – Electrolytic cells
      • Reactivity 3.2.9 – Oxidation of functional groups in organic compounds
      • Reactivity 3.2.10 – Reduction of functional groups in organic compounds
      • Reactivity 3.2.11 – Reduction of unsaturated compounds
      • Reactivity 3.2.12 – The standard hydrogen electrode
      • Reactivity 3.2.13 – Standard electrode potentials
      • Reactivity 3.2.14 – Electrode potentials and Gibbs energy changes
      • Reactivity 3.2.15 – Electrolysis of aqueous solutions
      • Reactivity 3.2.16 – Electroplating
    • Reactivity 3.3: Electron sharing reactions
      • Reactivity 3.3.1 – Radicals
      • Reactivity 3.3.2 – Homolytic fission
      • Reactivity 3.3.3 – Radical substitution reactions of alkanes
    • Reactivity 3.4: Electron-pair sharing reactions
      • Reactivity 3.4.1 – Nucleophiles
      • Reactivity 3.4.2 – Nucleophilic substitution reactions
      • Reactivity 3.4.3 – Heterolytic fission
      • Reactivity 3.4.4 – Electrophiles
      • Reactivity 3.4.5 – Electrophilic addition of alkenes
      • Reactivity 3.4.6 and 3.4.7 – Lewis acids and Lewis bases
      • Reactivity 3.4.8 – Complex ions
      • Reactivity 3.4.9 and 3.4.10 – SN1 and SN2 nucleophilic substitution mechanisms
      • Reactivity 3.4.11 – Electrophilic addition reaction mechanism
      • Reactivity 3.4.12 – Addition of hydrogen halides to asymmetrical alkenes
      • Reactivity 3.4.13 – Electrophilic substitution of benzene
• Green Chemistry
• Theory of Knowledge in chemistry
• Internal Assessment
• Skills in the study of chemistry
• Strategies for success
• Extended Essay
• Index
• Back Cover

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