Higher Level Chemistry for the IB Diploma Programme

Höfundur: Catrin Brown (Útgáfa: 3)
Higher Level Chemistry for the IB Diploma Programme

Kaup valmöguleikar

Co-published with the IB to fully align with the new 2023 Chemistry Subject Guide for first assessments in 2025 to ensure that every student has the right content for their learning journey, at the right time. New and updated material with familiar features, including Nature of science, global applications, skills, TOK, key fact and ‘Challenge yourself’ boxes that signpost and extend key learning points and contexts.

Conceptual approach offers a flexible route through the syllabus, with topics linked to increase depth of understanding. Plain language with scientific terms highlighted in bold and explained. Internal and external assessment support, with exercises and exam-style practice questions for revision and worked examples with solutions. eBook resources including auto-marked quizzes, lab worksheets and activities.

Nánar um bókina

Útgefandi
Pearson International Content
ISBN
9781292466705
Print ISBN
9781292427720
Format
Page Fidelity (PDF)
Útgáfa
3
Höfundar
Catrin Brown
Tungumál
English
Útgefið
2023-07-24
Prent takmörkun á líftíma
100
Prent takmörkun
2
Afritunar takmörkun
2

Kaflar

  • 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