Chemistry for the IB Diploma Third edition
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Description
Contents
Reviews
Language
English
ISBN
9781398371637
Cover
Title Page
Copyright
Contents
Introduction
How to use this book
Tools and Inquiry
Structure
S1 Models of the particulate nature of matter
S1.1 Introduction to the particulate nature of matter
Introduction
Elements and compounds
Compounds
Solvation
Mixtures
Separation techniques
Kinetic molecular theory
Temperature
S1.2 The nuclear atom
Atomic structure
Electron arrangement
Nuclide notation
Isotopes
Mass spectrometry
S1.3 Electron configurations
Introduction
Light
Electron excitation
Energy levels and spectra
Orbitals and energy levels
Filling atomic orbitals
Ionization energies
S1.4 Counting particles by mass: the mole
The mole
Chemical equations
Measuring moles
Calculating quantities
Determining the masses of the products of a reaction
Molecular formula and empirical formula
Molar and mass concentration
Titrations
Avogadro’s law
S1.5 Ideal gases
Introduction
Ideal gases
Real gases
Molar volume of a gas
The gas laws
The ideal gas equation
Graphical plots of ideal gas behaviour
S2 Models of bonding and structure
S2.1 The ionic model
Introduction to ionic bonding
Formation of ions and lattice in sodium chloride
Naming ionic compounds
Ionic formulas
Ion charges and electron configurations
Ionic bonding and electronegativity
Properties of ionic compounds
Lattice enthalpy
S2.2 The covalent model
Covalent bond formation and notation
Bond lengths and enthalpies
Complex ions
The shapes of molecules
Molecular polarization
Covalent network structures
Intermolecular forces
Chromatography
Introduction to molecular orbital theory
Resonance
Benzene
S2.3 The metallic model
Metallic bonding
Physical properties of metals
Uses of metals and alloys
Melting points in s and p block metals
Properties of transition elements
S2.4 From models to materials
Chemical models
The bonding triangle (van Arkel diagram)
Alloys
Polymers
Condensation polymers
Condensation and hydrolysis reactions
S3 Classification of matter
S3.1 The periodic table: classification of elements
Introduction to the periodic table
Trends in atomic properties down groups
Electronegativity
Trends in atomic properties across periods
Group 1 (alkali metals)
Group 17 (halogens)
Oxides
Oxidation states
Transition elements
Formation of complex ions
S3.2 Functional groups: classification of compounds
Organic molecules
Representing molecules
Functional groups
Trends in physical properties in a homologous series
Nomenclature of organic compounds
Isomerism
Stereoisomers
Spectroscopy
Reactivity
R1 What drives chemical reactions?
R1.1 Measuring enthalpy changes
Heat and temperature
Conservation of energy
Endothermic and exothermic reactions
Potential energy profiles
Calculating heat energy transferred
Enthalpy changes
Measuring the standard enthalpy change of a chemical reaction
R1.2 Energy cycles in reactions
Bond-breaking absorbs and bond-forming releases energy
Bond enthalpies
Hess’s law
Standard enthalpy of combustion, ∆Hc⦵, and formation, ∆Hf⦵
Applications of Hess’s law
Energy changes in ionic compounds
Born–Haber cycles
R1.3 Energy from fuels
Combustion reactions
Fossil fuels
Renewable energy sources
Fuel cells
R1.4 Entropy and spontaneity (HL only)
What are spontaneous processes?
Entropy
Standard entropy changes
The second law of thermodynamics
Gibbs energy change
Gibbs energy change and temperature
Gibbs energy change and equilibrium
R2 How much, how fast and how far?
R2.1 How much?: The amount of chemical change
Chemical equations
Reacting masses and volumes
Stoichiometry problems
Limiting reactant
Percentage yield
Green chemistry
Atom economy
R2.2 How fast?: The rate of chemical change
Introduction
Collision theory
Factors affecting the rate of reaction
The relative effect of factors affecting rates of reaction
Calculating reaction rates
Measuring rates of reactions
Rate equations
Reaction mechanisms
Chain reactions
Rate constant and temperature
R2.3 How far?: The extent of chemical change
Reversible reactions
Equilibrium
The equilibrium law
Types of equilibrium
Shifting the position of equilibrium
Graphs involving Le Châtelier’s principle
Reaction quotient
Calculating equilibrium constants
Relationship between equilibrium constant, spontaneity and Gibbs energy change
Relationship between thermodynamics and equilibrium
R3 What are the mechanisms of chemical change?
R3.1 Proton transfer reactions
Acids and bases – Arrhenius definitions
Ionic equations
Reactions of acids and bases
Brønsted–Lowry theory
Strong and weak acids and bases
Conjugate acid–base pairs
The pH and pOH scales
Ion product constant of water
Titration curves
Dissociation constants
Salt solutions
Indicators
Buffer solutions
R3.2 Electron transfer reactions
Oxidation and reduction
More half-equations
Electrochemical cells
Oxidation of functional groups in organic compounds
Reduction of functional groups
Types of half-cell
Standard electrode potentials
Standard cell potentials
Cell spontaneity
Electrolysis of aqueous solutions
R3.3 Electron sharing reactions
Introduction to radicals
Forming radicals
Halogenation of alkanes in radical substitution reactions
Radical reactions with other organic molecules
R3.4 Electron pair sharing reactions
Nucleophiles and electrophiles
Nucleophilic substitution reactions
Heterolytic fission
Electrophilic addition reactions with alkenes
Lewis acids and Lewis bases
Nucleophilic substitution reactions of halogenoalkanes
Electrophilic addition of alkenes
Addition of a hydrogen halide
Electrophilic substitution reactions of benzene
Acknowledgements
Index
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