Why do certain substances react together in the way that they do? What determines the shape of molecules? And how can we predict whether a particular reaction will happen at all?
Such questions lie at the heart of chemistry - the science of understanding the composition of substances, their reactions, and properties. Though introductory chemistry is often broken into three sections-inorganic, organic, and physical-the only way for students to fully understand the subject is to see it as a single, unified whole.
Chemical Structure and Reactivity rises to the challenge of depicting the reality of chemistry. Offering a fresh approach to the subject by depicting it as a seamless discipline, the text shows how organic, inorganic, and physical concepts can be blended together in order to achieve the common goal of understanding chemical systems.
With a lively and engaging writing style enhanced by vivid illustrations, only Chemical Structure and Reactivity makes teaching chemistry with an integrated approach possible.
Special Features
--The only introductory text to take a truly integrated approach in explaining the fundamentals of chemistry.
--Fosters an orbital-based understanding of reactions, with clear curly-arrow mechanistic detail throughout.
--A two-part structure allows flexibility of use: Part I lays down the core of the subject, while Part II describes a series of relatively standalone topics, which can be selected to fit a particular course.
--Numerous concepts are illustrated with fully cross-referenced custom-developed online modules, enabling students to develop an understanding through active learning.
--Self-test exercises embedded in the text (with solutions at the end of each chapter) and extensive question sets encourage hands-on learning, to help students master the subject and gain confidence.
--The Online Resource Centre features a range of additional resources for both students and registered adopters of the book.
New to this Edition
--A new chapter on symmetry has been added to Part I.
--Discussions of organometallic chemistry, spectroscopy, and molecular geometry have been expanded.
--Cross references from Part I to Part II have been increased to make the links between core concepts and more advanced topics clearer.
--More self-test questions and exercises have been provided.
Author(s): James Keeler, Peter Wothers
Edition: 2
Publisher: Oxford University Press
Year: 2014
Language: English
Pages: 877
City: Oxford
Cover
Contents
Part I: The fundamentals
1 Molecules and molecular structures: an overview
1.1 Simple covalent molecules
1.2 Structure determination by X-ray diffraction
1.3 Where are the bonds?
1.4 Types of bonding
1.5 Weaker non-bonded interactions
1.6 Solids
1.7 How to draw molecules
1.8 Common names and abbreviations
1.9 The ideal gas
1.10 Moving on
Answers to self-test exercises
2 Electrons in atoms
2.1 Introducing quantum mechanics
2.2 Introducing orbitals
2.3 Hydrogen atomic orbitals
2.4 Spin
2.5 Hydrogen-like atoms
2.6 Multi-electron atoms
2.7 Ionization energies
2.8 Moving on
Further reading
Answers to self-test exercises
3 Symmetry
3.1 Why symmetry is important
3.2 Symmetry elements and symmetry operations
3.3 Point groups
3.4 Applications of symmetry
3.5 Classification of orbitals according to symmetry
3.6 Moving on
Further reading
Answers to self-test exercises
4 Electrons in molecules: diatomics
4.1 Introducing molecular orbitals
4.2 H[sub(2)], He[sub(2)] and their ions
4.3 Homonuclear diatomics of the second period
4.4 Photoelectron spectra
4.5 Heteronuclear diatomics
4.6 Moving on
Further reading
Answers to self-test exercises
5 Electrons in molecules: polyatomics
5.1 The simplest triatomic: H[sup(+)][sub(3)]
5.2 More complex linear triatomics
5.3 MOs of water and methane
5.4 Hybrid atomic orbitals
5.5 Comparing the hybrid and full MO approaches
5.6 Extending the hybrid concept
5.7 Bonding in organic molecules
5.8 Delocalized bonding
5.9 Delocalized structures including heteroatoms
5.10 Moving on
Further reading
Answers to self-test exercises
6 Bonding in solids
6.1 Metallic bonding: introducing bands
6.2 Ionic solids
6.3 Moving on
Further reading
Answers to self-test exercises
7 Thermodynamics and the Second Law
7.1 Spontaneous processes
7.2 Properties of matter: state functions
7.3 Entropy and the Second Law
7.4 Heat, internal energy and enthalpy
7.5 Entropy in terms of heat
7.6 Calculating the entropy change of the Universe
7.7 Gibbs energy
7.8 Chemical equilibrium
7.9 Finding the standard Gibbs energy change
7.10 Interpreting the value of Δ[sub(r)] G[sup(°)]
7.11 Δ[sub(r)]H[sup(°)] and Δ[sub(r)]S[sup(°)] for reactions not involving ions
7.12 Δ[sub(r)]H[sup(°)] and Δ[sub(r)]S[sup(°)] for reactions involving ions in solution
7.13 Applications
7.14 Acidity, basicity and pK[sub(a)]
7.15 How much product is there at equilibrium?
7.16 Moving on
Further reading
Answers to self-test exercises
8 Trends in bonding
8.1 Electronic configuration and the periodic table
8.2 Orbital energies and effective nuclear charges
8.3 Atomic sizes across the periodic table
8.4 Ionization energies and electron affinities
8.5 Trends in oxidation states across the periodic table
8.6 Summary of the trends in orbital energies and sizes
8.7 Bonding in the elements – non-metals
8.8 Metallic structures
8.9 The transition from metals to non-metals
8.10 Moving on
Further reading
Answers to self-test exercises
9 Bonding between the elements
9.1 The effect of orbital size and energy mismatch
9.2 The classification of compounds as ionic or covalent
9.3 Structural trends across the periodic table
9.4 Radius ratio rules
9.5 Compounds with lower coordination numbers
9.6 Moving on
Further reading
Answers to self-test exercises
10 Describing reactions using orbitals
10.1 The redistribution of electrons in a reaction
10.2 HOMO–LUMO interactions
10.3 Interactions involving nonbonding LUMOs
10.4 Interactions involving π antibonding LUMOs
10.5 Interactions involving γ antibonding LUMOs
10.6 Summary of the effects of different HOMO–LUMO interactions
10.7 The role of protonation in reactions
10.8 Intramolecular orbital interactions
10.9 Rearrangement reactions
10.10 Moving on
Answers to self-test exercises
11 Organic chemistry 1: functional groups
11.1 Functional groups
11.2 Changing functional group level
11.3 Level two to level one – carbonyl addition reactions
11.4 Transformations within functional group level two
11.5 Transformations within functional group level three
11.6 Moving down from functional group level three
11.7 Transformations within level one
Further reading
Answers to self-test exercises
12 The rates of reactions
12.1 The rate of a reaction
12.2 Rate laws
12.3 Temperature dependence
12.4 The energy barrier to reaction
12.5 Elementary reactions and reaction mechanisms
12.6 Reactions in solution
12.7 Sequential reactions
12.8 Analysing the kinetics of complex mechanisms
12.9 Chain reactions
Further reading
Answers to self-test exercises
Part II: Going further
13 Spectroscopy
13.1 Mass spectrometry
13.2 Spectroscopy and energy levels
13.3 IR spectroscopy – introduction
13.4 Interpreting IR spectra
13.5 Nuclear Magnetic Resonance (NMR)
13.6 Coupling in NMR
13.7 More complicated coupling patterns – proton NMR
Further reading
Answers to self-test exercises
14 Organic chemistry 2: three-dimensional shapes
14.1 The relationships between isomers
14.2 The effect of rotations about bonds
14.3 Isomerism in alkenes
14.4 Enantiomers and chirality
14.5 Symmetry and chirality
14.6 The conformation of cyclic molecules
14.7 Moving on
Further reading
Answers to self-test exercises
15 Organic chemistry 3: reactions of π systems
15.1 Elimination reactions – the formation of alkenes
15.2 Electrophilic addition to alkenes
15.3 Enols and enolates
15.4 The reactions of enols and enolates
15.5 Introduction to aromatic systems
Further reading
Answers to self-test exercises
16 Main-group chemistry
16.1 Overview
16.2 Key concepts in main-group chemistry
16.3 Hydrolysis of chlorides
16.4 Oxides
16.5 Brief survey of the chemistry of each group
16.6 Moving on
Further reading
Answers to self-test exercises
17 Transition metals
17.1 Orbital energies and oxidation states
17.2 Complexes
17.3 Bonding in octahedral complexes
17.4 High-spin and low-spin octahedral complexes
17.5 Magnetic and spectroscopic properties of complexes
17.6 Consequences of the splitting of the d orbitals
17.7 Tetrahedral and square-planar complexes
17.8 Crystal-field theory
17.9 Organometallic complexes
17.10 Aqueous chemistry and oxoanions
17.11 Moving on
Further reading
Answers to self-test exercises
18 Quantum mechanics and spectroscopy
18.1 The postulates of quantum mechanics
18.2 A free particle moving in one dimension
18.3 Particle in a box
18.4 Particle in a two-dimensional square well
18.5 The harmonic oscillator
18.6 Spectroscopy and energy levels
18.7 The IR spectrum of a diatomic
18.8 Vibrations of larger molecules
18.9 Raman spectroscopy
18.10 Summary of the features of vibrational spectroscopy
18.11 The rigid rotor
18.12 The microwave spectrum of a diatomic
18.13 Vibration–rotation spectrum of a diatomic
18.14 The hydrogen atom
18.15 Electronic transitions
Further reading
Answers to self-test exercises
19 Chemical thermodynamics
19.1 The First Law
19.2 Work of gas expansions
19.3 Internal energy, enthalpy and heat capacity
19.4 The Gibbs energy
19.5 The mixing of ideal gases
19.6 Chemical equilibrium
19.7 Equilibria involving other than gases
19.8 Determination of the standard Gibbs energy change
19.9 The temperature dependence of the equilibrium constant
19.10 Determination of absolute entropies
Further reading
Answers to self-test exercises
20 Chemical kinetics
20.1 Measuring concentration
20.2 Integrated rate laws
20.3 Other methods of analysing kinetic data
20.4 Collision theory
20.5 Potential energy surfaces
20.6 Transition state theory
Further reading
Answers to self-test exercises
21 Electrochemistry
21.1 Electrochemical cells
21.2 Thermodynamic parameters from cell potentials
21.3 The Nernst equation and standard cell potentials
21.4 The spontaneous cell reaction
21.5 Summary
21.6 Types of half cells
21.7 Assessing redox stability using electrode potentials
21.8 The limits of stability in aqueous solution
21.9 Using cell potentials to determine thermodynamic parameters
21.10 Oxidation state diagrams
21.11 Measurement of concentration
Further reading
Answers to self-test exercises
Part III: Reference material
22 Dimensions, units and some key mathematical ideas
22.1 Dimensional analysis
22.2 Units
22.3 Trigonometric functions
22.4 The exponential function
22.5 Calculus: differentiation
22.6 Calculus: integration
22.7 Differential equations
Further reading
Answers to self-test exercises
Index
A
B
C
D
E
F
G
H
I
K
L
M
N
O
P
Q
R
S
T
U
V
W
X
Z
Orbital energies
