General chemistry textbooks are usually lengthy and present chemistry to the student as an unconnected list of facts. In inorganic chemistry, emphasis should be placed on the connections between valence shell electron configuration and the physical and chemical properties of the element. Basic Principles of Inorganic Chemistry: Making the Connections is a short, concise book that emphasises these connections, in particular the chemistry of the Main Group compounds. With reference to chemical properties, Lewis Structures, stoichiometry and spider diagrams, students will be able to predict or calculate the chemistry of simple polyatomic compounds from the valence shell configuration and will no longer be required to memorise vast amounts of factual chemistry. This book is ideal for students taking chemistry as a subsidiary subject as well as honours degree students.

Basic Principles of Inorganic Chemistry

Making the Connections

The Royal Society of Chemistry

Contents

Chapter 1 Moles and Molarity, 1, 
Aims and Objectives, 1, 
States of Matter, 1, 
Elements, Atoms and Molecules, 1, 
Elements, Mixtures and Compounds (Molecules), 2, 
Simple Chemical Names, 3, 
Cations and Anions, 3, 
Types of Chemical Formula, 4, 
Atomic Weight, 4, 
Avogadro's Number, 5, 
Empirical Formula, 5, 
Chemical Equations, 6, 
Balancing Chemical Equations, 7, 
Molar Solutions, 8, 
Volumetric Reactions, 9, 
Volumetric Titrations, 10, 
Limiting Reactions, 11, 
Worked Example No. 1, 11, 
Worked Example No. 2, 13, 
Chapter 2 The Structure of the Atom, Electron Configuration and the Build-up to the Periodic Table, 14, 
Aims and Objectives, 14, 
The Structure of the Atom, 14, 
Bohr Model of the Atom, 17, 
The Build-up Process for the Periodic Table, 27, 
Chapter 3 The Physical Properties of the Elements and the Periodic Table, 31, 
Aims and Objectives, 31, 
The Periodic Table, 31, 
Variation in the Atomic Radii, 34, 
Variation in the Ionisation Potentials, 34, 
Variation in the Electron Affinities or Attachment Enthalpies, 37, 
Summary, 38, 
Chapter 4 Chemical Properties of the Elements and the Periodic Table, 39, 
Aims and Objectives, 39, 
Introduction, 39, 
Characteristic or Group Oxidation Numbers, 41, 
Oxidation Numbers, 43, 
Rules for the Determination of Oxidation Numbers, 44, 
Main Group Variable Valence, 44, 
Transition Metal Variable Valence, 46, 
Chemical Stoichiometry, 49, 
The Calculation of Chemical Stoichiometry Factors – Worked Examples, 51, 
Redox Reactions, 52, 
Covalent Bonds, 53, 
Polyatomic Covalent Molecules, 56, 
Molecular Orbital Theory of Diatomic Molecules, 56, 
Bond Order, 60, 
Chapter 5 The Lewis Structures of Molecules, Cations and Anions, Including Oxyanions, 61, 
Aims and Objectives, 61, 
Introduction, 61, 
The Working Method for Drawing Lewis Structures, 64, 
Example 1: Methane (CH4) and Carbon Tetrachloride (CCl4), 65, 
Example 2: The Ammonium Cation (NH4-) and the Tetrafluorborate Anion (BF4-), 66, 
Example 3: Ammonia (NH3) and Water (OH2), 68, 
Example 4: Beryllium Dihydride (BeH2) and Boron Trifluoride (BF3, 69, 
Example 5: Phosphorus Pentchloride (PCl5) and Sulfur Hexafluoride (SF6), 70, 
Example 6: l,l,-Dichloromethanone (C12CO) and Ethene (C2H4), 71, 
Example 7: Ethyne (C2H2), 73, 
The Oxyacids and Oxyanions of the Main Group Elements, 74, 
The Position of the Hydrogen Atoms in the Oxyacids, 74, 
The Free Valence of the Terminal Oxygen Atoms, 76, 
Resonance in the Structures of the Oxyanions, 78, 
The Application of the Working Method to the Lewis Structures of the Oxyanions, 79, 
Example 1: Carbonic Acid, H2CO3, 79, 
Example 2: Sulfuric Acid, H2SO4, 81, 
The Use of Formal Charges, 84, 
Summary, 86, 
Chapter 6 Shape and Hybridisation, 88, 
Aims and Objectives, 88, 
The Shapes of Covalent Molecules, 88, 
The Working Method for Using VSEPR Theory, 92, 
Deviations from Regular Shapes, 94, 
The Advantages of VSEPR Theory, 95, 
The Disadvantages of VSEPR Theory, 95, 
The Shape of Dinuclear Molecules, 95, 
Hybridisation of Atomic Orbitals, 99, 
Hybridisation in Polynuclear Molecules, 104, 
Summary, 106, 
Chapter 7 A Features of Interest Approach to Systematic Inorganic Chemistry, 107, 
Aims and Objectives, 107, 
Introduction, 107, 
The Preparation of Simple Compounds from the Elements, 109, 
The Reactions of Simple Compounds, 113, 
Reaction with Water, 113, 
Volumetric Reactions, 114, 
The Effect of Heat, 115, 
Features of Interest of Simple Compounds – Working Method, 116, 
The Applicaton of the Working Method to a Selection of Simple Compounds, 
Example 1: Methane, (CH4), 119, 
Example 2: Hydrochloric Acid (HCl), 120, 
Example 3: Sodium Chloride (NaCl), 121, 
Example 4: Phosphorus Pentachloride (PCl5), 122, 
Example 5: Copper (II) Oxide, (CuO), 123, 
Example 6: Iron (II) Chloride (FeCl2), 124, 
Example 7: Iron (II) Sulfate Hexahydrate ([Fe(OH2)6]SO4), 125, 
Example 8: Carbonic Acid (H2CO3), 126, 
Writing an Essay or Report from a Spider Diagram, 128, 
Conclusions, 130, 
Suggested Ways Forward, 130, 
Phase II – Features of Interest, 130, 
Phase III – Features of Interest, 131, 
The Advantages of the Features of Interest Approach, 139, 
The Disadvantages of the Features of Interest Approach, 139, 
Appendices, 144, 
Periodic Table of the Elements, 148, 
Subject Index, 149,