This book is intended to be a brief introduction of general inorganic chemistry, written primarily for students in their first year of chemistry. The text is organized into seven chapters, two appendices, and an alphabetical subject index. Each chapter begins with a one-paragraph statement of its aims and objectives. Chapter headings reflect the material covered in the 143 pages of actual text. They are as follows.

1. Moles and Molarity. Differences between atoms and molecules, between cations and anions, and between compounds and mixtures are discussed. Numerical examples are given to show the calculation of both molecular weight and atomic weight percentage from molecular structure, of molarity from the grams of solute dissolved in a given volume of solution, and of amount of chemicals produced as the result of chemical reactions involving limiting reagents. The authors unfortunately use the terms "atomic weight" and "molecular weight" throughout the book. Most chemistry textbooks used in the United States distinguish between weights and masses.

2. The Structure of the Atom, Electron Configuration and the Build-up of the Periodic Table. The chapter presents in abbreviated fashion several of the early models for the atom and discusses the spectroscopic evidence for atomic orbitals. The four quantum numbers are introduced and the shapes of s, p, and d orbitals are depicted. Electron configurations for the first 30 elements in the periodic table are deduced using the Pauli exclusion principle and Hund's maximum multiplicity rule. The outer electron configurations for Cr and Cu were given as 3d⁴ and 3d⁹, respectively. Nowhere in the chapter was it ever mentioned that these two elements have abnormal ground-state electron configurations in that an electron is removed from the 4s orbital and placed into one of the 3d orbitals. The chapter's coverage could have been expanded to show electron configurations of simple ions, such as Na⁺, Mg²⁺, and F^-.

3. The Physical Properties of the Elements and the Periodic Table. Periodic trends in atomic radii, first ionization potential, and electron affinity are presented in both tabular and graphical format. Only a superficial explanation is given to justify each observed trend.

4. Chemical Properties of the Elements and the Periodic Table. Molecular bonding is discussed in terms of the sharing of electrons between adjacent atoms. Electronegativity is introduced and rules are presented for the assignment of oxidation numbers for simple molecules and ionic compounds. The variable valences of select first-row transition metals are discussed. Structural formulas of several polyatomic covalent molecules are presented to show how the number of valence electrons determines the number of covalent bonds that will be formed. Molecular orbital theory of diatomic molecules is briefly presented using H₂, H₂⁺, He₂⁺ and He₂. An equation is given for the calculation of bond order. The discussion of molecular orbital theory is inadequate in that no mention is given to the formation of p-bonds, despite the fact that the authors state that a bond order of two corresponds to a double bond, and a bond order of three corresponds to a triple bond.

I was disappointed to find very little attention given to chemical nomenclature. For example, in Chapter 4, molecular and ionic formulas such as KMnO₄, HClO₄, and SO₄^2- are presented without names. Even in the authors' discussion of variable valences, none of the common transition metal cations are named. Naturally, one must wonder how the authors expect readers to learn chemical nomenclature from their book.

I also noted that the authors did give the electron configurations of Cr and Cu as [Ar]s¹d⁵ and [Ar]s¹d¹⁰ in both Table 4.1 and Figure 4.4. Readers not already familiar with how to write electron configurations will undoubtedly note the discrepancies between Figures 2.11 and 4.4, and wonder which of the electron configurations are correct.

5. The Lewis Structures of Molecules, Cations and Anions, Including Oxyanions. The chapter is entirely devoted to constructing Lewis dot structures. Examples are given for both molecules and ions that obey the octet rule, and for those that have an expanded octet containing either 10 or 12 electrons. Resonance structures are drawn if applicable. Oxyacids and oxyanions of the main group elements are treated in detail. Formal charges are calculated, and when needed are used to predict which of several alternative dot structures is the most reasonable.

6. Shapes and Hybridization. Molecular shapes are predicted on the basis of the valence state electron pair repulsion (VSEPR) theory. Examples are depicted showing both bond orders and bond angles. Advantages and disadvantages of the VSEPR theory are stated. The basic hybridization schemes are briefly reviewed, with simple diagrams given to depict the formation of p-bonds through the overlap of atomic p orbitals.

7. A Features of Interest Approach to Systematic Inorganic Chemistry. Properties and reactivity of select molecules are summarized in a "Features of Interest Spider Diagram". The diagram includes the electron configuration, electronegativity, and oxidation number of each element in the molecule, as well the molecule's shape and Lewis dot structure and select chemical reactions involving the molecule. Contrary to the authors' claims, however, it is not apparent to me how the spider diagram allows one to predict 80% of the chemistry of simple molecules, anions, and cations.

The book concludes with two appendices listing six additional texts and papers and ten tutorials, and a dozen or so possible topics and questions for discussion. Personally, I found the book to be completely unsuitable as either a textbook or reference book for classroom instruction in the United States. I suspect that it was written for the British educational system. It is much too narrowly focused to be used as a general chemistry textbook. The few topics that are covered in the book I find covered in greater depth in most standard general chemistry textbooks. The book contains no problems for students to work. Many of the examples that are presented are extremely simple, and are not meant to challenge even the average student.