The Periodic Table: A Very Short Introduction

Citation

Scerri, E. R. (2019). The Periodic Table: A Very Short Introduction (2nd ed.). Oxford University Press. Very Short Introductions.

Chapter Summary

The second edition runs to about 145 pages in ten chapters. Oxford's description says it covers what led to the construction of the periodic table and how the deeper meaning of its structure emerged with atomic theory and quantum mechanics, and that this edition marks the completion of the seventh period, with elements 113, 115, 117 and 118 named nihonium, moscovium, tennessine and oganesson, and adds recent work on the origin of the elements. The book is mostly historical in arrangement: after two orienting chapters, Chapters 3–9 follow the table's development from early atomic weights to synthetic elements, and Chapter 10 asks which form of the table is best.

Chapter 1: The elements

The history of the idea of an element: the four Greek elements and their association with the Platonic solids, elements known since antiquity and those that needed new techniques to isolate, disputes over naming, and the move from alchemical symbols to the letter symbols used today.

Chapter 2: A quick overview of the modern periodic table

How elements are arranged and what the periodic law states: after regular but varying intervals the elements show an approximate repetition of properties. The chapter traces the ordering principle from equivalent weight to atomic weight to atomic number, notes that many versions of the table exist, and explains how quantum mechanics, relativity and the synthesis of artificial elements (bringing the total to 118) have changed ideas about periodicity.

Chapter 3: Atomic weight, triads, and Prout

The shift from qualitative to quantitative chemistry: Dalton's atomic theory, Avogadro's diatomic molecules, Gay-Lussac's combining volumes, Prout's hypothesis that atomic weights are multiples of hydrogen's, Döbereiner's triads, and Kremers's first attempts to relate chemically dissimilar elements.

Chapter 4: Steps towards the periodic table

The tables of the 1860s that followed the Karlsruhe conference and its standardised atomic weights: de Chancourtois, Newlands and his law of octaves, Odling, Hinrichs and Lothar Meyer, each of whom grasped part of periodicity.

Chapter 5: The Russian genius

Mendeleev's life and work: how he differed from rivals by rejecting Prout's hypothesis and triads, the table he sketched in 1869, its successful and failed predictions, and the accommodation of the noble gases after their isolation in the 1890s.

Chapter 6: Physics invades the periodic table

Rutherford's nuclear atom, van den Broek's idea of atomic number, Moseley's measurements showing exactly which elements were missing, and Soddy's isotopes.

Chapter 7: Electronic structure

Planck's quantum theory, Bohr's shell model and its extension to other elements using chemical evidence, Lewis's cubic atom and electron-pair bond, and Bury's work on the order in which shells fill.

Chapter 8: Quantum mechanics

Why Bohr's theory failed for many-electron atoms and how Schrödinger's wave equation treats electrons as waves to quantise their energies, with a discussion of recent work on electron configurations by Eugen Schwarz.

Chapter 9: Modern alchemy

From transmutation by Rutherford and Soddy to cyclotron synthesis of heavier elements, the filling of gaps in the table, the placement of the elements beyond uranium in their own section, and relativistic effects, which leave chemical periodicity remarkably intact.

Chapter 10: Forms of the periodic table

The many published designs, including moving hydrogen and helium or rearranging elements to form triads, and the question of whether there is an optimal table, which the chapter frames as a philosophical choice between realist and instrumentalist views of periodicity.

Key Concepts

Chapters 1–2: Elements and the Modern Table

• Periodic law: after regular but varying intervals, elements show an approximate repetition of their properties.
• Atomic number: the ordering principle that replaced equivalent weight and atomic weight.

Chapters 3–5: The Discovery of Periodicity

• Prout's hypothesis and triads: early numerical patterns in atomic weights that pointed towards periodicity.
• Mendeleev's predictions: the use of the periodic system to forecast unknown elements, with successes and errors.

Chapters 6–8: Physics and the Table

• Moseley's work and isotopes: experimental evidence that atomic number, not weight, orders the elements.
• Electron shells and quantum mechanics: from Bohr's model to Schrödinger's equation as the explanation of periodicity.

Chapters 9–10: New Elements and New Tables

• Synthetic elements: elements made by nuclear transmutation and particle accelerators, completing the seventh period.
• Realism and instrumentalism: two views on whether an optimal periodic table exists.

Critical Analysis

Strengths

• History told in depth. Five chapters cover the period before quantum mechanics, including lesser-known contributors such as Kremers, Odling, Hinrichs and Bury, so the table appears as the work of many people rather than of Mendeleev alone.
• Physics as explanation. Chapters 6–8 show how atomic number, electronic structure and quantum mechanics explained a pattern chemists had already found, giving students a reason for the trends they will learn.
• Up to date at publication. The second edition includes the naming of elements 113, 115, 117 and 118 and recent ideas about the origin of the elements.
• Engages with open questions. The final chapter treats the form of the table as a live question with philosophical dimensions, useful for students who assume the table on the classroom wall is the only possible one.

Limitations

• Little descriptive chemistry. The book explains the table rather than the chemistry of the elements in it; group properties and periodic trends in size, ionisation energy or reactivity are not the subject of any chapter.
• History-heavy for some readers. Chapters 3–5 are history of science; students who want only the scientific explanation can move faster through them.
• Not a course text. At about 145 pages it supplies context, not the quantitative skills that inorganic courses assess.

Where It Fits in the Course

In this inorganic chemistry course, Scerri's book is background reading on the organising framework of the whole subject. It pairs naturally with Rayner-Canham and Overton's Descriptive Inorganic Chemistry, which surveys the elements group by group after setting out the principles behind their behaviour: Scerri explains why the table has its shape, and Rayner-Canham and Overton describe what the elements in it do.

The more theoretical textbooks on the list go much further. Housecroft's Inorganic Chemistry and Shriver, Weller, Overton and colleagues' Inorganic Chemistry combine atomic structure, bonding, symmetry and spectroscopy with systematic chemistry of the blocks; Pfennig's Principles of Inorganic Chemistry develops symmetry, group theory and molecular orbital models; and Crabtree's The Organometallic Chemistry of the Transition Metals is a graduate text on metal–carbon compounds. Scerri's chapters on electronic structure and quantum mechanics are a gentle preface to the opening chapters of those books.

How to Use This Book

The book suits first-year chemistry students starting inorganic chemistry, students in physics, materials or earth sciences who use the table every day, and readers interested in the history and philosophy of chemistry. School chemistry is enough.

A practical plan:

• Before the course: read Chapters 1–2 for an overview of the table and the periodic law, and Chapters 6–8 for the physical explanation of periodicity.
• Alongside the course: read Chapters 3–5 and 9 as the story behind the table, ideally when the course reaches atomic structure or the heavy elements.
• Afterwards or for discussion: Chapter 10 is a good basis for a seminar or essay on whether there is a best form of the table.

Keep a copy of the periodic table to hand while reading, and use the book to understand the framework that descriptive and theoretical inorganic textbooks take for granted.