An Elementary Study of Chemistry

The Story

An Elementary Study of Chemistry opens by presenting itself as a practical textbook, built to be clear, teachable, and moderate in its claims. The authors do not try to astonish the reader with originality; instead, they explain that they want an elementary course that still includes real chemical principles, even when those principles can only be stated in partial form. The preface sets the tone for the whole book: chemistry is not treated as a list of isolated facts, but as a system of laws, reactions, measurements, and methods of reasoning that the student can actually follow. From the outset, the book insists that elementary study should not mean empty simplification.

From there the book moves through the foundations of chemical behavior, and much of its argument is built around oxygen. Oxygen appears as a gas essential to respiration, to decay, and to some medical treatments. The treatment of decay is especially important because it shows the book’s habit of joining ordinary life to chemical process: decay is described as oxidation carried on with the help of bacteria, turning dead plant and animal matter into harmless substances. The discussion then turns to ozone, a modified form of oxygen produced by sparks or by certain chemical reactions. Ozone is presented as more active and more dangerous than ordinary oxygen, with a sharp odor, explosive tendencies, and enough chemical power to be used in manufacturing. This section widens the reader’s view of what “oxygen” means by showing that even a familiar element can exist in forms with very different properties.

The book then turns to measurement and proof. The composition of water is established through experimental results by Berzelius, Dumas, and Morley, and the comparison of these results demonstrates the care required in chemistry. Water is not simply assumed to be a compound of hydrogen and oxygen; it is shown, by repeated experiment, to contain those elements in a fixed ratio. The text uses these studies to make a larger point: chemical composition is known by experiment alone, and the value of a result depends on the purity of materials, the skill of the investigator, and the accuracy of the method. This emphasis on quantitative proof carries into later sections on atomic and molecular weights. The book explains proportions, formulas, and reactions by calculating how much of one substance combines with or is obtained from another, and it uses water, mercuric oxide, zinc, and sulphuric acid as working examples. Chemistry here becomes a discipline of relation and weight, not merely of observation.

The next major movement is into solutions and physical change. The book defines saturated and supersaturated solutions, then explains how dissolved substances distribute themselves through liquids and how solutes raise boiling points. These topics seem modest, but they expand the reader’s sense of chemistry beyond dramatic reactions. A solution is not an inert mixture; it is a condition of equilibrium that changes with temperature and concentration. The same practical attention appears in the discussions of gases and industrial processes. Methane is shown as a mine gas, dangerous in explosive mixtures with air, and Sir Humphry Davy’s safety lamp appears as a response to that danger. Acetylene follows as another useful gas, made from calcium carbide and used for brilliant white light. The book is repeatedly interested in substances not just as formulas but as things people use, handle, fear, and manufacture.

The chemistry of nitrogen and sulfur deepens this practical orientation. Ammonia is prepared in the laboratory from ammonium chloride and sodium hydroxide or calcium hydroxide, but the text also explains the commercial method, in which ammonia is recovered from gas liquor produced in coal distillation. Sulphurous acid, formed when sulphur dioxide dissolves in water, is described through its acid, reducing, bleaching, and antiseptic properties. It bleaches paper and straw goods, preserves food, and arrests fermentation. The book then moves to sulphur trioxide and the later steps toward sulphuric acid chemistry. What links these sections is the sense that chemical properties are not abstract labels but powers that matter in trade, preservation, cleaning, and industry.

The treatment of fluorine and hydrofluoric acid provides one of the book’s most concrete demonstrations of chemistry as an interaction between matter and material culture. Hydrofluoric acid is shown attacking silicon dioxide, which is why it etches glass and cannot be stored in glass vessels. The book gives a practical method for etching designs on glass, where the acid removes the luster and makes the exposed pattern opaque. That same combination of explanation and use runs through the later discussion of carbon compounds. Methane’s structure leads to its explosive danger; acetylene’s flame gives light; and the fuel and lighting properties of such gases place them within a larger world of technology.

The second half of the book broadens further into metallurgy and industrial chemistry. It discusses the periodic group containing antimony, bismuth, and related elements, noting their alloying uses and low melting points. Bismuth is especially notable for its role in low-melting alloys like Wood’s metal. Sodium hydroxide is then introduced through the Acker process, with a detailed technical description of a furnace that produces chlorine and caustic soda. The text explains how melted lead serves as a cathode, how sodium alloys with it, and how steam converts the alloy into sodium hydroxide and hydrogen. This is one of the book’s most vivid examples of chemistry on the industrial scale: not a bottle reaction, but a managed furnace operation with chambers, pipes, and a flowing product stream.

Calcium carbonate, cement, and aluminum compounds extend this industrial focus into building and materials. Calcium carbonate appears in limestone, chalk, marble, coral, pearls, and shells, tying geology, biology, and construction together. The text then shows how cement, concrete, and artificial stone become central building materials. Aluminium oxide and hydroxide are discussed next, not only as compounds but as mineral forms such as corundum, emery, sapphire, and ruby. The book stresses hardness, purification, and use in cutting, grinding, and aluminium production. Chromium follows with its resistance to air, its compounds, and its role in ferrochromium and steel work. Again the pattern is clear: the element is important because of the properties that make it useful in the world.

Copper is treated with similar breadth. The book names its ores, explains how sulphide ores are roasted and converted into crude matte, and describes later refining through a process resembling Bessemer steelmaking. Copper is not only a metal in itself; it is the result of a chain of transformations from ore to refined product. The same is true of sodium compounds and hydrolysis, where salts react with water to yield basic or acidic solutions. At the far end of the book’s chemical landscape are ethereal salts, glycerin nitrates, fats, and nitroglycerin. The text explains that some acids react with alcohols to form compounds with hydrocarbon radicals in place of metals, and from there it moves to nitroglycerin and dynamite. The final pages, including tables of atomic weights and gas densities, confirm the book’s underlying purpose: to give students a framework in which the behavior of matter can be measured, compared, named, and used.

The People

• William McPherson is the guiding voice behind the book. He wants an elementary text that is simple without being shallow, modern without being reckless, and teachable without sacrificing important principles. What stands in his way is the usual tension in introductory science: how to include real laws, measurements, and exceptions without overwhelming beginners. He ends by offering chemistry as a disciplined way of seeing, not just a list of facts.

• The student is the implied central learner throughout. This figure wants understanding that can be used in later study as well as in ordinary life. What stands in the way is the abstraction of chemical law and the difficulty of connecting formulas to real substances. The book repeatedly helps this student by moving from experiments, to proportions, to industry, and finally to materials they can recognize.

• Oxygen functions almost like a character because the book keeps returning to its roles. It wants to be understood not just as a gas in the air but as a purifier, a support for life, and a participant in decay and combustion. What stands in the way is the reader’s tendency to think of it as simple and uniform. The book changes that view by showing ozone, oxidation, and industrial use.

• Ammonia is one of the book’s practical working substances. It wants to be explained both in the laboratory and in commerce, since it comes from ammonium salts in one setting and coal-gas operations in another. Its obstacle is instability: ammonium hydroxide breaks down into ammonia and water, and the compound must be handled as a process rather than a thing.

• Hydrofluoric acid stands out as a destructive and specialized chemical. It wants to act on silicon dioxide and glass, and it is defined by that action. What stands in its way is containment, since it cannot be stored in ordinary glass vessels. The book gives it a place in etching and in warnings about danger.

• Copper represents industrial transformation. It wants to be refined from ore into metal, and the text tracks it through roasting, smelting, matte, conversion, and refining. Its obstacle is the complexity of sulphide ores. By the end, copper becomes a lesson in how chemistry reorganizes mining and metallurgy.

In Its Own Voice

The book’s preface states its intention plainly:

“it has been their aim to prepare a text-book constructed along lines which have become recognized as best suited to an elementary treatment of the subject.”

In its discussion of water, it insists on experiment as the basis of knowledge:

“water must be regarded as a compound containing hydrogen and oxygen in the proportion of 1 part by weight of hydrogen to 7.94 parts by weight of oxygen.”

When it turns to practical chemistry, it describes hydrofluoric acid’s effect on glass with directness:

“Wherever the hydrofluoric acid comes in contact with the glass it acts upon it, destroying its luster and making it opaque, so that the exposed design will be etched upon the clear glass.”

What It's Really About

At its core, the book argues that chemistry is a science of lawful relationships made visible through careful work. It does not present substances as isolated curiosities. Instead, every chapter ties properties to composition, composition to measurement, and measurement to use. Water becomes a proof case for experimental method. Ozone, sulphurous acid, hydrofluoric acid, methane, acetylene, ammonia, sodium hydroxide, and copper each become examples of how a substance can be understood only by tracing how it behaves, how it is prepared, and what it does in contact with other matter. The book’s deepest habit is to connect the microscopic and the practical without treating either as secondary.

That impulse is especially clear in the way it handles equilibrium, reversibility, and industrial process. Saturated and supersaturated solutions are not introduced as abstract theory alone; they help the reader understand how matter behaves when conditions change. The reversible formation of sulphurous acid, the equilibrium of solutions, and the transformations in the Acker process all teach the same lesson: chemistry is change under constraint, not just transformation in isolation. Even when the book keeps to elementary language, it returns to underlying order.

Another major theme is the unity of nature across ordinary categories. Calcium carbonate appears in limestone, chalk, shells, coral, pearls, and marble; aluminium oxide appears as corundum, emery, sapphire, and ruby; coal becomes a source of ammonia; and hydrofluoric acid makes use of the very properties that make glass a useful material. The book keeps collapsing boundaries between minerals, organisms, household materials, and industrial products. In doing so, it suggests that chemistry is the study of continuity in matter, where familiar things are made of the same elements as rare ones, and where usefulness often depends on the same reactions that make substances dangerous.

The tone also matters. The book is confident but restrained. It does not treat chemistry as magic, and it does not flatten difficulty. Instead, it acknowledges that some laws cannot be fully deduced in an elementary setting, while still insisting that students can understand their essential features. That balance is one of the book’s real themes: science should be rigorous without becoming inaccessible. The result is a text that trains the reader to think in ratios, reactions, and processes while also showing why those things matter in the wider world.

Why Read It Today

Readers who like the history of science, the logic of experiments, or the material side of modern life will find a great deal here. The book has a clear, patient rhythm: define, illustrate, calculate, and then show the practical consequence. It is especially rewarding if you want to see how chemistry was taught when textbook authors still expected students to work through methods step by step and when industrial examples were part of the lesson rather than an afterthought.

What stays with you is the way the book makes familiar substances newly specific. Oxygen is not just air. Water is not just a liquid. Limestone is not just rock. Each becomes a node in a network of measurement, use, and transformation. The industrial passages, especially on sodium hydroxide, copper, cement, and explosives, give the book a strong historical feel. It is interested in the world built by chemistry as much as in chemistry itself.

Its difficulty is also part of its character. The notation is old-fashioned, the tables and formulas assume patience, and some sections move quickly through technical detail. The book belongs to a period when chemical education still assumed a willingness to learn by repeated example. That can feel dense, but it also gives the text its usefulness. It reads like a working introduction to a science that is simultaneously theoretical, industrial, and everyday.