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Transactions of the Royal Society of Edinburgh 15, pp.265–276. Original historical experimental report. The publisher's extract describes very pure waters, carbonate deposits and modification of attack by dissolved salts; online publication in 2013 is the digitization date, not the historical date.
John G. Murphy wrote a nineteenth-century chemistry review for medical students. Its treatment of nitric oxide uses an older formula convention and an elemental gas-volume comparison, documenting how chemical notation and quantitative interpretation have changed.[ref]
Author identified on the title page of Review of Chemistry for Students by John G. Murphy. No further biographical identity is inferred from the name.
A class of organic materials that are solid or plastic at ordinary temperatures and melt on heating. Candle waxes can include hydrocarbons, esters and mixtures; paraffin wax is one example.
Lead acetate usually denotes lead(II) acetate, , often supplied as a hydrate. Two singly charged acetate ions balance lead(II).
Mercury(II) chloride is , with mercury in oxidation state . Its bonding and coordination behavior are not captured by treating it as elemental mercury mixed with chloride.
It differs from mercury(I) chloride, , which contains a mercury-mercury bonded dimeric cation. The Roman numeral therefore distinguishes different compounds and electronic structures.
Tannic acid refers to a gallotannin material containing multiple galloyl-derived groups, often based on a sugar core. Commercial material need not be one chemically uniform molecule with a unique molecular mass.
Its many oxygen-containing groups support hydrogen bonding and interaction with proteins and metal ions. This makes it a useful example of a natural polyphenolic material whose collective binding behavior depends on more than one isolated functional group.
Turpentine is a volatile mixture of terpenes obtained from plant resin, commonly containing substantial pinene components. It is therefore a variable-composition material rather than one pure compound.
Its ability to dissolve many hydrophobic substances follows from the molecular character of its components. Composition and oxidation during storage can change its properties, so one fixed molecular formula cannot adequately specify turpentine.
Monosodium urate is a sodium salt of uric acid, often encountered as the monohydrate. Its urate ion is chemically distinct from neutral uric acid.
Crystal formation depends on solution composition and saturation. This makes it an example of how acid-base speciation and solubility combine to determine whether a biological solute remains dissolved or forms a solid.
Potassium sulfate is the ionic chemical compound . Two singly charged potassium ions balance one doubly charged sulfate ion.
The formula illustrates electroneutrality in an ionic material. On dissolution, the formula-unit ratio must be distinguished from the total concentration of separate dissolved ions.
Benzoic acid is , an aromatic carboxylic acid. Deprotonation gives benzoate, whose negative charge is delocalized over the two oxygen atoms of the carboxylate group.
Its combination of an aromatic ring and an acid group makes it useful for comparing hydrophobic interactions with acid-base behavior. Changing the solution pH changes the balance between neutral benzoic acid and its charged conjugate base.
Camphor is a bicyclic ketone with formula . Its rigid carbon framework and stereochemistry make it a useful example of how three-dimensional structure influences reactions at a carbonyl group.
It is also a familiar volatile natural product with a characteristic odor. The molecular formula alone does not describe its bridged skeleton or distinguish its enantiomers.
Potassium acetate is the salt , containing potassium ions and the conjugate base of acetic acid. Its dissolution separates these ions into solution.
Potassium citrate is a potassium salt of citric acid; fully neutralized tripotassium citrate contains the citrate ion . Hydrated forms also occur.
Because citric acid can lose three protons, the extent of neutralization must be specified. Its citrate component participates in acid-base equilibria and can coordinate metal ions.
Potassium tartrate is a potassium salt of tartaric acid. The fully neutralized form contains two potassium ions per tartrate dianion, while potassium hydrogen tartrate retains one acidic hydrogen.
These names describe different stoichiometries and acid-base behavior. Hydration state and stereochemical form can also matter when specifying a sample.
Ferrous sulfate is iron(II) sulfate, , occurring in several hydration states. The common heptahydrate contains seven waters of crystallization per formula unit.
Ferrous carbonate is iron(II) carbonate, , with iron in oxidation state . The mineral siderite has this composition.
Its reaction with acid consumes carbonate and releases carbon dioxide. Distinguishing the iron oxidation state matters because oxidation can transform the material into chemically different iron(III)-containing products.
Bismuth subsalicylate is a bismuth-containing salicylate material in which bismuth-oxygen bonding connects organic salicylate units with inorganic structural features. The word subsalicylate does not describe a simple molecule made by attaching one isolated salicylate to a free bismuth atom.
Its identity illustrates the importance of coordination and extended structure in metal-containing compounds. A compact empirical formula can record average composition without displaying all of the bonded framework.
Chemical breakdown caused by heating. A balanced chemical equation does not by itself determine the decomposition rate or every possible pathway.
Pinned article: Introduction to the OurBigBook Project
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