John Dalton

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In the vestibule of the Manchester Town Hall are placed two life-sized marble statues facing each other. One of these is that of John Dalton, by Chantrey; the other that of James Prescott Joule, by Gilbert. Thus honour is done to Manchester's two greatest sons - to Dalton, the founder of modern Chemistry and of the Atomic Theory, and the discoverer of the laws of chemical-combining proportions; to Joule, the founder of modern Physics and the discoverer of the law of the Conservation of Energy. The one gave to the world the final and satisfactory proof of the great principle, long surmised and often dwelt upon, that in every kind of chemical change no loss of matter occurs; the other proved that in all the varied modes of physical change no loss of energy takes place. Dalton, by determining the relative weights of the atoms which take part in chemical change, proved that every such change - whether from visible to invisible, from solid to liquid, or from liquid to gas - can be represented quantitatively by a chemical equation; and he created the Atomic Theory of Chemistry by which these changes are explained. Joule, by exact experiment, proved the truth of the same statement for the different forms of energy. —Sir Henry Roscoe, John Dalton and the Rise of Modern Chemistry. 1895.

John Dalton (1766-1844), an English scientist, considered one of the founders of modern chemistry, taught mathematics and physical sciences at New College, Manchester. Dalton inferred from experimental studies an atomic theory of matter, which he applied to a table of atomic weights and used in developing his law of partial pressures (Dalton's law). He was color-blind and studied that affliction, also known as Daltonism.

Another important achievement of Dalton's was his law of multiple proportions: If two elements form more than one compound, the weights in different compounds of an element are ratios of integral numbers. For instance, consider the elements nitrogen and oxygen. The element oxygen occurs in the compounds NO and NO₂. The ratio of oxygen weights (1:2) in these compounds contains the integral numbers 1 and 2. (Note that in modern chemistry the concept "weight", used by Dalton, is replaced by "number of atoms". Now we say that the ratio of numbers of O-atoms in different NO_x compounds is a rational number. Or, by extension of Dalton's law of multiple proportions, the subscripts m, n, k, ... in a compound A_mB_nC_k⋅⋅⋅ are integral numbers.) This law led Dalton to take the mass of the lightest element, hydrogen, as unit of atomic mass.

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