The law of multiple proportions explains that when two elements form more than one compound, the masses of one element that combine with a fixed mass of the other are in ratios of small whole numbers. Niels Bohr later refined this by introducing quantized electron orbits.
Dalton Atomic Theory Chemical Reactions: Explaining Fixed Ratios and Indivisible Atoms
Dalton sought to explain why elements combine in fixed ratios, why gases exhibit simple weights when they react, and why substances cannot be divided indefinitely. He also failed to account for the existence of subatomic particles such as electrons, protons, and neutrons, believing the atom to be a featureless, indivisible sphere.
These atoms of a given element are identical in mass and properties, while atoms of different elements possess distinct masses and characteristics. His atomic theory was not a single revelation but a collection of testable principles designed to impose order on the chaotic diversity of chemical observations, effectively turning chemistry into a quantitative science.
Dalton Atomic Theory Chemical Reactions: Explaining Fixed Ratios and Indivisible Atoms
Because atoms are neither created nor destroyed in a chemical reaction, the total mass of the reactants must equal the total mass of the products. The atom acted as a fundamental accounting unit, ensuring that matter persisted through transformations.
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