The law of definite proportions states that a chemical compound always contains its component elements in fixed ratio by mass, regardless of source or preparation method. He incorrectly assumed that all atoms of an element were absolutely identical, ignoring the existence of isotopes—atoms of the same element with different masses.
John Dalton's Atomic Theory Postulates and Core Assumptions
Dalton’s Revolutionary Postulates At the heart of Dalton’s model were several bold assertions that directly challenged the prevailing fluid view of matter. This led to the plum pudding model and eventually to Ernest Rutherford’s nuclear model, which identified a dense nucleus surrounded by electrons.
For instance, water is always composed of hydrogen and oxygen in a mass ratio of roughly 1:8. These advancements demonstrated that Dalton’s “indivisible” atom was, in fact, a composite system.
Dalton’s Revolutionary Atomic Postulates and Model
From Indivisible to Subatomic The discovery of the electron by J. 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.
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