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They also could not convince everybody, so atomism was but one of a number of competing theories on the nature of matter.
It was not until the 19th century that the idea was embraced and refined by scientists, when the blossoming science of chemistry produced discoveries that only the concept of atoms could explain.
In 1905, Albert Einstein proved the reality of these molecules and their motions by producing the first Statistical physics analysis of Brownian motion.
The Geiger–Marsden experiment Top: Expected results: alpha particles passing through the plum pudding model of the atom with negligible deflection. Thomson measured the mass of cathode rays, showing they were made of particles, but were around 1800 times lighter than the lightest atom, hydrogen.
In the early 1800s, John Dalton used the concept of atoms to explain why elements always react in ratios of small whole numbers (the law of multiple proportions).
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The protons and neutrons in the nucleus are attracted to each other by a different force, the nuclear force, which is usually stronger than the electromagnetic force repelling the positively charged protons from one another.
An illustration of the helium atom, depicting the nucleus (pink) and the electron cloud distribution (black).
The nucleus (upper right) in helium-4 is in reality spherically symmetric and closely resembles the electron cloud, although for more complicated nuclei this is not always the case.
This common pattern in chemistry suggested to Dalton that elements react in whole number multiples of discrete units—in other words, atoms.
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In the case of tin oxides, one tin atom will combine with either one or two oxygen atoms.The black bar is one angstrom ( An atom is the smallest constituent unit of ordinary matter that has the properties of a chemical element.
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