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History of the Atomic Model
1 months ago
J.J. Thompson showed atoms as evenly spaced spheres of positive matter filled with negatively charged electrons.
John Dalton showed that common substances always broke down into the same proportions and that the various compounds were combinations of atoms of different elements that couldn't be created or destroyed.
Ernest Rutherford concluded that atoms consisted largely of empty space with just a few electrons, while most of the mass was concentrated in the centre, which he named the nucleus.
Using Niels Bohr's planetary model, experiments showed that rather than simply being discrete particles, electrons simultaneously behaved like waves, not being confined to a particular point in space.
Erwin Schrödinger found that his quantum mechanical model did not define the exact path of an electron, but rather, predicts the odds of the location of an electron, the model is also portrayed as a nucleus surrounded by an electron cloud. The probability of finding an electron is greatest in the most dense part of the cloud, while the electron is less likely to be found in a less dense area of the cloud.
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