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Thompson discovered the atom what we might call the chocolate chip cookie model of a atom. He showed atoms as uniformly packed spheres of positive matter filled with negatively charged electrons. Thompson's model of the atom did not stick around for long.

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He showed it was impossible to determine both the exact position and speed of electrons as they move around a atom. The more we nail down the particle's position, the less we know about its speed.

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Bohr expanded on Rutherford's nuclear model. He stipulated that electrons orbit the nucleus at fixed energies and distances. Bohr's planetary model took center stage then encountered complications. Experiments showed that the electrons behave like waves, not being defined to a particular point in space.

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Rutherford described the atom as having a tiny, dense, and positively charged core called the nucleus. Rutherford established that the mass of the atom is concentrated in its nucleus. He concluded that atoms consisted largely of empty space with just a few electrons, while most of the mass was concentrated in the center.

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Dalton showed that common substances always broke down the same elements in the same proportions. He concluded that the various compounds were combinations of atoms of different elements, each of a particular size and mass. Atomic theory was then accepted by the scientific community.