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Atomic Theory is the product of hundreds if not thousands of scientists' different insights.  Some of the beginning Atomic Theories like that of Leucippus were blind guesses.  Leucippus and Democritus came up with the general idea of atoms. They thought the world was made up of two fundamental elements, atoms, and void. In summary, they thought that since atoms were the smallest unit of matter, they were indivisible. As time continued on there were theories from the results of careful experimentation, and work continued on by series of scientists.

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The following significant advances in atomic theory took around 2300 years to materialize. Antoine Lavoisier, a French scientist first formulated the idea of conservation of mass, which states that despite a change in shape or form, matter retains its original mass. Another big step, was when James Dalton, an English professor, discovered that elements are individual packets of matter. In the 1870s scientists used discharge tubes, which are essentially gas-filled tubes with electrodes at either end that emit light when an electrical current flows through them, to investigate the materials that things were made of. Eugen Goldstein, a German physicist, discovered in 1886 that the tubes also produced light from the positive electrode, or, more specifically, a ray that was traveling in the opposite direction, indicating that matter must also have a positive charge. Then, English physicist J.J. Thompson carried out additional research using discharge tubes. He discovered that the cathode "rays" were actually very light, extremely small negatively-charged particles by measuring how much heat they produced, and how much they could be bent by magnets and other things. He referred to them as "corpuscles"; we refer to them as "electrons."

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Thomson proposed the plum pudding model of the atom, which contained negatively charged electrons inside of a positively charged "soup." New Zealander Ernest Rutherford made the next significant advancement in 1909.  In the now-famous experiment, alpha particles were seen to scatter away from a gold foil in the reverse direction. In actuality, though, some of the particles were bent sharply and occasionally almost straight backward. The only way to explain this was that an atom's entire positive charge, which would deflect an alpha particle, must be concentrated in a very small region that he dubbed "the nucleus." Rutherford correctly surmised that the majority of an atom is made up of void space.

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The findings of Rutherford's gold foil experiment were published in 1911. To study with Rutherford, Bohr traveled to England. Bohr eventually realized Rutherford's atomic model could be used to illustrate these mathematical ideas. His evaluation of the gold foil experiment and calculations based on the percentage of throughput for alpha particles. Lead him to believe that each orbit (orbital, shell) has a fixed energy and that electrons move in fixed orbitals (shells) and not anywhere else. Theoretical physicist Werner Heisenberg from Germany made the important mathematical discovery that it is impossible to determine with absolute certainty both the momentum of an electron or any subatomic particle and its precise location.

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It suggests that electrons were neither particles nor waves, but rather had characteristics of both. According to this line of reasoning, the configuration of electrons surrounding a nucleus could only be explained in terms of chance. In other words, there are some places where it is considerably more likely to find an electron. These areas are referred to as "orbitals." Also known as the "cloud model."