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The Greek philosopher Democritus, had believed that matter was made by tiny indivisible particles, believing that it was impossible to be able to go any further. His atomic model was not based on any scientific evidence.

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John Dalton had believed that atoms of the same element were equal in size and mass; atoms of different elements were the opposite. The model is represented as a spherical particle. In his eyes it was considered the smallest entity of matter. His model was seen differently in comparison to Democritus as the model had a uniformed composition throughout. His atom was faulty seeing how the atom could be further divided, not taking subatomic particles into account.

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J.J. Thompson, founder of the Plum Pudding Model took things to the next level when introducing electrons into the atomic model. He had believed that all atoms were made of small negative charges; electrons simply floating around in the sea of positive matter.  His model represented a Plum Pudding, but is best represented as a Chocolate Chip Cookie in the modern day. The "chocolate chips" represent the electrons while the rest of the cookie is considered the "sea of positive matter". His way of discovering the electrons was through an experiment, using a tube/generator with two plates. One with a (+) charge and one with a (-) charge. He came to the conclusion that electrons had a negative charge, seeing how it moved to the positive plate (opposites attract). This atomic model was thrown aside for a reason, Thompson had no explanation for the electrons; only mentioned that they had existed.

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Ernest Rutherford created the "Nuclear Model", the most popular one to this day when brought up the topic of envisioning an atom. The model consists of several rings, each orbiting the center (nucleus) at an equal distance. Within those rings, are where electrons are found. His way of discovering this was through an experiment called the "Gold Foil Experiment". The experiment consisted of using a sheet of gold foil and firing it with alpha particles. He came to the discovery that the atom's majority was empty space, allowing the atom's to pass right through the gold foiled sheet. From the constant reaction of reflection and deflection the gold foil had with the atoms he came to a conclusion; the nucleus was small, dense, had a positive charge, and was the focal point for mass. A limitation from this model was that Rutherford had never mentioned the arrangement of the electrons. Instead, he simply stated that they orbited around the nucleus.

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The Planetary model lives up to its name, it's appearance quite similar to our solar system. While Bohr's Planetary model was in fact similar to Rutherford's Nuclear model; with the same idea of the nucleus and the electrons around it, there was a difference. That difference being that the electrons in Bohr's model were positioned in predictable orbital patterns, something Rutherford did not include in his own. The experiment that Bohr took into account while making his own model was Rutherford's, explaining the similarity. Bohr soon came to the conclusion that the closer the electrons ((-) charged) were to the nucleus, the weaker/less energy the electron contained. His model was soon rejected after years due to it's inaccuracy. Despite this model being another huge step like Rutherford's the model did not accurately depict how electrons do not emit electromagnetic radiation; let alone mention it.

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This model simply expanded on the Planetary model's observations and ideas. Erwin Schrodinger added on to the idea; all electrons in atoms existed in orbitals. He went to further explain that orbitals were "regions" in which electrons were most likely to be found; at least, the majority of the time.