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460 B.C. - 370 B.C.
Greek philosopher first to suggest atoms. His theory consisted of believing that atoms were visible and indestructible.

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1887-1961
He used Bohr's results to find the quantum mechanical model. This model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus. The model does not involve an exact path in which the electron takes around the nucleus unlike the Bohr model.

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1885-1962
Danish physicist and student of Rutherford proposed that an electron is found only in a specific circular path, or orbits, around the nucleus. Fixed energies is an electron that can have energy levels. The quantum of energy is the amount of energy required to move an electron from one level to another.

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1871-1937
Former student of Thomson, performed tests that led to The Rutherford Atomic Model. He proposed that the atom is mostly empty space that lacks defection of most alpha particles. The nucleus is the central core of an atom that is composed of protons and neutrons.

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1891-1974
English physicist confirmed the existence of yet another subatomic particle, the neutron. The neutron has a neutral charge, or no charge.

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1850-1930
Observed a cathode-ray tube and found rays traveling in the opposite direction to that of the cathode rays. The canal rays concluded that they were composed if positive particles, or protons.

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1856-1940
An English physicist that discovered the electron, which was found by experiments that involved passing electric current through gases at low pressure. The electrode and the anode became positive which directs the the cathode ray. The cathode ray is a glowing beam traveled from the cathode to the anode.

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1766-1844
Modern process of discovery regarding atoms began with Dalton. Dalton was a chemist and a school teacher. His theory consisted of experimental methods that transformed Democritus's ideas of an atom into a scientific theory. It resulted in the atomic theory.

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1868-1953
Robert carried out experiments to find the quantity of charge carried by an electron. It used this value and the charge-to-mass ratio of an electron measured by Thomson. An electron carries exactly one unit of negative charge and mass is 1/1840 the mass of hydrogen atom.