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Dalton's Atomic Model
Consists of a solid sphere. John Dalton was physicist, meteorologist, and chemist. Dalton poposed that atoms can't be divided and that they're extremely small. He also developed the law of multiple proportions. -
Rutherford's Atomic Model
Ernest Rutherford was from New Zealand but he worked at the University of Manchester in England. His model is the classic model of the atom, even though it's no longer considered and accurate representation. This model shows that an atom is mostly empty space, with electrons orbiting a fixed, positively charged nucleus in set, predictable paths. -
Thomson's Atomic Model
Also known as the "Plum pudding model". It is a model proposed by J.J. Thomson. It stablished that negative electrons occupied a region of space that was uniformly positevely charged (often considered as a kind of "soup" or "cloud" of positive charge). -
Bohr's Atomic Model
Niels Bohr received a Nobel Prize for this model. It says that the energy is absorbed or emitted when an electron moves from an orbit to another, and that the electrons that orbit the nucleus have a defined shape and energy and the energy levels have a different number of electrons. -
Schrödinger's Atomic Level
Also known as the "Mechanic quuantum model". It describes the wavy behavior of electrons. It is made up of 4 quantum numbers: Principal Quantum Number (n): Indicates size and energy levels from 1 to 7. Angular Momentum (l): Specifies the shape, with the sublevels, s p d and f. Magnetic Quantum Number (m): Specifies the orientation in space. Spin Quantum Number (s): Specifies the orientation of the spin.
