Atomic Theory Timeline Quiz

Study Notes

John Dalton (1766 - 1844) introduced the Solid Sphere model in 1803, marking the transition from philosophical concepts to scientific theories.
Dalton's model presented atoms as dense and solid entities without internal structure or subatomic particles.

J.J. Thomson proposed the Plum Pudding model in 1897, describing atoms as positively charged spheres with electrons embedded within, akin to raisins in pudding.
This marked the first atomic model based on experimental evidence and quantitative observations, contributing to modern atomic theory's foundation.

Ernest Rutherford introduced the Nuclear model in 1911, asserting that atoms consist of a small, dense, positively charged nucleus with electrons orbiting around it, resembling planets in a solar system.
Rutherford's experiments revealed electrons as distinct particles, reshaping the understanding of atomic structure.

Niels Bohr advanced the Planetary model in 1913, proposing that electrons occupy quantized, discrete energy levels around the nucleus.
This model clarified the emission and absorption of energy by electrons during their transitions between energy levels, facilitating further atomic structure exploration.

Developed by Erwin Schrodinger in the 1920s, the Quantum model replaced definite orbits of electrons with wave functions, illustrating probability distributions for electron locations.
Schrodinger's work provided a comprehensive understanding of electron behavior, laying the groundwork for modern atomic theory and explaining phenomena in multi-electron atoms.

J.J. Thomson's work on the Plum Pudding model helped establish the idea of fundamental particles (electrons) within the atom.
Rutherford's Nuclear Model explained the behavior of alpha particles in the gold foil experiment, leading to the discovery of the nucleus.
Bohr's Planetary Model introduced the quantization of energy levels, which elucidated atomic spectra and the stability of atoms.
Schrodinger's Quantum mechanics emphasized the dual particle-wave nature of electrons and became the foundation for understanding atomic structure and behavior.

John Dalton (1766 - 1844) introduced the Solid Sphere model in 1803, marking the transition from philosophical concepts to scientific theories.
Dalton's model presented atoms as dense and solid entities without internal structure or subatomic particles.

J.J. Thomson proposed the Plum Pudding model in 1897, describing atoms as positively charged spheres with electrons embedded within, akin to raisins in pudding.
This marked the first atomic model based on experimental evidence and quantitative observations, contributing to modern atomic theory's foundation.

Ernest Rutherford introduced the Nuclear model in 1911, asserting that atoms consist of a small, dense, positively charged nucleus with electrons orbiting around it, resembling planets in a solar system.
Rutherford's experiments revealed electrons as distinct particles, reshaping the understanding of atomic structure.

Niels Bohr advanced the Planetary model in 1913, proposing that electrons occupy quantized, discrete energy levels around the nucleus.
This model clarified the emission and absorption of energy by electrons during their transitions between energy levels, facilitating further atomic structure exploration.

Developed by Erwin Schrodinger in the 1920s, the Quantum model replaced definite orbits of electrons with wave functions, illustrating probability distributions for electron locations.
Schrodinger's work provided a comprehensive understanding of electron behavior, laying the groundwork for modern atomic theory and explaining phenomena in multi-electron atoms.

J.J. Thomson's work on the Plum Pudding model helped establish the idea of fundamental particles (electrons) within the atom.
Rutherford's Nuclear Model explained the behavior of alpha particles in the gold foil experiment, leading to the discovery of the nucleus.
Bohr's Planetary Model introduced the quantization of energy levels, which elucidated atomic spectra and the stability of atoms.
Schrodinger's Quantum mechanics emphasized the dual particle-wave nature of electrons and became the foundation for understanding atomic structure and behavior.