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In atomic physics, the Bohr model or Rutherford–Bohr model was the first successful model of the atom. Developed from 1911 to 1918 by Niels Bohr and building on Ernest Rutherford 's nuclear model , it supplanted the plum pudding model of J J Thomson only to be replaced by the quantum atomic model in the 1920s.
Bohr dropped his work on the Thomson model in favor of Rutherford's nuclear model, developing the Rutherford–Bohr model over the next several years. Eventually Bohr incorporated early ideas of quantum mechanics into the model of the atom, allowing prediction of electronic spectra and concepts of chemistry.
The prevailing model of atomic structure before Rutherford's experiments was devised by J. J. Thomson. [1]: 123 Thomson had discovered the electron through his work on cathode rays [2] and proposed that they existed within atoms, and an electric current is electrons hopping from one atom to an adjacent one in a series.
Repulsive and attractive forces balance at ≈ 0.8 fm, and become maximally attractive at ≈ 1.0 fm, as illustrated in the diagram. [3] Because energy is required to separate them, the pair of nucleons are said to be in a bound state. The proton-neutron (p-n) bound state, or p-n pair, is stable and ubiquitous in baryonic matter. [24]
Modello atomico di Rutherford; Usage on it.wikibooks.org Scienze per la scuola media/L'atomo; Chimica per il liceo/Le grandezze fisiche e la loro misura; Chimica per il liceo/La struttura atomica, da Bohr al modello quantomeccanico; Chimica per il liceo/La struttura atomica, da Bohr al modello quantomeccanico/P; Usage on li.wiktionary.org ...
The Rutherford–Bohr model of the hydrogen atom After Bohr's use of Einstein 's explanation of the photoelectric effect to relate energy levels in atoms with the wavelength of emitted light, the connection between the structure of electrons in atoms and the emission and absorption spectra of atoms became an increasingly useful tool in the ...
The Rutherford–Bohr model of the hydrogen atom (Z = 1) or a hydrogen-like ion (Z > 1). In this model, it is an essential feature that the photon energy (or frequency) of the electromagnetic radiation emitted (shown) when an electron jumps from one orbital to another be proportional to the mathematical square of atomic charge (Z 2).
I created this file to be an SVG alternative to Image:Bohratommodel.png and Image:Bohr model Balmer 32.png. I did not draw the orbitals to scale like the latter diagram because I could not readily find information about the orbitals' radii. For some reason, the "+" on the nucleus is rendering off-centered. The SVG doesn't look like that.