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2. Bohr–Sommerfeld model - Wikipedia

   en.wikipedia.org/wiki/Bohr–Sommerfeld_model

   Orbitals of the Radium. (End plates to [1]) 5 electrons with the same principal and auxiliary quantum numbers, orbiting in sync. ([2] page 364) The Sommerfeld extensions of the 1913 solar system Bohr model of the hydrogen atom showing the addition of elliptical orbits to explain spectral fine structure.

3. Periodic table (electron configurations) - Wikipedia

   en.wikipedia.org/wiki/Periodic_table_(electron...

   The periodic table of electron configurations shows the arrangement of electrons in atoms, organized by increasing atomic number and chemical properties.

4. Isotope - Wikipedia

   en.wikipedia.org/wiki/Isotope

   A nuclide is a species of an atom with a specific number of protons and neutrons in the nucleus, for example, carbon-13 with 6 protons and 7 neutrons. The nuclide concept (referring to individual nuclear species) emphasizes nuclear properties over chemical properties, whereas the isotope concept (grouping all atoms of each element) emphasizes chemical over nuclear.

5. Bohr model - Wikipedia

   en.wikipedia.org/wiki/Bohr_model

   The Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell model. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics and thus may be considered to be an obsolete scientific theory.

6. Electron configuration - Wikipedia

   en.wikipedia.org/wiki/Electron_configuration

   For example, chromium hexacarbonyl can be described as a chromium atom (not ion) surrounded by six carbon monoxide ligands. The electron configuration of the central chromium atom is described as 3d 6 with the six electrons filling the three lower-energy d orbitals between the ligands. The other two d orbitals are at higher energy due to the ...

7. Lewis structure - Wikipedia

   en.wikipedia.org/wiki/Lewis_structure

   The nitrogen atom has only 6 electrons assigned to it. One of the lone pairs on an oxygen atom must form a double bond, but either atom will work equally well. Therefore, there is a resonance structure. Tie up loose ends. Two Lewis structures must be drawn: Each structure has one of the two oxygen atoms double-bonded to the nitrogen atom.