Editing Periodic table (electron configurations)

{{Periodic table (electron configuration)}}
* Configurations of elements 109 and above are not available. Predictions from reliable sources have been used for these elements.
* <span style="color:gray">Grayed out</span> electron numbers indicate subshells filled to their maximum.
* Bracketed noble gas symbols on the left represent inner configurations that are the same in each period. Written out, these are:
:: He, 2, [[helium]] : 1s<sup>2</sup>
:: Ne, 10, [[neon]] : 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup>
:: Ar, 18, [[argon]] : 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup>
:: Kr, 36, [[krypton]] : 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>10</sup> 4p<sup>6</sup>
:: Xe, 54, [[xenon]] : 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>10</sup> 4p<sup>6</sup> 5s<sup>2</sup> 4d<sup>10</sup> 5p<sup>6</sup>
:: Rn, 86, [[radon]] : 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>10</sup> 4p<sup>6</sup> 5s<sup>2</sup> 4d<sup>10</sup> 5p<sup>6</sup> 6s<sup>2</sup> 4f<sup>14</sup> 5d<sup>10</sup> 6p<sup>6</sup>
:: Og, 118, [[oganesson]] : 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>10</sup> 4p<sup>6</sup> 5s<sup>2</sup> 4d<sup>10</sup> 5p<sup>6</sup> 6s<sup>2</sup> 4f<sup>14</sup> 5d<sup>10</sup> 6p<sup>6</sup> 7s<sup>2</sup> 5f<sup>14</sup> 6d<sup>10</sup> 7p<sup>6</sup>
* Note that these electron configurations are given for neutral atoms in the gas phase, which are not the same as the electron configurations for the same atoms in chemical environments. In many cases, multiple configurations are within a small range of energies and the small irregularities that arise in the d- and f-blocks are quite irrelevant chemically.<ref name=Jorgensen>{{cite book |last=Jørgensen |first=Christian K. |date=1988 |title=Handbook on the Physics and Chemistry of Rare Earths |volume=11 |chapter=Influence of rare earths on chemical understanding and classification |pages=197–292 |doi=10.1016/S0168-1273(88)11007-6|isbn=9780444870803 }}</ref> The construction of the periodic table ignores these irregularities and is based on ideal electron configurations.<ref name=Jensen2009>{{cite journal|author1-link=William B. Jensen |last1=Jensen |first1=William B. |date=2009 |title=Misapplying the Periodic Law |url=http://www.che.uc.edu/jensen/W.%20B.%20Jensen/Reprints/170.%20Misapplying%20the%20Periodic%20Law.pdf |journal=Journal of Chemical Education |volume=86 |issue=10 |pages=1186 |doi=10.1021/ed086p1186 |bibcode=2009JChEd..86.1186J |access-date=16 May 2020|doi-access=free }}</ref>
* ''Note the non-linear shell ordering, which comes about due to the different energies of smaller and larger shells.''

== References ==
See list of sources at [[Electron configurations of the elements (data page)]].
{{reflist}}

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