Difference between revisions of "Electron subshell"
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| − | An '''electron subshell''' is a division of a larger [[electron shell]] with the same azimuthal [[quantum number]] based on energy levels. The number of electrons permitted in a subshell is equal to 2''l'' + 1.<ref>http://antoine.frostburg.edu/chem/senese/101/electrons/glossary.shtml</ref> Energy subshells identified by the angular momentum | + | An '''electron subshell''' is a division of a larger [[electron shell]] with the same azimuthal [[quantum number]] based on energy levels. The number of electrons permitted in a subshell is equal to 2''l'' + 1.<ref>http://antoine.frostburg.edu/chem/senese/101/electrons/glossary.shtml</ref> Energy subshells identified by the angular momentum quantum number, <math>l</math>. They can also be described using spectroscopic notation: |
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Revision as of 00:30, September 19, 2017
An electron subshell is a division of a larger electron shell with the same azimuthal quantum number based on energy levels. The number of electrons permitted in a subshell is equal to 2l + 1.[1] Energy subshells identified by the angular momentum quantum number, <math>l</math>. They can also be described using spectroscopic notation:
| Angular momentum quantum number | Spectroscopic notation | Spectroscopic name |
|---|---|---|
| 0 | s | Sharp |
| 1 | p | Principal |
| 2 | d | Diffuse |
| 3 | f | Fundamental |
Spectroscopic notation originates from before a quantum model of the hydrogen atom, where in the spectrum of hydrogen it was noticed that the lines had different shapes. Subshells of with an angular momentum number greater than 3 are represented by the letters after f, so <math>l=4</math> corresponds to the g subshell and so on.
Each subshell corresponds to a particular shape of the location in which electrons can be found, for example the s subshells take the shape of a sphere while the p subshells take the shape of a dumbbell. The number of electrons that can be held in each subshell varies, with s holding 2, p holding 6, d holding 10 and f holding 14. It can be seen that the maximum number of electrons a subshell can have is <math>4l+2</math>. Generally electrons around an atom are primarily divided in energy levels by shell and then subshell, although this is not always the case (for instance the 3d subshell is of a higher energy level than the 4s subshell).