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An '''electron subshell''' is a division of a larger [[electron shell]] based on energy levels. Energy subshells are denoted by the letters s, p, d, f with each letter indicating a higher energy region. 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. 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).
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:
{| class="wikitable"
|-
!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).
==See also==
==See also==
* [[Orbital]]
* [[Orbital]]
[[Category:Chemistry]]
==References==
{{Reflist}}
[[Category:Subatomic Physics]]