Electron Configuration

When looking at a periodic table going to the right increases the atomic number and the # of electrons. This increase in electrons results in the valence (outermost) electrons shifting the structure of the atom. These valence shells are classifed into various subshells these include:
s (holds 2 valence electrons at max), p (holds 6 electrons at max), d (holds 10 electrons at max), f (holds 14 electrons at max), and g (holds 18 electrons at max).
After the first shell (row) p is used as well as s, after the second the d shell is used, after the third f and so on. after

Everytime one goes down a row the shell increases by one and is denoted by a # before the subshell for instance 1s or 3p and,
the number of electrons in a sub shell is denoted by a superscript of how many electrons here we will use ^ for instance 1s^2 2s^2 2p^6 3s^2 is magnesium at ground state.
One can also shorten the electron configuration by using the closest noble gas in brackets for instance for Mg I could've used [Ne] 3s^2. When writing for the d shell you have to go down one shell level and write that before d (this is due to the way in which electrons act in the d subshell) this is present for the rest of the subshells.

Practice finding the electron configuration of different elements and ions. Hover over for solutions.






Now try ions

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