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Due to its functional architecture, ADOMAH Periodic Table provides the most convenient and logical way of deriving electron configurations.

The ADOMAH PT, also known as Tetrahedral Periodic Table, reflects electron configuration of 120th element, just count number of elements in each column vertically and you will get number of electrons in electron shells:


Same thing can be done for any element with atomic number less than 120. Simply ignore all elements that have greater atomic number than the element you selected and count remaining elements in each vertical column (straight down).

For example, if you want to write electron configuration of Er(68), cross out elements 69 through 120, as shown on diagram below , and count all remaining elements in each vertical column. You will get: 2-8-18-30-8-2. (When you count the elements, ignore diagonal lines between the blocks and stay in vertical columns.) You can also divide the electrons in order of subshells s, p, d and f if you count all the elements that were not crossed out starting at the bottom of each column and going upward vertically:

1S2 2S2 2P6 3S2 3P6 3d10 4S2 4P6 4d10 4f12 5S2 5P6 6S2,

where first number in each group of three characters corresponds to electron shell (column number), the letter corresponds to the electron orbital (subshell) and the third number corresponds to number of electrons in that orbital.

If you wish to write the electron configuration in order of filling of the orbitals, follow the "cascades" and count the elements that were not crossed out, starting at the top of each cascade and going downward, along the slanted lines:

1S2 2S2 2P6 3S2 3P6 4S2 3d10 4P6 5S2 4d10 5P6 6S2 4f12.

This is so logical and simple ! Compare this with the standard or any other Periodic Table.

To start using this simple method of deriving electron configurations, print copy of the ADOMAH PT (PDF) HERE.


Not all electron configurations derived this way correspond to the lowest atomic energy levels. There are eighteen common exceptions to electron configurations for atoms in the lowest energy state, also called the ground state. Here they are:

Cr (..., 3d5, 4s1); Cu (..., 3d10, 4s1); Nb (..., 4d4, 5s1); Mo (..., 4d5, 5s1); Ru (..., 4d7, 5s1); Rh (..., 4d8, 5s1); Pd (..., 4d10, 5s0); Ag (..., 4d10, 5s1); La (..., 5d1, 6s2); Ce (..., 4f1, 5d1, 6s2); Gd (..., 4f7, 5d1, 6s2); Au (..., 5d10, 6s1); Ac (..., 6d1, 7s2); Th (..., 6d2, 7s2); Pa (..., 5f2, 6d1, 7s2); U (..., 5f3, 6d1, 7s2); Np (..., 5f4, 6d1, 7s2) and Cm (..., 5f7, 6d1, 7s2).

For further discussion on writing electron configurations in order of orbital filling refer to this blog by Eric Scerri.

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