Figure 6.26 illustrates the traditional way to remember the filling order for atomic orbitals. Electrons enter higher-energy subshells only after lower-energy subshells have been filled to capacity. Each added electron occupies the subshell of lowest energy available (in the order shown in Figure 6.24), subject to the limitations imposed by the allowed quantum numbers according to the Pauli exclusion principle. This procedure is called the Aufbau principle, from the German word Aufbau (“to build up”). Beginning with hydrogen, and continuing across the periods of the periodic table, we add one proton at a time to the nucleus and one electron to the proper subshell until we have described the electron configurations of all the elements. To determine the electron configuration for any particular atom, we can “build” the structures in the order of atomic numbers. The notation 3 d 8 (read "three–d–eight") indicates eight electrons in the d subshell (i.e., l = 2) of the principal shell for which n = 3.įigure 6.25 The diagram of an electron configuration specifies the subshell ( n and l value, with letter symbol) and superscript number of electrons.
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