![]() ![]() Figure 2 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 4 in section 7.3), subject to the limitations imposed by 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. Electron configuration of hydrogen is 1s 1, which indicates there is one electron in the s subshell of the principal shell n=1. The notation 3 d 8 (read “three–d–eight”) indicates eight electrons in the d subshell of the principal shell for which n = 3. ![]() A superscript number that designates the number of electrons in that particular subshell.įor example, the notation 2 p 4 (read “two–p–four”) indicates four electrons in a p subshell with a principal quantum number ( n) of 2. ![]()
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