Therefore, we have a diagonal rule for electron filling order in the different subshells using the Aufbau principle. So, all these are basics of How filling of electrons will be done in different subshells, obviously, you don’t have so much time for writing electron configuration by using so many rules. ⇒ For two different subshells having same (n + l) value, then the subshell with lower value of n has lower energy. ⇒ Lower the value of (n + l) for an subshell, the lower its energy, hence, it will be filled first with electrons. Generally, (n + l) rule is used to predict the energy level of subshells. Now, the electron configuration of an atom can be built by filling the electrons in a lower energy subshell first then higher, higher, and higher. So, in short, the s subshell can hold a maximum of 2 electrons(1 orbital), the p subshell can hold 6 electrons(3 orbitals), the d subshell can hold 10 electrons(5 orbitals), and the f subshell can hold at most 14 electrons(7 orbitals). These subshells can hold a maximum number of electrons on the basis of a formula, 2(2l + 1) where ‘l’ is the azimuthal quantum number. Simply understand that there are commonly four different types of subshells – s, p, d, and, f. For example, the 1s orbital will be filled first with electrons before the 2s orbital.In short, the electrons will be filled in the orbital in order of their increasing energies. It states that the orbital with the lowest energy level will be filled first before those with high energy levels.The Aufbau rule simply gives the order of electrons filling in the orbital of an atom in its ground state.The word ‘Aufbau’ in German means ‘building up’.
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