Remember, the order of filling the orbital goes from the lowest energy level to the highest considering the position of sublevels ( s, p, d, f) as well. And because each orbital can only take a maximum of two electrons, there can only be a maximum of two electrons in any s sublevel, 6 electrons in the p subshell, 10 in the d, and 14 in the f sublevel.Įverything we discussed in the article about electron configurations holds true, so if you have forgotten things like the Aufbau Principle, and the orbital map to easily recognize what orbitals a given element has, check the linked article.
Next, remember the number and capacity of s, p, d, and f are energy sublevels There can only be 1 s orbital in the given energy level, 3 p orbitals, 5 d orbitals, and 7 f orbitals. So, if the electrons are in the same orbital, they must have the same n, l, m l, and therefore, the only one that can be different is the m s which is the spin of the electron shown by the position of the arrow. This is according to the Pauli exclusion principle which states that no two electrons in an atom can have the same four quantum numbers. Notice that if there are two electrons in the orbital, the arrows must be shown in opposite directions which indicates that they must have opposite spins. Just like in writing electron configurations, remember that each orbital, whether it is s, p, d, or f can accommodate two electrons at most, so you cannot put more than two arrows in a box. This is a way of showing the electron configuration of the atom.įor example, the orbital diagram of Li can be shown as: Each box represents one orbital, and each arrow indicates one electron. In orbitals diagrams, the orbitals are shown as boxes, and the electrons in them as arrows pointing up or down.
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