Three instances can be constructed that perform not follow the Octet Rule, and also as such, lock are well-known as the exception to the Octet Rule. Complying with the Octet ascendancy for Lewis Dot frameworks leads to the most accurate depictions of stable molecular and atomic structures and because of this we always want to usage the octet rule when drawing Lewis period Structures. However, that is difficult to imagine the one rule might be followed by every molecules. There is always an exception, and also in this case, three exceptions. The Octet rule is violated in these 3 scenarios:

as soon as there are an odd number of valence electrons when there room too couple of valence electrons when there space too plenty of valence electrons

Reminder: always use the Octet preeminence when illustration Lewis period Structures, these exceptions will certainly only take place when necessary.




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Exception 1: species with Odd numbers of Electrons

The first exception to the Octet dominance is once there are an odd variety of valence electrons. An example of this would be the nitrogen (II) oxide molecule (\(NO\)). Nitrogen atom has 5 valence electrons while the oxygen atom has actually 6 electrons. The complete would it is in 11 valence electrons to be used. The Octet rule for this molecule is fulfilled in the above example, but that is v 10 valence electrons. The critical one walk not understand where to go. The lone electron is dubbed an unpaired electron. Yet where should the unpaired electron go? The unpaired electron is usually put in the Lewis Dot structure so that each element in the structure will have the lowest formal charge possible. The formal fee is the viewed charge ~ above an individual atom in a molecule once atoms do not add equal numbers of electron to the bond they participate in. The formula to uncover a formal charge is:

Formal Charge= <# the valence e- the atom would have actually on that own> - <# of lone pair electron on that atom> - <# the bonds the atom participates in>

No formal fee at all is the many ideal situation. An example of a stable molecule v an odd variety of valence electrons would certainly be nitrogen monoxide. Nitrogen monoxide has actually 11 valence electrons (Figure 1). If friend need more information around formal charges, watch Lewis Structures. If we were to consider the nitrogen monoxide cation (\(NO^+\) through ten valence electrons, climate the adhering to Lewis framework would be constructed:

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Figure 1. Lewis dot framework for the \(NO^+\) ion through ten valence electrons.

Nitrogen normally has 5 valence electrons. In figure 1, it has two lone pair electrons and also it participates in 2 bonds (a double bond) through oxygen. This results in nitrogen having actually a formal charge of +1. Oxygen normally has six valence electrons. In figure 1, oxygen has 4 lone pair electrons and it participates in 2 bonds v nitrogen. Oxygen therefore has a formal fee of 0. The in its entirety molecule here has a formal charge of +1 (+1 because that nitrogen, 0 for oxygen. +1 + 0 = +1).

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However, if we add the eleventh electron come nitrogen (because we desire the molecule to have actually the lowest complete formal charge), the will carry both the nitrogen and also the molecule"s overall charges to zero, the many ideal formal fee situation. That is specifically what is done to get the exactly Lewis framework for nitrogen monoxide: