Three situations can be built that execute not monitor the Octet Rule, and as such, they are recognized as the exceptions to the Octet Rule. Following the Octet ascendancy for Lewis Dot structures leads come the many accurate depictions of secure molecular and atomic structures and also because the this we always want to usage the octet dominance when illustration Lewis period Structures. However, it is hard to imagine that one rule could be complied with by all molecules. Over there is constantly an exception, and also in this case, 3 exceptions. The Octet dominion is violated in these 3 scenarios:

as soon as there room an odd number of valence electrons when there space too couple of valence electrons once there space too many valence electrons

Reminder: always use the Octet dominance when illustration Lewis period Structures, these exceptions will only occur when necessary.

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Exception 1: varieties with Odd number of Electrons

The an initial exception to the Octet ascendancy is as soon as there room an odd number of valence electrons. An instance of this would be the nitrogen (II) oxide molecule (\(NO\)). Nitrogen atom has 5 valence electrons while the oxygen atom has 6 electrons. The complete would it is in 11 valence electrons to it is in used. The Octet dominance for this molecule is fulfilled in the above example, yet that is with 10 valence electrons. The last one does not recognize where to go. The lone electron is dubbed an unpaired electron. However where need to the unpaired electron go? The unpaired electron is usually inserted in the Lewis Dot structure so the each facet in the structure will have the lowest formal fee possible. The formal fee is the viewed charge on an individual atom in a molecule as soon as atoms perform not contribute equal numbers of electrons to the bond they participate in. The formula to discover a formal charge is:

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

No formal charge at all is the most ideal situation. An example of a secure molecule through an odd number of valence electrons would be nitrogen monoxide. Nitrogen monoxide has actually 11 valence electron (Figure 1). If friend need an ext information around formal charges, check out Lewis Structures. If we were to think about the nitrogen monoxide cation (\(NO^+\) v ten valence electrons, then the following Lewis framework would it is in constructed:

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

Nitrogen usually has five valence electrons. In number 1, it has actually two lone pair electrons and it participates in 2 bonds (a twin bond) through oxygen. This outcomes in nitrogen having actually a formal charge of +1. Oxygen typically has 6 valence electrons. In figure 1, oxygen has four lone pair electrons and it participates in two bonds v nitrogen. Oxygen as such has a formal fee of 0. The overall molecule here has actually a formal charge of +1 (+1 because that nitrogen, 0 for oxygen. +1 + 0 = +1).

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However, if we include the eleventh electron to nitrogen (because we want the molecule to have the lowest complete formal charge), it will bring both the nitrogen and also the molecule"s overall charges to zero, the many ideal formal fee situation. The is precisely what is excellent to acquire the exactly Lewis structure for nitrogen monoxide: