Three situations can be built that do not monitor the Octet Rule, and as such, lock are well-known as the exceptions to the Octet Rule. Following the Octet dominance for Lewis Dot structures leads to the many accurate depictions of steady molecular and also atomic structures and because the this we always want to use the octet ascendancy when illustration Lewis dot Structures. However, the is tough to imagine the one rule could be adhered to by all molecules. There is always an exception, and also in this case, 3 exceptions. The Octet dominance is violated in these three scenarios:

as soon as there space an odd variety of valence electrons once there space too couple of valence electrons once there space too many valence electrons

Reminder: always use the Octet rule when drawing Lewis dot Structures, this exceptions will only take place when necessary.

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Exception 1: varieties with Odd number of Electrons

The an initial exception come the Octet dominion is once there space an odd number of valence electrons. An example of this would be the nitrogen (II) oxide molecule ((NO)). Nitrogen atom has actually 5 valence electrons while the oxygen atom has actually 6 electrons. The full would it is in 11 valence electrons to be used. The Octet preeminence for this molecule is fulfilled in the over example, however that is with 10 valence electrons. The critical one does not recognize where come go. The lone electron is dubbed an unpaired electron. However where must the unpaired electron go? The unpaired electron is usually put in the Lewis Dot structure so that each facet in the structure will have actually the lowest formal fee possible. The formal charge is the perceived charge ~ above an individual atom in a molecule as soon as atoms do not contribute equal numbers of electrons to the bonds they get involved in. The formula to discover a formal charge is:

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

No formal charge at every is the many ideal situation. An example of a steady molecule with an odd variety of valence electrons would certainly be nitrogen monoxide. Nitrogen monoxide has 11 valence electron (Figure 1). If you need much more information around formal charges, watch Lewis Structures. If us were to think about the nitrogen monoxide cation ((NO^+) through ten valence electrons, then the adhering to Lewis structure would be constructed:

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

Nitrogen normally has 5 valence electrons. In figure 1, it has two lone pair electrons and also it participates in two bonds (a double bond) v oxygen. This outcomes in nitrogen having a formal fee of +1. Oxygen generally has 6 valence electrons. In number 1, oxygen has four lone pair electrons and it participates in two bonds with nitrogen. Oxygen as such has a formal fee of 0. The in its entirety molecule here has a formal fee of +1 (+1 for 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 actually the lowest complete formal charge), it will lug both the nitrogen and also the molecule"s overall charges come zero, the many ideal formal charge situation. The is exactly what is excellent to acquire the correct Lewis structure for nitrogen monoxide: