The simple answer is no, N2O (nitrous oxide) does not violate the octet rule, but it is a bit more nuanced than that.
The octet rule states that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. In the case of N2O, we have two nitrogen atoms and one oxygen atom.
When we look at the Lewis structure of N2O, we see that the nitrogen atoms share electrons with the oxygen atom. The structure can be represented as:
In this structure, the central oxygen atom follows the octet rule by having eight electrons in its outer shell. The nitrogen atoms also follow the octet rule since they each end up with six electrons in their valence shell when involved in a triple bond with each other and a single bond with oxygen.
Thus, while N2O may not adhere to a strict interpretation of the octet rule for both nitrogen atoms under some resonance forms, it does not truly violate it. This compound is a good example of how Lewis structures can sometimes lead to confusion about electron arrangements and stability.