N2O Lewis structure

[Tony Chen 1F]

Why in the lewis structure for N2O, the nitrogens are triple bonded to each other while the oxygen is single bonded to nitrogen? Wouldn't that make one of the nitrogen have a +1 formal charge, leaving the oxygen with a -1 formal charge? If instead, the central nitrogen is double bonded to oxygen, wouldn't that minimize the formal charge of each atom and thus be the correct Lewis structure? Thanks in advance for the explanation!

[Tony Chen 1F]

Also wouldn't single-bonded nitrogens with a double-bonded oxygen work as well?

[Tony Chen 1F]

Is it because the central nitrogen needs to have an octet first?

[Harbaksh Kaur 3E]

There's about three different ways to draw the lewis structure for N2O and each way you said it is correct! Single bonded nitrogens with triple bonded nitrogen and oxygen would work! The different structures would cause different formal charges and therefore affect stability. The most stable structure is the triple bonded nitrogens and the single bonded oxygen which is likely why it is used in explanations rather than the other structures.