Final answer:
The N₂O molecule has two valid resonance structures with nitrogen as the central atom, involving different placements of double bonds and distribution of formal charges.
Step-by-step explanation:
When drawing a Lewis structure for N₂O (nitrous oxide), with nitrogen as the central atom, we need to account for a total of 16 valence electrons. Possible structures vary with the placement of the double bond and the assignment of formal charges. Here are the valid resonance structures:
- Nitrogen (central) single-bonded to Nitrogen and double-bonded to Oxygen, with formal charges adjusted accordingly.
- Nitrogen (central) double-bonded to Nitrogen and single-bonded to Oxygen, with formal charges adjusted accordingly.
Resonance in N₂O means the actual electronic structure is an average of these resonance structures, represented by a double-headed arrow between them.
The Lewis structure of N₂O can be drawn as follows:
O-N=N
In this structure, there is a double bond between one oxygen atom and the nitrogen atom, and a single bond between the other oxygen atom and the nitrogen atom. This is one valid Lewis structure for N₂O.
N₂O has two valid resonance structures. The second valid resonance structure can be drawn with the double bond between the other oxygen atom and the nitrogen atom. The position of the double bond can switch between the two oxygen atoms, resulting in resonance.