How ti draw the lewis structure of N3H4O ??? sample structure is given.
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Answers
“Stable” in the context of compounds containing Nitrogen-Nitrogen bonds is not the first term that comes to ones mind!
In the context of the “best” Lewis structure for this compound, two general structures can be taken as the basis: a linear structure and a cyclic structure.
When you count the valence electrons of the three nitrogen and one hydrogen atom (16 electrons) and spread them out to fulfill the octet of each atom, for the linear case, you would get two possible structures each having a formal charge of +1 on one of the nitrogens and -1 on another nitrogen (search for Hydrazoic acid on wikipedia, and you can see how they look).
If you consider a cyclic structure, which is not usually done in general chemistry courses, then you end up with a 3 membered all nitrogen ring with a lone pair on the three nitrogens, one nitrogen having a bond with the hydrogen atom, and a double bond between the two other nitrogens. The formal charge of all the atoms would be 0. Technically speaking this would be the most “stable” Lewis structure, but would probably be the first of the three to spontaneously explode due to the unstable 3-ring structure!