No2 can react with the no in smog, forming a bond between the n atoms. draw the structure of the resulting compound, including formal charges.

The formal charge of N₂O(the resulting compound) is 0, -1 and +1

Formal charges are usually used to explain the bonding of the Lewis structure. The structural form of a molecule can have several types based on the Lewis structure. Formal charge calculations can determine which molecule is more stable, by choosing the smallest charge, even though atoms such as C, N, and O the priority is to fulfill the octet rule first.

Formal charges can be formulated:

FC (formal charge) = number of valence electrons - number of free electrons - 1/2 binding electrons

In the reaction, NO₂ and NO will produce N₂O compounds, nitrous oxide

Reactions that occur:

NO₂ + NO ---> N₂O + O₂

N₂O based on its lewis structure can have 3 possible shapes (single, triple or triple bond) but the most stable and suitable one is the three bond between its N atoms

The formal charge of N₂O is:

So that the total formal charge = 0 + (+ 1) + (- 1) = 0, according to the charge on neutral N₂O compounds

the formal charges

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the resonance forms of N₂O

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Keywords: formal charge, N₂O, the valence electron, bond, the octet rule

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