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Answer :
OK, here are the steps to solve this problem:
1) Nitrogen (N) exists in the +5 oxidation state in NO2 (nitrogen dioxide). Each O atom has a -2 charge, so the NO2 molecule has no net charge.
2) NO also has nitrogen in the +5 oxidation state. So when the N atoms from NO2 and NO bond together, the sum of the oxidation states on the shared nitrogen atom is still +5 (from +5 + 0).
3) To determine the formal charges, we count the valence electrons around each atom:
NO2:
N: 5 electrons
O: 6 electrons (2 per O)
So N has a +4 formal charge and each O has a -1 formal charge.
4) When NO2 bonds to NO, the electrons from the bonds are shared equally among the nitrogen atoms. So each N will have 6 valence electrons, giving a +3 formal charge (6e - 5 for N).
5) Therefore, the resulting compound from the reaction of NO2 and NO has the following structure and formal charges:
N2O3
N (+3) - N (+3) - O (-2) - O (-2)
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Rewritten by : Barada
The resulting compound from NO_2 reacting with NO in smog is called N_2O_3. It has a linear structure with a formal charge of +1 on one nitrogen atom and -1 on the other.
Nitrogen oxides (NOx) are harmful air pollutants that can cause respiratory problems and contribute to the formation of acid rain and ozone depletion. NO_2 is a common byproduct of power plants and automobiles and can react with NO in the presence of sunlight to form a bond between the N atoms. This resulting compound is called nitrogen trioxide or N_2O_3. The structure of N_2O_3 is linear, with two nitrogen atoms sharing a triple bond and one oxygen atom bonded to each nitrogen atom. One nitrogen atom has a formal charge of +1, while the other nitrogen atom has a formal charge of -1. This indicates that one nitrogen atom has lost an electron and the other has gained an electron, resulting in a polar molecule. The formation of N_2O_3 is a significant contributor to the formation of smog and is a concern for air quality.
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