The Lewis structure corresponding to the reactants and products in the reaction is attached in the image.
Further Explanation:
The free radicals are high energy chemical species that must stabilize themselves either via electron combination with another free radical or abstraction of proton from another radical.
The Lewis structure is the chemical representation of an element along with the nonbonding pairs. For covalent molecules, the number of electrons involved in bonding and the remaining nonbonding pairs can be represented while writing the Lewis structures. Lewis structures along with the formal charges that they carry help predict the geometry, polarity, and reactivity of the molecules.
The nitrogen radical itself is unstable, and nitrogen monoxide also has an unpaired electron. So these two reactants can stabilize themselves by combination of their unpaired electron and form dinitrogen oxide molecule.
Lewis structure of :
The total number of valence electrons of is calculated as,
Total valence electrons = [(2) (Valence electrons of N) + (1) (Valence electrons of O)]
Formal charge:
It is the charge that an atom acquires in a molecule assuming that the electron pairs that constitute the bond pairs are shared equally between the two atoms, irrespective of their electronegativities.
The formula to calculate the formal charge on an atom is as follows:
O forms one single bond with a nitrogen atom and 3 lone pairs are present on it.
Total number of valence electrons in the free oxygen atom is 6.
Total number of nonbonding electrons in O is 6.
Total number of bonding electrons in O is 2.
Substitute these values in equation (1) to find the formal charge on O.
Total number of valence electrons in the free nitrogen atom is 5.
Total number of nonbonding electrons in N is 0.
Total number of bonding electrons in N is 6.
Substitute these values in equation (1) to find the formal charge on N.
The formal charge of nitrogen is +1.
Nitrogen atom has 5 valence electrons, and oxygen atom has 6 valence electrons. The central nitrogen atom forms a triple bond with other nitrogen atom and a single bond with oxygen atom. The central nitrogen atom, therefore, acquire positive charge and oxygen atom will acquire negative charge. Therefore the Lewis structure of is attached in the image.
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Molecular structure and chemical bonding
Keywords: Lewis structure, valence electrons, NO, formal charge, N2O, oxygen, double bonds, single bond, bonding electrons, non-bonding electrons, total valence electrons and resonance hybrid.