Complete the three Lewis structures for N(NO2)2– by adding missing lone pair electrons and assigning formal charges. Do not add resonance arrow

Structure 1 formal charges:

N₁ = +1; O₁₁ = +1; O₁₂ = -1; N₂ = 0; N₃ = +1; O₃₁ = -1; O₃₂ = -1

Structure 2 formal charges:

N₁ = +1; O₁₁ = +1; O₁₂ = -1; N₂ = -1; N₃ = +1; O₃₁ = -1; O₃₂ = +1

Structure 3 formal charges:

N₁ = +1; O₁₁ = -1; O₁₂ = -1; N₂ = +1; N₃ = +1; 0₃₁ = -1; O₃₂ = -1

Explanation:

The formal charge of an atom in a molecule is the charge assigned to the atom if the electrons in all chemical bonds were redistributed evenly between the atoms.

Formal charge can be calculated as follows:

Formal charge =  number of valence shell electrons in the neutral atom − ( number of lone pair electrons + ½ bonding electrons)

Structure 1:

N₁ = 5 - 4 = +1

O₁₁ = 6 - 5 = +1

O₁₂ = 6 - 7 = -1

N₂ = 5 - 5= 0

N₃ = 5 - 4 = +1

O₃₁ = 6 - 7 = -1

O₃₂ = 6 - 7 = -1

Structure 2:

N₁ = 5 - 4 = +1

O₁₁ = 6 - 5 = +1

O₁₂ = 6 - 7 = -1

N₂ = 5 - 6= -1

N₃ = 5 - 4 = +1

O₃₁ = 6 - 7 = -1

O₃₂ = 6 - 5 = +1

Structure 3:

N₁ = 5 - 4 = +1

O₁₁ = 6 - 7 = -1

O₁₂ = 6 - 7 = -1

N₂ = 5 - 4 = +1

N₃ = 5 - 4 = +1

0₃₁ = 6 - 7 = -1

O₃₂ = 6 - 7 = -1

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