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