Question

NO+, NO2-, NO2H, and NO3-.

Based on the Lewis structures, list all of the the N-O bonds lengths in order of shortest to longest

i) N - O bond in NO2-

ii) N - O double bond in NO2H

iii) N - O bond in NO2H

iv) N - O bond in NO+

v) N - O bond in NO3-

Answer 1

According to Lewis structure

a) N-O bond length in NO₂^- >>> 3

b) N-O double bond in NO₂H >>> 1

c) N-O single bond in NO₂H >>> 5

d) N-O bond length in NO⁺>>> 2

e) N-O bond length in NO₃^- >>> 4

NO⁺, with only one oxygen, has a formal charge of +1 on oxygen and 0 on nitrogen.

NO₂^- with two oxygens, since there is a 0 formal charge on nitrogen, then the oxygens each share a −1/2 charge (−1/2×2 = −1 charge overall).

NO₃^- with three oxygens, since there is a +1 formal charge on nitrogen, the remaining charge gets distributed onto all three oxygens, balancing out to be −2/3 per oxygen (−2/3×3+1=−1 charge overall)

Therefore , the N-O bonds lengths in order of shortest to longest

c) N-O single bond in NO₂H < d) N-O bond length in NO⁺ < a) N-O bond length in NO₂^- < e) N-O bond length in NO₃^- < b) N-O double bond in NO₂H