Arrange the following in the increasing order of the N-O bond lenght

Question

NO₂Cl

NO₂^-

NH₂OH

NO2⁺

 

Answer 1

Hello Aaftab

 

You need to draw the lewis structure of each molecule to see the differences in N-O bond formation between each compound. The presence of multiple (pi) bonds affects the bond length as well.  In general, the order of increasing bond length is: triple bond < double bond < single bond.

 

For the above molecules, the order of increasing N-O bond length is:

 

NO₂⁺ < NO₂Cl < NO₂^- < NH₂OH

 

a) NH₂OH contains only a sigma (single) N-O bond, therefore, this will be the longest.

 

b) NO₂⁺ has two N-O double bonds.  [O=N=O]⁺, therefore, this will have the shortest bond length.

 

c) NO₂Cl and NO₂^- both have one N-O double bond (N=O), and one N-O single bond.  However, the presence of the electronegative Cl atom will make the N=O and N-O bonds shorter in NO₂Cl when compared to NO₂^-.