whereas for NO3-, you get like three double bonds shared between 3 N-O bonds, so that is 1 original double bond shared between 3 N-O bonds through delocalisation, bond order: 1/3 post again if you dont get this Log in or register to post comments 82 answers. its not just simple... its very very simple. Bond order = Total number of bonding pairs / Number of NO bond locations . 2. Thus bond order is the average of 2, 1, 1 bond order = no.of nonduna electrons- no. 11.3K people helped. Bond order = 3/2 = 1.5-In NO 3-, there is one double bond and two single bonds. soo for NO+. There are 3 bonding pairs of electrons and 2 NO bond locations. N=O has a bond order of two, and both N … I am doing a multiple choice question for which one of the possible answers is, for the Lewis structure of NO3- (one of the oxygens is double bonded to the nitrogen and the other two are single bonded), "one of the N-O bonds is shorter than the other two". You will see 2 single bonds and 1 double bond in three resonance structures. The correct order of N - O bond lengths in NO, NO2-, NO3- and N2O4 is (A) N2O4 > NO2- > NO3- > NO (B) NO > NO3- > N2O4 > NO2- (C) NO3- > NO2- > The Lewis structure for NO 3 - is given below: To find the bond order of this molecule, take the average of the bond orders. Due to resonance the double bond is equally distributed to three oxygen atoms. Favorite Answer. Draw or look up the Lewis structure for NO3^-. There is a double bond between the two oxygen atoms; therefore, the bond order of the molecule is 2. The bond order is the average. bond order = (8 - 2)/2 = 6/2 = 3... triple … of antibonding electrons/2. Ambitious.