Question

PART II a) Draw all of the Lewis structures possible for the molecules below (resonance structures) and b) Indicate the formal charge on all of the atoms in your structures. Based on the formal charges, are the structures equivalent or not equivalent. If not determine the "best" resonance structure. (a) CO, (b) NO, (c) NO, (d) N,

Answer 1

Answer a # Lewis structure of co2. Valence electrons of the atomis. o = 4, Valence electron o = 6 valence electron. ou o plow calculate the formal charge. formula. Formal charge a Valence electron - [bond & dots) (Formal charge 2a 6-(1+6). for single bondect oxygen S = 6-7 = -1 Formal charge on double bondred oxygen = 6-(2+4) - 6-6 20

Formal charge on carbon = 4 - (4+0) = 4-4 zo Hare two oxygen atom single bonded so that total number of formal charge is - 30. are resonance structure Abave three structure. Noa (6) # Lewis structure of Valence ebectron on N= s valence electron on o=6 o=N-O: Formal charge on N= valence election - (bond + dots) = 5- (3+2) = s-s=0 Formal charge on single bonded oxygen = 6-(1+6) = 6-7=-1

oxygen. on double bonded Formal charge = 6-(2+4) 6-6 =0

(C) # Leuris structure of Nož Number of valence electron on Natom and o- atom already mentioned in Part B. Formal charge on N-atom =s-(4+ o dots) - S-4 = tl charge formal charge for single bonded oxygen and double bonded oxygen is already calculated in part b. 1:or N +2= 1.0=N-O: t1 N o final Resonance structure

W # valence electron of N= s Possible structure of No ("M=N=N: ] [:N-NEN:] [:NEN-N: Formal charge for (1) Criddle N) = = valence electron- (bond+dot) S-(4+0) = 5~4=+1 s-(2+4)=8-6=-1 Formal chaoge - (side N) Formal charge on second and third structure. formal charge on triple bonded N = 5- (3+2) = 5-S=0 Formal charge on single bonded N =s-(1+6) = 5-7 = -2 final Stracture. [. = NENEHNEN:) orizi TiN-NEN: NE NON