2B.15 (7th ed)  [ENDORSED]

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2B.15 (7th ed)

Postby Duby3L » Sun Nov 04, 2018 12:43 am

Draw the Lewis structures that contribute to the resonance hybrid of nitryl chloride, ClNO2 (N is the central atom).

How come the solution to this problem doesn't show two double bonds between both oxygens and nitrogen? Is it not allowed? Can someone please explain when we are allowed to make multiple double bonds?

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Re: 2B.15 (7th ed)  [ENDORSED]

Postby ChathuriGunasekera1D » Sun Nov 04, 2018 12:33 pm

Hi! You are allowed to have one double bond (between the N and O), but you cannot have two for both N O bonds. Because N is not in the 3rd period, it cannot make an expanded octet using the empty 3d orbital. If it could, then it could have five bonds (two double bonds to O and one single bond to Cl), however because it can't, it sticks to the four bonds (one double bond to O, one single bond to O, and one single bond to Cl). You would have 3 lone pairs on Cl, none on N, 2 on the double bonded O, and 3 on the single bonded O.

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