2B.15

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Ellen Amico 2L
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Joined: Thu Sep 19, 2019 12:16 am

2B.15

Postby Ellen Amico 2L » Mon Nov 04, 2019 9:09 pm

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

I'm confused as to why there even needs to be resonance structures if both oxygens can have double bonds since nitrogen has enough electrons for it... is there a reason as for why this can't happen?

Nyari Muchaka_Discussion 4A
Posts: 53
Joined: Thu Sep 19, 2019 12:17 am

Re: 2B.15

Postby Nyari Muchaka_Discussion 4A » Mon Nov 04, 2019 9:27 pm

Nitrogen cannot form a double bond with both oxygen and a single bond with chlorine as that forms a total of five bonds(10 shared electrons), and nitrogen does not have the ability to expand past the octet rule(can only take on eight electrons). Atoms in row three and below can do this as they have the d orbital to put the extra electrons but nitrogen is in row two and only has the s and p orbital which totals eight valence electrons. Your structure should be nitrogen in the center with a single bond on one oxygen, double bond on the other, and single bond with chlorine. The chlorine should then have three long pairs, the single bound oxygen three lone pairs, and the double bound oxygen two lone pairs. The formal charges would be zero on the double bond oxygen, negative one on the single bond, zero on the chlorine, and plus one on the nitrogen which results in a neutral molecule. The oxygen will carry the negative charge as it is more electronegative than chlorine, so the chlorine will never be double bonded to the nitrogen. Resonance now exists as either oxygen can have the double bond and the other a single bond.


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