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Tim Foster 2A
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Postby Tim Foster 2A » Sat Nov 11, 2017 12:47 pm

What does the correct lewis structure for this molecule look like?

Hellen Truong 2J
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Postby Hellen Truong 2J » Sat Nov 11, 2017 1:46 pm

To determine the Lewis structure for HOCO, I first counted the electrons to get 17. Then, I linked single bonds so the structure looked like H-O-C-O. I added a double bond between C and the second O and then filled in 2 lone pairs for each oxygen. At this point, 16 electrons have been filled in and I put the last one on C. This makes all the formal charges zero and also shows that HOCO is radical because of the unpaired electron on C.

Michelle Lu 1F
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Postby Michelle Lu 1F » Sat Nov 11, 2017 3:10 pm

Yes, I agree with the above reply. I also did the same thing. If you are wondering why the unpaired electron would go on the Carbon, there are two main reasons. One is that by giving Oxygen two bonded pairs and two unbonded pairs, both Oxygens get a FC of zero, which is ideal. Second, Carbon is less electronegative than Oxygen and therefore would be the atom most likely to have an unpaired electron.

Rita Dang 3D
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Postby Rita Dang 3D » Sat Nov 11, 2017 3:32 pm

Remember when drawing Lewis Structures, we almost always have to satisfy the octet rule for Oxygen first because it has a high electronegativity.

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