2C #15

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Lea Chamoun 2J
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2C #15

Postby Lea Chamoun 2J » Sun Nov 08, 2020 4:18 pm

Two contributions to the resonance structure are shown below for each species. Determine the formal charge on each atom and then, if possible, identify the Lewis structure of lower energy for each species.
What is the best way to determine which structure is the lowest energy? Would I just use the formal charges I calculated?

Helena Xu 1I
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Re: 2C #15

Postby Helena Xu 1I » Sun Nov 08, 2020 5:14 pm

The Lewis structure with the lower energy would have formal charges closer to zero because it would be more stable.

Jasmine Ho 3I
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Re: 2C #15

Postby Jasmine Ho 3I » Sun Nov 08, 2020 5:40 pm

The structure with the lowest energy would have formal charges closer to zero. However, I think it is also important to consider what charges are next to each other because two negatively charged atoms repel each other = more energy.

Ansh Patel 2I
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Re: 2C #15

Postby Ansh Patel 2I » Sun Nov 08, 2020 5:45 pm

Hi! The Lewis structure that has the lowest formal charge (closest to zero) would be considered to have the lowest energy because the atoms are more stable in this state.

Michael Iter 2F
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Re: 2C #15

Postby Michael Iter 2F » Sun Nov 08, 2020 5:46 pm

Yes and I think the most stable structures are the ones where the most electronegative elements are the ones with negative formal charges if there has to be negative formal charges somewhere

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Re: 2C #15

Postby IshanModiDis2L » Sun Nov 08, 2020 6:01 pm

The formal charges with the lowest energy/energy that is closest to zero would be more stable. Also, the most electronegative element will be more stable with a negative charge.

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Re: 2C #15

Postby Yijia_Yang_3A » Wed Nov 11, 2020 7:02 am

Formal charges is low is when it's the most stable. If that's achieved, second rule is that more electronegative atoms are better off having a negative charge (closer to noble gas form).

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