Lewis Structure

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Kyle Thorin
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Joined: Sat Aug 24, 2019 12:16 am

Lewis Structure

Postby Kyle Thorin » Sun Oct 27, 2019 3:14 pm

In drawing the Lewis Structure for Sulfate, why is it more accurate to draw the structure with two double bonds than just lone pairs on each oxygen atom.

Sarah Blake-2I
Posts: 153
Joined: Fri Aug 30, 2019 12:16 am

Re: Lewis Structure

Postby Sarah Blake-2I » Sun Oct 27, 2019 3:17 pm

It makes sulfate more stable to have the double bond rather than lone pairs on the oxygen.

Jamie Lee 1H
Posts: 54
Joined: Fri Aug 09, 2019 12:15 am

Re: Lewis Structure

Postby Jamie Lee 1H » Sun Oct 27, 2019 3:21 pm

the sulfate ion can hold more than 8 electrons and if that's the case with any element, you want to be able to fill up the central element first. If you can go further than the octet rule, you would like to create a Lewis structure that contains the better formal charges (more with a formal charge of 0) and in this case it would be when using the double bonds.

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Re: Lewis Structure

Postby Vivianvelazquez_1J » Sun Oct 27, 2019 3:22 pm

It is more accurate to draw the structure with two double bonds for Sulfate because the formal charge = 0 at that point which is the most stable.

Kendall 3H
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Re: Lewis Structure

Postby Kendall 3H » Sun Oct 27, 2019 3:37 pm

I agree with the earlier answers. I believe the main reason and the reason expressed most to us in Lecture was that the structure with 2 double bonds has a formal charger closer to 0 than the structure with 4 single bonds. When drawing Lewis Structures, you always want to option with the formal charge closest to 0.

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Re: Lewis Structure

Postby ABombino_2J » Sun Oct 27, 2019 7:32 pm

The 2 double bonds on the sulfate atom bring the formal charge of sulfate to 0. It is more important to have a lower formal charge on the central atom because it has a lower electron affinity.

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