Homework #4.13 part a (6th edition)

(Polar molecules, Non-polar molecules, etc.)

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Dana Wilks 3I
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Joined: Fri Sep 28, 2018 12:23 am

Homework #4.13 part a (6th edition)

Postby Dana Wilks 3I » Thu Nov 15, 2018 11:57 am

For the I3- molecule, I understand how to draw the correct lewis structure with 3 lone pairs on the central I atom. However, because the lone pairs are not symmetrical, I am confused as to why the shape wouldn't be angular instead of linear.

Theodore_Herring_1A
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Joined: Fri Sep 28, 2018 12:29 am

Re: Homework #4.13 part a (6th edition)

Postby Theodore_Herring_1A » Thu Nov 15, 2018 12:23 pm

When looking at the Lewis structure, notice how there are 5 electron densities around the central Iodine: two iodines and 3 lone pairs. This gives a trigonal bipyramidal shape. The three electron pairs will want to maximize their distance from one another, so they will take up positions 120 degrees from one another. Thus, the last two iodines will be on opposite ends 180 degrees from one another, and the shape of the three iodines will be linear.
(Image credit to Topper Learning)
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