(Polar molecules, Non-polar molecules, etc.)
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I just want to confirm that if for example you had to find the molecular geometry for I3- it would be linear because they're all iodines? I got 3 lone pairs for that and thought it would be bent but it was linear instead
Hey! So you are right in that there are three lone pairs on the middle Iodine. This makes five electron densities, and that would be trigonal bipyramidal. The three lone pairs take all the equatorial electron densities, leaving only the axial atoms as Iodine. This makes the linear shape. Hope this helps!
My preferred method would be to determine the number of electron densities around the central atom and then figure out which ones are bonding pairs and which ones are lone pairs. This requires some memorization or visualization skills. For example, like someone mentioned before, this molecule has five electron densities around the central atom. From there, you can substitute three bonding pairs for lone pairs. You can either memorize that AX2E3 is linear or you can visualize that the three lone pairs occupy the equatorial atoms making the remaining atoms axial (linear).
You have to take into consideration the amount of lone pairs on the structure, as they can modify the shape and push down on the other bonds, lessening the bond angles.It doesn't matter if the lewis structure is all the same element, it's all about lone pairs and regions of electron density.
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