What is the Molecular Geometry of ICl3?

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zattyzatzat
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The back of my textbook says this shape is a trigonal planar. But when I check online it's says it's a T-Shape molecule. Which one is it?
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charco
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(Original post by zattyzatzat)
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The back of my textbook says this shape is a trigonal planar. But when I check online it's says it's a T-Shape molecule. Which one is it?
Iodine starts off with 7 electrons and each chlorine provides it with 1, giving a total of 5 pairs.

These five electron pairs arrange themselves into a trigonal bipyramidal orientation.

You now have to locate the two lone pairs. These will both go into equatorial positions to minimise repulsions. In that way they will be at 120º to each other and 90º to two bonding pairs and 120º to the third bonding pair..

If they go into axial positions they will both be at 90º to three bonding pairs, althogh this would minimise the repulsion between the two one pairs.

Apparently the first case is lowest energy, giving a T shaped molecule, that will distort the axial bonding pairs to minimise repulsions, giving bond angles of less than 90º.
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