Problem 4.9

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

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Lily Emerson 1I
Posts: 27
Joined: Fri Apr 06, 2018 11:02 am

Problem 4.9

Postby Lily Emerson 1I » Wed May 30, 2018 11:23 pm

Why is the shape of ICl3 T-shaped instead of trigonal planar or trigonal pyramidal?

Yadira Flores 1G
Posts: 41
Joined: Wed Nov 15, 2017 3:01 am

Re: Problem 4.9

Postby Yadira Flores 1G » Thu May 31, 2018 9:13 am

The 2 lone pairs on the I in the lewis structure does not allow for the shape to correspond to trigonal planar nor trigonal pyramidal. The VSEPR formula of AX3E2 corresponds to the t-shape.

jessicasam
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Re: Problem 4.9

Postby jessicasam » Thu May 31, 2018 9:18 am

If you draw the lewis structure, you will see that I forms 1 bond with each Cl atom. After giving each Cl a full octet, there are still 4 electrons that are left over. Two lone pairs are added to I because it can have more than an octet. The lewis structure will now have 3 bonds and 2 lone pairs around the central atom. This configuration is T-shaped.

Faisal Alshamaa - 1L
Posts: 31
Joined: Fri Apr 06, 2018 11:01 am

Re: Problem 4.9

Postby Faisal Alshamaa - 1L » Fri Jun 01, 2018 12:18 am

Trigonal pyramidal takes on the form of A-X3-E, with 3 atoms bonded to a central atom and a lone pair of the central atom.
ICl3, when you draw the lewis structure, has 2 lone pairs and 3 atoms bonded to the central atom, which takes on the form of A-X3-E2, which is T-Shaped.


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