HW 4.13

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

Moderators: Chem_Mod, Chem_Admin

Shimran Kumar 1C
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am

HW 4.13

Postby Shimran Kumar 1C » Fri May 25, 2018 5:55 pm

The problem asks for the molecular shape of I3-. The Lewis structure shows 3 lone pairs and 2 bonding pairs around the central Iodine. The solutions manual states the shape is linear.

Why would the shape be linear if there is an odd number of lone pairs pushing on the atoms? I thought the molecule would be bent.

Jack Martinyan 1L
Posts: 32
Joined: Thu Feb 22, 2018 3:00 am
Been upvoted: 1 time

Re: HW 4.13

Postby Jack Martinyan 1L » Fri May 25, 2018 8:51 pm

When you draw the Lewis structure of the I3- ion, you end up with two iodines attached to a central iodine. The central iodine also has three lone pairs on it. This gives you 5 regions of electron density around the central atom. This gives a trigonal bipyramidal shape. The electron pairs repel each other, so they want to maximize their distance from one another, so they take up equatorial positions 120 degrees from one another, and the two other iodines are 180 from one another. Thus the overall shape is linear.



viewtopic.php?t=16372

Shimran Kumar 1C
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am

Re: HW 4.13

Postby Shimran Kumar 1C » Mon May 28, 2018 2:21 pm

That actually makes perfect sense! Thank you so much!


Return to “Determining Molecular Shape (VSEPR)”

Who is online

Users browsing this forum: No registered users and 1 guest