2C.7

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Ziyan Wang 3J
Posts: 51
Joined: Wed Sep 18, 2019 12:22 am

2C.7

Postby Ziyan Wang 3J » Thu Nov 07, 2019 10:16 am

I don't quite understand how to draw the Lewis structure of ICl2 +, ICl4 -, ICl3, ICl5

John Liang 2I
Posts: 102
Joined: Fri Aug 30, 2019 12:18 am

Re: 2C.7

Postby John Liang 2I » Thu Nov 07, 2019 4:13 pm

Icl2+ has two lone pairs and two single bonds to cl.
Icl4- has two lone pairs and four single bonds to cl.
Icl3 has two lone pairs and three single bonds to cl.
Icl5 has one lone pair and five single bonds to cl.

hope this helps!

Camellia Liu 1J
Posts: 51
Joined: Sat Aug 24, 2019 12:15 am

Re: 2C.7

Postby Camellia Liu 1J » Thu Nov 07, 2019 4:15 pm

I always start by counting the number of electrons that I have to work with. For ICL2+, I counted 20 electrons, and since I is less electronegative than Cl, I placed it as the central atom. Then it comes down to placing the single bonds in and determining where the lone pairs go. For ICl2+, I got 2 bonding and 2 lone pairs for I. Since we know that Cl is more electronegative, we can assume that there won't be double bonds on these structures. You can just use this process of arranging the bonds and electrons to get the structures--while keeping formal charge in mind.


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