## Question 61 Chapter 3

Emerald Ellspermann 1K
Posts: 28
Joined: Wed Sep 21, 2016 3:00 pm
Been upvoted: 2 times

### Question 61 Chapter 3

Here is the problem-
Determine the numbers of electron pairs (both bonding and lone pairs) on the iodine atom in (a)$ICl_{2}^{+}$ ; (b) $ICl_{4}^{-}$ (c) $ICl_{3}$ ; (d) $ICl_{5}$.

I was having trouble with drawing the lewis structure for $ICl_{4}^{-}$. Why is the structure drawn with two of the chlorine atoms at an angle? How do we know when to draw the lewis structure at an angle like this?

Eugenia Kwon 3O
Posts: 18
Joined: Wed Sep 21, 2016 2:59 pm

### Re: Question 61 Chapter 3

We'll be talking about molecular shapes soon during the lecture regarding the positions of the bonds and lone pairs that contribute to the final structure. In this case, since there are two lone pairs and 4 bonds, the shape forms an octahedral and the angle between the I and Cl atoms are drawn at a 90˚ angle (The molecular shape would be a square planar though)