Question 4.5

[K Stefanescu 2I]

The question asks us to determine the shape of ClO2+ and determine its bond angle. However, my question pertains only to determining the Lewis structure of the compound.

The book lists the following as the correct Lewis structure-
.. .. ..
:O - Cl - O:
.. ..

Why wouldn't it be the following?
.. .. ..
O = Cl = O
.. ..

The second structure would give us a formal charge of 0 on all of the atoms, whereas the book's answer gives a formal charge of -1 on both oxygen atoms and +3 on the chlorine atom.

Why is the first structure correct and the second one incorrect?

[Nishma Chakraborty 1J]

Hey!

I'm not sure if I interpreted the drawing of the Lewis structures correctly because of formatting, but if you were to draw double bonds on the chlorine (as in the second structure shown), it would have a formal charge of +3 which is undesirable.

[Iris Shim 1E]

When you're drawing the Lewis structure, you have to get minimize the formal charge overall and on each ion. The less formal charge, the more stable it is. The correct answer shown in the book minimizes the overall formal charge.