Moderators: Chem_Mod, Chem_Admin

Emily 1E
Posts: 27
Joined: Fri Apr 06, 2018 11:03 am


Postby Emily 1E » Sun May 20, 2018 12:24 pm

The question asks to draw the Lewis structure of ClO, which is a radical. How to you know whether the single lone electron goes on the Cl molecule or the O molecule?

Anna De Schutter - 1A
Posts: 66
Joined: Wed Feb 21, 2018 3:01 am

Re: 3.59a

Postby Anna De Schutter - 1A » Sun May 20, 2018 3:10 pm

I had the same question, because when I calculated the formal charges of chlorine and oxygen in the solution's manual configuration I got:
Cl: 7valence electrons - 5 lone pair electrons - 0.5*2 bonding electrons = +1
O: 6valence electrons -6 lone pair electrons - 0.5*2bonding electrons = -0.5

Whereas if I put the radical on oxygen and give chlorine a full octet (with just a single bond between Cl and O), I got:
Cl: 7-6-0.5*2=0
O: 6-5-0.5*2=0

Am I calculating the formal charges the wrong way? Or missing something? Why don't we choose the molecule where the formal charge of each element equals 0?

Thank you!
Anna De Schutter - section 1A

Posts: 18901
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 734 times

Re: 3.59a

Postby Chem_Mod » Sun May 20, 2018 9:05 pm

Return to “Ionic & Covalent Bonds”

Who is online

Users browsing this forum: No registered users and 2 guests