Page 1 of 1
Posted: Sun Nov 04, 2018 8:37 pm
In a molecule with a radical how do you identify which element the radical is on?
Posted: Sun Nov 04, 2018 8:46 pm
you put one dot on the element that has the radical
Posted: Sun Nov 04, 2018 9:01 pm
How would you define a radical?
Posted: Sun Nov 04, 2018 9:41 pm
A radical is an atom, molecule, or ion that has an unpaired valence electron. These unpaired electrons make radicals highly chemically reactive. Most organic radicals have short lifetimes because of this.
Posted: Sun Nov 04, 2018 11:01 pm
Put the radical on whatever atom will give it the last formal charge (attempt to get the molecule stable as possible).
Posted: Mon Nov 05, 2018 9:44 am
The radical is placed with the atom based on the formal charge. Remember that we want a FC closer to 0.
Posted: Mon Nov 05, 2018 11:03 am
Placing the radical on the atom that will have a formal charge as close to 0 as possible!
Posted: Mon Nov 05, 2018 1:14 pm
As a rule, we always try to get formal charge as close to zero as possible so place the radical based on that.
If everything is zero then just pick one (Try to follow the octet guideline, dont give it to any elements with a full octet that isn't in group 3 as they can't take more than 8.)
Posted: Sun Nov 11, 2018 7:03 pm
Also, you wouldn't make the atom that has the most electronegativity a radical, because it would want a full octet.
Posted: Wed Nov 14, 2018 11:23 am
Just for clarification when we say radical we can mean both the molecule with the unpaired valence electron OR the single electron as well? The word is used to describe both?
Posted: Wed Nov 14, 2018 11:32 am
Does anyone know if there are certain atoms that typically get the unpaired electron in a radical molecule?
Posted: Wed Nov 14, 2018 3:01 pm
The atom with an incomplete lone electron pair is what makes the molecule a radical molecule. Typically it'll be like nitrogen or something. Because they're reactive they don't last very long and they can be very damaging.
Posted: Thu Nov 15, 2018 10:50 pm
Aim to get formal charge close to 0 and base the placement of your radical on that.
Posted: Sun Nov 25, 2018 5:18 pm
Quick question, are we going to have to know in-depth about radicals or just know a basic application of it for the final?
Posted: Sun Nov 25, 2018 5:28 pm
I think just the basic application, and where it comes up and how it affects the molecule (ie makes it more unstable)
Posted: Sun Nov 25, 2018 5:45 pm
I remember doing a homework question where you have to draw the lewis structure of ClO. Since there are only 13 electrons available for the structure, I naturally thought that Cl had a full octet and O had only 7 electrons, with one electron by itself to show that ClO is a radical. However, the answer key says that O has a full octet instead. What's the difference and why is the latter structure more correct?
Posted: Sun Nov 25, 2018 7:47 pm
Molecules usually with an odd number of electrons will be considered a radical.