Radicals

(Polar molecules, Non-polar molecules, etc.)

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Abby Ellstrom 1I
Posts: 53
Joined: Fri Sep 29, 2017 7:04 am

Radicals

Postby Abby Ellstrom 1I » Thu Nov 16, 2017 6:47 pm

How do you know where to put the radical when drawing a lewis structure?

SantanaRodriguezDis1G
Posts: 56
Joined: Sat Jul 22, 2017 3:00 am

Re: Radicals

Postby SantanaRodriguezDis1G » Thu Nov 16, 2017 8:03 pm

A radical is electrons with unpaired spins. I assume you must first evaluate all the elements of the compound. For example on the midterm it would not make sense to put the one electron on oxygen or hydrogen because their octets are already full, leaving the electron to be put on carbon.

Madelyn Gehrich 1E
Posts: 23
Joined: Fri Sep 29, 2017 7:05 am
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Re: Radicals

Postby Madelyn Gehrich 1E » Thu Nov 16, 2017 8:26 pm

Generally, you would put the radical on the central atom.

David Zhou 1L
Posts: 61
Joined: Fri Sep 29, 2017 7:04 am

Re: Radicals

Postby David Zhou 1L » Fri Nov 17, 2017 7:54 pm

Elements that are more electronegative will attract the electrons more so than less electronegative elements. Therefore, the single unpaired electron will tend to be on the less electronegative element, since the more electronegative elements will likely attract full valence shells.

Also, it's always a good idea to check formal charge, that will give you clues as to where to put it too.

Diego Zavala 2I
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Re: Radicals

Postby Diego Zavala 2I » Sat Nov 18, 2017 2:10 pm

I calculate the formal charges on every atom in the compound and if one atom has a +1 formal charge (assuming all other atoms have a formal charge of zero), then I would place the radical electron on the atom with the +1 formal charge so that the new formal charge will be 0 and the molecule will be more stable


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