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Using lewis structure,determine which of CO and OH is a radical (2)Why is it possible for a molecule to have polar bonds yet have a dipole moment of zero?
##OH## is a radical.
A radical is a molecule or ion that has an unpaired electron. You can use the of the two to see if either of them has an unpaired electron.
Start with carbon monoxide. The molecule has a total of 10 , 4 from carbon and 6 from oxygen.
Its Lewis structure will looks like this
The triple bond that exists between carbon and oxygen accounts for 6 of the 10 of the molecule, the rest being distributed as lone pairs on carbon and on oxygen, respectively.
As you can see, this molecule does not have an unpaired electron, so it cannot be radical.
Now take a look at ##OH##, which is actually the neutral form of the hydroxide anion, ##OH^(-)##. Since the hydroxide anion has a -1 negative charge, its neutral form will have one less electron.
The hydroxide ion has a total of 8 - 6 from oxygen, 1 from hydrogen, and 1 extra electron that gives it the negative.
Take a look at the Lewis structure of the hydroxide anion
In order to get the neutral form, you're going to have to remove an electron from the ion. This electron can only come from a lone pair located on oxygen.
This will get you
Now the ion has an unpaired electron, which means that it is a radical.
More often than not, you'll see ##OH##, which is called hydroxyl radical, written as ##*OH##.