HOCl vs OCl - oxidation state two ways?

[MrNeuro]

1) so for H - O - Cl

O can be H --- - O + --- Cl

O is 0 ( +1 -1 = 0)

or

2)
H = +1
O = -2
Cl = +1 based upon the rules of oxidation state naming.....

which one is right?

also how would you find the ox state of O in OCl- using the first method

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[BerkReviewTeach]

1) so for H - O - Cl

O can be H --- - O + --- Cl

O is 0 ( +1 -1 = 0)

or

2)
H = +1
O = -2
Cl = +1 based upon the rules of oxidation state naming.....

which one is right?

also how would you find the ox state of O in OCl- using the first method

Your first option is not true. Oxygen is more electronegative than chlorine, so it will take a negative and give Cl a positive in that bond. H+ —— -O- —— +Cl. This matches with your second option.

For ClO-, there is a negative formal charge on oxygen, so it would be: -O- —— +Cl, making O -2 and Cl +1. Deprotonating hypochlorous acid will not change oxidation states on any atom. They only change in redox reactions.

 

[chiddler]

oxidation state is determined by the ligands bound to a given atom. if they are more electronegative, that atom gets -1 and the atom of interest gets +1. in this case, oxygen is the most electronegative and therefore cannot be 0.

really the only time you see 0 oxidation state oxygen is when it is elemental.

 

[misseskwee]

Nope, in HOCl, O is still going to have an oxidation state of -2, H is +1, so Cl is +1. Remember that O is more electronegative so it should be the negative one between it and Cl. Also O is almost always -2 unless it's with peroxides in which case it'll be -1.

 

[MrNeuro]

Your first option is not true. Oxygen is more electronegative than chlorine, so it will take a negative and give Cl a positive in that bond. H+ —— -O- —— +Cl. This matches with your second option.

For ClO-, there is a negative formal charge on oxygen, so it would be: -O- —— +Cl, making O -2 and Cl +1. Deprotonating hypochlorous acid will not change oxidation states on any atom. They only change in redox reactions.

oxidation state is determined by the ligands bound to a given atom. if they are more electronegative, that atom gets -1 and the atom of interest gets +1. in this case, oxygen is the most electronegative and therefore cannot be 0.

really the only time you see 0 oxidation state oxygen is when it is elemental.

Nope, in HOCl, O is still going to have an oxidation state of -2, H is +1, so Cl is +1. Remember that O is more electronegative so it should be the negative one between it and Cl. Also O is almost always -2 unless it's with peroxides in which case it'll be -1.

so why is it easier to remove oxygen from HOCl than from -OCl??? is it because of the negative formal charge?