16 posts • Page 1 of 1
Holdup... isn't the oxidation state of O2 equal to zero? O2 has two oxygens, which means that they both have the same electronegativity and as a result, they share the electrons equally among themselves. Therefore the oxygen should not have gained electrons from itself. The oxidation numbers of pure elements (such as O3) is zero since the electrons aren't pulled to one atom specifically due to their equal electronegativities. Oxygen in a compound with different atoms will have an oxidation state of -2 (except for peroxides) since it likes electrons more than the other atoms in the compound.
Michelle Song 1I wrote:Shouldn't the oxidation state of oxygen in O2 be zero?
The oxidation state of each individual oxygen in compounds that have other elements of different electronegativity is -2, except in peroxides where it's -1. In O2, where there's no polarity in the bonds shared due to the fact that both oxygen atoms have the same electronegativity, the average oxidation state would be 0.
(It is possible but most likely unlikely that you are thinking of the standard enthalpy of formation of O2, which is 0 because that is in its standard state.)
Who is online
Users browsing this forum: No registered users and 3 guests