Kclo3 > kcl+3/2o2 assign oxidation states to each element on each side of the equation.(reactants and produc? kclo3 > kcl+3/2o2 which element is oxidized?

K will always have an oxidation state of +1. Now O is -2 except in peroxides, this is not a peroxide, so total charge will be -6, if you subtract the +1 of K from it, it leaves -5 charge to be neutralized by Cl in KClO3, so Cl will be +5. In the product side, K will still have the same oxdiation which is +1 and Cl would have -1. O2 will have zero. Now, Cl is gaining the electrons to go from +5 to -1, so it is getting reduced while O2 is losing electrons to go from -2 to zero so it is getting oxidized.

100%sorry if i’m wronghope this good luck: )