I'm trying to help lead my daughter to a solution and my high school chemistry is almost 30 years ago.
For the following reaction, indicate the species being oxidezed and reduced and show the oxidation numbers above these symbols. Lastly, indicate the number of electrons that have been lost or gained.
$$\ce{2 KBrO3 -> 2 KBr + 3 O2}$$
What is being oxidized, and what is being reduced? My daughter tells me that since the charge on the two components doesn't change there isn't reduction or oxidation. You could almost say the $\ce{KBr}$ is being 'de-oxidized' because it's losing oxygen, but that would mean the oxygen is being oxidized, which in this case seems nonsensical.
If someone can explain to me which it is and why, so I can walk her through it, or direct me to a place where this is done, I'd appreciate it. This is beyond my knowledge.