Write the reduction half-reaction for the reduction of elemental oxygen in the presence of water, producing hydroxide ions
This does not make sense to me - a half reaction (from what I understand) is when you have an "element + some number of electrons -> element charged" or "charged element -> element + some number of electrons"
Reaction:
$\ce{HOH + O -> 2OH}$
Oxidation States: They all seem to be neutral to me - but I may be missing something.
So, how is a half reaction being introduced into this and what would it look like? Also, how can i know which element/compound is reduced/oxidized and is the reducing agent/oxidizing agent?
I am really sorry if this seems simple but I am a chem noob and I was out for a month and my teacher is behind schedule so he is giving us worksheets without teaching and i do not understand a lot. Thank you for your time