[mdk2121]

Hi! I am still trying to wrap my mind around redox chemistry and have a quick question about water. I understand that water can act as an oxidizing or reducing agent. The example I have read of this behavior is when two water molecules react, forming H₃O⁺ and OH^-.

However, I am confused about how this demonstrates water acting as a reducing and oxidizing agent. In the above reaction, I thought that one water molecule was simply acquiring the other water molecule's H+, which would be the transfer of a proton. And when I look at the oxidation states of the individual atoms involved in the final reaction, all O oxidation states seem to be -2 and all H oxidation states seem to be +1. I of course understand that charge is changing in terms of molecules, but I don't see how it represents transfer of electrons or changes in individual atoms' oxidation states. What am I missing?

Thank you so much!

[mjc123]

You are right. That is not a redox reaction.

[mdk2121]

Oh! Thank you! I suppose my source was incorrect, then.

[Babcock_Hall]

This may be on a tangent, but water is the reductant in photosynthesis.