[alingy1]

Hi everyone, first post here!
I'm asked to determine if water acts as an acid in the following reaction:
2(Na₂O₂)+2(H₂O) 4 NaOH + O₂

I drew the lewis structure. I see that NaOH was added a hydrogen. But the corrector says that water is not an acid in this case. I don't understand why.

[Corribus]

I see that NaOH was added a hydrogen.

Are you sure about that?  If a substance like water acts as a Bronsted acid, what are your anticipated products?

[alingy1]

The product(s) is/are added a proton. Na2O2 separated itself in two. The water gave a hydrogen atom to each separated part of Na2O2. Am I lost?

[Corribus]

What makes you so sure that Na₂O₂ "separated itself in two"?  If your proposed mechanism is correct, then how did dioxygen form?  Think about the reaction and where each oxygen and hydrogen goes.  It might be helpful to label the oxygens "a" and "b" to keep track of them.

Let me ask another question.  Do you notice anything about the oxidation states of any of the elements?

[9-92-6-19]

It's not dioxygen; it's actually called peroxide. Normal oxide (O^2-) is very different than peroxide (O₂^2-). This may be important to your Lewis dot structure.

[Corribus]

Dioxygen (O₂) is a product in the reaction as it was written:

2(Na₂O₂)+2(H₂O) 4 NaOH + O₂