How Does Na2O Behave As A Reducing Agent?

Na2O behaves as a reducing agent by donating electrons to another substance and thereby causing its reduction. Specifically, in the presence of a substance that can accept electrons (an oxidizing agent), Na2O will donate one or more electrons to the oxidizing agent, itself becoming oxidized in the process. This electron transfer can often be observed through the change in oxidation state of the reactants and products involved.

More specifically, when Na2O reacts with an oxidizing agent, it can transfer electrons to reduce the oxidizing agent. For example, when Na2O is added to a solution containing CuO, the following reaction occurs:

2Na2O + CuO → 2Na2O·CuO

In this reaction, Na2O donates electrons to CuO, which results in the formation of a new compound, Na2O·CuO, where Cu has a lower oxidation state than in CuO (i.e., Cu2+ → Cu+). The Na2O itself becomes oxidized in the process, gaining oxygen to form a peroxide (i.e. Na2O → Na2O2).

Overall, Na2O acts as a reducing agent by donating electrons to an oxidizing agent and thereby facilitating its reduction.