Explain why this reaction is considered a redox reaction
A redox reaction is a type of chemical reaction that involves a transfer of electrons between two species. In this type of reaction, one species loses electrons (oxidation) while another species gains those electrons (reduction).
To determine if a reaction is a redox reaction, we need to assess the change in oxidation states of the elements involved. Oxidation state, or oxidation number, is a way to keep track of the electrons gained or lost by an atom in a compound.
In a redox reaction, the oxidation state of at least one element changes. Let's consider an example reaction:
2Na + Cl2 -> 2NaCl
In this reaction, sodium (Na) is initially in its elemental state with an oxidation state of 0. Chlorine (Cl) is also in its elemental state with an oxidation state of 0. However, after the reaction takes place, sodium becomes positively charged as it donates one electron to chlorine. So, the oxidation state of Na goes from 0 to +1, indicating oxidation. On the other hand, chlorine receives this electron and its oxidation state changes from 0 to -1, indicating reduction.
Since there is a transfer of electrons between the sodium and chlorine, this reaction is considered a redox reaction.