In the redox reaction AgNO3 + Na, the sodium (Na) metal acts as a reducing agent, while the silver nitrate (AgNO3) acts as the oxidizing agent. The overall reaction can be represented as follows:

2AgNO3 + 2Na → 2NaNO3 + 2Ag

In this reaction, sodium loses electrons (oxidation), while silver gains electrons (reduction).

Here's a more detailed explanation of the process:

1. Oxidation of Sodium (Na):

- Sodium (Na) atoms lose one valence electron each, forming sodium ions (Na+).

- Each sodium atom undergoes oxidation, resulting in an increase in its oxidation state from 0 (in elemental sodium) to +1 (in sodium ions).

- The oxidation half-reaction can be represented as:

2Na → 2Na+ + 2e-

2. Reduction of Silver (Ag):

- Silver ions (Ag+) gain electrons from the sodium atoms.

- Each silver ion accepts one electron, resulting in a decrease in its oxidation state from +1 (in silver ions) to 0 (in elemental silver).

- The reduction half-reaction can be represented as:

2Ag+ + 2e- → 2Ag

By combining the two half-reactions, we get the overall redox reaction:

2AgNO3 + 2Na → 2NaNO3 + 2Ag

In summary, sodium (Na) undergoes oxidation, losing electrons and increasing its oxidation state, while silver (Ag) undergoes reduction, gaining electrons and decreasing its oxidation state.