Write the oxidation and reduction half-reactions (without states of matter) for the following reaction:→+Nas  Ag+aq + Na+aq  Ags

To break down the given redox reaction involving silver ions ($\text{Ag}^+$) and sodium ($\text{Na}$), we need to identify the oxidation and reduction processes separately.

1. Break Down the Problem

The overall reaction is: $\text{Na} + \text{Ag}^+ \rightarrow \text{Na}^+ + \text{Ag}$

From this, we can determine the half-reactions for oxidation and reduction.

2. Relevant Concepts

• Oxidation is the process where an atom, ion, or molecule loses electrons.
• Reduction is the process where an atom, ion, or molecule gains electrons.

3. Analysis and Detail

1. Oxidation Half-Reaction: Sodium ($\text{Na}$) is oxidized to sodium ions ($\text{Na}^+$). $\text{Na} \rightarrow \text{Na}^+ + e^-$

2. Reduction Half-Reaction: Silver ions ($\text{Ag}^+$) are reduced to silver metal ($\text{Ag}$). $\text{Ag}^+ + e^- \rightarrow \text{Ag}$

4. Verify and Summarize

Both half-reactions are balanced in terms of charge and mass. In the oxidation half-reaction, sodium goes from a neutral state to a +1 state (losing one electron). In the reduction half-reaction, silver goes from a +1 state to a neutral state (gaining one electron).

Final Answer

The oxidation half-reaction is: $\text{Na} \rightarrow \text{Na}^+ + e^-$

The reduction half-reaction is: $\text{Ag}^+ + e^- \rightarrow \text{Ag}$