try comparing the e values with of silver and i think you will see a reason why..
To compare the E values of silver, we need to refer to a reference table called the Standard Electromotive Series. This table lists the E values of different elements and allows us to compare their relative tendencies to undergo oxidation or reduction reactions.
The E value for silver, also known as the standard reduction potential (E°), is +0.80 V. This value indicates the tendency of silver to undergo reduction (gain electrons) in an electrochemical cell.
By comparing the E values of different elements, we can determine the likelihood of a redox reaction occurring between them. A higher E value indicates a greater tendency to be reduced, while a lower E value indicates a greater tendency to be oxidized (lose electrons). The larger the difference in E values between two elements, the more favorable the redox reaction is.
For example, if we compare the E value of silver with another metal like copper, which has an E value of +0.34 V, we can see that silver has a higher E value. This means that silver is more likely to be reduced (gain electrons) compared to copper. Therefore, in a redox reaction between a silver ion (Ag+) and a copper ion (Cu2+), silver ions will tend to gain electrons and be reduced while copper ions will tend to lose electrons and be oxidized.
In summary, the reason why silver has a higher E value than some other elements is that it has a greater tendency to be reduced in a redox reaction. This indicates its ability to gain electrons and become an electrically neutral metal.