Chapter 21, Problem 7RAT

What element is oxidized in the following equation and what element is reduced?

${\text{Sn}}^{2+}+\text{2Ag}\to \text{Sn}+2{\text{Ag}}^{+}$

(a) The tin ion, ${\text{Sn}}^{2+}$ , is oxidized, while the silver, $\text{Ag}$ , is reduced.

(b) The tin ion, ${\text{Sn}}^{2+}$ , is reduced while the silver, $\text{Ag}$ , is oxidized.

(c) Both the tin ion, ${\text{Sn}}^{2+}$ , and the silver, $\text{Ag}$ , are reduced.

(d) Bob the tin ion, ${\text{Sn}}^{2+}$ , and the silver, $\text{Ag}$ , are oxidized.

To determine

The correct option for the statement “What element is oxidized in the following equation and what element is reduced?”

${\text{Sn}}^{2+}+\text{2Ag}\to \text{Sn}+2{\text{Ag}}^{+}$

Answer to Problem 7RAT

The correct option for the statement “What element is oxidized in the following equation and what element is reduced?” is option (b).

Explanation of Solution

The electrons are donated in an oxidation reaction while in reduction reaction the electrons are gained.

The given equation is shown below.

${\text{Sn}}^{2+}+\text{2Ag}\to \text{Sn}+2{\text{Ag}}^{+}$

The silver atoms, $\text{Ag}$ , lost the electrons. So, it is oxidized.

The tin ions, ${\text{Sn}}^{2+}$ , gained the electrons. So, it is reduced.

Conclusion:

Therefore, the correct option for the statement “What element is oxidized in the following equation and what element is reduced?” is option (b).