What element is undergoing reduction in the following reaction?
Zn(s) + AgNO3(aq) --> Zn(NO3)2 + 2 Ag(s)
Oxidation is the loss of electrons. Remember the mnemonic Leo goes Grrr. Leo stands for loss electron exidation.
Reduction is the gain of electrons.
Look at Ag since Gaveen answered Ag. Ag is +1 oxidation state on the left. It is zero on the right. So silver goes from +1 to zero which is a gain of electrons. That is reduction.
To determine which element is undergoing reduction in the given reaction, we need to compare the oxidation states of each element on both sides of the reaction.
In the reactants, zinc (Zn) has an oxidation state of 0 since it is in its elemental form. Nitrate (NO3-) has an oxidation state of -1. Silver (Ag) has an oxidation state of +1, and nitrate (NO3-) has an oxidation state of -1.
In the products, zinc (Zn) now has an oxidation state of +2 in Zn(NO3)2, and silver (Ag) has an oxidation state of 0 since it is in its elemental form.
Therefore, zinc (Zn) is undergoing oxidation, while silver (Ag) is undergoing reduction in the given reaction.
To determine which element is undergoing reduction in a reaction, we need to compare the oxidation states of the elements involved before and after the reaction.
In this reaction:
Zn(s) + AgNO3(aq) --> Zn(NO3)2(aq) + 2 Ag(s)
We can assign oxidation states to each element:
- The oxidation state of Zn in Zn(s) is 0.
- The oxidation state of Ag in AgNO3(aq) is +1.
- The oxidation state of N in AgNO3(aq) is +5.
- The oxidation state of O in AgNO3(aq) is -2.
In Zn(NO3)2(aq), the overall charge for NO3 is -1, and since there are two nitrate ions, the total charge is -2. Therefore, the oxidation state of Zn in Zn(NO3)2(aq) is +2.
In Ag(s), the oxidation state of Ag is 0.
So, let's compare the oxidation states of Zn before and after the reaction:
- Before the reaction: Zn (0)
- After the reaction: Zn in Zn(NO3)2 (aq) (+2)
Based on the changes in oxidation states, we can see that Zn is going from an oxidation state of 0 to +2. This means Zn is being oxidized during the reaction.
On the other hand, Ag is going from an oxidation state of +1 in AgNO3 to 0 in Ag(s). This means Ag is being reduced during the reaction.
Therefore, in the reaction Zn(s) + AgNO3(aq) --> Zn(NO3)2(aq) + 2 Ag(s), the element undergoing reduction is silver (Ag).