what element is undergoing oxidation in the following reaction Zn(s)+AgNO3(aq) Zn(NO3)2(aq)+2Ag(s)
To determine which element is undergoing oxidation in a chemical reaction, you need to identify the changes in oxidation states of the elements involved.
In the given reaction:
Zn(s) + AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s)
We can assign oxidation states to the elements:
Zn(s): The oxidation state of an element in its elemental form is always zero.
AgNO3(aq): Ag has an oxidation state of +1, and NO3 has an oxidation state of -1.
Zn(NO3)2(aq): Zn has an oxidation state of +2, and NO3 has an oxidation state of -1.
2Ag(s): Ag is in its elemental form, so the oxidation state is zero.
Now, let's look at the changes in oxidation state:
Zn(s) → Zn(NO3)2(aq) (oxidation state changes from 0 to +2)
AgNO3(aq) → 2Ag(s) (oxidation state changes from +1 to 0)
From the changes in oxidation states, we can observe that the element zinc (Zn) is undergoing oxidation. Its oxidation state increases from 0 in Zn(s) to +2 in Zn(NO3)2(aq).
In the given reaction Zn(s) + AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s), the element undergoing oxidation is zinc, represented by the symbol Zn.
To determine the oxidation state of an element, we need to compare the number of electrons gained or lost by that element.
In this reaction, zinc (Zn) goes from a neutral state (oxidation state of 0) in the reactant (Zn(s)) to a positive oxidation state of +2 in the product (Zn(NO3)2(aq)). This means that zinc lost 2 electrons during the reaction, indicating oxidation.
Hence, zinc is undergoing oxidation in this reaction.
Zn goes from +2 on the left to zero on the right.
Ag goes from +1 on the left to zero on the right.
Oxidation is the loss of electrons.