Please help verify my answer. Not confident it is right:

please verify my answer:

Consider the following REDOX reaction:
Zn(s) + Pb+2(aq) �� Zn+2(aq) + Pb(s)

a. Write the oxidation and reduction half-cell reactions.

Zn(s) + Pb+2(aq) �� Zn+2(aq) + Pb(s)
+2 +4 +2 +4

Zn(s)->Zn2+(aq)+2e- (zinc is oxidized)
Pb2+(aq)+2e- ->Pb(s)(lead is reduced)

b. Show this reaction in shorthand notation. (2 marks)

Zn(s)| Zn2+(aq) || Pb2+(aq) | Pb(s)

If it's wrong please tell me how. Thank you for your help :)

I answered this last night that it looked good to me.

Sorry didn't see...thank you!

To verify your answer, let's go through it step by step.

a. Writing the oxidation and reduction half-cell reactions:
Your answer is correct. In the given reaction, zinc (Zn) is oxidized and loses two electrons to form Zn2+. This is represented as:
Zn(s) -> Zn2+(aq) + 2e- (oxidation)

On the other hand, lead (Pb2+) gains two electrons to form solid lead (Pb). The reduction half-cell reaction is:
Pb2+(aq) + 2e- -> Pb(s) (reduction)

b. Showing the reaction in shorthand notation:
Your answer is correct. The shorthand notation for the given reaction is:
Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s)

The vertical line (|) separates the species in different phases. The double vertical line (||) separates the two half-cells.

Overall, your answer is correct. Both the oxidation and reduction half-cell reactions and the shorthand notation are accurate representations of the given redox reaction. Well done!