Ni2+(aq)+Mg(s)→Ni(s)+Mg2+(aq)

Indicate the half-reaction occurring at Anode.
Indicate the half-reaction occurring at Cathode.

Anode oxidation

Mg -----> Mg2^+ + 2e^-

Cathode reduction

Ni2^+ 2 e^- -------> Ni

Anode: "Hey, I'm feeling a little negative today, so I'll be the anode! Watch me go from Ni2+ to Ni(s). It's like I'm shedding my positive vibes and becoming a shiny nickel!"

Cathode: "Ah, the cathode, the place where all the magic happens! Here, our friend Mg(s) will take center stage and go from its elemental form to Mg2+ in the solution. It's like watching a metallic superstar make a guest appearance in a chemical reaction!"

To determine the half-reaction occurring at the anode and the cathode in the given redox reaction:

Step 1: Identify the species that is oxidized and reduced.
In this reaction, Ni2+ is reduced to Ni, and Mg is oxidized to Mg2+.

Step 2: Write out the half-reactions for oxidation and reduction.
Oxidation half-reaction: Mg(s) → Mg2+(aq) + 2e-
Reduction half-reaction: Ni2+(aq) + 2e- → Ni(s)

Step 3: Determine the anode and cathode.
The anode is where oxidation occurs, and the cathode is where reduction occurs.
So, the oxidation half-reaction occurs at the anode, and the reduction half-reaction occurs at the cathode.

Therefore, the half-reaction occurring at the anode is:
Mg(s) → Mg2+(aq) + 2e-

And the half-reaction occurring at the cathode is:
Ni2+(aq) + 2e- → Ni(s)

To determine the half-reactions occurring at the anode and cathode in the given reaction:

Step 1: Understand the process:
In an electrochemical cell, oxidation occurs at the anode, while reduction occurs at the cathode. In this case, Ni2+ ion is being reduced to Ni metal, indicating the cathode. At the same time, Mg metal is being oxidized to Mg2+ ion, which indicates the anode.

Step 2: Identify the changes in oxidation states:
In the reaction:

Ni2+(aq) + Mg(s) → Ni(s) + Mg2+(aq)

The oxidation state of Ni changes from +2 to 0. Therefore, the half-reaction for reduction (cathode) is:

Ni2+(aq) + 2e- → Ni(s)

The oxidation state of Mg changes from 0 to +2. Therefore, the half-reaction for oxidation (anode) is:

Mg(s) → Mg2+(aq) + 2e-

So, the half-reaction occurring at the anode is:
Mg(s) → Mg2+(aq) + 2e-

And the half-reaction occurring at the cathode is:
Ni2+(aq) + 2e- → Ni(s)