What is the oxidation half-reaction for Mg(s)+ZnCL2(aq)>MgCL2(aq)+Zn(s)?

To determine the oxidation half-reaction in the given chemical equation, let's identify the oxidation states of each element involved.

In this equation, we have:

Mg(s) + ZnCl2(aq) → MgCl2(aq) + Zn(s)

Oxidation states:
- Magnesium (Mg) has an oxidation state of 0 since it is in its elemental form.
- Chlorine (Cl) has an oxidation state of -1.
- Zinc (Zn) also has an oxidation state of 0 since it is in its elemental form.

To write the oxidation half-reaction, we need to show the change in oxidation state of the element that is being oxidized.

In this case, magnesium (Mg) is being oxidized as it goes from an oxidation state of 0 to +2 in the compound MgCl2. Therefore, the oxidation half-reaction for Mg is:

Mg(s) → Mg^2+(aq) + 2e-

To balance the charges, two electrons (2e-) are added on the right-hand side of the equation.

So, the oxidation half-reaction for Mg(s) in the given chemical equation is:

Mg(s) → Mg^2+(aq) + 2e-

To determine the oxidation half-reaction in this chemical equation, we need to identify the element that is being oxidized (undergoing oxidation) and the element that is being reduced (undergoing reduction).

In this reaction, magnesium (Mg) is being oxidized, meaning it is losing electrons, and zinc (Zn) is being reduced, meaning it is gaining electrons.

To write the oxidation half-reaction, we need to show how magnesium is losing electrons. Since magnesium is a neutral atom, it needs to lose two electrons to achieve a stable electron configuration.

So, the oxidation half-reaction for this reaction is:

Mg ➝ Mg2+ + 2e-

This half-reaction represents the oxidation of magnesium, where magnesium loses two electrons to form a magnesium ion with a +2 charge.

Remember, oxidation involves the loss of electrons, and the oxidation state of magnesium increases from 0 (as a neutral atom) to +2 (as a magnesium ion).

For the reduction half-reaction, we need to write the half-reaction for zinc gaining electrons. The reduction half-reaction is:

Zn2+ + 2e- ➝ Zn

This half-reaction represents the reduction of zinc, where zinc gains two electrons to form a neutral zinc atom.

Remember, reduction involves the gain of electrons, and the oxidation state of zinc decreases from +2 (as a zinc ion) to 0 (as a neutral atom).

By combining these oxidation and reduction half-reactions, you get the overall balanced chemical equation for the given reaction:
2Mg(s) + ZnCl2(aq) ➝ 2MgCl2(aq) + Zn(s)

Oxidation is the loss of electrons. Which of the half reactions has lost electrons. Write each one.

Mg(s) ==> Mg^2+(aq) + 2e
Zn^2+(aq) + 2e ==> Zn(s)