Half equation for Iron(ll) oxidized to (lll) show step by step working out?

The half equation for the oxidation of Iron(II) to Iron(III) can be written as:

Fe^2+ -> Fe^3+ + e^-

Step by step working out:

1. Write down the oxidation states of Iron in both the reactant and product:

Fe^2+ (Iron(II)) -> Fe^3+ (Iron(III))

2. Identify the change in oxidation state:

Fe^2+ -> Fe^3+

3. Determine the number of electrons involved in the oxidation process:

Fe^2+ loses one electron to become Fe^3+.

4. Write the half equation for the oxidation process:

Fe^2+ -> Fe^3+ + e^-

Step 1: Write the unbalanced half-equation.

Fe(II) → Fe(III) + e-

Step 2: Balance the atoms.

Since there is one Fe atom on both sides of the equation, it is already balanced with respect to Fe.

Step 3: Balance the charges.

The Fe(II) ion has a charge of +2, while the Fe(III) ion has a charge of +3. To balance the charges, we need to add one electron to the right-hand side of the equation:

Fe(II) → Fe(III) + e-

Balanced half-equation:

Fe(II) → Fe(III) + e-