Question

what is the net ionic equation of Fe3+ and Br-, the species oxidized/reduced.

what is the net ionic equation of I2 and Br-, and the species oxidized/reduced, the stronger oxidizing agent.

Answer 1

I_{​​​​​​2} + 2Br^{​​​​​-} ----------> 2I^- + Br_{​​​​​2}

Oxidation state of Iodine in I_{​​​​​​2} : 2x = 0

x = 0

Oxidation state of Iodine in I^{​​​​​​-} is x = -1

Oxidation state of Bromine in Br_​​​2 is 2x = 0

x = 0

Oxidation state of Bromine in Br^{​​​​​-} is x = -1

Oxidation state of Iodine decreases from 0 to -1;

Therefore it is a reduction Reaction

Similarly oxidation state of Bromine increases from -1 to 0. So it is a oxidation.

Oxidation state of Iodine decreases from 0 to -1. So it is a reduction.

Iodine oxidizes bromide ion to bromine. So iodine is a oxidizing agent.

Similarly Bromide ion reduces iodine to iodide. So Bromide ion is a reducing agent.

2)

Net ionic equation between Ferric ion (Fe^{​​​​​3+} ) and Bromide ( Br^{​​​​​-} ion ) is

2Fe^{​​​​​3+} +2 Br^{​​​​​-} -----------> 2 Fe^{​​​​​2+} + Br_{​​​​​2}

Oxidation state of Fe in Fe^{​​​​​3+} is +3

Oxidation state of Fe in Fe^{​​​​​2+} is +2

Oxidation state of Bromine in Br_​​​2 is 2x = 0

x = 0

Oxidation state of Bromine in Br^{​​​​​-} is x = -1

oxidation state of Bromine increases from -1 to 0. So it is a oxidation.

Oxidation state of Fe^​​​ decreases from +3 to +2. So it is a reduction.

Fe^{​​​​​3+} ion oxidizes bromide ion to Bromine. Ferric ion (Fe^{​​​​​3+} ) is a reducing agent.

Bromide ion (Br^{​​​​​-} ), reduces Ferric ion to ferrous ion. Bromide ion is a reducing agent.