In the electrolysis of a molten mixture of KI and, identify the product that forms at the anode and at the cathode.

The process of dissolving ionic compounds into their constituent components by delivering a direct electric current through the complex in a fluid form is known as electrolysis. At the cathode, cations are reduced, whereas anions are oxidized.

Because it has a lower affinity for electrons, the less electronegative anion forms at the anode during the electrolysis of molten mixtures and is thus more easily oxidized. In the periodic table, electronegativity increases as you move to the right and upwards. Between $I^{-}$and $F^{-}$, $F^{-}$is the less electronegative of the two. At the anode,$I_2$ is produced.

The cation with the highest ionization energy forms in the cathode. When a cation has a higher ionization energy, it signifies that more energy is required to remove the electron, that the atom and electron have a stronger attraction, and that the oxidizing table is stronger. Ionization energy increases upwards and to the right.$M{g}^{2+}$ has a larger ionization energy than ${\text{K}}^{\text{+}}$, and hence will be transformed to magnesium metal in the cathode.