In the electrolysis of a molten mixture of NaCl 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 cathode 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. When comparing $C{l}^{-}$and$B{r}^{-}$,$B{r}^{-}$ is the less electronegative of the two. At the anode,$B{r}_2$ is produced.

The cation with the highest ionization energy forms in the cathode. When a cation's ionization energy is higher, it means that more energy is required to remove the electron, and there is a stronger attraction between the atom and the electron, making it a more powerful oxidizing agent. Ionization energy grows upwards and to the right in the periodic table.$C{a}^{2+}$ has a larger ionization energy than $N{a}^{+}$, and will thus be transformed to calcium metal in the cathode.