Which of the following choice is correct for the reaction?

$2\mathrm{Na}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\to 2{\mathrm{Na}}^{+}{\mathrm{Cl}}^{-}\left(\mathrm{s}\right)$

Na acts as reducing agent and Cl acts as oxidizing agent

All of the above are correct

Na is oxidised to ${\mathrm{Na}}^{+}$ by the loss of ${\mathrm{e}}^{-}$

Cl is reduced to ${\mathrm{Cl}}^{-}$ by the gain of ${\mathrm{e}}^{-}$