Sodium metal is produced at the anode

Chloride ions are reduced at the positive electrode

Sodium ions are oxidised at the negative electrode

Chlorine gas is produced at the anode

The more reactive metal has a higher ionization energy

The more reactive metal is a stronger oxidizing agent

The more reactive metal is more easily oxidized

The more reactive metal has a lower electronegativity

$\text{NaOH}+\text{HCl}\to \text{NaCl}+{\text{H}}_2\text{O}$

${\text{BaCl}}_2+{\text{Na}}_2{\text{SO}}_4\to {\text{BaSO}}_4+2\text{NaCl}$

${\text{Cu}}^{2+}+\text{Zn}\to \text{Cu}+{\text{Zn}}^{2+}$

${\text{CaCO}}_3\to \text{CaO}+{\text{CO}}_2$

$+2\to +3$

$0\to +1$

$+5\to +2$

$-1\to 0$

They involve the sharing of electrons between atoms.

They always occur in covalent bond formations.

They result in the oxidation of one species and the reduction of another.

They do not affect the oxidation states of the elements involved.