An atom of sodium loses one electron and a chlorine atom accepts one electron. This results in the formation of a sodium chloride molecule. This type of molecule will be:

If the enthalpy of sublimation of $Li$ is $155 \ kJ \ mol^{-1}$,enthalpy of dissociation of $F_2$ is $150 \ kJ \ mol^{-1}$,ionization enthalpy of $Li$ is $520 \ kJ \ mol^{-1}$,electron gain enthalpy of $F$ is $-313 \ kJ \ mol^{-1}$,and standard enthalpy of formation of $LiF$ is $-594 \ kJ \ mol^{-1}$,then the magnitude of the lattice enthalpy of $LiF$ is . . . . . . $kJ \ mol^{-1}$ (nearest integer).

The ionization of $AlCl_3$ in aqueous solution occurs because ........

Favourable conditions for electrovalency are

Provide the steps and their corresponding enthalpies for the formation of $NaCl$ (sodium chloride).

In the formation of $NaCl$ from $Na$ and $Cl$,which of the following occurs?