Amongst sodium halides $(NaF, NaCl, NaBr, NaI)$,$NaF$ has the highest melting point because of:

Arrange the bonds in order of increasing ionic character in the molecules: $LiF$,$K_{2}O$,$N_{2}$,$SO_{2}$ and $ClF_{3}$

Which of the following has the highest melting point?

The compound that has the highest ionic character associated with the $X-Cl$ bond is

When sodium and chlorine react,then:

Use the following data to calculate $\Delta _{lattice}H^{\theta }$ for $NaBr$. $\Delta _{sub}H^{\theta }$ for sodium metal $= 108.4 \ kJ \ mol^{-1}$,ionization enthalpy of sodium $= 496 \ kJ \ mol^{-1}$,electron gain enthalpy of bromine $= -325 \ kJ \ mol^{-1}$,bond dissociation enthalpy of bromine $= 192 \ kJ \ mol^{-1}$,$\Delta _{f}H^{\theta }$ for $NaBr_{(s)}$ $= -360.1 \ kJ \ mol^{-1}$.