What is the effect of a more electronegative atom on the strength of an ionic bond?

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).

Which one of the following is true about $NaCl$ and $KCl$?

Which of the following is not correct regarding the properties of ionic compounds?

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:

The electronic configurations of four elements $L$,$P$,$Q$,and $R$ are given as: $L (1s^2, 2s^2 2p^4)$; $Q (1s^2, 2s^2 2p^6, 3s^2 3p^5)$; $P (1s^2, 2s^2 2p^6, 3s^1)$; $R (1s^2, 2s^2 2p^6, 3s^2)$. The formulas of the ionic compounds that can be formed between these elements are: