The four major attractive forces between particles are ionic bonds, dipole-dipole attractions, hydrogen bonds, and dispersion forces. consider the compounds below, and classify each by its predominant attractive or intermolecular force among atoms or molecules of the same type

NaCl : In case of Sodium chloride Ionic bonding exists, as sodium is a cation and chloride is an anion. So, these two opposite charged species will attract each other and form ionic bond.

HF : In case of Hydrogen fluoride, Hydrogen bond interactions are found this is because when hydrogen is attached to either Oxygen, Nitrogen or Fluorine atom it gets involve in hydrogen bonding interactions with the neighbor oxygen, nitrogen or fluorine atom (highly electronegative).

HCl :  In Hydrogen chloride dipole dipole interactions exist. A partial positive hydrogen atoms interacts with a partial negative chlorine atom of neighbor molecule.

F2 : As fluorine molecule is neutral and charge less, so it will interact with another fluorine molecule through London dispersion forces.

Ifound this on google “these two compounds have a different ionic structure. caesium ion is larger in size when compared to the sodium ion. the charge gets more area to spread out evenly. so caesium chloride has a lower melting point than sodium chloride.” i hope this you for what your looking for

The answer is the first option just took the test