In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy. Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. ||lattice energy||

The question is incomplete, the complete question is:

In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, rank these compounds of their expected lattice energy..

Note: Many sources define lattice energies as negative values. Please rank by magnitude and ignore the sign. |Lattice energy| = absolute value of the lattice energy.

RbCl ,RbBr ,Rbl ,RbF

RbF> RbCl>RbBr>RbI

Explanation:

As it was rightly stated in the question, the lattice energy depends on the size of the ions and their distance if separation according to Coulomb's law.

Looking at the ionic salts stated, the action size is the same but the anion sizes vary. The smaller, the anion size, the higher the lattice energy.

Since ionic size increases steadily from Fluorine to iodine, lattice energy decreases in that order since the distance of separation of the ions increases as the ions become larger. Hence the answer.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.