This means we can usually assume that ions with greater magnitude charges will result in greater lattice energies, and without having to take into consideration the atomic radii. Generally the charges of the ions have more bearing than the distance between them when determining lattice energies.
If the goal is to maximize the lattice energy then you'd want ions with larger magnitude charges and/or small in size ions. So both the magnitude of the ion's charges and their atomic radii effect the lattice energy. And the denominator consists of of the distance between the two ions, squared. If we observe the equation of Coulomb's Law the numerator consists of the product of the absolute value of the charges of the ions. So lattice energy is measuring how attracted both the ions are to each other in an ionic compound. In ionic compounds the force is always attractive since the ions have different charges.
Whether the force is attractive or repulsive depends on whether the charges have the same sign or not. Coulomb's Law describes the force of attraction (or repulsion) between two point charges. Lattice energies of ionic compounds broadly correspond with Coulomb's Law which Sal provided in the video.
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