In Coulomb's Law, what is the effect of distance on the interaction between charges?

Coulomb's Law states that the force between two charged particles is inversely proportional to the square of the distance between them. This means that as the distance between the charges increases, the force of interaction (either attraction or repulsion) decreases significantly. The nature of the interaction—whether it is an attractive force (as with opposite charges) or a repulsive force (as with like charges)—depends on the types of charges involved. Thus, the effect of distance is fundamental to how strong the force of attraction or repulsion will be, verifying that distance indeed affects both the magnitude of the force and the nature of the interaction based on the types of charges involved.

Options that suggest no effect or that distance does not influence attraction misrepresent this fundamental principle of electrostatics, as they overlook the crucial role distance plays in determining the strength of the force according to Coulomb's Law, which is mathematically defined as ( F = k \cdot \frac{|q_1 \cdot q_2|}{r^2} ), where ( r ) is the distance between the charges.