Final answer:
The statement that the force of attraction between ions in an ionic compound increases with the charge and decreases with increased distance is true, aligning with Coulomb's Law in electrostatic attraction.
Step-by-step explanation:
The force of attraction between ions in an ionic compound increases with the charge value and decreases with increased distance. This statement is True. The ionic bond is a manifestation of the electrostatic force that adheres oppositely charged ions together. The strength of this attraction is directly proportional to the magnitude of the charges on each ion and inversely proportional to the square of the distance between them, as described by Coulomb's Law.
For example, ions with a 2+ or 2- charge will have a stronger ionic bond compared to ions with a 1+ or 1- charge, given the same separation distance. Conversely, as the distance between ions increases, the attractive force diminishes. Hence, a larger ion, which by definition has a larger radius, will have a weaker ionic bond due to the greater distance between its outermost electrons and the nucleus of an oppositely charged ion.
To illustrate, consider two ions of single charge separated by a distance 'd'. The force of attraction is inversely proportional to the square of the distance (d²). If the distance is doubled (2d), the force of attraction becomes inversely proportional to (2d)², or 4 times d², which is a weaker force. Similarly, two ions of double charge separated by distance 'd' have an attractive force proportional to (2)(-2)/d², which is stronger compared to ions with single charges.