ccc matter and energy explain how you would expect the strength of the ionic bonds in potassium bromide…

Brief Explanations:

Ionic bond strength is influenced by ion size and charge. In (KBr) and (LiBr), the charge on both (K^{+}) and (Li^{+}) is (+ 1), and the charge on (Br^{-}) is (-1) in both compounds. However, the (Li^{+}) ion is smaller than the (K^{+}) ion ((Li^{+}) has a smaller atomic radius as it is higher up in the alkali - metal group). According to Coulomb's law ((F = k\frac{q_1q_2}{r^{2}}), where (q_1) and (q_2) are the charges of the ions and (r) is the distance between the ions), when the charges ((q_1) and (q_2)) are the same, a smaller distance ((r)) (due to smaller ion size) leads to a stronger force of attraction. Since the distance between (Li^{+}) and (Br^{-}) is smaller than the distance between (K^{+}) and (Br^{-}), the ionic bonds in (LiBr) are stronger than those in (KBr).

Answer:

The ionic bonds in (LiBr) are stronger than those in (KBr).