Arrange the ions Rb⁺, Br^-, and Sr²⁺ from the smallest to the largest. (LO 6.4) (a) Br^- < Rb⁺ < Sr²⁺ (b) Sr²⁺ < Br^- < Rb⁺ (c) Rb⁺ < Sr²⁺ < Br^- (d) Sr²⁺ < Rb⁺ < Br^-

Ionic radius refers to the size of an ion in a crystal lattice. Cations (positively charged ions) are generally smaller than their neutral atoms due to the loss of electrons, which reduces electron-electron repulsion. Conversely, anions (negatively charged ions) are larger than their neutral atoms because the addition of electrons increases repulsion among them. Understanding ionic radius is crucial for comparing the sizes of different ions.

The charge of an ion significantly influences its size. Cations with higher positive charges, such as Sr²⁺, are smaller than those with lower positive charges, like Rb⁺, because the increased nuclear charge pulls the remaining electrons closer to the nucleus. In contrast, anions like Br^- are larger than cations due to the added electron, which increases electron-electron repulsion, leading to a larger ionic size.

Trends in the periodic table, such as atomic size and ionic size, help predict the relative sizes of ions. Generally, ionic size decreases across a period from left to right due to increasing nuclear charge and increases down a group due to the addition of electron shells. Recognizing these trends allows for a systematic approach to comparing the sizes of ions like Rb⁺, Br^-, and Sr²⁺.