Lattice energy changes with ion charges: which statement is true?

Lattice energy changes with ion charges: which statement is true?

• A. Decreases with Larger Charges
• B. Unrelated to Ion Charges
• C. Increases with Larger Charges
• D. Depends Only on Ion Size

Answer: (C)

Lattice energy reflects the strength of the electrostatic attraction between ions in a solid, so stronger attractions mean more energy needed to separate the ions. This energy scales with the product of the ions' charges and with how close they are to one another. When the charges are larger, the interaction is stronger, making the lattice energy larger. For example, an ionic compound with charges of ±2 (like MgO) has a higher lattice energy than one with ±1 (like NaCl), all else being equal. The size of the ions also matters—smaller ions bring ions closer together and increase lattice energy—but the charge magnitude is a key factor, and saying it depends only on ion size ignores the crucial role of the charges.

Lattice energy reflects the strength of the electrostatic attraction between ions in a solid, so stronger attractions mean more energy needed to separate the ions. This energy scales with the product of the ions' charges and with how close they are to one another. When the charges are larger, the interaction is stronger, making the lattice energy larger. For example, an ionic compound with charges of ±2 (like MgO) has a higher lattice energy than one with ±1 (like NaCl), all else being equal. The size of the ions also matters—smaller ions bring ions closer together and increase lattice energy—but the charge magnitude is a key factor, and saying it depends only on ion size ignores the crucial role of the charges.