Which statement best explains which compound, NaCl or BeO, has a stronger ionic bond?

• A. BeO has a weaker ionic bond than NaCl because beryllium and oxygen are smaller atoms.
• B. BeO has a stronger ionic bond than NaCl because Be and O have higher charges, resulting in greater electrostatic attraction.
• C. NaCl has a stronger ionic bond than BeO because it forms a larger crystal lattice.
• D. NaCl has a stronger ionic bond than BeO because sodium and chlorine are more electronegative.

Answer: (B)

Verified step by step guidance

1. Recall that the strength of an ionic bond depends primarily on the electrostatic attraction between the ions, which is described by Coulomb's law: \(F = \dfrac{k \cdot |q_1 \cdot q_2|}{r^2}\), where \(q_1\) and \(q_2\) are the charges of the ions and \(r\) is the distance between their centers.
2. Compare the charges of the ions in NaCl and BeO: NaCl consists of Na\(^{+}\) and Cl\(^{-}\) ions, each with a charge magnitude of 1, while BeO consists of Be\(^{2+}\) and O\(^{2-}\) ions, each with a charge magnitude of 2.
3. Consider the effect of ionic size: smaller ions mean a smaller distance \(r\) between ion centers, which increases the electrostatic force according to Coulomb's law. Be and O are smaller atoms compared to Na and Cl, so \(r\) is smaller in BeO.
4. Combine these factors: BeO has ions with higher charges and smaller ionic radii, both of which increase the electrostatic attraction and thus the ionic bond strength compared to NaCl.
5. Conclude that the stronger ionic bond in BeO is due to the higher charges on the ions and the smaller distance between them, resulting in a greater electrostatic attraction than in NaCl.