Understanding Ionic Bonds
Ionic bonds form between metals and nonmetals. The metal loses electrons to become a positively charged ion (cation), while the nonmetal gains electrons to become a negatively charged ion (anion). The electrostatic attraction between these oppositely charged ions creates the bond.
Let's analyze the pairs:
* Mg and F: Magnesium (Mg) is a metal in Group 2, and Fluorine (F) is a nonmetal in Group 17. This pair will readily form an ionic compound. Magnesium will lose two electrons to become Mg²⁺, and Fluorine will gain one electron to become F⁻. The resulting compound is MgF₂ (magnesium fluoride).
* O and Cl: Oxygen (O) and Chlorine (Cl) are both nonmetals. While they can form covalent bonds with each other (like in the molecule Cl₂O), they are unlikely to form a stable ionic compound. Nonmetals tend to share electrons rather than completely transfer them.
Conclusion:
The pair Mg and F is most likely to form an ionic compound because it involves a metal (Mg) and a nonmetal (F), fulfilling the key requirement for ionic bond formation.
