A Level Chemistry OCR Practice Exam

Which of the following describes the nature of ionic bonds?

1. Weak forces that hold molecules together.

2. Strong interactions between oppositely charged ions.

3. Covalent bonds formed between non-metals.

4. Attractive forces that arise from dipole interactions.

The correct answer is: Strong interactions between oppositely charged ions.

The characteristic nature of ionic bonds is indeed represented by strong interactions between oppositely charged ions. Ionic bonds form when one atom donates an electron to another, resulting in the creation of positively charged cations and negatively charged anions. The electrostatic attraction between these oppositely charged ions is what constitutes the ionic bond, and this attraction is typically quite strong compared to other types of chemical bonds. This strong nature of ionic bonds contributes to the high melting and boiling points of ionic compounds, as significant energy is required to overcome these interactions. Ionic bonding also results in the formation of crystalline structures, which is reflective of the orderly arrangement of the ions in a lattice that maximizes the attractive forces between them. The other choices presented do not accurately define ionic bonds. Instead, they refer to different types of interactions. For instance, weak forces that hold molecules together typically describe van der Waals forces or hydrogen bonding rather than ionic bonding. Covalent bonds, formed between non-metals, involve the sharing of electrons rather than the transfer seen in ionic bonds. Finally, attractive forces arising from dipole interactions pertain to polar molecules rather than the distinct ion-ion interactions in ionic bonding.