What is the primary force that holds ionic compounds together?

Ionic compounds are formed when atoms transfer electrons, leading to the formation of ions with opposite charges. The primary force that holds these ions together is the ionic bond, which arises from the electrostatic attraction between the positively charged cations and negatively charged anions. This attraction is quite strong; hence, ionic compounds typically have high melting and boiling points and form crystalline structures.

In an ionic bond, the transfer of electrons results in the formation of stable electron configurations, similar to those of noble gases. This stability is a key factor that drives the formation of ionic compounds.

The other types of forces listed, such as covalent bonds, metallic bonds, and Van der Waals forces, are distinct in their mechanisms and characteristics. Covalent bonds involve the sharing of electrons between atoms, metallic bonds consist of a 'sea' of delocalized electrons around positively charged metal ions, and Van der Waals forces are weak intermolecular attractions. None of these forces encapsulate the unique interaction characteristic of ionic compounds, which is why the ionic bond is the correct answer.