Where are electrons transferred between in an ionic bond?

In an ionic bond, electrons are transferred between positive metal atoms and negative non-metal atoms. This process occurs because metals tend to lose electrons and form positively charged ions (cations), whereas non-metals typically gain those electrons to form negatively charged ions (anions).

When a metal atom gives up one or more of its electrons, it becomes positively charged, while the non-metal, by accepting those electrons, becomes negatively charged. This transfer results in the formation of oppositely charged ions, which are then held together by strong electrostatic forces of attraction. This is the key characteristic of ionic bonding.

In contrast, other options do not accurately describe the behavior of electrons in ionic bonds. Non-metal atoms generally do not transfer electrons to each other, neutral atoms do not engage in the formation of ionic bonds (as they require changes in charge), and ions of the same charge would repel each other rather than form a bond.