What occurs when a metal reacts with a non-metal to form an ionic bond?

When a metal reacts with a non-metal to form an ionic bond, the characteristic behavior is that the metal loses electrons. This loss of electrons results in the formation of a positive ion, also known as a cation. Metals tend to have a relatively low electronegativity, meaning they can easily lose their outer electrons during chemical reactions.

As the metal loses one or more electrons, it becomes positively charged because it now has more protons than electrons. This positively charged ion can then interact with a non-metal. Non-metals, on the other hand, have a higher electronegativity and tend to gain electrons to achieve a full outer shell, resulting in the formation of a negatively charged ion, or anion.

The ionic bond is formed due to the electrostatic attraction between the positively charged metal ion and the negatively charged non-metal ion. This mutual attraction stabilizes both ions and leads to the formation of ionic compounds, which have distinct properties compared to covalently bonded substances.