What happens to electrons when an ionic solution is formed?

Answer 1

Generally the electrons are transfered from the metal elements to the nonmetalic elements so that both form stable electron configurations. For example, in sodium chloride one sodium atom loses an electron so that it has the stable electron configuration of Neon and chlorine gains one electron so that it has the stable electron configuration of Argon. This results in negativley charged chlorine atoms and positively charged sodium atoms which are then attracted to each other and form the ionic bond. Having a lot of those atoms and therefore a lot of those bonds gives an ionic compound. Generally no bonds are fully ionic or covalent; they have what is called percent ionic character that is a measurement of how much the bond resembles an ionic bond rather than a covalent bond (in covalent bonds electrons are shared between the atoms).

Answer 2

In ionic compounds, electrons are transferred from the metal to the non-metal. This gives each ion a full outer main energy level (or electron shell), thus making them stable particles.

Take sodium chloride. Sodium needs to lose one electron, while chlorine needs to accept an electron, if they're to have full outer energy levels. The electron from sodium moves to the chlorine, forming ions in the process.

Answer 3

In an ionic solution, electrons are transferred from one atom to another, resulting in the formation of ions. The atom that loses electrons becomes a positively charged cation, while the atom that gains electrons becomes a negatively charged anion. These ions are then free to move and carry an electric current within the solution.

Answer 4

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