Ionic bonding

Ionic bonding is the electrostatic attraction between oppositely charged ions. It commonly arises when electron transfer creates cations and anions that assemble into extended solids.

Ion: An atom or molecule with a net electric charge because it has gained or lost electrons. Ionic bonding acts between ions rather than neutral atoms.
Electrostatic force: The force of attraction or repulsion between electrically charged bodies. Ionic bonding is the collective electrostatic attraction among oppositely charged ions.
Sodium chloride: An ionic compound composed of sodium cations and chloride anions in a 1:1 ratio. Its rock-salt crystal is a standard example of an ionic solid.
Covalent bond: A chemical bond formed when atoms share one or more pairs of electrons. It contrasts electron sharing with the electrostatic attraction between ions.
Cation: A positively charged ion formed by losing one or more electrons. Cations provide the positive charges attracted to anions.
Coulomb's law: A law describing how the electric force between point charges depends on their magnitudes and separation. It predicts stronger attraction for larger charges and shorter ion-to-ion distances.
Magnesium oxide: An ionic compound of magnesium and oxygen with formula MgO. Its doubly charged ions illustrate how charge magnitude strengthens lattice attraction.
Metallic bond: A bond in metals arising from attraction between positive atomic cores and delocalized electrons. It explains conductivity in solids without requiring distinct cations and anions.
Anion: A negatively charged ion formed by gaining one or more electrons. Anions provide the negative charges attracted to cations.
Ionization energy: The energy required to remove an electron from an isolated atom or ion in the gas phase. Electron transfer must overcome the energy cost of creating a cation.

Linked from 110 pages