Ionic bonds typically occur between metals and nonmetals. In this type of bond, electrons are transferred from one atom to another, leading to the formation of charged ions.
Here's a more detailed breakdown of how this process works:
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Electron Transfer: A metal atom, which has a low electronegativity, tends to lose one or more electrons to achieve a stable electron configuration, often resembling that of the nearest noble gas. This loss of electrons converts the metal atom into a positively charged ion, known as a cation.
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Formation of Anion: A nonmetal atom, which has a higher electronegativity, tends to gain electrons in order to achieve a full outer shell, again resembling the nearest noble gas configuration. This gain of electrons turns the nonmetal atom into a negatively charged ion, known as an anion.
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Electrostatic Attraction: Once the cation and anion are formed, they are attracted to each other due to their opposite charges. This strong electrostatic force of attraction between the positively charged cation and the negatively charged anion constitutes the ionic bond.
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Crystal Lattice Structure: In solid form, ionic compounds tend to form a crystalline structure where ions are arranged in a repeating pattern, maximizing attractions and minimizing repulsions among the charged ions.
In summary, ionic bonds are formed through the transfer of electrons from metals to nonmetals, resulting in the formation of cations and anions that are held together by electrostatic forces.