What Triggers Ionic Bonding in Atoms?

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Ionic bonds form through the transfer of electrons between atoms, typically involving a metal and a non-metal. In the example of sodium and chlorine, the sodium atom has one valence electron that it can easily lose, while chlorine has seven valence electrons and a strong tendency to gain one to achieve a stable octet configuration. The driving force behind this electron transfer is the difference in electronegativity between the two atoms, with chlorine having a much higher electronegativity than sodium. This creates a favorable energy change, as the formation of an ionic bond results in a lower energy state for the system. The process can be explained thermodynamically, where the energy released during the formation of the ionic bond compensates for the energy required to remove the electron from sodium. Thus, the interaction is not due to a "magic" force but rather the fundamental principles of atomic structure and energy stability.
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So I never got too far into chemistry and had never had much thought put into this. What exactly causes an ionic bond? And I mean, I know the usual 'one atom releases an electron and another gains it, causing net electric charges on both atoms', but what causes the electron to leave an atom to join another?

For example, a sodium atom coming near a chlorine atom. What causes the valence electron to disassociate with the sodium atom in the first place? A stronger dipole moment on the chlorine? magic? :)
 
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This has to be explained thermodynamically. I find this site pretty good.
 

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