Concept:Ionic bonds form so that both participating atoms can achieve a stable, lower-energy electron configuration, typically an octet.
Formula:$$ \text{Na} \rightarrow \text{Na}^+ \ ([\text{Ne}]) \quad ; \quad \text{Cl} + e^- \rightarrow \text{Cl}^- \ ([\text{Ar}]) $$
Solution:- Metals lose electrons to empty their valence shell, exposing the full stable shell beneath (becoming isoelectronic with the preceding noble gas).
- Nonmetals gain electrons to completely fill their current valence shell (becoming isoelectronic with the succeeding noble gas).
- Thus, in stable ionic crystal lattices, both the resulting cations and anions achieve a stable noble gas configuration.
Why other options are incorrect:- Option A & Option D: It is not an exclusive process; both ions achieve stability simultaneously.
- Option C: While true that total electrons lost equals total gained in the bulk compound, option B is the fundamental driving force for the individual ions' stability as per standard textbook phrasing.
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