Which of the following processes is not exhibited by atoms in order to attain more stable electron configuration?

Analyze the question

The question asks which process atoms do NOT use to reach a stable electron configuration (usually a full outer shell, like the noble gases).

Explain the concept

Atoms become stable by achieving an octet (or duplet for H and He). They do this through three main routes:

1. Gaining electrons: non-metals like Cl and O form anions (ionic bonding). Example: Cl + e⁻ → Cl⁻
2. Losing electrons: metals like Na and Mg form cations (ionic bonding). Example: Na → Na⁺ + e⁻
3. Sharing electrons: non-metals form covalent bonds. Example: H₂, H₂O, CH₄

Evaluate each option

• A. Gaining of electrons: a way atoms become stable (e.g., Cl⁻).
• B. Hybridization of orbitals: this is a theoretical model that describes the mixing of atomic orbitals (e.g., sp³ in methane) to explain molecular geometry and bond formation. It is not a process by which atoms gain, lose or share electrons to fill their outer shell. It happens as part of bonding but is not itself a way of attaining a noble gas configuration.
• C. Losing electrons: a way atoms become stable (e.g., Na⁺).
• D. Sharing electrons: a way atoms become stable (covalent bonding).

Answer

Option B, hybridization of orbitals, is the process not exhibited by atoms as a means of attaining a stable electron configuration.

Tip

When you see "attain stable configuration," think of the three electron-transfer routes: gain, lose, share. Anything else, such as hybridization, is a model for explaining shape and not a stabilizing electron process.