Final answer:
Sodium achieves stability by losing its one valence electron to form a sodium cation (Na+), resulting in a positive charge and a stable electron configuration resembling that of neon. Option b is the answer.
Step-by-step explanation:
The most likely way for sodium (Na), with an atomic number of 11, to become stable is by losing its one valence electron to form a sodium cation (Na+). This process results in the sodium atom having one more proton than electrons, giving it a positive charge. The valence electron sodium loss originates from the 3s orbital, following a 1s²2s²2p⁶3s¹ electron configuration. By losing this electron, sodium achieves an electron configuration that resembles the noble gas neon ([Ne]), which signifies stability.
Noble gases like neon have a full valence shell, which is the most stable electron arrangement. Sodium, being an alkali metal, finds stability by losing its outermost electron to match the noble gas electron configuration. Therefore, through this transformation, sodium becomes a cation, specifically a Na+ ion with a full outer shell.