* Electronegativity: Aluminum (Al) has an electronegativity of 1.61, while sulfur (S) has an electronegativity of 2.58. The difference in electronegativity between these two elements is significant (2.58 - 1.61 = 0.97), indicating a large difference in their ability to attract electrons.
* Electron Transfer: Aluminum, a metal, tends to lose electrons to achieve a stable octet configuration. Sulfur, a nonmetal, tends to gain electrons to achieve a stable octet configuration. In this case, aluminum will lose three electrons to form a 3+ cation (Al³⁺), while sulfur will gain two electrons to form a 2- anion (S²⁻).
* Ionic Bond Formation: The electrostatic attraction between the positively charged aluminum ion (Al³⁺) and the negatively charged sulfur ion (S²⁻) forms an ionic bond.
Therefore, the resulting compound is aluminum sulfide (Al₂S₃), where the ratio of aluminum to sulfur atoms is 2:3 to maintain electrical neutrality.
