To understand the transfer of electrons in aluminum chloride (AlCl3), we start by looking at the elements involved: aluminum (Al) and chlorine (Cl).
Aluminum has three electrons in its outermost shell (valence shell), while each chlorine atom has seven electrons in its valence shell. To achieve a stable electronic configuration, aluminum can lose its three valence electrons, while each chlorine atom needs one electron to complete its outer shell.
The Lewis dot structure for aluminum chloride can be drawn by showing aluminum in the center with three dots (representing its valence electrons) and surrounding it with three chlorine atoms, each with seven dots. Each chlorine atom will receive one electron from aluminum, forming ionic bonds.
In summary, the transfer of electrons results in aluminum losing three electrons to form a positively charged aluminum ion (Al3+), and each chlorine atom gaining one electron to form negatively charged chloride ions (Cl–).
The chemical formula for this compound is AlCl3, indicating that one aluminum ion bonds with three chloride ions.