The proper formula for the compound formed between aluminum and fluorine is AlF3, as aluminum has a +3 charge and fluorine has a -1 charge, and these combine in a 1:3 ratio to balance the charges.
The correct chemical formula for the compound formed by aluminum and fluorine is AlF3. The rationale behind this formula lies in the charges of the individual ions. Aluminum, as an element, carries a charge of +3 (Al3+), while fluorine is known for its charge of -1 (F-).
When these ions combine to create an ionic compound, the goal is to establish a ratio that equalizes the total positive and negative charges, achieving charge neutrality. In the case of aluminum and fluorine, the most stable and balanced arrangement is realized when one aluminum ion, carrying a +3 charge, combines with three fluorine ions, each bearing a -1 charge.
This 1:3 ratio ensures that the resulting compound, AlF3, maintains overall electrical neutrality. The empirical formula AlF3 represents the simplest whole-number ratio that effectively balances the charge disparity between aluminum and fluorine ions.