Answer:
Here are the empirical formulas of four binary ionic compounds that could be formed from the given ions:
- MgF2 (magnesium fluoride)
- Al2O3 (aluminum oxide)
- MgO (magnesium oxide)
- AlF3 (aluminum fluoride)
The empirical formula of an ionic compound gives the simplest whole-number ratio of the ions present in the compound. The formula is determined by balancing the charges of the cation and anion so that the compound as a whole is electrically neutral.
Step-by-step explanation:
The empirical formula of a compound is the simplest whole-number ratio of the atoms in the compound. Binary ionic compounds are formed by the combination of a metal cation with a non-metal anion.
In this case, the given ions are Mg2+, Al3+, F−, and O2−. To form binary ionic compounds, we need one cation and one anion.
Here are some possible combinations of these ions, along with their empirical formulas:
- Mg2+ and F−: MgF2
- Al3+ and F−: AlF3
- Mg2+ and O2−: MgO
- Al3+ and O2−: Al2O3
In each case, the positive and negative charges of the ions balance to form a neutral compound. The empirical formula is found by writing the subscripts for each element in the simplest ratio that achieves this balance.