Final answer:
The four ionic compounds are magnesium phosphate (Mg₃(PO₄)₂), magnesium nitrate (Mg(NO₃)₂), iron(III) phosphate (FePO₄), and iron(III) nitrate (Fe(NO₃)₃), created by combining Mg²⁺ and Fe³⁺ with PO₄³⁺ and NO₃⁺, ensuring charge balance in each compound.
Step-by-step explanation:
The formulas for the four ionic compounds formed by combining the cations Mg²⁺ and Fe³⁺ with the anions PO₄³⁺ and NO₃⁺ are as follows:
- Magnesium phosphate: Mg₃(PO₄)₂
- Magnesium nitrate: Mg(NO₃)₂
- Iron(III) phosphate: FePO₄
- Iron(III) nitrate: Fe(NO₃)₃
The naming of each compound takes into account the charges of the ions to ensure electrical neutrality. For example, because PO₄³⁺ has a -3 charge, three Mg²⁺ ions are needed to balance the charge, resulting in Mg₃(PO₄)₂. Similarly, one Fe³⁺ ion balances with one PO₄³⁺ ion to form FePO₄.
When combining the cations Mg²⁺ and Fe³⁺ with the anions PO₄³⁻ and NO³⁻, we can form four ionic compounds:
Mg₃(PO₄)₂ - Magnesium phosphate
Mg(NO₃)₂ - Magnesium nitrate
FePO₄ - Iron(III) phosphate
Fe(NO₃)₃ - Iron(III) nitrate
The formula for each compound can be determined by finding the combination of charges that balances out to zero. For example, the magnesium ion (Mg²⁺) with the phosphate ion (PO₄³⁻) results in the compound Mg₃(PO₄)₂.