Final answer:
The empirical formulas of the ionic compounds formed from the given pairs of elements are: MgCl₂, CsBr, GaI₃, Na₂O, SrF₂, and Ca₃(PO₄)₂.
Step-by-step explanation:
The empirical formula of an ionic compound is the simplest whole number ratio of the ions present in the compound. To predict the empirical formulas of the ionic compounds formed, we need to consider the charges of the ions. Here are the empirical formulas for the given pairs of elements:
Mg and Cl: The magnesium ion has a charge of +2 (Mg2+), and the chloride ion has a charge of -1 (Cl-). To balance the charges, we need two chloride ions for every one magnesium ion. Therefore, the empirical formula is MgCl₂.
Cs and Br: The cesium ion has a charge of +1 (Cs+), and the bromide ion has a charge of -1 (Br-). The charges are already balanced, so the empirical formula is CsBr.
Ga and I: The gallium ion has a charge of +3 (Ga3+), and the iodide ion has a charge of -1 (I-). To balance the charges, we need three iodide ions for every one gallium ion. Therefore, the empirical formula is GaI₃.
Na and O: The sodium ion has a charge of +1 (Na+), and the oxide ion has a charge of -2 (O2-). To balance the charges, we need two sodium ions for every one oxide ion. Therefore, the empirical formula is Na₂O.
Sr and F: The strontium ion has a charge of +2 (Sr2+), and the fluoride ion has a charge of -1 (F-). To balance the charges, we need two fluoride ions for every one strontium ion. Therefore, the empirical formula is SrF₂.
Ca and P: The calcium ion has a charge of +2 (Ca2+), and the phosphate ion has a charge of -3 (PO₄³-). To balance the charges, we need three calcium ions for every two phosphate ions. Therefore, the empirical formula is Ca₃(PO₄)₂.