Question

Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions. Choose the correct options from the provided choices.

A. Sodium (Na+) and Chloride (Cl-)
B. Magnesium (Mg2+) and Sulfide (S2-)
C. Aluminum (Al3+) and Oxygen (O2-)
D. Potassium (K+) and Iodide (I-)

Answer 1

The empirical formulas for binary ionic compounds between given ion pairs are NaCl, MgS, Al2O3, and KI, determined by neutralizing the charges of the ions to create a neutral compound. The correct answer is D. Potassium (K+) and Iodide (I-).

Step-by-step explanation:

The empirical formula of a binary ionic compound is determined by the charges of the ions involved, ensuring that the overall charge of the compound is neutral. Here is how we write the empirical formula for the given binary ionic compounds:

A. Sodium (Na+) and Chloride (Cl-): The empirical formula is NaCl, as the charges balance out with one sodium ion for each chloride ion. B. Magnesium (Mg2+) and Sulfide (S2-): The empirical formula is MgS, achieved by combining one magnesium ion with one sulfide ion. C. Aluminum (Al3+) and Oxygen (O2-): The empirical formula is Al2O3, since two aluminum ions will balance with three oxide ions. D. Potassium (K+) and Iodide (I-): The empirical formula is KI, with one potassium ion for each iodide ion. To determine these formulas, we use the criss-cross method, swapping the magnitude of each ion's charge to become the subscript of the other ion. The correct answer is D. Potassium (K+) and Iodide (I-).