Which of the following is the correct formula for an ionic compound formed between Ba^{2+} ions and Cl^{-} ions?

• A. BaCl_2
• B. Ba_2Cl_2
• C. Ba_2Cl
• D. BaCl

Answer: (A)

Verified step by step guidance

1. Identify the charges of the ions involved: Ba^{2+} has a charge of +2, and Cl^{-} has a charge of -1.
2. Determine the ratio of ions needed to balance the total positive and negative charges so that the compound is electrically neutral.
3. Since Ba^{2+} has a +2 charge, and each Cl^{-} has a -1 charge, two Cl^{-} ions are needed to balance one Ba^{2+} ion.
4. Write the formula by placing the cation first followed by the anion, using subscripts to indicate the number of each ion: \(\mathrm{BaCl_2}\).
5. Verify that the total positive charge equals the total negative charge: \(+2\) from Ba^{2+} and \$2 \times (-1) = -2$ from two Cl^{-} ions, confirming the compound is neutral.