How many Mg^{2+} ions are present in 3.00 moles of MgCl_2?

• A. 6.02 \times 10^{23} ions
• B. 9.03 \times 10^{24} ions
• C. 3.61 \times 10^{24} ions
• D. 1.81 \times 10^{24} ions

Answer: (C)

Verified step by step guidance

1. Identify the chemical formula of the compound: MgCl_2 contains one Mg^{2+} ion per formula unit.
2. Determine the number of moles of Mg^{2+} ions in 3.00 moles of MgCl_2. Since each mole of MgCl_2 contains 1 mole of Mg^{2+}, the moles of Mg^{2+} ions is equal to 3.00 moles.
3. Recall Avogadro's number, which is the number of particles (atoms, ions, molecules) in one mole: \$6.02 \times 10^{23}$ particles/mole.
4. Calculate the total number of Mg^{2+} ions by multiplying the moles of Mg^{2+} ions by Avogadro's number: \(\text{Number of ions} = 3.00 \text{ moles} \times 6.02 \times 10^{23} \text{ ions/mole}\).
5. Express the final answer in scientific notation to match the format of the options given.