Multiple Choice
Which of the following is the correct chemical formula for the ionic compound formed between magnesium and iodine?
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3. Chemical Reactions
Writing Ionic Compounds
Multiple Choice
Which of the following is the correct formula for the ionic compound formed when Mg^{2+} reacts with P^{3-}?
A
Mg_2P
B
Mg_3P_2
C
MgP
D
Mg_2P_3
Verified step by step guidance1
Identify the charges on the ions involved: magnesium ion is \(\mathrm{Mg^{2+}}\) and phosphide ion is \(\mathrm{P^{3-}}\).
To form a neutral ionic compound, the total positive charge must balance the total negative charge.
Determine the smallest whole number ratio of \(\mathrm{Mg^{2+}}\) and \(\mathrm{P^{3-}}\) ions that results in charge neutrality. This means finding the least common multiple (LCM) of the charges 2 and 3.
The LCM of 2 and 3 is 6, so the total positive charge should be +6 and the total negative charge should be -6.
Calculate the number of each ion needed: for \(\mathrm{Mg^{2+}}\), \$3\( ions give \(3 \times (+2) = +6\); for \(\mathrm{P^{3-}}\), \)2$ ions give \(2 \times (-3) = -6\). Therefore, the formula is \(\mathrm{Mg_3P_2}\).
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