Fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table:
| cation | anion | empirical formula | name of compound |
|---|---|---|---|
| [tex]Mg ^{2+}[/tex] | [tex]SO _4^{2-}[/tex] | | |
| [tex]Pb ^{2+}[/tex] | [tex]MnO _4[/tex] | | |
| [tex]K ^{+}[/tex] | [tex]PO _3^{3-}[/tex] | | |
Answer (1)
Determine the empirical formula for M g 2 + and S O 4 2 − : M g S O 4 .
Determine the empirical formula for P b 2 + and M n O 4 − : P b ( M n O 4 ) 2 .
Determine the empirical formula for K + and P O 3 3 − : K 3 P O 3 .
The names of the compounds are magnesium sulfate, lead(II) permanganate, and potassium phosphite, respectively. M g S O 4 , magnesium sulfate ; P b ( M n O 4 ) 2 , lead(II) permanganate ; K 3 P O 3 , potassium phosphite
Explanation
Problem Analysis We are given a table with cations and anions, and we need to determine the empirical formula and name of the ionic compound formed by each cation-anion pair.
Magnesium Sulfate For the first pair, we have M g 2 + and S O 4 2 − . The charges are +2 and -2, respectively. To form a neutral compound, we need one magnesium ion and one sulfate ion. Therefore, the empirical formula is M g S O 4 . The name of the compound is magnesium sulfate.
Lead(II) Permanganate For the second pair, we have P b 2 + and M n O 4 − . The charges are +2 and -1, respectively. To form a neutral compound, we need one lead(II) ion and two permanganate ions. Therefore, the empirical formula is P b ( M n O 4 ) 2 . The name of the compound is lead(II) permanganate.
Potassium Phosphite For the third pair, we have K + and P O 3 3 − . The charges are +1 and -3, respectively. To form a neutral compound, we need three potassium ions and one phosphite ion. Therefore, the empirical formula is K 3 P O 3 . The name of the compound is potassium phosphite.
Final Answer The empirical formulas and names of the ionic compounds are:
M g S O 4 , magnesium sulfate P b ( M n O 4 ) 2 , lead(II) permanganate K 3 P O 3 , potassium phosphite
Examples
Ionic compounds are used in various applications in everyday life. For example, sodium chloride (NaCl), also known as table salt, is used to season food. Calcium carbonate (CaCO3) is a common ingredient in antacids and is also used in the construction industry as a component of cement. Potassium iodide (KI) is added to table salt to prevent iodine deficiency. Understanding the formation and properties of ionic compounds is crucial in many fields, including chemistry, biology, and materials science.
