Questions: Fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table: Some ionic compounds cation anion empirical formula name of compound Mg^2+ P^3- Mg^2+ S^2- Mg^2+ N^3- Mg^2+ O^2-

Fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table:

Some ionic compounds

cation anion empirical formula name of compound

Mg^2+ P^3-

Mg^2+ S^2-

Mg^2+ N^3-

Mg^2+ O^2-

Transcript text: Fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table: \begin{tabular}{|l|c|c|c|} \hline \multicolumn{3}{|c|}{ Some ionic compounds } \\ \hline cation & anion & empirical formula & name of compound \\ \hline $\mathrm{Mg}^{2+}$ & $\mathrm{P}^{3-}$ & $\square$ & $\square$ \\ \hline $\mathrm{Mg}^{2+}$ & $\mathrm{S}^{2-}$ & $\square$ & $\square$ \\ \hline $\mathrm{Mg}^{2+}$ & $\mathrm{N}^{3-}$ & $\square$ & $\square$ \\ \hline $\mathrm{Mg}^{2+}$ & $\mathrm{O}^{2-}$ & $\square$ & $\square$ \\ \hline \end{tabular}

Solution

Solution Steps

Step 1: Determine the Empirical Formula for Each Compound

To find the empirical formula of an ionic compound, balance the total positive and negative charges. The cation is $\mathrm{Mg}^{2+}$, and the anions are $\mathrm{P}^{3-}$, $\mathrm{S}^{2-}$, $\mathrm{N}^{3-}$, and $\mathrm{O}^{2-}$.

For $\mathrm{Mg}^{2+}$ and $\mathrm{P}^{3-}$:
- The least common multiple of 2 and 3 is 6.
- Therefore, we need 3 $\mathrm{Mg}^{2+}$ ions and 2 $\mathrm{P}^{3-}$ ions to balance the charges.
- Empirical formula: $\mathrm{Mg}_3\mathrm{P}_2$.
For $\mathrm{Mg}^{2+}$ and $\mathrm{S}^{2-}$:
- The charges are already balanced with one $\mathrm{Mg}^{2+}$ and one $\mathrm{S}^{2-}$.
- Empirical formula: $\mathrm{MgS}$.
For $\mathrm{Mg}^{2+}$ and $\mathrm{N}^{3-}$:
- The least common multiple of 2 and 3 is 6.
- Therefore, we need 3 $\mathrm{Mg}^{2+}$ ions and 2 $\mathrm{N}^{3-}$ ions to balance the charges.
- Empirical formula: $\mathrm{Mg}_3\mathrm{N}_2$.
For $\mathrm{Mg}^{2+}$ and $\mathrm{O}^{2-}$:
- The charges are already balanced with one $\mathrm{Mg}^{2+}$ and one $\mathrm{O}^{2-}$.
- Empirical formula: $\mathrm{MgO}$.

Step 2: Determine the Name of Each Compound

The name of an ionic compound is typically the name of the cation followed by the name of the anion.

For $\mathrm{Mg}_3\mathrm{P}_2$:
- Cation: Magnesium
- Anion: Phosphide
- Name: Magnesium phosphide
For $\mathrm{MgS}$:
- Cation: Magnesium
- Anion: Sulfide
- Name: Magnesium sulfide
For $\mathrm{Mg}_3\mathrm{N}_2$:
- Cation: Magnesium
- Anion: Nitride
- Name: Magnesium nitride
For $\mathrm{MgO}$:
- Cation: Magnesium
- Anion: Oxide
- Name: Magnesium oxide

Final Answer

\[ \begin{array}{|l|c|c|c|} \hline \text{cation} & \text{anion} & \text{empirical formula} & \text{name of compound} \\ \hline \mathrm{Mg}^{2+} & \mathrm{P}^{3-} & \boxed{\mathrm{Mg}_3\mathrm{P}_2} & \boxed{\text{Magnesium phosphide}} \\ \hline \mathrm{Mg}^{2+} & \mathrm{S}^{2-} & \boxed{\mathrm{MgS}} & \boxed{\text{Magnesium sulfide}} \\ \hline \mathrm{Mg}^{2+} & \mathrm{N}^{3-} & \boxed{\mathrm{Mg}_3\mathrm{N}_2} & \boxed{\text{Magnesium nitride}} \\ \hline \mathrm{Mg}^{2+} & \mathrm{O}^{2-} & \boxed{\mathrm{MgO}} & \boxed{\text{Magnesium oxide}} \\ \hline \end{array} \]

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