Let's complete the table by filling in the empirical formula and name of each ionic compound with cations Cu²⁺, Fe²⁺, Co³⁺, and Mn³⁺, paired respectively with anions O²⁻, S²⁻, N³⁻, and P³⁻.
1. For the cation Cu²⁺ and anion O²⁻:
- The charges cancel out each other because Cu has a +2 charge and O has a -2 charge.
- Therefore, the empirical formula for this compound is CuO.
- The name of the compound is Copper(II) Oxide.
2. For the cation Fe²⁺ and anion S²⁻:
- The charges cancel out each other because Fe has a +2 charge and S has a -2 charge.
- Therefore, the empirical formula for this compound is FeS.
- The name of the compound is Iron(II) Sulfide.
3. For the cation Co³⁺ and anion N³⁻:
- The charges cancel out each other because Co has a +3 charge and N has a -3 charge.
- Therefore, the empirical formula for this compound is CoN.
- The name of the compound is Cobalt(III) Nitride.
4. For the cation Mn³⁺ and anion P³⁻:
- The charges cancel out each other because Mn has a +3 charge and P has a -3 charge.
- Therefore, the empirical formula for this compound is MnP.
- The name of the compound is Manganese(III) Phosphide.
So, the completed table is:
[tex]\[
\begin{tabular}{|l|l|l|l|}
\hline
\multicolumn{2}{|c|}{Some ionic compounds} \\
\hline
cation & anion & empirical formula & name of compound \\
\hline
Cu²⁺ & O²⁻ & CuO & Copper(II) Oxide \\
\hline
Fe²⁺ & S²⁻ & FeS & Iron(II) Sulfide \\
\hline
Co³⁺ & N³⁻ & CoN & Cobalt(III) Nitride \\
\hline
Mn³⁺ & P³⁻ & MnP & Manganese(III) Phosphide \\
\hline
\end{tabular}
\][/tex]
