Certainly! Let's complete the table by filling in the symbols for the cations and anions for the given ionic compounds.
1. For [tex]\( \text{MnBr}_2 \)[/tex]:
- The cation is [tex]\( \text{Mn}^{2+} \)[/tex].
- The anion is [tex]\( \text{Br}^{-} \)[/tex].
2. For [tex]\( \text{VCl}_2 \)[/tex]:
- The cation is [tex]\( \text{V}^{2+} \)[/tex].
- The anion is [tex]\( \text{Cl}^{-} \)[/tex].
3. For [tex]\( \text{AuF}_3 \)[/tex]:
- The cation is [tex]\( \text{Au}^{3+} \)[/tex].
- The anion is [tex]\( \text{F}^{-} \)[/tex].
4. For [tex]\( \text{Fe}_2\text{S}_3 \)[/tex]:
- The cation is [tex]\( \text{Fe}^{3+} \)[/tex].
- The anion is [tex]\( \text{S}^{2-} \)[/tex].
Here is the completed table:
[tex]\[
\begin{tabular}{|c|c|c|}
\hline \begin{tabular}{c}
ionic \\
compound
\end{tabular} & cation & anion \\
\hline NaCl & $Na ^{+}$ & $Cl ^{-}$ \\
\hline $MnBr _2$ & $Mn ^{2+}$ & $Br ^{-}$ \\
\hline $VCl _2$ & $V ^{2+}$ & $Cl ^{-}$ \\
\hline $AuF _3$ & $Au ^{3+}$ & $F ^{-}$ \\
\hline $Fe _2 S_3$ & $Fe ^{3+}$ & $S ^{2-}$ \\
\hline
\end{tabular}
\][/tex]
These are the symbols for the cations and anions in each of the ionic compounds.
