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Complete the table below by writing the symbols for the cation and anion.

\begin{tabular}{|c|c|c|}
\hline
\begin{tabular}{c}
Ionic \\
Compound
\end{tabular} & Cation & Anion \\
\hline NaCl & [tex]$Na^{+}$[/tex] & [tex]$Cl^{-}$[/tex] \\
\hline [tex]$MnBr_2$[/tex] & [tex]$\square$[/tex] & [tex]$\square$[/tex] \\
\hline [tex]$VCl_2$[/tex] & [tex]$\square$[/tex] & [tex]$\square$[/tex] \\
\hline [tex]$AuF_3$[/tex] & [tex]$\square$[/tex] & [tex]$\square$[/tex] \\
\hline [tex]$Fe_2S_3$[/tex] & [tex]$\square$[/tex] & [tex]$\square$[/tex] \\
\hline
\end{tabular}



Answer :

GinnyAnswer
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.

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