Questions: Complete the table below by writing the symbols for the cation and anion that make up each ionic compound. The first row has been completed for you. ionic compound cation anion ------------------------------- NaCl Na+ Cl- AuBr3 MnI4 Cr2 S3 FeCl2

Complete the table below by writing the symbols for the cation and anion that make up each ionic compound. The first row has been completed for you.

 ionic compound  cation  anion 
-------------------------------
 NaCl            Na+     Cl-   
 AuBr3                         
 MnI4                          
 Cr2 S3                        
 FeCl2
Transcript text: Complete the table below by writing the symbols for the cation and anion that make up each lonic compound. The first row has been completed for you. \begin{tabular}{|c|c|c|} \hline \begin{tabular}{c} ionic \\ compound \end{tabular} & cation & anion \\ \hline NaCl & $\mathrm{Na}^{+}$ & $\mathrm{Cl}^{-}$ \\ \hline $\mathrm{AuBr}_{3}$ & $\square$ & $\square$ \\ \hline $\mathrm{MnI}_{4}$ & $\square$ & $\square$ \\ \hline $\mathrm{Cr}_{2} \mathrm{~S}_{3}$ & $\square$ & $\square$ \\ \hline $\mathrm{FeCl}_{2}$ & $\square$ & $\square$ \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Identify the Cation and Anion for Each Compound

To complete the table, we need to identify the cation and anion for each ionic compound. An ionic compound is composed of positively charged ions (cations) and negatively charged ions (anions).

Step 2: Determine the Cation and Anion for Each Compound
  1. For \(\mathrm{AuBr}_{3}\):

    • Cation: Gold (III) ion, \(\mathrm{Au}^{3+}\)
    • Anion: Bromide ion, \(\mathrm{Br}^{-}\)
  2. For \(\mathrm{MnI}_{4}\):

    • Cation: Manganese (IV) ion, \(\mathrm{Mn}^{4+}\)
    • Anion: Iodide ion, \(\mathrm{I}^{-}\)
  3. For \(\mathrm{Cr}_{2}\mathrm{S}_{3}\):

    • Cation: Chromium (III) ion, \(\mathrm{Cr}^{3+}\)
    • Anion: Sulfide ion, \(\mathrm{S}^{2-}\)
  4. For \(\mathrm{FeCl}_{2}\):

    • Cation: Iron (II) ion, \(\mathrm{Fe}^{2+}\)
    • Anion: Chloride ion, \(\mathrm{Cl}^{-}\)

Final Answer

\[ \begin{array}{|c|c|c|} \hline \text{Ionic Compound} & \text{Cation} & \text{Anion} \\ \hline \mathrm{NaCl} & \mathrm{Na}^{+} & \mathrm{Cl}^{-} \\ \hline \mathrm{AuBr}_{3} & \mathrm{Au}^{3+} & \mathrm{Br}^{-} \\ \hline \mathrm{MnI}_{4} & \mathrm{Mn}^{4+} & \mathrm{I}^{-} \\ \hline \mathrm{Cr}_{2}\mathrm{S}_{3} & \mathrm{Cr}^{3+} & \mathrm{S}^{2-} \\ \hline \mathrm{FeCl}_{2} & \mathrm{Fe}^{2+} & \mathrm{Cl}^{-} \\ \hline \end{array} \]

\[ \boxed{ \begin{array}{c} \mathrm{AuBr}_{3}: \, \mathrm{Au}^{3+}, \, \mathrm{Br}^{-} \\ \mathrm{MnI}_{4}: \, \mathrm{Mn}^{4+}, \, \mathrm{I}^{-} \\ \mathrm{Cr}_{2}\mathrm{S}_{3}: \, \mathrm{Cr}^{3+}, \, \mathrm{S}^{2-} \\ \mathrm{FeCl}_{2}: \, \mathrm{Fe}^{2+}, \, \mathrm{Cl}^{-} \\ \end{array} } \]

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